Atomic Structure, Quantum Numbers, and Electron Configuration

Question 1

List the 3 particles that make up an atom from lightest in mass to heaviest.

Answer 1

Electron = to light to matter 
Proton = 1 amu
Neutron = 1 amu

Question 2

What makes up the electron cloud?

Answer 2

Orbitals/Shells

Question 3

Isotopes

Answer 3

element with a different number of neutrons shown on periodic table

Question 4

Mass Number

Answer 4

Protons + Neutrons

Question 5

Atomic Number

Answer 5

Protons

Question 6

Atomic Weight

Answer 6

Average weight of all isotopes of that element

Question 7

Ions

Answer 7

Atom with negative charge (anion, more electrons) or positive charge (cation, less electrons)

Question 8

Which suffix indicates a greater positive charge on cations?

Answer 8

-ic. -ous has a lesser charge

Question 9

What suffix to monatomic atoms use

Answer 9

• ide

ex: O^-2

Question 10

List the prefixes and suffixes that indicate more oxygens from greater to lesser.

Answer 10

Per-
-ate
-ite
Hypo-

Question 11

In what order are orbitals labeled.

Answer 11

From increasing distance from nucleus. n=1 is closest to nucleus and has the lowest energy.

Question 12

What is the orbital with the lowest energy called.

Answer 12

Groundstate

Question 13

When do electrons become excited?

Answer 13

When it absorbs a photon and jumps from a lower energy level to a higher one.

Question 14

When do electrons stop being excited?

Answer 14

When it emits a photon and jumps from a higher energy to a lower one.

Question 15

List wavelengths from largest (weakest) to smallest (strongest).

Answer 15

Radio 
Microwave
Infrared
Visible (red to blue)
Ultra Violet
X-ray
Gamma Ray

Question 16

Heisenberg Uncertainty Principle

Answer 16

The exact position and velocity of an electron cannot be simultaneously measured

Question 17

How many unique quantum numbers are there? What are they?

Answer 17

4
1. Principal Quantum Number (n)
2. Angular Momentum Quantum Number 
    (Azimuthal) (𝓁)
3. Magnetic Quantum Number (ml)
4. Spin Quantum Number (ms)

Question 18

Principal Quantum Number (n)

Answer 18

Specifies energy level of electron

Ranges from 1 and up

Question 19

Angular Momentum Quantum Number (Azimuthal) (𝓁)

Answer 19

Specifies the shapes of the orbital (subshell)

𝓁 = 0 to n-1

Question 20

Magnetic Quantum Number (ml)

Answer 20

Specifies spatial orientation of the orbital.

-𝓁 to 𝓁of given subshell

Question 21

Spin Quantum Number (ms)

Answer 21

Specifies negative half or positive half spin

+1/2 and -1/2

Question 22

How many electrons can each orbital hold no matter its energy level?

Answer 22

2

Question 23

Pauli Exclusion Principle

Answer 23

No two electrons in an atom can have the same four quantum numbers

Question 24

Aufbau Principle

Answer 24

Electron fills orbital in order of lowest to highest energy

Question 25

Electron Configuration

Answer 25

Shows orbitals filled and amount of electrons.

Question 26

Anion electron configuration move to the?

Answer 26

right on the periodic table

Question 27

Cation electron configurations move to the?

Answer 27

left on the periodic table

Question 28

How are electrons removed?

Answer 28

They are always removed from the subshell with the highest electron number first. So youd remove electrons from 4s before 3d

Question 29

Hund’s Rule

Answer 29

Every orbital in a subshell is occupied by one electron before any orbital is occupied by two.

Question 30

Weird exception to electron configuration?

Answer 30

Half filled or fully filled subshells are the most stable so d orbitals prefer 5 or 10 electrons. So sometimes electrons are stolen from s orbital.