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Additional Science: Chemistry (II) > Additional Science: Chemistry (II) > Flashcards

Additional Science: Chemistry (II) Flashcards

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1
Q

Draw and label an atom

A
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2
Q

What are the masses and charges of these parts of an atom

Proton

Neutron

Electron

A

Protons = +ve (mass 1)

Neutrons = neutral (mass 1)

Electrons = -ve (mass 1/2000th)

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3
Q

Why do atoms usually have no overall electrical charge?

A

Atoms usually have no overall charge because they have equal numbers of protons (+ve) and electrons (-ve), which cancel one another out

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4
Q

All atoms of a particular element (e.g. carbon) all have the same number of what?

A

Protons

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5
Q

What are the following numbers called?

A

a = relative atomic mass

b = atomic number

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6
Q

What do the numbers tell you about the atom?

A

a = relative atomic mass – the number of protons and neutrons in the atom

b = atomic number – the number of protons (usually the same as the number of electrons)

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7
Q

What is an alloy and why are they used?

Give some examples

A

Alloys are mixtures of metals with other elements, e.g. iron + carbon → steel

They have a combination of properties, e.g. bronze, brass, steel etc…

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8
Q

What is a smart alloy and why are they used (shape-memory)?

Give some examples

A

Smart alloys can return to their original shape after being deformed – e.g. glasses and braces

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9
Q

What do these terms means: -

Element

Compound

Mixture

A

Element – pure substance with only 1 type of atom (e.g. gold)

Compound – 2 or more elements chemically bound (e.g. carbon dioxide)

Mixture – more than 1 element or compound not chemically bound (e.g. air)

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10
Q

What are the symbols for the following atoms: -

Oxygen

Nitrogen

Chlorine

Hydrogen

Sodium

Copper

Potassium

Helium

Calcium

Zinc

Iron

Carbon

A

Oxygen (O)

Nitrogen (N)

Chlorine (Cl)

Hydrogen (H)

Sodium (Na)

Copper (Cu)

Potassium (K)

Helium (He)

Calcium (Ca)

Zinc (Zn)

Iron (Fe)

Carbon (C)

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11
Q

What happens to atoms when they chemically react to form a compound?

A

They share, give away, or take electrons

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12
Q

What are the names of these compounds, and which atoms are found in them?

H2O

CaCO3

H2SO4

HCl

CO2

A

Water (H2O)

Calcium carbonate (CaCO3)

Sulfuric acid (H2SO4)

Hydrochloric acid (HCl)

Carbon dioxide (CO2)

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13
Q

What is an isotope?

A

An isotope is an atom with a different amount of neutrons

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14
Q

Use the periodic table to draw the electron structure of the following: -

Neon

Calcium

Sodium

How can you tell which group these atoms are in?

A

The number of electrons in the outer shell is the same as their group number

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15
Q

How many electrons can occupy the 1st and 2nd shell (energy level) of an atom?

A

2 in the 1st shell and 8 in the 2nd shell

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16
Q

The electron structure of sodium can be represented as 2,8,1 – what does this mean?

Represent these atoms: -

Fluorine

Oxygen

Potassium

Magnesium

A

2,8,1 means 2 electrons in the 1st shell, 8 electrons in the 2nd shell and 1 electron in the 3rd shell

Fluorine = 2,7

Oxygen = 2,6

Potassium = 2,8,8,1

Magnesium = 2,8,2

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17
Q

Define these terms: -

Element

Compound

Mixture

A

Element – a pure substance made from 1 type of atom only

Compound – 2 or more elements chemically bound

Mixture – 2 or more elements or compounds mixed together which are not chemically bound

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18
Q

What happens to the electrons of 2 atoms when they chemically react?

A

During a chemical reaction electrons are either given away, taken, or shared

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19
Q

What is an ion?

How are +ve ions formed?

How are -ve ions formed?

A

An ion is an atom with a charge

+ve ions have lost electrons

-ve ions have gained electrons

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20
Q

Explain how the following atoms become ions (will they be +ve or –ve)?

Potassium

Magnesium

Chlorine

Oxygen

A

Potassium – loses 1 electron (K+)

Magnesium – loses 2 electrons (Mg2+)

Chlorine – gains 1 electron (Cl-)

Oxygen – gains 2 electrons (O2-)

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21
Q

Use diagrams to show how these atoms for ionic bonds: -

Sodium + Chlorine

A
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22
Q

Describe and use a diagram to show the structure of ionic compounds

A

Ionic compounds have a giant structure – they are bonded to 6 other ions by electrostatic bonds

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23
Q

What are the melting and boiling points of ionic compounds like?

Why is this?

A

Ionic compounds have high melting points and boiling points – to melt them you have to supply enough energy to break the 6 bonds attached to each ion

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24
Q

What happens to the electrons when atoms form ionic bonds and covalent bonds?

Which is the strongest?

A

Ionic bonds – 1 atom loses electrons and another gains electrons

Covalent bonds – electrons are shared

An individual covalent bond is stronger than an ionic bond

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25
Q

Use diagrams to show how the following compounds are formed: -

Hydrogen

Oxygen

Hydrogen Chloride

A
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26
Q

Use a diagram to show how water is formed

A

Water (H2O)

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27
Q

What are the melting and boiling points of covalent compounds like?

Explain why this is

A

Covalent compounds have low melting and boiling points (are often gases) as there is no attraction between the molecules

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28
Q

How are the elements of the periodic table arranged?

What are the rows called?

What are the columns called?

A

Elements are arranged in order of atomic number

Rows are called periods

Columns are called groups

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29
Q

Which 2 elements would be out of order in the periodic table if they were arranged by atomic mass instead of atomic number?

A

Potassium and Argon

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30
Q

Why do elements in the same group have similar properties?

A

Elements in the same group have similar properties as they all have the same number of electrons in their outer shell

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31
Q

What do these symbols mean?

(s)

(l)
(g)

(aq)

A

(s) = solid
(l) = liquid
(g) = gas
(aq) = aqueous

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32
Q

What are the symbols for these compounds?

Calcium carbonate

Sodium chloride
Hydrochloric acid

A

Calcium carbonate – CaCO3

Sodium chloride – NaCl

Hydrochloric acid - HCl

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33
Q

Why do covalent compounds not conduct electricity when dissolved?

A

Covalent compounds do not conduct because they do not break down into ions

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34
Q

Give the names of 3 covalent compounds which have giant ionic structures?

What is the structure of each like?

A

Diamond – 4 carbon-carbon covalent bonds

Graphite – 3 carbon-carbon covalent bonds

Silicon dioxide – 2 double silicon-oxygen covalent bonds

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35
Q

Why does graphite conduct electricity?

A

Graphite conducts electricity because it is only bonded 3x (meaning there is a delocalised electron to pass the charge)

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36
Q

Explain why ionic compounds have a giant structure

A

Ionic compounds have giant structures because the ions keep their charge and attract up to 6 other ions – forming a giant lattice

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37
Q

What does monatomic mean and why are noble gases monatomic?

A

Monatomic means an atom which only exists on its own (does not react)

Noble gases are monatomic as they have a full shell and are un-reactive

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38
Q

What does diatomic mean and why are elements such as the halogens, hydrogen and oxygen diatomic?

A

Diatomic – atoms in pairs, e.g. H2 and O2

Halogens will form diatomic molecules because they covalently bond with each other, forming pairs

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39
Q

What is the bonding in metals like?

A

The bonding in metals creates delocalised electrons (free to move and pass on electrical current)

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40
Q

Why do metals conduct electricity?

A

The bonding in metals creates delocalised electrons (free to move and pass on electrical current)

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41
Q

Why do ionic compounds conduct electricity when they are dissolved / molten?

A

Ionic compounds conduct electricity when dissolved or molten because they remain as ions (which will pass a current)

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42
Q

What are the symbols for these compounds?

Sulfuric acid

Sodium hydroxide
Nitric acid

A

Sulfuric acid = H2SO4

Sodium hydroxide = NaOH

Nitric acid = HNO3

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43
Q

Use diagrams to show how magnesium oxide forms ionic bonds

A
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44
Q

Use diagrams to show how calcium chloride forms ionic bonds

A
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45
Q

Use diagrams to show how methane (CH4) is formed

A
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46
Q

Use diagrams to show how ammonia (NH3) is formed

A
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47
Q

What are the symbols for these compounds?

Magnesium oxide

Ammonia

Methane

A

Magnesium oxide = MgO

Ammonia = NH3

Methane = CH4

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48
Q

Which group of the periodic table do not form ions?

Explain why this is

A

Noble gases do not form ions as they already have a full outer shell

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49
Q

What are the names of the following groups in the periodic table?

Group 1

Group 2
Middle metals

Group 7

Group 0

A

Group 1 = alkali metals

Group 2 = alkaline Earth metals

Middle metals = transition metals

Group 7 = halogens

Group 0 = Nobel gases

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50
Q

What are nano-materials and what are they used for?

A

Nano-materials (1-100nm) are very small (one nano-metre = one-thousand-millionth of a metre)

They are used for self-cleaning coats on glass etc…

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51
Q

What are smart materials and what are they used for?

A

Smart materials return to their original shape, e.g. metals which can be stretched and then return to their original shape (metals used in braces / spectacles)

52
Q

What is a macromolecule?

Give some examples

A

Macromolecules – are formed by giant covalent bonds, e.g. diamond, graphite, silicon dioxide etc…

53
Q

What is the bonding like in diamonds?

A

Each carbon atom forms 4 covalent carbon-carbon bonds with the carbons around them creating a giant structure and makes them very hard

54
Q

What is the bonding like in graphite?

A

Each carbon forms 3 covalent carbon-carbon bonds with the carbons around them creating a sea of delocalised electrons which will pass an electrical current

55
Q

What is meant by thermosetting plastic?

A

Thermosetting – sets when heated and will not melt again, e.g. a kettle

56
Q

What is meant by thermosoftening plastic?

A

Thermosoftening – will melt when heated, and can be re-shaped

57
Q

How is LD polythene and HD polythene made?

A

LD polythene – heating ethene to 200oC under high pressure

HD polythene – heating ethene to a lower temperature and pressure with a catalysts

58
Q

What is polymerisation?

A

Polymerisation is when small molecules are joined to make longer, more useful molecules (e.g. ethane makes poly(ethane))

59
Q

Give 6 uses of polymers

A

New packaging, waterproof coatings, dental-polymers, hydrogels, smart materials (shape memory polymers)

60
Q

What are the two types of polymer and how does this affect their properties?

A

Low density (LD) polymers (often flexible)

High density (HD) polymers (often more rigid)

E.g. LD polythene for plastic bags and HD polythene for water tanks

61
Q

Why are metals easily shaped?

A

Metals are easily shaped because the atoms are closely arranged and can slide past one another

62
Q

How can you calculate atomic mass?

A

Add the relative atomic masses of the elements within the compound

63
Q

How can you calculate empirical formula?

A

Empirical formula (the simplest possible compound) – divide each element by its mass

Divide each result by the smallest result

Round the numbers up to find out the number of each element

64
Q

How can you calculate percentage yield?

A

Percentage yield – work out the masses for each compound

Divide the mass of one compound by the mass you have been given

Divide the other compounds by this result

65
Q

What is relative atomic mass based on?

A

Relative atomic mass used on a comparison of the mass with 12C isotope

66
Q

What is a mole and how can the mass of a mole of an element be worked out?

A

The relative formula mass of a substance (grams) is known as one mole of that substance

67
Q

How can you calculate the percentage of an element in a compound?

A

(mass of element ÷ mass of compound) x 100

68
Q

Give 3 reasons why a reaction may not give the theoretical yield

A

The reaction may not go to completion because it is reversible

Some of the produce may be lost when it is separated from the reaction mixture

Some of the reactants may react in ways different to the expected reaction

69
Q

What is theoretical yield?

A

The maximum yield that could be obtained if all atoms reacted

70
Q

What is atom economy?

A

In reactions with high atom economy all the atoms react and are not ‘wasted’

71
Q

What is a reversible reaction?

Give an example

A

A reversible reaction is not a permanent reaction and will break back down into the reactants (e.g. the Haber process)

72
Q

What is equilibrium?

A

Equilibrium is reached when the reactions occur at exactly the same rate in both directions

73
Q

What is the Haber process used to manufacture and what is the equation?

A

Ammonia

N2 + 3H2 → 2NH3

74
Q

What are the raw materials used for in the Haber process, and where can these be obtained?

A

Nitrogen – from the air

Hydrogen – from natural gas / water

75
Q

What are the conditions needed for the Haber process

Temperature

Pressure

Catalyst

A

Temperature = 450°C

Pressure = 200atm

Catalyst = iron

76
Q

What happens to the unused nitrogen and hydrogen?

A

Unused nitrogen and hydrogen are recycled

77
Q

During the Haber process how is the ammonia removed?

A

It is liquefied

78
Q

How can the relative amounts of substances in a reversible reaction be altered?

A

Changing the temperature / pressure

79
Q

How does increasing the temperature affect a reversible reaction?

A

Increasing the temperature increases the amount of the endothermic side of the reaction

80
Q

How does decreasing the temperature affect a reversible reaction?

A

Decreasing the temperature increases the amount of the exothermic side of the reaction (however it also slows it down)

81
Q

How does increasing the pressure affect a reversible reaction?

A

Increasing the pressure increases the side of the reaction with the lowest volume

82
Q

How does decreasing the pressure affect a reversible reaction?

A

Decreasing the pressure increases the side of the reaction with the highest volume

83
Q

Why may it be important to companies to understand the conditions of a reversible reaction?

A

So they can get the most amount of product (and therefore the most amount of profit)

84
Q

What type of salts are made from the following?

Hydrochloric acid

Sulfuric acid

Nitric acid

A

Hydrochloric acid – chlorides

Sulfuric acid – sulfates

Nitric acid – nitrates

85
Q

What is electrolysis used for?

A

Separating ions in solution

86
Q

What types of ions do the following form?

Metals

Non-metals

A

Metals = +ve

Non-metals = -ve

87
Q

During electrolysis where are these ions attracted to

Positive

Negative

A

+ve electrode = negative

-ve electrode = positive

88
Q

What are the scientific names for the following?

+ve electrode

-ve electrode

A

+ve electrode = anode

-ve electrode = cathode

89
Q

What is the gain of electrons called?

What is the loss of electrons called?

A

Oxidation = loss

Reduction = gain

OIL RIG

90
Q

During electrolysis where does oxidation occur?

A

Oxidation occurs at the +ve electrode (electrons are lost)

91
Q

During electrolysis where does reduction occur?

A

Reduction occurs at the -ve electrode (electrons are gained)

92
Q

Write out the half equations which happen during the electrolysis of brine

A

2Cl- → Cl2 + 2e-

2H+ + 2e- → H2

93
Q

What are the products of the electrolysis of sodium chloride (brine)?

A

Hydrogen (-ve electrode)

Chlorine (+ve electrode)

Sodium hydroxide (solution)

94
Q

How can electrolysis be used to obtain pure copper from impure copper?

A

Impure copper used as the +ve electrode

Pure copper as the –ve electrode

Solution containing copper ions (e.g. copper sulfate)

95
Q

What is an insoluble salt and how can it be formed?

A

Insoluble salts will not dissolve in water

They are formed by mixing appropriate solutions and filtering the precipitate

96
Q

How can precipitation of unwanted salts be used to treat drinking water?

A

Filter the precipitate (removing unwanted salts)

97
Q

Give 3 ways in which a soluble salt can be prepared

A

Metal + acid

Insoluble base + acid

Acid + alkali

98
Q

How can a solid salt be obtained from a salt solution?

A

Evaporating to leave the salt crystals

99
Q

What is a base?

Give some examples

A

Metal oxides and hydroxides are bases

100
Q

What is the difference between a base and an alkali?

Give some examples

A

Metal oxides and hydroxides are bases

Soluble hydroxides are alkalis (e.g. sodium hydroxide)

101
Q

How are ammonium salts made?

What are they used for?

A

Ammonia is dissolved in water to produce an alkaline solution

This can then be used to neutralise an acid to produce an ammonium salt

These are important in the production of plant fertilisers

102
Q

What type of ions are found in the following?

Acids

Alkalis

A

Acids = H+ (hydrogen)

Alkalis = OH- (hydroxide)

103
Q

What happens to the H+ ions and the OH- ions during a neutralisation reaction?

Include an equation

A

H+ reacts with the OH- to produce water (H2O)

H+(aq) + OH-(aq) → H2O(l)

104
Q

In the following rate of reaction graph: -

Which is the faster reaction?

Which reaction makes the most gas?

A

X = most gas

Y = fastest

105
Q

Using the rate of reaction graph: -

Draw a reaction which happened at a lower temp.

Draw a reaction which added a catalyst

A
106
Q

Using the rate of reaction graph: -

Draw a reaction which had 2x the reactants

Draw a reaction which had ¼ of the reactants

A
107
Q

Why are catalysts used in industry?

A

Catalysts lower the activation energy reducing the amount of energy needed (and therefore the cost)

They can also be used repeatedly as they are not used up in the reaction

108
Q

What does a catalyst do to a reaction?

A

A catalyst lowers the activation energy needed to start the reaction

Iron – Haber process

Magnesium dioxide – decomposition of hydrogen peroxide

109
Q

What happens to a catalyst at the end of a reaction?

A

Nothing – the catalyst is not used up and can be used again

110
Q

How can the rate of a reaction be measured?

A

Amount of reactant used ÷ time

Or

Product formed ÷ time

111
Q

Give 4 things which can increase the rate of a reaction?

A

Temperature

Concentration / pressure

Surface area

Catalyst addition

112
Q

Why does temperature affect the rate of reaction?

A

Increasing the temperature gives the particles energy – the particles move faster, colliding more often and with more force

113
Q

Why does concentration / pressure affect the rate of reaction?

A

The higher the concentration of a liquid or the higher the pressure of a gas then the higher the chance of a collision = an increased rate of reaction

114
Q

Why does surface area affect the rate of a reaction?

A

The larger the surface area the more exposed particles there are to react

115
Q

How can you increase the surface area of reactants?

A

The surface area can be increased by cutting the object into smaller pieces – powder has a very large surface area

116
Q

What must happen for a reaction to take place?

A

Particles must collide with enough force

117
Q

What is activation energy?

A

The energy needed to start a reaction (minimum energy required by the particles to react)

118
Q

What is an exothermic reaction?

Give an example

A

A reaction which gives out energy (usually heat), e.g. combustion / respiration

119
Q

What is an endothermic reaction?

Give an example

A

A reaction which takes energy in from the surroundings, e.g. photosynthesis uses light energy

120
Q

How can artificial colours be separated?

A

Chromatography (colours split based on ability to dissolve / molecular size)

121
Q

What advantage do machines have at analysing unknown substances?

A

Very sensitive

Very fast

Very accurate

122
Q

What is gas chromatography?

A

Gas chromatography separates out mixtures of compounds allowing the substances present to be identified

123
Q

What is an indicator and what is pH?

A

An indicator is a dye which changes colour

pH (1-14) is a measure of how acid or alkaline a solution is

124
Q

What is electroplating?

A

Electroplating uses electrolysis to coat the surface of one metal with another (e.g. silver onto brass to make it look nice)

125
Q

In electrolysis why is cryolite used?

A

Aluminium oxide is dissolved in molten cryolite (ore of aluminium) lowering the temperature (and therefore the cost)

Negative electrode: Al3+ + 3e- → Al

Positive electrode: 2O2- → O2 + 4e

Additional Science: Chemistry (II) (1 decks)

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