Biswarup Chandra Dey

Fluoroform (CHF3) has a central carbon (C) atom with 4 valence electrons, bonded to three fluorine (F) atoms and one hydrogen (H) atom. Each F contributes 7 valence electrons, and H contributes 1, totaling 26 electrons. The Lewis structure shows three single C-F bonds and one single C-H bond, with no lone pairs on carbon. CHF3 adopts a tetrahedral geometry with bond angles of approximately 109.5°. The molecule is polar due to the high electronegativity of fluorine (3.98) compared to carbon (2.55) and hydrogen (2.20), influencing its physical properties like boiling point and solubility, and its use as a refrigerant.

CHF3 is known as fluroform. It is a similar structure to methane and is also known as trifluoromethane. Three H atoms are replaced in methane by fluorine atoms. As it is similar to methane so the shape and bond angle is also similar to methane which is tetrahedral shape and bond angle near about 109.5⁰. C-H and C-F bond lengths are different due to two substituents.

The hybridization of the CHF3 lewis structure is sp³. Due to the presence of different substituents and different electronegativity and asymmetric shapes, the molecule is polar. It can be soluble in organic non-polar solvents also. It is a greenhouse gas like chlorofluorocarbon.

Some important facts about CHF3

In the physical state, the CHF3 is a colorless gaseous molecule. As it is a gaseous species so it has some vapor pressure of about 4.38 MPa at 20 °C temperature. The melting point and boiling point of this molecule are 118 K and 191.1 K respectively. First, it was synthesized by the reaction of Iodoform and dry silver fluoride.

But in the laboratory, it is prepared by the reaction of Chloroform in the presence of Hydrogen fluoride.

CHCl₃ + 3HF = CHF₃ + 3HCl

Biologically, it can be produced by decarboxylation of trifluoroacetic acid.

In the organic reaction, it can act as a source of nucleophiles.

1.    How to draw the CHF3 lewis structure?

Lewis structure is a very important tool for every covalent molecule. With the help of lewis’s structure, it can easily predict the bonding electrons, the shape of the molecule, lone pairs, and valence electrons of the molecule.

Before proceeding with the CHF3 lewis structure there are a few rules we should be kept in our mind.

First of all, we should count the valence electrons for all the individual atoms in the CHF3 molecule and then added together. Now we have to select the central atom based on less electronegativity. Based on the size and less electronegativity C is the central atom here and one H and three F atoms are the surrounding atoms here.

Now we will connect all the atoms via a single bond. The valence electrons of C are four, H is one, and F has seven electrons. In the CHF3 lewis structure, the number of electrons involved will be  [4+1+ (3*7)] = 26 and from the octet rule the electrons needed [4*8 +1*2] = 34 electrons, and the required bonding electrons will be 34-26 = 8 electrons and the minimum bond required, 8/2 = 4 bonds.

So, in the CHF3 lewis structure, there will be a minimum of 4 bonds required and all the bonds are single. Attaching all the atoms with the central c atom via four bonds all the atoms completed their octet so no need to add multiple bonds here.

After that, the lone pairs are assigned to the respective atoms. F has seven electrons in its valence shell and the bond formation used only one electron so the remaining six electrons exit as lone pairs over F atoms.

2.    CHF3 lewis structure shape

CHF3 lewis structure shape can be predicted from the Valence Shell Pair Electrons Repulsion theory. According to this theory if the bonding electrons count for any molecule will be 8 then the shape of the molecule will be tetrahedral.

8 electrons count molecule will adopt generally square planner or tetrahedral geometry. But in the square planner moiety, the bond angle in between atoms will be 90⁰ and there is a high chance of steric crowding.

But in the tetrahedral geometry, the bond angle increases, and the free space among the molecule also increases so the chance of steric crowding of any kind of repulsion will be minimized.

In the CHF3 lewis structure, the central atom is here C and the surrounding atoms H and three F atoms are adjusted at the four vertices of the tetrahedral moiety and arranged with proper bond angle and spacing.

3.    CHF3 valence electrons

In the CHF3 lewis structure, the valence electrons are considered for C, H, and F atoms which are present at their outermost or valence orbitals. Maybe they are involved in the bond formation or maybe exist as lone pairs.

The electronic configuration of H, C and F are 1s¹, [He]2s²2p², [He]2s²2p² respectively. So, we can say that there is one electron from H which is also a valence electron, C has four electrons in its valence shell and F has seven electrons.

H and F involved one electron to form a covalent bond with C, and the rest of the six electrons of F exist as lone pairs and all the four valence electrons of C are involved with one H and three F to form the CHF3 lewis structure.

So, the total valence electrons in this molecule are the summation of three atoms valence electrons and the number of valence electrons will be, 1+4+(7*3) = 26 electrons.

4.      CHF3 lewis structure octet rule

In the CHF3 lewis structure, all the individual atoms will follow the octet rule to complete their valence shell and gain the nearest noble gas configuration by accepting a suitable number of electrons.

From the electronic configuration of every atom, we see that H has one electron in its valence shell and it needs one more to gain the same configuration as He. So, one electron of H and one electron of C share in a bond and complete the octet of H.

F has seven electrons in its outermost orbital and among them, six exist as lone pairs, and one electron shares with one electron of C in a covalent bond and complete the octet of F by gaining eight electrons in its valence orbital.

C has four electrons in its valence shell and its hare has four electrons with three F atoms and one H atom and also gains eight electrons in its valence orbital to complete the octet.

According to octet, S orbital contains a maximum of two electrons like H atoms and p orbitals contain six electrons like C and F.

5.    CHF3 lewis structure formal charge

The formal charge is a hypothetical concept like resonance and by this concept, we can predict the charge over a particular atom in a CHF3 molecule by their bonding electrons.

The formula we can use to calculate the formal charge, F.C. = N_v – N_l.p. -1/2 N_b.p.

Where N_v is the number of electrons in the valence shell or outermost orbital, N_l.p is the number of electrons in the lone pair, and N_b.p  is the total number of electrons that are involved in the bond formation only.

In the CHF3 lewis structure, C and H are different substituents so we have to calculate the formal charge of C, H, and F individually.

The formal charge over the C atom is, 4-0-(8/2) = 0

The formal charge over the H atom is, 1-0-(2/2) = 0

The formal charge over the F atom is, 7-6-(2/2) = 0

So, the formal charge over the CHF3 lewis structure is zero as no individual charge contains any formal charge.

6.    CHF3 lewis structure lone pairs

Lone pairs are those electrons that are present as valence shells but do not participate in the bond formation they are valence electrons also. In the CHF3 lewis structure, only F has lone pairs, and H and C lack lone pairs.

From the electronic configuration, we can say that F has six electrons in its valence shell and according to the octet rule, it shares one electron with C to complete its octet via the formation of one single covalent bond. The remaining six electrons are present as three pairs of lone pairs.

For H and C after bond formation, they have no electrons in their valence shell, so they lack lone pairs.

So, the total lone pairs in the CHF3 lewis structure will be, 3*3 = 9 pairs of lone pairs.

7.    CHF3 lewis structure bond angle

The bond angle will be 109.5⁰ which will be for ABX₃ or AX₄ molecules like CHF3. It adopts a tetrahedral structure so the bond angel is perfect for that geometry.

The CHF3 lewis structure adopts tetrahedral geometry according to the VSEPR theory. According to this theory, the bond angle of the molecule will be 109.5⁰. The size of F and H is very small so there is no chance for lone pairs- bond pair repulsion and for this reason, there is no deviation of the actual bond angle.

But due to electronegativity F try to pull the electron density towards it and for this reason, the F-C-F bond angle is about 108⁰ but the F-C-H bond angle remains 109.5⁰.

8.    CHF3 lewis structure resonance

There is no resonance structure observed for the CHF3 lewis structure. Resonance is the concept by which in a molecule the delocalization of electron occurs in its different skeleton structure.

For the CHF3 lewis structure, there is a different skeleton structure is not possible, F is most electro-negative so it does not release the electron density from it and H is lack electron density. So, there is no possibility to form the resonating structure for the CHF3 lewis structure.

9.    CHF3 hybridization

Hybridization is also a hypothetical concept by which the mixing of different orbitals of different energy to form a new hybrid orbital of equivalent energy. For the CHF3 lewis structure, the orbitals of C, H, and F get mixed to form an sp3 hybrid orbital.

We calculate the CHF3 hybridization by using the following formula,

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

For the CHF3 lewis structure, C has 4 valence electrons which are involved in the bond formation, and one H and three F atoms are present.

So, the central C in the CHF3 lewis structure is, ½(4+4+0+0) = 4 (sp³) hybridized.

According to VSEPR theory we can say that from the above table, if the central atom hybridization value is 4 then it is sp³ hybridized.

In the box diagram, it is shown that one s orbital and three p orbitals or C undergo missing to form an sp³ hybrid orbital. Only sigma bonds are allowed in the hybridization.

10.    CHF3 solubility

CHF3 is an organic molecule so it is expected to be soluble in organic solvents like benzene, toluene, ethanol, etc. But it has a solubility in water.

Although CHF3 is an organic molecule it is a polar molecule and water is a polar solvent so it gets dissolved in a water molecule (like dissolve like).

11.    Is CHF3 ionic?

All the covalent molecule has some % of ionic character according to Fajan’s rule. So, it is expected that the CHF3 lewis structure also has an ionic character.

F is the most electronegative atom and in the ionization form of CHF3 lewis structure, it can ionize Fluoride. Again, from the ionic potential of this molecule, we can say that the molecule can be polarizable so it has some ionic character.

12.    Is CHF3 acidic or basic?

CHF3 is lesser acidic. It has acidic proton in it.

Due to the presence of three electronegative atoms F they will drag the electron density towards itself and for this reason, the C_H bond becomes weaker and it can easily be cleaved and H released easily.

So, we can say that the CHF3 molecule donates proton or H atom and behaves as an acid but from the pka value, it is less acidic.

13.    Is CHF3 polar or nonpolar?

From the CHF3 lewis structure, we can say that the molecule is asymmetric due for this reason it is a polar molecule. Because it has a permanent dipole moment.

In the CHF3 lewis structure, the dipole moment acts from C to more electronegative F atoms. For the asymmetric structure, there is no chance to cancel out the dipole moment and the molecule has some resultant dipole moment and making it polar.

14.    Is CHF3 tetrahedral?

Yes, the CHF3 molecule is tetrahedral. The hybridization value and according to the VSEPR theory, also confirmed its structure.

15.    Is CHF3 linear?

No, the molecule is not linear. As discussed earlier it is tetrahedral geometry and it has a permanent dipole moment for its asymmetric structure.

Conclusion

From the whole discussion about the CHF3 lewis structure, we can conclude that the molecule is tetrahedral with sp3 hybridization. The molecule is acidic due to the presence of acidic proton and the molecule is also polar for its asymmetric structure.

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This article contains about the XeO4 lewis structure, Hybridization, bond angle, and other 13 important detailed facts.

The XeO4 lewis structure has tetrahedrally shaped having a bond angle of 109.5⁰. It is a very stable compound of a noble gas which is a very exceptional case.  Due to the tetrahedral geometry, the central Xe is sp³ hybridized. All the valence electrons of Xe are being used for the formation of sigma and π bonds, so there are no lone pairs available for Xe in this molecule.

Bartlett 1^st discovered the noble gas as a compound which was XeF. Due to the presence of electronegative substituents O, the positive charge density over Xe increases to such an extent that the energy of 5s and 5p decreases and they become comparable to the O.

Some important facts about XeO4

XeO4 is a yellow solid crystalline molecule that is stable at below temperature, at room temperature it decomposes. The melting point and boiling points are 237.1 K and 273 K respectively. The oxidation state of Xe in the Xeo4 lewis structure is +8 so it has its most stable oxidation state. 

XeO4 is formed by the reaction of concentrated Sulphuric acid on sodium and barium perxenates.

4XeF₆ + 18Ba(OH)₂ =3Ba₂XeO₆ + Xe +12BaF₂ + 18H₂O

Ba₂XeO₆ + 2H₂SO₄ = 2BaSO₄ + XeO₄ + 2H₂O

How to draw lewis structure for XeO4 ?

Lewis structure is a very useful tool by the help of this structure we can find out the valence electrons, shape, and lone pairs of any covalent molecule.  So, it’s important to draw the XeO4 lewis structure. There are some techniques we should keep in mind to draw the lewis structure of XeO4.

So, at first, we count the total valence electrons for Xe and O atoms. Then we identify the central atom by its electronegativity, we know Xe is less electronegative than O, so in the XeO4 lewis structure, Xe is the central atom. The molecule bears no extra charge upon it so no need to add extra electrons or subtract electrons here. Now Xe and four O atoms are attached by a single bond as well as a double bond to complete the octet. The lone pairs exist only over O atoms.

XeO4 lewis structure shape

The valence electrons for Xe in the sigma bond formation will be four and there are four O atoms each contributing one electron, so the total electrons count will be, 4+(1*4) =8. According to the VSEPR (Valence Shell Electrons Pair Repulsion) theory of a covalent molecule if the total bonding electrons count will be 8 then the shape of the molecule will be tetrahedral.

The whole electron density is lie over the Xe in the XeO4 lewis structure as Xe is the central atom here. All the four O atoms are present at the four corners of a tetrahedral geometry. The Bond angle made by central Xe and four O atoms in the tetrahedral moiety is 109.5⁰.

XeO4 lewis structure lone pairs

In the XeO4 lewis structure, Xe forms eight bonds with four O atoms. Out of eight bonds, four bonds are sigma bonds and four bonds are π bonds. So, there are no available of valence electrons for Xe which can exist as lone pair.

From the XeO4 lewis structure, we can see that the lone pairs are assigned only over O atoms. O is VIA or group 16^th  element and from the electronic configuration we can say that there are only six electrons are present at the valence shell of O and those electrons are involved in the bond formation with the central Xe atom. O used only two valence electrons for one sigma and one π bond with Xe. So, it has four electrons remaining in its valence shell which exist as lone pairs. So, the total number of lone pairs in the XeO4 lewis structure is (4*2)= 8 pairs which are only from the O site.

XeO4 lewis structure formal charges

By assuming the same electronegativity of all atoms in a molecule we can calculate the particular charge present over a specific atom or molecule is called a formal charge. So here in the XeO4 lewis structure, we consider the same electronegativity for Xe and O.

The formula we can use to calculate the formal charge of XeO4, F.C. = N_v – N_l.p. -1/2 N_b.p.

Where N_v is the number of electrons in the valence shell or outermost orbital, N_l.p is the number of electrons in the lone pair, and N_b.p  is the total number of electrons that are involved in the bond formation only.

We have to calculate separately the formal charge for Xe as well as O.

The formal charge over Xe, 8-0-(16/2) = 0

The formal charge over O, 6-4-(4/2) = 0

So, we can say that there is no formal charge over Xe as well as O cause the molecule is neutral. So, by calculating the formal charge we can also say whether the molecule is charged or not.

XeO4 lewis structure resonance

Resonance is a hypothetical concept, by which an electron cloud of any molecule can delocalize between different skeleton forms of that molecule In the Xeo4 lewis structure, the electron clouds delocalize between O and Xe atoms in different canonical forms.

From the XeO4 lewis structure, all five are the different resonating structures of XeO4. Among them, structure V is the most contributing structure as it contains a higher number of covalent bonds so its contribution is the highest. After that structure IV then III, II, and the least contributing is Structure I.

XeO4 lewis structure octet rule

In the XeO4 lewis structure, Xe and O both try to complete their octet by donating or accepting a suitable number of electrons from their valence shell or to the valence shell and gaining the nearest noble gas configuration.

In the XeO4 lewis structure, Xe is a group 18 element so it has a filled valence shell and no need to complete its octet. But O is a group of 16 elements, so it has six electrons in its outermost electrons and its octet is not completed. So, O form a double bond with Xe by sharing two of its electrons and two of Xe electrons and four electrons are present in its lone pairs. This way Oxygen completes its octet.

Xe is itself a noble gas and it participates in bond formation with O involving all the eight electrons in the valence shell.

XeO4 hybridization

In the XeO4 lewis structure, the molecular orbital energy of Xe and O are not the same, so Xe and O must undergo hybridization to form a hybrid orbital of equivalent energy and form a covalent bond.

We calculate the XeO4 hybridization by using the following formula,

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

For the XeO4 lewis structure, Xe has four electrons that are forming a sigma bond and four O atoms are surrounded.

So, the hybridization of central Xe in XeO4 is, ½(4+4+0+0)= 4 (sp³)

From the above table of hybridization, we can say that if the hybridization value of central atom is 4 then the central atoms is obviously sp³ hybridized involving one s and three p orbitals via mixing.

From the box diagram of the XeO4 lewis structure, it is evident that we only consider the sigma bond in hybridization, not the π bond or multiple bonds. In the covalent bond, we also consider the sigma bond.

Xe has eight electrons in its outermost orbital in the ground state. When it gets excited four electrons are transferred to the vacant 5d orbitals. Then Xe has four unpaired electrons in 5s and 5p orbital. These four unpaired electrons undergo hybridization with four O atoms and make a covalent bond.

Here One 5s orbital and 3 5p orbitals are involved in the hybridization. So, the hybridization is sp³. This sp³ hybridized orbital is of equivalent energy of Xe as well as O so that they can make bonds. The remaining four electrons of Xe in the 5d orbital are involved in π bond formation with O and they are not involved in hybridization.

From the hybridization value, we can predict the bond angle of this molecule. In the XeO4 lewis structure, the hybridization is sp3, so here the % of s character is 1/4th or 25%. Now from Bent’s rule bond angle of a molecule is, COSθ =s/s-1, where s is the % of s character in hybridization and θ is the bond angle.

Now using the formula, we get, COSθ = (¼)/(1/4)-1

Θ= 109⁰, so we can say that from the hybridization value we can evaluate the bond angle of a molecule or vice versa. Again, from VSEPR  theory the bond angle for a tetrahedral-shaped molecule will be 109.5⁰.

So VSEPR and hybridization theory can be correlated. The bond angle is perfectly 109.5⁰ which is ideal for tetrahedral molecules. Actually, in the XeO4 lewis structure, there is no deviation factor is present for bond angle. Xe has no lone pairs and the size of the Xe is very large compared to O. Though four O make the double bond with central Xe there is enough space in tetrahedral moiety to minimize the lone pair-bond pair repulsion. So, there is no deviation in the bond angle.

Is XeO4 polar?

we know that the polarity of any molecule depends on the value of the resultant dipole moment. To understand the polarity of the XeO4 lewis structure we have to find out its dipole moment value of it.

In the XeO4 lewis structure, the shape of the molecule is tetrahedral. The shape is symmetrical which means all the O atoms are present they are exactly neutralizing the dipole-moment value of each other. So, in the XeO4 lewis structure, the final resultant dipole moment value is zero, which makes the entire molecule nonpolar.

Being Xe is noble gas though it can form compounds like XeO4. Why?

From the values of Ionization energy, it can be said that the threshold of chemical reactivity is reached at Kr and it has been found that Xe can form quite a large number of compounds with highly electronegative substituents like O and F atoms.

This is due to the presence of electronegative substituents F and O the positive charge density over Xe increases to such an extent that the energy of 5s and 5p decreases and they become comparable to the O and F. Thus, the 5s and 5p orbital of Xe may overlap 2p of the F and O.

The bond length Xe-O is expected to be shorter. why?

The single Xe-O bond length is near about 160 pm. But in the XeO4 lewis structure, the molecule possesses a double bond character, so the bond length is decreased.

Xe is group 18^th element which is a noble gas and generally, the valence shell is fully occupied. From the electronic configuration, Xe has eight electrons in its valence shell which completed its outermost orbital, and all of the electrons are involved in bond formation with four O atoms (Sigma as well as π bonds) with O. O can form a stable double bond with suitable substituents like Xe and for this reason, there are no lone pairs or single bond character present between Xe-O bond.

Xe forms four sigma bonds as well as four π bonds with O atoms. Making the double bond makes the molecule more stable. The double bond is always shorter than the single bond and stronger than the single bond also.

Conclusion

From the above discussion of the XeO4 lewis structure, we can say that noble gas can also participate in reaction in the presence of strong electronegative substituents. The molecule is most stable due to the formation of a double bond so it cannot further participate in any other reaction. There is no lone pair-bond repulsion factor is present so the bond angle does not deviate and ideal for tetrahedral that is 109.5⁰.

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The common name of CH4 is methane. It is the simplest hydrocarbon in the organic molecule and it is a hydride of C. In the CH4 lewis structure, the molecule is a tetrahedral shape and has a bond angle of perfectly 109.5⁰.  The molecule undergoes is sp³ hybridization. One H atom is below the molecular plane and the other is above the molecular plane.

CH4 is used to synthesize higher-order hydrocarbon in organic reactions. It is a simple alkane because all the C-H bonds are single.

How to draw the CH4 Lewis structure?

Drawing the Lewis structure for methane (CH4) is pretty straightforward, but let’s walk through the process step-by-step. Methane is a simple molecule, consisting of one carbon atom bonded to four hydrogen atoms. Here’s how you can draw its Lewis structure:

Count the Total Number of Valence Electrons: In methane, the central carbon atom has 4 valence electrons, and each hydrogen atom has 1 valence electron. Since there are 4 hydrogen atoms, that’s 4 valence electrons from hydrogen, plus the 4 from carbon, giving us a total of 8 valence electrons to work with.

Determine the Central Atom: Carbon is less electronegative than hydrogen, and it can form more bonds, so carbon will be the central atom in the structure.

Sketch a Skeleton of the Molecule: Place carbon in the center and arrange the four hydrogen atoms around it. It’s like picturing a plus sign, with carbon at the intersection and hydrogen atoms at the ends of each line.

Distribute the Valence Electrons: Starting with the outer atoms, place electrons around them to represent the bonds between the carbon and hydrogen atoms. Each bond between carbon and hydrogen will use 2 of the 8 valence electrons. Since we have 4 C-H bonds in methane, all 8 electrons are used up in forming these bonds.

Check the Octet Rule: Every atom in methane follows the rules they love to live by. Carbon gets its full octet because it shares 4 electrons with hydrogen (one from each bond), and each hydrogen is happy with 2 electrons (a full outer shell for hydrogen).

Add Lone Pairs if Necessary: In the case of methane, there are no lone pairs because we used all the valence electrons in forming bonds, and every atom has its required full outer shell.

So, final CH4 Lewis Structure is:

That’s it! You’ve got the Lewis structure for methane. Visually, you’d see the carbon in the center with single lines (representing single bonds) stretching out to the hydrogens at the four compass points. Methane’s structure is a perfect example of a tetrahedral molecular geometry, but that’s diving a bit into molecular shapes.

CH4 lewis structure shape

According to the VSEPR (Valence Shell Electrons Pair Repulsion) theory if the electrons count of any molecule is 8 then the molecule adopts tetrahedral geometry. The electrons contribution for C is 4 and four H atoms contribute 1 electron each, so the total electron count will be 8. So, the CH4 lewis structure is tetrahedral.

In the CH4 lewis structure, the whole electron density lies over the central C atoms only. The C is surrounded by four H atoms in the tetrahedral moiety. The shape of the molecule is ideal and no deviation in the shape and geometry because there is no lone pair present and no destabilization factor is present too.

CH4 valence electrons

The electrons present at the valence or outermost shell of an atom are known as valence electrons. For C the number of valence electrons is 4 and for H the number of valence electrons is 1.

In the CH4 lewis structure, the C atom is a Group 14^th element, having electronic configuration [He]2s²2p² so, it has four electrons in its outermost orbital and all the electrons are involved in the sigma bond formation with four H atoms. For H atom we all know only one electron is present and that is its valence electron and it is involved in the bond formation with C.

So, in the CH4 lewis structure, the total number of valence electrons is 4+(4*1) = 8 electrons and it is shown that the number octet is fully satisfied by this molecule.

CH4 lewis structure formal charge

Accounting for the same electronegativity for all the atoms in a particular molecule calculates the specific charge over the molecule or individual atoms is called the formal charge. The formal charge is a hypothetical concept, by this concept, we can predict whether the molecule is charged or not.

The formula we can use to calculate the formal charge, F.C. = N_v – N_l.p. -1/2 N_b.p.

Where N_v is the number of electrons in the valence shell or outermost orbital, N_l.p is the number of electrons in the lone pair, and N_b.p  is the total number of electrons that are involved in the bond formation only.

In the CH4 lewis structure, C and H are different substituents so we calculate the formal charge of C and H individually.

The formal charge over C is, 4-0-(8/2) = 0

The formal charge over H is, 1-0-(2/2) = 0

So, the formal charge over C as well as H is zero. It is also reflected that in the CH4 lewis structure that the molecule is also neutral.

So, the individual formal charge also gives the proper explanation of a charged or neutral molecule.

CH4 lewis structure lone pairs

The electrons are present at the valence shell or outermost orbital of an atom but are not involved in direct bond formation but exist as pairs are called lone pairs. From the CH4 lewis structure, we can say there are no lone pairs over the molecule.

In the CH4 lewis structure, there are two substituents present, C and H. H has only one electron in its shell and that electron is also the valence electron for it. That one electron of H is involved in the sigma bond formation with the central c atom, so there is no lone pair for H atom.

C is group 14^th element and it has four electrons in its outermost orbital all of the electrons are involved in the sigma bond formation with four H atoms. So, there are no electrons present for C in its outermost orbital. So, C also lacks lone pairs and the whole CH4 lewis structure does not contain any lone pairs.

CH4 lewis structure octet rule

Every atom except noble gas tries to complete its valence shell but accepts a suitable number of an electron from another source and tries to gain the nearest noble gas configuration according to the o octet rule. CH4 lewis structure also tries to complete its octet by bond formation between C and H.

In the CH4 lewis structure, the electronic configuration of C is [He]2s²2p². So, there are four electrons in the outermost shell for C and it needs four more electrons to complete its octet. Now in CH4 molecule C form four sigma bonds with four H atoms via sharing electrons and completing its octet.

Again, for H there is only one electron, and that one electron is the valence electron which is present at the valence shell for H. H needs one more electron to complete its octet and gain the nearest noble gas configuration like He. Now H forms a bond with C via sharing its one electron and one electron from C and completing its octet too.

CH4 lewis structure bond angle

A bond angle is a specific angle made by the atoms in a particular molecule for arranging them in a particular manner. In the CH4 lewis structure, the bond angle is 109.50, which is ideal for tetrahedral geometry.

From the CH4 lewis structure, we know that the methane molecule adopts tetrahedral geometry and from VSEPR theory we know that the bond angle for tetrahedral geometry is 109.50. In this structure, there is no deviation from the ideal bond angle and the reason behind this is that there is no deviation factor present. The size of C, as well as H, are very small so there is no repulsion between them and there are no lone pairs over the molecule. So, no chance of lone pair-bond pair repulsion.

So, the H-C-H is perfectly 109.5⁰ in the ideal tetrahedral moiety.

CH4 lewis structure resonance

Delocalization of electronic clouds in between different skeletons of a particular molecule is called resonance. But in the CH4 lewis structure, there is no resonance occurs.

Resonance occurs among the atoms which lie at the same plane only. But in the CH4 lewis structure, two of the H atoms are present at the molecular plane but another two lie below and above the molecular plane. So, resonance cannot occur there. Again, for resonance, there is a need an extra electronic cloud that can be delocalized but C and H both are electropositive and lack of electronic cloud.

So, in the CH4 lewis structure resonance cannot be occurred. So, there are no resonating structures are observed for the CH4 lewis structure.

CH4 hybridization

Hybridization is a theoretical concept by which two or more orbitals having different energy undergo mixing to produce a hybrid orbital of equivalent energy and form a covalent bond. CH4 lewis structure is a covalent molecule so it also shows hybridization and the central C atom is sp3 hybridized.

We calculate the CH4 hybridization by using the following formula,

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

For the CH4 lewis structure, c has 4 valence electrons which are involved in the bond formation, and four H atoms are present.

So, the central C in the CH4 lewis structure is, ½(4+4+0+0) = 4 (sp³) hybridized.

                  From the above table of hybridization, we can conclude that if the hybridization value is 4 then the central atoms is sp³ hybridized.

From the box diagram of the CH4 lewis structure, we can say that in the ground state c is unable to form a bond because there are two electrons paired in the 2s orbital. In the excited state, C formed a bond with four H atoms involving its one s and three p orbitals. So, the mode of hybridization is sp³.

In the hybridization, we only consider the sigma bond, not the double or multiple bonds.

CH4 solubility

From the CH4 lewis structure, we also can predict the solubility of this molecule. The methane molecule is nonpolar so it is mostly dissolved in a nonpolar solvent or organic solvent. But due to H bonding, it is also soluble in polar solvents like water.

From the dipole moment calculation, we see that the molecule is nonpolar so it is expected that it is soluble in benzene, an ethanol-like organic solvent. But in methane molecules there are four H atoms are present and they can easily form H bonding with the lone pair of the water molecule and the molecule gets soluble in water also.

Is CH4 ionic?

According to Fajan’s rule, we can say every covalent molecule shows some % of ionic character.

In the CH4 lewis structure, the size of the C atom is small but the charge density is also less so the ionic potential is very low, so it cannot polarize H properly but the size of the hydride ion is very large. So is a view of ionic potential has some ionic character too.

Is CH4 acidic or basic?

The polarity of a molecule is depend on the value of the resultant dipole moment. For CH4 lewis structure, it is nonpolar due to zero dipole moment.

In the CH4 lewis structure, we can see that all the C-H bonds are equal and they have the same electronegativity difference the structure is symmetrical so four dipole moments cancel out each other and the net result is zero dipole moment for the CH4 molecule and makes the molecule non-polar.

Is CH4 tetrahedral?

Yes, CH4 is a tetrahedral molecule. From VSEPR the total electron count for the methane molecule is 8 and this is the reason the shape of the molecule is tetrahedral.

From the CH4 lewis structure and hybridization, we see that the molecule adopts tetrahedral geometry. The molecule is sp³ hybridized and this is also reflected in the geometry of the molecule tetrahedral.

Some detailed facts about CH4

CH4 is a colorless, odorless, and very lighter gaseous molecule. Every hydrocarbon on combustion produced carbon dioxide, so on combustion of methane also produced carbon dioxide and water vapor. The melting point and boiling point of methane molecule are 90 K and 116 K respectively.

The molecule is synthesized in the presence of Ni catalyst, Hydrogen gas, and carbon monoxide.

CO + 3H₂ = CH₄ + H₂O

Methane is used as fuel in different automobile systems and refined methane is also used as rocket fuel. It readily participates in many radical reactions and forms methyl radical which is a more reactive species.

Conclusion

From the above discussion of CH4 lewis structure, we can say that this molecule is a perfectly tetrahedral molecule and the bond angle is 109.50 and there is no deviation factors present due to C and H both being small in size. Although methane is nonpolar but soluble in water and the methanium ion behaves as a super acid.

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In this article, we should discuss the SO2Cl2 lewis structure, shape of the molecule, bond angle, and many detailed facts.

SO2Cl2 is known as sulfuryl chloride. The molecule is tetrahedral in shape and has a different bond angle in it. Two Oxygen atoms are attached to central S by a double bond and two Cl are attached via a single bond only. Due to the different environments of bond order, the bond angle is different in this molecule.

The S-O bond length is shorter than S-Cl because of oxygen attached via a double bond and we know a double bond is stronger but shorter than a single bond. The oxidation state of central S in this molecule is +6.

Some important facts about SO2Cl2

SO2Cl2 is a colorless liquid in its physical state at room temperature and the odor of the molecule is pungent. In nature, it cannot exist in its state because the molecule shows rapid hydrolysis. The molar mass of the molecule is 136.96 g/mol. The boiling point and melting point of sulfuryl chloride are 342.5 K and 219.1 K respectively. As it is liquid in its physical state, its refractive index is 1.4437.

Sulfuryl Chloride is synthesized in the laboratory by the reaction of sulfur dioxide and Chlorine in presence of activated charcoal as a catalyst.

SO₂ + Cl₂ = SO₂Cl₂

How to draw the lewis structure for SO2Cl2? 

With the help of lewis structure, we can predict the molecular shape, the number of electrons involved in bond formation, and the number of lone pairs available of SO2Cl2.

Before drawing the SO2Cl2 lewis structure we should keep in mind some important points. At first, we count the total number of valence electrons of S, O, and Cl atoms. Then we have to identify the central atom on the basis of electronegativity. Among S, O, and Cl less electronegative atom is S, so S is the central atom is here.

In the SO2Cl2 lewis structure, the total number of electrons involved in the bond formation is, 6+(2*6)+(2*7)=32 and the electrons required according to the lewis dot formula is (5*8)= 40 electrons, so the bonding electrons will be (40-32)= 8 electrons and the minimum number of bonds required (8/2)= 4 bonds.

Now we should assign the lone pairs, S has six electrons in its valence shell and 4 electrons are involved in the four sigma bonds and two electrons are involved in two π bonds with two O. So, no lone pairs are available on the S.

SO2Cl2 lewis structure shape

The valence electrons for S involved in sigma bond formation is 4 and the surrounding atoms are two O and two Cl contribute 1 electron each is 4 electrons. So, the total electrons involved in the sigma bond formation is 4+(1*4)=8 electrons.

According to VSEPR (Valence Shell Electrons Repulsion) theory if the electrons count in bond formation for any molecule is 8 then it should adopt tetrahedral geometry.

In the SO2Cl2 lewis structure, the whole electron density lies around the central S atom, and two Cl and two O are present at four sites of the tetrahedral moiety. The ideal bond angle should be 109.5⁰ for tetrahedral but here the scenario is different.

Here both O form a double bond with S so it required more space and due to the larger size of Cl, there is massive lone pair-bond pair repulsion occurs. To minimize this kind of repulsion the molecule adopts different bond angles to arrange every atom.

SO2Cl2 lewis structure formal charges

From the SO2Cl2 lewis structure, we calculate the formal charge assuming the same electronegativity for S, O, and Cl.

The formula we can use to calculate the formal charge, F.C. = N_v – N_l.p. -1/2 N_b.p.

We calculate the formal charge separately for S, O, and Cl because they are different molecules and experience different environments.

The Formal charge over S is, 6-0-(12/2) = 0

The Formal charge over O is, 6-4-(4/2) = 0

The formal charge over Cl is, 7-6-(2/2) = 0

So, we can see that there is no formal charge over any atom in the SO2Cl2 lewis structure. It is also proved that the molecule is neutral in nature so no formal charge over it.

SO2Cl2 lewis structure lone pairs

In the SO2Cl2 lewis structure, only O and Cl contain lone pair over it. S does not have any lone pair because all the valence electrons of S are involved in sigma as well as π bonds.

S is a group VIA element, so it has six electrons in its valence shell. Among six electrons four electrons are involved in the sigma bond formation with two Cl and two o atoms. The rest of the two electrons are also involved in the π bond formation with two O atoms. So, no free electrons are present in the valence shell of S, so S does not have any lone pair.

O is also a group VIA element and it has also six electrons in its valence shell one electron is involved in sigma bond formation with S and another one is an π bond with S. So, the remaining 4 electrons are present as two pairs of lone pairs over O atom.

Cl is a group VIIA element and it has one more electron in the valence shell than O or S which means seven electrons in its outermost orbital. Only one electron is involved in bond formation with S and the rest of the six electrons exist as 3 pairs of lone pairs.

So, the total number of lone pairs available in the SO2Cl2 is (2*2)+(3*2)=10 pairs of lone pairs.

SO2Cl2 Octet rule

According to the octet rule S, O and Cl all are try to complete their valence shell by either donating or accepting the suitable number of electrons in SO2Cl2 lewis structure.

In the SO2Cl2 lewis, structure S make a total of six bond, four sigma bonds, and two π bonds with O and Cl. So, S invests its six electrons to form six bonds and it has nothing in its valence shell. S is a group VIA element and it has six electrons in its valence shell when it forms a bond with two O and two Cl by sharing four electrons then it can complete its octet.

Now for Cl, it has seven electrons in its valence shell and it shares one electron with S to complete its octet.

For O, it has six electrons in its valence shell like S and it forms two bonds with S one is sigma and the other is a π bond by sharing two electrons with S, and this way it also completed its octet and gains the nearest noble gas configuration in SO2Cl2 lewis structure.

SO2Cl2 lewis structure resonance

In the SO2Cl2 lewis structure, the electrons clouds delocalized only between O and S atoms in the different canonical forms via resonance.

In the SO2Cl2 lewis structure, all of the above are different resonating structures. Among them, Structure III is the most contributing because it has a higher number of covalent bonds. After that Structure II and then least contributing is Structure I as it contains a lower number of covalent bonds and the positive charge is present in the S atom.

SO2Cl2 hybridization

In the SO2Cl2 lewis structure S, O, and Cl undergo hybridization via mixing their orbitals of different energy to form a new equivalent hybrid orbital to form a stable covalent molecule.

We calculate the CCl4 hybridization by using the following formula,

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

For central atom S in SO2Cl2 lewis structure, S has six valence electrons but four electrons are involved in the sigma bond and surrounding atoms are two Cl and two O atoms.

So, the hybridization of central S is, ½(4+4+0+0) = 4(sp³)

From the above table of hybridization, we can conclude that if the hybridization value is 4 then the central atoms is sp³ hybridized.

Form the box diagram we can say that we only consider the sigma bond in hybridization not the π bond.

Here One s and three p orbitals of S are involved in the sp³ hybridization.

Is SO2Cl2 polar or nonpolar?

In the SO2Cl2 lewis structure, all the molecule is not opposite to each other so it has a resultant dipole moment and the molecule is polar.

In the SO2Cl2 lewis structure, the dipole moment acts from S to O and S to Cl atoms as Cl and O both are more electronegative than S.

In the tetrahedral moiety, the shape is not symmetric so each molecule’s position is not opposite to each other and each has a specific dipole moment as a result the molecule has a specific value of dipole moment and makes the molecule polar.

From the above discussion of SO2Cl2 lewis structure, we can say that the molecule is polar having a resultant dipole moment. The double bond requires more space than a single bond otherwise the molecule suffers massive bond pair lone pair repulsion.

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The Lewis structure of CCl4, also known as carbon tetrachloride, is a representation of how the atoms are arranged in the molecule. It is a commonly used solvent and was historically used as a fire extinguisher. In the Lewis structure, carbon is the central atom surrounded by four chlorine atoms. Each chlorine atom shares one electron with carbon, resulting in a total of eight valence electrons around the carbon atom. This arrangement allows carbon to have a full octet of electrons, making it stable. The Lewis structure of CCl4 is important in understanding its chemical properties and reactions.

Key Takeaways

Understanding the Lewis Structure

In chemistry, the Lewis structure is a way to represent the molecular structure of a chemical compound using Lewis dot symbols. It provides a visual representation of the arrangement of atoms and valence electrons in a molecule, helping us understand its molecular geometry and chemical bonding.

What is a Lewis Structure?

A Lewis structure, also known as a Lewis dot structure, is a diagram that shows the valence electrons of atoms in a molecule. Valence electrons are the outermost electrons of an atom that participate in chemical bonding. By representing these electrons as dots around the atomic symbol, we can determine the number of covalent bonds an atom can form.

Lewis Structure of CCl4

Let’s take the example of carbon tetrachloride (CCl4) to understand the concept of Lewis structures. Carbon tetrachloride is a chemical compound composed of one carbon atom and four chlorine atoms. To draw its Lewis structure, we need to consider the valence electrons of each atom.

Carbon is located in group 14 of the periodic table, so it has four valence electrons. Chlorine, on the other hand, is in group 17 and has seven valence electrons. Therefore, the total number of valence electrons in CCl4 is:

Valence electrons of carbon (4) + Valence electrons of chlorine (4 × 7) = 32

Steps to Draw the CCl4 Lewis Structure

To draw the Lewis structure of CCl4, we follow these steps:

1. Determine the total number of valence electrons in the molecule.
2. Identify the central atom, which is usually the least electronegative atom. In this case, carbon is the central atom.
3. Connect the central atom to the surrounding atoms using single bonds.
4. Distribute the remaining valence electrons around the atoms to satisfy the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.
5. If there are still remaining valence electrons, place them on the central atom as lone pairs until it satisfies the octet rule.
6. Check if all atoms have achieved an octet, and adjust the placement of electrons if necessary.

Lewis Dot Structure of CCl4

Following the steps mentioned above, the Lewis dot structure of CCl4 can be represented as:

Cl
|
Cl-C-Cl
|
Cl

In this structure, the carbon atom is in the center, bonded to four chlorine atoms. Each chlorine atom is connected to the carbon atom by a single bond, and the remaining valence electrons are placed as lone pairs on the chlorine atoms.

The Lewis dot structure of CCl4 reveals that it has a tetrahedral structure, with the carbon atom at the center and the chlorine atoms positioned at the four corners of a tetrahedron. This arrangement gives the molecule a symmetrical shape.

It’s important to note that CCl4 is a nonpolar molecule due to the symmetrical distribution of the chlorine atoms around the central carbon atom. The electronegativity difference between carbon and chlorine is negligible, resulting in a balanced distribution of charge.

Understanding Lewis structures and molecular models is crucial in chemistry education as it helps us visualize and comprehend the structural properties of various chemical compounds. By analyzing the Lewis dot structure, we can gain insights into the valency of carbon, the bonding between carbon and chlorine atoms, and the overall molecular structure of CCl4.

Properties of CCl4

Polar or Nonpolar

Carbon tetrachloride (CCl4) is a chemical compound that consists of one carbon atom bonded to four chlorine atoms. When determining the polarity of a molecule, we consider the molecular geometry and the electronegativity difference between the atoms. In the case of CCl4, the molecule is nonpolar.

Nonpolar Nature of CCl4

The nonpolar nature of CCl4 can be attributed to its symmetrical tetrahedral structure. Each chlorine atom is positioned at the corners of the tetrahedron, with the carbon atom at the center. The bond dipoles cancel each other out due to the symmetry, resulting in a nonpolar molecule.

Resonance in CCl4

Resonance is a phenomenon that occurs when multiple Lewis dot structures can be drawn for a molecule. However, in the case of CCl4, resonance does not occur. The molecule has a single, well-defined structure with no alternative resonance structures.

Bond Angle in CCl4

The bond angle in CCl4 is approximately 109.5 degrees. This angle is a result of the tetrahedral arrangement of the chlorine atoms around the central carbon atom. The bond angles in a tetrahedral structure are all equal due to the symmetry of the molecule.

Lone Pairs in CCl4

In the Lewis dot structure of CCl4, there are no lone pairs of electrons on the central carbon atom. All four valence electrons of carbon are involved in forming covalent bonds with the chlorine atoms. Therefore, there are no lone pairs present in the CCl4 molecule.

Formal Charge in CCl4

The formal charge of an atom in a molecule is a measure of the distribution of electrons. In the case of CCl4, each chlorine atom has a formal charge of zero, and the carbon atom also has a formal charge of zero. This indicates that the electrons are evenly distributed among the atoms in the molecule.

Low Melting Point of CCl4

CCl4 has a relatively low melting point compared to other compounds. This can be attributed to the weak intermolecular forces between the CCl4 molecules. The molecules are held together by London dispersion forces, which are relatively weak compared to other types of intermolecular forces.

Molecular Geometry and Shape

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, while molecular shape describes the overall shape of the molecule. Understanding the molecular geometry and shape is crucial in chemistry as it helps us predict the physical and chemical properties of compounds.

VSEPR Model for CCl4

The VSEPR (Valence Shell Electron Pair Repulsion) model is a useful tool for predicting the molecular geometry of a compound. It is based on the idea that electron pairs in the valence shell of an atom repel each other, causing them to arrange themselves in a way that minimizes repulsion.

Let’s take the example of carbon tetrachloride (CCl4) to understand the VSEPR model. Carbon tetrachloride is a chemical compound composed of one carbon atom and four chlorine atoms. To determine its molecular geometry, we need to consider the Lewis dot structure, valence electrons, and covalent bonds.

In the Lewis dot structure of CCl4, carbon is surrounded by four chlorine atoms, each sharing a single covalent bond. Carbon has four valence electrons, while each chlorine atom contributes one valence electron, resulting in a total of eight valence electrons. According to the octet rule, atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.

Molecular Shape of CCl4

Based on the VSEPR model, the molecular shape of CCl4 is tetrahedral. In a tetrahedral structure, the central carbon atom is located at the center, with the four chlorine atoms positioned at the four corners of a tetrahedron. The bond angles between the carbon-chlorine bonds are approximately 109.5 degrees, resulting in a symmetrical and balanced shape.

To visualize the molecular structure of CCl4, we can use molecular models or a structural formula. Molecular models provide a three-dimensional representation of the molecule, allowing us to observe its shape and arrangement of atoms. The structural formula, on the other hand, uses lines to represent bonds and shows the connectivity between atoms.

Why CCl4 is Tetrahedral

The tetrahedral structure of CCl4 can be explained by the VSEPR theory. In the VSEPR model, the electron pairs around the central atom repel each other and try to maximize their distance from one another. This repulsion leads to the arrangement of the four chlorine atoms in a tetrahedral shape around the central carbon atom.

Additionally, the valency of carbon and the chlorine atoms in CCl4 also contribute to its tetrahedral shape. Carbon has a valency of four, meaning it can form four covalent bonds. Each chlorine atom contributes one electron to form a covalent bond with carbon, resulting in the formation of four carbon-chlorine bonds.

It is important to note that CCl4 is a nonpolar molecule despite its tetrahedral shape. This is because the four chlorine atoms are symmetrically arranged around the central carbon atom, resulting in a cancellation of dipole moments. Therefore, the overall molecular polarity of CCl4 is zero.

CCl4 as a Lewis Acid or Base

Is CCl4 a Lewis Acid or Base?

When it comes to discussing the Lewis acidity or basicity of carbon tetrachloride (CCl4), it is important to understand its molecular structure and electron configuration. CCl4 is a chemical compound composed of one carbon atom and four chlorine atoms, arranged in a tetrahedral structure. The Lewis dot structure of CCl4 shows that the carbon atom shares its four valence electrons with the four chlorine atoms through covalent bonds.

In terms of Lewis acid-base theory, a Lewis acid is a substance that can accept an electron pair, while a Lewis base is a substance that can donate an electron pair. Based on this definition, CCl4 does not exhibit the characteristics of a Lewis acid or base. This is because the carbon atom in CCl4 has a complete octet of electrons, satisfying the octet rule. It does not have any unshared electron pairs to accept or donate.

To further understand why CCl4 is not a Lewis acid, we can examine its molecular geometry and electron pair distribution. The tetrahedral structure of the CCl4 molecule ensures that the electron pairs are evenly distributed around the central carbon atom. Each chlorine atom is positioned at one of the four corners of the tetrahedron, resulting in a symmetrical arrangement. This symmetrical distribution of electron pairs cancels out any potential polarity of CCl4, making it a nonpolar molecule.

Why CCl4 is not a Lewis Acid

The electron configuration of the carbon atom in CCl4 is 1s2 2s2 2p2, with two electrons in the 2s orbital and two electrons in the 2p orbital. The valency of carbon is four, meaning it can form four covalent bonds. In the case of CCl4, each chlorine atom shares one electron with the carbon atom, resulting in four covalent bonds. This completes the octet of electrons around the carbon atom, satisfying the stability requirements of the octet rule.

Applications and Importance of CCl4

Carbon tetrachloride (CCl4) is a versatile chemical compound with various applications in different fields. Its unique properties make it valuable in several scientific and industrial processes. Let’s explore some of the important applications of CCl4.

Use of CCl4 in NMR (Nuclear Magnetic Resonance)

One significant application of CCl4 is in Nuclear Magnetic Resonance (NMR) spectroscopy. NMR is a powerful analytical technique used to study the structure and properties of molecules. CCl4 is often used as a solvent in NMR experiments due to its non-reactive nature and its ability to dissolve a wide range of organic compounds. Its low boiling point and high boiling point make it suitable for NMR studies at different temperatures.

In NMR, the Lewis dot structure and molecular geometry of CCl4 play a crucial role. The CCl4 molecule consists of one carbon atom bonded to four chlorine atoms, forming a tetrahedral structure. This arrangement allows for the efficient measurement of nuclear spin interactions and provides valuable information about the chemical bonding and molecular structure of the compounds being studied.

Other Applications of CCl4

Apart from its use in NMR, CCl4 finds applications in various other fields:

1. Cleaning and Degreasing: CCl4 is an effective solvent for removing grease, oil, and dirt from surfaces. It is commonly used in industrial cleaning processes and as a degreasing agent for machinery and electronic components.

2. Fire Extinguisher: In the past, CCl4 was used as a fire extinguishing agent due to its ability to suppress flames by displacing oxygen. However, its use in fire extinguishers has significantly decreased due to environmental concerns.

3. Refrigerant: CCl4 was once used as a refrigerant in cooling systems. However, its use has been phased out due to its harmful effects on the ozone layer.

4. Chemical Synthesis: CCl4 is used as a reactant in various chemical synthesis processes. It is involved in the production of chlorofluorocarbons (CFCs), which were widely used as refrigerants and propellants before their environmental impact was discovered.

5. Solvent for Dyes and Perfumes: CCl4 is used as a solvent in the production of dyes and perfumes. Its ability to dissolve a wide range of organic compounds makes it suitable for extracting and purifying aromatic substances.

Frequently Asked Questions

What is the Lewis structure of CCl4?

The Lewis structure of CCl4, also known as carbon tetrachloride, is a representation of the molecule’s molecular structure. It shows the arrangement of atoms and valence electrons in the molecule. In the Lewis structure of CCl4, there is a central carbon atom bonded to four chlorine atoms. Each chlorine atom is connected to the carbon atom by a single covalent bond. The Lewis dot structure of CCl4 can be represented as follows:

Cl
|
Cl-C-Cl
|
Cl

Is the Lewis structure of CCl4 polar or nonpolar?

The Lewis structure of CCl4 suggests that the molecule is nonpolar. This is because the carbon atom and the four chlorine atoms are arranged symmetrically around the central carbon atom, resulting in a tetrahedral molecular geometry. In a nonpolar molecule, the distribution of electrons is balanced, and there is no significant separation of charge. Therefore, CCl4 does not have a dipole moment and is considered nonpolar.

Does CCl4 have a resonance structure?

No, CCl4 does not have a resonance structure. Resonance occurs when there are multiple valid Lewis structures that can be drawn for a molecule. In the case of CCl4, the arrangement of atoms and bonds is fixed, and there is no possibility for resonance. The Lewis structure of CCl4, with a central carbon atom bonded to four chlorine atoms, accurately represents the molecule’s structure.

What is the VSEPR model for CCl4?

The VSEPR (Valence Shell Electron Pair Repulsion) model is used to predict the molecular geometry of a molecule based on the arrangement of electron pairs around the central atom. In the case of CCl4, the central carbon atom is bonded to four chlorine atoms, resulting in a tetrahedral molecular geometry. According to the VSEPR model, the electron pairs (both bonding and non-bonding) repel each other and arrange themselves as far apart as possible, leading to the tetrahedral shape of CCl4.

Why does CCl4 have a tetrahedral shape?

The tetrahedral shape of CCl4 is a result of the arrangement of its electron pairs around the central carbon atom. In CCl4, the carbon atom is bonded to four chlorine atoms, and there are no lone pairs of electrons on the central atom. According to the VSEPR theory, the electron pairs repel each other and arrange themselves as far apart as possible. This arrangement leads to a tetrahedral shape, where the bond angles between the carbon and chlorine atoms are approximately 109.5 degrees.

Why does CCl4 have a low melting point?

CCl4 has a low melting point due to its molecular structure and the nature of its intermolecular forces. In CCl4, the carbon atom is bonded to four chlorine atoms, resulting in a nonpolar molecule. Nonpolar molecules have weak intermolecular forces, such as London dispersion forces, which are caused by temporary fluctuations in electron distribution. These weak forces are easily overcome, leading to a low melting point for CCl4.

Why is CCl4 used in NMR?

CCl4 is commonly used as a solvent in Nuclear Magnetic Resonance (NMR) spectroscopy. NMR spectroscopy is a technique used to study the structure and properties of molecules by analyzing their interaction with a magnetic field. CCl4 is preferred as a solvent in NMR because it is nonpolar and does not contain any hydrogen atoms. This allows for better resolution and interpretation of the NMR spectra, as the signals from CCl4 do not interfere with the signals of the molecules being studied.

Is CCl4 a Lewis acid or base?

CCl4 is neither a Lewis acid nor a Lewis base. In Lewis acid-base theory, a Lewis acid is a substance that can accept a pair of electrons, while a Lewis base is a substance that can donate a pair of electrons. CCl4 does not have any available electron pairs to donate or accept, as all its valence electrons are involved in bonding with the chlorine atoms. Therefore, CCl4 does not exhibit Lewis acid or base behavior.

What is the formal charge in the Lewis structure of CCl4?

The Lewis structure of CCl4, also known as carbon tetrachloride, is a representation of its molecular structure using Lewis dot symbols. It helps us understand the arrangement of atoms and the distribution of valence electrons in the molecule. In the Lewis structure of CCl4, we can determine the formal charge on each atom to assess its stability.

How do you draw the Lewis structure of CCl4?

To draw the Lewis structure of CCl4, we need to follow a few steps. Let’s break it down:

1. Determine the total number of valence electrons: Carbon (C) has 4 valence electrons, and each chlorine (Cl) atom has 7 valence electrons. Since there are four chlorine atoms, the total number of valence electrons is 4 + (4 × 7) = 32.

2. Identify the central atom: In CCl4, carbon (C) is the central atom as it is less electronegative than chlorine (Cl). Carbon can form four covalent bonds, one with each chlorine atom.

3. Connect the atoms with single bonds: Start by drawing a carbon atom in the center and four chlorine atoms surrounding it. Each chlorine atom should be connected to the carbon atom with a single bond.

4. Distribute the remaining electrons: Place the remaining electrons around the atoms to satisfy the octet rule. Begin by placing the electrons as lone pairs on the chlorine atoms. Once each chlorine atom has eight electrons (including its lone pairs), distribute the remaining electrons as lone pairs on the central carbon atom.

5. Check for octet rule and formal charges: Count the number of electrons around each atom to ensure they have an octet (except for hydrogen, which follows the duet rule). In the Lewis structure of CCl4, carbon has eight electrons (including its lone pairs), and each chlorine atom also has eight electrons. The formal charge on an atom can be calculated by subtracting the number of lone pair electrons and half the number of shared electrons from the number of valence electrons.

The formal charge formula is: Formal Charge = Valence Electrons – Lone Pair Electrons – 1/2 * Bonding Electrons

For CCl4, the formal charge on carbon and each chlorine atom is zero. This means that the Lewis structure of CCl4 is stable and satisfies the octet rule for all atoms.

Here is a visual representation of the Lewis structure of CCl4:

Cl
|
Cl - C - Cl
|
Cl

Frequently Asked Questions

What is the Lewis dot structure of CCl4?

The Lewis dot structure of CCl4, also known as carbon tetrachloride, is a central carbon atom surrounded by four chlorine atoms. Each chlorine atom is connected to the carbon atom by a single covalent bond, and each atom has an octet of electrons.

Is CCl4 a polar or nonpolar molecule?

CCl4 is a nonpolar molecule. Despite the polar covalent bonds between the carbon and chlorine atoms, the molecule’s overall polarity is zero due to its symmetrical tetrahedral structure.

Why is CCl4 considered a nonpolar molecule?

CCl4 is considered a nonpolar molecule because it has a symmetrical tetrahedral structure. This means that the polarities of the individual C-Cl bonds cancel each other out, resulting in an overall nonpolar molecule.

Does CCl4 have a resonance structure?

No, CCl4 does not have a resonance structure. This is because all the bonds in the molecule are identical, and there are no multiple bonds or lone pairs on the central atom that could lead to resonance.

What is the bond angle in the CCl4 Lewis structure?

The bond angle in the CCl4 Lewis structure is approximately 109.5 degrees, which is characteristic of a tetrahedral molecular geometry.

Is CCl4 a Lewis base?

No, CCl4 is not a Lewis base. A Lewis base is a species that donates an electron pair. CCl4 does not have any lone pairs of electrons to donate, so it cannot act as a Lewis base.

How many valence electrons are in the CCl4 Lewis structure?

In the CCl4 Lewis structure, there are 32 valence electrons in total. The carbon atom contributes 4 electrons, and each of the four chlorine atoms contributes 7 electrons.

What is the molecular geometry of the CCl4 Lewis structure?

The molecular geometry of the CCl4 Lewis structure is tetrahedral. This is due to the four pairs of electrons around the carbon atom, each of which is bonded to a chlorine atom.

Does CCl4 have any lone pairs of electrons?

No, CCl4 does not have any lone pairs of electrons. All of the valence electrons are involved in bonding with the chlorine atoms.

Why is CCl4 tetrahedral in shape?

CCl4 is tetrahedral in shape because the carbon atom forms four bonds with the chlorine atoms. This arrangement of bonds minimizes the repulsion between the electron pairs, resulting in a tetrahedral shape.

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This article contains the BrO2- lewis structure, mode of hybridization, bond angle, and many more detailed facts.

In the BrO2- lewis structure molecule is bent shaped but due to the presence of two pairs of lone pair geometry is tetrahedral. The central Br atom sp³ hybridized with bond angle 109⁰ with no deviation from the ideal bond length. Two Oxygen atoms bind with Br via a double bond single bond.

Bromite is an oxoanion of Br. The Br-O bond length is around 178 pm for a single bond and 153 pm for a double bond and the molecule is asymmetric so it has some dipole moment and it is a polar molecule.

1.    How to draw BrO2- lewis structure?

Lewis structure or lewis dot structure helps us to find the number of electrons involved in the bond formation or the number of lone pairs available in a molecule.

In BrO3- lewis structure, the total electrons involved is 7+ (6*2)+1 = 20, where 1 is for negative charge and the electrons needed 8+(8*2)= 24, So the bonding electrons will be 24- 20= 4 electrons and the number of the total bond will be 4/2 =2 bonds. So, in the BrO2- there will be at least two sigma bonds present.

To draw the BrO2- lewis structure we need to calculate the total valence electrons of individual atoms that is Br and O and they are added together. Now we have to find the central atom based on its less electronegativity. Compare between Bromine and O, Br is less electronegative than O so, Br is the central atom here.

Now Bromine and O are connected via covalent bonds. Two Oxygen are getting connected with Br via a single bond and one oxygen is attached via a double bond to complete the octet.

Lone pairs are assigned to the central Br and the negative charge is on one of the Oxygen atoms which is connected through a single bond only.

2.    BrO2- lewis structure shape

In the BrO2- lewis structure the electron density lies around the central Br atom only.

From the BrO2- lewis structure it is evident that the molecule is bent shape like a water molecule with two lone pairs present over the Br atoms only. Considering the lone pair, it will adopt tetrahedral geometry as is evident from its bond angle data.

Unlike water here one double bond is present and due to the more electronegative atom is present so the bond angle is near about 109⁰ in its tetrahedral geometry.

3.    BrO2- valence electrons

In the BrO2- lewis structure Br and O contain valence electrons in their valence shell.

In the BrO2- lewis structure the central Br are connected with two O atoms via a single bond and a double bond respectively. There are two lone pairs are present over the Br atom and a negative charge is present in the oxygen atom which connected through a single bond only.

From the electronic configuration of Bromine and O, we know that there are seven and six electrons present in their valence shell of them respectively. Among seven electrons Br used 3 electrons for bond formation and four electrons exist as two pairs of lone pairs.

One oxygen gets seven electrons in its valence shell due to a negative charge over it.

In the BrO2- lewis structure total valence electrons are = 7+7+6=20 electrons.

4.    BrO2- lewis structure formal charge

Considering the same electronegativity for all atoms in a molecule to find the charge accumulated by them is called a formal charge.

The formula we can use to calculate the formal charge, F.C. = N_v – N_l.p. -1/2 N_b.p.

In the BrO2- lewis structure there are two types of Oxygen atoms present one is bearing a negative charge and one is forming a double bond so their formal charge will be different.

Formal charge accumulated by Br = 7-4-(6/2) = 0

The formal charge accumulated by O containing double bond = 6-4-(4-2) = 0

The formal charge accumulated by O bearing negative charge  = 6-6-(2/2) = -1

Bromite anion is also containing a negative charge and it is also derived from its formal charge also. The formal; charge also satisfies the number of ionic species.

5.    BrO2- lewis structure lone pairs

Electrons present in the valence shell or outermost orbitals of an atom in a molecule but not involving direct bond formation are called lone pairs.

From the BrO2- lewis structure Br and O both are P block elements and they are from group VIIA and VIA respectively. That means Br has seven and O has six electrons in their valence shell.

Out of seven electrons of Br in BrO2- lewis structure three electrons participate in bond formation and the rest of the two electrons are present as two pairs of lone pairs.

For O which formed a double bond with Br having four electrons left in its valence shell which exists as lone pairs and for that o which contains negative charge has six electrons in its valence shell and they present as three pairs of lone pairs.

So, the total number of lone pairs available in BrO2- lewis structure which is not involved in bond formation is, 2+2+3 =7 pairs of lone pairs which means 14 electrons.

6.    BrO2- lewis structure octet rule

Every atom in bromite tries to complete its valence shell by accepting or donating a suitable number of electrons and adopting the nearest noble gas configuration in accordance to octet rule.

From the BrO2- lewis structure it is evident that out of seven electrons of Br in its valence shell it formed 3 bond pairs and there will be two lone pairs present on it.

Br is a group VIIA element so it has seven electrons in its valence shell where four electrons are present as lone pairs and Br shares two electrons with two O atoms to form two sigma bonds which mean four electrons are involved in the bond pair.

O is a group VIA element so it has six electrons in its valence shell and out of six electrons four electrons are present as lone pairs and the rest of the four electrons are involved in bond formation with Br via sharing electrons with Br. This way O complete its octet.

Now one Oxygen atom which forms only a single bond with Bromine has six electrons as lone pairs and shares two electrons with Br to form a sigma bond and complete its octet too via adopting a negative charge.

7.    BrO2- lewis structure bond angle

In the Bromite structure, Br and two O form a particular bond angle in the perfect arrangement of the molecule to stabilize the molecule.

From the BrO2- lewis structure molecular shape is bent. From the VSEPR (Valence Shell Electrons Pair Repulsion) theory, we can be told that the bent-shaped molecule has a bond angle lower than 120⁰.

The geometry of the molecule is tetrahedral due to the presence of two lone pairs over the Br atom. So, the bond angle is expected to be 109.5⁰ and the Br-O-Br bond angle in bromite is 109⁰ which is the almost ideal bond angle for tetrahedral geometry.

This data govern that there is no reason for deviation of bond angle from its ideal value because Br is large and there will be only two O atoms present so the chance of lone pair repulsion is minimized here but due to some electronegativity, there is some sort of bond angle.

8.    BrO2- lewis structure resonance

In BrO2- lewis structure it can adopt many skeleton structures where the electronic clouds of the molecule can be delocalized, the process is called resonance.

In BrO2- lewis structure it is possible to adopt all the above structures.

Structures I and II are similar and they are the highest contributor to the resonance of Bro2- lewis structure because they have a higher number of covalent bonds and electronegative atom O gets a negative charge.

Structure III is less contributor as it carries a lower number of the covalent bond and electronegative atom Br gets a positive charge which is a destabilization factor.

9.    BrO2- hybridization

In BrO3- lewis structure the molecule is sp³ hybridized where two orbitals of Br and O atoms of different energy undergo mixing to give a new hybrid orbital of equivalent energy.

For bromite ions, hybridization is calculated by the formula,

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

In BrO3- lewis structure, Br has four electrons as lone pairs and two electrons are involved for two sigma bond formation with two O atoms.

So, the central atom Br is, ½(6+2+0+0)= 4 (sp³ hybridized)

                    If the hybridization value is 4 then we can told that the central atom should be sp³ hybridized.

From the box diagram of BrO2- lewis structure it is evident that we consider only sigma bonding in hybridization, not the π bond.

Br has five electrons in its 4p orbital in the ground state, In the excited state, it transferred one electron to its 4d orbital and for two sigma bonds with two unpaired electrons present in the 4p orbital. So, for Br, there are two lone pairs one in 4s and the other in 4p orbital, and two bond pairs in 4p orbitals are involved in hybridization.

So here one 4s and three 4p orbitals are undergoing mixing to give an sp³ hybrid orbital.

Again, from hybridization, we can say that if the molecule is sp³ hybridized then the central atom makes 109.5⁰ with other substituents and the bond angle of BrO2- is around 109⁰ which is match its hybridization value also.

 So, we can say that hybridization and VSEPR theory can predict the same result for the bond angle of a molecule, where one can predict the bond angle from the structure and one can from its hybridization value.

10.    BrO2- solubility

The solubility of bromite ion depends on the temperature and particular solution.

In the BrO2- lewis structure there is one negative charge present to make the molecule more anionic and for this reason, it can ionizable in water and gets soluble in it. The lone pair also help to be soluble in the solution to coordinate with the solution.

11.      Is BrO2- ionic?

From the BrO2- lewis structure we can say that it has some ionic character along with the covalent character. According to Fajan’s rule, all the covalent molecules have some ionic character and it depends on their ionic potential and polarizability. Br has less tendency to polarize small anions like oxygen so it has lower polarizability and lower value of ionic character.

Also, Br has higher ionic potential for its electronegativity so the molecule possesses some ionic character, and also the molecule is charged so it has ionic nature in it.

12.    Is BrO2- acidic or basic?

It is a conjugate base of Bromous acid so generally, it is basic. The counter ion H⁺ can be attached to the BrO2- lewis structure which gives the Bromous acid.

So, we can say that on ionized Bromous acid we get bromite as the counter anion, and it is a conjugate base of the respective acid. As Bromous acid is a weaker acid so its conjugate base bromite is stronger.

13.    Is BrO2- polar or nonpolar?

Due to the bent shape of the bromite ion, it is a polar molecule.

From the BrO2- lewis structure it is evident that the molecule is a bent shape and the dipole moment acts from Br to O (as the dipole moment acts from more electronegative substituents to less electronegative substituents). There will be some resultant dipole moment shown in the BrO2- lewis structure so the molecule is polar.

Conclusion

From the above discussion of BrO2- lewis structure we can conclude that it is bent shape but with the presence of lone pair, it adopts tetrahedral geometry with bond angle 1090. There is no deviation factor is present for bond angle. Due to its bent shape, it has a dipole moment and makes the molecule polar. Bromite is a stronger conjugate base of a weak acid.

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In this article, we should learn about BrO3- lewis structure, shape, geometry, bond angle, and many more detailed facts.

In the BrO3- lewis structure molecule is trigonal pyramidal but due to lone pair geometry is tetrahedral. The central Br atom sp³ hybridized with bond angle 104⁰ slightly deviated due to the repulsion of the lone pairs. Three Oxygen atoms bind with Br via a double bond or one can bind a single bond only.

Bromate is an oxoanion of Br. The Br-O bond length is around 165 pm and the molecule is asymmetric so it has some dipole moment and it is a polar molecule.

Some important facts about BrO3-

Bromine gas is converted to bromate via the photoactivation process. But in the laboratory bromate can be prepared by dissolving bromine into a concentrated solution of potassium hydroxide solution.

Br + 2 OH^– = BrO^– + H₂O

3BrO^–  = BrO^– + 2Br^–

The main process of formation of bromate is a reaction between ozone and bromide.

O₃ + Br^– = BrO₃^–

Bromate-containing water is bad for human life.

1.    How to draw BrO3- lewis structure?

With the help of lewis structure or lewis dot structure number of electrons participating in bond formation or the number of lone pairs available can predict.

In BrO3- lewis structure, the total electrons involved is 7+ (6*3)+1 = 26 and the electrons needed 8+(8*3)= 32, So the bonding electrons will be 32- 26= 6 electrons and the number of the total bond will be 6/2 =3 bonds.

For drawing BrO3- lewis structure we consider the valence electrons of individually Br as well as Oxygen atoms. Now we have to identify the central atom on the basis of electronegativity. Br is less electronegative than O, so Br will be at the central position and three oxygen atoms are present at three corners.

The molecule is anionic so for one negative charge one electron should be added and from the above calculation we can say that in the molecule there will be a minimum of three sigma bonds should be present. Sometimes two oxygen atoms are connected via a double bond and one lone pair over Br.

2.      BrO3- lewis structure shape

The total electron density of the molecule is present over the central Br atom.

In BrO3- lewis structure the geometry of the molecule is trigonal pyramidal but the shape is tetrahedral along with lone pairs. Due to the repulsion of the lone pairs, the bond angle has deviated and there will be two O atoms connected via a double bond.

3.    BrO3- valence electrons

In the Bro3- lewis structure the central Br atoms attached double bond with two Oxygen atoms and via single bond with another oxygen atom and containing one pair of lone pair.

The electronic configuration of Br is [Ar]3d¹⁰4s²4p⁵ and the for O is [He]2s²2p⁴. So, there are 7 and 6 electrons present in the valence shell for Br and O respectively. One negative charge is present in one of the Oxygen atoms so one electron should be added.

 So, the total valence electrons for bromate is 7+ (6*3)+1 = 26

4.    BrO3- lewis structure formal charge

The formal charge is a hypothetical concept assuming the same electronegativity for all atoms and can calculate the charge accumulate.

The formula we can use to calculate the formal charge, F.C. = N_v – N_l.p. -1/2 N_b.p.

Where N_v is the number of electrons in the valence shell or outermost orbital, N_l.p is the number of electrons in the lone pair, and N_b.p  is the total number of electrons that are involved in the bond formation only.

In the BrO3- lewis structure we can see that there are two types of Oxygen present one is bonding via a single bond only other bonding single bonds as well as double bonds. So, the formal charges are different for two types of oxygen atoms.

F.C. of Br is = 7-2-(10/2)=0

F.C. of O (single bond) = 6-6-(2/2)= -1

F.C. of O (double bond) = 6-4-(4/2) =0

So, the formal charge of the single bond containing Oxygen atoms is -1. As the molecule is charged so it has a formal charge too.

5.    BrO3- lewis structure lone pairs

The electrons present in the valence shell of an atom in a molecule but do not participate in the bond formation are called lone pairs.

In the BrO3- lewis structure, both Br and O are p block elements so their outermost orbital is P.

Br is VIIA and O is a VIA element so they have seven and six electrons in their valence shell respectively. In the bond formation out of seven electrons, Br used five electrons and two electrons are reminded as lone pair.

For Oxygen atoms out of six electrons, two electrons are involved for one sigma and one π bond, so the rest of the four electrons are present as two pairs of lone pairs. But one oxygen atom formed only a sigma bond and a negative charge is present over it. Here six electrons are not involved in bond formation so here the number of lone pairs is 3.

So, the total number of lone pairs available in bromate is 1+(2*2)+3=8 pairs of lone pairs

6.    BrO3- lewis structure octet rule

Every atom in a molecule tries to complete its valence shell by donating or accepting a suitable number of electrons and gaining the nearest noble gas configuration for stabilization.

In the BrO3- lewis structure, there are three sigma bonds present and for each bond two electrons are involved one from Bromine and one from O. Br has one pair of lone pair also. To complete an octet Br can form a bond with three oxygen atoms.

Again, Oxygen has six electrons in its valence shell, so they form a double bond with Br and four electrons are present as lone pair. So, this way they complete their octet. But for one single oxygen atom only form a single bond with Br and bears a negative charge on it to complete its octet.

7.    BrO3- lewis structure bond angle

In a particular molecule, all the atoms make a particular bond angle after the formation of the bond for perfect alignment.

In the BrO3- lewis structure, geometry is tetrahedral along with one lone pair present over Br. From VSEPR (Valence Shell Electrons Pair Repulsion) theory a molecule having tetrahedral geometry the ideal bond angle is around 109.5⁰ but here O-Br-O bond angle is 104.07⁰. So, it deviated from its ideality.

There are one lone pair over Br and two lone pairs over O atoms. So, there is massive lone pairs repulsion and to minimize the repulsion the molecule aligns the bond angle reduce to 104.07⁰.

 Again, due to the electronegativity of the three oxygen atoms they pull the electron density toward them and the molecule is bent and the angle will be changed.

8.    BrO3- lewis structure resonance

Delocalization of electrons clouds in the same molecule but in a different skeleton.

In the BrO3- lewis structure, there are four resonance structures skeleton possible. The structure I, II, and III are equivalent, and structure IV is different from them.

The most contributing structure is structure IV as it contains a higher number of covalent bonds and electronegative atom Br gets a negative charge as well. So, it has more contribution to the resonance structure.

9.      BrO3- hybridization

By this hypothetical concept, two different orbitals of different energy undergo mixing and form a new hybrid orbital to form a stable covalent bond.

For bromate ion hybridization is calculated by the formula,

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

In the BrO3- lewis structure the valence electrons for Br involved in the bond formation (only sigma bond) is 3, one lone pair and the surrounding atom will be 3. The negative charge is on the O atom only so we will not consider it in hybridization.

So, the mode of hybridization of central Br is = ½(5+3+0+0)=4 (sp³)

From the above table, we can be told that if the hybridization value is 4 for any molecule then the molecule is sp³ hybridized. Where lone pairs present as s orbital and three p orbitals are involved in bond formation with three oxygen atoms.

From the box diagram of BrO3- lewis structure it is evident that we cannot consider the π bond in hybridization. Only sigma bonds are involved.

For Br, there are five electrons in the 4p orbital in the ground state and two electrons are transferred in the 4d orbital, and two electrons are present in the 4s orbital as lone pairs. The three unpaired electrons in the 4p orbital now combine with three oxygen atoms to form three new hybrid sigma bonds along with one lone pair.

So here one s and three p orbitals are involved in the hybridization to form an sp³ hybrid orbital. By the mixing of orbital both Br and O can complete their octet.

According to VSEPR theory and the table of hybridization, we can say a molecule having tetrahedral geometry the bond angle will be 109.5⁰, but here the scenario is different due to lone pairs repulsion which is present at the sp³ hybrid orbital.

10.    BrO3- solubility

The solubility of any molecule depends on the temperature and nature of the solution and solute also.

In the BrO3- lewis structure, as we can see that bromate is an anion so it is surely soluble in water by the hydration effect. The counter cation of it can attract the bromate molecule and helps the solubility.

It is also soluble in ammonia but insoluble in methanol.

11.      Is BrO3- ionic?

According to Fajan’s rule, every molecule has some ionic as well as covalent character.

From the BrO3- lewis structure it is evident that there is a negative charge over the molecule so the molecule possesses some ionic character and it can be ionizable in a particular solution in water. Even Br has some ionic potential but it has less tendency to polarize the small size of oxygen atom as the size of Br is large.

Again, due to the small size of Oxygen, it is less polarizable but the ionic potential of oxygen is high due to its negative charge on it. So, it has some ionic character along with the covalent character.

12.    Is BrO3- acidic or basic?

Bromate is a conjugate base of Bromic acid.

From the BrO3- lewis structure we can say that it is the anion of any other salt of any molecule. The counter cation of bromate will be Na⁺, K⁺, and H⁺. Apart from H^+, other cations will form a neutral salt with bromate anion.

But when it is attached to H⁺ then it will form bromic acid (HBrO3). Which is a moderate acid and bromate is its conjugate base.

13.    Is BrO3- polar or nonpolar?

Bromate is an asymmetric molecule so it has a resultant dipole moment.

By the value of dipole moment, a molecule can be decided whether is it polar or nonpolar. From the BrO3- lewis structure we can see that it is a tetrahedral shape which is an asymmetric molecule and it has some resultant dipole moment.

The dipole moment acts from Br to O as it is work from less electronegative to more electronegative substituents.

From this structure, it is evident that there is some resultant dipole moment present. So, the molecule is polar in nature.

Summary

From the above discussion of Bro3- lewis structure we can conclude with a few things being tetrahedral geometry but the bond angle is lesser than expected due to the lone pair repulsion. The molecule is a conjugate base of the acid, due to its asymmetric shape, it is polar.

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This article should learn about BeI2 lewis structure, shape, bond angle, hybridization, and many more detailed fact.

In the BeI2 lewis structure, the shape of the molecule is linear having sp hybridization. The molecule is linearly shaped and two iodine each contain three pairs of lone pairs. As it is a linear molecule so the bond angle of I-Be-I is 180⁰.

BeI2 is a halogenated salt of alkaline earth metal. Be is alkaline earth metal and can form a strong base with respective anions. The charge over Be is +2 and it is fully satisfied by two iodide anions.

Some important facts about BeI2

BeI2 is solid in its physical state and the color is white. The molecule is hygroscopic which means it can hold the water molecule by absorbing it.

The molecule’s melting point and boiling points are 753 K and 863 K, respectively. In the lattice crystal structure, the BeI2 is orthorhombic.

In presence of elemental Iodine, BeI2 is formed and reacted with Be metal at 500-700⁰C temperature.

Be + I₂ =BeI₂

1.    How to draw BeI2 lewis structure?

Before proceeding with the lewis structure drawing we should know lewis structure or lewis dot structure can briefly describe the electrons involved in a molecule for bond formation.

First, we taking consideration of valence electron of Be as well as I. Here Be is a lack of two electrons where two I contain one more electron in their valence shell. Identify the central atom by the electropositivity so here Be is the central atom as Iodine is more electronegative.

The molecule is neutral so the charge over Be and I are fully satisfied by the bond formation so no need to add or remove electrons then three atoms are attached by a single bond only. After that, the lone pairs are assigned to the respective atoms that in over Iodines only.

2.    BeI2 lewis structure shape

In the BeI2 lewis structure, the whole electron density of the molecule lies on the central Be atom.

The structure is linear and Be atom is present at the central position where two iodines are at the terminal site. Lone pairs are present on the Iodines atoms only

3.    BeI2 valence electrons

From the BeI2 lewis structure, it is shown that the linear molecule is attached by a single bond only.

The ground state electronic configuration of Be is 1s²2s² and in the excited state i.e. for Be²⁺ the electronic configuration will be 1s², so valence electrons will be two. Again, for I the ground state electronic configuration is [Kr]4d¹⁰5s²5p⁵ so the valence electrons will be 7 as 5s and 5p are the valence shell for each I.

So, the total number of valence electrons in BeI2 is (7*2)+2 =16

4.    BeI2 lewis structure formal charge

The formal charge is a hypothetical concept accounting for the same electronegativity for all atoms.

The common formula for calculation of formal charge is, F.C. = N_v – N_l.p. -1/2 N_b.p.

Where N_v is the number of electrons in the valence shell, N_l.p is the number of electrons in the lone pair, and N_b.p  is the total number of electrons that are involved in the bond formation only.

Here in the BeI2 lewis structure, we calculate formal charge separately for Be as well as I.

Formal charge over Be is =2-0-4/2 = 0

Formal charge over I =7-6-2/2 =0

So, the overall molecule is neutral and it is also reflected in the formal charge.

5.      BeI2 lewis structure lone pairs

The lone pairs are those electrons that are not involved in the bond formation.

From the above BeI2 lewis structure we can see that the lone pairs are only over the I only. So, we add the total number of lone pairs in two I atoms, each I contains 3 pairs of lone pair because the valence electrons for I is 7 and one electron from that participate in bond formation. So, the remaining 6 electrons exist as 3 pairs of lone pairs and Be is lack of lone pair.

So total number of lone pairs in BeI2 is 6+6=12

6.    BeI2 lewis structure octet rule

The octet rule is for every atom is complete its valence shell by accepting or donating a respective number of electrons and trying to gain the nearest noble gas configuration.

In the BeI2 lewis structure, central Be is from the s block and I is from the P block element. Be is an II element whereas Iodine is a VIIA element which means Be has two electrons in its outermost shell and I have & electrons. Be already gain stability due to s orbital filled (s orbital contains maximum electrons) but for I short of one electron to complete its octet, so it shares one electron from Be and completes its octet.

7.    BeI2 lewis structure bond angle

A bond angle is a specific angle between atoms in a particular molecule.

From VSEPR(Valence Shell Electrons Pair Repulsion) theory we can say that in the BeI2 lewis structure the bond angle I-Be-I is 180⁰ that its shape is linear. There is no violation of that bond angle in this molecule due to the large size of I the lone pair lone pairs repulsion is minimized here. So BeI2 shows an ideal linear shape angle that is 180⁰.

8.    BeI2 lewis structure resonance

Resonance is a hypothetical concept that can describe the transfer of electron cloud in the same molecule but a different skeleton.

From the BeI2 lewis structure different skeleton forms, the stable is III as it contains more covalent bonds. After that, we consider the charge distribution of the atom, that if an electronegative atom gets a negative charge or an electropositive atom gets a positive charge is more stable than the reverse.

9.      BeI2 hybridization

Hybridization is also a hypothetical concept to determine the mode of bonding of a covalent molecule by mixing orbitals of two or more atoms to get hybrid orbitals.

The hybridization of any molecule is calculated by the formula

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

So here in the BeI2 lewis structure, the central Be atom has two valence electrons in its s orbital and two I atoms are present at the terminal position.

So, the hybridization of BeI2 is = ½ (2+2+0+0) =2 (sp)

From the above table, it is shown that if the hybridization value is 2 then the mode of hybridization is sp. So BeI2 is sp hybridized. Where S orbital of central Be and P orbital of two Iodine are mixing together to give a new sp hybrid orbital.

10.    BeI2 solubility

Solubility is the phenomenon to which extent a molecule will be soluble in a given solution.

BeI2 reacts with a water molecule to give a new compound. As it is a covalent molecule so its solubility in water is very poor. But it has a greater solubility in methanol and even carbon disulfide also.

11.    Is BeI2 ionic?

According to Fajan’s rule and ionic potential, we can say that no molecule is 100% ionic or covalent.

The size of Be2+ is small so it can easily polarize the larger anion like Iodide. Iodide is larger so it can be easily polarizable by Be2+ ion. So, the molecule possesses an ionic character along with its covalent nature. Be2+ has higher ionic potential as its size is small and charge density is also high so BeI2 shows ionic character.

13.    Is BeI2 polar or nonpolar?

If a molecule has some resultant dipole-moment then it is polar otherwise nonpolar.

From the above BeI2 lewis structure, we can see that there are two dipole-moment acts opposite to each other. So, the dipole moment of this molecule is zero. So BeI2 is nonpolar. The direction of the dipole-moment always acts from a more electropositive atom toward electronegative an atom.

Here Iodine is more electronegative and Be is electropositive so the dipole-moment acts from Be to I site. As the structure is linear so the direction of the two dipole-moment is opposite and cancels out each other to make the molecule nonpolar.

13.    Is BeI2 acidic or basic?

BeI2 itself is a neutral complex but it when reacts with water the solution turns acidic.

In BeI2 lewis structure, central Be is sp hybridized with vacant 2p orbital and the lone pairs of oxygen in water molecule can be attacked there and it can accept the electron and a strong acid hydrogen Iodide is formed.

BeI2 + 2H2O = Be(OH)2 + 2HI

So, it behaves as acidic in water solution, but in molecular form, there are two electronegative atoms I present, and the electronegativity of two halogens the accessibility of vacant p orbital will be increased.

Conclusion

From the above discussion of the BeI2 lewis structure we can conclude that the molecule has 16 valence electrons, sp hybridized, linear structure along with bond angle 180 degree, and six pairs of lone pair.

Be is not a complete octet but it is still stable due to zero formal charge and has a filled s orbital. Although it is neutral in an aqueous solution it can produce acid and has zero dipole moment making the molecule non-polar.

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