LM25-26

Question 1

Sigma bonds form where in relation to axis?

Answer 1

the axis between two atoms

Question 2

Pi bonds form where in relation to axis?

Answer 2

off the axis between two atoms

Question 3

A chemical bond/molecular orbital is

Answer 3

an overlap of electron dense regions between two atomic orbitals

Question 4

VB Theory tells us

Answer 4

locations of every valence electron and a visual representation of atomic orbitals

Question 5

A covalent bond is

Answer 5

the force that attracts shared electron pairs to the two opposite nuclei

Question 6

The strength of a covalent bond is proportional to

Answer 6

the extent of overlapping of atomic orbitals

Question 7

Molecular orbital is

Answer 7

the result of shared electrons between overlapping atomic orbitals

Question 8

s orbitals always create (explanation)

Answer 8

sigma bonds, spherical electron rich region always aligns with the inter-nuclear axis

Question 9

p orbitals that do not overlap head on create

Answer 9

pi bonds

Question 10

Sideways overlap corresponds to

Answer 10

pi bonds

Question 11

Head-on overlap corresponds to

Answer 11

sigma bonds

Question 12

How many orientations of p orbitals can form pi bonds?

Answer 12

2

Question 13

Single bond is what type of bond

Answer 13

Sigma

Question 14

Double bonds include what types of bonds

Answer 14

1 sigma and 1 pi

Question 15

Triple bonds include what types of bonds

Answer 15

1 sigma and 2 pi

Question 16

Resonance includes what types of bonds

Answer 16

1 sigma and a fraction of a pi bond

Question 17

Hybrid Orbitals

Answer 17

a mixture of s, p, or d orbitals

Question 18

How many possible hybrid orbitals are there?

Answer 18

5: sp, sp2, sp3, dsp3, d2sp3

Question 19

The number of hybrid orbitals corresponds with

Answer 19

number of electronic geometries/e rich regions

Question 20

Hybrid orbitals can only form (explanation)

Answer 20

Sigma bonds, all hybrids have s character

Question 21

Why is methane hybridized?

Answer 21

There is only 1 spectral peak for the 4 equivalent C-H bonds, indicating they are all the same because of hybridization

Question 22

sp hybridization (number of e- rich regions, shape)

Answer 22

2 electron dense regions, linear

Question 23

sp2 hybridization (number of e- rich regions, shape)

Answer 23

3 electron dense regions, trigonal planar

Question 24

sp3 hybridization (number of e- rich regions, shape)

Answer 24

4 electron dense regions, tetrahedral

Question 25

dsp3 and d2sp3 only appear in atoms that are

Answer 25

hypervalent (d orbitals, n=3)

Question 26

dsp3 hybridization (number of e- rich regions, shape)

Answer 26

5 electron rich regions, trigonal bipyramidal

Question 27

d2sp3 hybridization (number of e- rich regions, shape)

Answer 27

6 electron rich regions, octahedral

Question 28

As bond length decreases, bond energy

Answer 28

increases

Question 29

Molecular orbitals correspond to

Answer 29

types of bonds

Question 30

Atomic orbitals correspond to

Answer 30

types of orbitals + hybrids

Question 31

Which hybrid typically doesn’t form pi bonds

Answer 31

sp3