Topic: Fundamentals Archives - TutorMyself Chemistry

Fundamentals quiz

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Hydr0Gen2020-02-16T15:32:22+00:00Categories: Uncategorized|Tags: Quiz, Topic: Fundamentals|

Flashcards: Fundamentals

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Fundamentals flashcards

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Hydr0Gen2019-08-28T14:00:28+00:00Categories: Uncategorized|Tags: Chemistry, Flashcards, GCSE, Topic: Fundamentals|

Q&A slides – Fundamentals

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Hydr0Gen2019-11-12T07:40:50+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Q&A slides, Topic: Fundamentals|

1:01 understand the three states of matter in terms of the arrangement, movement and energy of the particles

Solid

Arrangement: Particles are close together and regularly packed.

Movement: Particles vibrate around a fixed point.

Energy: Particles have less kinetic energy than both liquids and gasses.

Liquid

Arrangement: Particles are close together but irregular.

Movement: Particles are free to move.

Energy: Particles have less kinetic energy than gasses but more than solids.

Gas

Arrangement: Particles are far apart and there are no forces between them.

Movement: Particles are free to move.

Energy: Particles have more kinetic energy than liquids and solids.

Hydr0Gen2022-11-29T13:49:09+00:00Categories: (a) States of matter, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:01, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Fundamentals|

States of matter – video

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Sam Mahal2022-09-14T15:10:26+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Fundamentals, Video|

1:02 understand the interconversions between the three states of matter in terms of: the names of the interconversions, how they are achieved and the changes in arrangement, movement and energy of the particles

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Melting: When a solid is heated, the energy makes the particles vibrate fast enough so that the forces of attraction between the particles break. For example H₂O(s) –> H₂O(l)

Freezing: When a liquid is cooled, the particles move slow enough so that the forces of attraction between them will hold them into a solid. For example H₂O(l) –> H₂O(s)

Boiling: When a liquid is heated strongly, the energy makes the particles move fast enough so that all forces of attraction are broken. For example H₂O(l) –> H₂O(g)

Condensing: When a gas is cooled, the particles move slow enough so that the forces of attraction between them will hold them as a liquid. For example H₂O(g) –> H₂O(l)

Sublimation: A small number of substances have the ability to change directly from a solid to a gas when heated. For example CO₂(s) –> CO₂(g)

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Hydr0Gen2022-11-30T13:57:13+00:00Categories: (a) States of matter, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:02, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Fundamentals|

1:08 understand how to classify a substance as an element, a compound or a mixture

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Element: The simplest type of substances made up of only one type of atom.

Compound: A substance that contains two or more elements chemically joined together in fixed proportions.

Mixture: Different substances in the same space, but not chemically combined.

Note: elements such as oxygen (O₂) are described as diatomic because they contain two atoms.

The full list of elements that are diatomic is:

Hydrogen (H₂)
Nitrogen (N₂)
Fluorine (F₂)
Oxygen (O₂)
Iodine (I₂)
Chlorine (Cl₂)
Bromine (Br₂)

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Hydr0Gen2022-11-30T13:57:56+00:00Categories: (b) Elements, compounds and mixtures, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:08, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Fundamentals|

Element, compounds mixture – video

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Sam Mahal2022-09-14T15:12:03+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Fundamentals, Video|

Harry Potter does The Elements – video

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Watch Daniel Radcliffe sing the names of all the elements – it’s just a shame there are now more elements than were written into Tom Lehrer’s famous song…..

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Hydr0Gen2019-02-10T18:43:37+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Fundamentals, Video|

1:09 understand that a pure substance has a fixed melting and boiling point, but that a mixture may melt or boil over a range of temperatures

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Pure substances, such as an element or a compound, melt and boil at fixed temperatures.

However, mixtures melt and boil over a range of temperatures.

Example: although pure water boils at 100⁰C, the addition of 10g of sodium chloride (NaCl) to 1000cm³ of water will raise the boiling point to 100.2⁰C.

Example: although pure water melts at 0⁰C, the addition of 10g of sodium chloride (NaCl) to 1000cm³ of water will lower the melting point to -0.6⁰C.

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Hydr0Gen2023-05-11T16:37:43+00:00Categories: (b) Elements, compounds and mixtures, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:09, Chemistry, ChemistrySpecPointsNew2019, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Fundamentals|

1:14a know what is meant by the terms atom

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Atom: An atom is the smallest part of an element.

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Hydr0Gen2019-05-23T15:17:51+00:00Categories: Uncategorized|Tags: 1:14a, Chemistry, Double, GCSE, GCSE_Chemistry_SpecPoint, SpecPoint, SubSpecPoint, Topic: Fundamentals|

1:15 know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles

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An atom consists of a central nucleus, composed of protons and neutrons.

This is surrounded by electrons, orbiting in shells (energy levels).

Atoms are neutral because the numbers of electrons and protons are equal.

	Mass	Charge
Proton	1	+1
Neutron	1	0
Electron	negligible (1/1836)	-1

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Hydr0Gen2022-11-30T14:11:04+00:00Categories: (c) Atomic structure, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:15, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Calculations, Topic: Fundamentals, Topic: Simple Molecules & Covalent Bonding|

Atomic structure – Tyler de Witt video

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This video explains the basics of atomic structure, telling you what is inside an atom:

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Hydr0Gen2022-09-15T08:42:42+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Calculations, Topic: Fundamentals, Video|

Build an atom – interactive

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This is a good interactive demonstration showing how subatomic particles make up the atoms in the Periodic Table.

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Hydr0Gen2019-05-28T16:17:41+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Fundamentals, Video|

1:16a know what is meant by the terms atomic number, mass number and relative atomic mass (Aᵣ)

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Atomic number: The number of protons in an atom.

Mass number: The number of protons and neutrons in an atom.

Relative atomic mass (A_r): The average mass of an atom compared to 1/12th the mass of carbon-12.

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Hydr0Gen2019-05-23T15:18:05+00:00Categories: Uncategorized|Tags: 1:16a, Chemistry, Double, GCSE, GCSE_Chemistry_SpecPoint, SpecPoint, SubSpecPoint, Topic: Fundamentals, Topic: Simple Molecules & Covalent Bonding|

1:18 understand how elements are arranged in the Periodic Table: in order of atomic number, in groups and periods

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The elements in the Periodic Table are arranged in order of increasing atomic number.

Columns are called Groups. They indicate the number of electrons in the outer shell of an atom.

Rows are called Periods. They indicate the number of shells (energy levels) in an atom.

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Hydr0Gen2023-01-10T12:19:15+00:00Categories: (d) The Periodic Table, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:18, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Fundamentals, Topic: Halogens (D), Topic: Metal Reactivity & Halogens, Topic: Metals (D), Topic: Simple Molecules & Covalent Bonding|

1:20a understand how to use electrical conductivity to classify elements as metals or non-metals

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Metals

conduct electricity

Non – Metals

do not conduct electricity (except for graphite)

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Hydr0Gen2019-05-23T15:18:19+00:00Categories: Uncategorized|Tags: 1:20a, Chemistry, Double, GCSE, GCSE_Chemistry_SpecPoint, SpecPoint, SubSpecPoint, Topic: Fundamentals|

1:21 identify an element as a metal or a non-metal according to its position in the Periodic Table

Metals on the left of the Periodic Table.

Non-Metals on the top-right, plus Hydrogen.

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Hydr0Gen2023-01-10T12:26:21+00:00Categories: (d) The Periodic Table, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:21, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Fundamentals, Topic: Halogens (D), Topic: Metal Reactivity & Halogens, Topic: Metals (D), Topic: Simple Molecules & Covalent Bonding|

1:25 write word equations and balanced chemical equations (including state symbols): for reactions studied in this specification and for unfamiliar reactions where suitable information is provided

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Example:

Sodium (Na) reacts with water (H₂O) to produce a solution of sodium hydroxide (NaOH) and hydrogen gas (H₂).

Word equation:

sodium + water –> sodium hydroxide + hydrogen

Writing the chemical equation

A chemical equation represents what happens in terms of atoms in a chemical reaction.

Step 1: To write a chemical equation we need to know the chemical formulae of the substances.

Na + H₂O –> NaOH + H₂

Step 2: The next step is to balance the equation: write a large number before each compound so the number of atoms of each element on the left hand side (reactants) matches the number on the right (products). This large number is the amount of each compound or element.

During this balancing stage the actual formulas for each compound must not be changed. Only the number of each compound changes.

2Na + 2H₂O –> 2NaOH + H₂

If asked for an equation, the chemical equation must be given.

State symbols are used to show what physical state the reactants and products are in.

State symbols	Physical state
(s)	Solid
(l)	Liquid
(g)	Gas
(aq)	Aqueous solution (dissolved in water)

Example:

A solid piece of sodium (Na) reacts with water (H₂O) to produce a solution of sodium hydroxide (NaOH) and hydrogen gas (H₂).

2Na(s) + 2H₂O(l) –> 2NaOH(aq) + H₂(g)

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Hydr0Gen2023-09-18T11:05:10+00:00Categories: (e) Chemical formulae, equations and calculations, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:25, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Alkanes & Crude Oil, Topic: Fundamentals, Topic: Ions, Topic: Key Reactions, Topic: Moles|

Balancing equations – Tyler de Witt videos

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This excellent Tyler de Witt video is an introduction to balancing equations:

And here’s another of the lovely Tyler’s videos with some practice questions and answers on equation balancing:

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Hydr0Gen2019-02-10T13:12:49+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Fundamentals, Topic: Key Reactions, Topic: Moles, Video|

Balancing equations – interactive

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This is useful to help you to practice how to balance equations:

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Hydr0Gen2019-05-28T16:02:04+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Fundamentals, Video|

1:26 calculate relative formula masses (including relative molecular masses) (Mᵣ) from relative atomic masses (Aᵣ)

Relative formula mass (M_r) is mass of a molecule or compound (on a scale compared to carbon-12).

It is calculated by adding up the relative atomic masses (A_r) of all the atoms present in the formula.

Example:

The relative formula mass (M_r) for water (H₂O) is 18.

Water = H₂O

Atoms present = (2 x H) + (1 x O)

M_r = (2 x 1) + (1 x 16) = 18

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Hydr0Gen2022-11-30T14:12:46+00:00Categories: (e) Chemical formulae, equations and calculations, 1 Principles of chemistry, Edexcel iGCSE Chemistry|Tags: 1:26, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Calculations, Topic: Fundamentals, Topic: Key Calculations, Topic: Moles|

Calculation of relative formula mass – Tyler de Witt video

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Here’s an excellent Tyler de Witt video explaining how to calculate the relative formula mass of compounds with:

a simple formula
a formula which includes brackets
a formula which includes a dot (water of crystallisation)

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Hydr0Gen2019-02-10T12:17:13+00:00Categories: Uncategorized|Tags: Chemistry, GCSE, Topic: Calculations, Topic: Fundamentals, Topic: Key Calculations, Topic: Moles, Video|

3:01 know that chemical reactions in which heat energy is given out are described as exothermic, and those in which heat energy is taken in are described as endothermic

Exothermic: chemical reaction in which heat energy is given out.

Endothermic: chemical reaction in which heat energy is taken in.

(So, in an exothermic reaction the heat exits from the chemicals so temperature rises)

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Hydr0Gen2023-01-10T11:58:37+00:00Categories: (a) Energetics, 3 Physical chemistry, Edexcel iGCSE Chemistry|Tags: 3:01, Chemistry, Double, GCSE, GCSE_Chemistry_Single, GCSE_Chemistry_SpecPoint, SpecPoint, Topic: Crude oil to plastics (D), Topic: Energetics, Topic: Energetics (D), Topic: Equilibria, Topic: Fundamentals, Topic: Reversible Reactions (D)|