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9- Science > Chemistry 2 > Flashcards

Chemistry 2 Flashcards

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1
Q

What are the three types of strong chemical bond?

A

Ionic, covalent, metallic.

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2
Q

What particles are found in:
Ionic bonding
Covalent bonding
Metallic bonding

A

Ionic bonding oppositely charged ions.

Covalent bonding atoms which share electrons.

Metallic bonding Atoms which share delocalised electrons.

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3
Q

Which type of bonds occurs when metals combine with non-metals?

A

Ionic.

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4
Q

What type of bonding occurs in carbon dioxide? Why?

A

Covalent; two non-metals.

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5
Q

What type of bonding occurs in alloys?

A

Metallic.

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6
Q

What happens to the electrons in ionic bonding?

A

Transferred.

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7
Q

What electronic structure do the ions produced by metals in Groups 1 and 2 and the non-metals in Groups 6 and 7 have?

A

Electronic structure of a noble gas.

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8
Q

What is the link between the charge number on the ions in groups 1, 2 and 3 and their group number ?

A

Charge number is same as Group number.

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9
Q

What is an ionic compound?

A

Giant structure of ions.

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10
Q

How are ionic compounds held together?

A

Strong electrostatic forces of attraction; between oppositely charged ions.

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11
Q

Why is the ball and stick model not an accurate representation of the structure of an ionic compound?

A

Does not accurately depict the millions of ions in the lattice. The ions should touch each other/ there are no gaps between the ions.

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12
Q

How are strong covalent bonds formed?

A

Atoms share pairs of electrons.

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13
Q

What are the three types of structure that can be formed by covalent bonding?

A

Small molecules, very large molecules, giant covalent molecules.

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14
Q

What are polymers an example of?

A

Very large molecules.

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15
Q

What type of structure do the following covalently bonded substances have?

Water H2O

Silicon dioxide SO2

Diamond C

Poly(ethene) .

A

Water H2O Small covalent.

Silicon dioxide SO2 Giant covalent.

Diamond C Giant covalent.

Poly(ethene) Very large molecule.

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16
Q

What are the limitations of using dot and cross diagrams to represent covalent bonds?

A

It shows the electrons differently, when they are the same and it does not show the bond angles or shape of the molecule.

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17
Q

How are atoms arranged in a metal?

A

Giant structures of atoms, arranged in a regular pattern, delocalised electrons.

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18
Q

Why are metallic bonds so strong?

A

Sharing of delocalised electrons.

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19
Q

Describe the arrangement of particles in a metal.

A

Atoms arranged neatly in rows; sea of delocalised electrons.

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20
Q

Why are the particles that make up a metal described as positively charged?

A

The metal atoms lose outer shell electrons and therefore there
are more protons (+) than electrons (−).

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21
Q

What are delocalised electrons?

A

They are free-moving electrons within structure; not associated with a particular atom.

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22
Q

What are the three states of matter?

A

Solid, liquid, gas.

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23
Q

What is used to represent particles in the simple particle model?

A

Small solid spheres.

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24
Q

What takes place at the melting point?

A

Melting and freezing.

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25
Q

What takes place at the boiling point?

A

Boiling and condensing.

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26
Q

What factor affects the amount of energy needed to change state?

A

Forces between molecules.

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27
Q

In chemical equations what symbols are used to show the states of matter?

A 
Solid = (s);
liquid = (l);
gas = (g);
aqueous = (aq)
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28
Q

In what state of matter do particles have the most energy?

A

Gas.

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29
Q

What would eventually happen to a gas if pressure is increased?

A

Condense into a liquid.

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30
Q

Explain the limitations of the particle model.

A

No forces, particles are shown as spheres, spheres are solid.

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31
Q

Describe the structure of ionic compounds.

A

Regular, giant ionic lattice.

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32
Q

Why do ionic compounds have high melting and boiling points?

A

Strong electrostatic forces of attraction between ions.

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33
Q

Why can ionic compounds conduct electricity when melted or dissolved in water?

A

Ions are free to move, carry the charge.

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34
Q

What state of matter are small molecules normally found in?

A

Gas or liquid.

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35
Q

Why do small molecules have low melting and boiling points?

A

Weak forces between molecules/ intermolecular forces.

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36
Q

What happens to the melting and boiling points as small molecules get bigger? Why?

A

Increases, intermolecular forces get bigger.

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37
Q

Why don’t small molecules conduct electricity?

A

Do not have an overall electric charge.

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38
Q

What are polymers?

A

Very large molecules made of repeating units.

39
Q

How are the atoms in a polymer linked together?

A

Strong covalent bonds.

40
Q

Why are polymers normally solid at room temperature?

A

Intermolecular forces relatively strong.

41
Q

Give an example of a giant covalent structure.

A

Diamond, graphite, silicon dioxide.

42
Q

Why do giant covalent structures have very high melting and boiling points?

A

Strong covalent bonds must be broken.

43
Q

Why do most metals have high melting and boiling points?

A

Strong metallic bonding.

44
Q

How are atoms arranged in pure metals?

A

Layers.

45
Q

What is an alloy?

A

Mixture of two elements, one of which is a metal.

46
Q

Why do we use alloys, rather than pure metals, for many uses?

A

They are harder as the layers are distorted.

47
Q

Why are metals good conductors of electricity?

A

Electrical charge carried by delocalised electrons.

48
Q

What is thermal energy?

A

Heat energy.

49
Q

Why are metals good conductors of thermal energy?

A

Energy is transferred by delocalised electrons.

50
Q

In a diamond, how many covalent bonds does each carbon make?

A

4

51
Q

Diamond does not conduct electricity. Why?

A

No delocalised electrons.

52
Q

Name 2 other properties of diamond.

A

Hard, very high melting point.

53
Q

In graphite, how many covalent bonds does each carbon make?

A

3

54
Q

Describe the structure of graphite.

A

Layers of hexagonal rings.

55
Q

Why is graphite soft?

A

Layers can slide over each other, weak forces between layers, no covalent bonds between layers.

56
Q

Why does graphite conduct electricity?

A

Each carbon has one delocalised electron.

57
Q

How is graphite similar to metals?

A

It contains delocalised electrons.

58
Q

What is graphene?

A

Single layer of graphite, 1 atom thick.

59
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes.

60
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene.

61
Q

What are carbon nanotubes?

A

Cylindrical fullerenes.

62
Q

What are carbon nanotubes useful for?

A

Electronics, nanotechnology and materials.

63
Q

What does nanoscience refer to?

A

Structures that are 1-100nm in size, a few hundred atoms.

64
Q

What are nanoparticles?

A

Smaller than fine particles.

65
Q

Why do nanoparticles have different properties from those for the same materials in bulk?

A

They have a high surface area to volume ratio. Smaller quantities are needed to be effective.

66
Q

Name 5 uses of nanoparticles.

A

Medicine, electronics, cosmetics, sunscreens, deodorants, catalysts.

67
Q

What is another name for an electron shell?

A

Orbital

68
Q

What are the most outer electrons called?

A

Valance electrons.

69
Q

Define Ductile.

A

Can be drawn into wires.

70
Q

Define Malleable.

A

Can be hammered into shapes.

71
Q

Fluorine is a non-metal. A fluorine atom has nine electrons. In terms of electrons, what happens when fluorine atoms react?

A

They gain an electron (1) to become a negative ion.

72
Q

Why are the Noble gases unreactive?

A

Very stable due to full outer shells.

73
Q

Explain how the positions of the elements in the periodic table are linked o the electronic structure of their atoms.

A

Atoms in the same group have the same number of electrons in their outer shells/energy levels.

74
Q

What is the trend of reactivity for group 1 elements?

A

the reactivity increases as you go down.

75
Q

What elements are in the halogens or noble gases?

A

Fluorine, chlorine, bromine.

76
Q

List 6 basic facts about Halogens.

A
  1. Halogens are non-metals.
  2. Halogens are found in group 7 of the periodic table.
  3. They react with metals to from IONIC compounds w/ charge of -1.
  4. From molecular compounds with non-metallic elements.
  5. They exist as diatomic molecules.
  6. A more reactive Halogen can replace a less reactive Halogen from an aqueous solution of its salt.
77
Q

As we go down group 7.. what trends increases or decreases?

A 
The reactivity increases. 
The boiling point increases.
The relative molecular mass increases.
The conduction of electricity heat decreases.
The density increases.
78
Q

What is a Mixture?

A

Mixture consists of two or more elements or compounds NOT chemically combined together. The chemical properties of each substance in the mixture are unchanged.

79
Q

What is Chromatography?

A

Chromatography is a physical method of separating a mixture of soluble substances.

80
Q

What is Chromatography used for?

A

Chromatography is a method used by scientists for separating organic and inorganic compounds so that they can be analyzed and studied.

81
Q

Why do the inks separate in chromatography?

A

The separation depends on how soluble the chemical is in the solvent and how strongly the chemical is attracted to the paper.

82
Q

What is the mass number in an element.

A

number of protons=+number of neutrons.

83
Q

Define Solvent.

A

The liquid in which a solute dissolves.

84
Q

Define Solute

A

The substance that dissolves in a liquid to form a solution.

85
Q

Define Solution.

A

It is the mixture formed when a solute has dissolved in a solvent.

86
Q

Define Soluble.

A

Describes a substance that will dissolve.

87
Q

Define Insoluble.

A

It describes a substance that will not dissolve.

88
Q

Why is metal malleable?

A

Positive ions are arranged in regular layers, so if stress is added the layers will be able to move.

89
Q

Why is metal Ductile?

A

It can be stretched to make wires for electrical usage.

90
Q

Why is metal good conductor of heat?

A

It has delocalised electrons which are free to move and collide with other particles, passing energy to each other.

91
Q

Why is metal a good conductor of heat?

A

It has delocalised electrons which carry force. Electrons can move and collide with other particles to carry energy.

92
Q

Why does metal have high melting and high boiling points?

A

It is strong. There is a strong force of attraction between free electrons and metal ions.

93
Q

What is delocalised mean?

A

To move freely.

9- Science (7 decks)

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