Chapter 02 Chemical Basis of Life
Chemistry - _____________ of the structure and interactions of matter.
Matter - anything that takes up space and has ____________.
Element - substance that _______________ be broken down into other substances by chemical reactions.
Oxygen, _____________, hydrogen, and nitrogen are the most common elements in the human body.
I. Atoms and atomic structure
Atom - structural ____________ of matter; consist of neutrons, protons, and electrons in different proportions.
Protons - positively charged and stay in the nucleus; have ______________.
Neutrons - not charged (neutral) and stay in the _____________; have mass.
Electrons - ______________ charged; orbit nucleus; have very, very little mass.
Atomic number = # protons; defines which ______________ is which. Example:
# _______________ = # protons
______________ number = # protons + # neutrons
II. Isotopes
Isotopes - elements that have different mass numbers and hence different numbers of ________________.
Example:
Radioactive isotopes - _____________ isotopes.
Half-life - the time it takes for ______________ of the radioactive materials to decay.
Electron shells - 2, 8, 8
III. Be able to diagram an element.
Na, atomic # ________, mass # ____________
Ions - charged _____________
Cations - elements with a ____________ charge; from losing an electron. Example:
Cl, atomic # ________, mass # ____________
Anions - elements with a negative charge; from _______________ an electron. Example:
Molecule - 2 or more ____________ join together.
- formed by covalent bond
Example:
Compound - ________ or more elements get together.
- formed by ionic bond
Example:
IV. Types of Bonds
Ionic bond - transfer or acceptance of electrons; breaks into cations and anions; conducts electricity. Example:
Nonpolar covalent bonds - share electrons ___________.
Single bonds - atoms share _________ pair of electrons. Example:
Double bonds - atoms share 2 pairs of ______________. Example:
________________ bonds - atoms share 3 pairs of electrons. Example:
Polar covalent bonds - share electrons unevenly. Example:
Hydrogen bonds - an attraction between a H and an O that are already bonded to other elements. Example:
By exchanging ________________ atoms can combine to form different chemicals.
_____________ is one of the basic compounds that we need for life.
V. Solutions
Solvent - ______________ that things are being dissolved in.
Solute - the thing being dissolved. Example:
Solution - a liquid with substances ______________ dissolved in it. Example:
Suspension - the solute is __________ completely dissolved in the solvent.
Because ____________ is a polar molecule, it is an excellent solvent.
There is __________ universal solvent.
VI. Properties of Water
Cohesion - _____________ bonds hold a substance together.
Surface tension - how difficult it is to break the ___________ of a liquid.
Adhesion - one substance clings to _____________.
VII. pH Scale
H20 = H+ (hydrogen ion) + OH- (hydroxide ion)
pH = -log of the concentration of the hydrogen ions; how ____________ a solution is.
Acid - pH less than _________; more H+. Example:
Base (alkaline) - pH ______________ than 7; more OH-. Example:
Neutral - _____________ 7; H+ = OH-. Example:
An acid will turn litmus paper ____________.
A base will turn litmus paper _____________.
Changing the pH by 1 unit is ________________ more or less H+ than your body likes.
Adding pure water does ____________ dilute an acid.
Buffers - converts strong acids / bases into ____________ acids / bases.
VIII. Acid Rain
Acid rain - rain that has a pH less than ______________
A major source of acid rain is burning fossil fuels like coal, ____________, and gas in car and factories.
Acid rain can
1. make lakes too acidic to support _____________.
2. kill ____________.
3. interfere with crop growth.
4. kill _____________.
5. increase the exposure to toxic metals because they dissolve ______________ in acids.
Acid rain does NOT contribute to _______________________________ or the hole in the ozone layer.
IX. Organic Chemistry
Inorganic compounds - ______________ contain carbon.
Organic compounds - contain _____________ usually covalently bonded to H, O, N, S, or P.
Functional groups - various attachments to organic molecules; know the formula, the name, and recognize an
example.
1. Hydroxyl (-OH) - an ____________; name ends in -ol; methanol, ethanol.
2. Carboxyl (-COOH) - carboxylic acids; acetic acid.
3. Amino (-__________) - amines
Amino acid - has both -COOH and -NH2; glycine, lysine
4. Phosphate (-P with some _____________) - phosphates; adenosine triphosphate.
All of these functional groups give __________________ properties to their compounds.
Large Molecules
Polymer - molecule made up of _______________ repeating units.
Monomer - molecule with __________ repeat.
Dehydration reaction - 2 molecules are covalently joined by losing an -OH from one and an -H from the other
making __________________.
Hydrolysis - water used to break a polymer into 2 monomers; one monomer gains an _____________, the other
gains an -H.
1. Carbohydrates
Carbohydrates - usually 1 or more ____________ molecules hooked together.
A. Monosaccharide - one sugar molecule with ____________ carbon molecules. Example:
B. Disaccharide - 2 _____________ molecules hooked together through dehydration synthesis. Example:
Glycosidic linkage - covalent ____________ between saccharides.
C. Polysaccharide - more than 2 sugar molecules hooked together. Example:
a. Glycogen - polymer of glucose used by ____________ to store glucose in the liver and muscle cells.
b. Starch - polymer of glucose used by _____________; can be broken down by animals in digestive tract.
c. Cellulose - polymer of glucose in plant cell walls; fiber; ______________ be broken down by most
animals in digestive tract.
d. Chitin - polymer of glucose with a ________________ containing group; used in insects' exoskeleton.
2. Lipids
Lipids - large hydrophobic molecules; _____________, phospholipids, and steroids.
Fat - glycerol and fatty acids together.
Triglycerides - a glycerol + __________ fatty acids; fats in storage.
Saturated fatty acids - have __________ single bonds; bad fats.
Unsaturated fatty acids - have 1 or more double bonds; ___________ fats.
Phospholipids - glycerol + 2 fatty acids + 1 phosphate group; used in ____________ membranes; has a
hydrophilic head and a hydrophobic tail
Hydrophilic - water ____________
Hydrophobic - water _____________
Hydrophobic bond - 2 hydrophobic ends can stay together to keep ____________ out.
Steroids - have ________ rings of carbon atoms; cholesterol, sex hormones, bile salts, Vitamin D.
3. Proteins
Proteins - cellular building blocks made of different combinations of ___________ amino acids.
Peptide bond - covalent bond between amino acids.
Dipeptide - _____ amino acids joined together
Tripeptide - ________ amino acids joined together
Polypeptide - many _________________ joined together; protein.
Denaturation - destroying _________________ by destroying its shape.
4. Nucleic Acids
Nucleic acids - polymers of nucleotides
Nucleotide - nitrogenous base (that varies), a ____________ carbon sugar (ribose), and a phosphate group.
DNA - deoxyribonucleic acid; hereditary information on how to make ________________ protein the body will
ever need.
RNA - ribonucleic acid; a copy of the instructions for ____________ single protein that is needed now.
ATP - adenosine triphosphate; _________________.
Last Updated: 11/8/2006
Chemistry - _____________ of the structure and interactions of matter.
Matter - anything that takes up space and has ____________.
Element - substance that _______________ be broken down into other substances by chemical reactions.
Oxygen, _____________, hydrogen, and nitrogen are the most common elements in the human body.
I. Atoms and atomic structure
Atom - structural ____________ of matter; consist of neutrons, protons, and electrons in different proportions.
Protons - positively charged and stay in the nucleus; have ______________.
Neutrons - not charged (neutral) and stay in the _____________; have mass.
Electrons - ______________ charged; orbit nucleus; have very, very little mass.
Atomic number = # protons; defines which ______________ is which. Example:
# _______________ = # protons
______________ number = # protons + # neutrons
II. Isotopes
Isotopes - elements that have different mass numbers and hence different numbers of ________________.
Example:
Radioactive isotopes - _____________ isotopes.
Half-life - the time it takes for ______________ of the radioactive materials to decay.
Electron shells - 2, 8, 8
III. Be able to diagram an element.
Na, atomic # ________, mass # ____________
Ions - charged _____________
Cations - elements with a ____________ charge; from losing an electron. Example:
Cl, atomic # ________, mass # ____________
Anions - elements with a negative charge; from _______________ an electron. Example:
Molecule - 2 or more ____________ join together.
- formed by covalent bond
Example:
Compound - ________ or more elements get together.
- formed by ionic bond
Example:
IV. Types of Bonds
Ionic bond - transfer or acceptance of electrons; breaks into cations and anions; conducts electricity. Example:
Nonpolar covalent bonds - share electrons ___________.
Single bonds - atoms share _________ pair of electrons. Example:
Double bonds - atoms share 2 pairs of ______________. Example:
________________ bonds - atoms share 3 pairs of electrons. Example:
Polar covalent bonds - share electrons unevenly. Example:
Hydrogen bonds - an attraction between a H and an O that are already bonded to other elements. Example:
By exchanging ________________ atoms can combine to form different chemicals.
_____________ is one of the basic compounds that we need for life.
V. Solutions
Solvent - ______________ that things are being dissolved in.
Solute - the thing being dissolved. Example:
Solution - a liquid with substances ______________ dissolved in it. Example:
Suspension - the solute is __________ completely dissolved in the solvent.
Because ____________ is a polar molecule, it is an excellent solvent.
There is __________ universal solvent.
VI. Properties of Water
Cohesion - _____________ bonds hold a substance together.
Surface tension - how difficult it is to break the ___________ of a liquid.
Adhesion - one substance clings to _____________.
VII. pH Scale
H20 = H+ (hydrogen ion) + OH- (hydroxide ion)
pH = -log of the concentration of the hydrogen ions; how ____________ a solution is.
Acid - pH less than _________; more H+. Example:
Base (alkaline) - pH ______________ than 7; more OH-. Example:
Neutral - _____________ 7; H+ = OH-. Example:
An acid will turn litmus paper ____________.
A base will turn litmus paper _____________.
Changing the pH by 1 unit is ________________ more or less H+ than your body likes.
Adding pure water does ____________ dilute an acid.
Buffers - converts strong acids / bases into ____________ acids / bases.
VIII. Acid Rain
Acid rain - rain that has a pH less than ______________
A major source of acid rain is burning fossil fuels like coal, ____________, and gas in car and factories.
Acid rain can
1. make lakes too acidic to support _____________.
2. kill ____________.
3. interfere with crop growth.
4. kill _____________.
5. increase the exposure to toxic metals because they dissolve ______________ in acids.
Acid rain does NOT contribute to _______________________________ or the hole in the ozone layer.
IX. Organic Chemistry
Inorganic compounds - ______________ contain carbon.
Organic compounds - contain _____________ usually covalently bonded to H, O, N, S, or P.
Functional groups - various attachments to organic molecules; know the formula, the name, and recognize an
example.
1. Hydroxyl (-OH) - an ____________; name ends in -ol; methanol, ethanol.
2. Carboxyl (-COOH) - carboxylic acids; acetic acid.
3. Amino (-__________) - amines
Amino acid - has both -COOH and -NH2; glycine, lysine
4. Phosphate (-P with some _____________) - phosphates; adenosine triphosphate.
All of these functional groups give __________________ properties to their compounds.
Large Molecules
Polymer - molecule made up of _______________ repeating units.
Monomer - molecule with __________ repeat.
Dehydration reaction - 2 molecules are covalently joined by losing an -OH from one and an -H from the other
making __________________.
Hydrolysis - water used to break a polymer into 2 monomers; one monomer gains an _____________, the other
gains an -H.
1. Carbohydrates
Carbohydrates - usually 1 or more ____________ molecules hooked together.
A. Monosaccharide - one sugar molecule with ____________ carbon molecules. Example:
B. Disaccharide - 2 _____________ molecules hooked together through dehydration synthesis. Example:
Glycosidic linkage - covalent ____________ between saccharides.
C. Polysaccharide - more than 2 sugar molecules hooked together. Example:
a. Glycogen - polymer of glucose used by ____________ to store glucose in the liver and muscle cells.
b. Starch - polymer of glucose used by _____________; can be broken down by animals in digestive tract.
c. Cellulose - polymer of glucose in plant cell walls; fiber; ______________ be broken down by most
animals in digestive tract.
d. Chitin - polymer of glucose with a ________________ containing group; used in insects' exoskeleton.
2. Lipids
Lipids - large hydrophobic molecules; _____________, phospholipids, and steroids.
Fat - glycerol and fatty acids together.
Triglycerides - a glycerol + __________ fatty acids; fats in storage.
Saturated fatty acids - have __________ single bonds; bad fats.
Unsaturated fatty acids - have 1 or more double bonds; ___________ fats.
Phospholipids - glycerol + 2 fatty acids + 1 phosphate group; used in ____________ membranes; has a
hydrophilic head and a hydrophobic tail
Hydrophilic - water ____________
Hydrophobic - water _____________
Hydrophobic bond - 2 hydrophobic ends can stay together to keep ____________ out.
Steroids - have ________ rings of carbon atoms; cholesterol, sex hormones, bile salts, Vitamin D.
3. Proteins
Proteins - cellular building blocks made of different combinations of ___________ amino acids.
Peptide bond - covalent bond between amino acids.
Dipeptide - _____ amino acids joined together
Tripeptide - ________ amino acids joined together
Polypeptide - many _________________ joined together; protein.
Denaturation - destroying _________________ by destroying its shape.
4. Nucleic Acids
Nucleic acids - polymers of nucleotides
Nucleotide - nitrogenous base (that varies), a ____________ carbon sugar (ribose), and a phosphate group.
DNA - deoxyribonucleic acid; hereditary information on how to make ________________ protein the body will
ever need.
RNA - ribonucleic acid; a copy of the instructions for ____________ single protein that is needed now.
ATP - adenosine triphosphate; _________________.
Last Updated: 11/8/2006
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