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Chapter 3: Problem 54

Draw a Lewis structure of a covalent compound in which oxygen has: (a) Two single bonds and two unshared pairs of electrons (b) One double bond and two unshared pairs of electrons

Short Answer

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(a) Example: H鈧侽; (b) Example: O鈧�.

Step by step solution

01

Identify the Valence Electrons

Oxygen has 6 valence electrons as it is in Group 16 of the periodic table. This will help us determine how the electrons will be shared or paired.
02

(a) Two Single Bonds and Two Unshared Pairs

To draw a Lewis structure where oxygen has two single bonds and two unshared pairs: 1. Assign each single bond two electrons to connect oxygen to another element, such as hydrogen. 2. Use the remaining four electrons to complete the two unshared pairs around oxygen. For example, in water (H鈧侽), each hydrogen shares an electron with oxygen.
03

(b) One Double Bond and Two Unshared Pairs

To draw a Lewis structure where oxygen has one double bond and two unshared pairs: 1. Assign the double bond by sharing two pairs of electrons between oxygen and another atom, such as in an oxygen (O鈧�) molecule. 2. The remaining four electrons form the two unshared pairs around the oxygen atom.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Valence Electrons
Valence electrons are the outermost electrons in an atom and they play a crucial role in chemical bonding. For oxygen, which resides in Group 16 of the periodic table, it possesses 6 valence electrons. Understanding the number of valence electrons helps us predict how an atom will bond with others. These electrons can be imagined as dots around the chemical symbol in a Lewis structure. This representation helps us visualize the potential bonds an oxygen atom can form and the arrangement of its electrons. Since every electron wants to be paired, the way these valence electrons are distributed significantly impacts the molecule's shape and stability.
Covalent Bonding
Covalent bonding occurs when two atoms share one or more pairs of electrons. This kind of bond typically happens between non-metal atoms with similar electronegativities. In the case of oxygen-based molecules, the oxygen atom often forms covalent bonds by sharing its valence electrons with other atoms.
  • Single bonds: When only one pair of electrons is shared, such as in the case of water (H鈧侽), oxygen forms single covalent bonds with hydrogen atoms.
  • Double bonds: When two pairs of electrons are shared, as seen in an oxygen molecule (O鈧�), forming a double covalent bond between two oxygen atoms.
Covalent bonds are strong and vital for creating stable compounds, which are essential for various chemical and biological processes.
Unshared Pairs
Unshared pairs, also known as lone pairs, are pairs of valence electrons that are not involved in bonding. In our examples with oxygen, unshared pairs play a pivotal role. Each oxygen atom has typically two unshared pairs. These non-bonding electrons affect the geometry and the physical properties of the molecule. For instance, in water, the two unshared pairs on the oxygen atom push the hydrogen atoms closer together, resulting in a bent shape rather than a straight line. Unshared pairs also contribute to the reactivity and polarity of molecules, influencing how they interact with other compounds.
Oxygen Compounds
Oxygen is a highly reactive element known for forming a wide range of compounds. It readily engages in forming covalent bonds due to its high electronegativity and the presence of 6 valence electrons. Oxygen compounds are prevalent and essential in various chemical contexts.
  • Water (H鈧侽): Exhibits two single bonds and supports life through its unique properties.
  • Oxygen Gas (O鈧�): Comprised of a double bond, necessary for respiration in living organisms.
  • Carbon Dioxide (CO鈧�): Contains two oxygen atoms each with double bonds, playing a crucial role in the earth's carbon cycle.
Each compound exhibits different chemical behaviors and properties influenced by the type of bonds and the presence of unshared pairs in their structure.

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Most popular questions from this chapter

Answer true or false. (a) For Group 1A and Group 2A elements, the name of the ion each forms is simply the name of the element followed by the word ion; for example, \(\mathrm{Mg}^{2+}\) is named magnesium ion. (b) \(\mathrm{H}^{-}\) is named hydride ion. (c) The nucleus of \(\mathrm{H}^{+}\) consists of one proton and one neutron. (d) Many transition and inner transition elements form more than one positively charged ion. (e) In naming metal cations with two different charges, the suffix -ous refers to the ion with a charge of +1 and -ic refers to the ion with a charge of +2 (f) \(\mathrm{Fe}^{3+}\) may be named either iron(III) ion or ferric ion. (g) The anion derived from a bromine atom is named bromine ion. (h) The anion derived from an oxygen atom is named oxide ion. (i) \(\quad \mathrm{HCO}_{3}^{-}\) is named hydrogen carbonate ion. (j) The prefix \(b i-\) in the name "bicarbonate" ion indicates that this ion has a charge of -2 (k) The hydrogen phosphate ion has a charge of +1 and the dihydrogen phosphate ion has a charge of +2 (l) The phosphate ion is \(\mathrm{PO}_{3}^{4-}\) \((\mathrm{m})\) The nitrite ion is \(\mathrm{NO}_{2}^{-},\) and the nitrate ion is \(\mathrm{NO}_{3}^{-}\) (n) The carbonate ion is \(\mathrm{CO}_{3}^{2-},\) and the hydrogen carbonate ion is \(\mathrm{HCO}_{3}^{-}\)

Name these binary covalent compounds. (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{SO}_{3}\) (c) \(\mathrm{PCl}_{3}\) (d) \(\mathrm{CS}_{2}\)

What is the charge on each ion in these compounds? (a) \(\mathrm{CaS}\) (b) \( \mathrm{MgF}_{2}\) (c) \(\mathrm{Cs}_{2} \mathrm{O}\) (d) \(\operatorname{ScCl}_{3}\) (e) \(\mathrm{Al}_{2} \mathrm{S}_{3}\)

Why does nitrogen have three bonds and one unshared pair of electrons in covalent compounds?

Write formulas for the following ionic compounds: (a) Potassium bromide (b) Calcium oxide (c) Mercury(II) oxide (d) Copper(II) phosphate (e) Lithium sulfate (f) Iron(III) sulfide
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