Chem Exam 2

Question 1

what is the principal quantum number symbol?

Answer 1

n

Question 2

what is the symbol for the angular momentum quantum number?

Answer 2

l

Question 3

what is the magnetic quantum number symbol?

Answer 3

m*l

Question 4

what is the spin quantum number symbol?

Answer 4

m*s

Question 5

ionization energy

Answer 5

energy needed to remove an electron from an atom or ion in gas state

Question 6

electron affinity

Answer 6

change in energy associated with adding an electron to a gaseous atom or ion

Question 7

ionization energy trends down groups

Answer 7

removes valence electrons from higher energy levels, so less energy needs to be added (IE decreases)

Question 8

ionization energy trends across periods

Answer 8

nucleus attraction increases so more energy is needed to overcome it (IE increases)

Question 9

electron affinity trends down groups

Answer 9

the atomic number is increasing so the new electron enters a higher energy orbital (EA decreases)

Question 10

electron affinity trends across periods

Answer 10

New electrons are more strongly attracted to the nucleus (EA increases)

Question 11

atomic radius down groups

Answer 11

radius increases

Question 12

atomic radius across periods

Answer 12

radius decreases

Question 13

transition metal exception - valence electrons

Answer 13

valence electrons include electrons in the highest d sublevel

Question 14

Aufbau principle

Answer 14

Fill energy levels from lowest to highest

Question 15

Pauli exclusion principle

Answer 15

each electron has to have a unique set of quantum numbers, only 2 electrons are allowed per orbital and those electrons must have opposite spins

Question 16

Hunts rule

Answer 16

occupy each degenerate orbital with one electron before you start to pair them

Question 17

valence electrons

Answer 17

electrons in the highest principal energy level, typically s and p orbitals

Question 18

s orbitals

Answer 18

0 planar nodes (l=0)
1 orbital per sublevel (m*l=0)

Question 19

p orbitals

Answer 19

1 angular node (l=1)
3 orbitals per sublevel (m*l= -1,0,+1)
degenerate - all three orbitals have the same energy

Question 20

d orbitals

Answer 20

2 angular nodes (l=2)
5 degenerate orbitals per sublevel
(m*l= -2,-1,0,+1,+2)
lobes in between axes: dxy, dxz, dyz
lobes on axes: dx^2-y^2, dz^2

Question 21

f orbitals

Answer 21

3 planar nodes (l=3)
7 degenerate orbitals per sublevel
(m*l= -3,-2,-1,0,+1,+2,+3)

Question 22

standing waves

Answer 22

waves confined to a certain space (ex: wave on a string)

Question 23

frequency equation

Answer 23

C/lamda

Question 24

Energy equation

Answer 24

E=(hc/lamda) or E=h*frequency

Question 25

transition metal exceptions - cations

Answer 25

lose highest s electrons first, then d

Question 26

transition metal exceptions - electron configuration

Answer 26

Cr and Mo; Cu, Ag, and Au
(and all ions with the same electron config)
“move” an electron from the highest s orbital to a d orbital to reach fully filled or half-filled d sublevels

Question 27

wavelength

Answer 27

distance between peaks on a wave (units: nm)

Question 28

frequency

Answer 28

of peaks pass a point in space per second (unit: m/s)