Group 7 and Redox Flashcards

1
Q

Properties of F2

A

Yellow gas
Very reactive
Toxic

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2
Q

Cl2 properties

A

Green gas
Very reactive
Toxic

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3
Q

Br2 properties and uses

A

Orange liquid
Very reactive
Toxic
Often used as a solution in water -bromine water Br2(aq)

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4
Q

I2 properties

A

Grey crystals
Reactive
Toxic
Easily turns into purple vapour on heating
Used in solution as antiseptic

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5
Q

Trend in atomic radius

A

Atomic radius increases
More shells/more shielding
Bigger atoms

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6
Q

Trend in electronegativity

A

Electro negativity decreases
Bigger atoms/more shells
More shielding
Weaker attraction between nucleus and 2 electrons in covalent bond

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7
Q

What is electronegativity

A

The power of an atom to attract the 2 electrons in a covalent bond

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8
Q

Melting and boiling point trend

A

Increases
Bigger molecules
More VDW forces
Higher mpt/bpt between MOLECULES

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9
Q

Trend in first ionisation energy

A

Decreases
Atoms get bigger / more shells
More shielding
Therefore weaker attraction from nucleus to electron in outer shell I’m

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10
Q

What is the reaction equation for Cl2 and Br-?

A

Cl2 + 2 Br- → 2 Cl- + Br2

This reaction shows the conversion of chlorine and bromide ions to chloride ions and bromine.

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11
Q

What color solution forms when bromine is present in aqueous solution?

A

Yellow solution forms

This indicates the presence of bromine in its aqueous form.

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12
Q

What is the reaction equation for C/2 and I2?

A

Cl2 + 21- → 2 Cl- + I2

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13
Q

What happens to the solution when Br2 is added to I-?

A

Brown solution forms

This indicates the formation of iodine in the solution.

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14
Q

What is the reaction equation for Br2 and I-?

A

Br2 + 2I- → 2 Br- + I2

This reaction results in the formation of bromide ions and iodine.

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15
Q

What color solution does I2 form in aqueous solution?

A

Brown solution forms

This indicates the presence of iodine in its aqueous form.

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16
Q

What happens to the solution when I2 is present?

A

Stays brown solution (no reaction)

This indicates that there is no further reaction occurring in the presence of iodine.

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17
Q

What is the state of Br2 in aqueous solution?

A

Stays yellow solution (no reaction)

This indicates that bromine remains in its aqueous form without reacting further.

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18
Q

What is the trend of oxidising power among halogens?

A

Cl, > Br2 > I2

This trend indicates that chlorine is the strongest oxidising agent among the three.

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19
Q

What happens when a halogen acts as an oxidising agent?

A

It gains electrons (taken from the oxidised species)

This process is represented by the equation: X2 + 2e- → 2X.

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20
Q

Fill in the blank: When a halogen gains electrons, the reaction can be represented as _______.

A

X2 + 2e- → 2X

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21
Q

Why does the ability of halogens to gain electrons decrease down the group?

A

Atoms are larger & there is more shielding (due to extra electron shell)

This increased distance and shielding makes it harder for halogens to attract additional electrons.

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22
Q

True or False: It becomes easier to gain an electron as you move down the group of halogens.

A

False

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23
Q

What is the reaction of Cl2 and 2 Br-?

A

cl2 + 2Br- =2 Cl- + Br2

This reaction indicates the formation of chloride ions and bromine.

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24
Q

What color solution forms in the organic layer when Br2 is produced?

A

Yellow solution

The yellow solution indicates the presence of bromine in the organic layer.

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25
Q

What is the reaction cl2 + I-

A

cl2 + 2I-=2 CI- + I2

This reaction shows the formation of iodide ions and iodine.

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26
Q

What color solution forms in the organic layer when I2 is produced?

A

Purple solution

The purple solution indicates the presence of iodine in the organic layer.

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27
Q

What is the result of the reaction Br2 + I-

A

Br2+2I- = 2Br-+ I2

This reaction results in the formation of bromide ions and iodine.

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28
Q

What is the chemical reaction for burning magnesium?

A

2Mg (s) + O2(g) → 2MgO (s)

This represents the combustion of magnesium in the presence of oxygen.

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29
Q

What process occurs when magnesium burns?

A

Oxidation

Oxidation involves the addition of oxygen to a substance.

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30
Q

What happens to magnesium during its oxidation?

A

Magnesium is oxidised to magnesium oxide

The resulting compound is magnesium oxide (MgO).

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31
Q

What is an oxidising agent?

A

An oxidising agent allows oxidation to happen by providing oxygen

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32
Q

In the reaction of burning magnesium, which substance is the oxidising agent?

A

Oxygen

Oxygen is responsible for oxidising magnesium in the reaction.

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33
Q

What is the chemical reaction for reducing copper oxide?

A

CuO/s) + H2 (g) → CU/s) + H2 (l)

This reaction shows the transformation of copper oxide to copper through reduction.

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34
Q

What does reduction involve?

A

Removing oxygen

In the context of this reaction, reduction refers to the process of removing oxygen from copper oxide.

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35
Q

What is reduced in the reduction of copper oxide?

A

Copper oxide is reduced to copper

This indicates that copper oxide loses oxygen and becomes elemental copper.

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36
Q

What is a reducing agent?

A

A reducing agent is a substance that donates electrons to another substance, causing the reduction.

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37
Q

Which substance acts as the reducing agent in the reduction of copper oxide?

A

Hydrogen

In this reaction, hydrogen provides the electrons needed to reduce copper oxide.

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38
Q

What type of reaction is CuSO4 + Mg(s) → MgSO4 (aq) + CU(S)?

A

Redox reaction

Reduction and oxidation occur in this type of reaction.

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39
Q

What elements are involved in the reaction CuSO4 + Mg(s)?

A

Copper (Cu), Sulfur (S), Magnesium (Mg), Oxygen (O)

The reaction includes these elements in the compounds.

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40
Q

In the reaction CuS Of + Mg(s), what happens to oxygen?

A

No oxygen is involved

This distinguishes redox reactions from others that require oxygen.

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41
Q

Fill in the blank: The reaction CuS Of + Mg(s) → MgSO4 (aq) + CU(S) is an example of a _______ reaction.

A

Displacement reaction

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42
Q

What is the oxidation number of elements?

A

0

This applies to all elements in their standard state.

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43
Q

What is the oxidation number of H2?

A

0

H2 is a diatomic molecule where each hydrogen atom has an oxidation state of 0.

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44
Q

What is the oxidation number of Na?

A

0

Sodium (Na) in its elemental form has an oxidation state of 0.

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45
Q

What is the oxidation number of each element in a simple ion?

A

The oxidation number of each element is the same as its charge.

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46
Q

What is the overall oxidation number for an uncharged ionic substance?

A

The overall oxidation number is 0.

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47
Q

What is the oxidation number of Na in NaCl?

A

+1

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48
Q

What is the oxidation number of Cl in NaCl?

49
Q

What is the oxidation number of Al in AlBr?

50
Q

What is the oxidation number of Br in AlBr?

51
Q

What is the chemical symbol for Hydrogen?

52
Q

In which group of the periodic table is Hydrogen classified?

53
Q

In which group of the periodic table is Aluminium classified?

54
Q

What is the oxidation state of Hydrogen when not joined to a metal?

A

+1 (unless joined to a metal, -1)

55
Q

What is the oxidation state of Aluminium?

56
Q

What is the oxidation state of Oxygen?

57
Q

What is the oxidation state of Fluorine?

58
Q

What is the oxidation state of Chlorine?

59
Q

What is a compound ion?

A

A group of atoms covalently bonded that have an overall charge

60
Q

How are compound ions treated in terms of oxidation numbers?

A

Exactly the same as molecules

61
Q

What must the overall oxidation number of a compound ion add up to?

A

The overall charge

62
Q

What must be balanced in a chemical equation?

A

All reactants and products must be balanced

This includes atoms, ions, charges, and electrons.

63
Q

What law states that mass is conserved in a chemical reaction?

A

Law of conservation of mass

This law implies that the total mass of reactants equals the total mass of products.

64
Q

Fill in the blank: The law of conservation of mass states that all reactants and products must be _______.

65
Q

What types of entities must be balanced in a chemical equation?

A
  • Atoms
  • Ions
  • Charges
  • Electrons

Each of these entities must be accounted for to ensure a balanced equation.

66
Q

What are the components allowed in half equations?

A

The substance you start from, what it is oxidised or reduced to, hydrogen ions (H+), water, and electrons.

67
Q

In half equations, what ion is used unless the substance is alkaline?

68
Q

In alkaline conditions, what ion is used in half equations?

69
Q

What must be included in a half equation to represent oxidation or reduction?

70
Q

Fill in the blank: In half equations, you are only allowed to write the substance you start from and what it is _______.

A

oxidised or reduced to

71
Q

True or False: Water can be included in half equations.

72
Q

What is the reducing power trend among halide ions?

A

Cl < Br < I-

73
Q

What happens when a halide ion acts as a reducing agent?

A

It loses electrons.

74
Q

What is the general reaction for a halide ion acting as a reducing agent?

A

2 X → X2 + 2 e

75
Q

What happens to the ease of losing an electron down the group of halide ions?

A

It becomes easier to lose an electron.

76
Q

Why does it become easier to lose an electron down the group of halide ions?

A

Ions are larger & there is more shielding due to extra electron shell.

77
Q

What is disproportionation in chemistry?

A

A reaction where an element simultaneously oxidises and reduces.

78
Q

What is the reaction of chlorine with water?

A

Cl2 (g) + H2O (l) = HClO (aq) + HCl (aq)

79
Q

What happens when universal indicator is added to the solution of chlorine and water?

A

It first turns red due to acidity and then turns colourless as HCIO bleaches the colour.

80
Q

What occurs when chlorine is bubbled through water in bright sunlight?

A

2Cl2 + 2H2O → 4H+ + 4Cl- + O2

81
Q

What happens to the greenish colour of chlorine water when exposed to sunlight?

A

It fades as Cl reacts and a colourless gas (O2) is produced.

82
Q

What is the cause of the greenish colour of chlorine solutions?

A

The presence of Cl.

83
Q

What is a primary use of chlorine in water treatment?

A

To kill bacteria.

84
Q

What are the benefits of using chlorine for water treatment?

A

The benefits to health outweigh its toxic effects.

85
Q

Fill in the blank: Disproportionation is a reaction where an element simultaneously _______ and _______.

A

[oxidises] and [reduces]

86
Q

True or False: Chlorine water retains its greenish colour in sunlight.

87
Q

What is the reaction of chlorine with cold dilute NaOH solution?

A

Cl2 (aq) + 2 NaOH (aq) → NaCl (aq) + NaClO (aq) + H2O (l)

The colour of the halogen solution will fade to colourless.

88
Q

What is the use of the mixture of NaCl and NaClO?

A

Used as bleach and to disinfect/kills bacteria

This mixture is effective in sanitizing and cleaning.

89
Q

What is the IUPAC naming convention for compounds containing sulfur and chlorine with oxygen?

A

Called sulfates and chlorates with relevant oxidation number given in Roman numerals

Remember to add the oxidation number when naming these compounds.

90
Q

What is the oxidation number for sodium chlorate(I)?

A

NaClO

This indicates that chlorine has an oxidation state of +1.

91
Q

What is the oxidation number for sodium chlorate(V)?

A

NaClO3

This indicates that chlorine has an oxidation state of +5.

92
Q

What is the oxidation number for potassium sulfate(VI)?

A

K2SO4

This indicates that sulfur has an oxidation state of +6.

93
Q

What is the oxidation number for potassium sulfate(IV)?

A

K2SO3

This indicates that sulfur has an oxidation state of +4.

94
Q

What are ammonium ions represented by?

95
Q

In which solutions are ammonium ions present?

A

Dilute ammonia solution and any ammonium salt, such as ammonium chloride.

96
Q

How can ammonium ions be identified in a solution?

A

By adding dilute sodium hydroxide solution and gently heating.

97
Q

What happens to ammonium ions when heated with dilute sodium hydroxide?

A

They are converted to ammonia gas.

98
Q

What color change occurs in damp red litmus paper when ammonium ions are present?

A

Turns blue.

99
Q

What is the effect of ammonium ions on damp universal indicator paper?

A

Turns blue.

100
Q

Action of AgNo3 on the halides

A

F- = no precipitate
Cl- = white ppt
Br-= cream ppt
I- = yellow ppt

101
Q

Action of dilute NH3 On the halides

A

F-= x
Cl-= soluble
Br-= insoluble
I-= insoluble

102
Q

Action of concentrated NH3 on halides

A

F-= x
Cl- = soluble
Br-= soluble
I-= insoluble

103
Q

What ions can be detected when testing for carbonate ions?

A

Carbonate ions, CO32-

104
Q

What is added to the test compound to detect carbonate ions?

A

An acid, such as dilute hydrochloric acid

105
Q

What indicates the presence of carbonate ions during the test?

A

Carbon dioxide gas bubbles

106
Q

What is used to confirm that the gas produced is carbon dioxide?

107
Q

What happens to limewater when carbon dioxide is bubbled through it?

A

It turns from clear to milky

108
Q

Fill in the blank: Carbonate ions can be detected whether in a solid compound or in _______.

109
Q

What is the formula for sulfate ions?

A

SO42-

Sulfate ions are polyatomic ions commonly found in various chemical compounds.

110
Q

What solution is used to detect sulfate ions?

A

Barium chloride solution

Barium chloride reacts with sulfate ions to form a precipitate.

111
Q

What is the first step in testing for sulfate ions?

A

The test solution is acidified using a few drops of dilute hydrochloric acid

Acidification helps to eliminate interference from other ions.

112
Q

What occurs after adding barium chloride solution to the acidified test solution?

A

A white precipitate of barium sulfate forms if sulfate ions are present

This precipitation reaction is a key indicator of sulfate ions.

113
Q

Write the chemical equation for the reaction between barium chloride and sodium sulfate.

A

BaCl2(aq) + Na2SO4(aq) → 2NaCl(aq) + BaSO4(s)

This equation shows the formation of sodium chloride and barium sulfate.

114
Q

True or False: Barium sulfate is soluble in water.

A

False

Barium sulfate is an insoluble compound, which is why it precipitates out of solution.

115
Q

What is the method to test for hydroxide ions in a solution?

A

Test a 1 cm depth of solution in a test tube with red litmus paper or universal indicator paper.

116
Q

What color change indicates the presence of hydroxide ions?

A

Hydroxide will turn damp red litmus paper blue.

117
Q

Fill in the blank: Hydroxide ions will turn _______ red litmus paper blue.

118
Q

What is an alternative method suggested for testing a solution?

A

Think about how you could use a solution of magnesium ions.