Grade 10 Chemistry Notes Review

This set of flashcards covers important concepts and definitions from the Grade 10 Chemistry curriculum, focusing on atomic structure, electron behavior, and periodic table trends.

Atom

The smallest unit of a chemical element, consisting of protons, neutrons, and electrons.

Nucleus

The dense center of an atom, composed of protons and neutrons.

Electron Cloud

The region around the nucleus where electrons are likely to be found, not in fixed paths.

Rutherford Model

Proposed that the atom has a dense, positive nucleus and that electrons move around it.

Bohr Model

Describes electrons orbiting the nucleus in fixed paths known as energy levels.

Atomic Number (Z)

The number of protons in the nucleus of an atom, which determines the element.

Mass Number

The total number of protons and neutrons in an atom's nucleus.

Democritus

An ancient philosopher who proposed that matter is made up of indivisible particles called atoms.

Dalton's Atomic Theory

States that atoms cannot be created or destroyed and that atoms of the same element are identical.

Thomson Experiment

Experiment that led to the discovery of the electron using a cathode ray.

Gold Foil Experiment

Conducted by Rutherford to demonstrate the existence of a dense nucleus in atoms.

Electromagnetic Spectrum

The range of all types of electromagnetic radiation, including gamma rays and radio waves.

Photon

A particle of light that carries energy and has both wave and particle properties.

Wavelength (λ)

The distance between successive crests of a wave, inversely related to frequency.

Heisenberg Uncertainty Principle

States that it is impossible to know both the exact position and momentum of an electron simultaneously.

Schrödinger’s Equation

A mathematical formula that predicts the likelihood of finding an electron in a given region of space.

Orbitals

Regions in an atom where there is a high probability of finding electrons, represented by specific shapes.

Aufbau Principle

The principle that electrons fill the lowest energy orbitals first.

Pauli Exclusion Principle

The principle stating that no two electrons in an atom can have the same set of quantum numbers.

Hund’s Rule

The rule stating that electrons will fill degenerate orbitals singly before pairing up.

Atomic Radius

The distance from the nucleus to the outermost electrons.

Ionization Energy

The energy required to remove an electron from an atom.

Electronegativity

A measure of an atom's ability to attract and bond with electrons.

Electron Affinity (EA)

The energy change that occurs when an atom gains an electron.

Metals

Elements that are good conductors of heat and electricity and tend to lose electrons.

Nonmetals

Elements that are poor conductors and tend to gain electrons.

Metalloids

Elements with properties intermediate between metals and nonmetals, often used as semiconductors.

Alkali Metals

Highly reactive metals found in Group 1 of the periodic table.

Transition Metals

Elements found in Groups 3-12 that often have variable oxidation states and form colorful compounds.

Noble Gases

Group 18 elements that are inert and have full outer electron shells.