4) Electrons and Bonding Flashcards
What is the maximum number of electrons in the first shell?
2.
What is the maximum number of electrons in the second shell?
8.
What is the maximum number of electrons in the third shell?
18.
What is the maximum number of electrons in the fourth shell?
32.
What is an atomic orbital?
A region around the nucleus that can hold up to two electrons, with opposite spins.
Use this card to test knowledge of s- and p- orbitals from ‘Electrons & Bonding’ card.
Rate knowledge 1-5.
What is ionic bonding?
The electrostatic attraction between positive and negative ions.
What is covalent bonding?
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
What does Average Bond Enthalpy measure?
Covalent bond strength.
Describe the structure and bonding shown by magnesium.
- Mg has a giant structure.
- Mg has metallic bonding with positive ions and delocalised electrons.
- There is electrostatic attraction between positive ions and electrons.
Describe the structure and bonding shown by chlorine.
- Cl has London forces between molecules.
- London forces are weak.
Describe the bonding and structure in graphite.
- Giant covalent lattice.
- Layered.
Why is graphite a good conductor of electricity?
Because it has delocalised electrons which can move.
Why does graphite have a high melting and boiling?
Because strong covalent bonds have to be broken.
Why is graphite soft?
Because there are weak London forces between the layers and the layers can slide.
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?
- Because the ions cannot move in a solid.
- But the ions can are mobile in solution.
- And can, therefore, carry the charge.
Explain, with the aid of a labelled diagram (use ‘Electrons & Bonding’ card to check diagram), what is meant by the term metallic bonding.
-Metallic bonding is the strong electrostatic attraction between delocalised electrons and positive ions.
Explain the electrical conductivity of Sodium.
Sodium is a good conductor because it has delocalised electrons which are free to move.
Explain the electrical conductivity of Sodium Oxide.
- 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.
What feature of the accepted model of metallic bonding allows metals to conduct electricity?
The electrons move.
Why does pure water not conduct electricity?
Because there are no free charge carriers since water
molecules are uncharged.
Sulphuric acid was added to aqueous barium hydroxide. Explain why the electrical conductivity decreased as the sulphuric acid was added.
- The original solution contains mobile ions.
- The charge carriers are removed as reaction takes place.
What is the general structure of Sodium Chloride?
Has ionic bonds.
What is the general structure of graphite?
Covalent structure.
Explain Sodium Chloride’s poor electrical conductivity in terms of bonding and structure.
- Ions cannot move.
- Ions can only move when molten or in solution.
Explain graphite’s good electrical conductivity in terms of bonding and structure.
- Delocalised electrons between layers.
- Electrons conduct electricity.
Explain Sodium Chloride’s high melting and boiling point in terms of bonding and structure.
- Bonds are strong.
- Large amount of energy is needed to break bonds.
Explain graphite’s high melting and boiling point in terms of bonding and structure.
- Bonds are strong.
- Large amount of energy is needed to break bonds.
What is the difference between a covalent bond and a dative covalent bond?
In a dative covalent bond, the bonded pair comes from the same atom.
At room temperature, X is a liquid which does not conduct electricity. What does this information suggest about the bonding and structure in X?
Simple molecular.
Why is chlorine is a stronger oxidising agent than iodine?
-Chlorine atom is smaller, meaning it has fewer shells
and therefore the electron to be captured will be more attracted.
How does ionic bonding hold particles in MgF2 together?
- Electrostatic attraction.
- Between oppositely charged ions.
