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GCSE Chem > paper 2 > Flashcards

paper 2 Flashcards

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1
Q

Concentration = (of a solution)

A

moles (mol) / volume of solution (dm^3)

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2
Q

Number of Moles = (in a solution)

A

concentration (mol/dm^3) x volume (dm^3)

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3
Q

Volume = (in a solution)

A

Moles (mol) / Concentration (mol/dm^3)

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4
Q

Grams per dm^3 =

A

Mass of chemical (g) / volume of solvent (dm^3)

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5
Q

Avagrado’s Law =

A

One mole of gas occupies 24 dm^3

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6
Q

Convert the moles of any gas at RTP to a volume:

A

Volume (dm^3) = Moles of gas x 24

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7
Q

Calculating volumes in reactions with known masses:

A

1) Calculate the moles of the known substance.
2) Find the moles of gas using the balanced equation.
3) Convert the moles into a volume using vol = mol x 24

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8
Q

Define Electrolysis:

A

Breaking down of a substance using electricity

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9
Q

What is Oxidation and Reduction?

A

Oxidation is the loss of electrons

Reduction is the gain of electrons

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10
Q

What is a cation?

A

positive ions in the electrolyte

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11
Q

What is a cathode?

A

The negative electrode

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12
Q

What is the anode?

A

The positive electrode

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13
Q

How does electrolysis occur?

A

An electric current is passed through an electrolyte (molten or dissolved ionic compound), causing it to decompose.

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14
Q

Why can molten ionic compounds be electrolylsed?

A

The ions can move freely

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15
Q

What is an ionic half equation?

A

They show what is happening at each electrode, (splits the equation up so it is easier to understand).

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16
Q

What is attracted to the cathode?

A

The Positive (+ve) ions are attracted to the cathode (-ve)

17
Q

What is attracted to the anode?

A

The Negative (-ve) ions are attracted to the anode (+ve).

18
Q

What are the electrodes made from?

A

Inert material so they don’t take part in the reaction.

19
Q

What is an electrochemical cell, and what components are in them?

A

A circuit made from an anode, cathode, electrolyte, power source and wires connecting the electrodes.

20
Q

Which inert elements are usually used in the electrodes?

A

Graphite or Platinum

21
Q

Why are aqueous solutions harder to electrolyse?

A

Aqueous solutions contain all the ions from the ionic compound as well as Hydrogen and Hydroxide ions from the water.

22
Q

What is the charge on ions

Hydrogen and Hydroxide

A 
Hydrogen = H+
Hydroxide = OH-
23
Q

At the cathode in an Aqueous solution, what happens if Hydrogen & Metal Ions are present?

A

If hydrogen is more reactive than the Metal then Hydrogen gas is produced.
If the Metal ion is more reactive than Hydrogen then a solid pure metal layer is produced.

24
Q

At the anode in an Aqueous solution, what happens is Hydroxide and Halide Ions are present?

A

Molecules of Chlorine, Bromine or Iodine will be formed.

25
Q

How many electrons are present in the outer shell of group 1 elements.

A

1 outer shell electron

26
Q

Why do atoms become more reactive as you move down the group? (in group 1)

A

The outer shell electron is further from the nucleus, meaning there is less attraction between them. The outer shell electron is more easily lost and they become more reactive.

27
Q

How many atoms does a Halogen need to gain to form a stable outer shell?

A

Needs to gain an electron and form a 1 - atom.

28
Q

Does reactivity decrease or increase for Halogens as they go down the group.

A

Reactivity decreases as the outer shell is further away from the nucleus so the attraction is weaker.

29
Q

What are reaction profiles?

A

Diagrams that show the relative energies of the reactants and products in a reaction, and how energy changes in the course of a reaction.

30
Q

In an reaction profile for an endothermic reaction, which has more energy, the products or reactants?

A

The products, as the energy is taken in during the reaction

31
Q

In an reaction profile for an exothermic reaction, which has more energy, the products or reactants?

A

The reactants, as energy is given out during the reaction

GCSE Chem (19 decks)

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