GCSE Chemistry: Bonding, Structure and Properties Flashcards

Question 1

Define Ionic Bonding.

Accepted Answer

The strong electrostatic attraction between oppositely charged ions, acting in all directions through a giant lattice. It forms when a metal transfers outer electrons to a non-metal.

Question 2

Define Covalent Bond.

Accepted Answer

A shared pair of electrons between two non-metal atoms. The bond is strong because both nuclei are attracted to the shared pair.

Question 3

Define Metallic Bonding.

Accepted Answer

The strong attraction between positive metal ions arranged in a regular pattern and the sea of delocalised outer electrons that they share.

Question 4

What is Ion?

Accepted Answer

An atom or group of atoms that carries an electric charge because it has lost or gained one or more electrons.

Question 5

Define Ion Charge from Group Number.

Accepted Answer

For Groups 1 and 2, ion charge equals the group number as a positive charge; for Groups 6 and 7, it equals the group number minus eight.

Question 6

Define Electrostatic Force.

Accepted Answer

The force of attraction between particles with opposite electric charges, or repulsion between like charges. It holds ions together in an ionic lattice.

Question 7

Define Giant Ionic Lattice.

Accepted Answer

A regular three-dimensional arrangement of a very large number of oppositely charged ions, held in place by ionic bonds acting in every direction.

Question 8

Define Dot and Cross Diagram.

Accepted Answer

A drawing of the outer shell electrons of bonded atoms, with dots for one atom's electrons and crosses for the other's, showing transfer or sharing.

Question 9

Define Ball and Stick Model.

Accepted Answer

A model where balls represent atoms or ions and sticks represent bonds. It shows 3D shape but exaggerates the gaps between particles.

Question 10

Define Small Molecule.

Accepted Answer

A particle made of a few atoms joined by covalent bonds. Substances made of small molecules usually have low melting and boiling points.

Question 11

Define Intermolecular Forces.

Accepted Answer

The weak attractions between separate molecules, much weaker than the covalent bonds inside each molecule. Their strength rises with the size of the molecule.

Question 12

Define Double Covalent Bond.

Accepted Answer

Two shared pairs of electrons between the same two atoms, drawn as a double line between their symbols in a displayed formula.

Question 13

What is Polymer?

Accepted Answer

A very large molecule made of many repeating units joined by strong covalent bonds. Its repeating unit is drawn in brackets with a subscript n.

Question 14

Define Giant Covalent Structure.

Accepted Answer

A huge network of atoms in which every atom is joined to others by strong covalent bonds, so the substance has a very high melting point.

Question 15

Define Silicon Dioxide.

Accepted Answer

A giant covalent compound of silicon and oxygen, also called silica, with every atom covalently bonded into a hard network. It is the main compound in sand.

Question 16

What is Diamond?

Accepted Answer

A form of carbon in which each atom forms four covalent bonds to other carbon atoms in a rigid giant covalent structure.

Question 17

What is Graphite?

Accepted Answer

A form of carbon in which each atom bonds to three others, forming layers of hexagonal rings with only weak forces between the layers.

Question 18

What is Graphene?

Accepted Answer

A single layer of graphite, one atom thick, made of carbon atoms in hexagonal rings. It is very strong, light and conducts electricity.

Question 19

What is Fullerene?

Accepted Answer

Any molecule of carbon atoms with a hollow shape, such as a sphere or tube, built mainly from six-membered rings with some five- or seven-membered rings.

Question 20

What is Buckminsterfullerene?

Accepted Answer

The C60 molecule: sixty carbon atoms arranged as a hollow sphere of hexagons and pentagons. It was the first fullerene discovered, in 1985.

Question 21

Define Carbon Nanotube.

Accepted Answer

A fullerene rolled into a cylinder, very long compared with its narrow diameter, which makes it strong and able to conduct electricity.

Question 22

Define Delocalised Electrons.

Accepted Answer

Electrons that are not tied to one atom or bond and can move freely through a whole structure, letting it conduct electricity.

Question 23

What is Alloy?

Accepted Answer

A mixture of a metal with one or more other elements, usually other metals. Alloys are harder than pure metals and are used where strength matters.

Question 24

Define Pure Metal Layers.

Accepted Answer

In a pure metal, identical atoms sit in regular layers that can slide over each other, which makes pure metals soft enough to bend and shape.

Question 25

Define Melting Point.

Accepted Answer

The temperature at which a substance turns from solid to liquid, the same temperature at which the liquid freezes back to a solid.

Question 26

Define Boiling Point.

Accepted Answer

The temperature at which a liquid turns into a gas throughout, the same temperature at which the gas condenses back to a liquid.

Question 27

Define Particle Model.

Accepted Answer

A simple model of solids, liquids and gases that draws each particle as a small solid sphere, showing arrangement and movement in each state.

Question 28

Define State Symbols.

Accepted Answer

Letters in brackets after each formula in a chemical equation that show its state: (s) solid, (l) liquid, (g) gas and (aq) aqueous.

Question 29

Define Bulk Properties.

Accepted Answer

Properties such as hardness, colour or conductivity that belong to a large amount of a substance. Single atoms do not have them.

Question 30

What is Nanometre?

Accepted Answer

A unit of length equal to one billionth of a metre, written 1 nm or 1 × 10⁻⁹ m. A typical atom has a radius of about 0.1 nm.

Question 31

What is Nanoparticle?

Accepted Answer

A particle between 1 and 100 nm across, made of a few hundred atoms. Its high surface area to volume ratio can give it properties the bulk material lacks.

Question 32

Define Fine Particles (PM2.5).

Accepted Answer

Particles with diameters between 100 and 2500 nanometres. They are larger than nanoparticles and can be breathed deep into the lungs.

Question 33

Define Coarse Particles (PM10).

Accepted Answer

Particles with diameters between 2500 and 10,000 nanometres (2.5 × 10⁻⁶ m to 1 × 10⁻⁵ m), often referred to as dust.

Question 34

Define Surface Area to Volume Ratio.

Accepted Answer

The surface area of an object divided by its volume. For a cube it equals 6 divided by the side length, so smaller particles have higher ratios.

Question 35

Define Uses of Nanoparticles.

Accepted Answer

Applications that rely on the small size and large surface area of nanoparticles, including medicine, electronics, cosmetics, sun creams, deodorants and catalysts.