Organic Chemistry Chp 4

Question 1

Pauli Exclusion Principle

Answer 1

each orbital accommodates 2 e- that have the opposite spin

Question 2

Hunds Rule

Answer 2

In degenerate orbitals, one e- is placed in each degenerate orbital before e- pair up.

Question 3

When 2 ____ orbitals overlap, they are replaced by 2 ___ orbitals that are associated with the entire molecule

Answer 3

When 2 Atomic orbitals overlap, they are replaced by 2 MOLECULAR orbitals that are associated with the entire molecule

Question 4

out of bonding Mos and Antibonding Mos, which ones have higher energy

Answer 4

Bonding Mo’s are lower energy and are thus more stable.

Antibonding Mo’s result in higher energy molecular orbitals.

Question 5

______ interference results in _____ molecular orbits

Answer 5

DESTRUCTIVE interference results in ANTIBONDING molecular orbits

Question 6

degenerate orbitals

Answer 6

orbitals with the same energy level but different nodes.

Question 7

how many degenerate orbitals are in the p orbital?

Answer 7

3 (they are all energetically equivalent)

Question 8

methane is sp__ hybridized

Answer 8

sp3

Question 9

what kind of bond results from p orbitals overlapping?

Answer 9

pi orbitals

Question 10

What kind of bond results from sp2 hybridized orbitals overlapping?

Answer 10

sigma bonds

Question 11

what kind of bonds make up a double bond?

Answer 11

1 pi bond, and 1 sigma bond

Question 12

two things that a compound must not have if it is saturated

Answer 12

1) no pi bonds

2) no rings

Question 13

what is the hybridization of a carbocation

Answer 13

sp2 hybridized

Question 14

a molecule that is more stable will be ____ reactive

Answer 14

less

Question 15

A molecule’s stability is _____ related to its reactivity

Answer 15

inversely related to its reactivity

Question 16

2 major ways for organic intermediates to be stabilized

Answer 16

1) inductive effects

2) resonance effects

Question 17

electron-donating groups tent to stabilize _______ intermediates

Answer 17

electron deficient intermediates.

Question 18

why is trichloric acid a better acid than acetic acid? think of methods of stabilization

Answer 18

the trichloric acid is a better acid due to its inductive effects. The chlorines withdraw electrons from the carbon center, making it easier for the -OH group to deprotonate. Essentially, the chlorines “destabilize” the molecule so that it can deprotonate into it’s conjugate base.

it is a better acid than acetic acid because the CH3 groups of acetic acid do not withdraw electrons as intensely as trichloric acid’s chlorines

Question 19

which type of bonds does induction work through?

Answer 19

only sigma bonds. a double bond does not allow inductive effects. ex/ a ketone oxygen will not contribute to inductive effects of a molecule

Question 20

All the carbons in benzene are ____ hybridized, meaning they have an unhybridized p orbital.

Answer 20

sp2 hybridized. They all have resonance

Question 21

bond angle associated with sp, sp3 and sp2 hybridization

Answer 21

sp= 180 degrees
sp3= 109
sp2=120

Question 22

3 criteria for resonance structure stability

Answer 22

1) a resonance structure is more stable if more atoms in the molecule fulfill their octet rule
2) a resonance structure has increased stability if there is a minimized separation of charge and if there are not multiple formal charges on the same molcule
3) a resonance structure has increased stability if the negative charges are placed on an electronegative atom rather than a less electronegative atom

Question 23

A nitro group substituent on a phenol ring in para position will ____ acidity

Answer 23

increase acidity, it is electron withdrawaing and will draw electrons away from the acidic hydrogen

Question 24

a methoxyphenol group substituent on a phenol ring in para position will ____ acidity

Answer 24

decrease acidity. It is electron donating and will destabilize the conjugate base when the molecule is deprotonated because it does not contribute to resonance effects

Question 25

nucleophiles typically take on what type of charge?

Answer 25

negative

Question 26

electrophiles typically take on what type of charge?

Answer 26

positive

Question 27

nucleophiles are also known as

Answer 27

lewis bases

Question 28

how does electronegativity play a role in nucleophilicity?

Answer 28

the LESS electronegative an atom is, the HIGHER the nucleophilicity. It wants positive charges more than an En atom

Question 29

the ___ electronegative an atom is, the _____ the nucleophilicity

Answer 29

the LESS electronegative an atom is, the HIGHER the nucleophilicity. It wants positive charges more than an En atom

Question 30

an electrophile is also known as a lewis ___

Answer 30

acid

Question 31

what happens when an electrophile accepts electrons from a nucleophile?

Answer 31

they form a covalent bond between each other