The Periodic Table - BBC Bitesize (2024)

Copper has been used by humans for as much as 7000 years and elements such as gold, silver, tin, lead and mercury have been known for many thousands of years. However, the first scientific discovery of an element occurred in 1649 when Hennig Brand discovered phosphorous. The discovery of other elements followed regularly and soon it became necessary to arrange them in some sort of order.

The earliest attempt to classify the elements was in 1789, when Antoine Lavoisier grouped the elements based on their properties into gases, non-metals, metals and earths. Several other attempts were made to group elements together over the coming decades.

Then in 1869, a Russian scientist called Dmitri Mendeleev produced one of the first practical periodic tables. He wrote the properties of the elements on pieces of card and rearranged them until he realised that, by putting them in order of increasing atomic weight, certain properties of elements regularly occurred. At that time, he had only 50 elements to arrange.

Not only did Mendeleev arrange the elements in the correct way, but he also had the foresight to leave gaps for undiscovered elements. Over time these gaps have gradually been filled in as scientists unearthed new elements. For instance they discovered phosphorus when they isolated it from urine.

Mendeleev never received a Nobel Prize for his work, but element 101 was named Mendelevium, Md, after him. Not to miss out, element 102, Nobelium, No, is named in honor of Alfred Nobel, who set aside his vast fortune to establish Nobel Prizes.

The modern periodic table is based closely on the ideas he used:

• the elements are shown by the symbol for their atom
• the elements are arranged in mass order (order of increasing atomic number)
• the horizontal rows are called periods
• the vertical columns are called groups
• elements in the same group (same vertical column) have similar chemical properties
• there are 118 known elements

The main groups are numbered from 1 to 7 going from left to right, and the last group on the right is group 0. The section in the middle of the table is called the Transition Metals.

If you know what one of the elements in a group is like, you can make predictions about the other elements in a group. For example, all the elements in group 1 are reactive metals, and all the elements in group 0 are unreactive non-metals.

The zigzag, staircase, line in the diagram of the periodic table above separates the metals, on the left, from non-metals, on the right. Hydrogen is a non-metal, but it is often put in the middle.

Notice that most elements are metals, rather than non-metals. In fact, nearly 75% of elements are metals.

You will remember from the Chemical study guide that:

An element is a substance that is made up of only one kind of atom and cannot be broken down into any other, simpler substance

A simple shorthand system is used for representing elements. The symbol for the element is the first letter of its English or Latin name, written as a capital letter. If several elements have the same first letter, a second, lower case letter is added.

A list of some common elements and their symbols is shown below

Elements in the same group have similar chemical properties

Group 1 elements have similar physical and chemical properties:

• they are very reactive
• low density - the first three – lithium, sodium and potassium – are less dense than water and so float on water
• very soft - they are easily cut with a knife
• shiny when first cut, but tarnish rapidly in air
• low melting points - the melting points decrease as the atoms get bigger going down the group

The alkali metals are very reactive:

• the reactivity increases as you go down the group because the atoms become larger
• lithium, at the top of the group, fizzes with water; francium, at the bottom of the group, reacts explosively with water
• use tweezers when lifting alkali metals
• use a safety screen
• wear safety glasses and gloves
• use small pieces of metal
• they must be stored under oil to prevent them reacting with air or water vapour

Reaction with water

All Group 1 elements react with water to produce a metal hydroxide and hydrogen. The metal hydroxide produced dissolves in water to form an alkaline solution. The solutions turn universal indicator purple, showing they are strongly alkaline. This is why the group 1 elements are called alkali metals.

Remember: strong alkalis are corrosive - care must be taken when they are used, goggles and gloves should be worn.

The word equation for the reaction between sodium and water is:

sodium + water → sodium hydroxide + hydrogen

The physical properties of the group 1 alkali metals:

All the elements in group 7:

• are non-metals
• have a distinctive or unpleasant smell
• are poisonous (toxic) - a fume cupboard is used for experiments
• are coloured
• have low melting points
• made up of molecules of two atoms e.g. bromine molecule \(Br_2\), chlorine molecule, \(Cl_2\)
• less reactive as you move down the group

The melting points and boiling points of the halogens increase going down group 7, and their colour gets darker.

Astatine is the rarest naturally occurring element in the Earth's crust.

The elements in group 0 are:

• very unreactive
• non-metals
• gases
• colourless
• odourless
• have low boiling points – in fact helium, at the top of group 0, has the lowest boiling point of any element
• found in the Earth’s atmosphere in small amounts
• used in advertising signs as they can glow with distinctive colours when a high voltage is applied across them
• formed of particles with one atom

All noble gases have low boiling points. Their boiling points increase as you move down the group. The density of the gas increases as you move down the group too.

The Group 0 elements are called noble gases because they are so “majestic” that, in general, they don't react with anything. For this reason, they are also known as inert gases.

The transition metals are in the block in the middle of the Periodic Table, between Groups 2 and 3. They are all metals and include many common metals such as chromium (Cr), iron (Fe), nickel (Ni) and copper (Cu).

The transition metals are:

• all metals
• high density
• conductors of electricity
• conductors of heat
• have high melting point (except mercury which is liquid at room temperature)
• often form coloured compounds

The table below compares the physical properties of the transition metals and the alkali metals.

Some of the coloured compounds:

Groups in the periodic table contain elements with similar properties. The trends in properties allow scientists to make predictions.

For example:

the group 1 alkali metals are:

The chemical elements of the human body, in order of % found are:

Small traces of several other elements can also be found:

Fluorine (bones, teeth), Chlorine (in body liquids), Manganese (in enzymes), Iron(in enzymes, blood)As well as minimal traces of:Aluminium, Arsenic, Bromine, Cobalt, Copper, Iodine, Lead, Lithium, Molybdenum, Selenium, Silicon, Strontium, Vanadium, Zinc

Summary

• The modern periodic table is based on Dmitri Mendeleev’s 1896 observations that chemical elements can be grouped according to common chemical properties
• the elements are arranged in order of increasing atomic number
• atomic number increases from left to right and from top to bottom
• the horizontal rows are called periods
• the vertical columns are called groups
• elements in the same group have similar chemical properties
• trends in properties of the elements in a group allow us to make predictions
• group 1 – the alkali metals
• group 7 – the halogens
• group 0 – the noble gases
• the central block between groups 2 and 3 – the transition metals
• there are 118 known elements
• the only letter not in the periodic table is the letter J