1 - Atomic Structure

Question 1

Symbol for proton

Answer 1

+1e or +1

Question 2

What subatomic particles are in the nucleus?

Answer 2

Protons, neutrons

Question 3

What charge does a neutron have?

Answer 3

No charge

Question 4

What is the mass of a proton?

Answer 4

1 amu (atomic mass unit)

Question 5

Atomic number symbol & where is it found in isotope nomenclature?

Answer 5

Z, bottom left

Question 6

How do you denote electrons?

Answer 6

-1e or -1

Question 7

Mass number symbol & where is it found in isotope nomenclature?

Answer 7

A, top left

Question 8

Isotope definition

Answer 8

Atoms that share atomic number (same element) but different mass numbers (due to different number of neutrons)

Question 9

Atomic mass vs atomic weight

Answer 9

Mass - unique mass for each isotope
Weight - average of the different isotopes (periodic table)

Question 10

Planck relation equation

Answer 10

E = hf
h = Planck’s constant
f = frequency

Question 11

Angular momentum equation

Answer 11

L = nh/2pi

Question 12

Energy of electron equation

Answer 12

E = -R_H/n²

Question 13

Rydberg unit of energy (constant)

Answer 13

2.18 x 10^-18 J/electron

Question 14

Bohr model (what does it look like?)

Answer 14

Nucleus in center, with rings (orbitals) around it

Question 15

Electromagnetic energy of photons equation

Answer 15

E = hc/λ

Question 16

Lyman series

Answer 16

Transitions from higher energy level to n=1

Question 17

Balmer series

Answer 17

Transitions from higher energy level to n=2

Question 18

Paschen series

Answer 18

Transitions from higher energy level to n=3

Question 19

Equation for finding energy difference between higher and lower energy states

Answer 19

E = R_H[1/n_i² - 1/n_f²]

Question 20

Color visible is the light that is/is not absorbed by the compound.

Answer 20

Is not

Question 21

Bohr postulated . . .

Answer 21

Electrons follow a clear circular pathway at a fixed distance from the nucleus

Question 22

Heisenberg uncertainty principle

Answer 22

Impossible to determine both the momentum and position of an electron

Question 23

Pauli exclusion principle

Answer 23

No 2 electrons can have the same set of 4 quantum numbers (energy state)

Question 24

Conditions for 2 electrons to have parallel spins

Answer 24

Same spin quantum number (+ or -)
Occupy different orbital

Question 25

Aufbau principle

Answer 25

Electrons fill from lower to higher energy subshells

Question 26

Where to subtract electrons for electron configuration of cation

Answer 26

Sub shell with highest n value and highest l value

Question 27

Hund’s rule

Answer 27

There is a maximum number of half-filled orbitals with parallel spins
AKA electrons fill each orbital before pairing

Question 28

Paramagnetic

Answer 28

Unpaired electrons will orient spin to align magnetic field

Question 29

Diamagnetic

Answer 29

All paired, slight repulsion by magnetic field

Question 30

Atomic absorption spectrum is unique per element because . . .

Answer 30

Electron must jump by absorbing the energy that is exactly the difference between 2 levels

Question 31

Atomic emission spectrum is unique per element because . . .

Answer 31

Electron emits energy that is exactly equal to energy difference between 2 levels
Energy emitted may correspond to frequency in visible light range

Question 32

Principal quantum number describes . . .

Answer 32

Average energy of a shell, n

Question 33

Azimuthal quantum number describes . . .

Answer 33

Subshells within a given principal energy level, l

Question 34

Magnetic quantum number describes . . .

Answer 34

Particlular orbital within subshell where electron is likely to be found in at a given time, m_l

Question 35

Spin quantum number describes . . .

Answer 35

Spin orientation (+/- 1/2), m_s

Question 36

n + 1 rule

Answer 36

Electrons fill principle energy levels and subshells bind increasing energy

Question 37

2n²

Answer 37

Maximum number of electrons allowed in a single atomic energy level

Question 38

4l + 2

Answer 38

Maximum number of electrons that fill subshell