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Biol 235 > Chapter 2: The Chemical Level of Organization > Flashcards

Chapter 2: The Chemical Level of Organization Flashcards

1
Q

List the main chemical elements of the human body

A
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2
Q

The science of the structure and interactions of matter

A

Chemistry

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3
Q

Matter

A

Anything that occupies space and has mass; made up of chemical elements

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4
Q

Mass

A

The amount of matter in any object, which does not change

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5
Q

Weight

A

The force of gravity acting on matter; this can change

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6
Q

Three states of matter

A

solids, liquids and gas

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7
Q

Chemical Elements

A

Make up all forms of matter, living and non-living.

There are 118; 92 are naturally occuring

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8
Q

How many chemical elements are normally present in your body?

A

26

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9
Q

Name the 4 major elements that constitute approximately 96% of the body’s mass

A

oxygen (O)
carbon (C)
hydrogen (H)
nitrogen (N)

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10
Q

Name the 8 lesser elements that contribute to about 3.6% of the body’s mass

Carla Plays Poker So She Can Make Ingenious <wins></wins>

A

Calcium (Ca)
Phosphorus (P)
Potassium (K)
Sulfur (S)
Sodium (Na)
Chloride (Cl)
Magnesium (Mg)
Iron (Fe)

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11
Q

What is the term for the remaining elements that make up 0.4% of body mass

A

Trace Elements

Eg Iodine

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12
Q

Three categories of elements

A
  1. Major Elements
  2. Lesser Elements
  3. Trace Elements
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13
Q

The smallest units of matter that retain the properties and characteristics of an element

A

Atom

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14
Q

These make up atoms

A

Subatomic Particles

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15
Q

3 types of subatomic particles

A

Proton, neutron, and electrons

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16
Q

Nucleus of an atom

A

The dense central core

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17
Q

Where are protons, p+, and neutrons, N0, found within the atom

A

The nucleus

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18
Q

Where are electrons, e-, found in an atom?

How do they move?

A

They move about in a space surrounding the nucleus

Form a ‘cloud’ around the nucleus and do not move in a fixed pathway

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19
Q

Certain regions around the nucleus that specific groups of electrons are most likely to move about within. Each one of these can hold a specific number of electrons.

A

Electron Shells

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20
Q

How many electrons does each electron shell hold?

A

First (closest to nucleus) = max 2
Second = max of 8
Third = max 18

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21
Q

Atomic Number

A

The number of protons within an atoms nucleus

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22
Q

Mass Number

A

The sum of an atoms protons and neutrons

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23
Q

Sodium has 11 protons and 12 neutrons, what is it’s atomic number and it’s mass number?

A

Atomic number is 11
Mass number is 23

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24
Q

Isotopes

A

Atoms of an element that have different numbers of neutrons and therefore different mass numbers

Identical chemical properties because they have the same number of electrons

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25
Q

Radioactive Isotopes

A

Unstable isotopes; these atoms have a nuclei that will decay to a stable configuration and will emit radiation (either subatomic particles or packets of energy) and often will turn into a different element

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26
Q

The time required for half of the radioactive atoms in a sample of an isotope to decay into a more stable form

A

Half-life

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27
Q

Atomic Mass

A

The average mass of all of an elements naturally occuring isotopes; usually close to most abundant isotope

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28
Q

Ion

A

An atom that has a positive or negative charge because it has unequal numbers of protons and electrons

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29
Q

Ionization

A

The process of giving up or gaining electrons

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30
Q

Molecule

A

When two or more atoms share electrons

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31
Q

Compound

A

A substance that ocntains atoms of two or more different elements

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32
Q

Free Radical

A

An atom of group of atoms with an unpaired electron in it’s outermost shel

Makes it unstable, highly reactive and destructive to nearby molecules

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33
Q

The forces that hold together the atoms of a molecule or compound

A

Chemical Bonds

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34
Q

Valence Shell

A

An atoms outer most shell; likelihood of chemical bonds occuring depends on the number of electrons in this shell

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35
Q

Octet Rule

A

One atom is more likely to interact with another atom if doing so will leave both with eight valence electrons; can donate, take or share electrons

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36
Q

Name three types of chemical bonds

A

Ionic
Covalent
Hydrogen

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37
Q

Positive and negative charged ions are attracted to one another and can create this type of chemical bond

A

Ionic Bonds

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38
Q

Cation

A

A positively charged ion (loses electrons and therefore has more protons)

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39
Q

Anion

A

A negatively charged ion (gains electrons and therefor has more electrons)

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40
Q

Electrolyte

A

An ionic compound that breaks apart into positive and negative ions in solution

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41
Q

When two or more atoms share electrons rather than gaining or losing them, a _________________ bond is formed. The more electrons shared between them, the stronger the bond

A

Covalent Bond

  • most common bond in the human body
  • can be the between atoms of same or different elements
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42
Q

Covalent bond numbers

A

Single - one pair shared
Double = two pairs shared
Triple E three pairs shared

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43
Q

Nonpolar Covalent bonds

A

when two atoms share the electrons equally, eg between two atoms of same element

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44
Q

Polar covalent bond

A

Sharing of electrons is unequal, the nucleus of one atom attracts the shared electrons more strongly than the nucleus of the other atom

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45
Q

Electronegativity

A

When polar covalent bond forms, the atom with the stronger pull on the electrons has a partial negative charge and has greater electronegativity

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46
Q

An important polar covalent bond in living systems

A

H20 The bond between hydrogen and oxygen

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47
Q

Polar covalent bonds that form between hydrogen atoms and other atoms

A

Hydrogen Bonds

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48
Q

How does a hydrogen bond form?

A

When a hydrogen atom with a partial positive charge attracts the partial negative charge of neighboring electronegative atoms

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49
Q

What type of bond forms because of attraction of oppositely charged PARTS of molecules rather than sharing of electrons or donating/taking electrons

A

Hydrogen Bonds

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50
Q

Bond that cannot bind atoms into molecules; weakest bond;

A

Hydrogen Bonds

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51
Q

Surface Tension

A

Caused by hydrogen bonds of water molecules and measures the difficulty of stretching or breaking the surface of a liquid

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52
Q

Chemical Reaction

A

When new bonds form or old bonds break between atoms; interactions of valence electrons are basis of all chemical reactions; involves energy changes

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53
Q

Metabolism

A

All chemical reactions occuring in the body

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54
Q

Reactants

A

Starting substances

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55
Q

Products

A

ending substances

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56
Q

What are the two principle forms of energy?

A

Potential and kinetic

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57
Q

Potential Energy

A

Energy stored by matter due to its position

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58
Q

Kinetic Energy

A

The energy associated with matter in motion

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58
Q

Law of conservation of energy

A

Total amount of energy remains the same; it cannot be created nor destroyed, but can be converted from one form to another

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58
Q

Chemical Energy

A

a form of potential energy that is stored in the bonds of compounds and molecules

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58
Q

Exergonic Reaction

A

A chemical reaction that releases more energy than is absorbed

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58
Q

Endergonic Reaction

A

A chemical reaction where more energy is absorbed than is released.

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59
Q

Activation energy

A

The collision energy needed to break the chemical bonds of a reactant; needed to start a reaction because it causes enough energy to be absorbed that their chemical bonds become unstable and new combinations begin to be formed

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60
Q

The more particles of matter present in a confined space, the greater the chance they will collide

A

Concentration affects reactions

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61
Q

As temperature increases, the particles of matter move more rapidly, increasing likeliness of more forceful collisions and therefore more likely the collision will produce a reaction

A

Temperature affects reactions

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62
Q

Chemical compounds that speed up chemical reactions by lowering the activation energy needed for a reaction to occur. Eg enzymes

A

A catalyst

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63
Q

Synthesis Reactions - Anabolism

A

When two or more atoms, ions or molecules combine to form new or larger molecules. Usually energonic.

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64
Q

Decomposition Reactions - Catabolism

A

Split up larder molecules into smaller atoms, ions or molecules. Usually exergonic.

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65
Q

Exchange reactions

A

Reactions that consist of both synthesis and decomposition reactions

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66
Q

Reversible reactions

A

the products of a reaction can revert to the original reactants (indicated by two half hours pointing in opposite directions)

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67
Q

Oxidation-Reduction Reactions

Important in breaking down food molecules and producing energy

A

Oxidation - loss of electrons where oxidized substance releases energy

Reduction - gain of electrons, the reduced substance gains energy

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68
Q

Compounds that usually lack carbon and are structurally simple. Eg water, salts, etc. ionic or covalent bonds.

A

Inorganic compounds

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69
Q

What percentage of a lean human body does water make up?

A

55-60%

Other inorganic matter makes up about 1-2%

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70
Q

Inorganic compounds that contain carbon are:

A

Carbon Dioxide
Bicarbonate
Carbonic Acid

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71
Q

Compounds that always contain carbon, usually contain hydrogen and always have covalent bonds

A

Organic Compounds

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72
Q

What percent of the lean body is made up of organic compounds?

A

38-43%

73
Q

The most important and abundant inorganic compound in all living systems

A

Water

74
Q

The most important property of water

A

It’s polarity

75
Q

Solution is made up of:

A

Solvent that has dissolved a solute

76
Q

Solutes that are charged or contain covalent bonds are

A

Hydrophillic

77
Q

Molecules that ocntain mainly nonpolar covalent bonds

A

Hydrophobic (not very water soluble)

78
Q

Hydrolysis

A

The breakdown of large nutrient molecules into smaller molecule by adding water molecules that takes place during decomposition reactions

79
Q

When two smaller molecules combine to form a larger molecule and a water molecule is one of the products formed

A

Dehydration synthesis reaction

80
Q

Three types of mixtures (mixed together but not bound by chemical bonds)

A

Solution - transparent
Colloid - opaque from larger molecules
Suspensions - suspended material will settle out

81
Q

Moles per liter (mol/L)

A

molarity; total number of molecules in a given volume of solution

82
Q

Percentage (mass per volume)

A

Number of grams of a substance per 100ml of solution

83
Q

When inorganic acids, bases or salts dissolve in water and seperate into ions, becoming surrounded by water molecules

A

dissociate

84
Q

Acids

A

Has more H+ than OH- molecules; pH below 7

Disocciate in water into one or more H+ (hydrogen) ions and one or more anions
(proton donor)

85
Q

Bases

A

Has more OH- than H+ molecules ; pH above 7

Disocciate into one or more hydroxide ions (OH-) and one or more cations

(proton acceptor)

86
Q

When added to water, these dissociate into cations and anions, neither of which are H+ or OH-

A

Salts

87
Q

The measure of a solutions acidity or alkalinity is expressed using this scale which is based on the concentration of H+ in moles per liter

A

pH scale

88
Q

What is the normal pH of the blood

A

7.35-7.45 slightly more basic than water

89
Q

These function to convert strong acids or bases into weak acids or bases by adding or removing protons H+

A

buffer systems

90
Q

Carbonic acid-bicarbonate buffer systen

A

This buffer system is important in maintaining homestatic pH levels in the body

91
Q

What bond are organic compounds usually held together with?

A

Covalent

92
Q

Elements that commonly bond with carbon in organic compounds

A

hydrogen, oxygen, and nitrogen

Some sulfur and phosphorus

93
Q

The chain of carbon in an organic molecule

A

Carbon Skeleton

94
Q

When many carbons are bonded to hydrogen atoms

A

Hydrocarbon

95
Q

Functional Groups

A

Atoms or molecules bound to the hydrocarbon skeleton. Each type of functional group has a specific arrangement of atoms that confers characteristic chemical properties on the organic molecule it it attached to

96
Q

When small organic molecules combine into very large molecules

A

Macromolecules; usually polymers;

97
Q

What is a polymer?

A

A polymer is a large molecule formed by the covalent bonding of many identical or similar small molecules called monomers

98
Q

Dehydration Synthesis

A

When two monomers join through reaction by the removal of a hydrogen atom from one monomer and a hdroxyl group for the other, this forms a molecule of water

99
Q

Molecules with the same molecular formula but different structures and therefore different chemical properties

eg. glucose and fructose

A

Isomers

100
Q

Sugars, glycogen, staches, and cellulose

A

Carbohydrates “watered carbon”

101
Q

Three major groups of carbohydrates

(2-3% of total body mass)

A

Monosaccharides

Disaccharides

Polysaccharides

102
Q

“Simple Sugars”

A

Mono and di saccharides

103
Q
  • The monomers of carbohydrates
  • contain 3-7 carbon atoms
  • ‘ose’ name with prefix for number of carbons eg. Triose to heptose
A

Monosaccharides

104
Q

Hexose Glucose

A
  • broken down by body to produce ATP
105
Q

A molecule formed from the combination of 2 monosaccharides by dehydration synthesis (producing also a water molecule).

These can be broken back down into their monosaccharides by adding a water molecule

A

Disaccharide

106
Q

Contains tens or hundreds of monosaccharides joined through dehydration synthesis reactions

Insoluble in water

do not taste sweet

A

Polysaccharides

107
Q

Main polysaccharide in the human body

Made up of glucose monomers linked to one another in branching chains

Stored in liver and skeletal muscles

A

Glycogen

108
Q

Major carbohydrates in the diet

Found in pasts and potatoes

Formed from glucose by plants

A

Starches

109
Q

A polysaccharide produced by plants that cannot be digested by humans but does provide bulk to helpe eliminate feces

A

Cellulose

110
Q

Organic compound that makes up 18-25% of body mass

Contain hydrogen, carbon and ocygen

Fewer polar covalent bonds than carbohydrates due to lower numbers of electronegative oxygen

Hydrophobic; not soluble in in polar solvents

A

Lipids

111
Q

How do small lipids become more soluble in blood plasma?

A

They join with hydrophyllic proteins to form lipoproteins

112
Q

Lipoproteins are soluble because…

A

The water soluble protein is on the outside of the complex and the lipids are on the inside

113
Q

Some types of lipids

A

Fatty acids
triglycerides,
steroids,
phospholipids
eicosanoids (20 carbon lipids)
fat soluble vitamins (A, D, E, K)
lipoproteins
and more

114
Q

These are used to synthesize triglycerides and phospholipids

The simplest of lipids

Consists of a carboxyl group and a hydrocarbon chain

Can be catabolized to generate ATP

A

Fatty acids

115
Q

This fatty acid contains only a single covalent bond between the carbon atoms of the hydrocarbon chain. Each carbon is saturated with hydrogen atoms

A

saturated fatty acids

116
Q

These fatty acids contain one or more double covalent bonds and are not completely saturated with hydrocarbon atoms

A

Unsaturated Fatty Acids

117
Q

The most abundant lipids in the human body and diet

A

Triglycerides

118
Q

What are the two types of building blocks that make triglycerides?

A

A single 3-carbon glycerol molecule (backbone of the triglyceride)
3 fatty acids (one attached to each carbon through dhydration synthesis)

119
Q

triglyceride that is solid at room temperature

A

A fat

120
Q

What is a saturated fat

A

A fat that mainly consists of saturated fatty acids. Because of the lack of double bonds the y can closely pack together forming a solid at room temp

121
Q

Where are saturated fats mostly found?

A

Meats, but also palm oil, cocoa butter and coconut oil

122
Q

What is a triglyceride that is liquid at room temperature?

Their fatty acid are mostly unsaturated

A

An oil

123
Q

Two types of fatty acids in oils that are believed to reduce the risk of heart disease

A

Monounsaturated - olive oil, peanut oil, canola oil, nuts, avocados

Polyunstaurated - corn oil, fatty fish, etc

124
Q

What is the body’s most highly concentrated form of chemical energy?

These provide more than twice the energy as carbohydrates and proteins

A

Triglycerides

125
Q

What are excess carbohydrates, protein, fats and oils stored as?

A

Triglycerides in the adipose tissue

126
Q

This type of lipid has a 3 carbon glycerol, however only the first 2 carbons have a fatty acid chain attached and the third one has a phosphate group that links a small charged group that contains nitrogen to the backbone

A

Phospholipids

127
Q

Describe the head of a phsopholipid and its tails

A

The head is the group containing nitrogen, it is polar, and can form hydrogen bonds with water molecules

The tails are the two fatty acids

128
Q

Molecules that have both polar and non-polar parts are said to be ____________

A

amphipathic

129
Q

How are phospholipids involvref in the membrane surrounding a cell

A

They line up tail to tail to form a double row that makes up most of the membrane that surrounds a cell

130
Q

These lipids have 4 rings of carbon atoms

A

Steroids

131
Q

This has a large nonpolar region consisting of 4 carbon rings and a hydrocarbon tail

A

Cholesterol

132
Q

Lipids derived from 20-carbon fatty acids called arachidonic acid

Primarily prostaglandings and leukotrienes

A

Eicosanoids

133
Q

These had a wide variety of functions. The modify responses to hormones, contribute to the inflammatory response, prevent stomach ulcers, dilate airways to the lungs, regulate body temperature, and influence the formation of blood clots, etc

A

Prostaglandins

134
Q

These eicosanoids participate in allergic and inflammatory repsonses

A

Leukotrienes

135
Q

These are large molecules that contain carbon, hydrogen, oxygen and nitrogen. Some may contain sulfur.

Much more complex than carbohydrates or lipids

A

Proteins

136
Q

What percentage of a lean adult body is protein?

A

12-18%

137
Q

Some common protein functions

A
  • largely responsible for the structure of body tissues
  • enzymes are proteins
  • may work as motors to drive myscle contractions
  • antibodies are proteins
  • some hormones are proteins
138
Q

What are the monomers of proteins? How many are there?

A

Amino Acids; 20

139
Q

What makes up an amino acids?

A

Each one has:
1. Hydrogen atom
2. An acideic carboxyl group
3. A side chain (R group)

140
Q

What gives each amino acid it’s distint chemical identity?

A

The different side chains

141
Q

What is the name of the covalent bond that joins two amino acids?

A

A peptide bond

142
Q

Where does a peptide bond always form?

What else is created?

A

Between the carbon of the carboxyl group of 1 acid and the nitrogen of the amino group of the second acid.

And H20 molecule is also formed and removed

143
Q

What type of reaction breaks a peptide bond?

A

A hydrolysis reaction (adding an H20 molecule)

144
Q

A dipeptide

A

2 amino acids combined

145
Q

A tripeptide

A

3 combined amino acids

146
Q

A chainlike peptide has how many amino acides?

A

4-9

147
Q

How many amino acids are in a polypeptide?

A

10+

148
Q

What is the process where a protein that encounters an altered environment unravels and loses its characteristic shape?

Eg heat to an egg cause irreversible ________ to the protein

A

Denturation

149
Q

What are most catalysts in living cells?

A

protein molecules called enzymes

150
Q

What is an apoenzyme and a cofactor?

A

Apoenzyme - a protein portion of an enzyme
Cofactor - a metal ion or organic molecule called a coenzyme (usually derived from vitamins)

151
Q

What is the suffix of an enzyme name? Examples?

A

-ase

Anhydrase - removes water
proteinases - break down proteins
lipases - break down triglycerides

152
Q

What are three important properties of enzymes?

A
  1. Highly specific - they only bind to specific substrates
  2. Very efficient - increase reaction rates to 100 million to 10 billion times the time without enzymes
  3. Have cellular controls - controlled by cells genes and activation of them are determined by chemical environment within cells
153
Q

What is a substrate?

A

The reactant molecules on which an enzyme acts. Each enzyme can only bind with certain substrates.

154
Q

What is the active site of an enzyme?

A

the part of the enzyme that catalyzes the reaction

May fit the substrate like a lock and key

or May change shape to fit snugly around the substrate (induced fit)

155
Q

How does an enzyme work?

  • enzyme-substrate complex created
  • substrate molecule changed
  • Enzyme unchanged
A
  1. Substrate makes contact with active site of enzyme; forms a temp compound “enzyme-substrate complex”
  2. Molecules of substrate transformed by breakdown of the mocule, rearrangement of existing atoms or combination of several substrate molecules
  3. Enzyme is unchanged and reusable
156
Q

What do nucleic acids contain?

A

carbon, hydrogen, oxygen, nitrogen, phosphorus

157
Q

What is DNA

A

Deoxyribonucleic Acid

forms inherited genetic material inside each cell nucleus

158
Q

This is a segment of DNA molecules that determine the traits we inhereit and controls protein synthesis

Passed on with each cell division

A

Genes

159
Q

What is RNA

A

Ribonucleic Acid

relays instructions from the genes to guide the synthesis of proteins from amino acids

160
Q

Nucleotides

A

The monomers that make up a nucleic acid

161
Q

What 3 parts does each nucleotide of a DNA consist of?

A
  1. Nitrogenous base
  2. Pentose sugar (deoxyribose)
  3. Phosphate group
162
Q

What are the 4 different nitrogen bases in DNA?
A, T, C, G

A

Adenine
Thymine
Cytosine
Guanine

163
Q

Which two nitrogen bases are purines and have larger double rings

A

Adenine and Guanine

164
Q

Which two nitrogen bases are smaller, single ringed bases called pyrimidines

A

Cytosine and thymine

165
Q

What is the DNA model called that resembles a spiral ladder?

Describe the visual

A

Double Helix Model

Two strands of alternating phosphate groups and deoxyribose sugars form the uprights of the ladder.

Paired bases held together by hydrogen bonds form the rungs

166
Q

Which bases pair with which?

A

Adenine and thymine

Cytosine and Guanine

167
Q

What is a change that occurs in the base sequence of a DNA strand that can results in the death of a cell, cause cancer or produce genetic defects in future generations?

A

A mutation

168
Q

How does RNA differ from DNA in humans?

A
  • single stranded
  • the pentose sugar is ribose
  • contains the pyrimidines bases Uracil instead of thymine
169
Q

Name the 4 bases in DNA with their complement
AT, CG

A

Adenine and Thymine
Cytosine and Guanine

170
Q

Name the 4 bases in RNA with their complement

AU, CG

A

Adenine and Uracil
Cytosine and Guanine

171
Q

3 types of RNA

A
  • messenger RNA
  • ribosomal RNA
  • transfer RNA
172
Q

What uses the energy from exergonic catabolic reactions to power cellular activities that require energy (energonic reactions)

A

ATP

Adenosine Triphosphate

173
Q

What are some examples of reactions ATP is used for

A
  • muscular contractions
  • movment of chromosomes during cell division
  • movement of structures within cells
    -transport of substances across cell membranes
  • synthesis of larger molecules from smaller ones
174
Q

What is ATP (adenosine triphosphate) composed of?

A

Three phosphate groups attached to an adenosine

175
Q

What is adenosine made up of?

A

Adenine and a ribose (5 carbon sugar)

176
Q

How does ATP release energy?

A

When a water molecule is added to ATP, the third phosphate group is removed and energy is liberated

177
Q

What enzyme catalyzes the hydrolysis of ATP?

A

ATPase

178
Q

What is produced when the third phosphate group is removed from ATP through hydrolysis (adding a water molecule)?

A

Adenosine Diphosphate (ADP)

179
Q

ATP + water With ATPase*
=???

A

ADP + Phosphate Group + energy

180
Q

What enzymes helps replenish ATP when stores are low?

A

ATP synthase

181
Q

ADP + Phosphate group + Energy with ATP synthase* =

A

ATP + water molecule

182
Q

What role does the catabolism of glucose through cellular respiration play int he production of ATP?

A

This catabolism through cellular respiration provides the needed energy to attach a phosphate group to create ATP from ADP

183
Q

What are the two phases of cellular respiration?

A

Anaerobis Phase

Aerobic Phase

184
Q

Describe the anaerobic phase of cellular respiration

A
  • no oxygen, glucose partially broken down into pyruvic acid
  • 2 molecules of ATP produced from from each glucose molecule that is converted into pyruvic acid
185
Q

Describe the aerobic phase of cellular respiration

A
  • in presence of oxygen, glucose broken down completely into CO2 and water
  • this creates heat and 30-32 ATP molecules

Biol 235 (5 decks)

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