Chapter 2 Flashcards
(99 cards)
1
Q
anything that occupies space and has mass.
A
Matter
2
Q
the amount of matter in an object.
A
Mass
3
Q
International unit for mass
A
kilogram (kg)
4
Q
the gravitational force acting on an object of a given mass
A
Weight
5
Q
composed of subatomic particles.
A
Atoms
6
Q
no electrical charge
A
Neutrons
7
Q
one positive charge.
A
Protons
8
Q
one negative charge.
A
Electrons
9
Q
formed by protons and neutrons.
A
Nucleus
10
Q
Most of the volume of an atom occupied by electrons. Represented as an?
A
electron cloud.
11
Q
If the valence shell is incomplete, the atom is chemically reactive and forms chemical bonds to achieve an octet called what rule
A
Octet rule
12
Q
two or more forms of same element with same number of protons and electrons but different neutron number. They have the same atomic number but different mass numbers.
A
Isotopes
13
Q
average mass of naturally occurring isotopes.
A
Atomic Mass
14
Q
The unified atomic mass unit is 1/12 of the mass of 12C; called the?
A
Dalton (Da)
15
Q
equal to number of protons in each atom, which is equal to the number of electrons.
A
Atomic Number
16
Q
number of protons plus number of neutrons.
A
Mass Number
17
Q
are formed when electrons in the outermost energy level (valence shell) are either shared with or transferred to another atom.
A
Chemical bonds
18
Q
electrons are transferred from one atom to another.
A
lonic Bonding
19
Q
two or more atoms share electron pairs.
A
Covalent Bonding
20
Q
solutions made by the dissociation of cations (+) and anions (-) in water.
• Have the capacity to conduct an electric current.
• Currents can be detected by electrodes.
A
Electrolytes
21
Q
solutions made by molecules that dissolve in water, but do not dissociate; do not conduct electricity.
A
Nonelectrolytes
22
Q
Atoms, ions, molecules or compounds interact to form or break chemical bonds.
A
Chemical reaction
23
Q
substances that enter into a chemical reaction
A
Reactants
24
Q
substances that result from the reaction
A
Products
25
(synthesis-)?
anabolism
26
(decomposition;)? during chemical reactions.
catabolism
27
collective term used for the sum of all of the anabolic and catabolic reactions in the body
Metabolism
28
Two or more reactants chemically combine to form a new and larger product. Collective term for synthesis reactions in body is?
anabolism
29
synthetic reaction where water is a product.
Dehydration reaction
30
A large reactant is broken down to form smaller products. Collective term for decomposition reactions in body is?
catabolism
31
water is split into two parts that contribute to the formation of the productions
Hydrolysis reactions
32
rate of product formation is equal to rate of reactant formation.
Equilibrium
33
loss of an electron by an atom
Oxidation
34
gain of an electron by an atom
Reduction
35
the complete or partial loss of an electron oby one atom is accompanied by the gain of that electron by another atom.
Oxidation-reduction reactions
36
is the capacity to do work (for example, to move matter).
Energy
37
energy stored in chemical bonds; energy that could do work if it were released. Breaking chemical bonds releases energy.
Potential energy
38
does work and moves matter.
Kinetic energy
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principal states that the total amount of energy in the universe is constant. Energy is neither created nor destroyed, it only changes form.
Conservation of energy
40
energy resulting from the position or movement of objects.
Mechanical energy
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energy resulting from the position or movement of objects.
Mechanical energy
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form of potential energy in the chemical bonds of a substance.
Chemical energy
43
energy that flows between objects of different temperatures.
Heat energy
44
A form of energy that flows from a hotter object to a cooler object.
Heat Energy
45
minimum energy reactants must have to start a chemical reaction.
Activation Energy
46
substances that increase the rate of chemical reactions without being permanently changed or depleted.
Catalysts
47
protein catalysts that increase the rate of chemical reactions by lowering the activation energy necessary for reaction to begin
Enzymes
48
• Increase in ___ means increase of kinetic energy.
• Molecules move faster, collide harder and more frequently.
Temperature
49
increases, rate of reaction increases
• Example: A decrease of O2 in cells can cause death as rate of aerobic chemical reactions decreases.
Concentration of reactants
50
substances that do not contain carbon-hydrogen obonds.
• Water, oxygen, carbon dioxide, calcium
• phosphate, metal ions.
Inorganic Chemistry
51
study of carbon-containing substances.
Organic Chemistry
52
substances attracted to water; "water-loving".
Hydrophilic
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substances not attracted to water; “water-fearing".
Hydrophobic
54
is the attraction of one water molecule to another; creates a surface tension
Cohesion
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is the attraction of water molecules to other molecules; causes the upward movement of water in the xylem of plants.
Adhesion
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allows transport throughout the body.
Mixing medium
57
substances physically but not chemically combined.
Mixture
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mixture of liquids, gasses, or solids that are uniformly distributed.
Solution
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that which dissolves the solute.
Solvent
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materials separate unless stirred.
Ex: Sand and water; blood cells in plasma
Suspension
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dispersal of tiny particles through a medium that do not settle out.
• Milk, plasma of the blood, cell interior
Colloid
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measure of number of particles of solute per volume of solution.
Concentration
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reflects the number of particles dissolved in one kilogram of water.
Osmolality
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One osmole (Osm) is equal to ___ of particles in one kilogram of water?
Avogadro's number
65
Unit used by physiologists is ___ because of the low concentrations in the human body?
milliosmoles (mOsm)
66
mOsm is average in the human body?
300
67
a proton acceptor or any substance that binds to or accepts hydrogen ions.
Base
68
a proton donor or any substance that releases hydrogen ions.
HCI → H+ + CI
Acid
69
Refers to the hydrogen ion concentration in a solution
The pH Scale
70
pH of 7 or equal amounts of hydrogen and hydroxide ions.
Neutral
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pH of less than 7 with a greater concentration of hydrogen ions.
Acidic
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pH of greater than 7 and a greater concentration of hydroxide ions.
Alkaline (basic)
73
The normal pH range for human blood is?
7.35 to 7.45
74
blood pH drops below 7.35, a condition called?
acidosis
75
If blood pH rises about 7.45, a condition called?
alkalosis
76
a compound consisting of a cation other than a hydrogen ion and an anion other than a hydroxide ion.
Example: NaCl
Salt
77
a solution of a conjugate acid-base pair in which acid and base components occur in similar concentrations; this combination resists changes in pH when either acids or bases are added to the solution.
Buffer
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required in the final step in the series of reactions used to extract energy from food.
Oxygen (O2)
79
produced during the catabolism of organic compounds.
• Metabolic waste product.
• Combines with water in plasma and forms H+ thus affecting acid-base balance.
Carbon dioxide (CO2)
80
bound together by covalent bonds constitute the backbone of many large biomolecules by varying the length of the carbon chains and the combination of atoms involved.
Carbon atoms
81
composed of carbon, hydrogen, oxygen.
• Divided into monosaccharides, disaccharides, polysaccharides.
• Energy sources, structure, and bulk for elimination.
• Water soluble
Carbohydrates
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composed mostly of carbon, hydrogen, oxygen.
• Relatively insoluble in water.
• Functions: protection, insulation, physiological regulation, component of cell membranes, energy storage.
Lipids
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composed of carbon, hydrogen, oxygen, nitrogen, sometimes sulfur.
• Functions: regulate processes, aid transport, protection, muscle contraction, structure, energy.
Proteins
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composed of carbon, hydrogen, oxygen, nitrogen, phosphorus.
• Examples: ATP, DNA, RNA.
Nucleic Acids
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One fatty acid replaced with a phosphate group; polar (hydrophilic) at one end; nonpolar (hydrophobic) at the other.
Lipids: Phospholipids
86
composed of glycerol and fatty acids.
• Each fatty acid has a carboxyl group.
• Fatty acids combine with glycerol to form triglyceride.
Triglycerides
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building blocks of protein.
Amino acids
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covalent bonds formed between amino acids during protein synthesis by dehydration.
Peptide bonds
89
the amino acid sequence
Primary structure
90
results from hydrogen bonding between amino acids.
• Pleated (folded) sheets.
• Helices.
Secondary structure
91
change in shape caused by breaking of H-bonds by heat or pH changes.
Denaturation
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large-scale folding due to interactions within protein and surrounding environment which is generally water.
Tertiary structure
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Three-dimensional shape contains an ___ where reactants attach?
active site
94
reaction occurs when reactants bind to active site
Lock-and-key model
95
enzymes change shape to accommodate the shape of specific reactants.
Induced fit model
96
nonprotein substances that combine with active site and make nonfunctional enzymes functional.
Cofactors
97
Genetic material of cells copied from one generation to next.
Composed of 2 strands of DNA nucleotides.
DNA
98
sequence of bases that codes for synthesis of RNA or protein.
Gene
99
Adenosine Triphosphate (ATP)
~Energy currency of the body because it both stores energy and provides energy.
~Provides energy for other chemical reactions as anabolism or drive cell processes as muscle contraction.
~All energy-requiring chemical reactions stop when there is inadequate
