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Chemical Bonding(11th) formulas

Master Chemical Bonding(11th) through 22 JEE Advanced-level formulas, systematically structured with every variable spelled out. Revise concept-wise, identify the areas where you need improvement, and focus your preparation with greater precision.

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Chemical Bonding(11th), every formula

22 formulas, typeset and free. Print it, or keep it open beside your practice.

Formal charge
$F C = V - L - \frac{1}{2} B$
V=valence e⁻, L=lone-pair e⁻, B=bonding e⁻
Bond order (MOT)
$B O = \frac{1}{2} (N_{b} - N_{a})$
Dipole moment
$μ = q \times d$
Q1MCQDipole moment
The dipole moment is:
- A
  $q\times d$
- B
  $\dfrac{q}{d}$
- C
  $q+d$
- D
  $\dfrac{d}{q}$
Dipole moment units
$1 D = 3.336 \times 1 0^{- 30} C m$
Q1MCQDebye
One Debye equals:
- A
  $3.336\times10^{-30}$ C·m
- B
  $10^{-10}$ C·m
- C
  $1.6\times10^{-19}$ C·m
- D
  $9\times10^{9}$
Percent ionic character
$% = \frac{μ _{o b ser v e d}}{μ _{i o ni c}} \times 100$
Q1MCQ% ionic character
The percent ionic character is:
- A
  $\dfrac{\mu_{obs}}{\mu_{ionic}}\times100$
- B
  $\dfrac{\mu_{ionic}}{\mu_{obs}}\times100$
- C
  $\mu_{obs}\times100$
- D
  $\mu_{ionic}$
Fajans' rules
$covalent character ↑ with small cation, large anion, high charge$
Q1MCQFajans
By Fajans' rules, covalent character increases with:
- A
  a small cation and large anion
- B
  a large cation and small anion
- C
  low charge
- D
  noble gas configuration
Hybridisation (steric number)
$H = \frac{1}{2} (V + M - C + A)$
V=valence, M=monovalent, C/A=charge
Q1MCQHybridisation
The steric number formula for hybridisation is:
- A
  $\tfrac12(V+M-C+A)$
- B
  $V+M$
- C
  $\tfrac12 V$
- D
  $V-M$
sp geometry
$linear, 18 0^{\circ}$
Q1MCQsp geometry
An $sp$-hybridised atom has geometry:
- A
  linear ($180^{\circ}$)
- B
  tetrahedral
- C
  trigonal planar
- D
  octahedral
sp² geometry
$trigonal planar, 12 0^{\circ}$
Q1MCQsp² geometry
An $sp^{2}$-hybridised atom has geometry:
- A
  trigonal planar ($120^{\circ}$)
- B
  linear
- C
  tetrahedral
- D
  octahedral
sp³ geometry
$tetrahedral, 109. 5^{\circ}$
Q1MCQsp³ geometry
An $sp^{3}$-hybridised atom has geometry:
- A
  tetrahedral ($109.5^{\circ}$)
- B
  linear
- C
  trigonal planar
- D
  octahedral
sp³d geometry
$trigonal bipyramidal$
Q1MCQsp³d geometry
An $sp^{3}d$-hybridised atom has geometry:
- A
  trigonal bipyramidal
- B
  octahedral
- C
  tetrahedral
- D
  square planar
sp³d² geometry
$octahedral, 9 0^{\circ}$
Q1MCQsp³d² geometry
An $sp^{3}d^{2}$-hybridised atom has geometry:
- A
  octahedral ($90^{\circ}$)
- B
  tetrahedral
- C
  trigonal bipyramidal
- D
  linear
VSEPR lone-pair effect
$lp-lp > lp-bp > bp-bp repulsion$
Q1MCQVSEPR repulsion
The order of repulsion strength is:
- A
  lp–lp $>$ lp–bp $>$ bp–bp
- B
  bp–bp $>$ lp–bp $>$ lp–lp
- C
  all equal
- D
  lp–bp $>$ lp–lp
Bond length vs bond order
$bond length ↓ as bond order ↑$
Q1MCQBond length
As bond order increases, bond length:
- A
  decreases
- B
  increases
- C
  is unchanged
- D
  becomes zero
Bond energy vs bond order
$bond energy ↑ as bond order ↑$
Q1MCQBond energy
As bond order increases, bond energy:
- A
  increases
- B
  decreases
- C
  is unchanged
- D
  becomes zero
Magnetic character (MOT)
$unpaired e⁻ \Rightarrow paramagnetic$
Q1MCQMagnetic character
A molecule with unpaired electrons is:
- A
  paramagnetic
- B
  diamagnetic
- C
  ferromagnetic
- D
  non-magnetic
Number of σ and π bonds
$single = 1 σ, double = 1 σ + 1 π, triple = 1 σ + 2 π$
Electronegativity difference
$Δ E N > 1.7 \Rightarrow ionic$
Q1MCQEN difference
A bond is largely ionic when the electronegativity difference is:
- A
  $>1.7$
- B
  $<0.5$
- C
  $=0$
- D
  $<1.7$
Lattice energy (Born–Landé)
$U \propto \frac{q _{+} q _{-}}{r _{+} + r _{-}}$
Q1MCQLattice energy
The lattice energy of an ionic solid is proportional to:
- A
  $\dfrac{q_+ q_-}{r_++r_-}$
- B
  $q_+ q_-(r_++r_-)$
- C
  $\dfrac{r_++r_-}{q_+ q_-}$
- D
  $q_+ + q_-$
Hydrogen bond strength
$\approx 10 - 40 kJ/mol$
Q1MCQH-bond strength
The strength of a hydrogen bond is about:
- A
  $10$–$40$ kJ/mol
- B
  $200$–$400$ kJ/mol
- C
  $1$ kJ/mol
- D
  $1000$ kJ/mol
Bond order (fractional)
$B O = \frac{total bonds}{resonance structures}$
Dipole of symmetric molecule
$μ = 0$
Q1MCQSymmetric dipole
The net dipole moment of a symmetric molecule like $CO_2$ is:
- A
  $0$
- B
  maximum
- C
  $q d$
- D
  positive

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Chemical Bonding(11th) formulas

Chemical Bonding(11th), every formula

Formal charge

Bond order (MOT)

Dipole moment

Dipole moment units

Percent ionic character

Fajans' rules

Hybridisation (steric number)

sp geometry

sp² geometry

sp³ geometry

sp³d geometry

sp³d² geometry

VSEPR lone-pair effect

Bond length vs bond order

Bond energy vs bond order

Magnetic character (MOT)

Number of σ and π bonds

Electronegativity difference

Lattice energy (Born–Landé)

Hydrogen bond strength

Bond order (fractional)

Dipole of symmetric molecule

More JEE Advanced Chemistry formula sheets

Other ways to revise this chapter

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