Write electron configurations for each of the following. a. \(\mathrm{Ti}, \mathrm{Ti}^{2+}, \mathrm{Ti}^{4+}\) b. \(\operatorname{Re}, \mathrm{Re}^{2+}, \mathrm{Re}^{3+}\) c. \(\mathrm{Ir}, \mathrm{Ir}^{2+}, \mathrm{Ir}^{3+}\)

Using the periodic table, find the atomic numbers for the elements mentioned in the exercise. a. Titanium (Ti): Atomic number 22 b. Rhenium (Re): Atomic number 75 c. Iridium (Ir): Atomic number 77

Write the electron configurations for each element using the elements' atomic numbers. Remember to follow the aufbau principle, the Pauli exclusion principle, and Hund's rule. a. Titanium (Ti) - Atomic number: 22 \(\mathrm{Ti: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2}\) b. Rhenium (Re) - Atomic number: 75 \(\mathrm{Re: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^5}\) c. Iridium (Ir) - Atomic number: 77 \(\mathrm{Ir: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^7}\)

Use the electron configurations from step 2 to find the electron configurations for the given ions. Remember to remove electrons when forming positive ions. a. Titanium Ions - \(\mathrm{Ti^{2+}: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^2}\) (Remove two electrons from the highest energy level - 4s) - \(\mathrm{Ti^{4+}: 1s^2 2s^2 2p^6 3s^2 3p^6}\) (Remove four electrons from the highest energy levels - 3d, and 4s) b. Rhenium Ions - \(\mathrm{Re^{2+}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^3}\) (Remove two electrons from the highest energy level - 6s) - \(\mathrm{Re^{3+}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^2}\) (Remove three electrons from the highest energy levels - 6s, and 5d) c. Iridium Ions - \(\mathrm{Ir^{2+}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^5}\) (Remove two electrons from the highest energy level - 6s) - \(\mathrm{Ir^{3+}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^4}\) (Remove three electrons from the highest energy levels - 6s, and 5d)