{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

2.14 (3) - not all paired The electrons add to the five...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Key for Micro Exam 2 Question 14 Question 14: Which of the following atoms are diamagnetic? Zn 2+ , Fe, Ti 2+ , Ar, S Answers: (a) Ti 2+ , Ar (b) Fe, Ti 2+ , Ar, S (c) Zn 2+ , Fe, Ti 2+ (d) Ar, Fe, S (e) Zn 2+ , Ar (f) Zn 2+ , Fe, Ti 2+ , Ar, S A diamagnetic species has all of its electrons paired up. We need to locate each of the elements on the periodic table and eliminate those choices that have unpaired electrons. This question may be more difficult that it initially appears. The first ion, Zn 2+ has 28 electrons since the neutral atom has 30 and this ion has lost two. The electrons lost are those of the 4s orbital since the 4s orbital electrons are the valence shell electrons. This means that the 3d orbital is completely filled and the electrons are all paired. While the Fe atom has 26 electrons, the 3d electrons are
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: not all paired. The electrons add to the five different orbitals within the 3d orbital set one at a time and are thus not all paired. (NOTICE that even though Fe has an even number of electrons, that does not mean that all the electrons are paired!) Ti 2+ has a similar configuration in that the two 4s electrons are lost but the two 3d electrons occupy different 3d orbitals. Ar is a diamagnetic species since its valence shell is filled and all of its electrons are paired. S is not diamagnetic because it has four 3p electrons which are spread out among the three 3p levels, leaving two electrons unpaired....
View Full Document

{[ snackBarMessage ]}

Ask a homework question - tutors are online