Bonding

Question 1

Principal quantum number

Answer 1

n= energy level of a given electron in an atom to measure size
Range from 1 to 7

Question 2

Azimuthal quantum number

Answer 2

l= number of subshells

Range from 0 to n-1

Question 3

Values of l & corresponding letter

Answer 3

s=0
p=1
d=2
f=3

Question 4

Magnetic quantum number (ml)

Answer 4

Orbitals within a subshell

Ranges from -1 to +1

Question 5

Spin quantum number (ms)

Answer 5

Electrons in each orbital

+/- 1/2

Question 6

Molecular orbital

Answer 6

Combination of tow atomic orbitals

Question 7

Bonding orbital

Answer 7

If signs of wave functions are the same–>more stable

Question 8

Antibonding orbital

Answer 8

If signs of wave functions are different –>less stable

Question 9

Sigma bond

Answer 9

Molecular bond of head to head or tail to tail overlap

All single bonds

Question 10

Pi bond

Answer 10

When two p-orbitals line up in parallel to causes electron cloud overlap
Double and triple bonds
Hinder rotation
Cannot have pi bond without sigma
More bonds, shorter & stronger bond length
Weaker than single bonds though to break

Question 11

Hybrid orbitals

Answer 11

Mixing types of orbitals
Merging of orbitals
Used to minimize repulsion

Question 12

Percent s character

Answer 12

sp3 = 25%
sp2= 33%
sp=50%

Question 13

Tetrahedral bond angles

Answer 13

109.5

Question 14

Conjugation

Answer 14

Alternating single and multiple bonds because this pattern aligns a number of unhybridized p orbitals down backbone of a molecules
Adds stability of pi bonds