Question

table to answer the questions:
rect electron configuration for
2d1
3s1
which of the following is the correct electron
configuration for titanium (ti)?
1s²2s²2p⁶3s²3p⁶4s²3d²
1s²2s²2p⁶3s²3p⁶3d⁴
1s²2s²2p⁶3s²3p⁶4s²4p²
done

Explanation:

Step1: Determine the atomic number of titanium

Titanium (Ti) has an atomic number \(Z = 22\).

Step2: Follow the Aufbau principle

According to the Aufbau principle, electrons fill orbitals in the order \(1s<2s < 2p<3s<3p<4s<3d<4p\cdots\).

• The \(1s\) orbital can hold \(2\) electrons (\(1s^{2}\)).
• The \(2s\) orbital can hold \(2\) electrons (\(2s^{2}\)).
• The \(2p\) orbital can hold \(6\) electrons (\(2p^{6}\)).
• The \(3s\) orbital can hold \(2\) electrons (\(3s^{2}\)).
• The \(3p\) orbital can hold \(6\) electrons (\(3p^{6}\)).
• The \(4s\) orbital is filled before the \(3d\) orbital (due to lower energy of \(4s\) compared to \(3d\) initially). The \(4s\) orbital can hold \(2\) electrons (\(4s^{2}\)).
• After filling \(4s\), we fill the \(3d\) orbital. For \(Z = 22\), after filling \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}\) (which accounts for \(2 + 2+6 + 2+6 + 2=20\) electrons), we have \(22- 20 = 2\) electrons left for the \(3d\) orbital (\(3d^{2}\)).

Answer:

\(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{2}\)