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Chemistry Yr 11 > Properties and Structure of Materials > Flashcards

Properties and Structure of Materials Flashcards

1
Q

Define nanomaterials.

A

Substances that contain particles in the size range of 1-100 nm.
They have specific properties relating to the size of these particles which may differ from those of the bulk material.

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2
Q

Define matter.

A

It has mass and occupies space.

All substances are made up of elements, compounds or mixtures.

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3
Q

Define pure substances.

A

Homogenous matter with a definite fixed composition.

Examples are both elements and compounds.

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4
Q

5 examples of pure substances.

A

Fe, N₂, CO₂, HCl, H₂O

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5
Q

Define elements.

A

Pure substances made entirely of atoms of one element.

Cannot be separated into similar substances by chemical change.

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6
Q

4 examples of elements.

A

Ne, Al, Br₂, S₈

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7
Q

Define compounds.

A

Pure substances composed of two or more different elements chemically combined in fixed proportions.

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8
Q

4 examples of compounds.

A

CO₂, HF, C₆H₁₂O₆, H₂O

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9
Q

Define mixture.

A

A substance that contained 2 or more pure substances.

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10
Q

Define solution.

A

Also called homogeneous mixtures.

A mixture of constant bc imposition and properties throughout.

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11
Q

4 examples of solutions.

A

Air, seawater, stainless steel, smoke

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12
Q

Define heterogeneous mixtures.

A

Mixtures that have variable composition and properties throughout.

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13
Q

3 examples of heterogeneous mixtures.

A

Granite, soil, concrete

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14
Q

Define reactants.

A

Substances that exist before a chemical reaction.

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15
Q

Define products.

A

Substances formed as a result of a chemical reaction.

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16
Q

Define molecules.

A

A group of atoms bonded together, forming a small independent group.
Both elements and compounds exist as molecules.

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17
Q

2 examples of molecules.

A

N₂, CO₂

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18
Q

Define physical properties.

A

Properties of a substance that can be determined without changing the chemical composition.

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19
Q

3 examples of physical properties.

A

Boiling point, odour, colour

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20
Q

Define chemical properties.

A

Properties of a substance that relate to the ability of the substance to form new substances.

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21
Q

3 examples of chemical properties.

A

Ability to react with water, oxygen or acids

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22
Q

Define boiling point.

A

The temperature at which the vapour pressure of a liquid is equal to surrounding atmospheric pressure.

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23
Q

Define melting point.

A

The temperature at which a solid changes state into a liquid

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24
Q

Define hardness.

A

A measure of how resistant solid matter is to various kinds of permanent shape change when a force is applied.

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25
Q

Define solubility.

A

The ability of any substance to dissolve in a solvent to form a homogenous solution.

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26
Q

Define conductivity.

A

A measure of the ability of a substance to conduct an electric current.

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27
Q

Define malleability.

A

The ability of a material to be beaten into a sheet.

Metals tend to be malleable, other materials tend do be brittle.

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28
Q

Define ductility.

A

The ability of a material to be drawn in to a wire.

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29
Q

Define lustre.

A

The ability of a substance to reflect light.

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30
Q

Define density.

A

The mass per unit volume of a substance.

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31
Q

Equation for density.

A

Density = mass ÷ volume
⍴ = m ÷ v
Measured in kg/m³ or kg/L

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32
Q

Define chemical change.

A

Changes in which new substances with different compositions and properties are formed. These are usually irreversible.

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33
Q

2 examples of chemical change.

A

Hydrogen Peroxide decomposing, burning Propane

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34
Q

Define physical change.

A

A change only to physical properties, no change is made to the composition of the substance.

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35
Q

2 examples of physical change.

A

Substances dissolving, substances evaporating

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36
Q

Define filtration and crystallisation

A

Allows mixtures of an insoluble solid to be separated from a soluble solid

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37
Q

What physical property are filtration and crystallisation based on?

A

Solubility

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38
Q

How does filtration and crystallisation work?

A

Mixture added to solvent such as water
Passed through filter paper
Insoluble material retained on filter paper
Soluble material able to pass through

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39
Q

3 examples of filtration and crystallisation.

A

Separating:

Sugar from sand, mud from water, dust from air

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40
Q

What physical property is distillation based on?

A

Differences in the boiling points of the different substances.

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41
Q

How does distillation work?

A

In mixtures of liquids:
Mixture is heated
Liquid with lowest boiling point boils first
Vapour is collected and condensed

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42
Q

2 examples of distillation.

A

Crude oil being separated into fuels, alcohol being distilled

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43
Q

What physical property is chromatography based on?

A

The size of the particle or the degree with which the particle is attracted to the stationary phase.

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44
Q

How does chromatography work?

A

Mixture is passed in a mobile phase through a stationary phase.

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45
Q

Example of chromatography.

A

Separating inks using water rising up through filter paper.

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46
Q

Define decanting.

A

Used to separate mixtures of a liquid and an insoluble solid.

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47
Q

How does decanting work?

A

Liquid is carefully pored from the insoluble sediment at the bottom of the container.
Often separation is incomplete and small amount of solution is left behind in the container.

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48
Q

2 examples of decanting.

A

Decanting:

Wine from sediment, water from a soil solution

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49
Q

Define materials.

A

Pure substances with distinct measurable properties or mixtures with properties dependent on the relative amounts of the substances that make up the mixture.

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50
Q

What are chemical bonds caused by?

A

Electrostatic attractions that arise as a result of the sharing or or transfer between participating ions.

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51
Q

Define valency.

A

The measure of the bonding capacity of an atom.

52
Q

Define ions?

A

Atoms or groups of atoms that are electrically charged due to a loss or gain of electrons.

53
Q

Define octet rule.

A

When other elements react to form bonds, they do so in such a way as to obtain an inert gas electron configuration, that is, achieve the stability by having a full valence shell.

54
Q

Describe metallic bonding.

A

It is non directional bonding.
The electrostatic attraction must be overcome if a metal is to melt/boil.
The more valence electrons, the higher the attraction, therefore higher melting/boiling point

55
Q

Describe ionic bonding.

A

Electrostatic attraction between positive metal ion and negative metal ion.
Attraction must be overcome before melting/boiling can occur.
Large charge can lead to stronger attraction, hence a higher melting/boiling point.

56
Q

Describe covalent bonding.

A

Shared electrons between non-metal atoms.
Attraction is between the positive nuclei on either side if the shared electrons.
Strong intramolecular forces between atoms.
Weak intermolecular forces between molecules therefore low melting/boiling point.

57
Q

Define ionic compound.

A

A substance formed from a cation and an anion.

58
Q

Define simple ion.

A

A single element with a charge.

59
Q

Define cation.

A

A positive ion.

60
Q

Define anion.

A

A negative ion.

61
Q

Define polyatomic ion.

A

More than 1 element in a compound with an overall charge.

62
Q

What are ionic compounds produced by?

A

The combinations of Metal and Ammonium ions with non-metals.

63
Q

What do ionic compounds consist of?

A

Positively charged, metallic ions with negatively charged, non-metallic ions.

64
Q

How are the ions in ionic compounds arranged?

A

In a neutral, crystalline lattice or framework.
Each positive ion is surrounded by a fixed number of negative ions.
Each negative ion is surrounded by a fixed number of positive ions.

65
Q

How are the ions held together in ionic compounds?

A

The ions are in fixed positions.
The positive cations stick to the negative anions by electrostatic forces.
These are called ionic bonds.
Overall charge is 0.

66
Q

Define continuous lattice.

A

When bonding like metallic or ionic continued throughout the whole structure.

67
Q

List the 4 physical properties of ionic substances.

A

Crystalline structure
Rigid or brittle
High melting/boiling point because of strong forces between ions
Conductivity:solids don’t conduct electricity. Substances dissolved in solution and molten substances do conduct electricity

68
Q

Why can molten ionic compounds conduct electricity but solid ionic compounds can’t?

A

Ionic compounds can only conduct electricity if their ions are free to move.

69
Q

Which type of elements tend to form ionic compounds? Why?

A

Metals and non-metals

Metals like to lose electrons, non-metals like to gain electrons

70
Q

How can metallic bonding be modelled?

A

As a regular arrangement of forces of attraction between the nuclei of these atoms and their delocalised elections which are mobile.

71
Q

What can the metallic bonding model be used to explain?

A

The physical properties of metals.

72
Q

Why can covalent bonding be modelled?

A

The sharing of pairs of electrons result in electrostatic forces of attraction between the shared electrons and the nuclei of adjacent atoms.

73
Q

What are the 5 physical properties of metals?

A 
Good conductors of heat and electricity
High melting/boiling point
Malleable and ductile
Lustrous
High density
74
Q

What does a high density mean?

A

Many atoms are tightly packed together

75
Q

What do malleability and ductility indicate?

A

The cations have cushions of electrons so they have a stronger attraction

76
Q

What does high electrical conductivity indicate?

A

The metallic structure has mobile electrons

77
Q

How are the properties of covalent network substances explained?

A

Modelling covalent networks as three-dimensional structures that comprise of covalently bonded atoms.

78
Q

How can the properties of covalent molecular substances be explained?

A

The absence of mobile, charged particles in their molecular structure.

79
Q

Describe the conductivity of covalent structures?

A

When solid or molten they cannot conduct heat or electricity.
Some are able to conduct in aqueous solution (eg HCl)

80
Q

Why are some covalent structures able to conduct heat and electricity in aqueous solution?

A

They can react with water and form ions.

These ions can then carry charge.

81
Q

Describe melting/boiling point of covalent structures.

A

Generally low

82
Q

Why do covalent structures have a generally low melting/boiling point?

A

The forces of attraction between molecules are weak.

83
Q

What physical properties are often found from solids formed from molecules.

A

They are often soft or brittle.

84
Q

How to find the percentage composition.

A

For AwBz
% A in compound = w × relative atomic mass of A over relative formula mass of a compound (molecular) × 100
% B in compound = z × relative atomic mass of B over relative formula mass of a compound (molecular) × 100

85
Q

Define organic chemistry.

A

The study of the many compounds which are based on the element Carbon.

86
Q

What is the name of the two elemental forms of Carbon.

A

Allotropes

87
Q

What are the two elemental forms of Carbon?

A

Diamond and Graphite

88
Q

What molecular shape do single atom Carbon compounds have?

A

Tetrahedral

89
Q

Define Hydrocarbons.

A

An organic compound made of only Carbons and Hydrogen

90
Q

How are Carbohydrates different to Hydrocarbons?

A

Carbohydrates contain C, H and O

91
Q

Define Aliphatic Hydrocarbons.

A

Compounds of Hydrogen and Carbon that form long chains and do not form rings.

92
Q

Define Alicyclic Hydrocarbons.

A

Compounds of Hydrogen and Carbon that contain one or more Carbon rings.

93
Q

Define Aromatic Hydrocarbons.

A

Compounds that contain Benzene as a part of the structure.

94
Q

Define Benzene.

A

A Cyclic Hydrocarbon with the formula C₆H₆

95
Q

What are the 3 main groups that Aliphatic Hydrocarbons can be divided into?

A

Alkanes
Alkenes
Alkynes

96
Q

Define Alkanes.

A

Aliphatic Hydrocarbons that contain only single Carbon to Carbon bonds.

97
Q

Alkanes formula.

A

CnH2n+2

98
Q

Define Alkenes.

A

Aliphatic Hydrocarbons that contain one or more Carbon to Carbon double bonds.

99
Q

Alkenes formula.

A

CH2n

100
Q

Define Alkynes.

A

Aliphatic Hydrocarbons that contain one or more Carbon to Carbon triple bonds.

101
Q

Alkynes formula.

A

CnH2n-2

102
Q

Define Saturated Hydrocarbons.

A

Molecules that only contain single Carbon to Carbon bonds and a maximum amount of Hydrogen atoms bonded to the Carbon atoms present (Alkanes)

103
Q

Define Unsaturated Hydrocarbons.

A

Molecules that contain one or more Carbon to Carbon triple bonds and could hold more Hydrogen atoms (Alkenes and Alkynes)

104
Q

What are the 2 types of reactions that Alkanes undergo?

A

Substitution

Combustion

105
Q

Define Alkane substitution reactions.

A

A reaction between an Alkanes and a Halogen where one or more Hydrogen atoms are substituted by a Halogen atom.

106
Q

General equation for Alkane substitution reactions.

A

UV light

Alkane + Halogen ➝ Halogenated Alkane + Hydrogen Halide

107
Q

Define Alkane combustion reactions.

A

When Alkanes are ignited in the presence of O₂

108
Q

What are the 2 possible reactions that can occur in Alkane combustion reactions?

A

Excess O₂

Limited O₂

109
Q

What does an excess O₂ reaction produce?

A

CO₂ and H₂O

110
Q

What does a limited O₂ reaction produce?

A

CO and H₂O

111
Q

Define structural isomer.

A

A compound with the same molecular formula but different structural formula.

112
Q

What is the prefix cis?

A 
H₃C     CH₃
     \      /
     C=C
     /      \
   H      H
When the Hydrogens are across from each other.
113
Q

What is the prefix trans?

A 
H     CH₃
     \      /
     C=C
     /      \
H₃C      H
When the Hydrogens are diagonal to each other.
114
Q

What are the two reactions that Alkenes can undergo?

A

Combustion (same as Alkanes) and Addition

115
Q

Why are Alkenes more reactive than Alkanes?

A

The double bond can be broken. This frees 2 electrons that allow bonding with other atoms.

116
Q

What is the characteristic reaction for an Alkene?

A

Addition reactions.

117
Q

Define Hydrogenation reactions.

A

Where Alkenes are converted to Alkanes by the double bond breaking and each Carbon atom bonding with a Hydrogen atom.

118
Q

General equation for Hydrogenation reactions.

A

Catalyst

Alkene + H₂ ➝ Alkane

119
Q

Define Halogenated reactions.

A

When a Halogen reacts with an Alkene, Halogen atoms are added across the double bond.

120
Q

Define Markownikoff’s rule.

A

The Hydrogen atom of an acid which reacts with a Hydrocarbon will bond with the Carbon with the most Hydrogens already attached.
You must apply this rule to all Hydrohalogenation and Hydration reactions.

121
Q

Define Hydration reactions.

A

Where water reacts in the presence of concentrated Sulphuric acid as a catalyst to produce alcohol.

122
Q

What are the two reactions Aromatics can undergo?

A

Combustion and substitution

123
Q

What are the tree types of substitution reactions Aromatics can undergo?

A

Halogenation
Nitration
Alkylation

124
Q

Define Halogenation substitution aromatic reactions?

A

Benzene can be halogenated by the addition of a halogen and a suitable catalyst.

125
Q

Define Nitration reactions.

A

Benzene can have a nitro group added by the addition of Nitric acid and Sulphuric acid as a catalyst.

126
Q

Define Alkylation reactions.

A

Benzene can have an alkyl group added by the addition of a chloroalkane in the presence of Aluminium Chloride as a catalyst.

127
Q

Define nomenclature.

A

All Benzene compounds are named ending in Benzene. All other substituted Carbons are numbered with the functional groups labeled for each position they are on.

Chemistry Yr 11 (13 decks)

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