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Chemistry > FINAL BUFFER > Flashcards

FINAL BUFFER Flashcards

1
Q

Alkali metals

A

Elements found in Group 1 of the periodic table

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2
Q

Why are they called alkali metals?

A

Because when reacted with water they form alkaline solutions

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3
Q

What are the typical poroperties of Group 1 elements?

A

Shiny when freshly cut, good conductors of electricity, solid at room temperature, soft

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4
Q

As you go down the Group 1 Elements…

A

their density increases and their melting point decreases and reactivity increases

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5
Q

Why are Group 1 elements stored in oil?

A

To make sure they are not exposed to oxygen which they react rapidly with

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6
Q

alkali metal + water =

A

metal hydroxide + hydrogen

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7
Q

How does lithium react with water?

A

fizzes steadily and slowly disappears

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8
Q

How does sodium react with water?

A

melts to form a silvery ball, fizzes vigourously and quickly disappears

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9
Q

How does potassium react with water?

A

immediately ignites, burns with a lilac flame and very quickly disappears

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10
Q

Explain the trend in reactivity in Group 1 Elements

A

All atoms in Group 1 have one electron in their outer shell. The easier it is for an atom of a Group 1 Element to lose its outer electron, the more reactive the element is due to forces of attraction between the negatively charged electron and positively charged nucleus.

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11
Q

What do Group 7 elements exist as?

A

diatomic molecules with weak intermolecular forces

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12
Q

What is fluorine at room temperature?

A

a pale yellow gas

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13
Q

What is chlorine at room temperature?

A

a green gas

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14
Q

What is bromine at room temperature?

A

orange-brown liquid that vapourises easily

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15
Q

What is iodine at room temperature?

A

a shiny grey-black crystalline solid that sublimes to form a purple vapour

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16
Q

As you go down Group 7…

A

density increases, melting and boiling points increase, reactivity decreases

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17
Q

Halogens

A

Group 7 elements which react with metals to produce salts

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18
Q

Explain the trend in reactivity for halogens

A

All halogens have seven electrons in the outer shell. The easier it is for a halogen atom to gain an outer electron, the more reactive the element is due to forces of attraction between the electrons and the nucleus.

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19
Q

Halide

A

a compound containing a Group 7 element and another element usually hydrogen or a metal

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20
Q

What happens in a halogen displacement reaction?

A

a halogen will displace a less reactive halogen from its halide ions in solution

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21
Q

Noble gases

A

Unreactive elements found in Group 0 of the periodic table

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22
Q

Why are noble gases so unreactive?

A

They havecomplete outer shells meaning they have no tendency to lose or gain electrons to form ions

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23
Q

What do noble gases exist as?

A

monoatomic molecules with very weak forces of attraction between them

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24
Q

Why do noble gases have such low boiling points?

A

Having weak forces of attraction between atoms means these forces are very easily overcome by heating

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25
Q

As you go down Group 0…

A

attractive forces between atoms get stronger and boiling point increases and density increases

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26
Q

Why do noble gases have very low densities?

A

Their atoms are very far apart in the gas state

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27
Q

Transition metals

A

Metals found between Group 2 and Group 3 on the periodic table

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28
Q

What are the properties of transition metals?

A

shiny when freshly cut, good conductors of electricity, strong, malleable

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29
Q

Compared to alkali metals, transition metals…

A

are stronger and harder, have higher densities, have have higher melting points (except for mercury)

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30
Q

How do you detect carbon dioxide?

A

Bubble carbon dioxide through limewater (calcium hydroxide solution) and it will turn cloudy white if there is CO2 [as the reaction between limewater and CO2 produces a white precipitate of calcium carbonate]

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31
Q

How do you detect chlorine?

A

Hold damp blue litmus paper near a container that holds chlorine and if it is present then the paper will turn red then white

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32
Q

How do you detect hydrogen?

A

Hold a lighted splint near the mouth of a container of gas and it should ignite with a squeaky poop at the presence of hydrogen

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33
Q

How do you detect oxygen?

A

Hold a glowing splint near a container of oxygen and if it is present the splint should relight

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34
Q

Flame test colour for lithium ion

A

red

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35
Q

Flame test colour for sodium ion

A

yellow

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36
Q

Flame test colour for potassium ion

A

lilac

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37
Q

Flame test colour for calcium ion

A

orange-red

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38
Q

Flame test colour for copper ion

A

green-blue

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39
Q

Hydroxide precipitate test colour for iron(II) ion

A

green

40
Q

Hydroxide precipitate test colour for iron(III) ion

A

orange-brown

41
Q

Hydroxide precipitate test colour for copper(II) ion

A

blue

42
Q

Hydroxide precipitate test colour for calcium ion

A

white

43
Q

Hydroxide precipitate test colour for zinc ion

A

white

44
Q

How do you detect sulfate ions in a solution?

A

add a few drops of dilute hydrochloric acid then a few drops of barium chloride solution. if sulfate ions are present, a white precipitate will form

45
Q

How do you detect carbonate ions?

A

add a few drops of dilute hydrochloric acid adn if a carbonate is present, bublles of CO2 gas will be produced

46
Q

How do you detect halide ions?

A

add a few drops of dilute nitric acid and then a few drops of silver nitrate solution

47
Q

Halide ion test precipitate colour for chloride ion

A

white

48
Q

Halide ion test precipitate colour for bromide ion

A

cream

49
Q

Halide ion test precipitate colour for iodide ion

A

yellow

50
Q

What are advantages of instrumental methods of analysis?

A
  • Instruments can analyse very small amounts of substances
  • Instruments are very accurate
  • Instruments can analyse quickly and can run all the time
51
Q

Theoretical yield equation

A

(mass of limiting reactant / sum of Mr for limiting reactant) * sum of Mr for products

52
Q

Percentage yield equation

A

(actual yield / theoretical yield) * 100

53
Q

What makes the percentage yield less?

A

Reactants may react in a different way than expected, reaction may not go to completion, some of the product may be lost when transfering substances between containers.

54
Q

Atom economy equation

A

(sum of Mr of desired product / sum of Mr of all products) * 100

55
Q

Concentration equation

A

Mass (g) or mol of solute / Volume of solution (dm3)

56
Q

How much volume does one mole of any substance in the gas state occupy at the same temperature and pressure?

A

24dm3 (/mol)

57
Q

Volume of a gas equation

A

volume (dm3) = mol * 24

58
Q

Rate of reaction equation

A

amount of reactant used OR amount of product formed / time taken

59
Q

Successful collision

A

a collision of particles that leads to a reaction

60
Q

A reaction can only happen if…

A

reactant particles collide with each other and the colliding particles have enough energy to react

61
Q

As the temperature of a reaction mixture increases…

A

particles move more quickly so they collide more often and a greater proportion of the collidiong particles have the activation energy

62
Q

Rate of reaction equation in terms of reaction time

A

1 / reaction time

63
Q

The rate of reaction increases as concentration or pressure increases because:

A

the particles become more crowded, so they collide more often

64
Q

The rate of reaction increases as surface area increases as…

A

more particles are available for collisions and collisions are more likely so particles collide more often

65
Q

Why do catalysts work?

A

they provide an alternate reaction pathway with a lower activation eneergy

66
Q

Dynamic equilibrium

A

forward and backward reaction rates become equal in a closed system

67
Q

What happens to the equilibrium position when pressure is increased?

A

shifts to the side with fewer moles of gas

68
Q

What happens to the equilibrium position when concentration of a substance is increased?

A

shifts to the side away from the substance where concentration has increased

69
Q

What happens to the equilibrium position when temperature is increased?

A

shifts to the side of the endothermic change

70
Q

symptoms of nitrogen deficiency in plants

A

poor growth, yellow leaves

71
Q

Symptoms of phosphorus deficiency in plants

A

poor root growth, discoloured leaves

72
Q

Symptoms of potassium deficiency in plants

A

poor fruit growth, discoloured leaves

73
Q

Haber process

A

manufactures ammonia from nitrogen and hydrogen

74
Q

Haber process equation

A

N2(g) + 3H2(g) ⇌ 2NH3(g)

75
Q

Raw materials for the Haber process

A

air, natural gas, steam

76
Q

How is nitrogen obtained to be used in the Haber process?

A

fractional distillation of liquefied air

77
Q

How is hydrogen obtained to be used in the Haber process?

A

reacting natural gas with steam

78
Q

Conditions of the Haber process

A

200 atmospheres of pressure, 450C and iron catalyst

79
Q

The forward reaction of the Haber process is

A

exothermic

80
Q

What process is used to make ethanol?

A

Fermentation

81
Q

Equation for making ethanol

A

glucose -> carbon dioxide + ethanol

82
Q

Ore

A

rock or mineral that contains enough metal to make it economical to extarct it

83
Q

Metal compound found in malachite ore

A

copper carbonate

84
Q

Metal compound found in bauxite ore

A

aluminium oxide

85
Q

Metal compound found in haematite

A

iron(III) oxide

86
Q

How is copper extracted from a compound?

A

Reduction with carbon as copper is lower than carbon in the reactivity series

87
Q

What happens in a blast furnace when extarcting iron?

A

Coke burns in hot air making carbon dioxide, more coke reduces carbon dioxide to carbon monoxide, carbon monoxide reduces iron(III) oxide to iron at 1500C

88
Q

How is aluminium oxide electrolysed to extact aluminium?

A

aluminium oxide is dissolved in molten cryolite and electrolysis takes place to lower the temperature needed to electrolyse

89
Q

What is the main metal in steel and what are its typical uses?

A

Iron; buildings, bridges, cars

90
Q

What are the main metals in duralumin and what are its typical uses?

A

aluminum and copper; aircraft parts

91
Q

What are the main metals in solder and what are its typical uses?

A

tin and copper; joining electrical components

92
Q

What are the main metals in brass and what are its typical uses?

A

copper and zinc; musical instruments

93
Q

What are the main metals in bronze and what are its typical uses?

A

copper and tin; bells

94
Q

Why are alloys typically stronger and harder than their individual metals?

A

Atoms within an alloy are different sizes, making it more difficult for atoms to slide over each other.

95
Q

Rust equation

A

iron + oxygen + water -> hydrated iron(III) oxide

96
Q

How can you reduce rusting?

A

painting, coating with oil, galvanising (plating with zinc), plating with tin

97
Q

Sacrificial protection

A

Coating an iron or steel object with a more reactive metal such as zinc so that the metal corrodes first before the iron

Chemistry (26 decks)

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