Questions: tungsten: [Xe] 6s^2 4f^14 5d^4 inner electrons: 1s^1 2s^2 2p^6 3s^2 3d^10 3p^6 4s^2 4d^10 5p^6 outer electrons: 6s^2

Transcript text: tungsten: $[\mathrm{Xe}] 6 s^{2} 4 f^{14} 5 d^{4}$ inner electrons: $1 s^{1} 2 s^{2} 2 p^{6} 3 s^{2} 3 d^{10} 3 p^{6} 4 s^{2} 4 d^{10} 5 p^{6}$ outer electrons: $6 s^{2}$

Solution

Solution Steps

Step 1: Understanding the Electron Configuration of Tungsten

The electron configuration of tungsten is given as: \[ [\mathrm{Xe}] 6s^{2} 4f^{14} 5d^{4} \]

This notation indicates that tungsten has the same electron configuration as xenon, plus additional electrons in the $6s$, $4f$, and $5d$ orbitals.

Step 2: Identifying Inner Electrons

The inner electrons are those that are not in the outermost shell. The configuration for the inner electrons is given as: \[ 1s^{1} 2s^{2} 2p^{6} 3s^{2} 3d^{10} 3p^{6} 4s^{2} 4d^{10} 5p^{6} \]

These electrons fill the lower energy levels and are not involved in bonding.

Step 3: Identifying Outer Electrons

The outer electrons are those in the highest energy level, which are typically involved in chemical bonding. The outer electrons for tungsten are given as: \[ 6s^{2} \]

These are the electrons in the highest principal quantum number shell (n=6).