1. 2
Basic Chemistry

2. Power Point Assignment
For all the items marked with an * fill in the indicated information using Chapter 2 information. Do not look up these items in the glossary. The professor will not necessarily review these items so it is critical to your understanding of the material that you complete these notes on your power point. It is a good idea to download and print the powerpoint out and bring it to class.

3. I. Introduction A. Matter and Energy
1. Matter:* Define
2. Energy:* Define
a. Chemical
b. Electrical
c. Mechanical
d. Radiant

4. B. Composition of Matter
1. Elements:* Define
96 percent of the body = four elements
C * What does this letter stand for?
O * What does this letter stand for?
H * What does this letter stand for?
N * What does this letter stand for?
2. Atoms—building blocks of elements

5. 3. Subatomic Particles
a. Nucleus *Where is it and what does it contain
Protons * Charge & location:
Neutrons * Charge & location:
b. Electrons: Orbiting the nucleus
Electrons * Size, Charge & Location
c. Atomic Number = Number of protons (equals numbers of electrons) in an atom; different for each
d. Atomic mass number:
Helium atom e- e-
Proton
Neutron

6. How many protons, neutrons, and electrons does Hydrogen normally have?
Helium?
Lithium?
Figure 2.2

7. 4. Isotopes
Isotopes = Atoms of an element vary in the number of ______________
Isotopes have the same number of?
Atomic Weight of Isotopes

8. Radioactivity Radioisotope = Stability? Decomposes: Radioactivity:
Examples: Uranium, Iodine, …

9. 5. IONS = Positive & Negative Ions Properties as compared to atoms:
Table Salt

10. Ions Examples… Cl ¯1 ion or Cl ¯ ion
A Chlorine Atom gains an electron from another atom
Cl ¯1 ion or Cl ¯ ion

11. Properties of atoms compared to their ions …
Figure 2.4

12. C. Making Larger Chemicals out of the Atoms or Elements 1
C. Making Larger Chemicals out of the Atoms or Elements 1. Chemical Formulas
2. Molecules and Compounds
Molecule—two or more atoms, of the same or different elements, combined chemically
H2O O2 NaCl
b. Compound—two or more atoms of different elements combined chemically

13. One CHEMICAL BOND = ____ electrons
3. Chemical Bonds
Bonding involves interactions between electrons in outer part of 2 atoms
One CHEMICAL BOND = ____ electrons
a. Ionic Bonds (Electrovalent Bonds)
Bond Formed When:
Example: SALT
Na atom Cl atom Na Cl ¯

14. b. Covalent Bonds
i) Bonds occurs when:
ii) Types
Non Polar—electrons are:

15. The Oxygen: Polar Covalent Bonds Bond– electrons are: Example: WATER
The Hydrogens:
Polarity
Polar Molecule
Attraction between Polar Molecules
-1/2
Oxygen
+1/2
+1/2
2 Hydrogens
-1/2
Figure 2.8
+1/2
+1/2

16. Polar Molecules … Example: Attraction between Water Molecules creates surface tension Hydrogen Bonds
Figure 2.9

17. D. Chemical Reactions c. Process of making Products
a. Reactants =
b. Products =
c. Process of making Products
Bonds broken in ______________
Atoms rearranged
New bonds in _______________
H2O CO > H2CO3
Reactants > Products

18. 2. Types of Chemical Reactions
a. Synthesis reaction =
Example: Synthesis of Proteins

19. b. Decomposition Reactions =
Example: Glycogen is broken down into ______

20. c. Exchange reaction: Parts moved around
Example:

21. E. SOLUTIONS SOLUTION = a mixture of chemicals in a liquid
- AQUEOUS SOLUTIONS = the liquid is WATER
1. Solvent: the liquid
2. Solute: the dissolved chemicals
3. The Concentration of a Solution: can use percentages
% Solvent + % Solutes = 100%

22. 4. Movement of chemicals in Solutions a. Diffusion:
b. Osmosis:
water
solute

23. II. Biochemistry: Essentials for Life
TWO TYPES
Organic
Inorganic
A. Inorganic compounds
No “C” framework
simpler
Examples

24. Inorganic Compounds … Water -- STUDENTS READ IN TEXT 2. Salts ions
Vital
some conduct electrical currents
Examples:

25. + H – O H + Na+ Na+ Cl– Cl– Salt crystal Ions in solution
Water molecule
Na+
Na+
Cl–
Cl–
Salt
crystal
Ions in
solution
Figure 2.11

26. Release ______________ (H+) 4. Bases Release hydroxyl ions (OH–)
Inorganic Compounds …
3. Acids
Release ______________ (H+)
4. Bases
Release hydroxyl ions (OH–)
Are ______________ acceptors
Neutralization reaction
Acids + bases - water + salt

27. pH concentration of hydrogen ions Neutral = Acidic = Basic =
Buffers—regulate pH change

28. B. ORGANIC CHEMICALS = framework of ____________ Types Fossil Fuels
Biochemicals
Carbohydrates
Lipids
Proteins
Nucleic Acids

29. Biochemicals 1. Carbohydrates Elements: General Function:
Ratio of Hydrogen to Oxygen:
General Function:
Classification
Monosaccharides
Disaccharides
Polysaccharides

30. 2. Lipids Elements: Ratio of H to C: Solubility in water: Types
Organic Compounds …
2. Lipids
Elements:
Ratio of H to C:
Solubility in water:
Types

31. Lipids Types Neutral fats (triglycerides) Location: Function:
Composed of:
Glycerol & 3 Fatty Acids

32. Saturated Fats
Figure 2.16a

33. Un-Saturated Fat
Figure 2.16b

34. Important Characteristic:
Lipids …
Types …
Phospholipids
Composition:
Function:
Important Characteristic:
Glycerol Fatty Acids
Phosphate
(Charged)

35. Cholesterol is the basis for all steroids made in the body Function:
Lipids …
Steroids
Have rings
Cholesterol is the basis for all steroids made in the body
Function:

36. Important Organic Compounds …
3. Proteins
Elements:
Subunit:
structure
R group

37. Level of Complexity in Structure
Primary structure.
sequence of amino acids.
Amino
acids
Hydrogen bonds
Amino
acids
Secondary structure. Initial Folding into
2-D structure
-pleated sheet
Alpha-
helix
Figure 2.18a-b

38. Two or more polypetides
Tertiary Structure
3-D
Quaternary Structure
Two or more polypetides
Figure 2.18c-d

39. Proteins– Structure & Function
Fibrous proteins, Structural proteins
Function
Stability
Examples:

40. Figure 2.19a

41. Proteins 3-D proteins have specific Functions Stability– Denaturation
Carriers
Long-distance transport
Hormones
Enzymes

42. (b) Hemoglobin molecule composed of the
Heme group
Globin
protein
(b) Hemoglobin molecule composed of the
protein globin and attached heme groups.
(Globin is a globular or functional protein.)
Figure 2.19b

43. Enzymes
Function:
How Function:
active site

44. Substrates bind to active 2 Structural changes Enzyme (E)
Product (P)
e.g., dipeptide
Substrates (S)
e.g., amino acids
Energy is
absorbed;
bond is
formed.
Water is
released.
Peptide
bond +
H2O
Active site
Enzyme-substrate
complex (E-S)
Enzyme (E) 1
Substrates bind to active 2
Structural changes
Enzyme (E)
site. Enzyme changes shape
to hold substrates in proper
position.
occur, resulting in the
product. 3
Product is released.
Enzyme returns to
original shape, ready
to catalyze another
reaction.
Figure 2.20

45. Organic Compounds … 4. Nucleic Acids Types: Built from nucleotides
Pentose (5 carbon) sugar
A phosphate group
A nitrogenous base
A = Adenine
G = Guanine
C = Cytosine
T = Thymine
U = Uracil.

46. (a) Adenine nucleotide (Chemical structure)
Deoxyribose
Phosphate
sugar
Adenine (A)
(a) Adenine nucleotide
(Chemical structure)
KEY:
Thymine (T)
Cytosine (C)
Adenine (A)
Guanine (G)
Figure 2.21a

47. Nucleic Acids DNA Location Structure: Type sugar: deoxyribose Bases:
Function:

48. (d) Diagram of a DNA molecule
Hydrogen bond
Deoxyribose
sugar
Phosphate
(d) Diagram of a DNA molecule
KEY:
Thymine (T)
Cytosine (C)
Adenine (A)
Guanine (G)
Figure 2.21c-d

49. Nucleic Acids Ribonucleic acid (RNA) Structure: Sugar Bases Types
Released mRNA
Nucleic Acids
Ribonucleic acid (RNA)
Structure:
Sugar
Bases
Types
Function:

50. Nucleic Acid Derivatives
Adenosine triphosphate (ATP)
Modified Nucleotide of adenine with three phosphate groups
Function: __________________________
Examples

51. (a) Adenosine triphosphate (ATP)
Adenosine diphosphate
(ADP)
(b) Hydrolysis of ATP
Figure 2.22a-b