Involves attraction between oppositely charged ions; is typical of metal compounds.

Are strong and substantial energy is required to break ionic bonds.

Involves a shared pair of electrons; is typical of non-metallic elements and compounds.

Are strong and substantial energy is required to break covalent bonds.

Two or more atoms covalently bonded.

Two atoms covalently bonded in a molecule.

Attraction between the positive ions in a regular lattice and the delocalised electrons.

Intermolecular forces

Weak forces between covalent molecules; called van der Waals’ forces.

Molecular covalent substances

Small molecules covalently bonded together e.g. water, carbon dioxide, methane; many are insoluble in water.

A mixture of two or more elements, at least one of which is a metal, and the resulting mixture has metallic properties.

A single layer of carbon atoms, bonded in a hexagonal shape.

Delocalised electrons

Electrons that can move away from their atom to carry energy (electrical or heat).

Structures that are 1–100 nm in size and contain a few hundred atoms.

A substance that consists of only one type of atom and cannot be broken down into simpler substances by chemical means.

A vertical column in the Periodic Table.

A horizontal row in the Periodic Table.

Relative atomic mass (Ar)

The mass of the atom compared with that of the carbon-12 isotope, which has a mass of exactly 12

Relative formula mass (Mr)

a weighted mean of the mass numbers of a compound and the percentage of an element, by mass, in a compound.

Mass of one mole of a substance in grams is numerically equal to the relative formula mass. One mole of a substance is defined as the amount of that substance that contains the same number of particles (atoms, molecules, ions, or other entities) as there are in exactly 12 grams of carbon-12.

Dissolve in water to produce hydrogen (H+ (aq)) ions; the higher the concentration of hydrogen ions in an acidic solution, the lower the pH.

Dissolve in water to produce hydroxide (OH– (aq)) ions.

A metal oxide or hydroxide that neutralises an acid to produce a salt and water and that an alkali is a soluble base.

Strong acids and strong alkalis

Are completely ionised in water.

Weak acids and weak alkalis

Are partially ionised in water.

The reaction between the hydrogen ions in an acid and the hydroxide ions in an alkali to produce water. H+ (aq) + OH– (aq) → H2O(l).

A reaction in which heat is given out.

A reaction in which heat is taken in.

Apply a lighted splint and a popping sound results.

Limewater (calcium hydroxide solution) will change from colourless to milky if the test is positive.

A compound formed when some or all of the hydrogen ions in an acid are replaced by metal ions or ammonium ions. Group 1 (I), Group 2 (II), aluminium and zinc salts are white and if they dissolve in water they give colourless solutions, and that transition metal salts are generally coloured.

A single element or compound not mixed with any other substance.

The temperature at which a solid changes to a liquid.

The temperature at which a liquid rapidly changes to a gas.

A mixture that has been designed as a useful product and is formed by mixing together several different substances in carefully measured quantities to ensure the product has the required properties.

A substance that dissolves in a particular solvent.

CCEA Chemistry Unit 1 Definitions Flashcards

Student preview

72 questions

Show all answers

1.

FLASHCARD QUESTION

Front

Atom

Back

A central positively charged nucleus containing protons and neutrons (most of the mass) surrounded by orbiting electrons in shells.

2.

FLASHCARD QUESTION

Front

Atomic number

Back

The number of protons in an atom.

3.

FLASHCARD QUESTION

Front

Atomic mass

Back

The total number of protons and neutrons in an atom.

4.

FLASHCARD QUESTION

Front

Isotope

Back

Atoms of an element with the same atomic number but a different mass number, indicating a different number of neutrons.

5.

FLASHCARD QUESTION

Front

Compound

Back

Two or more elements chemically combined.

6.

FLASHCARD QUESTION

Front

Ion

Back

A charged particle formed when an atom gains or loses electrons.

7.

FLASHCARD QUESTION

Front

Molecular ion

Back

A charged particle containing more than one atom.

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