Youtube Channels:
1. Allery Chemistry is great:
IAL Unit 1 June 2015 Paper Solve : https://www.youtube.com/watch?v=LHviH6qm7yI
Books:
1. The Student Book helps since it is exactly up to your syllabus
2. For a more detailed explanation, check the book by George Facer
Enthalpies, periodic table etc
Why magnesium has higher melting point than sodium
1. Mg2+ has a smaller ion (Magnesium ions are smaller than sodium ions)
2. Mg2+ has a larger charge than sodium ion
3. Contributes more electrons to the sea of electrons
4. Stronger attraction between positive ions and delocalised electrons
5. More energy/ heat required to overcome bonds
Why ionisation energy increases across a period
1. More protons; greater nuclear charge
2. The outer electrons stay in the same shell; same shielding
3. Overall greater force of attraction between nucleus and outer electrons
Enthalpy change of formation
1. Energy change when 1 mole of a compound is formed from its elements
2. Under standard conditions of 298 K and 1 atm
Enthalpy change of atomisation
1. Energy change when number of moles of reactants react as stated in the balanced
equation
First ionisation energy
1. The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to
form 1 mole of gaseous ions
2. Give equation (X → X+ and e-)
Bond enthalpy
1. The average amount of energy required to break one mole of covalent bonds in the
gaseous state
,
1. Allery Chemistry is great:
IAL Unit 1 June 2015 Paper Solve : https://www.youtube.com/watch?v=LHviH6qm7yI
Books:
1. The Student Book helps since it is exactly up to your syllabus
2. For a more detailed explanation, check the book by George Facer
Enthalpies, periodic table etc
Why magnesium has higher melting point than sodium
1. Mg2+ has a smaller ion (Magnesium ions are smaller than sodium ions)
2. Mg2+ has a larger charge than sodium ion
3. Contributes more electrons to the sea of electrons
4. Stronger attraction between positive ions and delocalised electrons
5. More energy/ heat required to overcome bonds
Why ionisation energy increases across a period
1. More protons; greater nuclear charge
2. The outer electrons stay in the same shell; same shielding
3. Overall greater force of attraction between nucleus and outer electrons
Enthalpy change of formation
1. Energy change when 1 mole of a compound is formed from its elements
2. Under standard conditions of 298 K and 1 atm
Enthalpy change of atomisation
1. Energy change when number of moles of reactants react as stated in the balanced
equation
First ionisation energy
1. The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to
form 1 mole of gaseous ions
2. Give equation (X → X+ and e-)
Bond enthalpy
1. The average amount of energy required to break one mole of covalent bonds in the
gaseous state
,
