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IP Secondary 4 Chemistry > Chapter 1 - The Periodic Table > Flashcards

Chapter 1 - The Periodic Table Flashcards

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1
Q

What is an element?

A

A substance that cannot be split into two or more simpler substances by chemical processes or electricity

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2
Q

What does the proton (atomic) number represent?

A

The number of protons in the nucleus of an atom

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3
Q

What does the nucleon (mass) number represent?

A

The number of protons and neutrons in the nucleus of an atom

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4
Q

How are elements arranged in the Periodic Table?

A

Elements are arranged in order of their increasing proton (atomic) numbers

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5
Q

Metals are located on the ________ of the Periodic Table.

A

left and middle

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6
Q

Non-metals are located on the ________ of the Periodic Table

inclusive of ________ located at the top of the Periodic Table

A

right

hydrogen

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7
Q

Metalloids are located near the ________ between metals and non-metals

A

dividing line

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8
Q

What are the metalloids?

A

boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), polonium (Po), astatine (At)

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9
Q

How is the group number determined?

A

Determined by the number of valence electrons

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10
Q

What do elements in the same group have in common?

A
  • Same number of valence electrons

- Similar chemical properties

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11
Q

Elements with 1, 2 or 3 valence electrons (metals) tend to ________ electrons to form ________ charged ions, or ________

A

lose
positively
cations

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12
Q

Elements with 5, 6 or 7 valence electrons (non-metals) tend to ________ electrons to form ________ charged ions, or ________

A

gain
negatively
anions

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13
Q

How is the period number determined?

A

Determined by the number of electron shells

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14
Q

What do elements in the same period have in common?

A

Same number of electron shells

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15
Q

Why do the atomic radii of the elements increase down the group gradually?

A

The number of electron shells or energy levels increases down the group as the number of electrons increases.
Each subsequent electron shell or energy level is further away from the nucleus which causes the outer electrons to be more shielded from the attraction of the nucleus (decrease in effective nuclear charge) and less strongly bound, therefore leading to increase of the atomic radii down the group.

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16
Q

Why are ionic radii for elements that form positive charge smaller while that for elements that form negative charge larger?

A

As electrons are removed from the outer shell to form positive ion, the attraction for the electrons increases which results in a decrease in ionic radius.
As electrons are added to the outer shell to form negative ion, the repulsion between the electrons causes the ionic radius to increase.

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17
Q

Define “metallic character”

A

The tendency of an element to lose electrons and form positive ions (cations)

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18
Q

Define “non-metallic character”

A

The tendency of an element to gain electrons and form negative ions (anions)

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19
Q

Properties of elements become ________ metallic down the group (i.e. elements lose electrons ________ easily).

A

more

more

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20
Q

Properties of elements become ________ metallic from left to right across the period (i.e. elements lose electrons ________ easily).

A

less

less

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21
Q

Properties of elements become ________ non-metallic from left to right across the period (i.e. elements gain electrons ________ easily).

A

more

more

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22
Q

Group I elements are known as the ________

A

alkali metals

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23
Q

What are the Group I metals?

A

lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), francium (Fr)

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24
Q

What are the physical properties characteristic of Group I metals?

A
  • Are soft and can be cut by a knife
  • Have a low density (lithium, sodium and potassium float on water)
  • Have relatively low melting and boiling points
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25
Q

What are the physical properties of Group I metals that are typical of most metals?

A
  • Are good conductors of heat and electricity

- Are shiny (seen only when alkali metals are freshly cut)

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26
Q

What is the physical properties trend of Group I metals?

  • Softness ________ down the group
  • Density ________ down the group
  • Melting and boiling points ________ down the group
A

increases
increases
decrease

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27
Q

What are the chemical properties of Group I metals?

A

Are very reactive

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28
Q

What happens in the reaction of alkali metals with oxygen (oxidation)?

A

Alkali metals react with oxygen in the air to form metal oxides
alkali metal + oxygen → alkali metal oxide

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29
Q

Oxidation: The rate with which alkali metals react with oxygen in the air ________ down the group

  • lithium – tarnishes ________
  • sodium – tarnishes ________
  • potassium – tarnishes ________
A

increases
slowly
quickly
very quickly

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30
Q

Oxidation: How are alkali metals stored?

A

Stored in oil to prevent them from reacting with oxygen and tarnishing

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31
Q

Oxidation: Equation for reaction of lithium with oxygen

A

lithium + oxygen → lithium oxide

4Li(s) + O2(g) → 2Li2O(s)

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32
Q

Oxidation: Equation for reaction of sodium with oxygen

A

sodium + oxygen → sodium oxide

4Na(s) + O2(g) → 2Na2O(s)

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33
Q

What happens in the reaction of alkali metals with water?

A

Alkali metal reacts with water to form a metal hydroxide

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34
Q

Reaction with water: Observations for reaction of lithium with water

A
  • Reacts quickly with water
  • Lithium floats on water
  • No flame is seen
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35
Q

Reaction with water: Equation for reaction of lithium with water

A

lithium + water → lithium hydroxide + hydrogen

2Li(s) + 2H2O(l) → 2LiOH(aq) + H2(g)

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36
Q

Reaction with water: Observations for reaction of sodium with water

A
  • Reacts very quickly with water
  • Sodium dissolves and darts around the water surface
  • A yellow flame is seen
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37
Q

Reaction with water: Observations for reaction of potassium with water

A
  • Reacts violently with water
  • Potassium dissolves and darts around the water surface very quickly
  • A lilac flame is seen
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38
Q

Reaction with water: Observations for reaction of rubidium and caesium with water

A

Violent reactions, which may result in an explosion

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39
Q

What is the chemical properties trend of Group I metals?

- Reactivity ________ down the group

A

increases

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40
Q

Compounds of alkali metals:

  • Have ________ chemical formulae
  • Have ________ bonds
  • Are ________ in water
A

similar
ionic
soluble

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41
Q

Group VII elements are known as the ________

A

halogens

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42
Q

What are the halogens?

A

fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At)

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43
Q

What are the physical properties of halogens?

A

Have low melting and boiling points

fluorine and chlorine are gases, bromine is a liquid and iodine is a solid at room temperature

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44
Q

Why do halogens have low melting and boiling points?

A

They exist as simple discrete molecules with only weak van der Waals’ forces between the molecules

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45
Q

What is the physical properties trend of halogens?

  • Change from a ________ to a ________ down the group
  • Colour becomes ________ down the group
  • Melting and boiling points ________ down the group
A

gas, solid
darker
increase

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46
Q

Why do the melting and boiling points of halogens increase down the group?

A

The strength of the van der Waals’ forces increase due to the increase in relative molecular mass and size of the molecule

47
Q

What are the chemical properties of halogens?

A
  • Are very reactive

- Are diatomic elements

48
Q

Why do halogens exists as diatomic molecules?

A
  • All halogen atoms require one more electron to obtain a full outer shell and become stable
  • Each atom can achieve this by sharing one electron with another atom to form a single covalent bond
49
Q

What happens in the displacement reactions of halogens?

A

A halogen takes the place of another halogen in a compound

50
Q

Displacement reaction: What are halides?

A

Salts in which a halogen reacts with another metal

51
Q

Displacement reaction: A ________ halogen will always displace a ________ reactive halogen from its halides in solution

A

more

less

52
Q

Displacement reaction: Equation for reaction of fluorine with sodium chloride

A

fluorine + sodium chloride → sodium fluoride + chlorine

F2(aq) + 2NaCl(aq) → 2NaF(aq) + Cl2(aq)

53
Q

Displacement reaction: Will chlorine and potassium bromide react?

A

Yes

produces potassium chloride and bromine

54
Q

Displacement reaction: Will chlorine and potassium iodide react?

A

Yes

produces potassium chloride and iodine

55
Q

Displacement reaction: Will bromine and potassium chloride react?

A

No

56
Q

Displacement reaction: Will bromine and potassium iodide react?

A

Yes

produces potassium bromide and iodine

57
Q

Displacement reaction: Will iodine and potassium chloride react?

A

No

58
Q

Displacement reaction: Will iodine and potassium bromide react?

A

No

59
Q

What is the chemical properties trend of halogens?

- Reactivity ________ down the group

A

decreases

60
Q

Halides:

  • Have ________ chemical formulae
  • Have ________ bonds
  • ________ and ________ halides are soluble in water
A

similar
ionic
Group I metal, ammonium

61
Q

Group 0 elements are known as the ________

A

noble gases

62
Q

What are the noble gases?

A

helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), radon (Rn)

63
Q

What are the physical properties of noble gases?

A
  • Have low melting and boiling points
  • Are all colourless gases at room temperature
  • Are insoluble in water
64
Q

What is the physical properties trend of noble gases?

- Melting and boiling points ________ down the group

A

increase

65
Q

What are the chemical properties of noble gases?

A
  • Have full outer electron shells and do not need to gain, lose or share electrons
  • Are very stable and chemically unreactive
  • Are monatomic elements (they exist as individual atoms)
66
Q

Uses of helium

A

Used in balloons and airships

67
Q

Uses of neon

A

Used in red glowing advertising signs

68
Q

Uses of argon

A

Used as a gas blanket in arc wielding
Used in fluorescent tubes and low energy light bulbs
Used to fill the spaces between the panes in double-glazed windows

69
Q

Uses of krypton

A

Used in lasers for eye surgery

70
Q

Uses of xenon

A

Used in sunbeds

Used as a general anaesthetic and in medical imaging as well as in instruments for radiation detection

71
Q

Uses of radon

A

Used in radiotherapy to treat cancers

72
Q

The block of metals between Groups I and III is known as the ________

A

transition metals

73
Q

What are the physical properties of transition metals?

A
  • Are lustrous (bright and shiny)
  • Are hard and strong
  • Have high densities
  • Are malleable (can be bent and pressed into different shapes) and ductile (can be drawn into wires)
  • Are good conductors of heat and electricity
  • Have high melting and boiling points (except mercury, which is a liquid at room temperature)
74
Q

Compared to the alkali metals, the transition metals are ________ and ________; they ________ be cut with a knife

A

harder
stronger
cannot

75
Q

Compared to the alkali metals, the transition metals have ________ density

A

higher

76
Q

Why are the densities of the transition metals higher than those of the alkali metals?

A

Transition metals have closed packed structures and relatively small radii.
There are more atoms in a fixed volume of transition metal than there are of an alkali metal.

77
Q

Compared to the alkali metals, the transition metals have ________ melting and boiling points, except ________

A

higher

mercury

78
Q

Why are the melting and boiling points of the transition metals higher than those of the alkali metals?

A

In alkali metals, only 1 or 2 electrons per atom are delocalised while in transition elements, both 3d and 4s electrons are delocalised as there is a small energy difference between 3d and 4s orbitals.
Thus, the metallic bonds are stronger in transition elements.

79
Q

Colour of Cr2+ ion

A

Sky blue

80
Q

Colour of Cr3+ ion

A

Green / Violet

81
Q

Colour of Mn2+ ion

A

Pink

82
Q

Colour of Fe2+ ion

A

Green

83
Q

Colour of Fe3+ ion

A

Yellow / Brown

84
Q

Colour of Ni2+ ion

A

Green

85
Q

Colour of Cu2+ ion

A

Blue

86
Q

Colour of Cr2O3 oxide

A

Green

87
Q

Colour of MnO oxide

A

Black

88
Q

Colour of MnO2 oxide

A

Black / Brown

89
Q

Colour of FeO oxide

A

Black

90
Q

Colour of Fe2O3 oxide

A

Reddish-brown

91
Q

Colour of NiO oxide

A

Black

92
Q

Colour of CuO oxide

A

Black

93
Q

Colour of Cu2O oxide

A

Brick-red

94
Q

Colour of CrO4^2- (chromate)

A

Yellow

95
Q

Colour of Cr2O7^2- (dichromate)

A

Orange

96
Q

Colour of MnO4^- (permanganate)

A

Purple

97
Q

Colour of MnO4^2- (manganate)

A

Green

98
Q

Colour of MnO3^-

A

Blue

99
Q

Colour of FeO4^2-

A

Red

100
Q

Transition metals are ________ reactive than alkali metals

A

(much) less

101
Q

Transition metals react ________ with air, water and acid

A

slowly

103
Q

The general trend for transition metals is a ________ in reactivity from left to right across the Periodic Table

A

decrease

104
Q

Uses of iron

A

Converted to steel to make cars and buildings

105
Q

Uses of platinum

A

Used as a catalyst in catalytic converters of cars

106
Q

Uses of copper

A

Used as roofing material

107
Q

Uses of nickel

A

Used to make glass frames that can be bent and twisted yet still retaining their shape
Used as a catalyst to make margarine

108
Q

Uses of mercury

A

Used in thermometers and in sphygmomanometer

109
Q

Uses of titanium

A

Used for hip replacements

Used as a catalyst in making plastics such as cling film

110
Q

Uses of aluminium

A

Used to make walker (Zimmer frame)

111
Q

Uses of transition metals as catalysts

A
  • Platinum: used in catalytic converters to remove polluting gases (carbon monoxide and nitrogen oxides) from exhausts
  • Nickel: used as a catalyst in the production of margarine
  • Iron: used as a catalyst in the production of ammonia from nitrogen and hydrogen via the Haber Process
  • Titanium: used as a catalyst in the production of plastics
112
Q

Uses of transition metals in building

A
  • Iron: used in building materials due to it being hard, strong, abundant and cheap
  • Copper: used in electric cables due to good electrical conductivity
  • Copper: used in plumbing as it is unreactive with water
  • Copper: a durable roofing material because it reacts slowly with air to form a thin green layer of copper compounds
113
Q

Uses of transition metals in jewellery

A
  • Gold, silver, platinum: used to make jewellery and decoration as they are shiny and do not react with air
  • Copper: used in bracelets which may ease rheumatic pains
114
Q

Uses of transition metals in medicine

A
  • Titanium: used in artificial joints such as hip replacements (as strong as steel but much lighter and more resistant to corrosion)
  • Mercury: used in thermometers and also in sphygmomanometer
  • Platinum: used in platinum-based antineoplastic drugs (chemotherapeutic agents to treat cancer)
115
Q

Uses of alloys (brass and zinc)

A
  • Brass (70% copper and 30% zinc): used to make locks, gears (low friction applications), musical instruments such as horns and bells (high workability and durability)
  • Steel (iron and other elements such as carbon, nickel and chromium): used to make cutlery, surgical instruments, pressure vessels, handrails etc (due to its high tensile strength, good corrosion resistance and cheap)

IP Secondary 4 Chemistry (3 decks)

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