AQA GCSE Combined Science Foundation (8464), Foundation tier · Chemistry › Atomic structure and the periodic table › The periodic table
Practise Metals and non-metals. 6 exam-style questions on this subtopic, at up to four difficulty levels, with full mark schemes and a progress tracker. Free, no account needed.
Where metals and non-metals are in the periodic table, how their properties differ, and how their atomic structure explains this: metals react to form positive ions, non-metals do not. Questions often give data or properties and ask you to classify an element and explain why.
Key facts
Metal: an element that reacts to form positive ions
Non-metal: an element that does not form positive ions
Metals: left and bottom; non-metals: right and top
Metals: shiny, conductors, malleable, usually high melting point
Non-metals: dull, poor conductors, brittle, low melting point
Metal oxides are basic; non-metal oxides are usually acidic
Metals lose outer electrons; non-metals gain or share electrons
Notes
Where they are
diagram
Most elements are metals.
Metals are found to the left and towards the bottom of the periodic table. Non-metals are found towards the right and the top.
Metals: left and bottom. Non-metals (shaded): top right, plus hydrogen.
Elements that react to form positive ions are metals. Elements that do not form positive ions are non-metals.
Typical properties
Metals: shiny, usually high melting and boiling points, good conductors of heat and electricity, malleable (can be hammered into shape).
Non-metals: dull, low melting and boiling points (many are gases at room temperature), poor conductors, brittle when solid.
Metals form positive ions, and their oxides are basic (they react with acids).
Non-metals form negative ions or share electrons, and their oxides are usually acidic (those that dissolve in water form acidic solutions).
These are typical properties, not rules: Group 1 metals are soft with low melting points, mercury is a liquid, and carbon (a non-metal) has a very high melting point and, as graphite, conducts electricity.
Explaining with electrons
Metal atoms usually have only a few electrons (1, 2 or 3) in their outer shell. In reactions they lose these electrons to form positive ions.
Non-metal atoms usually have 4 to 7 outer electrons. In reactions they gain electrons to form negative ions, or share electrons.
Across a period the number of outer electrons increases, so the elements change from metals on the left to non-metals on the right.
How to answer each type of question
Classify an element from its properties
2 to 3 marksGrade 5
Decide which properties point to a metal and which to a non-metal.
Give your answer.
Quote the evidence from the question for each reason.
Example. Element X melts at 44 °C, does not conduct electricity, and forms an oxide that dissolves in water to give a solution of pH 2. Is X a metal or a non-metal? Give two reasons for your answer.
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Non-metal. Any two reasons: it does not conduct electricity (1); its oxide is acidic, pH 2 (1); it has a low melting point (1).
Compare the properties of a metal and a non-metal
2 to 3 marksGrade 5
Pick properties that differ: conductivity, melting point, appearance, malleability.
Write each point about both elements, with a comparative word.
Example. Compare the physical properties of magnesium and sulfur.
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Magnesium conducts electricity but sulfur does not (1). Magnesium has a higher melting point than sulfur (1). Magnesium is shiny and malleable, but solid sulfur is dull and brittle (1).
Don’t lose marks
Saying all metals have high melting points and densities. Group 1 metals have low melting points and low densities.
Saying non-metals form positive ions.
Classifying from one property only: graphite conducts electricity but carbon is a non-metal.
Using 'strong' to mean 'hard' or 'high melting point'. Use the exact property.
More tips
Memory tricks
Picture a staircase line running roughly from boron down to astatine: metals are to its left, non-metals to its right.
Metals lose electrons; non-metals gain or share them.
When classifying, use the evidence in the question and say which property points to which answer.
For 'compare', write about both elements using comparative words (higher, better conductor).
The definition examiners look for: metals react to form positive ions.
What each grade needs
What you need to be able to do, from the first marks up to the top grade.
Grade 3
Locate metals and non-metals in the tableMetals are on the left and towards the bottom; non-metals are on the right and towards the top.
Grade 4
Define metals by the ions they formElements that react to form positive ions are metals; elements that do not are non-metals.
Grade 4
Compare physical properties of metals and non-metalsMetals are usually shiny, high melting, malleable conductors; non-metals are usually dull, brittle, low melting and poor conductors.
Grade 5
Compare the oxides of metals and non-metalsMetal oxides are basic; non-metal oxides are usually acidic.
Quick recall
Cover the answers and test yourself. The app has these as flashcards that come back just before you'd forget them.
The elements in the periodic table can be classified as metals or non-metals. Give two physical properties that are typical of metals.
e.g. good conductors of electricity; shiny
Sample questions
Written for this site in the style of AQA exam questions. They are not taken from real past papers.
Question 1Easy5 marks
The elements in the periodic table can be classified as metals or non-metals.
(a) Where are metals found in the periodic table? Tick (✓) one box.[1]
To the left and towards the bottom
To the right and towards the top
Only in Group 0
Only in the first row
(b) Complete the sentence. Tick (✓) one box. Metals are elements that react to form ................[1]
negative ions
positive ions
shared pairs of electrons
small molecules
(c) Give two physical properties that are typical of metals.[2]
(d) Are most elements metals or non-metals?[1]
Show the answer and mark scheme
(a)Answer: To the left and towards the bottom
(b)Answer: positive ions
(c)Answer: e.g. good conductors of electricity; shiny
good conductor of electricity
good conductor of heat / thermal energy
shiny (when freshly cut or polished)
malleable / can be hammered into shape
ductile / can be drawn into wires
high melting point
high density
sonorous
(d)Answer: metals
metals
Question 2Medium6 marks
The way an element reacts depends on the arrangement of electrons in its atoms.
(a) Explain, in terms of electronic structure, why the elements on the left-hand side of the periodic table are metals.[2]
(b) The electronic structure of aluminium is 2,8,3. Aluminium forms ions with a charge of 3+. Explain why.[2]
(c) The electronic structure of sulfur is 2,8,6. Sulfur is a non-metal. Predict the charge on a sulfide ion. Explain your answer.[2]
Show the answer and mark scheme
(a)Answer: Their atoms have only 1, 2 or 3 outer electrons, which they lose to form positive ions.
(atoms have) few electrons in the outer shell / 1, 2 or 3 outer electrons
(so they) lose electrons to form positive ions
(b)Answer: Each atom loses its 3 outer electrons, leaving a full outer shell (2,8).
aluminium atoms lose 3 (outer) electrons
to get a full outer shell / the electronic structure of a noble gas / 2,8
(c)Answer: 2−; each sulfur atom gains 2 electrons to fill its outer shell (2,8,8).
2− / −2
sulfur atoms gain 2 electrons (to get a full outer shell / 2,8,8)