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Chemistry Trilogy > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

How many types of bonding are there?

A

3 - metallic, covalent and ionic

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2
Q

How are ionic bonds formed?

A

Strong electrostatic attraction between positive and negative ions

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3
Q

How are metallic bonds formed?

A

Strong electrostatic attraction between the -ve electrons in the ‘sea of electrons’ and the +ve metal ions

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4
Q

How are covalent bonds formed?

A

Strong electrostatic attraction between the shared - ve electrons and the +ve protons in the nucleus

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5
Q

What do ionic compounds form?

A

Giant lattice structures

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6
Q

What are macromolecules?

A

Giant colvalent structures such as diamond, graphite, graphene and silicon dioxide

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7
Q

What are simple covalent molecules?

A

Small molecules formed from two or more non-metals bonded together e.g. H2, CO2, H2O

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8
Q

How do negative ions form?

A

Non-metals gain electrons

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9
Q

How do positive ions form?

A

Metals lose electrons

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10
Q

How do you work out the charge on a -ve ion?

A

8 - the group number

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11
Q

How do you work out the charge on a +ve ion?

A

The group number

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12
Q

What are dot and cross diagrams?

A

Diagrams to show the movement of electrons between atoms

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13
Q

Name some properties of small covalent molecules?

A

Small molecules are usually gases or liquids that have relatively low melting points and boiling points. These substances have only weak forces between the molecules (intermolecular forces)

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14
Q

Name some properties of macromolecules?

A

Substances that consist of giant covalent structures are solids with very high melting points. All of the atoms in these structures are linked to other atoms by strong covalent bonds

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15
Q

Why do covalent molecules not conduct electricity?

A

Because they do not have charged particles that are free to move (exception is graphite)

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16
Q

What is an alloy?

A

When a metal is mixed with another metal or non-metals such as carbon to alter its properties

17
Q

Why can graphite conduct electricity?

A

Because it has delocalised electrons sitting between the carbon layers. These -ve charged electrons are free to move

18
Q

How can we find the ionic formula of a compound?

A

Use the crossover rule

19
Q

What is a fullerene?

A

The fullerenes are a large class of allotropes of carbon and are made of balls, ‘cages’ or tubes of carbon atoms

20
Q

What is an allotrope?

A

Different structural forms of carbon e.g. graphite, diamond, fullerenes

21
Q

What is the abbreviation for an aqueous Solution?

A

aq

22
Q

What is the state symbol for a gas?

A

g

23
Q

What is the state symbol for a solid?

A

s

24
Q

Covalent bonding is the ……..

A

The attraction between two atoms that share one or more pairs of electrons

25
Q

Ionic bonding is……………………………

A

The electrostatic force of attraction between positively and negatively charged ions

26
Q

What are intermolecular force?

A

The attraction between one MOLECULE and a neighbouring MOLECULE

27
Q

What is the empirical formula?

A

The simplest ratio of elements in a compound

28
Q

What is a mixture?

A

When some elements or compounds are mixed together and intermingle but do not react together (i.e. no new substance is made). A mixture is not a pure substance.

29
Q

Metals conduct electricity because…..

A

They have free electrons that can move.

30
Q

Metals are strong because….

A

They have strong metallic bonds.

31
Q

Metals are malleable and ductile because…..

A

They have layers of atoms that can slide over each other.

32
Q

In covalent molecules, a pair of shared electrons form a ….. bond

A

Single bond

33
Q

In covalent molecules, two pairs of shared electrons form a ….. bond

A

Double bond

34
Q

In covalent molecules, three pairs of shared electrons form a ….. bond

A

Triple bond

35
Q

What are intramolecular forces?

A

Forces between ATOMS in a compound

36
Q

What are the states of matter?

A

Solids, liquids and gases

37
Q

Why are alloys often stronger?

A

Because the layered structure is disrupted and layers can no longer slide over each other

38
Q

A heating curve is a line graph showing the temperature of a substance plotted against the amount of energy it has absorbed. It represents the change of state of matter, typically from a solid to a liquid to a gas.

In a heating curve, what do the flat areas (plateaus) on the graph represent?

A

The flat areas represent a change in state - energy is being used to change state so you see no increase in temperature

39
Q

Is this a graph of a cooling or heating curve?

A

Cooling

Chemistry Trilogy (16 decks)

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