Module 2 F321 definitions

AS level Chemistry module 2 definitions for OCR- please leave feedback. 

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  • Created by: Amy Mc
  • Created on: 24-11-14 09:34
First ionisation energy
The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.
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Electron shielding
The repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus on the outer shell electrons.
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Electron shell
A group of atomic orbitals with the same principal quantum number, n.
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Principle quantum number, n
A number representing the relative overall energy of each orbital, which increases with distance from the nucleus.
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Atomic orbital
A region within an atom that can hold up to 2 electrons, with opposite spins.
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Sub-shell
A group of the same type of atomic orbitals (s, p, d or f) within a shell.
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Compund
A substance formed from 2 or more chemically bonded elements in a fixed ratio, usually shown by a chemical formula.
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Ionic bond
The electrostatic attraction between oppositely charged ions.
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Giant ionic lattice
A giant 3-D structure of oppositely charged ions, held together by strong ionic bonds.
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Covalent bond
A bond formed by a shared pair of electrons.
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Lone pair
An outer shell pair of electrons not involved in chemical bonding.
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Dative covalent/ coordinate bond
A shared pair of electrons which has been provided by one of the atoms only.
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Electronegativity
A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond.
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Permanent dipole
A small charge difference across a bond which results from a difference in the electronegativities of the bonded atoms.
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Polar covalent bond
A bond formed by a shared pair of electrons which has a permanent dipole.
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Intermolecular force
An attractive force between neighbouring molecules.
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Permanent dipole-dipole bond
A weak attractive force between permanent dipoles in neighbouring polar molecules.
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van der Waal's forces
Attractive forces between induced dipoles in neighbouring molecules.
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Hydrogen bond
A strong dipole-dipole attraction between an electron deficient hydrogen atom and a lone pair of electrons on a highly electronegative atom (Nitrogen or Oxygen).
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Metallic bonding
The electrostatic attraction between positive metal ions and delocalised electrons.
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Delocalised electrons
Electrons shared between more than 2 atoms.
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Giant metallic lattice
3-D structure of positive ions and delocalised electrons, bonded together by strong metallic bonds.
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Simple molecular lattice
3-D structure of molecules, bonded together by weak intermolecular forces.
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Giant covalent lattice
3-D structure of atoms, bonded together by strong covalent bonds.
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Other cards in this set

Card 2

Front

The repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus on the outer shell electrons.

Back

Electron shielding

Card 3

Front

A group of atomic orbitals with the same principal quantum number, n.

Back

Preview of the back of card 3

Card 4

Front

A number representing the relative overall energy of each orbital, which increases with distance from the nucleus.

Back

Preview of the back of card 4

Card 5

Front

A region within an atom that can hold up to 2 electrons, with opposite spins.

Back

Preview of the back of card 5
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