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Chapter 6: Problem 44

Give the symbols of (a) all the elements in period 5 that have at least two half-filled \(5 \mathrm{p}\) orbitals. (b) all the elements in Group 1 that have full \(3 \mathrm{p}\) orbitals. (c) all the metalloids that have paired \(3 p\) electrons. (d) all the nonmetals that have full \(3 \mathrm{~d}\) orbitals and 3 half- filled \(3 \mathrm{p}\) orbitals.

Short Answer

Expert verified
Question: Identify the following elements based on their electron configurations: a) Elements in period 5 with at least two half-filled 5p orbitals. b) Elements in Group 1 with full 3p orbitals. c) Metalloids with paired 3p electrons. d) Nonmetals with full 3d orbitals and 3 half-filled 3p orbitals. Answer: a) Krypton (Kr) b) None c) Silicon (Si) and Germanium (Ge) d) None

Step by step solution

01

a) Elements in period 5 with at least two half-filled 5p orbitals.

To solve this part, we first need to understand what period 5 and half-filled 5p orbitals mean. Period 5 corresponds to elements with principal quantum number n=5, while half-filled 5p orbitals mean that there are at least 2 electrons among the three 5p orbitals. In other words, the electron configuration should look like this: \(5\mathrm{p}^2\). Let's find the elements in period 5 that meet this condition: 1. Krypton (Kr) with electron configuration \([Ar] 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^2\) Since we found the element that meets the given criteria, our final answer for this part is Krypton (Kr).
02

b) Elements in Group 1 with full 3p orbitals.

Group 1 elements are alkali metals and always have one valence electron in the outermost s orbital. Thus, they cannot have full 3p orbitals, as they don't have 3p electrons in their electron configuration. Therefore, there are no elements in Group 1 with full 3p orbitals.
03

c) Metalloids with paired 3p electrons.

To have paired 3p electrons, an element must have all the 3p electron orbitals filled with two electrons each. Therefore, we are looking for metalloids that have \(3\mathrm{p}^6\) configuration. 1. Silicon (Si) with electron configuration \([Ne] 3s^2 3p^6\). 2. Germanium (Ge) with electron configuration \([Ar] 4s^2 3d^{10} 4p^6\). Silicon (Si) and Germanium (Ge) are both metalloids and meet the given criteria. Therefore, our final answer for this part is Silicon (Si) and Germanium (Ge).
04

d) Nonmetals with full 3d orbitals and 3 half-filled 3p orbitals.

Nonmetals generally have their outermost p orbitals partially filled, while full 3d orbitals mean that there are 10 electrons in the 3d orbitals. This would result in an electron configuration containing \(3\mathrm{d}^{10}\). However, no nonmetal has full 3d orbitals and 3 half-filled 3p orbitals, as this would mean having more than 8 valence electrons, which is not possible for nonmetals. Therefore, there are no nonmetals that meet the given criteria.

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Most popular questions from this chapter

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