Topic 3/13 Periodicity Review
1.
2.
3.
Explain the trends in electronegativity, ionization energy, atomic and ionic radii, and melting points across periods and up
and down groups.
Identify and explain properties of period 3 oxides (ionic vs. covalently bound, melting points, conductivity, acids or bases in
aqueous solutions, etc.).
Be able to write balanced equations for the reactions of period 3 oxides in water.
For example:
Na2O(s) + H2O (l)  2Na+(aq) + 2OH- (aq)
4.
Be able to write balanced equations for reactions involving alkali metals and/or halogens. Also realize that more reactive
halogens will oxidize less reactive halogens *Some of these can be treated as single displacement reactions where the most
reactive metal or nonmetal displaces the less reactive metal or nonmetal respectively. Material in Chapter 3.3 of Online
Text
For example:
Cl2 (aq) + 2 I- (aq)  I2 (aq) + 2 Cl- (aq)
5.
6.
7.
Explain why Sc and Zn are not considered to be transition metals (even though they are in the ‘d’ block of the periodic table.
Define “ligand” and be able to give examples of common ligands.
Explain why some complex ion solutions of transition metals are colored (and why others are not).
Topic 3/13 Periodicity Review
1.
2.
3.
Explain the trends in electronegativity, ionization energy, atomic and ionic radii, and melting points across periods and up
and down groups.
Identify and explain properties of period 3 oxides (ionic vs. covalently bound, melting points, conductivity, acids or bases in
aqueous solutions, etc.).
Be able to write balanced equations for the reactions of period 3 oxides in water.
For example:
Na2O(s) + H2O (l)  2Na+(aq) + 2OH- (aq)
4.
Be able to write balanced equations for reactions involving alkali metals and/or halogens. Also realize that more reactive
halogens will oxidize less reactive halogens *Some of these can be treated as single displacement reactions where the most
reactive metal or nonmetal displaces the less reactive metal or nonmetal respectively. Material in Chapter 3.3 of Online
Text
For example:
Cl2 (aq) + 2 I- (aq)  I2 (aq) + 2 Cl- (aq)
5.
6.
7.
Explain why Sc and Zn are not considered to be transition metals (even though they are in the ‘d’ block of the periodic table.
Define “ligand” and be able to give examples of common ligands.
Explain why some complex ion solutions of transition metals are colored (and why others are not).