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Chemistry - Module 2 > 4) Electrons and Bonding > Flashcards

4) Electrons and Bonding Flashcards

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1
Q

What is the maximum number of electrons in the first shell?

A

2.

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2
Q

What is the maximum number of electrons in the second shell?

A

8.

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3
Q

What is the maximum number of electrons in the third shell?

A

18.

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4
Q

What is the maximum number of electrons in the fourth shell?

A

32.

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5
Q

What is an atomic orbital?

A

A region around the nucleus that can hold up to two electrons, with opposite spins.

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6
Q

Use this card to test knowledge of s- and p- orbitals from ‘Electrons & Bonding’ card.

A

Rate knowledge 1-5.

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7
Q

What is ionic bonding?

A

The electrostatic attraction between positive and negative ions.

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8
Q

What is covalent bonding?

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

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9
Q

What does Average Bond Enthalpy measure?

A

Covalent bond strength.

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10
Q

Describe the structure and bonding shown by magnesium.

A
  • Mg has a giant structure.
  • Mg has metallic bonding with positive ions and delocalised electrons.
  • There is electrostatic attraction between positive ions and electrons.
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11
Q

Describe the structure and bonding shown by chlorine.

A
  • Cl has London forces between molecules.

- London forces are weak.

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12
Q

Describe the bonding and structure in graphite.

A
  • Giant covalent lattice.

- Layered.

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13
Q

Why is graphite a good conductor of electricity?

A

Because it has delocalised electrons which can move.

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14
Q

Why does graphite have a high melting and boiling?

A

Because strong covalent bonds have to be broken.

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15
Q

Why is graphite soft?

A

Because there are weak London forces between the layers and the layers can slide.

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16
Q

Why when ammonium chloride is solid does it not conduct electricity. However, when ammonium chloride is dissolved in water, the resulting solution does conduct electricity?

A
  • Because the ions cannot move in a solid.
  • But the ions can are mobile in solution.
  • And can, therefore, carry the charge.
17
Q

Explain, with the aid of a labelled diagram (use ‘Electrons & Bonding’ card to check diagram), what is meant by the term metallic bonding.

A

-Metallic bonding is the strong electrostatic attraction between delocalised electrons and positive ions.

18
Q

Explain the electrical conductivity of Sodium.

A

Sodium is a good conductor because it has delocalised electrons which are free to move.

19
Q

Explain the electrical conductivity of Sodium Oxide.

A
  • Sodium Oxide does not conduct as a solid as the ions cannot move in a solid.
  • Sodium Oxide conducts when it is a liquid as the ions can move when liquid.
20
Q

What feature of the accepted model of metallic bonding allows metals to conduct electricity?

A

The electrons move.

21
Q

Why does pure water not conduct electricity?

A

Because there are no free charge carriers since water

molecules are uncharged.

22
Q

Sulphuric acid was added to aqueous barium hydroxide. Explain why the electrical conductivity decreased as the sulphuric acid was added.

A
  • The original solution contains mobile ions.

- The charge carriers are removed as reaction takes place.

23
Q

What is the general structure of Sodium Chloride?

A

Has ionic bonds.

24
Q

What is the general structure of graphite?

A

Covalent structure.

25
Q

Explain Sodium Chloride’s poor electrical conductivity in terms of bonding and structure.

A
  • Ions cannot move.

- Ions can only move when molten or in solution.

26
Q

Explain graphite’s good electrical conductivity in terms of bonding and structure.

A
  • Delocalised electrons between layers.

- Electrons conduct electricity.

27
Q

Explain Sodium Chloride’s high melting and boiling point in terms of bonding and structure.

A
  • Bonds are strong.

- Large amount of energy is needed to break bonds.

28
Q

Explain graphite’s high melting and boiling point in terms of bonding and structure.

A
  • Bonds are strong.

- Large amount of energy is needed to break bonds.

29
Q

What is the difference between a covalent bond and a dative covalent bond?

A

In a dative covalent bond, the bonded pair comes from the same atom.

30
Q

At room temperature, X is a liquid which does not conduct electricity. What does this information suggest about the bonding and structure in X?

A

Simple molecular.

31
Q

Why is chlorine is a stronger oxidising agent than iodine?

A

-Chlorine atom is smaller, meaning it has fewer shells

and therefore the electron to be captured will be more attracted.

32
Q

How does ionic bonding hold particles in MgF2 together?

A
  • Electrostatic attraction.

- Between oppositely charged ions.

Chemistry - Module 2 (5 decks)

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