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What determines the shape of a

molecule?

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Draw and name the bonding in the following four

molecules. Label the bond angles.

a) AlCl3

b) SiF4c) SF6d) CO2

Put the strengths of repulsion in order.

lone-lone bonded-bonded bonded-lone

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Now draw the following moleculesexplaining the bond angles in

each.

CH4NH3

H2O

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Why is the hydrogen-hydrogen bondNON-POLAR in H2?

What happens to the bond if we haveHCl?

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Define:

-electro negativity

-Permanent dipole

Why is CH4 a non-polar moleculedespite having permanent dipoles?

Why is H2O polar and CO2 non-polar?

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In terms of electronegativitywhich types of elements are

most likely to form- A non polar covalent bond

- An ionic bond

- Polar covalent bonding?

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What causes intermolecular forces?

What are the 3 types?

Can you put them in order of relativestrength?

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Where do permenant dipole-dipoleinteractions come from?

Can you give an example?

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Explain how van der waals forces occur.

What increases the strength of van der

waals forces?

Explain why boiling point increases down agroup.

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What is a hydrogen bond? Give

an example in your answer.

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Explain these properties of H2Oin terms hydrogen bonds.

1. Ice is less dense than water

2. Water has relatively highmelting and boiling points

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Draw a picture and explain it to describe

metallic bonding.

Why do metals have high melting andboiling points?

Why can they conduct electricity?

Why are the malleable/ductile?

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How does metallic bonding differfrom covalent bonding?

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Draw and explain the giant ionic latticestructure between sodium and

chlorine.

Why does the MgO lattice have highermelting and boiling points than NaCl

lattice?

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Explain the difference in electricconductance of an ionic compound

when solid, molten or aqueous.

Why do ionic compounds dissolve in polar

solutions but not non-polar?

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16/18

Draw a simple molecular lattice of I2molecules naming and labelling any

BONDS and any FORCES.

When I2 melts or boils what is happening?

Describe the

a) melting/boiling pointb) Electrical conducancec) Solubility

Of simple molecular lattices

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What is the difference betweensimple molecular structures and

giant covalent structures?

What properties do giant covalentstructures GENERALLY have?

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Diamond Graphite

Drawing

ElectricalConductivity

Hardness