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Chemistry > Bonding And Structure And Properties Of Matter > Flashcards

Bonding And Structure And Properties Of Matter Flashcards

(63 cards)

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1
Q

What are ions

A

Electrically charged particles which have a different number of protons and electrons

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2
Q

What are ionic substances made from

A

Metal and non metal

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3
Q

What is the structure of ionic substance

A

Giant lattice

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4
Q

What is a giant lattice structure

A

A massive number of particles in a regular structure that continues in all directions throughout the substance

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5
Q

All ionic substances are what state at room temperature and why

A

Solids because each ion is attracted to all the ions of opposite charge around it and this attraction is very strong

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6
Q

What is the attraction between positive and negative ions called

A

Electrostatic attraction.

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7
Q

Advantage of dot and cross diagram

A

Shows the electronic structure of the ions

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8
Q

Disadvantage of dot and cross diagram

A

Can give the impression that the structure is made of pairs of ions rather than being a continuous structure containing massive number of ions

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9
Q

Advantage of 2D space-filling structure

A

Very easy to draw

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10
Q

Disadvantage for all diagrams presenting ions in a lattice (for dot and cross its pair rather than a few)

A

Can give the impression that the structure is limited to a few ion rather than being a continuous structure with a massive number of ions

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11
Q

Advantage of 3D space-filling structure

A

Gives very good representation of how the ions are packed together

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12
Q

Disadvantage of 2D space filling structure

A

Only shows the structure in 2D

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13
Q

Advantage of Ball and stick structure

A

Helps to show how the ions are arranged relative to each other

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14
Q

Disadvantage of ball and stick structure

A

May make you think the ions are a long way apart or may make you think there are covalent bonds.

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15
Q

4 ways of representing ions in a lattice

A

Dot and cross diagram
2D space-filling structure
3D space-filling structure
Ball and stick structure

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16
Q

What are the melting and boiling points of ionic substances and why

A

High melting and boiling points because the strong attraction between positive and negative ions has is difficult to overcome and requires a lot of energy

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17
Q

What is the electrical conductivity of ionic substances

A

As a solid the ions cannot move so they cannot conduct electricity but when meted the ions can move and carry charge and many ionic substances but not all dissolve in water and if this happens then they will conduct electricity because the ions can mor

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18
Q

What is a molecule

A

Particle made from atoms joined together by covalent bonds

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19
Q

What is a covalent bond

A

Two shared electrons joining atoms together

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20
Q

What are most compounds made from and example

A

A combination of non metals such as glucose

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21
Q

What is the structure of molecular substances

A

A molecular substance is made of many identical molecules that are not joined to each other. Within each molecule, the atoms are joined together by very strong covalent bonds. However, the molecules are not bonded to each other and are held together by intermolecular force

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22
Q

What are intermolecular forces

A

Weak forces between molecules

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23
Q

What are the melting and boiling points of molecular substances and why

A

Low melting and boiling points because the molecules are not bonded to each other and the intermolecular forces are only weak and easy to overcome

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24
Q

What states are most molecular substances at room temperature

A

Gases and liquids

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25
How does melting and boiling points of molecular substances vary
The biggest the molecules the stronger the forces Between them so large molecules such as glucose have higher melting and boiling points
26
Do the covalent bonds break when molecular substances change state
No they do not do water molecules are still identical no water the state just with different intermolecular forces
27
Do molecular substances conduct electricity
Molecules are electrically juwtral which means that molecular substance do not conduct electricity at all as they do not contain delocalised electrons or charges ion. However if there are any ionic substances dissolve in pure water then it can.
28
What is a polymer
Long chain molecule made from joining lots of small molecules together by covalent bonds
29
What is a monomer
The building block of a polymer
30
Whay is the state of polymers at room temperature and why
Solids because the atoms are joined to each other by strong covalent bonds
31
What are polymers sometimes referred to
Macromolecules
32
Examples of giant covalent substances
Diamond Graphite Silicon Silicon dioxide (silica)
33
What is the structure of giant covalent substances
All the atoms are in a giant lattice. They are all joined together by covalent bonds in a continuous network throughout the structure
34
are giant covalent substances molecules
No as in molecular substances there are lots of separate molecules with the atoms in each molecule joined by covalent bonds but the molecules are not joined together
35
Melting and boiling points of giant covalent substances and why
Very high because all the atoms are joined by covalent bonds which are very strong so require a lot of energy to break them
36
Do giant covalent substances conduct electricity
Most do not however graphite does as it has delocalised electrons
37
The structure of metallic substances
Consist of a giant lattice of positively charged atoms arranged in a regular pattern. The outer shell electrons from each atom are delocalised.
38
What is metallic bonding
The strong attraction between the positive nucleus of the atoms and the delocalised electrons
39
Melting and boiling points of metallic substanc s
High because the metallic bonding is strong due to the strong attraction between the positive nucleus of atoms and the delocalised electrons
40
Electrical conductivity of metallic substances
Good conductors because the delocalised electrons are free to move through the structure and carry electrical charge through the metal
41
Thermal conductivity of metals
Good thermal conductors as the delocalised electrons transfer this thermal energy
42
Why is copper used in electrical cables
Because it is an excellent electrical conductor, has a high melting point and can be shaped into wires easily
43
Malleability of metals and why
They are malleable meaning they can be bent and hammered into shape. Because the layers of atoms can slide over each other maintains the metallic bonding. Making them soft.
44
Why are some metals made into alloys
Because pure metals are very malleable and make them too soft for most uses as they lose their shape easily
45
What is an alloy
A mixture of a metal with small amounts of other elements, usually other metals
46
Example of alloy from iron
Steel
47
Why are alloys of gold used in jewellery rather than pure gold
Because pure gold would lose its shape too easily
48
Why are alloys less malleable and harder than metals
They also have metallic structures however some of the atoms in an alloy are a different size to those of the metal. This distorts the layers in the structure and makes it more difficult for the layers of atoms to slide over each other.
49
Structure of the noble gases
They are monatomic and made of many Separate atoms. The atoms are not bonded to each other and there are very weak forces of attraction between the atoms
50
How many carbon atoms is each carbon atom joined to
Four other carbon atoms
51
Where is graphite found
Grey substance that runs through the inside of a pencil and rubs off onto the paper.
52
Structure of graphite
All carbon atoms joined by covalent bongs in a giant lattice with every single one joined with three others and they are bonded together in flat layers. The layers are not bonded to each other and there are only very weak attractive forces between these layers of atoms
53
Why does graphite conduct electricity
Because on each carbon atom the bonding leaves one outer shell electron which is delocalised and free to move along the layers.
54
Is graphite soft
Yes because of layers
55
What is graphene
Single layer of graphite
56
Why is graphene semi see through
Because it is just one atom thick
57
Is graphene strong
It is extremely strong due to giant covalent structure
58
What is graphene used in
Electronics such as touchscreens and composite materials like carbon fibres
59
What are fullerenes
Family of carbon molecules with carbon atoms linked in rings to form a hollow sphere or tube
60
Uses of fullerenes
For delivery of drugs into specific parts of the body In lubricants to reduce friction in machinery as the spherical shape of the molecule allows molecules to roll past each other Catalysts
61
What are carbon nanotubes (buckytubes)
Cylindrical fullerenes also can be thought of as being tubes or graphene sheets
62
What makes carbon nanotubes special
Very high length to diameter ratios
63
Uses of carbon nanotubes
High tensile strengths h High thermal and electrical conductivity Can be used in tennis racquets

Chemistry (9 decks)

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