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Chemistry semester 1 > 1.4: The Periodic table and patterns of change > Flashcards

1.4: The Periodic table and patterns of change Flashcards

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1
Q

How is the periodic table arranged as of 2014?

A
  • reading left to right, arranged in order of increasing atomic number.
  • 7 horizontal period and 18 vertical groups
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2
Q

What does the position of the elements mean?

A

Linked to physical and chemical properties, which allows for prediction

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3
Q

What are vertical columns called?

A

groups

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4
Q

What do the groups correspond to?

A

elements in the same group have similar chemical properties, they have the same amount of electrons in their outer shell

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5
Q

What are group 1 elements called?

A

Alkali metals

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6
Q

What do group 1 metals do in terms of reactions/reactivity?

A

They react with water to form hydrogen gas and an alkaline solution of the metal hydroxide.

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7
Q

What happens to reactivity as you go down group 1?

A

they become more reactive

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8
Q

What is the name of group 2?

A

Alkaline earth metals

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9
Q

What happens to reactivity as you go down group 2?

A

they become more reactive

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10
Q

What is the name of group 7/17?

A

halogens

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11
Q

What is important about group 7?

A

they are the most reactive non-metallic group

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12
Q

What happens to reactivity as you go down group 7?

A

reactivity decreases

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13
Q

what is the name of group 0?

A

noble gases

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14
Q

What happens to group 0?

A

They are inert/unreactive

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15
Q

What are the horizontal rows called?

A

periods

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16
Q

What do periods show?

A

The number of the period, gives the number of the highest occupied energy electron shell

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17
Q

What blocks are present on the periodic table?

A

s, d, f, p (same as orbitals)

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18
Q

What are elements that behave like both metals and non-metals called?

A

metalloids

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19
Q

Why are group 2 called alkaline earth metals?

A

Because they form an alkaline solution with water

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20
Q

What happens to group 2 in terms of atomic radius?
WHY?

A

It increases down the group
- number of electrons increases
- number of main electron shells increase
- more shielding to outermost electrons
- outer electrons repelled further from the nucleus

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21
Q

What happens to group 2 in terms of Ionisation Energies?
WHY?

A

decreases down the group:
- atomic radius increases
- number of main electrons shells increase
- more shielding to outermost electrons
- weaker nuclear attraction to outermost electrons

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22
Q

What happens to group 2 in terms of melting/boiling points?
WHY?

A

Decrease down the group:
- more shells and shielding
- weaker electrostatic attraction between positive cation
- less energy needed to overcome attraction

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23
Q

What happens to group 2 in terms of reactivity?
WHY?

A

increases down the group
- will lose 2 e- which requires energy

  • outer electron (s) in shell further from nucleus
  • more shielding
  • weaker nuclear attraction
  • outer electron(s) more easily lost
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24
Q

Metal + oxygen –>

A

metal oxide (basic oxide)

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25
Q

Metal + oxygen –>
example - magnesium

A

2Mg(s) + O₂(g) –> 2MgO (s)

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26
Q

Metal + oxygen –>
What is observed when magnesium reacts?

A

Bright white flame for Mg, white solid oxides formed

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27
Q

Metal + oxygen –>
example - calcium

A

2Ca(s) + O₂ –> 2CaO(s)

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28
Q

Metal + oxygen –>
what is observed when calcium reacts?

A

Red flame for calcium, white solid oxides formed

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29
Q

Metal + water –>

A

Metal hydroxide + hydrogen

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30
Q

Metal + water –>
example - magnesium

A

Mg(s) + 2H₂O(l) –> Mg(OH)₂ (aq) + H₂O
PH - 8/9

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31
Q

Metal + water –>
What is observed when magnesium reacts?

A

Very slow formation of bubbles of gas seen on the surface of magnesium

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32
Q

Metal + steam –>

A

Metal oxide + hydrogen (Mg only)

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33
Q

Metal + steam –>
example - magnesium

A

Mg(s) + H₂O –> MgO (s) + H₂(g)

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34
Q

Metal + steam –>
What is observed when magnesium reacts?

A

White solid formed

35
Q

Metal + water –>
example - calcium

A

Ca(s) + 2H₂O(l) –> Ca(OH)₂(aq) + H₂
PH - 10/11

36
Q

Metal + water –>
what is observed when calcium reacts?

A

Bubbles of gas and a white precipitate form

37
Q

Metal + acid –>

A

metal salt + hydrogen

38
Q

Metal + acid –>
example: calcium + hydrochloric acid

A

Ca(s) + 2HCl (aq)–> CaCl₂(aq) + H₂(g)
(calcium chloride + hydrogen)

39
Q

Metal + acid –>
magnesium + sulfuric acid

A

Mg(s) + H₂SO₄(aq) –> MgSO₄(aq) + H₂(g)
Magnesium sulfate + hydrogen

40
Q

Metal + acid –>
Barium + nitric acid

A

Ba(NO₃)₂(aq) + H₂(g)
Barium Nitrate + hydrogen

41
Q

Metal + acid –>
what observations are seen?

A

Bubbles of gas (effervescence), metal dissolves to form a colourless solution

42
Q

Metal oxide + Water –>

A

Metal hydroxide (all group 2)

43
Q

Metal oxide + Water –>
example - Magnesium

A

MgO(s) + H₂O –> Mg(OH)₂ (aq)
Magnesium hydroxide

44
Q

Metal oxide + Water –>
what is observed when magnesium reacts?

A

White solid dissolves

45
Q

What molecules do halogens form?

A

Diatomic molecules

46
Q

what kind of structure do halogens have and why?

A

The atoms are covalently bonded together so the halogens have a simple covalent structure

47
Q

What happens to melting and boiling point as you go down group 2?
WHY?

A

Melting and boiling point increase
- More electrons
- stronger London forces
- more energy need to overcome attraction

48
Q

What is the physical state of chlorine and fluorine at room temp?

A

gases

49
Q

What is the physical state of bromine at room temp?

A

liquid

50
Q

What is the physical state of iodine at room temp?

A

Solid

51
Q

What kind of structure of halogens form?

A

simple molecular lattice

52
Q

What happens to reactivity as you down group 7?
WHY?

A

decreases
- outer electron(s) in a shell further from nucleus
- more shielding
- weaker nuclear attraction
- electrons less easily gained

53
Q

What happens to the atomic radius of the atoms as you go across each period?
WHY?

A

it get smaller
- increasing number of protons
- electrons are added to the same shell
- no extra shielding
- so a greater nuclear attraction for the outer shell of electrons to the nucleus
- atomic radius decreases

54
Q

How are melting and boiling point determined?

A

By the structure and bonding of the substance

55
Q

What Melting and boiling points do giant structures have?
WHY?

A

High
- strong attractive forces between particles that must be broken
- large amount of energy is therefore needed to break the bonds

56
Q

What are giant structures?

A

Giant metallic / giant covalent

57
Q

What Melting and boiling points do simple molecules and atoms have?
WHY?

A

Relatively low
- weak intermolecular forces between particles
- forces depend on number of electrons
- less energy is needed to overcome the intermolecular forces

58
Q

Where are transition elements located on the periodic table?

A

with in the d-block (scandium through to zinc)

59
Q

What is a d-block element?

A

An element with its outer electron in a d sub shell/orbital

60
Q

What are transition metals?

A

An element that forms one or more stable ion which have a partially filled d-sub shell

61
Q

What are the characteristics of transition metals?

A
  • variable oxidation states
  • acts as catalysts
  • they form complex ions
  • they form coloured compounds
62
Q

Using the table in your book learn the bold oxidation states!

A

Transition metals

63
Q

What is the oxidation number of: Fe²+

A

+

64
Q

What transition elements act as catalysts?

A

iron, platinum, palladium, rhodium, nickel

65
Q

What is iron used for?

A

Making ammonia (haber process)

66
Q

What is platinum, palladium, rhodium used for?

A

Catalytic converters

67
Q

What is nickel used for?

A

Making margarine, hydrogenation of vegetable oils

68
Q

What is a complex ion?

A

A central metal ion surrounded by ligands

69
Q

What is a ligand?

A

A molecule or ion that donates a lone pair of electrons to the central metal ion to form a dative covalent (coordinate) bond

70
Q

What is a coordination number?

A

The number of dative covalent bonds around the central metal ion

71
Q

What is an example of ligands?

A

H₂O : Cl - : NH₃

72
Q

What do all transition metals form when dissolved in water?

A

Hexaaqua ion

73
Q

What is the formula for hexaaqua ion?

A

[X(H₂O)₆]²+

74
Q

What is the formula for a hexaaqua Cooper (II) complex?

A

[Cu(H₂O)₆]²+

75
Q

What is the Cooper ion surrounded by (in hexaaqua Cooper (II) complex)?

A

6 water ligands

76
Q

What does the water molecule donate in the hexaaqua Cooper (II) complex.
what does it form

A

Donates oxygen, to a lone pair of electrons to the central metal ions
- forms a dative covalent/coordinate bond

77
Q

What is the shape of the hexaaqua Cooper (II) complex?

A

Octahedral

78
Q

What is the coordinate number in hexaaqua Cooper (II) complex?
What is the bond angle?

A

6
90 degrees

79
Q

What colour does copper ion form?

A

Blue solution

80
Q

What is copper complex ion hexaaqua ion?

A

[Cu(H₂O)₆]²+

81
Q

What colour does iron (II) form?

A

Pale green solution

82
Q

What is iron (II) complex ion hexaaqua ion?

A

[Fe(H₂O)₆]²+

83
Q

What colour does iron (III) form?

A

pale yellow solution

84
Q

What is iron (III) complex ion hexaaqua ion?

A

[Fe(H₂O)₆]³+

Chemistry semester 1 (8 decks)

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