Chapter 21: Problem 19

Write electron configurations for each of the following. a. \(\mathrm{Ti}, \mathrm{Ti}^{2+}, \mathrm{Ti}^{\mathrm{i}+}\) b. \(\operatorname{Re}, \mathrm{Re}^{2+}, \mathrm{Re}^{3+}\) c. \(\mathrm{Ir}, \mathrm{Ir}^{2+}, \mathrm{Ir}^{3+}\)

Short Answer

Expert verified

a. Ti: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\); Ti²⁺: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^2\); Ti³⁺: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^1\) b. Re: \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^5\); Re²⁺: \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^3\); Re³⁺: \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^2\) c. Ir: \([Xe]6s^2 4f^{14} 5d^7\); Ir²⁺: \([Xe]6s^2 4f^{14} 5d^5\); Ir³⁺: \([Xe]6s^2 4f^{14} 5d^4\)

Step by step solution

Identify the number of electrons for each species

Using the periodic table, we can see that Titanium (Ti) has an atomic number of 22, which means it has 22 electrons. Ti²⁺ has lost 2 electrons, so it has 20 electrons. And Ti³⁺ has lost 3 electrons, so it has 19 electrons.

Write the electron configuration for each species

Using the periodic table to fill in orbitals, we can write the electron configurations as follows: Ti (22 electrons): \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\) Ti²⁺ (20 electrons): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^2\) Ti³⁺ (19 electrons): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^1\) b. Electron configurations for Re, Re²⁺, Re³⁺

Identify the number of electrons for each species

Rhenium (Re) has an atomic number of 75, which means it has 75 electrons. Re²⁺ has lost 2 electrons, so it has 73 electrons. And Re³⁺ has lost 3 electrons, so it has 72 electrons.

Write the electron configuration for each species

Using the periodic table to fill in orbitals, we can write the electron configurations as follows: Re (75 electrons): \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^5\) Re²⁺ (73 electrons): \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^3\) Re³⁺ (72 electrons): \([Kr]5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^2\) c. Electron configurations for Ir, Ir²⁺, Ir³⁺

Identify the number of electrons for each species

Iridium (Ir) has an atomic number of 77, which means it has 77 electrons. Ir²⁺ has lost 2 electrons, so it has 75 electrons. And Ir³⁺ has lost 3 electrons, so it has 74 electrons.

Write the electron configuration for each species

Using the periodic table to fill in orbitals, we can write the electron configurations as follows: Ir (77 electrons): \([Xe]6s^2 4f^{14} 5d^7\) Ir²⁺ (75 electrons): \([Xe]6s^2 4f^{14} 5d^5\) Ir³⁺ (74 electrons): \([Xe]6s^2 4f^{14} 5d^4\)

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Write electron configurations for each of the following. a. \(\mathrm{Ti}, \mathrm{Ti}^{2+}, \mathrm{Ti}^{\mathrm{i}+}\) b. \(\operatorname{Re}, \mathrm{Re}^{2+}, \mathrm{Re}^{3+}\) c. \(\mathrm{Ir}, \mathrm{Ir}^{2+}, \mathrm{Ir}^{3+}\)

Short Answer

Step by step solution

Identify the number of electrons for each species

Write the electron configuration for each species

Identify the number of electrons for each species

Write the electron configuration for each species

Identify the number of electrons for each species

Write the electron configuration for each species

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