Paper 1

• What is an Isotope? (2m)

  Same number of protons but different numbers of neutrons.
• Elements:

  • located on the right-hand side of the periodic table
  • E.g Gold is pure (can't be broken down)
• Compounds:

  • Bonds of 2 different chemically combined atoms
• Molecule:

  • Different substances together which aren't chemically combined, e.g H2O, Co, O2
• What is the test for carbon dioxide?


  Turns limewater to cloudy
• What is the test for Oxygen?


  Flame test - Relights a glowing splint
• What is an Atom?


  Basic unit of matter, composed of protons, neutrons, and electrons
• What is the Nucleus


  Central part of an atom containing protons and neutrons
• What is a Proton?


  Positively charged subatomic particle found in the nucleus
• What is a Neutron?


  Neutral subatomic particle found in the nucleus
• What is an Electron?


  Negatively charged subatomic particle moving around the nucleus
• What is Relative Atomic Mass?


  Average mass of all isotopes of an element, considering their abundances
• What is a Covalent bond?


  Chemical bond between 2 non-metals where atoms share electrons
• What is Ionic Bond?


  Chemical bond between a metal and a non-metal formed by attraction between oppositely charged ions.
• What is Metallic Bonding?


  Type of bonding in metals leading to their physical properties like malleability and conductivity
• What is the Nuclear Model of the Atom?


  Atomic model with a nucleus surrounded by electrons in fixed shells
• What is the Plum Pudding Model?


  Atomic model suggesting positive cloud with scattered electrons
• What is the Development of Periodic table?


  Arrangement of elements by atomic number and properties predicted by Mendeleev
• • What happens to the reactivity in Group 1 as you go down the group?

  • Distance when positive nucleus and negative electrons increase
  • Due to extra shielding (electron shells)
  • Weaker electrostatic attraction
  • Easier to lose electrons because of the distance.
• What happens to the reactivity in Group 7 as you go down the group?


  • Distance when positive nucleus and negative electrons decrease
  • Due to less shielding
  • Stronger electrostatic attraction
  • Easier to gain electrons
• Electrostatic attraction:

  • Weaker when the distance of electrons and it's shells are further away from each other which makes it easier to lose electrons.
  • Stronger when the distance of electrons and it's shells are near each other which makes it easier to gain electrons.
• Why are some elements more reactive than others?

  Wanting to become stable and loses/gaining electrons.
• Who discovered the "Plum Pudding Model"?


  JJ Thompson
• Who discovered that "Atoms are solid spheres"?


  John Dalton
• Who discovered the "Nuclear Model"?


  Rutherford
• Who discovered the "Neutron"?


  James Chadwick
• Who discovered that "Electrons orbit in shells/energy levels"?


  Niels Bohr
• How many protons, neutrons, and electrons are there in Potassium?


  • Protons = 19
  • Neutrons = 20 (39 - 19)
  • Electrons = 19

  
• Diamond:

  • Bonded to 4 carbon atoms
  • Has strong bonds
  • Weak intermolecular forces
  • Can't slide due to no layers
  • High melting and boiling point
  • Hard

  
• Graphite:

  • Bonded to 3 carbon atoms
  • Has weak bonds
  • Strong intermolecular forces
  • Can slide because it has layers
  • Soft

  
• What are the 2 properties of Noble gases?


  Stable full outer shell and colourless (can't see how it looks like)
• What would you expect Copper chloride to be a solid or gas at room temperature? why?

  Solid, Ionic compound with high melting point
• Left-side of the periodic table = non-metals

  Right-side of the periodic table = metals
• State the formula used to calculate the Rf value in chromatography.


  Rf = distance substance travels / distance solvent travels
• What type of bonding would you find in Carbon dioxide?

  Covalent because carbon is a non-metal
• Why will Potassium chloride conduct electricity when it is dissolved but not when it is a solid?


  • Has ionic bonding with charged ions
  • when dissolved the ions are free to move
  • If it is a solid it can't move as they are compact together
• What ion do all alkalis contain?

  OH-
• Why does increasing concentration increase the rate of reaction?


  Collision theory - has more frequent collisions with enough energy
• What is an ion?


  A charged particle that has lost or gained an electron(s)
• Name 3 types of bondings:

  • Ionic
  • Covalent
  • Metalic