Chapter 2: The Chemical Level Of Organization Flashcards
1
Q
Matter
A
Anything that occupies space and has mass
2
Q
Mass
A
Is the amount of matter in an object which does not change
3
Q
Weight
A
The force of gravity acting on matter, does not change
4
Q
Major Elements
A
4 elements:
Carbon
Oxygen
Hydrogen
nitrogen
Constitute 96% of body’s mass
5
Q
Oxygen
A
BM- 65.0
Part of water and many organic molecules
Generates ATP
6
Q
Organic
A
Carbon containing
7
Q
ATP
A
Molecules used by cells to temporary store chemical energy
8
Q
Carbon
A
Bm-18.5
Forms backbone chains and rings of all organic molecules
9
Q
Organic Molecules
A
Carbohydrates
Lipids (fats)
Proteins (amino acids)
Nucleic Acids (RNA, DNA)
10
Q
Hydrogen
A
BM-9.5
Constituent of water and most organic molecules
Ionized form H+ , Makes body fluids more acidic
11
Q
Nitrogen
A
BM-3.2
Component of all proteins and Nucleic acids
12
Q
Chemical elements
A
Building blocks that make up all forms of matter, living/non living. These elements can not be split into simpler substance by ordinary means.
13
Q
Chemical Symbol
A
Name that is designated by one or two letters in english, Latin or another language.
(Ie) H, C, Ca
14
Q
Lesser Elements
A
8 elements
Calcium
Phosphorus
Magnesium
Iron
Potassium
Sulfur
Sodium
Chloride
Constitutes 3.6% of body’s Mass
15
Q
Trace Elements
A
14 Elements
Present in body in tiny amounts. Makes up 0.4 % of body’s mass.
(Ie) Iodine: makes thyroid hormones
16
Q
Atom
A
Smallest unit of matter that retain the properties and characteristics of the element
17
Q
Subtonic Particles
A
Compose individual atoms.
Protons, Neurons and Electrons
18
Q
Nucleus
A
Core of atom
19
Q
Protons
A
Positively charged
20
Q
Neurons
A
Uncharged(neutral)
21
Q
Electrons
A
Negatively Charged
Move around in a large space surrounding the nucleus
22
Q
Electron Shells
A
Regions where specific groups of electrons move around the nucleus
23
Q
Atomic Number
A
THe number of protons in the nucleus
24
Q
Mass Number
A
Sum of proton and neutrons added together
25
Isotopes
Atoms of an element that have different numbers of neutrons and therefore have different mass numbers
26
Radioactive Isotopes
or radioisotopes
Unstable, their nuclei decay into stable configuration
27
Half Life of Isotope
The time required for half the radiation atoms in a sample to decay into more stable form.
28
Dalton
Standard unit of measure for mass of atoms and their subatomic particles
29
Atomic Mass
Or atomic weight
The average mass of all its naturally occurring isotopes
30
Ion
Forms when an atoms either gives up or gains electrons
It has a pos or neg charge because it has unequal numbers of protons and electrons.
31
Ionization
The process of giving up or gaining electrons
32
Molecule
When two or more atoms share electrons
Can consist of two atoms of the same kind (ie) O2
33
Compound
Contains atoms of two or more different elements
(Ie) H20
34
Free Racial
Atom or group of atoms with an unpaired electron in the outermost shell
When unpaired-unstable, highly reactive, and destructive to near by molecules
Becomes Stable: by giving up unpaired electrons or taking electron form.
35
Chemical Bonds
The force that holds together the atoms of a molecule or a compound
36
Valence Shell
The likely hood that an atom will form a chemical bond with another atoms. Depends of the electrons in the outermost shell
37
Ionic Bond
The force of attraction that hold together ions with opposite charges
38
Cation
Pos charged ion
Electrons are lost
39
Anion
Neg charged ion
Electrons are gained
40
Electrolytes
Ionic compound that breaks apart into positive and negative ions in solution
41
Covalent Bond
Two or more atoms share electrons rather than gaining or losing them
42
Single Covalent Bond
Two or more atoms share one electron pair
43
Double Covalent bond
Two or more atoms share two pairs of electrons
44
Triple Covalent Bond
Two or more atoms share three pairs of electrons
45
Non polar Covalent Bond
Two atoms share the electrons equally. One atoms does not attract the shared electron more strongly than the other.
46
Polar covalent Bond
The sharing of electrons between two atoms is unequal.
(Ie) the bond between oxygen and hydrogen in a molecule of water
47
Electronegativity
The power to attract electrons to itself.
48
Hydrogen Bond
Forms when a hydrogen atoms with a partial pos charge attracts the partial negative charge of nitrogen atoms.
49
Cohesion
The tendency of like particles to stay together.
50
Surface Tension
A measure of the difficulty of stretching or breaking the surface of liquid.
51
Exergonic Reaction
Releases more energy than they absorb
52
Endergonic Reaction
Absorb more energy than they release.
53
Catalysts
Speed up chemical reaction by lowering the activation energy needed for a reaction to occur.
54
Inorganic Compounds
Lack carbon and are structurally simple
55
Organic Compounds
Contain carbon, usually contain hydrogen and always have covalent bonds.
56
Solution
Homogenous mixture. Made up of a solute dissolved with a solvent
57
Solvent
Dissolves another substance
Usually present in a greater amount in a solution
58
Solute
A substance that can be dissolved into a solution by a solvent. Can be in form of gas, liquid or solid.
59
Hydrophilic
Solutes that are charged or contain polar covalent bonds
(Ie) sugar, salt
60
Hydrophoic
Molecules that contain mainly non polar covalent bonds. Not very water soluble.
(Ie) vegetable oil
61
Hydrolysis
To break down large nutrients molecules into smaller molecules by the addition of water.
62
Lubricating fluids
Found through the body. Especially in the chest (pleural and pericardial cavity) and abdomen (peritoneal cavity) where internal organ touch and slider over one another.
63
Mixture
Combination of elements or compounds that are physically blended together but not bound by chemical bonds.
64
Colloid
Differs from a solution due to the size of particles. The particles can shatter light. Appears translucent or opaque.
65
Suspension
Any suspended material may mix with liquid or suspend in liquid, but will eventually settle out.
66
Heat Capacity in Water
Has high heat capacity due to large numbers of hydrogen bonds in water. As water absorbs heat energy, this breaks apart hydrogen bonds. Less energy is left over causing the temperature in water to rise.
67
Mole
The amount of any substance that has a mass in grams equal to the same of the atomic masses of all its atoms.
68
Base
Have a biter tase and feel slippery.
Called a Proton Acceptor as it removed or take up H+ from a solution.
69
Acid
Have a sour taste.
Called Proton Donor as it dissociates and releases hydrogen ions in detectable amounts.
70
Salt
Dissolves in water. Dissociates into cations and anions, neither of which are H+ or OH- (Hydroxide).
71
Ph Scale
Extends from 0-14. Based ion the concentration of H+ in moles over liter.
72
Bicarbonate Ion
Important base in the body, abundant in blood.
73
Ammonia
Common Base. Waste product of protein breakdown in the body.
74
Ph Concentration
The more hydrogen ions in a solution the more acidic. The total number of hydroxyl ions the more basic.
75
Buffer System
Functions to convert strong acids or bases into weaker acids or bases.
76
Buffer
Chemical compound that can convert strong acids or bases into weaker one.
77
Macromolecules
When small organic molecules combine into very large molecules.
78
Polymers
A large chain like molecule formed by a covalent bond of many identical or similar small molecules called monomers.
79
Monomers
Identical or similar units
80
Isomers
Molecules that have the same molecular formula but different structures.
81
Carbohydrates
Include sugar, glycogen, startches and cellulose.
3 major groups: monosaccharides, disaccharide and polysaccharides.
82
Monosaccharides
Simple sugars. Single chain or ring structures containing 3 -7 carbons atoms.
83
Disaccharides
Simple sugar (double sugar). Is formed when two monosaccharides combine by dehydration synthesis.
84
Dehydration Synthesis
A water molecule is lost as a bond is made.
85
Polysaccharides
This modules contains tens of hundreds of monosaccharides joined together through dehydration synthesis reaction.
Usually insoluble in water and do not taste sweet.
86
Glycogen
Acts as storage. Main polysaccharide in the human body.
87
Starches
Polysaccharides formed from glucose by plants.
88
Cellulose
Polysaccharide formed from plants that cannot be digested by humans. Does provide bulked to help emulate feces.
89
Lipids
Organic compound. Make up 18-25% of body mass.
Contain carbon, hydrogen and oxygen.
Insoluble in water: hydrophobic
90
Lipoproteins
Lipid modules join with hydrophilic protein modules. Undergo this change to be more soluble in blood. Are more solvable because the proteins are on the outside and the lipid inside.
91
Fatty Acid
Simplest lipids. Used to synthesis triglycerides and phospholipids.
Catabolize to generate ATP.
92
Saturated Fatty Acid
Contain only single covalent bonds between the carbon atoms of the hydrocarbon chain. They lack double bonds so the carbon and hydrocarbon are saturated with hydrogen atoms.
93
Unsaturated Fatty Acids
Contains one or more double covalent bonds between the carbon atoms of the hydrocarbon chain. Thus the fatty acid is not completely saturated with hydrogen atoms.
94
Triglycerides
Most plentiful in the body. The body’s highest concentrated form of chemical energy. Can be solid or liquid.
Consists of a single glycerol (3 carbon) molecule and 3 fatty acid molecules.
Glycerol forms the back bone of a triglyceride.
95
Fat
A triglyceride at room temperature (solid).
96
Oil
Triglyceride that is liquid at room temperature.
97
Saturated Fat
Mainly contains saturated fatty acids. Found in meats and non skim dairy products.
98
Monounsaturated Fats
Triglycerides that mostly consist of monounsaturated fatty acids like: olive, peanut and canola oil, most nuts and avocados.
99
Polyunsaturated Fats
Triglycerides that mostly consist of poly-unsaturated fatty acid like corn oil, saff lower oil, sunflower oil, soybean oil and fatty fish.
100
Phospholipids
Glycerol backbone and 2 fatty acid chains attached to the first 2 carbons. 3rd position is a phosphate group po43-
The head is polar and tail (fatty acid) is non polar.
101
Proteins
Large molecules. Contain carbon, hydrogen, oxygen and nitrogen. Some contain sulfur.
Responsible for the structure of body tissue
102
Amino Acids
Building blocks of proteins or monomers.
Has H+ atoms and 3 important function groups:
1. Amino group; NH2
2. Acid carbon group: COOH
3. Side Chain: R group
All amino acids are identical except for the R group that make them chemically unique.
103
Peptide bond
Covalent bond that join each pair of amino acid together.
104
Dipeptide
When 2 amino acids combine
105
Tripeptide
Produced when another amino acid is joined to a dipeptide.
106
Peptide
4-9 amino acids joined together
107
Polypeptide
10-2000 or more amino acids are joined together.
108
Apoenzyme
Protein portion of enzyme
109
Cofactor
Non protein portion of an enzyme.
110
DNA
Deoxyribonucleic Acid
Forms the inherited genetic material inside each human cell.
Adenine always pairs with thymine
Cytosine always pairs with guanine
111
Gene
Segment of human DNA molecule
112
RNA
Ribonucleic Acid
Relays instructions from the genes to guide each cells synthesis of protein from amino acids.
113
Nucleotide
A chain of repeating monomers
114
Double Helix Model
Watson-Crick Model
DNA resembles a spiral ladder.
Upright ladder: 2 strands of alternating phosphate groups and deoxyribose sugars
Rungs: paired bases held together by hydrogen bonds
115
Ribose
Penrose sugar in RNA nucleotide
116
Purines
A - adenine
G- guanine
A and G are larger double ring bases
117
Pyrimidines
T- thymine
C- cytosine
T and C are smaller single ring base
118
Deoxyribose
5 carbon sugar
119
ATPase
Enzyme catalyzes the hydrolysis of ATP.
120
Chemical Reaction
Occurs when new bonds form or old bonds break between atoms
Foundation of all life process
Interaction with VE is the base of this type of reaction.
121
Energy
Capacity to do work
All reactions involve energy changes
122
Dissociate
Seepage into ions and become surround by water molecules.
123
Concentration
Expressed in 2 ways:
Percentage: mass per volume
Molarity: moles per liter
124
Molaridy
Total number of molecules in a given volume of solution
125
Chemically Stable
Meaning it is unlikely to form a bond with another atom
126
Rule of 8 or Octet Rule
Is shell 1 is full with 2 electrons
Atoms tend to intact so they have 8 electrons in their valence shell. Atoms will lose or gain electrons to obtain 8 in the outer moser shell.
127
Potential Energy
Energy stored by matter due to its postion
128
Chemical ENergy
Form of potential energy that is sorted in the bonds of compounds and molecules
129
Kinetic Energy
Energy associated with matter in motion
130
Activation Energy
Collision energy needed to break the chemical bonds of reactions. This can disrupt the movement of valence electrons causing an existing chemical bond to break, forming a new one.
131
Law of Conservation of Energy
Energy can not be neither created or destroyed. It may be converted from one form to another.
Example: conversion of energy from one form to another, produces heat which is used to maintain normal body temp.
132
Syntheses Reaction
Happens when 2 or more atoms, ions, or molecules combine to form new and large molecules
133
Decomposition Reaction
Split up large molecules into smaller atoms, ions and molecules.
134
Exchange Reaction
Consists of both syntheses and decomposition reactions, many reactions in the body are these reactions.
135
Reversible Reactions
Productions can revert to original reactants
136
Oxidation
Reduction reaction. Refers to loss of electrons, releases energy.
137
Acid Base Balance
To ensure homeostasis, ICF and ECF must contain almost balanced quantity of acids and bases.
138
Carbonic Acid Bicarbonate Buffer System
Important in human body.
Carbonic acid- acts as weak acid
Bicarbonate-acts as weak base.
Can compensate for wither an excess or shortage of H+
H+ + HCO3- - H2CO3
139
Hydrocarbon
Carbon Skeleton: Chain of carbon atoms are bonded by hydrogen atoms
140
Functional Group
Atoms or molecule bound together to hydrogen skeleton. Linked by strong coolant bonds and function in chemical reactions as a single unit.
1. Hydroxl-polar
2. Carboxl-fatty acid
3.Amino- proteins
4. Methyl-amino acids
5. Phosphate-phosolipids, neulotides
141
Function of Carbohydrates
To provide readily, easily used source of cellular fuel. Energy is used to synthesis ATP. When energy is sufficient, carbs are converted to glucose or fat and is stored.
142
Amphipathic
Both polar and non polar parts
143
Function of Phospholipids
Chief material of cell membrane
Participates in transport of lipids in plasma
Prevalent in nervous tissue
144
Steroids
4 ring carbon atom. Fat soluble and contain little 02.
Most important: cholesterol
145
Function of Cholesterol
Structural basis for manufacture of all body steroids.
146
Desaturation
When proteins encounter an altered environment and loose their shape. They are no longer functional.
147
Enzymes
Proteins that speed up chemical reactions.
Consist of:
1. Apoenzyme: protein portion
2. Cofactor: non protein portion, can be metal ion, zinc or organic molecule called coenzyme.
148
3 Properties of Enzymes
1. High Specific: each enzyme binds only to specific substrate
2. Efficient: enzymes can catalyze reactions at rapid rates
3. Subject to variety of cellular controls: the rate of synthesis and concentration are under the control of a cell gene.
