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Chemistry > 4.2 Bonding Structure And The Properties Of Matter > Flashcards

4.2 Bonding Structure And The Properties Of Matter Flashcards

1
Q

What are the three types of strong chemical bonds

A

Covalent mettalic and ionic

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2
Q

What are the particles in ionic bonding?

A

The particles are oppositely charged ions

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3
Q

What are the particles in covalent bonding?

A

Atoms which share pairs of electrons

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4
Q

What are the particles in metallic bonding?

A

Atoms which share delocalised electrons

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5
Q

When does ionic bonding occur?

A

In compounds formed from metals combined with non metals

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6
Q

When does covalent bonding occur?

A

In most non metallic elements and in compounds of non metals

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7
Q

When does metallic bonding occur?

A

In metallic elements and alloys

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8
Q

What is ionic bonding?

A

The electrostatic force of attraction between positively and negatively charged ions

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9
Q

What is covalent bonding?

A

The attraction between 2 atoms that share one or more pairs of electrons

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10
Q

What 2 elements react to cause ionic bonding?

A

Metals and non metals

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11
Q

Explain how ionic bonding works?

A

When a metal reacts with a non metal atom electrons in the outer shel of the metal atom are transferred

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12
Q

How do metal atoms become positive charged?

A

By losing electrons

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13
Q

How do non metal atoms become negatively charged?

A

By gaining electrons

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14
Q

What do groups 1 2 6 7 have the electronic structure of?

A

Noble gases

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15
Q

How can electron transfer during the formation of an ionic compound be represented by ?

A

A dot and cross diagram

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16
Q

What does the charge of metals and non metals in group 1 2 6 7 relate to?

A

The group number of the element in the periodic table

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17
Q

What is n ionic compound?

A

A giant structure of ions

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18
Q

How are ionic compounds held together?

A

By strong electrostatic forces of attraction between oppositely charged particles

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19
Q

What fo we call the ionic compounds lattice?

A

Giant ionic lattice

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20
Q

Why do ionic compounds have high melting and boiling points?

A

They have a high melting and boiling because a lot of energy is needed to over come the strong electrostatic forces of attraction points

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21
Q

What are some characteristics of ionic compounds?

A

Can conduct electricity when molten or aqueous and has high melting and boiling points

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22
Q

When can ionic compounds conduct electricity and why?

A

When molten or dissolved in water because their ions become free to move when dissolved allowing them to carry an electrical charge

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23
Q

Explain the limitations of using dot and cross diagrams?

A

It shows how the electrons are transferred but not that this is a giant structure and does not show the 3d lattice structure of the ionic compound

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24
Q

What are the limitations of using the 3d diagrams?

A

It is not to scale

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25
What are the limitations of a ball and stick diagram?
Fails at indicating the movement of electrons. The atoms are placed far apart from each other, which in reality is not the case as the gaps between atoms are much smaller.
26
What is a covalent bond ?
The bond between two atoms that share one or more pairs of electrons
27
Are the bonds between atoms in covalent bonds strong or weak?
Strong
28
What do some covalently bonded substances consist of?
Small molecules and others have large molecules such as polymers
29
What do diamond and silicon dioxide have ?
Giant covalent structures
30
What do metals consist of?
Giant structures of atoms arranged in a regular pattern
31
The electrons are delocalised and are free to move through the whole structure in what?
The outer shell of metal atoms
32
What does the sharing of delocalised electrons give to strong metallic bonds ?
The sharing of delocalised electrons gives rise to strong metallic bonds
33
What are the 3 states of matter?
Solid liquid gas
34
When do melting and freezing take place?
At the melting point
35
When do boiling and condensing take place?
At the boiling point
36
What does the amount of energy needed to change state from solid to liquid and from liquid to gas depend on ?
The strength of the forces between the particles of the substance
37
The stronger the forces between the particles the……
Higher the melting point and boiling point of the substance
38
What are the limitations of the simple model to represent the states of matter?
Doesn’t show forces and all particles are represented as spheres and that the spheres are solid
39
What is particle theory?
explains the properties of matter by describing how particles are arranged and move in solids, liquids, and gases
40
Explain the limitations of the particle theory in relation to changes of state?
by showing particles as same sized, inelastic spheres. The model does not show the attraction between the particles which affects the amount of energy needed to change state.
41
What are state symbols for solid liquids and gas and aqueous solution?
S l g aq
42
Why are ionic compounds strong?
They have regular structures ( giant ionic lattices) in which there are strong electrostatic forces of attraction in all direction between oppositely charged ions
43
What are substances that consist of small molecules usually?
Gases or liquids that have relatively low melting points and boiling points
44
Why are the simple molecules of covalent bonds easy to melt?
Because they have weak intermolecular forces between molecules
45
What happens when a simple molecule melts?
The intermolecular forces are overcome not the covalent bonds
46
Wht does The intermolecular forces increase with ?
The size of the molecules
47
Why do larger molecules have higher melting and boiling points ?
Because intermolecular forces increase with the size of the molecules
48
Why don’t simple molecules conduct electricity?
Because they have no overall charge so they can’t carry electrical charge
49
What is a polymer?
A substance made from very large molecules made up of many repeating units
50
What do polymers have?
Very large molecules
51
How are the atoms in the polymer molecules linked to other atoms?
By strong covalent bonds?
52
Why are polymers solid at room temperature?
Because the intermolecular forces between polymer molecules are relatively strong
53
What are substance that consist of giant covalent structures?
Solids with very high melting points
54
How are the atoms in giant covalent structures linked to other atoms ?
By strong covalent bonds
55
What needs to happen to be able to melt giant covalent structures?
The strong covalent bonds must be overcome
56
What are some examples of giant covalent structures ?
Diamond and graphite ( forms of carbon) and silicon dioxide ( silica)
57
Why do most metals have higher melting melting and boiling points?
Because metals have giant structures of atoms with strong metallic bonding which needs a lot of energy to overcome
58
Why can metals be bent and shaped?
Because atoms are are arranged in layers which can slide over each other
59
What is an alloy?
Is a mixture of 2 or more elements at least one of which is a metal
60
What are the properties of alloys?
Less malleable since the atoms are distorted and not in even layers which means it won’t slide over each other . Alloys are much harder since there are different sizes of atoms in the alloy structure disrupt the regular arrangement of atoms, making it more difficult for the layers to slide past each other when force is applied. Can conduct electricity since there are delocalised electrons
61
What are the properties of pure metals?
Good conductors of heat and electricity, malleable and have high melting and boiling points
62
Why are metals good conductors of electricity?
Because the delocalised electrons in the metal array electrical charge through the metal
63
64
Why are metals good conductors of thermal energy?
Because thermal energy is transferred by the delocalised electrons
65
In diamond what does each carbon atom form?
4 covalent bonds with other carbon atoms in a giant covalent structure
66
Why is diamond very hard ?
Because each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure
67
Why does diamond have a very high melting point?
because a large amount of energy is needed to overcome the many strong covalent bonds
68
Why does diamond not conduct electricity?
There are no electrons or other charged particles that are free to move so diamond does not conduct electricity.
69
In graphite what does each carbon atom form?
3 covalent bonds with three other carbon atoms forming layers of hexagonal rings which have no covalent bonds between the layers
70
Why can graphite conduct electricity ?
Because of the delocalised electrons that can move along its layers
71
What are the properties of graphite?
High melting point and insoluble in water
72
Why is graphite insoluble in water?
Attractions between solvent molecules and carbon atoms will never be strong enough to overcome the strong covalent bonds in graphite.
73
What is graphene?
A single layer of graphite and has properties that make it useful in electronics and composites
74
Why does graphene have high melting points and can conduct electricity ?
strong covalent bonds and delocalized electrons
75
What are fullerenes?
Form of the element carbon that can exist as large cage like structures based on hexagonal rings of carbon atoms
76
How many carbon atoms are there in the hexagonal ring in fullerenes?
5 to 7
77
What was the first fullerene to be discovered?
Buckminsterfullerene c60 which has a spherical shape
78
What are carbon nanotubes ?
Cylindrical fullerenes with very high length to diameter ratios
79
What are some uses of fullerenes?
A transport mechanism for drugs to specific sites in the body, as catalysts and as reinforcement for composite materials
80
What are coarse particles often referred to
Dust
81
What are nano particles smaller than?
Fine particles
82
What is nanoscience?
Refers to to structures that are 1-10nm in size of the order of a few hundred atoms
83
As the side of cube decreases by a factor of 10 the…
Surface area to volume ratio increases by a factor of 10
84
1 nanometre = ?
1x 10 to the power of -9
85
Why might nanoparticles have different properties from those for the same material in bulk?
Because of their high surface area to volume ratio
86
Why are smaller quantities of nanoparticles needed?
To be effective than for materials with normal particles sizes
87
What do nanoparticles have many applications in?
Medicine electronics cosmetics and sun creams deodorant and as catalyst

Chemistry (10 decks)

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