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Chemistry > IAL Chemistry Topic 1 > Flashcards

IAL Chemistry Topic 1 Flashcards

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1
Q

Atom

A

An atom is the smallest part of an element that has the properties of that element.

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2
Q

Element

A

An element is chemically the simplest substances that cannot be broken down by chemical reactions.

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3
Q

Ion

A

Ion consists of one or more atoms joined together and have a positive or negative charge.

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4
Q

Spectator ion

A

Spectator ion is an ion that is not involved in the reaction.

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5
Q

Molecule

A

A molecule is a particle made of two or more atoms bonded together.

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6
Q

Compound

A

A compound is a pure substance that contains two or more different kinds of element that is chemically bonded. Its formation is a chemical change in which new substances are formed. It can be separated into its constituent by chemical methods.

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7
Q

Isotope

A

Isotopes of the atoms of the same element have the same number of protons and electrons but different numbers of neutrons.

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8
Q

Empirical formula

A

Empirical formula shows the smallest whole number ratio of atoms of each element in a compound.

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9
Q

Molecular formula

A

Molecular formula shows the actual number of atoms of each element present in a compound.

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10
Q

Mole

A

Mole is the amount of substance that contains the same number of particles as the number of carbon atoms in exactly 12g of the 12C isotope.

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11
Q

Avogadro constant

A

Avogadro constant is the number of particles in one mole of a substance which is 6.02 × 10^23 particles.

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12
Q

Mole equations

A

Moles= mass / molar mass
= number of particles / Avogadro’s constant
= molarity (concentration) × volume
= PV / RT
= volume (dm^3) / 24

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13
Q

Ionic equation

A

Ionic equation only shows the reacting ions and can be written for any reaction involving ion in solution. The ions not included are called spectator ions.

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14
Q

Relative atomic mass (Ar)

A

Relative atomic mass is the weighted mean mass of an atom relative to 1/12 of the mass of a carbon-12 atom.

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15
Q

Relative formula mass (Mr)

A

Relative formula mass is the sum of the relative atomic masses of atoms in a formula unit which is used for giant ionic structures.

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16
Q

Relative molecular mass (Mr)

A

Relative molecular mass is the sum of the relative atomic masses of atoms in a molecule.

17
Q

Molar mass (M)

A

Molar mass is the mass per mole of a substance measured in gmol^-1.

18
Q

ppm

A

ppm is the ratio of parts of solute to 1000000 parts of solution.

19
Q

Concentration

A

Concentration is the amount of solute dissolved per dm^3 of solution.

20
Q

Concentration equations

A

Concentration (g dm^-3) = Mass / Volume
Concentration (mol dm^-3) = Moles / Volume

21
Q

RTP

A

Room temperature and pressure
20 degree Celsius
1 atmospheric pressure

22
Q

Ideal gas law formula

A

PV = nRT

23
Q

Percentage yield formula

A

Percentage yield = (Actual yield/Theoretical yield) × 100%
(IN MOLES)

24
Q

Why might the actual yield of product be less than expected?

A
  1. Incomplete reaction
  2. Unwanted side reactions
  3. Practical losses (eg some solid may get lost when being transferred between beakers)
25
Q

Atom economy

A

Atom economy is a measure of the efficiency of the reaction. It looks at the amount of reactants that get turned into useful products.
(The higher the atom economy, the more sustainable and efficient the process.)

26
Q

Atom economy formula

A

Atom economy = (Molar mass of desired product / total molar mass of products) × 100%

27
Q

Displacement reaction

A

Displacement reaction occurs when an element replaces another element in a compound.

28
Q

Acid reacts with a metal equation + observations

A

Acid + metal –> salt + hydrogen
Observations:
1. Colourless gas produced
2. Gas produced burns with a burning splint to give a “pop” sound
3. Solution temperature increases as it is an exothermic reaction which releases heat
(Metal dissolves as the state changes from solid to aqueous state)
(Solution colour may change)

29
Q

Acid reacts with a metal oxide / insoluble metal hydroxide equation + observations

A

Acid + metal oxide –> salt + water
Acid + metal hydroxide –> salt + water
Observations:
1. Solution temperature increases
(Metal dissolves)
(Solution colour may change)

30
Q

Acid reacts with alkalis equation + observations

A

Acid + alkali –> salt + water (neutralisation)
Observations:
1. Temperature rises as it is an exothermic reaction

31
Q

Acid reacts with a metal carbonate (or metal sulphite) equation + observations

A

Acid + metal carbonate –> salt + water + carbon dioxide
Observations:
1. Gas bubbles formed
2. Solution temperature increases

32
Q

Acid reacts with hydrogencarbonates (or hydrogensulphite) equation + observations

A

Acid + metal hydrogencarbonates –> salt + water + carbon dioxide
Observations:
1. Gas bubbles formed
2. Solution temperature increases

33
Q

Application of acid + hydrogencarbonates

A
  1. Baking soda (NaHCO3 / sodium bicarbonate)
    HCO3- –> (heat) CO2 + H2O
    Baking soda and acid in lemon juice
    sodium hydrogencarbonate + citric acid –> sodium citrate + water + carbon dioxide
  2. Baking powder (NaHCO3)
    baking powder + solid acid cannot react
    NaHCO3 (s) –> (water) NaHCO3 (aq) + acid (aq)
    HCO3- + H+ –> H2O + CO2
  3. Fizzy drink tablet
    Vitamin C (s) + CaCO3 (s) –> (water) vitamin C (aq) + CO32- (aq)
    precaution: store in dry/cool place as carbonate decomposes under high temperature
  4. Eggshell in vinegar
    CaCO3 (s) + CH2COOH
    CO32- + H+ –> H2O + CO2
    Observations:
    -Eggshell dissolves
    -Gas bubbles fizzes
34
Q

Acid reacts with ammonia equation + observations

A

Acid + ammonia –> salt + (water)
(do not have to write water in equation)
(neutralisation process)

35
Q

Precipitation reactions

A

Precipitation reactions are reactions between two soluble salts which form an insoluble salt – the precipitate.
(note: precipitates can be extracted by filtration)

36
Q

Testing for carbonate or hydrogencarbonate ions

A

Add an aqueous acid and to test the gas produced with limewater

37
Q

Test for carbon dioxide

A

Carbon dioxide is bubbled through calcium hydroxide solution (limewater), a white precipitate of calcium carbonate is formed.
Ca(OH)2 + CO2 –> CaCO3 + H2O

38
Q

Test for sulphates

A

Addition of barium ions (from barium chloride or barium nitrate solutions)
SO42- + Ba2+ –> BaSO4

39
Q

Test for halides

A

Addition of silver ions (from silver nitrate solution)
Cl- + Ag+ –> AgCl

Chemistry (3 decks)

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