valence shell electron pair repulsion theory
DESCRIPTION
chemistryTRANSCRIPT
Kips Unit 4, UHS Topic 4(A), 2 MCQ’s
Contents• VSEPR Theory• VBT• Hybridization• Bond energy, Bond
length• Bond Polarity
Chemical Bonding
Muhammad Farooq Mukhtar
Valence Shell Electron Pair Repulsion Theory
Features• Only applicable for AB2 and above
systems.• Molecular geometry depends on
both lp and bp of e’s.• Maximum separation between
electron pairs to minimize repulsions.
• Space occupied: lp > bp
• lp- lp > lp- bp > bp- bp
In ABx type molecule B representsA. Bond pairsB. Lone pairsC. Electron pairsD. Bonded atoms
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Valence Shell Electron Pair Repulsion Theory
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Type Total e pairs Bond pairs Lone pairs Electronic
geometryMolecular geometry Angle Example
AB2 2 2 - Linear Linear 180o
AB3 3
3 -
Triangular planner
Triangular planner 120o
2 1 BentLess than 120o
Valence Shell Electron Pair Repulsion Theory
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Type Total e pairs Bond pairs Lone pairs Electronic
geometryMolecular geometry Angle Example
AB4 4
4 -
Tetrahedral
Tetrahedral 109.5o
3 1 Trigonal pyramidal
Less than
109.5o
2 2 BentLess than
109.5o
Valence Shell Electron Pair Repulsion Theory
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Valence Shell Electron Pair Repulsion Theory
All are incorrect statements about bond angle in NH3 & NF3 excepts
A. Both have 104.5o
B. Both have 107.5o
C. NF3 has greater bond angle
D. NH3 has greater bond angle
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Pick the one with bent shapeA. CO2
B. SnCl2
C. CS2
D. HgCl2
The H-O-H bond angle in H2O(s)
isA. 104.5o
B. 107.5o
C. 109.5o
D. Less than 104.5o
H2S & H2O has same hybridization and no of lone pairs. Select the correct option about bond angle
A. Both have same bond angleB. H2S has greater bond angle
C. H2O has greater bond angle
D. Difficult to predict
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Valence Bond Theory
Bond formation
No of bonds = unpaired e’s
Overlapping of atomic orbitals
Strength of bond α extent of overlapping
Which one will result in stronger covalent bondA. s-s overlapB. s-p overlapC. p-p overlapD. All have same strength
All statements are correct about VBT exceptA. No idea about paramagnetismB. Justifies valencies of all elementsC. Colour of complexes is not
explainedD. Maximum sigma bonds b/w two
atoms is always one
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Valence Bond Theory
Formation of s bond
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Valence Bond Theory
s bond
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Sidewise overlapping
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Sidewise overlapping
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Sidewise overlapping
Planar molecule with p cloud above and below the plane
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Formation of p Bond
Hybridization
Features• Intermixing of atomic orbitals of
slightly different energy and shapes to form hybrid orbitals of same energy and shape.
• No of hybrid orbitals = No of atomic orbitals intermixed
• Occupied by lp and bp of sigma bond
• It decreases reactivity of molecules.
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Hybridization
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Property sp3 sp2 sps-orbitals 1 1 1
p-orbitals 3 2 1
Hybrid orbitals 4 3 2
% s character 25 % 33 % 50 %
% p character 75 % 66 % 50 %
Unhybrid orbitals 0 1 2
Sigma bonds 4 3 2
Pi bonds 0 1 2
Geometry Tetrahedral Triangular planner Linear
Bond angle 109.5o 120o 180o
Example CH4, CCl4 BF3, AlCl3 BeCl2, CO2
sp3 Hybridization
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
sp3 Hybridization
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
sp2 Hybridization
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
sp Hybridization
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Overlap of Be and Cl orbitals to form BeCl2
Which hybridized carbon is more electronegativeA. sp3 hybridizedB. sp2 hybridizedC. sp hybridizedD. Electron attracting power of
C-atom is always same
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Which one the following has only sigma bonds
A. Acetic acidB. Ethyl alcoholC. PropeneD. Benzene
The hybrid state of S in SO3 is similar to C atom in
A. C2H2
B. C2H6
C. CO2
D. C2H4
The pair having similar geometry is
A. BF3 , NH3
B. BeF2 , H2O
C. BF3 , AlCl3
D. BF3 , PCl3
Hybridization
Bond Energy & Bond Length
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Bond Energy
Directly related toi) ∆ E.N
ii) % s characteriii) B.O
Inversely related toi) Size
ii) Lone pairsiii) B.L
Bond Energy & Bond Length
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Bond Length
Inversely related toi) ∆ E.N
ii) % s characteriii) B.O
Directly related toi) Size
ii) Lone pairs
Which of the following overlap will result in minimum bond lengthA. sp3 – s overlapB. sp2 – s overlapC. sp – s overlapD. p-p overlap
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Minimum bond energy is observed in which of the following
A. HFB. HClC. HBrD. HI
Maximum bond energy is in the case of
A. C-CB. N-NC. O-OD. F-F
Bond Energy & Bond Length
No lone pair in CA- 348 Kjmol-1
B- 163 Kjmol-1
C- 146 Kjmol-1
D- 139 Kjmol-1
A- 566 Kjmol-1
B- 431 Kjmol-1
C- 366 Kjmol-1
D- 299 Kjmol-1
Dipole Moment
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Features• Mathematical determination of polarity of bond.
µ = q × rUnits: (SI Unit = Cm) (Derived Unit = Debye)
1D = 3.336 × 10-30 Cm• %age ionic character = µobserved ÷ µionic × 100• Geometry of molecule
Atomicity µ = 0 µ ǂ 0
AB2 Linear -
AB3 Triangular Planner Bent
AB4 Tetrahedral Pyramidal, Bent
Which of the following is non-polar but contains polar bondsA. H2O
B. SO2
C. CS2
D. All are polar
KIPS UNIT 4, UHS TOPIC 4(A), 2 MCQ’s
Which of the following isomer of xylene posses maximum polarity
A. B.
C. D. All same
Which one has zero dipole momentA. B.
C. D. All same
Dipole Moment
QUESTIONS