UNIT 1 - Module 2 - Electrons, bonding and structure

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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 Sheilding
|the repulsion between electrons in different inner shells. Sheilding reduces the net attractive force from the positive nucleus on the outer shell electrons.
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Successive Ionistation Energies
The energy required to remove each electron in turn from one mole of gaseous ion to form one mole of gaseous X+ ion.
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Shell
A group of atomic orbitals with the same priciple quantum number.
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Principle Quantum Number
The number representing the relative overall energy of each orbital, which increases with distance to the nucleus.
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Atomic Orbital
A region within an atom that can hold up to two 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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Electron Configuration
The arrangement of electrons in an atom
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Compound
A substance formed from two or more chemically bonded elements in a fixed ratio.
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Ionic Bond
The electrostatic attraction between oppositely charged ions.
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Giant Ionic Lattice
A 3D 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 that is not involved in chemical bonding.
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Dative Bond
A shared pair of electrons which has been provided by one of the bonded atoms only.
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Electronegativity
A measure of the attraction of a bonded atoms for the pair of electrons in a covalent bond.
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Permanent Dipole
A small charge difference across a bond that results from a difference in the electronegativities of the bonded atoms.
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Polar Covalent Bond
A covalent bond which has a permanent dipole.
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Polar Molecule
Has a overall dipole, when you take into account any dipoles across the bonds.
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Intermolecular Forces
An attractive force between neighbouring molecules.
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Permanent Dipole-Dipole Force
A weak attractive force between permanent dipoles in a neighbouring polar molecules.
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Van der Waals Forces
Attractive forces between induced dipoles in neighbouring molecules.
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Hydrogen Bond
A strond dipole-dipole attraction between an electron deficient hydrogen atom on one molecule; and a lone pair of electrons on a highly electronegative atom on a different molecule.
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Metallic Bonding
The electrostatic attraction between positive metal ions and delocalised electrons.
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Giant Metallic Lattice
A 3D structure of positive ions and delocalised electrsons, bonded together by strong metallic bonds.
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Simple Molecular Lattice
A 3D structure of molecules, bonded together by weak intermolecular forces.
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Giant Covalent Lattice
A 3D 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. Sheilding reduces the net attractive force from the positive nucleus on the outer shell electrons.

Back

Electron Sheilding

Card 3

Front

The energy required to remove each electron in turn from one mole of gaseous ion to form one mole of gaseous X+ ion.

Back

Preview of the back of card 3

Card 4

Front

A group of atomic orbitals with the same priciple quantum number.

Back

Preview of the back of card 4

Card 5

Front

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

Back

Preview of the back of card 5
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