Chemistry86 views·Updated 20 Jun 2026·4 pages

Chemistry Paper 1: Important Key Concepts

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--- OCR Start ---
CHEMISTRY-KEY
CONCEPTS
Paper 1
Topic 1
>atomic Structure
•Protons +1
neutrons = 0
• Electrons:-1
Isotopes = same element
d

Atomic Structure and Chemical Bonding

Every element is made up of atoms containing protons $+1 charge$ , neutrons (no charge), and electrons $-1 charge$ . Isotopes are atoms of the same element with different numbers of neutrons - they're like identical twins with slightly different weights.

The periodic table is your roadmap to understanding elements. Groups (vertical columns) contain elements with similar properties, whilst periods (horizontal rows) show how properties change across elements. Group 1 metals (alkali metals) are soft, reactive metals that get more explosive as you go down the group - they react with water to produce hydrogen gas and alkalis.

Chemical bonding happens in three main ways. Ionic bonding occurs between metals and non-metals where electrons transfer completely, creating charged ions that attract each other strongly. Covalent bonding happens between non-metals that share electrons to form molecules like water. Metallic bonding involves a "sea" of free electrons that can move around, which is why metals conduct electricity and heat so well.

Quick tip: Remember that Group 7 (halogens) are coloured, toxic non-metals that get less reactive going down, whilst Group 0 (noble gases) are completely unreactive because they have full outer electron shells.

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Chemical Formulae and Reactions

Chemical formulae tell you exactly what's in a compound - H₂O means two hydrogen atoms and one oxygen atom. State symbols show whether something is solid (s), liquid (l), gas (g), or dissolved in water (aq). These details matter because they affect how substances behave in reactions.

Conservation of mass is a fundamental rule - atoms can't just disappear during reactions, so the mass before equals the mass after. You'll use relative atomic mass (Ar) and relative formula mass (Mr) to calculate this. Moles are just a way of counting atoms - one mole contains 6.02 × 10²³ particles, and you calculate moles using: moles = mass ÷ Mr.

Acids produce H⁺ ions and turn litmus red, whilst bases neutralise acids and alkalis (soluble bases) produce OH⁻ ions, turning litmus blue. The key reaction is: acid + base → salt + water. Limiting reactants determine how much product you can make - like running out of bread when making sandwiches.

Exam focus: Master separation techniques - filtration for insoluble solids, crystallisation for soluble solids, distillation for liquids, and chromatography for coloured mixtures.

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Reactivity and Metal Extraction

The reactivity series ranks metals by how easily they form positive ions - think of it as a league table of chemical aggression. More reactive metals displace less reactive ones from compounds, like magnesium kicking copper out of copper sulfate. This is called a displacement reaction.

Metal extraction depends on reactivity. Less reactive metals like iron can be extracted using carbon reduction - carbon steals oxygen from metal oxides. More reactive metals need electrolysis, where electricity breaks down compounds into elements. During electrolysis, the anode (positive electrode) attracts negative ions, whilst the cathode (negative electrode) attracts positive ions.

Strong acids like HCl completely split into ions in water, whilst weak acids only partially ionise in a reversible reaction. This affects their pH and reaction rates. Oxidation means losing electrons or gaining oxygen, whilst reduction is the opposite - gaining electrons or losing oxygen.

Memory trick: For electrolysis, remember "PANIC" - Positive Anode, Negative Is Cathode. Reduction happens at the cathode, oxidation at the anode.

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Electrolysis and Energy Changes

Electrolysis splits ionic compounds when they're molten or dissolved. In lead bromide electrolysis, lead ions (Pb²⁺) gain electrons at the cathode to form lead metal, whilst bromide ions (Br⁻) lose electrons at the anode to form bromine gas. With aqueous solutions, water complicates things - hydrogen gas forms at the cathode if the metal is more reactive than hydrogen.

Energy changes in reactions follow simple rules. Exothermic reactions release energy to surroundings (like combustion and neutralisation), making things feel warmer. Endothermic reactions absorb energy, making surroundings cooler - photosynthesis is a classic example.

Bond energy calculations help predict energy changes. Breaking bonds requires energy input, whilst forming bonds releases energy. If more energy is needed to break bonds than is released forming new ones, the reaction is endothermic. If more energy is released than needed, it's exothermic.

Calculation shortcut: Energy change = Energy needed to break bonds - Energy released forming bonds. Negative values mean exothermic, positive values mean endothermic.

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Chemistry86 views·Updated 20 Jun 2026·4 pages

Chemistry Paper 1: Important Key Concepts

holly@holly123

Add to Google sources

Chemistry can seem overwhelming, but it's really about understanding how atoms behave and interact with each other. This guide covers the essential concepts you'll need for Paper 1, from atomic structure and bonding to chemical reactions and energy changes.

of 4

Atomic Structure and Chemical Bonding

Quick tip: Remember that Group 7 (halogens) are coloured, toxic non-metals that get less reactive going down, whilst Group 0 (noble gases) are completely unreactive because they have full outer electron shells.

of 4

Chemical Formulae and Reactions

Exam focus: Master separation techniques - filtration for insoluble solids, crystallisation for soluble solids, distillation for liquids, and chromatography for coloured mixtures.

of 4

Reactivity and Metal Extraction

Memory trick: For electrolysis, remember "PANIC" - Positive Anode, Negative Is Cathode. Reduction happens at the cathode, oxidation at the anode.

of 4

Electrolysis and Energy Changes

Calculation shortcut: Energy change = Energy needed to break bonds - Energy released forming bonds. Negative values mean exothermic, positive values mean endothermic.