Metallic bonding and properties of Metals

Question 1

How do metals become ions

Answer 1

Metal atoms need to lose electrons from their outer shells to become a positive ion.

Question 2

What do the electrons in a metal atom look like

Answer 2

In metals the electrons are free to move around in a giant lattice structure. They are delocalised

Question 3

What is metallic bonding?

Answer 3

Metallic bonding is the attraction between the positive ions in a regular lattice and the delocalised electrons

Question 4

What is the relationship between metallic bonding and periodic groups

Answer 4

The group they’re in shows how many electrons they’re losing from their outer shell in an ion e.g.:
Magnesium=2+ (2 lost electrons as they’re in group 2)
Sodium=+ (1 lost electron as they’re in group 1)

Question 5

Why are metals good conductors of heat and electricity?

Answer 5

Because delocalised electrons can move and carry a current throughout the structure. The delocalised electrons also transfer energy as they move, so metals are good conductors of heat

Question 6

Properties of metals

Answer 6

Shiny metallic appearance
Sonorous
Heat conductors
Electricity conductors
Solids at room temperature (except Mercury)
Ductile(flexible)
Malleable (able to be shaped)
High density
High melting points
High tensile strength

Question 7

What is an alloy

Answer 7

A mixture of metal and at least one other element. Alloys can change the structure and properties of a metal. e.g., Steel is iron mixed with carbon and other elements

Question 8

Why is Steel stronger than Iron?

Answer 8

The atoms in pure Iron are arranged in densely packed layers. The atoms of other elements are different sizes. When other elements are added to Iron, it distorts/disrupts the regular structure of Iron atoms. It is more difficult for the layers of iron atoms in Steel to slide over each other and so this alloy is stronger than Iron