C3 - Structure and Bonding Flashcards

1
Q

What are the 3 states of matter?

A
  • Solid, liquid and gas.
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2
Q

What are the particles like in a solid?

A
  • Packed closely together.

- Vibrate around fixed positions.

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3
Q

What are the particles like in a liquid?

A
  • Also close together.

- Can slip and slide over each other in random motion.

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4
Q

What are the particles like in a gas?

A
  • Lots of space between them and zoom around randomly.
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5
Q

What happens in melting and boiling in the states of matter?

A
  • Energy is transferred from the surroundings to the substance.
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6
Q

What happens in freezing and condensing in the states of matter?

A
  • Energy is transferred from the substance to the surroundings.
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7
Q

How do elements form to create compounds?

A
  • By gaining or losing electrons or by sharing electrons.
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8
Q

What happens in a reaction between group 1 elements and group 7 elements (halogens)?

A
  • Atoms of group 1 elements can lose one electron to gain the stable electronic structure of a noble gas.
  • The electron can be given to an atom from group.7 which will also now have the electronic structure of a noble gas.
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9
Q

What ions do group 1 form?

A
  • 1+ ions.
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10
Q

What ions do group 2 form?

A
  • 2+ ions.
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11
Q

What ions do group 3 form?

A
  • 3+ ions when they form ions as opposed to sharing electrons.
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12
Q

What ions do group 4 form?

A
  • They do not form ions; however, led and tin form ions at the bottom of the group.
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13
Q

What ions do group 5 form?

A
  • 3- ions when they form ions as opposed to sharing electrons.
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14
Q

What ions do group 6 form?

A
  • 2- ions when they form ions as opposed to sharing electrons.
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15
Q

What ions do group 7 form?

A
  • 1- ions when they form ions as opposed to sharing electrons.
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16
Q

What ions do group 0 form?

A
  • Never form ions in compounds.
17
Q

How are ionic compounds held together?

A
  • Strong forces of attraction between their oppositely charged ions
  • This is called ionic bonding.
18
Q

What ions can form ionic compounds?

A
  • Group 1 and group 7.

- Group 2 and group 6.

19
Q

Features of strong ionic bonds.

A
  • Operate in all different directions holding a giant ionic lattice together, therefore ionic compounds have high melting points; they are all solid at room temperature.
20
Q

Features of ionic compounds.

A
  • Conduct electricity when molten or dissolved in water.; their ions can then become mobil and carry charge through the liquid.
21
Q

What is a covalent bond?

A
  • When non-metals are bonded together.
22
Q

How are covalent bonds formed?

A
  • When atoms of non metals share pairs of electrons together.
  • Each shared pair of electrons is a covalent bond.
23
Q

What do many substances with covalent bonds have?

A
  • Consist of simple molecules but have some giant covalent structures.
24
Q

What are the boiling points of simple molecule substances likely to have?

A
  • Low melting and boiling points.
25
Q

What are the forces of simple molecules like?

A
  • They are weak; the weak intermolecular forces explain why substances made of simple molecules have low melting and boiling points.
26
Q

What is the charge like in simple molecules?

A
  • No overall charge, therefore they cannot carry electrical charge.
  • Substances of simple molecules cannot conduct electricity.
27
Q

Why are models used to show bonding?

A
  • To help the understanding of its bonding but each models has its limitations in representing reality.
28
Q

What are giant covalent structure substances’ boiling points like?

A
  • Very high - melting and boiling points.
29
Q

What are the giant covalent bonds like in graphite?

A
  • Giant layers of covalently bonded carbon atoms.
  • No covalent bonds between the layers.
  • They can slide over each other, making graphite soft and slippery.
  • Carbon atoms in diamond have a rigid giant covalent structure making it a very hard structure.
30
Q

Can graphite conduct electricity?

A
  • Yes.

- Also can conduct thermal energy because of the delocalised electrons that can move along its layers.

31
Q

What are fullerenes?

A
  • As well as diamond and graphite, carbons also exists in fullerenes, which can form large cage-like structures and tubes, based on hexagonal rings of carbon atoms.
32
Q

What are fullerenes being used for?

A
  • Finding uses as a transport mechanism for drugs to specific sites in the body, as catalysts, and as a reinforcement for composite materials.
33
Q

What is graphene and what properties does it possess?

A
  • A single layer of graphite and so is just one atom thick.
  • Its properties: excellent electrical conductivity; will help create new developments in the electronics industry in the future.
34
Q

What are the atoms like in metals?

A
  • Closely packed together and arranged in regular layers.
35
Q

How can you think of metallic bonding?

A
  • Positively charged metal ions held together by electrons from the outermost shell of each metal atom.
  • These delocalised electrons are free to move throughout the giant metal lattice.
36
Q

What are metals like in a giant metallic structure?

A
  • Can be bent or shaped because the layer of atoms (or positively charged ions) can slide over each other.
37
Q

Why are alloys harder than pure metals?

A
  • Regular layers in a pure metal are distorted by atoms of different sizes in an alloy.
38
Q

What delocalised electrons in metals do?

A
  • Enable electricity and thermal energy to be transferred through metal easily.