Indicates the shell that the electrons occupy. the larger n is the further the shell is from the nucleus and the higher the energy level
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Atomic orbital
A region of space where up to 2 electrons can be found with opposite spins
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Sub-shell
Orbitals of the same type grouped together in a shell eg. 1s,2p,3d
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Ionic Bonding
The electrostatic force of attraction between two oppositely charged ions (metal and non-metal)
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Covalent Bonding
A shared pair of electrons between the nuceli of the two bonded non metal atoms. Elements reach noble gas configuration
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Lone pair
A pair of electrons not used for bonding
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Average bond enthalpy
A measure of the average energy of a bond and therefore the energy required to break it. Always positive as nond breaking is endothermic so requires energy. Bigger the value the stronger and more energy required to break the bond.
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Dative covalent bond (coordinate bond)
Where one of the atoms supplies both the shared electrons to the covalent bond. Shown as an arrow in the direction of donation
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Modified Octet Rule
1.Unpaired electrons pair up 2.max number of electrons that can pair up is equivalent to the number of electrons in the outer shell
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Electron Pair Repulsion Theory
as electrons all have a negative charge, each electron pair repels other electron pairs. The shape adopted will be the shape that allows all the pairs of electrons to be as far apart as possible.
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Electronegativity
Measures the attraction of a bonded atom for the pair of electrons in a covalent bond. Increases towards the top right of the periodic table
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Non-polar bonds
The nucleus of each bonded atom is equally attracted to the bonding electron pair and the electrons in the bond are evenly distributed between the atoms so each atom has an equal share of the pair of electrons eg.H2
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Polar bond
One atom more likely to attract the bonding electrons more, it is more electronegative eg.HCl
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Intermolecular forces
Forces between molecules that attract individual compounds to each other. Caused due to the random movements of electrons within the shells of the atoms in the molecule
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Permanent dipole-induced dipole interactions
Some molecules have a permanent dipole due to polar bonds being present. When near a non-polar molecule is causes electrons in the shells in the nearby molecule to shift slightly causing it to become slightly polar and an attraction occurs.
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Permanent dipole-permanent dipole interactions
Polar molcules have permanent dipoles that are attracted to each other, with opposite ends being attracted to each other eg. molecules of HCl attracted to each other
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London (dispersion) forces
Very weak forces between non-polar molecules caused by the random movement of electrons in atoms shells. This disrupts the charge within electron shells causing an instantaneous dipole that induces a dipole in neighbouring molecules.
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Hydrogen Bonding
A strong permanent dipole-permanent dipole attraction between an electron deficient hydrogen atom (O-H,N-H,F-H) and a lone pair of electrons on a highly electronegative atom (O,N,F) on a different molecule
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Other cards in this set
Card 2
Front
A region of space where up to 2 electrons can be found with opposite spins
Back
Atomic orbital
Card 3
Front
Orbitals of the same type grouped together in a shell eg. 1s,2p,3d
Back
Card 4
Front
The electrostatic force of attraction between two oppositely charged ions (metal and non-metal)
Back
Card 5
Front
A shared pair of electrons between the nuceli of the two bonded non metal atoms. Elements reach noble gas configuration
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