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inorganic chemistry reactions Flashcards

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1
Q

group 2 metals burn in air forming

A

white solid oxides

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2
Q

why do some group 2 metals burn with characteristic flame colors

A

because of their 2+ ions formed in the reaction

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3
Q

chemical eq and describe the observation of combustion of Mg

A

2Mg(s) + O2(g) -> 2MgO(s)

bright white flame (no colour)

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4
Q

chemical eq and describe the observation of combustion of Ca

A

2Ca(s) + O2(g) -> 2CaO(s)

brick red flame

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5
Q

chemical eq and describe the observation of combustion of Sr

A

2Sr(s) + O2(g) -> 2SrO(s)

scarlet flame

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6
Q

chemical eq and describe the observation of combustion of Ba

A

2Ba(s) + O2(g) -> 2BaO(s)

green flame

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7
Q

with group 2 metals as X, write chemical eq of their reaction with water. describe the general observations and trends down the group.

A

X(s) + 2H2O(l) -> X(OH)2(aq) + H2(g)
metal becoming smaller then disappears
cloudy white suspension formed
going down the group, vigor increases, bubbles of H2 gas released more rapidly, the value of pH increases and less amount of white ppt because more OH- dissolves.

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8
Q

chemical eq and describe the observation of the reaction between Mg and steam

A

Mg(s) + H2O(g) -> MgO(s) + H2(g)

vigorous reaction with hot Mg, white solid formed

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9
Q

chemical eq and describe the observation of the reaction between group 2 elements (as X) with dilute HCl. vigor trend down the group

A

X(s) + 2HCl(aq) -> XCl2(aq) + H2(g)
the metal sinks then disappears
bubbles of H2 gas
more vigorous

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10
Q

the appearance of a metal chloride solution

A

colorless

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11
Q

group 2 elements as X with dilute H2SO4 chem eq

A

X(s) + H2SO4(aq) -> XSO4(aq) + H@(g)

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12
Q

observations of Mg(s) + H2SO4(aq) -> MgSO4(aq) + H2(g)

A

bubbles of H2 gas. metal sinks then disappears. colorless solution of metal sulfate

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13
Q

observations of Ca(s) + H2SO4(aq) -> CaSO4(s) + H2(g)

A

only little bubbles of H2 gas. Ca sinks then disappears very slowly or incompletely. white ppt of CaSO4

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14
Q

observations of Sr(s) + H2SO4(aq) -> SrSO4(s) + H2(g)

A

a layer of insoluble sulfate, the reaction is slowed down or stopped entirely. metal remains and is coated with a white solid.

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15
Q

observations of Ba(s) + H2SO4(aq) -> BaSO4(s) + H2(g)

A

a layer of insoluble sulfate, the reaction is slowed down or stopped entirely. metal remains and is coated with a white solid.

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16
Q

chem eq of group 2 elements with HNO3 at dilute and moderate concentrations

A

at very dilute concentrations,
X(s) + 2HNO3(aq) -> X(NO3)2(aq) + H2(g)
at moderate concentrations (and even with very dilute acid, this may happen to some extent):
3X(s) + 8HNO3(aq) -> 3X(NO3)2(aq) + 2NO(g) + 4H2O(l)

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17
Q

appearance of NO2

A

deep red-orange gas

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18
Q

chem eq of group 2 oxides with water. trend of vigor

A

XO(s) + H2O(l) -> X(OH)2(aq)

increases down the group

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19
Q

formation of slaked lime

A

CaO(s) + H2O(l) -> Ca(OH)2(s)

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20
Q

describe the exothermicity observation of group 2 oxides with water, especially Ca to Ba

A

it gives off so much heat, some of the water boils off. metal oxide lump appears to expand and cracks open

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21
Q

group 2 oxides with dilute acids

A

forms salt and water

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22
Q

the ionic equation of group 2 metal hydroxides with water

A

O2-(s) + H2O(l) -> 2OH-(aq)

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23
Q

chem eq to show what happens when Ca(OH)2 put in water

A

Ca(OH)2(s) –water–> Ca2+(aq) + 2OH-(aq)

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24
Q

group 2 metal hydroxides with dilute acids

A

forms salt and water

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25
Q

group 2 metal carbonates with water

A

no reaction

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26
Q

group 2 metal carbonates with dilute acids

A

forms salt+water+CO2

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27
Q

what observations indicate that the reaction is exothermic

A

heat is released, there is an increase in temperature measured

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28
Q

what observations indicate that the reaction is endothermic

A

heat is absorbed, there is a decrease in temperature measured

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29
Q

the solubility of hydroxides and sulfates trend in g2

A

going down the group, increases and decreases respectively

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30
Q

thermal decomposition of group 2 carbonates chem eq

A

XCO3(s) –heat–> XO(s) + CO2(g)

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31
Q

thermal decomposition of group 2 nitrates chem eq

A

2X(NO3)2(s) –heat–> 2XO(s) + 4NO2(g) + O2(g)

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32
Q

in agriculture, to treat acidic soils by neutralisation, raising their pH using (basic) hydroxides. also provides calcium for plant nutrition.
using what specific substance?

A

slaked lime, calcium hydroxide Ca(OH)2 in aqueous state

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33
Q

quicklime

A

CaO

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34
Q

what is it and uses of powdered limestone in agriculture

A

calcium carbonate CaCO3 in aqueous state neutralise acidic soils, and in solid state supplying calcium for plant nutrition

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35
Q

physical properties of ceramics

A

hard, strong, brittle, high melting points, good electrical insulators

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36
Q

explain the strength of ceramics

A

strong bonds holding the atoms together in 3 dimensions make the ceramic hard and strong but also brittle

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37
Q

explain melting point of ceramics

A

strong covalent or ionic bonds holding the giant structure together need to be overcome with very high temperature

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38
Q

explain why ceramics are good electrical insulators

A

if they are covalent, there are no free electrons to move around. if they are ionic, the ions arent free to move in the solid.

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39
Q

explain high melting point of MgO in ceramics

A

strong electrostatic attraction of Mg2+ and O2- ions in the giant ionic lattice.

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40
Q

what are MgO ceramics used for and the good of it

A

due to it having no free electrons and the ions aren’t free to move in the solid, it is a good electrical insulator.
for furnace linings (refractory bricks)
for heating elements e.g. electric cookers: for safety measures, as a protective layer around the metal core

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41
Q

what are Al2O3 ceramics used for and the good of it, another use of it

A

for high temperature and high voltage electrical insulators: strong electrostatic forces holding aluminium and oxide ions together make it very resistant to wear; it is also chemically resistant because of the large amount of energy needed to separate the ions.
for replacement hip joints

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42
Q

uses of sio2 ceramics

A

as furnace linings (refractory bricks) in furnaces for the production of glass. due to its light weight and high melting point, to make ceramic tiles to protect the space shuttle

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43
Q

giant covalent structured ceramics

A

Al2o3, sio2

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44
Q

for periodicity, review all tables and graphs in the book.

A

i will right now

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45
Q

flame colors when period 3 elements burn in o2, in order

A

Na bright yellow, Mg bright white/no colour, Al bright white/no colour, Si no, P yellow or white, S blue, Cl2 and Ar no reaction

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46
Q

burning period 3 elements with O2 vigor trend

A

Na to Al vigorous, Si slow, P vigorous and rapid, S slow

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47
Q

burning period 3 elements with O2 products’ states

A

Na2O to P4O10 solid, SO2 gas

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48
Q

SO2 smell

A

pungent

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49
Q

special thing about burning Al with O2

A

vigorous initial reaction. forms a layer of al2o3 that prevents further reaction. though when powdered, reacts well.

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50
Q

special thing about burning P with O2

A

ignite when exposed to air hence no heating required. “clouds” of white solid formed.

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51
Q

2SO2(g) + O2(g) 2SO3(g)

A

yup i know

52
Q

read aloud the back page of the 12th sheet of ur notebook

A

OK

53
Q

period 3 oxides with H2O

A

Na2O and MgO with H2O form alkali
Al2O3 and SiO2 with H2O no reaction
P4O10, SO2 and SO3 with H2O form acid (H3PO4, H2SO3 and H2So4 respectively)

54
Q

MgO(s) + HCl(aq)

A

-> MgCl2(aq) + H2O(l)

55
Q

Mg(OH)2(s) + HCl(aq)

A

-> MgCl2(aq) + H2O(l)

56
Q

Al2O3(s) + H2SO4(aq)

A

-> Al2(SO4)3(aq) + H2O(l)

57
Q

Al2O3(s) + NaOH(aq) + H2O(l) and condition

A

-> NaAl(OH)4(aq).

hot concentrated alkali

58
Q

SiO2(s) + NaOH(aq) and condition

A

-> Na2SiO3(aq) + H2O(l).

hot concentrated alkali

59
Q

MgCl2(s) with H2O

A

MgCl2(s) –water–> Mg2+(aq) + 2Cl-(aq)

60
Q

chloride of Al without water

A

Al2Cl6

61
Q

hydrolysis, chloride of Al with H2o, chem eq and explain

A

[Al(H2O)6]3+(aq) -> [Al(H2O)5OH]2+(aq) + H+(aq)
Al2Cl6, dimer of alcl3, is broken down. Al3+ and Cl- ions enter the solution. each Al3+ ion is hydrated, attracted to e- pairs of O and form octahedral complex, water molecule bonded to it lose an H+ ion turning the solution acidic

62
Q

SiCl4(l) + H2O(l) and specialty

A

-> SiO2(s) + HCl(g)

off-white ppt of SiO2. white fumes HCl gas. some HCl dissolve in water, leaving acidic solution.

63
Q

PCl5(s) + H2O(l) and solution left behind

A

-> H3PO4(aq) + HCl(g)

both products soluble in water and are highly acidic

64
Q

2Na(s) + Cl2(g) -> 2NaCl(s)

describe observation

A

vigorous reaction, Na burns with orange/yellow flames, heat released, white solid forms

65
Q

Mg(s) + Cl2(g) -> MgCl2(s)

describe observation

A

vigorous reaction, Mg bursts into brilliant white flames, heat released, white solid forms

66
Q

note condition for 2Al(s) + 3Cl2(g) -> Al2Cl6(s) and observations

A

Pass dry Cl2 gas over heated aluminium foil.

vigorous reaction, Al glows red, heat released, white solid forms

67
Q

note condition for Si(s) + 2Cl2(g) -> SiCl4(L) and observations

A

in excess Cl2 gas.

slow reaction, Si burst with yellow flame, heat released, colorless liquid forms

68
Q

note condition for 2P(s) + 5Cl2(g) -> 2PCl5(s) and observations

A

in excess Cl2 gas

slow reaction, heat released. colorless liquid forms

69
Q

ionic equation. H2SO4(aq) + H2O(l)

A

-> H3O+(aq) + HSO4-(aq)

70
Q

appearance of fluorine at room temp

A

pale yellow gas

71
Q

appearance of chlorine at room temp

A

(poisonous) yellow green gas

72
Q

appearance of bromine at room temp

A

(toxic) red brown liquid

73
Q

appearance of iodine at room temp

A

dark grey solid which gives off purple vapor when heated

74
Q

appearance of astatine at room temp

A

black solid

75
Q

explain the volatility trend of g17

A

going down the group, more electrons, stronger van der waals’ forces, the closEr the molecules, the less volatile

76
Q

reactivity pattern of g17 corresponding to the trend in electronegativity going down the group. read aloud this from your notebook

A

got it on my head

77
Q

H2(g) + F2(g) and observation

A

-> HF(g)

reacts explosively even in cool, dark conditions

78
Q

H2(g) + Cl2(g) and description of reaction

A

-> HCl(g)

reacts explosively in sunlight

79
Q

H2(g) + Br2(g) and description of reaction

A

-> HBr(g)

reacts slowly on heating

80
Q

H2(g) + I2(g) and description of reaction

A

⇌ HI(g)

forms an equilibrium mixture on heating

81
Q

hydrogen halides get less thermally stable going down g17, explain why, using example of HI

A

the bond energies decrease going down the group, making it easier to break the hydrogen-halogen bond. because iodine atom is the largest, so the OVERLAP of its OUTER SHELL with a H atom gives a much longer bond length than with smaller halogen atoms. longer bond = weaker = less energy required to break it, HI least stable.

82
Q

Cl2(aq) + Br-(aq)

A

-> Cl-(aq) + Br2(aq)

83
Q

Br2(aq) + Cl-(aq)

A

no reaction

84
Q

color of dissolved iodine in cyclohexane

A

purple

85
Q

color of dissolved bromine in cyclohexane

A

orange

86
Q

color of dissolved chlorine in cyclohexane

A

very pale green

87
Q

testing for identifying halide ions steps

A

dissolve unknown compound in dilute HNO3,
add AgNO3 solution,
see the color of precipitate.

88
Q

colors of silver halide precipitates

A

AgCl white, AgBr cream, AgI pale yellow.

89
Q

ionic eq for precipitation reaction of halide ions with AgNO3 solution

A

Ag+(aq) + X-(aq) -> AgX(s)

90
Q

effect on silver halide precipitate of adding dilute ammonia solution

A

AgCl dissolves, AgBr and AgI remain insoluble

91
Q

effect on silver halide precipitate of adding concentrated ammonia solution

A

AgCl and AgBr dissolves, AgI remain insoluble

92
Q

ionic equation when H2SO4 acts as an acid with halide ions

A

H2SO4(l) -> HSO4-(s) + H+(g)

93
Q

NaCl(s) + H2SO4(l)

A

-> NaHSO4(s) + HCl(G)

94
Q

NaBr(s) + H2SO4(l)

A

-> NaHSO4(s) + HBr(G)

2HBr(g) + H2SO4(l) -> Br2(g) + SO2(g) + 2H2O(l)

95
Q

NaI(s) + H2SO4(l)

A

-> NaHSO4(s) + HI(g)
2HI(g) + H2SO4(l) -> I2(g) + SO2(g) + 2H2O(l)
6HI(g) + H2SO4(l) -> 3I2(g) + S(s) + 4H2O(l)
8HI(g) + H2SO4(l) -> 4I2(g) + H2S(g) + 4H2O(l)

96
Q

observation of h2s

A

strong smell of bad eggs

97
Q

spectator ions definition

A

ions present in a reaction mixture that do not take part in the reaction

98
Q

disproportionation definition

A

the simultaneous reduction and oxidation of the same species in a chemical reaction

99
Q

chlorine in cold alkali NaOH (15 degrees C) chem eq

A

Cl2(aq) + 2NaOH(aq) -> NaCl(aq) + NaClO(aq) + H2O(l)

100
Q

chlorine in cold alkali NaOH (15 degrees C) ionic eq

A

Cl2(aq) + 2OH-(aq) -> Cl-(aq) + ClO-(aq) + H2O(l)

101
Q

chlorine in cold alkali NaOH (15 degrees C) chem eq reduction half eq

A

1/2 Cl2(aq) + e- -> Cl-(aq)

102
Q

chlorine in cold alkali NaOH (15 degrees C) chem eq oxidation half eq

A

1/2 Cl2(aq) + 2OH-(aq) -> ClO-(aq) + H2O(l)

103
Q

chlorine in hot alkali NaOH (70 degrees C) chem eq

A

3Cl2(aq) + 6NaOH(aq) -> 5NaCl(aq) + NaClO3(aq) + 3H2O(l)

104
Q

chlorine in hot alkali NaOH (70 degrees C) ionic eq

A

3Cl2(aq) + 6OH-(aq) -> 5Cl-(aq) + ClO-(aq) + 3H2O(l)

105
Q

chlorine in hot alkali NaOH (70 degrees C) reduction half eq

A

5/2 Cl2(aq) + 5e- -> 5Cl-(aq)

106
Q

chlorine in hot alkali NaOH (70 degrees C) oxidation half eq

A

1/2 Cl2(aq) + 6OH-(aq) -> ClO3-(aq) + 3H2O(l) + 5e-

107
Q

chlorine in water purification making it safer to drink, chem eq. what kind of reaction is it?

A

Cl2(aq) + H2O(l) -> HCl(aq) + HClO(aq)

disproportionation reaction

108
Q

HClO word formula

A

chloric(I) acid

109
Q

HClO theory in chlorination of water

A

HClO produced decomposes slowly in solution.
one theory suggests that it produces reactive O atoms that can kill bacteria in water
HClO -> HCl + [O]

110
Q

bleach composition and explain uses

A

equal mixture of NaCl and NaClO made from Cl2 and cold alkali. O atoms from the chlorate(I) ions ClO- oxidise dye and other colored molecules. can also kill bacteria, e.g. clean toilets

111
Q

uses of halogens and their compounds

A

water chlorination, bleach, PVC, halogenated hydrocarbons as solvents, refrigerants and in aerosols

112
Q

NaX + H3PO4
X as halide ion
conc. h3po4

A

-> HX + Na2HPO4

113
Q

hcl + mno2

A

-> cl2 + mncl2 + h2o

114
Q

state of Mg(OH)2 and Ca(OH)2

A

solid

115
Q

Al(OH)3 + NaOH

A

->NaAl(OH)4

116
Q

Al(OH)3 + H2SO4

A

-> Al2(SO4)3 + H2O

117
Q

What forms a brownish-red ppt when reacted with NaOH and Na2CO3

A

Fe3+

118
Q

fecl3 is a yellow solution

A

ok

119
Q

what forms a white ppt with naoh, and dissolve in excess naoh

A

Al3+

120
Q

ionic eq of Fe2(SO4)3 with NaOH

A

[Fe(H2O)6]3+ + 3OH- –> Fe(H2O)3(OH)3 + 3H2O

121
Q

ionic eq of Fe2(SO4)3 with Na2CO3

A

[Fe(H2O)6]3+ + 3CO3 2- –> 2Fe(H2O)3(OH)3 + 3H2O + 3CO2

122
Q

ionic eq of Fe2(SO4)3 with HCl

A

[Fe(H2O)6]3+ + 4Cl- –> [FeCl4]- + 6H2O

123
Q

a diagnostic test used to detect abnormalities of the esophagus, stomach and small bowel using X-ray imaging.

A

“barium meal”

124
Q

solubility of carbonates down g2

A

decreases.

note that all their states are solid alr. so appears as ppt.

125
Q

an element that forms an oxide that is a reducing agent

A

S or C

chemistry 11b (10 decks)

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