Question

a neutral atom has the following characteristics: - it has 10 valence electrons - its a transition metal - the highest quantum level occupied is n = 4 what is the identity of this atom? enter either the element name or symbol (case insensitive). answer:

Explanation:

Step1: Determine the electron configuration

For a neutral atom, the number of electrons equals the atomic number. Since it's a transition metal with the highest quantum level \(n = 4\), the general form of the electron configuration for transition metals in the fourth period is \([Ar]4s^{x}3d^{y}\). The valence electrons for transition metals come from \(ns\) and \((n - 1)d\) orbitals. Here \(n=4\), so valence electrons are from \(4s\) and \(3d\) orbitals. Given there are 10 valence electrons. The \(4s\) orbital can hold a maximum of 2 electrons. Let the number of electrons in \(4s\) be \(x\) and in \(3d\) be \(y\), then \(x + y=10\). Since \(x\leqslant2\), if \(x = 2\), then \(y = 8\).
The electron configuration is \([Ar]4s^{2}3d^{8}\).

Step2: Calculate the atomic number

The atomic number of \(Ar\) is 18. The total number of electrons in the atom is \(18+2 + 8=28\).

Answer:

Nickel or \(Ni\)