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CHEMICAL BONDING > Chemical bonding > Flashcards

Chemical bonding Flashcards

1
Q

What is H-H bond enthalpy in H2 ?

A

435.8 kJ mol-1

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2
Q

What is the concept of resonance?

A

Whenever a single Lewis structure cannot describe a molecule accurately, a no. of structures with similar energy, positions of nuclei, bonding and non bonding pairs of electrons are taken as canonical structures of the hybrid which describes the molecule accurately.

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3
Q

What is N(triple bond)N in N2?

A

946.0 kJ mol-1

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4
Q

What is the bond dissociation enthalpy for HCl?

A

431.0 kJ mol-1

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5
Q

What is bond order?

A

Number of bonds between the two atoms in a molecule.

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6
Q

What is average bond enthalpy?

A

Total bond dissociation enthalpy upon number of bonds broken.

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7
Q

Which molecules and ions have identical bond orders?

A

Isoelectronic.

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8
Q

What will increase if we increase the bond order?

A

Bond enthalpy

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9
Q

How is resonance represented?

A

By double headed arrow.

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10
Q

What are the features of Resonance?

A
  1. Resonance stabilizes the molecule as the energy of the resonance hybrid is less than the energy of any single canonical structure.
  2. Resonance averages the bond characteristics as a whole.
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11
Q

What is non polar covalent bond?

A

When covalent bond is formed between two similar atoms, the shared pair of electron is equally attracted by two atoms. As a result electron pair is situated exactly between the two identical nuclei. This bond is called non polar covalent bond.

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12
Q

What is dipole moment?

A

Product of the magnitude of the charge and the distance between the centers of positive and negative charge.

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13
Q

In which unit is dipole moment expressed?

A

Debye units.

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14
Q

What is the value of 1 Debye?

A

1Debye = 3.33564 x 10^-30 C m

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15
Q

What decreases with increase in bond order?

A

Bond length

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16
Q

What is mathematical meaning of dipole moment?

A

Product of charge and distance of separation.

17
Q

What is the net dipole moment of two O-H bonds in H2O?

A

1.85D = 6.17 x 10^-30 C m

18
Q

What is the molecule (AB) HF:

a) Dipole moment?
b) Geometry?

A

a) 1.78 D

b) linear

19
Q

What is molecule( AB )HCl :

a) Dipole moment?
b) Geometry?

A

a) 1.07 D

b) linear

20
Q

What is molecule(AB) HBr:

a) Dipole moment?
b) Geometry?

A

a) 0.79 D

b) linear

21
Q

What is molecule (AB) HI:

a) Dipole moment?
b) Geometry?

A

a) 0.38 D

b) linear

22
Q

What is molecule (AB) H2:

a) Dipole moment?
b) Geometry?

A

a) 0 D

b) linear

23
Q

What is molecule (AB2) H2O:

a) Dipole moment?
b) Geometry?

A

a) 1.85 D

b) bent

24
Q

What is molecule (AB2) H2S:

a) Dipole moment?
b) Geometry?

A

a) 0.95 D

b) bent

25
Q

What is molecule (AB2) CO2:

a) Dipole moment?
b) Geometry?

A

a) 0

b) linear

26
Q

What is molecule (AB3)
NH3, NF3, BF3:
a) Dipole moment?
b) Geometry?

A

a) 1.47 D, 0.23 D, 0 D

b) trigonal pyramidal, trigonal pyramidal, trigonal planar

27
Q

What is molecule (AB4)
CH4, CHCl3, CCl4
a) Dipole moment?
b) Geometry?

A

a) 0 D, 1.04 D, 0 D

b) all tetrahedral

28
Q

What are the main postulates of VSEPR theory?

A

1) Shape of a molecule depends upon valence shell electron pairs(bonding and anti bonding) around central atom.
2] Pairs of electron in valence shell repel each other because their electron clouds are negatively charged.
3] These pairs of electrons tend to occupy such positions in spaces that minimize repulsion and thus maximize distance between them.
4) The valence shell is taken as a sphere with the electron pairs localizing on the spherical surface at maximum distance from one another.
5) A multiple bond is treated as if it is a single electron pair and two or three electron pairs of a multiple bond are treated as a single super pair.
6) Where two or more resonance structures can represent a molecule, the VSEPR model is applicable to any such structure.

29
Q

What is the repulsive interaction of electron pairs order?

A

Lone pair-lone pair > lone pair-bond pair > bond pair- bond pair.

30
Q

What is O=O bond enthalpy in O2?

A

498 kJ mol-1

31
Q

What is N triple bond N bond enthalpy?

A

946.0 kJ mol^-1

32
Q

What is average bond enthalpy of H2O?

A

464.5 kJ mol^-1

33
Q

What is bond order?

A

Number of bonds between two atoms in a molecule.

34
Q

What increases with increase in bond order?

A

Bond enthalpy

35
Q

What decreases with bond order?

A

Bond length

36
Q

What is resonance?

A

When a single Lewis structure can’t describe a molecule accurately, a no. of structures with similar energy, positions of nuclei, bonding and non-bonding pairs of electrons are taken as the canonical structures of the hybrid which describes the molecule accurately.

37
Q

What is the example of resonance in O3 molecule?

A

Written in GoodNotes. Follow and learn it as it is.

CHEMICAL BONDING (1 decks)

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