Chapter 2 The Chemistry of Life
All Matter Consists of Elements Made of Atoms Atoms contain: Protons: positive charge; have mass Neutrons: no charge; have mass Electrons: negative charge; negligible mass
FIGURE 2.1 An atom of helium, showing protons and neutrons in the nucleus and electrons occupying a region around the nucleus.
TABLE 2.1 REVIEW OF SUBATOMIC PARTICLES
Chemical bonds form between the atoms of a compound The atoms in a compound are held together by covalent, ionic or hydrogen bonds
FIGURE 2.7 Atoms of hydrogen, carbon, and oxygen. Each of the concentric circles around the nucleus represents a shell occupied by electrons.
Covalent Bonds Covalent bonds are the strongest bonds Form when two or more atoms share the electrons in their outer shells
Single Covalent Bonds FIGURE 2.8a Covalent bonds form when electrons are shared between atoms. Shown here are examples of single, double, and triple covalent bonds. For each example, the structural formula is shown on the far right.
Double Covalent Bonds FIGURE 2.8b Covalent bonds form when electrons are shared between atoms. Shown here are examples of single, double, and triple covalent bonds. For each example, the structural formula is shown on the far right.
Triple Covalent Bonds FIGURE 2.8c Covalent bonds form when electrons are shared between atoms. Shown here are examples of single, double, and triple covalent bonds. For each example, the structural formula is shown on the far right.
Ionic Bonds An ion is an atom or group of atoms with a positive or negative electrical charge Ionic bonds, weaker than covalent bonds, result from the attraction of oppositely charged ions, rather than shared electrons
FIGURE 2.9 An ionic bond involves the transfer of electrons between atoms. Such a transfer creates oppositely charged ions that are attracted to one another.
Hydrogen Bonds Hydrogen bonds are the attraction formed between a slightly positively charged hydrogen atom and another slightly negatively charged atom Many hydrogen bonds can collectively add up to formation of tightly bound molecules, e.g., DNA double helix
Hydrogen Bonds Hydrogen bonds account for the unique properties of water and the geometric shape of many biological molecules
FIGURE 2.10a The hydrogen bonds of water
FIGURE 2.10b The hydrogen bonds of water
TABLE 2.2 REVIEW OF CHEMICAL BONDS
Acids and Bases Acids and bases react differently to water Acids release hydrogen ions (H+) when placed in water and bases produce hydroxide ions (OH-) when added to water
The pH Scale: Each unit equals A 10 fold change In H+ concentration FIGURE 2.12 The pH scale and the pH of some body fluids and other familiar substances.
Acids and Bases The lower the pH on the pH scale, the greater the acidity and the higher the pH, the more basic a solution
TABLE 2.3 REVIEW OF THE CHARACTERISTICS OF ACIDS AND BASES
Synthesis and Hydrolysis of Polymers Biological macromolecules are the giant molecules of life (proteins, nucleic acids, lipids, carbohydrates) They are long chains called polymers made of repeating units called monomers
Synthesis of Polymers When polymers are made, water is removed and the reaction is called a dehydration synthesis
FIGURE 2.13a Formation and breaking apart of polymers.
Hydrolysis of Polymers Conversely, when the same molecules are broken apart, water is added and the reaction is a hydrolysis
FIGURE 2.13b Formation and breaking apart of polymers.