Topic 2 - Electron Configuration

Question 1

What are the exceptions for the Schrodinger model

Answer 1

Chromium and Copper

Question 2

Within each shell…

Answer 2

there are subshells

Question 3

each subshell is made up of…

Answer 3

orbitals

Question 4

How many electrons can orbitals hold?

Answer 4

2

Question 5

What are orbitals

Answer 5

Locations of electrons in the Schrodinger model

Question 6

For Abbreviated Configuration what are the rules?

Answer 6

The Nobel gas must be in [ ]
Has to be in shell order, not energy levels.

Question 7

3 Critical Elements

Answer 7

Magnesium - 100-500
Uranium - 5-50
Phosphorus - 50-100

Question 8

Critical Elements are

Answer 8

elements that are heavily relied on for industry and society in areas such as renewable energy, electronics, food supply and medicine. Many exist in only very small quantities on earth. The use is not sustainable.

Conflict element (around war)
- gold, tin, tungsten and tantalum

Question 9

S Group

Answer 9

Group 1 and 2

Question 10

D Group

Answer 10

Transition metals, 3-12, and last column of the ones at the bottom

Question 11

F Group

Answer 11

The ones at the bottom except for last column

Question 12

P Group

Answer 12

Groups 13-18

Question 13

S has…

Answer 13

1 Orbital
2 Electrons

Question 14

P has…

Answer 14

3 Orbitals
6 Electrons

Question 15

D has…

Answer 15

5 Orbitals
10 Electrons

Question 16

F has…

Answer 16

7 Orbitals
14 Electrons

Question 17

Elements in the same ____ have similar properties

Answer 17

Group

Question 18

Why is calcium more reactive than zinc

Answer 18

Zinc has more protons so it has a stronger pull. Electrons are closer to the nucleus and are less likely to be lost or donated

Question 19

Why does fluorine have a higher ionization energy than iodine

Answer 19

It’s harder to get electrons off fluorine because it has a higher electronegativity. The shielding effect caused Iodine to have a lower electronegativity, the pushing makes it harder for iodine to grab electrons

Question 20

what is ionization energy

Answer 20

the amount of energy required to remove an electron
the larger th ionization energy, the more difficult it is to remove an electron

top - bottom = decrease
left - right = increases

Question 21

What is electronegativity

Answer 21

an atom’s desire to grab another atom’s electrons

top - bottom = decreases
left - right = increases

Question 22

What is the atomic radius?

Answer 22

the total distance from an atom’s nucleus to the outermost orbital of the electron

top - bottom = increases
left to right = decreases

Question 23

Shielding Effect

Answer 23

electrons in inner energy levels tend to push electrons in outer energy levels away from the nucleus.

Question 24

What causes the difference in atomic radius

Answer 24

less protons = less attraction to the electron = larger
extra shell = larger

Question 25

Do non-metals have larger ionization energies?

Answer 25

Yes

Question 26

What is electronegativity

Answer 26

an atom’s desire’ to grab another atom’s electrons

top - bottom = decreases
left - right = increases

Question 27

Core/nuclear Charge

Answer 27

Is the pulling power of the nucleus

top - bottom = constant (as you go down the outer electrons are held less tightly
left - right = increases

Question 28

subshell electron configuration

Answer 28

1,2,3,4 shell order

Question 29

Phosphorus

Answer 29

• essential for life (DNA)
• used in fertilizers

Question 30

what determines the chemical properties of an element

Answer 30

number of electrons