In Depth Flashcards
(127 cards)
1
Q
Front
A
Back
2
Q
What is the rate of a chemical reaction?
A
It is the speed at which reactants are converted into products.
3
Q
Give an example of a fast reaction.
A
Explosion or combustion.
4
Q
Give an example of a slow reaction.
A
Rusting or fermentation.
5
Q
How can the rate of reaction be measured?
A
By measuring the amount of product formed or reactant used over time.
6
Q
Name 5 factors that affect rate of reaction.
A
Temperature, concentration, surface area, catalyst, pressure (for gases).
7
Q
What does collision theory state?
A
Particles must collide with enough energy for a reaction to occur.
8
Q
What does a steeper slope on a rate graph represent?
A
A faster reaction.
9
Q
What does REDOX stand for?
A
Reduction and Oxidation.
10
Q
Define oxidation in terms of electrons.
A
Loss of electrons.
11
Q
Define reduction in terms of electrons.
A
Gain of electrons.
12
Q
What is OIL RIG?
A
Oxidation Is Loss, Reduction Is Gain (of electrons).
13
Q
What is an oxidizing agent?
A
A substance that causes oxidation and gets reduced.
14
Q
What is a reducing agent?
A
A substance that causes reduction and gets oxidized.
15
Q
What is electrolysis?
A
Chemical decomposition of a substance by passing electric current through it.
16
Q
What is an electrolyte?
A
A substance that conducts electricity and breaks down during electrolysis.
17
Q
What is the cathode?
A
The negative electrode where reduction occurs.
18
Q
What is the anode?
A
The positive electrode where oxidation occurs.
19
Q
What is produced at the cathode during electrolysis of molten NaCl?
A
Sodium metal.
20
Q
What is produced at the anode during electrolysis of molten NaCl?
A
Chlorine gas.
21
Q
Which ion is discharged at the cathode if the metal is more reactive than hydrogen?
A
Hydrogen ion (H⁺).
22
Q
What is electroplating?
A
Using electrolysis to coat an object with a metal.
23
Q
List 3 physical properties of metals.
A
Good conductors, malleable, high melting points.
24
Q
What do metals form when reacting with oxygen?
A
Metal oxides.
25
What gas is produced when metals react with acids?
Hydrogen.
26
Which metals can displace hydrogen from acid?
Metals above hydrogen in the reactivity series.
27
What is an alloy?
A mixture of metals to improve properties.
28
Give an example of an alloy.
Steel (iron + carbon) or bronze (copper + tin).
29
Give two properties of non-metals.
Poor conductors, brittle.
30
Name a non-metal that conducts electricity.
Graphite.
31
What are the allotropes of carbon?
Diamond and graphite.
32
What are hydrocarbons?
Compounds made of hydrogen and carbon only.
33
What is the general formula for alkanes?
CnH₂n+2
34
What is the general formula for alkenes?
CnH₂n
35
What is a homologous series?
A family of compounds with the same functional group and similar properties.
36
What is the test for alkenes?
They decolorize bromine water.
37
What are the products of complete combustion of hydrocarbons?
Carbon dioxide and water.
38
What is produced during incomplete combustion?
Carbon monoxide (CO).
39
What do groups in the periodic table represent?
Elements with the same number of valence electrons.
40
What do periods in the periodic table represent?
Elements with the same number of shells.
41
What happens to reactivity down Group I?
Increases.
42
What happens to reactivity down Group VII?
Decreases.
43
Why are noble gases unreactive?
They have a full outer electron shell.
44
What is the Haber process used for?
To produce ammonia.
45
Write the balanced equation for the Haber process.
N₂ + 3H₂ ⇌ 2NH₃
46
What is the catalyst used in the Haber process?
Iron.
47
What is sulphuric acid used for?
Making fertilizers, detergents, batteries.
48
What flame colour does sodium produce?
Yellow.
49
What flame colour does potassium produce?
Lilac.
50
What is the test for hydrogen gas?
A lighted splint gives a 'pop' sound.
51
What is the test for oxygen gas?
A glowing splint relights.
52
What is the test for carbon dioxide?
Turns limewater milky.
53
What is the result when CO₃²⁻ reacts with acid?
Effervescence due to CO₂ release.
54
What reagent is used to test for chloride ions?
Silver nitrate (AgNO₃) with nitric acid.
55
What is the result of chloride ion test?
White precipitate forms.
56
How does temperature affect rate of reaction?
Increasing temperature gives particles more energy, leading to more successful collisions.
57
How does concentration affect rate of reaction?
Higher concentration means more particles in the same space, increasing collision frequency.
58
How does surface area affect rate of reaction?
Greater surface area exposes more particles for reaction, increasing the rate.
59
What is a catalyst?
A substance that speeds up a reaction without being used up.
60
How does pressure affect gas reactions?
Higher pressure pushes particles closer, increasing collision frequency.
61
What is activation energy?
The minimum energy required for a reaction to occur.
62
How do catalysts lower activation energy?
By providing an alternative pathway with lower activation energy.
63
How can you measure reaction rate using gas collection?
Measure the volume of gas produced over time.
64
What is a redox reaction?
A reaction where both oxidation and reduction occur.
65
In redox, what happens to the oxidation number during oxidation?
It increases.
66
In redox, what happens to the oxidation number during reduction?
It decreases.
67
Give an example of a redox reaction.
Zn + CuSO₄ → ZnSO₄ + Cu (Zn is oxidized, Cu²⁺ is reduced).
68
What is a half-equation?
An equation showing either oxidation or reduction alone.
69
Write a half-equation for oxidation of Zn.
Zn → Zn²⁺ + 2e⁻
70
Write a half-equation for reduction of Cu²⁺.
Cu²⁺ + 2e⁻ → Cu
71
How can you tell a substance is reduced?
It gains electrons or its oxidation number decreases.
72
Name one use of electrolysis.
Extraction of reactive metals like aluminum.
73
What happens to ions at the electrodes?
Cations go to the cathode and anions to the anode.
74
What is the electrolyte in electroplating with copper?
Copper(II) sulfate solution.
75
What metal is used as the anode in copper electroplating?
A pure copper sheet.
76
What happens to the mass of the anode during electrolysis?
It decreases.
77
What happens to the mass of the cathode during electrolysis?
It increases.
78
What determines which ions are discharged during electrolysis of aqueous solutions?
Reactivity of the ions and concentration.
79
Why is electrolysis of molten compounds simpler than aqueous?
No competition with water ions.
80
How are metals arranged in the reactivity series?
From most reactive (potassium) to least reactive (gold).
81
What is the test for hydrogen gas?
A lit splint produces a 'pop' sound.
82
What is corrosion?
Gradual destruction of metals by chemical reactions with the environment.
83
How can corrosion be prevented?
Painting, galvanizing, or coating with oil.
84
Why is aluminum resistant to corrosion?
It forms a protective oxide layer.
85
What is thermal conductivity?
Ability of a substance to conduct heat.
86
What are transition metals?
Elements in the middle block of the periodic table with variable oxidation states.
87
Name one use of copper.
Electrical wiring due to its high conductivity.
88
Name two diatomic non-metals.
Oxygen (O₂), nitrogen (N₂).
89
What type of bonding do non-metals typically form?
Covalent bonding.
90
Why is graphite a good conductor?
It has delocalized electrons that move freely.
91
What are the uses of diamond?
Jewelry and cutting tools due to hardness.
92
Why is carbon essential in organic compounds?
It can form four covalent bonds.
93
What is sublimation?
Direct change from solid to gas without becoming liquid.
94
What are acidic oxides?
Non-metal oxides that dissolve in water to form acids.
95
Give an example of an acidic oxide.
Carbon dioxide (CO₂).
96
Name the first four alkanes.
Methane, ethane, propane, butane.
97
What is the functional group of alkenes?
Carbon-carbon double bond (C=C).
98
What are isomers?
Compounds with the same molecular formula but different structures.
99
What is cracking?
Breaking large hydrocarbons into smaller, more useful ones.
100
What are the products of cracking?
Alkanes and alkenes.
101
What is fermentation?
Breakdown of glucose to ethanol and CO₂ using yeast.
102
What is polymerization?
Joining small molecules (monomers) to form a polymer.
103
Name a common synthetic polymer.
Polyethene (plastic).
104
What are metalloids?
Elements with properties of both metals and non-metals.
105
Give an example of a metalloid.
Silicon.
106
What are transition elements?
Elements in the center block of the periodic table with variable valency.
107
Why are alkali metals stored in oil?
To prevent reaction with air or water.
108
What happens to atomic size across a period?
It decreases.
109
What happens to atomic size down a group?
It increases.
110
What are halogens?
Group VII non-metals like fluorine, chlorine, bromine.
111
What is a displacement reaction in halogens?
More reactive halogens displace less reactive ones from compounds.
112
Name three fertilizers made in industry.
Ammonium nitrate, ammonium sulfate, urea.
113
What is the contact process used for?
Manufacture of sulfuric acid.
114
What are the raw materials for sulfuric acid production?
Sulfur dioxide, oxygen, water.
115
What is the formula of sulfuric acid?
H₂SO₄
116
Name one use of ammonia.
Making nitric acid and fertilizers.
117
What is a batch process?
Chemical manufacturing in separate steps or quantities.
118
What is a continuous process?
Ongoing large-scale chemical manufacturing.
119
Why is recycling important in industry?
Reduces waste, conserves resources, saves energy.
120
What colour flame does calcium produce?
Brick red.
121
What colour flame does barium produce?
Green.
122
What is the test for ammonia gas?
Turns damp red litmus paper blue.
123
What is the test for chlorine gas?
Bleaches damp litmus paper white.
124
What is the result of sulfate ion test with BaCl₂?
White precipitate of barium sulfate.
125
How do you test for nitrate ions?
Add NaOH and aluminium, then warm. Ammonia gas is released.
126
What is the colour of copper(II) ion in flame?
Blue-green.
127
What is the precipitate formed with Fe³⁺ and NaOH?
Reddish-brown precipitate.
