5: Covalent Bonding and Simple Molecular Compounds
- Page ID
- 469231
\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)
\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)
\( \newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\)
( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\)
\( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)
\( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\)
\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)
\( \newcommand{\Span}{\mathrm{span}}\)
\( \newcommand{\id}{\mathrm{id}}\)
\( \newcommand{\Span}{\mathrm{span}}\)
\( \newcommand{\kernel}{\mathrm{null}\,}\)
\( \newcommand{\range}{\mathrm{range}\,}\)
\( \newcommand{\RealPart}{\mathrm{Re}}\)
\( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)
\( \newcommand{\Argument}{\mathrm{Arg}}\)
\( \newcommand{\norm}[1]{\| #1 \|}\)
\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)
\( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\AA}{\unicode[.8,0]{x212B}}\)
\( \newcommand{\vectorA}[1]{\vec{#1}} % arrow\)
\( \newcommand{\vectorAt}[1]{\vec{\text{#1}}} % arrow\)
\( \newcommand{\vectorB}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)
\( \newcommand{\vectorC}[1]{\textbf{#1}} \)
\( \newcommand{\vectorD}[1]{\overrightarrow{#1}} \)
\( \newcommand{\vectorDt}[1]{\overrightarrow{\text{#1}}} \)
\( \newcommand{\vectE}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{\mathbf {#1}}}} \)
\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)
\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)
Ionic bonding results from the transfer of electrons among atoms or groups of atoms. In this chapter, we will consider another type of bonding—covalent bonding. We will examine how atoms share electrons to form these bonds, and we will begin to explore how the resulting compounds, such as cholesterol, are different from ionic compounds.
- 5.0: Prelude to Covalent Bonding and Simple Molecular Compounds
- Cholesterol, a compound that is sometimes in the news, is a white, waxy solid produced in the liver of every animal, including humans. It is important for building cell membranes and in producing certain hormones (chemicals that regulate cellular activity in the body). As such, it is necessary for life, but why is cholesterol the object of attention? Most medical professionals recommend diets that minimize the amount of ingested cholesterol as a way of preventing heart attacks and strokes.
- 5.1: Covalent Bonds
- You have already seen examples of substances that contain covalent bonds. One substance mentioned previously was water (H₂O). You can tell from its formula that it is not an ionic compound; it is not composed of a metal and a nonmetal. Consequently, its properties are different from those of ionic compounds. A covalent bond is formed between two atoms by sharing electrons.
- 5.2: Covalent Compounds- Formulas and Names
- Molecules can be represented using formulas, which give information about the number and type of atoms bonded together. Different types of structural formulas show the bonds between atoms and sometimes give information about molecular shape as well.
- 5.3: Drawing Lewis Structures
- Molecules can be represented using Lewis structures, which show how electrons are arranged around the atoms in a molecule as bonded pairs of electrons (bonds) and lone pairs of electrons. These structures are useful for explaining and depicting molecular shapes and chemical reactivity.
- 5.4: The Shapes of Molecules
- According to valence-shell electron-pair repulsion theory, VSEPR, the electron groups minimize repulsion by getting as far apart as possible from each other. Therefore, the approximate shape of a molecule can be predicted from the number of electron groups and the number of surrounding atoms.
- 5.5: Polar Covalent Bonds and Electronegativity
- Covalent bonds between different atoms have different bond lengths. Covalent bonds can be polar or nonpolar, depending on the electronegativity difference between the atoms involved.
- 5.6: Polar Molecules
- The molecular polarity of a diatomic molecule is determined by the bond polarity. The polarity of molecules with more than one bond must be determined by first identifying the molecular structure and then the bond polarity. If the dipole moments point in a similar direction, there is a net molecular dipole. If the dipole moments point in opposite directions, they cancel out and there is no net dipole.
- 5.7: Organic Chemistry
- Organic chemistry is the study of the chemistry of carbon compounds. Organic molecules can be classified according to the types of elements and bonds in the molecules.
- 5.E: Covalent Bonding and Simple Molecular Compounds (Exercises)
- These are homework exercises to accompany Chapter 4 of the Ball et al. "The Basics of GOB Chemistry" Textmap.
- 5.S: Covalent Bonding and Simple Molecular Compounds (Summary)
- To ensure that you understand the material in this chapter, you should review the meanings of the following bold terms in the following summary and ask yourself how they relate to the topics in the chapter.