Chemistry Unit 1

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WJEC A-Level Chemistry

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264 Terms

1
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Formulae of Sulfur Dioxide

SO2

2
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Formulae of Methane

CH4

3
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Formulae of Hydrochloric Acid

HCl

4
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Formulae of Sulfuric Acid

H2SO4

5
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Formulae of Nitric Acid

HNO3

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Formulae of Ammonia

NH3

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Formulae of Ammonium Chloride

NH4Cl

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Formulae of Sodium Hydroxide

NaOH

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Formulae of Sodium Chloride

NaCl

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Formulae of Sodium Carbonate

Na2CO3

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Formulae of Sodium Hydrogencarbonate

NaHCO3

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Formulae of Sodium Sulfate

Na2SO4

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Formulae of Calcium Hydroxide

Ca(OH)2

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Formulae of Calcium Carbonate

CaCO3

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Formulae of Calcium Chloride

CaCl2

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Formulae of Copper (II) Oxide

CuO

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Formulae of Copper (II) Sulfate

CuSO4

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How to find charge of ion?

Use group number

e.g. group 7 has charge of -

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Charge for Hydrogencarbonate

HCO3-

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What is a redox reaction?

A reaction where one substance is reduced and another is oxidised.

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What is a reducing agent?

  • reduce other species

  • give electrons

  • are themselves oxidised

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What is a oxidising agent?

  • oxidise other species

  • accept electrons

  • are themselves reduced

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What is the oxidation of an uncombined element?

0

e.g. O2 = 0

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What is the oxidation of a simple ion?

Charge of the ion

e.g. O2- = -2

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What is the oxidation of a compound?

The sum must equal 0

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What is the oxidation of group 1 and 2 metals in a compound?

Same as their group number

e.g. BaSO4 = Ba=+2

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What is the oxidation of a complex ion?

The sum must equal the charge

e.g. CO32- = C=+4, O=-2

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What is the oxidation of Hydride?

H = -1

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What is the oxidation of Fluorine?

F = -1

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What is the oxidation of Peroxide?

O = -1

31
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Steps to work out ionic equations

  1. word equation

  2. balanced symbol equation

  3. balanced ionic equation (usually for precipitate (s) )

  4. spectator ions

<ol><li><p>word equation</p></li><li><p>balanced symbol equation</p></li><li><p>balanced ionic equation (usually for precipitate (s) )</p></li><li><p>spectator ions</p></li></ol><p></p>
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Charge for Hydroxide

OH-

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Charge for Nitrate

NO3-

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Charge for Oxide

O2-

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Charge for Sulfide

S2-

36
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Charge for Carbonate

CO32-

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Charge for Sulfate

SO42-

38
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Charge for Phosphate

PO43-

39
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Charge for Ethanoate

CH3COO-

40
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What is the mass/charge of proton/neutron/electrons?

knowt flashcard image
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What charge does the nucleus have?

Positive - contains protons and neutrons

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What charge does an atom have in general?

Neutral - same amount of protons and electrons

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What is an ion?

Charged atoms caused by the gain or loss of electrons

44
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What is an isotope?

Atoms of the same element with a different number of neutrons.

45
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Alpha particle

  • Helium nucleus

  • Mass - 4 units

  • Absorbed by - paper or few cm of air

  • High ionising power

<ul><li><p>Helium nucleus</p></li><li><p>Mass - 4 units</p></li><li><p>Absorbed by - paper or few cm of air</p></li><li><p>High ionising power</p></li></ul><p></p>
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Beta particle

  • Fast moving electron

  • Mass - negligible

  • Absorbed by - Aluminium

  • Medium ionising power

<ul><li><p>Fast moving electron</p></li><li><p>Mass - negligible</p></li><li><p>Absorbed by - Aluminium</p></li><li><p>Medium ionising power</p></li></ul><p></p>
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Gamma ray

  • Electromagnetic wave

  • Mass - 0

  • Absorbed by - thick lead

  • Low ionising power

<ul><li><p>Electromagnetic wave</p></li><li><p>Mass - 0</p></li><li><p>Absorbed by - thick lead</p></li><li><p>Low ionising power</p></li></ul><p></p>
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Electric field effect on radioactive particles

  • Beta - light so fully attracted

  • Alpha - heavy so slightly attracted

<ul><li><p>Beta - light so fully attracted</p></li><li><p>Alpha - heavy so slightly attracted</p></li></ul><p></p>
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Alpha decay

  • mass number decreases by 4

  • atomic number decreases by 2

<ul><li><p>mass number decreases by 4</p></li><li><p>atomic number decreases by 2</p></li></ul><p></p>
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Beta decay

  • mass number remains the same

  • atomic number increases by 1

<ul><li><p>mass number remains the same</p></li><li><p>atomic number increases by 1</p></li></ul><p></p>
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Positron

  • mass number remains the same

  • atomic number decreases by 1

<ul><li><p>mass number remains the same</p></li><li><p>atomic number decreases by 1</p></li></ul><p></p>
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Electron capture

  • mass number remains the same

  • atomic number decreases by 1

<ul><li><p>mass number remains the same</p></li><li><p>atomic number decreases by 1</p></li></ul><p></p>
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Why is ionising radiation unsafe for humans?

Damages cells and DNA causing mutations to occur

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What are the safe uses of radioactivity?

  • tracers

  • carbon dating

  • smoke alarms

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What is tracers?

  • radioactive isotopes are inserted into a sample and tracked using x-rays

  • medical tracers/water pipe blockages/biochemistry of plants

  • must be low ionising power and short half life if used in the body

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What is carbon dating?

  1. Carbon-14 is a beta emitter

  2. When an organism is living the amount of Carbon-14 is consistent

  3. When an organism dies the amount of Carbon-14 decreases

  4. This allows scientists to determine the age of organisms that have been dead for many years

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What is half life?

Time taken for the mass/activity of a radioactive isotope to fall to half of its original value

58
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What is an orbital?

Volume where there is a high probability of finding an electron

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How many electrons can each orbital have?

2 electrons each

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S orbital

  • spherical

  • all energy levels

  • groups of 1

  • size increases with energy level

<ul><li><p>spherical</p></li><li><p>all energy levels</p></li><li><p>groups of 1</p></li><li><p>size increases with energy level</p></li></ul><p></p>
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P orbital

  • dumbbell shape

  • all energy levels except n=1

  • groups of 3

  • lobes become longer and larger with energy level

<ul><li><p>dumbbell shape</p></li><li><p>all energy levels except n=1</p></li><li><p>groups of 3</p></li><li><p>lobes become longer and larger with energy level</p></li></ul><p></p>
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How many D orbitals are in a group?

groups of 5

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How many F orbitals are in a group?

groups of 7

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How many G orbitals are in a group?

groups of 9

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What is the order of orbitals?

S, P, D, F, G

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Subshells

knowt flashcard image
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What is the electronic configuration?

gives information on atom

<p>gives information on atom</p>
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What are the rules of electronic confurguration?

  1. Put electron in lowest possible energy level as there’s more energy away from nucleus

  2. Fill electrons into orbitals singly before adding 2 electrons to minimise electron repulsion

<ol><li><p>Put electron in lowest possible energy level as there’s more energy away from nucleus</p></li><li><p>Fill electrons into orbitals singly before adding 2 electrons to minimise electron repulsion</p></li></ol><p></p>
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Example of electronic configuration

knowt flashcard image
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Exceptions to the electronic configuration rules

Copper and Chromium

  • Orbitals are more stable if half-filled or fully-filled

  • 4s and 3d are similar in energy one electron can move from 4s to 3d

Copper - [Ar] 4s1 3d10

Chromium - [Ar] 4s1 3d5

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What is the Molar first ionisation energy?

The energy needed to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions

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What is the equation for Molar first ionisation energy?

X(g) X+(g) + e-

X4+(g) X5+(g) + e-

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What happens down a group with Molar first ionisation energy?

  • distance from nucleus increases

  • shielding from inner electrons increases

  • weaker electrostatic forces of attraction

  • outer electron easier to remove

<ul><li><p>distance from nucleus increases</p></li><li><p>shielding from inner electrons increases</p></li><li><p>weaker electrostatic forces of attraction</p></li><li><p><strong>outer electron easier to remove</strong></p></li></ul><p></p>
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What happens across a period with Molar first ionisation energy?

  • increased nuclear charge

  • outer electron harder to remove

<ul><li><p>increased nuclear charge</p></li><li><p><strong>outer electron harder to remove</strong></p></li></ul><p></p>
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What happens in successive ionisation energy?

A single atom loses it’s electrons one by one

  • outer electron is easiest to remove as most shielding and furthest

  • 3rd shell/2nd shell harder to remove as closer, slowly increases as protons are holding electrons more tightly because charge becomes imbalanced (effective nuclear charge)

  • 1st shell hardest as no shielding and closest

<p>A single atom loses it’s electrons one by one</p><ul><li><p>outer electron is easiest to remove as most shielding and furthest</p></li><li><p>3rd shell/2nd shell harder to remove as closer, slowly increases as protons are holding electrons more tightly because charge becomes imbalanced (effective nuclear charge)</p></li><li><p>1st shell hardest as no shielding and closest</p></li></ul><p></p>
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Order of electromagnetic spectrum

knowt flashcard image
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What is quantisation?

The amount of energy that the molecule can absorb/emit and is a specific value, this allows us to identify a molecule

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Energy =

energy (J) = Planck’s constant x frequency (Hz)

<p>energy (J) = Planck’s constant x frequency (Hz)</p>
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Speed of light =

speed of light = frequency (Hz) x wavelength (m)

<p>speed of light = frequency (Hz) x wavelength (m)</p>
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Absorption spectra

  1. Electrons are in ground state so lowest energy levels

  2. Giving atoms energy can cause electrons to move to a higher energy level. They are then in an excited state

  3. The difference between energy levels is a fixed value

  4. The energy relates to a particular frequency (E=hf), the frequency relates to a specific wavelength/colour of light (C=fλ)

  5. The missing wavelengths show dark bands on a coloured background

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Emission spectra

  1. Electrons have been absorbed so in an excited state

  2. The electron falls to a lower energy level

  3. The difference between energy levels is a fixed value

  4. The energy relates to a particular frequency (E=hf), the frequency relates to a specific wavelength/colour of light (C=fλ)

  5. The emitted wavelengths show coloured bands on a dark background

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Atomic spectrum of Hydrogen

knowt flashcard image
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Why is the spectrum a series of lines?

Each line is equal to the difference in energy between particular energy levels which is a fixed value

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Why do the lines converge?

The energy levels become closer and eventually converge

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What is the significance of the convergence limit?

In the Lymans series, it is the ionisation energy

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Lyman series

  • UV part of spectrum

  • electron moves to and from 1st energy level

  • convergence limit tells us ionisation energy

  • highest energy

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Balmer series

  • visible part of spectrum

  • electron moves to and from 2nd energy level

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Paschen series

  • infrared part of spectrum

  • electron moves to and from 3rd energy level

  • lowest energy

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Series on a graph

knowt flashcard image
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What is the relative isotopic mass?

The mass of an atom of an isotope relative to one-twelfth the mass of one atom of carbon-12.

e.g. 35Cl has a relative isotopic mass of 35

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What is the relative atomic mass (Ar)?

The average mass of one atom of the element relative to one-twelfth the mass of one atom of carbon-12.

  • found on a periodic table

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What is the relative formula mass (Mr)?

The average mass of a molecule relative to one-twelfth the mass of one atom of carbon-12.

  • add up all the Ar

e.g. CaCO3 40.1 + 12 + (16×3) = 100.1

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What is a mole?

One mole is the amount of substance that contains the same number of particles as there are atoms of carbon in exactly 12g of carbon-12.

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Mass =

Mr x moles

<p>Mr x moles</p>
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What is the molar mass?

One mole of any substance has a mass equivalent to the Mr of that substance in grams (gmol-1).

e.g. MgCl2 - Mr=95.3, molar mass = 95.3 gmol-1

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What is the empirical formula?

Simplest formula of a substance

  1. symbol of elements

  2. % or mass

  3. Ar

  4. moles

  5. divide by smallest mole

  6. ratio

<p>Simplest formula of a substance</p><ol><li><p>symbol of elements</p></li><li><p>% or mass</p></li><li><p>Ar</p></li><li><p>moles</p></li><li><p>divide by smallest mole</p></li><li><p>ratio</p></li></ol><p></p>
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How to calculate reacting masses?

  1. balanced equation

  2. moles of one

  3. ratio for moles of what we need

  4. mass=mrxmoles

<ol><li><p>balanced equation</p></li><li><p>moles of one</p></li><li><p>ratio for moles of what we need</p></li><li><p>mass=mrxmoles</p></li></ol><p></p>
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Percentage yield =

mass of product obtained / maximum theoretical mass x 100

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Why will percentage yield always be less than 100%?

Due to loss of product during transfer,separation or an incomplete reaction

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Atom economy =

mass of required product / total mass of reactants x 100