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Chemistry A Level > 2.1 Atoms and reactions > Flashcards

2.1 Atoms and reactions Flashcards

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1
Q

What is the relative charge and relative mass of an electron?

A

Relative charge: -1

Relative mass: 1/2000

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2
Q

What is the relative charge and relative mass of a neutron?

A

Relative charge: 0

Relative mass: 1

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3
Q

What is the relative charge and relative mass of a proton?

A

Relative charge: +1

Relative mass: 1

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4
Q

What is the mass number?

A

The number of protons and neutrons

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5
Q

What is the atomic number?

A

The number of protons

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6
Q

What are ions?

A

Atoms that have lost/gained electrons

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7
Q

What are isotopes?

A

Isotopes are elements with the same number of protons but different number of neutrons

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8
Q

What is the relative atomic mass (Ar)?

A

The weighted mean mass of an atom of an element compared to 1/12th of the mass of an atom of carbon-12

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9
Q

What is the relative molecular mass (Mr)?

A

Mean mass of a molecule, compared to 1/12th of the mass of an atom of carbon-12

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10
Q

What is the relative isotopic mass?

A

The mass of an atom of an isotope, compared to 1/12th of the mass of an atom of carbon-12

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11
Q

How can you calculate relative atomic mass?

A

(Abundance of A x mass) + (Abundance of B x mass) / total abundance

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12
Q

How are ions created?

A

Ions are created when electrons are transferred from one atom to another. They attract each other to form compounds.

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13
Q

What is the formula of these molecular ions:

  • Hydroxide
  • Nitrate
  • Ammonium
  • Sulfate
  • Carbonate
  • Zinc ion
  • Silver ion
A
  • OH−
  • NO3−
  • NH4+
  • (SO4)2−
  • (CO3)2−
  • Zn2+
  • Ag+
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14
Q

What is the meaning of hydrated and anhydrous?

A

Hydrated- with water

Anhydrous- without water

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15
Q

What is water of crystallisation?

A

When water molecules exist within crystal structures we call this water of crystallisation. For every mole of salt you have a certain number of moles of water of crystallisation. We write this as XH20

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16
Q

How can you calculate water of crystallisation?

A
  1. Write out the 2 molecules
  2. Write the masses of each molecule
  3. Find moles by doing n=m/Mr
  4. Divide all the numbers by the smallest number of moles
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17
Q

What are spectator ions?

A

Ions that don’t get involved in the reaction but are present

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18
Q

What is the mole used to measure?

A

Amount of substance

19
Q

What is Avogadro’s number?

A

1 mole= 6.02 x 10 ^23 (Avogadro’s number)

20
Q

What is the equation for the number of particles?

A

Number of particles= Avogadro’s Number x Number of moles

21
Q

How can you calculate the number of moles using concentration and volume?

A

Number of moles= concentration x volume

22
Q

What is the ideal gas equation?

A

pV= nRT

23
Q

How can you work out theoretical mass?

A
  1. Write out the balanced equation
  2. Work our the Ar/Mr of species involved
  3. Divide to find 1g and then multiply by the number of grams in the question. Do the same to the other side.
24
Q

What is the empirical formula and how do you work it out?

A

The empirical formula is the simplest whole number ratio of elements in a compound.

The steps are:

  1. Write out the elements involved
  2. Write the percentages as masses
  3. Divide the masses by relative atomic mass to get number of moles
  4. Divide the numbers by the smallest number of moles
25
Q

How do you work out percentage yield?

A

Percentage yield= actual yield/theoretical yield x100

26
Q

How do you work out percentage atom economy?

A

% atom economy= molecular mass of desired product/sum of molecular masses of all products x 100

27
Q

Why is atom economy important? (3 marks)

A
  • High atom economies produce less waste and benefit the environment
  • It also means that raw materials are used more efficiently which is more sustainable
  • Less by-products are produced which means less time and money is spent separating these from the desired product
28
Q

Acids are known as proton ____

Bases are known as proton ____

A

donors

acceptors

29
Q

What is an alkali?

A

An alkali is a soluble base. They produce OH- ions when added to water

30
Q

What ions do acids produce when added to water?

A

H+

31
Q

What is the difference between strong acids and weak acids and strong bases and weak bases in terms of ions produced?

A

Weak acids don’t produce many H+ ions. Strong acids produce lots of H+ ions. Weak bases produce few OH- ions and strong bases produce lots of OH- ions.

32
Q

What is produced when a metal reacts with an acid?

A

Salt and hydrogen

33
Q

What is produced when a metal oxide reacts with an acid?

A

Salt and water

34
Q

What is produced when a metal hydroxide reacts with an acid?

A

Salt and water

35
Q

What is produced when a metal carbonate reacts with an acid?

A

Salt, carbon dioxide and water

36
Q

How do you carry out a titration?

A
  1. Have an acid/alkali with a known concentration in the burette
  2. Have an acid/alkali with an unknown concentration but known volume in the conical flask and add a few drops of indicator
  3. Add the chemical in the burette to the conical flask until it changes colour (end point)
  4. Read how much of the chemical was added from the burette to neutralise the chemical in the conical flask (read below the meniscus)
  5. Repeat until you get two concordant results (within 0.10cm^3 of each other)
37
Q

What is a standard solution?

A

A solution with a known concentration

38
Q

How are standard solutions made? Describe the process.

A

Standard solutions are made from solids with a known mass dissolved in water to fixed volume in a volumetric flask

  1. Weigh out the amount of solid precisely using a balance and weighing boat
  2. Transfer the solid from the weighing boat to a beaker. Wash any solid left behind into the beaker using distilled water
  3. Dissolve the solid
  4. Transfer the solution to a volumetric flask using a funnel and rinse the beaker and glass rod with water
  5. Use more water to fill up to the graduation line. Use a pipette as you start to get closer to the line
  6. Invert the flask a few times to mix it
39
Q

What does OIL RIG stand for?

A

Oxidation Is Loss

Reduction Is Gain

40
Q

What is a redox reaction?

A

When a reaction involves reduction and oxidation

41
Q

What are reducing and oxidising agents?

A

Reducing agents lose electrons and are oxidised themselves

Oxidising agents gain electrons and are reduced themselves

42
Q

What are the oxidation state rules? (9)

A
  1. Elements in their natural state have an oxidation number of 0
  2. In simple ions the oxidation number is the same as the charge on the ion
  3. Group 1 have an oxidation number of +1
  4. Group 2 always have an oxidation number of +2
  5. Group 3 always have an oxidation number of +3
  6. Hydrogen is always +1 (except in hydrides where it is -1)
  7. Chlorine is always -1 (except in a compound with F and O where it is positive)
  8. Fluorine always -1
  9. Oxygen always -2 (except in peroxides where it is -1)
43
Q

What must all the oxidation number add up to?

A

The overall charge on the molecule

Chemistry A Level (6 decks)

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