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. It reduces the attractive forces between positive nucleus and the outer-shell electrons.
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Successive Ionosation Energies
A measure of the energy required to remove each electron in turn. e.g 2nd Ionisation enerdy of Li = Li^+ -> Li^2+(g) + e^-
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A Shell
A group of atomic orbitlals with the same principle quantum number.
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Atomic Orbital
The region in 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,f) within a shell.
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Ionic Bond
The electrostatic attraction between two oppositely charged ions.
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A Group
Verticle column in the periodic table. Elements in the same group have similar properties. Their atoms have the same number of outer-shell electrons.
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Covalent Bond
A bond formed by a shared pair of electrons.
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Dative Covalent Bond
A shared mpair of electrons that has bveen provided by ONE of the bonding atoms only.
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Trigonal Planar
No. electron pairs = 3 Bond angle = 120
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Tetrahedral
No. electron pairs = 4 Bond angle = 109.5
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Octahedral
No. electron pairs = 6 Bond angle = 90
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Linear
2 bonding regions Bond angle = 180
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Pyramidal
3 electron pairs 1 lone pair Bond angle = 107
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Non- linear
2 electron pairs 2 lone pairs Bond angle = 104.5
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Lone pair
Not bonded to any atom. Reduces other bond angles in the molecule by 2.5.
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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 that results from a difference in the electro negatives of the bonded atoms.
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Polar Covalent Bond
Has a permanent dipole
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A Polar Molecule
Has an overall dipole, when you take in to account the dipoles across the bonds.
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Intermolecular Force
An attractive force between neighbouring molecules.
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Permanent Dipole-Dipole Force
A weak attractive force between permanent dipoles in 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 strong attraction between: - An electron-deficient hydrogen atom (O-H[delta +], N-H[delta +]) on one molecule and - A lone pair of electrons on a highly electronegative atom (H-O[delta -], H-N[delta -]) on a different molecule.
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Metllic Bonding
The electrostatic attraction between positive metal ions and delocalised electrons.
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Delocalised Electrons
Are shared between more than 2 atoms.
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A Giant Metallic Lattice
A 3D structure of positive ions and delocalised electrons, 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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A 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. It reduces the attractive forces between positive nucleus and the outer-shell electrons.
Back
Electron Shielding
Card 3
Front
A measure of the energy required to remove each electron in turn. e.g 2nd Ionisation enerdy of Li = Li^+ -> Li^2+(g) + e^-
Back
Card 4
Front
A group of atomic orbitlals with the same principle quantum number.
Back
Card 5
Front
The region in an atom that can hold up to 2 electrons with opposite spins.
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