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Question 3 of 9

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Each of the following questions consists of two statements, I in the left-hand column and II in the right-hand column. For each question, determine whether statement I is true or false and whether statement II is true or false. Select the appropriate answer combination from the choices below. Choices with a filled CE oval denote that statement II is a correct explanation of the true statement I.

An element that has the electron configuration

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {3 d}^{3} {4 s}^{2}

is a transition element

BECAUSE

in atoms of transition elements, the

1 s

,

2 s

,

2 p

,

3 s

, and

3 p

orbitals are completely filled in the ground state.

Select an Answer

Correct Answer:

No

Correct Answer:

Yes

Correct Answer:

No

Correct Answer:

No

Correct Answer:

No

View Correct Answer

The correct answer is T, T.

The element with the electron configuration shown is vanadium (atomic number = $23$ ). The transition elements are those in groups 3-12 (or groups $IIIB - IIB$ , depending on how a particular periodic table is labeled). Therefore, statement $I$ is true. It is also true that the $1 s$ , $2 s$ , $2 p$ , $3 s$ , and $3 p$ orbitals are completely filled in the transition elements. However, statement $II$ is not a correct explanation of statement $I$ . For example, statement $II$ is true for $Ar$ , $Kr$ , $Xe$ , $Rn$ , and other elements that are not transition elements.