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Chemistry F4 EoY > Basics > Flashcards

Basics Flashcards

1
Q

solids

A
  • fixed shape/ volume
  • can’t be compressed
  • least KE
  • regular arrangement
  • vibrates in place
  • strong intermolecular forces
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2
Q

liquids

A
  • no fixed shape
  • takes shape of bottom of container
  • flows
  • can’t be compressed
  • no regular arrangement
  • moves randomly
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3
Q

gases

A
  • no fixed shape
  • takes shape of whole container
  • can be compressed
  • no fixed volume
  • weakest intermolecular forces
  • no regular arrangement
  • moves randomly quickly
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4
Q

solid to liquid

A

melting

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5
Q

liquid to gas

A

boiling/ evaporating

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6
Q

gas to liquid

A

condensation

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7
Q

liquid to solid

A

freezing

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8
Q

kinetic particle theory

A
  • more kinetic energy= weakest forces
  • higher temp. = more kinetic energy
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9
Q

pressure in gases decreases

A

volume increases

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10
Q

concentration

A

measure of a number of particles in a given volume

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11
Q

diffusion

A

net movement of particles from a region of high conc. to a region of low conc. down the conc. gradient

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12
Q

concentration gradient

A

difference in conc. of a fluid between 2 areas

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13
Q

greater molecular mass

A

particles move slower

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14
Q

effect of temperature on rate of diffusion

A
  • higher temp. = more kinetic energy = move faster = increases rate of diffusion
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15
Q

element

A

substances made up of only one type of atom

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16
Q

compound

A

elements chemically bonded together (not easily separated)

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17
Q

mixture

A

substances found together, not chemically bonded (easily separated)

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18
Q

electrical conductivity in metals

A
  • good electrical conductors
    (they have delocalised electrons and are free to carry the charge)
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19
Q

thermal conductivity in metals

A
  • good thermal conductors
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20
Q

malleability in metals

A
  • very malleable
    (easy to shape and bend)
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21
Q

ductility in metals

A
  • very ductile
    (easily stretched into wires)
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22
Q

melting/ boiling point of metals

A
  • high melting/ boiling points
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23
Q

solvent

A

liquid in which a solute dissolves in

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24
Q

solute

A

substance that is dissolved in a solvent

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25
Q

solution

A

mixture of (1 or more) solutes dissolved in a solvent

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26
Q

saturated solution

A

solution with maximum conc. of a solute dissolved

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27
Q

filtrate

A

liquid/ solution that passed through a filter

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28
Q

residue

A

substance that remains after evap./ distillation/ filtration

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29
Q

Rf formula

A

distance travelled by solvent

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30
Q

mass number

A

larger number

31
Q

proton number

A

smaller number

32
Q

number of outershell electrons

A

group number

33
Q

number of shells

A

period number

34
Q

isotopes

A

atoms with the same proton number but different neutron number

35
Q

group 7 (halogens)

A
  • diatomic
  • non-metals
  • density increases going down
  • melting point increases going down
  • reactivity decreases going down
    -iodine= grey-black solid
  • bromine= red-brown liquid
  • chlorine= yellow-green gas
36
Q

transition elements

A
  • high density
  • high melting point
  • unreactive
  • catalysts
  • forms coloured compounds
  • ions with variable oxidation numbers
37
Q

group 8 (noble gases)

A
  • colourless gases
  • monoatomic
  • very unreactive (inert)
38
Q

collision theory

A
  • particles must collide with correct orientation and sufficient energy (activation energy)
39
Q

activation energy

A

minimum energy needed to create a reaction

40
Q

effect of catalysts in activation energy

A

lowers it

41
Q

cations

A

positive ions

42
Q

anions

A

negative ions

43
Q

ionic bond

A

strong electrostatic attraction between oppositely charged ions

44
Q

properties of ionic compounds

A
  • high melting/ boiling point
  • good conductor when aqueous/ molten
  • poor conductor when solid
  • giant ionic lattice
  • regular arrangement of alternating positive and negative ions
45
Q

properties of covalent bonds

A
  • low melting/ boiling point
    -poor electrical conductor
46
Q

covalent bonds

A

pair of electrons is shared between 2 atoms leading to a noble gas electronic configuration

47
Q

diamond

A
  • giant covalent
  • carbon atoms only
  • each carbon bonded to 4 others
  • no delocalised electrons
  • can’t conduct
  • very hard, used for cutting tools
  • high melting point
  • doesn’t dissolve in water
48
Q

graphite

A
  • only carbon
  • each carbon boded to 3 other
  • organised in hexagons, making layers
  • conducts electricity
  • layers can slide over eachother (soft and slippery) (weak forces between layers)
  • used as lubricant and electrode
49
Q

silicon (IV) dioxide (SiO2)

A
  • silicon bonded with 4 oxygens, oxygen bonded with 2 silicons
  • high melting point
  • doesn’t conduct
  • doesn’t dissolve
  • hard
50
Q

metals and dilute acid

A

make salt and hydrogen

51
Q

metals and water

A

make metal hydroxide and hydrogen

52
Q

metals and oxygen

A

makes metal oxides

53
Q

aluminium properties

A
  • very low density
  • strong
  • good conductor
  • corrosion resistant

used to make:
- aircrafts (low den.)
- overhead electrical cables (low den.)(good cond.)
- food containers (corrosion resistant)

54
Q

copper use

A
  • electrical wiring (ductile/ elec. cond.)
55
Q

reactivity series order

A

potassium
sodium
calcium
magnesium
aluminium
carbon
zinc
iron
hydrogen
copper
silver
gold

56
Q

potassium and water

A
  • violent
  • potassium floats , melts, catches fire
  • burns with lilac flame
  • hydrogen gas released
57
Q

sodium and water

A
  • floats, moves rapidly
  • heat melts it
  • hydrogen gas released
58
Q

calcium and water

A
  • water becomes milky white
  • hydrogen gas released
59
Q

aluminium’s unreactivity

A
  • surface atoms react with oxygen in the air to form a protective aluminium oxide layer
  • barrier to prevent inner metal from corroding
60
Q

displacement reactions

A
  • more reactive metal elements displace less reactive metal ions
  • less reactive= reduced= gains electrons
  • more reactive= oxidised= loses electrons
61
Q

metallic bonding

A

electrostatic attraction between the positive metal ions in a giant metallic lattice and a sea of delocalised electrons

62
Q

alloys

A

mixture of a metal with other elements

63
Q

brass

A

mixture of copper and zinc

64
Q

stainless steel

A

mixture of iron and chromium, nickel and carbon

used for cutlery (hard + resistant to rusting)

65
Q

redox reactions

A

involving oxidation and reduction reactions and loss and gain of electrons and loss and gain of oxygen

66
Q

oxidation

A
  • gain of oxygen
  • loss of electrons
  • increase in oxidation number
67
Q

reduction

A
  • loss of oxygen
  • gain of electrons
  • decrease in oxidation number
68
Q

oxidising agent

A

oxidises another substance and reduces itself

69
Q

reducing agent

A

reduces another substance and oxidises itself

70
Q

rusting

A

oxidation of iron
- conditions: air and moisture

iron + water + oxygen –> hydrated iron (iii) oxide

71
Q

barrier methods

A

painting, coating with plastic, greasing, galvanising, sacrificial protection, greasing

72
Q

sacrificial protection

A
  • placing iron/ steel in contact with a more reactive metal (ie zinc)
73
Q

galvanising

A
  • coating iron/ steel with zinc
  • barrier formed and if it is scratched, it is more reactive, so it corrodes instead of iron

Chemistry F4 EoY (5 decks)

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