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Flashcards in Period 3 Trends Deck (10):
1

Describe and explain the trend in the first three elements of group 3

They increase because the ions increase in charge meaning that the electro static forces of attraction are much stronger and thus require more energy to overcome

2

Why is silicon got the highest boiling point of the non metals in group 3

Giant structure

3

After the metals in group 3 ( except silicon) how are the boiling points determined

Size of the molecule due to van deer walls
P4
Cl2
Argon is a single atom

4

Describe and explain the trend in atomic radius across group 3

Decreases because nuclear charge increases but no increase in shielding

5

Why does atomic radius increase down a group

Less energy on outer shell due to shielding

6

Explain first ionisation energy down the group

More filled inner layers
Shi doing increases
Electron further from nucleus
Decreases

7

Why does first ionisation increase across a period

Number of protons increase but no new shells nuclear charge thus rises

8

Explain the drop in ionisation energy between group 2 and 3 of period 3

Al has an elctrons in 3p1 shell which is easier to remove from than 3s2 which is where the elctrons lie in magnesium

9

Explain the drop between group 5 and 6

Silicon has paired electrons which repel each other thus decreasing the ionisation energy

10

Where would you find a leap in successive ionoisation energy

Where it electrons are being removed from a different energy level