Chapter #3

Question 1

ionic bonds

Answer 1

electrons are transferred from one atom to another and the resulting ions are held together by electrostatic interactions

Question 2

covalent bonds

Answer 2

electrons are shared between atoms

Question 3

which electrons participate in bonding?

Answer 3

valence electrons in the outermost shell

Question 4

principal quantum number

Answer 4

n, corresponds to the energy level of a given electron in an atom and is essentially a measure of size

Question 5

electrons further away from the nucleus have ____ energy

Answer 5

greater

Question 6

azimuthal quantum number

Answer 6

l, subshells, energy increases as this number increases 
l=0: s
l=1: p
l=2: d
l=3: f

Question 7

what is the range of values for the principal quantum number?

Answer 7

n, could be up to infinity (MCAT tests up to 7)

Question 8

what is the range of values for the azimuthal quantum number?

Answer 8

l, 0-n-1

Question 9

Pauli exclusion principle

Answer 9

each electron has a unique combination of quantum numbers

Question 10

magnetic quantum number

Answer 10

ml, the specific orbital within a subshell

Question 11

what is the range of values for the magnetic quantum number?

Answer 11

-l to l

Question 12

what is the range of values for the spin quantum number?

Answer 12

-1/2 and 1/2

Question 13

spin quantum number

Answer 13

ms, indicates the relative spin of an electric in the orbital of a specific subshell.

Question 14

what is the shape of the s subshell

Answer 14

sphere

Question 15

what is the shape of the p subshell

Answer 15

two lobes like a dumbbell located symmetrically about the nucleus with a node at the nucleus

Question 16

node

Answer 16

where the probability of finding an electron is 0.

Question 17

how do molecular orbitals form?

Answer 17

the combination of 2 atomic orbitals

Question 18

when the signs of atomic orbital wave functions are the same, a ________ is produced and if the signs are different then a ________ is produced.

Answer 18

lower-energy (more stable) bonding orbital

higher-energy (less stable) antibonding orbital

Question 19

does a bonding orbital or antibonding orbital have higher energy and which is more stable?

Answer 19

antibonding has higher energy

bonding is more stable

Question 20

what type of bonds are sigma bonds?

Answer 20

single bonds

Question 21

a head-head or tail-tail overlap results in a ___ bond

Answer 21

sigma

Question 22

how is a pi bond formed?

Answer 22

when the p orbitals line up in a side by side fashion, get electron cloud overlap.

Question 23

a double bond has how many sigma bonds and how many pi bonds

Answer 23

1 sigma and 1 pi

Question 24

a triple bond has how many sigma bonds and how many pi bonds

Answer 24

1 sigma and 2 pi

Question 25

the more bonds that are formed between atoms, the overall _____ the bond length

Answer 25

shorter

Question 26

shorter bonds require ____ energy to break

Answer 26

more

Question 27

are sigma or pi bonds stronger?

Answer 27

sigma

Question 28

double bonds have ____ energy than single bonds

Answer 28

more

Question 29

hybrid orbitals

Answer 29

formed by the mixing of different types of orbitals

Question 30

atomic vs. molecular vs. hybrid orbitals

Answer 30

atomic: for one atom molecular: combined when atoms bond hybrid: mixing different types of orbits

Question 31

explain the process of hybridization when you have 2s and 2p electrons

Answer 31

one s goes into the p and then there are 4 electrons each in their own orbital. Then mixing occurs to form the 4 sp^3 hybrid orbitals.

Question 32

___ orbitals participate in pi bond

Answer 32

unhybridized p orbitals

Question 33

the more s character in a bond, the _____ the bond

Answer 33

stronger

Question 34

conjugation

Answer 34

requires alternating single and multiple bonds because this pattern aligns a number of unhybridized p-orbitals down the backbone of the molecule. pi electrons can then delocalized through this p-orbital system adding stability to the molecule.

Question 35

if the stability of the various resonance forms differs, then the true electron density will favor ____

Answer 35

the most stable form

Question 36

electron density is ______ among resonance forms, none of them actually exist on their own (like switching back and forth)

Answer 36

spread out

Question 37

resonance ____ the stability of a molecule

Answer 37

increases

Question 38

what types of resonance forms are favored?

Answer 38

lack formal charge, full octets on EN atoms, stabilize charges through induction or aromaticity,

Question 39

formula for number of electrons in a given energy level

Answer 39

2n^2

Question 40

unhybridized p orbitals

Answer 40

just dont participate in the hybridization process

Question 41

the electron density in a molecule is the weighted average of _____

Answer 41

all possible resonance structures