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Electronic Structures | GCSE Chemistry (9-1) || MOREducation

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Ions and Isotopes | GCSE Chemistry (9-1) || MOREducation

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Go through powerpoint and make notes. Complete worksheets then answer past paper questions

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All substances are made of atoms. An atom is the smallest part of an element that can exist.

Atoms of each element are represented by a chemical symbol, for example:

O represents an atom of oxygen

Na represents an atom of sodium

There are about 100 different elements. Elements are shown in the Periodic Table.

Compounds are formed from elements by chemical reactions. Chemical reactions always involve the formation of one or more new substances, and often involve a detectable energy change. Compounds contain two or more elements chemically combined in fixed proportions and can be represented by formulae using the symbols of the atoms from which they were formed. Compounds can only be separated into elements by chemical reactions.

Chemical reactions can be represented by word equations or equations using symbols and formulae.

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Atoms, Elements and Compounds | AQA C1 | revisechemistry.uk

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All substances are made of atoms. An atom is the smallest part of an element that can exist. Atoms of each element are represented by a chemical symbol, for example: O represents an atom of oxygen Na represents an atom of sodium There are about 100 different elements.

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On the Periodic Table you will find every element that we know about, which in turn is a list of every that we have discovered. It is ordered by atomic number, meaning that reading from left to right increases the proton number by one every time.

The Periodic Table is arranged in such a way that elements with similar properties can be found together in columns called ' groups' - for example the group 1 metals are all very reactive with water. Elements in the same group have the same number of electrons in their outershell (these are known as valence electrons).

Elements in the same period have the same number of electron shells.

The Periodic Table is split with metals all found on the left side of the table, and non metals found on the right.​ Metals have either 1, 2 or 3 electrons on their outermost shell, so want to lose electrons to form positive ions ( cations). Non-metals that have either 5, 6 or 7 electrons on their outermost shell want to gain electrons to form negative ions ( anions). Non-metals with 8 electrons, the Noble Gases, don't lose or gain electrons to form ions, as they are stable (and therefore inert).

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The Periodic Table | AQA C1 | revisechemistry.uk

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On the Periodic Table you will find every element that we know about, which in turn is a list of every that we have discovered. It is ordered by atomic number, meaning that reading from left to right increases the proton number by one every time.

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AQA Chapter 1 - Atomic Structure and the Periodic Table Revision Mat

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1.1 Simple Model, symbols, RAM ,charge,isotopes

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I will be setting work for you all to complete.

Year 10 - As we have completed the content for this year. We are going to be revising starting with year 9 chemistry.

Year 9 - Start final Physics topic - Waves

Take Care,

Miss Kankam

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I have made a youtube channel to teach GCSE Chemistry content. I will be uploading one video each day from Monday - Friday, starting with Atomic Structure content.

Subscribe for updates and share with your friends

Thanks,

Miss Kankam

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Atoms, Elements and Compounds | GCSE Science Chemistry (9-1) || MOREducation #StayHome

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Separating Mixtures (Part 1)  | GCSE Science Chemistry (9-1) || MOREducation #StayHome

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Separating Mixtures (Part 2)  | GCSE Science Chemistry (9-1) || MOREducation #StayHome

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History of the atom  | GCSE Science Chemistry (9-1) || MOREducation #StayHome

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Go through powerpoint and make notes. Complete worksheets then answer past paper questions

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Solids (s), liquids (l) and gases (g) can be represented using particle diagrams. In these diagrams, particles are represented by solid spheres.

Particles in solids have less energy than liquids, which in turn have less energy than gases. To get from a solid to a liquid, or a gas, energy has to be supplied - usually through heating. During these changes the particles gain energy, which is used to break or overcome the intermolecular forces of attraction.

Fluids (liquids and gases) are able to take the shape of their containers, however, only gases can be compressed as their particles are far apart and have space to move into.

The amount of energy required to change state depends on the strength of the intermolecular forces between the particles of each substance. Some of the forces need to be broken during melting, whereas all of the forces must be broken during evaporating/boiling. Changing from one state to another is a physical change as you end up with the same chemical as you began with (whereas a chemical change would lead to different chemicals).

State changes

Solids can turn into liquids through the process of melting. This involves increasing the energy of the particles normally by heating. Liquids can be turned back into solids by freezing, lowering the amount of energy particles have.

Liquids can turn into gases by evaporation or boiling (again by increasing the energy of the particles). Gases can be turned back into liquids by condensation, lowring the amounf of energy particles have.

Some solids can turn straight into a gas, skipping the liquid phase; this is called sublimation.

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Chemical Bonds, Ionic, Covalent and Metallic | AQA C2

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Solids (s), liquids (l) and gases (g) can be represented using particle diagrams. In these diagrams, particles are represented by solid spheres. Particles in solids have less energy than liquids, which in turn have less energy than gases. To get from a solid to a liquid, or a gas, energy has to be supplied - usually through heating.

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Nanoscience refers to structures that are 1-100 nm in size, of the order of a few hundred atoms. Nanoparticles, are smaller than fine particles (PM 2.5), which have diameters between 100 and 2500 nm (1 x 10⁻⁷ m and 2.5 x 10⁻⁶ m). Coarse particles (PM ₁₀) have diameters between 1 x 10⁻⁵ m and 2.5 x 10⁻⁶ m. Coarse particles are often referred to as dust.

As the side of a cube decreases by a factor of 10 the surface area to volume ratio increases by a factor of 10.

Nanoparticles may have properties different from those for the same materials in bulk because of their high surface area to volume ratio. It may also mean that smaller quantities are needed to be effective than for materials with normal particle sizes.

Nanoparticles have many applications in medicine, in electronics, in cosmetics and sun creams, as deodorants, and as catalysts. New applications for nanoparticulate materials are an important area of research.

titanium dioxide blocks ultraviolet light, so it is used in sunscreens

in bulk, titanium dioxide is white - it is used as a pigment in white paint

individual particles (nanoparticulate) of titanium dioxide have no colour and cannot be seen when it is spread on skin

Risks of nanoparticles:

people are concerned the small size of nanoparticles makes it possible to breathe them in, or to pass into cells

inside the body, they might catalyse reactions that are harmful producing toxic substances

modern nanoparticulate materials have not been used for long, so it is difficult for scientists to determine their risks

The large surface area to volume ratio of nanoparticulates mean they work as great catalysts. Compared to the same substance in bulk, they might:

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Bulk and Surface Properties of Matter | AQA C2 | revisechemistry.uk

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Nanoscience refers to structures that are 1-100 nm in size, of the order of a few hundred atoms. Nanoparticles, are smaller than fine particles (PM 2.5), which have diameters between 100 and 2500 nm (1 x 10-7 m and 2.5 x 10-6 m).

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Watch videos 1 - 6, you have only been taught up until alkenes

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Watch videos 1 - 6, you have only been taught up until alkenes

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9-1 GCSE Chemistry Paper 2 Organic Chemistry - YouTube

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Don't forget if you need help, feel free to email me at: nkankam@uai.org.uk

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All of AQA Energy explained in 7 minutes - GCSE Physics 9-1 REVISION

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Don't forget if you need help, feel free to email me at: nkankam@uai.org.uk

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AQA GCSE Chemistry Core Practical 1: Making a salt

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Week Beginning 1st June (complete over the next two weeks) 

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Week Beginning 1st June (complete over the next two weeks) 

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Don't forget if you need help, feel free to email me at: nkankam@uai.org.uk

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Week Beginning 1st June (complete over the next two weeks) 

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Week Beginning 1st June (complete over the next two weeks) 

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Don't forget if you need help, feel free to email me at: nkankam@uai.org.uk

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Don't forget if you need help, feel free to email me at: nkankam@uai.org.uk

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Lesson 2 - Transverse and longitudinal waves

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Lesson 2 - Transverse and longitudinal waves

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Structure of an atom  | GCSE Science Chemistry (9-1) || MOREducation #StayHome

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Ions and Isotopes | GCSE Chemistry (9-1) || MOREducation

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Until 17th June

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Lesson 8 - Reflection, refraction and wave fronts