Exam Pick Ups Flashcards
(125 cards)
1
Q
Formula for ammonium nitrate?
A
NH4NO3
2
Q
Two problems caused by release of sulfur dioxide into the environment?
A
Acid Rain
Leaches into soil causing minerals to be washed out.
3
Q
Chemical equation for making carbon dioxide in the lab, using HCL and Calcium carbonate (CaCO3)
A
CaCO3 + 2HCL -> CaCl2 + H2O + CO2
4
Q
Equation for the weakly acidic solution that is formed when carbon dioxide reacts with water?
A
CO2 + H2O (Half arrows) H2CO3(aq)
5
Q
What is the name of the weakly acidic compound formed when carbon dioxide dissolves in water?
A
Carbonic acid.
6
Q
Observations of Magnesium when burnt?
A
Ash.
Bight light flame.
7
Q
Suggest what is seen from this reaction?
A
If nothing obvious, assume it is a gas.
8
Q
Potassium hydroxide?
A
KOH
9
Q
Test for Hydrogen?
A
Lit splint, should hear a squeeky pop.
10
Q
Thermal decomposition of magnesium carbonate?
A
MgCO3 -> MgO + CO2
11
Q
How would you get a pure dry carbonate sample?
A
(If asking method, mix, then stir)
Filter
Wash
dry by gently warming.
12
Q
In the reaction of Zinc and Copper (II) Sulphate what would you see?
A
pink coating on the zinc.
solution becomes colorless.
13
Q
Why does the student filter the mixture?
A
To obtain the in-soluble part or the product.
14
Q
Colour of Bromine in displacement reactions?
A
Colourless to Brown.
15
Q
Test for chlorine?
A
bleaches damp litmus paper, turning it white.
16
Q
Test for Oxygen?
A
Relight a glowing splint.
17
Q
Test for Hydrogen?
A
Squeky pop
18
Q
Test for carbon dioxide?
A
turns lime water cloudy
19
Q
Test for Ammonia?
A
Turns damp litmus paper blue.
20
Q
Chemical test for water?
A
white anhydrous copper(II) sulphate, goes blue in presence of water.
21
Q
testing for cations?
A
flame tests
22
Q
cations: Copper(II) Cu2+
A
Blue
23
Q
Cations: Iron(II) Fe2+
A
Sludgy Green
24
Q
Cations: Iron(III) Fe3+
A
Reddish brown
25
testing for Anions: carbonates?
carbonates give off CO2 with HCL
26
Testing anions: sulfates?
Sulphates ions produce a white precipitate
27
Testing for anions: Halides?
Nitric acid and silver nitrate.
28
Protons in carbon 12?
6
29
State what is meant by the term relative atomic mass?
- The mean mass of an atom of an element.
| - Compared to mass of Carbon-12.
30
Carbon-12 98.9% and carbon-13 1.1%?
(12 x 98.9) + (13 x 1.1) =
/100
= 12.01
31
Two changes that occur in the formation of an addition polymer?
- one of the bonds in the double bond breaks
| - many of the monomers then join together.
32
Explain why cracking is important process in the oil industry?
- Produces smaller shorter molecules
- smaller molecules more useful as have a greater demand.
- Produces alkenes.
- smaller shorter molecules burn better and are used to make fuel.
33
Movement of gasses in a tube?
Diffusion
34
How can higher temp change the time taken in a reaction?
- Less time
- particles have more kinetic energy.
- Particles and gas move quicker and diffuse quicker.
35
How many bonds does oxygen form?
2
36
Most of the time non-metals ....... RIG
gain electrons so are reduced.
37
Two gasses given off when heating ammonia chloride?
ammonia, hydrogen chloride
38
Solid made when ammonia chloride is heated?
ammonia chloride
39
What processes occur when ammonia chloride is heated?
decomposition and neutralization
40
color of lead?
silver
41
metal hydroxide + metal sulfate ->
metal hydroxide + sodium sulfate
42
test for carbonate ions?
HCL
| Fizzing.
43
test for sulfate ions?
Barium chloride
| You will see a white precipitate.
44
Test for ammonia ions?
- add NaOH and warm
- test gas
- litmus paper should turn blue
45
Example structural formula of propane?
CH3 CH2 CH3
46
solid and gas products formed during in complete combustion?
Carbon
| carbon monoxide
47
condition needed for hydrogen bromide reaction?
UV light
48
Organic product from hydrogen bromide reaction?
bromomethene
49
Equation for reaction between methane and bromine?
C3H8 + 5O2 -> 3CO2 + 4H2O
50
Strength of metals depend on the strength of electrostatic forces of attraction between two types of particles?
Elections
| Cations
51
breaking bonds.......
absorbs energy
52
making bonds.......
releases energy
53
when a reaction is exothermic....
more energy is released than is absorbed.
54
equation for anhydrous copper(II) sulfate test with water?
CuSO4 + 5H2O -> CuSO4.5H2O
55
Suggest why universal indicator is more suitable than methyl orange.
shows if the substance is weakly or strongly acidic, uses more then one color.
56
Suggest two substances that can be used to compare the re-activity.
Water
| Oxygen
57
Industrial uses of hydrogen?
Ammonia and HCL
58
Process in which particles more through a tube in experiment to make chlorides?
Diffusion.
59
Color of Bromine water test?
Orange/Yellow
| to colourless
60
Dibromethane.
4 hydrogens, 2 Bromine, 2 Carbon
61
Use of Aluminium?
aircraft material.
| LOW DENSITY
62
Two observations of all Group 1 metals?
Fizz, turn into a ball
63
Group one metals turn UI....
Blue, Alkali solution OH- ions
64
ionic bonding question 3 marks?
Electrons being transferred between oxygen and sodium.
idea of sodium losing.
Correct number of electrons involved.
65
Bromides are
acidic
66
Chlorides are
alkali
67
if solution is acidic..
H+ ions formed
68
If solution is alkali...
OH- ions formed
69
Hydrogen chloride gas dissociates in water......
but not in Methylbenzene
70
When hydrogen chloride dissolves in water.....
molecules split up into H+ ions and Cl- ions, this is dissociation.
71
When hydrogen chloride dissolves in methylbenzene..
it does not dissociate
| LITMUS PAPER BLUE!!!
72
What happens during neutralization reactions?
Acid contains Hydrogen ions
A base contains hydroxide ions
They neutralize and the products are neutral
73
neutralization reaction?
acid + base -> salt + water.
74
Example of base?
- copper oxide
| - zinc hydroxide.
75
Bases that are also soluble in water are called
Alkalis
76
Example of Alkalis?
- sodium hydroxide
| - potassium hydroxide
77
All alkalis are
bases
78
compounds with .H2O are....
hydrated
79
two metals that can be reacted with water to safely produce hydrogen?
iron
| magnesium
80
Solid used in the extraction of both iron and aluminium?
carbon
81
gas that is needed to the extraction of iron? why?
oxygen - to combust and produce heat
82
formula name and quickname of: Calcium oxide and calcium silicate?
CaO - quicklime
| CaSiO3 - Slag
83
Properties of limestone that need to be kept the same when retesting?
- Surface area
| - Mass
84
Why universal indicator may not be good in a experiment?
Color change is gradual, not sharp or defined.
| Alternatives litmus paper or methyl orange.
85
increasing pressure on a equilibrium reaction?
shifts to the side with fewest gas molecules.
86
why is aluminium a good conductor?
delocalised electrons.
| they are able to move between atoms are flow.
87
Two ways of collecting gas?
- test tube, downward displacement of water.
| - gas syringe.
88
Colour of Mg and MgO?
Gray silver
| white
89
Phenolphthalein?
colourless -> pink
| H2SO4
90
test for carbonate?
add named acid.
| - test for CO2
91
hydrogen chloride dissolved in water?
UI goes red
| H+ ions
92
hydrogen chloride dissolved in methylbenzene?
No color change.
| No h+ ions formed.
93
How does sacrificial protection work (2)
metal more reactive then other
| metal reacts in preference to other.
94
How can u find positive of metal x nitrate in re activity series?
- make solution of x nitrate
- add metal
- if reaction occurs metal is more reactive then x
- Work down the re-activity series till reaction occurs.
95
What is the type of reaction that occurs with the rusting of iron?
oxidation
96
Chemical test for chloride ions?
Silver nitrate solution.
Nitric acid.
White precipitate.
97
HCL + Mg
MgCl2 + Cl2
98
Exothermic reaction, increase the temperature?
Increase the rate of reaction.
| Kinetic theory
99
which side has the fewest gas molecules?
| N2 + 3H2 = 2NH3
right, discount ratio!!!
100
Ammonium nitrate
(NH4)(NO3)
101
why is it difficult to get a an accurate formula for air?
Mixture of different gasses
102
Advantage of using helium over hydrogen?
non-flammable
103
Properties of Aluminium?
Malleable
| Low density
104
what type of reaction is the bromine water test?
Addition reaction
105
a substance that can be added to lower PH?
Any acid.
106
why has excess of substance X been used?
to displace all of other element.
107
what colour does bromine turn most things?
Brown
108
Carbonates are normally in ............. form?
solid
109
Explain graphs points to include?
Trend
Linear, non-linear
Proportional?
110
Why must litmus paper be damp before use?
water needed to form OH- or H+ ions
111
suggest why the actual yield of ammonia is lower than the expected yield?
equilibrium not reached.
112
Two features of a dynamic equilibrium?
- rate of forward reaction = rate of reverse reaction
| - forwards and backwards reactions still occurring.
113
How is ammonia separated from un-reacted hydrogen and nitrogen?
- mixture of gasses cooled.
| - ammonia condenses.
114
Burning alcohols: explain why students results are lower then data book entry's?
- Lost heat to surroundings
| - Flame is moved around by draughts.
115
How is energy given out during a reaction?
- Braking bonds is endothermic/ takes in heat energy.
- Making bonds is exothermic gives out energy
- MORE HEAT ENERGY GIVEN OUT THEN TAKEN IN.
116
How does carbon dioxide cause cloudlessness in limewater?
caused by formation of white precipitate
117
What apparatus be used to collect dry oxygen gas
gas syringe
118
Explain how carbon dioxide is effective in fire extinguishers
blankets the fuel.
| prevents oxygen from reaching the fuel .
119
testing for ammonium ions, why nitric acid?
to remove carbonate ions
120
white precipitate with silver nitrate?
silver chloride
121
what fuel is formed when C2H6 is cracked to make C2H4?
H2 hydrogen
122
What is meant by the term bio degrade?
polymer breaks down, decomposes
| by bacteria or microbes
123
property that prevents addition polymers from easily bio degrading?
inert or unreactive
124
Calculate relative atomic mass of isotope
1) mass 85 72%
2) mass 87 28%
(85 x 0.72) + (87 x 0.28) =
125
colour when H2SO4 neutralizes the 2NaOH?
pink to colourless
