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Chemistry > Topic 4 - Inorganic Chemistry > Flashcards

Topic 4 - Inorganic Chemistry Flashcards

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1
Q

Group 1 - Alkali Metals

Properties of group 1 metals (alkali metals)

A

soft

reactive

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2
Q

Group 1 - Alkali Metals

order of reactivity in group 1 (alkali metals)

A

as you go down the group, metals become more reactive.

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3
Q

Group 1 - Alkali Metals

melting and boiling points in group 1 (alkali metals)

A

as you go down the group, melting and boiling points decrease.

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4
Q

Group 1 - Alkali Metals

why does reactivity increase as you go down group 1 (alkali metals)

A

the forces of attraction between the nucleus and the outer electron decrease, so it is lost more easily as the number of shells increases.

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5
Q

Group 1 - Alkali Metals

alkali metal + water —>

A

metal hydroxide + hydrogen

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6
Q

Group 1 - Alkali Metals

group 1 (alkali metals) reacting with oxygen

A

Lithium + Oxygen -> Lithium Oxide (Li2O)

Sodium + Oxygen -> Sodium Oxide (Na2O)

Sodium + Oxygen -> Sodium Peroxide (Na2O2)

Potassium + Oxygen -> Potassium Peroxide (K2O2)

Potassium + Oxygen -> Potassium Superoxide (KO2)

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7
Q

Group 7 - Halogens

Colour of Halide salts

E.g. KCl, KBr, Kl

A

colourless

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8
Q

Group 7 - Halogens

colour of Bromine water

A

orange

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9
Q

Group 7 - Halogens

Colour of chlorine water

A

colourless

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10
Q

Group 7 - Halogens

colour of iodine water

A

brown

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11
Q

Group 7 - Halogens

State of fluorine at room temp

A

poisonous yellow gas

most reactive halogen

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12
Q

Group 7 - Halogens

State of chlorine at room temp

A

Green gas

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13
Q

Group 7 - Halogens

State of bromine at room temp

A

poisonous red-brown liquid

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14
Q

state of iodine at room temp

A

grey solid

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15
Q

Group 0 - Noble Gases

why are noble gases inert?

A

they have a full outside shell of electrons

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16
Q

diatomic molecules

A

each molecule consists of two atoms, joined together by a covalent bond

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17
Q

Group 7 - Halogens

melting and boiling points in group 7 (halogens)

A

as you go down group 7, melting and boiling points increase.

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18
Q

Group 7 - Halogens

properties of group 7

A

-1 charge
-form covalent bonds with other nonmetals

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19
Q

percentage of nitrogen in the atmosphere

A

78%

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20
Q

percentage of oxygen in the atmosphere

A

21%

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21
Q

percentage of argon in the atmosphere

A

1%

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22
Q

percentage of carbon dioxide in the atmosphere

A

0.04%

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23
Q

thermal decomposition

A

the process of breaking something down using heat

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24
Q

thermal decomposition of metal carbonate

metal carbonate ->

A

metal oxide + carbon dioxide

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25
Q

practical: heating copper (II) carbonate

A
  • copper (II) carbonate is a green powder
  • it will decompose into copper (II) oxide, a black powder and carbon dioxide, a colourless gas
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26
Q

atmosphere

A

layer of gases surrounding the earth held in place by gravity

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27
Q

greenhouse gases

A

carbon dioxide

methane

water vapour

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28
Q

global warming

A

overall increase in earth’s temperature

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29
Q

climate change

A

CONSEQUENCE OF GLOBAL WARMING

effects on climate, such as shifts in weather patterns

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30
Q

weather

A

short term atmospheric conditioms

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31
Q

climate

A

typical weather conditions in an entire location for a very long time

e.g. singapore is humid

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32
Q

greenhouse effect

A
  • solar radiation from the sun passes through the atmosphere and hits the earth
  • energy reflects back out to space, some is absorbed by earth
  • most energy is absorbed by greenhouse gases
  • trapped energy keeps the atmosphere warmer
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33
Q

metals always form

A

cations

34
Q

metal + acid —>

A

salt + hydrogen

35
Q

corrosion

A

process by which metals are slowly broken down by reacting with surrounding substances

36
Q

rusting

A

special type of corrosion

refers specifically to the corrosion of IRON

redox reaction

37
Q

iron rusting half equation

A

Fe -> Fe3+ + 3e-

38
Q

redox reaction

A

reaction involving both oxidation and reduction

39
Q

conditions required for rusting to occur

A

water and oxygen

40
Q

Methods of preventing rusting

Barrier Method

A

coating the iron in something (like paint) to prevent water and oxygen from touching the iron

41
Q

Methods of preventing rusting

Sacrificial prevention

A

add a more reactive metal to the iron, that metal reacts with oxygen instead

42
Q

Methods of preventing rusting

Galvanisation

A

coating the iron with a layer of zinc. prevents rust as zinc is more reactive than iron

43
Q

why is pure gold found in the ground, but not pure iron?

A
  • gold is unreactive, so doesnt react with other elements
  • iron is reacted enough to combine with other elements, so can be found in its ore
44
Q

separating metals from metal oxides

A
  • using carbon
  • carbon causes metal to lose its oxygen
  • metal becomes reduced
  • ONLY WORKS FOR METALS LESS REACTIVE THAN CARBON
45
Q

neutral pH

A

7

46
Q

acidic pH

A

1-6

47
Q

alkaline pH

A

8-14

48
Q

universal indicator in acidic solutions

A

turns red

49
Q

universal indicator in alkaline solutions

A

purple

50
Q

pH of pure water

A

7 (neutral)

51
Q

acid + metal oxide —>

A

salt + water

52
Q

acid + metal hydroxide —>

A

salt + water

53
Q

acid + metal carbonate —>

A

salt + water + carbon dioxide

54
Q

neutralisation

A

a reaction between an acid and a base

55
Q

to find formula of salt in an equation

A

positive ion from base + negative ion from acid

56
Q

obtaining salt crystals from acid-base reaction

A
  1. dilute acid in a beaker and heat gently
  2. add solid base bit by bit until no further reaction, meaning it’s in excess
  3. isolate salt solution by filtering out excess solid base using filter paper and funnel
  4. heat solution in water bath until crystals form
  5. let solution cool further, causing more crystals to form
  6. filter out salt crystals using filter paper and funnel
57
Q

titration

A

experimental technique used to find unknown concentration of an acid or alkali

58
Q

titration equipment

A
  1. pipette to measure volume of acid or alkali
  2. conical flask to contain liquid from pipette
  3. burette to add alkali or acid to conical flask
  4. white tile to place conical flask on
59
Q

titration method

A
  1. use pipette to add 25cm^3 of alkali to conical flask
  2. add 3 drops indicator to conical flask on a white tile
  3. fill burette with acid and not starting volume
  4. slowly add acid from burette to alkali in conical flask, stirring to evenly distribute
  5. stop adding when indicator has changed colour
  6. note final volume reading, calculate how much acid added
  7. repeat titration until volumes are within 0.10cm^3 of each other
  8. use results to calculate mean volume of acid required to neutralise alkali
60
Q

salt

A

compound that contains a positive cation and a negative anion

some are insoluble in water, some are soluble in water

61
Q

soluble and insoluble salts

common salts of sodium, potassium, ammonium

A

soluble

62
Q

soluble and insoluble salts

nitrates

A

soluble

63
Q

soluble and insoluble salts

common chlorides

A

soluble

except silver chloride and lead chloride

64
Q

soluble and insoluble salts

common sulfates

A

soluble

except lead sulfate, barium sulfate, calcium sulfate

65
Q

soluble and insoluble salts

common carbonates and hydroxides

A

insoluble

except sodium, potassium, ammonium

66
Q

test for chlorine gas

A

bleaches damp blue litmus paper

67
Q

test for oxygen gas

A

relights a glowing splint

68
Q

test for hydrogen gas

A

lit splint produces a squeaky pop sound

69
Q

test for carbon dioxide gas

A

turns limewater cloudy when bubbled through

70
Q

anion

A

negatively charged ion

71
Q

test for carbonate ion

A
  • react w hydrochloric acid
  • if it contains carbonate ion, carbon dioxide gas will bubble out of solution
  • collect gas and bubble through limewater
  • if limewater turns cloudy, carbonate ions are present
72
Q

test for sulfate ion

A
  • react w hydrochloric acid to remove carbonate ions
  • add barium chloride solution
  • white precipitate will form if sulfate ions are present
73
Q

test for halide ion

A
  • react w nitric acid to remove carbonate + sulfate ions
  • add silver nitrate solution
  • chloride ions -> white precipitate
  • bromide ions -> cream precipitate
  • iodide ions -> yellow precipitate
74
Q

cation

A

positively charged ion

75
Q

testing for cations

method for flame test

A
  1. take nichrome wire loop and clean it by dipping in dilute hydrochloric acid and heating over bunsen burner
  2. dip wire in compound
  3. hold wire over hottest part of bunsen burner
  4. observe flame colour
76
Q

testing for cations

lithium flame colour

A

red

77
Q

testing for cations

sodium flame colour

A

yellow

78
Q

testing for cations

potassium flame colour

A

lilac

79
Q

testing for cations

calcium flame colour

A

orange-red

80
Q

testing for cations

copper flame colour

A

green blue

ICE PRINCESS

Chemistry (6 decks)

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