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Chemical bonding flash cards

Flash cards on ionic, covalent and metallic bonding, ion charges, giant and simple structures, diamond and graphite, alloys and the properties each type of bonding gives.

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The cards, front and back

1
Front
Why do atoms form bonds?
Back
To reach a more stable arrangement, usually a full outer shell of electrons, like the noble gases.
2
Front
What is ionic bonding?
Back
The strong electrostatic attraction between oppositely charged ions. It forms when a metal transfers electrons to a non-metal.
3
Front
What happens to the electrons when sodium reacts with chlorine?
Back
Each sodium atom loses its one outer electron to become Na⁺, and each chlorine atom gains one electron to become Cl⁻. The ions attract to form sodium chloride.
4
Front
What charge do ions from groups 1, 2, 6 and 7 usually have?
Back
Group 1: +1. Group 2: +2. Group 6 (group 16): −2. Group 7 (group 17): −1.
5
Front
Describe the structure of an ionic compound.
Back
A giant ionic lattice: a regular, repeating arrangement of positive and negative ions held together by strong attractions in all directions.
6
Front
Properties of ionic compounds
Back
High melting and boiling points, because a lot of energy is needed to overcome the strong attractions. They conduct electricity when molten or dissolved in water, because the ions are free to move, but not when solid.
7
Front
What is the formula of magnesium oxide, and of calcium chloride?
Back
Magnesium oxide is MgO (Mg²⁺ and O²⁻). Calcium chloride is CaCl₂ (one Ca²⁺ for every two Cl⁻), so the charges balance.
8
Front
What is covalent bonding?
Back
A bond formed when two atoms share a pair of electrons. It usually happens between non-metal atoms.
9
Front
What are single, double and triple covalent bonds?
Back
One, two or three shared pairs of electrons. Hydrogen (H₂) has a single bond, oxygen (O₂) a double bond and nitrogen (N₂) a triple bond.
10
Front
Why do simple molecular substances have low melting and boiling points?
Back
The covalent bonds inside each molecule are strong, but the forces between molecules (intermolecular forces) are weak and easy to overcome.
11
Front
Do simple molecular substances conduct electricity?
Back
No. Their molecules have no overall charge and there are no free electrons or ions to carry a current.
12
Front
Describe the structure of diamond.
Back
A giant covalent structure in which each carbon atom is bonded to four others. It is very hard, has a very high melting point and does not conduct electricity.
13
Front
Describe the structure of graphite.
Back
Each carbon atom is bonded to three others in flat layers of hexagons. The layers slide over each other, so it is soft and slippery. One electron per atom is delocalised, so graphite conducts electricity.
14
Front
Name a giant covalent compound other than a form of carbon.
Back
Silicon dioxide (silica), found in sand. Like diamond, it has a very high melting point.
15
Front
What is metallic bonding?
Back
The attraction between a lattice of positive metal ions and a sea of delocalised electrons that move freely through the structure.
16
Front
Why do metals conduct electricity and heat?
Back
Their delocalised electrons can move through the structure, carrying charge and transferring energy.
17
Front
Why can metals be bent and shaped?
Back
The layers of ions can slide over each other while the delocalised electrons keep holding the structure together.
18
Front
Why are alloys harder than pure metals?
Back
An alloy contains atoms of different sizes, which distort the layers and make it harder for them to slide over each other.
19
Front
What is a dot-and-cross diagram?
Back
A diagram showing the outer electrons of each atom, with dots for one atom and crosses for the other, to show how electrons are transferred or shared in a bond.
20
Front
Why are the noble gases so unreactive?
Back
Their atoms already have a full outer shell of electrons, so they have no tendency to gain, lose or share electrons.
21
Front
Why does water have a higher boiling point than expected for such a small molecule?
Back
Water molecules attract each other by hydrogen bonds, which are stronger than the usual intermolecular forces between small molecules.

How to use this template

This deck covers the three main types of chemical bonding and how they explain the properties of substances. It includes ionic bonding and ion charges, giant ionic lattices, writing simple ionic formulas, covalent bonding with single, double and triple bonds, simple molecules and intermolecular forces, giant covalent structures such as diamond, graphite and silicon dioxide, metallic bonding, alloys and dot-and-cross diagrams. It suits GCSE and IGCSE chemistry, Year 10 and Year 11 science, high school chemistry and a quick review for AP, IB or first-year university chemistry. Learn the definitions first, then the property explanations, using Test mode and spaced repetition. Print it double-sided for revision in pairs.

Tips

For every property question, link three things: the type of bonding, the structure, and what has to be overcome or what moves.
Be precise about what breaks when a simple molecular substance melts: the weak forces between molecules, not the covalent bonds.
Practise dot-and-cross diagrams for NaCl, MgO, H₂O, CO₂ and CH₄ until you can draw them without checking.
Remember the conduction rule: something conducts only when charged particles (ions or electrons) are free to move.
Use group numbers to work out ion charges quickly rather than memorising each ion.

Make it fit

Add cards on polymers, fullerenes, graphene or nanoparticles if your course includes them.
Add electronegativity and polar bonds for a higher-level course.
Make a separate card for each compound your teacher asks you to draw, with the diagram described step by step on the back.
Split the deck into a bonding types set and a properties set.

Updated October 28, 2026

The cards, front and back

How to use this template

Tips

Make it fit

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