Brainscape's Knowledge GenomeTM

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


See full index

ScienceKS3 > Y10 Autumn Term Chemistry Roundup > Flashcards

Y10 Autumn Term Chemistry Roundup Flashcards

1
Q

What can you do to measure the rate of a reaction?

A

To measure the rate of a reaction you can:
- Measure how fast the reactants are used up
- Measure how fast the products are made

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

Name some examples of how you can measure the rate of reaction.

A

1) Measure mass due to gas formed
2) Measure volume of gas produced
3) Measure time for soluble product to form

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

What is the equation for working out the rate of a reaction?

A

Rate = Volume of gas / time (cm/s)

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

What is collision theory?

A

Collision theory is the term for what is needed for a reaction to take place

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

What do the reactants need to do for a reaction to happen?

A

The reactants need to:
- Collide with enough energy (activation energy)
- A successful collision is one that leads to a reaction
- So to increase the rate of reaction you must either:
a) Increase the frequency/energy of collisions
b) Decrease the energy needed for a collision to be successful
- Factors that effect the rate are concentration + pressure
- The more particles there are in the same space the more collisions will happen

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

How does surface area effect the rate of reaction?

A

The more particles that are available to react = the more frequently collisions will occur

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

How does temperature effect the rate of reaction?

A

Particles move faster so they collide more frequently. Particles collide with more energy so more collisions are successful.

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

How do catalysts effect the rate of reaction?

A
  • Lower energy needed for successful collisions
  • Not used up
  • Biological catalysts = enzymes
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are reversible reactions?

A

Reactions that can go in both directions. If a reaction is exothermic one way it’ll be endothermic in the other.

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

What is a closed system?

A

A system where nothing can get in or out

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

What is equilibrium?

A

Equilibrium is where the rate of reaction is the same on both sides

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

What happens at equilibrium?

A
  • Rate of forward reaction = rate of backward reaction
  • Amount of products + reactants don’t change
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Name the metals of the reactivity scale in order of most to least reactive

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum

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

What does reactivity depend on?

A

Reactivity depends on tendency to form a metal ion

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

What are other names for positive and negative ions

A

Cations (positive) + Anions (negative)

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

What does OILRIG stand for?

A

Oxidation
Is
Loss of electrons
Reduction
Is
Gain of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What happens to metals when you react them with:
a) Oxygen
b) Water
c) Acid

A

a) Metal oxide
b) Metal hydroxide + hydrogen
c) Metal salt + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What happens to acids when you react the with:
A) metal
B) alkali
C) insoluble gas
D) carbonate

A

A) salt + hydrogen
B) salt + water
C) salt + water
D) salt + water + carbon dioxide

19
Q

How do you prepare a dry sample of a soluble salt?

A

1) Choose correct acid + Add base to excess
2) Warm
3) Filter off excess
4) Evaporate of water

20
Q

Which number(s) are considered acidic on the pH scale?

A

1-6

21
Q

Which number(s) are considered neutral on the pH scale?

A

7

22
Q

Which number(s) are considered alkaline on the pH scale?

A

8-14

23
Q

What happens to strong acids in water

A
  • Completely ionises in water
  • Breaks down fully into ions
  • Hydrogen = positive
24
Q

What happens to weak acids in water?

A
  • Only partially ionises in water
  • Only some acid molecules split up
  • Amount of H+ ions = less pH is higher
25
Q

What is electrolysis?

A

Electrolysis is a technique that uses direct electric current to drive an otherwise non-spontaneous chemical reaction using negative non-metal ions + positive metal ions

26
Q

What happens at the cathode of electrolysis of molten?

A

Pb 2+ + 2e- ——> Pb

27
Q

What happens at the anode of electrolysis of molten?

A

2Br- ——> Br2 + 2e-
or
2Br- — 2e- —> Br2

28
Q

What happens at the cathode of electrolysis of solutions?

A

Least reactive

29
Q

What happens at the anode of electrolysis of solutions?

A

Halide (Gp 7) + Oxygen

30
Q

What is quantitative chemistry? (1)

A

The law of conservation of mass states that no atoms are lost/made during a chemical reaction so the mass of the products = mass of the reactants.

31
Q

What is quantitative chemistry? (2)

A

In a balanced equation, the sum of the relative formula masses of the reactants in the quantities shown = the sum of the relative formula masses of the products in the quantities shown.

32
Q

What is quantitative chemistry? (3)

A

When a metal reacts w/ oxygen the mass of the oxide produced > the mass of the metal.

33
Q

What is quantitative chemistry? (4)

A

In thermal decompositions of metal carbonates, carbon dioxide is produced + escapes into the atmosphere leaving the metal oxides as the only solid product.

34
Q

What is quantitative chemistry? (5)

A

The masses of the reactants + products can be calculated from balanced (symbol) equations. Chemical equations can be interpreted in terms of moles. Shows that 1 mole of magnesium reacts w/ 2 moles of hydrochloric acid to produce 1 mole of magnesium chloride + 1 mole of hydrogen gas.

35
Q

What is quantitative chemistry? (6)

A

In a chemical reaction involving 2 reactants, it’s common to use an excess of 1 of the reactants to ensure that all of the other reactant is used up.

36
Q

What is quantitative chemistry? (7)

A

The percentage atom economy of a reaction is calculated using the balanced equation.

37
Q

What is Avogadro Constant?

A

The number of atoms/molecules/ions in a mole of any substance

38
Q

What is a Mole?

A

The amount of substance in the relative atomic/formula mass of a substance in grams. Unit symbol = mol.

39
Q

What is Concentration?

A

The amount of substance dissolved in a given volume of liquid.

40
Q

What is a Limiting Reactant?

A

The reactant in a chemical reaction that when used up causes the reaction to stop.

41
Q

What is Percentage Yield?

A

The actual mass of of product collected in a reaction / the maximum mass that could’ve been formed in theory x 100. Amount obtained = yield.

42
Q

What is Relative Formula Mass (Mr)?

A

The total of the relative atomic masses added up in the ratio shown in the chemical formula of substance.

43
Q

What is Relative Atomic Mass (Ar)?

A

The average mass of the atoms of an element compared w/ carbon (=12). The average mass must take into account the proportions of the naturally occurring isotopes of the element.

44
Q

What is the formula triangle for this?

A

Mass = moles x Mr

ScienceKS3 (18 decks)

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