Chapter 2

Front 1

Define matter, and list its three forms.

Back 1

Matter has mass and occupies space.

92 naturally occurring elements make up matter.

3 forms: Solid, Liquid, and Gas.

Front 2

Describe and differentiate among the subatomic particles that compose atoms.

Back 2

Neutrons: No charge

Protons: Postive charge (+)

Electrons: Negative Charge (-), located in varying distance from the nucleus in regions called orbitals.

Front 3

Explain the arrangement of elements in the periodic table based on atomic number.

Back 3

Chemical symbol

-Unique to each element (Usually identified by first letter, or first letter plus an additional letter, e.g., C is carbon)

Atomic number

-Number of protons in an atom of the element (Located above symbol name)

-Elements arranged by anatomic number within rows

Average atomic mass

-Mass of both protons and neutrons (Shown below the element’s symbol on the table)

Front 4

Describe an isotope.

Back 4

1 or 2 or more atoms that have the same atomic number (the same number of protons) but a different number of neutrons.

Front 5

Explain how radioisotopes differ from other types of isotopes.

Back 5

The difference is that radioisotopes are very unstable and contain high levels of nuclear energy and emit this energy in the form of nuclear radiation.

Front 6

Describe how elements are organized in the periodic table based on the valence electron number.

Back 6

An element's location in the periodic table is largely dependent on its electrons; the number of valence shell electrons determines it is a group, and the type of orbital in which the valence electrons lie in determines the element's block.

Front 7

State the octet rule.

Back 7

The octet rule says that atoms like to have full outer shells of only eight electrons. Atoms will lose or gain valence electrons to make their outer shells full with eight electrons, and they do this by bonding with other atoms.

Front 8

What are the major elements that compose 98% body weight?

Back 8

Oxygen(65%), Carbon(18%), Hydrogen(10%), Nitrogen(3%), Calcium(1.5%), and Phosphorus (1%).

Front 9

What are the minor elements that compose less than 1% body weight?

Back 9

Sulfur (0.25%), Potassium (0.20%), Sodium (0.15%), Chlorine (0.15%), Magnesium (0.05%), and Iron (0.006%).

Front 10

How do you determine the number of subatomic particles for protons? Neutrons? Electrons?

Back 10

Proton number = atomic number

Neutron number = atomic mass – atomic number

--Neutron number = (p + n) – p

--Neutron number of Na = 23 – 11 = 12

Electron number = proton number

Front 11

What are negatively charged ions called?

What are some common anions?

Back 11

Anions

Chloride Ion, Bicarbonate ion, and Phosophate ion.

Front 12

What is a positive charged ions called?

Back 12

Cations

Front 13

Polyatomic Ions are?

Back 13

anions with more than one atom

(ex. bicarbonate ion and phosphate ion)

Front 14

Atoms with 1, 2, or 3 electrons in valence shell become _________.

Back 14

Cations.

*Reaches stability by donating 2 electrons. (Develops a charge of +2)

Front 15

Atoms with 5, 6, or 7 electrons become _________.

Back 15

Anions.

*Reaches stability by gaining 1 electrons. (Develops a charge -1)

Front 16

Elements on the left side of the periodic are called?

The tend to lose ____.

Back 16

Metallic side.

Electrons.

Front 17

Elements on the right side of the periodic are called?

They tend to gain _____.

Back 17

Nonmetallic side.

Electrons.

Front 18

What is an ionic bond?

Back 18

Cations and anions bound by electrostatic forces.

=Form Salts

Front 19

Formation of an Ionic bond involve _____ and ______.

Back 19

Sodium and Chloride.

Front 20

What is the charge for a magnesium ion, based on its position in the periodic table?

Back 20

Magnesium is in group 2A.

It has two outer or valence electrons in a 2s subshell. These two electrons can be removed relatively easily. The cation has a charge of +2 just like calcium.

Front 21

Could an ionic bond form between two cations?

Back 21

No, an ionic bond could not be created between two cations. Cations such as H+ have no electron to pass to each other, and therefore cannot great a bond.

Front 22

Define a molecular formula.

Back 22

a formula giving the number of atoms of each of the elements present in one molecule of a specific compound.

Ex. C6H1206

Front 23

Describe a structural formula, and explain its use in differentiating isomers.

Back 23

Shows # and types of atoms

Shows their arrangement w/in the molecule

Provides a means for differentiating isomers

-Molecules w/ the same # and kinds of elements arranged differently in space(glucose, galactose, fructose)

Front 24

Describe a covalent bond and explain its formation based on the octet rule.

Back 24

Covalent bond: atoms share electrons

Occurs w/ atoms that have four to seven electrons in their outer shell, they share to make shell full.

Front 25

List the four most common elements in the human body.

Back 25

Four elements most commonly form covalent bonds:

Oxygen

Carbon

Hydrogen

Nitrogen

Front 26

Distinguish between single, double, and triple covalent bonds.

Back 26

Single: A pair of electrons are shared(2 H atoms)

Double: Two pairs of electron are shared(2 O atoms)

Triple: Three pairs are shared (2 N atoms)

Front 27

Explain polar and nonpolar covalent bonds.

Back 27

Polar: They are partially charge, one charge may be stronger than the other, unequal sharing

Nonpolar: Equally charged, equally shared

Front 28

Describe the difference between a nonpolar molecule and a polar molecule.

Back 28

Polar: unequal sharing. H2O

Nonpolar: equal sharing. CO2

Front 29

Define an amphipathic molecule.

Back 29

Polar in one region and nonpolar in another.

Phospholipids; Hydro Phillic and Phobic

Front 30

Describe the hydrogen bonding between polar molecules.

Back 30

Attraction b/w partially positive hydrogen atom and partially negative atom

Individually weak, collectively strong

Front 31

List and define the intermolecular attractions between nonpolar molecules.

Back 31

van der Walls forces: electrons orbiting nucleus briefly, unevenly distributed

hydrophobic interactions: nonpolar placed in polar substance

Front 32

What is a covalently bonded molecule?

Back 32

Electrons shared between atoms of two or more different elements.

Termed molecular compounds.

E.g., carbon dioxide (CO2), but not molecular oxygen (O2)

Front 33

What is a molecular formula?

Back 33

Indicates number and type of atoms.

E.g., carbonic acid (H2CO3)

Front 34

What is a structural formula?

Back 34

Indicates number and type of atoms.

Indicates arrangement of atoms within the molecule.

E.g., O=C=O (carbon dioxide).

Allows differentiation of isomers

Same number and type of elements, but arranged differently in space

Front 35

Glucose vs. Galactose vs. Fructose

Back 35

Same molecular formula.

6 carbon, 12 hydrogen, 6 oxygen.

Atoms arranged differently

Front 36

What information about a molecule is gained by a structural formula?How does this differ from a molecular formula?

Back 36

The molecular formula exhibits the type and number of atoms in a molecule; the structural formula also provides information on how the atoms are arranged.

Front 37

What is an isomer?

Back 37

Isomers are molecules composed of the same type and number of elements, but are arranged differently.

Front 38

What is a covalent bond?

Back 38

Atoms share electrons.

Occurs when both atoms require electrons.

Occurs with atoms with 4 to 7 electrons in outer shell.

Front 39

What are the most common elements used to form covalent bonds in the body?

Back 39

Hydrogen, Oxygen, Nitrogen, and Carbon.

Front 40

Oxygen needs ___ electrons to complete the outer shell. It forms ___ covalent bonds.

Back 40

2.

2.

Front 41

Nitrogen forms _____ bonds.

Back 41

3.

Front 42

Carbon forms ____ bonds.

Back 42

4.

Front 43

The simplest covalent bond an atom is able to form occurs between ______ _______ atoms.

Back 43

2 hydrogen.

Front 44

What is a single covalent bond?

Back 44

One pair of electrons shared.

E.g., between two hydrogen atoms

Front 45

What is a double covalent bond?

Back 45

Two pairs of electrons shared.

E.g., between two oxygen atoms

Front 46

What is a triple covalent bond?

Back 46

Three pairs of electrons shared.

E.g., between two nitrogen atoms

Front 47

Carbon needs ____ electrons to satisfy the _____ rule.

What are the most commonly known formations?

Back 47

4. Octet.

Methane (CH4), Carbon Dioxide (CO2), and Ethanol (C2H5OH).

Front 48

What is a carbon skeleton formation?

Back 48

Bonds in straight chains, branched chains, or ring.

Carbon present where lines meet at an angle

Additional atoms are hydrogen

Front 49

What is electronegativity?

Back 49

Electronegativity—relative attraction of each atom for electron.

Determines how electrons are shared in covalent bonds

Two atoms of same element have equal attraction for electrons

Resulting bond is nonpolar covalent bond Sharing of electrons unequally = polar covalent bond

Front 50

In the periodic table, electronegativity increases ___________ acrosses the row, _______ in the column.

Back 50

Left to right.

Bottom to top.

Front 51

What the most common elements composing living organisms?

List them from least to greatest electronegativity.

Back 51

Oxygen, nitrogen, carbon, and hydrogen.

Hydrogen < Carbon < Nitrogen

Front 52

More electronegative atom develops a ______ ______ charge.

Back 52

Partial Negative.

Front 53

Less electronegative atom develops a ______ _____ charge.

Back 53

Partial Positive.

Front 54

*EXCEPTION*

Back 54

To rule of a polar bond forming between 2 different atoms.

ex. Carbon bonding with hydrogen

Front 55

What type of bond is formed between two oxygen atoms?

Back 55

Oxygen atoms each contain six electrons in their outer orbitals and each have room for two more. In a double bond they share two pairs of electrons and thereby each satisfies the octet rule.

Front 56

Why are some covalent bonds nonpolar and others polar?

Back 56

A covalent bond between atoms of the same element will result in an equal distribution of electrons across the molecule since both atoms are equally electronegative, resulting in a nonpolar molecule. Molecules composed of different atoms result in an unequal distribution of charge across the molecule, where more electronegative atoms have a slightly negative charge and less electronegative atoms are slightly less negative.

Front 57

What is a nonpolar molecule?

Back 57

Contain nonpolar covalent bonds.

Ex. O--O and C--H are nonpolar bonds

Front 58

What are polar molecules?

Back 58

Molecules contain polar covalent bonds.

O—H is a polar bond in the polar molecule water (H2O)

Front 59

What is an amphipathic molecule?

Back 59

Large molecules with both polar and nonpolar regions

E.g., phospholipids

Front 60

Is molecular oxygen nonpolar or polar?

Back 60

No polarity, since it is electronegative .

Front 61

Is carbon dioxide polar or nonpolar?

Back 61

*

Front 62

What is an intermolecular attraction?

Back 62

Weak chemical attractions between molecules.

Important for shape of complex molecules.

E.g., DNA and proteins

Front 63

What a hydrogen bond?

Back 63

Forms between polar molecules.

Attraction between partially positive hydrogen atom and a partially negative atom

Individually weak, collectively strong.

Influences how water molecules behave

Front 64

Van der Waals force is ______.

Back 64

An extremely weak electrical force, but the bigger the molecule, the stronger it is.

Front 65

Define hydrophobic.

Back 65

Hydro= Water

Phobic= Fear

Hydrophobic= fear of water.

If occurring between 2 large molecules, it is termed as intramolecular attraction.

Front 66

What is the name of the intermolecular attraction between a partially charged hydrogen of one polar molecule with a partially negative atom of another polar molecule?

Back 66

A Hydrogen bond is an intermolecular attraction between a slightly positive hydrogen atom and another slightly negative atom.

Front 67

Describe the molecular structure of water and how water molecules form four hydrogen bonds.

Back 67

*

Front 68

List the different properties of water and provide an example of the importance of each property within the body.

Back 68

Transports

Substances dissolved in H20 moved throughout body

Lubricates

Decreases friction b/w body structure (serous fluid)

Cushions

Absorbs sudden forces of body movements (CSF)

Excretes Waste

Front 69

Compare substances that dissolve in water with those that both dissolve and dissociate in water. Distinguish between electrolytes and nonelectrolytes.

Back 69

Covalently bonded compounds such as glucose will not dissociate when dissolved in water; however, they will remain in solution after the mixture is no longer agitated. Ionic compounds such as sodium chloride (NaCl) will disassociate in water. The polar water molecules will disrupt the electrostatic interactions between sodium and chloride ions, thereby separating them

Front 70

Describe the chemical interactions of nonpolar substances and water.

Back 70

*

Front 71

Explain how amphipathic molecules interact in water to form chemical barriers.

Back 71

*

Front 72

What composes 2/3s of the human body by weight?

Back 72

WATER!!!!

Front 73

Water is a polar molecule that has ________.

Back 73

oOneoxygen atom bonded to two hydrogen atoms

oOxygenatom has two partial negative charges

oHydrogenshave single partial positive charge

Front 74

Water can form ___ hydrogen bonds with adjacent molecules.

Back 74

4.

Central to water's properties.

Front 75

What are the 3 phases of water?

Define each.

Back 75

Gas (water vapor)- substance with low molecular mass.

Liquid (water)- almost all water in the body

Solid (ice)

Front 76

What are the functions of liquid water?

Define each.

Back 76

Transports

-Substances dissolved in water move easily throughout body

Lubricates

-Decreases friction between body structures

Cushions

-Absorbs sudden force of body movements Excretes wastes

-Unwanted substances dissolve in water are easily eliminated

Front 77

What is cohesion?

Back 77

Attraction between water molecules due to hydrogen bonding

Front 78

What is surface tension?

Back 78

Inward pulling of cohesive forces at surface of water.

Causes moist sacs of air in lungs to collapse

--Surfactant, a lipoprotein, prevents collapse

Front 79

What is adhesion?

Back 79

Attraction between water molecules and a substance other than water

Front 80

What is temperature?

Back 80

Measure of kinetic energy of atoms or molecules within a substance

Front 81

What is specific heat?

Back 81

Amount of energy required to increase temperature of 1 gram of a substance by 1 degree Celsius.

Water’s value extremely high due to energy needed to break hydrogen bonds.

Contributes to keeping body temperature constant

Front 82

What is the heat of vaporization?

Back 82

Heat required for release of molecules from a liquid phase into a gaseous phase for 1 gram of a substance.

Water’s value very high due to hydrogen bonding

Sweating cools body

-Excess heat dissipated as water evaporates

Front 83

Which property of water contributes to the need to produce surfactant to prevent the collapse of the alveoli?

Back 83

*

Front 84

Which property contributes to body temperature regulation through sweating?

Back 84

The high heat of vaporization of water molecules makes them an effective mechanism for dissipating heat at the surface of the skin.

Front 85

Why is sweating less effective in cooling the body on a humid day?

Back 85

*

Front 86

Water is a ______ of the body.

Back 86

Solvent.

Front 87

Define solute.

Back 87

Solutes are substances that dissolve in water

Front 88

Why is water defined as the universal solvent?

Back 88

Water is called universal solvent because most substances dissolve in it

Front 89

What determines whether a substance will dissolve or not?

Back 89

The chemical property.

Front 90

Define Hydrophilic.

Back 90

Water Loving.

Front 91

Water surrounds substances and forms a _____ _______.

Back 91

Hydration shell.

Front 92

What is a nonelectrolyte?

Back 92

A substance that remains intact, but does not conduct a current.

Front 93

Substances _____ and _______ (separate).

Back 93

Dissolve.

Dissociate.

Front 94

What can an electrolyte conduct?

Back 94

It can conduct a current.

Front 95

Define Hydrophobic exclusion.

Back 95

cohesive water molecules “force out” nonpolar molecules

Front 96

Define hydrophobic interaction.

Back 96

"excluded molecules”

Front 97

Hydrophobic substances require _______ _______ to be transported within the blood

Back 97

Carrier proteins.

Front 98

Amphipathic molecules have polar and nonpolar regions.

Back 98

Polar portion of molecule dissolves in water.

Nonpolar portion repelled by water

Front 99

Phospholipid molecules are ______.

Back 99

Amphipathic.

Polar heads have contact with water.

Nonpolar tails group together.

Results in bilayers of phospholipid molecules. E.g., membranes of a cell

Front 100

Other amphipathic molecules form a ______.

Back 100

Micelle.

Front 101

Describe what is formed when water dissociates.

Back 101

*

Front 102

Explain the difference between an acid and a base.

Back 102

*

Front 103

Define pH and explain the relative pH values of both acids and bases.

Back 103

*

Front 104

Explain the term neutralization, and describe how the neutralization of both an acid and a base occur.

Back 104

*

Front 105

Describe the action of a buffer.

Back 105

Buffers maintain the pH of physiologic solutions within a normal range by absorbing hydrogen ions when an acid is added or hydroxyls when a base is added to the solution.

Front 106

Water can spontaneously dissociate to form ____.

Back 106

Ions.

Front 107

How does the interaction of a nonelectrolyte and water differ from the interaction of an electrolyte and water?

Back 107

Nonelectrolytic molecules such as glucose do not dissociate in water. Electrolytes such as sodium chloride (NaCl) disassociate into constituent ions in an aqueous environment, forming a solution capable of conducting electricity.

Front 108

Why is water neutral?

Back 108

*

Front 109

Acid dissociates in water to produce?

Back 109

H+ and an anion.

Proton donor

Increases concentration of free H+

More dissociation of H+ with stronger acids

-----E.g., HCl in the stomach

Less dissociation of H+ with weaker acids

-----E.g., carbonic acid in the blood

Substance A (an acid in water) --> H+ + Anion

Front 110

Base accepts _____ when added to a solution.

Back 110

H+.

Proton acceptor.

More absorption of H+ with stronger bases

--E.g., ammonia and bleach

Less absorption of H+ with weaker bases

--E.g., bicarbonate in blood and in secretions released into small intestine

Substance B (a base in water) + H+ B—H

Front 111

pH is a measure of ____.

Back 111

H+.

Range between 0-14.

Front 112

pH and H+ concentration are inversely related because ___?

Back 112

Inverse of the log for a given H+ concentration

As H+ concentration increases, pH decreases

As H+ concentration decreases, pH increases

Front 113

Solutions with equal concentrations of H+ and OH–, have a?

Back 113

have a pH of 7 and are neutral.

Front 114

Solutions with greater H+ than OH–

Back 114

Have a pH of <7 and are acidic.

Front 115

Solutions with greater OH– than H+

Back 115

Have a pH >7 and are basic (alkaline)

Front 116

What is neutralization?

Back 116

When an acidic or basic solution is returned to neutral (pH 7)

Acids neutralized by adding base

Bases neutralized by adding acid

Front 117

What is a buffer?

Back 117

Help prevent pH changes if excess acid or base is added

Act to accept H+ from excess acid or donate H+ to neutralize base

------Carbonic acid (weak acid) and bicarbonate (weak base) buffer blood pH

------Both help maintain blood pH in a critical range (7.35 to 7.45)

Front 118

What type of substances release H+ when added to water?

Back 118

An acid is capable of releasing hydrogen ions in an aqueous environment

Front 119

What is the general relationship of H+ and pH?

Back 119

pH is the relative measure of hydrogen ions in a solution

Front 120

Why are buffers important?

Back 120

Buffers maintain the pH of physiologic solutions within a normal range by absorbing hydrogen ions when an acid is added or hydroxyls when a base is added to the solution.

Front 121

Compare and contrast the three different types of water mixtures.

Back 121

*

Front 122

Explain how an emulsion differs from other types of mixtures.

Back 122

*

Front 123

Explain the different ways to express the concentration of solute in a solution.

Back 123

*

Front 124

Define mixture.

Back 124

Mixtures are formed from combining two or more substances

Front 125

What are the 2 defining features of a mixture?

Back 125

Substances mixed are not chemically changed.

Substances can be separated by physical means

Front 126

What are the 3 categories of water mixtures?

Define each.

Back 126

Suspension: material larger in size than 100 nanometers mixed with water (does not remain mixed unless in motion, scatters light and appears opaque/cloudy)

Colloid: protein of size from 1to100 nanometers (Remains mixed when not in motion, scatter light)

Solution: homogeneous mixture of material smaller than 1 nanometer (Does not scatter light or settle if solution is not in motion.

Front 127

What is the special category of suspension?

Back 127

Emulsion.

Water and a nonpolar liquid substance, does not mix unless shaken.

Front 128

What is concentration determined by?

Back 128

Concentration is determined by the amount of solute dissolved in a solution

Front 129

What are the expressions of concentration?

Back 129

Mass/volume

--Mass of solute per volume of solution

Mass/volume percent

--Grams of solute per 100 mL solution

Molarity

--Moles solute/L solution (more easily measure in the body, than molality)

Molality

--Moles solute/kg solvent (slightly more accurate than molarity)

Front 130

What is Osmoles?

Back 130

Osmoles (osm) is the unit of measurement for the number of particles in a solution.

Reflects whether a substance dissolves, or dissolves and dissociates.

Can be expressed as osmolarity or osmolality.

Front 131

Define Osmolarity.

Back 131

Number of particles in a 1 liter solution.

Easier to measure.

Blood serum expresses as milliosmoles

Front 132

Define Osmolality.

Back 132

Number of particles in 1 kg of water.

More accurate, but difficult to measure

Front 133

A water mixture of unknown type shows settling of materials to the bottom of the tube when it is not in motion. What type is it?

Back 133

*

Front 134

What are the four ways solution concentration may be expressed?

Back 134

*

Front 135

Differentiate between an organic molecule and an inorganic molecule.

Back 135

*

Front 136

Describe the general chemical composition of biomolecules.

Back 136

*

Front 137

Define a monomer and polymer.

Back 137

*

Front 138

Describe the role of water in both dehydration and hydrolysis reactions in altering biomolecules.

Back 138

*

Front 139

Describe the general characteristics of a lipid.

Back 139

*

Front 140

Identify the four types of lipids and their physiologic roles.

Back 140

*

Front 141

Describe the distinguishing characteristics of carbohydrates.

Back 141

*

Front 142

Explain the relationship between glucose and glycogen.

Back 142

*

Front 143

Name some other carbohydrates found in living systems.

Back 143

*

Front 144

Describe the general structure of a nucleic acid.

Back 144

*

Front 145

Describe the structure of a nucleotide monomer.

Back 145

*

Front 146

Distinguish between DNA and RNA.

Back 146

*

Front 147

Name other important nucleotides.

Back 147

*

Front 148

List the general functions of proteins.

Back 148

catalyzing chemical reactions

synthesizing and repairing DNA

transporting materials across the cell

receiving and sending chemical signals

responding to stimuli

providing structural support

Front 149

Describe the general structure of amino acids and proteins.

Back 149

*

Front 150

What are the three biomolecules that are polymers?

Back 150

There are four major classes of biomolecules:

Carbohydrates

Lipids

Proteins

Nucleic acids

Front 151

What are the monomers that compose them?

Back 151

C- monosaccharides

P- amino acids

N. A.- nucleotides

L- glycerol and fatty acids

Front 152

Which class of lipids forms cell membranes?

Back 152

Phospholipid

Front 153

What is a lipid?

What are the main functions of a lipid?

Back 153

Diverse group of fatty, water-insoluble molecules.

Function as stored energy, cellular membrane components, hormones

Front 154

What are the 4 primarily classes of a lipid?

Back 154

1.Triglycerides

2.Phospholipids

3.Steroids

4.Eicosanoids

Front 155

What is a triglyceride?

Back 155

Most common form of lipid in living things. Long-term energy storage in adipose tissueStructural support, cushioning, insulation. Formed from a glycerol molecule and three fatty acids

—H from the glycerol, an —OH from the fatty acid

Formed during a dehydration synthesis

Front 156

Define Saturated, unsaturated, and polyunsaturated.

Back 156

Saturated, lack double bonds

Unsaturated, one double bondPolyunsaturated, two or more double bonds

Front 157

Define Lipogenesis.

Back 157

formation of triglycerides when conditions of excess nutrients exist

Front 158

Define Lipolysis.

Back 158

Breakdown of triglycerides when nutrients are needed

Front 159

What is a phospholipid?

Back 159

Amphipathic molecules that form chemical barriers of cell membranes

Front 160

What is a steroid?

Back 160

Composed of hydrocarbons arranged in multiringed structure

Four carbon rings; three have 6 carbon atoms, one has 5 carbon atoms

Front 161

What is an eicosanoid?

What are the primary functions?

Back 161

Modified 20-carbon fatty acids

Primary functions in the inflammatory response and nervous system communication.

Front 162

What are 4 class of Eicosanoids?

Back 162

1.Prostaglandins

2.Prostacyclins

3.Thromboxanes

4.Leukotrienes

Front 163

Which class of lipids forms cell membranes?

Back 163

Phospholipid

Front 164

Most animal fats are _______, at room temperature.

Back 164

Saturated

Front 165

Most vegetable fats are ________, generally healthier.

Back 165

Unsaturated.

Front 166

Partial hydrogenation may lead to ______ _____.

Back 166

Trans Fats.

Front 167

What is the repeating monomer of glycogen?

Back 167

Glucose monomer

Front 168

Where is glycogen stored in the body?

Back 168

Glycogen is made and mainly stored primarily in the cells of the liver and the muscle hydrated with 3 or 4 parts of water.

Front 169

Is galactose a monosaccharide, disaccharide or polysaccharide?

Back 169

Monosaccharide

Front 170

Is sucrose a monosaccharide, disaccharide or polysaccharide?

Back 170

Disaccharide

Front 171

What are the structural differences between RNA and DNA?

Back 171

RNA has the sugar ribose, it is single stranded and has the base U instead of T

DNA has the sugar deoxyribose, it is double stranded and has the Base T not U

Front 172

What are the functions of proteins?

Back 172

Serve as catalysts (enzymes) in metabolic reactions

Act in defense Aid in transport

Contribute to structural support

Cause movement

Perform regulation

Provide storage

Front 173

Define N-terminal end.

Define C-terminal end.

Back 173

N-terminal end has free amine group.

C-terminal end has free carboxyl group

Front 174

What are the monomers of proteins?

Back 174

Amino acids

Front 175

Name the categories of amino acids.

Back 175

*

Front 176

Distinguish between nonpolar, polar, and charged amino acids.

Back 176

*

Front 177

Give examples of amino acids with special characteristics.

Back 177

*

Front 178

Describe the different types of intramolecular attractions that participate in both the folding of a protein and in maintaining its three-dimensional shape.

Back 178

*

Front 179

Distinguish between the four structural hierarchy levels of proteins.

Back 179

1.Primary structure

The sequence of amino acids in the protein's polypeptide chain(s).

2. Secondary structure

Arises from segments of the polypeptide chain repeatedly coiled and folded in patterns because of hydrogen bonding between parts of the polypeptide back bone.

Secondary structure can be:

a) Alpha-helix: cyclindrical coil

b) Beta-sheet: a pleated sheet

c) Random coil: no regular structure

Tertiary structure

Overall shape of the polypeptide resulting from interactions between side chains (R groups) of amino acids.

Quaternary structure

The number and relative positions of polypeptide subunits in a multimeric protein.

Front 180

Explain what is meant by denaturation and list factors that can cause it.

Back 180

Heat, pH extremes, chemicals, electricity, radiation, and by other causes all denature protein, which means enzymes (proteins) become altered.

Front 181

Distinguish between the primary, secondary, tertiary, and quaternary levels of protein organization?

Back 181

There are different levels of protein organization; primary protein structure, secondary protein structure, tertiary protein structure, and quaternary protein structure. Primary protein structure is a chain of a sequence of amino acids. Secondary protein structure occurs when the sequence of amino acids are linked by hydrogen bonds. Secondary is the most common and includes alpha helix and beta pleated sheets. Tertiary protein structure are three dimensional structures that form from globular proteins. The 3D shape comes from interatcions of secondary strucutres. Quaternary protein structure occurs when two or more folded polypeptides in a tertiary structure form a functional protein.