Fill in the blank with the appropriate numbers for both electrons and bonds (considering that single bonds are counted as one, double bonds as two, and triple bonds as three). (a) Iodine has ___________ valence electrons and makes ___________ bond(s) in compounds. (b) Silicon has ___________ valence electrons and makes ___________ bond(s) in compounds. (c) Phosphorus has ___________ valence electrons and makes ___________ bond(s) in compounds. (d) Sulphur has ___________ valence electrons and makes ___________ bond(s) in compounds.

Short Answer

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(a) Iodine has \(7\) valence electrons and makes \(1\) bond in compounds. (b) Silicon has \(4\) valence electrons and makes \(4\) bonds in compounds. (c) Phosphorus has \(5\) valence electrons and makes \(3\) bonds in most of its compounds. (d) Sulphur has \(6\) valence electrons and makes \(2\) bonds in most of its compounds.

Step by step solution

01

Determine the valence electrons

For each element, recall the periodic table's position and determine their respective number of valence electrons. The group number (column) can help with this task. (a) Iodine has \(7\) valence electrons, as it belongs to Group 17 of the periodic table. (b) Silicon has \(4\) valence electrons, as it belongs to Group 14 of the periodic table. (c) Phosphorus has \(5\) valence electrons, as it belongs to Group 15 of the periodic table. (d) Sulphur has \(6\) valence electrons, as it belongs to Group 16 of the periodic table.
02

Determine the number of bonds each element forms

For each element, relate the number of valence electrons to the number of bonds they form, considering that elements tend to follow the octet rule, striving to have 8 electrons in their valence shell. (a) Iodine forms \(1\) bond - it needs one more electron to achieve a stable octet configuration; it can share one electron with another atom via a single bond. (b) Silicon forms \(4\) bonds - it needs four more electrons to achieve a stable octet configuration; it can share four electrons with other atoms via four single bonds or combinations of double and triple bonds. (c) Phosphorus forms \(3\) bonds in most of its compounds - it needs three more electrons to achieve a stable octet configuration; it can share three electrons with other atoms via three single bonds or combinations of double and triple bonds. It's important to note that in some compounds, phosphorus can also form 5 bonds (such as in the case of PF5 - Phosphorus Pentafluoride) due to its ability to expand its octet. (d) Sulphur forms \(2\) bonds in most of its compounds - it needs two more electrons to achieve a stable octet configuration; it can share two electrons with other atoms via two single bonds, a double bond, or combinations of double and triple bonds. However, like phosphorus, sulphur can also expand its octet in few compounds (such as in SF6 - Sulfur Hexafluoride) and form more than 2 bonds. So the exercise solution looks like this: (a) Iodine has \(7\) valence electrons and makes \(1\) bond in compounds. (b) Silicon has \(4\) valence electrons and makes \(4\) bonds in compounds. (c) Phosphorus has \(5\) valence electrons and makes \(3\) bonds in most of its compounds. (d) Sulphur has \(6\) valence electrons and makes \(2\) bonds in most of its compounds.

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Most popular questions from this chapter

You and a partner are asked to complete a lab entitled "Carbonates of Group 2 metal" that is scheduled to extend over two lab periods. The first lab, which is to be completed by your partner, is devoted to carrying out compositional analysis and determine the identity of the Group 2 metal (M). In the second lab, you are to determine the melting point of this compound. Upon going to lab you find two unlabeled vials containing white powder. You also find the following notes in your partner's notebook-Compound 1: \(40.04 \% \mathrm{M}\) and \(12.00 \%\) C, \(47.96 \%\) O (by mass), Compound \(2: 69.59 \% \mathrm{M}\), \(6.09 \% \mathrm{C},\) and \(24.32 \% \mathrm{O}\) (by mass). (a) What is the empirical formula for Compound 1 and the identity of $\mathrm{M} ?(\mathbf{b})$ What is the empirical formula for Compound 2 and the identity of \(\mathrm{M}\) ? Upon determining the melting points of these two compounds, you find that both compounds do not melt up to the maximum temperature of your apparatus, instead, the compounds decompose and liberate colorless gas. (c) What is the identity of the colorless gas? (d) Write the chemical equation for the decomposition reactions of compound 1 and 2. (e) Are compounds 1 and 2 ionic or molecular?

Draw the dominant Lewis structures for these chlorineoxygen molecules/ions: $\mathrm{ClO}, \mathrm{ClO}^{-}, \mathrm{ClO}_{2}^{-}, \mathrm{ClO}_{3}^{-}, \mathrm{ClO}_{4}^{-}$. Which of these do not obey the octet rule?

Write Lewis structures that obey the octet rule for each of the following, and assign oxidation numbers and formal charges to each atom: $(\mathbf{a}) \mathrm{OCS},(\mathbf{b}) \mathrm{SOCl}_{2}(\mathrm{~S}$ is the central atom), (c) \(\mathrm{BrO}_{3}^{-}\), (d) \(\mathrm{HClO}_{2}(\mathrm{H}\) is bonded to \(\mathrm{O})\).

(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.

Potassium peroxide is composed of \(70.96 \% \mathrm{~K}\) and $29.04 \% \mathrm{O}\(. Each peroxide ion has a net charge of \)2^{-}$. (a) Given the molecular weight of the compound is 110.19 , determine the chemical formula of potassium peroxide. \((\mathbf{b})\) What is the number of valance electron pairs in the peroxide ion? (c) Draw the Lewis structure of the peroxide ion. (d) Compare the \(\mathrm{O}-\mathrm{O}\) bond distance in oxygen molecule and potassium peroxide.

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