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Chemistry - Y10 + Y11 > Atomic Structure and periodic table > Flashcards

Atomic Structure and periodic table Flashcards

1
Q

How can you separate a soluble solid from a liquid?

A
  • Evaporation
  • Crystallisation
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2
Q

What is filteration?

A

Separating insoluble solids from liquid

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3
Q

Problems with evaporation

A
  • Can cause solids to decompose when heated
  • Called thermal decomposition
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4
Q

What does filter paper have?

A

small holes that are large enough to allow liquid particles to move through, but too small to allow solids through. This separates the solids from the liquids in filtration.

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5
Q

What is simple distillation?

A

Separates liquid from solution

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6
Q

Equipment for simple distillation

A
  • Flask w/ solution
  • Bund on flask
  • Thermometer through bung
  • Condensor with water jacket (cold)
  • Beaker to capture
  • Bunsen burner under flask
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7
Q

What is fractional distillation?

A

Separating mixtures of liquids

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8
Q

What does a fractionating column have?

A
  • Full of glass rods - prodive large SA
  • Tall - cooler at top than bottom
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9
Q

Compared to group 1, how are the transition elementd?

A
  • Harder
  • Stronger
  • High melting points (not mercury)
  • Higher densities
  • Les reactive and dont react as vigourosly with o2 or water
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10
Q

Propertie of chromium

A
  • Lustrous
  • Brittle
  • hard metal
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11
Q

Properties of manganese

A
  • Hard
  • Very brittle
  • Difficult to fuse
  • Easy to oxidise
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12
Q

Properties of iron

A
  • Good conductor
  • Rusts easily in air
  • Strong
  • Ductile
  • Malleable
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13
Q

Typical properties of transition metals

A
  • Useful as catalysts
  • Form coloured compounds
  • Have ions with many diff charges
  • Hard and strong metals
  • High density
  • High melting points
  • Less reactive than group 1
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13
Q

Properties of copper

A
  • Highly ductile
  • Conductive
  • Malleable and soft
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13
Q

Properties of nickel

A
  • Hard malleable
  • Ductil
  • Good conductor of heat and elect.
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13
Q

Uses of Gold and why

A
  • Jewellery - doesnt react with air or water at room temp, malleable
  • Electrical connectors
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14
Q

Properties of cobalt

A
  • Brittle
  • Hard high melting point
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15
Q

Uses of silver and why

A
  • Jewellery - doesnt react with air or water at room temp
  • Printed circuit boards and electrical contacts
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16
Q

Uses of copper and why

A
  • Electrical wires
  • Printed circuit boards
  • Water pipes - doesnt react with water at room temp, can be hammered into a shape
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17
Q

Uses of iron and why

A
  • Building material like bridges, buildings, ships,cars - strong, sheets easil shaped, cheaper than other metals
  • Catalyst in the chemicl industry eg Haber process - increases rate of certain reactions, unchanged
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18
Q

Uses of chromium and why

A
  • To coat other metals like iron on cars and bicycles - stays shiny when polished, resistant to corrosion
  • Catalyst in the chemical industry - increases rate of reaction
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19
Q

Features of group 1 alkali metals

A
  • Soft metals
  • low melting points
  • low density
  • reactive rapidly with o2, chlorine and water
  • form 1+ charge
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20
Q

What colour is iron (111) oxide?

A

Red

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21
Q

What colour is manganese (11) chloride?

A

Pink

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22
Q

What colour is chromium (111) chloride?

A

purple

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23
Q

What colour is copper (11) sulfate?

A

Blue

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24
Q

What happens when potassium reacts with water

A
  • Flame
    Gas produced
    alkaline solution forming
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25
Q

metal + water

A

metal hydroxide + hydrogen

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26
Q

Why does reactivity increase as you go down group 1?

A
  • Radius of atoms increase - greater distance between positive nucleus and negative electons - outer electron is less attracted to nucleus - easier to lose
  • Outer electron is repelled by electrons in the internal energy levels - electron shielding - decreases attraction between nucleus and electron, as you go down, elements have more electrons in internal energy levels, increases shielding as you go down
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27
Q

Proporties of group 7

A
  • Non- metals
  • Diatomic - covalent bond
  • Melting/boiling point increase as you go down
  • Relative molecular mass increases (size) as you go down
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28
Q

2 elements that are gases in group 7

A

Fluorine and Chlorine

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29
Q

What is a liquid in group 7? Solid?

A

L = bromine
S = iodine

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30
Q

What is formed when group 7 elements when they react with other non metal elements

A

Covelent compounds that all have simple molecular structures

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31
Q

What is formed when halogens react with metals?

A

Ionic compounds

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32
Q

Describe fluroine

A

posonous yellow gas

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33
Q

Describe chlorine

A

poisonous dense green gas

34
Q

Describe bromine

A

poisonous, dense, red-brown volatile liquid

35
Q

Describe iodine

A

dark grey crystalline solid or purple vapour

36
Q

What happens in group 7 as you go down?

A
  • Become less recative
  • High melting and boiling points
  • high relativr atomic masses
37
Q

What happens as you go down group 1

A
  • Increased recativity
  • Lower melting and boiling point
  • High relative atomic masses
38
Q

What do alkali metals only react to form?

A

Ionic compounds - generally white soids that dissolve in water to form colourless solutions

39
Q

Group 1 and water

A
  • React vigourously
  • Produce H2 and metal hydroxides - compounds that dissolv ein water to produce alkaline solutions
  • Amount of energy given out by reaction increases as you go down
40
Q

Group 1 and chlorine

A
  • Vigoursly
  • Form white metal chloride salts
  • as you go down, becomes more vigourous
41
Q

Group 1 and oxygen

A
  • Form metal oxide
  • Lithium = lithium oxide
  • sodium = mixture of sodium oxide and sodium perioxide
  • potassium = mixture of potassium perioxide and potassium superoxide
42
Q

Properties of group 0 noble gases

A
  • 8 electrons in outer energy level + 2 (He)
  • inert, stable
  • exist as monoatomic gase - single atoms
  • colourless gases
  • non flammable as inert
43
Q

What happens as you go down groupp 0?

A
  • Boiling points increase
  • Increasing relative atomic mass
44
Q

Why does boiling point increase as you go down group 0?

A
  • Due to increase in number of electrons
  • each atoms having a greater intermolecular forces between them
  • Lots of energy needde to break them
45
Q

Where are metals and non metals placed?

A

Metals = left side + centre
non metal - right

46
Q

Proporties of non metals

A
  • dull looking
  • more brittle
  • not always solids at room temp
  • dont conduct electricity
  • low density
47
Q

What did John Dalton say?

A
  • Atoms are solid spheres
  • diff spheres made of diff elements
48
Q

What did Thomson say?

A
  • atoms werent solid spheres
  • found electrons
  • plum pudding model
49
Q

What is the plum pudding model

A
  • atom is ball of + charge
  • negative electrons embedded
50
Q

What did Dobereiner do?

A
  • Noticed elements with similar chemical propoerties often occured in 3s
  • eg lithium, na, k - metals that react rapidly in water
  • called these triads
  • scientists wondered if elemtents could be arraged into some logical order
51
Q

What did John Newlands do?

newlands octaves

A
  • arranged elements in order of increaasing atomic weight
  • every 8th element reacts in a similar way
52
Q

Why wasnt newlands law of octaves taken seriously?

A
  • Problem = by always sticking to the exact order of atomic weight, sometimes elements were grouped together when they have diff properties
53
Q

How did Mendeleev arrange table?

A
  • Arranged elements in increasing atomic weight
  • Switch order of specific elements - so it fit properties of others in the same group
  • Left gaps for undiscovered elements
  • He predicted propoerties of undiscovered elements based on other elements in same group
  • Properties matched predictions
  • Scientists accept
54
Q

Diff between modern and Mendeleev periodic table

A
  • Modern - ordered in order of atmoic number - protons - werent discovered
  • Mendeleev - order of aotmic weight
  • Modern - group 0 - not fully discovered back then
55
Q

Prob with Mendeleev ordering in atomic weight

A
  • can appear in wrong order due to presence of isotopes
56
Q

What is the alpha scattering experiment? Why was it done?

A
  • Test plum pudding
  • Thin sheet of gold
  • Fired alpha particles to foil
  • Alpha particles - + charge
  • Most went straight through
  • Some deflected - changed dirction
  • Some bounced straight back off gold foil
  • replaced plum pudding with nuclear model
57
Q

Why did most of the alpha p. go straight through?

A
  • Atom is mostly empty space
  • Plum pudding is wrong
58
Q

Why did some alpha p. deflect?

A
  • Centre has a positive charge
  • alpha p is positive so its repelled and changes direction
59
Q

Why did some alpha p. bounce back?

A
  • centre of atom has a great deal of mass - nucleus
60
Q

Describe nuclear model

A
  • Positive nucleus
  • empty space mostly
    • electrons
61
Q

What did Niels Bohr say?

A
  • Electrons orbit nucleus at specific distances
  • Accepted by other scientists experiment results
  • we called it energy shells
62
Q

What did Chadwick do?

A
  • Found neutrons
  • nucleus has neutrons
63
Q

radius of atom

A

1 X 10-10m

64
Q

radius of nucleus

A

1 X 10-14m

65
Q

atoms in the same period have the same number of ?

A

shells

66
Q

What are fullerenes?

A
  • allotropes of carbon
  • made by bending sheets of graphene into hollow structures
67
Q

Why are nanotubes useful in electronics?

A

each carbon atom has 1 delocalised electron - carry charge

68
Q

2 uses of fullerenes

A
  • catalysts in chemical reactions
  • delivery of medicines around body
69
Q

Why are fullerenes useful catalysts?

A

high sa: v ratio

70
Q

Why is carbon nanotubes useful in tennis racket frames?

A

high strengh to weight ratio

71
Q

Are transition elements metals?

A

yes

72
Q

Alkali metals characteristics

A
  • low density
  • low melting points
  • soft metals
  • react rapidly with oxygen, chlorine, water
  • form ions with 1+ charge
73
Q

Properties of transition elements

A
  • Hard and strong
  • high melting points except mercery (liquid at room temp)
  • high density
  • less reactive than alkali metals - useful for pipes (Cu)
  • form ions with diff charges
  • form coloured compounds
  • form catalysts
  • high density
74
Q

What colour is iron III oxide?

A

Red

75
Q

What colour is manganese II chloride?

A

pink

76
Q

What colour is chromium III chloride?

A

purple

77
Q

What colour is copper II sulfate?

A

blue

78
Q

Name transition metals

A
  • Chromium
  • Manganese
  • Iron
  • Cobalt
  • Nickel
  • copper
79
Q

What colour and ions does Chromium form?

A
  • Cr 2+ = dark blue
  • Cr 3+ = green
  • Cr 6+ = orange
80
Q

What colour and ions does Manganese form?

A
  • Mn 2+ = pale pink
  • Mn 7+ = vivid purple
  • also forms 3+, 4+, 6+
81
Q

What colour and ions does iron form?

A
  • Fe2+ = pale green
  • Fe 3+ = brown
82
Q

What colour and ions does cobalt form?

A
  • Co 2+ = salmon pink
  • Co 3+
83
Q

What colour and ions does nickel form?

A
  • Ni2+ = green
84
Q

What colour and ions does copper form?

A
  • Cu2+ = blue
  • Cu+
85
Q

Why are transition metals used as catalysts

A
  • they form a range of ions
  • eg iron = in haber process
  • eg vanadium used to produce sulfuric acid
86
Q

Reactions with transition metals

A
  • slow reactions
  • less reactive than group 1

Chemistry - Y10 + Y11 (10 decks)

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