How to calculate percentage (%) ionic character in covalent compounds?

 Henry & Smith equation:

The percentage ionic character in covalent compound arises due to the electronegative difference of bonding atoms. And percentage ionic character of covalent bond calculates by Henry and Smith equation;

Solved Questions:

(2) A given compound AB whose electronegative difference is 1.9 . Atomic radius of A and B are 4 and 2 Angstroms the distance between A and B means dA-B is ?

(2) The C–C single bond length is 1.54 Angstroms and that of Cl–Cl is 1.98 Angstroms. If the electronegativity of Cl and C are 3.0 and 2.5 respectively, the C–Cl bond-length will be equal to ?

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic density ? give the periodicity of atomic density in periods and groups.

(6) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(7) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(8) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(9) The electron affinity of sulphur is greater than oxygen. Why?

(10) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

Stevenson & Schromaker Equation: Determination covalent radius of Heterogeneous Molecules.

 Stevenson & Schromaker Equation:

Covalent radius of heterogeneous molecule like A-B etc determine by Stevenson & Schromaker Equation, if atoms are formed different type of covalent bond i.e. on atom is more electronegative than the other combined atom. Then the covalent radius is calculated by the relation given by Stevenson & Schromaker, given as:

For a diatomic Hetero molecule:

Bond Length (l_A-B) = r_A + r_B- 0.09(X_A-X_B)

Where X_A= Electronegativity of more electronegative atom

Where X_B= Electronegativity of less electronegative atom

Solved Questions:

(2) A given compound AB whose electronegative difference is 1.9 . Atomic radius of A and B are 4 and 2 Angstroms the distance between A and B means dA-B is ?

(2) The C–C single bond length is 1.54 Angstroms and that of Cl–Cl is 1.98 Angstroms. If the electronegativity of Cl and C are 3.0 and 2.5 respectively, the C–Cl bond-length will be equal to ?

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic density ? give the periodicity of atomic density in periods and groups.

(6) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(7) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(8) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(9) The electron affinity of sulphur is greater than oxygen. Why?

(10) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

(11) The electronegativities of B, Al, Ga are 2.0, 1.5, 1.6 respectively. The trend is not regular. Explain.

(12) Li2CO3 decomposes on heating but other alkali metal carbonates don’t. Explain.

(13) Of all noble metals, gold has got a relatively high electron affinity. Explain.

(14 Ionization energy of Boron is smaller than Beryllium even though effective nuclear charge is higher?

(15) What are the increasing order of ioni radii of first group elements in water ?

(16) What are the increasing order of molar conductivity of first group elements in water ?

A given compound AB whose electronegative difference is 1.9 . Atomic radius of A and B are 4 and 2 Angstroms the distance between A and B means dA-B is

 For a diatomic Hetero molecule:

 Bond Length (l) = r_A + r_B- 0.09(X_A-X_B)

Where X_A= Electronegativity of more electronegative atom

Where X_B= Electronegativity of less electronegative atom

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic density ? give the periodicity of atomic density in periods and groups.

(6) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(7) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(8) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(9) The electron affinity of sulphur is greater than oxygen. Why?

(10) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

(11) The electronegativities of B, Al, Ga are 2.0, 1.5, 1.6 respectively. The trend is not regular. Explain.

(12) Li2CO3 decomposes on heating but other alkali metal carbonates don’t. Explain.

(13) Of all noble metals, gold has got a relatively high electron affinity. Explain.

(14 Ionization energy of Boron is smaller than Beryllium even though effective nuclear charge is higher?

(15) What are the increasing order of ioni radii of first group elements in water ?

(16) What are the increasing order of molar conductivity of first group elements in water ?

The C–C single bond length is 1.54 Angstroms and that of Cl–Cl is 1.98 Angstroms. If the electronegativity of Cl and C are 3.0 and 2.5 respectively, the C–Cl bond-length will be equal to

For a diatomic Hetero molecule:

Bond Length (l) = r_A + r_B- 0.09(X_A-X_B)

Where XA= Electronegativity of more electronegative atom

Where XB= Electronegativity of less electronegative atom

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic density ? give the periodicity of atomic density in periods and groups.

(6) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(7) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(8) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(9) The electron affinity of sulphur is greater than oxygen. Why?

(10) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

(11) The electronegativities of B, Al, Ga are 2.0, 1.5, 1.6 respectively. The trend is not regular. Explain.

(12) Li2CO3 decomposes on heating but other alkali metal carbonates don’t. Explain.

(13) Of all noble metals, gold has got a relatively high electron affinity. Explain.

(14 Ionization energy of Boron is smaller than Beryllium even though effective nuclear charge is higher?

(15) What are the increasing order of ioni radii of first group elements in water ?

(16) What are the increasing order of molar conductivity of first group elements in water ?

General Inorganic Chemistry (Interactive mechanism of inorganic reactions):

(1)-Classification of Elements & Periodicity in properties

(2) Structure of atom and Electronic configuration

(3)-Chemical bonding & Molecular Structures

3.1 Chemical Bonds

3.2 Ionic Bond

3.3 Covalent bond (sigma and pi Bond)

3.4 Coordinate bond

3.5 Valence Bond Theory

3.5 Hybridization

3.6 VSEPR Theory

3.6 MOT

(4)-General Inorganic Chemistry (G.Ino.C)

3.1 Dipole Moment

3.2 Fajan’s Rule

3.3 Resonance

3.4 D-Orbital resonance

3.5 Bent’s rule of hybridization

3.6 Drago’s rule: No need of hybridization

3.7 Back bond

3.8 Bridge Bond: Multi-centered Bond

3.9 Vander Waal’s force

3.10 Hydrogen Bond

3.11 Metallic Bond

5-Acid-Base Concepts/theories

4.1 Arrhenius Acid–Base concept

4.2 Bronsted Lowery Acid-base concept:

4.3 Lewis Acid-Base concepts:

4.4 The Solvent System (Self or Auto Ionization of Solvent):

4.5 The Lux-Flood Acids-base concepts:

4.6 The Usanovich Acid-base concepts:

6-Oxides (Acid anhydrides)

5.1 Classification of oxides: (On the Basis of oxygen content):

5.2 Classification of oxides: (On the basis of Acid-Base Interaction):

7-Oxy acids and its Salts

6.1 Oxy acids of Boron:

6.2 Oxy acids of Silicon:

6.3 Oxy acids of Nitrogen:

6.4 Oxy acids of Phosphorous:

6.5 Oxy acids of Sulphur:

6.6 Oxy acids of Chlorine:

(8)-Type of inorganic reactions

(9)-Hydrolysis Mechanism

8.1 Hydrolysis of Halides of 13^th group:

8.2 Hydrolysis of Halides of 14^th group:

8.3 Hydrolysis of Halides of 15^th group:

8.4 Hydrolysis of Halides of 16^th group:

8.5 Hydrolysis of Interhalogen compounds:

8.6 Hydrolysis of Halides of 18^th group:

8.7 Hydrolysis of peroxy acids:

8.8 Hydrolysis of Oxides:

8.9 Hydrolysis of Carbides:

8.10 Hydrolysis of Nitrides:

8.11 Hydrolysis of Hydrides:

8.12 Hydrolysis of phosphides:

8.13 Hydrolysis of sulphides:

8.14 Hydrolysis of Silicides:

8.15 Hydrolysis of Borides:

8.16 Hydrolysis of Phosphides:

(10)-Effect of heat on compounds (acids, bases and Salts)

9.1 Thermal stability of salts

9.2 Thermal Decomposition Reactions

(11)- The Coordination compounds

(12)- Quantitive Analysis (Salts Analysis):

 

What is/are correct statement about Boroxine ion (B3O6-3) and Borazole (Inorganic Benzene)/ B3N3H6?

 (A) Both are planer and non polar

(B) Both have aromatic character

(C) Both have p_pi-p_pi bond formed by pairing of unpaired electrons

(D) Electrophilic subtitution  reaction occurs at B₃N₃H₆

SOLUTION:( A,B,D) In Boraxine ion boron and oxygen atom alternatively combined to form six member ring and also each boron atom linked with extra oxygen atoms. Both boron and oxygen atoms have sp2 hybridization (by Back bonding and all oxygen atom involved in back bonding) and planer structure due to fact ring become aromatic but due to sp3 hybrisation of oxygen atom molecule become polar.

In Borazine (Inorganic Benzene) molecule, nitrogen is more electro negative than the boron. Nitrogen acquires partial negative charge and boron acquires partial positive charge and back bonding take place between boron and nitrogen.

Even though Borazine and Benzene have same stricture their chemical properties are different.

(1) Organic benzene is C₆H₆ while Inorganic benzene is Borazine having chemical formula B₃N₃H₆

(2) Borazine is more reactive than Benzene with repect to electrophic addition reactions  due to high polarity (B-N polar bond) of Borazine plecules.

(3) Aromaticity of borazine is less than benzene  hence it is less reactive  toward Eectrophilic  substitution reactions than Benzene. 

Hence options (A), (B) and (D) is correct  But Option (C) is Incorrect Both have  pi-bond due to back bonding not due to formed by pairing of unpaired electrons

 Related Questions: 

Why aqueous solution of AlCl3 is acidic in nature ?

What happen when aq AlCl3 react with Acid or Base?

Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

Why BF3 do not exist as dimer?. Explain.

Why B-F bond length in BF3 is shorter (130 pm) than B-F bond Iength in BF4- (143 pm)?. Explain.

B-F bond length in BF3 is shorter than B-F bond length in (BF4)- why?

When B2H6 is allowed to react with following Lewis bases, then how may given Lewis base form adduct through symmetrical Cleavage of B2H6.

What is product of reaction between diborane (B2H6) and ammmonia (NH3)?

Why methylation of Diborane (B2H6) replace four hydrogen only ?

What is Use of Boric Acid?

What is use of Orthoboric acids?

What is basicity of "Boric acid" ?

Why Boric acid exist in solid state ?

What is structure of solid Ortho Boric acid ?

What is effect of heat on Borax?

What is the structure of trimetaboric acid and trimetaborate ion?

What is the Sodium per borate ,give the structure and its uses?

Why aqueous solution of borax reacts with two moles of acids ?

What is the molecular formula of Borax ?

Why Boric acid become strong acid in the presence of cis 1,2-diol or 1,3-diol ?

Why Borazine is more reactive than benzene towards Electrophic Aromatic substitution reactions ?

Why Borazine (B3N3H6) is also known as inorganic benzene ?.

Four-center two-electron bond (4C-2e Bond): Structure of AlCl3:

What is the difference between the structure of AlCl3 and diborane?

Why is BCl3 a strongerLewis acid than BF3 ?

The strength of a Lewis acid is a measure of its ability to attract a pair of electrons on a molecule that is behaving as a Lewis base. Fluorine is more electronegative than chlorine, so it appears that three fluorine atoms should withdraw electron density from the boron atom, leaving it more positive.This would also happen to some extent when the peripheral atoms are chlorine, but chlorine is less electronegative than fluorine. On this basis, we would expect BF₃ to be a stronger Lewis acid. However,in the BF₃ molecule, the boron atom uses sp2 hybrid orbitals, which leaves one empty 2p orbital that is perpendicular to the plane of the molecule. The fluorine atoms have filled 2p orbitals that can overlap with the empty 2p orbital on the boron atom to give some double bond character (Back Bond) to the B–F bonds.

 

As a result of the contribution by resonance structures having some double bond character, the boron atom in BF₃ is not as electron deficient as it is in BCl₃. And hence BCl₃ a stronger Lewis acid than BF₃

How to determine order of bond angle of Me-O-Me, H3Si-O-SiH3 and (ph)3Si-O-Si(Ph) ?

 (1) Oxygen of Me-O-Me is sp3 hybridised so C-O-C bond angle is more than 109’28” approx 110” due to crowding of methyl group.

(2) In disilyl ether , oxygen is Sp2 hybridised and planer due to back bonding between oxygen and silicon atom.  In this back bonding lone pair of oxygen atom donate to the vacant d orbital of silicon atom  due to this fact bond lengths of Si-O is decrease and  increases (approx 140”).

(3) In (Ph)3Si-O-Si(Ph)3  compounds Si-O-Si bond angle is Approx 180 due to back bonding and hybridisation is Sp.

Related Questions:

Why trimethylamine amine ( N(CH3)3) is tetrahedral while trisilyl amine (N(SiH3)3) planner.?

Why trimethyl amine {(CH3)3 N:} is pyramidal while trisilyl amine {(SiH3)3N:} is trigonal planer?

Which is/are the correct statement/s about structure of methyl isothiocyanate (H3CNCS) and Silyl isothiocyanate(SiH3NCO)?

What is the Si–N–C bond angle in Silyl isothiocyanate and methyl isothiocyanate (H3CNCS)?

What are the order of extent back bonding, Lewis acid character and nucleophilicity of (BF3, BCl3, BBr3, BI3)boron trihalides?

Arrange the silicon halides into decreasing order of Lewis acids Character? SiF4, SiCl4, SiBr4, SiI4

Which of the following correct statement about structure of Ortho boric acid (H3BO3 ) is/are? Statements are as

Which of the following is correct order of (B-O) bond length of following compounds? (1) B(OH)3 (2) B(OMe)3 and (3) B(Me)2OH

What are the structure of (1) N(SiH3)3 (2) {(Me)3Si}2N-Si(Me)3 (3) HN(SiH3)2 and give the Answers of following questions?

How to compared bond angle (C-N-C) and (Si-N-Si) in trimethyl amine and trisilyl amine respectively?

Nitrogen (N) atom in trimethyl amine [N(CH₃)₃] is sp3 hybridised and tetrahedral ( bond angle ~107)  due to non bonding electron pair of N is localised (more basic). On the other hand N atom of trisilyl amine [N(SiH₃)₃] is sp2 hybridised and trigonal planner (bond angle~120).This is due to the participation of non-bondlng pair of N into pπ-dπ back banding. Due to this delocalization of non-bonding electron pair of N in trisilyl amine it is also less basic

Related Questions:

Why trimethylamine amine ( N(CH3)3) is tetrahedral while trisilyl amine (N(SiH3)3) planner.?

Why trimethyl amine {(CH3)3 N:} is pyramidal while trisilyl amine {(SiH3)3N:} is trigonal planer?

Which is/are the correct statement/s about structure of methyl isothiocyanate (H3CNCS) and Silyl isothiocyanate(SiH3NCO)?

What is the Si–N–C bond angle in Silyl isothiocyanate and methyl isothiocyanate (H3CNCS)?

What are the order of extent back bonding, Lewis acid character and nucleophilicity of (BF3, BCl3, BBr3, BI3)boron trihalides?

Arrange the silicon halides into decreasing order of Lewis acids Character? SiF4, SiCl4, SiBr4, SiI4

Which of the following correct statement about structure of Ortho boric acid (H3BO3 ) is/are? Statements are as

Which of the following is correct order of (B-O) bond length of following compounds? (1) B(OH)3 (2) B(OMe)3 and (3) B(Me)2OH

What are the structure of (1) N(SiH3)3 (2) {(Me)3Si}2N-Si(Me)3 (3) HN(SiH3)2 and give the Answers of following questions?

What is structure (CF3)2-Al-O-Al-(CF3)2 and also find the number of pi bond or Back bond?

What is structure (CF3)2-Al-O-Al-(CF3)2 and also find the number of pi bond or Back bond?

Generally neutral atom donates only one lone pair to back bonding because after that, electron density on that atom itself highly reduced but the compound [(CF₃)₂-Al-O-Al-(CF₃)₂] is a rare example of two lone pair donation.

Related Questions:

Why trimethylamine amine ( N(CH3)3) is tetrahedral while trisilyl amine (N(SiH3)3) planner.?

Why trimethyl amine {(CH3)3 N:} is pyramidal while trisilyl amine {(SiH3)3N:} is trigonal planer?

Which is/are the correct statement/s about structure of methyl isothiocyanate (H3CNCS) and Silyl isothiocyanate(SiH3NCO)?

What is the Si–N–C bond angle in Silyl isothiocyanate and methyl isothiocyanate (H3CNCS)?

What are the order of extent back bonding, Lewis acid character and nucleophilicity of (BF3, BCl3, BBr3, BI3)boron trihalides?

Arrange the silicon halides into decreasing order of Lewis acids Character? SiF4, SiCl4, SiBr4, SiI4

Which of the following correct statement about structure of Ortho boric acid (H3BO3 ) is/are? Statements are as

Which of the following is correct order of (B-O) bond length of following compounds? (1) B(OH)3 (2) B(OMe)3 and (3) B(Me)2OH

What are the structure of (1) N(SiH3)3 (2) {(Me)3Si}2N-Si(Me)3 (3) HN(SiH3)2 and give the Answers of following questions?