Chapter 11: Chemical Bonding
Enhanced Introductory College Chemistry
by Gregory Anderson; Caryn Fahey; Jackie MacDonald; Adrienne Richards; Samantha Sullivan Sauer; J.R. van Haarlem; and David Wegman;
Chapter Contents
- 11.1 Ionic Bonding
- 11.2 Covalent Bonding
- 11.3 Lewis Symbols and Structures
- 11.4 Formal Charges and Resonance
- 11.5 Strengths of Ionic and Covalent Bonds
- 11.6 Molecular Structure and Polarity
- Summary
- Review
Except where otherwise noted, this OER is licensed under CC BY 4.0
Please visit the web version of Enhanced Introductory College Chemistry to access the complete book, interactive activities and ancillary resources.
In this chapter, you will learn about
- The types of bonds that can occur when elements interact
- Application of electron configurations to predict chemical bonding
- Molecular structures and bond strengths
To better support your learning, you should be familiar with the following concepts before starting this chapter:
- Periodic Table
- Electron valence configuration of elements
It has long been known that pure carbon occurs in different forms (allotropes) including graphite and diamonds. But it was not until 1985 that a new form of carbon was recognized: buckminsterfullerene, commonly known as a “buckyball.” This molecule was named after the architect and inventor R. Buckminster Fuller (1895–1983), whose signature architectural design was the geodesic dome, characterized by a lattice shell structure supporting a spherical surface. Experimental evidence revealed the formula, C60, and then scientists determined how 60 carbon atoms could form one symmetric, stable molecule. They were guided by bonding theory—the topic of this chapter—which explains how individual atoms connect to form more complex structures.
Watch How atoms bond – George Zaidan and Charles Morton (4 mins)
Video source: TED-Ed. (2013, October 15). How atoms bond – George Zaidan and Charles Morton [Video]. YouTube.
Indigenous Perspective: Iglu
Igluit are built over the depression from where the blocks are cut. The entryway for the iglu is below ground level. The thermal properties ensures that the inside of the iglu is sufficiently warm even when the temperature outside is very low. (Anderson & Rayner-Canham, para. 11)
“As a result of the unique open crystal structure, snowflakes do not pack well together. This phenomenon results in one of the most important attributes of snow: its thermal insulation properties.” “When the Inuit transitioned from building igluit to using cabins and houses, we used the snow instead to pack tightly against the walls to insulate our homes.”
Source: Andersen, C.C., & Rayner-Canham, G. (2019, December). Snow: Making life possible in the Arctic: Chemistry Inuit Life and Culture. Chem 13 News Magazine.