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Chemistry Paper 1 > Chemical Changes > Flashcards

Chemical Changes Flashcards

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1
Q

From what pH’s is an acidic solution ?

A

0-6 pH

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2
Q

What pH is a neutral solution ?

A

7

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3
Q

What pH is a more alkaline solution?

A

8-14

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4
Q

How can you measure the pH of a solution ?

A

1) An indicator - use universal indicator to determine the pH. Add the dye to the solution and then compare to a pH chart
2) pH probe - attached to a pH meter and is measured electronically . A more accurate way of testing the pH

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5
Q

What type of ions do acids form in water ?

A

H+ ions

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6
Q

A base is a substance with a pH greater than ..

A

7

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7
Q

What type of ions does an alkaline in water make ?

A

OH- ions

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8
Q

A reaction between an acid and a base is called what …

A

A neutralisation reaction

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9
Q

What is the symbol equation for the neutralisation reaction ?

A

H+ (aq) + OH-(aq) = H20

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10
Q

Strong acids do what in water ?

A

Completely ionise

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11
Q

Weaker acids do not do what in water ?

A

Ionise completely

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12
Q

If the concentration of a H+ ion is higher …

means what for stronger and weaker acids

A

The rate of reactions will be faster so strong acids react faster than the weaker acid at the same concentration

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13
Q

What is the general formula to find the concentration of H+ ions from the pH?

A

Factor H+ ion concentration changes by = 10^(-X)

X = is the difference in the pH

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14
Q

An acids strength tells you what ?

A

The proportion of acid molecules ionise in water

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15
Q

The concentration of an acid tells you what ?

A

How much acid there is in a certain volume

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16
Q

X + Y = Salt + Water

What are X & Y ?

A

1) X = Acid
Y = Metal Oxide

2) X= Acid
Y= Metal Hydroxide

17
Q

Acid + Metal Carbonate = X + Y + Z

What are X , Y and Z?

A

X Salt
Y Water
Z Carbon Dioxide

18
Q

What does the reactivity series base how reactive the metals are ?

A

How easily they lose their electrons

The higher up the list they Are the more reactive

19
Q

What is in the reactivity series ?

A 
Potassium 
Sodium 
lithium 
Calcium 
Magnesium 
Carbon 
Zinc 
Iron 
Hydrogen 
Copper
20
Q

When a metal reacts with an acid how can you tell the sped of the reaction ?

A 
How quickly hydrogen bubbles are given off 
Temperature Change (mass & surface area have to be the same )
21
Q

Metal + Water = X + Y

What are X&Y?

A

X. Metal hydroxide

Y. Hydrogen

22
Q

Metals react with oxygen to form oxides . What do they metals need to be extracted from and what sort of a reaction is it ?

A

Ores

Oxidation

23
Q

What are the two ways to separate metals from their oxides ?

A

Oxidation

Reduction

24
Q

What does OIL RIG Stand for ?

A

OIL - oxidation is lose of electrons ( and gain of oxygen )

RIG - reduction is gain of electrons ( and lose of oxygen )

25
Q

Metal with higher reactivity have to be extracted by what and what are these metals ?

A

Electrolysis

Potassium , sodium , lithium , calcium , magnesium

26
Q

The less reactive metals are extract by what and what are these metals ?

A

Reduction using carbon & blast furnace ?

Zinc , iron , copper

27
Q

What is a redox reaction ?

A

When oxidation and reduction happens at the same time

28
Q

What is the rule for a displacement reaction ?

A

A more reactive metal will always displace a less reactive metal from its compound

29
Q

In dis placement reaction what happens to the metal ion and what happens to a metal atom ?

A

The metal ion gains electrons and is reduced

The metal atom loses electrons and is oxidised

30
Q

What happens during electrolysis ?

A

1) an electric current is passes through an electrolyte ( liquid or solution that can conduct electricity/ a molten or dissolved ionic compound ). The ions move towards the electrodes ( a solid that can conduct electricity and is submerged in the electrolyte) , where they will react and the compound will decompose.
2) Positive ions in the electrolyte will move towards the cathode (-ve) and gains electrons - reduction
3) Negative ions move towards the anode (+ve) and lose electrons -oxidation
4) This creates a flow of charge
5) The uncharged element will be discharge from the electrolyte

31
Q

Why can’t an ionic solid be electrolysed ?

A

Because the ions are in fixed positions and can’t move ?

32
Q

During electrolysis positive metal ions are …. And Negative
non - metal ions are …..

A

Positive metal ions are reduced at the cathode

Negative non - metal ions are oxidised at the anode

33
Q

In aqueous solutions there will be what type of ions from the water ?

A

Hydrogen ions and Hydroxide ions

34
Q

During electrolysis os an aqueous solution at the cathode , if H+ ions and and metal ions are present what will be produced if what happens ?

A

Hydrogen if the metal ions form an elemental element which is more reactive than hydrogen
However If the elemental metal is less reactive than hydrogen the a pure metal is produced instead

35
Q

What do half equations show ?

A

Show the reactions at the electrodes

Chemistry Paper 1 (2 decks)

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