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C2 > Structure And Bonding/Properties (2 topics) > Flashcards

Structure And Bonding/Properties (2 topics) Flashcards

1
Q

What is the Atomic Number?

A

Number of protons (which is the number of electrons

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2
Q

What is the mass number?

A

Atomic number + the number of neutrons

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3
Q

The number of neutrons

A

Mass number - Atomic number

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4
Q

What is the charge for a:
Proton
Neutron
Electron?

A

Positive (+1)
No charge (N/A)
Negative (-1)

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5
Q

Where in the atom are these found:
Proton
Neutron
Electron?

A

Nucleus
Nucleus
Energy Level or electronic shell

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6
Q

What is the relative charge for:
Proton
Neutron
Electron?

A

1
1
1/2000 (massless)

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7
Q

What is an ionic bond?

A

The electrostatic force of attraction between oppositely charged ions that acts in all directions. It involves transferring electrons

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8
Q

In ionic bonding what do atoms have to do to form ions?

A

Lose or gain electrons to gain a full outer shell, for a stable structure

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9
Q

What are ions?

A

Charged particles

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10
Q

Do metals lose or gain electrons in ionic bonding? Do they form positively or negatively charged ions?

A

Lose as they generally have a lower number of electrons in their outer shell than non-metals. They form positively charged ions

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11
Q

What is cation?

A

A positively charged ion

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12
Q

What is anion?

A

A negatively charged ion

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13
Q

What is the (structure) arrangement of the ionic bonds between the charged particles?

A

Giant Structure or Giant Lattice

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14
Q

What is the Giant Lattice like?

A

If we could stand among the ions they would seem to go on in all directions.
The force exerted by an ion acts equally in all directions which is why the structure is held strongly together.
The giant structure is very regular because they lack very neatly together

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15
Q

What is the overall charge in an ionic compound?

A

Zero

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16
Q

Why are the melting points of ionic bonds so high?

A

The electrostatic forces of attraction between oppositely charged ions are very strong so require a lot of energy to break

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17
Q

What is covalent bonding?

A

When non-metals react together their atoms share pairs of electrons to form molecules.

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18
Q

What is a giant covalent structure?

A

Structures where huge numbers of atoms are held together by a network of covalent bond.
They can also be called macromolecules.

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19
Q

Give three examples of giant covalent structures

A

Diamond
Graphite
Silicon Dioxide
Fullerenes

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20
Q

Why do metals form crystals?

A

The atoms in metals are built up layer upon layer in a regular pattern.

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21
Q

What is a compound?

A

This contains two or more different elements which are chemically combined.

22
Q

How do delocalised electrons help in metallic bonding?

A

The outer electrons from each metal atom can easily move throughout the structure. The outer electrons from the energy level form a sea of free electrons surrounding the positively charged metal ions. Strong electrostatic forces of attraction between the oppositely charged ions bond the teal ions to each other. They act a bit like a glue.

23
Q

How can metallic bonding be described?

A

Metals are another example of giant structures, it can be like a lattice of positively charged ions. They are arranged in regular layers.

24
Q

How do giant ionic structures carry an electric charge in molten or liquid?

A

Once enough energy to separate the ions from the lattice has been applied, they are free to move around. That’s when the ionic solid melts and becomes a liquid where the ions are free to move anywhere in. This means they can carry an electric charge

25
Why can't solid giant ionic structures carry an electric charge?
The ions are held in a fixed position in the lattice so can only vibrate not move around.
26
How can solutions of ionic compounds conduct electricity?
The ionic compounds can dissolve in water, and then the lattice is split up by the water molecules. Then the ions are free to move around in the solution formed so can conduct electricity.
27
What type of bond are simple molecules usually?
Covalent bond
28
Why are many substances made of simple molecules liquids or gases at room temperature?
They have low melting and boiling points so don't need as much energy to separate the bonds
29
Why do covalent simple molecules have low melting and boiling points?
The attraction between the individual molecules are relatively small so they have weak intermolecular forces, which means or much energy is needed to overcome these forces.
30
Are covalent bonds strong or weak?
Strong
31
Can simple molecules conduct electricity?
No, because they have no overall charge so they can't carry an electrical charge or conduct electricity
32
What are some special properties of giant covalent structures?
They are held in position by strong covalent bonds so they are very hard, have high melting and boiling points and are insoluble in water.
33
Why is diamond (giant covalent structure) very hard?
All its carbon atoms form four strong covalent bonds.
34
Why is graphite (giant covalent structure) a soft slippery material?
In graphite carbon atoms are only bonded to three other carbon atoms forming hexagons which are arranged in layers. There are no covalent bonds between the layers but only weak intermolecular forces so they slide over each other.
35
How does graphite (giant covalent structure) conduct electricity?
Carbon atoms have four electrons in its outer shell available for bonding. This means that because graphite forms three strong covalent bonds, there is one spare outer electron on each carbon atom. This delocalised electron is free to move along the layers of carbon atoms which means it can act like a metallic structure and conduct electricity.
36
What structures do fullerenes (carbon giant covalent structure) form?
A large cage like structure based on hexagonal rings of carbon atoms.
37
Why can we hammer and bend metals into different shapes and draw them out into wires? (Giant metallic structures)
This is because the layers of atoms in a pure metal are able to slide easily over each other.
38
Why is pure iron soft and easily shaped? (Giant metallic structures)
The atoms are arranged in closely packed layers and because of this regular arrangements the atoms can slide over each other easily.
39
What is an alloy?
A mixture of usually metals.
40
Why are alloys harder than the pure metals used to make them?
In an alloy there are different sizes of atoms so it is more difficult for the layers to slide over each other.
41
How are the positive ions in a metal's giant structure held together?
By a sea of delocalised electrons that act a bit like a glue because of their negative charge being attracted to the positively charged ions. The electrons are able to move throughout the whole giant lattice. The delocalised electrons enable the lattice to distort because of this. When struck the metal atoms can slip past one another without breaking up the metal's structure.
42
Why are metals good conductors of heat and electricity?
Because the delocalised electrons can flow through the giant metallic lattice so the electrical current and heat are transferred quickly through the metal by free electrons.
43
What are shape memory alloys?
These have a special property that alloy them to be bent into different shapes but can return to its original shape on heating
44
What are polymers made from?
Small molecules called monomers
45
What do the properties of polymers depend on?
1. The monomers used to make it 2. The conditions we choose to carry out the reaction: - temperature - pressure - catalyst
46
What is Thermosetting?
These don't melt when heated and have strong covalent bonds forming 'crosslinks' between chains.
47
What is Thermosoftening?
These are polymers that's often easily melted when heated and reset when they cool down. Made of tangles polymer chains
48
What type of bonds do polymer chains have within them?
Strong covalent bonds, between them are weak intermolecular forces.
49
What is nanoscience?
This is the study of small particles compared to normal sized particles, that are between 1 and 100 nanometers in size.
50
NANOSCIENCE IN TEXTBOOK
Read textbook as I haven't done many flash cards

C2 (4 decks)

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