Final answer:
The correct order for both decreasing atomic radius and increasing first ionization energy is option 4: Ca, Ga, Cl, S, P. The arrangement aligns with the trends in the periodic table,, where atomic radius decreases across a period and increases down a group, while ionization energy increases across a period and decreases down a group.
So option (4) is correct.
Step-by-step explanation:
To arrange the atoms according to decreasing atomic radius and increasing first ionization energy (IE), we must understand the periodic trends. The atomic radius decreases across a period from left to right and increases down a group. Conversely, the first ionization energy tends to increase across a period from left to right and decreases down a group.
Given the elements, Ca (Calcium), Ga (Gallium), Cl (Chlorine), S (Sulfur), and P (Phosphorus), their position in the periodic table determines these properties:
Decreasing atomic radius: Cl, S, P, Ga, Ca
Increasing first ionization energy: Ca, Ga, P, S, Cl
The correct arrangement that satisfies both decreasing atomic radius and increasing first ionization energy is
option 4: Ca, Ga, Cl, S, P.
For the other examples, the order of increasing ionization energy would be:
Na, K, Ca, O, Ne
Rb, Li, N, F
Si, Mg, S, N, He
Mg, Si, S, O
Na, Mg, Ca, K, Rb, Sr
Similarly, the order of increasing atomic radii would be:
Cl, S, Mg, Na
Mg, Ca, Rb, Cs
Cl, Si, Ca, Sr
Atoms with a valence shell electron configuration of ns²np³ are from Group 15 (Pnictogens), while those with ns² are from Group 2 (Alkaline Earth Metals).