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Chemistry GCSE > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

1
Q

In a periodic table, what is a:

  1. Group?
  2. Period?
A
  1. A column

2. A row

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2
Q

What are the three main components of an atom?

A
  1. Protons
  2. Neutrons
  3. Electrons
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3
Q

What is in the nucleus of an atom?

A
  1. Protons

2. Neutrons

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4
Q

What is the formula for the maximum number of electrons that can occupy an atom’s nth shell?

A

Electron capacity = 2n²

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5
Q

What does the group number of an atom tell you?

A

The number of electrons in the outer shell

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6
Q

What does the period number of an atom tell you?

A

The number of shells the atom has

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7
Q

Why do groups have similar properties?

A

They have the same number of electrons in the outer shell

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8
Q

Why are noble gases inert?

A

They have stable electronic arrangements i.e. they have 8 atoms in their outer shell

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9
Q

How can atoms of elements other than noble gases achieve stable electronic structures?

A
  1. Gaining or losing electrons to form ions

2. Sharing electrons to form covalent bonds

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10
Q

How does ionic bonding work?

A

Electrons transfer from metal to non-metal, forming two oppositely charged ions. The ions are held together by strong electrostatic forces

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11
Q

How does electron transfer affect the electronic structure of an ion?

A

The ion has a complete highest energy level, so the electronic structure of an ion is the same as that of a noble gas

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12
Q

What are the four steps of ion formation?

A
  1. Electron transfer
  2. Formation of ions
  3. Electrostatic attraction
  4. Formation of lattice
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13
Q

How is an ionic lattice formed?

A
  1. Oppositely charged ions attract each other
  2. Each ion attracts oppositely charged ions from all directions
  3. Each of these ions attract more ions in turn
  4. A giant ionic structure made up of millions of ions is formed, making a crystal
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14
Q

Ionic bond

A

A strong electrostatic attraction between two oppositely charged ions. Ionic bonds always produce giant ionic structures, and occur only between metals and non-metals

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15
Q

Ionic compounds:

  1. Melting and boiling points
  2. Conductivity as solid
  3. Conductivity when melted
  4. Solubility in water
  5. Conductivity of solution
  6. Type of substances
A
  1. High
  2. Do not conduct
  3. Conducts
  4. Soluble (usually)
  5. Conducts
  6. Metal and non-metal
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16
Q

How do different charges affect the strength of the ionic bond?

A

The bigger the charges, the stronger the bonds. This is because there is a stronger electrostatic attraction between the ions

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17
Q

Covalent bond

A

A chemical bond that involves the sharing of pairs of electrons between atoms. Occurs mainly between non-metal elements

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18
Q

Giant covalent macromolecules

A

Giant lattices of covalent bonds

19
Q

Examples of giant covalent compounds

A
  1. Diamond

2. Graphite

20
Q

Giant covalent compounds:

  1. Melting and boiling points
  2. Conductivity as solid
  3. Conductivity when melted
  4. Solubility in water
  5. Conductivity of solution
  6. Type of substances
A
  1. Very high
  2. Do not conduct (except for graphite)
  3. Do not conduct
  4. Insoluble
  5. Insoluble
  6. Non-metal
21
Q

Why do giant covalent compounds have such high melting points?

A

The covalent bonds between the atoms are very strong, and there are many of them. This means that a lot of energy is needed to separate them

22
Q

Arrangement of atoms in graphite

A
  1. Three covalent bonds to each carbon atom
  2. Weak intermolecular forces between layers
  3. Covalent lattice - lots of strong covalent bonds
23
Q
  1. Why do layers of graphite slide over each other?

2. What is graphite used in as a result of this property?

A
  1. The weak forces between the layers of graphite make them slippery
  2. Lubricant and pencil lead
24
Q
  1. Why does graphite conduct electricity?

2. What is graphite used in as a result of this property?

A
  1. As each carbon atom is only bonded to three others, graphite contains delocalised electrons. These can carry charge
  2. Electrodes
25
Q

Arrangement of atoms in diamonds

A
  1. Four covalent bonds to each carbon atom
  2. Lots of strong covalent bonds
  3. Atoms arranged in a tetrahedral arrangement
26
Q
  1. Why doesn’t diamond conduct electricity?

2. What are diamonds used in as a result of this property?

A
  1. Each carbon atom is bonded to four others, so there are no delocalised electrons to carry charge
  2. Insulating material
27
Q
  1. Why is diamond one of the hardest materials known?

2. What are diamonds used in as a result of this property?

A
  1. Its arrangement means that it has a lot of strong covalent bonds
  2. Cutting tools and drills
28
Q

What are graphite and diamond used in due to their high melting points?

A

Graphite: crucibles to hold molten metal
Diamond: jewellery

29
Q

Simple molecular substances

A

Molecules in which the atoms are joined by covalent bonds, but the molecules themselves have much weaker intermolecular forces between them

30
Q

Simple molecular substances:

  1. Melting and boiling points
  2. Conductivity as solid
  3. Conductivity when melted
  4. Solubility in water
  5. Conductivity of solution
  6. Type of substances
A
  1. Low
  2. Do not conduct
  3. Do not conduct
  4. Insoluble (usually)
  5. Insoluble (usually)
  6. Non-metal
31
Q

What state of matter do simple molecular substances tend to be?

A

Gases, liquids or solids with low boiling points

32
Q

What happens when simple molecular substances are heated?

A

The weak intermolecular forces are overcome - no covalent bonds are broken!

33
Q

Why don’t simple molecular substances conduct electricity?

A
  1. No delocalised electrons

2. No overall charge

34
Q

Differences between ionic and covalent bonds

A
  1. No electron transfer in covalent bonding
  2. The same type of atom can be held together by covalent bonds
  3. No charges involved in covalent compounds
  4. Covalent bonds are usually between two non-metals, while ionic bonds are between metals and non-metals
35
Q

Metallic bond

A

The strong force of attraction between closely packed positive metal ions and a ‘sea’ of delocalised electrons

36
Q

Metallic bonds:

  1. Melting and boiling points
  2. Conductivity as solid
  3. Conductivity when melted
  4. Solubility in water
  5. Conductivity of solution
  6. Type of substances
A
  1. High
  2. Conducts
  3. Conducts
  4. Insoluble
  5. Insoluble
  6. Metal
37
Q

Properties of metallic bonding

A
  1. High melting and boiling points
  2. Conduct electricity
  3. Malleable: easy to bend into shape
  4. Ductile: can be constructed into wires
38
Q

Why do metals have high melting points?

A

There are strong electrostatic forces between the positive ions and negative electrons

39
Q

Why do metals conduct electricity?

A

Delocalised electrons are free to move and pass charges

40
Q

Why are metals malleable and ductile?

A

The layers of atoms are able to move over each other, allowing them to be bent or shaped

41
Q

Oxidation

A

Loss of electrons

42
Q

Reduction

A

Gain of electrons

43
Q

Metal

A

A giant structure of positive ions surrounded by a sea of delocalised electrons

Chemistry GCSE (4 decks)

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