Chapter 2 - Chem Flashcards
(125 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
•the gravitational force acting on an object of a given mass.
A
weight
4
Q
•the simplest type of matter with unique chemical properties; composed of atoms of only one kind.
A
element
5
Q
smallest particle of an element that has chemical characteristics of that element.
A
atom
6
Q
The four most common elements in the body are
A
•hydrogen (H), carbon (C), nitrogen, (N), and oxygen (O).
7
Q
Other elements that are important to body function are found in small or trace amounts and include
A
fluorine (F), sodium (Na), magnesium (Mg), phosphorus (P), sulfur (S), chlorine (Cl), potassium (K), calcium (Ca), iron (Fe), and iodine (I).
8
Q
composed of subatomic particles.
A
Atoms
9
Q
•no electrical charge.
A
neutrons
10
Q
•one positive charge.
A
protons
11
Q
•one negative charge.
A
electrons
12
Q
formed by protons and neutrons.
A
nucleus
13
Q
Most of the volume of an atom occupied by electrons. Represented as:
A
electron cloud
14
Q
equal to number of protons in each atom, which is equal to the number of electrons.
A
atomic number
15
Q
number of protons plus number of neutrons
A
mass number
16
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
17
Q
average mass of naturally occurring isotopes.
A
atomic mass
18
Q
The unified atomic mass unit is 1/12 of the mass of carbon-12
A
Dalton (Da)
19
Q
6.022 x 10^23
A
Avogadro’s number
20
Q
mass of one mole of a substance in grams, which is equal to its atomic mass units.
A
molar mass
21
Q
formed when electrons in the outermost energy level (valence shell) are either shared with or transferred to another atom.
A
chemical bonds
22
Q
electrons are transferred from one atom to another.
A
ionic bonding
23
Q
two or more atoms share electron pairs.
A
covalent bonding
24
Q
a chemical property that measures an atom’s ability to attract electrons when it forms a chemical bond with another atom.
A
electronegativity
25
the closer an atom is achieving to an octet, the _____ its electronegativity
higher
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atoms that have gained or lost 1 or more electrons.
ions
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•are positively charged because they lost electrons.
cations
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negatively charged because they gained electrons
anions
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electrons are transferred between atoms, creating oppositely charged ions that are attracted to each other.
ionic bond
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Atoms share one or more pairs of electrons because the atoms have similar electronegativities.
covalent bonds
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•two atoms share one pair of electrons.
single covalent
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two atoms share 4 electrons.
double covalent
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•Electrons shared equally because nuclei attract the electrons equally.
nonpolar covalent
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Electrons not shared equally because one nucleus attracts the electrons more than the other does.
polar covalent
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two or more atoms chemically combined to form an independent unit.
molecules
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a substance composed of two or more different types of atoms chemically combined.
compounds
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determined by adding up atomic masses of its atoms or ions.
molecular mass
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Forces between molecules. Result from weak electrostatic attractions between oppositely charged parts of molecules, or between ions and molecules. Weaker than forces producing chemical bonding. Determine the properties of solubility and dissociation.
intermolecular forces
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ability of one substance to dissolve in another.
solubility
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in ionic compounds, cations are attracted to negative end and anions attracted to positive end of water molecules; the ions separate and each becomes surrounded by water molecules.
dissociation (separation)
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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.
electrolytes
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solutions made by molecules that dissolve in water, but do not dissociate; do not conduct electricity. Maintaining a proper electrolyte balance is important for many physiological body processes.
nonelectrolytes
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Atoms, ions, molecules or compounds interact to form or break chemical bonds.
chemical reaction
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•substances that enter into a chemical reaction.
reactants
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•substances that result from the reaction.
products
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collective term used for the sum of all of the anabolic and catabolic reactions in the body
metabolism
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Two or more reactants chemically combine to form a new and larger product. Collective term for synthesis reactions in body is
anabolism
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•synthetic reaction where water is a product. •Produce chemicals characteristic of life: carbohydrates, proteins, lipids, and nucleic acids.
dehydration reaction
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A large reactant is broken down to form smaller products. Collective term for decomposition reactions in body is
catabolism
50
•water is split into two parts that contribute to the formation of the products.
hydrolysis reaction
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•rate of product formation is equal to rate of reactant formation.
equilibrium
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loss of an electron by an atom.
oxidation
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gain of an electron by an atom.
reduction
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the complete or partial loss of an electron by one atom is accompanied by the gain of that electron by another atom.
oxidation-reduction reactions
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is the capacity to do work
energy
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•energy stored in chemical bonds; energy that could do work if it were released. Breaking chemical bonds releases energy.
potential energy
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•does work and moves matter.
kinetic energy
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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 principle
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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
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energy that flows between objects of different temperatures.
heat energy
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minimum energy reactants must have to start a chemical reaction.
activation energy
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substances that increase the rate of chemical reactions without being permanently changed or depleted.
catalysts
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•protein catalysts that increase the rate of chemical reactions by lowering the activation energy necessary for reaction to begin.
enzymes
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2 influences on reaction rate
temperature and concentration of reactants
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substances that do not contain carbon-hydrogen bonds.
inorganic chemistry
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study of carbon-containing substances
organic chemistry
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•substances attracted to water; “water-loving”.
hydrophilic
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•substances not attracted to water; “water-fearing”.
hydrophobic
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•the attraction of one water molecule to another; creates a surface tension
cohesion
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•the attraction of water molecules to other molecules; causes the upward movement of water in the xylem of plants.
adhesion
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%? of blood is composed of water
0.92
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properties of water;
stabilizing body temperature, protection, participates in chemical reactions, and mixing medium
74
•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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•which dissolves the solute.
solvent
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•which dissolves in the solvent.
solute
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•materials separate unless stirred. Examples: Sand and water; blood cells in plasma
suspension
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•dispersal of tiny particles through a medium that do not settle out. Example: Milk, plasma of the blood, cell interior
colloid
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measure of number of particles of solute per volume of solution. Percent solutions are based on the percent of solute by weight per volume of a solution.
concentration
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•reflects the number of particles dissolved in one kilogram of water.
osmolality
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one ____ is equal to Avogadro’s number of particles in one kilogram of water.
Osmole (osm)
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•Unit used by physiologists is _____ because of the low concentrations in the human body.
milliosmoles (mOsm)
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a proton donor or any substance that releases hydrogen ions.
acid
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a proton acceptor or any substance that binds to or accepts hydrogen ions. Many bases acts as hydrogen receptors because they release hydroxide ions (OH^-) when they dissociate
base
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•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)
89
The normal pH range for human blood is
7.35 to 7.45
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a condition in which the nervous system becomes depressed and the individual may become disoriented and possibly comatose. blood pH dropping below 7.35
acidosis
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a condition in which the nervous system becomes overexcitable and the individual may be very nervous or have convulsion. If blood pH rises about 7.45
alkalosis
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a compound consisting of a cation other than a hydrogen ion and an anion other than a hydroxide ion. Example: NaCl.
salt
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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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•what remains of an acid once it loses its hydrogen ion.
conjugate base
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•what is formed when a proton is transferred to the base.
conjugate acid
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required in the final step in the series of reactions used to extract energy from food.
oxygen
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produced during the catabolism of organic compounds.
carbon dioxide
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four major groups of organic molecules essential to living organisms
carbohydrates, lipids, proteins, and nucleic acids
99
composed of carbon, hydrogen, oxygen. Divided into monosaccharides, disaccharides, polysaccharides. Energy sources, structure, and bulk for elimination. Water soluble
carbohydates
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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: A T P, D N A, R N A.
nucleic acids
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molecules that have the same number/types of atoms but differ in their 3-D arrangement.
isomers
104
composed of glycerol and fatty acids. Each fatty acid has a carboxyl group. Fatty acids combine with glycerol to form triglyceride.
triglycerides
105
•contains all single bonds in the carbon chain, which produces a more rigid structure; generally solid. Fatty acid
saturated
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•contains one (mono) or more (poly) double bonds in the carbon chain, which produces a more relaxed structure; generally liquid. Better because they do not stick to the inside of blood vessels. Fatty acid
unsaturated
107
unsaturated fats that are artificially altered to be more saturated. Are the highest cardiovascular risk fat.
trans fats
108
Derived from fatty acids. Function: important regulatory molecules. Include thromboxanes, leukotrienes, and prostaglandins.
eicosanoids
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nonpolar molecules essential for normal functioning.
fat-soluble vitamins
110
Lipids with four ring-like structures. Examples: cholesterol, bile salts
steroids
111
building blocks of protein.
amino acids
112
covalent bonds formed between amino acids during protein synthesis by dehydration.
peptide bonds
113
the amino acid sequence
primary structure
114
results from hydrogen bonding between amino acids. Pleated (folded) sheets/ Helices. (protein structure)
secondary structure (protein)
115
change in shape caused by breaking of H-bonds by heat or pH changes.
denaturation
116
large-scale folding due to interactions within protein and surrounding environment which is generally water. Polar regions tend to remain unfolded and in contact with water while nonpolar regions tend to fold inward away from water. Stabilized by disulfide bonds. Determines shape of a domain and the function of the protein.
tertiary structure
117
results from the association of two or more proteins (subunits). protein structure
quaternary structure
118
reaction occurs when reactants bind to active site.
Lock-and-key model
119
enzymes change shape to accommodate the shape of specific reactants.
Enzyme names usually end in –ase and often have the same word stem as the reactant; for example, a lipid is a reactant for lipase.
Induced fit model
120
nonprotein substances that combine with active site and make nonfunctional enzymes functional.
Cofactors
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composed of nucleotides. Include deoxyribonucleic acid (D N A), ribonucleic acid (R N A), and A T P.
nucleic acids
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•Composed of a five-carbon sugar (deoxyribose or ribose), a nitrogenous base, and a phosphate.
nucleotides
123
sequence of bases that codes for synthesis of R N A or protein. Base sequence determines the primary structure of a protein.
Gene
124
Genetic material of cells copied from one generation to next. Composed of 2 strands of D N A nucleotides.
•A and T; G and C = complementary base pairs held by H-bonds. •Connect like rungs of a ladder and twist to form double helix.
The two strands of a D N A molecule are antiparallel.
•Sugar-phosphate backbones oriented in opposite directions.
DNA
125
•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.
ATP
