1. The Chemistry of Life Biochemistry
=Branch of science that deals with the chemical composition (makeup) and processes of living things

2. I. Atoms The basic unit of matter
(Matter = anything that has mass and takes up space)
There are three subatomic particles that are combined to make each atom.
* Proton (+)
* Neutron (o)
* Electron (-)
move around nucleus in electron cloud
Nucleus (+)
Energy Levels
1st = 2
2nd = 8
3rd = 18

3. C. Isotopes – Atoms of the same element with different number of neutrons 1. Identified by mass number (atomic mass) 2. Ex.: Carbon-12; Carbon-13; Carbon-14

4. II. Elements An element is a substance that contains one type of atom
We can find
information about
all known elements
in the
Periodic Table
of Elements

5. Element Key Atomic Number (+), (-) Chemical Symbol
Element Name
Atomic Mass/ Mass Number
(+ ; o) (protons plus neutrons)
Atomic Number = number of protons in nucleus
All atoms of the same element have same atomic number
This number also equals number of electrons in electron cloud
Atomic Mass = average of all the isotopes of that element
Mass Number = number of protons and neutrons that make up atom nucleus 1 H
Hydrogen
1.0079

6. Equations to know: At. Mass = p + n p = protons
At. No. = p = e n = neutrons
e = p e = electrons
All substances are made up of elements
On Earth 90 elements occur naturally
25 elements are essential to living things
* Carbon ( C)
* Hydrogen (H)
* Oxygen (O)
* Nitrogen (N)
96 % of human body

7. III. Combining Atoms
When two or more atoms are combined a molecule is formed (O₂)
When two or more atoms of different elements combine a compound is formed (CO₂)

8. ALL COMPOUNDS ARE MOLECULES, BUT NOT ALL MOLECULES ARE COMPOUNDS!!!!!!
Be able to explain this statement.

9. We can describe the composition of compounds by using a chemical formula
Ex: H₂O (2 atoms of hydrogen, 1 atom of oxygen)
C₆H₁₂O₆ (6 carbon, 12 hydrogen, 6 oxygen)

10. Chemical properties = characteristics
The chemical properties of each compound are different from each of the elements that form it.
Chemical properties = characteristics
Ex: Sodium (Na) – silver metal, soft, reacts violently with water
Chlorine (Cl) – poisonous, green gas
Sodium Chloride (NaCl) or table salt
White solid, dissolves easily in water, essential for survival of living things

11. IV. Chemical Bonds Bonds : a force that holds atoms together
Covalent Bonds
Forms when atoms share electrons
Share 2 = single bond
Share 4 = double bond
Share 6 = triple bond
Ex: water

12. a. Formed when atoms lose or gain electrons
Ionic Bonds
a. Formed when atoms lose or gain electrons
b. Creates electrically charged atoms called ions (different number of protons/electrons)
* if atom loses electron = + ion
* if atom gains electron = - ion
c. Ions with opposite charges are attracted to each other.

13. d. Ex: NaCl

14. Hydrogen Bonds
a. Form when the positive end of one molecules is attracted to the negative end of another molecules
b. Form without the interaction of electrons
c. Responsible for the cohesion of water
*allows raindrops to form or water to bead
d. Easily broken

15. V. Mixtures and Compounds
Mixture: two or more substances that are not chemically combined
Heterogeneous: components not evenly mixed; all components keep their own identity
Example: sand, salad, soup
Homogeneous: components
are evenly mixed; cannot see
each component; also called
solution
Example: kool-aid, air

16. 1. Solute: substance being dissolved C. Suspensions
Components of a mixture can be separated by physical means, while components of a compound must be separated by chemical means.
B. Parts of a Solution
1. Solute: substance being dissolved
2. Solvent: substance doing the dissolving
C. Suspensions
1. form when some materials do not dissolve
2. ex: blood – mostly H₂O, dissolved compounds, cells, and misc. particles

17. VI. Acids/Bases/pH
Acids – a solution with a high concentration of Hydrogen ions (H+)
B. Bases – a solution with a high concentration of hydroxide ions (OH-)
C. pH – means potential for hydrogen

18. pH Scale: a measurement system used to indicate
pH Scale: a measurement system used to indicate the concentration of H+ ions
ranges from
0.1 – 6.9 = acid (pop, juice, coffee)
= neutral (pure water)
7.1 – 14 = base (blood, soap, some cleaning products)
pH can determine what type of organisms can live in an environment or what types of chemical reactions can take place
7.0
pure water

20. 2 H₂ + O₂ → 2 H₂O Balancing Equations
Steps to Solve Equation 1. write down elements on reactants side 2. write down elements on product side 3. write number of atoms for each element on each side 4. Begin adding coefficients to balance equation

21. Practice Problems ____ N₂ + ____ H₂ → ____ NH₃
____ Cu₂O + ____ C → ____ Cu + ____CO₂
____ Mg + ____ O₂ → ____MgO
____CH₄ + ____ O₂ → ____CO₂ + ____ H₂O

22. 5. ___ Zn + ____ CrCl₃ → ____CrCl₂ + ____ZnCl₂ 6
5. ___ Zn + ____ CrCl₃ → ____CrCl₂ + ____ZnCl₂ 6. ___ CO₂ + ___ H₂O → ____C₆H₁₂O₆ + ____ O₂ 7. ____C₂ + ____H₂ + ____OH → ____C₃H₇OH 8. ____C₃ + ____H₂O → ____C₉H₈O₄

23. 9. ____O₂ + ____Cl₂S₃ → ____Cl₂O₄ + ____ SO₂ 10
9. ____O₂ + ____Cl₂S₃ → ____Cl₂O₄ + ____ SO₂ 10. ____N₂ + ____H₂ + ____Cl₃ → ____NH₄Cl

24. ORGANIC CHEMISTRY
Organic chemistry is the study of compounds that contain bonds between carbon atoms
Carbon atoms have 4 valence electrons; therefore, each electron can join with electrons from another atom to form strong covalent bonds
Carbon can bond with:
* Hydrogen (H) * Phosphorus (P)
* Oxygen (O) * Carbon (C)
* Nitrogen (N) * Sulfur (S)

25. C. Carbon can form chains of unlimited lengths

26. II. Organic Compounds Found in All Living Things
Carbohydrates
Lipids
Proteins
Nucleic acids

27. A. Carbohydrates Made up of C, H, and O in a 1 : 2 : 1 ratio Uses
Energy (quick)
Structural building blocks (cellulose – plant cell walls)
Sugars and Starches
Monosaccharides (one)
Disaccharides (two)
Polysaccharides (many)

28. Monosaccharides Simple sugar Chemical formula: C₆H₁₂O₆
Ex: Glucose, Fructose, and Galactose are 3 isomers of a monosaccharide
= molecules with same chemical formula
but different structure

29. Disaccharides A two-sugar molecule
When 2 carbohydrate monomers are joined, a dehydration synthesis(removal of H₂O) takes place to form a disaccharide.
Chemical formula: C₁₂H₂₂O₁₁
Ex: glucose + galactose → Lactose
When disaccharides are used for energy, they are digested by enzymes that break them up into monosaccharides which are metabolized in the process of cellular respiration

30. Hydrolysis Reaction
glucose + galactose → Lactose
(C₆H₁₂O₆) (C₆H₁₂O₆) (H₂O) = C₁₂H₂₂O₁₁
Monomer = a single unit/molecule
To digest lactose (sugar in dairy), you need lactase enzyme
Lactose intolerant people can’t produce lactase

31. Polysaccharides
Large macromolecules or polymers that can consist of hundreds or thousands of monomers (C₆H₁₀O₅)n
Starches (plant: corn & wheat)
a. Amylase (enzyme) breaks it down into monomers which are absorbed into the bloodstream to be used by the cells.
Glycogen (animal starches)
a. Stored in the liver and muscles when there is excess monosaccharides
Cellulose
a. Can not be digested = roughage

32. B. Lipids Made up mostly of C and H with some O Uses:
Energy – 2x the amount of chemical energy per gram compared to carbohydrates
Making biological membranes
Ex: plasma membrane in cells
Water proof coverings in plants
Physical & thermal insulation to animals

33. Lipids are generally insoluable in water
Formed when a glycerol molecule (C₃H₅O₃) joins a fatty acid
Saturated fats form when each carbon atom in the fatty acid chain is joined to another carbon atom by a single covalent bond
Solid at room temperature
Ex: butter

34. Unsaturated fats form when there is a least one
carbon-carbon double bond
liquid at room temperature
Olive oil
c. Polyunsaturated fats form when there are two or more carbon-carbon double bonds
Corn, sesame & peanut oil

35. Steroids are lipids whose C, H, and O atoms are arranged in rings
Estrogen, Androgen, Cholesterol

36. C. Proteins 1. Made up of C, H, O, and N Uses:
a. Regulate cell processes and control reaction rates
b. Make up bulk of all solid material in the body (muscle, bone, skin, hair)
c. Transport substances in and out of cell

37. Proteins are polymers of amino acids
a. Amino acids are compounds
with an amino group (NH₂) at
one end and a
carboxyl group (COOH)
at the other.
b. There are 20 different amino acides
c. Amino acids are joined together by peptides bonds to form a dipeptide or a polypeptide molecule

38. Enzymes are proteins that are formed during the process of protein synthesis
Enzymes are biological catalysts that control the rate of chemical reactions.
Each type of enzyme catalyzes only one type of reaction.
Names of enzymes usually end in –ase and are named for the reaction they catalyze.
Example: lactase → lactose
protease → protein

39. D. Nucleic Acids Made up of C, H, O, N, and P Uses:
a. Store and transmit genetic information
b. Make proteins
Made up of nucleotides
5 – Carbon sugar
Phosphate group
Nitrogenous base
4. Example: DNA and RNA