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Anatomy and Physiology 1 > Chapter Two: Chemistry > Flashcards

Chapter Two: Chemistry Flashcards

1
Q

Matter

A

Anything that occupies space and has mass

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2
Q

States of Matter

A

Solid, Liquid, or Gas

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3
Q

Energy

A

The capacity to do work or put matter into motion

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4
Q

Two types of energy

A

Kinetic and Potential

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5
Q

What is an atomic symbol

A

One of two letter chemical shorthand for each element

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6
Q

What is the atomic number?

A
  • Element’s defining trait
  • Tells the number of protons and electrons

Top number above the atomic symbol

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7
Q

Where is the atomic mass found?

A

Bottom number

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8
Q

What is the formula to find number of neutrons?

A

Atomic mass - atomic number = neutrons

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9
Q

What charge are protons?

A

Positive

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10
Q

What charge are electrons?

A

Negative

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11
Q

What is the formula to find number of nucleons?

A

Protons + Neutons

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12
Q

What is the backbone of biological macromolecules?

A

Carbon

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13
Q

What are physical elements?

A

Detectable with our senses

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14
Q

What are chemical elements?

A

How atoms interact and bond with one another

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15
Q

What 4 elements make up 96.1% of the body’s mass?

A

Hydrogen
Oxygen
Carbon
Nitrogen

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16
Q

Which 9 elements make up 3.9% of body mass

A

Calcium
Phosphorus
Potassium
Sulfur
Chlorine
Magnesium
Iodine
Iron

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17
Q

What are trace elements?

A

Very minute mounts of 11 elements that make up less than 0.01% of the body’s mass

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18
Q

Chemical energy

A

Stored in bonds of chemical substances

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19
Q

Electrical energy

A

Results from movement of charged particles

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20
Q

Mechanical energy

A

Directly involved in moving matter

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21
Q

Atoms

A

- Smallest stable unit of matter
- Unique building blocks for each element
- Give each element its physical & chemical properties
- Smallest particles of an element with properties of that element

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22
Q

Atoms are composed of __ particles

A

subatomic particles

Protons, neutrons, and electrons

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23
Q

Protons, neutrons, and electrons are

A

Subatomic particles

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24
Q

Where are protons located?

A

In the nucleus

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25
Q

Where are neutrons located?

A

In the nucleus

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26
Q

Where are electrons located?

A

In orbit in an electron cloud

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27
Q

What is the charge and mass of protons?

A
  • positive charge
  • Mass = 1 amu
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28
Q

What is the charge and weight of a neutron?

A
  • no charge
  • Mass = 1 atomic mass unit (amu)
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29
Q

What is the charge and weight of an electron?

A
  • Negative charge
  • o amu
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30
Q

Number of __tons and __trons are always equal

A

Number of protons and electrons are always equal

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31
Q

Atomic number

A
  • Number of protons in nucleus of the atom
    Written as subscript to left of atomic symbol
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32
Q

Mass number

A
  • Total number of protons and neutrons in nucleus of the atom
  • Total mass of atom
  • Written as superscript to left of atomic symbol
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33
Q

What are Isotopes?

A
  • Structural variations of atoms
  • Differ in the number of neutrons they contain
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34
Q

Atomic weight

A

Average of mass numbers (relative weights) of all isotopes of an atom

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35
Q

Radioisotopes

A
  • Heavy isotopes decompose to more stable forms
  • Similar to tiny explosion
  • Can transform into different element
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36
Q

__ are energy relationships between electrons of reacting atoms

A

Chemical bonds

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37
Q

Electrons can occupy up to __ electron shells (energy levels) around nucleus

A

7

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38
Q

Valence shell

A
  • outermost electron shell
  • Electrons here have most potential energy and are chemically reactive electrons
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39
Q

Octet rule

A

Except for the first shell (full with two electrons) atoms interact to have eight electrons in their valence shell

Rule of 8’s

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40
Q

Chemically Inert Elements

A
  • Stable and unreactive
  • Valence shell fully occupied or contains eight electrons
  • Noble gases
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41
Q

Chemically reactive elements

A
  • Valence shell is not full
  • Tend to gain, lose, or share electrons to achieve stability
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42
Q

Three major types of chemical bonds

A

Ionic
Covalent
Hydrogen

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43
Q

Ions

A

Atom gains or loses electrons and becomes charged

When the number of Protons ≠ Number of Electrons

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44
Q

Anion

A

Atom that gained one or more electrons

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45
Q

Atom that gained one or more electrons

A

Anion

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46
Q

Cation

A

Atom that lost one or more electrons

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47
Q

Atom that lost one or more electrons

A

Cation

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48
Q

Attraction of opposite charges results in an __ bond

A

ionic

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49
Q

Covalent bonds

A
  • Formed by sharing of two or more valence shell electrons
  • Allows each atom to fill its valence shell at least part of the time
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50
Q

Nonpolar covalent bonds

A
  • Electrons shared equally
  • Produces electrically balanced, nonpolar molecules such as CO2
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51
Q

Small atoms with six or seven valence shell electrons are __

A

electronegative

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52
Q

Most atoms with one or two valence shell electrons are __

A

electropositive

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53
Q

Ionic bond

A

Complete transfer of electrons

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54
Q

Polar covalent bond

A

Unequal sharing
of electrons

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55
Q

Nonpolar covalent bond

A

Equal sharing of
electrons

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56
Q

Molecule

A
  • Two or more atoms bonded together
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57
Q

Compound

A

Two or more different kinds of atoms bonded together
(Can only be seperated by breaking bonds)

All are homogeneous

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58
Q

Mixture

A

Two or more components physically intermixed
(No chemical bonding between components - Can be separated by physical means, such as straining or filtering)

Heterogeneous and homogeneous

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59
Q

Three types of mixtures

A
  • Solutions
  • Colloids
  • Suspensions
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60
Q

Homogeneous mixtures

A

Solutions

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61
Q

Heterogeneous mixtures

A

Colloids
Suspensions

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62
Q

Solvent

A
  • Substance present in great amount in a mixture
  • usually water
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63
Q

Solute

A

smaller amounts in a mixture, dissolved in a solvent

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64
Q

Colloids

A

Emulsions
- large solute particples do not settle out

ex: jello

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65
Q

Suspensions

A

Large visible solutes settle out

EX: blood

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66
Q

Chemical reactions occur when

A

chemical bonds are formed, rearranged, or broken

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67
Q

Patterns of chemical reactions

A
  • synthesis
  • decomposition
  • exchange
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68
Q

reactants

A

The number and kinds of the interacting substances

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69
Q

products

A

The chemical composition of the result of the reaction

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70
Q

The number and kinds of the interacting substances

A

Reactants

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71
Q

The chemical composition of the result of the reaction

A

Products

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72
Q

When atoms or molecules combine to form a larger, more complex molecule

A

Synthesis

73
Q

a molecule is broken down into smaller molecules or its constituent atoms

A

Decomposition

74
Q

What type of reaction includes both synthesis and decomposition?

A

Exchange/displacement

75
Q

Bonds formed by sharing of two or more valence shell electrons

A

Covalent bonds

76
Q

Acidosis

A

A condition of acidity or low pH (below 7.35) of the blood
- high hydrogen ion concentration

77
Q

Alkalosis

A
  • A condition of basicity or high pH (above 7.45) of the blood
  • low hydrogen ion concentration.
78
Q

Most ionic compounds are __

A

salts

79
Q

Attraction of opposite charges results in an ___ bond

A

ionic

80
Q

Atoms with one or two valence shell electrons are

A

electropositive

81
Q

What is the difference between nonpolar and polar covalent bonds?

A

Nonpolar covalent bonds : electrons are shared equally, and balanced nonpolar molecules are produced
Polar covalent bond: unequal sharing of electrons - can be electronegative or electropositive

82
Q

How can compounds be separated?

A

Only by breaking bonds

83
Q

Stored in bonds of chemical substances

A

Chemical energy

84
Q

Results from movement of charged particles

A

Electrical energy

85
Q

Directly involved in moving matter

A

Mechanical energy

86
Q

Elements

A

– Matter is composed of elements
– Elements cannot be broken into simpler
substances by ordinary chemical methods

87
Q

Which property is detectable with our senses/measurable?

A

Physical

88
Q

Which property relates to how atoms bond with one another?

A

Chemical

89
Q

___ are energy relationships between electrons of reacting atoms

A

Chemical bonds

90
Q

Electrons in valenceshell
- Have most ___ energy
– Are chemically __electrons

A

Potential energy
Chemically reactive

91
Q

In terms of reactivity and stability, noble gases are ___ and ____

A

stable and unreactive

92
Q

Chemically Reactive Elements tend to ___ with other atoms to achieve stability

A

gain, lose, or share electrons

93
Q

Anion is what charge

A

Negative

94
Q

Cation is what charge

A

positive

95
Q

Attraction of opposite charges results in a(n) ___ bond

A

Ionic

96
Q

Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule results in which bond?

A

Hydrogen bond

97
Q

Which reaction is this?

Atoms or molecules combine to form larger, more complex molecule
– Always involve bond formation
– Anabolic

A

Synthesis

98
Q

In a synthesis reaction, __ particles are bonded together to form larger, more complex molecules

A

smaller

99
Q

Which reaction is this?

– Molecule is broken down into smaller
molecules or its constituent atoms * Reverse of synthesis reactions
– Involve breaking of bonds
– Catabolic

A

Decomposition

100
Q

What type of reaction is shown here?

AB → A + B

A

Decomposition

101
Q

What type of reaction is shown here?

A + B → AB

A

Synthesis

102
Q

Which reaction is this?

– Also called displacement reactions
– Involve both synthesis and decomposition – Bonds are both made and broken

A

Exchange

103
Q

What type of reaction is shown here?

AB + C → AC + B

A

Exchange

104
Q

Exergonic Reactions

net __ of energy

A

Release

105
Q

Exergonic reactions

Products have __ potential energy than reactants

A

less

106
Q

Endergonic reactions

net __ of energy

A

Absoption

107
Q

All chemical reactions are theoretically __

A

reversible

108
Q

Chemical equilibrium occurs if neither a forward nor reverse reaction is __

A

dominant

109
Q

Why are most biological reactions essentially irreversible?

A

energy requirements and removal of products

110
Q

Catalysts: ↑ Rate without being chemically ___ or part of product

A

changed

111
Q

___ are biological catalysts

A

Enzymes

112
Q

What affects the rate of chemical reactions?

A

Temperature
Concentration of reactant
Particle size

113
Q

Biochemistry is defined as

A

Study of chemical composition and reactions of living matter

114
Q

Water, salts, and many acids and bases are examples of which class of compound?

A

Inorganic

115
Q

Carbohydrates, fats, proteins, and nucleic
acids are examples of which class of compound?

A

organic compounds

116
Q

Which classification of compound contains carbon?

A

organic

117
Q

What is the most important inorganic compound?

A

Water

118
Q

What is the most abundant inorganic compound? What percent of volume does it make up in living cells?

A

Water, and it makes up 60-80% of the volume of living cells

119
Q

Water has a __ heat capacity
and a __ heat of vaporization

A

high heat capacity and high heat of vaporization

120
Q

Salts

A

Ionic compounds that dissociate into ions in water

121
Q

Ions (electrolytes) conduct __ currents in solution

A

electrical

122
Q

Acids and Bases
- __ are electrolytes
- Ionize and __ in water

A
  • Both
  • dissociate
123
Q

Acids and Bases
- Both are __
- __ and dissociate in water

A
  • electrolytes
  • ionize
124
Q

Acids are __ donors

A

proton

125
Q

Acids are proton __

A

donors

126
Q

Bases are __ acceptors

A

proton

127
Q

Bases are proton __

A

acceptors

128
Q

Acids release __ in solution

A

H+

129
Q

Take up H+ from solution

A

Bases

130
Q

Bases take up __ from solution

A

H+

131
Q

As free [H+] increases, __ increases

A

acidity

132
Q

As free [H+] decreases __ increases

A

alkalinity

133
Q

What type of solution is being described?

[H+], ↓ pH

A

An acidic solution

134
Q

What type of solution is being described?

[H+], ↑ pH

A

A basic solution
- Alkaline

135
Q

Acidic pH values:

A

0–6.99

136
Q

Alkaline pH values:

A

7.01–14

137
Q

All neutral solutions are pH __

A

7

138
Q

Results from mixing acids and bases

A

Neutralization

139
Q

pH is regulated by ___

A

kidney, lungs, and chemical buffers

140
Q

Biological macromolecules

A

Carbohydrates, lipids, proteins, and nucleic acids

141
Q

Polymers are __

A

chains of monomers that are similar units

142
Q

Which biological macromolecule is not a polymer?

A

lipids

143
Q

Biological macromolecules are synthesized by __

A

dehydration synthesis

144
Q

Biological macromolecules are __ by dehydration synthesis

A

synthesized

145
Q

Biological macromolecules are broken down by __ reactions

A

hydrolysis

146
Q

Hydrolysis

A

Water molecule breaks down one or more chemical bonds

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

147
Q

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

148
Q

What are the three classes of carbohydrates?

A

Monosaccarides
Disaccharides
Polysaccharides

149
Q

What are the functions of carbohydrates?

A
  • Major source of cellular fuel
  • Structural molecules
150
Q

Simple sugars containing three to seven C atoms

A

Monosaccharides

151
Q

Double sugars that are too large to pass through cell membranes

A

Disaccharides

152
Q

Sucrose, maltose, and lactose are what type of saccharides?

A

Disaccharides

153
Q

Long chains of linked monosaccharides

A

Polysaccharides

154
Q

Starch and glycogen are what type of saccharides?

A

Polysaccharides

155
Q

Are polysaccharides soluble?

A

Polysaccharides are not very soluble

156
Q

What are the main types of lipids?

A
  • Neutral fats or triglycerides
  • Phospholipids
  • Steroids
157
Q

solubility

Lipids are __ in water

A

Insoluble

158
Q

Neutral Fats or Triglycerides are called __ when solid and __ when liquid

A

fats when solid, oil when liquid

159
Q

Triglycerides are comprised of __

A

Three fatty acids bonded to a glycerol molecule

160
Q

What are the main functions of triglycerides?

A
  • energy storage
  • insulation
  • protection
161
Q

Solid animal fats are __ fatty acids

A

saturated

162
Q

olive oil is an example of a(n) __ fatty acid

A

unsaturated

163
Q

Single covalent bonds between C atoms make up

A

saturated fatty acids

164
Q

One or more double bonds between C atoms make up

A

unsaturated fatty acids

165
Q

Phosholipids are important for __

A

cell membrane structure

166
Q

What is the most important steroid?

A

Cholesterol

167
Q

Important in cell membranes, vitamin D synthesis, steroid hormones, and bile salts

A

Cholesterol

168
Q

Lipoproteins transport __ in the blood

A

fats

169
Q

__ are the monomers in proteins

A

amino acids

170
Q

What are the 4 sequences of protein structure?

A
  1. Primary structure:
    The sequence of amino acids forms the polypeptide chain.
  2. Secondary structure:
    The primary chain forms spirals (α-helices) and sheets (β-sheets).
  3. Tertiary structure:
    Superimposed on secondary structure. α-Helices and/or β-sheets are folded up to form a compact globular molecule held together by intramolecular bonds.
  4. Quaternary structure:
    Two or more polypeptide chains, each with its own tertiary structure, combine to form a functional protein.
171
Q

keratin, elastin, and collagen are examples of what proteins?

A

Fibrous

172
Q

Fibrous (structural) proteins provide __ support and __ strength

A

mechanical support and tensile strength

173
Q

antibodies, hormones, molecular chaperones, and enzymes are examples of what proteins?

A

Globular (functional)

174
Q

Proteins that are compact, spherical, water-soluble and sensitive to environmental changes

A

Globular

175
Q

Proteins that are standlike, water-insoluble, and stable

A

Fibrous proteins

176
Q

What can cause protein denaturation?

A

Decreased pH or increased temperature

177
Q

When denaturization occurs, Globular proteins __

A

unfold and lose shape

178
Q

Globular proteins that act as biological catalysts

A

Enzymes

179
Q

what is the function of Catalysts

A

regulate and increase speed of chemical reactions

Anatomy and Physiology 1 (9 decks)

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