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Chapter 8: Problem 49

Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.

Short Answer

Expert verified
The correct statement about formal charge is option (b): To draw the best Lewis structure, you should minimize formal charge.

Step by step solution

01

Option (a): Formal charge is the same as oxidation number.

Formal charge and oxidation number are different concepts. Formal charge is the charge assigned to an atom in a molecule, assuming that electrons are shared equally between atoms. Oxidation number is the number of electrons that an atom loses or gains in a chemical reaction. Therefore, option (a) is false.
02

Option (b): To draw the best Lewis structure, you should minimize formal charge.

Minimizing formal charge helps in obtaining a more accurate representation of the molecule in the Lewis structure. By minimizing the formal charge, one can account for the most stable electron distribution within the molecule. Therefore, option (b) is true.
03

Option (c): Formal charge takes into account the different electronegativities of the atoms in a molecule.

Formal charge does not take into account the electronegativity of the atoms within a molecule. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons, while formal charge is calculated based on the assumption that electrons are equally shared between atoms. So, option (c) is false.
04

Option (d): Formal charge is most useful for ionic compounds.

Ionic compounds have a transfer of electrons between atoms, resulting in ions with whole number charges. Formal charge is more useful for covalent compounds, where electrons are shared between atoms. Option (d) is false.
05

Option (e): Formal charge is used in calculating the dipole moment of a diatomic molecule.

Dipole moment in a diatomic molecule is determined by the product of the charge difference between the two atoms and the distance between their nuclei. Formal charge does not directly determine the dipole moment as it focuses on the electron distribution around the atoms in a molecule. So, option (e) is false. From the analysis of the various options, we can conclude that: The correct answer is option (b): To draw the best Lewis structure, you should minimize formal charge.

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Most popular questions from this chapter

The hypochlorite ion, \(\mathrm{ClO}^{-},\) is the active ingredient in bleach. The perchlorate ion, \(\mathrm{ClO}_{4}^{-},\) is a main component of rocket propellants. Draw Lewis structures for both ions.

Draw the Lewis structures for each of the following ions or molecules. Identify those in which the octet rule is not obeyed; state which atom in each compound does not follow the octet rule; and state, for those atoms, how many electrons surround them: $(\mathbf{a}) \mathrm{HCl},(\mathbf{b}) \mathrm{ICl}_{5},\( (c) \)\mathrm{NO}\( (d) \)\mathrm{CF}_{2} \mathrm{Cl}_{2},(\mathbf{e}) \mathrm{I}_{3}^{-}$

(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 common form of elemental phosphorus is the white phosphorus, where four \(\mathrm{P}\) atoms are arranged in a tetrahedron. All four phosphorus atoms are equivalent. White phosphorus reacts spontaneously with the oxygen in air to form \(\mathrm{P}_{4} \mathrm{O}_{6} .\) (a) How many valance electron pairs are in the \(\mathrm{P}_{4} \mathrm{O}_{6}\) molecule? (b) When $\mathrm{P}_{4} \mathrm{O}_{6}\( is dissolved in water, it produces a \)\mathrm{H}_{3} \mathrm{PO}_{3}\(, molecule. \)\mathrm{H}_{3} \mathrm{PO}_{3}$ has two forms, \(\mathrm{P}\) forms 3 covalent bonds in the first form and \(\mathrm{P}\) forms 5 covalent bonds in the second form. Draw two possible Lewis structures of \(\mathrm{H}_{3} \mathrm{PO}_{3}\). (c) Which structure obeys the octet rule?

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?
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