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Cambridge AS and A Level Chemistry (9701) Flashcards
50 question-and-answer cards covering Chemistry (9701) as it is examined in Cambridge AS and A Level. 24 of them are printed below, taken from across the deck — no signup, no paywall on the preview.
24 sample cards from the Chemistry (9701) deck
Sampled from the end of the deck, so these are different cards from the ones shown on the syllabus page.
How is the number of moles of a gas calculated from its volume at r.t.p.?
Moles = volume (dm³) / 24 (or volume in cm³ / 24000).
Define percentage yield.
Percentage yield = (actual amount of product / theoretical amount of product) × 100.
What is the limiting reagent in a reaction?
The reactant that is completely used up first, which therefore determines the maximum amount of product formed.
Define an ionic bond.
The electrostatic attraction between oppositely charged ions, formed by the transfer of electrons from a metal to a non-metal.
Define a covalent bond.
A shared pair of electrons between two atoms, where the shared electrons are attracted to both nuclei.
Define a dative (coordinate) covalent bond.
A covalent bond in which both shared electrons are provided by one atom.
Define metallic bonding.
The electrostatic attraction between positive metal ions and a sea of delocalised electrons.
Why do metals conduct electricity and are malleable?
Delocalised electrons are free to move and carry charge; layers of ions can slide over one another without breaking the metallic bonding.
State the main idea of VSEPR theory.
Electron pairs around a central atom repel each other and arrange themselves as far apart as possible to minimise repulsion, determining molecular shape.
What is the shape and bond angle of a molecule with 4 bonding pairs and no lone pairs (e.g. CH₄)?
Tetrahedral, with a bond angle of 109.5°.
What is the shape and bond angle of ammonia (NH₃, 3 bonding pairs and 1 lone pair)?
Pyramidal (trigonal pyramidal), with a bond angle of about 107°.
What is the shape and bond angle of water (H₂O, 2 bonding pairs and 2 lone pairs)?
Bent (non-linear), with a bond angle of about 104.5°.
What are the shapes and bond angles for 2, 3, 5 and 6 bonding pairs (no lone pairs)?
2 = linear (180°), 3 = trigonal planar (120°), 5 = trigonal bipyramidal (90° and 120°), 6 = octahedral (90°).
Rank the repulsion strengths of lone pair (lp) and bonding pair (bp) interactions.
lp–lp > lp–bp > bp–bp (lone pairs repel more strongly, reducing bond angles).
List the three types of intermolecular forces in order of increasing strength.
Van der Waals (London dispersion) forces < permanent dipole-dipole forces < hydrogen bonding.
What causes van der Waals (London dispersion) forces?
Temporary instantaneous dipoles caused by the random movement of electrons, which induce dipoles in neighbouring molecules.
What three conditions are required for hydrogen bonding?
Hydrogen bonded to a highly electronegative atom (N, O or F), and a lone pair on the N, O or F of a neighbouring molecule.
Why does ice have a lower density than liquid water?
Hydrogen bonds hold water molecules in an open, ordered lattice in ice, so the molecules are spaced further apart than in liquid water.
Define electronegativity.
The ability of an atom to attract the bonding (shared) pair of electrons in a covalent bond towards itself.
How does electronegativity vary across a period and down a group?
It increases across a period (left to right) and decreases down a group.
Why is CO₂ a non-polar molecule even though it has polar bonds?
It is linear and symmetrical, so the two bond dipoles act in opposite directions and cancel out, giving no overall dipole.
State the ideal gas equation and define each term with its SI unit.
pV = nRT, where p = pressure (Pa), V = volume (m³), n = moles, R = gas constant (8.31 J K⁻¹ mol⁻¹), T = temperature (K).
Why does graphite conduct electricity but diamond does not?
In graphite each carbon forms 3 bonds, leaving one delocalised electron per atom free to move; in diamond all 4 outer electrons are used in covalent bonds, leaving none free.
Define standard enthalpy change of formation (ΔHf°) and standard enthalpy change of combustion (ΔHc°).
ΔHf°: enthalpy change when one mole of a compound is formed from its elements in their standard states under standard conditions. ΔHc°: enthalpy change when one mole of a substance is completely burned in oxygen under standard conditions.
What this deck covers
The Chemistry (9701) deck follows the Cambridge AS and A Level Chemistry (9701) syllabus — 11 chapters and 39 topics — so questions land on material that is genuinely examinable rather than trivia around it. That works out to roughly 4.5 cards per chapter.
Answers are written to be recallable, not just readable — averaging about 108 characters, which is long enough to carry the reasoning and short enough to say out loud.
A deck like this earns its keep on the second and third pass. Read the syllabus first so you know the shape of the subject, then use the cards to find the specific facts that have not stuck.
Chemistry (9701) flashcards FAQ
How many Chemistry (9701) flashcards are in this Cambridge AS and A Level deck?
50 cards. This page previews 24 of them, sampled evenly across the deck so you can judge the difficulty before installing anything.
Are these Cambridge AS and A Level flashcards free?
Yes. The preview here is free to read with no signup, and the full 50-card deck is free inside the Examius app.
What do the Chemistry (9701) cards cover?
They follow the Cambridge AS and A Level Chemistry (9701) syllabus — 11 chapters and 39 topics — so the questions track what is actually examinable.
How should I use these flashcards?
Read the syllabus first so you know the shape of the subject, then drill the deck. Examius schedules each card with spaced repetition, so cards you keep missing come back sooner and ones you know drift further apart.