Question

question 3 (2 points)
a metal \m\ has 2 valence electrons and a non - metal \x\ has 6 valence electrons.
what would be the formula for an ionic compound between \m\ and \x\?
mx₂
m₂x₆
mx₃
m₂x
mx

Explanation:

Step1: Determine the charge of metal M

A metal with 2 valence electrons will lose 2 electrons to achieve a stable electron configuration. So, the charge of \(M\) is \(M^{2 +}\).

Step2: Determine the charge of non - metal X

A non - metal with 6 valence electrons will gain 2 electrons to achieve a stable electron configuration. So, the charge of \(X\) is \(X^{2-}\).

Step3: Form the ionic compound

In an ionic compound, the sum of the charges of cations and anions must be zero. For \(M^{2+}\) and \(X^{2 -}\), using the criss - cross method (the magnitude of the charge of one ion becomes the subscript of the other ion), we get the formula \(MX\).

Answer:

MX