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inorganic chemistry reactions Flashcards

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
group 2 metal carbonates with water
no reaction
26
group 2 metal carbonates with dilute acids
forms salt+water+CO2
27
what observations indicate that the reaction is exothermic
heat is released, there is an increase in temperature measured
28
what observations indicate that the reaction is endothermic
heat is absorbed, there is a decrease in temperature measured
29
the solubility of hydroxides and sulfates trend in g2
going down the group, increases and decreases respectively
30
thermal decomposition of group 2 carbonates chem eq
XCO3(s) --heat--> XO(s) + CO2(g)
31
thermal decomposition of group 2 nitrates chem eq
2X(NO3)2(s) --heat--> 2XO(s) + 4NO2(g) + O2(g)
32
in agriculture, to treat acidic soils by neutralisation, raising their pH using (basic) hydroxides. also provides calcium for plant nutrition. using what specific substance?
slaked lime, calcium hydroxide Ca(OH)2 in aqueous state
33
quicklime
CaO
34
what is it and uses of powdered limestone in agriculture
calcium carbonate CaCO3 in aqueous state neutralise acidic soils, and in solid state supplying calcium for plant nutrition
35
physical properties of ceramics
hard, strong, brittle, high melting points, good electrical insulators
36
explain the strength of ceramics
strong bonds holding the atoms together in 3 dimensions make the ceramic hard and strong but also brittle
37
explain melting point of ceramics
strong covalent or ionic bonds holding the giant structure together need to be overcome with very high temperature
38
explain why ceramics are good electrical insulators
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.
39
explain high melting point of MgO in ceramics
strong electrostatic attraction of Mg2+ and O2- ions in the giant ionic lattice.
40
what are MgO ceramics used for and the good of it
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
41
what are Al2O3 ceramics used for and the good of it, another use of it
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
42
uses of sio2 ceramics
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
43
giant covalent structured ceramics
Al2o3, sio2
44
for periodicity, review all tables and graphs in the book.
i will right now
45
flame colors when period 3 elements burn in o2, in order
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
46
burning period 3 elements with O2 vigor trend
Na to Al vigorous, Si slow, P vigorous and rapid, S slow
47
burning period 3 elements with O2 products' states
Na2O to P4O10 solid, SO2 gas
48
SO2 smell
pungent
49
special thing about burning Al with O2
vigorous initial reaction. forms a layer of al2o3 that prevents further reaction. though when powdered, reacts well.
50
special thing about burning P with O2
ignite when exposed to air hence no heating required. *"clouds"* of white solid formed.
51
2SO2(g) + O2(g) 2SO3(g)
yup i know
52
read aloud the back page of the 12th sheet of ur notebook
OK
53
period 3 oxides with H2O
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
MgO(s) + HCl(aq)
-> MgCl2(aq) + H2O(l)
55
Mg(OH)2(s) + HCl(aq)
-> MgCl2(aq) + H2O(l)
56
Al2O3(s) + H2SO4(aq)
-> Al2(SO4)3(aq) + H2O(l)
57
Al2O3(s) + NaOH(aq) + H2O(l) and condition
-> NaAl(OH)4(aq). | hot concentrated alkali
58
SiO2(s) + NaOH(aq) and condition
-> Na2SiO3(aq) + H2O(l). | hot concentrated alkali
59
MgCl2(s) with H2O
MgCl2(s) --water--> Mg2+(aq) + 2Cl-(aq)
60
chloride of Al without water
Al2Cl6
61
hydrolysis, chloride of Al with H2o, chem eq and explain
[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
SiCl4(l) + H2O(l) and specialty
-> SiO2(s) + HCl(g) | off-white ppt of SiO2. white fumes HCl gas. some HCl dissolve in water, leaving acidic solution.
63
PCl5(s) + H2O(l) and solution left behind
-> H3PO4(aq) + HCl(g) | both products soluble in water and are highly acidic
64
2Na(s) + Cl2(g) -> 2NaCl(s) | describe observation
vigorous reaction, Na burns with orange/yellow flames, heat released, white solid forms
65
Mg(s) + Cl2(g) -> MgCl2(s) | describe observation
vigorous reaction, Mg bursts into brilliant white flames, heat released, white solid forms
66
note condition for 2Al(s) + 3Cl2(g) -> Al2Cl6(s) and observations
Pass dry Cl2 gas over heated aluminium foil. | vigorous reaction, Al glows red, heat released, white solid forms
67
note condition for Si(s) + 2Cl2(g) -> SiCl4(L) and observations
in excess Cl2 gas. | slow reaction, Si burst with yellow flame, heat released, colorless liquid forms
68
note condition for 2P(s) + 5Cl2(g) -> 2PCl5(s) and observations
in excess Cl2 gas | slow reaction, heat released. colorless liquid forms
69
ionic equation. H2SO4(aq) + H2O(l)
-> H3O+(aq) + HSO4-(aq)
70
appearance of fluorine at room temp
pale yellow gas
71
appearance of chlorine at room temp
(poisonous) yellow green gas
72
appearance of bromine at room temp
(toxic) red brown liquid
73
appearance of iodine at room temp
dark grey solid which gives off purple vapor when heated
74
appearance of astatine at room temp
black solid
75
explain the volatility trend of g17
going down the group, more electrons, stronger van der waals' forces, the closEr the molecules, the less volatile
76
reactivity pattern of g17 corresponding to the trend in electronegativity going down the group. read aloud this from your notebook
got it on my head
77
H2(g) + F2(g) and observation
-> HF(g) | reacts explosively even in cool, dark conditions
78
H2(g) + Cl2(g) and description of reaction
-> HCl(g) | reacts explosively in sunlight
79
H2(g) + Br2(g) and description of reaction
-> HBr(g) | reacts slowly on heating
80
H2(g) + I2(g) and description of reaction
⇌ HI(g) | forms an equilibrium mixture on heating
81
hydrogen halides get less thermally stable going down g17, explain why, using example of HI
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
Cl2(aq) + Br-(aq)
-> Cl-(aq) + Br2(aq)
83
Br2(aq) + Cl-(aq)
no reaction
84
color of dissolved iodine in cyclohexane
purple
85
color of dissolved bromine in cyclohexane
orange
86
color of dissolved chlorine in cyclohexane
very pale green
87
testing for identifying halide ions steps
dissolve unknown compound in dilute HNO3, add AgNO3 solution, see the color of precipitate.
88
colors of silver halide precipitates
AgCl white, AgBr cream, AgI pale yellow.
89
ionic eq for precipitation reaction of halide ions with AgNO3 solution
Ag+(aq) + X-(aq) -> AgX(s)
90
effect on silver halide precipitate of adding dilute ammonia solution
AgCl dissolves, AgBr and AgI remain insoluble
91
effect on silver halide precipitate of adding concentrated ammonia solution
AgCl and AgBr dissolves, AgI remain insoluble
92
ionic equation when H2SO4 acts as an acid with halide ions
H2SO4(l) -> HSO4-(s) + H+(g)
93
NaCl(s) + H2SO4(l)
-> NaHSO4(s) + HCl(G)
94
NaBr(s) + H2SO4(l)
-> NaHSO4(s) + HBr(G) | 2HBr(g) + H2SO4(l) -> Br2(g) + SO2(g) + 2H2O(l)
95
NaI(s) + H2SO4(l)
-> 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
observation of h2s
strong smell of bad eggs
97
spectator ions definition
ions present in a reaction mixture that do not take part in the reaction
98
disproportionation definition
the simultaneous reduction and oxidation of the same species in a chemical reaction
99
chlorine in cold alkali NaOH (15 degrees C) chem eq
Cl2(aq) + 2NaOH(aq) -> NaCl(aq) + NaClO(aq) + H2O(l)
100
chlorine in cold alkali NaOH (15 degrees C) ionic eq
Cl2(aq) + 2OH-(aq) -> Cl-(aq) + ClO-(aq) + H2O(l)
101
chlorine in cold alkali NaOH (15 degrees C) chem eq reduction half eq
1/2 Cl2(aq) + e- -> Cl-(aq)
102
chlorine in cold alkali NaOH (15 degrees C) chem eq oxidation half eq
1/2 Cl2(aq) + 2OH-(aq) -> ClO-(aq) + H2O(l)
103
chlorine in hot alkali NaOH (70 degrees C) chem eq
3Cl2(aq) + 6NaOH(aq) -> 5NaCl(aq) + NaClO3(aq) + 3H2O(l)
104
chlorine in hot alkali NaOH (70 degrees C) ionic eq
3Cl2(aq) + 6OH-(aq) -> 5Cl-(aq) + ClO-(aq) + 3H2O(l)
105
chlorine in hot alkali NaOH (70 degrees C) reduction half eq
5/2 Cl2(aq) + 5e- -> 5Cl-(aq)
106
chlorine in hot alkali NaOH (70 degrees C) oxidation half eq
1/2 Cl2(aq) + 6OH-(aq) -> ClO3-(aq) + 3H2O(l) + 5e-
107
chlorine in water purification making it safer to drink, chem eq. what kind of reaction is it?
Cl2(aq) + H2O(l) -> HCl(aq) + HClO(aq) | disproportionation reaction
108
HClO word formula
chloric(I) acid
109
HClO theory in chlorination of water
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
bleach composition and explain uses
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
uses of halogens and their compounds
water chlorination, bleach, PVC, halogenated hydrocarbons as solvents, refrigerants and in aerosols
112
NaX + H3PO4 X as halide ion conc. h3po4
-> HX + Na2HPO4
113
hcl + mno2
-> cl2 + mncl2 + h2o
114
state of Mg(OH)2 and Ca(OH)2
solid
115
Al(OH)3 + NaOH
->NaAl(OH)4
116
Al(OH)3 + H2SO4
-> Al2(SO4)3 + H2O
117
What forms a brownish-red ppt when reacted with NaOH and Na2CO3
Fe3+
118
fecl3 is a yellow solution
ok
119
what forms a white ppt with naoh, and dissolve in excess naoh
Al3+
120
ionic eq of Fe2(SO4)3 with NaOH
[Fe(H2O)6]3+ + 3OH- --> Fe(H2O)3(OH)3 + 3H2O
121
ionic eq of Fe2(SO4)3 with Na2CO3
[Fe(H2O)6]3+ + 3CO3 2- --> 2Fe(H2O)3(OH)3 + 3H2O + 3CO2
122
ionic eq of Fe2(SO4)3 with HCl
[Fe(H2O)6]3+ + 4Cl- --> [FeCl4]- + 6H2O
123
a diagnostic test used to detect abnormalities of the esophagus, stomach and small bowel using X-ray imaging.
"barium meal"
124
solubility of carbonates down g2
decreases. | note that all their states are solid alr. so appears as ppt.
125
an element that forms an oxide that is a reducing agent
S or C

chemistry 11b (10 decks)

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