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Chapter 8: Problem 1

For each of these Lewis symbols, indicate the group in the periodic table in which the element \(\mathrm{X}\) belongs: [Section 8.1\(]\) $$(\mathbf{a}) \cdot \dot{\chi} \cdot \quad(\mathbf{b}) \cdot \mathbf{X} \cdot \quad(\mathbf{c}) : \dot{\chi}$$

Short Answer

Expert verified
The elements \(\mathrm{X}\) with given Lewis symbols belong to the following groups in the periodic table: - (a) \(\cdot \dot{\chi} \cdot\) , 2 valence electrons: Group 2 (Alkaline earth metals) - (b) \(\cdot \mathbf{X} \cdot\) , 1 valence electron: Group 1 (Alkali metals) - (c) \(: \dot{\chi}\) , 3 valence electrons: Group 13 (Boron group)

Step by step solution

01

Determine the number of valence electrons for each Lewis symbol

A Lewis symbol represents the element with its valence electrons. The number of valence electrons can be determined by counting the number of dots around the element symbol. For each given Lewis symbol, we will count the dots and determine the valence electrons: - (a) \(\cdot \dot{\chi} \cdot\) , there are 2 dots, so 2 valence electrons - (b) \(\cdot \mathbf{X} \cdot\) , there is 1 dot, so 1 valence electron - (c) \(: \dot{\chi}\) , there are 3 dots, so 3 valence electrons
02

Identify the group in the periodic table

The number of valence electrons determines the group in the periodic table to which the element belongs. Here are the groups that correspond to each number of valence electrons: - 1 valence electron: Group 1 (Alkali metals) - 2 valence electrons: Group 2 (Alkaline earth metals) - 3 valence electrons: Group 13 (Boron group) Now, we can assign each element with its number of valence electrons to the appropriate group in the periodic table: - (a) \(\cdot \dot{\chi} \cdot\) , 2 valence electrons: Group 2 (Alkaline earth metals) - (b) \(\cdot \mathbf{X} \cdot\) , 1 valence electron: Group 1 (Alkali metals) - (c) \(: \dot{\chi}\) , 3 valence electrons: Group 13 (Boron group)

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Most popular questions from this chapter

Use Lewis symbols and Lewis structures to diagram the formation of \(\mathrm{PF}_{3}\) from \(\mathrm{P}\) and \(\mathrm{F}\) atoms, showing valence- shell electrons. (a) How many valence electrons does P have initially? (b) How many valence electrons does each F have initially? ( c) How many valence electrons surround the Pin the PF_ \(_{3}\) molecule? (d) How many valence electrons surround each \(\mathrm{F}\) in the \(\mathrm{PF}_{3}\) molecule? (e) How many bonding pairs of electrons are in the \(\mathrm{PF}_{3}\) molecule?

By referring only to the periodic table, select (a) the most electronegative element in group \(6 \mathrm{A} ;(\mathbf{b})\) the least electronegative element in the group Al, Si, P; (c) the most electronegative element in the group \(\mathrm{Ga}, \mathrm{P}, \mathrm{Cl}, \mathrm{Na} ;(\mathbf{d})\) the element in the group \(\mathrm{K}\) \(\mathrm{C}, \mathrm{Zn}, \mathrm{F}\) that is most likely to form an ionic compound with Ba.

Which of the following bonds are polar? (a) \(\mathrm{B}-\mathrm{F}\) (b) Cl-Cl, (c) Se-O, (d) H-I. Which is the more electronegative atom in each polar bond?

(a) Construct a Lewis structure for \(\mathrm{O}_{2}\) in which each atom achieves an octet of electrons. (b) How many bonding electrons are in the structure? (c) Would you expect the \(\mathrm{O}-\mathrm{O}\) bond in \(\mathrm{O}_{2}\) to be shorter or longer than the \(\mathrm{O}-\mathrm{O}\) bond in compounds that contain an \(\mathrm{O}-\mathrm{O}\) single bond? Explain.

(a) True or false: An element's number of valence electrons is the same as its atomic number. (b) How many valence electrons does a nitrogen atom possess? (c) An atom has the electron configuration 1\(s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}\) . How many valence electrons does the atom have?
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