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Chemistry > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

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1
Q

What are ions?

A

Ions are charged particles that can be single atoms or groups of atoms.

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2
Q

How are ions formed?

A

Ions are formed when atoms lose or gain electrons to achieve a full outer shell.

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3
Q

Which groups of elements are most likely to form ions?

A

Groups 1, 2, 6, and 7 are the most likely to form ions.

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4
Q

What happens when metals form ions?

A

When metals form ions, they lose electrons from their outer shell to form positive ions (cations).

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5
Q

What happens when non-metals form ions?

A

When non-metals form ions, they gain electrons into their outer shell to form negative ions (anions).

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6
Q

How is the charge of an ion determined?

A

The number of electrons lost or gained is the same as the charge on the ion. E.g., if 2 electrons are lost, the charge is 2+.

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7
Q

What do elements in the same group have in common?

A

Elements in the same group have the same number of outer electrons and form ions with the same charges.

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8
Q

What charge do Group I elements form?

A

Group I elements form 1+ ions.

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9
Q

What charge do Group 2 elements form?

A

Group 2 elements form 2+ ions.

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10
Q

What charge do Group 6 elements form?

A

Group 6 elements form 2- ions.

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11
Q

What charge do Group 7 elements form?

A

Group 7 elements form 1- ions.

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12
Q

How does a sodium atom (Na) form an ion?

A

A sodium atom loses 1 electron to form a sodium ion (Na+) with the same electronic structure as neon: Na → Na+ + e.

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13
Q

How does a magnesium atom (Mg) form an ion?

A

A magnesium atom loses 2 electrons to form a magnesium ion (Mg2+) with the same electronic structure as neon: Mg → Mg2+ + 2e.

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14
Q

How does a chlorine atom (Cl) form an ion?

A

A chlorine atom gains 1 electron to form a chloride ion (Cl-) with the same electronic structure as argon: Cl + e → Cl-.

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15
Q

How does an oxygen atom (O) form an ion?

A

An oxygen atom gains 2 electrons to form an oxide ion (O2-) with the same electronic structure as neon: O + 2e → O2-.

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16
Q

What are the three types of bonding?

A

Ionic, covalent, and metallic.

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17
Q

What happens during ionic bonding?

A

A metal atom loses electrons to form a positively charged ion, and a non-metal gains these electrons to form a negatively charged ion.

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18
Q

What is the attraction between oppositely charged ions called?

A

Ionic bond.

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19
Q

What do dot and cross diagrams represent?

A

The arrangement of electrons in an atom or ion, where each electron is represented by a dot or a cross.

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20
Q

How is sodium chloride (NaCl) formed?

A

The sodium atom gives up its outer electron, becoming an Na ion, while the chlorine atom picks up the electron, becoming a Cl ion.

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21
Q

What do the dots and crosses represent in sodium chloride’s dot and cross diagram?

A

Dots represent Na electrons and crosses represent Cl electrons.

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22
Q

How is magnesium oxide (MgO) formed?

A

The magnesium atom gives up its two outer electrons, becoming an Mg2+ ion, and the oxygen atom picks up the electrons, becoming an O2- ion.

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23
Q

How is magnesium chloride (MgCl2) formed?

A

The magnesium atom gives up its two outer electrons, becoming an Mg2+ ion, and two chlorine atoms pick up one electron each, becoming two Cl ions.

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24
Q

How is sodium oxide (Na2O) formed?

A

Two sodium atoms each give up their single outer electron, becoming two Na ions, while the oxygen atom picks up the two electrons, becoming an O2- ion.

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25
Q

What do dot and cross diagrams not show?

A

The structure of the compound, the size of the ions, or how they are arranged.

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26
Q

What is the significance of an atom’s group number in ionic bonding?

A

It helps determine how many electrons an atom will gain or lose.

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27
Q

What structure do ionic compounds have?

A

Ionic compounds have a structure called a giant ionic lattice.

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28
Q

How are ions arranged in an ionic compound?

A

The ions form a closely packed regular lattice arrangement.

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29
Q

What holds the ions together in an ionic lattice?

A

There are very strong electrostatic forces of attraction between oppositely charged ions.

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30
Q

What is a single crystal of sodium chloride?

A

A single crystal of sodium chloride is one giant ionic lattice.

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31
Q

What happens to ionic compounds when they melt?

A

When ionic compounds melt, the ions are free to move and can carry electric charge.

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32
Q

What are the properties of ionic compounds?

A

Ionic compounds have high melting points and high boiling points due to strong bonds between the ions.

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33
Q

What is required to overcome the attraction in ionic compounds?

A

It takes lots of energy to overcome the attraction between the ions.

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34
Q

What happens to ionic compounds when they dissolve in water?

A

The ions separate and are free to move in the solution, allowing them to carry electric charge.

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35
Q

How can you determine the empirical formula of an ionic compound?

A

You can work out the empirical formula from a diagram of the compound by balancing the charges of the ions.

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36
Q

What is the empirical formula for potassium and oxide ions?

A

The empirical formula is K2O.

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37
Q

What is ionic bonding?

A

The electrostatic attraction between oppositely charged ions is ionic bonding.

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38
Q

Why can ionic compounds conduct electricity when molten?

A

The ions are free to move when molten, allowing them to carry electric charge.

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39
Q

What are covalent bonds?

A

Covalent bonds are formed when non-metal atoms share pairs of electrons.

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40
Q

How do covalent bonds form?

A

The positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces.

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41
Q

What do atoms share in covalent bonding?

A

Atoms only share electrons in their outer shells (highest energy levels).

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42
Q

What does each single covalent bond provide?

A

Each single covalent bond provides one extra shared electron for each atom.

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43
Q

Why do atoms make enough covalent bonds?

A

Each atom involved generally makes enough covalent bonds to fill up its outer shell, achieving the electronic structure of a noble gas.

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44
Q

In which compounds does covalent bonding occur?

A

Covalent bonding happens in compounds of non-metals (e.g., H2O) and in non-metal elements (e.g., Cl2).

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45
Q

What are dot and cross diagrams used for?

A

Dot and cross diagrams are used to show the bonding in covalent compounds.

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46
Q

What do the electrons in dot and cross diagrams represent?

A

Electrons drawn in the overlap between the outer orbitals of two atoms are shared between those atoms.

47
Q

What do dot and cross diagrams not show?

A

They don’t show the relative sizes of the atoms, or how the atoms are arranged in space.

48
Q

What does the displayed formula of ammonia (NH3) show?

A

The displayed formula shows the covalent bonds as single lines between atoms.

49
Q

What is the molecular formula of ethane based on its diagram?

A

The molecular formula of ethane is C2H6.

50
Q

What do 3D models of molecules show?

A

3D models show the atoms, the covalent bonds, and their arrangement in space.

51
Q

What is a molecular formula?

A

A molecular formula shows how many atoms of each element are in a molecule.

52
Q

How can you find the molecular formula of a simple molecular compound?

A

By counting up how many atoms of each element there are in any of the diagrams.

53
Q

What is the significance of dot and cross diagrams?

A

They are a great way of showing how atoms are connected in large molecules.

54
Q

What are allotropes of carbon?

A

Allotropes are different structural forms of the same element in the same physical state.

55
Q

What is the structure of diamond?

A

Diamond has a giant covalent structure, made up of carbon atoms that each form four covalent bonds.

56
Q

Why is diamond very hard?

A

The strong covalent bonds in diamond take a lot of energy to break, giving it a very high melting point.

57
Q

Does diamond conduct electricity?

A

No, diamond doesn’t conduct electricity because it has no free electrons or ions.

58
Q

What is the structure of graphite?

A

In graphite, each carbon atom forms three covalent bonds, creating sheets of carbon atoms arranged in hexagons.

59
Q

Why does graphite have a high melting point?

A

Graphite has a high melting point due to the strong covalent bonds within the layers.

60
Q

How does graphite conduct electricity?

A

Graphite conducts electricity because each carbon atom has one delocalised (free) electron that can move.

61
Q

What are the properties of graphite?

A

Graphite is soft and slippery, making it ideal as a lubricating material.

62
Q

What is graphene?

A

Graphene is a sheet of carbon atoms joined together in hexagons, just one atom thick.

63
Q

What are the properties of graphene?

A

Graphene is very strong, incredibly light, and can improve the strength of composite materials without adding much weight.

64
Q

What are fullerenes?

A

Fullerenes are molecules of carbon that can conduct electricity through the whole structure.

65
Q

What shapes can fullerenes form?

A

Fullerenes can form spheres and tubes, shaped like closed tubes or hollow balls.

66
Q

What is the structure of fullerenes?

A

Fullerenes are mainly made up of carbon atoms arranged in hexagons, but can also contain pentagons or heptagons.

67
Q

What are some uses of fullerenes?

A

Fullerenes can ‘cage’ other molecules, be used as industrial catalysts, and make great lubricants.

68
Q

What is Buckminsterfullerene?

A

Buckminsterfullerene was the first fullerene to be discovered.

69
Q

What are nanotubes?

A

Nanotubes are tiny carbon cylinders that can conduct both electricity and thermal energy.

70
Q

What is the tensile strength of nanotubes?

A

Nanotubes have a high tensile strength and do not break when stretched.

71
Q

What is nanotechnology?

A

Nanotechnology is technology that uses very small particles such as nanotubes.

72
Q

What are some applications of nanotubes?

A

Nanotubes can be used in electronics or to strengthen materials without adding much weight, such as in tennis racket frames.

73
Q

What is metallic bonding?

A

Metallic bonding involves delocalised electrons and strong electrostatic forces between positive metal ions and shared negative electrons.

74
Q

What structure do metals consist of?

A

Metals consist of a giant structure where the outer shell electrons are delocalised.

75
Q

Why are most metals solid at room temperature?

A

Most metals are solid at room temperature due to very high melting and boiling points caused by strong metallic bonds.

76
Q

What properties do delocalised electrons produce in metals?

A

Delocalised electrons produce properties such as electrical and thermal conductivity.

77
Q

Why are metals good conductors of electricity and heat?

A

Metals are good conductors because delocalised electrons carry electrical charge and thermal energy through the structure.

78
Q

What does it mean for metals to be malleable?

A

Malleability means that metals can be bent, hammered, or rolled into flat sheets due to the ability of atom layers to slide over each other.

79
Q

Why are alloys harder than pure metals?

A

Alloys are harder because the different sized atoms distort the layers of metal atoms, making it more difficult for them to slide over each other.

80
Q

Why are alloys used instead of pure metals for certain applications?

A

Alloys are used because pure metals are often too soft for certain jobs, and mixing with other metals makes them harder.

81
Q

What is an example of a metallic element?

A

Copper is an example of a metallic element.

82
Q

Why is copper suitable for electrical circuits?

A

Copper is suitable for electrical circuits due to its excellent electrical conductivity.

83
Q

Why is an alloy of copper used for making door hinges?

A

An alloy of copper is used for making door hinges because it is harder and more durable than pure copper.

84
Q

What are the three states of matter?

A

The three states of matter are solid, liquid, and gas.

85
Q

What determines the state of a substance at a certain temperature?

A

The state depends on the strength of the forces of attraction between the particles, which is influenced by the material, temperature, and pressure.

86
Q

Describe the particle arrangement in solids.

A

In solids, particles are held close together in fixed positions, forming a very regular lattice arrangement.

87
Q

What is the movement of particles in solids?

A

Particles in solids vibrate about their positions and do not move from them.

88
Q

How do solids respond to heat?

A

The hotter the solid becomes, the more the particles vibrate, causing solids to expand slightly when heated.

89
Q

Describe the particle arrangement in liquids.

A

In liquids, particles are randomly arranged and free to move past each other, but they tend to stick closely together.

90
Q

What is the movement of particles in liquids?

A

Particles in liquids are constantly moving with random motion.

91
Q

How do liquids respond to heat?

A

The hotter the liquid gets, the faster the particles move, causing liquids to expand slightly when heated.

92
Q

Describe the particle arrangement in gases.

A

In gases, the force of attraction between particles is very weak, allowing them to move freely and be far apart.

93
Q

What is the movement of particles in gases?

A

Particles in gases move constantly with random motion and travel in straight lines.

94
Q

How do gases respond to heat?

A

The hotter the gas gets, the faster the particles move, causing gases to either expand when heated or increase in pressure.

95
Q

What is particle theory?

A

Particle theory is a model used to explain how particles behave in the three states of matter.

96
Q

What are state symbols in chemical equations?

A

State symbols indicate the physical state of reactants and products: (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous.

97
Q

What does ‘aqueous’ mean?

A

‘Aqueous’ means ‘dissolved in water.’

98
Q

What happens to a substance that does not have a definite shape or volume?

A

It is in the gas state.

99
Q

What happens to the particles of a solid when it is heated?

A

The particles gain more energy and vibrate more, weakening the forces that hold the solid together.

100
Q

What is the melting point?

A

The temperature at which particles have enough energy to break free from their positions, turning a solid into a liquid.

101
Q

What is melting?

A

The process where a solid turns into a liquid as particles gain enough energy.

102
Q

What happens to the particles of a liquid when it is heated?

A

The particles gain even more energy, move faster, and weaken the bonds holding the liquid together.

103
Q

What is the boiling point?

A

The temperature at which particles have enough energy to break their bonds, turning a liquid into a gas.

104
Q

What is boiling (or evaporating)?

A

The process where a liquid becomes a gas as particles gain enough energy.

105
Q

What happens at the melting point?

A

So many bonds have formed between the particles that they are held in place, and the liquid becomes a solid. This is called freezing.

106
Q

What happens when a liquid cools?

A

The particles have less energy and move around less.

107
Q

What is condensing?

A

The process where a gas becomes a liquid as bonds form between the gas particles.

108
Q

How does the strength of forces between particles affect melting and boiling points?

A

The stronger the forces, the more energy is needed to break them, resulting in higher melting and boiling points.

109
Q

Which molecular substance is a liquid at room temperature (25 °C)?

A

Bromine, as it melts at -7 °C and boils at 59 °C.

110
Q

What state is ethanol in at 100 °C?

A

Gas, as ethanol boils at 78 °C.

111
Q

What state is ethanol in at 25 °C?

A

Liquid, as it is between its melting point (-114 °C) and boiling point (78 °C).

112
Q

What state is ethanol in at 0 °C?

A

Liquid, as it is above its melting point (-114 °C).

113
Q

What state is ethanol in at -150 °C?

A

Solid, as it is below its melting point (-114 °C).

Chemistry (10 decks)

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