WEEK 2 Flashcards
1
Q
This state of matter is compact and has a definite shape and volume.
A
Solid
2
Q
The science of the structure and interactions of matter.
A
Chemistry
3
Q
The force of gravity acting on matter. Change
A
Weight
4
Q
All forms of matter are made up of limited number of building blocks called
A
Chemical Elements
5
Q
The four elements that constitute about 96% of the body’s mass are called
A
Major elements.
6
Q
Anything that occupies space and has mass
A
Matter
7
Q
The amount of matter in any object. No change
A
Mass
8
Q
How many different chemical elements are normally present in Rafael John F Dubria’s body?
A
26
9
Q
Has a definite shape and volume; takes the shape of their container
A
Liquid
10
Q
The smallest atoms; diameter less than 0.1 nanometer (0.1 x 10-9m = 0.0000000001 m) Not sure pila ka 0 pero u get the gist
A
Hydrogen Atoms
11
Q
These 14 elements are present in tiny amounts. Account for 0.4% of the body’s mass; some function as cofactors.
A
Trace Elements
12
Q
Have neither a definite shape nor volume.
A
Gas
13
Q
Each named element is designated by one or two letters of the English alphabet, Latin, or another language. What is this designation called?
A
Chemical Symbol
14
Q
Rest question
A
Rafael John F. Dubria is handsome
15
Q
The dense central core of an atom is called…………………….
A
Nucleus
16
Q
These 8 elements contribute about 3.6% of the body’s mass
A
Lesser Elements.
17
Q
This element is a part of water and many organic (carbon-containing) molecules; used to generate ATP, a molecule used by cells to temporarily store chemical energy. About 65% of the body’s mass
A
Oxygen
18
Q
This subatomic particle is positively charged ++++++++++++++++++++++++++++++++++++++++++++
A
Protons
19
Q
A certain region around the nucleus where groups of electrons are most likely to move around in.
A
Electron Shell
20
Q
This designation of an element is = number of protons
A
Atomic Number
21
Q
The sum of an element’s protons and neutrons
A
Mass Number
22
Q
Atoms of an element that have different numbers of neutrons and therefore different mass numbers.
A
Isotopes
23
Q
Certain Isotopes are unstable. What are these unstable isotopes called hmm?
A
Radioactive Isotopes/Radioisotopes
24
Q
Some radioisotopes are used to follow the movement of certain substances through the body. What are these radioisotopes called, team?
A
Tracers
25
The time required for half of the radioactive atoms in a sample of an isotope to decay into a more stable form
Half-life
26
The standard unit for measuring the mass of atoms and their subatomic particles is called?????????????????????????????????????????????????????????????????
Dalton
27
Substance that contains atoms of two or more different elements
Compound
28
An atom or group of atoms with an unpaired electron in the outermost shell
Free Radical
29
The average mass of all naturally occurring isotopes in an element
Atomic Mass
30
An atom that has a positive or negative charge because of its unequal amount of protons and electrons
Ions
31
These subatomic particles are negatively charged ----------------------
Electrons
32
Substances that inhibit oxygen-derived free radicals
Antioxidants
33
Under the right conditions, two or more atoms can interact in ways that produce a chemically stable arrangement of eight valence electrons for each atom. What chemical principle is this?
Octet Rule
33
Under the right conditions, two or more atoms can interact in ways that produce a chemically stable arrangement of eight valence electrons for each atom. What chemical principle is this?
Octet Rule
34
The force of attraction that holds together ions with opposite charges.
Ionic Bond
35
The total number of electrons exceed the number of protons; a negatively charged ion
Anion
36
The total number of protons exceeds the number of electrons; a positively charged ion
Cation
37
An ionic compound that breaks apart into positive and negative ions in solutions
Electrolyte
38
Two or more atoms share electrons rather than gaining or losing them.
Covalent Bonds
39
This bond results when two atoms share one electron pair.
Single Covalent Bond
40
This bond results when two atoms share two pairs of electrons.
Double Covalent Bond
41
This bond results when two atoms share three pairs of electrons.
Triple Covalent Bond
42
In some covalent bonds, two atoms share the electrons equally— one atom does not attract the shared electrons more strongly than the other atom
Nonpolar Covalent Bond
43
the sharing of electrons between two atoms is unequal—the nucleus of one atom attracts the shared electrons more strongly than the nucleus of the other atom.
Polar Covalent Bond
44
The power of atoms to attract electrons to themselves.
Electronegativity
45
This type of bond forms when a hydrogen atom with a partial positive charge attracts the partial negative charge of neighboring electronegative atoms.
Hydrogen Bond
46
True or False: Hydrogen bonds occur because hydrogen atoms in one water molecule are attracted to the partial negative charge of the oxygen atom in another water molecule.
True
47
A measure of the difficulty of stretching or breaking the surface of a liquid.
Surface Tension
48
The energy currency of living systems; transfers energy liberated in exergonic catabolic reactions to power cellular activities that require energy
Adenosine Triphosphate(ATP)
49
Occurs when new bonds form or old ones break between atoms.
Chemical Reactions
50
The starting substances of chemical reactions.
Reactants
51
The ending substances of chemical reactions
Products
52
The capacity to do work
Energy
53
Energy stored by matter due to its position
Potential Energy
54
Energy associated with matter in motion
Kinetic Energy
55
A form of potential energy that is stored in the bonds of compounds and molecules.
Chemical Energy
56
Although energy can be neither created nor destroyed, it may be converted from one form to another. What principle is this?
Law of Conservation of Energy
57
Release more energy than they absorb
Exergonic Reactions
58
Absorb more energy than they release
Endergonic Reactions
59
The collision energy needed to break the chemical bonds of the reactants is called the?
Activation Energy
60
The more particles of matter present in a confined space, the greater the chance that they will collide
Concentration
61
Trueorfalse:As temperature rises, kingdoms fall, and particles move about more rapidly, increasing the chances of collisions occurring and causing a chemical reaction.
HMM, TRUE
62
Chemical compounds that speed up chemical reactions by lowering the activation energy needed for a reaction to occur.
Catalysts
63
This word means "to put together"
Synthesis
64
This type of reaction occurs when two or more atoms, ions, or molecules combine to form new and larger molecules
SYNTHESIS REACTION
65
All of the synthesis reactions that occur in your body are collectively referred to as./.?:
Anabolism
66
This type of reaction splits up large molecules into smaller atoms, ions, or smaller molecules.
Decomposition Reactions
67
The decomposition reactions that occur in your body are collectively referred to as?
Catabolism
68
These types of reactions consist of both synthesis and decomposition reactions.
Exchange Reactions
69
These types of reactions revert products into the original reactants
Reversible Reactions
70
Refers to the loss of electrons; in the process the substance releases energy
Oxidation
71
Refers to the gain of electrons; in the process, the reduced substance gains energy
Reduction
72
These types of reactions are always parallel; when one substance is oxidized, another is reduced at the same time.
Oxidation-Reduction Reactions
73
These compounds usually lack carbon and are structurally simple. Their molecules also have only a few atoms and cannot be used by cells to perform complicated biological functions
Inorganic Compounds
74
These compounds always contain carbon, and hydrogen, and always have covalent bonds. These make up 38-43% of the human body.
Organic Compounds
75
The most important and abundant inorganic compound in all living systems
Water
76
Is a special type of homogeneous mixture composed of two or more substances
Solution
77
A substance that dissolves in another substance
Solvent
78
A substance in which another substance is dissolved in
Solute
79
Dissolve easily in water, water-loving; Polar covalent bonds
Hydrophilic
80
Does not easily dissolve in water, water-fearing; Nonpolar Covalent Bonds
Hydrophobic
81
Decomposition reactions break down large nutrient molecules into smaller molecules by the addition of water molecules.
Hydrolysis
82
When two smaller molecules join to form a larger molecule, a water molecule is one of the products formed.
Dehydration Synthesis Reaction
83
A combination of elements or compounds that are physically blended together but not bound by chemical bonds.
Mixture
84
Differs from a solution mainly because of the size of its particles.
Colloid
85
The suspended material may mix with the liquid or suspending
medium for some time, but eventually it will settle out.
Suspension
86
Gives the relative mass of a solute found in a given volume of solution.
Percentage
87
A way to express concentration in units of moles per liter.
Molarity
88
When inorganic acids, bases, or salts dissolve in water, they separate into ions and become surrounded by water molecules.
Dissociate
89
A substance that dissociates into one or more hydrogen ions; also referred to as proton donors
Acid
90
Removes H+ from a solution; a proton acceptor
Base
91
When dissolved in water, dissociates into cations and anions,
Salt
92
A solution’s acidity or alkalinity is expressed on what scale?
pH Scale
93
A solution that has more H+ than OH− and has a pH below 7
Acidic Solution
94
A solution that has more OH− than H+ and has a pH above 7
Basic (Alkaline) Solution
95
The pH of the blood falls below 7.35, which results in a condition called?
Acidosis
96
The pH of the blood rises above 7.45, which results in a condition called?
Alkalosis
97
Functions to convert strong acids or bases into weak acids or bases.
Buffer Systems
98
The chemical compounds that can convert strong acids or bases into weak ones
Buffers
99
This buffer system can compensate for either an excess or a shortage of H+.
Carbonic Acid-Bicarbonate Buffer System
100
The chain of carbon atoms in an organic molecule
Carbon Skeleton
101
Many of the carbons are bonded to hydrogen atoms, yielding a what?
Hydrocarbons
102
Simple sugars that contain from 3 to 7 carbon atoms
Monosaccharides
103
Simple sugars formed from the combination of two monosaccharides by dehydration synthesis
Dissacharides
104
From tens to hundreds of monosaccharides joined by dehydration synthesis
Polysaccharides
105
VERY LARGE MOLECULES
Macromolecules
106
A large molecule formed by the covalent bonding of many identical or similar small building-block molecules
Polymer
107
Small building-block molecules
Monomers
108
Molecules that have the same molecular formula but different structures
Isomers
109
Include sugars, glycogen, starches, and cellulose.
Carbohydrates
110
The main polysaccharide in the human body
Glycogen
111
Are polysaccharides formed from glucose by plants
Starches
112
A polysaccharide formed from glucose by plants that cannot be digested by humans but do provide bulk to help eliminate feces.
Cellulose
113
These organic compounds make up 18–25% of body mass in lean adults. Most of these organic compounds are insoluble in polar solvents such as water; they are hydrophobic.
Lipids
114
To become more soluble in blood plasma, other lipid molecules join with hydrophilic protein molecules. The resulting lipid-protein complexes are termed?
Lipoproteins
115
Used to synthesize triglycerides and phospholipids.
Fatty Acids
116
Contains only single covalent bonds between the carbon atoms of the hydrocarbon chain.
Saturated Fatty Acids
117
Contains one or more double covalent bonds between the carbon atoms of the hydrocarbon chain.
Unsaturated Fatty Acids
118
Consists of two types of building blocks: a single glycerol molecule and three fatty acid molecules; three-carbon glycerol forms its backbone
Triglyceride
119
A fat that mainly consists of saturated fatty acids
Saturated Fat
120
A triglyceride that is a solid at room temperature.
Fat
121
A triglyceride that is a liquid at room temperature
Oil
122
Contain triglycerides that mostly consist of monounsaturated fatty acids
Monounsaturated Fats
123
Contain triglycerides that mostly consist of polyunsaturated fatty acids
Polyunsaturated Fat
124
A group of fatty acids that are essential to human health
Essential Fatty Acids
125
Have a glycerol backbone and two fatty acid chains attached to the first two carbons.
Phospholipids
126
Molecules that have both polar and nonpolar parts
Amphipathic
127
Have four rings of carbon atoms
Steroids
128
In the body, the commonly encountered steroids, such as cholesterol, estrogens, testosterone, cortisol,
bile salts, and vitamin D, are known as?
Sterols
129
Are lipids derived from a 20-carbon fatty acid called arachidonic acid.
Eicosanoids
130
They modify responses to hormones, contribute to the inflammatory response, prevent stomach ulcers, dilate (enlarge) airways to the lungs, regulate body temperature, and influence the formation of blood clots,
Prostaglandins
131
Participate in allergic and inflammatory responses.
Leukotrienes
132
Large molecules that contain carbon, hydrogen, oxygen, and nitrogen.
Proteins
133
Monomers of proteins
Amino Acids
134
Form structural framework of various parts of the body
Structural Proteins
135
Promotes chemical reactions; lower the required activation energy
Enzymes
136
Amino acids linked through through dehydration synthesis
Peptides
137
Covalent bond connects the carboxylic acid group of one amino acid to the amino group of another
Peptide Bond
138
2 amino acids linked together
Dipeptide
139
3 or more amino acids linked together
Polypeptides
140
Change in protein tertiary or quaternary structure; protein shape changes and function deteriorates
Denaturation
141
The specific region of an enzyme where substrates must bind;
Active Site
142
Reactants in enzymatic reactions; interactions among these yield specific products
Substrates
143
Multiple enzymes in each cell; each enzyme is active under its own set of conditions; enzyme activation or inactivation is an important method of short-term control over reaction rates and pathways
Control of Reaction Rates
144
Substrate concentration required to have maximum rate of reaction;
Saturation Limit
145
Protein portion of an enzyme
Apoenzyme
146
Nonprotein portion of an enzyme
Cofactor
147
The substrates make contact with the active site on the surface of the enzyme molecule, forming a temporary intermediate compound
Enzyme-substrate Complex
148
Huge organic molecules that contain carbon, hydrogen, oxygen, nitrogen, and phosphorus.
Nucleic Acids
149
The first type of nucleic acid; forms the inherited genetic material inside each human cell.
Deoxyribonucleic Acid (DNA)
150
The second type of nucleic acid relays instructions from the genes to guide each cell’s synthesis of proteins from amino acids.
Ribonucleic Acid (RNA)
151
A nucleic acid is a chain of repeating monomers called
Nucleotides
152
Contain atoms of C, H, O, and N.
Nitrogenous Base
153
Adenine and guanine are larger, double-ring bases called
Purines
154
Thymine and cytosine are smaller, single-ring bases called
Pyrimidines
155
Five-carbon sugar called deoxyribose attaches to each base in DNA
Pentose Sugar
156
Thisgroupalternates with pentose sugars to form the “backbone” of a DNA strand; the bases project inward from the backbone chain
Phosphate Group
157
A technique used in research and in courts of law to ascertain whether a person's DNA matches the DNA obtained from samples or pieces of legal evidence such as blood stains or hairs.
DNA Fingerprinting
158
A series of reactions that do not require oxygen, glucose is partially broken down by a series of catabolic reactions into pyruvic acid
Anaerobic Phase
159
In the presence of oxygen, glucose is completely broken down into carbon dioxide and water. These reactions generate heat and about 30 or 32 ATP molecules
Aerobic Phase
