18 Questions
What does bond order represent?
The number of bonds shared by two atoms
How does the bond dissociation energy vary with bond polarity?
Increases with greater bond polarity
What is the bond angle for sp hybridization?
180⁰
How does the number of pi bonds affect bond strength?
Increases with more pi bonds
What happens to bond energy as bond length decreases?
Increases
What influences the bond angle in a molecule?
Electronegativity of adjacent atom
Which type of bond has the shortest bond length?
C-F single bond
In which type of hybridization does the bond length decrease with increasing polarity?
sp3
What effect does the number of bonds have on the bond length in a molecule?
Decreases the bond length
Which type of bond has the most ionic character?
C-F single bond
How does the s character of a bond affect its ability to attract electrons and bond length?
More s character increases ability to attract electrons and decreases bond length
Which type of electron delocalization affects bond length?
Pi electron delocalization
In which type of hybridization does Carbon form four bonds with Hydrogen?
Tetrahedral hybridization (sp3)
What is the electronic configuration of Carbon in its ground state?
1s2 2s2 2px1 2py1 2pz0
What type of hybridization occurs to account for the C-H bonds in Carbon?
Tetrahedral hybridization (sp3)
Which type of bond orbitals are involved in Trigonal hybridization?
sp2
What is the structure of Carbon after undergoing Digonal hybridization?
Linear with sp hybridized orbitals
Which type of hybridization is expected to have the highest bond dissociation energy?
sp
Study Notes
Bond Properties
- The number of bonds shared by two atoms is generally related to valency multiplicity between atoms in molecules.
- Bond order includes pi and sigma bonds, while mobile bond order considers only the pi bonds.
- Bond order and mobile bond order for different types of bonds:
- -C–C-: 1, 0
- -C=C-: 2, 1
- -C≡C-: 3, 2
Bond Dissociation Energy
- The amount of energy released or absorbed when a bond is formed, measuring bond strength.
- The greater the bond polarity, the greater the bond energy or bond strength.
- The higher the s character, the greater the bond strength.
- Bond energy increases as the bond length decreases.
- The greater the number of pi bonds, the greater the bond strength.
- Bond energy decreases when there is loss of overlap of hybrid orbitals.
Bond Length
- The intermolecular distance between two atoms sharing a bond.
- Influenced by:
- Repulsion between 2 electron clouds (-) (-)
- Repulsion between 2 nuclei (+) (+)
- Attraction between the nucleus of each and the electrons of the other (+) (-)
- Bond length decreases as the s character increases.
- The more electronegative the adjacent atom, the shorter the bond length.
- Bond length and polarity for different types of bonds:
- C–C: 1.538
- C–N: 1.471
- C–O: 1.430
- C–F: 1.380
Bond Angle
- The angle between any two bonds in a molecule.
- Influenced by hybridization:
- sp3: 109.5⁰
- sp2: 120⁰
- sp: 180⁰
- The greater the number of lone pairs, the smaller the bond angle.
- The more electronegative the adjacent atom, the smaller the bond angle.
Bond Polarity
- Separation of charge in a bond due to differences in electronegativity between atoms.
- Relative electronegativities of atoms:
- F, O, N: 4.0, 3.5, 3.0
- Cl, Br: 2.8, 2.5
- C, S, I: 2.1, 2.1, 2.1
- H, P: 2.1
- The greater the bond polarity, the shorter the bond length.
Hybridization
- The tendency to form bonds is strong among atoms due to the stabilization imparted by bond formation.
- The intermixing of pure atomic orbitals (s,p,d,f) to form a new set of orbitals with distinct properties.
- Hybridization occurs in Carbon to create stable compounds.
- Three types of hybrid bond orbitals:
- Tetrahedral hybridization (sp3)
- Trigonal hybridization (sp2)
- Digonal hybridization (sp)
- Tetrahedral hybridization (sp3) in Carbon:
- Forms four bonds with Hydrogen.
- Accounts for the C-H bonds by hybridizing 2s and 2p orbitals.
Test your knowledge on bond properties including bond order, dissociation energy, length, angle, and polarity. Understand the concepts of bond order and mobile bond order, as well as the energy involved in bond formation.
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