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Chapter 8: Problem 11

Write the Lewis symbol for atoms of each of the following elements: (a) \(\mathrm{Al}\), (b) \(\mathrm{Br}\), (c) \(\mathrm{Ar}\), (d) \(\mathrm{Sr}\).

Short Answer

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Short Answer: The Lewis symbols for the given elements are as follows: (a) Al\( \cdot \cdot \) (3 valence electrons) (b) Br with seven valence electrons as: ``` . . Br . . ``` (c) Ar with eight valence electrons arranged according to the octet rule: ``` . . . Ar . . . ``` (d) Sr\( \cdot \cdot \) (2 valence electrons)

Step by step solution

01

(a) Writing the Lewis Symbol for Al

Aluminum (Al) is a Group 13 element in the periodic table, hence it has 3 valence electrons. To write the Lewis symbol, we first write the chemical symbol for the element, Al, and then place three dots around it to represent the valence electrons. Lewis Symbol for Al: Al\( \cdot \cdot \) We've placed three valence electrons around the symbol of Aluminum.
02

(b) Writing the Lewis Symbol for Br

Bromine (Br) belongs to Group 17 in the periodic table, which means it has 7 valence electrons. To write the Lewis symbol, we first write the chemical symbol for Bromine, Br, and then place seven dots around it to represent valence electrons. Lewis Symbol for Br: Br\( \cdot \) ``` . . Br . . ``` We've placed seven valence electrons around the symbol of Bromine.
03

(c) Writing the Lewis Symbol for Ar

Argon (Ar) is a Group 18 element, indicating that it has 8 valence electrons. To write the Lewis symbol, we first write the chemical symbol of Argon, Ar, and then place eight dots around it to represent valence electrons. Lewis Symbol for Ar: Ar\( \cdot \) ``` . . . Ar . . . ``` The eight valence electrons are distributed according to the octet rule and placed around the symbol of Argon.
04

(d) Writing the Lewis Symbol for Sr

Strontium (Sr) is located in Group 2 of the periodic table, meaning that it has 2 valence electrons. To write the Lewis symbol, we write the chemical symbol for Strontium, Sr, and then place two dots around it to represent the valence electrons. Lewis Symbol for Sr: Sr\( \cdot \cdot \) We've placed two valence electrons around the symbol of Strontium. To sum up, we've written the Lewis symbols for each of the following elements: (a) \(\mathrm{Al}\), (b) \(\mathrm{Br}\), (c) \(\mathrm{Ar}\), and (d) \(\mathrm{Sr}\).

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Most popular questions from this chapter

Predict the chemical formula of the ionic compound formed between the following pairs of elements: (a) \(\mathrm{Al}\) and \(\mathrm{F},(\mathrm{b}) \mathrm{K}\) and \(\mathrm{S},(\mathrm{c}) \mathrm{Y}\) and \(\mathrm{O}\), (d) \(\mathrm{Mg}\) and \(\mathrm{N}\).

Acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and nitrogen \(\left(\mathrm{N}_{2}\right)\) both contain a triple bond, but they differ greatly in their chemical properties. (a) Write the Lewis structures for the two substances. (b) By referring to Appendix \(C\), look up the enthalpies of formation of acetylene and nitrogen and compare their reactivities. (c) Write balanced chemical equations for the complete oxidation of \(\mathrm{N}_{2}\) to form \(\mathrm{N}_{2} \mathrm{O}_{5}(g)\) and of acetylene to form \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(g)\). (d) Calculate the enthalpy of oxidation per mole of \(\mathrm{N}_{2}\) and \(\mathrm{C}_{2} \mathrm{H}_{2}\) (the enthalpy of formation of \(\mathrm{N}_{2} \mathrm{O}_{5}(\mathrm{~g})\) is \(11.30 \mathrm{~kJ} / \mathrm{mol}\) ). How do these comparative values relate to your response to part (b)? Both \(\mathrm{N}_{2}\) and \(\mathrm{C}_{2} \mathrm{H}_{2}\) possess triple bonds with quite high bond enthalpies (Table 8.4). What aspect of chemical bonding in these molecules or

(a) When talking about atoms in a Lewis structure, what is meant by the term formal charge? (b) Does the formal charge of an atom represent the actual charge on that atom? Explain. (c) How does the formal charge of an atom in a Lewis structure differ from the oxidation number of the atom?

Based on data in Table \(8.2\), estimate (within \(30 \mathrm{~kJ} / \mathrm{mol}\) ) the lattice energy for (a) LiBr, (b) \(\mathrm{CsBr}\), (c) \(\mathrm{CaCl}_{2}\).

Would you expect AlN to have a lattice energy that is larger or smaller than ScN? Explain.
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