Chemical Bonding Formulas

Chemical Bonding is the Study of Bonds that exist between atoms or molecules. In this article of ours, you will learn all about Chemical Bonding Formulas to make your work simple. Quickly revise the Chemical Bonding Formulae and have an overview of the Concept. Solve questions related to Chemical Bonding easily taking the help of Cheat Sheet & Tables provided in the forthcoming modules.

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Formulae Sheet of Chemical Bonding

Have a complete understanding of the concept of Chemical Bonding by referring to the Chemical Bonding Formula Collection over here. Get a good grip on the concept by practicing the Formulas provided on a regular basis. Clear all your queries during your homework or assignments with the Important Formulas of Chemical Bonding given.

1. Works Associated with Scientists:

Discovery Discovered by
1. VBT Hietler & London
2. MOT Hund & Muliken
3. Initial Information of VESPER theory Seizwiek and Pawel
4. Hybridisation Pauling
5. H-Bond Latimer – Rod Bush
6. Co-ordinate bond Seizwiek
7. Ionic Radius Pauling
8. Directional prop, in VBT Pauling
9. VESPER Theory Gillispe & Nhyhom
10. Resonance Pauling
11. Octet Law Lewis Kossel
12. Discovery of max. transuranic elements Seberg
13. Co-ordinate bond was told dative bond by Munji
14. Isotopes Sodi

2. Valency:

  • In Period (Li – F) valency with respect to H increases firstly from 1 to 4 then decreases to 1.
  • In Period(Na -Cl) valency with respect to O increases from 1 to 7.

3. Exception of Octet Law:
PCl5, SF6, IF5, IF<sub7, CO, NO, NO2, ClO2, BF3, AlCl3, GaCl3, BeCl2, Ti+3, Mn+2, Li, H, He.

4. (a) Condition necessary for formation of ionic crystal:
[EA + Lattice Energy] > [Sublimation Energy + IP + (Bond dissociation E/2)]

(b) Condition necessary for solubility:
Solvation Energy > Lattice Energy

5. Exceptions of covalent compounds Hard Solid:
AIN, SiC, SiO2, Diamond.

6. (A) Fajan’s Factors:
Following factors are helpful in bringing covalent character in Ionic compounds

  • Small cation
  • Big anion
  • High charge on cation
  • High charge on anion
  • Cation having pseudo inert gas configuration (ns2 p6d10) eg. Cu+, Ag+, Zn+2, Cd+2
  • Coming of colour or darkness of colour in compounds formed with colourless ions.

(B) Ionic potential (Φ) = Charge on cation/radius of cation

7. Molecular Orbital Theory (MOT):

  • Bond order = \(\frac{1}{2}\)(Nb – Na)
  • Molecule having unpaired e– → NO, NO2, O2

8. Relative Bond Strength :
sp3 d2 – >dsp2 – >sp3 – >sp2 – >sp – >p – p (Co-axial) > s – p > s – s > p – p (Co-lateral)

9. VESPER Theory:
(a) (lp – lp) repulsion > (lp – bp) > (bp – bp)
(b) NH3 → Bond Angle 106°45’ because (lp – bp) repulsion > (bp – bp)
H2O → 104°27’ becuase (lp – lp) repulsion > (lp – bp) > (bp – bp)

10. Dipole Moment (µ):
(a) % ionic character = µp/µr × 100 where µr = ed
(b) µ = \(\sqrt{\mu_{\mathrm{A}}^{2}+\mu_{\mathrm{B}}^{2}+2 \mu_{\mathrm{A}} \mu_{\mathrm{B}} \cos \theta}\)
(c) for o, m, p compounds θ is 60°, 120° & 180° respectively.
(d) examples of
µ = 0 [H2, Cl2, F2, CO2, CCl4, BeF2, BF3, PH3, CH4, CS2]
(e) µ NH3 (1.7D) > µ NF3 (0.12D)

Table
Chemical Bonding formulas img 1

11. Bond angle:
(a) NH3 > PH3 > ASH3
(b) H2O > H2S > H2Se
(c) NH3 > NF3
(d) Cl2O > OF2 THO = σt, + Lt
Steric No. = Atoms attached + (LP)t

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