Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

old chemistry > Chemical changes > Flashcards

Chemical changes Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

How do metals react with air (oxygen)

A

Metal + oxygen —> metal oxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is oxidation?

A

Oxidation is the loss of electrons, gain of oxygen.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is reduction?

A

Reduction is the gain of electrons, loss of oxygen.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the arrangement of metals in reactivity series?

A 
Pottasium
Sodium 
Calcium
Magnesium
Aluminium
CARBON
Zinc 
Iron
HYDROGEN
Copper
Silver
Gold
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are displacement reactions?

A

A more reactive element can displace a less reactive element out of its compound during a chemical reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

How do metals and dilute acids react?

A

metal + acid –> salt + hydrogen

salt = (metal plus acid)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How do metals and water react?

A

metal + water –> metal hydroxide + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Relate the reactivity series to its tendency to form positive ions.

A

When metals react with other substances, the metal atoms lose electrons to form positive ions. (They lose an electron to gain a full outer shell).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are native metals?

A

Native metals are unreactive metals that are found in the Earth as the metal itself (no chemical reactions are needed to separate it as it is not part of a compound).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How can carbon be used to extract metals?

A

If a metal is less reactive than carbon, it can be extracted from its oxide by heating with carbon.
The carbon displaces the metal from the compound, and removes the oxygen from the oxide.
This leaves the metal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What happens with the ions in ionic displacement reaction equations?

A

Ions have to be the same on both sides. The less reactive metal loses the ions and gives it to the more reactive metal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are redox reactions?

A

Where both reduction and oxidation takes place.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is neutralisation?

A

Neutralisation is the reaction of an acid with a base that results in the pH moving towards 7.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is a base?

A

A base is a substance that can neutralize the acid by reacting with hydrogen ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are two examples of bases?

A

Metal oxides and alkalis.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What happens when you mix an acid and alkali?

A

Acid + alkali –> salt + water

Neutralises acid

17
Q

What happens when you mix an acid and metal oxide?

A

Acid + metal oxide –> salt + water

Neutralises acid

18
Q

What happens when an acid mixes with a metal carbonate?

A

Acid + metal carbonate —> salt + water + carbon dioxide

Neutralises acid

19
Q

How can soluble salt be made from acids?

A

Acid + insoluble reactant –> soluble salt

20
Q

What is the pH scale?

A

1 ———> 7 ———> 13

acid neutral alkali

21
Q

What is an acid in relation to hydrogen ions (H+)?

A

An acid is a substance that produces hydrogen ions, H+, when dissolved in water.

22
Q

What is an alkali in relation to hydroxide ions (OH-)?

A

An alkali is a substance that produces hydroxide ions, OH-, when dissolved in water.

23
Q

How does universal indicator work (pH scale)?

A

If universal indicator is added to a solution it changes to a colour that shows the pH of the solution.

24
Q

What are the terms concentration and dilute referring to (acids)?

A

A concentrated acid is one in which many acid molecules are dissolved in a set volume of solution, while a dilute acid will have very few molecules per unit volume.
CONCENTRATED = LOTS OF ACID MOLECULES
DILUTE = FEW ACID MOLECULES

25
Q

What are the terms weak and strong referring to (acids)?

A 
Weak = only slightly ionises in  an aqueous solution
Strong = completely ionised in an aqueous solution.
26
Q

Why do ionic compounds conduct electricity when dissolved in water or liquid?

A

Ionic compounds conduct electricity when liquid or in aqueous solution, because their ions are free to move from place to place. Ionic compounds cannot conduct electricity when solid, as their ions are held in fixed positions and cannot move.

27
Q

What are electrolytes?

A

A substance that breaks up into ions (particles with electrical charges) when it is dissolved in water. It can conduct electricity as its ions are free to move, allowing charge to flow.

28
Q

What are ions?

A

Particles that have electrical charge.

29
Q

What is electrolysis?

A

Electrolysis is the process by which ionic substances are broken down into simpler substances.
An electric current is passed through them.

30
Q

Describe the process of electrolysis (molten ionic compounds).

A

Positively charged ions move to the negative electrode (CATHODE). They receive electrons and are reduced.
Negatively charged ions move to the positive electrode (ANODE). They lose electrons and are oxidised.
OPPOSITES ATTRACT!

31
Q

How do you predict what will form at either the anode or cathode during electrolysis?

A

The METAL is formed at the CATHODE because that is where the positive metal ions are attracted.
The NON-METAL is formed at the ANODE where the negative non-metal ions are attracted.
OPPOSITES ATTRACT!

32
Q

Why are some metals extracted using electrolysis and not carbon?

A

Because the metals are more reactive than carbon.

33
Q

How do you extract metals using electrolysis?

A

EXAMPLE - aluminium
Aluminium oxide and want to make it just aluminium.
Positively charged aluminium ions gain electrons from the cathode, and form molten aluminium.
Oxide ions lose electrons at the anode, and form oxygen molecules.

34
Q

What are metal ions?

A

They are positively charged so are attracted the the negative electrode (CATHODE).

35
Q

Describe electrolysis of ionic compounds.

A

CATHODE:
The METAL is produced at the cathode if it is LESS RECATIVE than HYDROGEN.
HYDROGEN is produced at the cathode if the METAL if the metal is LESS REACTIVE.
ANODE:
OXYGEN is produced, unless HALIDE IONS (chloride, bromide or iodide ions) are present. In that case, the negatively charged halide ions lose electrons and form the corresponding halogen (CHLORINE, bromine or iodine).

36
Q

Which out of oxidation and reduction happens at the anode and cathode?

A

The reaction at the anode is oxidation.

The reaction at the cathode is reduction.

old chemistry (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions