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GCSE CHEMISTRY > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

1
Q

What are the three types of chemical bonds?

A

Ionic, covalent and metallic bonds.

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2
Q

What is an ionic bond?

A

A bond between a metal and non-metal in which electrons have been exchanged.

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3
Q

What is a covalent bond?

A

A bond between two non-metals in which electrons are shared.

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4
Q

What is a metallic bond?

A

A bond between metal atoms in which electrons are delocalised.

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5
Q

How does an ionic compound form?

A

The metal loses electrons to get a full outer shell becoming a positively charged ion while the non-metal gains electrons becoming a negatively charged ion. The oppositely charged ions are electrostatically attracted to each other.

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6
Q

What is the charge of an ion from group 1?

A

1

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7
Q

What is the charge of an ion from group 2?

A

2

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8
Q

What is the charge of an ion from group 6?

A

-2

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9
Q

What is the charge of an ion from group 7?

A

-1

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10
Q

.What is an ionic compound?

A

.A giant structure of ions which are held together by strong electrostatic forces of attraction between oppositely charged ions.

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11
Q

.What are simple molecules?

A

.Small molecules such as oxygen and water that contain atoms joined together by covalent bonds.

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12
Q

.What is the state symbol for a solid?

A

.(s)

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13
Q

.What is the state symbol for a liquid?

A

.(l)

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14
Q

.What is the state symbol for a gas?

A

.(g)

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15
Q

.What is the state symbol for a solution?

A

.(aq)

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16
Q

.What are the properties of ionic compounds?

A

.High melting and boiling point. Don?t conduct electricity when solid but do when molten or dissolved.

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17
Q

.Why do ionic compounds have high melting and boiling points?

A

.Strong bonds between molecules which takes lots of energy to overcome.

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18
Q

.Why can?t ionic compounds conduct electricity when solid?

A

.Ions are unable to move freely.

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19
Q

.Why can ionic compounds conduct electricity when molten or dissolved?

A

.Ions are free and so are able to move.

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20
Q

.What are the properties of simple molecules?

A

.Low melting and boiling point. Poor conductors.

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21
Q

.Why do simple molecules have low melting and boiling points?

A

They have have intermolecular forces which are require less energy to overcome than bonds?

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22
Q

Explain why chlorine and fluorine form covalent bonds

A

They are both non-metals

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23
Q

Complete the sentence: In covalent bonds, electrons are _______________________

A

Shared

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24
Q

In ionic bonds, electrons are ___________________

A

Transferred

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25
What is the name given to the structure of diamond, graphite and silicon dioxide?
Giant covalent
26
How many bonds does each carbon have in diamond?
4
27
Explain why diamond has a high melting point
Giant structure, Strong covalent bonds between the atoms, requires a lot of energy to break
28
Explain why most giant covalent substances do not conduct electricity (3 marks)
There are no electrons/ions/charged particles that are free to move
29
Explain why graphite conducts electricity
Has delocalised electrons between the layers that can move through the graphite
30
Explain why graphite can act as a lubricant
Weak forces between layers which are free to slide over each other
31
What is graphene?
One layer of graphite
32
What is a fullerene?
Substance made of carbon atoms arranged in a cage
33
What type of substance are methane and water?
Simple molecular (or simple molecules)
34
What is a molecule?
A group of atoms chemically bonded together
35
Describe the structure of simple covalent molecules
Strong covalent bonds between atoms, weak forces holding the molecules together
36
What are intermolecular forces?
Weak forces between molecules which hold them together
37
Explain why methane has a low melting point
It is a simple molecular substance with weak forces between the molecules (which are easy to break)
38
What is a polymer?
Millions of small molecules joined together in a chain to form a large molecule
39
Describe the main features of metals in terms of their structure
Positive metal ions arranged in layers with delocalised electrons
40
Explain why metals can conduct electricity
Delocalised electrons are free to carry charge
41
Explain why pure metals are soft
Layers of metal ions are free to slide over each other
42
What is an alloy?
A mixture of two or more elements, at least one of which is a metal
43
Give a reason for alloying a metal
To make it harder, to make it less reactive
44
Explain why alloys can be harder than pure metals
Different size of atoms disturb the layers to stop them sliding over each other
45
What charge do electrons have?
-1
46
What charge will an ion of lithium take?
1+ (one electron in the outer shell, needs to lose it)
47
What charge will an ion of beryllium take?
2+ (two electrons in the outer shell, needs to lose them both)
48
What charge will an ion of barium take?
2+ (group 2 so two electrons in the outer shell, needs to lose them both)
49
What charge will an ion of fluorine take?
1- (7 electrons in the outer shell, needs to gain one)
50
If something has gained electrons, what charge will it have?
Negative
51
If something has lost electrons, what charge will it have?
Positive (because they have lost a negative!)
52
What charge will an ion of oxygen take?
2- (6 electrons in outer shell so needs to gain two)
53
What charge will an ion of Selenium take?
2- (group 6, so has 6 electrons in the outer shell and needs to gain two)
54
Explain in terms of electrons what occurs when lithium bonds with chlorine
One electron transferred from lithium to chlorine
55
Why do atoms transfer electrons in ionic bonding?
So that they can have full outer shells
56
Explain in terms of electrons what occurs when lithium bonds with fluorine
One electron transferred from lithium to fluorine
57
Explain in terms of electrons what occurs when magnesium bonds with oxygen
Two electrons transferred from magnesium to oxygen
58
Explain in terms of electrons what occurs when beryllium bonds with oxygen (3 marks)
Two electrons transferred from beryllium to oxygen
59
Explain in terms of electrons what occurs when magnesium bonds with chlorine
One electron transferred from magnesium to two different chlorine atoms
60
Explain in terms of electrons what occurs when sodium bonds with oxygen
Two electrons transferred to an oxygen atom from two different sodium atoms
61
Why do sodium ions and chlorine ions form an ionic bond?
There is an electrostatic force of attraction between oppositely charged ions
62
Why don't sulphur ions and oxygen ions form ionic bonds with each other?
Both have negative charges so would repel
63
What is the name for a substance made of billions of oppositely charged ions joined together?
Giant ionic lattice
64
Define giant ionic lattice
A huge 3D network of ions
65
State the melting points of ionic substances
High
66
Explain why ionic substances have high melting points.
Strong bonds between oppositely charged ions are hard to break
67
Will NaCl(s) conduct electricity?
No
68
Will NaCl (aq) conduct electricity?
Yes (aq stands for aqueous which means it is dissolved in water)
69
Will NaCl (l) conduct electricity?
Yes
70
What does molten mean?
Melted
71
Explain why ionic compounds do not conduct electricity when solid
Because the ions are not free to move
72
Explain why ionic compounds conduct electricity in solution
Because the ions are free to move
73
Explain why ionic compounds conduct electricity when molten
Because the ions are free to move
74
What does soluble mean?
Dissolves in water
75
What does insoluble mean?
Does not dissolve in water
76
Magnesium carbonate is insoluble. What do you need to do before it will conduct electricity?
Melt it
77
Sodium fluoride is soluble. Explain what the easiest way for it to conduct electricity is
Dissolve it in water because this does not require high temperatures

GCSE CHEMISTRY (4 decks)

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