Intermolecular forces

Created by: jodi
Created on: 08-01-19 18:55

What structures are sulfur, iodine and water?

Molecular covalent crystals.

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What are the properties of molecular covalent crystals?

Low melting and boiling points due to weak intermolecular forces; don't conduct electricity as there are no free electrons/ions to carry the charge.

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Explain the bonding of diamond.

Each carbon atom is covalently bonded to four others in a tetrahedral arrangement. Its rigid 3-D structure combined with the many covalent bonds makes it hard. It doesn't conduct electricity as there are no delocalised electrons to carry the charge.

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Expalin the bonding of graphite.

Each carbon is covalently bonded to three others in a layered haxagonal structure. The delocalised electrons within layers can move and carry the charge so in the solid state, graphite can conduct electricity. Molten graphite does not conduct.

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Why does graphite act as a lubricant?

The layers can slide over each other due to the weak bonds between them.

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State the trend in melting point across period 3.

From sodium to argon, the melting point increases to silicon then decreases.

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Explain the trend in melting point across period 3. (Na to Al)

Fron Na to Al, the metallic bond increases in strength because there are more outer shell electrons that can be delocalised so there is a greater attraction between the electrons and the ions in the metallic structure.

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Explain the trend in melting point across period 3. (S)

Silicon has a giant covalent structure so it's melting point is very high as a substantial amount of energy is required to break the large number of strong covalent bonds.

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Explain the trend in melting point across period 3. (P to Ar)

Only van der waals forces of attraction exist between molecules of P, S and Cl. S has the highest boiling point between the three as it has the most electrons hence the VDWs are stronger requiring more energy to break.

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Other cards in this set

Card 2

Front

What are the properties of molecular covalent crystals?

Back

Low melting and boiling points due to weak intermolecular forces; don't conduct electricity as there are no free electrons/ions to carry the charge.

Card 3

Front

Explain the bonding of diamond.

Back

Card 4

Front

Expalin the bonding of graphite.

Back

Card 5

Front

Why does graphite act as a lubricant?

Back

View more cards

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Intermolecular forces