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17 Terms

1
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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

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Dipole - dipole

Difference in electronegativity

One slightly + one slightly -

Attracted to each other

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Hydrogen bonding F O N H

Big difference in electronegativity between H and FONH

Attraction of H+ and rest -

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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 +

7
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Why’s graphite soft

Planes

Weak forces between planes

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Metallic bond

Attraction force between + ions and delocalised e-. More protons more attraction

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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

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Bonds

Ionic - giant ionic lattice

Covalent - simple molecular or giant molecular

11
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Electro negativity

Power of an atom to attract pairs of electron in a covalent bond towards itself

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High Factors effecting electronegativity

  • High nuclear charge - higher attraction force

  • Atomic radius smaller

  • Shielding less

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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

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