Chapter 3 - Chemistry Flashcards

1
Q

What are the properties of a solid?

A

Each particle in a solid is touching it’s nearest neighbours and they remain in this fixed agreement. They cannot move around but they do vibrate constantly.

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2
Q

What are the properties of a liquid?

A

The particles in a liquid are also very close together but they can move past each other. This results in a constant changing, random arrangement of particles.

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3
Q

What are the properties of a gas?

A

The particles in a gas have much more space between them. They can move around at high speeds in any direction. The hotter the gas is, the faster the particles move.

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4
Q

When does a solid turn into a liquid?

A

At it’s melting point.

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5
Q

When does a liquid turn into a gas?

A

At it’s boiling point.

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6
Q

What does a compound contain?

A

Two or more elements, which are chemically combined.

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7
Q

What happens when non-metals react with metals?

A

The non-metals atoms gain electrons to achieve the stable electronic structure of a noble gas.

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8
Q

How do elements react?

A

Elements react together to form compounds by gaining or losing electrons or by sharing electrons.

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9
Q

What happens when the elements from group 7 and group 1 react?

A

As they react, atoms of group 1 elements can each lose one electron to gain the stable electronic structure of a noble gas. This electron could be given to a group 7 element.

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10
Q

What are ionic compounds held by?

A

Strong forces of attraction between their oppositely charged ions. This is called ionic bonding.

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11
Q

What happens when an ionic compound is dissolved in water?

A

The lattice is split up by the water molecules.

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12
Q

Why do ionic compounds conduct electricity when molten or dissolved in water?

A

This is because their ions can then become mobile and then carry charge through the liquid.

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13
Q

What is covalent bonding?

A

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

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14
Q

How are covalent bonds formed?

A

When atoms of non-metals share pairs of electrons with each other.

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15
Q

What do substances containing covalent bonds consist of?

A

Simple molecules, but some have giant covalent structures

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16
Q

What are polymers made up of?

A

Many small reactive molecules that bond to each other to form long chains.

17
Q

What do substances made up of simple molecules have?

A

Low melting points and boiling points.

18
Q

Why do substances made up of simple molecules have low melting and boiling points?

A

The forces between the simple molecules are now weak.

19
Q

What charge do simple molecules have?

A

They have no overall charge, so they cannot carry electrical charge. Therefore, substances with simple molecules are not conductors of energy.

20
Q

What are models used for?

A

To help understand bonding, but each model has it’s limitations in representing reality.

21
Q

What are giant covalent structures held together by?

A

Covalent bonds throughout the lattice.

22
Q

What are the properties of covalently-bonded structures?

A

These substances have very high boiling and melting points.

23
Q

What does graphite contain?

A

Giant layers of covalently bonded carbon atoms.

24
Q

Why can graphite conduct electricity and thermal energy?

A

This is because of the delocalised electrons that can move along it’s layers.

25
Q

What does carbon (also) exist as?

A

Fullerenes, which can form large cage-like structures and tubes.

26
Q

What is graphene?

A

Graphene is a single layer of graphite and so it is just one atom thick.

27
Q

How are the atoms in metals built up?

A

They are built up as layer on layer in a regular pattern and are closely packed together.

28
Q

What does a metal consist of?

A

A metal consists of positively charged metal ions surrounded by a “sea” of delocalised electrons.

29
Q

What are alloys?

A

An alloy is a mixture of two or more elements, at least one if them is a metal

30
Q

Why can metals be bent or shaped?

A

Because the layer of the atoms (or positively charged atoms) in a giant metallic structure can slide over each other

31
Q

Why are alloys harder than metals?

A

Because the regular layers in a pure metal are distorted by atoms of different sizes in an alloy

32
Q

What do delocalised electrons in metals enable?

A

Electricity and thermal energy to be transferred through a metal easily.