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AS/A-Level Chemistry- Periodicity applications

Periodicity applications

· A-level Chemistry,period 3 elements,periodicity,periodic table,question analysis

Let's see some questions to consolidate your knowledge on A-Level Chemistry periodicity!

1. Explain why Cl has a greater electronegativity than Na

  • Cl has a greater number of protons, greater nuclear charge than Na
  • Cl has a smaller size, greater charge density than Na
  • Cl has similar shielding to Na
  • Cl attracts the bonding pair of electrons to the nucleus more

2. Explain why Mg has a higher boiling point than Na

  • Mg2+ion has a greater charge, greater charge density than Na+ion
  • Stronger electrostatic forces of attraction between positively-charged Mg2+ions and the negatively-charged sea of delocalised electrons, stronger metallic bonding between positively-charged Mg2+ions and the negatively-charged sea of delocalised electrons
  • More energy required to break the stronger metallic bonding 

3. State the equations and observations for the reactions of Na, Mg, Al, Si, P and S with oxygen

  • 4Na + O2 ⇨ Na2O
  • Vigorous exothermic reaction, yellow flame, white solid
  • 2Mg + O2 ⇨  2MgO
  • Vigorous exothermic reaction, white flame, white solid powder
  • 4Al + 3O2 ⇨ 2Al2O3
  • White flame, white solid powder
  • Si + O2 ⇨SiO2
  • White flame, white solid powder
  • 4P + 5O2 ⇨ P4O10
  • Vigorous exothermic reaction, white flame, white solid powder
  • S + O2 ⇨ SO2
  • Blue flame, colourless gas, choking gas fumes
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4. Explain why MgO has a higher melting point and boiling point than MgCl2 and Li2O has a higher melting point and boiling point than Na2O

  • O2-has a greater charge density than Cl- ion
  • there are stronger electrostatic forces of attraction between oppositely-charged ions, O2-and Mg2+ions, stronger ionic bonds between oppositely-charged ions, O2- and Mg2+ions
  • Li+ ion is smaller than the Na+ ion
  • there are stronger electrostatic forces of attraction between oppositely-charged ions, Li+ and O2-ions, stronger ionic bonds between oppositely-charged ions, Li+and O2- ions

5. State the link between electronegativity and the type of bonding and explain whether Na2O or P4O10 has a higher melting point in terms of the types of bonding and structures

  • P4O10: Small difference in electronegativity, more covalent character, less ionic character
  • Na2O: Big difference in electronegativity, more ionic character, less covalent character
  • Na2O has ionic bonding and a giant ionic lattice structure
  • strong electrostatic forces of attraction and strong ionic bonds between oppositely-charge ions between oppositely-charged ions, Na+and O2-ions
  • P4O10has covalent bonding between P and O atoms and a simple molecular structure
  • Weak van der Waals forces between molecules
  • Therefore Na2O has a greater melting point than P4O10

6. Explain why Al2O3is not soluble in water

  • Ionic bonding with additional covalent character
  • Al3+ ion has a small size, can get close to the O2-ion
  • Al3+ ion has a high charge density
  • Al3+ ion has high electronegativity
  • Al3+ ion polarises the O2- ion, distorts the O2- ion electron cloud

7. Explain how Na2O reacts with water to form an alkaline solution and suggest why Na2O should not be added in excess for neutralisation of a lake whereas MgO can be added in excess for neutralisation of a lake

  • O2- ion reacts with water, accepts a proton
  • Forms OH- ions, produces NaOH
  • Excess NaOH would make the lake alkaline, kill wildlife
  • MgO is sparingly soluble, would make the lake weakly alkaline

CLICK HERE TO LEARN MORE ABOUT OUR A-LEVEL CHEMISTRY COURSE

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Drafted by Eunice Wong (Chemistry)

References: 

https://gph.is/g/E1651mr

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