Question

Which represents the correct electron distribution of a transition element in the ground state?

A) 2-8-8-1
B) 2-8-8-2
C) 2-8-18-2
D) 2-8-18-3

Answer 1

The correct electron configuration of a transition element in the ground state is option C) 2-8-18-2, where the last two electrons are in the 4s sub-shell typical for transition metals in the d-block of the periodic table.

Step-by-step explanation:

The electron distribution that represents the correct electron configuration of a transition element in the ground state is C) 2-8-18-2. Transition elements typically have their outer electrons in the d sub-shell. The given configurations can be associated with the period and block of the elements in the periodic table. Transition elements are found in the d-block and typically display a configuration where the last electrons occupy the d sub-shell. When predicting electron configurations, one looks at the atomic number and allocates electrons according to the order of filling: 1s, 2s, 2p, 3s, 3p, 4s, 3d, and so on. Considering this order, 2-8-18-2 corresponds to a transition metal that has two electrons in its outermost 4s sub-shell, and a partially filled 3d sub-shell which is characteristic of transition elements.

Answer 2

I believe both C) and D) are correct, because both have enough electrons to show that the element has enough protons to be a transition metal, and both elements seem to have an electron configuration that exists in the ground state. We may need more information.