482848
Description
Flashcards by katiehumphrey, updated more than 1 year ago
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Created by katiehumphrey
over 10 years ago
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| Question | Answer |
| atomic number and mass number of elements |
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atoms.gif (image/gif)
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| 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 |
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ionic_bond (image/jpg)
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| 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 |
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ions (image/jpg)
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| covalent bonding sharing electrons fill outer shell |
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covalent (image/jpg)
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| 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 |
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diamond (image/jpg)
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| graphite 3 covalent bonds slide over each other weak intermolecular forces |
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graphite (image/jpg)
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| metallic structures sea of free electrons conduct heat/electricity electrostatic attraction: positive metal ions and negative electrons |
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metal (image/jpg)
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| polymers thermosoftening: weak intermolecular forces - no crosslinks - free slide over thermosetting: strong intermolecular forces - crosslinks - solid structure |
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polymers (image/jpg)
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| relative formula mass atomic mass |
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co2 (image/jpg)
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| 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 |
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Catalyst_effect (image/png)
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| 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 |
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reversible (image/jpg)
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| acids and alkalis neutralise acids: H+ ions alkali: OH- ions |
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ph (image/jpg)
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| 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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