C1.4 Keywords

(3) - C1:3

Extended writing (3) - C1:3

explain why covalent substances do not conduct electricity.

Melting point (2) - C1:2

The temperature at which a change of state occurs from a solid to a liquid.

Graphite (2) - C1:2

each carbon atom is only covalently bonded to three other carbon atoms, rather than to four as in diamond. Graphite contains layers of carbon atoms. The layers slide over each other easily because there are only weak forces between them, making graphite slippery.

Metallic bonding is the strong attraction between closely packed positive metal ions and a 'sea' of delocalised electrons. (1) - C1:1

Giant Ionic (1) - C1:1

Ionic compound (1) - C1:1

This is why metals have high melting points and boiling points. (1) - C1:1

Working with nanoparticles is called nanotechnology.nanometre, 1 nm, is one billionth of a metre (or a millionth of a millimetre) (1) - C1:1

Nanoscience (1) - C1:1

peptide bond (1) - C1:1

A bond created between two amino acids.

Molecule (1) - C1:1

A molecule is an electrically neutral group of two or more atoms held together by chemical bonds.

polypeptides (1) - C1:1

A polymer made of amino acids.

polymerisation (1) - C1:1

A reaction between monomers to create polymers.

monomer (1) - C1:1

A small unit component that can be used to make a polymer.

Alloy (1) - C1:1

An alloy is a mixture of two elements, one of which is a metal. substance made of a metal bond

Negative ion (1) - C1:1

An atom that has gained an electron.

Positve ion (1) - C1:1

An atom that has lost an electron.

Covalent (1) - C1:1

Bonding between two non metals.

Covalent bonding (1) - C1:1

Bonding occurs between two non metals

Ionic bonding (1) - C1:1

Bonding that occurs between a metal and a non metal.

DNA (1) - C1:1

Deoxyribonucleic acid.

Diamond (1) - C1:1

Diamond has a giant molecular structure. Each carbon atom is covalently bonded to four other carbon atoms.

Delocalised (1) - C1:1

Electrons are free to move.

GF (1) - C1:1

Explain why pure water does not conduct electricity but tap water does conduct electricity.

Alkenes (1) - C1:1

Hydrocarbons that contain double bonds.

Sodium Chloride (1) - C1:1

Ionic Compound

lattice (1) - C1:1

Ionic compounds have regular structures in which there are strong electrostatic forces of attraction in all directions between oppositely charged ions.

Condensation reaction (1) - C1:1

Losing water during a reaction.

Polymer (1) - C1:1

Made of chain of chemically bonded monomers.

amine group (1) - C1:1

NH2

Nanoparticles (1) - C1:1

Nanoparticles, are smaller than fine particles (PM2.5), which have diameters between 100 and 2500 nm

Polymers (1) - C1:1

Produced when monomers react.

Fullerenes (1) - C1:1

The fullerenes are a large class of allotropes of carbon and are made of balls, 'cages' or tubes of carbon atoms. Buckminster fullerene is one type of fullerene.

Metallic bonding (1) - C1:1

The particles in a metal are held together by metallic bonds.

Monomer (1) - C1:1

The smallest unit of a polymer.

Surface area (1) - C1:1

The surface area of a solid object is a measure of the total area that the surface of the object occupies.

Volume ratio (1) - C1:1

The surface-area-to-volume ratio, also called the surface-to-volume ratio and variously denoted sa/vol or SA:V, is the amount of surface area per unit volume of an object or collection of objects.

Boiling Point (1) - C1:1

The temperature at which a change of state occurs from a liquid to a gas.

Conduction (1) - C1:1

Transfer of electricity or thermal energy.

intermolecular forces of attraction (1) - C1:1

Weak forces between the molecules

Particles (1) - C1:1

You can use the idea of particles to explain the properties of solids, liquids and gases.

electrostatic forces of attraction (1) - C1:1

attraction in all directions between oppositely charged ions.