Question

6. For each set of elements below, make a list of the largest radius, smallest radius, highest first ionization energy, lowest first ionization energy, most metallic, and least metallic. It may help to design a table that lists the elements in the first column and then has 6 headings to answer the other questions. a. Na, K, Rb, Cs b. B, N, F.Ne c. C, Ge, Sn, Pb

Answer 1

(a) Na, K, Rb,Cs are in I A group elements in the periodic table

ATOM	largest radius	smallest radius	highest first ionization energy	lowest ionization energy	most metallic	least metallic
Na		Na	Na			Na
K
Rb
CS	Cs			Cs	Cs

Explanation: Atomic Radius : In the group from top to bottom atomic size increases then atomic radius increases. So from Na to Cs atomic radius increases. Na has smallest radius and Cs has highest radius Ionization Energy: ionization energy is inversely proportional to atomic radius largest radius atom has lowest first ionization energy. smallest radium atom has highest first ionization energy. in the group from top to bottom first ionization energy decreases due to increase in atomic radius. so Cs has lowest first ionization energy and Na has highest ionization energy   Metallic character: Metallic property increases from top to bottom in a group   So Na is least metallic and Cs has most metallic (b) B,N,F, Ne - These are 2 st period elements.

atom	largest radius	smallest radius	highest first ionization energy	lowest ionization energy	most metallic	least metallic
B	B			B	B
N
F
Ne		Ne	Ne			Ne

In period atomic radius decreases from left to right. In period ionization energy increases fro left to right. in period metallic property decreases from left to right. in 2nd period left to right the elements in the order is B, N , F , Ne (c) c, Ge, Sn ,Pb - these are iv a group elements

atom	largest radius	smallest radius	highest first ionization energy	lowest ionization energy	most metallic	least metallic
C		C	C			C
Ge
Sn
Pb	Pb			Pb	Pb