Aparna Dev

Difluoroethane (C2H2F2) has two carbon (C) atoms, each with 4 valence electrons, connected by a single bond. Each C atom is also bonded to one hydrogen (H) atom and one fluorine (F) atom. The Lewis structure shows four single bonds (two C-H and two C-F), with no lone pairs on the carbon atoms, using 18 valence electrons. C2H2F2 adopts a tetrahedral geometry around each carbon atom with bond angles close to 109.5°, characteristic of sp³ hybridization. The molecule is nonpolar overall, with polar C-F and C-H bonds due to electronegativity differences (C: 2.55, F: 3.98, H: 2.20). This structure influences its physical properties and reactivity, such as in refrigeration applications.

Difluoromethane is a haloalkane compound with two fluorine atoms. The strong carbon fluorine bonds in this molecule determines its chemical properties.

Facts about Difluoromethane

Difluromethane is an organic dihalo compound. It’s molecular formula is CH₂F₂. Two hydrogens atoms in methane is substituted by a  fluorine atom. It have other names like difluromethylene, HFC- 32, methylene fluoride.

It is a colorless substance with gaseous nature. It has high thermal stability. But it’s boiling point and melting point is found to be very low that is -136⁰C and -52⁰C respectively. It’s a substance with 52.024g/mol which has the ability to undergo endothermic process. It is used as a refrigerant and as a fire extinguisher.

Lewis structure of Difluoromethane, CH₂F₂

Structures of molecules drawn through this concept is an easy way for understanding the bond formation between different atoms. Here the electrons and bonds are denoted by dots and lines respectively. So structures can be termed as Lewis dot structures.

Difluromethane is formed by the substitution of two hydrogen atoms by fluorine. The sum total of valence electrons in difluromethane is 20.

Carbon is the central atom and all the four other atoms are placed around it along with their valence electrons. Carbon forms four steady bonds with two fluorine and hydrogen.

Resonance in Difluoromethane, CH₂F₂

The motion of electrons in association with an atom results more than one structure to a molecule. Such structures are called resonance structure and process is resonance. Usually this can be seen in double bonded compounds. It is important to retain the electronic arrangements of atoms during resonance. There is no resonance structure found for difluromethane.

Difluoromethane, CH₂F₂  Octet Rule

We all know that difluromethane consists of one carbon attached with two hydrogen and fluorine. Carbon is the middle atom and has four outer electrons. Fluorine and hydrogen with seven and one outer electrons are present around carbon atom .

When the bond formation takes place carbon acquire four more electrons from Fluorine and hydrogen. So it’s valence shell now filled with eight electrons. Similarly fluorine has seven before bond formation and eight after bond making.

But hydrogen needs only two electrons for stable existence and it is obtained through bonds. So carbon and fluorine obeys octet rule. Even though hydrogen doesn’t obey octet rule it is stable.

Difluoromethane, CH₂F₂ Shape and Bond angle

Molecules acquire different shape after their bond construction. They can have different shape dependent with the lone pairs present in the central atom. Here the central carbon has no lone pairs and is AX₄ type. So it’s geometry is tetrahedral with an angle of 109.5⁰ .

Here there are two different bonds. One is carbon- fluorine and latter is carbon- hydrogen. The polarity of former is much greater than the latter.

Difluoromethane, CH₂F₂ Lone pairs

The number electrons which doesn’t take any role in bond formation is its lone pair of electrons. Here there is no lone pair for carbon and hydrogen. But there is lone pairs associated with two fluorine atoms. Out of seven outer electrons only one is used for bonding and the remaining six exist as three lone pairs. So total six lone pairs are present here.

Difluoromethane, CH₂F₂ Formal charge

The charge given to the atoms after bond construction is called formal charge. It can be either positive or negative and zero.

Formal charge = valence electrons – no. of dots – no. of bonds

Formal charge of carbon = 4-0-4 = 0

Formal charge of fluorine = 7-6-1 = 0

Formal charge of hydrogen = 1-0-1 =0

Formal charge of carbon, fluorine and hydrogen is zero.

Difluoromethane, CH₂F₂  Valence electrons

The total electrons seen in the outermost shell of any atom which has a major role in bond formation is called valence electrons. The total valence electrons in difluromethane is found by taking sum of valence electrons in each atom. So it is

Valence electrons in carbon – 4

Valence electrons in fluorine – 7

Valence electrons in hydrogen – 1

So total in Difluoromethane, CH₂F₂ is 4+7×2+1×2 = 20 electrons.

Difluoromethane, CH₂F₂ Hybridisation

Difluromethane is found to be a tetrahedral molecule in shape which follows sp³ hybridization. During sp³ hybridization the s and p orbitals of carbon atom overlapps to give a new set of sp³ orbitals with equal shape and energy. Then they combine with hydrogen and fluorine atoms orbitals shares its electrons with this sp³ orbitals to form bonds.

Difluoromethane, CH₂F₂ Solubility

Difluromethane is not much soluble in every solvents. One of the reason for this is its strong carbon- fluorine bond. There is vanderwaals dispersion force and dipole -dipole interactions exist in between difluromethane molecules.

When we try to dissolve this in water, there needs more energy to overcome these interactions. It has to overcome the energy due to hydrogen bonding between water molecules. So it is difficult to break this bonds and to create new one with the haloalkane and water.

Therefore it is sparingly miscible in water even though it is polar. But difluro methane is found to be soluble in ethanol.

Is Difluoromethane, CH₂F₂ Ionic or not ?

Difluromethane is a covalent compound formed by common sharing of electrons between carbon, hydrogen and fluorine. It follows sp³ hybridization. So it is not an ionic compound.

Is Difluoromethane, CH₂F₂ Polar or not ?

Difluromethane is a polar compound. The electronegativity of carbon, Fluorine and hydrogen is 2.55, 3.98, 2.20. Fluorine is the most electronegative atom so the electrons in carbon – fluorine bond is always towards fluorine atom.

So fluorine has partial negative charge and carbon has partial positive charge. So the carbon Fluorine bond is highly polarised. The electronegativity difference of carbon and hydrogen is 0.35 which is very low.

So it’s polarisation is low compared to C-F bond. Due to the high electronegativity difference seen in carbon- Fluorine and carbon- hydrogen bond difluromethane is found to be a polar molecule.

Is Difluoromethane, CH₂F₂  Acidic or Basic ?

The bond between carbon – fluorine is very strong so the bond can’t be broke very easily. Therefore difluro methane doesn’t undergo any type of chemical reactions. So it’s acidity and basicity cannot be distinguished.

Conclusion

Difluoromethane, CH2F2  is stable covalently bonded compound which is polar. It is because of strong carbon – fluorine bond. It follows sp3 hybridisation with tetrahedral shape and angle is about 109.50. Its Lewis structure is drawn here in this article. It has 20 valence electrons with six lone pairs around two fluorine atoms with zero formal charge.

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cf4 lewis structure and other important details regarding tetrafluoro methane is going to be discussed in this article.

Tetrafluoro methane, CF₄ is a haloalkane or halo methane formed by replacing four hydrogen atoms of methane with fluorine atoms. It is a colorless, odourless gas which is used as refrigerant. It is an infalammable gas.

How to draw Tetrafluoromethane, CF₄ Lewis structure ?

When two or more atoms join together a process called bond formation takes place. They do so by two ways. One is sharing of electrons and the latter is donating or accepting electrons. Since it is a big process we need to understand it in a simple way.

For this we use certain easy structures which shows how bond making takes place. This concept based structures are called Lewis dot structures. It is drawn by taking valence electrons in consideration. This electrons are denoted by dots and bonds through lines.

Electrons are denoted by dots so it is called Lewis dot structures. Here explains the fine details of depicting Lewis structure of tetra fluoro methane.

• In First step we need to find the sum of valence electrons of every atom in tetra fluoro methane. Sum total of valence electrons in carbon and fluorine  is 4+7×4 = 32 electrons.
• Draw the symbol of carbon atom enclosed with four fluorine in its four sides along with their valence electrons. The valence electrons linked with carbon also denoted by dots.

• In this last step we are going to see how this forms a bond. The carbon and fluorine shares their outer electrons and make four firm bonds. Those bonds are indicated by four lines in the structure.

Tetrafluoromethane, CF₄ Resonance

Let’s discuss something about the organisation of electrons around the bonds and atoms. We can arrange these electrons in more than one way. Each organisation gives new structures. Those structures are called resonance structure and the phenomena is resonance. When we sketch these structures the bonds associated with the atoms should not be changed or removed.

If it do so the entire structure of that compound got destroyed. Usually double bonded compounds shows this phenomenon. In tetrafluoromethane it’s electrons can be arranged in only one way. So there is no more structures are possible for this molecule. So there is no resonating structure.

Tetrafluoromethane, CF₄ Shape

Atoms joined together as a result of bond making always tends to occupy certain positions from the central atom. They do so for their stability to exist. That positioning of atoms in a bond assigns them certain shape. It can be linear, tetrahedral, pyramidal, triagonal depending upon the bonds made and atoms. The shape of tetrafluoromethane is tetrahedral.

Tetrafluoromethane, CF₄ Formal charge

The positive, negative or neutral charge given to each atom in a molecule which formed a stable bond is its formal charge. The formal charge calculating equation is

Formal charge = valence electrons – No. of dots –  No. of bonds

Formal charge of carbon = 4-0-4 = 0

Formal charge of fluorine = 7-6-1 = 0

So the whole formal charge of atoms in CF₄ is zero.

Tetrafluoromethane, CF₄ Bond angle

The angle formed as a result of bond construction is called bond angle. It can be different depending upon the shape of molecule. Sometimes it’s values undergo slight variation due to other factors like bond length, lone pair of electrons, repelsion factors. Tetrafluoromethane makes an angle of 109.5⁰ between carbon fluorine bonds.

Tetrafluoromethane, CF₄ Octet rule

Based on octet rule there should be eight electrons in every atom’s outer shell to be in a stable state. Here fluorine has seven electrons and carbon has four in their outer shell. When they combine together each of them shares their electrons with each other. Then carbon get extra four electrons and each fluorine gets one electron. Thus carbon and fluorine get total eight electrons in total in their valence shell. So they obeys octet rule completely.

Tetrafluoromethane, CF₄ Lone pair of electron

Sometimes all the valence electrons don’t go for bond building. Some of them will remain in its shell. Those electrons are called lone pair of electrons.

Tetrafluoromethane, CF₄ Valence electrons

The electrons found in the valence shell of an atom which plays a crucial role in bond making is its valence electrons. It is usually found in outer shell of an atom.

Total valence electrons in CF₄ = 4+7×4 = 32 electrons.

Tetrafluoromethane, CF₄ Hybridisation

The merging of atomic orbitals of an atom to create fresh orbitals is called hybridization. The orbitals united is different in energy but the fresh ones formed is equal in its energy. There are different types of this process depending upon the orbitals got combined. They are sp, sp²,sp³,sp³d², sp³d.

In tetrafluoromethane, five atoms exist. One Carbon and four fluorine atoms. Here carbon is the central or middle atom. Let’s discuss it’s hybridization.

Carbon _{(ground state)}   1s² 2s²  2p²

Carbon _{(excited state)}   1s² 2s²  2p³

So one s and three p orbitals in carbon hybridise to form four sp hybrid orbitals. So here occurs sp3 hybridization. They are indistinguishable in shape. Then arrives the four fluorine atom with one electron in 2p_z orbital and shares with the freshly formed sp³ orbitals. The shape of tetra fluoro methane is tetrahedral with an angle made is 109.5⁰.

Solubility of  Tetrafluoromethane, CF₄

The capability of a substance called solute to dissolve in a different substance called solvent is called solubility. The solute and solvent can be solid, liquid or gas. Water, ethanol, acetone, diethyl ether, benzene, hexane are some of the all time used solvents to dissolve substances. CF₄ is partially miscible in water while get miscible in benzene and chloroform.

This is because if it get dissolved in water it has to break the hydrogen bonds between water molecules. More energy is needed for this to occur. As a result of less energy released during CF₄ water solvation , CF₄  not able to get dissolve in water.

About 18.8 mg/L Tetra fluoro methane is miscible in water at 20⁰C.  But in the case of organic solvents the energy released as result of solvation of tetrafluoro methane it is much more than the older bonds between solvent molecules. So the older bonds can be easily broken and new one is formed.

Is Tetrafluoromethane, CF₄  Ionic or not ?

Tetrafluoromethane is a covalent compound. Because each bond is made by sharing of electrons between carbon and fluorine.

Is Tetrafluoromethane, CF₄  Acidic or not ?

Acidity is the talent of substance to accept electrons from other substances or acid is a substance which can donate protons of H ions into a solution. Basicity can be defined as donating OH^– ions or electrons to other substances. Tetra fluoro methane is neither acidic or basic.

It is a neutral compound. When it reacts water it forms hydrogen fluoride. Hydrogen fluoride is one of weak acid. So tetrafluoro methane is neutral but when dissolved in water release HF which is acidic in nature.

 Is Tetrafluoromethane, CF₄ Polar or not ?

When there is a high electronegativity change is seen in between different bonds present in an atom their polarity will be different. Polarity commonly arrives due to the presence of an electronegative atom in a molecule. Most of the elements in halogen group were found to be always electronegative in nature.

Here in tetrafluoromethane there are four carbon fluorine bonds and their electronegativities are same. But the bonds in CF₄ are equidistant to each other the dipole moment of each bond got cancelled and therefore it get non polar character.

Conclusion

Tetrafluoro methane,CF4 is a non polar, sp3 hybridised, covalent molecule which is acidic in water. It has 32 valence electrons out of which 12 lone pairs are present in fluorine. Its Lewis structure is also drawn here. The formal charge of CF4 is zero with tetrahedral shape and angle 109.50.

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In this article we will discuss about Dibromine,Br₂ its lewis structure, properties and other facts.

Dibromine, Br₂ consists of two bromine atoms joined through a single bond. Bromine is one of the lightest element in halogen family. Dibromine is a reddish brown liquid with a pungent smell which is very toxic for inhalation.

  How to draw Br₂ lewis structures ?

Lewis structure of a molecule is mainly drawn to understand how the bond formation takes place when two atoms or more got united. The lewis structure of a compound  is drawn by considering only the valence electrons present in the outermost shell. It uses dots and lines to depict electrons and bonds respectively.

So the structures drawn by this concept are called lewis dot structures.

Lewis dot structures can be drawn for both covalently bonded and ionic bonded compounds. Dibromine,Br₂ is chemical compound with two bromine atoms combined together. Let’s see how to draw the lewis structure of Br2.

• Calculate the total number of valence electrons. Bromine is a group 7 element having seven electrons in its valence shell. Since dibromine has two bromine atoms the total number of valence electrons present in Br₂ is 7×2 = 14 electrons.
• In this step we draw the symbols for two bromine atoms surrounding with their seven valence electrons.

• In the next step the two bromine atoms shares their one electron each other to form a single bond. Now both the bromine atoms are combined together and they attained stability by satisfying octet rule.

Br₂ resonance

Resonance can be defined as the movement or the delocalistion of electrons present in an atom of any compound. Resonance can only seen in compounds with double bonds and the electrons involved with these bonds are easy to move across the bonds.

While drawing the resonance structure the actual properties like the number of electrons present around the atom shouldn’t change. Even though there is double bond in dibromine it is not allowed to move across, because if they do so the molecular structure  not exist. So there is no resonance structure for dibromine.

Br₂  Shape

Dibromine is a linear shaped molecule with one bromine – bromine sigma bonds. Br₂  is symmetrical in its structure.

Br₂ Formal charge

Formal charge is a charge assigned to an atom when it is get combined with other atoms to form a stable compound. The formal charge assigned to an atom can be easily found out by the below equation

Formal charge of an atom = ( Valence electrons – No. of lone pairs – No. of bonds formed)

Valence electrons present in bromine is 7. In which 6 were lone pairs and one electron is shared to make bond with another bromine atom

Formal charge of  bromine is = 7-6-1

                                                = 0

So the formal charge of bromine in Dibromine, Br₂ is 0.

Br₂ Bond angle

Bond angle is the angle made between three atoms when they combine together to form a stable compound. Dibromine is a linear or symmetrical molecule with one Br- Br sigma bonds. The bond angle made by a linear molecule is 180⁰. So the bond angle of Br₂ is 180⁰.

 Br₂ Octet rule

According to octet rule, when atoms combine together to form compounds they are found to be more stable when their outermost shell are filled with eight electrons. Atoms lose or gain electrons to obey the octet rule. In the case of dibromine there is two bromine atoms.

Each bromine has seven electrons in its valence shell. It need one more electron to attain stability. When these two atoms combines together both of them shares their electrons to each other. Hence their valence shell is filled with eight electrons and they are stable now. Since both of the bromine atom has eight electrons in its valence shell Dibromine obeys octet rule.

Br₂ Lone pair of electrons

Lone pair of electron or non bonding electrons are the electrons present in the valence shell of an atom which doesn’t took participation in bond formation. Since they doesn’t form bonds they can be called as non bonding electrons.

The lone pair of electrons in one bromine is 3. So the total number of lone pair of electrons present in two bromine atoms of dibromine 6.

Br₂ valence electrons

The electrons present in the valence shell or the outermost shell of an atom is called as its valence electrons.

Total number of valence electrons present in dibromine is 14.

Br₂ Hybridisation

According to the concept of hybridisation, the atomic orbitals with slightly different energies unites together to form atomic orbitals with same energy and shape. The new orbitals formed are stable and named as hybrid orbitals. The  number of hybrid orbitals is equal to that of the orbitals got united.

There is different types of hybridisation called

1. sp³
2. sp²
3. sp
4. sp³d
5. sp³d²
6. sp³d³

Hybridisation of a molecule can be found through a formula, which is

Hybridisation of a molecule = No. of sigma bonds + No. of lone pairs

 If the count is 4 then sp³ hybridisation ,3 then sp² and if 2 then sp.

In dibromine there is one sigma bond and three lone pair of electrons.

Hybridisation of Br₂ = 1+3  = 4

 So the hybridisation in dibromine is sp³. Its structure is linear.

Br₂ Solubility

Solubility can be defined as the ability of a substance or solute to get dissolved in a solvent to form a solution. The most commonly used solvents in field of chemistry is water, ethanol, acetone, ether, benzene, chloroform  etc.

 Dibromine is slightly soluble in water because it is not a polar molecule like water. But dibromine is found to be soluble in most of the organic solvents like benzene, gasoline, chloroform, ether, methanol, ethanol, carbon disulphide, carbon tetra chloride,CCl₄.

 Is Br₂  Ionic or not ?

A covalent bond is formed by the sharing of electrons between the combining atoms but ionic bond formation takes place through the electrostatic force of attraction between a positive and negative ion. The positive and negative ions are cation and anion respectively.

Dibromine is formed by the mutual sharing electrons between two bromine atoms. So Br₂ is a covalent compound not an ionic compound.

Is Br₂ Polar or not ?

There are only two bromine atoms are attached together through a single bond in dibromine. So it is non polar in nature.

Is Br₂ Acidic or Basic ?

Dibromine is a lewis acid.  A lewis acid is a substance which can accepts electrons.

Summary

Dibromine is a chemical compound which exists as liquid and gas in room temperature. This article summarise the following key points

1. Dibromine is a covalent compound with non polar character.
2. Dibromine shows acidic behaviour.
3. Br₂ follows sp³ hybridisation.
4. It is soluble in organic solvents and sparingly soluble in water.
5. Its lewis structure drawing pattern.

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We are going discuss about beryllium fluoride,BeF₂ lewis structure, hybridisation, valence electrons and other detailed information in this article.

Beryllium fluoride,BeF₂ is an inorganic compound which looks like a white solid substance. Its structure is similiar to quartz and has some special optical properties.

How to draw BeF₂ Lewis structures ?

 The bond formation between two or more atoms can be easily understand by illustrating its Lewis structure. While sketching the Lewis structure of an atom only its valence electrons are considered. The valence electrons and bonds between the atoms are indicated by some dots and lines respectively. Structures depicted  by this way are called Lewis dot structure.

We can draw Lewis dot structures for both covalently bonded and ionic bonded compounds. Beryllium fluoride is an inorganic compound having one  beryllium and two fluorine atom. Beryllium is a second group alkaline earth metal and fluorine is from halogen family. We have to keep certain rules for drawing the Lewis structure of any compound. They are

• For drawing the Lewis structure first we need to calculate the entire number of valence electrons present in the given compound. It is done by adding the electrons present in the outer shell of each atom. In BeF₂, Be has 2 and fluorine has 7 outer electrons. So in total, there is 2+7×2 = 16 electrons.
• In BeF₂, there is one beryllium atom having two valence electrons and two fluorine atoms with seven valence electrons.

•  Beryllium atom shares two of its valence electrons to the two fluorine atom and hence they form two Be – F single bonds.

• So the Lewis structure of  beryllium fluoride, BeF2 is 

BeF₂ Resonance

The delocalisation of electrons linked with an atom is the cause of resonance. Due to this process a molecule or compound can have more than one structures. Such structures are called its resonating structure or resonance structure. This process can be seen in double bonded compounds and compounds with lone pair of electrons.

When we draw this structure the molecular formula of the compound shouldn’t change. Since there is no double bond present in between beryllium and fluorine there is no resonance structure for beryllium fluoride.

BeF₂  Shape

Beryllium fluoride is made by sharing of electrons between one beryllium atom and two fluorine atoms. Its shape is linear. A linear molecule is a molecule where the atoms are arranged along a straight line. Here the two fluorine atoms are arranged on both the sides of beryllium through a straight line pattern.

BeF₂ Formal charge

The charge allotted to an atom as a result of its bond formation with another atom is called formal charge. The equation for finding the formal charge of an atom is 

Formal charge of an atom = ( Valence electrons – No. of lone pairs – No. of bonds formed)

Formal charge of Beryllium in BeF₂ = 2 – 0- 2

                                                        = 0

Formal charge of fluorine in BeF₂ = 7 – 6- 1

                                                            = 0

So the formal charge of both the beryllium and fluorine in BeF₂ is 0.

BeF₂ Bond angle

When atoms combines to form stable compound, an angle is formed in between the bonds. The angle formed as result of bond formation between two or more atoms is called bond angle.

Beryllium fluoride is a linear shaped molecule. In a linear shaped molecule the atoms will be arranged in straight line. So the bond angle between the beryllium and fluorine atoms is 180⁰.

BeF₂ Octet rule

Octet rule states that, whenever atoms undergo combination to form stable compounds their outermost shell should be filled with eight electrons. In the case of covalent compound they share their electrons to obey octet rule. In ionic compound they will either lose or gain electrons to make their octet filled.

In the case of beryllium fluoride, beryllium has two electrons and fluorine has seven a electrons in its valence shell. When beryllium shares its two electrons with two fluorine atoms then fluorine got satisfied with octet rule. After bond formation between Be and F the fluorine atom has eight electrons in its outer shell. But beryllium contains only four electrons. Molecules like hydrogen, helium, lithium, beryllium don’t need eight electrons in their valence shell to get stabilised. So beryllium in BeF₂ is an exception to octet rule.

BeF₂ Lone pair of electrons

Some of the electrons present in the valence shell doesn’t participate in bond formation and they will stay with the atom. Those electrons are termed as lone pair of electrons or non bonding electrons.

In beryllium there is no lone pair of electron.

The lone pair of electrons present  in Fluorine atom is 3.

BeF₂ Valence electrons

The electrons connected with an atom which can only participates in bond construction is known as valence electrons.

In Be there is two valence electrons and Fluorine there is seven valence electrons. So in total there is 2+7×2 = 16 valence electrons in BeF₂.

BeF₂ Hybridisation

 Sometimes atomic orbitals with various energies combines to form new orbitals with same energy and shape. This is called hybridisation. Hybrid orbitals are the new orbitals formed by this way. The number of orbitals formed will be equal to the number of orbitals undergo hybridisation.

The electronic configuration of  Be in its ground state is 1s² 2s². In the next step one electron in 2s orbital will be excited to the 2p_x orbital. Then its electronic arrangement changes to 1s² 2s¹ 2p¹. After this the 2s and 2p_x orbital overlap together to form two sp orbitals with same energy. The angle between these two orbitals is 180⁰ and they are oriented in opposite direction.

Then two fluorine atom shares one electron from its 2p_z  orbital to beryllium. This results the formation of  BeF₂ bond. This results the formation two sigma or single bond  between beryllium and fluorine. So the hybridisation in beryllium fluoride is sp hybridisation.

The orbitals formed as result of Hybridisation has 50% s character and 50% p character. This can be also termed as diagonal hybridisation.

BeF₂ Solubility

The capability of the substance to get dissolved in a solvent is called solubility. The frequently used solvents are water, ethanol, acetone, chloroform, ether, CCl₄, benzene. Beryllium fluoride is found to be miscible in water and are sparingly soluble in ethanol.

 Is BeF₂  Ionic or not ?

 A positive charged and negative charged ion attracts together to form ionic bond. These positive and negative ions are cation and anion respectively. A covalent bond is formed by the common distribution of electrons between the atoms with same or different electronegativity value.

Beryllium fluoride is formed by the sharing of atoms between beryllium and fluorine. So BeF₂ is a covalent compound with linear shape.

Is BeF₂ Polar or not ?

BeF₂ is a molecule which exhibits Non polar character. Because the two Be – F bonds are symmetrical to each other their dipole moment got cancelled each other. So the net dipole moment is 0. Therefore Beryllium fluoride is Non polar molecule.

Is BeF₂ Acidic or Basic ?

BeF₂ is acidic in nature. Lewis acid is an acid which can accepts electrons from other atoms. Beryllium fluoride can be a good lewis acid because beryllium can accepts more electrons.

Summary

Beryllium fluoride is an inorganic compound with formula BeF2.It is a white solid which is used as precursor for the synthesis of beryllium. This article explains the lewis structure of  beryllium fluoride and its other properties like its hybridisation, solubility, acidic behaviour and its polar nature.

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CCl₂H₂ Lewis structure, and other important facts are going to be discussed in this article.

Dichloromethane, CCl₂H₂ is an organo chlorine compound. It is a colorless liquid which is volatile in nature and has chloroform like sweet smell. It can be used as a good solvent.

How to draw Lewis structure of  Dichloromethane, CCl₂H₂ ?

Atoms join together to form a stable bond by sharing their electrons. This process can be easily understand by drawing certain simple structures. These structures are called Lewis structure. Generally dots and lines are used to denote electrons and bonds in the Lewis structure.

So the structures designed on the basis of this is called Lewis dot structures.
Before drawing the Lewis structure of dichloromethane we need to understand which of the atoms are present here and their valence electrons.

• In dichloromethane there is one carbon atom attached with two hydrogen and chlorine.  Now let’s see the valence electrons in dichloromethane. Carbon contains four electrons, hydrogen has one and chlorine has seven electrons in their outer shell. So the total number is 4+1×2+7×2= 20 electrons.
• In the second step we draw the symbol of carbon atom surrounded with chlorine and hydrogen atoms. Their valence electrons are also indicated here.

• In the third step we show how they share their electrons each other to form the stable bond.

Dichloromethane, CCl₂H₂  Resonance

When atoms are linked with double bonds and lone pair of electrons, the electrons has a tendency to move across the bonds. This movement cause different structures for one molecule. This process is called resonance and structures are resonating structures.

It is important to maintain the structure of molecule as it is during the movement of electrons. In case of dichloromethane there is no double bond. The lone pair of electrons linked with chlorine atom doesn’t play a role for the making of resonance structure. So there is no resonating structure for dichloromethane.

Dichloromethane, CCl₂H₂  Shape

When two hydrogen atoms of methane got substituted by chlorine, then forms a compound called dichloromethane. The structure of dichloromethane is found to be tetrahedral. It is due to sp³ hybridization.

Dichloromethane, CCl₂H₂   Formal charge

The charge assigned to an atom due its  bond making with other atoms termed as formal charge. There is one equation for finding formal charge. It is

Formal charge =( valence electrons – No. of dots – No. of bonds)
The formal charge of four atoms in dichloromethane is

For carbon = (4-0-4) = 0
For chlorine = (7-6-1) = 0
For hydrogen = (1-0-1) = 0

Hence we understood that the formal charge assigned to dichloromethane is zero.

Dichloromethane, CCl₂H₂   Angle

The bond angle of dichloromethane is 109.5. There is two carbon – chlorine joined and carbon – hydrogen joined bonds are present in dichloromethane. The atoms attached to the central carbon are located on the corners of a tetrahedron.

Dichloromethane, CCl₂H₂   Octet Rule

When there is eight electrons are present in the outermost shell of an atom after bond formation then it is said to be stable. This rule can be called as octet rule. Here carbon and chlorine has eight electrons in the valence shell after bond making. So they fulfill octet rule.

But hydrogen has only two electrons. Certain atoms need not be filled with eight to exist as stable compound. Hydrogen needs only two electrons to remain stable and it is obtained after bond making. So it is stable but don’t obey octet rule due to the absence of eight electrons in its outer shell.

Dichloromethane, CCl₂H₂  Lone pair of electrons

Sometimes the whole valence electrons doesn’t involve in bond making. So those electrons that has no role in bond making process are called lone pair electron.

There is zero lone pair seen in hydrogen and carbon atom of dichlormethane  but we can see 3 lone pair in the chlorine atom. So in total there is six lone pairs are found in dichloromethane.

Dichloromethane, CCl₂H₂   Hybridisation

Atomic orbitals with different energy combines to form new set of orbitals with indifferent energy it is termed as hybridization. The new set formed will be equal to the orbitals got united. The speciality of the new orbitals are its identical shape and energy.

Let’s start with the electronic configuration of carbon first because it is the central atom.
Carbon_{( ground state)}  1s² 2s² 2p²

In the next step what happens is the excitation of one electron from 2s to 2p level. Then

Carbon _{( excited state)} 1s² 2s¹ 2p³

So these three orbitals that is one 2s and three 2p undergo hybridization to make four sp3 hybrid orbitals. At last the two hydrogen and chlorine atoms distributes their electrons to the central located carbon atom to form dichloromethane. The shape of dichloromethane thus made is tetrahedral with angle 109.5⁰. All the bonds are single bonds and are stable.

Dichloromethane, CCl₂H₂   Solubility

The capacity of a substance to be dissolved in a given solvent is its solubility. The solubility ability of compounds will be different. Some will be easily soluble in all solvents but some will not. Usually we use water, ethanol, acetone, ether as solvents.
Dichloromethane is not much soluble in water. It can be made water soluble by decreasing temperature of the system. When temperature is 60 then 5.2 g/L get dissolved, at 60 15.8g/L dissolves. But we found out that dichloromethane is soluble in organic solvents like ethyl acetate, ethanol, hexane, benzene,CCl4, ether, chloroform, phenol, aldehydes and ketones.

 Is Dichloromethane, CCl₂H₂   Ionic or Covalent ?

There are two types of bond, ionic and covalent. First one forms due to attraction between two oppositely charged ions. Latter is because of the mutual distribution of electrons between the atoms.

In dichloromethane there is zero charged ions. All atoms existing here shares their electrons each other to form the compound they want. So they made a covalent bond. So dichloromethane is not at all ionic.

Is Dichloromethane, CCl₂H₂   Acidic or not ?

Dichloromethane is found to be acidic. It acts a good Lewis acid. A Lewis acid has vaccant orbitals to accept electrons. This compound accepts electrons from other bases. So it is a Lewis acid like substance.

Is Dichloromethane, CCl₂H₂   polar or not ?

We all know that dichloromethane has one central carbon joined with two chlorine and hydrogen atoms. Here two carbon- chlorine and carbon- hydrogen bonds can be seen. Chlorine atom present here is electronegative in nature. It’s electronegativity is much more than that of carbon and hydrogen.

So there arises a dipole moment difference between the bonds made here. This is almost equal to 1.6 D. So it’s dipole moment value is not zero. This indicates that dichloromethane is found to be a polar molecule.

Summary

Dichloromethane is a organo chlorine compound. Its molecular weight is 84.93g/mol with refractive index 1.42. It is found in wetlands and emitted into atmosphere due to automobile emissions. It is used as a good solvent.

This article describes that dichlormethane is a covalently bonded molecule with polar behaviour which undergo sp³ hybridisation. It acts like a lewis acid and its valence electrons are also mentioned here.

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Ba₃N₂, its lewis structure, shape, bond angle, hybridisation, stability were briefly discussed in this article.

Barium nitride is a compound with chemical formula Ba₃N₂ having three barium and two nitrogen atoms combined through ionic bond. Its molecular weight is 440 and has various applications.

How to draw Ba₃N₂ lewis structures ?

Lewis structure of a molecule is mainly drawn to understand how the bond formation takes place when two atoms or more got united. The lewis structure of a compound is drawn by considering only the valence electrons present in the outermost shell and it is represented as dots. So the structures drawn by this concept are called lewis dot structures.

Lewis dot structures can be drawn for both covalently bonded and ionic bonded compounds. Barium nitride is a compound having three barium and two nitrogen atoms. Barium is a second group alkaline earth metal and nitrogen is fifteen group element. There are certain rules or steps are there to reach up to the lewis structure of any compound.

• Calculate the total number of valence electrons. Here barium has 2 electrons in its outermost shell and nitrogen has five valence electrons. So the total number of valence electrons in barium nitride, Ba₃N₂ is 2×3+5×2 = 16 electrons.
• Three barium atoms with two valence electrons and two nitrogen atoms with five valence electrons are present in barium nitride, Ba₃N₂.

• Each barium atom donates its two electrons to nitrogen atom to form a barium cation, Ba²⁺. When nitrogen accepts this electrons it get converted to a anion called nitride,N^3-.

• So a positive barium cation and a negative nitride anion formed will undergo electrostatic force of attraction to form a stable compound called barium nitride.

Ba₃N₂  resonance

Resonance can be defined as the movement or the delocalistion of electrons present in an atom of any compound. Resonance can only seen in compounds with double bonds and the electrons involved with these bonds are easy to move across the bonds. While drawing the resonance structure the actual properties like the number of electrons present around the atom shouldn’t change.

Even though there is double bond in barium nitride it is not allowed to move across, because if they do so the molecular structure not exist. So there is no resonance structure for barium nitride.

Ba₃N₂  Shape

Barium nitride is a bent shaped molecule with Ba- N bonds. In which two barium – nitrogen bonds are double bonded while one of the barium is attached to two nitrogen atoms through single bonds.

Ba₃N₂  Formal charge

Formal charge is a charge assigned to an atom when it is get combined with other atoms to form a stable compound. The formal charge assigned to an atom can be easily found out by the below equation

Formal charge of an atom = ( Valence electrons – No. of lone pairs – No. of bonds formed)

Formal charge of  Barium in Ba₃N₂ = 2 – 0- 2

                                                        = 0

Formal charge of  Nitrogen  in Ba₃N₂ = 5 – 2- 3

                                                            = 0

So the formal charge of both the barium and nitrogen in Ba₃N₂ is 0.

Ba₃N₂ Bond angle

Bond angle is the angle made between three atoms when they combine together to form a stable compound. Since barium nitride is a molecule with bent shape its bond angle may be 109.4⁰. Since there is two lone pair of electrons are present in the nitrogen atoms there is a probability for a change.

Ba₃N₂ Octet rule

According to octet rule, when atoms combine together to form compounds they are found to be more stable when their outermost shell are filled with eight electrons. Atoms lose or gain electrons to obey the octet rule. In the case of barium nitride barium loses its two electrons to nitrogen.

Nitrogen atom accepts these two electrons from barium and got satisfied with eight electrons in its valence shell. So nitrogen atom satisfy octet rule.

Ba₃N₂ Lone pair of electrons

Lone pair of electron or non bonding electrons are the electrons present in the valence shell of an atom which doesn’t took participation in bond formation. Since they doesn’t form bonds they can be called as non bonding electrons.

The lone pair of electrons in barium is 0.

The lone pair of electrons in nitrogen is 2.

Ba₃N₂ valence electrons

The electrons present in the valence shell or the outermost shell of an atom is called as its valence electrons.

Number of valence electrons present in barium is 2 and nitrogen is 5.

So the total number of valence electrons in Ba₃N₂ is 16.

Ba₃N₂ Hybridisation

When the atomic orbitals of atoms with slightly different energies intermixes together to form atomic orbitals with same energy and shape that process  is called hybridisation. The new orbitals formed are called hybrid orbitals and their number is equal to that of the orbitals undergo hybridisation.

Hybridisation is a concept that we applied in the case of covalent compounds. Covalent bonds are formed by mutual sharing of electrons between the bonding  atoms. Barium nitride is not formed by this way. Here barium losses its electron while nitrogen accepts that to form bond. A mutual sharing can’t be seen here. So hybridisation can’t be applied for this compound.

Ba₃N₂ Solubility

Solubility can be defined as the ability of a substance or solute to get dissolved in a solvent to form a solution. The most commonly used solvents in field of chemistry is water, ethanol, acetone, ether, benzene etc. Barium nitride is soluble in water and are insoluble in organic solvents.

Barium nitride is a polar molecule and water is also a polar solvent. Therefore barium nitride easily soluble in water. Barium nitride reacts with water to form a solution of barium hydroxide and evolution of ammonia gas takes place.

  Ba₃N₂ + 6H₂O  → 3Ba(OH)₂ + 2NH₃

 Is Ba₃N₂  Ionic or not ?

An ionic bond is formed by the electrostatic force of  attraction between a positive and negative ion. The positive ion is called cation and negative ion is called anion. Barium nitride, Ba₃N₂ is an ionic compound.

Barium donates its two electrons to nitrogen to form Barium cation, Ba²⁺ and nitrogen accepts these electrons to form nitride ion, N^3-. Then these positive and negatively charged atoms attracts to form their ionic bond.

The electronegativity of barium and nitrogen is 0.89 and 3.04 respectively. Their electronegativity difference is 2.15. When compounds have electronegativity value greater than 1.7 then that compound will be ionic in nature. Here 2.15 is greater than 1.7 so barium nitride can be considered as an ionic compound.

Is Ba₃N₂ Polar or not ?

A compound is said to be polar in nature when the electronegativity difference of atoms present is more than 0.4. The electronegativity value of barium is 0.89 and nitrogen is 3.04. Their electronegativity difference is 2.15, which is greater than 0.4. So barium nitride, Ba₃N₂ is polar in its nature.

Is Ba₃N₂ Acidic or Basic ?

Barium nitride is an ionic compound which shows polar behaviour. An ionic compound is said to be acidic when it has hydrogen ion and basic when it has basic ions like hydroxide(OH^–) and oxide(O^2-) present in it.

Ionic compounds without the presence of these ions are called salts and they are formed by acid base reactions. Since there is no hydrogen and hydroxide ions present in barium  nitride it is neither acid nor base. So barium nitride can be considered as a salt.

Summary

Barium nitride, Ba₃N₂ is an ionic compound which is polar in nature. This article briefly explains about its lewis structures, lone pairs, valence electrons and hybridisation. Barium nitride is used as flux in GaN growth medium, precursor of metal nitrides and dopants in optical materials.

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Arsenic pentachloride (AsCl5) features a central arsenic (As) atom with 5 valence electrons, each forming a single bond with five chlorine (Cl) atoms, contributing 7 valence electrons each. The Lewis structure shows five single As-Cl bonds, using 40 valence electrons, with no lone pairs on arsenic. AsCl5 adopts a trigonal bipyramidal geometry, with three Cl atoms in equatorial positions and two in axial positions, resulting in 90° and 120° bond angles. The molecule’s symmetry makes it nonpolar, despite the polar As-Cl bonds due to the electronegativity difference (As: 2.18, Cl: 3.16). This structure influences its reactivity and use in research, though it’s less stable and common than AsCl3.

Arsenic pentachloride,AsCl₅ is a chemical compound formed by arsenic and chlorine. Arsenic chloride has similiar structure like phosphurus pentachloride but has no stable existence.

How to draw AsCl₅ Lewis structure ?

The Lewis dot structures are drawn to get facts related with the bonding in molecules and ions. This mainly deals with the shared pairs of electrons between the atom and the octet rule. While drawing lewis structure only the valence electrons are considered. The valence electrons are denoted as dots in lewis structures. So the structures drawn with the help of this concept is called lewis dot structures.

The lewis structure of Arsenic pentachloride or AsCl­₅ can be drawn easily. Before that it is important to understand how the compound is formed. The atomic number of arsenic is 33 and chlorine is 17. The valence electrons present in the outer  shell of arsenic is 5.

The electrons present in the valence shell of chlorine is 7. Here there are 5 chlorine atoms so the total number of valence electrons of five chlorine atoms is 35. Arsenic pentachloride is a covalent compound formed by the mutual sharing of atoms between one arsenic and five chlorine atoms. So the lewis structure of Arsenic pentachloride can be drawn like this

AsCl₅ Resonance structure

Resonance is the movement of  electrons delocalised in an  atom of a molecule. This is mainly depicted through some contributing structures. Such structures or figures are called as its resonance structures. The resonance structure of arsenic pentachloride is same as its shape. There is no delocalistion of electrons takes place here in this case.

AsCl₅ Shape

Arsenic pentachloride is formed by the sharing of five valence electrons of arsenic with five chlorine atoms. The shape of the compound is found to be triagonal bipyramidal structure. There are five bonds between arsenic and chlorine.

The two bonds are axial bonds and the remaining three is equatorial bonds. The bond length of axial bonds are greater than the equatorial bonds. The bond length of axial and equatorial bonds are 220.7 pm and  210.6 pm respectively.

AsCl₅ Formal charge

Formal charge is a charge assigned to an atom  when all of  its valence electrons are perfectly shared with other atoms to form a chemical bond.

Formal charge of a molecule can be given as,

Formal charge of an atom = [No. of valence electrons –( No. of electrons +  No.of  bonds  formed)].

The total number of valence electrons present in Arsenic is 5, the lone pair of electron in As is 0, the number of  bonds formed by arsenic with five chlorine atoms is 5. So the formal charge of As can be

Formal charge of Arsenic = 5-0-5

= 0

The number of valence electrons present in Chlorine is 7, the electrons available as lone pairs in Cl is 6, the number of  bonds formed with one arsenic  is 1. So the formal charge of Cl will be

Formal charge of  Chlorine = 7-6-1

= 0

The formal charge present in Arsenic and chlorine in AsCl₅ is 0.

AsCl₅ Bond Angle

The Bond angle in a molecule is the angle between the bonds of atoms when different or same atoms combine together to form a compound. AsCl₅ is a compound with five bonds between arsenic and five chlorine atoms with triagonal bipyramidal structure. The bond angle of equitorial bonds in AsCl₅ is 120⁰ and axial bond is 90⁰ respectively.

AsCl₅ Octet rule

The octet rule explains that the atoms are found to be very stable when their valence shell or outermost shell are filled with eight electrons. In the case of arsenic penta chloride there is one arsenic atom and five chlorine atoms are present.

The valence shells of each chlorine atom has 7 electrons when it forms five bond with arsenic then the valence shell of each of chlorine atom has eight electrons. So the octet of chlorine atoms in AsCl₅ is completely satisfied hence it obeys octet rule. While in arsenic its valence shell contains five electrons and need three more to satisfy the octet rule.

But when it forms five bonds with chlorine atoms its valence shell is now filled with ten that is more than eight electrons. So arsenic shows deviation from octet rule. Hence arsenic is considered as a hypervalent molecule.

A hypervalent molecule is a molecule  with one or more elements which has more than eight electrons in its valence shell due to bond formation with other atoms.

AsCl₅ Lone pair of electrons

Lone pair of electrons are the electron pair present in the outermost shell of an atom that is not shared or get bonded to another atom. It can be also called as non bonding electron since it doesn’t took part in a bond formation.

The lone pair of electron in a molecule can be found out through the following equation.

Lone pair of electron in an atom =  ( No. of valence electrons – No. of electrons shared by the atom) /2

Lone pair of electron in As = (5 – 5)/2

= 0

There is no lone pair in Arsenic atom in Arsenic pentachloride

Lone pair of electron in Cl = (7-1)/2

= 3

The lone pair of electrons in Chlorine is 3. Here there are five chlorine atoms each with three lone pair of electrons.

AsCl₅ Valence electrons

Valence electrons are the electrons present in the outermost shell of an atom. Valence electrons participate in a chemical reaction by sharing the electrons to form stable compounds. Before bond formation arsenic has five and chlorine has seven valence electrons in the outermost shell.

After the bond formation arsenic has ten electrons in its valance shell and each chlorine atoms has eight valence electrons in its outermost shell. So the total number of valence electrons present  in arsenic chloride is 40.

AsCl₅ Hybridisation

The intermixing of atomic orbital with slightly different energy to form a set of new orbitals with same energy and shape  is called Hybridisation. This concept gives a good picture about the bond formation in covalent compounds. The number of  hybrid orbitals  formed will be equal to the number of atomic orbitals got hybridised.

The freshly formed those orbitals are called as hybrid orbitals.

The ground state electronic configuration of Arsenic is 3d¹⁰ 4s² 4p³. In its excited state electronic configuration is 4s1 4p3 4d1. One of electron in the 4s is excited to 4d level.

One 4s, three 4p and one 4d orbitals hybridise together to form five sp³d hybrid orbitals with same energy. The five chlorine atoms shares one electron present in its 3p orbital to form five covalent bonds.  So the hybridisation in AsCl₅ is sp³d hybridisation.

AsCl₅ Solubility

Since AsCl₅ is unstable compound its solubility is not found out.

Is AsCl₅ is Acidic or Basic ?

The acidic or basic character of arsenic pentachloride is doesn’t determined due to its unstable nature.

Is AsCl₅ Ionic or Covalent ?

A covalent bond is formed by the mutual sharing of electrons between the bonded atoms. Arsenic pentachloride is formed by through sharing of electrons between arsenic and five chlorine atoms. Therefore Arsenic pentachloride AsCl₅ is a covalent compound.

 Is AsCl₅  Polar or Non polar ?

Arsenic pentachloride is a covalent compound with non – polar nature.

Is AsCl₅ triagonal bipyramidal ?

Arsenic pentachloride is a compound with triagonal bipyramidal geometry with two axial and three equatorial bonds.

Why is AsCl₅ Unstable ?

Arsenic pentachloride is unstable. It due to the incomplete shielding of the 4p orbitals seen in between the nucleus and 4s orbital. Because of this reason  electrons of 4s orbital are less available for bonding. Therefore it is unstable in its nature.

Conclusion

This article explains about full details regarding Arsenic pentachloride, a chemical compound. Its lewis structure, valence electrons, lone pairs, octet rule were discussed here. Inaddition to this its shape,solubility and polar nature are explained. Arsenic pentachloride is a compound with sp³d hybridisation with least stability.  

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