1. Chemistry of Life
Biology A

2. CHEMISTRY MADE SIMPLE

3. Why Learn Chemistry?
A basic knowledge of chemistry will help you understand biology better because all organisms, including yourself, are made up of matter.
Matter – anything that has mass and volume.

4. I. Matter and Atoms
Atom – the smallest particle of matter that cannot be broken down by chemical means.
Atoms are composed of three particles: electrons, protons, and neutrons.

6. Electrons are negatively charged. (-)
Protons are positively charged (+)
Neutrons are neutrally charged, that means they have no charge (0)

8. Because protons (+) and electrons (-) are oppositely charged they are attracted to one another.
Protons (+) and neutrons (0) are found inside the nucleus of an atom.
Electrons (-) are found in orbitals around the nucleus.

10. II. Different Types of Atoms
Different amounts of electrons (-), protons (+), and neutrons (0) create different types of atoms.
“The Periodic Table of Elements” lists over 110 different types of atoms.
Element – a substance made of only one type of atom.

13. Interesting Facts:
More than 90% of the atoms in your body are either nitrogen (N), oxygen (O), carbon (C), or hydrogen (H).
Only 30 elements are important for living organisms.

14. A. Periodic Table Information
Atomic Number (# of protons)
Chemical Symbol (1-3 letter abbreviations)
Atomic Mass (# of protons & neutrons)

15. Most of the time the number of protons (+) and electrons (-) are equal in the atom so it has a net charge of 0.
When an atom gains an electron it is called a negative ion and when an atom loses an electron it is called a positive ion.
Electrons move around the nucleus at very high speeds in one of seven different Energy Levels.

17. Electrons in the outer energy levels have more energy than those in inner Levels.
Each Energy Level (orbital) can hold only a certain number of electrons.
1st level = 2 electrons
2nd level = 8 electrons
3rd level = 8 electrons
4th and 5th levels = 18 electrons
6th and 7th levels = 32 electrons

18. The number neutrons (0) is often, but not always equal to the number of protons (+) and electrons (-) in an atom.
Atoms that contain different numbers of neutrons are called isotopes.

21. Chemistry of Life
Biology A

23. Atoms Can Bond
Atoms can join together with other atoms to form new substances.
A compound is a substance made up of the joined atoms of two or more different elements.

24. Types of Bonds
Covalent Bond
Hydrogen Bond
Ionic Bond

25. Two hydrogen atoms equally share electrons.
Covalent Bond
A bond where two or more atoms SHARE electrons to form a molecule.
(i.e. H2O, CO2, etc.)
Two hydrogen atoms equally share electrons.

26. Multiple Bonding Single Bond – two electrons shared.
Double Bond – four electrons shared.
Triple Bond – six electrons shared.

28. Important Facts:
Carbon atoms are the best at bonding because they have four electrons in their outer orbit and therefore can bond with up to four other atoms.
Carbon atoms are essential to life.
Organic molecules all contain Carbon.

29. Hydrogen Bond
A bond where shared electrons are attracted more strongly to one atom than the other.
Two hydrogen atoms and one oxygen atoms share electrons,
but the oxygen attracts the electrons more.

30. Ionic Bond
A bond where two or more atoms GAIN or LOSE electrons in order to form stable energy levels.
(i.e. NaCl, KBr, etc.)
Sodium (solid) + Chlorine (gas) = Salt