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CCEA GCSE Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Atoms tend to lose or gain electrons to form…?

1 mark

A

A full outer shell.

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2
Q

What is an Ion?

5 marks

A
  • A charged particle.
  • formed (by the transfer of electrons) when atoms gain/lose electrons to form a full outer shell.
  • they are charged because the number of protons is different from the number of electrons.
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3
Q

How are Ions formed?

3 marks

A

By the transfer of Electrons - when atoms gain/lose electrons to form a full outer shell.

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4
Q

Why are Ions charged?

2 marks

A

They are charged because the Number of Protons is different from the Number of Electrons.

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5
Q

What is a Molecular Ion?

2 marks

A

A particle made of more than one atom that has an overall positive or negative charge.

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6
Q

What is a Negative Ion called?

1 mark

A

an Anion

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7
Q

What is a Positive Ion called?

1 mark

A

a Cation

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8
Q

Describe Simple Ions.

2 marks

A

Have full outer shells and the stable Electronic Configuration of the Noble Gases.

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9
Q

Describe a Molecular Ion.

4 marks

A

A particle made of more than one atom that has an overall positive or negative charge.

  • Negative Ion is called an Anion.
  • Positive Ion is called a Cation.
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10
Q

How are negative ions (anions) formed?

5 marks

A

Atoms gain Electrons in their outer shell when they form Negative Ions (anions).

  • These Ions are negative because they contain more Electrons than Protons.
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11
Q

Give an Example of the formation of a Negative Ion (anion).

2 marks

A

An Oxygen atom gains 2 Electrons to form an Oxide Anion.

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12
Q

How are Positive Ions (Cations) formed?

5 marks

A

Atoms lose Electrons from their outer shell when they form Positive Ions (Cations).

These Ions are positive because they contain more Protons than Electrons.

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13
Q

Give an Example of the formation of a Positive Ion (Cation).

(3 marks)

A

A Sodium Atom loses 1 Electron to form a Sodium Cation.

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14
Q

Give (Na) Sodium’s Ion Symbol.

1 mark

A

Na^+

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15
Q

Give (Mg) Magnesium’s Ion Symbol.

1 mark

A

Mg^2+

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16
Q

Give (O2) Oxygen’s Ion Symbol.

1 mark

A

O2^-

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17
Q

Give (Cl) Chlorine’s Ion Symbol.

1 mark

A

Cl^-

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18
Q

What is Sodium’s Group on the Periodic table?

2 marks

A

Group 1: H and Alkali Metals.

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19
Q

What is Magnesium’s Group on the Periodic Table?

2 marks

A

Group 2: Alkaline Earth Metals.

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20
Q

What is Oxygen’s Group on the Periodic Table?

2 marks

A

Group 16: Chalcogens.

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21
Q

What is Chlorine’s Group on the Periodic Table?

2 marks

A

Group 17: Halogens.

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22
Q

When writing the charge on the Ion what should you remember?

(2 marks)

A

Put the number before the positive or negative symbol (2+).

Just write + or – if the charge is 1+ or 1-.

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23
Q

Name 3 Types of Bonding.

3 marks

A
  • Ionic bonding
  • Covalent bonding
  • Metallic bonding
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24
Q

What is Ionic bonding? And where does it occur?

6 marks

A

Ionic bonding occurs in Compounds that contain a Metal (usually a Group 1 or 2 elements)
with a non-metal (usually a Group 6 or 7 element).

  • They bond to form Metal Compounds.
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25
Q

Describe Ionic Bonding.

3 marks

A

Ionic bonding is;

  • a bond between Compounds that contain a Metal and Compounds that contain a Non-Metal
  • to form Metal Compounds.
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26
Q

What happens when forming an Ionic Compound?

6 marks

A

Electrons are transferred from the Metal Atom to the Non-Metal Atom.

  • forming Oppositely-charged Ions.
  • the Metal Ion has a Positive charge.
  • the Non-Metal Ion has a Negative charge.

an Ionic Bond is the attraction between these oppositely-charged ions.

27
Q

What is required to break an Ionic Bond?

2 marks

A

Ionic bonding is strong + requires substantial amounts of energy to break.

28
Q

How can you draw a Dot and Cross diagram for the formation of Ions?
Give each step.

(5 marks)

A
  1. Draw the Electronic Configuration of each Atom – 1 element with dots + 1 with crosses.
  2. Work out how many Electrons need to be transferred.
  3. Draw the Electronic Configuration of the resulting Ions.
  4. Write the charge of each Ion.
29
Q

What are Dot and Cross diagrams useful for?

2 marks

A

They help us to model when Ions are formed from Atoms.

30
Q

What is a Covalent bond?

3 marks

A

A shared pair of Electrons: Formed when 2 atoms share Electrons to obtain a Noble Gas Configuration.

31
Q

What type of Atoms does a Covalent Bond Occur between?

1 mark

A

A Covalent Bond occurs between non-metal atoms.

32
Q

What is required to break a Covalent Bond?

1 mark

A

They are strong and require substantial amounts of energy to break.

33
Q

What is a Molecule?

2 marks

A

A Molecule is 2 or more Atoms Covalently Bonded together.

34
Q

What is a Diatomic Molecule?

2 marks

A

A Diatomic Molecule is 2 Atoms Covalently Bonded together in a Molecule.

35
Q

Give 3 Examples of Diatomic Molecules.

3 marks

A

O2, N2 and Cl2.

36
Q

How can Dot and Cross Diagrams be used for Covalent Bonding?

(1 mark)

A

We can use Dot and Cross Diagrams to show how a pair of Electrons forms a Covalent Bond.

37
Q

What is the Dot and Cross Diagram for Oxygen (O2), a diatomic molecule made up of?

(3 marks)

A
  • 2 Covalent Bonds

- 4 lone pairs of Electrons (2 on each Atom)

38
Q

How many Covalent Bonds and lone pairs of Electrons make up Hydrogen (H2)?

(2 marks)

A

Hydrogen is made up of

  • 1 Covalent Bond
  • 0 lone pairs
39
Q

How many Covalent Bonds and lone pairs of Electrons make up Chlorine (Cl2)?

(3 marks)

A

Chlorine is made up of;

  • 1 Covalent Bond
  • 6 lone pairs (3 on each Chlorine Atom)
40
Q

How many Covalent Bonds and lone pairs of Electrons make up Hydrogen Chloride (HCl)?

(3 marks)

A

Hydrogen Chloride is made up of;

  • 1 Covalent Bond
  • 3 lone pairs (on the Chlorine Atom)
41
Q

How many Covalent Bonds and lone pairs of Electrons make up Water (H2O)?

(4 marks)

A

Water is made up of;

  • 2 Covalent Bonds (1 pair for each H - O Bond)
  • 2 lone pairs (on the Oxygen Atom)
42
Q

How many Covalent Bonds and lone pairs of Electrons make up Ammonia (NH3)?

(4 marks)

A

Ammonia is made up of;

  • 3 Covalent Bonds (1 pair for each N - H Bond)
  • 1 lone pairs (on the Nitrogen Atom)
43
Q

How many Covalent Bonds and lone pairs of Electrons make up Methane (CH4)?

(3 marks)

A

Methane is made up of;

  • 4 Covalent Bonds (1 pair for each C - H Bond)
  • 0 lone pairs
44
Q

What can represent a Covalent Bond?

2 marks

A

A covalent bond can be represented by a line (–) in structural formulae.

45
Q

Name the different kinds of Covalent Bonds.

3 marks

A
  1. A Single Covalent Bond
  2. A Double Covalent Bond
  3. A Triple Covalent Bond
46
Q

Describe a Single Covalent Bond.

2 marks

A

A Single Covalent Bond is when 2 Atoms share a single pair of Electrons.
- Represented by a single line (–).

47
Q

Describe a Double Covalent Bond.

3 marks

A

A Double Covalent Bond is when 2 atoms share 2 pairs of Electrons.
- Represented by a double line (＝).

48
Q

Describe a Triple Covalent Bond.

3 marks

A

A Triple Covalent Bond is when 2 atoms share 3 pairs of Electrons.
- Represented by a triple line (≡).

49
Q

Give Examples of molecules with double and triple covalent bonds.

(10 marks)

A

Oxygen : 2 Oxygen Atoms - 2 Bonds

Nitrogen : 2 Nitrogen Atoms - 3 Bonds

Carbon Dioxide : 2 Oxygen Atoms + 1 Carbon Atom - 4 Bonds

50
Q

How many Covalent Bonds and lone pairs of Electrons make up Nitrogen (N2)?

(3 marks)

A

Nitrogen is made up of;

  • 3 Covalent Bonds
  • 2 lone pairs (1 pair on each Nitrogen Atom)
51
Q

How many Covalent Bonds and lone pairs of Electrons make up Carbon Dioxide (CO2)?

(4 marks)

A

Carbon Dioxide is made up of;

  • 4 Covalent Bonds (2 pairs for each O-C bond)
  • 4 lone pairs (2 pairs on each Oxygen Atom)
52
Q

What is Metallic bonding?

4 marks

A

Metallic Bonding is the attraction between the Positive Ions in a Regular Lattice and the Delocalised Electrons.

  • Delocalised electrons are free to move throughout the whole structure.
53
Q

What are Delocalised Atoms free to do?

1 mark

A

Delocalised electrons are free to move throughout the (whole) structure of an Atom.

54
Q

When drawing a diagram of a Metal’s structure, how should the Ions be drawn?

(1 mark)

A

The Ions should be drawn in regular rows.

55
Q

What is the structural formula for an Oxygen?

2 marks

A

O = O

56
Q

What is the structural formula for Nitrogen?

2 marks

A

N ≡ N

57
Q

What is the structural formula for Carbon Dioxide?

3 marks

A

O = C = O

58
Q

What is the structural formula for Hydrogen?

2 marks

A

H - H

59
Q

What is the structural formula for Chlorine?

2 marks

A

Cl - Cl

60
Q

What is the structural formula for Hydrogen Chloride?

3 marks

A

H - Cl

61
Q

What is the structural formula for Water?

4 marks

A

O
/ \
H H

62
Q

What is the structural formula for Ammonia?

6 marks

A

H - N - H
|
H

63
Q

What is the structural formula for Methane?

4 marks

A 
H
        |
H - C - H
        |
       H

CCEA GCSE Chemistry (7 decks)

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