Group 1 - Alkali Metals

How can you predict how different elements will react?

From their positions in the periodic table - elements in the same group will react in similar ways

What are the Group 1 Metals known as?

Alkali Metals

What are the Group 1 Metals?

Lithium, sodium, potassium, rubidium, caesium and francium

How many electrons do alkali metals have in their outer shell?

1 - so they all have similar chemical properties

What are the properties of alkali metals?

Low melting and boiling points (compared with other metals) and very soft - they can be cut with a knife

What do alkali metals form?

Ionic compounds - they lose their single outer electron so easily that sharing it is out of the question, so they don’t form covalent bonds

How reactive are Group 1 Metals?

Very - metals readily lose their single outer electron to form 1+ ion with a stable electronic structure

What does it mean if a metal is more readily to lose their outer electrons?

The more reactive it is

What happens as you go down Group 1?

The alkali metals get more reactive - the outer electron is more easily lost because it’s further from the nucleus (the atomic radius is larger) so it’s less strongly attracted to the nucleus and less energy is needed to move it

How is the reactivity of the alkali metals increasing as you move down the group clearly shown?

When they react with water - reactions with cold water produce hydroxide and hydrogen

What happens when alkali metals react with water?

They react vigorously (strongly) and produces hydrogen gas and hydroxide of the metal

What happens when hydrogen gas is present?

It will make a ‘squeaky pop’ with a lighted splint