Question

Using periodic trends only, which element is described by each of the following?

A.) smallest atomic radius in Group 6

B.) Highest EN in Period 6

C.) Highest IE1 in group 14

D.) Lowst IE1 in Period 5

E.) Most metallic in Group 15

F.) Period 4 element with filled outer level

G.) Condensed ground-state electron configuration is [Ne] 3s2 3p2

H.) Form 2 + ion with electron configuration [Ar]

Answer 1

A. Smallest atomic radius in group 6: Oxygen (O)

Ionic radius increases as we go down from top to bottom in a group, because energy level gets added up as we move down which increases the size. Oxygen is element in 1st period and 6th group.

B. Highest EN in period 6: Gold (Au)

The electronegativity is the element's ability to attract electrons. As we move across the period, the electronegativity increases. However, if the orbitals are little less than half or full configuration of electrons, then they become more electronegative as they need only one electron to become full. Au has electronic configuration of [Xe]4f¹⁴5d¹⁰6s¹. So,it needs only one electron to complete its s orbital.

C. Highest IE1 in period 14: Carbon (C)

Ionisation energy is the energy need to remove an electron from the atom. As, we move down the group, IE decreases, because the size increases and it becomes easy to remove the electron from the shell. But Carbon being the smallest, has the highest IE.

D. Lowest IE1 in period 5: Rubidium (Rb)

As we move across the period, the size decreases and the IE increases. Thus, in period %, Rb has the lowest IE. Secondary, on removing one electron from Rb will lead to a stable electronic configuration as it lies in group 1. It will attain electronic configuration of Kr, which is a noble metal.

E. Most metallic in Group 15. Bismuth (Bi)

In the group 15, Bi has the lowest EN, thus it can easily lose one electron and becomes most metallic in the group.

F. Period 4 element with filled outer orbital: Krypton (Kr)

Krypton is the noble element and lies in the 18th group. Being a noble metal, it has all the orbitals completely filled. Rest of the elements in period 4 do not have all the orbitals completely filled.

G. Condensed ground-state electron configuration is [Ne] 3s² 3p² : Germanium (Ge)

[Ne] 3s² 3p² means the atomic number is 32. And Germanium has atomic number 32.

H. Form 2+ ion with electron configuration [Ar] 3d³: Vanadium (V)

Vanadium ground state electronic configuration is [Ar] 3d³4s². On losing 2 electrons, it become V²⁺. the electronic configuration of V²⁺ is[Ar] 3d³.