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Chapter 7: Problem 152

How many unpaired electrons are present in each of the firstrow transition metals in the ground state?

Short Answer

Expert verified
In the ground state, the first-row transition metals have the following unpaired electrons: Scandium (Sc) - 1, Titanium (Ti) - 2, Vanadium (V) - 3, Chromium (Cr) - 5, Manganese (Mn) - 5, Iron (Fe) - 4, Cobalt (Co) - 3, Nickel (Ni) - 2, Copper (Cu) - 1, and Zinc (Zn) - 0.

Step by step solution

01

Determine Electron Configurations

For each element, we will write down its electron configuration, focusing on the d orbital. Sc: [Ar] 4s2 3d1 Ti: [Ar] 4s2 3d2 V: [Ar] 4s2 3d3 Cr: [Ar] 4s1 3d5 Mn: [Ar] 4s2 3d5 Fe: [Ar] 4s2 3d6 Co: [Ar] 4s2 3d7 Ni: [Ar] 4s2 3d8 Cu: [Ar] 4s1 3d10 Zn: [Ar] 4s2 3d10
02

Count Unpaired Electrons

We will now count the unpaired electrons in the d orbital for each of these elements. Sc: 1 unpaired electron Ti: 2 unpaired electrons V: 3 unpaired electrons Cr: 5 unpaired electrons Mn: 5 unpaired electrons Fe: 4 unpaired electrons Co: 3 unpaired electrons Ni: 2 unpaired electrons Cu: 1 unpaired electron Zn: 0 unpaired electrons In summary, the first-row transition metals have the following unpaired electrons in their ground state: - Scandium (Sc): 1 - Titanium (Ti): 2 - Vanadium (V): 3 - Chromium (Cr): 5 - Manganese (Mn): 5 - Iron (Fe): 4 - Cobalt (Co): 3 - Nickel (Ni): 2 - Copper (Cu): 1 - Zinc (Zn): 0

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Most popular questions from this chapter

Write equations corresponding to the following. a. the fourth ionization energy of Se b. the electron affinity of \(\mathrm{S}^{-}\) c. the electron affinity of \(\mathrm{Fe}^{3+}\) d. the ionization energy of \(\mathrm{Mg}\)

Using only the periodic table inside the front cover of the text, write the expected ground-state electron configurations for a. the third element in Group \(5 \mathrm{~A}\). b. element number 116 . c. an element with three unpaired \(5 d\) electrons. d. the halogen with electrons in the \(6 p\) atomic orbitals.

Three elements have the electron configurations \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}\), \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}\), and \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}\). The first ionization en- ergies of these elements (not in the same order) are \(0.590,0.999\), and \(0.738 \mathrm{MJ} / \mathrm{mol}\). The atomic radii are 104,160 , and \(197 \mathrm{pm}\). Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration. Complete the following table with the correct information.

Rank the elements \(\mathrm{Be}, \mathrm{B}, \mathrm{C}, \mathrm{N}\), and \(\mathrm{O}\) in order of increasing first ionization energy. Explain your reasoning.

How many orbitals in an atom can have the designation \(5 p\), \(3 d_{z^{2}}, 4 d, n=5, n=4 ?\)
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