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Chemistry Challenge > Of The Elements > Flashcards

Of The Elements Flashcards

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1
Q

Period

A

Horizontal row

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2
Q

Group 1

A

Alkali metals

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3
Q

Group 7

A

Halogens

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4
Q

Group 8

A

Noble gases

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5
Q

From metal to non metal

A

From left to right

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6
Q

Group 1 elements physical properties

A

Good conductors of electricity and heat
Soft snd easily cut w knife
Low MPs and bps
Low densities (float on water)

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7
Q

Group 1 chemical properties

A

Shiny surfaces when cut
Becomes dull/tarnished when it reacts w oxygen
Burn in air or oxygen to form white solid oxides

2M + O2 -> M2O

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8
Q

Group 1 react w water

A

2M + 2H2O -> 2MOH + H2

Moves around water
Hissing sound
Bubbles of gas
Gets smaller eventually disappearing 
(Melts into shiny ball)
(Burns w lilac flame)

Potassium more reactive

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9
Q

Group 1 reactivity

A

More reactive further down group
Although they all have 1 electron on outer shell
Size of atom increase so outer ejection gets further away
Therefore outer electron less attracted to the nucleus

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10
Q

Chlorine colour at room temp

A

Gas

Pale green

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11
Q

Bromine at room temp

A 
Liquid
Red brown (readily evaporates into brown gas)
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12
Q

Iodine at room temp

A

Solid
Black
(Sublimes when heated to form purple gas)

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13
Q

Halogen reaction w iron

A

Chlorine- hit iron wool glows brightest
Brown smoke forms and brown solid left behind

Bromine- glows less brightly
Brown smoke and brown solid formed

Iodine- even less brightly
Brown gas and solid formed

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14
Q

Halogen w iron forms a…

A

Metal halide (halide= compound of halogen)

Iron + chlorine = iron(III) chloride

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15
Q

Halogen reactivity trend

A

Decreases down the group because of increasing size of atoms
Needs to attract extra electron
Further away outer shell from nucleus the less attraction

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16
Q

Halogen + hydrogen

A

Forms a hydrogen halide

Hydrogen+ chlorine-> hydrogen chloride

H2+ Cl2 -> 2HCl

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17
Q

Displacement reaction

A

More reactive will replace in metal halide

From an aqueous solution of a metal halide

Chlorine+ potassium bromide solution
-> potassium chloride solution + bromine

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18
Q

Aqueous chlorine

A

Pale green- usually appears colourless as it is so dilute

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19
Q

Aqueous bromine

A

Orange

Turn yellow when diluted

20
Q

Aqueous iodine

A

Brown

21
Q

Group

A

Vertical column

22
Q

Hydrogen chloride + water

A

Hydrochloric acid

23
Q

Hydrochloric acid properties

A

Turns litmus red
Turns universal I red
Reacts w metal to form a metal chloride and hydrogen
W a metal carbonate to form a metal chloride, water and co2
With a metal hydroxide or oxide to form a metal chloride in solution and water

24
Q

Percentages of air

A

Nitrogen 78%
Oxygen 21%
Argon 0.9%
Carbon dioxide 0.04%

25
Q

Using copper

A 
Gas syringes
Silica tube
Copper
Pass air backwards and forwards
Need copper in excess
Calculate volume lost
26
Q

Using iron w oxygen

A

Iron filings
Burette end
Water will rise up from trough
Volume lost is equal to oxygen

27
Q

Using phosphorus and oxygen

A 
Phosphorus in water 
Same level inside and outside tube
Heat with iron rod
Reacting place bung on
Water levels will change
28
Q

How to prepare oxygen

A 
W hydrogen peroxide
Decomposes to form water and oxygen
Manganese 4 oxide as catalyst
Oxygen not soluble so not much is list
Collected and measured using gas syringe
29
Q

Oxygen and magnesium

A

Bright white flame

Forms white solid

30
Q

Oxygen and carbon

A

Yellow flame

Forms colourless gas

31
Q

Oxygen and sulfur

A

Blue flame

Forms colourless gas

32
Q

Magnesium oxide and water

A

Magnesium hydroxide

Mg(OH)2

33
Q

Carbon dioxide and water

A

Acidic oxide
Dissolves in water to form acidic solutions
H2CO3 carbonic acid
PH 5-6

34
Q

Sulfur dioxide and water

A 
Acidic oxide
Dissolves in water to form an acidic solution 
H2SO3
Sulfurous acid 
pH 3-4
35
Q

Oxides of metals are

A

Basics

Dissolve in water or don’t to form alkaline solutions

36
Q

Oxides of non metals

A

Often acidic

Dissolve in water to form acidic solutions
Some oxides are neutral- eg carbon monoxide

37
Q

Preparations of carbon dioxide

A

Metal carbonate+ acid
Eg calcium carbonate

By downward delivery as it is much denser than air

Thermal decomposition when heating metal carbonates

38
Q

Copper carbonate

A

Green to black

39
Q

Magnesium carbonate

A

No observable change

Stays white

40
Q

Calcium carbonate

A

Stays white

No observable change

41
Q

Zinc carbonate

A

White to yellow when hot

And white again when cold

42
Q

Sodium carbonate

A

No observable change
Stays white
Doesn’t compose in a Bunsen flame

43
Q

Uses of co2

A

Making carbonated drinks- pressure increased to increase solubility
In fizzy drinks

In fire extinguishers- co2 doesn’t support combustion
More dense than air so it sits on top of the burning fuel and prevent oxygen from getting to it

44
Q

Carbon dioxide and climate change

A

Contributing?
Absorbs infrared radiation
Fossil fuels

45
Q

Acid rain causes

A

Sulfur dioxide
Nitrogen

Causes a drop in ph lower than 6

46
Q

Acid rain effects

A

Leaving vital minerals from the soil causing death of trees
Lowering ph of rivers killing fish
Weather of buildings and structures made out of limestone, marble and iron

Chemistry Challenge (8 decks)

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