Recall — GCSE Flashcards
⚗️ GCSE Chemistry Flashcards
Atomic structure, bonding and reactions — 10 free revision cards. Study them below, or add the whole deck to Recall and let FSRS spaced repetition schedule your revision so it actually sticks.
What are the three subatomic particles and their charges?
| Particle | Charge | Relative mass |
|---|---|---|
| Proton | +1 | 1 |
| Neutron | 0 | 1 |
| Electron | -1 | ~0 (1/1836) |
|---|---|---|
| Proton | +1 | 1 |
| Neutron | 0 | 1 |
| Electron | -1 | ~0 (1/1836) |
What is an isotope?
Atoms of the same element (same number of protons) but different numbers of neutrons.
Example: Carbon-12 and Carbon-14. Same chemistry, different mass.
Example: Carbon-12 and Carbon-14. Same chemistry, different mass.
Describe ionic bonding.
A metal transfers electrons to a non-metal.
- Metal becomes a positive ion (cation)
- Non-metal becomes a negative ion (anion)
Electrostatic attraction holds them in a giant ionic lattice (e.g. NaCl).
- Metal becomes a positive ion (cation)
- Non-metal becomes a negative ion (anion)
Electrostatic attraction holds them in a giant ionic lattice (e.g. NaCl).
Describe covalent bonding.
Non-metals share pairs of electrons.
- Simple molecular (H₂O, CO₂) — weak intermolecular forces, low MP/BP
- Giant covalent (diamond, graphite, SiO₂) — strong throughout, very high MP
- Simple molecular (H₂O, CO₂) — weak intermolecular forces, low MP/BP
- Giant covalent (diamond, graphite, SiO₂) — strong throughout, very high MP
What are the first 4 alkanes?
Methane (CH₄), Ethane (C₂H₆), Propane (C₃H₈), Butane (C₄H₁₀).
General formula: $C_nH_{2n+2}$. Saturated (only single bonds).
General formula: $C_nH_{2n+2}$. Saturated (only single bonds).
How do you test for the four common gases?
Hydrogen: lit splint → squeaky pop
Oxygen: glowing splint → relights
CO₂: bubble through limewater → goes cloudy
Chlorine: damp blue litmus → bleached white
Oxygen: glowing splint → relights
CO₂: bubble through limewater → goes cloudy
Chlorine: damp blue litmus → bleached white
State Le Chatelier's principle.
If a dynamic equilibrium is disturbed by changing temperature, pressure or concentration, the position of equilibrium shifts to oppose the change.
Example: Increase pressure → shift to side with fewer gas moles.
Example: Increase pressure → shift to side with fewer gas moles.
What are the three types of electrolysis products to remember?
Molten ionic compound: metal at cathode, non-metal at anode.
Aqueous solution:
- Cathode: H₂ (unless metal is below H in reactivity → metal)
- Anode: O₂ (unless halide present → halogen)
Aqueous solution:
- Cathode: H₂ (unless metal is below H in reactivity → metal)
- Anode: O₂ (unless halide present → halogen)
Define exothermic and endothermic reactions.
Exothermic: releases energy → surroundings get hotter ($\Delta H < 0$). Examples: combustion, neutralisation.
Endothermic: absorbs energy → surroundings get cooler ($\Delta H > 0$). Examples: thermal decomposition, photosynthesis.
Endothermic: absorbs energy → surroundings get cooler ($\Delta H > 0$). Examples: thermal decomposition, photosynthesis.
What is the rate equation (qualitatively) and what affects rate?
Rate of reaction = $\dfrac{\Delta \text{amount of reactant/product}}{\text{time}}$
Increased by: higher temperature, higher concentration/pressure, larger surface area, catalyst.
Increased by: higher temperature, higher concentration/pressure, larger surface area, catalyst.
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