Electron Arrangement

Question 1

What ideas did Bohr propose in 1913?

Answer 1

atoms consist of tiny positive nucleus orbited by negative electrons in shells of fixed size

Question 2

What did Chadwick discover in 1932?

Answer 2

Neutron

Question 3

What were Lewis’s ideas to atoms?

Answer 3

-inertness of noble gases due to full outer shell
-ions formed by loss or gain of electrons
-atoms can bond by sharing electrons

Question 4

How are electrons arranged?

Answer 4

In shells/orbitals

Question 5

How do orbitals/shells fill?

Answer 5

first shell closest to nucleus fills then the second and so forth

Question 6

What rule is applied to the number of electrons in each shell?

Answer 6

2n2 (n is the shell number)

Question 7

What is the link between the number of protons and number of electrons?

Answer 7

they are directly proportionate (same number)

Question 8

What do electrons have in shells?

Answer 8

Differing amounts of energy

Question 9

What are the 4 sub-levels?

Answer 9

s,p,d and f

Question 10

What sub levels does level one consist of?

Answer 10

Only an s

Question 11

What sub levels does level two consist of?

Answer 11

s and p

Question 12

What sub levels does level three consist of?

Answer 12

s, p and d

Question 13

What are the shapes of the s,p and d orbitals?

Answer 13

S-spherical
P-dumbbell
D-cloverleaf

Question 14

For each main level, how many sub levels are there in each?

Answer 14

level one has a single s orbital
level two has one s and three p orbitals
level three has one s, three p and five d orbitals

Question 15

How many electrons are in the s-orbital?

Answer 15

hold up to two electrons

Question 16

How many electrons does a p-orbital hold?

Answer 16

up to six electrons

Question 17

How many electrons does a d-orbital hold?

Answer 17

up to ten electrons

Question 18

Where are electrons removed from?

Answer 18

from the lowest energy sub level

Question 19

Why is the 4s sub level labelled before the 3d sub level?

Answer 19

4s sub level is of slightly lower energy

Question 20

How is spin applied to electrons?

Answer 20

two electrons in the same orbital must have opposite spin

Question 21

How is spin represented?

Answer 21

Arrows pointing up and down

Question 22

What are the three main rules for putting electrons in their orbitals?

Answer 22

1. atomic orbitals of lower energy are filled first
2. atomic orbitals fill singly before pairing because electrons repel
3. no atomic orbital can hold more than two electrons

Question 23

Which elements do not follow the main rules of electronic configurations?

Answer 23

Copper and Chromium

Question 24

What is the electronic configuration of Copper?

Answer 24

1s2 / 2s2 / 2p6 / 3s2 / 3p6 / 3d10 / 4s1

Question 25

What is Chromium’s electronic configuration?

Answer 25

1s2 / 2s2 / 2p6 / 3s2 / 3p6 / 3d5 / 4s1