Module 1

Question 1

mass number

Answer 1

biggest number (number on top)
protons + neutrons

Question 2

atomic number

Answer 2

smaller number (bottom number)
number of protons (or number of electrons)

Question 3

isotopes

Answer 3

atoms of the same element with different numbers of neutrons

Question 4

atomic orbitals

Answer 4

where electrons are found and have complex shapes

Question 5

orbital properties: n=1, where n is the number of energy levels

Answer 5

s orbitals

Question 6

orbital properties: n=2

Answer 6

s + p orbitals

Question 7

orbital properties, n=3

Answer 7

s+p+d orbitals

Question 8

s orbitals

Answer 8

Spherically symmetrical
Electrons can get close to the nucleus
Higher energy level (n), larger the size of the s orbital (not all equal in energy)
only one in each energy level

Question 9

p orbitals

Answer 9

Shape is bi-lobed
electrons further from nucleus
energy is degenerate (the same)
up to 3 p orbitals

Question 10

d orbitals

Answer 10

Have more complex shapes
up to 5 p orbitals

Question 11

Aufbau principle

Answer 11

used to fill orbitals and makes use of Hund’s rule and Pauli exclusion principle

Question 12

Hund’s rule

Answer 12

orbitals are filled in order of energy which the lowest energy level filled first

Question 13

what spins should degenerate orbitals have

Answer 13

parallel spins denoted by an arrow

Question 14

Pauli exclusion principle

Answer 14

An orbital can hold up to 2 electrons, but they must have opposite spins (one up, one down)

Question 15

what is [He] shorthand for

Answer 15

1s^2

Question 16

what is [Ne] shorthand for

Answer 16

1s^2 2s^2 2p^6

Question 17

Trends across (the first 3 rows of) the periodic table: Valence electrons

Answer 17

same group= same number of valence electrons

Question 18

Trends across (the first 3 rows of) the periodic table: electronegativity

Answer 18

Increases from bottom left to top right
Important ones for later: O > N > C

Question 19

Trends across (the first 3 rows of) the periodic table: Van der Waals/ atomic radius

Answer 19

Increases as you move down each group (more electrons)
Decreases as you move from left to right (electron contraction)