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OCR A-Level Chemistry: Chapter 5 - Electrons and Bonding Part 2

Chemistry23 CardsCreated 2 months ago

A flashcard deck covering important concepts from Chapter 5 of OCR A-Level Chemistry, focusing on electrons and bonding.

What is the rule regarding orbitals with the same energy?

Within a sub shell, the orbitals have the same energy. One electron occupies each orbital before pairing begins.
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Key Terms

Term
Definition
What is the rule regarding orbitals with the same energy?
Within a sub shell, the orbitals have the same energy. One electron occupies each orbital before pairing begins.

How can electron configuration be shortened?

1s2 can be expressed as [He].
1s2 2s2 2p6 can be expressed as [Ne].
1s2 2s2 2p6 3s2 3p6 can be expressed as [Ar].

What happens in terms of energy sub-shells when forming ions?
The highest energy sub-shells lose or gain electrons.
What is ionic bonding?
The electrostatic attraction between positive and negative ions.
What is the result of ions attracting oppositely charged ions in all directions?
Giant ionic lattice
What happens to the melting points for giant ionic lattices, when ionic charge increases?
Melting point increases as there is a stronger attraction between ions.

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TermDefinition
What is the rule regarding orbitals with the same energy?
Within a sub shell, the orbitals have the same energy. One electron occupies each orbital before pairing begins.

How can electron configuration be shortened?

1s2 can be expressed as [He].
1s2 2s2 2p6 can be expressed as [Ne].
1s2 2s2 2p6 3s2 3p6 can be expressed as [Ar].

What happens in terms of energy sub-shells when forming ions?
The highest energy sub-shells lose or gain electrons.
What is ionic bonding?
The electrostatic attraction between positive and negative ions.
What is the result of ions attracting oppositely charged ions in all directions?
Giant ionic lattice
What happens to the melting points for giant ionic lattices, when ionic charge increases?
Melting point increases as there is a stronger attraction between ions.
Are ionic compounds soluble?
They dissolve in polar solvents such as water.

What does solubility require?

The ionic lattice must be broken down.

Water molecules must attract and surround the ions.

What does solubility (of ionic compounds) depend on?
The relative strengths of the attractions within the giant ionic lattice and the attractions between ions and water molecules.

When can ionic compounds conduct electricity?

Not in the solid state.

| When molten or dissolved in water.

Why can't ionic compounds conduct electricity when solid?

The ions are in a fixed position.

| There are no mobile charge carriers.

Why can ionic compounds conduct electricity when molten or dissolved in water?

The solid ionic lattice breaks down.

| The ions are now free to move as mobile charge carriers.

Summarise the properties of most ionic compounds

High melting and boiling points.
Tend to dissolve in polar solvents such as water.
Conduct electricity only in the liquid state or in aqueous solution.

What is covalent bonding?
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
What is a covalent bond?
The overlap of atomic orbitals, each containing one electron, to give a shared pair of electrons.
How does covalent bonding differ to ionic bonding?
The attraction is localised, acting only on the shared pair of electrons and the two nuclei of the bonded atoms.
How can covalent bonding be displayed?
With dot and cross diagrams.
What is a multiple covalent bond?
Two atoms share more than one pair of electrons.
What is a double bond?
The electrostatic attraction is between two shared pairs of electrons, and the nuclei of the bonding atoms.
What is a triple bond?
The electrostatic attraction is between three shared pairs of electrons, and the nuclei of the bonding atoms.
What is a dative covalent bond?
The shared pair of electrons has been supplied by one of the bonding atoms only.
Give an example of a dative covalent bond
An ammonia molecule donates its lone pair of electrons to an H+ ion. Forming an ammonium ion.
What is average bond enthalpy?
A measurement of covalent bond strength. Larger value = stronger bond.