3.1.1 Periodic trends in bonding and structure

Question 1

properties of most metals

list

Answer 1

• strong metalllic bonds - attraction between teh positive ions and delocalised electrons
• High electrical conductivity
• high melting and boiling points

Question 2

When do metals conduct electricity

Answer 2

In solids and in liquids

Question 3

Why do metals have high melting and boiling points

Answer 3

For most metals, high temperature is required to provide the large amount of energy needed to overcome the strong electrostatic attraction between the cations and electrons. This strong attraction results in most metals having high melting and boiling points

Question 4

describe the solubility of metals

Answer 4

Metals do not dissolve

Question 5

desribe the melting point across periods 2 and period 3

Answer 5

• The melting point increases from group 1 to group 14
• There is a sharp decrease in melting point between group 14 and group 15 - this marks the change from giant to simple molecular structures.
• the melting points are comparatitively low from group 15 to group 18

Question 6

Why do simple molecules have lower melting points that giant structures

Answer 6

On melting giant structures have strong forces to overcome so have high melting points whereas simple molecular structures have weak intermolecular forces to overcome so have much lower melting points.