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A&P I & II > Chapter 2 > Flashcards

Chapter 2 Flashcards

0
Q

Chemical elements

A

Building blocks that make up all matter

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1
Q

Chemistry

A

The science of structure and interactions of matter

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2
Q

Chemical symbol

A

Designates each element. Uses one or two letters of the elements name in English Latin or another language

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3
Q

Major elements

A

Four elements that constitute about 96% of the bodies mass: Oxygen, carbon, hydrogen, and nitrogen

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4
Q

How many chemical elements are normally present in the human body?

A

26

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5
Q

Lesser elements

A

Contribute about 3.6% to the bodies mass: Calcium, phosphorus, potassium, sulfur,sodium,chlorine, magnesium,and iron.

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6
Q

Trace elements

A

additional 14 elements that altogether Account for the remaining .4% of the body’s mass.

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7
Q

Oxygen

A

Major element
O
About 65% of body mass
Part of water and many organic molecules used to generate ATP, a molecule used by cells to temporarily store chemical energy

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8
Q

Carbon

A

C
Major element
About 18.5% of total body mass
Forms backbone chains and rings of all organic molecules; Carbohydrates, lipids, proteins and nucleic acids (DNA and RNA)

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9
Q

Hydrogen

A

H
Major element
9.5% Of total body mass
Constituent Of water and most organic molecules; ionized form (H+) Makes body fluids more acidic

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10
Q

Nitrogen

A

N
Major element
3.2% Of total body mass
Components of all proteins and nucleic acids

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11
Q

What are the major elements?

A

Oxygen
carbon
hydrogen
nitrogen

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12
Q

Calcium

A

Ca
Lesser element
About 1.5% Of total body mass
Contributes to hardness of bones and teeth; ionized form (Ca2+) Needed for blood clotting, release of some hormones, contraction of muscles and many other processes

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13
Q

Phosphorus

A

P
Lesser element
1% of total body mass
Component of nucleic acids and ATP; Required for normal bone and tooth structure.

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14
Q

Potassium

A

K
Lesser element
.35% of total body mass
Ionized form (K+) Is the most plentiful cation (Positively charged particle) in intracellular fluid; Needed to generate action potentials

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15
Q

Sulfur

A

S
Lesser element
.25% of total body mass
Component of some vitamins and many proteins

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16
Q

Sodium

A

Na
Lesser element
.2% of total body mass
Ionized form (Na+) is the most plentiful cation in extracellular fluid; Essential for maintaining water balance; needed to generate action potentials.

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17
Q

Chlorine

A

Cl
Lesser element
.2% of total body mass
Ionized form (Cl-) Is the most plentiful anion in extracellular fluid; Essential for maintaining water balance

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18
Q

Magnesium

A

Mg
Lesser element
.1% of total body mass
Ionized form (Mg2+) Needed for action of many enzymes, molecules that increase the rate of chemical reactions organisms

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19
Q

Iron

A

Fe
Lesser element
.005% of total body mass
Ionized forms (Fe2+ and Fe3+) Are part of hemoglobin

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20
Q

Trace elements

A

Lesser elements that make up about .04% of total body mass
Aluminum, boron, chromium, cobalt, copper, fluorine, iodine, Manganese, molybdenum, Selenium, silicon, tin, vanadium, and zinc

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21
Q

Hemoglobin

A

Oxygen-carrying protein in red blood cells

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22
Q

Cation

A

Positively charged particle

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23
Q

Anion

A

Negatively charged particle

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24
Q

Atoms

A

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

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25
Q

Subatomic particles

A

Compose individual atoms

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26
Q

Nucleus

A

The dense central core of an atom

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27
Q

Protons

A

(p+)

A stable positively charged subatomic particle Within the nucleus of an atom

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28
Q

Neutron

A

(n0)

Electrically neutral subatomic particle within the nucleus of an atom

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29
Q

Electron

A

(e-)

Negatively charged subatomic particle That move about in a large space surrounding the nucleus of an atom

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30
Q

Electron shells

A

A grouping of electrons surrounding the nucleus of an atom

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31
Q

Atomic number

A

The number of protons in the nucleus of an atom

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32
Q

Mass number of an atom

A

The sum of its protons and neutrons

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33
Q

Isotopes

A

Atoms of an element that have different numbers of neutrons and therefore different mass numbers
Pg 31

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34
Q

Radioactive isotopes

A

Are unstable; There nuclei Decay into a stable configuration

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35
Q

Half life of an isotope

A

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

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36
Q

Dalton

A

The standard unit for measuring the mass of atoms and their sub atomic particles

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37
Q

Atomic mass also called atomic weight

A

The average mass of all naturally occurring isotopes of an element

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38
Q

Ion

A

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

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39
Q

Ionization

A

The process of giving up or gaining electrons

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40
Q

Molecule

A

When two or more atoms share electrons

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41
Q

Compound

A

A substance that contains Adams of two or more different elements

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42
Q

Free radical

A

An atom or group of atoms with an unpaired electron in the outermost shell

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43
Q

Antioxidants

A

Substances that in activate oxygen derived free radicals. Thought to slow the pace of damage caused by free radicals

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44
Q

Chemical bonds

A

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

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45
Q

Valence shell

A

The outermost layer of an atom. Contains electrons.

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46
Q

Octet rule

A

Under the right conditions to a more Adams can interact in ways that produce a chemically stable arrangement of eight valence electrons for each atom

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47
Q

Ionic bond

A

The force of attraction that holds together ions with opposite charges

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48
Q

Cation

A

Positively charged ion

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49
Q

Anion

A

Negatively charged ion

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50
Q

Electrolyte

A

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

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51
Q

Covalent bond

A

When two or more atoms share electrons rather than gaining or losing them

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52
Q

True or false covalent bonds may form between atoms of the same element or between atoms of different elements?

A

True

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53
Q

Single covalent bond

A

When two atoms share one electron pair

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54
Q

Double covalent bond

A

Results when two atoms share two pairs of electrons

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55
Q

Triple covalent bond

A

When two atoms share three pairs of electrons

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56
Q

Nonpolar covalent bond

A

In some covalent bonds two atoms share the electrons equally one atom does not attract the shared electrons more strongly than the other atom

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57
Q

Polar covalent bond

A

The sharing of electrons between two atoms is unequal the nucleus of one atom attracts the shared electrons more strongly than the nucleus of the other atom

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58
Q

Electronegativity

A

An atoms power to attract electrons to itself

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59
Q

Hydrogen bond

A

Forms when a hydrogen atom with a partial positive charge attracts the partial negative charge of neighboring electronegative atoms. Most often larger oxygen or nitrogen atoms.

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60
Q

Surface tension

A

A measure of the difficulty of stretching or breaking the surface of liquid.

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61
Q

Chemical reaction

A

Occurs when new bonds form or old bonds break between atoms

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62
Q

Reactants

A

The starting substance in a chemical reaction

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63
Q

Products

A

The ending substances in a chemical reaction

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64
Q

Energy

A

The capacity to do work

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65
Q

Each chemical reaction involves ______ changes.

A

Energy

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66
Q

Potential energy

A

Energy stored by matter due to its position

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67
Q

Kinetic energy

A

The energy associated with matter in motion

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68
Q

Examples of kinetic energy

A

Energy stored in water behind a dam or a person poised to jump down some steps

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69
Q

Chemical energy

A

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

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70
Q

The law of conservation of energy

A

Although energy can be neither created nor destroyed it may be converted from one form to another

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71
Q

Example of the law of conservation of energy

A

Some of the chemical energy in the foods we eat is eventually converted into various forms of kinetic energy such as mechanical energy used to walk and talk.

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72
Q

Exergonic reactions

A

Release more energy than they absorb.

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73
Q

Endergonic reactions

A

Absorb more energy than they release.

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74
Q

Activation energy

A

The collision energy needed to break the chemical bonds of the reactants

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75
Q

Concentration (As related to chemical reactions)

A

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

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76
Q

Temperature (as related to chemical reactions)

A

As the temperature rises particles of matter move about more rapidly. This the higher the temperature of matter the more forcefully particles will collide and the greater the chance of collision will produce a reaction.

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77
Q

Catalyst

A

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

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78
Q

Raising the temperature and the number of reacting particles of matter in the body could increase the frequency of collisions and thus increase the rate of chemical reactions but doing so could also damage or kill the body cells. What chemical compounds solve this problem?

A

Catalysts

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79
Q

Synthesis reactions

A

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

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80
Q

Anabolism

A

All synthesis reactions that occur in the body.

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81
Q

Decomposition reactions

A

Split up large molecules into smaller atoms, ions, or molecules

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82
Q

Catabolism

A

The decomposition reactions that occur in your body.

83
Q

Exchange reactions

A

Consist of both synthesis and decomposition reactions.

84
Q

Reversible reaction

A

The products can revert to the original reactants.

85
Q

Oxidation

A

The loss of electrons and in the process the oxidized substance releases energy

86
Q

Reduction

A

Refers to the gain of electrons and in the process the reduced substance gains energy.

87
Q

Oxidation reduction reactions

A

Are always parallel. When one substance is oxidized another is reduced at the same time.

88
Q

when a food molecules such as glucose is oxidized the energy produced is used by a cell to carry out its various functions. What is this called?

A

Oxidation reduction reaction

89
Q

Inorganic compounds

A

Usually lack carbon and are structurally simple. Their molecules also have only a few atoms and cannot be used by cells to perform complicated biological functions.

90
Q

Name some in organic compounds.

A

Water, many salts, acids and bases.

91
Q

Organic compounds

A

Always contain carbon usually contain hydrogen and always have covalent bonds. Most are large molecules and many are made up of long chains of carbon atoms.

92
Q

What percentage of the human body is made up of organic compounds?

A

38-43%

93
Q

What percent of an adult human body is made up of in organic compounds besides water?

A

1-2%

94
Q

What percentage of an adult human body is made up of water?

A

55 to 60%

95
Q

What is the most important and abundant inorganic compound in all living systems?

A

Water

96
Q

Solvent

A

The substance in a solution that dissolves another substance

97
Q

Solute

A

The substance in a solution that is dissolved by another substance

98
Q

Hydrophilic

A

Solutes that are charged or contain polar covalent bonds.

99
Q

Hydrophobic

A

Molecules that contain mainly nonpolar covalent bonds

100
Q

Hydrolysis

A

Decomposition of a compound by reaction with water.

101
Q

During digestion decomposition reactions breakdown large nutrient molecules into smaller molecules by the addition of water molecules. What kind of reaction is this?

A

Hydrolysis

102
Q

Mixture

A

A combination of elements or compounds that are physically blended together but not bound by chemical bonds.

103
Q

Solution

A

?

104
Q

Colloid

A

?

Example milk

105
Q

Suspension

A

In a solution material that may mix with the liquid or suspending medium for some time but eventually settles out

106
Q

Concentration

A

?

107
Q

Percentage

A

One common way to express the concentration of a solution which gives the relative mass of the solute found in a given volume of solution

108
Q

Moles per liter

A

A way to express concentration of a solution in units which relates to the total number of molecules in a given volume of a solution

109
Q

Mole

A

The amount of any substance that has a mass in grams equal to the sum of the atomic masses of all it’s atoms

110
Q

Disociate

A

When inorganic, acids, bases or salts dissolved in water they separate into ions and become surrounded by water molecules

111
Q

Acid

A

A substance that disassociates into one or more hydrogen ions and one or more anions

112
Q

Proton donor

A

Acid

113
Q

Base

A

Removes hydrogen ions from a solution and is therefore a proton acceptor

114
Q

What is another name for a base?

A

Proton acceptor

115
Q

Hydroxide ions

A

?

116
Q

A salt Does what when dissolved in water?

A

When dissolved in water dissociates into cations and anions neither of which is hydrogen ions or hydroxide ions

117
Q

Ph scale

A

The scale in which a solution’s acidity or alkalinity is expressed

118
Q

Buffer systems

A

Function to convert strong acids or bases into weak acids or bases

119
Q

Even though strong acids and bases are continually taken into and formed by the body, the pH of fluids inside and outside cells remains almost constant. Why?

A

The buffer system

120
Q

Buffers

A

The chemical compounds that can convert strong acids or bases into weak ones.

121
Q

Carbonic acid-bicarbonate buffer system

A

Can compensate for either an excess or shortage of hydrogen ions

122
Q

Hydrocarbon

A

Carbons that are bonded to hydrogen

123
Q

Carbon skeleton

A

The chain of carbon atoms in an organic molecule

124
Q

Macromolecules

A

Small organic molecules that combine into very large molecules

125
Q

Polymers

A

A large molecule formed by the covalent bonding of an identical or similar small building block molecules called monomers

126
Q

Monomers

A

Small building block molecules

127
Q

Isomers

A

Molecules that have the same molecular formula but different structures

128
Q

Carbohydrates

A

Organic compounds that have several functions. Sugars, glycogen, starches and cellulose. Function mainly as a source of chemical energy for generating ATP needed to drive metabolic reactions

129
Q

Simple sugars

A

Monosaccharides and disaccharides.

130
Q

Monosaccharides

A

The monomers (Small building blocks of molecules) of carbohydrates

131
Q

Disaccharide

A

A molecule formed from the combination of two monosaccharides by dehydration synthesis

132
Q

Polysaccharides

A

A major group of carbohydrates. Each polysaccharide molecule contains tens or hundreds of monosaccharides joined to dehydration synthesis

133
Q

Glycogen

A

The main polysaccharide in the human body which is made entirely of glucose monomers linked to one another in branching chains.

134
Q

Starches

A

Polysaccharides formed from glucose by plants

135
Q

Cellulose

A

A Polysaccharide formed from glucose by plants cannot be digested by humans but does provide bulk to eliminate feces

136
Q

Lipids

A

Important group of organic compounds. Make up 18 to 25% of body mass in lean adults

137
Q

Liptoteins

A

To become more soluble in blood plasma other lipid molecules join with Hydrophilic protein molecules

138
Q

Types of lipids in the body. Pg 47

A

Fatty acids. Triglycerides. Phospholipids. Steroids. Eicosanoids.

139
Q

Fatty acids

A

Among the simplest lipids which are used to synthesize triglycerides and phospholipids

140
Q

Saturated fatty acid

A

Contains only single covalent bonds between carbon atoms of the hydrogen carbon chain.

141
Q

Unsaturated fatty acid

A

Contains one or more double covalent bonds between carbon atoms of the hydrocarbon chain

142
Q

Triglycerides/triacyglycerols

A

The most plentiful lipids in your body and in your diet

143
Q

Glycerol

A

A three carbon molecule that forms the backbone of a triglyceride

144
Q

Fat

A

A triglyceride that is a solid at room temperature

145
Q

Saturated fat

A

A fat but mainly consists of saturated fatty acids

146
Q

Oil

A

A triglyceride that is liquid at room temperature

147
Q

Monosaturated fats

A

Contain triglycerides that mostly consist of monounsaturated fats
Olive oil peanut oil canola oil most nuts and avocado

148
Q

Polyunsaturated fats

A

Contain triglycerides that mostly consists of polyunsaturated fatty acids. Corn oil safflower oil sunflower oil soybean oil fatty fish

149
Q

Phospholipids

A

Have a glycerol Backbone and two fatty acid chains attached the first two carbons

150
Q

Amphipathic

A

Molecules that have both polar and nonpolar parts

151
Q

Steroids

A

Have four rings of carbon atoms

152
Q

Sterols

A

Steroids I that have at least one hydroxyl group (Not 100% sure on this definition)

153
Q

Eivosanoids

A

Lipids derived from a 20 carbon fatty acid called arachidonic acid.

154
Q

Prostaglandins

A

Modify responses to hormones, contribute to the inflammatory response, prevent stomach ulcers, dilate airways to lungs, regulate body temperature and influence formation of blood clots. One of two principal subclasses of eicosanoids

155
Q

Leukotrienes

A

Participate in allergic and inflammatory responses. A subclass of eicosanoids

156
Q

Proteins

A

Large molecules that contain carbon, hydrogen, oxygen and nitrogen. Some proteins also contain sulfur. A normal lean adult body is 12 to 18% protein.

157
Q

Amino acids

A

Monomers of proteins.

158
Q

How many different types of amino acids are there?

A

20

159
Q

True or false each amino acid has a hydrogen Adam and three important functional groups?

A

True

160
Q

What are the three important functional groups attached to a central Carbon atom of an amino acid?

A

An amino group, and acidic carboxyl group, and a side chain

161
Q

Peptide bond

A

The covalent bond joining each pair of amino acids

162
Q

Structural protein

A

Form structural framework of various parts of the body

Example collagen in bone and other connective tissue

163
Q

Regulatory protein

A

Function as hormones that regulate various physiological processes; control growth and development; as neurotransmitters, mediate responses of nervous system
Example insulin

164
Q

Contractile

A

Allow shortening of muscle cells which produces movement.

Examples myosin and actin

165
Q

Immunological protein

A

Aid responses that protect body against foreign substance and invading pathogens.
Examples antibodies, interleukins

166
Q

Transport proteins

A

Carry vital substances throughout the body.

Example hemoglobin transports most oxygen and some carbon dioxide in the blood.

167
Q

Catalytic protein

A

Act as enzymes that regulate biochemical reactions.

Example salivary amylase, sucrase, ATPase

168
Q

Dipeptide

A

The combination of two amino acids

169
Q

Tripeptide

A

The combination of three amino acids

170
Q

Peptide

A

4 to 9 amino acids

171
Q

Polypeptide

A

10 to 2000 or more amino acids

172
Q

Primary structure

A

The unique sequence of amino acids that are linked by covalent peptide bonds to form a polypeptide chain

173
Q

Sickle cell disease

A

When a nonpolar amino acid replaces a polar amino acid through two mutations in the oxygen-carrying protein hemoglobin. This change amino acids diminishes hemoglobins water solubility. As a result the altered hemoglobin tends to form crystals inside the red blood cells producing deformed sickle shaped cells that cannot properly squeeze through narrow blood vessels

174
Q

How many levels of structural organization do proteins have?

A

Four

175
Q

What are the four levels of structural organization in protein?

A

Primary structure, secondary structure, tertiary structure, quaternary structure.

176
Q

Secondary structure of proteins

A

The repeated twisting or folding of neighboring amino acids in the polypeptide chain.

177
Q

What are the two common secondary structures of protein?

A

Alpha helixes and beta-pleated sheets

178
Q

Tertiary Structure of protein

A

Three-dimensional shape of the polypeptide chain.

179
Q

True or false each protein has the same tertiary structure determines how it will function.

A

False each protein has a unique tertiary structure

180
Q

Quaternary structure of protein

A

In those proteins that contain more than one polypeptide chain the arrangement of the individual polypeptide chains relative to one another.

181
Q

Fibrous proteins

A

In soluble in water and their polypeptide chains formed long strands are parallel to each other

182
Q

What are some structural Functions of fibrous proteins?

A

Collagen (strengthens bones, ligaments and tendons)
Elastin - provides stretch and skin, blood vessels, and lung tissue
Keratin - Forms structure of hair and nails and waterproofs the skin
More on page 54

183
Q

Globular proteins

A

Are more or Less soluble in water and their polypeptide chains and are spherical in shape

184
Q

Denaturation

A

When a protein encounters an altered environment and unravels and loses its characteristic shape

185
Q

Enzymes

A

In living cells most catalysts are protein molecules

186
Q

Apoenzyme

A

In some enzymes; the protein portion

187
Q

Cofactor

A

Nonprotein portion of an enzyme

188
Q

Substrate

A

The specific reactant molecules on which the enzyme acts

189
Q

Active site

A

In some cases the part of the enzyme that catalyzes the reaction

190
Q

Enzyme substrate complex

A

The subtrates make contact with the active site on the surface of the enzyme molecule, forming a temporary intermediate compound

191
Q

Nucleic acid

A

Huge organic molecules that contain carbon, hydrogen, oxygen, nitrogen and phosphorus

192
Q

DNA - deoxyribonucleic acid

A

Forms the inherit genetic material inside each human cell

193
Q

Gene

A

A segment of a DNA molecule

194
Q

Ribonucleic acid - RNA

A

The second type of nucleic acid that relays instructions from the genes to guide each cells synthesis of proteins from amino acids

195
Q

Nucleotides

A

The repeating chain of monomers that build nucleic acid.

196
Q

Nitrogenous bases

A

Adenine, thymine, cytosine, and guanine.

197
Q

Adenine and guanine Are larger double ring bases called

A

Purines

198
Q

Pyrimidines

A

Smaller single ring bases; thymine and cytosine

199
Q

Each nucleotide of DNA consists of what three parts?

A

Nitrogenous base, pentose sugar, phosphate group

200
Q

Pentode sugar

A

A five carbon sugar called deoxyribose attaches to each Base in DNA

201
Q

Double helix

A

A spiral ladder model of DNA

202
Q

Ribose

A

The sugar in the RNA nucleotide

203
Q

DNA fingerprinting

A

A technique used in the research and in courts of law to ascertain whether a person’s DNA matches the DNA obtained from samples or pieces of legal evidence such as blood stains or hairs

204
Q

Adenosine triphosphate - ATP

A

The energy currency of living systems

205
Q

Adenosine diphosphate - ADP

A

A molecule that results from the removal of the third phosphate group in ATP

A&P I & II (16 decks)

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