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Biology 235 > Chapter 2: The Chemical Level Of Organization > Flashcards

Chapter 2: The Chemical Level Of Organization Flashcards

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1
Q

Matter

A

Anything that occupies space and has mass

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2
Q

Mass

A

Is the amount of matter in an object which does not change

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3
Q

Weight

A

The force of gravity acting on matter, does not change

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4
Q

Major Elements

A

4 elements:
Carbon
Oxygen
Hydrogen
nitrogen
Constitute 96% of body’s mass

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5
Q

Oxygen

A

BM- 65.0
Part of water and many organic molecules
Generates ATP

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6
Q

Organic

A

Carbon containing

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7
Q

ATP

A

Molecules used by cells to temporary store chemical energy

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8
Q

Carbon

A

Bm-18.5
Forms backbone chains and rings of all organic molecules

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9
Q

Organic Molecules

A

Carbohydrates
Lipids (fats)
Proteins (amino acids)
Nucleic Acids (RNA, DNA)

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10
Q

Hydrogen

A

BM-9.5
Constituent of water and most organic molecules
Ionized form H+ , Makes body fluids more acidic

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11
Q

Nitrogen

A

BM-3.2
Component of all proteins and Nucleic acids

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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.

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13
Q

Chemical Symbol

A

Name that is designated by one or two letters in english, Latin or another language.
(Ie) H, C, Ca

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14
Q

Lesser Elements

A

8 elements
Calcium
Phosphorus
Magnesium
Iron
Potassium
Sulfur
Sodium
Chloride
Constitutes 3.6% of body’s Mass

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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

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16
Q

Atom

A

Smallest unit of matter that retain the properties and characteristics of the element

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17
Q

Subtonic Particles

A

Compose individual atoms.
Protons, Neurons and Electrons

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18
Q

Nucleus

A

Core of atom

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19
Q

Protons

A

Positively charged

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20
Q

Neurons

A

Uncharged(neutral)

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21
Q

Electrons

A

Negatively Charged
Move around in a large space surrounding the nucleus

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22
Q

Electron Shells

A

Regions where specific groups of electrons move around the nucleus

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23
Q

Atomic Number

A

THe number of protons in the nucleus

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24
Q

Mass Number

A

Sum of proton and neutrons added together

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25
Q

Isotopes

A

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

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26
Q

Radioactive Isotopes

A

or radioisotopes
Unstable, their nuclei decay into stable configuration

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27
Q

Half Life of Isotope

A

The time required for half the radiation atoms in a sample to decay into more stable form.

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28
Q

Dalton

A

Standard unit of measure for mass of atoms and their subatomic particles

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29
Q

Atomic Mass

A

Or atomic weight
The average mass of all its naturally occurring isotopes

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30
Q

Ion

A

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.

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31
Q

Ionization

A

The process of giving up or gaining electrons

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32
Q

Molecule

A

When two or more atoms share electrons
Can consist of two atoms of the same kind (ie) O2

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33
Q

Compound

A

Contains atoms of two or more different elements
(Ie) H20

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34
Q

Free Racial

A

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.

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35
Q

Chemical Bonds

A

The force that holds together the atoms of a molecule or a compound

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36
Q

Valence Shell

A

The likely hood that an atom will form a chemical bond with another atoms. Depends of the electrons in the outermost shell

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37
Q

Ionic Bond

A

The force of attraction that hold together ions with opposite charges

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38
Q

Cation

A

Pos charged ion
Electrons are lost

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39
Q

Anion

A

Neg charged ion
Electrons are gained

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40
Q

Electrolytes

A

Ionic compound that breaks apart into positive and negative ions in solution

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41
Q

Covalent Bond

A

Two or more atoms share electrons rather than gaining or losing them

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42
Q

Single Covalent Bond

A

Two or more atoms share one electron pair

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43
Q

Double Covalent bond

A

Two or more atoms share two pairs of electrons

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44
Q

Triple Covalent Bond

A

Two or more atoms share three pairs of electrons

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45
Q

Non polar Covalent Bond

A

Two atoms share the electrons equally. One atoms does not attract the shared electron more strongly than the other.

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46
Q

Polar covalent Bond

A

The sharing of electrons between two atoms is unequal.
(Ie) the bond between oxygen and hydrogen in a molecule of water

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47
Q

Electronegativity

A

The power to attract electrons to itself.

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48
Q

Hydrogen Bond

A

Forms when a hydrogen atoms with a partial pos charge attracts the partial negative charge of nitrogen atoms.

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49
Q

Cohesion

A

The tendency of like particles to stay together.

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50
Q

Surface Tension

A

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

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51
Q

Exergonic Reaction

A

Releases more energy than they absorb

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52
Q

Endergonic Reaction

A

Absorb more energy than they release.

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53
Q

Catalysts

A

Speed up chemical reaction by lowering the activation energy needed for a reaction to occur.

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54
Q

Inorganic Compounds

A

Lack carbon and are structurally simple

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55
Q

Organic Compounds

A

Contain carbon, usually contain hydrogen and always have covalent bonds.

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56
Q

Solution

A

Homogenous mixture. Made up of a solute dissolved with a solvent

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57
Q

Solvent

A

Dissolves another substance
Usually present in a greater amount in a solution

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58
Q

Solute

A

A substance that can be dissolved into a solution by a solvent. Can be in form of gas, liquid or solid.

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59
Q

Hydrophilic

A

Solutes that are charged or contain polar covalent bonds
(Ie) sugar, salt

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60
Q

Hydrophoic

A

Molecules that contain mainly non polar covalent bonds. Not very water soluble.
(Ie) vegetable oil

61
Q

Hydrolysis

A

To break down large nutrients molecules into smaller molecules by the addition of water.

62
Q

Lubricating fluids

A

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
Q

Mixture

A

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

64
Q

Colloid

A

Differs from a solution due to the size of particles. The particles can shatter light. Appears translucent or opaque.

65
Q

Suspension

A

Any suspended material may mix with liquid or suspend in liquid, but will eventually settle out.

66
Q

Heat Capacity in Water

A

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
Q

Mole

A

The amount of any substance that has a mass in grams equal to the same of the atomic masses of all its atoms.

68
Q

Base

A

Have a biter tase and feel slippery.
Called a Proton Acceptor as it removed or take up H+ from a solution.

69
Q

Acid

A

Have a sour taste.
Called Proton Donor as it dissociates and releases hydrogen ions in detectable amounts.

70
Q

Salt

A

Dissolves in water. Dissociates into cations and anions, neither of which are H+ or OH- (Hydroxide).

71
Q

Ph Scale

A

Extends from 0-14. Based ion the concentration of H+ in moles over liter.

72
Q

Bicarbonate Ion

A

Important base in the body, abundant in blood.

73
Q

Ammonia

A

Common Base. Waste product of protein breakdown in the body.

74
Q

Ph Concentration

A

The more hydrogen ions in a solution the more acidic. The total number of hydroxyl ions the more basic.

75
Q

Buffer System

A

Functions to convert strong acids or bases into weaker acids or bases.

76
Q

Buffer

A

Chemical compound that can convert strong acids or bases into weaker one.

77
Q

Macromolecules

A

When small organic molecules combine into very large molecules.

78
Q

Polymers

A

A large chain like molecule formed by a covalent bond of many identical or similar small molecules called monomers.

79
Q

Monomers

A

Identical or similar units

80
Q

Isomers

A

Molecules that have the same molecular formula but different structures.

81
Q

Carbohydrates

A

Include sugar, glycogen, startches and cellulose.
3 major groups: monosaccharides, disaccharide and polysaccharides.

82
Q

Monosaccharides

A

Simple sugars. Single chain or ring structures containing 3 -7 carbons atoms.

83
Q

Disaccharides

A

Simple sugar (double sugar). Is formed when two monosaccharides combine by dehydration synthesis.

84
Q

Dehydration Synthesis

A

A water molecule is lost as a bond is made.

85
Q

Polysaccharides

A

This modules contains tens of hundreds of monosaccharides joined together through dehydration synthesis reaction.
Usually insoluble in water and do not taste sweet.

86
Q

Glycogen

A

Acts as storage. Main polysaccharide in the human body.

87
Q

Starches

A

Polysaccharides formed from glucose by plants.

88
Q

Cellulose

A

Polysaccharide formed from plants that cannot be digested by humans. Does provide bulked to help emulate feces.

89
Q

Lipids

A

Organic compound. Make up 18-25% of body mass.
Contain carbon, hydrogen and oxygen.
Insoluble in water: hydrophobic

90
Q

Lipoproteins

A

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
Q

Fatty Acid

A

Simplest lipids. Used to synthesis triglycerides and phospholipids.
Catabolize to generate ATP.

92
Q

Saturated Fatty Acid

A

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
Q

Unsaturated Fatty Acids

A

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
Q

Triglycerides

A

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
Q

Fat

A

A triglyceride at room temperature (solid).

96
Q

Oil

A

Triglyceride that is liquid at room temperature.

97
Q

Saturated Fat

A

Mainly contains saturated fatty acids. Found in meats and non skim dairy products.

98
Q

Monounsaturated Fats

A

Triglycerides that mostly consist of monounsaturated fatty acids like: olive, peanut and canola oil, most nuts and avocados.

99
Q

Polyunsaturated Fats

A

Triglycerides that mostly consist of poly-unsaturated fatty acid like corn oil, saff lower oil, sunflower oil, soybean oil and fatty fish.

100
Q

Phospholipids

A

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
Q

Proteins

A

Large molecules. Contain carbon, hydrogen, oxygen and nitrogen. Some contain sulfur.
Responsible for the structure of body tissue

102
Q

Amino Acids

A

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
Q

Peptide bond

A

Covalent bond that join each pair of amino acid together.

104
Q

Dipeptide

A

When 2 amino acids combine

105
Q

Tripeptide

A

Produced when another amino acid is joined to a dipeptide.

106
Q

Peptide

A

4-9 amino acids joined together

107
Q

Polypeptide

A

10-2000 or more amino acids are joined together.

108
Q

Apoenzyme

A

Protein portion of enzyme

109
Q

Cofactor

A

Non protein portion of an enzyme.

110
Q

DNA

A

Deoxyribonucleic Acid
Forms the inherited genetic material inside each human cell.
Adenine always pairs with thymine
Cytosine always pairs with guanine

111
Q

Gene

A

Segment of human DNA molecule

112
Q

RNA

A

Ribonucleic Acid
Relays instructions from the genes to guide each cells synthesis of protein from amino acids.

113
Q

Nucleotide

A

A chain of repeating monomers

114
Q

Double Helix Model

A

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
Q

Ribose

A

Penrose sugar in RNA nucleotide

116
Q

Purines

A

A - adenine
G- guanine
A and G are larger double ring bases

117
Q

Pyrimidines

A

T- thymine
C- cytosine
T and C are smaller single ring base

118
Q

Deoxyribose

A

5 carbon sugar

119
Q

ATPase

A

Enzyme catalyzes the hydrolysis of ATP.

120
Q

Chemical Reaction

A

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
Q

Energy

A

Capacity to do work
All reactions involve energy changes

122
Q

Dissociate

A

Seepage into ions and become surround by water molecules.

123
Q

Concentration

A

Expressed in 2 ways:
Percentage: mass per volume
Molarity: moles per liter

124
Q

Molaridy

A

Total number of molecules in a given volume of solution

125
Q

Chemically Stable

A

Meaning it is unlikely to form a bond with another atom

126
Q

Rule of 8 or Octet Rule

A

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
Q

Potential Energy

A

Energy stored by matter due to its postion

128
Q

Chemical ENergy

A

Form of potential energy that is sorted in the bonds of compounds and molecules

129
Q

Kinetic Energy

A

Energy associated with matter in motion

130
Q

Activation Energy

A

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
Q

Law of Conservation of Energy

A

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
Q

Syntheses Reaction

A

Happens when 2 or more atoms, ions, or molecules combine to form new and large molecules

133
Q

Decomposition Reaction

A

Split up large molecules into smaller atoms, ions and molecules.

134
Q

Exchange Reaction

A

Consists of both syntheses and decomposition reactions, many reactions in the body are these reactions.

135
Q

Reversible Reactions

A

Productions can revert to original reactants

136
Q

Oxidation

A

Reduction reaction. Refers to loss of electrons, releases energy.

137
Q

Acid Base Balance

A

To ensure homeostasis, ICF and ECF must contain almost balanced quantity of acids and bases.

138
Q

Carbonic Acid Bicarbonate Buffer System

A

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
Q

Hydrocarbon

A

Carbon Skeleton: Chain of carbon atoms are bonded by hydrogen atoms

140
Q

Functional Group

A

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
Q

Function of Carbohydrates

A

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
Q

Amphipathic

A

Both polar and non polar parts

143
Q

Function of Phospholipids

A

Chief material of cell membrane
Participates in transport of lipids in plasma
Prevalent in nervous tissue

144
Q

Steroids

A

4 ring carbon atom. Fat soluble and contain little 02.
Most important: cholesterol

145
Q

Function of Cholesterol

A

Structural basis for manufacture of all body steroids.

146
Q

Desaturation

A

When proteins encounter an altered environment and loose their shape. They are no longer functional.

147
Q

Enzymes

A

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
Q

3 Properties of Enzymes

A
  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.

Biology 235 (29 decks)

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