Y10 Whole Curriculum

• Three States of Matter

  1. Solid
  2. Liquid
  3. Gas
• Matter 1: 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.
• Matter 2: 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.
• Matter 3: 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.
• Melting

  1. Solid is heated

  2. Energy makes particles vibrate fast enough

  3. Turns into a liquid
• Freezing


  1. Liquid is cooled

  2. Particles move slowly enough

  3. Held into a solid
• Boiling


  1. Liquid is heated strongly

  2. Energy makes particles move fast enough

  3. Turns into gas
• Condensing


  1. Gas is cooled

  2. Particles move slowly enough

  3. Held as a liquid
• Sublimation


  Solid changes directly to gas when heated
• Diffusion


  The gradual movement of particles from a place containing a high concentration of particles to a low concentration of particles.
• Solvent 


  The liquid a solid is dissolving into
• Solute 


  The substance that is being dissolved
• Solution


  A mixture of a solute and a solvent that does not separate out
• Saturated Solution


  A solution where the maximum amount of solute has been dissolved, so no more solute will dissolve in the solution.
• Atom 


  A smallest part of an element that can exist
• Molecule


  2 or more atoms covalently bonded together to create a molecule
• Atomic Number


  The number of Protons in an Atom
• Mass Number


  The amount of Protons and Neutrons in an Atom
• Isotope


  An Isotope is an atom with the same amount of protons but a changed amount of neutrons eg: Cl-35 & Cl-37
• Relative Atomic Mass


  the ratio of the average mass of one atom of an element to one twelfth of the mass of an atom of carbon-12.
• Understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals


  metals:

  -conduct electricity because they allow charge to pass through them

  -metal oxides are basic

  this means they will neutralize acids

  -metal oxides that dissolve will form solutions with a pH of more than 7

  (pH is a measure of acidity)
• Understand how to use electrical conductivity and the acid-base character of oxides to classify elements as non-metals

  neutralize

  non-metals:

  -poor conductors of electricity

  -non-metal oxides are acidic

  this means they will neutralize bases.

  -non-metal oxides that dissolve will form solutions with a pH of less than 7
• identify an element as a metal or a non-metal according to its position in the periodic table

  -metals are on the left side

  -non-metals are on the right side

  -they are separated by a zig-zag going from boron to astatine
• understand how the electronic configuration of a main group element is related to its position in the periodic table

  Number or numbers of circles = Period number

  Number of electrons in outer shell = group number

  Total number of electrons in all shells = Atomic number
• Calculate Relative Formula Mass

  ● Relative formula mass (Mr) of a compound: sum of the relative atomic masses of the atoms in the numbers shown in the formula
• Calculate Relative Atomic Mass


  you can also use relative formula mass to find the % of one of the elements for example

  Mr of CuO = 79.5

  % of Cu = 63.5 / 79.5 x 100 = 79.9%
• Moles Formula


  Mass/Mr
• calculate reacting masses using experimental data and chemical equation

  1. find the mol of one of the substances
  2. look at the reacting ratio and see if you need to multiply and divide to find the mols of another substance
  3. use mass = mols x mr
• Calculate Percentage Yield

  percentage yield = amount of product produced / maximum amount of product produced x 100
• understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water, and salts containing water of crystallization


  example experiment to find the formula of magnesium oxide:

  ● weigh some pure magnesium

  ● Heat magnesium to burning in a crucible to form magnesium oxide, as the magnesium will react with the oxygen in the air

  ● weigh the mass of the magnesium oxide

  ● Known quantities:

  ○ calculate the ratio of moles of magnesium to moles of oxygen

  ○ use the ratio to form an empirical formula
• Empirical Formula Definition

  The empirical formula shows the simplest whole number ratio of the atoms present in a compounds
• Molecular Formula Definition

  The molecular formula shows the actual number of each element present in a molecule (covalent compound) or formula unit (ionic compound) of a compound
• Calculate empirical and molecular formulae from experimental data

  draw a table with the following grids:

  Masses, g

  mass / mr

  mols

  divide by the smallest number to find the ratio

  ratio of moles

  • empirical formula

  % can be used instead of mass
• Determine the formula of a metal oxide by reduction


  1. Weigh a crucible with a lid

  2. Place a piece of magnesium ribbon about 10 cm long in the crucible and weigh the crucible and the contents

  3. Set up apparatus

  4. Heat the crucible strongly using a roaring flame

  5. Lift the lid every few seconds

  6. Weigh the crucible and the contents
• Experiment Facts

  when mg burns with a white flame it turns to MgO, a white powder.

  A lid is placed on the crucible to prevent the white powder from escaping but the lid must lifted every 30 seconds to allow oxygen to react with mg

  then calculate the empirical formula with a table
• Understand how ions are formed by electron loss or gain

  Ions are electrically charged particles formed when atoms lose or gain electrons. This loss or gain leaves a full outer shell, so the electronic structure of an ion is the same as that of a noble gas (such as helium, neon, or argon).
• Know the Charges of these Ions

  know the charges of these ions:

  • metals in Groups 1, 2 and 3

  • non-metals in Groups 5, 6 and 7

  • Ag+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+

  • hydrogen (H+), hydroxide (OH-), ammonium (NH4+), carbonate (CO32-),

  nitrate (NO3-), sulfate (SO42-).
• How does Lithium, Sodium & Potassium similarly react with water

  When they react with water, they all react vigorously

  The reaction produces a metal hydroxide solution. The solution is Alkaline (Alkali Metals)
• Potassium reactions in water

  • Bubbles of gas

  • Melts into a shiny ball that dashes around the surface

  • Burns with a lilac-coloured flame
• Lithium reaction in water

  • Bubbles of gas