Part c identify the general outer electron configuration for each group of elements shown in this periodic table outline. drag each label to the appropriate target.

From left to right:

1) Answer is: ns¹.

This is group 1 (alkaline metals).

For example, sodium (Na) is an element with atomic number 11 and it has one valence electron (3s¹) like all alkaline metals.

Electron configuration of sodium atom: ₁₁Na 1s² 2s² 2p⁶ 3s¹.

2) Answer is: ns²(n-1)d¹.

For example, scandium (Sc) is an element with atomic number 21.

Electron configuration of scandium atom: ₂₁Sc 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹.

3) Answer is: ns²(n-2)f⁷.

For example, europium (Eu) is an element with atomic number 63.

Electron configuration of europium atom: ₆₃Eu [Xe] 6s² 4f⁷.

4) Answer is: ns²(n-2)f¹⁴(n-1)d¹⁰np¹.

For example, thallium (Tl) is an element with atomic number 81.

Electron configuration of thallium atom: ₈₁Tl [Xe] 6s²4f¹⁴ 5d¹⁰ 6p1¹.

5) Answer is: ns²(n-1)d¹⁰np⁴.

For example, selenium (Se) is an element with atomic number 34.

Electronic configuration of selenium atom: ₃₄Se 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴.

6) Answer is: ns²np⁶.

For example, neon (symbol: Ne) is an element (noble gas) with atomic number 10, which means it has 10 protons and 10 electrons.

Electron configuration of neon atom: ₁₀Ne 1s²2s²2p⁶.

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."