Download AP2A Ch2 Chemistry-2017

CH. 2 CHEMISTRY
TERMS & CONCEPTS TO KNOW PRIOR TO CLASS–
Mostly Bio 1 topics
BASIC CHEMISTRY
 Matter: solid, liquid, gas
 Energy: Kinetic, Potential energy
 Four chemicals of life
 Atomic Structure: protons, neutrons, electrons
 Atomic number
 Isotopes
 Compounds, Molecules and Ions
 Chemical Bonds: ionic, covalent (polar & nonpolar), hydrogen
 Chemical Reactions: reactants and products; synthesis,
decomposition, and exchange reactions
 Factors affecting chemical reactions: temperature, concentration,
particle size, catalysts
TERMS & CONCEPTS TO KNOW PRIOR TO CLASS …
Biochemistry
 Inorganic and Organic chemicals, pH scale
 Polymers & Monomers
 Carbohydrates: monosaccharides, disaccharides,
polysaccharides
 Lipids: glycerol and fatty acids (saturated and unsaturated),
phospholipids
 Proteins: amino acids, structural levels of proteins (primary,
secondary, and tertiary, and quaternary)
 Enzymes, active site, denaturation
 Nucleic Acids: RNA and DNA; Adenine, Guanine, Cytosine,
Thymine; ATP
I. Definition of concepts: Matter & Energy
A. Matter:
 States of matter:
B. Energy:
1. Types
2. Forms of Energy
 Chemical:
 Electrical:
 Mechanical:
 Radiant or electromagnetic
3. Energy Conversions
C. Composition of Matter: Atoms & Elements
1. Elements:
 92
 Atomic Symbol:
 4 elements = 96% of body:
PERIODIC TABLE
OF ELEMENTS
 Other Elements
 Deficiencies
2. Atoms & = Atomic
Structure
a) Nucleus
 Protons (p+)
 Neutrons (n0)
b) Electrons (e-)
 Orbitals
 1st = 2 e 2nd … = 8 e All atoms are electrically neutral
Figure 2.1
3. Atomic Number:
• How related to number of electrons:
4. Atomic Mass
• Atomic mass unit
Figure 2.1
D. Isotopes
 Protons:
 Neutrons:
 Symbol: H-1 or ¹H
 Atomic weight:
 The smaller the isotope, the stronger it is held
together
Figure 2.3
Radioisotopes
 *Radioisotope:
 Radioactivity—process of spontaneous atomic decay
 PET Scan using glucose
E. IONS
 Cations
 Anions
 Importance:
Example
 ATOM
Na
ION
Na+ = Cation
 IONS …
 Anions
ATOM
Cl
ION
Cl-
II. How Matter is Combined: Molecules &
Mixtures
A. Molecules
 Molecular Weight = weight in grams of 6.02 x 10 to the 23
power
 Compound
Figure 2.4
B. Mixtures
1. Solutions
a) Solvent
b) Solute
c) Concentration
i) Solute Percent
ii) Weight solute per volume of Solvent
iii) Molarity:
C. Chemical Bonds
Rule: atoms try to get a full shell of electrons for
the outer shell
1. Ionic Bonds
Na
Cl
Sodium atom (Na)
(11p+; 12n0; 11e–)
Chlorine atom (Cl)
(17p+; 18n0; 17e–)
Figure 2.6, step 2
 IONS & IONIC COMPOUNDS
 Opposite charges attract each other
ATOMS
Na
Cl
IONS  Ionic Compound
Na+
Cl-
•
Crystals
cation
anion
Na
Cl
+
Na
Cl
Sodium atom (Na)
(11p+; 12n0; 11e–)
Chlorine atom (Cl)
(17p+; 18n0; 17e–)
Sodium ion (Na+)
–
Chloride ion (Cl–)
Sodium chloride (NaCl)
Figure 2.6, step 3
2. Covalent Bonds:
Figure 2.7a
2 Types of Covalent Bonds
a. Non-polar covalent:
b. Polar bonds:
 Polar Molecule:
 Why chemicals dissolve
in water:
Figure 2.8
• Example: double bond
(Text p. 52)
Figure 2.7b
Comparison of Ionic, Polar & Nonpolar Covalent Bonds
Figure 2.9
3. Hydrogen Bonds
• Between: Molecules/compounds, not individual
atoms in one molecule or compound
• Created by: Polarity
• Strength of Bond:
Figure 2.9
III. Chemical Reactions
A. The Role of Energy in Chemical Reactions
- chemical energy
Figure 2.10a
B. Characteristics of Chemical Reactions
- Reactants
- Products
- Chemical Equations
Na
Cl
Sodium atom (Na)
(11p+; 12n0; 11e–)
Chlorine atom (Cl)
(17p+; 18n0; 17e–)
2Na
+
Cl2
Na
Sodium ion (Na+)
Cl
Chloride ion (Cl–)
Sodium chloride (NaCl)

2NaCl
Figure 2.10a
C. Types of Chemical Reactions
1. Synthesis Reactions
Dehydration Synthesis Reaction:
molecule 1
molecule 2
OH

1
O
O
+ H 2O
Figure 2.10a
2. Decomposition Reactions:
a) Hydrolysis Reaction:
H2O
molecule 1
molecule 2
O

OH
O
Figure 2.10b
3. Exchange reaction (AB + CAC + B)
Figure 2.10c
4. Mixed Reactions
a) Oxidation-Reduction (Redox) Reactions
 Is a Decomposition and Exchange Reaction
 Function:
 Exchange of: e- and/or hydrogen atoms
 Oxidized Reactant:
 Reduced Reactant:
 Cellular Respiration
C6H12O6 + 6O2  6CO2 + 6H2O + ATP
• Glucose is oxidized to Carbon Dioxide
• Oxygen is reduced to Water
D. Reversibility of Chemical Reactions
A + B
AB
 Indicated by double arrows in opposite directions
 Chemical Equilibrium:
 Adding or Removing either the reactants or products
causes:
 An increase in a substance causes:
 A decrease in a substance causes:
Example: H2CO3
HCO3- + H+
- If more H+ (acid) is added, then:
- If a base is added that reacts with H+, then:
E. Factors Influencing the Rate of Chemical
Reactions
Temperature
Concentration
Pressure
Catalysts
- Enzymes
Biochemistry
I. Inorganic Compounds
Types of Chemicals
 Organic compounds:
 Examples:
 Biochemicals
 Inorganic compounds:
I. Inorganic Compound …
A. WATER = 60-80%
1. Functions
a) Lubricant/cushioning
b) Heat Sink
c) Chemical Reactions ( text p. 59)
 Dehydration Synthesis
 Hydrolysis
d) Solvent of living things forming
Mixtures
1 Solutioins
 Solvent
 Solute
 Concentration of Solutions:
% solute = (amount solute) X 100%
(total amount)
Concentrations of Solutions …
 Milligrams per deciliter of solution
 Molarity = moles/liter
 1 mole = 6.02 x 10
substance
2 Colloids
3 Suspensions
23
molecules of a
B. SALT: ionic compounds not
having H+ or OH-
C. ACIDS and BASES
1. Have H+ and OH2. Proton (H+) donors and
acceptors
3. pH
 pH scale
4. BUFFERS—chemicals that can regulate pH change
 Are composed of a weak acid and its weak base
 Example: Carbonic acid—Bicarbonate system
H2CO3
----- HCO3-
+
H+
If H+ is added to the solution:
If OH- is added to the solution:
Figure 2.12
II. Organic Compounds Essential to Human
Functioning
 Carbon & Covalent Bonding
 Macromolecules
 Polymers and Monomers:
A. Carbohydrates
1. Elements:
2. Functions:
3. Saccharides = Sugars
4. Three Forms
a) Monosaccharides
• # carbons
• Glucose
• Fructose
4. Three Forms …
b) Disaccharieds
 Formation & Decomposition:
 Sucrose
 Lactose
 Maltose (malt sugar)
c) Polysaccharides
 Glycogen
 Starch
 Cellulose
Glycogen
5. Isomers
Isomers
Glucose


Glucose
6. Combined w other Biochemicals
Glycolipid
 Glycolipids
Galactose
 Glycoproteins
Lipid
B. Lipids
1. Contain Elements:
 Ratio
2. In water
3. Functions:
4. Formation:
5. Types
a) Triglycerides (fat)
4. Types …
 Triglycerides = Neutral Fats
 Composition
 Saturated vs. Unsaturated vs. Trans Fats
 Omega-3 fatty acids
 Phospholipids
=
 Function
 Steroids
 Prostaglandins
P
C. Proteins
1. Subunit =
R
 Elements:
 NH2 (amine) and COOH (carboxyl)
 R- group:
 Formation
Structure of amino acid
2. Peptide Bond: dehydration synthesis
• Dipeptide, …
• Polypeptide
Figure 2.16
3. Structural Levels of Proteins (Text p. 73)
• Primary:
• Secondary:
• Often Fibrous
Figure 2.18a–c
Structural Levels of Proteins …
• Tertiary:
• Globular
• Fibrous
• Quaternary:
• Globular
Figure 2.18b,d,e
4. Protein Denaturation =
Figure 2.19b
5. over half body’s organic matter
6. Combine with other biochemicals
 Glycoproteins & Proteoglycans
 Lipoproteins
7. Functions:
 Build Structures
Collagen
 Movement
 Hormones
 Antibodies
 Buffers
 Transport substances across the
cell membrane or through blood
 Enzymes  details next slide
Hemoglobin
7. Functions …
Enzymes and Enzyme Activity
 Enzymes =
 General Function–Catalyst
 Characteristics of Enzymes
 Shape
 Recycling
 Cofactors and
Coenzymes
Enzyme
 “ase” ending
 Mechanism of
Action  Next Slide
Products
Reactants
Mechanism of Enzyme Activity
Active site
Amino acids
+
Enzyme (E)
Substrates (S)
Enzyme-substrate
complex (E-S)
1 Enzyme-Substrate Complex
• Substrate
• Active Site
2 Internal Rearrangement
• Breaking of bonds & Formation of new bonds
• Energy of Activation
3 Release of Product
Figure 2.21
Active site
Amino acids
+
Enzyme (E)
Substrates (S)
Enzyme-substrate
complex (E-S)
H2O
Internal rearrangements
leading to catalysis
Figure 2.21
Active site
Amino acids
+
Enzyme (E)
Substrates (S)
Enzyme-substrate
complex (E-S)
H2O
Free enzyme (E)
Peptide bond
Internal rearrangements
leading to catalysis
Dipeptide product (P)
Figure 2.21
D. Nucleic Acids
1. Nucleic Acids =
2. Types: DNA and RNA
3. Elements
4. Nucleotides:
 Phosphate
 Monosaccharide
 Nitrogenous Base
 Purines: Adenine and Guanine
 Pyrimidines: Cytosine, Thymine, and Uracil
5. Dehydration Synthesis: sugar of one nucleotide to
phosphate of another nucleotide
6. Overview of DNA and RNA
6. Overview of DNA and RNA
DNA
 Nitrogenous Bases:
 Purines: A and G are two ring bases
 Pyrimidines:T, C, and U have one ring bases
 Sugar =
 Double Helix
 Complementary bases
 Function
Hydrogen
Bonds
RNA
 Sugar =
 U replaces T
 Single stranded
 Function
 Types
Released mRNA
RNA
Molecule
7. Other Related Chemicals
Adenosine Triphosphate (ATP)
 Function:
- Hydrolysis of phosphates
energy transfer
Food + O2 + ADP + Pi
ATP + CO2
- Phosphorylation
ATP + H2O
energy released
ADP/AMP + Pi + Energy
Adenosine Triphosphate (ATP) …
Membrane
protein
P
P
Solute
Solute transported
(a) Transport work
Released Energy is used
for:
ADP
+
P
ATP
Relaxed
muscle cell
Contracted
muscle cell
(b) Mechanical work
P
X
P
X
Y
+ Y
Reactants
Product made
(c) Chemical work
Energy liberated during
oxidation of food fuels
used to regenerate ATP
Figure 2.21
END
REVIEW QUESTION
1. What is the atomic number and atomic
mass of each of the above atoms?
Review Question
4. What sort of chemical reactions do you
suppose would be happening during
digestion?
What about when your body is making
more bone?
Review Question
5. What are the 4 major groups of biological
organic molecules? What is a major
function of each?
REVIEW QUESTION
 What are 2 variables that can distort the active
site of an enzyme and what is the distortion
process called?
Dysfunctional
Enzyme
1a.
REVIEW OF Ch. 1
1b.
1 a-d. Identify the
indicated regions of the
body.
1c.
1d.
2. What is the primary organ
found in the right
hypochondriac region?
3. Name an organ found in
hypogastric region?
 4. When the response to the effect of a
stimulus is in the opposite direction it is
called _______________ Feedback.