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Vander waals forces
Electron movement in first molecule , uneven distribution of electron / electron density creates temporary dipole
Induces a dipole in another molecule
Delta + attracts delta - in adjacent molecules
This attraction between 2 induced dipoles r called Vander waals
More electron stronger forces
Dipole - dipole
Difference in electronegativity
One slightly + one slightly -
Attracted to each other
Hydrogen bonding F O N H
Big difference in electronegativity between H and FONH
Attraction of H+ and rest -
How hydrogen bond forms between two molecules of ammonia
large difference in electronegativity between N and H+
Forms N- and H delta +
Lone pair on N attracts H delta +
Why’s graphite soft
Planes
Weak forces between planes
Metallic bond
Attraction force between + ions and delocalised e-. More protons more attraction
Why the acid strengths of ethanedioic acid and ethanoic acid are different
Acid is in for RCOOH
Ethanoic R = CH3
Ethanedioic R = COOH
unionised COOh in Ethanedioic contains 2 electronegative oxygen Atoms
Has a electron pulling effect
CH3 is positive inductive electron pushing
O-H bond in ethanedioc acid more polarised H becomes for +
More dissociated into H+
Ethanedioic acid stronger than ethanoic acid
Bonds
Ionic - giant ionic lattice
Covalent - simple molecular or giant molecular
Electro negativity
Power of an atom to attract pairs of electron in a covalent bond towards itself
High Factors effecting electronegativity
High nuclear charge - higher attraction force
Atomic radius smaller
Shielding less
Trends electronegativity
Down group decrease
nuclear charge increase
HIGH shielding prioritised
Across a period - increases
nuclear charge increases
Shrieking same
Regulars in smaller atomic radii