2: The Chemical Foundation of Life
- Page ID
- 12460
\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\)
- 2.1: Atoms, Isotopes, Ions, and Molecules - Overview of Atomic Structure
- Atoms are made up of particles called protons, neutrons, and electrons, which are responsible for the mass and charge of atoms.
- 2.2: Atoms, Isotopes, Ions, and Molecules - Atomic Number and Mass Number
- The atomic number is the number of protons in an element, while the mass number is the number of protons plus the number of neutrons.
- 2.3: Atoms, Isotopes, Ions, and Molecules - Isotopes
- Isotopes are various forms of an element that have the same number of protons, but a different number of neutrons.
- 2.4: Atoms, Isotopes, Ions, and Molecules - The Periodic Table
- Everything in the universe is made of one or more elements. The periodic table is a means of organizing the various elements according to similar physical and chemical properties.
- 2.5: Atoms, Isotopes, Ions, and Molecules - Electron Shells and the Bohr Model
- Niels Bohr proposed an early model of the atom as a central nucleus containing protons and neutrons being orbited by electrons in shells.
- 2.6: Atoms, Isotopes, Ions, and Molecules - Electron Orbitals
- Electron orbitals are three-dimensional representations of the space in which an electron is likely to be found.
- 2.7: Atoms, Isotopes, Ions, and Molecules - Chemical Reactions and Molecules
- Chemical reactions occur when two or more atoms bond together to form molecules or when bonded atoms are broken apart.
- 2.8: Atoms, Isotopes, Ions, and Molecules - Ions and Ionic Bonds
- Ionic bonds are attractions between oppositely charged atoms or groups of atoms where electrons are donated and accepted.
- 2.9: Atoms, Isotopes, Ions, and Molecules - Covalent Bonds and Other Bonds and Interactions
- Covalent bonds result from a sharing of electrons between two atoms and hold most biomolecules together.
- 2.10: Atoms, Isotopes, Ions, and Molecules - Hydrogen Bonding and Van der Waals Forces
- Hydrogen bonds and van der Waals interactions are two types of weak bonds that are necessary to the basic building blocks of life.
- 2.11: Water - Water’s Polarity
- Water’s polarity is responsible for many of its properties including its attractiveness to other molecules.
- 2.12: Water - Gas, Liquid, and Solid Water
- The orientation of hydrogen bonds as water changes states dictates the properties of water in its gaseous, liquid, and solid forms.
- 2.13: Water - Heat of Vaporization
- Evaporation of water requires a substantial amount of energy due to the high heat of vaporization of water.
- 2.14: Water - High Heat Capacity
- Water is able to absorb a high amount of heat before increasing in temperature, allowing humans to maintain body temperature.
- 2.15: Water - Water’s Solvent Properties
- Water’s polarity makes it an excellent solvent for other polar molecules and ions.
- 2.16: Water - Cohesive and Adhesive Properties
- Cohesion allows substances to withstand rupture when placed under stress while adhesion is the attraction between water and other molecules.
- 2.17: Water - pH, Buffers, Acids, and Bases
- Acids dissociate into H+ and lower pH, while bases dissociate into OH– and raise pH; buffers can absorb these excess ions to maintain pH.
- 2.18: Carbon - The Chemical Basis for Life
- Carbon is the most important element to living things because it can form many different kinds of bonds and form essential compounds.
- 2.19: Carbon - Hydrocarbons
- Hydrocarbons are important molecules that can form chains and rings due to the bonding patterns of carbon atoms.
- 2.20: Carbon - Organic Isomers
- Isomers are molecules with the same chemical formula but have different structures, which creates different properties in the molecules.
- 2.21: Carbon - Organic Enantiomers
- Enantiomers share the same chemical structure and bonds but differ in the placement of atoms such that they are mirror images of each other.
- 2.22: Carbon - Organic Molecules and Functional Groups
- Functional groups are groups of molecules attached to organic molecules and give them specific identities or functions.
- 2.23: Synthesis of Biological Macromolecules - Types of Biological Macromolecules
- Biological macromolecules, the large molecules necessary for life, include carbohydrates, lipids, nucleic acids, and proteins.
- 2.24: Synthesis of Biological Macromolecules - Dehydration Synthesis
- In dehydration synthesis, monomers combine with each other via covalent bonds to form polymers.
- 2.25: Synthesis of Biological Macromolecules - Hydrolysis
- Hydrolysis reactions result in the breakdown of polymers into monomers by using a water molecule and an enzymatic catalyst.