The periodic table is a list of elements arranged in order of increasing atomic number. The electronic configuration of the first 20 Elements is shown below:

Metal and Non-metals:

The periodic table can be split into metals and non-metals by the zig-zag line that starts between group 2 and 3 in period 3.

You may wonder who decided where to draw the line. There are numerous ways to classify elements as metals and non-metals and you may previously have used physical properties such as appearance to distinguish between them. E.g. metals are often shiny when freshly cut, metals are malleable etc.

Elements can also be classified by their chemical properties, in this case the acid/base nature of their oxides.

• Oxides of metals form bases e.g. magnesium oxide, MgO

• Oxides of non-metals form acids e.g. sulphur dioxide, SO₂

Group 1, The Alkali Metals

The alkali metals can be found in group 1 of the periodic table.

Physical Properties

1. Silvery/shiny when freshly cut

2. Soft (easily cut with a knife) – become softer as you move down the group

3. Low density – float on water

4. Conduct electricity

Chemical Properties

1. They react with water to give a metal hydroxide and hydrogen

Eg. $metal+ water → metal hydroxide + hydrogen$

2. They become more reactive with increasing atomic number (as you go down the group)

The reaction of Alkali Metals with Water

The alkali metals all react rapidly with water producing hydrogen gas and the corresponding metal hydroxide. This similarity in reactivity creates a family of elements referred to as a group. The similarity in chemical properties within a group is due to all the members having the same number of electrons in the outer shell.

Observation for Li

• Li is stored in oil to prevent it reacting with air

• Li is soft enough to cut with a knife

• Li Foats on water (its density must be less than that of water)

• Li moves slowly around the surface of the water

• Li fizzes when in reacting with water (hydrogen gas is given off)

• The piece of Li disappears once it has all reacted

• The water has become alkaline due to the formation of lithium hydroxide

  2Li(s) + 2H₂O(l)  →  2LiOH(aq) + H₂(g)

Observations for Na:

• Na is stored in oil to prevent it reacting with air

• Na is softer than Li 

• Na floats on water (its density must be less than that of water)

• The heat of the reaction melts the Na into ball

• Na moves quickly around the surface of the water

• Na fizzes rapidly when in reacting with water (hydrogen gas is given off)

• The piece of Na disappears once it has all reacted

• The water has become alkaline due to the formation of sodium hydroxide

  2Na(s) + 2H_2O —> SNaOH(aq) + H_2(g)

Observations for K:

vations for K

• K is stored in oil to prevent it reacting with air

• K is softer than Na 

• K floats on water (its density must be less than that of water)

• The heat of the reaction melts the K into ball

• K moves very quickly around the surface of the water

• K fizzes violently when in reacting with water (hydrogen gas is given off)

• The K ignites and burns with a lilac flame

• The piece of K disappears once it has all reacted

• The water has become alkaline due to the formation of potassium hydroxide

  2K(s) + 2H_2O(l)  → 2KOH(aq) + H_2(g)

Group 7, The Halogens and Redox

The halogens are all non-metals and found in group 7 of the periodic table. As elements they all occur as diatomic molecules. There are trends in some of the physical properties as you go down the group:

1. They become darker in colour

2. Their mpt/bpt increases (hence the gradual change in state at room temperature from gas to liquid to solid)

Key physical properties that you must learn have been highlighted in bold type. The other you can predict based on the trends listed above.

Relative reactivities of the Halogens:

The halogens become less reactive as you go down the group.  This can be illustrated by comparing their reactions with iron or hydrogen. As a result a more reactive halogen will displace a less reactive halogen from a solution of one of its salts.

Eg. If you add colourless chlorine water to a colourless solution of potassium bromide the chlorine will displace the bromine from the potassium bromide as chlorine is more reactive. The solution turns orange as bromine is formed.

To form the ionic equation we rewrite the equation splitting ionic compounds into their ions

$Cl_2(aq) + 2K^-(aq) +2Br_2(aq) → 2K^+(aq) +2Cl^-(aq) + Br_2(aq)$

Remove any ions that appear on both sides of the arrow, these are called spectator ions

$Cl_2(aq) + 2K^+(aq) +2Br^-(aq) → 2K^+(aq) +2Cl^-(aq) + Br_2(aq)$

What remains is the ionic equation

From the ionic equation we see that these displacement reactions are also redox reactions.

In the above example:

• Cl₂ has gained electrons and been reduced to form Cl^- ions

• Br^- ions have lost electrons and been oxidised to form Br₂

Group 8, The Noble Gases

The noble gases are a family of inert gases found in group 0 of the periodic table.  They are very unreactive because they all have full valence shells and hence have a valency of 0.  

The atoms hold onto their electrons too tightly to form covalent bonds or +ve ions.  They don’t gain electrons to form –ve ions because the electrons would have to go into the next shell but as this is further away from the nucleus the nuclear attraction would be insufficient.