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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Ionic

A

Strong electrostatic forces of attraction between oppositely charged ions

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2
Q

Sulfate

A

SO4 2-

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3
Q

Hydroxide

A

OH -

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4
Q

Nitrate

A

NO3 -

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5
Q

Carbonate

A

CO3 2-

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6
Q

Ammonium

A

NH4 +

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7
Q

Sodium chloride structure

A

Giant ionic lattice

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8
Q

Behaviour of ionic compounds

A
  • conduct electricity when molten or dissolved: ions free to move
  • high melting pt: strong electrostatic forces of attraction
  • tend to dissolve in water: water is polar, partial charges pull ions away from lattice
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9
Q

Covalent

A

2 or more non-metals strongly bonded together by shared pairs of electrons

Both positive nuclei electrostatically attracted to negative shared electrons

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10
Q

Giant covalent - graphite

A

Sheets of hexagons bonded by VdW with every 4th electron delocalised

  • slippery: VdW between layers, slide over each other
  • electrical conductor: delocalised electrons
  • low density: layers far apart compared to le goth of covalent bonds
  • high mpt: strong covalent bonds, sublimes over 3900K
  • insoluble: covalent bonds in sheets too strong
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11
Q

Giant covalent - diamond

A

Each C covalently bonded to 4 other C atoms in tetrahedral shape

  • high mpt, hard, insoluble: strong covalent bonds
  • thermal conductor: vibrations travel through stiff lattice
  • can’t conduct electricity: outer electrons in localised bonds
  • can ‘cut’ to form gemstones: refracts lights
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12
Q

Dative covalent

A

Both electrons donated by 1 atom

E.g. ammonium ion, nitrogen atom donates pair to H+

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13
Q

Valence-Shell Electron-Pair Repulsion Theory

A

Lone-pair/lone-pair angles biggest

Lone-pair/bonding-pair angles middle

Bonding-pair/bonding-pair angles smallest

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14
Q

Polarisation of covalent bonds

A

Differences in electronegativity

Polar bonds have permanent dipoles cause by shift in electron density in bond

Greater difference in electronegativity = more polar bond

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15
Q

Metallic

A

Metals have giant metallic lattice structure

Positive metal ions in a closely packed lattice surrounded by a sea of delocalised electrons

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16
Q

Properties of metals

A
  • high mpt: strong electrostatic forces of attraction between positive metal ions and sea of delocalised electrons (more delocalised electrons per atom = higher mpt)
  • thermal conductors: delocalised electrons can pass kinetic energy
  • electrical conductors: delocalised electrons can carry current
  • insoluble except in liquid metals: strong metallic bonds

Chemistry (3 decks)

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