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Anatomy and Physiology 1 > Chemistry Comes Alive > Flashcards

Chemistry Comes Alive Flashcards

1
Q

Our body is made up of many _____

A

Chemicals

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2
Q

Chemistry underlies all physiological reactions including:

A

Movement
Digestion
Pumping of the Heart
Nervous System

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3
Q

Chemistry can be broken down in to:

A

Basic Chemistry

Biochemistry

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4
Q

Anything that has mass and occupies space

A

Matter

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5
Q

Mass plus the effects of gravity is called ____

A

Weight

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6
Q

Definite shape and volume

A

Solid

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7
Q

Changeable shape; definite volume

A

Liquid

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8
Q

Changeable shape and volume

A

Gas

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9
Q

Capacity to do work or put matter into motion

A

Energy

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10
Q

Energy in action

A

Kinetic Energy

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11
Q

Stored (inactive) energy

A

Potential Energy

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12
Q

Energy can be transformed from _____ to _____.

A

Potential

Kinetic

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13
Q

Stored in bonds of chemical substances

A

Chemical Energy

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14
Q

Results from movement of charged particles

A

Electrical Energy

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15
Q

Directly involved in moving matter

A

Mechanical Energy

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16
Q

Travels in waves

A

Radiant or Electromagnetic Energy

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17
Q

All matter is composed of _____.

A

Elements

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18
Q

Substances that cannot be broken down into simpler substances by ordinary chemical methods

A

Elements

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19
Q

Four elements make up 96% of the body:

A

Carbon
Oxygen
Hydrogen
Nitrogen

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20
Q
  • Unique building blocs for each element
  • Smallest particles of an element with properties of that element
  • What give each element its particular physical and chemical properties
A

Atoms

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21
Q
  • Carry a positive charge

- Have an arbitrary 1 atomic mass unit

A

Proton

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22
Q
  • Have no electrical charge

- Have an arbitrary 1 atomic mass unit

A

Neutron

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23
Q
  • Carry a negative charge

- Are so tiny they have virtually no weight

A

Electron

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24
Q

Simplified and outdated because it incorrectly depicts electrons in and “orbit”

A

Planetary Model

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25
Q

Current model used that depicts orbitals rather than fixed orbits

A

Orbital Model

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26
Q

Total number of protons AND neutrons in an element

A

Mass Number

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27
Q
  • Structural variations of the same element

- Atoms contain same number of protons but sometimes differ in the number of neutrons they contain

A

Isotopes

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28
Q

Average of mass numbers of all isotope forms of an atom

A

Atomic Weight

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29
Q

Isotopes that decompose to more stable forms

A

Radioisotopes

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30
Q

Sometimes loss of various subatomic particles causes and isotope to become a _____ _____.

A

Different Element

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31
Q

Energy that is released when an isotope’s subatomic particles are being decayed

A

Radioactivity

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32
Q

General term for 2 or more atoms bonded together

A

Molecule

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33
Q

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

A

Compound

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34
Q

Two or more components that are physically intermixed

A

Mixture

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35
Q

Homogeneous mixtures, meaning particles are evenly distributed throughout

A

Solution

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36
Q

Substance present in greatest amount (usually a liquid)

A

Solvent

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37
Q

Substance dissolved in solvent and present in smaller amounts

A

Solute

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38
Q

Heterogeneous mixtures, meaning that particles are not evenly distributed throughout the mixture

A

Colloids (also known as emulsions)

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39
Q

Some colloids undergo a “sol-gel” or ___ ___ ___ transformation

A

Solution to Gel

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40
Q

Heterogeneous mixtures that contain large, visible solutes that DO settle out

A

Suspensions

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41
Q

Mixtures do not involve _____ _____ between components, unlike compounds.

A

Chemical Bonding

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42
Q

Mixtures can be separated by ______ _____, such as straining or filtering

A

Physical Means

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43
Q

Compounds can be separated only by breaking their _____ _____/

A

Chemical Bonds

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44
Q

Mixtures can be heterogeneous or homogeneous, compounds can only be ______.

A

Homogeneous

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45
Q

“Energy relationships” between electrons of reacting atoms

A

Chemical Bonds

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46
Q

Electrons are the ______ ______ that are involved in all chemical reactions.

A

Subatomic Particles

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47
Q

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

A

Electrons

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48
Q

Electrons can occupy areas around a nucleus called the _____ _____.

A

Electron Shell

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49
Q

Each electron shell contains electrons that have a certain amount of kinetic and potential energy, so shells are also referred to as ____ _____.

A

Energy Levels

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50
Q

Depending on its size, and atom can have up to ____ electron shells.

A

7

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51
Q

Shells can hold only a specific number of _____.

A

Electrons

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52
Q

The shell closest to the _____ is filled first.

A

Nucleus

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53
Q

Outermost electron shell is called the _____ _____.

A

Valence Shell

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54
Q
  • Atoms desire ____ electrons in their valence shell

- Desire to have ___ electrons is the driving force behind chemical reactions.

A

8 (Octet Rule)

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55
Q

Most atoms do not have full _____ _____.

A

Valence Shells

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56
Q

Atoms that have gained or lost electrons and have become charged

A

Ions

57
Q

Involve the TRANSFER of valence shell electrons from one atom to another

A

Ionic Bonds

58
Q

Attraction of ____ charges result in an ionic bond

A

Opposite

59
Q

Most ionic bonds form _____.

A

Salts

60
Q

Formed by sharing two or more valence shell electrons between two atoms

A

Covalent Bonds

61
Q
  • Equal sharing of electrons between atoms

- Results in electrically balanced, nonpolar molecules

A

Nonpolar Covalent Bonds

62
Q
  • Unequal sharing of electrons between 2 atoms
  • Results in electrically polar molecule
  • Atoms have different electron-attracting abilities, leading to unequal sharing
A

Polar Covalent Bonds

63
Q

Atoms with a greater electron-attracting ability

A

Electronegative

64
Q

Atoms with a less electron-attracting ability

A

Electropositive

65
Q
  • Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule
  • Not a true bond, more of a weak magnetic attraction
A

Hydrogen Bonds

66
Q

Occur when chemical bonds are formed, rearranged or broken

A

Chemical Reactions

67
Q

Chemical reactions can be written in symbolic form called ____ _____.

A

Chemical Equations

68
Q

Substances entering in to a reaction together

A

Reactants

69
Q

Resulting chemical end products

A

Products

70
Q

Involve atoms or molecules combining to form larger, more complex molecule

A

Synthesis Reactions

71
Q

Involve breakdown of a molecule into smaller molecules or its constituent atoms

A

Decomposition Reactions

72
Q

Involve both synthesis and decomposition

A

Exchange (or Displacement) Reactions

73
Q

In living systems, these reactions are also referred to as _____ _____ or _____ reactions.

A

Reduction-Oxidation

Redox

74
Q

Atoms are _____ when they gain electrons.

A

Reduced

75
Q

Atoms are _____ when they lose electrons

A

Oxidized

76
Q

All chemical reactions are either ______ or ______.

A

Exergonic

Endergonic

77
Q
  • Result in a net release of energy (give off energy)
  • Products have less potential energy than reactants
  • Catabolic and oxidative reactions
A

Exergonic Reactions

78
Q
  • Result in a net absorption of energy (use up energy)
  • Products have more potential energy than reactants
  • Anabolic rections
A

Endergonic Reactions

79
Q

Increased _____ usually increases the rate of the reaction

A

Tempera
Concentration
Particle Size (smaller)
Catalysts

80
Q

Substances that increase rxn rate without themselves being changed (enzymes)

A

Catalysts

81
Q

The study of chemical composition and reactions of living matter

A

Biochemistry

82
Q

Water, salts, and many acids and bases are____.

Do not contain carbon

A

Inorganic Compounds

83
Q

Carbohydrates, fats, proteins, and nucleic acids are____.

Contain carbon, are usually large, and are covalently bonded

A

Organic Compounds

84
Q
  • Most abundant inorganic compound
  • High heat capacity and heat of vaporization
  • Polar solvent properties
  • Reactivity
  • Cushioning
A

Water

85
Q

Ionic compounds that dissociate into separate ions in water

A

Salts

86
Q

Salts separate into _____ and _____.

A

Cations

Anions

87
Q

Positively charged molecules

A

Cations

88
Q

Negatively charged molecules

A

Anions

89
Q

All ions are called _____ because they can conduct electrical currents in solutions

A

Electrolytes

90
Q

Ionic balance is vital for _______.

A

Homeostasis

91
Q

_______ play a big role in maintaining proper balance of electrolytes

A

Kidneys

92
Q

If electrolyte balance is _____, virtually all organ systems cease to function.

A

Disrupted

93
Q

_____ are proton donors.

A

Acids

94
Q

Release hydrogen ions and bare protons into a solution

A

Proton Donors

95
Q

_____ are proton acceptors.

A

Bases

96
Q

The pick up hydrogen ions in a solution,

A

Proton Acceptors

97
Q

Measurement of concentration of hydrogen ions in a solution

A

pH Scale

98
Q

The more hydrogen ions in a solution, the more _____ it is.

A

Acidic

99
Q

Resist abrupt and large swings in pH

A

Buffers

100
Q

_____ can convert strong acids or bases into weak ones.

A

Buffers

101
Q

Organic molecules contain _____

A

Carbon

102
Q

Carbon is _______

A

Electroneutral

103
Q
  • Shares electrons; never gains or loses them
  • Forms four covalent bonds with other elements
  • Carbon is unique to living systems
A

Electronuetral (Carbon)

104
Q

Include sugar and starches

A

Carbohydrates

105
Q

One single sugar

A

Monosaccharides

106
Q

Smallest unit of carbohydrate

A

Monomers

107
Q

Two sugars

A

Disaccharides

108
Q

Many sugars

A

Polysaccharides

109
Q

_____ are made up of monomers of monosaccharides

A

Polymers

110
Q

Simple sugars containing three to seven carbon atoms

A

Monosaccharides

111
Q

Ribose and deoxyribose

A

Pentose Sugars

112
Q

Glucose

A

Hexose Sugars

113
Q
  • Double sugars
  • Too large to pass through cell membrane
  • Formed by dehydration synthesis of two momsaccharides
A

Disaccharides

114
Q
  • Polymers of monosaccharides
  • Formed by dehydration synthesis of many monomers
  • Not very soluble
A

Polysaccharides

115
Q
  • Contains C, H, O, but less than carbohydrates, and sometimes P
  • Insoluble in water
A

Lipids

116
Q
  • Called fats when solid and oils when liquid
  • Composed of three fatty acids bonded to a glycerol molecule
  • Used for energy storage, insulation, and protection
A

Triglycerides

117
Q
  • Modified triglycerides
  • Head is a polar region and is attracted to water
  • Tails are nonpolar and are repelled by water
  • Important in cell membrane structure
A

Phospholipids

118
Q
  • Consist of four interlocking ring structures
  • Most important steroid is cholesterol
  • Important in cell plasma membrane structure
A

Steroids

119
Q
  • Many different ones
  • Derived from a fatty acid found in cell membranes
  • Most important are prostaglandins
  • Play a role in blood clotting, control of blood pressure, inflammation, and labor contractions
A

Eicosanoids

120
Q
  • Comprise 20-30% of cell mass
  • Have most varied function of any molecule
  • Contain C, H, O, N, and sometimes S and P
A

Proteins

121
Q

All proteins are polymers made from ____ types of amino acids

A

20

122
Q

Four levels of protein structure determine ____ and _____.

A

Shape

Function

123
Q
  • Strandlike, water insoluble and stable
  • Most have tertiary or quaternary structure
  • Provide mechanical support and tensile strength
A

Fibrous (structural) Proteins

124
Q
  • Compact, spherical, water-soluble, and sensitive to environmental changes
  • Tertiary or quaternary structure
  • Specific functional regions (active sites)
A

Globular (functional) Proteins

125
Q
  • Globular proteins unfold and lose their functional 3-D shape
  • Can be caused by decreased pH or increased temperature
  • Usually reversible if normal conditions restored
  • Irreversible if changes are extreme
A

Denaturation

126
Q

Globular proteins that act as biological catalysts

A

Enzymes

127
Q

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

A

Catalysts

128
Q

Most functional enzymes

A

Holoenzymes

129
Q

Protein part of a holoenzyme

A

Apoenzyme

130
Q

Metal ion or organic molecule (often a vitamin) part a holoenzyme

A

Cofactor or Coenzyme

131
Q

Enzymes act on a very specific _____.

A

Substrate

132
Q
  1. Substrate binds to enzyme’s active site, temporarily forming ______-_____ complex.
  2. Complex undergoes rearrangement of _____, resulting in final product.
  3. Product is _____ from the enzyme.
A

Enzyme-substrate
Substrate
Released

133
Q

Composed of C,H, O, N, and P, are the largest molecules in the body

A

Nucleic Acids

134
Q

Made up of monomers called nucleotides and are composed of a nitrogen base, a pentose sugar and a phosphate group

A

Nucleic Acid Polymers

135
Q

Holds the genetic blueprint for the synthesis of all proteins

A

DNA

136
Q

Links DNA to protein synthesis and is slightly different from DNA

A

RNA

137
Q

Chemical energy released when glucose is broken down is captured in _____

A

ATP (adenosine triphosphate)

138
Q

ATP directly powers _____ _____ in cells and offers immediate, reusable energy needed by body cells

A

Chemical Reactions

Anatomy and Physiology 1 (2 decks)

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