Chapter 2 Flashcards
1
Q
Main Chemical Elements of Body
A
Matter, Chemical Element, Chemical Symbol, Major Elements, Lesser Elements, Trace Elements
2
Q
Define Matter
A
anything that occupies space. Includes Mass and Space
3
Q
Mass
A
the amount of matter in any object
4
Q
Weight
A
force of gravity acting on matter
5
Q
Chemical Element
A
All forms of matter. Both living and non-living are made up of a limited number of building blocks
6
Q
Chemical Symbol
A
Each element is a substance by ordinary chemical means, each named element is designated by a symbol, one or two letters of the elements name in English/Latin or another language
7
Q
Major Elements
A
96% of body’s mass. Include oxygen, carbon, hydrogen, and nitrogen
8
Q
Lesser Elements
A
3.6% of body’s mass. Include calcium phosphorus, potassium, sulfur, sodium, chlorine, magnesium, and iron
9
Q
Trace Elements
A
present in tiny amounts 0.4% of body mass
Include 14 elements
10
Q
Atom
A
smallest units of matter that retain the properties and characteristics of the elements
11
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Subatomic Particles
A
composed of individual atoms, protons/neurons/electrons
12
Q
Nucleus
A
Dense central core of an atom (# of electrons=# of protons)
13
Q
Total body mass and significance of O2
A
65%
Part of water and many organic molecules; used to generate ATPA
14
Q
ATP
A
a molecule used by cells to temporarily store chemical energy
15
Q
Total body mass and significance of Carbon
A
18.5%
Forms backbone chains and rings of all organic molecules
16
Q
Total body mass and significance of Hydrogen
A
9.5%
Constituent of water and most organic molecules
17
Q
Total body mass and significance of Nitrogen
A
Component of all proteins and nucleic acids
18
Q
Protons
A
positively charged
19
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Electrons
A
negatively charged
20
Q
Neutrons
A
uncharged
21
Q
Electron Shells
A
Maybe depicted as simple circles around the nucleus
22
Q
First Electron shell
A
no more then 2 electrons
23
Q
2nd Electron Shell
A
Max 8 electrons
24
Q
3rd Electron Shell
A
Max 18 electrons
25
Atomic #
of protons in the nucleus of an atom is an atom's atomic #
26
Mass #
Of an atom is the sum of its protons and neutrons
27
Isotopes
Atoms of an element that have different #'s of neutrons therefore different mass #'s
28
Radioactive Isotopes
Unstable; their nuclei decay into a stable configuration
29
Half-life
time required for half of the radioactive atoms in a sample of an isotope to decay into a more stable form
30
Dalton
standard unit for measuring the mass of atoms and their subatomic particles
31
Atomic Mass
atomic weight, the average mass of all the elements naturall occurring isotopes
32
Ion
happens if an atom either gives up or gains electrons. Has a positive or negative charge
33
Ionization
the process of giving up or gaining electrons
34
Molecule
2 or more atoms share electrons, the resulting combination
35
Compound
a substance that contains atoms of 2 or more different elements
36
Free radical
an atom or group of atoms with an unpaired electron in the outermost shell, an unpaired electron makes a free radical unstable, highly reactive, and destructive to nearby molecules
37
Chemical Bond
Forces that hold together the atoms of a molecule or a compound
38
Valence Shell of Electrons
Likelihood that an atom will form a chemical bond with another atom depends on the number of electrons in its outermost shell
39
Ionic Bond
+ or - charged ions are attracted to one another --> opposites attract. Force of attraction that holds together ions with opposite charges.
40
Cation
Total # of protons exceeds the # of electrons
41
Anion
Total # of electrons exceeds # or protons
42
Electrolyte
Ionic compound the breaks apart into + or - ions in solution
43
Covalent bond
forms 2 or more atoms that share electrons rather than gaining or losing them
44
Single Covalent bond
results when 2 atoms share one electron pair
45
Double Covalent bond
results when 2 atoms share 2 pairs of electrons
46
Triple Covalent bond
results when 2 atoms share 3 pairs of electrons
47
Non polar bond
the bonds between 2 identical atoms
48
Polar Bond
sharing of electrons more strongly than the nucleus of the other atom
49
Electronegativity
the power to attract electrons to itself
50
Hydrogen bond
forms when a hydrogen atom with a partial + charge attracts the partial - charge
51
Surface Tension
a measure of difficulty of stretching or breaking the surface liquid
52
Chemical Reaction
Occurs when new bonds form or old bonds break between atoms
53
Energy
The capacity to do work
54
Principal Forms of Energy
Potential Energy and Kinetic Energy
55
Potential Energy
Energy stored by matter due to its position
56
Reactants
Starting substances--> two H2 and one O2
57
Products
Ending Substances--> two molecules of H2O
58
Metabolism
refers to all the chemical reactions occurring in the body
59
Kinetic Energy
energy associated with matter in motion
60
Chemical Energy
form a potential energy that is stored in the bonds of compounds and molecules
61
Law of energy conservation
energy can be neither created nor destroyed, it maybe converted from on form to another
62
Exergonic Reactions
Release more energy than they absorb
63
Endergonic Reactions
absorb more energy than they release
64
Activation energy
collision of energy needed to break the chemical bonds of the reactants
65
Concentration
more particles of matter present in a confined space, the grater the chance that they will collide
66
Temperature
Temp rises, particles of matter move about more rapidly.
67
Catalysts
Are chemical compounds that speed up chemical reactions by lowering activation energy needed for reaction to occur
68
Synthesis reactions (Anabolism)
occur in the body collectively, overall anabolic reactions are usually energonic as they absorb more energy than they release
69
Decomposition Reactions (Catabolism)
Split up larger molecules into smaller atoms/ions/molecules. Decomposition reactions that occur within the body are catabolic reactions as they are usually exergonic because they release more energy than they absorb
70
Exchange Reaction
They consist of body synthesis and decomposition reactions. The bonds break between A and B and between C and Dand new bonds form between A and D and between B and C
71
Reversible Reactions
The Products can revert to the original reactans (AB combined into/breaks down into A + B)
72
Oxidation
Refers to the gain of electrons; in the process the reduced substance gains energy
73
Reduction
Refers to the gain of electrons; in the process the reduced substance gains energy
74
Oxidation-Reductions Reactions
Are always parallel; when one substance is oxidized, another is reduced at the same time
75
Inorganic Compound
Usually lack carbon and are structurally simple; their molecules also have only a few atoms and can't be used to cells to perform complicated biological functions
76
Organic Compounds
Always contain carbon, usually hydrogen; and always have covalent bonds; most large molecules many made up of long carbon atom chains
77
Water
most important and abundant inorganic compound in all living systems
78
Solvent
dissolved another substance (Water most versatile solvent)
79
Solute
Substance being dissolved by solvent
80
Solution
When a solvent dissolved a solute
81
Hydrophillic
solutes that are charge or contain polar covalent. Dissolve easier in water
82
Hydrophobic
Molecules that contain mainly nonpolar covalent bonds. Not very water-soluble
83
Water in Chemical Reactions
Serves as a medium for most chemical reactions in the body and participates as a reactant or product in certain reactions
84
Hydrolysis
Decomposition reactions break down large nutrient molecules into smaller molecules by addition of water molecules. Hydrolysis reactions enable dietary nutrients to be absorbed into the body
85
Dehydration synthesis reaction
a water molecule is one of the products formed
86
Thermal properties of water
water can absorb or release a relatively large amount of hear with only a modest change in its own temperatre. High heat capacity. Heat of vaporization also high
87
Water as a lubricant
Major component of mucus and other lubrication fluids throughout the body
88
Mixture
a combo of elements or compounds that are physically blended together but not bound by chemical bonds
89
Colloid
differes from a solution mainly because of particle size. The solute particles in a colloid are large enough to scatter light
90
Suspension
solutes in both solutions and colloids do not settle and accumulate at the bottom of the container. Suspended material may mix with the liquid or medium for sometime but will eventually settle.
91
Concentration
expressed in several ways: % -> gives reactive mass of a solute found in a given volume of solution
92
Moles/Liter (Molarity)
Relates to the total # of molecules in a given volume of solution
93
Mole
is the # of any substance that has a mass in grams = to the sum of the atomic masses of all its atoms
94
Dissociate
they separate into ions and become surrounded by water molecules
95
Acid
Substance that dissociates into 1 or more H+ ions and 1 or more anions
96
Base
removes the H+ from a solution and is therefore a proton acceptor
97
Salt
When dissolved in water, dissociates into cations and anions
98
pH
concept of pH intracellular and extracellular fluids must contain balanced quantities of acids and bases
99
pH scale
A solutions alkalinity or acidity which extends from 0-14
100
Acidic Solution
A solution that has more H+ than OH- and a pH lower then 7
101
Basic Solution
A solution that has more OH- then H+. pH above 7
102
Buffer System
Function to convert strong acids or bases into weak acids or bases
103
Buffers
Chemical compounds that can convert strong acids or cases into weak ones
104
Carbonic acid-bicarbonate buffer system
Carbonic acid can act as a weak acid and the bicarbonate ion can act as a weak base
105
Functional groups of organic molecules
carbon skeleton, hydrocarbon, functional groups
106
Carbon Skeleton
A chain of carbon atoms in an organic molecule
107
Hydrocarbon
Many of the carbon are bonded to hydrogen atoms
108
Functional groups
attached to the carbon skeletons, other atoms or molecules bound to the hydrocarbon skeleton
109
Macromolecules
small organic molecules combine into very large molecules
110
Polymers
A large molecule forms by the covalent bonding of many identical or similar small building-block molecules
111
Monomers
The reaction that joins 2 monomers is dehydration synthesis
112
Isomers
Molecules that have the same molecular formula but different structures
113
Building blocks of Carbohydrates
Carbohydrates, Monosaccharides, Disaccharides, Polysaccharides, Glycogen, Starches, Cellulose
114
Carbohydrates
includes sugar, glycogen, starches, and cellulose. 2-3% of body mass
115
Monosaccharides
Simple sugars, contain 3-7 carbon atoms
116
Disaccharides
molecule formed from the combination of 2 monosaccharides joined by dehydration synthesis reactions
117
Polysaccharides
3rd major group of carbs, each molecule contains hundreds of monosaccharides by dehydration synthesis reactions
118
Glycogen
made entirely of glucose monomers linked to 1 another in branching chains
119
Starches
Are polysaccharides forms from glucose by plants
120
Cellulose
Is a polysaccharide formed from glucose by plants that cannot be digested by humans but does provide bulk to help eliminate feces
121
Lipids
make up 18-25% of body mass in lean adults. Contain carbon hydrogen, oxygen. Are Hydrophobic
122
Lipoprotein
More soluble in blood plasma. Soluble because the proteins on the outside and lipids on the inside
123
Fatty Acids
Simplest lipids, which are used to synthesize triglycerides and phospholipids
124
Saturated fatty Acid
contains only single covalent bonds between the carbon atoms of the hydrocarbon chain. Lack double bonds
125
Unsaturated Fatty Acids
Contains 1 or more double covalent bonds between the carbon atoms of the hydrocarbon chain.
126
Triglycerides
most plentiful lipids in your body and in your diet
127
Glycerol
a 3 carbon molecule forms the backbone of a triglyceride
128
Phospholipids
Have a glycerol backbone and 2 fatty acid chains attached to the 1st two carbons
129
Amphiphatic
On both side, they line up tail-tail in a double row to make up much of the membrane that surrounds each cell
130
Steroid
4 rings of carbon atoms
131
Cholesterol
have at least one hydroxyl group. Needed for cell membrane structure
132
Eicosanoids
lipids derived from 20 carbon fatty acid called arachidonic acid
133
Prostaglandins
2 principal subclasses of eicosanoids
134
Leukotrienes
Participate in allergic and inflammatory responses
135
Protein
large molecules that contain carbon, hydrogen, oxygen, and nitrogen
136
Amino Acids
the monomers of protein, each of the 20 different amino acids has a H atom and 3 important finctional groups attached to a central carbon atom.
137
Peptide Bond
Covalent bond joining each pair of amino acids.
138
Dipeptide
When 2 amino acids combine
139
Tripeptide
Adding another amino acid to a dipeptide
140
Polypeptide
Further additions of amino acids result in the formation of a chainlike peptide or more amino acids
141
Denaturation
If a protein encounters an altered environment, it may unravel and lose its characteristic shape and are no longer functional.
142
Nucleic Acids
Were first discovered in nuclei of cells, huge organic molecules that contain carbon, oxygen, nitrogen, and phosphorus
143
DNA
forms the inherited genetic material inside each human cell
144
Gene
a segment of a DNA molecule
145
Ribonucleic Acid (RNA)
2nd type of nucleic acid relays intructions from the genes to guide each cell's synthesis of proteins from amino acids
146
Nucleotides
A chain of repeating monomers
147
Nitrogen Base
DNA contains 4 different nitrogenous bases which contain atoms of C, H, O, and N. In nitrogen the 4 bases are Adenine, Thymine, Cytosine, and Guanine
148
Deoxyribose
Pentose sugar is a 5 carbon sugar that attaches to each base in DNA
149
Phophate Group
Alternate with pentose sugar to form the backbone of a DNA strand; the base projects inward form the backbone chain
150
Double Helix
DNA resemble a spiral ladder, 2 strands alternating phosphate groups and deoxyribose sugars form the upright ladder, paired bases held together by hydrogen bonds, form the rings
151
Ribose
RNA is 2nd variety of nucleic acid, differs from DNA in several respects. In humans, RNA is single-stranded, the sugar in the RNA nucleotide is the pentose ribose.
152
ATP
the energy currency of living systemsh
153
What does ATP consist of
2 phosphate groups attached to adenosine
154
ADP
Energy needed to attach a phosphate group to ADP is supplied mainly by the catabolism of glucose in a process called cellular respiration
155
Cellular Respiration Phases
1. Anaerobic Phase
2.Aerobic Phase
156
Enzymes
In all living cells, most catalysts are these protein molecules.
157
Two Parts of Enzymes
Apoenzyme (protein portion) and cofactor (nonprotein factor)
158
Three important properties of enzymes
Enzymes are highly specific, Enzymes are very effecient, enzmes are subject to a variety of cellular controls
159
Substrates
reactant molecules on which the enzyme acts
160
Active Site
part of the enzyme that catalyzes the reaction
161
Enzyme-subtrate complex
In this reaction two substrate molecules are sucrose and water
