Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

A-Level Chemistry > 7 - bonding and structure > Flashcards

7 - bonding and structure Flashcards

1
Q

Define ionic bond

A

The electrostatic attraction between 2 oppositely charged ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What do ionic bonds form between?

A

A metal and a non-metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How do you draw dot and cross diagrams for atoms?

A

Draw a circle for the nucleus and put the symbol of the element inside it

Don’t draw any rings

Draw the outer shell without a ring around the nucleus

Draw the electrons as crosses in one atom and as dots around the other element

Put electrons in spin pairs whenever possible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How do you draw ions as dot and cross diagrams and how do you draw their reaction?

A

Draw the metal nucleus with no electrons on the outside (all been taken)

Put square brackets around it and put the charge as a superscript to the brackets

Draw the non-metal nucleus with the outer electrons of the atom as crosses and the added electrons (from the metal) as dots

Put electrons in spin pairs

Put brackets around the non-metal ion etc. as well

If you need more than one of an ion, but a big number before the brackets

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the charge of the ions in each of the groups?

A

Group 1 have +

Group 2 have 2+

Group 13 have 3+ except for boron (a non-metal)

Group 14 doesn’t form ions

Only the non-metals in group 15 form 3-

Only the non-metals in group 16 form 2-

Group 17 have -

Group 18 don’t form ions because they are noble gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Define giant ionic lattice

A

A 3D structure of oppositely charged ions, held together by strong ionic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are the 2 main properties of ionic compounds?

A

Conduct electricity when molten or liquid

High melting and boiling points

Exist as giant ionic lattices

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Why do ionic compounds conduct electricity as liquid or molten?

A

When you melt or boil, you pull apart ionic bonds

Allowing the ions (charged particles) to move and so they can carry a current

As a solid, the ions aren’t free to move so current isn’t carried

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Why do ionic compounds have high melting and boiling points?

A

Very strong electrostatic attractions between oppositely charged ions so a large energy is needed to pull them apart

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What effect does the charges of ions have on the ionic bonds?

A

A bond made by higher charges is harder to overcome

Requires more energy to overcome

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is a polar solvent?

A

A solvent which has slight negative and positive charges

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the most common polar solvent?

A

water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

How are ionic compounds and polar solvents linked?

A

Ionic compounds dissolve in polar solvents

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why do ionic compounds dissolve in polar solvents?

A

The ions of the compound are attracted to the small positive and negative charges of the polar solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are metallic bonds?

A

Strong electrostatic attractions between positive metal ions and delocalised electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is a giant metallic lattice?

A

The 3D structure of positive metal ions and delocalised electrons which are bonded by strong metallic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Where do the delocalised electrons in metals come from?

A

Electrons leave the outer shells of metal atoms so that they are free to move about the structure

The loss of electrons from the metal atoms makes them positive metal ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are the 8 properties of metals?

A

Conduct electricity and heat

Malleable

Ductile

Strong

High melting and boiling points

Sonorous

Shiny

Not soluble in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Why do metals conduct electricity and heat?

A

The free, delocalised electrons can carry the current through the structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What do malleable and ductile mean?

A

Malleable means that it can be compressed without breaking

Ductile means it can be stretched / pulled out without breaking

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Why do metals have high melting and boiling points?

A

The strong metallic bonds require a large amount of energy (and high temperature) to overcome

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What does sonorous mean?

A

It makes a ringing noise when hit

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

define covalent bond

A

What is a covalent bond?

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

When does covalent bonding occur and why?

A

Reactions between 2 non-metals

So that all atoms have a full outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What are the 2 ways of drawing covalent bonds?

A

The symbols for the atoms with lines between them to represent a shared pair

Dot and cross diagrams showing shared pairs between bonded atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is a bonded pair?

A

A pair of electrons which is shared between 2 atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is a lone pair?

A

An outer shell pair of electrons which is not involved in covalent bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is a multiple covalent bond?

A

When there are more than 1 shared pairs of electrons between 2 atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

How are multiple covalent bonds shown in each type of covalent diagram?

A

Multiple lines between atoms for simple diagram

Multiple shared pairs between atoms on dot and cross diagram

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What are dative covalent bonds?

A

A shared pair of electrons which has been provided by one of bonding atoms only

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What do dative covalent bonds usually form between

A

A lone pair is shared between its originator and a H+ ion (proton) usually

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is the other word for dative covalent bond?

A

Coordinate bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

How do you draw dative covalent bonds in dot and cross diagrams?

A

Draw the pair as 2 dots or 2 crosses

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

If there are 2 bonded pairs around a central atom, what shape is formed and what is it called?

A

A linear shape

The electron pairs go on to the opposite sides of the central atom forming a straight line

The bond angle is 180 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What is the shape called when there are 3 bonded pairs and what does it look like?

A

The shape is trigonal planar

The 3 bonds are on a flat plane

120 degrees bond angle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What is the shape for 4 pairs?

A

3D Tetrahedral shape

Bond angle is 109.5 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What is the shape for 6 pairs?

A

Octahedral shape

Bond angle is 90 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

What determines the shape of a molecule?

A

The electron pairs surrounding a central atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Why do the electron pairs surrounding a central atom form the shapes they do?

A

Each electron pair repels other electron pairs

The pairs push apart as much as possible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What is strange about beryllium?

A

Beryllium forms covalent bonds even though it’s a metal

E.g BeCl~2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What is the octet rule?

A

Covalent bonds form so that there are 8 electrons around each atom (in the outer shell)

42
Q

In which cases is there not quite 8 electrons and how many outer electrons are there in these cases?

A

BF~3

The boron has only 6 electrons

BeCl~2

The beryllium only has 4 outer electrons

43
Q

In which cases is there more than 8 electrons in the outer shell? (Expansion of octet rule)

A

SF~6

12 outer electrons to the fluorine

44
Q

What is the average bond enthalpy?

A

A measure of the energy needed to break a given bond

unit: kJ mol^-1

45
Q

When there are 3 bonded pairs and 1 lone pair, what is the 3D shape called?

A

Pyramidal

46
Q

How do you draw pyramidal molecules?

A

The same as tetrahedral but you don’t draw the bond at the top at all

47
Q

The same as tetrahedral but you don’t draw the bond at the top at all

A

For each lone pair in a molecule, the bond angle is reduced by 2.5 degrees from the bond angle if all pairs were bonded

48
Q

What is the bond angle of pyramidal molecules and why?

A

107 degrees

Because tetrahedral molecules have a bond angle of 109.5 degrees

But there is 1 lone pair in a pyramidal molecule

109.5 - 2.5 = 107

So the bond of angle of pyramidal molecules is 107 degrees

49
Q

What is the shape called when there are 2 bonded pairs and 2 lone pairs?

A

Non-linear

50
Q

What is the bond angle of non-linear molecules?

A

104.5 degrees

The same as tetrahedral but there are 2 lone pairs

109.5 - 2.5 - 2.5 = 104.5 degrees

51
Q

How do you draw a non-linear molecule?

A

Draw it like a trigonal planar molecule without one of the bonds

(Even though non-linear is completely unrelated to trigonal planar)

52
Q

What is the shape called if there are 4 bonded pairs and 2 lone pairs?

A

Square planar

53
Q

What is the bond angle of square planar molecules and why?

A

If all pairs were bonded, it would be octahedral with bond angle 90 degrees

In square planar molecules, the lone pairs go to opposite sides of the central atom so the bond angle isn’t affected by them

The bond angle is still 90 degrees for square planar molecules

54
Q

How do you draw a square planar molecule?

A

4 bonds around the central atom each with 90 degrees bond angle

55
Q

How does a multiple bond affect the bond angles?

A

Bond angles aren’t affected

A double bond is treated as a single bonded pair

56
Q

How do dative covalent bonds affect shape?

A

A dative bond is treated as a normal covalent bond

It makes no changes to the bond angle and it is drawn as a normal covalent bond

57
Q

Define electronegativity

A

A measure of the attraction of a given bonded atom to a shared pair of electrons in a covalent bond

58
Q

When is electronegativity at its maximum and why?

A

When the nucleus is as large as possible (more protons means more positive attraction)

When the number of shells is as small as possible (shared pair is closer to nucleus)

59
Q

Where is the electronegativity highest on the periodic table?

A

When the group is highest and when the period is smallest

60
Q

What is the most electronegative element?

A

Flourine

61
Q

What is the significance of 2 bonded atoms having the same electronegativity?

A

The molecule of the 2 atoms is non-polar

There are no dipoles

62
Q

When do 2 atoms have the same electronegativity?

A

only when they are the same element

Or by chance

63
Q

What is the Pauling scale?

A

The scale which measures electronegativity

64
Q

When is a covalent molecule polar and why?

A

When the difference in electronegativity between the bonded atoms is 0.4 or above, the shared pair of electrons will move closer to the more electronegative atom

This gives the more electronegative atom a delta negative charge and the less electronegative atom a delta positive charge

This is what makes the molecule polar

65
Q

What are the 3 bond types on the Pauling scale and what are their electronegativity difference values?

A

Non-polar covalent (less than 0.4 difference between the atoms)

Polar covalent (0.4 to 1.8 difference)

Ionic bonds (1.8 or above)

66
Q

What is the polarity of a C-H bond? You need to remember this

A

Non-polar

Unusual as it seems

67
Q

What happens when a molecule is symmetrical?

A

The small delta charges are in opposite directions so they all cancel out meaning the molecule is non-polar despite the electronegativity differences

68
Q

What is a dipole?

A

A dipole is simply 2 opposite, corresponding delta charges

69
Q

What happens when the molecule is not symmetrical?

A

The dipoles aren’t symmetrical so the molecule is polar (if the electronegativity difference is greater than 0.4)

70
Q

How do lone pairs affect the symmetry and polarity?

A

A lone pair means that the molecule isn’t symmetrical so the molecule will be polar

71
Q

What do we know about polarity if there are lone pairs?

A

If there are polar bonds, the molecule will be asymmetrical and therefore polar

72
Q

What are the 3 types of intermolecular force?

A

Permanent dipole-dipole forces

London forces

Hydrogen bonding

73
Q

When can permanent dipole-dipole forces occur?

A

When the molecules that are going to be held together are all polar

74
Q

Describe how permanent dipole-dipole forces work

A

The polar molecules have opposite delta charges on each side

The positive deltas of each molecule are attracted to the negative deltas of neighbouring molecules and vice versa

75
Q

When do London forces occur?

A

They occur in every substance (between any combination of polar and non-polar molecules)

Only talk about London forces if no other IMFs are present

76
Q

What will London forces sometimes be called?

A

INDUCED dipole-dipole forces

77
Q

Describe how London forces work

A

Because of the fast movement of electrons around atoms

At an instant, the electrons will be on one side of a molecule more than the other

This gives the “more electrons” area a delta - charge and the opposite side a delta + charge

These instantaneous dipoles induce a matching instantaneous dipole in neighbouring molecules

These matching dipoles cause there to be electrostatic attractions between molecules for an instant

These London forces are constantly breaking and forming between different molecules

78
Q

When are London forces stronger and why?

A

When the atoms have more electrons in total because the overall negative charge of the atoms will be greater

The London forces cause LARGER INDUCED DIPOLES

79
Q

What is a hydrogen bond?

A

An attraction between a lone pair of electrons and a delta + hydrogen atom

80
Q

What has to be true for hydrogen bonding to occur?

A

Hydrogen is bonded to something more electronegative (usually N, O or F)

The other element has to have lone pairs

81
Q

What is the order of strength of the different IMFs and why?

A

Hydrogen bonding is strongest due to the greater attraction of lone pairs

Then permanent dipole-dipole forces because the delta attractions are constant

Then London forces are the weakest because the attractions only remain for instants

82
Q

What are the 4 main properties decided by IMFs between covalent molecules?

A

Solubility

Electrical conductivity

Melting point

Boiling point

83
Q

Why is ice less dense than water?

A

The hydrogen bonding in ice holds the water molecules apart in a fixed open lattice

They are held apart so ice is less dense

84
Q

What is the other unusual property of water and why does this happen?

A

It has higher melting and boiling points because hydrogen bonds are stronger than the other IMFs

So more energy is needed to overcome them

85
Q

Why do ionic compounds dissolve in water?

A

Water is polar

So the dipoles of water are attracted to the positive and negative ions in the ionic compound

The water molecules surround the ions so the compound is dissolved

86
Q

What is the structure of simple covalent substances?

A

Covalently bonded molecules held together with IMFs

87
Q

What are the 2 properties of all covalent substances and why?

A

Low melting and boiling points due to weak IMFs

Don’t conduct electricity because there are no charges particles

88
Q

When do covalent substances dissolve?

A

Non-polar covalent substances dissolve in non-polar solvents

Polar covalent substances dissolve in polar solvents

89
Q

What are the 5 giant covalent substances?

A

Diamond

Graphite

Graphene

Silicon

Silicon dioxide

90
Q

What are the melting and boiling points for giant covalent substances?

A

High because strong covalent bonds need to be broken

91
Q

What is the strength for giant covalents?

A

Strong due to strong covalent bonds

92
Q

What are the 2 properties of only graphite and why?

A

It is soft because the separate layers of carbon atoms have weak IMFs between them so they can slide over each other

It can conduct electricity because of the delocalised electrons between its layers

93
Q

What is the structure of graphite?

A

Each carbon covalently bonded to 3 others

Delocalised electrons between layers

94
Q

What is the structure of graphene?

A

A single layer of graphite

Hexagonally arranged atoms

Delocalised electrons above the layer

95
Q

What is the structure of diamond?

A

Each carbon bonded to 4 others

Pyramid sort of shape

96
Q

Which other giant covalent has a similar structure to diamond?

A

Both silicon and silicon dioxide

97
Q

What is the conductivity of giant covalents and why?

A

No charged particles so don’t conduct

Except for graphite

98
Q

What is the solubility like for giant covalents and why?

A

All insoluble

Because strong covalent bonds need to be broken

99
Q

What do you have to remember about the polarity of H~2 S?

A

It doesn’t have dipoles

100
Q

What is the IMF for HCl?

A

Permanent dipole-dipole forces

You have to remember this

101
Q

What is interesting about the lone pairs on carbon?

A

Always no lone pairs

A-Level Chemistry (25 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions