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Chapter 4: Problem 142

Name each element and tell how many valence electrons it has: (a) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}\) (b) \([\mathrm{Ne}] 3 \mathrm{~s}^{1}\) (c) \([\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{3}\)

Short Answer

Expert verified
(a) Silicon (Si) with 4 valence electrons. (b) Sodium (Na) with 1 valence electron. (c) Arsenic (As) with 5 valence electrons.

Step by step solution

01

(a) Identify the element and valence electrons for \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}\)

We can determine the total number of electrons by adding the superscript of all the terms: \(1s^{2}\) has 2 electrons \(2s^{2}\) has 2 electrons \(2p^{6}\) has 6 electrons \(3s^{2}\) has 2 electrons \(3p^{2}\) has 2 electrons Adding all electrons, we get: 2+2+6+2+2=14 electrons An element with 14 electrons is Silicon (Si). The valence electrons are the outermost electrons, present in the 3rd shell: \(3s^{2} 3p^{2}\). Thus, Silicon has a total of 4 valence electrons.
02

(b) Identify the element and valence electrons for \([\mathrm{Ne}] 3 \mathrm{~s}^{1}\)

This electron configuration begins with the noble gas Neon (Ne) and has an additional electron in the \(3s^{1}\) orbital. Neon has 10 electrons; therefore, this element has 11 electrons in total. An element with 11 electrons is Sodium (Na). Since the additional electron is in the 3rd shell, Sodium has 1 valence electron.
03

(c) Identify the element and valence electrons for \([\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{3}\)

This electron configuration stars with the noble gas Argon (Ar) and has additional electrons in the \(4s^{2}\), \(3d^{10}\), and \(4p^{3}\) orbitals. Argon has 18 electrons; therefore, with the additional electrons, this element has 18+2+10+3 = 33 electrons in total. An element with 33 electrons is Arsenic (As). The valence electrons are in the 4th shell: \(4s^{2} 4p^{3}\). Thus, Arsenic has a total of 5 valence electrons.

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Most popular questions from this chapter

Taking all configurations to be for neutral atoms, identify the elements having the following electron configurations: (a) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{5}\) (b) \(1 s^{2} 2 s^{2} 2 p^{1}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{1}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{2} 4 d^{10} 5 p^{6} 6 s^{2} 4 f^{14} 5 d^{10} 6 p^{6}\) \(7 s^{2} 6 d^{1} 5 f^{3}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}\)

Rank visible light, gamma rays, X-rays, radio/ television waves, infrared radiation, and ultraviolet light in order of (a) increasing wavelength and (b) increasing energy.

What is the implication of thinking about atomic electrons as clouds that got Einstein so upset? What did Schrödinger call these clouds?

Arrange the following atoms in order of increasing atomic size: \(\mathrm{Ne}, \mathrm{As}, \mathrm{Se}, \mathrm{K}, \mathrm{S}, \mathrm{Cl}\)

Which of the following electron transitions in hydrogen would absorb the largest amount of energy? A. \(n=2\) to \(n=3\) B. \(\quad n=2\) to \(n=4\) C. \(n=1\) to \(n=4\) D. \(n=3\) to \(n=1\) E. \(n=7\) to \(n=1\)
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