Section 1 - Periodicity Flashcards Preview

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Flashcards in Section 1 - Periodicity Deck (15)
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1

What is the trend in atomic radius across a period and why?

Decreases 

-number of protons increases

- electrons are more attracted to nucleus

2

What is the trend in ionisation energy across a period and why?

Increases

- Number of protons increases

- Electrons are more attracted to the nucleus

3

What are the period 3 mpts?

(graph)

4

What is the structure and bonding of Na, Mg and Al?

Metals with metallic bonding - metal ions in a sea of delocalised electrons.

5

What is the trend in mpts of Na, Mg and Al and why?

Increases - metallic bonds get stronger because...

- metal ions have increasing positive charge

-increasing no. of electrons

- decreasing radius

6

What is the structure and bonding of Si?

Macromoleular with a tetrahedral structure - bonded with strong covalent bonds.

7

What is the mpt of Si like and why?

Very high - a lot of energy is required to overcome strong covalent bonds.

8

What is the structure and bonding of P, S and Cl?

Molecular - held together by Van der Waals.

9

What is the formula for a P molecule?

P4

10

What is the formula of a S molecule?

S8

11

What is the formula of a chlorine molecule?

Cl2

12

What are the mpts of P, S and Cl like and why?

Low because...

- Van der Waals are weak to overcome.

13

Which of P, S and Cl has the highest mpt and why?

S - it is the biggest molecule (S8)

14

What is the structure and bonding of Ar?

Ar exists as individual atoms held together by VdWs.

15

What is the mpt of Ar like?

Very low - hardly any VdWs.