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Inorganic Chemistry > Period 3 elements > Flashcards

Period 3 elements Flashcards

1
Q

Sodium with water equation

A

2 Na + 2H2O > 2 NaOH + H2

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2
Q

Sodium with water observation

A

fizzes around on surface

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3
Q

Magnesium with water equation

A

Mg + H2O > MgO + H2

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4
Q

Magnesium with water reaction

A

Mg + H2O > MgO + H2

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5
Q

Sodium with Oxygen equation

A

4 Na + O2 > 2 Na2O

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6
Q

Sodium with Oxygen observation

A

Burns with a yellow flame to produce a white solid

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7
Q

Mg and Oxygen equation

A

2 Mg + O2 > 2MgO

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8
Q

Mg, Al, Si and P with Oxygen observation

A

Burns with a white flame to give white solid smoke

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9
Q

Al with O2 equation

A

4 Al + 3O2 > 2Al2O3

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10
Q

Si with O2 equation

A

Si + O2 > SiO2

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11
Q

P with O2 equation

A

4P + 5O2 > P4O10

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12
Q

S with O2 equation

A

S + O2 > SO2

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13
Q

Sulfur with O2 observation

A

burns with blue flame to form an acidic choking gas

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14
Q

Why do Ionic oxides have a high melting point?

A

due their ionic giant lattice structures - strong forces of attraction between oppositely charged ions.

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15
Q

Ionic Oxides

A

Na2O, MgO, Al2O3

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16
Q

How do you prove ionic oxides contain ions?

A

melt the solids to show they conduct electricity

17
Q

macromolecular oxides

A

SiO2

18
Q

properties of macromolecular oxides

A

strong covalent bonds - high Mp and Bp

19
Q

simple molecular oxides

A

P4O10, SO2

20
Q

properties of simple molecular

A

weak intermolecular forces - lower mp. covalently bonded due to the small electronegativity difference.

21
Q

Metal ionic oxides with water

A

hydroxides

22
Q

eg of metal ionic oxide reaction

A

Na2O + H2O > 2 Na+ + 2OH-
pH 13, vigorous exothermic reaction

23
Q

Magnesium Oxide with water

A

MgO + H2O > Mg(OH)2
pH 9

24
Q

why is Mg(OH)2 only slightly soluble in water?

A

as its lattice is stronger so fewer free OH- ions are produced.

25
Q

Phosphorous Oxide with water reaction

A

P4O10 + 6H20 > 4H3PO4
pH 0

26
Q

Silicon dioxide with water

A

SO2 + H2O > H2SO3

27
Q

Silicon trioxide with water

A

SO3 + H2O > H2SO4

28
Q

ionic metal oxide behaviour

A

basic

29
Q

non-metal covalent oxides behaviour

A

acidic

30
Q

behaviour in aluminium oxide

A

amphoteric - act as both a base and acid

31
Q

basic oxide pattern

A

acid + base > salt + water

32
Q

aluminum oxide acting as a base eg

A

Al2O3 + 3H2SO4 > Al2(SO4)3 + 3H2O

33
Q

alumiunium oxide acting as a acid

A

Al2O3 + 2NaOH > 4Na3PO4 + 6H2O

Inorganic Chemistry (6 decks)

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