Electrons, bonding and structure

  • Created by: Kat098
  • Created on: 03-04-18 19:00
Orbitals
Hold two electrons
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Sub-shell
Group of same type of atomic orbitals (s, p, d, f) within a shell
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Shell/Energy level
Group of atomic orbitals with same principle quantum number, n
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Principle quantum number, n
relative overall energy of each orbitral, which increases with distance from nucleus
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Atomic orbital
Region within an atom that can hold up to two electrons, with opposite spins
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Electron configuration
Arrnagement of electrons in an atom
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Ionic bonding
Electrtostatic attraction between oppositely charged ions
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Giant ionic lattice
3D structure of oppositely charged ions, held together by strong ionic bonds
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Metallic bonding
Electrostatic attraction between positive metal ions and delocalised electrons
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Giant metallic lattice
3D structure of positive ions and delocalised electrons, bonded together by strong metallic bonds
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Covalent bonding
Bond formed by a shared pair of electrons
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Giant covalent lattice
3D structure of atoms that are bonded together by strong covalent bonds
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Simple molecular lattice
3D structure of moleucles, bonded together by weak intermolecular foces
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Dative bonding / Coordiante bonds
Shared pair of electrons provided by one of the bonding atoms only
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Lone pairs
Outer-shell pair of electrons that isn't involved in chemical bonding
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Linear shape
1/2 bonding pairs, bond angle 180
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Trigonal planar shape
3 bonding pairs, bond angle 120
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Tetrahedral
4 bonding pairs, bond angle 109.5
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Trigonal bipyramid
5 bonding pairs, bond angles 90/120
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Octahedral
6 bonding pairs, bond angle 90
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Pyramidal
3 bonding pairs, 1 lone pair, bond angle 107
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Bent/non-linear
2 bonding pairs, 2 lone pairs, bond angle 104.5
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Electronegativity
The ability of an atom to attract the shared pair of electrons in a covalent bond
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Permanent dipole-dipole
Weak attractive forces betwwen two polar molecules
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Intermolecular forces
Attractive forces between neighboruing molecules
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Londons forces
Attractive forces between induced dipoles in neighbouring molecules
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Hydrogen bonding
Strong permanent-dipole attraction between an electron-deficient hydrogen atom on one molecule, and a lone pair of electrons on a highly electronegative atom (F, N, O) on a different molecule
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Diatomic molecules
Molecules composed of only two atoms
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Other cards in this set

Card 2

Front

Group of same type of atomic orbitals (s, p, d, f) within a shell

Back

Sub-shell

Card 3

Front

Group of atomic orbitals with same principle quantum number, n

Back

Preview of the back of card 3

Card 4

Front

relative overall energy of each orbitral, which increases with distance from nucleus

Back

Preview of the back of card 4

Card 5

Front

Region within an atom that can hold up to two electrons, with opposite spins

Back

Preview of the back of card 5
View more cards

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