Cell membrane and Function
Review 1: The Chemistry and Molecules of Life
Please note that this is a general outline of some of the topics we will have discussed and are detailed in chapters 2-5 of your textbook. While this gives you an idea of some of the terms/phrases you are responsible for, not all the material we covered is included. You are responsible for everything discussed in class, but NOT for material in the book that was not addressed in lecture. Please do NOT assume that if you know the concepts/answers to the terms below, you are prepared for an exam. You need to spend time with your lecture notes, and prepare your own review questions in addition to the ones provided here. WHITE 301
General Themes and Topics
Atoms, Elements and Molecules (Chapter 2)
Describe the general structure of an atom and define atomic number, atomic mass, valence electrons, and isotopes.
Atomic number – the # of protons in the nucleus
Atomic mass – the number of protons and neutrons
Valence electrons – the number of electrons in the outermost shell
Isotopes – elements that have the same atomic number but different atomic mass
Distinguish between elements and compounds; name the most abundant elements in the human body if water is included; name some that are crucial but less abundant
An element is a pure substance that can’t be broken up
A compound consists of two or more different elements
Carbon, Hydrogen, Oxygen, and Nitrogen are the most abundant elements
Iron and Iodine are crucial but less abundant
Distinguish between ionic bonds, covalent bonds (how are nonpolar and polar covalent bonds different), and hydrogen bonds, noting their relative strengths and in what types of molecules they might be found. Give an example of each in a biological system.
Covalent bonds are bonds that involve the sharing of a pair of valence electrons by two atoms. This type of bond is usually only between two nonmetal elements. Covalent bonds are strong bonds compared to other bonds, except ionic
Please note that this is a general outline of some of the topics we will have discussed and are detailed in chapters 2-5 of your textbook. While this gives you an idea of some of the terms/phrases you are responsible for, not all the material we covered is included. You are responsible for everything discussed in class, but NOT for material in the book that was not addressed in lecture. Please do NOT assume that if you know the concepts/answers to the terms below, you are prepared for an exam. You need to spend time with your lecture notes, and prepare your own review questions in addition to the ones provided here. WHITE 301
General Themes and Topics
Atoms, Elements and Molecules (Chapter 2)
Describe the general structure of an atom and define atomic number, atomic mass, valence electrons, and isotopes.
Atomic number – the # of protons in the nucleus
Atomic mass – the number of protons and neutrons
Valence electrons – the number of electrons in the outermost shell
Isotopes – elements that have the same atomic number but different atomic mass
Distinguish between elements and compounds; name the most abundant elements in the human body if water is included; name some that are crucial but less abundant
An element is a pure substance that can’t be broken up
A compound consists of two or more different elements
Carbon, Hydrogen, Oxygen, and Nitrogen are the most abundant elements
Iron and Iodine are crucial but less abundant
Distinguish between ionic bonds, covalent bonds (how are nonpolar and polar covalent bonds different), and hydrogen bonds, noting their relative strengths and in what types of molecules they might be found. Give an example of each in a biological system.
Covalent bonds are bonds that involve the sharing of a pair of valence electrons by two atoms. This type of bond is usually only between two nonmetal elements. Covalent bonds are strong bonds compared to other bonds, except ionic