ChemistryScienceGCSEA-Level

Chemistry: GCSE & A-Level Core— MintDeck

150 cards covering the chemistry every GCSE and A-Level student needs. Six topics build from the atom up: atomic structure and the periodic table, the three types of bonding and the structures they create, quantitative chemistry and mole calculations, acids/bases/redox and key reactions, energetics/rates/equilibrium, and an introduction to organic chemistry. Each card gives a clear definition with a worked example, equation, or required-practical fact.

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Topics covered

Atomic Structure & Periodic Table

Subatomic particles, isotopes, electron shells, groups and periods

26 cards

Bonding & Structure

Ionic, covalent and metallic bonding; giant and simple structures

24 cards

Quantitative Chemistry (Moles)

Conservation of mass, moles, concentration, yield, atom economy

22 cards

Acids, Bases & Reactions

pH, neutralisation, redox, reactivity series, electrolysis, gas tests

26 cards

Energetics, Rates & Equilibrium

Exo/endothermic, collision theory, catalysts, Le Chatelier

24 cards

Organic Chemistry

Crude oil, alkanes, alkenes, alcohols, combustion, polymers

28 cards

Card format

Front

Chemistry term, concept, or equation

e.g. Atom economy

Back

Clear definition + a worked example or equation

Preview the cards

Showing 20 of 150

Click any card to flip it. These are the real cards in the deck — same content you get on import.

#1Front

Atom

chemistryatomic

#1Back

The smallest part of an element that can exist; a nucleus of protons and neutrons surrounded by electrons.

#2Front

Proton

chemistryatomic

#2Back

A positively charged subatomic particle in the nucleus; relative mass 1, charge +1.

#3Front

Neutron

chemistryatomic

#3Back

A neutral subatomic particle in the nucleus; relative mass 1, charge 0.

#4Front

Electron

chemistryatomic

#4Back

A negatively charged subatomic particle orbiting the nucleus in shells; relative mass ~1/1840, charge −1.

#5Front

Atomic number (Z)

chemistryatomic

#5Back

The number of protons in an atom; defines the element. Example: Carbon has Z = 6.

#6Front

Mass number (A)

chemistryatomic

#6Back

The total number of protons and neutrons in an atom's nucleus. Example: Neutrons = A − Z.

#7Front

Isotopes

chemistryatomic

#7Back

Atoms of the same element with the same protons but different numbers of neutrons. Example: Carbon-12 and carbon-14.

#8Front

Relative atomic mass (Ar)

chemistryatomic

#8Back

The weighted mean mass of an element's isotopes relative to 1/12 of a carbon-12 atom.

#9Front

Electron shells / energy levels

chemistryatomic

#9Back

Regions around the nucleus holding electrons; max 2, 8, 8 in the first three shells.

#10Front

Electronic configuration

chemistryatomic

#10Back

The arrangement of electrons in shells. Example: Sodium = 2,8,1.

#11Front

Ion

chemistryatomic

#11Back

A charged particle formed when an atom gains or loses electrons. Example: Na → Na+ + e−.

#12Front

Cation vs anion

chemistryatomic

#12Back

A cation is a positive ion (lost electrons); an anion is a negative ion (gained electrons).

#13Front

Periodic table

chemistryatomic

#13Back

Elements arranged in order of increasing atomic number, in periods and groups. Example: Devised by Mendeleev.

#14Front

Group

chemistryatomic

#14Back

A vertical column of the periodic table; elements share the same number of outer electrons and similar properties.

#15Front

Period

chemistryatomic

#15Back

A horizontal row of the periodic table; the number equals the number of occupied electron shells.

#16Front

Group 1 (alkali metals)

chemistryatomic

#16Back

Reactive metals with 1 outer electron; reactivity increases down the group. Example: Lithium, sodium, potassium.

#17Front

Group 7 (halogens)

chemistryatomic

#17Back

Reactive non-metals with 7 outer electrons; reactivity decreases down the group. Example: Fluorine, chlorine, bromine.

#18Front

Group 0 (noble gases)

chemistryatomic

#18Back

Unreactive non-metals with a full outer shell of electrons. Example: Helium, neon, argon.

#19Front

Transition metals

chemistryatomic

#19Back

Central block metals that form coloured compounds, act as catalysts, and have variable oxidation states. Example: Iron, copper, nickel.

#20Front

Metals vs non-metals

chemistryatomic

#20Back

Metals lose electrons to form positive ions and conduct; non-metals gain electrons and are mostly insulators.

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Who is this deck for?

· GCSE and IGCSE chemistry students revising for exams
· A-Level and IB students consolidating the fundamentals
· Students sitting combined/triple science who want quick recall
· Anyone returning to chemistry who wants the core in one place

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This deck is provided for educational purposes only and is not a substitute for a formal chemistry curriculum or specification.