Gr.11 T4 Chemistry Flashcards

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1
Q

What is an acid according to the Arrhenius model?

Won’t need to spell

A

Ionises in water to produce the hydrogen ion

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2
Q

What is a base according to the Arrhenius model?

A

Ionises in water to produce the hydroxide ion

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3
Q

What is an acid according to the Bronsted-Lowry model?

A

A proton donor

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4
Q

What is an a base according to the Bronsted-Lowry model?

A

A proton acceptor

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5
Q

Ampholytes

A

A substance that can act as an acid or base

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6
Q

Learn common acids and bases on p.242

A

🌺

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7
Q

What are the 4 types of reactions of acids and bases?

A

Acid+metal ➡️ salt+hydrogen (electron transfer - redox rection)

Acid+metal hydroxide ➡️ salt+water (neutralisation)

Acid+metal oxide ➡️ salt+water

Acid+metal carbonate ➡️ salt+water+carbon dioxide

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8
Q

What are the properties of acids and bases?

A

Acids:
Taste sour.
Their aqueous solutions conduct electricity (called electrolytes)
React with certain metals to produce hydrogen gas
CO2 produced when acids react with limestone

Bases:
Taste bitter
Solutions of alkalis, bases that are soluble in water, conduct electricity (called electrolytes)
Generally feel slippery/ soapy

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9
Q

What is the colour of red litmus in an acid, base and neutral substance?

A

Acid: red

Base: blue

Neutral: red

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10
Q

What is the colour of blue litmus in an acid, base and neutral substance?

A

Acid: red

Base: blue

Neutral: blue

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11
Q

What is the colour of phenolphthalein in an acid, base and neutral substance?

A

Acid: colourless

Base: pink

Neutral: colourless

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12
Q

What is the colour of bromothymol blue in an acid, base and neutral substance?

A

Acid: yellow

Base: blue

Neutral: light green

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13
Q

What is the colour of methyl orange in an acid, base and neutral substance?

A

Acid: red

Base: orange

Neutral: orange

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14
Q

Indicators

A

Organic substances that change colour in acids and bases.

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15
Q

What is universal indicator?

A

A mixture of dyes that can change into many different colours. (Shows the full range of pH colours)

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16
Q

Titation

A

A process used to neutralise an acid or base and to determine the concentration of an unknown solution.

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17
Q

Oxidation

A

A loss in electrons

18
Q

Reduction

A

A gain in electrons

19
Q

Oxidation number/ oxidation state

A

A number assigned to each atom to keep track of electrons during a reaction

20
Q

Give one exception to oxygen having an oxidation state of -2 (the only one I need to know)

A

H O
2 2

Oxygen has an oxidation state of -1

21
Q

What is a reducing agent?

A

A substance that causes reduction but it itself is oxidised

22
Q

What is an oxidising agent?

A

A substance that causes oxidation but it itself is reduced

23
Q

What is a redox reaction?

A

The transfer of electrons

24
Q

When does a hydrogen ion have an oxidation state of +1 and when does it have an oxidation state of -1?

A

+1 when bonded to non-metals

-1 when bonded to metals

25
Q

What are the 3 classifications of redox reactions?

A
  1. Displacement reaction
  2. Synthesis reaction (2+ reactants, 1 product)
  3. Decomposition reaction (1 reactant, 2+ products)
26
Q

What are the tests for oxygen gas and hydrogen gas?

A

Oxygen gas: glowing splint relights

Hydrogen gas: burning split ignites gas with popping sound

27
Q

Electrochemical reaction

A

Oxidation and reduction take place in separate compartments

28
Q

What energy transformation happens in an electrochemical reaction?

A

Chemical energy becomes electrical energy

29
Q

Electrochemical cell

A

Energy from the redox reaction is used as a source of electric current

30
Q

What happens at the anode and the cathode (oxidation/ reduction)? Does this cause the electrode to increase or decrease in mass?

A

Anode: oxidation (electrode decreases in mass)

Cathode: reduction (electrode increases in mass)

31
Q

What are the two functions of the salt bridge in an electrochemical cell?

A

It completes the circuit and it ensures that the electrolytes remain neutral

32
Q

Give the formula for the dichromate ion

A

-2
Cr O
2 7

33
Q

In electrochemical cells, electrons flow through the wire and ions flow through the salt bridge and electrolytes

A

🌺

34
Q

What is an electrochemical cell called if it has:

1) a spontaneous chemical reaction between chemicals
2) a non-spontaneous chemical reaction driven by chemical energy

A

1) galvanic cell (or voltaic cell)

2) electrolytic cell

35
Q

What is the name of the process that occurs in an electrolytic cell?

A

Electrolysis

36
Q

Cell potential

A

The potential difference between the cathode and anode

37
Q

What is a standard electrode potential?

A

The voltage measured under standard conditions when the half-cell is connected to a standard hydrogen electrode to form an electrochemical cell. (Measured in V)

38
Q

What are standard conditions?

A

p = 1 atm
-3
c = 1 mol.dm

temp.= 25*C

39
Q

Why is a platinum electrode used in a hydrogen half-cell?

A

It is chemically inert and a good electrical conductor.

40
Q

Look at how to write equations using table 4A

A

🌺