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Prepared by Patty Bostwick-Taylor,
Florence-Darlington Technical College
CHAPTER
2
Basic
Chemistry
© 2012 Pearson Education, Inc.
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I. Introduction
A. Matter and Energy
1. Matter:* Define
2. Energy:* Define
a. Chemical
b. Electrical
c. Mechanical
d. Radiant
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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
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3. Subatomic Particles
a. Nucleus *Where is it and what does it contain
Helium atom
• Protons * Charge & location:
e-
• Neutrons * Charge & location:
b. Electrons: Orbiting the nucleus
• Electrons * Size, Charge & Location
e-
Proton
Neutron
c. Atomic Number = Number of protons (equals numbers
of electrons) in an atom; different for each
d. Atomic mass number:
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• How many protons, neutrons, and electrons does Hydrogen
normally have?
• Helium?
• Lithium?
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Figure 2.2
4. Isotopes
•Isotopes = Atoms of an element vary in the
number of ______________
•Isotopes have the same number of?
• Atomic Weight of Isotopes
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Radioactivity
•Radioisotope =
•Stability?
•Decomposes:
•Radioactivity:
•Examples: Uranium, Iodine, …
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5. IONS =
• Positive & Negative Ions
• Properties as compared to atoms:
Na atom
A Sodium Atom loses its
outer electron to become
a Sodium Ion
Na+1 ion or Na+ ion
+
Table Salt
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Ions Examples…
an Electron
+
Cl atom
A Chlorine Atom gains an
electron from another atom
Cl ¯1 ion or Cl ¯ ion
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Properties of atoms compared to their ions …
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Figure 2.4
C. Making Larger Chemicals out of the Atoms
or Elements
1. Chemical Formulas
2. Molecules and Compounds
a. 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
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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
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Cl atom
Na+
Cl ¯
b. Covalent Bonds
i) Bonds occurs when:
ii) Types
Non Polar—electrons are:
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Polar Covalent Bonds
• Bond– electrons are:
• Example: WATER
The Oxygen:
-1/2
The Hydrogens:
Oxygen
• Polarity
+1/2
+1/2
• Polar Molecule
2 Hydrogens
-1/2
• Attraction between
Polar Molecules
+1/2
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+1/2
Figure 2.8
Polar Molecules …
Example: Attraction between Water Molecules
-- creates surface tension
Hydrogen Bonds
Figure 2.9
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D. Chemical Reactions
1. Chemical Reactions:
a. Reactants =
b. Products =
c. Process of making Products
• Bonds broken in ______________
• Atoms rearranged
• New bonds in _______________
H2O
+
Reactants
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CO2
--->
--->
H2CO3
Products
2. Types of Chemical Reactions
a. Synthesis reaction =
•Example: Synthesis of Proteins
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b. Decomposition Reactions =
•Example: Glycogen is broken down into ___
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c. Exchange reaction:
•Example:
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Parts moved around
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%
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•
4. Movement of chemicals in Solutions
a. Diffusion:
b. Osmosis:
water
solute
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II. Biochemistry: Essentials for Life
•TWO TYPES
•Organic
•Inorganic
A. Inorganic compounds
•No “C” framework
•simpler
•Examples
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Inorganic Compounds …
1. Water -- STUDENTS READ IN TEXT
2. Salts
•ions
•Vital
• some conduct electrical currents
•Examples:
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H
–
+
O
H
+
Water molecule
Na+
Na+
Cl–
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Salt
crystal
Cl–
Ions in
solution
Figure 2.11
Inorganic Compounds …
3. Acids
•Release ______________ (H+)
4. Bases
•Release hydroxyl ions (OH–)
•Are ______________ acceptors
•Neutralization reaction
•Acids + bases - water + salt
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pH
•concentration of hydrogen ions
•Neutral =
•Acidic =
•Basic =
•Buffers—regulate pH change
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B. ORGANIC CHEMICALS
= framework of ____________
Types
• Fossil Fuels
• Biochemicals
• Carbohydrates
• Lipids
• Proteins
• Nucleic Acids
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Biochemicals
1. Carbohydrates
•Elements:
• Ratio of Hydrogen to Oxygen:
•General Function:
•Classification
• Monosaccharides
• Disaccharides
• Polysaccharides
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Organic Compounds …
2. Lipids
•Elements:
•Ratio of H to C:
•Solubility in water:
•Types
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Lipids
•Types
•Neutral fats (triglycerides)
•Location:
•Function:
•Composed of:
Glycerol & 3 Fatty Acids
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Saturated Fats
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Figure 2.16a
Un-Saturated Fat
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Figure 2.16b
Lipids …
• Types …
•Phospholipids
•Composition:
•Function:
•Important Characteristic:
Glycerol + 2 Fatty Acids
Phosphate
(Charged)
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Lipids …
•Steroids
•Have rings
•Cholesterol is the basis for all steroids
made in the body
• Function:
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Important Organic Compounds …
3. Proteins
•Elements:
•Subunit:
•structure
•R group
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Level of Complexity in Structure
(a) Primary structure.
sequence of
amino acids.
Amino
acids
Hydrogen bonds
Amino
acids
(b) Secondary structure.
Initial Folding into
2-D structure
Alphahelix
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-pleated sheet
Figure 2.18a-b
Tertiary Structure
3-D
Quaternary Structure
Two or more
polypetides
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Figure 2.18c-d
Proteins– Structure & Function
•Fibrous proteins, Structural proteins
•Function
•Stability
•Examples:
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Figure 2.19a
Proteins
•3-D proteins have specific Functions
•Stability– Denaturation
•Functions:
•Carriers
•Long-distance transport
•Hormones
•Enzymes
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Heme group
Globin
protein
(b) Hemoglobin molecule composed of the
protein globin and attached heme groups.
(Globin is a globular or functional protein.)
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Figure 2.19b
Enzymes
•Function:
•How Function:
• active site
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Energy is Water is
absorbed; released.
bond is
H2O
formed.
Substrates (S)
e.g., amino acids
+
Product (P)
e.g., dipeptide
Peptide
bond
Active site
Enzyme-substrate
complex (E-S)
Enzyme (E)
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1 Substrates bind to active
site. Enzyme changes shape
to hold substrates in proper
position.
2 Structural changes
occur, resulting in the
product.
Enzyme (E)
3 Product is released.
Enzyme returns to
original shape, ready
to catalyze another
reaction.
Figure 2.20
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.
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Deoxyribose
Phosphate sugar
Adenine (A)
(a) Adenine nucleotide
(Chemical structure)
KEY:
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Thymine (T)
Cytosine (C)
Adenine (A)
Guanine (G)
Figure 2.21a
Nucleic Acids
•DNA
• Location
•Structure:
•Type sugar: deoxyribose
• Bases:
• Function:
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Hydrogen bond
Deoxyribose
sugar
Phosphate
(d) Diagram of a DNA molecule
KEY:
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Thymine (T)
Cytosine (C)
Adenine (A)
Guanine (G)
Figure 2.21c-d
Nucleic Acids
•Ribonucleic acid (RNA)
•Structure:
•Sugar
•Bases
•Types
•Function:
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Released mRNA
Nucleic Acid Derivatives
•Adenosine triphosphate (ATP)
•Modified Nucleotide of adenine with three
phosphate groups
•Function: __________________________
•Examples
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(a) Adenosine triphosphate (ATP)
Adenosine diphosphate
(ADP)
(b) Hydrolysis of ATP
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Figure 2.22a-b