Unit 5 Structure Properties And Uses

Question 1

What is the explanation for the low melting and boiling points of small molecules

Answer 1

They have week intermolecular forces between the molecules which are easily broken

Question 2

Phosphorus is a solid at room temperature. Suggest why?

Answer 2

It is large in size and increases the number of intermolecular forces resulting in a higher melting and boiling point

Question 3

Diamonds - each carbon atom in a diamond forms ….

Answer 3

4 VERY strong covalent bonds

Question 4

Diamonds - the 4 very strong covalent bonds along with the structure make diamond…

Answer 4

VERY hard and VERY strong with Very high melting points

Question 5

Do diamonds conduct electricity

Answer 5

NO

Question 6

What is the definition of metallic bonds?

Answer 6

The electrostatic force of attraction between a lattice of positive ions and delocalised electrons

Question 7

Explain how metals are able to conduct electricity

Answer 7

Metals contain delocalised electrons these electrons are free to move throughout the structure and this can carry charge

Question 8

Explain why metals are malleable?

Answer 8

Delocalised electrons allow metal atoms to slide over one another these are called slip planes

Question 9

Metal properties - most metals are

Answer 9

HARD STRONG / HIGH MELTING POINTS AND HIGH BOILING POINTS

Question 10

Explains why allows are stronger than the metals from which they are made.

Answer 10

Different elements have different sized atoms
When another element is mixed with a pure metal the new atom will distort the lattice structure this makes it difficult for the atoms to Slide Over the another the alloy is stronger