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Chapter 13: Problem 1

For each of the following neutral atoms give the core charge. a) Li. b) \(\quad \ddot{C l}\) c) He:

Short Answer

Expert verified
The core charges for Li, Cl, and He are +3, +7, +2 respectively.

Step by step solution

01

Determine core charge for Li

For Lithium (Li), the atomic number is 3, which means there are 3 protons. Lithium has no shielding electrons, because it only has 1 valence electron. Applying the formula \(Z_{eff}=Z-S\), we get \(3-0=3\). Hence, the core charge of Li is +3.
02

Determine core charge for Cl

For Chlorine (Cl), the atomic number is 17, which means there are 17 protons. Chlorine has 10 shielding electrons (total electrons minus valence electrons = 17-7). Applying the formula \(Z_{eff}=Z-S\), we get \(17-10=7\). Hence, the core charge of Cl is +7.
03

Determine core charge for He

For Helium (He), the atomic number is 2, which means there are 2 protons. Helium has no shielding electron, since it has 2 electrons which are both valence electrons. Applying the formula \(Z_{eff}=Z-S\), we get \(2-0=2\). Hence, the core charge of He is +2.

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Most popular questions from this chapter

Without attempting to draw a Lewis structure, calculate the total number of valence electrons in each of these molecules: a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)

What is the total number of electrons in the Lewis structure in Model 3 for each molecule: a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)

Given the shell model of the atom, suggest a possible reason that Lewis proposed a maximum of two electrons for hydrogen and a maximum of eight for carbon, nitrogen, oxygen, and fluorine atoms?

What is the likely formula for a molecule composed of hydrogen atoms and one sulfur atom? Draw the Lewis structure for this molecule.

Use your checklist to determine whether or not the following is a correct structure for \(\mathrm{CO}_{2}\) $$ \ddot{\mathrm{O}}=\mathrm{C}=\ddot{\mathrm{O}} $$
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