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Chemistry preliminary 2020 > Module 3: Reactive Chemistry > Flashcards

Module 3: Reactive Chemistry Flashcards

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1
Q

hydroxide

A

OH-

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2
Q

Nitrate

A

NO3 (-1)

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3
Q

Nitrite

A

NO2 (-)

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4
Q

Phosphate

A

PO4-3

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5
Q

Sulfate

A

SO4-2

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6
Q

Sulfite

A

SO3 (-2)

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7
Q

Carbonate

A

CO3 (-2)

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8
Q

ammonium

A

NH4 +

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9
Q

what is a physical change?

A

a type of change in which the form of matter is altered but one substance is not transformed into another.

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10
Q

What is a chemical change?

A

Chemical Changes occur when a new substance is formed and hence is called a chemical reaction

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11
Q

Physical change examples:

A

Melting Ice, boiling water, chopping wood

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12
Q

Chemical change examples:

A

Burning Wood, fireworks, cooking an egg`

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13
Q

Boiling of water versus electrolysis of water:

A

Boiling water= physical change as its particles remain the same. Electrolysis is a chemical change as it involves energy to remove separate hydrogen and oxygen molecules.

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14
Q

Indicators of a chemical change:

A

color change, formation of a precipitate, formation of a gas, odor change, temperature change

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15
Q

Model of chemical changes experiment:

-aim

A

Aim: To model what occurs at the atomic level during chemical reactions while ensuring that the law of conservation of mass applies

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16
Q

Model of chemical changes experiment:

-identify what occurred and why was it helpful

A

Identify- Modelling how bonds in chemical reactions are broken/formed
Describe: lollies= chemical and toothpicks= bonds
Explain: Chemicals + bonds/ reactions are too small to see, so models are used to teach a concept

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17
Q

what is a synthesis reaction?

A

A synthesis reaction involves the formation of a compound from its elements or from other, usually smaller, compounds.

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18
Q

Magenisum + Oxygen=

A

magnesium oxide

synthesis reaction

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19
Q

A non-metal oxide + water =

A

an acid

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20
Q

A metal oxide + water =

A

base

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21
Q

what is a decomposion reaction?

A

A decomposition reaction involves a single REACTANT breaking down to form a simple product. It usually involves energy from an external source (thermal or electrical)

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22
Q

Metal nitrate =

A

Metal nitrate + oxygen

decomposition

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23
Q

What is the Important example of a decomposition reaction?

A

electrolysis of water

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24
Q

metal carbonate=

A

metal oxide + Carbon dioxide

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25
Q

metal hydroxide =

A

metal oxide + water

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26
Q

What is ahydrocarbon?

A

Hydrocarbons (petrol, oil, coal, gas) contain hydrogen and carbon, because of this they make good fuels as energy is released when the bonds are broken following chemical reactions.

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27
Q

methane:

A

CH14

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28
Q

propane:

A

C3H8

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29
Q

ethane:

A

C2H6

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30
Q

Butane:

A

C4H10

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31
Q

Betane:

A

C5H12

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32
Q

What is complete combustion?

A

Hydrocarbons all burn in sufficient air or oxygen to produce carbon dioxide and water. Combustion is an exothermic chemical reaction. There is no net release of energy.

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33
Q

What is incomplete combustion?

A

Combustion requires oxygen, however in a low oxygen environment combustion can still occur but the products may be different. Carbon monoxide or soot (carbon) can result.

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34
Q

When does a precipitate form?

A

when the attraction between two oppositely charged ions is greater than the attraction between the individual ion and the water molecules. In this case, the oppositely charged ions will bond ionically to each other and precipitate out of the solution as an insoluble solid.

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35
Q

What is double displacement?

A

reactions occur when two elements in different compounds trade places:

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36
Q

What are the solubility rules?

-Soluble

A
  • Group 1 + NH4+ compounds
  • Nitrates
  • chlorides ( except Ag+ and Pb2+)
  • Sulfates ( except Ag+, Pb2+, Ba2+Sr2+, Ca2+)
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37
Q

What are the solubility rules?

-Insoluble

A

Carbonates (except group 1 and NH4+)

Hydroxides and oxides (except group 1, Nh4+ , Ba2+Sr2+, Ca2+)

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38
Q

Whats the difference between soluble and insoluble?

A

Soluble fiber dissolves in water, and Insoluble fiber doesn’t dissolve in water.

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39
Q

Whats an acid?

A

substance that in solution produces H+ ions

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40
Q

What are acids properties?

A

Taste sour, conduct electricity in solution , Ph < 7

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41
Q

What’s a base?

A

substance that in solution produces OH- ions

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42
Q

what are base properties?

A

feels slippery, tastes bitter, conducts electricity in solution, PH > 7

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43
Q

Hydrochloric acid:

A

HCL

44
Q

Sulfuric Acid:

A

H2SO42+

45
Q

Nitric acid

A

HNO₃

46
Q

carbonic acid:

A

H2CO3

47
Q

Acetic acid:

A

CH₃COOH

48
Q

What is a neutralisation reaction?

A

When an acid and base react they form a neutral salt and water:
Acid + Base = Salt + Water

49
Q

What are carbonates?

A

Carbonates are a group of ionic salts containing the polyatomic ion: CO32-.
Carbonates are basic salts as they can be used to neutralise acids.

50
Q

What happens in an acid/ carbonate reaction?

A

When an acid and a metal carbonate reacts, a salt, Carbon dioxide and water are formed:

Acid + Metal Carbonate = Salt + Carbon Dioxide + Water

51
Q

Reaction of Metals and Oxygen

A

All metals except silver, platinum and gold react with oxygen to form oxides.
Metal + Oxygen = Metal Oxide

52
Q

Reaction of Metals and Water

A

Some metals react with water or steam while others do not.

Metal + Water = Metal Hydroxide + Hydrogen Gas

53
Q

Reaction of Metals and Acid

A

Metals can react with acid to form a metal salt and hydrogen gas

Metal + Dilute Acid = Metal Salt + Hydrogen Gas

54
Q

How do you know if a displacement reaction has occurred?

A

Using the standard activity series you can determine if a displacement reaction has occurred

55
Q

What is an ionic equation?

A

shows how the ions present are reacting. In displacement reactions you can show how a metal is leaving its solid state to become an ion in solution. Or it can show how an ion in solution becomes a solid metal.

56
Q

Describe the trends between metal activity and ionisation energy:

A

As you move across the periodic table, the number of valence electrons increase and therefore the ionisation energy increases. Similarly, as you move down the periodic table, the ionisation energy decreases because the attraction between the valence electrons and the nucleus decreases.

57
Q

Describe the trends between metal activity and Atomic Radius:

A

Atomic radius increases down a group as an extra electron shell is added. Atomic radius decreases across a period due to the increasing size of the attractive charge from the nucleus which has the effect of drawing the outer shell electrons closer to the nucleus.
For the active metals in Groups I and II, atomic radius increases down the group, as does reactivity.

58
Q

Describe the trends between metal activity and electronegativity:

A

Electronegativity increases from left to right across a period on the periodic table and decreases from top to bottom. This is opposite to their reactivity as they are less likely to lose an electron. Because of this group one metals are more reactive than group two as they are less likely to lose an electron.

59
Q

What is a redox reaction?

A

A reaction in which one or more electrons are transferred from one atom to another

60
Q

What is oxidation?

A

Loss of electrons

61
Q

What is reduction?

A

Gain of electrons

62
Q

OILRIG

A

Oxidation is loss reduction is gain

63
Q

Apply the law of conservation to redox reactions:

A

There can be no overall loss or gain of electrons, therefore oxidation and reduction occur simultaneously.

64
Q

What is an oxidising agent?

A

A substance that oxidizes another agent and therefore is reduced

65
Q

What is a reducing agent?

A

A substance that reduces another agent and is therefore oxidised

66
Q

Why were oxidation numbers developed?

A

Sometimes it is not easy to tell which species is oxidised or reduced. Due to the difficulties, chemists developed numbers that allow us to decide easily whether or not oxidation or reduction are involved

67
Q

Oxidation rules:

A

The cation is always written first followed by the anion
The oxidation number for a free element is always=0
The oxidation number of a simple ion is equal to the charge of the ion
Group 1 and 2 metals have an oxidation number equal to the charge on their ions
Hydrogen has an oxidation number of +1 with non-metals
Oxygen normally has an oxidation number of -2
Chlorine,bromine and iodine are always -1, unless they are paired w oxygen
The sum of main group elements equals 0
The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion

68
Q

What are half equations?

A

Are used to demonstrate the transfer of electrons.You must show whether the electrons are being lost or gained by writing them in the reactants (gained) or products (lost) side of the equation. Your electrons MUST be equal in both half equations.

69
Q

What is a galvanic cell?

A

A galvanic cell is a cell capable of producing an electric current from a redox reaction that occurs within it

70
Q

What do galvanic cells allow?

A

The conversion of chemical energy into electrical energy

71
Q

What is a cathode?

A

a positive reduction electrode

72
Q

What is an anode?

A

A negative oxidation electrode

73
Q

What is the purpose of galvanic cells?

A

The purpose is to separate the oxidation and reduction half-cells in order to use the electricity which has been created in a spontaneous reaction.

74
Q

How is a battery formed?

A

A battery is formed when multiple galvanic cells are placed in series to get a higher potential (voltage)

75
Q

THE RED CAT ATE AN OX

A

reduction at cathode oxidation at anode

76
Q

What is an electrode ? galvanic cells

A

Solid metal piece placed in solution

77
Q

What is a solution? galvanic cells

A

What the electrodes are placed in. The solution will contain the ion of the specific electrode placed in it.

78
Q

What is a salt bridge?

A

Contains ions to balance the charges formed in the 2 compartments. It is placed as a “bridge” between the 2 solutions. Cations move towards the cathode and anions move towards the anode.

79
Q

What is a voltmetre?

A

Measures the voltage produced

80
Q

What is a beaker galvanic cells

A

Holds electrolyte solution

81
Q

What is a conducting wire galvanic cells?

A

Enables for the transfer of electrons and creates the circuit.

82
Q

How does a galvanic cell work?

A

When the cathode and anode are connected by a conducting wire, electrons will naturally flow from the less electronegative metal to the more electronegative metal. In doing so, a current is produced, which can be measured using a microammeter

83
Q

What is zinc in a galvanic cell?

A

Anode

oxidised

84
Q

What is Copper in a a galvanic cell?

A

Cathode

reduced

85
Q

What is the purpose of a salt bridge?

A

The salt bridge is a device that provides electrical contact between the two solutions. It allows ions to flow between the two beakers. As electrons are transferred from the oxidation half-cell to the reduction half-cell, a negative charge builds in the reduction half-cell and a positive charge in the oxidation half-cell. That charge build up would serve to oppose the current from anode to cathode, effectively stopping the electron flow.

86
Q

Standard Electrode Potentials:

A

The table of standard reduction potentials provides a list of values that can be used to calculate the overall voltage of a galvanic cell and also to determine whether a reaction will occur spontaneously.

87
Q

How do you know if a spontaneous reaction has occurred?

A

= a oxidising agent (reduced) must react with a reducing agent (oxidised) that is on the table of reduction potentials

If the value is positive, the reaction will occur spontaneously, if it is negative there will be no reaction.

88
Q

Steps to calculate voltage of a redox reaction:

A
  1. Determine the starting species; iron is a metal, so Fe(s), copper is in solution so Cu2+.
  2. Find the first substance in the table: Fe(s) is the tenth equation, (although it is reversed);
    Fe2+ + 2e- ⇌ Fe(s) - 0.44 V
  3. Reverse the equation and sign if necessary; as we are starting with Fe(s) not Fe2+,
    Fe(s) ⇌ Fe2+ + 2e- + 0.44 V
  4. Find the second substance in the table: Cu2+ is the sixteenth equation;
    Cu2+ + 2e- ⇌ Cu(s) + 0.34 V
  5. Reverse the equation and sign if necessary (not necessary in this case).
  6. Add the two half-equations to find the net ionic equation and the overall voltage.
    Fe(s) ⇌ Fe2+ + 2e- + 0.44 V
    Cu2+ + 2e- ⇌ Cu(s) + 0.34 V
    Cu2+ + Fe(s) ⇌ Cu(s) + Fe2+ + 0.78 V
89
Q

What does rate of reaction mean?

A

the rate of change of concentration with time.

90
Q

How do you calculate the average rate of reaction?

A

The average rate of reaction over a small time interval is the change in concentration divided by the time taken for the changes to occur.

91
Q

What is a catalyst?

A

A substance that increases the rate of a reaction without undergoing permanent chemical change in the reaction

92
Q

What is a homogenous reaction?

A

A Homogeneous reaction occurs when the reactants are present as a homogeneous mixture of gases or as a solution

93
Q

What factors influence a homogenous reaction?

A

Concentration of the reactants
Nature and concentration of any catalyst
temperature

94
Q

What is a heterogenous reaction?

A

reaction occurs at the interface of two phases such as between a gas and a solid or between a solution and a solid.

95
Q

What factors influence a heterogenous reaction?

A

It is also affected by extra factors:
State of division of the solid involved
Rate of stirring/ or if it was stirred at all

96
Q

WHat does the collision theory state?

A

The collision theory proposes that for a chemical reaction to occur, the reactant particles must:
Collide
Have more than a certain minimum amount of kinetic energy (in order to break the bonds)
Be correctly orientated ( to ensure that broken bonds don’t just reform but their is a new substance created as a result of the new bonds)

97
Q

What is activation energy?

A

The minimum amount of energy reactants must have to undergo reaction. The more rapidly the rate increases with temperature, the larger the activation energy.

98
Q

Why does kinetic energy make a reaction occur?

A

it breaks the bonds

99
Q

WHy does orientation matter for reaction to occur?

A

to ensure that broken bonds don’t just reform but their is a new substance created as a result of the new bonds

100
Q

What are enzymes?

A

Enzymes are biological catalysts that bring about important reactions in all living cells

101
Q

WHat does a heterogenous catalyst do?

A

A heterogeneous catalyst works by providing a surface that can break or weaken chemical bonds in a reactant molecule absorbed on it

102
Q

effect of temp on rate of reaction

A

Particles are always in motion and reactant particles may collide. If they don’t have enough energy, they will simply bounce off. Adding heat increases the kinetic energy allowing the particles to move quickly and have greater momentum when they collide

103
Q

effect of surface area on rate of reaction

A

When we increase the surface area of a reactant, more individual particles, ion, atoms, molecules, etc. are exposed to any other reactant. This increases the number of collisions and hence the rate of reaction.

104
Q

effect of concentration on rate of reaction

A

The greater the concentration, the larger number of reactant particles per unit volume, the greater the chances of collision and hence, the higher the reaction rate.

105
Q

aboriginal example

A

The cycad palms in N and NE Australia. The fruit is cut and placed in mesh bags which are then soaked in water for several days. This allows time for toxic chemicals to leach out of the fruit. Insoluble starchy compounds remain after this process which are safe for consumptio

Chemistry preliminary 2020 (5 decks)

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