electron configuration

• Oxidising agent


  None in this reaction
• Ionisation energy


  The energy required to remove an electron from an atom
• Trend in first ionisation energies of the elements in Group 2 from magnesium to barium

  • Decrease
  • Ions get bigger/more (energy) shells
  • Weaker attraction of ion to lost electron
• Use the Periodic Table to deduce the full electron configuration of calcium.

  1s22s22p63s23p64s2
• Write an ionic equation, with state symbols, to show the reaction of calcium with an excess of water

  Ca(s)+ 2H2O(l) ---> Ca2+(aq) + 2OH– (aq) + H2(g)
• State the role of water in the reaction with calcium.

  Oxidising agent
• Write an equation to show the process that occurs when the first ionisation energy of calcium is measured

  Ca(g) ---> Ca+ (g) + e–
• State and explain the trend in the first ionisation energies of the elements in Group 2 from magnesium to barium. Trend and explain

  Trend: Decrease

  Explication: Ions get bigger / more (energy) shells so weaker attraction of ion to lost electron
• State the element in Period 3 that has the highest melting point. Explain your answer.

  Element: Silicon/Si

  Explanation:

  -COVALENT bonds

  -Strong or many of the (covalent) bonds need to be broken / needs a lot of energy to break the (covalent) bonds
• State the element in Period 3 that has the highest first ionisation energy. Explain your answer.

  Element: Argon / Ar

  Explanation:

  -Large(st) number of protons / large(st) nuclear charge

  -Same amount of shielding / same number of shells / same number of energy levels
• Suggest the element in Period 3 that has the highest electronegativity value

  Chlorine / Cl
• Shape of ClF3. Write an equation to show the formation of one mole of ClF3 from its elements. 


  Shape:

  Equation: Equation: 1/2 Cl2 + 3/2 F2 ---> ClF3

  
• Shape of CCl2 and name.

  
  

  Shape:

  Name: Bent/v shape

  
• Which one of the following is a fundamental particle that would not be deflected by an electric field?

  A-electron

  B-neutron

  C-proton

  B-Neutron
• Complete the table

  Range between 3500 and 10 000 kJ mol−1

  
• Write an equation to show the process that occurs when the second ionisation energy of boron is measured. Include state symbols in your equation.

  B+ (g) ---> B2+(g) + e(−)

  B + (g) − e(−) ---> B2+(g)

  B + (g) + e(−) ---> B2+(g) + 2e(−)
• Explain why the second ionisation energy of boron is higher than the first ionisation energy of boron

  Electron being removed from a positive ion (therefore needs more energy) / electron being removed is closer to the nucleus
• State the block in the Periodic Table that contains nickel

  D block
• Explain, in terms of its structure and bonding, why nickel has a high melting point

  Contains positive (metal) ions or protons or nuclei and delocalised / mobile / free / sea of electrons
• Draw a labelled diagram to show the arrangement of particles in a crystal of nickel. In your answer, include at least six particles of each type.

  Diagram

  
• Explain why nickel is ductile (can be starched into wires)

  Layers / planes / sheets of atoms or ions can slide over one another
• Give the full electron configuration of the Ni2+ ion.

  1s2 2s2 2p6 3s2 3p6 3d8 (4s0 )
• Balance the following equation to show how anhydrous nickel(II) chloride can be obtained from the hydrated salt using SOCl2 Identify one substance that could react with both gaseous products. ......NiCl2.6H2O(s) + ...... SOCl2(g) ......NiCl2(s) + ......SO2(g) + ......HCl(g)


  NiCl2.6H2O + 6 SOCl2 ---> NiCl2 + 6 SO2 + 12 HCl

  Substance: NaOH / NH3 / CaCO3 / CaO
• Aluminium and thallium are elements in Group 3 of the Periodic Table. Both elements form compounds and ions containing chlorine and bromine.

  (a) Write an equation for the formation of aluminium chloride from its elements.

  Al + 1.5Cl 2 → AlCl3
• An aluminium chloride molecule reacts with a chloride ion to form the AlCl4 − ion. Name the type of bond formed in this reaction. Explain how this type of bond is formed in the AlCl4 − ion.

  Type of bond: Coordinate / dative (covalent)

  Explanation: Electron pair on Cl − donated to Al(Cl 3)
• Aluminium chloride has a relative molecular mass of 267 in the gas phase. Deduce the formula of the aluminium compound that has a relative molecular mass of 267 


  Al2Cl6 or AlBr
• Draw and name the shape of the TlBr5 2− ion. Shape of the TlBr5 2− ion.

  Name: Trigonal bipyramid(al)

  
• Deduce the name or formula of a compound that has the same number of atoms, the same number of electrons and the same shape as the AlCl4 − ion.

  SiCl4 / silicon tetrachloride
• Draw the shape of the TlCl2 + ion and explain why the TiCl2 has this shape

  (Two) bonds (pairs of electrons) repel equally / (electrons in) the bonds repel to be as far apart as possible

  
• Which one of the first, second or third ionisations of thallium produces an ion with the electron configuration [Xe] 5d106s1?

  Second
• Which change requires the largest amount of energy

  A)He+ (g) He2+(g) + e–