Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Bonding Structures > Flashcards

Bonding Structures Flashcards

1
Q

What is ionic bonding?

A

The strong electrostatic forces of attraction between oppositely charged ions.

Electrons are transferred from metal to non-metal.

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

What is a molecular ion?

A

A charged particle containing more than one atom.

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

Properties of ionic structures.

A

High melting and boiling points.

Conducts electricity when molten.

Soluble in water.

Brittle.

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

Why do ionic structures have high melting and boiling points?

A

Ionic bonds are strong and a lot of energy needed to break them.

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

Why do ionic structures conduct electricity?

A

When molten, ions are free to move and carry a charge.

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

How is covalent bonding formed?

A

2 non-metal atoms share electrons to obtain a stable electron structure.

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

What is a molecule?

A

Two or more atoms covalently bonded.

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

What are diatomic molecules?

A

Contain 2 atoms of same element covalently bonded together.

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

Properties of simple covalent molecules.

A

Low melting and boiling points - although strong covalent bonds within molecules, weak Van der Vaals forces between molecules.
Do not conduct electricity as have no charges or free electrons.
Low solubility.

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

What are allotropes?

A

Different forms of same element in same physical state.

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

Explain the structure of diamond.

A

Each carbon atom covalently bonded to 4 others in tetrahedral 3-dimensional structure.

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

Properties of diamond.

A

High melting and boiling points - many covalent bonds strong and need a lot of energy to break.
Does not conduct electricity as no free ions to move and carry charge.
Hard due to shape and strong bonds.

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

What are the uses of diamond?

A

Used in cutting tools to turn through hard rock, metals and glass.

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

Explain the structure of graphite.

A

Layers of carbon atoms arranged in hexagons, covalent bonds between atoms and weak Van der Vaals forces between layers. 3-dimensional with each carbon atom bonded to 3 others.

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

Properties of graphite.

A

High melting and boiling points - covalent bonds strong and need a lot of energy to break.
Conducts electricity as 1 electron free to move due to not being in bonds and carries a charge.
Soft because forces between layers are weak, layers can slide.

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

What are the uses of graphite?

A

Used as lubricants for machinery and in pencil leads.

17
Q

Explain the structure of graphene.

A

Single-atom thick layer of graphite with strong covalent bonds between each carbon atom. Atoms are arranged in hexagons, 2-dimensional.

18
Q

Properties of graphene.

A

High melting and boiling points - covalent bonds strong and need a lot of energy to break them.
Good conductor of electricity as 1 electron per carbon atom unbonded so is free to move and carry charge.
Very strong due to strong covalent bonds in the layer.

19
Q

What are the uses of graphene?

A

Used in solar cells and batteries.

20
Q

What is metallic bonding?

A

Electrostatic attraction between positive metal ions and sea of delocalised electrons.

21
Q

Properties of metallic bonding.

A

High melting point - strong attraction between positively charged metal ions and sea of electrons, large amount of energy needed to break bonds.
Conducts heat and electricity -delocalised electrons able to move and carry charge.
Strong, malleable and ductile - layers of metal ions bale to slide over each other, without disrupting bonding.

22
Q

What is an alloy?

A

Mixture of at least 2 elements, one of which is a metal.
Resulting material has metallic properties.

23
Q

Why are alloys stronger than metals?

A

Different sized atoms distort layers in pure metal. Greater force required for layers to slide over each other. Alloy is harder and stronger than pure metal.

24
Q

What is the method for the flame test?

A
  1. Drip nichrome wire into concentrated hydrochloric acid.
  2. Drip wire into rest solid.
  3. Place nichrome wire in blue bunsen flame p.
  4. Note colour of flame.
25
Q

What are the results for the flame test?

A

Lithium - crimson red
Sodium - orange
Calcium - brick red
Potassium - lilac
Copper - blue-green

Chemistry (9 decks)

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