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Chapter 6: Problem 74

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: (a) sodium, (b) sulfur, (c) fluorine.

Short Answer

Expert verified
In summary: a) Sodium: - Valence electrons: 1 - Core electrons: 10 - Unpaired electrons: 1 b) Sulfur: - Valence electrons: 6 - Core electrons: 10 - Unpaired electrons: 2 c) Fluorine: - Valence electrons: 7 - Core electrons: 2 - Unpaired electrons: 1

Step by step solution

01

Electron Configuration

Sodium has an atomic number of 11, which means it has 11 electrons. The electron configuration for sodium in its ground state is 1s²2s²2p⁶3s¹. Step 2: Identify the valence and core electrons
02

Valence and Core Electrons

The valence electrons are the electrons in the outermost energy level. In this case, there is only one valence electron (3s¹). The remaining 10 electrons are core electrons (1s²2s²2p⁶). Step 3: Determine the unpaired electrons
03

Unpaired Electrons

Sodium has only one unpaired electron in its 3s orbital. a) Summary for Sodium: - Valence electrons: 1 - Core electrons: 10 - Unpaired electrons: 1 b) Sulfur Step 1: Determine the electron configuration
04

Electron Configuration

Sulfur has an atomic number of 16, which means it has 16 electrons. The electron configuration for sulfur in its ground state is 1s²2s²2p⁶3s²3p⁴. Step 2: Identify the valence and core electrons
05

Valence and Core Electrons

The valence electrons are the electrons in the outermost energy level. In this case, there are six valence electrons (3s²3p⁴). The remaining 10 electrons are core electrons (1s²2s²2p⁶). Step 3: Determine the unpaired electrons
06

Unpaired Electrons

Sulfur has two unpaired electrons in its 3p orbitals. b) Summary for Sulfur: - Valence electrons: 6 - Core electrons: 10 - Unpaired electrons: 2 c) Fluorine Step 1: Determine the electron configuration
07

Electron Configuration

Fluorine has an atomic number of 9, which means it has 9 electrons. The electron configuration for fluorine in its ground state is 1s²2s²2p⁵. Step 2: Identify the valence and core electrons
08

Valence and Core Electrons

The valence electrons are the electrons in the outermost energy level. In this case, there are seven valence electrons (2s²2p⁵). The remaining two electrons are core electrons (1s²). Step 3: Determine the unpaired electrons
09

Unpaired Electrons

Fluorine has one unpaired electron in its 2p orbitals. c) Summary for Fluorine: - Valence electrons: 7 - Core electrons: 2 - Unpaired electrons: 1

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Most popular questions from this chapter

List the following types of electromagnetic radiation in order of descending wavelength: (a) UV lights used in tanning salons \((300-400 \mathrm{nm}) ;\) (b) radiation from an FM radio station at \(93.1 \mathrm{MHz}\) on the dial; (c) radiation from mobile phones \((450-2100 \mathrm{MHz}) ;\) (d) the yellow light from sodium vapor streetlights; (e) the red light of a light-emitting diode, such as in an appliance's display.

(a) Using Equation 6.5 , calculate the energy of an electron in the hydrogen atom when \(n=3\) and when \(n=6\). Calculate the wavelength of the radiation released when an electron moves from \(n=6\) to \(n=3 .(\mathbf{b})\) Is this line in the visible region of the electromagnetic spectrum?

Which of the following represent impossible combinations of \(n\) and $l ?(\mathbf{a}) 1 p,(\mathbf{b}) 4 s,(\mathbf{c}) 5 f,(\mathbf{d}) 2 d$

(a) For an He+ ion, do the \(2 s\) and \(2 p\) orbitals have the same energy? If not, which orbital has a lower energy? (b) If we add one electron to form the He atom, would your answer to part (a) change?

For orbitals that are symmetric but not spherical, the contour representations (as in Figures 6.23 and 6.24 ) suggest where nodal planes exist (that is, where the electron density is zero). For example, the \(p_{x}\) orbital has a node wherever \(x=0\). This equation is satisfied by all points on the \(y z\) plane, so this plane is called a nodal plane of the \(p_{x}\) orbital. (a) Determine the nodal plane of the \(p_{z}\) orbital. (b) What are the two nodal planes of the \(d_{x y}\) orbital? (c) What are the two nodal planes of the \(d_{x^{2}-y^{2}}\) orbital?
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