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chemistry > Chemical Changes And Structure #3: Atomic Bonds > Flashcards

Chemical Changes And Structure #3: Atomic Bonds Flashcards

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1
Q

What can atoms be joined together by?

A

Bonds

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2
Q

How is a molecule formed?

A

When two or more atoms join together

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3
Q

What happens when two or more of the same atoms join together?

A

They make a molecule of an element

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4
Q

What are diatomic molecules made up of?

A

Only 2 atoms

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5
Q

How many diatomic elements are there?

A

7

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6
Q

What are the 7 diatomic elements?

A

Oxygen, Fluorine, Chlorine, Nitrogen, Hydrogen, Iodine, Bromine
(Our Friend Claire Needs Her Irn Bru)

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7
Q

Why do atoms bond?

A

To achieve the most stable outer electron arrangement- a full outer shell

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8
Q

What is a covalent bond?

A

Two positive nuclei held together by their common attraction for the shared pair of negative electrons

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9
Q

What are covalent bonds usually formed between?

A

Two non-metal elements

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10
Q

How do you break a covalent bond?

A

You need a LOT of energy as they are very strong forces of attraction

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11
Q

How are double or triple bonds formed?

A

When two or three electrons join another 2 or 3 electrons to pair up

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12
Q

What is an example of chemical formula?

A

HCl or H20

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13
Q

What is an example of full structural formula?

A

H - Cl or H - O - H

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14
Q

How many dimensions do molecules exist in?

A

3

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15
Q

What does the shape of simple covalent molecules depend on?

A

The number and orientation of bonds around the central atom

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16
Q

How can we show the shape of a molecule?

A

By using perspective drawings

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17
Q

What is the perspective of a straight bond?

A

In the plane of the paper (flat)

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18
Q

What is the perspective of a wedge bond?

A

Coming towards you

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19
Q

What is the perspective of a dashed bond?

A

Going away from you

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20
Q

Linear molecules are bonded by…

A

1 straight bond

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21
Q

Angular molecules are bonded by…

A

Bonded by 2 straight bonds

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22
Q

Trigonal Pyramidal molecules are bonded by…

A

One straight, wedged, and dashed

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23
Q

Tetrahedral molecules are bonded by…

A

2 straight, 1 wedge, 1 dashed

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24
Q

How many atoms in a linear molecule?

A

2

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25
Q

How many atoms in an angular molecule?

A

3

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26
Q

How many atoms in a trigonal pyramidal molecule?

A

4

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27
Q

How many atoms in a tetrahedral molecule?

A

5

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28
Q

What do bonding diagrams do?

A

Give a simplified picture of an atom’s outer electron

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29
Q

How do you draw a bonding diagram?

A

Draw the element with its electrons, and have the electron pair(s) interlocking on one of the atom’s branches

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30
Q

What can covalent substances form?

A

Discrete molecular OR giant network substances

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31
Q

Discrete

A

Small or individual

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32
Q

How are covalent molecular structures held together?

A

By very weak forces of attraction (intermolecular) between molecules

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33
Q

What can covalent molecular substances be at room temp?

A

Solids, liquids, or gases

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34
Q

What happens when a covalent molecular compound melts or boils?

A
  • The weak intermolecular forces are broken
  • The strong covalent bonds are left in tact
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35
Q

Less energy required to melt or boil a covalent molecular compound =

A

Low melting and boiling points

36
Q

What are the ONLY type of bonds that covalent networks have?

A
  • covalent
  • NO INTERMOLECULAR BONDS
37
Q

What are covalent network structures held together by?

A

Strong covalent bonds

38
Q

Lots of energy required to break the strong covalent bonds =

A

High melting and boiling points

39
Q

2 Examples of covalent network substances

A
  • Carbon in the form of diamond
  • Silicon Dioxide
40
Q

Why is diamond considered the hardest substance?

A

Because it is a giant network structure held together by many covalent bonds

41
Q

What does the chemical formula or a covalent molecular substance give?

A

The number of atoms present in a molecule

42
Q

What does the formula of a covalent network substance give?

A

The simplest ration of atoms in the substance

43
Q

Example of covalent network formula

A

SiO2, for every silicon there 2 oxygen

44
Q

What is valency? (KEY TERM)

A

The ability of atoms to combine with other atoms

45
Q

What does an atom’s valency depend on?

A

How many out electrons an atom has, and so how many bonds it needs to make to achieve a full outer shell

46
Q

What elements use Roman Numerals to indicate their valency?

A

Transition metals

47
Q

What do Roman numerals indicate in a compound?

A

Indicates which valency is being used

48
Q

Ionic bonding is between….

A

Metals and non-metals (OPPOSITES ATTRACT)

49
Q

What is an ionic bond?

A

The electrostatic force of attraction between positive and negative ions

50
Q

What is an ionic lattice?

A

A giant arrangement on ions held together by electrostatic attraction (aka ionic bonds)

51
Q

Ionic bond is only found in… not…

A

Compounds, elements

52
Q

Elements are only arranged in what structures?

A

Covalent network, Covalent molecular, NOT ionic lattices

53
Q

What do ionic lattices consist of?

A

Millions of ions held together by ionic bonds

54
Q

Why does it require a lot of energy to break ionic lattices?

A

Because of the very strong ionic bonds

55
Q

Example of melting point of ionic lattice?

A

BaCl is 961°C

56
Q

Ionic lattices have very high…

A

Melting and boiling points

57
Q

Ionic compounds are always what?

A

Solid at room temperature

58
Q

What does the formula of an ionic compound give?

A

The simplest ration of ions in the substance

59
Q

What does ionic formulae show?

A

The charge on each of the ions

60
Q

What is the relationship between the group number and the charge in the ion?

A

How many electrons it must gain/lose to achieve a full outer shell

61
Q

What should the ionic formulae always equal to?

A

0, they should cancel eachother out

62
Q

What is a group ion?

A

An ion which gains more than one type of atom, basically a molecule with a charge

63
Q

ions can flow through…

A

Solutions

64
Q

Electrons can flow through…

A

Anything that’s not a solution

65
Q

Why can metals conduct electricity?

A
  • The outer electrons of metal atoms are not attached to a particular atom. They are DELOCALISED
  • Metals can conduct electricity because electrons can flow through them
66
Q

What do the atoms share in a covalent bond?

A

A pair of electrons

67
Q

What effect does the shared pair of electrons have on a covalent bond?

A

This means that the electrons are NOT free to move around and there is so conductivity of electricity

68
Q

Why can’t non-metals conduct?

A

They don’t have charged particles which can move

69
Q

What is the exception to non-metals being non-conductive?

A

Carbon in the form of graphite

70
Q

Why can graphite conduct even though it’s a non-metal?

A
  • It has a layered covalent network structure
  • Each carbon atom only uses 3 electrons for bonding. The remaining electron is DELOCALISED over the whole structure
  • This means that the electrons are free to move between the layers therefore graphite can conduct electricity because electrons flow through it
71
Q

Do covalent compounds (solids, liquids, solutions) conduct?

A

No

72
Q

Why do covalent compounds not conduct?

A

The electrons do not move

73
Q

Ionic compounds do not conduct electricity in what state?

A

Solid

74
Q

When can ionic compounds conduct?

A

When dissolved in water or molten

75
Q

Why do solid ionic compounds not conduct?

A

Because the ions are not free to move in the ionic lattice structure

76
Q

Why can ionic compounds dissolved in water conduct?

A

Because the lattice breaks

77
Q

Why can ionic compounds in the molten state conduct?

A

The melting breaks down the lattice and allows the ions to move

78
Q

What can be said about covalent substances that are insoluble in water?

A

They may dissolve in other substances

79
Q

What don’t covalent network substances do?

A

Conduct

80
Q

Ionic lattice in tact means…

A

No conduction

81
Q

What are many ionic compounds?

A

Soluble in water

82
Q

Why are many ionic compounds soluble in water?

A

As they dissolve, the lattice structure breaks up allowing water molecules to surround the separated ions

83
Q

4 Key facts about covalent molecular

A
  • solids, liquids, or gases at room temp
  • when a covalent molecular compound melts or boils, weak intermolecular forces are broken
  • strong covalent bonds stay in tact
  • less energy to break = low melting + boiling points
84
Q

3 key facts about covalent network

A
  • exist as giant network structures held together by strong covalent bonds
  • lots of energy required to break covalent bonds = high melting + boiling points
  • eg; carbon in the form of diamond, silicon dioxide
85
Q

5 key facts about ionic bonding

A
  • between a metal and non - metal
  • electrostatic force of attraction between positive and negative ions
  • opposites attract
  • ionic bonding is only found in compounds, not elements
  • elements = molecular, network, magnetic etc…

chemistry (7 decks)

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