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Chapter 1: Problem 23

How many electrons are in the valence shell of each atom? (a) Carbon (b) Nitrogen (c) Chlorine (d) Aluminum

Short Answer

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Question: How many valence electrons are in the following atoms: (a) Carbon (C) (b) Nitrogen (N) (c) Chlorine (Cl) (d) Aluminum (Al) Answer: (a) Carbon: 4 valence electrons (b) Nitrogen: 5 valence electrons (c) Chlorine: 7 valence electrons (d) Aluminum: 3 valence electrons

Step by step solution

01

Find the atomic numbers

To determine the atomic numbers of each atom, we can refer to the periodic table. The atomic numbers are: - Carbon (C): 6 - Nitrogen (N): 7 - Chlorine (Cl): 17 - Aluminum (Al): 13
02

Determine the electron configurations

To determine the electron configuration of each atom, we can use the atomic numbers as follows: - For Carbon (C), the atomic number is 6, the electron configuration is 1s^2 2s^2 2p^2. - For Nitrogen (N), the atomic number is 7, the electron configuration is 1s^2 2s^2 2p^3. - For Chlorine (Cl), the atomic number is 17, the electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^5. - For Aluminum (Al), the atomic number is 13, the electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^1.
03

Determine the valence electrons

The valence electrons are the electrons in the outermost energy level (shell). We can look at the electron configuration for each atom to determine the number of valence electrons: - Carbon (C): 2s^2 2p^2 => 4 valence electrons. - Nitrogen (N): 2s^2 2p^3 => 5 valence electrons. - Chlorine (Cl): 3s^2 3p^5 => 7 valence electrons. - Aluminum (Al): 3s^2 3p^1 => 3 valence electrons. So, the number of valence electrons for each atom is: (a) Carbon: 4 (b) Nitrogen: 5 (c) Chlorine: 7 (d) Aluminum: 3

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Most popular questions from this chapter

Which compounds have nonpolar covalent bonds, which have polar covalent bonds, and which have ions? (a) LiF (b) \(\mathrm{CH}_{3} \mathrm{~F}\) (c) \(\mathrm{MgCl}_{2}\) (d) \(\mathrm{HCl}\)

Using the symbols \(\delta-\) and \(\delta+\), indicate the direction of polarity in each polar covalent bond. (a) \(\mathrm{C}-\mathrm{N}\) (b) \(\mathrm{N}-\mathrm{O}\) (c) \(\mathrm{C}-\mathrm{Cl}\)

Which molecules are polar? For each that is polar, specify the direction of its dipole moment. (a) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (b) \(\mathrm{HCN}\) (c) \(\mathrm{H}_{2} \mathrm{O}_{2}\)

Draw Lewis structures for these ions, and show which atom in each bears the formal charge. (a) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) (b) \(\mathrm{CO}_{3}{ }^{2-}\) (c) \(\mathrm{OH}^{-}\)

Why does fluorine, the element in the upper right corner of the Periodic Table, have the largest electronegativity of any element?
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