Question

question 13 (2 points)
what element has the electron configuration 1s²2s²2p⁶3s²3p²?
o a nitrogen
b selenium
o c silver
d silicon

question 14 (1 point)
which of the following is true about the electron configurations of the noble gases?
o a the highest occupied s and p sublevels are partially filled.
b the highest occupied s and p sublevels are completely filled.
o c the electrons with the highest energy are in a d sublevel.
d the electrons with the highest energy are in an f sublevel.

question 15 (1 point)
elements that are characterized by the filling of p orbitals are classified as _.
o a inner transition metals
b transition metals
o c groups 1a and 2a
d groups 3a through 8a

Explanation:

Question 13

Step1: Calculate the number of electrons

The sum of the exponents in the electron configuration gives the number of electrons. \(2 + 2+6 + 2+2=14\) electrons.

Step2: Relate the number of electrons to atomic number

In a neutral atom, the number of electrons is equal to the atomic number. So the atomic number \(Z = 14\).

Step3: Identify the element

Looking at the periodic table, the element with atomic number \(14\) is silicon (\(Si\)).

Noble gases have a stable electron configuration. The highest - occupied \(s\) and \(p\) sublevels are completely filled. For example, helium (\(He:1s^{2}\)), neon (\(Ne:1s^{2}2s^{2}2p^{6}\)) etc.

• Inner - transition metals (\(f\) - block elements) are characterized by the filling of \(f\) orbitals.
• Transition metals (\(d\) - block elements) are characterized by the filling of \(d\) orbitals.
• Groups \(1A\) and \(2A\) are characterized by the filling of \(s\) orbitals (\(ns^{1}\) for \(1A\) and \(ns^{2}\) for \(2A\)).
• Groups \(3A - 8A\) (\(p\) - block elements) are characterized by the filling of \(p\) orbitals (\(ns^{2}np^{1 - 6}\))

Answer:

d. silicon

Question 14