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Chemistry > Topic 4 - Inorganic Chemistry > Flashcards

Topic 4 - Inorganic Chemistry Flashcards

1
Q

Group 1 - Alkali Metals

Properties of group 1 metals (alkali metals)

A

soft

reactive

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2
Q

Group 1 - Alkali Metals

order of reactivity in group 1 (alkali metals)

A

as you go down the group, metals become more reactive.

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3
Q

Group 1 - Alkali Metals

melting and boiling points in group 1 (alkali metals)

A

as you go down the group, melting and boiling points decrease.

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4
Q

Group 1 - Alkali Metals

why does reactivity increase as you go down group 1 (alkali metals)

A

the forces of attraction between the nucleus and the outer electron decrease, so it is lost more easily as the number of shells increases.

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5
Q

Group 1 - Alkali Metals

alkali metal + water —>

A

metal hydroxide + hydrogen

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6
Q

Group 1 - Alkali Metals

group 1 (alkali metals) reacting with oxygen

A

Lithium + Oxygen -> Lithium Oxide (Li2O)

Sodium + Oxygen -> Sodium Oxide (Na2O)

Sodium + Oxygen -> Sodium Peroxide (Na2O2)

Potassium + Oxygen -> Potassium Peroxide (K2O2)

Potassium + Oxygen -> Potassium Superoxide (KO2)

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7
Q

Group 7 - Halogens

Colour of Halide salts

E.g. KCl, KBr, Kl

A

colourless

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8
Q

Group 7 - Halogens

colour of Bromine water

A

orange

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9
Q

Group 7 - Halogens

Colour of chlorine water

A

colourless

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10
Q

Group 7 - Halogens

colour of iodine water

A

brown

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11
Q

Group 7 - Halogens

State of fluorine at room temp

A

poisonous yellow gas

most reactive halogen

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12
Q

Group 7 - Halogens

State of chlorine at room temp

A

Green gas

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13
Q

Group 7 - Halogens

State of bromine at room temp

A

poisonous red-brown liquid

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14
Q

state of iodine at room temp

A

grey solid

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15
Q

Group 0 - Noble Gases

why are noble gases inert?

A

they have a full outside shell of electrons

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16
Q

diatomic molecules

A

each molecule consists of two atoms, joined together by a covalent bond

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17
Q

Group 7 - Halogens

melting and boiling points in group 7 (halogens)

A

as you go down group 7, melting and boiling points increase.

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18
Q

Group 7 - Halogens

properties of group 7

A

-1 charge
-form covalent bonds with other nonmetals

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19
Q

percentage of nitrogen in the atmosphere

A

78%

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20
Q

percentage of oxygen in the atmosphere

A

21%

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21
Q

percentage of argon in the atmosphere

A

1%

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22
Q

percentage of carbon dioxide in the atmosphere

A

0.04%

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23
Q

thermal decomposition

A

the process of breaking something down using heat

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24
Q

thermal decomposition of metal carbonate

metal carbonate ->

A

metal oxide + carbon dioxide

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25
practical: heating copper (II) carbonate
- copper (II) carbonate is a green powder - it will decompose into copper (II) oxide, a black powder and carbon dioxide, a colourless gas
26
atmosphere
layer of gases surrounding the earth held in place by gravity
27
greenhouse gases
carbon dioxide methane water vapour
28
global warming
overall increase in earth's temperature
29
climate change
**CONSEQUENCE OF GLOBAL WARMING** effects on climate, such as shifts in weather patterns
30
weather
short term atmospheric conditioms
31
climate
typical weather conditions in an entire location for a very long time e.g. singapore is humid
32
greenhouse effect
- solar radiation from the sun passes through the atmosphere and hits the earth - energy reflects back out to space, some is absorbed by earth - most energy is absorbed by greenhouse gases - trapped energy keeps the atmosphere warmer
33
metals always form
cations
34
metal + acid --->
salt + hydrogen
35
corrosion
process by which metals are slowly broken down by reacting with surrounding substances
36
rusting
special type of corrosion refers specifically to the corrosion of IRON redox reaction
37
iron rusting half equation
Fe -> Fe3+ + 3e-
38
redox reaction
reaction involving both oxidation and reduction
39
conditions required for rusting to occur
water and oxygen
40
# Methods of preventing rusting Barrier Method
coating the iron in something (like paint) to prevent water and oxygen from touching the iron
41
# Methods of preventing rusting Sacrificial prevention
add a more reactive metal to the iron, that metal reacts with oxygen instead
42
# Methods of preventing rusting Galvanisation
coating the iron with a layer of zinc. prevents rust as zinc is more reactive than iron
43
why is pure gold found in the ground, but not pure iron?
- gold is unreactive, so doesnt react with other elements - iron is reacted enough to combine with other elements, so can be found in its ore
44
separating metals from metal oxides
- using carbon - carbon causes metal to lose its oxygen - metal becomes reduced - **ONLY WORKS FOR METALS LESS REACTIVE THAN CARBON**
45
neutral pH
7
46
acidic pH
1-6
47
alkaline pH
8-14
48
universal indicator in acidic solutions
turns red
49
universal indicator in alkaline solutions
purple
50
pH of pure water
7 (neutral)
51
acid + metal oxide --->
salt + water
52
acid + metal hydroxide --->
salt + water
53
acid + metal carbonate --->
salt + water + carbon dioxide
54
neutralisation
a reaction between an acid and a base
55
to find formula of salt in an equation
positive ion from base + negative ion from acid
56
obtaining salt crystals from acid-base reaction
1. dilute acid in a beaker and heat gently 2. add solid base bit by bit until no further reaction, meaning it's in excess 3. isolate salt solution by filtering out excess solid base using filter paper and funnel 4. heat solution in water bath until crystals form 5. let solution cool further, causing more crystals to form 6. filter out salt crystals using filter paper and funnel
57
titration
experimental technique used to find unknown concentration of an acid or alkali
58
titration equipment
1. **pipette** to measure volume of acid or alkali 2. **conical flask** to contain liquid from pipette 3. **burette** to add alkali or acid to conical flask 4. **white tile** to place conical flask on
59
titration method
1. use pipette to add 25cm^3 of alkali to conical flask 2. add 3 drops indicator to conical flask on a white tile 3. fill burette with acid and not starting volume 4. slowly add acid from burette to alkali in conical flask, stirring to evenly distribute 5. stop adding when indicator has changed colour 6. note final volume reading, calculate how much acid added 7. repeat titration until volumes are within 0.10cm^3 of each other 8. use results to calculate mean volume of acid required to neutralise alkali
60
salt
compound that contains a positive cation and a negative anion some are insoluble in water, some are soluble in water
61
# soluble and insoluble salts common salts of sodium, potassium, ammonium
soluble
62
# soluble and insoluble salts nitrates
soluble
63
# soluble and insoluble salts common chlorides
soluble **except silver chloride and lead chloride**
64
# soluble and insoluble salts common sulfates
soluble **except lead sulfate, barium sulfate, calcium sulfate**
65
# soluble and insoluble salts common carbonates and hydroxides
insoluble except sodium, potassium, ammonium
66
test for chlorine gas
bleaches damp blue litmus paper
67
test for oxygen gas
relights a glowing splint
68
test for hydrogen gas
lit splint produces a squeaky pop sound
69
test for carbon dioxide gas
turns limewater cloudy when bubbled through
70
anion
negatively charged ion
71
test for carbonate ion
- react w hydrochloric acid - if it contains carbonate ion, carbon dioxide gas will bubble out of solution - collect gas and bubble through limewater - if limewater turns cloudy, carbonate ions are present
72
test for sulfate ion
- react w hydrochloric acid to remove carbonate ions - add barium chloride solution - white precipitate will form if sulfate ions are present
73
test for halide ion
- react w nitric acid to remove carbonate + sulfate ions - add silver nitrate solution - chloride ions -> white precipitate - bromide ions -> cream precipitate - iodide ions -> yellow precipitate
74
cation
positively charged ion
75
# testing for cations method for flame test
1. take nichrome wire loop and clean it by dipping in dilute hydrochloric acid and heating over bunsen burner 2. dip wire in compound 3. hold wire over hottest part of bunsen burner 4. observe flame colour
76
# testing for cations lithium flame colour
red
77
# testing for cations sodium flame colour
yellow
78
# testing for cations potassium flame colour
lilac
79
# testing for cations calcium flame colour
orange-red
80
# testing for cations copper flame colour
green blue ICE PRINCESS

Chemistry (6 decks)

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