Chemistry for CSEC - States of Matter and Atomic Structure

Flashcards for reviewing chemistry concepts based on the provided textbook pages.

Matter

Anything that has mass and occupies space.

Particulate Theory of Matter

All matter is made up of particles.

Diffusion

Movement of particles from an area of higher concentration to an area of lower concentration until they are evenly distributed.

Osmosis

Movement of water molecules from a region with a lot of water molecules to a region with fewer water molecules through a differentially permeable membrane.

Melting Point

Constant temperature at which a solid changes into a liquid.

Boiling Point

Constant temperature at which a liquid changes into a gas.

Freezing Point

Constant temperature at which a liquid changes into a solid.

Saturated Solution

A solution which contains as much solute as can be dissolved at a given temperature, in the presence of undissolved solute.

Solubility

The mass of solute that will saturate 100 g of solvent at a given temperature.

Element

A pure substance that cannot be broken down into any simpler substances by any ordinary chemical or physical means.

Compound

A pure substance that contains two or more different types of element which are bonded together chemically in fixed proportions.

Mixture

Consists of two or more substances (elements and/or compounds) physically combined together in varying proportions.

Solution

A homogeneous mixture consisting of two or more components, one of which is usually a liquid.

Suspension

A heterogeneous mixture in which minute, but visible, particles are dispersed in another substance, usually a liquid.

Colloid

A heterogeneous mixture in which the particles of one substance are dispersed in another substance, usually a liquid.

Atom

The smallest component of an element that can exist and still have the same chemical properties as the element.

Atomic Number

Number of protons in the nucleus of one atom of an element.

Mass Number

Total number of protons and neutrons in the nucleus of one atom of an element.

Electronic Configuration

Arrangement of electrons in the energy shells of the atom.

Electrostatic Force of Attraction

Force that exists between two oppositely charged particles.

Isotopes

Different atoms of the same element that have the same number of protons and electrons but different numbers of neutrons.

Isotopy

Occurrence of atoms of the same element that have the same number of protons and electrons but different numbers of neutrons.

Relative Atomic Mass

Average mass of one atom of an element compared to one-twelfth the mass of an atom of carbon-12.

Radioactive Isotope

Has an unstable nucleus which decays spontaneously to a more stable form by emitting particles and radiation.

Periodicity

Recurrence of elements with similar physical and chemical properties at regular intervals in the periodic table.

Cation

Positively charged ion formed when a metal atom loses electrons.

Anion

Negatively charged ion formed when a non-metal atom gains electrons.

Covalent Bond

A chemical bond formed by the sharing of a pair of electrons between two atoms.

Molecule

A group of two or more atoms which are covalently bonded together strongly enough to behave as a single unit in a chemical reaction.

Chemical Bond

Force of attraction between atoms that results from the redistribution of their electrons.

Valence Number (Valency)

Maximum number of bonds an atom can form when it bonds with other atoms.

Ionic Bonds

Chemical bonds created by the electrostatic forces of attraction between the positively charged cations and negatively charged anions in ionic compounds.

Electronegativity

A measure of how strongly an atom attracts electrons.

Oxidising Agent

An oxidising agent brings about the oxidation of another reactant by causing an atom or ion in that reactant to lose electrons. In the process, the oxidising agent gains electrons.

Oxidising Strength

Measure of how easily one substance takes electrons from another substance.

Ion

Is an electrically charged particle formed when an atom loses or gains electrons.

Allotropes

Are different structural forms of the same element in the same physical state.

Allotropy

Is the existence of different structural forms of the same element in the same physical state.