Additional Chemistry flashcards

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GCSE Chemistry Flashcards on Additional Chemistry flashcards, created by katiehumphrey on 14/01/2014.
katiehumphrey
Flashcards by katiehumphrey, updated more than 1 year ago
katiehumphrey
Created by katiehumphrey over 10 years ago
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Resource summary

Question Answer
atomic number and mass number of elements
compounds: atoms of 2+ elements chemically bonded isotopes: different atomic forms of the same element - same number of protons different number of neutrons
ionic bonding transferring electrons to form charged particles (ions) atoms need full outer shell
ions: atoms lost or gained electron(s) electronic structure of noble gas group 1 and 2: metals lose electrons form positive ions group 6 and 7: nonmetals gain electrons form negative ions
positive ions group 1: +1 group 2: +2 negative ions group 6: -2 group 7: -1
sodium chloride ions
covalent bonding sharing electrons fill outer shell
simple molecular substances very strong covalent bonds to form small molecules of several atoms forces between molecules: weak low melting/boiling points intermolecular forces easily broken don't conduct electricity
giant covalent structures lattices: no charged ions strong covalent bonds high melting/boiling points don't conduct electricity carbon atoms: diamond, graphite
diamond 4 covalent bonds very rigid and hard
graphite 3 covalent bonds slide over each other weak intermolecular forces
metallic structures sea of free electrons conduct heat/electricity electrostatic attraction: positive metal ions and negative electrons
polymers thermosoftening: weak intermolecular forces - no crosslinks - free slide over thermosetting: strong intermolecular forces - crosslinks - solid structure
relative formula mass atomic mass
reacting mass calculations moles = mass divided by relative formula mass CaCO3 + 2HCl > CaCl2 + H2O + CO2 20g ? 20g divided by (Ca = 40, C = 12, O = (16 x 3) = 48) 100g moles = 0.2 moles of CaCO3 no numbers infront so 0.2 moles of CaCO3 gives 0.2 moles of CO2 (1:1) 0.2 x (C = 12, O = (16 x 2) = 32) 44g mass = 0.2 x 44 = 8.8g
balancing equations unbalanced: CaO + HCl > CaCl2 + H2O balanced: CaO + 2HCl > CaCl2 + H2O
catalysts: chemical that speeds up a reaction without being used up
rate of reaction temperature concentration catalyst surface area of solids
combining powers and charges of compounds name formula charge combining hydroxide OH -1 1 nitrate NO3 -1 1 hydrocarbonate HCO3 -1 1 ammonium NH4 +1 1 sulphate SO4 -2 2 carbonate CO3 -2 2 thiosulphate S2O3 -2 2 phosphate PO4 -3 3
measuring rates of reaction precipitation speed change in mass volume of gas given off
collision theory how often the reacting particles collide successfully higher temperature: more energy - particles move quicker higher concentration: more particles to collide larger surface area: particles have more area to collide
exothermic reaction: transfers energy to surroundings - heat e.g combustion, oxidation endothermic reaction: takes in energy from surroundings - heat e.g heat/cool packs
reversible reactions
acids and alkalis neutralise acids: H+ ions alkali: OH- ions
acid + base > salt + water H+ + OH- > H2O
symbols for physical state (s) - solid (l) - liquid (g) - gas (aq) - dissolved in water
acids reacting with metals acid + metal > salt + hydrogen hydrochloric acid > chloride salts sulfuric acid > sulfate salts nitric acid > nitrate salts
oxides, hydroxides and ammonia acid + metal oxide > salt + water acid + metal hydroxide > salt + water ammonia + nitric acid > ammonium nitrate
making salts insoluble base > soluble salts alkali > soluble salts precipitation > insoluble salts
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