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Chapter 8: Problem 60

Considering the nonmetals, what is the relationship between the group number for an element (carbon, for example, belongs to group \(4 \mathrm{~A} ;\) see the periodic table on the inside front cover) and the number of single covalent bonds that element needs to form to conform to the octet rule?

Short Answer

Expert verified
The relationship between the group number (G) of a nonmetal element and the number of single covalent bonds (B) needed to satisfy the octet rule can be given as \(B = 8 - G\). This relationship is applicable for nonmetals belonging to groups 4A, 5A, 6A, and 7A as they form covalent bonds to conform to the octet rule.

Step by step solution

01

Understand the Group Number and Valence Electrons of an Element

In the periodic table, elements are arranged in columns according to their group numbers. The group number is related to the number of valence electrons which are the outer shell electrons of an atom. These valence electrons participate in the covalent bonds to satisfy the octet rule. It is important to note that we are only considering nonmetal elements for this exercise.
02

Relate the Group Number to the Number of Valence Electrons

Elements in the same group (column) of the periodic table have the same number of valence electrons. For example, Carbon belongs to group 4A, which means it has 4 valence electrons. Similarly, Nitrogen belongs to group 5A, so it has 5 valence electrons.
03

Determine the Number of Covalent Bonds Required to Satisfy the Octet Rule

Since the octet rule requires an atom to have a total of 8 electrons (4 electron pairs), we can determine the number of covalent bonds required by subtracting the number of valence electrons from 8. For example, Carbon has 4 valence electrons, so it needs 4 more electrons (8 - 4 = 4) to satisfy the octet rule. Therefore, Carbon needs to form 4 single covalent bonds.
04

Find the Relationship between Group Number and the Number of Covalent Bonds

Now, we can find the general relationship between the group number and the number of single covalent bonds needed for nonmetal elements. Let G be the group number and B be the number of single covalent bonds required. Then the relationship can be given as: B = 8 - G This relationship will only work for nonmetals belonging to 4A, 5A, 6A, and 7A groups, as they form covalent bonds to satisfy the octet rule.

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Most popular questions from this chapter

The substance chlorine monoxide, \(\mathrm{ClO}(g)\), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has a dipole moment of \(1.24 \mathrm{D}\) and the (a) Determine the magnitude of \(\mathrm{Cl}-\mathrm{O}\) bond length is \(1.60 \mathrm{~A}\). the charges on the \(\mathrm{Cl}\) and \(\mathrm{O}\) atoms in units of the electronic charge, e. (b) Based on the electronegativities of the elements, which atom would you expect to have a negative charge in the ClO molecule? (c) By using formal charges as a guide, propose the dominant Lewis structure for the molecule. Are the formal charges consistent with your answers to parts (a) and (b)? Can you reconcile any differences you find?

How many elements in the periodic table are represented by a Lewis symbol with a single dot? Are all these elements in the same group? Explain.

Use Lewis symbols and Lewis structures to diagram the formation of \(\mathrm{PF}_{3}\) from \(\mathrm{P}\) and \(\mathrm{F}\) atoms.

(a) What is meant by the term covalent bond? (b) Give three examples of covalent bonding. (c) A substance XY, formed from two different elements, boils at \(-33{ }^{\circ} \mathrm{C}\). Is XY likely to be a covalent or an ionic substance? Explain.

(a) Construct a Lewis structure for \(\mathrm{O}_{2}\) in which each atom achieves an octet of electrons. (b) Explain why it is necessary to form a double bond in the Lewis structure. (c) The bond in \(\mathrm{O}_{2}\) is shorter than the \(\mathrm{O}-\mathrm{O}\) bond in compounds that contain an \(\mathrm{O}-\mathrm{O}\) single bond. Explain this observation.
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