Inquiry Question 2: Atomic Structures and Atomic Mass

Question 1

Bohr model

Answer 1

Electrons orbit the nucleus in shells of fixed size and energy

Question 2

Schrödinger model

Answer 2

Depicts electrons as matter waves
“zone of possibility in which electrons can be found -95%
Divides the shells of Bohr’s model in subshell

Question 3

Electron configuration

Answer 3

Principal quantum number = n
The further out a shell from the nucleus  greater its energy
Each shell split into subshells
each at a slightly different energy
Subshell made of a number of orbitals
Orbitals = exact space an electron can be found

Question 4

S

Answer 4

1 orbital
2 electrons
sphere

Question 5

P

Answer 5

3 orbital
6 electrons
dumbbell

Question 6

D

Answer 6

5 orbitals

10 electrons

Question 7

F

Answer 7

7 orbitals

14 electrons

Question 8

Aufbau principle

Answer 8

Orbitals must be filled from lowest energy first

Question 9

Pauli exclusion principle

Answer 9

No more than 2 electrons can occupy a single orbital

Paired electrons - opposite spin

Question 10

Hund’s rule:

Answer 10

every orbital in a subshell must contain 1 electron before it can be paired

Question 11

Flame test

Answer 11

atom in ground state is heated - electrons gain energy and atom becomes excited
electrons then relax back down to lower energy levels by emitting light of a specific wavelength
wavelength corresponds to difference in energy between shells of the atom

Question 12

Li

Answer 12

Crimson red

Question 13

Na

Answer 13

Intense yellow

Question 14

K

Answer 14

Lilac

Question 15

Ca

Answer 15

Brick red

Question 16

Sr

Answer 16

Crimson

Question 17

Ba

Answer 17

Apple green

Question 18

Cu

Answer 18

Green