vocab and calculations

Question 1

How to calculate electron affinity of a 1 electron species

Answer 1

electron affinity = – ionization energy
use energy from one electron species

Question 2

What to consider when determining melting/boiling point

Answer 2

molecular weight, bonds, structures

Question 3

Which atoms can do hydrogen bonding?

Answer 3

nitrogen, oxygen, fluorine

Question 4

lattice energy

Answer 4

inversely proportional to distance between ionic radius
as distance increases, energy decreases

Question 5

Van de wall forces in increasing strength

Answer 5

london dispersion, dipole - dipole, hydrogen bonding

Question 6

electronic transition

Answer 6

visible light and ultra violet

Question 7

rotational energy

Answer 7

microwaves

Question 8

vibrational energy/ionization

Answer 8

ultra violet and gamma ray

Question 9

seeing colour…

Answer 9

for the colour that’s seen, the opposite is absorbed
ex: if it’s shown as orange, it absorbed blue

Question 10

HOMO and LUMO

Answer 10

HOMO: the highest occupied molecular orbital (ni)
LUMO: the lowest unoccupied molecular orbital (nf)

Question 11

conjugated pi system

Answer 11

molecules with continuous chains of alternating multiple and single bonds
for multiple bonds, only one of the pi bonds are conjugated

Question 12

relationship between parent shape and hybridization of central atom in a molecule

Answer 12

linear: sp
trigonal planar: sp2
tetrahedral: sp3
trigonal bipyramidal: sp3d
octahedral: sp3d2

Question 13

for multi bonds in a molecule

Answer 13

first bond is sigma, others are pi

Question 14

for multi bonds in a molecule

Answer 14

first bond is sigma, others are pi
for a conjugated system, only one pi bond counts

Question 15

configuration for second period p-block oxygen and onward

Answer 15

sigma 2p, pi 2p, pi* 2p, sigma* 2p

Question 16

configuration for second period p-block before oxygen

Answer 16

pi 2p, sigma 2p, pi* 2p, sigma* 2p

Question 17

bond order =

Answer 17

(bonding e- – anti bonding e-)/2

Question 18

relationship between atomic orbitals and molecular orbitals

Answer 18

number of atomic orbitals = number of molecular orbitals

Question 19

electron affinity

Answer 19

the want to gain an electron
increases moving up and to the right of the periodic table

Question 20

ionization energy

Answer 20

increases moving up and to the right of the periodic table

Question 21

atomic radius

Answer 21

increases movind down and to the left of the periodic table

Question 22

ionic radius

Answer 22

cation: increase as you move to the left

Question 23

ionic radius

Answer 23

cation: increase as you move to the left of the periodic table
anion: increase as you move to the right of the periodic table

Question 24

excited state

Answer 24

when a species has an electron configuration that breaks either hunds rule of aufbau principle

Question 25

exceptions for electron configurations

Answer 25

cr: 4s1 3d5 cu: 4s1 3d 10

Question 26

where to transition metal ions lose electrons from first

Answer 26

the s orbital

Question 27

degenerate

Answer 27

orbitals with the same energy

Question 28

hunds rule

Answer 28

fill all orbitals of the same energy level with one electron before adding a second one

Question 29

pauli exclusion principle

Answer 29

no two electrons may have the same four quantum numbers

Question 30

aufbau principle

Answer 30

fill electrons in the lowest energy orbitals first before moving on

Question 31

relationship between quantum number l and ml

Answer 31

ml = 2l+1

Question 32

relationship between energy and wavelength

Answer 32

inversely proportional as energy increases, wavelength decreases and vice versa

Question 33

one electron species energy

Answer 33

as n increases, space between n values decrease

Question 34

1D particle in a box energy

Answer 34

as n increases, space between n values increase

Question 35

angular nodes

Answer 35

l value: s = 0 p = 1 d = 2 f = 3

Question 36

radial nodes

Answer 36

n - 1 - # of angular nodes (l value)

Question 37

principal quantum numbers

Answer 37

n = shell, in integers l = sub shell,