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NURSING 110 > BIOCHEMISTRY 111 > Flashcards

BIOCHEMISTRY 111 Flashcards

Final Exam

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1
Q

Matter

A

something that takes up space (volume) and weighs something (mass)
two types of matter: pure substance and mixtures

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2
Q

Pure Substance

A

matter made up of one type of element represented by one chemical formula
two types of Pure substance: element and compound

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3
Q

Element

A

the simplest form of matter

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4
Q

Compound

A

two or more elements that are chemically joined together

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5
Q

Mixture

A

a combination of two or more substances
two types of mixtures: heterogenous and homogenous

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6
Q

Homogenous Mixture

A

composition is the same throughout

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7
Q

Heterogenous Mixture

A

composition is different throughout

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8
Q

Atom

A

smallest unit of matter that can exist and keep its chemically unique characteristics

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9
Q

Periodic Table of Elements

A

the listing of all the elements found on earth

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10
Q

Chemical Symbol

A

the letters that represent the nam of each element

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11
Q

Group

A

the vertical column of blocks of elements that have similar chemical behaviors (number of valence electrons)

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12
Q

Period

A

the horizontal row of blocks numbered 1-7 with sections 6-7 set apart at bottom (number of energy levels)

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13
Q

Chemical Formula

A

represent compounds and the subscripts tell us how many atoms of the preceding element are present in the compound

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14
Q

4 Elements that make up biological molecules

A

CHON

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15
Q

Physical Change

A

a change int he state of matter but same identity

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16
Q

Chemical Change

A

a change in the chemical’s identity as a whole

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17
Q

Reactants

A

the starting material on the left side of the chemical equation

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18
Q

Products

A

the ending material on the right side of the chemical equation

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19
Q

The Law of conservation of mass

A

matter can not be destroyed or created

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20
Q

Percent

A

part over whole times 100

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21
Q

Mass

A

measure of the amount of material in an object

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22
Q

Weight

A

determined by the pull of gravity of an object

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23
Q

Volume

A

something that takes up or occupies space (1 mL=1cm^3)

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24
Q

Density

A

mass over volume

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25
Q

Temperature

A

the measure of coldness and hotness
OC, 32F,273K-> freezing point
37C,98.6F,310K-> normal body temp.
100C,212F,373K-> boiling point

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26
Q

State of matter

A

physical form in which matter exists

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27
Q

Solid

A

definite shape and volume

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28
Q

Liquid

A

definite volume

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29
Q

Gas

A

no definite volume or shape

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30
Q

Accuracy

A

means that you are taking measurements close to the actual value

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31
Q

Precision

A

means that you report similar in value even if it is not close to the actual value; reproducibility

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32
Q

Subatomic Particles

A

the smallest parts that organize to form atoms

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33
Q

Protons

A

a positively charged subatomic particle (P+)

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34
Q

Neutrons

A

subatomic particle with no charge (n)

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35
Q

Electrons

A

a subatomic particle with a negative charge (e-)

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36
Q

Nucleus

A

the central part of the atom containing protons and neutrons

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37
Q

electric Cloud

A

the area of an atom outside of the nucleus where the electrons can be found

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38
Q

Atomic Mass Unit (AMU)

A

the labels to quantify the mass of very small particles

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39
Q

Mass number

A

is the total number of protons and neutrons in an atom
mass #= protons + neutrons
# electrons = # protons

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40
Q

Atomic Number

A

the number above the symbol of an element that represents # of protons in an element

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41
Q

isotopes

A

two or more atoms of an element with same protons but different number of neutrons

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42
Q

Atomic Mass

A

the weighted average mass of all naturally occurring isotopes of an element

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43
Q

Nuclear Radiation

A

the energy emitted spontaneously from the nucleus of an atom

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44
Q

Radioactive

A

describes an element that spontaneously emit nuclear energy

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45
Q

Radioactive Decay

A

the process of a nucleus spontaneously emitting radiation for an isotope to become stable

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46
Q

How Severe is Radiation

A
  1. exposure
  2. type of radiation
  3. time
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47
Q

Radioisotope

A

a radioactive isotope of an element (unstable)

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48
Q

Alpha Particle

A

a form of nuclear radiation consisting of protons and 2 neutrons, 2+ charge and requires a sheet of paper to be blocked

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49
Q

Beta Particle

A

a form of nuclear radiation consisting of a high energy electron emitted from an unstable neutron, carries a negative charge; is blocked by heavy clothing and aluminum foil. (neutron-> proton)

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50
Q

Gamma Rays

A

high energy nuclear radiation emitted to stabilize radioactive nucleus, neither a charge or mass of the radioisotope will change; needs a concrete wall to be stopped or lead apron

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51
Q

Positron

A

a form of nuclear radiation having the same mass as beta particle but with a positive charge (proton-> neutron)

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52
Q

Neutron

A

has no charge, but has weight

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53
Q

Ionizing Radiation

A

a general name for high energy radiation of any kind (bad kind)

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54
Q

Nucelar Decay Equation

A

an equation where the reactant is the radioactive isotope and the products include the new isotope and an ionizing emission particle

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55
Q

Half Life

A

the time it takes for half of the atoms in a radioactive sample to decay
remaining material= original amount x (1/2)^n

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56
Q

Energy Levels

A

in atoms, the electrons can only occupy certain energy levels
electrons must fill lowest energy level first
2n^2= total number of electrons in each energy level
elements in the same group on the periodic table have the same number of electrons in their highest energy level

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57
Q

Valence Electrons

A

electrons found in the highest occupied energy level, the furthest electrons from the nucleus and are the electrons that combine when elements make compounds

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58
Q

Noble Gases

A

the group 8A(18) elements, satisfy the octet rule; elements are unreactive, thus stable

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59
Q

Octect Rule

A

the tendency of atoms to react with other atoms to obtain eight total electrons in their outershell

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60
Q

Ion

A

an atom with a charge due to an unequal number of protons and electrons

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61
Q

Anions

A

an ion with a negative charge; formed when electrons are gained

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62
Q

Cations

A

an ion with a positive charge; formed when electrons are lost

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63
Q

Polyatomic Ions

A

a group of atoms that interact to form an atom
1. hydroxide- OH^-
2.Sulfate- SO4^2-
3.Carbonate- CO3^2-
4. Nitrate- NO3^-
5.Ammonium- NH4^+
6.Phosphate- PO4^3-
7.Bicarbonate- HCO3^-

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64
Q

Ionic Bond

A

the strong attraction between an anion and cation

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65
Q

Ionic Compound

A

the result of two or more ions attracted by ionic bonds to form electrically neutral species

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66
Q

Covalent Bond

A

the result of atoms sharing electrons to achieve an octet in their valence shell (nonmetals)

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67
Q

Covalent Compound

A

a type of compound made up of atoms held together by covalent bond

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68
Q

Molecule

A

the smallest unit of a covalent bond formed when two or more nonmetal atoms are joined

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69
Q

Lewis Dot Structure

A

shows how atoms share electrons in covalent bonding, the electron dot symbol for any atom consists of the elemental symbol plus a dot for each electron

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70
Q

Bonding Pair

A

a pair of electrons shared by two atoms to form a covalent bond and is represented as a dash or line connecting the two electron dot symbols

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71
Q

Lone Pairs

A

a pair of electrons belonging to only one atom

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72
Q

Single Bond

A

a covalent bond formed when two atoms share one pair of electrons

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73
Q

double bond

A

sharing two of its electrons with one atom

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74
Q

Triple bond

A

covalent bonds formed when two atoms share three pairs of electrons

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75
Q

Molecular Formula

A

the chemical formula of a molecular compound

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76
Q

binary compounds

A

a compound that is composed of only two elements

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77
Q

Mole

A

unit to count small objects like atoms

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78
Q

Molar Mass

A

the mass in grams of one mole of a substance for an element

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79
Q

Avogadro’s Number

A

the number of particles, molecules, atoms in one mole
6.02x10^23 atoms= 1 mole

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80
Q

Tetrahedral

A

molecular shape with four atoms arranged around a central atom to give an atom an angle of 109.5 degrees

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81
Q

Linear

A

gives an atom an angle of 180 degrees

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82
Q

Bent

A

gives an atom an angle of 104.5 degrees

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83
Q

Pyramidal

A

gives an atom an angle of 107 degrees

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84
Q

Triangular planar

A

gives an atom an angle of 120 degrees

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85
Q

Valence Shell Electron Pair Repulsion Theory

A

determining molecular shape based on repulsion of groups of electrons in valence shell of central atom

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86
Q

electronegativity

A

a measure of the ability for an atom in a covalent bond to attract the bonding electrons

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87
Q

Polar Covalent Bond

A

bond where electrons are strongly attracted to one atom

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88
Q

Non Polar Covalent Bond

A

sharing equally by two atoms

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89
Q

Organic Compounds

A

compounds mainly composed of carbon and hydrogen

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90
Q

Biomolecules

A

the molecules of life including carbohydrates, lipids, nucleic acids, and proteins

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91
Q

Inorganic Compounds

A

compounds composed of elements other than carbon and hydrogen

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92
Q

Condensed Structural Formula

A

the arrangement of the carbons and hydrogens are expanded but bonds are not shown; the atoms are listed left to right in order to which they are connected

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93
Q

Molecular Formula

A

shows only the number of each atom in the molecule

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94
Q

Lewis Structure

A

shows the molecules complete connectivity, all atoms and bonds

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95
Q

Skeletal Structure

A

representation of organic compound that shows only the bonding of carbon framework; carbon atom understand to exist at a corned where two lines meet or at end of a line segment if no other element is present

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96
Q

Alkanes

A

a family of organic compounds whose composed of only single bonded carbons and hydrogens (saturated)
nonpolar because the electronegativity of carbon and hydrogen are so similar that the two elements form covalent bonds in which the electrons are shared equally

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97
Q

Straight Chain Alkanes

A

alkanes that have their carbon atoms connected in a single continuous chain

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98
Q

Cycloalkanes

A

hydrocarbons containing a ring of carbon atoms; folding back on itself if it contains one less carbon

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99
Q

Heteratom

A

atoms in an organic compound other than carbon and hydrogen

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100
Q

Alkane Names:

A
  1. Methane
  2. Ethane
  3. propane
  4. butane
  5. pentane
    6, hexane
    7, heptane
  6. octane
  7. nonane
  8. decane
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101
Q

Alkenes

A

(unsaturated) a family of organic compounds whose composed of one double bond; its no longer surrounded by hydrogen atoms
double bond between carbon atoms are shorter and stronger than single bonds

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102
Q

Alkynes

A

(unsaturated) a family of organic compounds whose functional group composed of triple bonds

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103
Q

Aromatics

A

(unsaturated) a family of cylic organic compounds whose functional group is a benzene ring, six membered ring with alternating double bonds

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104
Q

Saturated Hydrocarbons

A

organic compounds containing only carbons and hydrogen in which each carbon is bonded to the maximum number of hydrogen atoms (CnH2n+2)

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105
Q

Unsaturated Hydrocarbons

A

compounds composed of carbon and hydrogen atoms with one or more double or triple bonds (CnH2n or CnH2n-2)

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106
Q

Functional Group

A

similar group between organic structures that react in similar ways because they have similar functions

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107
Q

Fatty Acids

A

long alkane like hydrocarbon chains bounded to carboxyl group, non polar

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108
Q

Saturated Fatty Acid

A

do not contain double bonds (unhealthy)

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109
Q

Unsaturated Fatty Acid

A

do contain double bonds (healthy)

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110
Q

Branched Chain Alkanes

A

alkanes that have one chain of carbon atoms, the shorted chains are considered branches from the main, longer chain

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111
Q

Isomers

A

a compound with same molecular formula as another but a different arrangement

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112
Q

Structural Isomer

A

same molecular formula but different connectivity of atoms (different names)

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113
Q

Conformational Isomer

A

Same molecular formula with alters only by rotation, about one or more bonds (same name)

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114
Q

Stereoisomer

A

same connectivity but not superimposable

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115
Q

Chiral Center

A

carbon has 4 single bonds with different groups

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116
Q

Enantiomer

A

compounds containing at least one chiral center that are non-superimposable mirror image (rotate everything)

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117
Q

Cis Trans

A

same side or different side; double bonds prevent carbon from rotating

118
Q

Omega Number

A

Number specifies the position of the first double bond in a fatty acid chain when counting from methyl end
[#C:#DB], w-x

119
Q

Carbohydrate

A

simple or complex sugar composed of carbon, oxygen, and hydrogen (Cn(H2O)n)

120
Q

Monosaccharide

A

simple sugar unit containing three or more carbons
glucose galactose, mannose

121
Q

Dissacharides

A

a carbohydrate composed of two monosaccharides joined through glycosidic bond
sucrose, maltose, lactose

122
Q

Oligosaccharides

A

carbohydrates composed of three to nine monosaccharides joined by glycosidic bond

123
Q

Polysaccarides

A

a carbohydrate composed of many monosaccharides in a continuous chain or branched chain
starch, chitin, cellulose

124
Q

Glucose

A

(monosaccharides) can be broken inside the cells to produce energy

125
Q

Galactose

A

(monosaccharides) that combines with glucose to form lactose

126
Q

Mannose

A

(monosaccharides) found in some veg and fruits; not so easily digested

127
Q

Maltose

A

(disaccharides) two glucose units with glycosidic bond alpa (1-4)

128
Q

Lactose

A

(disaccharides) glucose and galactose units with glycosidic bond at beta (1-4)

129
Q

Sucrose

A

(disaccharide) glucose and fructose with glycosidic bond at beta (1-2)

130
Q

Aldehyde

A

a family of organic compounds whose functional group is a carbonyl bonded t at least one hydrogen

131
Q

Aldose

A

monosaccharide that contains an aldehyde functional group

132
Q

Alcohol

A

a fucntional group of organic molecules whose functional group is -OH; very polar

133
Q

Primary Alcohol

A

has only one alkyl group bonded to the carbon with -OH

134
Q

Secondary Alcohol

A

has two alkyl groups bonded to the carbon with -OH

135
Q

Tertiary Alcohol

A

has three alkyl groups bonded between the carbon with -OH

136
Q

Cellulose

A

(structural polysaccharides) beta D-glucose with beta (1-4) glycosidic bond

137
Q

Chitin

A

(structural Polysaccharides) beta D-acetylglucosamine with beta (1-4) glycosidic bond

138
Q

Amylose

A

(storage polysaccharides) alpha D-glucose with alpha (1-4) glycosidic bond

139
Q

Amylopectin

A

(storage polysaccharides) alpha (1-4) and alpha (1-6)

140
Q

Glycogen

A

(storage polysaccharides) alpha (1-4) and alpha (1-6)

141
Q

Keytone

A

a family of organic compounds whose functional group is a carbonyl bonded to at least two alkyl groups

142
Q

Ketose

A

monosaccharide that contains a ketone functional group

143
Q

Fischer Projection

A

horizontal line on a chiral center represents wedges and vertical lines on a chiral center center represent dashes; a chiral center is represented as intersection of lines
left is up and right is down

144
Q

D-Sugars

A

an enantiomer whose configuration is based on the arrangement of the attachments on D-glyceraldheyde, -OH is on the right side

145
Q

L-Sugars

A

an enantiomer whose configuration is based on the arrangements of the attachment on L-glyceraldhyde, -OH is on the left side

146
Q

Epimer

A

molecules where only one chiral center is changed

147
Q

Divasteriomers

A

are only stereisomers that are not mirror image

148
Q

Enantiomers

A

are pairs f molecules that are mirror images (just switch each chiral enter)

149
Q

Hemiacetal

A

the functional group formed when an alcohol and aldehyde group combine to form a Haworth Structure

150
Q

Anomer

A

sugar diasteromers differing only in the position of the hydroxyl at the anomeric carbon

151
Q

Anomeric Carbon

A

refers to the carbon that reacts to form the hemiocetal in any monosaccharide

152
Q

Pyranose

A

six membered ring form of monosaccharide that contains 5 carbon and one oxygen atom in the ring

153
Q

Furanose

A

five membered ring

154
Q

Reducing sugar

A

a carbohydrate with a free aldehyde group capable of reducing another substance

155
Q

Glycosidic Bond

A

formed when two hydroxyl groups join, one of which is on an anomeric carbon of a monosaccharide and the other is part of the second monosaccharide to form a disaccharide; H2O is produced

156
Q

Alpha Glycosidic bond

A

anomeric carbon to the oxygen of another monosaccharide is point downwards

157
Q

Beta Glycosidic Bond

A

upwards, same direction as the CH2OH

158
Q

Oxidation

A

losing electrons thus hydrogen and gaining oxygen

159
Q

reduction

A

gaining electrons thus hydrogen and losing oxygen

160
Q

Change of State

A

the change that occurs when a substance that exists in one state of matter becomes another state of matter

161
Q

Melting Point

A

the temperature at which molecules move from the solid to the liquid phase
stronger and more numerous forces between molecules = higher melting point. The longer the structure, the more they can pack thus have a high melting point. Unsaturated fats have lower melting points. cid double bond lowers melting point to 60 degrees in Oleic Acid

162
Q

Boiling Point

A

the temperature at which the molecules of a substance change from liquid to gas

163
Q

Attractive Forces

A

an attraction of opposite charges between molecules, strongly affect properties of solid and liquids

164
Q

London Forces

A

the weakest attractive forces, all compounds exhibit London forces

165
Q

Dipole Dipole attraction

A

attraction partially positive end of one polar molecule to a partially negative end of a second polar molecule

166
Q

Hydrogen Bonding

A

strong dipole dipole interaction of hydrogen atoms covalently bonded to O,N,F

167
Q

Ion Dipole Attractions

A

electrical attraction between an ion and a polar molecule

168
Q

Ionic Attractions

A

stronger than hydrogen bonding, an attraction between a + and - to form a salt

169
Q

Lipids

A

fatty acids that have a hydrophobic and hydrophilic region

170
Q

Oil

A

liquid at room temperature; low boiling point and can not get close because of cis double bonds

171
Q

Fat

A

solid at room temperature; high boiling point

172
Q

Amphipathic Compounds

A

have polar and nonpolar sections in one molecule

173
Q

Micelles

A

spherical structures that allow ion dipole interaction while non polar trails associate with each other

174
Q

Solution

A

a homogenous mixture where particles are dispersed individually and evenly throughout

175
Q

Solute

A

the solute is a substance in a solution present in the smaller amount

176
Q

Solvent

A

the substance in a solution present in the larger amount ; only one solvent in a solution

177
Q

Properties of Solutions

A
  1. particles are evenly distributed
  2. components do not chemically react with each other
  3. aqueous solutions are transparent
  4. components do not separate upon standing
  5. concentration can be changed
178
Q

Colloid

A

has smaller particles that do not separate; they stay mixed together

179
Q

Suspension

A

a mixture containing particles greater than 100nm in diameter; separate upon standing

180
Q

solubility

A

defined as the maximum amount of solute that will dissolve in solvent; depends on temperature and polarity of solute
temperature rises= increase solid solubility
temperature rises= decrease gas solubility

181
Q

Unsaturated Solution

A

a solution containing less than the maximum amount of solute capable of dissolving

182
Q

Saturated Solution

A

a solution containing the maximum amount of solute capable of dissolving in the solution at given temp

183
Q

Henry’s Law

A

as pressure goes up the solubility of gas in water also goes up. the amount of gas that can dissolve in a liquid increases as pressure of gas in the space above the liquid increases

184
Q

Electrolyte

A

a substance that conducts electricity because it dissociates into ions in aqueous solution

185
Q

Strong Electrolyte

A

is ionic compound dissolve in water it will completely dissociate

186
Q

Non-Electrolyte

A

a substance that doe not conduct electricity because it does not ionize in aqueous solution

187
Q

Weak Electrolyte

A

a substance that weakly conducts electricity because it partially ionizes in aqueous solutions covalent bonded compounds specifically carboxylic acid and amines

188
Q

Equivalent

A

a unit of concentration that relates the change in a solution of the number of ions or the moles of ions present in the solution
Na+= 1 Eq/1 mol
Ca2+=2Eq/1 mol

189
Q

Concentration

A

The amount of solute dissolved in a certain amount of solution
= amount of solute (g)/ amount of solution (mL)

190
Q

Molarity

A

a unit of concentration defined as the number of moles of solute dissolved per liter of solution
=moles of solute/Liters of solution

191
Q

percent concentration

A

number of parts out of the whole times 100
part solute/part solution times 100

192
Q

Percent Mass

A

mass of solute and mass of solvent
g solute/g solution times 100

193
Q

Percent mass Volume

A

g solute/mL solution times 100

194
Q

Dilution

A

changing the concentration
Ci x Vi=Cf x Vf
Vf/Vi= solution dilution factor

195
Q

Acid

A

a substance that dissolves in water and produces hydrogen ions (H+), according to the Arrhenius Theory. All acids are proton donors, according to the Bronsted Lowry Theory

196
Q

Bases

A

a substance that dissolves in water and produces hydroxide ions, according to Arrhenius Theory. All bases are proton acceptors according to Bronsted-Lowry Theory

197
Q

Strong Acids

A

an acid that completely ionizes in water, which means they break up completely into ions when placed in water, forming hydronium ions and anions

198
Q

Weak Acids

A

an acid that ionizes only slightly in solution

199
Q

Strong Bases

A

a base that completely ionizes in water because they are ionic compounds which dissociate in water to give aqueous solution containing a metal ion and a hydroxide ion

200
Q

Weak Bases

A

a base that ionizes only slightly in solution

201
Q

Acidic

A

a term that describes an aqueous solution in which the concentration of Hydronium ions is greater than the concentration of hydroxide ions
PH<7 [H+] increases

202
Q

Basic

A

a term that describes an aqueous solution in which the concentration of Hydronium ions is less than the concentration of hydroxide ions
PH>7 [H+] decreases

203
Q

Salt

A

an ionic compound containing a metal or a polyatomic ion as the cation and a nonmetal or plyatomic ion as an anion

204
Q

neutralization

A

the reaction between an acid and base (strong) to form salt and water

205
Q

Chemical Equilibrium

A

a state in a reversible chemical reaction where both the forward and reverse reactions are occurring at the same rate

206
Q

Equilibrium Constant

A

(k) a constant that is equal to the ration of concentration of products to reactants at equilibrium
k= [products]/[reactants]
k= [c]^c[D]^d/[A]^a[B]^b
solids and liquids are not included

207
Q

La Chatelier’s Principle

A

a chemical reaction that has been distributed from equilibrium will shift its equilibrium to offset the disturbance

208
Q

Acid Dissociation Constant

A

(ka) a constant that establishes the ratio of products to reactants for a weak acid at equilibrium
larger Ka value=stronger acid

209
Q

Conjugate Base

A

the product after an acid donates a proton in reverse reaction

210
Q

Conjugate Acid

A

the product after a base accepts a proton in the reverse reaction

211
Q

Auto-ionization of Water

A

spontaneous reaction of two water molecules to form hydronium and hydroxide

212
Q

Neutral PH

A

term that describes a solution with equal concentrations of H+ and OH-
PH=-log [H3O+]
10^-PH=[H3O+]

213
Q

Pka

A

a measure of the acidity of a weak acid
stronger acid= lower pka
PKa= -log [ka]
10^-PKa=[Ka]

214
Q

Henderson-Hasselbalch Equation

A

a modified form of the equilibrium constant expression useful for determining the ratio of conjugate base to acid at a give PH
PH=PKa+log [conjugate base]/[acid]
10^PH-PKa=[conjugate base]/[acid]
PH=PKa equilibrium
Ph>PKa conjugate base
PH<PKa acid

215
Q

Buffers

A

a solution containing a weak acid and its conjugate base or weak base and its conjugate acid that resists the change in PH when acids and bases are added

216
Q

Bicarbonate Buffer System

A

CO3+H2O-><-HCO3-+H30+

217
Q

Respiratory Acidiosis

A

blood PH is lower than 7.35 caused by change in breathing patterns; CO2 build up thus it shifts right due to hypoventilation

218
Q

Respiratory Alkalosis

A

when blood PH is too high due to hyperventilation; exhaling too much CO2 thus shifting left. The ph is too basic

219
Q

Metabolic Acidosis

A

excess acid is added to the bloodstream due to chemical reactions in the body, treatment includes administering bicarbonate which will increase PH

220
Q

Metabolic Alkalosis

A

indicates chemical reactions within the body caused by alkalization of the body; treatment includes breathing into paper bag which will increase CO2 level which will then increase H3O+ ions by shifting equilibrium to the right and lowering PH

221
Q

Alpha Carbon

A

the carbon in amino acids that is bonded to the carboxylate ion, the pronated amine, a hydrogen atom, and side chain R group (chiral center)

222
Q

Alpha Amino Group

A

the pronated Amine bonded to the alpha carbon in an amino acid

222
Q

Alpha carboxylate group

A

the carboxylate ion bonded to the alpha carbon in an amino acid

223
Q

Zwitteron ion

A

the ionic form of amino acid that has both a positive and negative charged groups

223
Q

Enantiomers

A

compounds that contain a single chiral center that can be in two forms
L-amino acid (pronated amine is on the left side)
R-amino acid (pronated amine is on the right side)

223
Q

peptide bond

A

an amide bond that joins two amino acids

224
Q

C Terminus

A

in peptide, the amino acid with the free carboxylate ion

225
Q

N terminus

A

in peptide bond, amino acid with the free left pronated amine

226
Q

Amide

A

a family of organic compounds characterized by a functional group containing a carbonyl bonded to a nitrogen atom

227
Q

Primary Structure

A

the order of the amino acids bonded by peptide bonds forming a polypeptide chain

228
Q

secondary structure

A

regularly repeating patterns of structure within the overall 3D structure of the protein stabilized by hydrogen bonding along protein backbone

229
Q

Alpha Helix

A

right handed coiled spring

230
Q

Beta Pleated Sheets

A

zig zag; fan structured

231
Q

Tertiary Strucutre

A

the folding through R groups associated with intermolecular forces between R groups

232
Q

Quaternary Structure

A

the binding of two or more polypeptide chains to form a biologically active protein

233
Q

Denaturation

A

a prcoess that disrutps the stabilizing attractive forces

234
Q

enzymes

A

act as catalyst compounds that accelerate the reactions of metabolism but are not consumed or changed by the reactions (tertiary structure)

235
Q

Proximity

A

enzyme brings together all the necessary components for a reaction to occur faster

236
Q

Orientation

A

the active site brings those components together in a particular way

237
Q

Bond Strength

A

weak substrate substances bonds which breaks faster

238
Q

Active Site

A

Formed during tertiary structure, a pocket lined with amino acids for substrate to bind

239
Q

Lock and Key Model

A

a model describing the initial interaction of an enzyme with its substrate; each enzymes has only one substrate with a shape complementary to the active site of the enzyme; fit together without changing shape

240
Q

Induced fit model

A

model describing the initial interaction of an enzyme to its substrate; an enzymes active site and its substrate have flexible shape that are roughly complementary and adjust to allow the formation of ES

241
Q

Cofactors

A

inorganic substances necessary for the function of some enzymes (minerals)

242
Q

coenzymes

A

organic substances necessary for funtion of some enzymes; vitamins

243
Q

Inhibitor

A

a molecule that causes an enzyme catalytic activity to decline

244
Q

Reversible inhibitor

A

the lowering of enzyme catalytic activity caused by competitive or noncompetitive inhibitor that can be reversed

245
Q

competitive

A

a molecule structurally similar to the substrate that composes for the active site

246
Q

noncompetitive

A

a molecule that inhibits an enzyme catalytic activity by interacting with a site other than the active site; resulting in the distortion if the enzyme shape

247
Q

Irreversible Inhibitor

A

the permeant loss of enzyme activity

248
Q

Ribose

A

oxygen on carbon 2 of pentose

249
Q

Deoxyribose

A

no oxygen on carbon 2 of pentose

250
Q

Nucleotide

A

a pentose sugar condensed with one of five of the nitrogenous bases at carbon 1 and up to three phosphates on C3

251
Q

Nucleoside

A

a pentose sugar condensed with one of the five nitrogenous bases at carbon 1

252
Q

Complementary Base Pair

A

adenine=thymine adenine=uracil guanine=cytosine

253
Q

Purine

A

adenine and guanine

254
Q

Pyriminine

A

cytosine, uracil, thymine

255
Q

Nucleic Acids

A

large molecules composed of nucleotides found in cells as double stranded helical DNA and single stand RNA

256
Q

Phosphodiester Bonds

A

bond linkage adjacent nucleotides in a nucleic acid; this bond connects the 3 prime end OH with phosphate linked on C5

257
Q

Transcription

A

the transfer of gene copt from DNA to RNA via RNA polymerase to create mRNA

258
Q

Translation

A

reading of codons on mRNA to construct amino acid chain via tRNA and rRNA

259
Q

5 prime end

A

phospate

260
Q

3 prime end

A

hydroxyl on third carbon

261
Q

Metabolism

A

sum of all the chemical processes that occur within a living organism in order to maintain life

262
Q

Catabolism

A

metabolic chemical reactions in which larger molecules are broken down into smaller ones. these reactions tend to be oxidative and produce energy (exergonic -delta G); hydrolysis

263
Q

Anabolism

A

metabolic chemical reactions in which smaller molecules are combined to form larger ones, these reactions tend to be reductive and require energy (endergonic + delta G); condensation

264
Q

Mitochondria

A

cell organelle where energy producing reactions take place

265
Q

ATP

A

Energy currency of the cell, undergoes hydrolysis to ADP

266
Q

Digestion

A

the breaking down of large molecules into smaller components for absorption, usually through hydrolysis starting from the saliva and all the way to the small intestine

267
Q

Emulsification

A

the breaking down of large insoluble globes into smaller droplets via an ampiphatic molecule

268
Q

Nutrition label conversion

A

protein-> 4 per gram
carb-> 4 per gram
fat -> 9 per gram
alcohol-> 7 per gram

269
Q

Gbuconeogensis

A

the anabolic process of synthesizing glucose

270
Q

Glycolysis

A

a process in which glucose is partially broken down by cells in enzyme reactions that do not need oxygen (10 reactions) that occur in cytoplasm
glucose+2 NAD+2ADP+2Pi->2 pyruvate +2ATP+2NADH+2H+

271
Q

Aerobic

A

when ample oxygen is present, pyruvate is oxidized further into acetyl coenzyme A

272
Q

Pyruvate Decarboxylation (link reaction)

A

is the conversion of pyruvate to acetyl COA by the enzyme complex pyruvate dehydrogenase complex
2 Pyruvate+2NAD+2COA->2 Acetly COA+2NADH+2CO2

273
Q

Anaerobic

A

when oxygen is in short supply, pyruvate is reduced to lactate. produces NAD+ cycles back into glycolysis to oxidize more G3P allowing production of more ATP

274
Q

Fermentation

A

anaerobic production of ethanol from pyruvate in yeast

275
Q

Oxidative Decarboxylation

A

an oxidation in which a carboxylate is released as a CO2

276
Q

Citric Acid Cycle

A

a series of reactions that degrades two carbon acetyl groups from acetyl cOA into CO2, generating high energy molecules in the process like NADH and FADH2
2 Acetyl COA+6NAH+2ADP+2Pi+2FADH-> 4 CO2+6 NADH+2FADH2+ATP+6H+

277
Q

Electron transport train

A

(inner mitochondrial membrane) electrons are passed from one molecule to another and energy released in these electrons transfers to form an electrical chemical gradient (4 complexes)
32 total ATP created

278
Q

Electrochemical Gradient

A

a difference in both concentration and electrical charge of an ion across a membrane, driving force of oxidative phosphorylation (the creation of ATP)

279
Q

Chemiosmotic Model

A

the conservation of energy from the transfer of electrons int eh ETC by pumping H+ into the inter membrane space to produce a H+ gradient that produces the energy to synthesize ATP

280
Q

Conversions of NADH and FADH2

A

2.5 ATP=1 NADH
1.5 ATP=1 FADH2

281
Q

Beta Oxidation

A

(mitochondrial matrix) the degradation of fatty acids by removing two carbon segments from a fatty acid at the oxidized carbon
count carbons and divide by two=acetyl coa molecules
10x number of acetyl coa molecules
#acetyl Coa molecules-1=cycles of beta oxidation

282
Q

Isomerization

A

the process where the reactant and product differ in structure while the molecular formula remains the same

283
Q

Phosphorylation

A

the process of adding a phosphate group, often indicated by prefix “phosphate” or “phospho”

284
Q

Phosphate transfer

A

process of transferring of a phosphate group (ADP to ATP)

285
Q

fructose vs glucose

A

in the liver, fructose is enzymatically converted to G3P and enters glycolysis at step 5, after all the regulation steps, all fructose in the cell will be converted to pyruvate
Fructose that is metabolized in the muscle enters the glycolysis as fructose 6 phosphate and is enzymatically regulated. fructose that is not metabolized in muscle is metabolized in the liver to yield pyruvate and acetyl COA, an excess of which would be stored as fat

286
Q

Bile salts

A

emulsify fats by breaking larger fat globules into smaller ones for internal absorption

287
Q

Digestion of Starch

A

glucose galactose and fructose

288
Q

Where does digestion take place?

A

starch undergoes digestion in the mouth
no carbohydrates are digested in stomach
disaccharides and oligosaccharides are digested in small intestine

289
Q
A

NURSING 110 (3 decks)

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