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Chemistry AS > Bonding > Flashcards

Bonding Flashcards

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1
Q

What are Ionic Compounds?

A

Oppositely charged ions which are held together by electrostatic attractions.

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2
Q

What ion does group one from?

A

1+ ions.

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3
Q

What ion does group two form?

A

2+ ions.

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4
Q

What ion does group three form?

A

3+ ions.

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5
Q

What ion does group five form?

A

3- ions.

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6
Q

What ion does group six form?

A

2- ions.

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7
Q

What ion does group seven form?

A

1- ions.

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8
Q

What is the molecular formula for hydroxide?

A

OH-

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9
Q

What is the molecular formula for nitrate?

A

NO3-

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10
Q

What is the molecular formula for ammonium?

A

NH4+

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11
Q

What is the molecular formula for sulfate?

A

SO4 ^2-

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12
Q

What is the molecular formula for carbonate?

A

CO3 ^2-

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13
Q

What type of elements does ionic bonds occur between?

A

A metal and a non-metal.

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14
Q

What is always the overall charge of an ionic bond?

A

Zero.

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15
Q

Can ionic compounds conduct electricity?

A

Only when they are molten or dissolved in a solution.

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16
Q

Are the melting points of ionic compounds high or low and why?

A

High as there are many, strong electrostatic forces between oppositely charged ions. There is a lot of energy needed to overcome these forces.

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17
Q

Do most ionic compounds dissolve in water and why?

A

Yes because water molecules are polar and can attract the positive and negative ions and break up the structure.

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18
Q

What is covalent bonding?

A

The sharing of outer electrons in order for atoms to obtain a full shell.

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19
Q

Where is the electrostatic attraction in covalent bonding?

A

Between the shared electrons and the positive nucleus.

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20
Q

What is a dative or coordinate bond?

A

Where one atom donates two electrons to an atom or ion to form a bond.

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21
Q

What type of elements does covalent bonding occur between?

A

Two non-metals.

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22
Q

How is a covalent bond indicated?

A

With a line.

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23
Q

How is a dative covalent bond indicated?

A

Using an arrow from the lone electron pair.

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24
Q

What are two examples of giant covalent structures?

A

Graphite and Diamond.

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25
Q

Describe the structure and properties of graphite.

A

Each carbon is bonded three times and the fourth electron is delocalised.
There are lots of strong delocalised bonds causing it to have a very high melting point.
It is made up of hexagons.
The layers slide easily.
Able to conduct electricity.

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26
Q

What causes graphite to have a very high melting point?

A

It has lots of strong covalent bonds.

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27
Q

What makes the layers in graphite slide easily?

A

There are weak forces between the layers.

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28
Q

What allows graphite to conduct electricity?

A

Delocalised electrons between the layers as they can carry a charge.

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29
Q

What causes a low density in graphite?

A

It’s layers are far apart in comparison to covalent bond length.

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30
Q

Why is graphite insoluble?

A

The covalent bonds are too strong to break.

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31
Q

What shape is diamond?

A

A tetrahedral shape, created by each carbon bonding four times.

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32
Q

What allows diamond to conduct heat well?

A

It has a tightly packed and rigid arrangement.

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33
Q

What gives diamond a very high melting point?

A

The many strong boiling points as well as it being very hard.

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34
Q

Why doesn’t diamond conduct electricity well?

A

It does not have any delocalised electrons.

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35
Q

Why is diamond insoluble?

A

It’s covalent bonds are too strong to break.

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36
Q

What is they key rule of shapes of molecules?

A

Use the number of bond pairs and lone pairs of electrons to work out the shape of the molecule.

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37
Q

Why do molecules have a specific shape with a specific angle?

A

This is because bonds repel each other equally as they contain electrons which will want to be as far apart as possible.

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38
Q

What happens if a lone pair is next to bond pairs?

A

It will repel further than two bonds together.

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39
Q

What is the general rule for lone pairs reducing angles?

A

The bond angles reduce by 2.5 degrees.

40
Q

What is the name of the shape if it has 2 bond pairs and 0 lone pairs?

A

Linear.

41
Q

What is the name of the shape if it has 3 bond pairs and 0 lone pairs?

A

Trigonal Planar.

42
Q

What is the name of the shape if it has 4 bond pairs and 0 lone pairs?

A

Tetrahedral.

43
Q

What is the name of the shape if it has 5 bond pairs and 0 lone pairs?

A

Trigonal Bipyramidal.

44
Q

What is the name of the shape if it has 6 bond pairs and 0 lone pairs?

A

Octahedral.

45
Q

What are the bond angles in a linear molecule?

A

180 degrees.

46
Q

What are the bond angles in a trigonal planar molecule with 0 lone pairs?

A

120 degrees.

47
Q

What are the bond angles in a tetrahedral molecule with 0 lone pairs?

A

109.5 degrees.

48
Q

What are the bond angles in a trigonal bipyramidal with 0 lone pairs?

A

90 degrees and 120 degrees.

49
Q

What are the bond angles in a octahedral molecule with 0 lone pairs?

A

90 degrees.

50
Q

What is the name of the shape if it has 3 bond pairs and 1 lone pair?

A

Pyramidal.

51
Q

What is the name of the shape if it has 2 bond pairs and 2 lone pairs?

A

Bent.

52
Q

What is the name of the shape if it has 3 bond pairs and 2 lone pairs?

A

Trigonal Planar.

53
Q

What is the name of the shape if it has 4 bond pairs and 2 lone pairs?

A

Square planar.

54
Q

What are the bond angles in a pyramidal molecule with 1 lone pair?

A

107 degrees.

55
Q

What are the bond angles in a bent molecule with 2 lone pairs?

A

104.5 degrees.

56
Q

What are the bond angles in a trigonal planar molecule with 2 lone pairs?

A

120 degrees.

57
Q

What are the bond angles in a square planar molecule with 2 lone pairs?

A

90 degrees.

58
Q

Why does the bond angle in trigonal and square planars not change when there are two lone pairs?

A

As the lone pairs repel equally from opposite sides.

59
Q

What is meant by electronegativity?

A

The ability for an atom to attract electrons towards itself in a covalent bond.

60
Q

What is the rule in increasing electronegativity?

A

The further up and right you go the more electronegative and element is excluding the noble gases.

61
Q

What does the Pauling scale show?

A

How to quantify how electronegative an element is.

62
Q

How can covalent bonds become polar?

A

If the atoms attached to it have a difference in electronegativity.

63
Q

What does an increase in the difference in electronegativity in a bond cause?

A

An increase in how polar the bond is.

64
Q

What two symbols show polarity?

A

Delta positive and delta negative.

65
Q

Which side of a bond do we put the delta negative symbol if it is polar?

A

Next to the least electronegative.

66
Q

Which side of a bond do we put the delta positive symbol if it is polar?

A

Next to the most electronegative.

67
Q

Are hydrocarbons classed as polar or non-polar?

A

Non-polar.

68
Q

What does an uneven distribution of charges lead to?

A

Polar Molecules.

69
Q

If a polar bond is arranged symmetrically what is the overall polarity?

A

Zero.

70
Q

What are Van der Waals forces also known as?

A

Induced dipole-dipole forces.

71
Q

What is Van der Waals forces also known as?

A

Induced dipole dipole forces.

72
Q

What do Van der Waals forces occur between?

A

Atoms and molecules.

73
Q

What are the three key types of intermolecular forces?

A

Hydrogen bonding,
Permanent dipole-dipole and
Van der Waals.

74
Q

What is the weakest type of intermolecular forces?

A

Van der Waals.

75
Q

What is the strongest type of intermolecular forces?

A

Hydrogen bonding.

76
Q

How can any atom or molecule with electrons form a dipole?

A

By moving near to another atom or molecule, this occurs as electrons in a molecule or atom can move from one end to another creating a temporary dipole.

77
Q

What structure can Van der Waals forces hold some molecules in?

A

Crystal structures.

78
Q

What increases the strength of Van der Waals forces?

A

An increase in the size of the molecule or atom as you have larger electron clouds.

79
Q

What are we breaking down when we boil a liquid?

A

Van der Waals forces.

80
Q

Why do longer, straight chains of hydrocarbons have a higher boiling point?

A

As they have more Van der Waals forces and this requires more energy to be able to overcome these forces.

81
Q

Why do branched hydrocarbons have lower boiling points?

A

They can’t pack close together which weakens the Van der Waals forces between the chains.

82
Q

Where do permanent dipole-dipole interactions exist?

A

In molecules with polarity.

83
Q

If a molecule has dipole-dipole forces what other force does it also have?

A

Van der Waals forces.

84
Q

When does hydrogen bonding occur?

A

When you have very electronegative elements.

85
Q

What are the three most electronegative elements which are also the only three elements which hydrogen bond?

A

Nitrogen, Oxygen and Fluorine.

86
Q

How do you show hydrogen bonds?

A

Use dotted lines between lone pairs and hydrogen.

87
Q

If a molecule has hydrogen bonding what other intermolecular forces does it also always have?

A

Van der Waals and Dipole-Dipole.

88
Q

What is formed in metallic bonding?

A

Giant lattice structures which have positive metal ions as they donate electrons to form a sea of delocalised electrons.

89
Q

Why does magnesium have a higher boiling point than sodium?

A

It can donate more electrons than sodium as the more electrons an atom can donate to the delocalised system, the higher the melting point.

90
Q

Why are metals good thermal conductors?

A

The delocalised electrons can transfer kinetic energy.

91
Q

Why are metals good electrical conductors?

A

The delocalised electrons are mobile and can carry a current.

92
Q

Pent - 1 - ene is formed by the elimination of water from pentan - 2 - ol. State the reagent and conditions for this reaction.

A

The reagent is concentrated sulfuric acid and the conditions must be hot.

93
Q

Na+ and F- have the same electron configuration, explain why a fluroride ion is larger than a sodium ion.

A

The fluoride ion has fewer protons and a lower nuclear charge. There is a weaker attraction between the nucleus and the outer electrons.

94
Q

Why is the melting point of sodium fluoride high? Explain in terms of structure and bonding.

A

There are electrostatic forces of attraction between the oppositely charged ions. Therefore a lot of energy is needed to overcome forces.

95
Q
A

Chemistry AS (16 decks)

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