This document contains questions and activities about periodic trends, including: - Comparing the ionic radii and electronic configurations of Li+ and Be2+ - Explaining why Na has a higher melting point than Cs - Discussing why ionic compounds don't have bond angles - Describing the periodic table in terms of proton number, periods, groups, and chemical properties - Explaining trends in ionization energy using knowledge of effective nuclear charge and electron shells

1.  Compare
the ionic radii of Li+ and Be2+.
Include their electronic configurations.
 Why does Na have a higher melting point
than Cs ?
 Why don’t ionic compounds have bond
angles?
 S&C
: Why do the noble gases not have an
atomic radius ?

2.  Must
: Describe PT in terms of proton
number, periods, groups, and chemical
property.
 Should : Comment on similar chemical
property of isoelectronic species.
 Could : Explain trend in ionisation energies
using knowledge of enc and shells.

3.  Periodicity


is a plate spinning activity :-
Plate 1 is effective nuclear charge
Plate 2 is number of shells.
 Which
one wins ?
 Complete
booklet.
and highlight pages 2 and 3 in your

4.  Activity
 On
your blank Periodic Tables draw trend
lines for :



Melting point – Groups 1,2,7
Ionisation energy
Atomic Radius
Electronic configurations of the TMs

5. 2) Which isoelectronic species has the largest radius?
a. Mg2+ b.N3- c. O2- d. F

6.  Pages
4,5,6

7.  Must
: Describe PT in terms of proton
number, periods, groups, and chemical
property.
 Should : Comment on similar chemical
property of isoelectronic species.
 Could : Explain trend in ionisation energies
using knowledge of enc and shells.