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Polytomic Ions Flashcards

1
Q

Thiosulfate

A

S2O3 ^2-

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3
Q

Sulfate

A

SO4 ^2-

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4
Q

Nitrate

A

NO3 ^-

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6
Q

Permanganate

A

MnO4 ^-

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7
Q

Dichromate

A

CrO7 ^2-

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8
Q

Carbonate

A

CO3 ^2-

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9
Q

Hydrogen Carbonate

A

HCO3 ^-

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11
Q

Nitrite

A

NO2 ^-

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12
Q

Hydroxide

A

OH ^-

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13
Q

Acetate/ethanoate

A

CH3COO-

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14
Q

Nitric acid

A

HNO3

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15
Q

Phosphoric acid

A

H3PO4

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16
Q

Carbonic acid

A

H2CO3

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17
Q

Sulfurous acid

A

H2SO3

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18
Q

Sulphuric acid

A

H2SO4

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19
Q

Metal+ o2

A

Metal oxide

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20
Q

Metal Oxide + Water

A

Metal Hydroxide

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21
Q

Metal + Water

A

Metal Hydroxide + H2

22
Q

Metal + acid

23
Q

Non metal +O2

A

Non metal oxide

24
Q

Non metal oxide + H20

25
Q

Ionic bonding

A

A transfer of electrons and subsequent

26
Q

Metallic bonding

A

between a positive kernel and a sea of delocalised electrons

27
Q

Covalent bonding

A

A sharing of at least one pair of electrons by two non metal atoms

28
Q

Metallic bonding summary

A

Metal atoms packed close together so outermost levels overlap and the atoms donate electrons which become delocalised electrons in which a strong electrostatic attraction between the delocalised e,extrinsic cloud and the metal cations. Form a crystal lattice

29
Q

Lattice structure

A

A symmetrical 3D arrangement of atoms inside a crystal

30
Q

Chlorate

31
Q

Hydrogen sulfate

32
Q

Sulfite

33
Q

Phosfate

34
Q

Non-polar covalent (pure covalent)

A

An equal sharing of electrons

35
Q

Polar covalent

A

Unequal sharing of electrons which leads to a diopole forming (As a result of the electronegativity difference)

36
Q

Electronegativity

A

A measure of tendency of an atom to attract a binding pair of electrons

37
Q

Dative Colvalent Bonding

A

a lone pair of electrons from one atom is shared with another atom which has an empty orbital in its outermost energy level.

38
Q

Ionic Properties

A
  1. High melting + boiling points= strong electrostatic force
  2. Dont conduct electricity when solid only when molten
  3. Soluble in water: solution conduct electricity
39
Q

Metallic Properties

A
  1. High melting and boiling: the more valence electrons+ stronger the attraction
  2. Good conductor: valence electrons are free to move
  3. Malleable and ductile: the ions are easily movable+ Deloc. Electrons create a buffer
  4. Lustrous, heat conductors, dense, high tensile strength
40
Q

Arsine

41
Q

Phosphine

42
Q

Stibine

43
Q

Hydrogen telluride

44
Q

Silicon tetrahydride

45
Q

Germane

46
Q

Stannane

Physics (14 decks)

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