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A&P 1 Summer 2023 > A&P Chapter 2 > Flashcards

A&P Chapter 2 Flashcards

1
Q

The body is made up of many ______

A

Chemicals

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2
Q

Chemistry underlies all ______ reactions

A

Physiological

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3
Q

What are some examples of physiological reactions?

A

Movement, digestion, pumping of the heart, and nervous system

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4
Q

Chemistry can be broken down into what two categories?

A
  1. Basic chemistry
  2. Biochemistry
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5
Q

What is matter?

A

Anything that has mass and occupies space

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6
Q

Matter can be:
1. _______
2. _______
and/or
3. _______

A

Seen, smelled, felt

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7
Q

Weight is _____ + the effects of what?

A

Mass + the effects of gravity

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8
Q

What are the three possible states that matter can exist in?

A
  1. Solid
  2. Liquid
  3. Gas
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9
Q

What are characteristics of a solid?

A

Definite shape and volume

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10
Q

What are characteristics of a liquid?

A

Changeable shape; definite volume

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11
Q

What are characteristics of a gas?

A

Changeable shape and volume

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12
Q

What is energy?

A

The capacity to do work or put matter into motion

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13
Q

What are the two possible forms of energy?

A

Kinetic and potential

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14
Q

What is kinetic energy?

A

Energy in action

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15
Q

What is potential energy?

A

Stored (inactive) energy

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16
Q

Energy can be transformed from ______ —> what?

A

Potential —> kinetic energy

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17
Q

Stored energy can be ______, resulting in action

A

Released

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18
Q

All matter is composed of what?

A

Elements

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19
Q

4 elements make up what percentage of the body and what are they?

A

96% of the body is made up of carbon, oxygen, hydrogen, and nitrogen

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20
Q

9 elements make up how much of the body?

A

3.9%

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21
Q

11 elements make up how much of the body?

A

<0.01%

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22
Q

The periodic table lists what elements?

A

All known

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23
Q

What are all elements made up of?

A

Atoms

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24
Q

What are atoms?

A
  1. Unique building blocks for each element
  2. Smallest particles of an element with properties of that element
  3. What gives each element its particular physical and chemical properties
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25
Q

What is an atomic symbol?

A

One or two letter chemical shorthand for each element

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26
Q

What is an example of an atomic symbol?

A

O for oxygen

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27
Q

What is another example of an atomic symbol?

A

C for carbon

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28
Q

How are atomic symbols determined?

A

Some symbols come from Latin names

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29
Q

What is an example of an atomic symbol being named after latin names?

A

Na = Sodium (Natrium)

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30
Q

What is another example of an atomic symbol being named after latin names?

A

K = Potassium (Kalium)

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31
Q

What is the atomic symbol for oxygen?

A

O

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32
Q

What is the approximate percentage of body mass that oxygen makes up?

A

65%

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33
Q

What is the function of oxygen in the body?

A

A component of both organic and inorganic molecules. As a gas, it is needed for the production of cellular energy (ATP)

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34
Q

What is the difference between organic and inorganic molecules?

A

Organic = Carbon containing
Inorganic = Non-carbon containing

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35
Q

What is the atomic symbol for carbon?

A

C

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36
Q

What is the approximate percentage of body mass does carbon make up?

A

18.5%

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37
Q

What is the function of carbon in the body?

A

A component of all organic molecules, which include carbohydrates, lipids, proteins, and nucleic acids

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38
Q

What are lipids?

A

Fats and oils

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39
Q

What is the atomic symbol for hydrogen?

A

H

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40
Q

What is the approximate percentage of body mass does hydrogen make up?

A

9.5%

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41
Q

What is the function of hydrogen in the body?

A

A component of all organic molecules. As an ion (proton), it influences the pH of body fluids

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42
Q

What is the atomic symbol for nitrogen?

A

N

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43
Q

What is the approximate percentage of body mass does nitrogen make up?

A

3.2%

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44
Q

What is the function of nitrogen in the body?

A

A component of proteins and nucleic acids

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45
Q

What is the atomic symbol for calcium?

A

Ca

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46
Q

What is the approximate percentage of body mass that calcium makes up?

A

1.5%

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47
Q

What is the function of calcium in the body?

A

Found as a salt in bones and teeth. It’s ionic form is required for muscle contraction, conduction of nerve impulses, and blood clotting.

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48
Q

What is the ionic form of calcium?

A

Ca2+

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49
Q

What is the atomic symbol for phosphorus?

A

P

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50
Q

What is the approximate percentage of body mass that phosphorus makes up?

A

1%

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51
Q

What is the function of phosphorus in the body?

A

Part of calcium phosphate salts in bones and teeth. Also present in nucleic acids, and as a part of ATP and phospholipids

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52
Q

What is the atomic symbol for potassium?

A

K

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53
Q

What is the approximate percentage of body mass does potassium make up?

A

0.4%

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54
Q

What is the function of potassium in the body?

A

Its ion is the major positive ion in cells. Necessary for conduction of nerve impulses and muscle contraction

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55
Q

What is a positive ion called?

A

Cation

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56
Q

What is a potassium ion?

A

K+

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57
Q

What is the atomic symbol for sulfur?

A

S

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58
Q

What is the approximate percentage of body mass that sulfur makes up?

A

0.3%

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59
Q

What is the function of sulfur in the body?

A

Components of proteins, particularly muscle proteins

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60
Q

What is the atomic symbol for sodium?

A

Na

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61
Q

What is the approximate percentage of body mass that sodium makes up?

A

0.2%

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62
Q

What is the function of sodium in the body?

A

As an ion, sodium is the major positive ion found in extracellular fluids. Important for water balance, conduction of nerve impulses, and muscle contraction

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63
Q

What is a sodium ion?

A

Na+

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64
Q

What is extracellular fluid?

A

Fluid outside the cell

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65
Q

What is the atomic symbol for chlorine?

A

Cl

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66
Q

What is the approximate percentage of body mass that chlorine makes up?

A

0.2%

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67
Q

What is the function of chlorine in the body?

A

Its ion is the most abundant negative ion in extracellular fluids

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68
Q

What is a negative ion called?

A

Anion

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69
Q

What is a chlorine ion?

A

Chloride, Cl-

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70
Q

What is the atomic symbol for magnesium?

A

Mg

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71
Q

What is the approximate percentage of body mass that magnesium makes up?

A

0.1%

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72
Q

What is the function of magnesium in the body?

A

Present in bone. Also an important cofactor in a number of metabolic reactions

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73
Q

What is the atomic symbol of iodine?

A

I

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74
Q

What is the approximate percentage of body mass that iodine makes up?

A

0.1%

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75
Q

What is the function of iodine in the body?

A

Needed to make functional thyroid hormones

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76
Q

What is the atomic symbol for iron?

A

Fe

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77
Q

What is the approximate percentage of body mass that iron makes up?

A

0.1%

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78
Q

What is the function of iron in the body?

A

Component of hemoglobin and some enzymes

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79
Q

What does hemoglobin do?

A

Transports oxygen within red blood cells

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80
Q

Atoms are composed of 3 subatomic particles, what are they?

A
  1. Protons
  2. Neutrons
  3. Electrons
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81
Q

What do protons carry?

A

A positive charge (+)

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82
Q

How much does a proton weigh?

A

An arbitrary 1 atomic mass unit (1 amu)

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83
Q

What do neutrons carry?

A

No electrical charge (0)

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84
Q

How much does a neutron weigh?

A

1 amu

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85
Q

What do electrons carry?

A

A negative charge (-)

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86
Q

How much does an electron weigh?

A

Virtually nothing because they are so small (0 amu)

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87
Q

The orbital model represents electrons as what?

A

A cloud of negative charge

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88
Q

The more simplified planetary model shows electrons as what?

A

Two small spheres on a circle around the nucleus

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89
Q

Different elements contain different numbers of what?

A

Subatomic particles

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90
Q

Hydrogen has _ proton, _ neutrons and _ electron

A

1 proton, 0 neutrons, 1 electron

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91
Q

Helium has _ protons, _ neutrons, and _ electrons

A

2 protons, 2 neutrons, 2 electrons

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92
Q

Lithium has _ protons, _ neutrons, and _ electrons

A

3 protons, 4 neutrons, and 3 electrons

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93
Q

How can you identify elements?

A

Atomic number and mass number

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94
Q

How is the atomic number determined?

A

Number of protons in the nucleus

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95
Q

How is an atomic number written?

A

As a subscript to the left of the atomic symbol (think denominator)

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96
Q

How is the mass number determined?

A

Total number of protons and neutrons in the nucleus, aka total mass of the atom

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97
Q

How is the mass number written?

A

As a superscript to the left of atomic symbol (think numerator)

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98
Q

What are isotopes?

A

Structural variations of the same element

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99
Q

Atoms contain the same number of _____ but differ in the number of _____ they contain

A

Same number of protons but differ in the number of neutrons they contain

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100
Q

So, in isotopes, atomic numbers are _____, but mass numbers are ______

A

Atomic numbers are the same, but mass numbers are different

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101
Q

What is an atomic weight?

A

Average of mass numbers of all isotope forms of an atom

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102
Q

What are radioisotopes?

A

Isotopes that decompose to more stable forms

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103
Q

In radioisotopes, the atom loses what?

A

Varius subatomic particles

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104
Q

When an atom loses subatomic particles, such as in radioisotopes, what can happen to the isotope?

A

Can become a different element

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105
Q

What is radioactivity?

A

As the isotope decays, subatomic particles that are being given off release a little energy. The energy is called radioactivity

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106
Q

What can radioactivity do?

A

Damage living tissue to cause or treat cancer

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107
Q

Radioactivity can be detected and measured by what?

A

Scanners

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108
Q

Most atoms chemically combine with other atoms to form ______ and _______

A

Molecules and compounds

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109
Q

What is a molecule?

A

General term for 2 or more atoms bonded together

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110
Q

What is a compound?

A

Specific molecule that has 2 or more different kinds of atoms bottom together

111
Q

What is an example of a compound?

A

C6H1206

112
Q

Molecules with only one type of atom, like H2 or O2 are called what?

A

Molecules

113
Q

What are chemical bonds?

A

Energy relationships between electrons of reacting atoms

114
Q

What are chemical bonds not?

A

Not actual physical structures

115
Q

What are the subatomic particles that are involved in all chemical reactions?

A

Electrons

116
Q

What do electrons determine?

A

Whether a chemical reaction will take place and if so, what type of chemical bond is formed

117
Q

Electrons can occupy areas around the nucleus called what?

A

Electron shells

118
Q

Each electron shell contains electrons that have a certain amount of kinetic and potential energy, so shells are also called what?

A

Energy levels

119
Q

Depending on the size of an atom, how many electron shells can an atom have?

A

Up to 7

120
Q

Shells can only do what?

A

Hold a specific number of electrons

121
Q

Which shell is filled first?

A

The one closest to the nucleus

122
Q

Shell one can hold only _ electrons?

A

2

123
Q

Shell 2 holds a maximum of how many electrons?

A

8

124
Q

Shell 3 holds a maximum of how many electrons?

A

8

125
Q

The outermost electron shell is called what?

A

Valence shell

126
Q

Electrons in the valence shell have the most ______ energy and why?

A

Potential energy because they are the farthest from the nucleus

127
Q

Which electrons are involved in chemical reactions?

A

Valence shell electrons

128
Q

What is the Octet rule/rule of 8th’s?

A

Atoms desire 8 electrons in their valence shell

129
Q

What are exceptions to the Octet rule?

A

Smaller atoms like H and He, they want only 2 electrons in shell 1

130
Q

The desire to have 8 electrons is the driving force behind what?

A

Chemical reactions

131
Q

What is special about noble gases?

A

They already have the full 8 valence electrons (or 2 electrons for He), so they are not chemically reactive

132
Q

Most atoms ____ ____ have full valence shells

A

Do not

133
Q

Atoms will _____, _____, or ___ electrons (aka form bonds) with other atoms to achieve stability of 8 electrons in the valence shell

A

Gain, lose, or share

134
Q

What are chemically inert elements?

A

Valence shell is complete

135
Q

What are 2 examples of chemically inert elements?

A
  1. Helium (He) 2p, 2n, 2e
  2. Neon (Ne) 10p, 10n, 10e
136
Q

What are chemically reactive elements?

A

Valence shell is incomplete

137
Q

What are examples of chemically reactive elements?

A
  1. Hydrogen (H) 1p, 0n, 1e
  2. Carbon (C) 6p, 6n, 6e
  3. Oxygen (O) 8p, 8n, 8e
  4. Sodium (Na) 11p, 12n, 11e
138
Q

What are ions?

A

Atoms that have gained or lost electrons and become charged

139
Q

The number of protons ___ ____ equal the number of electrons

A

Does not

140
Q

Ionic bonds involve what?

A

The transfer of valence shell electrons from one atom to another, resulting in ions. One becomes an anion, and one becomes a cation

141
Q

What is an anion?

A

Negative charge, the atom that gained one or more electrons

142
Q

What is a cation?

A

Positive charge, the atom that lost one or more electrons

143
Q

The attraction of what results in an ionic bond?

A

Opposite charges

144
Q

Most ionic compounds are what?

A

Salts

145
Q

What is an example of an ionic compound?

A

NaCl, sodium chloride

146
Q

What is an example of the formation of an ionic bond?

A

Sodium with 1e in the outer shell and chlorine with 7 in the outer shell
1. The lone outer electron of sodium joins the seven outer electrons of chlorine
2. The result is a cation (Na+) and an anion (Cl-), which can form ionic bonds

147
Q

What are covalent bonds?

A

Bonds formed by the sharing of two or more valence shell electrons between two atoms

148
Q

The sharing of 2 electrons results in what kind of bond?

A

Single

149
Q

The sharing of 4 electrons results in what kind of bond?

A

Double

150
Q

The sharing of 6 electrons results in what kind of bond?

A

Triple

151
Q

What do covalent bonds allow?

A

Allows each atom to fill its valence shell at least part of the time

152
Q

What are the two types of covalent bonds?

A

Polar and nonpolar

153
Q

What are nonpolar covalent bonds?

A

Equal sharing of electrons between atoms that results in electrically balanced, nonpolar molecules such as CO2

154
Q

Carbon dioxide molecules are ____ _____, which makes them ______

A

Linear and symmetrical, makes them nonpolar

155
Q

What are polar covalent bonds?

A

Unequal sharing of electrons between 2 atoms, resulting in electrically polar molecules

156
Q

How does unequal sharing occur?

A

Atoms have different electron attracting abilities

157
Q

What is an example of covalent bonds?

A

The formation of four single covalent bonds: Carbon shares four electron pairs with four hydrogen atoms, and the result looks like a + with C in the middle and H on the 4 sides

158
Q

What is an example of polar covalent bonds?

A

V-shaped water (H2O) molecules have two poles of charge, a slightly more negative oxygen end and a slightly more positive hydrogen end

159
Q

What are hydrogen bonds?

A

Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule

160
Q

A hydrogen bond is not a true bond but more of what?

A

A weak magnetic attraction

161
Q

What is an example of hydrogen bonds?

A

The slightly positive ends of the water molecules become aligned with the slightly negative ends of other water molecules

162
Q

When do chemical reactions occur?

A

When chemical bonds are formed, rearranged, or broken

163
Q

Chemical equations contain what 2 things?

A

Reactants and products

164
Q

What are reactants?

A

Substances entering into reaction together

165
Q

What is the product(s)?

A

Resulting chemical end products

166
Q

What is a synthesis reaction?

A

Smaller particles are bonded together to form larger, more complex molecules

167
Q

What is an example of a synthesis reaction?

A

Amino acids are joined together to form a protein molecule

168
Q

What is a decomposition reaction?

A

Bonds are broken in larger molecules, resulting in smaller, less complex molecules

169
Q

What is an example of a decomposition reaction?

A

Glycogen is broken down to release glucose molecules

170
Q

What is an exchange reaction/displacement reaction?

A

Bonds are both made and broken

171
Q

What is an example of an exchange reaction/displacement reaction?

A

ATP transfers its terminal phosphate group to glucose to form glucose-phosphate

172
Q

All chemical reactions are either _____ or _____

A

Exergonic or endergonic

173
Q

Exergonic reactions result in what?

A

A net release of energy (aka it gives off energy)

174
Q

The products in an exergonic reaction have _____ _____ _____ than reactants

A

Less potential energy

175
Q

What is are 2 examples of exergonic reactions?

A

Catabolic and oxidative reactions

176
Q

Endergonic reactions result in what?

A

A net absorption of energy (aka they use up energy)

177
Q

The products in an endergonic reaction have ____ ____ ____ than the reactants

A

More potential energy

178
Q

What is an example of an endergonic reaction?

A

Anabolic reactions

179
Q

The speed of chemical reactions can be affected by what and how?

A
  1. Temperature = increased temperatures usually increase the rate of reaction
  2. Concentration of reactants = increased concentrations usually increase rate
  3. Particle size = smaller particles usually increase rate
180
Q

What do catalysts do?

A

Increase the rate of reaction without being chemically changed or becoming part of the product

181
Q

What are biological catalysts?

A

Enzymes

182
Q

What is biochemistry?

A

The study of chemical composition and reactions of living matter

183
Q

All chemicals are either ____ or ____

A

Organic or inorganic

184
Q

What are some examples of inorganic compounds?

A

Water, salts, and many acids and bases

185
Q

Inorganic compounds do not contain what?

A

Carbon

186
Q

What are some examples of organic compounds?

A

Carbohydrates, fats, proteins, and nucleic acids

187
Q

Organic compounds contain what and what are their characteristics?

A

Contains carbon, are usually large, and are covalently bonded

188
Q

Organic and inorganic compounds are both _____ _____ for life

A

Equally essential

189
Q

What is the most abundant inorganic compound that accounts for 60-80% of the volume of living cells?

A

Water

190
Q

What are the properties of water?

A
  1. High heat capacity = ability to absorb and release heat with little temperature change, prevents sudden changes in temperature
  2. High heat of vaporization = heat is lost with evaporation
  3. Polar solvent properties = dissolves and dissociates ionic substances (used for transport in the body)
  4. Reactivity = hydrolysis and dehydration synthesis reactions
  5. Cushioning
191
Q

What is an example of water’s high heat capacity?

A

Water in the blood redistributes head among tissues to maintain homeostasis

192
Q

What is an example of water’s high heat of vaporization?

A

Sweat evaporates from skin

193
Q

What is an example of water cushioning?

A

Cushing body organs like in CSF

194
Q

What are salts?

A

Ionic compounds that dissociate into separate ions in water

195
Q

Ions play specialized roles in what and is vital for what?

A

Body functions and is vital for homeostasis

196
Q

What are common salts in the body?

A

NaCl, CaCO3, KCl, calcium phosphates

197
Q

Acids and bases are both _____, so they ionize and dissociate in water?

A

Electrolytes

198
Q

Acids are proton _____ and they release ____ _____ (H+) and bare protons in the solution

A

Donors and they release hydrogen ions

199
Q

What are important acids?

A

HCl, HC2H3O2, and H2CO3

200
Q

What is HCl?

A

Hydrochloric acid

201
Q

What is HC2H3O2?

A

Acetic acid (HAc)

202
Q

What is H2CO3?

A

Carbonic acid

203
Q

Bases are proton ______ and they pick up what type of ions in the solution?

A

Proton acceptors and they pick up H+ ions

204
Q

What are bare protons?

A

Protons that have no electrons

205
Q

When a base dissolves in solution, what does it release?

A

Hydroxyl ion (OH-)

206
Q

What are important bases?

A

Bicarbonate ion and ammonia

207
Q

What is HCO3-?

A

Bicarbonate ion

208
Q

What is NH3?

A

Ammonia

209
Q

On the pH scale, numbers 8-14 are _______ ____

A

Increasingly basic

210
Q

On the pH scale number 7 is ____

A

Neutral

211
Q

On the pH scale, numbers 6 and below is _____ _____

A

Increasingly acidic

212
Q

1M sodium hydroxide has a pH of what?

A

14 (the most basic)

213
Q

Oven cleaner, lye has a pH of what?

A

13.5 (basic)

214
Q

Household ammonia has a pH of what?

A

10.5 to 11.5 (basic)

215
Q

Household bleach has a pH of what?

A

9.5 (basic)

216
Q

Egg whites have a pH of what?

A

8 (the least basic)

217
Q

Blood has a pH of what?

A

7.4 (neutral)

218
Q

Milk has a pH of what?

A

6.3 to 6.6 (the least acidic)

219
Q

Black coffee has a pH of what?

A

5 (acidic)

220
Q

Wine has a pH of what?

A

2.5 to 3.5 (acidic)

221
Q

Lemon juice and gastric juice have a pH of what?

A

2 (acidic)

222
Q

1M of hydrochloric acid has a pH of what?

A

0 (the most acidic)

223
Q

What is a neutralization reaction?

A

Acids and bases are mixed together. Displacement reactions occur, forming water and a salt

224
Q

What is an example of a neutralization reaction?

A

NaOH + HCl —> NaCl + H20

225
Q

What are the major organic compounds?

A

Carbohydrates, lipids, proteins, and nucleic acids

226
Q

Many organic compounds are ______

A

Polymers

227
Q

What are polymers?

A

Chains of similar unites called monomers

228
Q

Organic compounds are synthesized by what?

A

Dehydration synthesis

229
Q

Organic compounds are broken down by what?

A

Hydrolysis reactions

230
Q

What is dehydration synthesis?

A

Monomers are joined by removal of OH from one monomer and removal of H from the other at the site of bond formation

231
Q

What is hydrolysis?

A

Monomers are released by the addition of a water molecule, adding OH to one monomer and H to the other

232
Q

Carbohydrates include what?

A

Sugars and starches

233
Q

What are monosaccharides?

A

Monomers of carbohudrates

234
Q

What are some examples of monosaccharides?

A

Hexose sugars = Glucose, fructose, galactose
Pentose = Deoxyribose and ribose

235
Q

What are disaccharides?

A

Consist of two linked monosaccharides

236
Q

What are some examples of disaccharides?

A

Sucrose = glucose + fructose
Maltose = glucose + glucose
Lactose = galactose + glucose

237
Q

What is a polysaccharides?

A

Long chains (polymers) of linked monosaccharides

238
Q

What do lipids contain?

A

C, H, and O, but less than in carbohydrates, and sometimes contain P

239
Q

Lipids are _____ in water

A

Insoluble

240
Q

Triglycerides or neutral fats are called _____ when solid and _____ when liquid

A

Fats when solid and poils when liquid

241
Q

What are the main functions of triglycerides/neutral fats?

A

Energy storage, insulation, protection

242
Q

What is the triglyceride formation?

A

Three fatty acid chains are bound to glycerol by dehydration synthesis

243
Q

The head and tail regions of phospholipids contain different properties, what are they?

A

Head is a polar region and is attracted to water, tails are nonpolar and are repelled by water

244
Q

Phospholipids are important in what structure?

A

Cell membrane

245
Q

What is the typical structure of a phospholipid molecule?

A

Two fatty acid chains (tail) and a phosphorus-containing group (head) are attached to the glycerol backbone like in Phosphatidylcholine

246
Q

What are common steroids?

A

Natural: cholesterol, vitamin D, steroid hormones, and bile salts
Man-made: Corticosteroids and anabolic

247
Q

What is the most important steroid and why?

A

Cholesterol, because it is the basis for all steroids formed in the body and it is important in cell plasma membrane structure

248
Q

What is the simplified structure of a steroid?

A

Four interlocking hydrocarbon rings

249
Q

What are eicosanoids?

A

Found in cell membranes

250
Q

What are the most important eicosanoids?

A

Prostaglandins, because they play a role in blood clotting, control of blood pressure, inflammation, and labor contractions

251
Q

All proteins are made from __ types of amino acids?

A

20

252
Q

All proteins are joined by covalent bonds called ____ bonds

A

Peptide

253
Q

Proteins can act as either an ____ or _____

A

Acid or base

254
Q

Proteins differ by which of ___ ____ ____ ____ is present

A

20 different “R groups” is present

255
Q

What is the primary structure of proteins?

A

The sequence of amino acids form the polypeptide chain

256
Q

What is the secondary structure of proteins?

A

The primary chain forms spirals (alpha helices) and sheets (beta sheets)

257
Q

What is the tertiary structure of proteins?

A

Superimposed on secondary structure, alpha helices and/or beta sheets are folded up to form a compact globular molecule held together by intramolecular bonds

258
Q

What is the quaternary structure of proteins?

A

Two or more polypeptide chains, each with its own tertiary structure, combines to form a functional protein

259
Q

What is denaturation?

A

Globular proteins unfold and lose their functional 3-D shape, and active sites become deactivated

260
Q

Why does denaturation occur?

A

Decreased pH (increased acidity) or increased temperature

261
Q

Is denaturation reversible?

A

If normal conditions are restored, but is irreversible if the changes are extreme, like how you can’t uncook an egg

262
Q

What are enzymes?

A

Globular proteins that act as biological catalysts

263
Q

What do catalysts do?

A

Regulate and increase the speed of chemical reactions without getting used up in the process

264
Q

What do enzymes do to the energy?

A

Lowers the energy needed to initiate a chemical reaction. Leads to an increase in the speed of a reaction. Allows for millions of reactions per minute

265
Q

What are nucleic acids?

A

Largest molecules in the body, composed of C, H, O, N and P

266
Q

What are nucleic acid polymers made up of?

A

Monomers called nucleotides, composed of a nitrogen base, a pentose sugar, and phosphate group

267
Q

What are the two major classes of nucleic acids?

A

Deoxyribonucleic acid (DNA) and ribonucleic acid (RNA)

268
Q

What does DNA hold?

A

The genetic blueprint for the synthesis of all proteins

269
Q

What is DNA?

A

A double-stranded helical molecule (double helix) located in the cell nucleus

270
Q

What do nucleotides contain?

A

A deoxyribose sugar, phosphate group, and one of four nitrogen bases

271
Q

What are the 2 groups that the four nitrogen bases fall into?

A

Purines: adenine (A) and guanine (G)
Pyrimidines: cytosine (C) and thymine (T)

272
Q

RNA links DNA to ____ _____ and is slightly different from DNA

A

Protein synthesis

273
Q

What is RNA?

A

Single-stranded linear molecule is active mostly outside the nucleus. Contains a ribose sugar

274
Q

What is thymine replaced with in RNA?

A

Uracil

A&P 1 Summer 2023 (17 decks)

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