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Yr 11 CHEM > Bonding and Shapes > Flashcards

Bonding and Shapes Flashcards

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1
Q

metallic bonding

A

electrostatic force of attraction between a lattice of positively charged ions (cations), and free moving sea of delocalised electrons

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2
Q

metallic bonding properties

A 
- good conductors of electricity when 
  solid 
- good conductors of heat 
- malleable and ductile 
- high boiling point
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3
Q

Metalic bonding

good conductors of electricity when solid

A

Delocalised electrons flowing through the lattice which move and carry electrical charge

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4
Q

Metallic bonding

good conductors of heat

A

delocalised electrons flowing through the lattice which collide with metal atoms and pass on heat energy

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5
Q

Metallic bonding

malleable and ductile

A

Attraction between the metal lattice and delocalised electrons can take a fair amount of force/stretching before the lattice breaks and so it maintains properties whilst changing shape

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6
Q

Metallic bonding

high melting and boiling points

A

Attraction between the metal cations and delocalised electrons requires a lot of energy to overcome

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7
Q

ALLOYS

A

Combinations of two or more metals

  • Harder than pure metals
  • Less malleable than pure metals
  • Poorer conductors than pure metals
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8
Q

Galvanisation

A

process of applying a protective zinc coating to steel or iron to prevent rusting

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9
Q

Ionic Bonding

A

3D ionic lattice held together by strong electrostatic forces of attraction between the oppositely charged ions eg. NaCl

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10
Q

Anion

A
  • negative ions

- it has gained electrons

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11
Q

Cations

A
  • positive ions

- loss of electrons

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12
Q

polyatomic ions

  • acetate (ethanoate):
  • nitrate:
  • hydroxide:
  • permanganate:
  • cyanide:
  • sulfate:
  • carbonate:
  • chromate:
  • dichromate:
  • phosphate:
  • ammonium:
  • hydrogen carbonate:
A
  • acetate (ethanoate): CH₃COO⁻
  • nitrate: NO₃⁻
  • hydroxide: OH⁻
  • permanganate: MnO4⁻
  • cyanide: CN⁻
  • sulfate: SO₄⁻²
  • carbonate: CO₃⁻²
  • chromate: CrO₄⁻²
  • dichromate: Cr2O7⁻²
  • phosphate: PO₄³⁻
  • ammonium: NH₄⁺
  • hydrogen carbonate: HCO₃⁻
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13
Q

covalent bonding

A
  • electrostatic force of attraction between the nuclei of two atoms in a shared pair (or pairs) of electrons between them
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14
Q

Dative covalent bond

A

Covalent bond of the shared electrons are contributed by one atom only

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15
Q

shape of molecule

A
  • 2 bonding pairs, no lone pairs : linear
  • 3 bonding pairs, no lone pairs : trigonal planar
  • 4 boding pairs, no lone pairs : tetrahedral
  • 3 bonding pairs, 1 lone pairs : trigonal pyramida;
  • 2 bonding pairs, 2 lone pairs : V shaped/ bent
  • 1 bonding pair, 3 lone pairs : linear
  • VESPER theory treats double and triple bonds as if they were single bond or
    lone pairs
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16
Q

types of giant covalent molecules

A

(1) Giant Covalent Molecules

(2) covalent layer structures

17
Q

covalent network structures

A
  • insoluble in water
  • high melting and boiling point
  • do not conduct electricity or heat
  • very hard
  • e.g. diamond silicon dioxide SiO2
18
Q

covalent layer structures

A
  • insoluble in water
  • high melting and boiling point
  • good conductors of heat :
    • spare electron becomes delocalised between the layers. these mobile
    electrons enable graphite to conduct electricity
  • soft :
    • graphite layers can slide over one another making it soft and slippery
    (dispersion forces between layers)
19
Q

intermolecular bonding

A

(1) dispersion
(2) dipole - dipole
(3) hydrogen

20
Q

dispersion

A
  • occur between all molecule ( polar/ non polar)
  • very weak
  • bigger the molecule, stronger the dispersion force between molecules when
    a change of state is required because there is a greater surface area for them
    to act across
  • instantaneous- induced dipole : electrons are constantly moving. at one
    instant there will be more electron at one of the molecule that the other. this
    is called temporary dipole.
21
Q

dipole-dipole

A
  • between polar molecules
  • a dipole arises when there is a difference between electronegativity between
    2 atoms in a molecule
22
Q

hydrogen

A
  • H bonded to N, O, F

Yr 11 CHEM (5 decks)

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