Unit 1

• Give the names of the 4 atomic orbitals


  S, P, D and F
• Where is the relative atomic mass found?

  The Periodic Table
• What is the trend ionisation energies as you go across the periods?


  Ionisation energy increases as you go across the period, because the nuclear charge increases but the shielding due to the inner shells staying the same. This means the electrostatic attraction of the nucleus to the other outer electrons increase.
• What are the forces between molecules?

  Intermolecular forces
• Metals in group 1, 2 and 3 normally form what ions?


  Positive ions, + 1 , + 2 and +3
• NH4^(+) ion is called?


  Ammonium
• What is the trend in ionisation energies as you go down the group?


  As a group is descended, the first ionisation energy decreases. This is because the outer electron being removed is further from the nucleus and there are more inner shells to shield the outer electron. This means the electrostatic attraction to the nucleus is less.
• Loss of electrons forms positive ions
• How is % yield calculated?


  Actual yield/theoretical yield x 100%
• How many electrons fit in the 2nd shell?


  8
• What is the trend in electron affinity as you descend a group?


  Electron affinity decreases down the group, as the shell which the electron is being added is further from the nucleus as it is shielded by inner electrons. This leads to a reduced electrostatic attraction between the electron being added and the nucleus.
• How many electrons fit in the 4th shell?

  32
• SO4^(2-) ion is called 


  Sulfate
• How many electrons fit in the 3rd shell

  18
• What is a dipole?


  The unequal distribution between charge leading to partial (delta positive/ negative) charges.
• How is concentration calculated?


  dividing moles by the volume of decimetres cubed

  (dm^3). The units of concentration are mol.dm^(-3)
• What is the trend for atomic radius on the periodic table ?


  Atomic radius increases down the groups and decreases across the periods.
• Ionic compounds have giant structures called lattices
• What is electron affinity


  This is the energy change when an electron is added to each atom in 1 mole of gaseous atoms.
• Describe Bohr theory 


  The spltting of main shells to sub-shells which is reflected into electron configurations.
• How are moles calculated?

  Mass / relative atomic mass
• CO3^(2-) ion is called 


  Carbonate
• What is an atomic orbital?

  The region in which an electron can be found
• Describe covalent bonding


  The strong electrostatic force of attraction between a nuclei and its shared pair of electrons
• The higher the charge of the ion the stronger the ionic bond it can form
• What charge do metals usually form?

  Positive
• What is meant by molarity?


  Molarity is the number of moles in a given volume.
• The smaller the ion the stronger the ionic bond it can form
• What is the definition of a mole?

  A mole is 6.02 x 10^(23) atoms or molecules of a substance.
• Give the properties of metals ( 4 points)

  Able to conduct electricity and thermal conductivity due to delocalised electrons, they have high meleting and boiling points due to their strong forces of attraction requiring lots of energy to break down, they are malleable and also ductile which means they're able to change their form but still remain the same without breaking and the layers of the cations are able to slide over each other
• What is ionisation energy?


  Energy required to move an electron in 1 mole of gaseous atoms
• How many electrons fit in the 1st shell

  2
• Ionic compounds have high melting points
• What is Aufbau principle?


  Electrons fill shells and sub-shells in order of increasing energy.
• The tetrahedral bond angle is 109.5 degrees.
• The force between the nucleus and the outer electron is Electronegativity
• Gain of electrons is known as Reduction
• What charge of ions do non-metas usually form?


  Negative
• Non- metals in groups 5,6 and 7 form what ions?


  -3 , -2 and -1
• What is hydrogen bonding?


  Attraction between the lone pair of an oxygen, nitrogen or fluorine atom and an electron- deficient(delta-positive) hydrogen.