Bonding
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- Created by: jodi
- Created on: 07-01-19 17:54
What is an ionic bond?
The electrostatic forces of attraction between oppositely charged ions in an ionic lattice.
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When do electrostatic forces of attraction increase in strength?
When the charge on the ion increases and the size of the ion decreases.
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Name and explain the properties of ionic compounds.
High melting and boiling points. A large amount of energy is required to break the ionic bonds.
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Name and explain the properties of ionic compounds.
Don't conduct electricity when solid but do when molten. Ions are free to move to carry the charge.
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Name and explain the properties of ionic compounds.
White crystalline solids. Arrangement of ions in a giant ionic lattice. The ions are tightly packed together and are unable to move past each other.
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What is a lattice?
A regular arrangement of atoms or ions.
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What is a covalent bond?
The electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms.
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What is a lone pair?
A pair of unshared electrons in the outer shell of an atom.
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Name and explain the properties of molecular substances.
Low melting and boiling points due to weak intermolecular forces between molecules.
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Name and explain the properties of molecular substances.
Do not conduct electricity in any state as there are no free ions or delocalised electrons to carry the charge.
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Name and explain the properties of molecular substances.
Soft. don't have a regular structure; weak intermolecular forces
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Define a co-ordinate bond.
Contains at least one shared pair of electrons between two atoms in which one atom provides both electrons.
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Define the octet rule.
When reacting, atoms tend to gain, lose or share electrons in order to obtain eight electrons in their outer shell.
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Define electronegativity.
The extent to which an atom attracts the bonding pairs of electrons in a covalent bond.
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Explain the trend in electronegativity across a period.
Nuclear charge increases as the size of the atom decreases; greater attraction between shared electrons and nucleus
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Explain the trend in electronegativity down a group.
Electronegativity decreases. The pair of electrons will be further from the nucleus therefore there will be decreased attraction from the nuclear charge. Inner electrons will shield the shared pair of electrons.
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What is a polar bond?
A covalent bond in which there is unequal sharing of bonding electrons.
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Why is CO non-polar?
Despite having polar bonds within the molecule, the shape is symmetrical therefore the dipoles cancel out.
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What is a metallic bond?
The attraction between layers of positive ions and a sea of delocalised electrons.
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Name and explain the properties of metals.
Conduct electricity; Delocalised electrons are free to move to carry the charge.
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Name and explain the properties of metals.
High melting and boiling points; Metallic bonding is strong and requires energy to break.
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Name and explain the properties of metals.
Malleable and Ductile; Layers of positive ions can slide over one another without disrupting the bonding.
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Why does the atomic radius decrease across a period?
Increasing nuclear charge pulls the electrons closer to the nucleus; no increase in shielding.
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Explain the trend in electrical conductivity from sodium to aluminium.
Increases; the number of delocalised electrons increases per atom. Mg and Al have a stronger conductivity as the atoms are more tightly packed and are more difficult to seperate.
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Other cards in this set
Card 2
Front
When do electrostatic forces of attraction increase in strength?
Back
When the charge on the ion increases and the size of the ion decreases.
Card 3
Front
Name and explain the properties of ionic compounds.
Back
Card 4
Front
Name and explain the properties of ionic compounds.
Back
Card 5
Front
Name and explain the properties of ionic compounds.
Back
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