lewis structure

This article is regarding about HSO3- lewis structure and other important characteristics and features. Let’s start with the HSO3- lewis structure.

HSO3- is a non-metal sulfite molecule. It is an oxoanion of sulfur. It is also a conjugate base of sulfurous acid. the central S is sp³ hybridized like in sulfurous acid. One of the -OH bonds is replaced in sulfurous acid by O^–, as H⁺ is released from sulfurous acid. It can act as both acids as well as base as it releases H⁺ as well OH^– under suitable conditions.

Central S is connected via one ketonic O, one -OH group, and other O bearing a negative charge. The negative charge can be delocalized between S and O atoms as they can accumulate the negative charge being an electronegative atom.

Some facts about HSO3-

There is always tautomerism existing between bisulfite anions. This phenomenon is observed in the NMR spectroscopy.  One tautomer has double bonded O and the other has -OH group. HSO3- can be prepared from sulfurous acid by the proton loss or from calcium bisulfite by loss of calcium cation.

H2SO3 = H⁺ + HSO3^–

CaHSO3 = Ca⁺ + HSO3^–

Again, when sulfur dioxide is reacted with a basic solution of a strong base then it gives HSO3^–.

SO₂ + OH^– = HSO₃^–

HSO₃^– is the conjugate base of sulfurous acid having pka 6.97, so it is less basic as well as less acidic. As HSO₃^– is a very weak acid so its conjugate base is SO₃^2-.

HSO₃^– = H⁺ + SO₃^–

Bisulfite is also a good reducing agent, it can give hydrogen easily.

2HSO⁻₃ + O₂ → 2SO²⁻₄ + 2H⁺

1.    How to draw HSO3- lewis structure?

HSO3- lewis structure plays a crucial role in the prediction of the different covalent characteristics of the anion. So, we try to learn how HSO3- lewis structure can be drawn.

First, we count the total valence electrons for the HSO3- lewis structure. The three constituents of HSO3- lewis structure are S, O, and H. the valence electrons for S, O, and H are 6,6, and 1 respectively. So, the total valence electrons for HSO3- lewis structure is (4*6) + 1 + 1 =26 electrons.

The presence of an extra negative charge is a sign of the presence of an extra electron and so we add 1 to the valence electrons.

Now we choose S as the central atom, as it has larger and less electronegative than O.

According to the octet rule the electrons required for HSO3- lewis structure is, 4*8 + 2 +1  = 35 electrons, but the valence electrons of HSO3- lewis structure are 26 electrons. So, shortage of electrons are 35-26 = 9 electrons.

Those shortage 9 electrons will be accumulated by a suitable number of bonds that is  4 bonds and 1 extra electron resides as a negative charge.

As O is more electronegative so negative charge on O is the most favorable case. After assigning all the bonds we should assure all the atoms should be satisfied by their valency.

O is bivalent atoms, so satisfying its valency we add a double bond between S and O. All the lone pairs are assigned over S and o atoms as they contain more electrons in their valence shell.

2.    HSO3- lewis structure shape

HSO3- lewis structure shape is as like H2SO3 molecular shape that is trigonal pyramidal. But the molecular geometry of HSO3- lewis structure is tetrahedral according to VSEPR theory and hybridization value.

In the HSO3- lewis structure central S undergoes sp³ hybridization along with its lone pair and makes π bond with the 3d orbital. So, according to VSEPR (Valence Shell Electrons Pair) theory, the molecule should adopt tetrahedral geometry to avoid any kind of steric repulsion as it is a tetracoordinate molecule, but the shape of the molecule is trigonal planar.

In the shape we check the geometry without the lone pair, only bond pairs are involved and there are three bond pairs responsible for the geometry and the best geometry is trigonal pyramidal.

3.    HSO3- valence electrons

The total valence electrons for HSO3- lewis structure are 26. These 26 electrons are the summation of individual atoms present in the anion.

The central atom S has six valence electrons because it belongs to group 16th, among them two are from 3s and four are from 3p orbital.

O has also six valence electrons as it belongs to the group VIA of the periodic table two electrons of O are from the 2s orbital and the rest four electrons belong to another valence shell 2p orbital.

H has only one valence electron as it is group IA and 1st-period element. The negative charge over the anion is also counted as one electron.

So, the total valence electrons present in the HSO3- lewis structure are (6*4) + 1 + 1 = 26.

4.    HSO3- lewis structure lone pairs

Only S and O contain lone pairs in the HSO3- lewis structure. The total lone pairs are the summation of the individual lone pairs present over O and S atoms.

S has six valence electrons but S has four bond pairs in the HSO3- lewis structure by sharing four electrons. So, the remaining two valence electrons exist as one lone pair over the S.

O has also six valence electrons and two O have two bond pairs via sharing two electrons and the rest of the four valence electrons as two pairs of lone pairs.

But one O has only one bond pair with S and it also contains one extra electron in its valence shell. So, it gets a negative charge and now it has seven electrons and only one bond pair via sharing one electron.

So, the remaining six electrons exist as three pairs of lone pairs for that O atom.

So, the total lone pairs for the HSO3- lewis structure are 1+2+2+3 =8 pairs of lone pairs.

5.    HSO3- lewis structure octet rule

Every atom after bond formation will follow the octet rule for stabilization and gain the noble gas configuration. So, every individual atom in the HSO3- lewis structure also obeys the octet rule for stabilization.

The electronic configuration of S is [Ne]3s²3p⁴. So, from the electronic structure of S, it is shown that it has six electrons in its outermost orbital which are 3s and 3p. It is a group VIA 3rd-period atom of the periodic table, so it has six valence electrons.

S needs two more electrons in its 3p orbital so its 3p orbital is filled because the p orbital can contains a maximum of six electrons as it has three subsets. After gaining two electrons in the p orbital of S, its p orbital is filled like the nearest noble gas and is also stable.

Then S has six electrons in the p orbital and two electrons in the s orbital, so S would have eight electrons in its valence orbital and complete its octet.

In the HSO3- lewis structure S makes three sigma and one π bonds with H and O atoms respectively. One electron is to be promoted to a vacant 3d orbital and that electron is formed a π bond. Now S has three unpaired electrons in its 3p orbital and these three electrons make bonds via sharing electrons.

Now S has six paired electrons in its 3p orbital and two electrons in the 3s orbital. So, finally, S has eight electrons in its valence shell that is in 3s and 3p orbitals and completes its octet like a noble gas.

 O has electronic configuration [He]2s²2p⁴, so it has also six electrons in its valence orbital which are 2s and 2p. As O belongs to group 16^th 2nd-period of periodic table so it also has six valence electrons like S. O has more than half-filled in its 2p orbital and needs two more electrons for the complete octet rule.

Two O atoms formed two bonds in the HSO3- lewis structure by using two electrons and now O has three paired electrons in its p orbital and it has two electrons in its 2s orbital. So, O has eight electrons now and complete its octet also.

One O atom contains a negative charge over it and has five electrons in its 2p orbital and needs one more electron.

That O formed a single bond with S by sharing one of its electrons and now it also has six electrons in its 2p orbital and two electrons in the 2s orbital already. So, that O also has eight electrons in its valence orbital like group 18^th element and completes its octet to gain the stabilization

H has only one electron in 1s orbital, and s orbital contains a maximum of two electrons, so it needs one more electron so it can form an electronic configuration like He. H forms a single bond with O shares one electron and its 1s orbital is completed.

6.    HSO3- lewis structure formal charge

As HSO3- lewis structure contains a negative charge over it so we have to calculate the formal charge to show which atom contains a negative charge.  We assume the same electronegativity for all atoms present in the molecule.

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.

The formal charge over S is, 6-2-(8/2) = 0

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

The formal charge over O is, 6-6-(2/2) = -1

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

SO, one of the O atoms contains a negative charge over it because O has a formal charge of value -1.

7.    HSO3- lewis structure angle

The O-S-O bond angle in HSO3- lewis structure is larger than expected. It should be around 109.5⁰ as central S is sp³ hybridized and geometry-like tetrahedral.

The bond angle is depending on the hybridization as well as VSEPR theory. So, naturally, the AX₃ type molecule having lone pair shows tetrahedral geometry and the bond angle will be 109.5⁰. lone pairs required more space and for that reason, geometry will be tetrahedral.

But if there is a deviation factor present within the molecule then the bond angle will be changed and will show the exception of VSEPR theory. In the HSO3- lewis structure there is a lone pair along with a double bond. So, there is massive lone pair-bond pair repulsion occurs. To minimize that repulsion molecule changes its geometry to trigonal pyramidal.

But the bond angle for trigonal planar is 120⁰. But there is a lone pair and bond pair repulsion the central molecule aligns the bond angle lower than 120⁰ which is 113⁰ for stable configuration, but the bond angle is higher than 109.5⁰.

8.    HSO3- lewis structure resonance

Due to the presence of excess electron density in the HSO3- lewis structure there will electrons cloud delocalization will be occurred. This phenomenon refers to resonance.

There will be three different resonating structures of HSO3- lewis structure that will be possible. Among all only structure III is the most stable canonical form of the molecule as it contains a higher number of covalent bonds so it is the most stable and most contributing as well.

The structure I and II are similar so, they have lesser stability than structure I.

9.    HSO3- hybridization

In the HSO3- lewis structure central S atom should be sp³ hybridized. There are different atoms present with different orbitals having different energy. So, they undergo hybridization to form hybrid orbitals having equivalent energy to form a stable bonding.

The hybridization of N is calculated by 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.

So, the hybridization of central S is, ½(6+1+1) = 4(sp³)

Structure	Hybridization value	State of hybridization of central atom	Bond angle
Linear	2	sp /sd / pd	1800
Planner trigonal	3	sp2	1200
Tetrahedral	4	sd3/ sp3	109.50
Trigonal bipyramidal	5	sp3d/dsp3	900 (axial), 1200(equatorial)
Octahedral	6	sp3d2/ d2sp3	900
Pentagonal bipyramidal	7	sp3d3/d3sp3	900,720

So, we can conclude from the above table if the hybridization is involved within 4 orbitals then the central tom should be sp³ hybridized.

Now we can understand the hybridization of S and the bond formation.

Again, from the box diagram, we can see that one of the electrons of S from the p orbital is get promoted to the vacant 3d orbital and that electron is forming a π bond with O which is not involved in hybridization. So, in the HSO3- lewis structure there will be one d_π-p_π bonding will be formed.

10.  HSO3- solubility

HSO3- is mostly water-soluble but it is also soluble in the following solutions,

• CCl4
• Methanol
• Benzene
• Toluene

11.  Is HSO3- soluble in water

Yes, HSO3- is water soluble.

The molecule is an anion and for this reason, it has some polarity and for this reason, it is soluble in polar solvents like water (like dissolves like).

12.  Is HSo3- an acid or base?

HSO3- acts as both acids as well as the base.

HSO3- is a conjugate base of H2SO3, so here it can act as a base and can donate -OH.

But in an aqueous solution HSO3- can release H⁺ and acts as an acid. its conjugate base is SO₃^2-.

13.  Is HSO3- a strong acid?

No, HSO3- is a very weak acid.

The pka value of this molecule is very high and positive making it weak and acidic. In water solution, it dissociates very slowly. But its conjugate acid sulfurous acid is a moderately strong acid.

14.  Is HSO3- a strong base?

No, HSO3- is not a strong base.

The pka value of HSO3- is nearly neutral. So, neither it is a strong acid nor neither is it a very strong base.

15.  Is HSO3- a bronsted base?

No, HSO3- is not a Bronsted base.

It can be thought that HSO3- can be accepted as a proton or H⁺ easily but after accepting proton it is transferred to sulfurous acid. So, once it accepted the proton but after accepting proton it will be no longer a base change to an acid.

16.  Is HSO3- aqueous?

No. HSO3- is not aqueous.

It is a colorless liquid in the physical state but in an aqueous solution is dissociated its proton is very slowly and no longer stays in its original form.

17.  Is HSO3- a lewis acid?

Yes, HSO3- acts as a lewis acid.

S has an energetically accessible vacant 3d orbital. So,  lone pairs from the suitable lewis base can be accepted there and make HSO3- as lewis acid.

18.  Is HSO3- neutral?

No, HSO3- is charged anion.

There will be a negative charge present over the molecule, actually more precisely the negative charge is on the O atom. So, the molecule is an acid radical.

19.  Is HSO3- polar or nonpolar?

HSO3- is a polar molecule.

There is a charge difference between S and O atoms. So, a net dipole moment will flow from the S to O site and due to the asymmetric shape of the molecule there is no chance of canceling out the dipole moment and the molecule has a resultant dipole moment. So, HSO3- is a polar molecule.

20.  Is HSO3- a conjugate acid or base?

HSO3- is both con jugate acid as well as the conjugate base.

HSO3- is the conjugate base of sulfurous acid. whereas it is an acid itself, which conjugate base is SO₃^2-. So, HSO3- can be both conjugate acid as well as a conjugate base.

21.  Is HSO3- a polyatomic ion?

Yes, HSO3- is a polyatomic ion.

HSO3- consists of three types of ion, the negative charge is over the O atom. So, it is a polyatomic anion.

Conclusion

HSO3- is a conjugate base of sulfurous acid. but hSo3- itself is an acid but very weak. It slowly ionized in a water solution.

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In this article, “n2h4 lewis structure”, different facts on hydrazine like lewis structure drawing, calculation of formal charge, valence electrons, lone pairs, polarity with some relevant topics are discussed briefly.

N₂H₄or hydrazine is an inorganic colourless and flammable liquid compound having ammonia like odour. It has a molar mass 32.0452 g/mol and density 1.021 g/cm³. The N-N single bond distance is 1.45 A⁰ having a pyramidal geometry. Hydrazine is a water-soluble compound. It is a polar compound having a permanent dipole moment.

Let’s highlight the following facts on hydrazine (N₂H₄).

How to draw N₂H₄ lewis structure?

Lewis structure is a molecular structural representation showing lone pairs or nonbonding electrons around the atoms.

1. Determining the valence electrons:  Due to having a significant role of valence shell, finding out the number of valence electrons is the most important factor. The constituent atoms, nitrogen and hydrogen have five and one electrons in their respective valence shell.
2. Finding out the bonding electrons: The two nitrogen atoms are bonded with each other by one single bond and four hydrogen atoms are also attached with two nitrogen atoms through four sigma bonds. Therefore, total bonding electrons are (5×2) = 10
3. Finding out the nonbonding electrons: In hydrazine, only nitrogen contains nonbonding electrons or lone pair. Each nitrogen atom has two nonbonding electrons.

N₂H₄ Lewis Structure Shape

Molecular shape can only be determined if the hybridization of the central atom is known because the hybridization decides the geometry of any molecule like-

Hybridization of central atom	Geometry
sp	Linear
sp2	Planar
sp3	Tetrahedral
sp3d	Trigonal bipyramidal (TBP)
sp3d2	Octahedral

The above table only will be followed if no repulsive factors are present. The repulsion can be created by the presence of lone pair-lone pair, lone pair-bond pair and bond pair-bond pair repulsion present in the molecule.

In hydrazine, nitrogen is central atom and both the nitrogen is sp³ hybridized having a pair of nonbonding electrons in each of the nitrogen. According to the above table containing hybridization and its corresponding structure, the structure or shape of N₂H₄ should be tetrahedral. But due to presence of nitrogen lone pair, N₂H₄ faces lone pair-lone pair and lone pair-bond pair repulsion and thus its molecular shape is distorted from its geometrical or ideal structure. The shape of hydrazine is trigonal pyramidal (ammonia like structure).

N₂H₄ Lewis Structure Formal Charge

In a molecule, the charge in each of the constituent atom are called as formal charge. Determining the most stable lewis structure is one of the significant use of calculation of formal charge.

• Formal charge = Total number of valance electrons – number of electrons remain as nonbonded – (number of electrons involved in bond formation/2)
• Formal charge of each of the nitrogen atom = 5 – 2 – (6/2) = 0
• Formal charge of each of the four hydrogen atoms = 1 – 0 – (2/2) = 0

From the formal charge calculation, it is clear that none of the constituent atom carry any charge in hydrazine.

N₂H₄ Lewis Structure Angle

Hybridization also determines the angle between two bonds or the angle containing central atom and its two substituent atoms in any molecule. Every bond angle is constant with corresponding to each of the hybridization if no repulsion is present in that molecule.

As N₂H₄ is a sp³ hybridized molecule, the ideal bond angle should be 109.5⁰. But due to facing repulsion involving lone pair and bond pair, the bond angle in hydrazine is slightly deviated from the actual bond angle. The bond angle shows the value between 107⁰– 109.5⁰(bond angle of ammonia 107⁰) because of the presence of lone pair-bond pair and lone pair-lone pair repulsion which decreases the bond angle from ideal. Thus, this deviation occurs.

N₂H₄ Lewis Structure Octet Rule

Octet rule states that atoms gain such electron configuration in their respective valence shell through sharing (covalent compound) or complete transferring (ionic compound) which matches with their nearest noble gas electron configuration (complete shell configuration).

Hydrazine is such type of molecule in which, all the constituent atoms obey octet rule. Nitrogen has five outer most shell electrons and when it forms bond with one nitrogen and two hydrogen atoms, it gains three more electrons in its valence shell. Therefore, the number of electrons in its valence shell (5+3) =8, which resembles with the electron configuration of its nearest noble gas, neon (2s² 2p⁶).

Hydrogen does not follow octet, rather it follows duplet, having two electrons in its valence shell. After having two electrons it matches with the valence shell electron configuration of Helium (1s²), nearest noble gas of hydrogen.

N₂H₄ Lewis Structure Lone Pairs

Lone pairs are those valence electrons which are shown around the respective atoms as electron dots in lewis structure and does not participate in bond formation.

• Nonbonded electron = Total number of valance electron – number of bonded electrons.
• Nonbonding electrons in each of the two nitrogen atoms = 5 – 3 = 2 or 1 pair of lone electron.
• Nonbonding electrons in each of the four hydrogen atoms = 1 – 1 = 0

Therefore, total number of nonbonding electrons = 2×2 = 4.

N₂H₄ Valence Electrons

Valence electrons reside in the outer most shell of any atom and involved in bond formation due to greater reactivity. Because the attraction of nucleus is least in the outer most shell.

N₂H₄ is made of two nitrogen and four hydrogen atoms. Nitrogen has electron configuration 1s² 2s² 2p³. The 2s and 2p electrons are regarded as valence shell electrons. Thus, the number of outer most shell electrons in nitrogen atom is 5. Hydrogen has one electron in 1s orbital (1s¹) and it is its valence electrons.

Therefore, total number of valence electrons in hydrazine = (2×2) + (1×4) = 8

Is N₂H₄ an electrolyte?

Electrolytes which are containing ions are dissolved in water and dissociated into two oppositely charged ions in aqueous solution. Electrolytes are basically ionic compound.

N₂H₄ is not an electrolyte because it is a covalent compound. It cannot be dissociated into two oppositely charged ions.

Is N₂H₄ ionic or covalent?

The basic difference between ionic and covalent compound is that valence electrons are completely transferred from one atom to another atom in ionic compound and are shared between two atoms in covalent compound depending upon the electronegativity difference.

N₂H₄ is a covalent compound because the electronegativity difference between nitrogen and hydrogen is not so high and both are nonmetal atoms. Valence shell electrons of each of the constituent atoms (two nitrogen and four hydrogen) are shared between them, not completely transferred from the valence shell of one atom having lesser electronegativity to the valence shell of another atom with greater electronegativity like any other ionic compound.

Bonding electrons are shifted towards the nitrogen due to having greater electronegativity with comparing to hydrogen.

Therefore, N₂H₄ is a covalent compound with six sigma covalent bonds.

Is N₂H₄ polar or nonpolar?

Presence of dipole moment makes a molecule polar and a molecule with zero dipole moment is considered as nonpolar. Polarity depends upon the electronegativity difference between the atoms involved in a bond formation and the orientation of the polar bonds. Though a molecule contains polar bonds but sometimes it can be nonpolar due to mutual cancellation of the direction of the polar bonds.

N₂H₄ is a polar molecule (µ= 1.85 D) as there is a difference of electronegativity between nitrogen and hydrogen, which makes the N-H bonds polar. The structure of N₂H₄ is trigonal pyramidal. Thus, mutual cancellation of the polar N-H bonds cannot be happened.

Therefore, N₂H₄ is a polar molecule.

Is N₂H₄ an acid or base?

N2H4 is a strong base even stronger than NH_3. It is a lewis base which can donate nonbonding electrons to the acid or any electron deficient atom or molecule. The two lone pairs of two nitrogen atoms make the hydrazine a strong base than ammonia having one nitrogen atom.

Aqueous solution of hydrazine (64 weight %) is highly alkaline in nature having pH = 12.75.

Is N₂H₄ a hydride?

N₂H₄ is basically a pnictogen hydride. Group-15 elements (N, P, As, Sb, Bi) are considered as pnictogen molecules. It is not a metal hydride like NaH. But hydrazine is also a very good reducing agent like any metal hydrides.

Is hydrazine corrosive?

Hydrazine or N₂H₄ is highly toxic substance if it is used in solution (NH₂NH₂. xH₂O). It can cause different complications in living body like skin and eye irritation, nausea, vomiting, breathing problem, headache, dizziness, depression lethargy and many more. Due to excessive use of hydrazone, organ damage like kidney, liver and central nervous system (CNS) can be happened.

Is hydrazine conjugate acid?

It is the conjugate base of hydrazinium ion (N₂H₅⁺). After elimination of one hydrogen atom from N₂H₅⁺, hydrazine is formed. Due to being a strong base, hydrazine can easily accept an H⁺ ion and form N₂H₅⁺. Thus, it is a conjugate base.

Does N₂H₄ dissolve in water?

Yes, N₂H₄ is a water-soluble liquid. It is also soluble in ethanol. N₂H₄ is a polar compound having a permanent dipole moment. Therefore, polar protic solvent can dissolve it.

Does N₂H₄ have hydrogen bonding?

Yes, N₂H₄ has hydrogen bonding. Hydrogen bonding can be two types-

1. Intramolecular hydrogen bonding (H-bonding between the atoms of same molecule).
2. Intermolecular hydrogen bonding (H-bonding between two molecules).

Hydrogen bonding is formed between a highly electronegative atoms and hydrogen atoms attached with an electronegative atom or polar group.

In N₂H₄, nitrogen is an electronegative atom and it participates in intermolecular hydrogen bonding (nitrogen from one hydrazine molecule with the hydrogen of another hydrazine molecule) with hydrogen atom.

Is N₂H₄ stable?

No, hydrazine is an unstable compound. It has two nitrogen atoms having two lone pairs which are facing repulsion from each other. Because nitrogen is a small atom and repulsion is greater in case of nitrogen with respect to other atoms of group-15 atoms. Thus, the N-N bond in N₂H₄ becomes weak and make hydrazine an unstable compound.

Conclusion

N₂H₄ is a trigonal pyramidal compound with a bond angle less than 109.5⁰. It is dissolved in water due to its polar nature and being a covalent compound. Excessive use of hydrazine can cause hazards to living body due to its high toxicity.

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HCO3- Lewis structure is reliable in denoting considerable chemical and physical properties of Bicarbonate. As Lewis structure brings forth a fundamental sketch of HCO3-, it is effective in highlighting the electronic fact about the compound.

HCO3- Lewis structure and the characteristics of this organic compound will be presented in a well-structured manner through this article. Several physical properties and chemical facts will be illustrated in this study to clarify the significance of drawing its Lewis structure.

Drawing HCO3^– Lewis structure

Drawing Lewis structure of Bicarbonate ion (HCO3-) is quite easy. This Lewis structure refers to the electronic structure of the compound imposing the sharing process. It highlights choice of central atom and the bond type generated by the shared electrons. Lewis structure formation  is followed by few easy steps. The systematic progression of the electron share procedure helps to identify some chemical facts about HCO3-.

Step 1: Finding the number of valence electrons present in the element participating in the formation of HCO3- ion is the fundamental step of drawing Lewis structure.

Step 2: Second step highlights the calculation of bond pairs that are assembled by the elements by sharing their valence electrons with each other.

Step 3: In this step the atom that is capable of holding the centre position is found by evaluating its electronegativity and number if participated atoms. In HCO3- ion, Carbon holds this position as electronegativity of Hydrogen is lower than carbon. Oxygen cannot stay in middle as three atoms participate in bonding.

Step 4: The fourth step significantly process the skeleton of the Lewis structure by determining the position of atoms. Connecting the paired electrons of different atoms by Sigma and Pi bonds in HCO3 is done in this step.

Step 5: Putting the other remaining electrons of oxygen around the atoms in the structure completes the whole Lewis structure. The electrons are denoted by dots.

HCO3- Lewis structure resonance

Lewis structure of compounds containing negative ions and pi bonds are reliable developing more than one resonating structure. Resonance take place in a compound due to the tendency of extra negative ion to create pi binds by breaking another pi bond present in the compound.

In HCO3-, one oxygen atom creates double bond with Carbon and another two create single bonds with the same and one of those hold a negative charge with the presence of extra electron. That electron influences the compound to impose resonance.

HCO3- Lewis structure shape

The position of central atom and bond angle are the factors that determine the shape of the compound. Lewis structure is reliable sketch of compounds, which insists information about shape of the compounds.

According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the shape of Bicarbonate ion is Trigonal planner. The compound to minimize the problem of electron pair repulsion obtains this shape.

HCO3- Lewis structure formal charge

Lewis structure of compound identifies the formal charge of the individual elements participate in the formation of the compound. There is a specific formula followed by the chemists to identify the formal charge of individual elements.

The formula is Formal charge = Number of valence electrons – Number of nonbonding valence electrons – (Bonding electrons/2)

Formal charge of carbon = (4-0-(4/2)) = 2

Formal charge of Oxygen with negative charge = -1

Formal charge of other two oxygen = (7-6-(1/2)) =0.5

Formal charge of Hydrogen = (1-0-(1/2)) = 0.5

The above calculation is exposing that this large size ion has a net charge of -1.

HCO3- Lewis structure angle

The shape or geometry of the compounds is responsible for recognising bond angle held by the overall structure. Lewis structure initiates the process of identifying the angle of between the bonds created by element through electron share.

An ideal angle of 120° is possessed by Bicarbonate ion. HCO3- has ben obtained with an idea shape of Triginal planner that denotes that the compound has 120° of bond angle.

HCO3- Lewis structure octet rule

Octet rule is key driver for manipulating the elements to undergo electron-sharing mechanisms. This rule executes the fact that each element in the periodic table wants to adopt eight electrons in its last energy level to achieve ultimate stability like their nearest noble gas element (Such as Helium, Argon, Redon, Xenon and Krypton).

Octet rule is fulfilled by the compound through donating the extra electron from valence shell of adopting electrons from other electrons to pack the deficiency of electron. In HCO3-, carbon, the central; atom shares its four electrons with oxygen atoms an adopt four electrons from them to make the last energy level filled with eight electrons.

HCO3- Lewis structure lone pairs

Detection of the presence of the lone pairs in the compounds is supported by Lewis structure, as this structure is reliable in implementing number and position of electrons in the compound.

Bicarbonate ion contains lone pair on oxygen atoms only as all the eight electron pairs of carbon are bonded. In right oxygen, two lone pairs and in left oxygen three lone pairs are present. The oxygen attached with hydrogen also contain two lone pairs only.  Therefore, the total number of lone pairs present in the structure of HCO3- is seven.

HCO3- valence electrons

Calculating the number of valence electrons is the most important factor for each atom to identify its deficiency or excesses of electrons. This calculation initiates the process of drawing Lewis structure of a compound.

The number of valence electron present in Carbon is four, in each of the oxygen it is seven. Hydrogen holds one valence electron. The total number of valence electron in HCO3- is (4+(3*7)+1) = 26.

HCO3- hybridization

The presence of lone pairs and bond pairs determine the hybridisation of the compounds. Geometric shape of the compounds is obtained from the Lewis structure of ions or compounds. This is a feature relates the fact of hybridisation.

Sp2 hybridisation is notice in HCO3- ion.  The number of lone pairs on the central atom (C) is zero and it has three sigma bonds with steric number of three. These criteria indicate sp2 hybridisation of Bicarbonate ion.

HCO3- solubility

Solubility of ions is highly dependent on the charge contained by the ions. Density of charges and energy inside the compounds are significant factor to identify solubility of the compounds.

HCO3- is highly soluble in water and slightly soluble in solvent containing OH (Hydroxyl) group. The bicarbonate salts are insoluble in acidic solvents.

HCO3- soluble in water

A single anion cannot be soluble in water it should always be bonded with a cation and form salt to show solubility in water. Bond strength is the feature, which determines the soluble nature of a compound or salt.

Maximum salts with Bicarbonate ion are highly soluble in water. Carbonates such as Ca(HCO3), Mg(HCO3) and many more are quite soluble in water.

HCO3- an electrolyte

Goof dissociation ability in solution refers to be a good electrolyte. After dissociating into separate ions, it helps the solution to conduct electricity superiorly, which is considered as most viable property of an electrolyte.

Bicarbonate is an electrolyte (22-29 mmol/L) as it displays the dissociation of H+ ion from the complex ionic structure. This negatively charged ion is helpful for maintaining pH balance in body and conduct electricity in molten state as well.

HCO3- a strong electrolyte

Bicarbonate ion is no doubt an electrolyte as it is capable of leaving H+ ion. giving out free ion can incorporate ability in the compounds to shoe competency as electrolyte by making them conduct electricity.

Conjugate acid of HCO3- (H2CO3) and Bicarbonate ion both are not strong electrolyte as the existence of free H+ ions in molten state is unstable which makes it is a weak base as well.

HCO3- acidic or basic

Acidic or basic nature of compounds or ions depends on the factor of having H+ and OH- ions. The number of H+ and OH- determines pH level of the compound that is supposed to describe the nature of the compound or ion.

HCO3- contains both H+ and OH- ions which denotes hybrid nature of the ion. Bicarbonate ion is generally noticed to be basic in nature but sometimes is exposes acidic behaviour as well.

HCO3- a strong acid

Strength of acidity depends on the free movement of H+ ions in a compound. in HCO3- the H+ ions do not impose free movements in solution which is refer to opposite characteristic for being a strong acid.

HCO3- is a weak acid as well as weak base. Naturally, it does not show dramatic change in pH level after being soluble in water. The H+ ions attached with bicarbonate ion, which highlights its basic appearance.  Hydrogen ions do not get dissociated in a huge amount which relies on the fact that the ion is a weak acid as well.

HCO3- polyprotic acid

Polyprotic acids refer to those acids which are capable of donating more than one proton (H+). Capacity of donating two or three or more than three protons respectively makes Polyprotic acids distinguishable from  Diprotic and Triprotic acids.

HCO3- is basically a weak base by nature still its acid form can donate one H+ but not more than that. Therefore, Bicarbonate ion cannot be considered as Polyprotic acid rather it can be presumed that it has a few potentiality in exposing Monoprotic nature.

HCO3- a Lewis acid

A Lewis acid refers to the elements which contain empty orbitals where it can accept electron pairs. Lewis acids has ability of accepting electron whereas Lewis bases are capable of donating electrons.

Bicarbonate is a Bonsted-Lowry acid, which cannot accept electrons. It is able to accept proton from HCL to form its conjugate acid that is carbonic acid, H2CO3. Therefore, HCO3- is not a Lewis acid.

HCO3- an Arrhenius acid

Arrhenius acids are those elements, which can readily lose protons (H+). Only criteria for losing H+ is that the element must be in molten state that is on dissociation in water that could release H+ ions.

Bicarbonate ion has been identified to donate one H+ ion at a time in molten state and form CO32- ion. Besides, the ion is active in donating OH- ion as well to give out CO2. Therefore, it can be considered as both Arrhenius acid and base.

HCO3- polar or nonpolar

Polarity depends on shape and bonding of the compounds. On the other hand difference between electronegativity of the elements also delivers a certain amount of polarity to the compounds.

In HCO3- the elements have huge difference in electronegativity and the shape of the compound is not symmetric as well. Therefore, a dipole-dipole interaction takes place among the elements, which makes it polar by nature.

HCO3- linear

Linear shape can be noticed on those compounds where two atoms are attached with one central atom and the angle of the compound is noticed to be 180°. Horizontal alignment is present in the linear compounds.

HCO3- is absolutely differ from linear its central atom, carbon holds three oxygen atoms around it. One oxygen is attached with double bonds and another two creates single bond with carbon.

HCO3- paramagnetic or diamagnetic

Presence of only unpaired electrons in any compound makes it diamagnetic whereas presence of only one unpaired electron refers to paramagnetic nature of a compound.

HCO3- is neither diamagnetic not paramagnetic as all the electrons in the compound are paired it has total 12 pairs of electrons where eight pairs are belonging from lone pair category.

HCO3- boiling point

the particular temperature at which a compound can change its liquid state into vapour is called the boiling point of that compound.

Bicarbonate ion itself cannot show physical property of boiling. When it is conjugated with any metal such as Sodium the overall molten state of that compound can impose a specific boiling point that is 851°C.

HCO3- bond angle

Lewis structure is a valid factor that reveals the angle of the bonds in any compound. Besides, VSEPR theory also effectively insists the fact of holding suitable bond angle adopted by the composite structure of elements.

The bond angle of Bicarbonate ion (HCO3-) has been identified120° through VSEPR theory. This theory says that this HCO3-wants to cut off the effect of lone pair lone pair and lone pair repulsions from its geometry. Therefore, for having a stable Trigonal Planner shapes with the angle of 120°.

HCO3- diprotic

Diprotic acids are those acids, which contain two proton or H+ ions as an important part of compounds. Carbonic acid is a great example of Diprotic acids, it hold two H+ ions and can donate one to gives out HCO3-, Bicarbonate ion. 

HCO3- is not diprotic as it has only one proton, which is not even readily donated by the ion rather than in molten state.

HCO3- ionic or covalent

When the atoms permanently donate their electrons to another atoms they make ionic bonds, when partially electron share takes place amid atoms the they form covalent bonds. According to tis bonding abilities the chemical nature of compounds are judged in chemistry.

Bicarbonate ion is formed by Hydrogen, oxygen and carbon by sharing valence electrons with each other partially to fill octet state. It helps them to generate sigma bonds with covalent structure. Therefore, the complex ion can be considered as a covalent compound.

HCO3- amphiprotic

Water is a great example of amphiprotic compound, which refers to the property of both accepting and donating proton. Water can Release H+ and OH- ions both Similarly HCO3- is also capable of donating both H+ and OH- ions.

Bicarbonate ion is able to accept and donate H+ ions, which deliberately impose the information that this ion is amphiprotic like Water. By losing proton, it gives carbonate ion and gaining the same it gives carbonic acid.

HCO3- a conjugate acid or base

According to Bronsted-Lowry Acid-base theory, when an acid donate one or more protons to a base it is considered as Conjugate acid of that particular base. Similarly, when a base loses its hydrogen ions as a reverse reaction that is called conjugate base.

Bicarbonate is a conjugate base of carbonic acid as when carbonic acid loses it Hydrogen ions HCO3- ion forms readily. Besides, when CO32- is formed from dissociation of H+ ion from acid HCO3-.

HCO3- a proton donor

Proton donor refers to that compounds which are good donor of H+ ions. According to chemical facts of carbonic acid, it can be said that Carbonic acid is able to lose proton and produce HCO3- ion fluently.  Therefore, H2CO3 is a proton donor.

Acid HCO3- also loses proton (H+) in molten state but cannot be stabilised in the dissociated form for long which makes it’s a bad proton donor.  It works as good  conjugate base.

HCO3- an electrolyte

Bicarbonate ion is reliable in highlighting its ability of losing free H+ electrons. Though the free electrons are not stable enough in solutions, the complex ion is capable of conducting electricity.

HCO3- is regulatory substance in human body, which help to balance acidity in Kidneys. The complex structure of Bicarbonate after bonding with sodium, potassium and chlorides it becomes an electrolyte and regulates pH balance in body.

HCO3- a polyatomic ion

Polyatomic ions have more than two different atoms in its geometry. Different physical properties of different elements refer to polyatomic structure of the compounds.

HCO3- is a polyatomic ion as it is containing three Oxygen atoms, one carbon and one Hydrogen atom. Hydrocarbonate contains carbon oxoanion, which is the result of removal of proton from carbonic acid.

HCO3- a precipitate

Hydrocabonate is not a precipitate itself but it has the property of giving precipitation of some compounds after added with metals like Sodium, Potassium and few more.

When NaCl is added with NH4HCO3, it gives out a precipitation of NaHCO3 that is Sodium hydrocarbonate. Here the ion shows its ability in forming precipitate.

We can conclude that the Lewis structure of bicarbonate ion (HCO3-) is faithful to reveal internal facts regarding electronic arrangement of the ion.  The VSEPR theory has been evaluated to identify the shape and angle of the compound through describing lone pair and bond pair structure of the HCO3-.  I have implemented both physical and chemical both kind of properties of Bicarbonate ion in this article. 

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In this article we want to discuss about cr2o3 lewis structure, characteristics and 21 most important characteristics regarding this topic.

Cr2o3 is mainly used in color industry which acts as a pigment. It is generally insoluble in water and it is an amphoteric oxide. Naturally it occurs as a dark green and hexagonal crystalline solid. For the preparation of chromium metal, for polishing of stainless steel cr2o3 is largely used.

Cr2o3 Lewis Structure Drawing

In cr2o3, out of 3 o atoms 1 o atom is shared both by cr atoms by covalent sigma bonds. 2 cr atoms forms 1 sigma and 1 pi bonds with o atoms.

The whole molecule is arrangd in a tetrahedral manner in which central o atom forms 2 bond with 2 cr atoms and it contains 2 lone pair and in all aspect all these bonds are purely covalent and formed by sharing of electrons. In cr2o3, terminal o atoms contain 2 lone pairs each.

Cr2o3 Lewis Structure Shape

In cr2o3 lewis structure, the central o atom is sp3 hybridized. This is because of the fact that it contains 2 sigma bonds with two cr atoms and remaining hybrid orbital contain 2 pairs. According to sp3 hybridization the structure should be tetrahedral but the actual shape is bent / V-shaped.

Cr2o3 Lewis Structure Formal Charges

The formal charge on the central o atom in cr2o3=6-4/2-4=0.

Formal charge on terminal oxygen atom in cr2o3=6-4/2-4=0.

Formal charge on 2 cr atoms in cr2o3=6-6/2-3=0.

Hence formal charge on central o atom in cr2o3 is 0 and also two o terminal atoms, two cr atoms also contain o formal charge. Hence this compound is overall electrically neutral.

Cr2o3 lewis Structure Lone Pairs

The lone pairs mean how many no of unshared electrons present in cr2o3 that does not take part in bonding. This can be calculated by the following way-

Lone pair present on central o atom in cr2o3=6-4=2 lone pairs.

Lone pair present on terminal cr atom in cr2o3=6-6=0 i.e. 0 lone pair of electron.

Lone pair present on terminal o atoms in cr2o3=6-4=2 lone pairs.

In cr2o3 compound these nonbonding electron pair are shown on the above mentioned atoms as electron dots.

Cr2O3 Hybridization

During hybridization means during bond formation central o atom uses sp3 hybrid orbital to form cr2o3 compound. Central o atom has 6 valance electron out of which 2 unpaired electrons is used for the formation of 2 sigma bonds with two cr atoms. Two cr atoms has 6 valance electron out of which 2 are used in bonding with 2 terminal o atoms.

2 terminal o atoms forms 1 sigma and 1 pi bonds with cr atoms by using its 2 unpaired electrons and remaining 4 electrons which does not take part in bonding with cr atoms present as lone pair of electron. Hence in cr2o3, central o atom uses sp3 hybrid orbital to form cr2o3 compound. according to sp3 hybridization its structure is pyramidal not tetrahedral due to presence of 2 lone pairs.

Cr2O3 solubility

Cr2o3 is insoluble in water, ethanol and even in acetone and also acids. By considering the fact mentioned above it is concluded that cr2o3 is a nonpolar compound. As it is nonpolar in nature, it is soluble in nonpolar solvents like carbon tetrachloride, carbon disulphide etc.

Cr2O3 valance electrons

The total no of valance elctron in cr2o3 is equal to the valance electron present in cr and o atoms. Cr contains 6 and O also contains 6 valance electron. The total no of valance electron present in cr2o3 is (6*2)+(6*3)=12+18=30.

Cr2O3 lewis structure angle

In cr2o3 lewis structure, central o atom is bonded with 2 cr atoms with which 2 o atoms are double bonded with cr atoms in a tetrahedral manner. The central O atom is sp3 hybridized in cr2o3 and also contain 2 lone pairs. As the structure is pyramidal, the angle should be 104.50.

Cr2o3 lewis Structure Resonance

In cr2o3 lewis structure when electron pair movement i.e resonance takes place, 3 resonating structure is obtained. In cr2o3, lone pair of electron present on central o atom is delocalized with the cr=o bonds i.e. with vacant ∏* orbital of cr=o bonds.

Cr2o3 lewis structure Octet Rule

The lewis structure of cr2o3 shows that all the atoms in cr2o3 fulfill their octet. In cr2o3, the central o atom forms 2 sigma bonds with 2 cr atoms and also contains 2 lone pairs. That is why, central o atom satisfy its octet. Two terminal o atom forms double bond with cr atom and also contain 2 lone pairs.

By this terminal o atoms fulfill their octet. 2 cr atoms forms 2 sigma bond and 1 pi bond with central and terminal o atoms. It also contains 1 lone pair. Hence it contains total of 8 electrons and fulfill its octet. Hence by applying octet rule the compound cr2o3 is a stable compound.

Cr2o3 Polar Or Nonpolar?

Cr2O3 is nonpolar compound. As we seen that it is a nonpolar compound it is insoluble in polar solvents like water. Its lattice energy is higher than hydration energy. To break it into Cr3+ and O2- ions higher energy is required. For this reason, it usually does not break into cr3+ and O2- ions.

Is cr2o3 ionic?

Cr2O3 is ionic compound. When cr2o3 ionizes, 2cr3+ ions and 3o2- ions are produced. As therefore, Cr2O3 is overall a neutral compound because total 6 positive charges is neutralized by total 6 negative charges. As because cr is metallic in nature, it acquires positive charge and o is nonmetallic in nature it acquires negative charge.

Is cr2o3 acidic or basic?

Cr2O3 is amphoteric in nature i.e. it both reacts with acid as well as base. When it reacts with acid it behaves like base and when it reacts with base it behaves like acid. When it reacts with acid, it produces hydrated Cr species which is capable of reacting with bases to produce complex salts.

Is cr2o3 tetrahedral?

In Cr2O3, central O atom is tetrahedral arranged around 2 lone pairs and 2 Cr=O fragments. Hence central O atom in cr2o3 is sp3 hybridized. That is why cr2o3 is tetrahedral in nature.

Is cr2o3 linear?

Cr2O3 is not linear because from structure of cr2o3 we see that 2 Cr atoms and 3 O atoms are arranged in angular manner i.e. in bent manner. Hence Question of linear structure does not arise.

Is cr2o3 symmetrical or asymmetrical?

Cr2O3 is symmetrical in nature. When a sigma or mirror plane passes through the compound it divided the compound into 2 symmetric halves. Actually, the mirror plane passes through the O atom in cr2o3 compound, 2 symmetric halves are obtained i.e. Cr=O part.

Cr2O3 Molar Mass

As cr2o3 contains 2 cr atoms and 3 o atoms in it. The molar mass of cr2o3 is equal to the sum of molar mass of 2 cr atoms and 3 atoms. Hence the molar mass of cr2o3 is 151.9904 gm/mol.

Cr2O3 Oxidation Number

O atom has -2 oxidation states. Hence 3 o atoms provide -6 oxidation states. Cr2o3 is overall a neutral compound. For this reason, -6 charge is neutralized by +6 charge. Hence each cr atom provides +3 oxidation state.

Cr2O3 Charge

Cr2O3 is overall a neutral compound. This is because of the fact that -6 charge of o atom is neutralized by +6 charge of cr atoms. Cr2o3 has overall a neutral compound.

Is Cr2O3 Paramagnetic?

Cr2O3 contains a total of 6 unpaired electrons i.e. each cr atoms provide 3 unpaired electron. Hence this compound is paramagnetic due to presence of unpaired of electrons. In cr2O3, each cr atom provides 3BM spin only magnetic moment.

Is Cr2O3 a Strong Electrolyte?

Cr2O3 contains 6 unpaired electrons. This unpaired free electron is responsible for the creation of electricity by cr2o3. For this reason, cr3o3 behaves as a strong electrolyte.

Conclusion

Keeping the above facts in mind about cr2o3 it is stated that cr2o3 is a neutral nonpolar tetrahedral compound. It reacts with both acid and bases to behave as an amphoteric oxide. In cr2o3 the two cr atoms contain +3 oxidation state and 3 o atoms contain -2 oxidation state each.

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GaI3 Lewis structure is represents almost 17 facts regarding the compound. The electronic formation of chemical bond in between Gallium and Iodine and their electron sharing process would be relevantly discussed in this article.

GaI3 Lewis structure is a basic sketch of the shape formed by Gallium and Iodine after sharing their valence electrons with each other where the electrons are denoted by using dots. The facts that would be highlighted in the articles are:

• Drawing GaI3 Lewis structure
• GaI3 Lewis structure resonance
• GaI3 Lewis structure shape
• GaI3 Lewis structure formal charge
• GaI3 Lewis structure angle
• GaI3 Lewis structure octet rule
• GaI3 Lewis structure lone pairs
• GaI3 valence electrons
• GaI3 hybridization
• GaI3 solubility
• Solubility of GaI3 in water
• GaI3 a strong electrolyte
• GaI3 acidic or basic
• GaI3 polar or nonpolar
• GaI3 a Lewis acid or base
• GaI3 linear
• GaI3 paramagnetic or diamagnetic

Drawing GaI3 Lewis structure

The drawing of a basic sketch of Lewis structure of a compound follows five strategic steps, which are not exceptional for Gallium iodide as well. These steps are being described below:

Step 1: Calculating the number of valence electrons in each of the elements that is Gallium and Iodine is the first fundamental step to follow before initiating the drawing. The number of valence electrons would be mentioned later in this article.

Step 2: The second significant step is to identify the atom which would hold centre position in the structure. Gallium takes the centre place in gallium Iodide as three Iodine atoms exist around one gallium atom.

Step 3: Third step is to put two electros, which would be partially shared by gallium and Iodine atoms with each other’s.  Those two dots or electrons would be the notation of chemical bond created by the atoms

Step4: The octet (octet rule would be defined later) would be filled with more electrons dots in the next steps. Electron dots would be represented for denoting the lone pairs on the outside atoms and imposing the valence electron pairs on them.

Step5: Calculation of the formal charges is the next step must to follow as this charges helps to identify the stability of Lewis structure of the compound.

GaI3 Lewis structure resonance

Resonance refers to the process of alternating the π bonds with the extra electron present in any atom of a compound. Resonating structures are represented by keeping the chemical formula intact.

In GaI3, there is no π bond exist, therefore; resonance process is irrelevant for this compound and resonating structure also cannot be represented for Gallium iodide.

GaI3 Lewis structure shape

After sketching the Lewis structure of a compound it gives a molecular geometry, which is considered as the shape of that compound.

The Lewis structure of Gai3 represents its molecular geometry by imposing the number and type of bonding. The shape of the compound is determined as Trigional planner.

GaI3 Lewis structure formal charge

Lewis structure of a compound is reliable in expressing the formal charge of overall compound. It significant to notify the number of bond pairs and lone pairs of electrons which are the main component in  calculating individual formal changes.

The formula of calculating formal changes is

Formal charge = Number of valence electrons – Number of nonbonding valence electrons – (Bonding electrons/2)

Formal charge of Gallium = 3 – 0 – (3/2) = 1.5

Formal charge of each of the Iodine atoms = 7 – 6 – (1/2) = 1.5

Therefore, the overall formal charge is zero.

GaI3 Lewis structure angle

The ideal bond angle of Trigonal planner geometry is 120°. This bond angle differs o the compounds having lone pairs. Lone pair – bond pair collision is the reason for giving distinct bond angle to the compounds.

The bond angle of GaI3 is 120° that denotes a symmetrical structure of the compound. zero formal charge and very little amount of of lone pair – lone pair contraction are not enough to provide different bond angle to the compound.

GaI3 Lewis structure octet rule

Octet rule has extensive value in the electron sharing process of preceded by the compounds. This rules refers to the need of electron among the periodic element to fill their last electron energy level with 8 electrons to get ultimate stability as their nearest noble gas.

GaI3 also undergoes electron-sharing process to satisfy their octet state. Gallium needs to 3 electron to stabilise its electronic geometry with 8 electrons whereas each of Iodine atom needs 1 electron to fill octet. There they share their electrons with each other and satisfy octet.

GaI3 Lewis structure lone pairs

After creating chemical bonds with other elements, the overall count of lone pairs of the compound is referred to the number of lone pairs present in central atom.

In Gallium trioxide, it can be easily identified from the Lewis structure that Gallium, the central atom does not possess any lone pair. Not all the valence electrons participate in bonding, which makes sure that gallium, has in lone pair.

GaI3 valence electrons

It is already mentioned above in this article that calculation of valence electrons of the individual elements in a compound is the foremost step to draw Lewis structure of any compound. the number of electrons present in last energy level of a element refers to valence electrons.

Gallium iodide, the metal halide has two periodic element, gallium and three Iodine atoms participates in the formation of this compound. Gallium has three valence electrons and each of the Iodine atom possesses seven valence electrons.

GaI3 hybridization

Hybridisation can be found from the shape of the compounds. The molecular geometry addresses the hybridisation formula.

According to the shape of GaI3, the hybridisation of gallium iodide is sp2.this hybridisation formula is ideal for representing tribunal planner geometry in chemistry, which is possessed by GaI3.

GaI3 solubility

Solubility of gaI3 depends on several chemical and physical properties of the compound. Fusion of two elements induces a specific bonding structure to highlight the geometry of the composite.  The forces for creation of those bonds is the feature which differs the solubility of the different compounds.

How, we can find that solubility of GaI3 is manipulated by its chemical property of binding. Intermolecular force of the hybrid is the main factor that regulates its solubility in any substance.  Gallium triiodide is preferably not soluble in acids organic substances.

Solubility of GaI3 in water

Ionic structure creates difficulties for the compounds to get soluble in water like substances. GaI3 has been recognised as a covalent compound so its solubility in water differs generally.

Solubility in water of GaI3 can be addressed as decomposition. The covalent compound decomposes in water in normal temperature, therefore; it can be accomplished that it is soluble in water.

GaI3 is a strong electrolyte

Hydrated solution of the compounds is the responsible for conducting electricity. In water when two ions dissociate the electrolytic nature of the compound showcased by the ion.

GaI3 readily dissociates in water and gives out Ga+ and I- ions. These ions superiorly conduct electron. Only one condition appears here that is presence if hydrated solution of the compound which drives the decomposition of compound and conduction of electricity.  Therefore, Gallium iodide is a strong electrolyte.

GaI3 acidic or basic

Acidity or basicity depends on the pH level of the compounds. Gallium is a metal with neutral pH level.  Moreover, Iodine atom is the last halogen in periodic series therefore, its acidity is highest.

GaI3 is mildly acidic as it consists of three iodine atoms.   The hydrated solution of the compound produces Ga(OH)3 which participates in metasynthesis reaction with acidic pH level.

GaI3 polar or nonpolar

Polarity depends on the electronic arrangements and the geometric shape of the compounds. Symmetric diagrams indicate zero polarity due to cancellation of tension from each side.

GaI3 has a symmetric geometry, which clarifies the fact that Gallium iodide is a non-polar inorganic compound.

GaI3 a Lewis acid or base

Lewis acid is the element, which contain on of more void orbital for accepting electrons whereas Leis base refers to the substances having extra electrons and that gives away electron to Lewis acids.

Gallium iodide is a covalent compound here gallium and Iodine both the element accepts electrons and shares electrons with each other. Therefore both of the element are considered as Lewis acid and Lewis base.  However, Iodine is more acidic than Gallium and it has deficiency of one electron in last energy level.

GaI3 linear

Linear shape can be defend by mentioning the bong angle of 180° of a compound having two different periodic element. Here one central atom holds only two other atoms in its both side.

GaI3 is a non-linear metal halide and it has three Iodine atoms circling around the central atom Gallium. The angle between the bonds is 120°.

GaI3 paramagnetic or diamagnetic

Paramagnetic nature of compound is exposed if any unpaired electrons can be shown to be present in it whereas Diamagnetic a compound have all the electron paired and arranged.

Gallium iodine has all the electron paired and lone pairs on Iodine atoms. Therefore, this compound is clearly a diamagnetic composite.

Conclusion

Gallium Iodide has been found as a strong covalent compound which is built up through electron sharing process. GaI3 Lewis structure has delivered effective knowledge about chemical properties of the compound as well as internal facts of the compound that are held by its geometry.

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In this article, we shall learn Fe₂O₃ Lewis Structure, how to draw the lewis dot structure and other relevant information about Fe(III) oxide.

Fe₂O₃ lewis structure is an oxide of iron, also known as ferric oxide, red iron oxide or hematite that can be obtained in various forms like or , which are known by simple term called as polymorphs.

Fe₂O₃ lewis structure is one of the main sources of iron for industry processes.

Fe₂O₃ lewis structure or Fe(III) oxides are also referred to as rust as this is the common oxidation of iron found in rust. It happens as they are easily attacked by molecular oxygen, water molecule and various other solvents found in the environmental conditions.

Though Fe(III) is somewhat oxidizing in nature but Fe(III) and Fe(II) states have a close range of stability.

How to draw Fe₂O₃ Lewis Structure ?

Fe₂O₃ lewis structure of a molecule is the electronic skeletal representation of a molecule that briefs about how the atoms are connected/oriented in space through covalent/dative bonds, presence of lone pairs of electrons etc.

Lewis dot structure is constructed in accord with the octet rule which states that every constituent atom tries to accommodate eight electrons in its valence shell to attain noble/stable gas configuration.

There are however, some elements which can expand its octet owing to its expanded shells like SF₆ or those that are electron deficient in nature like the H₂ molecule.

A noble gas element is the 7^th period of periodic table that has the maximum stability due to complete valence shell configuration.

Steps to draw Fe₂O₃ lewis structure :

Fe₂O₃ lewis structure is a slightly different case as the compound is ionic in nature hence electron transfer will be observed. Hence, the lewis structure will show how electrons are transferred from metal to a non-metal element.

Each oxygen atom requires 2 extra electrons to complete their octet and attain stability. Each Fe atom transfers 2 electrons to two of the three O atoms and the remaining O atom acquires one electron each from the two Fe atoms. As electrons are transferred from Fe atomic orbitals to the O atomic orbitals, it forms ionic bond.

Fe₂O₃ lewis structure shape :

Fe₂O₃ lewis structure has a bent shape similar to ‘W’ . Gamma-Fe₂O₃ is found to be reverse spinel.

However, it is much more beyond the bent shape.

Its shape or structure generally depends on the size of the crystals. Generally, it is found to be spherical if the nanometer range increases from 20 nm to 81 nm. Further, it has several forms like alpha, gamma, etc. depending on the experimental conditions.

Fe₂O₃ lewis structure formal charge :

Fe₂O₃ lewis structure is an ionic compound where metal in the oxidized state and non-metal in the reduced state are joined together to form the cluster of Fe₂O₃ . Since, it is a neutral compound, it means the total number of cation’s charge must equal the anion’s charge.

Further, formal charge is not the net charge of a molecule. The formal charge if found by the common mathematical formula shown below shows that the atoms do not bear any electronic charge. But, each atom has its specific net charge.

Formal charge = (Number of valence electrons in a free atom of the element) – (Number of unshared electrons on the atom) – (Number of bonds to the atom)

In addition, Charge on the molecule= sum of all the formal charges.

Moreover, formal charge can be found if the electrons are shared fairly between the atoms but in an ionic compound, electrons are transferred. Therefore, it is best to consider and talk about the net charge possessed by the atom in that particular oxidation state.

Fe is in +3 oxidation charge with a net charge of +3 and O has a net charge of -2.

Therefore, the total charge of the Fe₂O₃ lewis structure cancels out and becomes a neutral molecule.

2Fe⁺³ ( +3 * 2 = +6 ) and 3O^2- ( -2 * 3 = -6 )

Fe₂O₃ hybridization :

Fe₂O₃ lewis structure is an ionic compound. The concept of hybridization involves sharing of electrons i.e., by effective overlap of the orbitals.

As ionic compound involves transferring of electrons where in this case 3 electrons are transferred by each Fe atom to the O atom to give them stability. Hence, the concept of hybridization is invalid in Fe₂O₃ lewis structure.

Ground state of Fe : [Ar]4s²3d⁶

Excited state of Fe in +3 state : [Ar]4s⁰3d⁵ ( After transferring 3 electrons to O )

Ground state electronic configuration of O: [He]2s²2p⁴

Fe₂O₃ lewis structure resonance :

Fe₂O₃ lewis structure does have resonance structures but it is most stable when the atoms do not involve charge separation.

The ionic resonance structure is less stable due to charge separation involving a low resonance energy.

Fe₂O₃ lewis structure octet angle :

Fe₂O₃ lewis structure is an ionic molecule and the oxygen atoms in the crystal follows the octet rule.

Fe atoms transfer electrons to the valence orbital of oxygen atoms to complete their octet. Fe, being a transition metal, can accommodate more than 8 electrons. After losing 3 electrons by each Fe atoms, it has 5 electrons left in its valence 3d subshells.

Fe₂O₃ lewis structure lone pairs :

Fe₂O₃ lewis structure has 4 lone pairs of electrons residing on the two oxygen atoms.

The lone pairs are localized and do not involve in delocalization during resonance.

Lone pairs are the non bonded electron pairs that do not participate in chemical bond formation.

Fe₂O₃ valence electrons :

Fe₂O₃ lewis structure involves a total of 24 valence electrons. Six valence electrons from the two Fe atoms participate in transferring to the valence atomic orbitals of O atoms.

The two oxygen atoms involves a total of 18 valence electrons.

Valence electrons are the outermost electrons in the valence orbitals that participate in any type of chemical bond formation such as ionic bonds, covalent bonds or coordinate bonds.

Fe₂O₃ solubility :

Fe₂O₃ lewis structure has high affinity for protons to be incorporated in its crystal domains. As such it is found to be soluble in most of the acids.

Few solvents in which Fe₂O₃ is soluble and insoluble are shown below :

Solvents	Solubility
Water	Insoluble
Dilute mineral acids like HCl	Soluble
Sugar/Carbohydrate solution	Slightly soluble
Organic acids like Tartaric acid, Acetic acid	Fairly soluble

Is Fe₂O₃ acidic or basic ?

Fe₂O₃ lewis structure is an amphoteric oxide as it reacts with both acid and bases. Therefore, it can be stated to be both acid and base depending on the experimental and environmental conditions.

Two reactions where in one Fe₂O₃ acts as base and in the other as an acid are shown below :

Fe₂O₃ + 6HCl ——-> 2FeCl₃ + 3H₂O ( where Fe₂O₃  acts as base )

Fe₂O₃ + Na₂CO₃ ——–> 2NaFeO₂  + CO₂ ( where Fe₂O₃ acts as an acid )

Is Fe₂O₃ linear ?

Fe₂O₃ lewis structure is not a linear molecule, rather it has a W shaped geometry similar to two bent molecules joined together by an atom.

In this case, two Fe=O units are joined together by an oxygen atom acting like a bridge.

Is Fe₂O₃ tetrahedral ?

Fe₂O₃ lewis structure is not a tetrahedral molecule. It is a bent shaped molecule exhibiting the ‘W” shape.

Is Fe₂O₃ polar or non polar ?

Fe₂O₃ lewis structure is a polar molecule as it is ionic in nature.

The dipole moments are oriented in a way that they do not cancel each other. Hence, Fe2O3 lewis structure is polar with a definite dipole moment.

Is Fe₂O₃ amphoteric ?

Fe₂O₃ lewis structure is an amphoteric oxides where it can act as a base as well as an acid as justified by the following reactions shown below :

Fe₂O₃ + 6HCl ——-> 2FeCl₃ + 3H₂O ( where Fe₂O₃  acts as base )

Fe₂O₃ + Na₂CO₃ ——–> 2NaFeO₂  + CO₂ ( where Fe₂O₃ acts as an acid )

Amphoteric nature is a very useful quality as it can be tuned as per the conditions.

Is Fe₂O₃ ionic ?

Fe₂O₃ lewis structure is an ionic molecule. Electrons are transferred completely to the atomic orbitals of oxygen atoms by the Fe atoms.

Transfer of electrons take place when atoms are connected through ionic bonds and thus involves electrostatic force of attraction that is a characteristic of ionic connectivity.

Fe₂O₃ lewis structure angle :

Fe₂O₃ lewis structure has several polymorphs out of which the alpha form has an angle close to 149⁰ .

Is Fe₂O₃ symmetrical or asymmetrical ?

Fe₂O₃ lewis structure is a symmetrical molecule.

It is a planar molecule containing a plane of symmetry as well as a mirror plane cutting through the central oxygen atom that gives similar reflection on both sides of the mirror plane.

Is Fe₂O₃ rust ?

Fe₂O₃ lewis structure is similar to rust as it has similar composition and characteristics. Original composition of rust is Fe₂O₃.xH₂O .

Fe(III) oxides are defined as rust generally, but they are actually Hydrous ferric oxide. Hence, Fe₂O₃ can get hydrated in a well defined aqueous environment and act as a rust material.

Is Fe₂O₃ antiferromagnetic ?

α – Fe₂O₃ is antiferromagnetic where the spin undergoes reorientation and cancels each other as the domain align themselves opposite to the applied magnetic field.

This results in zero magnetism and are repelled by the magnetic field.

Is Fe₂O₃ paramagnetic or diamagnetic ?

Fe(III) or Fe₂O₃ is paramagnetic in nature as they are strongly attracted by the external magnetic field applied. The domains are always aligned parallel to the magnetic field.

In fact, the Fe(III) oxides exhibit strong superparamagnetic behavior in the nanometer scale ( below 10 nm ).

Fe(III) ions are not diamagnetic in nature.

Conclusion :

Fe₂O₃ lewis structure is a symmetrical ionic molecule with paramagnetic nature and are widely used in manufacturing of nanomaterials, nanotechnology.

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HOF is the chemical formula for hypofluorous acid. Here we are discussing about HOF lewis structure, characteristics and some facts about it.

HOF (hypofluorous acid) can also be written as FHO. HOF has some synonyms like fluoranol, fluoroalcohol, hydroxyl fluoride and fluoridohydridooxygen. HOF (hypofluoro acid) or fluoranol is an fluorine oxyacid which is a conjugate acid of hypofluorite. HOF has molecular weight of 36.006. HOF consists of three elements mainly hydrogen, oxygen and fluorine.

How to draw HOF lewis structure?

The lewis structure of HOF can be drawn by considering the following steps:

1. Predict the group positions of hydrogen, oxygen and fluorine atoms on periodic table
2. Count overall valence electrons available on HOF lewis structure.
3. Selection of central atom which is most electronegative from all the atoms and the rest of the atoms are being bonding atoms.
4. Make bonding within all H, O and F atoms of HOF lewis structure.
5. Remaining valence electrons are put on the bonding atoms which are being non – bonding electrons.
6. Then count the lone pair electrons on HOF lewis structure.
7. Check whether the H, O and F atoms have complete or incomplete octet in HOF lewis structure.
8. Finally predict the shape, hybridization and bond angle of HOF lewis structure.

HOF valence electrons

The HOF lewis structure composed of three elements i.e. hydrogen atom, oxygen atom and fluorine. Thus, the hydrogen atom belongs to 1^st periodic table group, oxygen atom belongs to 16^th periodic table group and the fluorine atom belongs to 17^th (7A) periodic table group. Therefore, the H, O and F atoms contain one, six and seven valence electrons respectively, in their valence shell outer orbital.

The total valence electrons available on hydrogen, oxygen and fluorine atoms of HOF lewis structure is calculated as follows:

Hydrogen atom of HOF lewis structure has valence electrons is = 01

Oxygen atom of HOF lewis structure has valence electrons is = 06

Fluorine atom of HOF lewis structure has valence electrons is = 07

Hence, total valence electrons on HOF lewis structure is = 1 (H) + 6 (O) + 7 (F) = 14.

Therefore, the valence electrons on HOF lewis structure are fourteen.

 If we see the total electrons pairs on HOF lewis structure, the HOF valence electrons get divided by two.

Thus, total electron pairs on HOF lewi structure = 14 / 2 = 7

Therefore, there are seven electron pairs in MOF lewis structure.

HOF lewis structure lone pairs

The HOF lewis structure has total 14 valence electrons, out of which four electrons are the bond pair electrons which forms two single sigma covalent bonds with hydrogen and oxygen (H-O) atom and oxygen and fluorine (O-F) atom. Hence, the remaining 10 valence electrons go to O and F atoms.

Thus, the oxygen atom has four non – bonding electrons and fluorine atom has six non – bonding electrons on HOF lewis structure. These 10 non-bonding electrons of HOF are being the five lone electron pairs. Hence, the HOF lewis structure has total five lone electron pairs available on it two on O atom and three on F atom.

HOF lewis structure octet rule

There is two lone pair electrons are on oxygen atom and three lone pair electrons are on fluorine atom of HOF lewis structure. Hence, the hydrogen atom of HOF lewis structure has two bonding electrons satisfied it’s valency as per it capacity. The O atom contains 4 bond pair electrons (creates H-O and O-F bonds) and 4 non-bonding electrons.

Hence O atom of HOF lewis structure has eight electrons and have complete octet. The fluorine atom of HOF lewis structure has two bonding electrons forming O-F bond and also it has six non – bonding electrons. Thus, F atom of HOF lewis structure has total eight electrons and its octet is also complete. So, in HOF lewis structure the O and F atoms has eighit electrons which shows complete octet.

HOF lewis structure formal charge

The presence of formal charge on any lewis structure makes it more stable structure. Evaluation of formal charge on any molecules is done with the help of below given formula:

Formal charge = (valence electrons – non-bonding electrons – ½ bonding electrons)

The HOF lewis structure formal charge evaluation is done with the help of using above given formula. Here, first we have to evaluate the formal charge present on each hydrogen, oxygen and fluorine atoms of HOF lewis structure.

Hydrogen atom: Valence electrons on hydrogen atom of HOF = 01

                           Non- bonding electrons on hydrogen atom of HOF = 00

                           Bonding electrons on hydrogen atom of HOF = 02 (2e = one bond)

Thus, Formal charge on hydrogen atom of HOF lewis structure is = (01 – 00 – 2/2) = 00

So, the Hydrogen atom of HOF lewis structure contains zero formal charge.

Oxygen atom: Valence electrons on Oxygen atom of HOF = 06

                        Non – bonding electrons on Oxygen atom of HOF = 04

                        Bonding electrons on oxygen atom of HOF = 04 (2e = one bond)

Thus, Formal charge present on oxygen atom of HOF lewis structure is = (6 – 4 – 4/2) = 00

So, the oxygen atom of HOF lewis structure contains zero formal charge.

Fluorine atom: Fluorine atom has Valence electrons on HOF = 07

                        Fluorine atom has Non- bonding electrons on HOF = 06

                        Fluorine atom has Bonding electrons on HOF = 2 (2e = one bond)

Thus, Formal charge present on fluorine atom of HOF lewis structure is = (07 – 06 – 02/2) = 00

So, the fluorine atom of HOF lewis structure contains zero formal charge on it.

Therefore, the HOF lewis structure has overall zero formal charge present on it.

HOF lewis structure resonance

In HOF lewis structure, there is no multiple bonds are present and also even there is no positive or negative formal charge is present on it. Thus, there is even no movement of electrons as all the atoms of HOF lewis structure already has complete octet. Hence, HOF lewis structure cannot show any resonance structure.

HOF lewis structure shape

HOF acid follows AX2E2 generic formula of VSEPR theory. Here, A is central atom, X is bonded atoms with central atom and X is lone electron pairs on central atom. According to which the HOF acid has bent molecular shape and tetrahedral electron geometry.

HOF lewis structure angle

The HOF acid has the bent molecular shape and tetrahedral electrons geometry as the central O atom has two bonding atoms and two lone electron pairs. Therefore, as per the VSEPR theory the HOF acid should have 109.5 degree bond angle. But in HOF the H-O bond angle is less than O-F bond angle, thus the bond angle of HOF get decreases and have 97.2 degree bond angle.

HOF hybridization

With accord to VSEPR theory module HOF lewis structure belongs to AX2E2 generic formula, so HOF shows bent shape and tetrahedral geometry. Also it has H-O-F bond angle of 109.5 degree. Thus, HOF (hyprflorous acid) acid has sp3 hybridization.

Why HOF has sp3 hybridization?

In HOF molecule, the central O atom has two bonds with H and F atoms and also it has two lone electron pairs. Thus as per VSEPR theory HOF molecule has tetrahedral electron geometry and sp3 hybridization.

HOF solubility

HOF is an explosive substance and mostly insoluble in most of the organic solutions. Thus when HOF get added to water it behaves as an intermediate substance for oxidation of water by fluorine. Also it get decomposes as O2 and HF molecules. Hence, HOF is insoluble in nature and also unstable.

Is HOF soluble in water?

Yes, HOF is soluble in water. When HOF gets added to water it shows rapid explosive nature of reaction and thus HOF acts as an intermediate substance for water oxidation by fluorine molecule. Also the decomposition of HOF acid gets occurs and it get dissociates into HF and O2 in alkaline condition. Also on reaction with water of HOF it can produce peroxide and hydrogen fluoride in acidic medium.

Is HOF a monobasic acid?

No, HOF is not a monobasic acid it gets ionizes as fluorine and oxygen when added to water. Thus it cannot act as monobasic acid.

Why HOF is not a monobasic acid?

Monobasic acids are those acids which can have only one detachable hydrogen atom (H+ ion) per molecule in water. All the halogen atoms can produce monobasic oxyacids except the case of HOF. HOF is also an oxyacid but it is not monobasic in nature.

HOF is an oxyacid but it is exists in unstable form. As on dissolving in water it shows explosive behaviour and thus decomposed as fluorine (HF) and oxygen (O2). Hence, HOF does not act as a monobasic acid in nature.

Is HOF polar or non- polar?

HOF is a polar acid in nature as it has asymmetrical arrangement of all atoms and the dipole creates get cancel each other.

Why HOF is polar?

In HOF molecule, there is more electronegativity difference between hydrogen, oxygen and fluorine atoms. The electronegativity difference between H and O atoms are 1.24 and electronegativity difference between F and O atom is 0.54.

Thus it creates a dipole within the molecule and developed the partial negative charge on central O atoms and partial positive charge on bonding H and F atoms. There is no electron density present on H atom. But the F atom has more electron density which pulls the electron cloud towards itself and hence cancels the dipoles in HOF molecule. Hence, HOF is a polar molecule.

Is HOF stronger than HOCl?

Yes, HOF acid is stronger than HOCl acid. The fluorine atom is more electronegative in nature than chlorine and thus HOF can be stronger than chlorine.

Why HOF is stronger than HOCl?

In oxyacids, the weaker the O-H bond the stronger is the acid as the H+ ions can readily dissociates. In HOF the O-F bond is quite stronger as compared to O-Cl bond in HOCl.

The atomic size of F atom is less than Cl atom and also F is more electronegative than Cl. In HOF the O-F bond is stronger due to which the O-H bond becomes weaker and hence HOF is stronger than HOCl.

Is HOF ionic or covalent?

HOF is not ionic because it is an unstable covalent compound having two H-O and O-F covalent bonds within HOF molecule.

Why HOF is covalent?

HOF acid is strong acid and has single sigma covalent bonds within H and O atoms (H-O) and O and F atoms (O-F). The covalent bond is a strong bond which does not breaks easily. Hence, the HOF cannot ionize easily and so it is a covalent acid.

Is HOF ionic hydride?

No, HOF is not ionic hydride because it is an oxyacid. Oxyacids formed when the halogen reacts with water.

Why HOF is not ionic hydride?

When halogen like fluorine reacts with water gives the production of unstable oxyacid like HOF (hypoflurous acid). HOF is an intermediated of oxidation of water and fluorine.

F2 + H2O → HOF + HF

Thus, HOF is being an oxyacid, so it is not ionic hydride.

Is HOF isoelectronic?

No, HOF is not isoelectronic in nature. HOF is only one oxyacid of fluorine atom. Isoelectronic compounds are those two or more compounds which has similar structure and similar atoms position and bonding with same electronic configuration but different in properties. HOF does not have any similar molecule and hence it is not isoelectronic.

Is HOF ionic or molecular?

HOF is molecular because it cannot form ions. HOF is a triatomic molecule consisting of three atoms i.e. hydrogen, oxygen and fluorine atoms. Also it is only the oxyacid of fluorine and on decomposition it forms molecules like HF and O2. Hence, it is a molecular and not ionic.

Is HOF ion dipole?

Yes, HOF has a net dipole moment of 2.23. In HOF molecule fluorine atom is more electronegative than O and H atoms and hence the net dipole pulls towards the F atom. Thus HOF acid has dipoles.

Conclusion:

HOF is only one oxyacid of fluorine. HOF lewis structure has 14 valence electrons and has 7 electrons pairs from them two are bond pair electrons and five lone pair electrons. There is no formal charge on HOF molecule and has covalent bonds within H-O and O-F. The HOF lewis structure has bent shape and tetrahedral geometry also it has bond angle of 97.2 degree. Hof is a polar acid.

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Hydrogen phosphate or HPO42- is the conjugate base of dihydrogen phosphate having molecular weight 95.98 g/mol. It is a divalent inorganic phosphate anion. It has one hydrogen, one phosphate and four oxygen atoms attached by one double bond and three single bonds around the phosphorous atom.

The Lewis structure of HPO4 2- features a phosphorus (P) atom at the center, bonded to one hydrogen (H) atom and three oxygen (O) atoms. Two of the O atoms are double-bonded to P, each carrying two pairs of non-bonding electrons. The third O atom is single-bonded to P and carries three pairs of non-bonding electrons, and is also bonded to the H atom. This results in a formal charge of -2 on the molecule, with the P atom having a formal charge of +1, one O atom (the one bonded to H) having a -1 charge, and the remaining atoms being neutral.

Let’s highlight the following topics on HPO₄^2-.

How to draw HPO₄ ^2- lewis structure?

To draw the lewis structure of any ion or molecule the following factors should be known perfectly.

1. Determining the number of valence electron: Phosphorus is a group 15 element. Thus, it has five valence electrons, whereas being a group 16 electron, oxygen has 6 electrons in its outer most shell and hydrogen has one valence electron in its 1s orbital.
2. Finding out the bonding electrons:  Total three single (sigma) and one double bond are present in HPO₄^2-. Therefore, the number of electrons involved in bonding are = (3×2) + (2×2) = 10
3. Finding out the nonbonding electrons:  Each of the single bonded oxygen (with phosphorus) has six electrons and the two oxygen atoms (one is attached with phosphorous by double bond and other one is attached by two single bonds with phosphorous and hydrogen atom) has four electrons as nonbonded electron pairs.

HPO₄^2- Lewis structure Shape

Lewis structure shape of any molecule denotes the geometrical structure of any molecule which can be determined by the hybridization of central atom and the lone pairs (if present in central atom). In the following table the changes of geometry with the changing of hybridization are shown-

Hybridization of central atom	Geometry
sp	Linear
sp2	Planar
sp3	Tetrahedral
sp3d	Trigonal bipyramidal (TBP)
sp3d2	Octahedral

Therefore, to determine the structure or shape of HPO₄^2-, the hybridization of central atom (phosphorous) should be determined first. The hybridization of phosphorous in this molecule is sp³. Thus, the geometrical structure should be tetrahedral. As phosphorous has no electrons left as nonbonding thus repulsion like lone pair-lone pair, lone pair-bond pair and bond pair-bond pair are not deviating its structure from the ideal geometry.

Otherwise, these repulsive factors the structure as well as bond angle of any molecule from the ideal case.

HPO₄ ^2- lewis structure Formal Charge

Formal charge calculation helps to identify the most stable lewis structure among different possible lewis structures. It also decides the total charge present in the molecule.

• Formal charge = Total number of valance electrons – number of electrons remain as nonbonded – (number of electrons involved in bond formation/2)
• Formal charge of central atom, phosphorous = 5 – 0 – (10/2) = 0
• Formal charge of each of the two oxygen atoms, attached with phosphorous by single bonds = 6 – 6 – (2/2) = -1
• Formal charge of another two oxygen atoms (one is OH oxygen and another oner is attached with phosphorous by double bond) = 6 – 4 – (4/2) = 0

From the calculation of formal charge, it is proved that this molecule has two negative charges on two oxygen atoms but these two negative charges are delocalized over the whole molecule.

HPO₄ ^2- Lewis Structure Angle

Like the geometrical molecular structure, bond angle in any molecule also depends upon the hybridization of central atom. There is a particular bond angle for each of the hybridization.

As the central atom phosphorous is sp³ hybridized in HPO₄^2-, the bond angle should be 109.5⁰. Due to absence of any repulsion involving bond pairs and lone pairs, it shows its actual bond angle without any deviation because phosphorous has no nonbonding electrons left to participate in lone pair-lone pair and lone pair-bond pair repulsion.

HPO₄ ^2- Lewis Structure Octet Rule

Octet rule tells about the valence shell electron configuration of any atom that should match with its nearest noble gas (according to periodic table) valence shell electron configuration.

In HPO₄ ^2-octet rule is not obeyed as phosphorous does not satisfy the octet rule. Phosphorous already contains five electrons in its valence shell (3s²3p⁵). After bond formation, it achieves five more electrons in its valence shell. Therefore, the total number of electrons in the valence shell of phosphorous become 10 which does not match with the valence electron numbers of its nearest noble gas, argon (3s² 3p⁶).

But octet rule is not violated for oxygen atom. It has six electrons and after bonding with neighboring phosphorous and hydrogen atom it achieves two more electrons in its outer most shell which resembles with its nearest noble gas, neon (2s² 2p⁶).

Hydrogen has one electron and after bond formation with oxygen, its valence shell is filled with two electrons like its nearest noble gas helium (1s²).

HPO₄ ^2- Lewis Structure Lone Pairs

Lone pairs are actually those valence electrons which are shown as the electron dot in lewis structure. They are not participating in bond formation with other atoms.

• Nonbonded electron = Total number of valance electron – number of bonded electrons.
• Nonbonding electrons in phosphorous = 5 – 5 = 0
• Nonbonding electrons of each of the two oxygen atoms, attached with phosphorous by single bonds = 6 – 2 = 4 or two pair of lone electrons.
• Nonbonding electrons of another two oxygen atoms (one is OH oxygen and another oner is attached with phosphorous by double bond) = 6 – 0 = 6 or three lone pairs.

Therefore, total numbers of nonbonding electrons in HPO₄^2- = (2×4) + (2×6) = 20

HPO₄ ^2- Valence Electrons

Valance electrons indicate the outer most shell electrons in every atom. The reactivity of valence electrons is the most and they mainly participate in bond formation. The reason behind this greater reactivity of valence electron is due to lesser attraction force of nucleus on the valence shell.

Phosphorous is nitrogen group (group 15) element. It has five electrons in its outer most shell and all the valence electrons are used up for bond formation. Hydrogen has one electron (1s¹) and it is regarded as the valence electron of hydrogen. Oxygen is group 16 element. It has total eight electrons and among these eight electrons, six electrons are in valence shell and are regarded as valence electrons.

Therefore the number of valence electron in HPO₄^2- = 5 + (4×6) + 1 = 30

HPO₄ ^2- Solubility

All phosphates are basically insoluble excluding sodium, potassium and ammonium phosphates in water but some hydrogen phosphates are soluble like disodium dihydrogen phosphate. The solubility of disodium dihydrogen phosphate is 7.7 g/100 ml at 20⁰ C and 11.8 g/100 ml at 25⁰ C which indicated that solubility in water of dihydrogen diphosphate increases with increasing temperature.

Is HPO₄ ^2- polar or nonpolar?

Polarity or dipole moment depends on the following factors-

• Electronegativity difference between the atoms
• Shape of the molecule or orientation of the bonds with respect to each other.

HPO₄^2- is tetrahedral shaped with the bond angle 109.5⁰. There is difference of electronegativity present between oxygen, phosphorous and hydrogen. Thus, the O-P bonds are polar. Due to tetrahedral shape, the bond moments are not cancelled by each other and the anion possesses a permanent dipole moment.

Therefore HPO₄^2- is a polar molecule.

 Is HPO₄ ^2- an acid or base?

Phosphoric acid (H₃PO₄) is an acid. After elimination of two hydrogen atom, HPO₄^2-is formed which is the conjugate base of H₂PO₄^–(formed after elimination of one hydrogen atom from H₃PO₄). Therefore, it can uptake two protons. It can also donate its last proton and form PO₄^3-.

Thus, it acts both as acid and base.

Is HPO₄ ^2- amphiprotic?

Yes, HPO₄^2-is an amphiprotic ion which means it can both accept and donate proton. It is the conjugate base of H₂PO₄^–, and the conjugate acid of PO₄^3-. After accepting two protons, it forms stable phosphoric acid (H₃PO₄).

H₂PO₄^– Lewis Structure

It is basically the conjugate base of phosphoric acid. After eliminating one proton from phosphoric acid, H₂PO₄^– is obtained. In this mono negative molecule, phosphorus is bonded with two OH group by two single bonds and with two oxygen atoms by a single bond and double bond respectively.

Is H₂PO₄^– an acid or base?

It is also an amphiprotic substance because it is the conjugate base of phosphoric acid. On the other hand, it can donate its two proton to form PO₄^3-. Thus, it also acts as Bronsted acid. For this dual behaviour as acid and base it is defined as an amphiprotic substance.

Is H₂PO₄^– stronger than HPO₄^2-?

H₂PO₄^– is stronger than HPO₄^2-because after accepting one hydrogen atom, H₂PO₄^– becomes phosphoric acid. As phosphoric acid is a weak acid and after eliminating one proton it becomes weaker and further donation of proton HPO₄^2-becomes the weakest.

Conclusion

It can be concluded from the above article on HPO₄^2- that it is conjugate base of H₂PO₄^– and it is a tetrahedral anion having bond angle 109.5⁰. It is a polar molecule having a permanent dipole moment.

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