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289 Cards in this Set
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The science of the composition, structure, properties, and reactions of matter, especially of atomic and molecular systems.
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Chemistry
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The science dealing with the composition of matter and the changes in composition that matter undergoes.
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Chemistry
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Chagnes that involve the rearrangement of the position of particles within the solid
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Memory
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1) Collect the facts or data that are relevent to the problem or question at hand
2) Formulate a hypothesis that will account for the data and that can be tested by further experimentation 3) Plan and do additional experiments to test the hypothesis 4) Modify the hypothesis as necessary so that it is compatible wit hall the pertinent data |
Scientific Method
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A tentative explanation of certain facts that provides a basis for further experimentation
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Hypothesis
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A well-established hypothesis is often called a __________ or model, An explanation of the general principles of certain phenomena with considerable evidence or facts to support it
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Theory
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Simple statements of natural phenomena to which no exceptions are known under the given conditions
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Scientific laws
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The quantity or amount of matter that an object possesses
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Mass
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A measure of the earth's gravitational attraction for a body
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Weight
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The number of digits that are known plus one estimated digit are considered significant in a measured quantity; also called significant digits
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Significant figures
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The process by which the value of the last digit retained is determined after dropping nonsignificant digits
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Rounding off numbers
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Writing a number as a power of 10; to do this, move the decimal point in the original numbers so that it is located after the first nonzero digit, and follow the new number by a multiplication sign and 10 with an exponent (called its power) that is the number of places the decimal point was moved.
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Scientific notation
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A decimal system of measurements; An agreed-upn standard system of measurements used by scientists around the world
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Metric system or SI
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The standard unit of length in the SI and metric systems; equals 39.37 inches
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Meter
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The standard unit of mass in the metric system; equals 2.205 lbs.
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Kilogram
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The amount of space occupied by matter; measured in SI units by cubic meters, but also commonly in liters and milliliters
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Volume
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A unit of volume commonly used in chemistry; =1000 mL
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Liter
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A form of energy associated with the motion of small particles of matter
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Heat
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A measure of the intensity of heat, or of how hot or cold a system is; SI unit is the kelvin
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Temperature
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The mass of an object divided by its volume
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Density
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The ratio of the density of one substance to the density of another substance taken as a standard. Water is usually the standard for liquids and solids; air, for gass
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Specific gravity
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Anything that has mass and occupies space
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Matter
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Has a definite shape and volume, with particles that coere rigidly to one another, can be independent of its container
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Solid
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Without shape or form
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Amorphous
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Has a definite volume, but not a definite shape, with particles that cohere firmly, but not rigidly, able to move freely
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Liquid
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Has indefinite volume and no fixed shape, with particles that move indeendently of one anothers
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Gas
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A particular kind of matter with a definite, fixed composition
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Substance
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Uniform in appearance and has the same properties throughout
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Homogeneous
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Matter consisting of two or more physically distinct phases
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Heterogeneous
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A homogeneous part of a system separated from other parts by physical boundaries
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Phase
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Simply the body of matter under consideration
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System
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A material containing two or more substances and can be either heterogeneous or homogeneous, variable in composition
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Mixture
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A fundamental or elementary substance that cannot be broken down by chemical means to simpler substances
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Element
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Smallest particle of an element
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Atom
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Abbreviation of an element, Ba I N O Ag
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Symbol
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Solids at room temperature, have high luster, are good conductors of heat and electricity, are malleable, and are ductile, have a high melting point and high density
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Metals
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Are not lustrous, have relatively low melting points and densities, and are generally poor conductors of heat and electricity, Combine with one another
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Nonmetals
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An element having properties that are intermediate between those of metals and nonmetals (ex. Silicon); these elements are useful in electronics
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Metalloids
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A distinct substance that contains two or more elements chemically combined in definite proportion by mass
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Compound
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The smallest uncharged individual unit of ompund formed by the union of two or more atoms
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Molecule
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A positively or negatively charged atom or group of atoms
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Ion
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Positively charged ions
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Cation
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Negatively charged ion
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Anion
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The molecules of elements that always contain two atoms. Seven elements occur: H2, N2, O2, F2, Cl2, Br2, and I2
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Diatomic molecules
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Used as abbreviations for compounds, shows the symbols and the ratio of the atoms of the elements in a compound
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Chemical formula
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Numbers that appear partially below the line and to the right of a symbol of an element
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Subscripts
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The characteristics, or traits, of substances that give them their unique identities, classified as physical or chemical
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Properties
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The inherent characteristics of a substance that can be determined without altering its composition; they are associated with its physical existance
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Physical properties
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Describe the ability of a substance to form new substances, either by reaction with other substances or by decomposition
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Chemical properties
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Changes in physical properties (such as size, shape, and density) or changes in the state of matter without an accompanying change in composition
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Physical changes
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New substances are formed that have different properties and composition from the original material. The new substances need not resemble the initial material in any way.
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Chemical change
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A shorthand expression showing the composition and the products of a chemical change (for example, 2H20= 2H2 + 02)
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Chemical equations
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The starting substances (water, copper, and oxygen)
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Reactants
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The substance produced (hydrogen, oxygen, and copper (II) oxide)
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Products
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States that no change is observed in the total mass of the substances involved in a chemical change
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Law of Conservation of Mass
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The capacity of matter to do work
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Energy
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Stored energy; or energy that an object possesses due to its relative position.
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Potential energy (PE)
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Energy that matter possesses due to its motion.
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Kinetic energy (KE)
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The SI unit of energy, see also calorie
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Joules
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A commonly used unit of heat energy; 1 calorie is a quantity of heat energy that will raise the temperature of 1 g of water 1° C
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Calorie
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The quantity of heat (lost or gained) required to cahnge the temperature of 1 g of that substance by 1° C
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Specific heat
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Energy can be neither created nor destroyed, though it can be transformed from one form to another
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Law of Conservation of Energy
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The first modern atomic theory to state that elements are composed of minute individual particles called atoms
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Dalton's atomic model
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A compound always contains two or more elements combined in a definite proportion by mass
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Law of Definite composition
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Atoms of two or more elements may combine in different ratios to produce more than one compound
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Law of Multiple proportions
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Electrons, protons, and neutrons
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Subatomic particles
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A particle with a negative electrical charge and a mass of 9.110 x 10 -28 g
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Electron (e-)
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A particle with a relative mass of 1 amu and an actual mass of 1.673 x 10 -24 g. Has relative charge (+1)
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Proton
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The electrons are negatively charged particles embedded in the atomic sphere, atoms are electrically neutral, sphere contains equal number of protons, or positive charges
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Thomson model of the atom
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Has neither a positive nor a negative charge and has a relatvie mass of about 1 amu. Slightly greater mass than proton
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Neutron
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The central part of an atom that contains all its protons and neutrons. Very dense and has a positive electrical charge
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Nucleus
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The number of protons in the nucleus of an atom of that element
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Atomic Number
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Atoms of an element having the same atomic number but different atomic masses
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Isotopes
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A unit of mass equal to one-twelth the mass of a carbon-12 atom.
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Atomic Mass Unit
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The average relative mass of the isotopes of that element compared to the atomic mass of carbon-12 ( exactly 12.0000... amu)
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Atomic Mass
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The system of names that chemists use to identify compounds
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Chemical nomenclature
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Compounds that do not generally contain carbon
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Inorganic compounds
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Two atoms bonded together to make a molecule, Seven of the elements
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Diatomic molecules
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Hydrogen, Oxygen, Nitrogen, Chlorine, Fluorine, Bromine, Iodine
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2
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Sulfur
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8
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Phosphorus
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4
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A charged particle can be produced by adding or removing one or more electrons from a neutral atom
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Ion
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Any neutral atom that loses an electron will form a(n) _______
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Cation
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Any neutral atom that gains an electron will form a(n) _________
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Anion
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To name an anion consisting of only one element, use the stem of the parent element name and change the ending to ________
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-ide
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Most often ions are formed when metals combine with ____________
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Nonmetals
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Compound that contains only two different elements
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Binary compound
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The cation is written first in the formula, followed by the ___________
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anion
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1) Cu 1+, copper (I)
2) Cu 2+, copper (II) 3) Hg 1+ (Hg2)2+, Mercury (I) 4) HG 2+, Mercury (II) |
1) Cuprous
2) Cupric 3) Mercurous 4) Mercuric |
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1) Fe 2+, Iron (II)
2) Fe 3+, Iron (III) 3) Sn 2+, Tin (II) 4) Sn 4+, Tin (IV) 5) Pb 2+, Lead (II) |
1) Ferrous
2) Ferric 3) Stannous 4) Stannic 5) Plumbous |
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1) Pb 4+, Lead (IV)
2) As 3+, Arsenic (III) 3) As 5+, Arsenic (V) 4) Ti 3+, Titanium (III) 5) Ti 4+, Titanium (IV) |
1) Plumbic
2) Arsenous 3) Arsenic 4) Titanous 5) Titanic |
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Symbols written and occur first in a series when a compound is formed between two nonmetals
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Si, B, P, H, C, S, I, Dr, N, Cl, O, F
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1) Nona
2) Hepta 3) Tetra 4) Mono |
1) 9
2) 7 3) 4 5) 1 |
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1) Deca
2) Octa 3) Hexa 4) Penta 5) Tri 6) Di |
1) 10
2) 8 3) 6 4) 5 5) 3 6) 2 |
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S₂F₁₀
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disulfur decafluoride
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CCl₄
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carbon tetrachlorid
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N₂O₅
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dinitrogen pentaoxide
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Composed of hyrdrogen and one other nonmetallic element
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Binary acids
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Binary Acids
1) HF 2) HCl 3) H₂S |
1) Hydrofluoric acid
2) Hydrochloric acid 3) Hydrosulfuric acid |
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1) HBr
2) HI 3) H₂Se |
1) Hydrobromic acid
2) Hydroiodic acid 3) Hydroselenic acid |
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1) Write the prefix hydro- followed by the stem of the second element and add the suffix ic
2) Write the word acid |
Naming binary acids
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An ion that contains two or more elements
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Polyatomic ion
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1) Acetate
2) Ammonium 3) Arsenate 4) Hydrogen carbonate 5) Hydrogen sulfate 6) Bromate 7) Carbonate 8) Chlorate 9) Chromate |
1) C₂H₃O₂⁻
2) NH₄⁺ 3) AsO₄ 3- 4) HCO₃⁻ 5) HSO₄⁻ 6) BrO₃⁻ 7) CO₃ 2- 8) ClO₃⁻ 9) CrO₄ 2- |
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1) Cyanide
2) Dichromate 3) Hydroxide 4) Nitrate 5) Nitrite 6) Permangante 7) Phosphate 8) Sulfate 9) Sulfite |
1) CN⁻
2) Cr₂O₇ 2- 3) OH⁻ 4) NO₃⁻ 5) NO₂⁻ 6) MnO₄⁻ 7) PO₄ 3- 8) SO₄ 2- 9) SO₃ 2- |
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A system that uses Roman numerals to name elements that form more than one type of cation
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Stock System
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1) Hypochlorite
2) Chlorite 3) Chlorate 4) Perchlorate |
1) ClO⁻
2) ClO₂⁻ 3) ClO₃⁻ 4) ClO₄⁻ |
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1) Hypochlorous acid
2) Chlorous acid 3) Chloric acid 4) Perchloric acid |
1) HClO
2) HClO₂ 3) HClO₃ 4) HClO₄ |
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1) Sulfate ion
2) Sulfite ion 3) Nitrate ion 4) Nitrite ion 5) Carbonate ion 6) Borate ion |
1) SO₄ 2-
2) SO₃ 2- 3) NO₃⁻ 4) NO₂⁻ 5) CO₃ 2- 6) BO₃ 3- |
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1) Phosphate ion
2) Phosphite ion 3) Iodate ion 4) Acetate ion 5) Oxalate ion 6) Bromate ion |
1) PO₄ 3-
2) PO₃ 3- 3) IO₃⁻ 4) C₂H₃O₂⁻ 5) C₂O₄ 2- 6) BrO₃⁻ |
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1 mol, 6.022 x 10^23
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Avagadro's Number
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6.022 x 10^23 items=
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1 mole
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The mass of avogadro's number of atoms or molecules
H- 1.008 amu- 1.008 g- 6.022 x 10^23 |
Molar Mass
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The mass percent represented by each element in a compound
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Percent composition of a compound
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Gives the smallest whole-number ratio of atoms present in a compound, gives the relative numbe of atoms of each element in the compound
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Empirical formula
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The true formula, representing the toal number of atoms of each element present in one molecule of a compound
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Molecular formula
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The substances entering the reaction are called
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the reactants
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The substances formed are called
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the products
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A shorthand expression for a chemical change or reaction, uses the chemical symbols and formulas of the reactants and products and other symbolic terms to represent a chemical reaction
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Chemical equation
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Contains the same number of each kind of atom on each side of the eqaution, obeys the law of conservation of mass
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Balanced equation
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Two reactants combine to give one product, A + B ---- AB
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Combination reaction
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One element reacts with a compound to replace one of the elements of that compound, yeilding a different element and a different compound
A + BC ---- B + AC or A + BC ---- C + BA |
Single-displacement reaction
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A single substance is decomposed, or broken down, to give two or more different substances. This reaction may be considered the reverse of combination
AB --- A + B |
Decomposition reaction
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Two compounds exchange partners with each other to produce two different compounds
AB + CD ---- AD + CB |
Double-displacement reaction
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Liberate heat
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Exothermic reactions
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Absorb heat
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Endothermic reactions
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The quantity of heat produced by a reaction is known as
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Heat of reaction
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Compounds containing only hydrogen and carbon
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Hydrocarbons
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The amount of energy that must be supplied to start a chemical reaction is called the
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Activation energy
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The sum of the atomic masses of all the atoms in an element or compound, applies to the mass of a mole of any formula unit- atoms, molecules, or ions; it is the atomic mass of an atom, or the sum of the atomic masses in a molecule or an ion (in grams)
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Molar mass
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The smallest unit of a molecular substance and a mole is Avogadro's number of molecules of that substance
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Relationship between molecule and mole
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The area of chemistry that deals with quantitative relationships among reactants and products is known as
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Stoichiometry
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A ratio between the number of moles of any two species involved in a chemical reaction
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Mole ratio
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It limits the amount of product that can be formed
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Limiting reactant
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The calculated amount of product that can be obtained from a given amount of reactant, according to the chemical equation
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Theoretical yield
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The amount of product that we finally obtain
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Actual yield
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The ratio of the actual yield to the theoretical yield multiplied by 100
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Percent yeild
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The distance between consecutive peaks (or troughs) in a wave
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Wavelength
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Tells how many waves pass a particular point per second
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Frequency
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Tells how fast a wave moves through space
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Speed
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A beam of light behaves like a stream of timy packets of energy called
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Photons
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Colored lines generated when light emitted by a gas is passed through a spectroscope.
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Line spectrum
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Energy is never emitted in a continuous stream buy only in small discrete packets called
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Quanta
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Number of energy levels are available, the lowest of which is called the ______ _______
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Ground state
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A cloudlike region around the nucleus where electrons are located. Considered to be energy sublevels (s,p,d,f) within the principal energy levels
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Orbitals
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Existing within the atom, these energy levels contain orbitals within which electrons are found
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Principal energy levels of electrons
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Each principal energy level is divided into
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Sublevels
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A property of an electron that describes its appearance of spinning on an axis like a globe
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Spin
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An atomic orbital can hold a maximum of two electrons, which must have opposite spins
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Pauli exclusion principle
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The orbital arrangement of electrons in an atom
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Electron configuration
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An electron in the outermost energy level of an atom; these electrons are the ones involved in bonding atoms together to form compounds
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Valence electrons
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Each horizontal row in the periodic table is called a
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Period
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Elements that behave in a similar manner are found in, form the vertical columns on the periodic table
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Groups or Families
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The A groups are known as the
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Representative elements
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The B groups and Group VIII are called
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Transition elements
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An atom is the energy required to remove an electron from the atom
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Ionization energy
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An atom is a representation that shows the valence electrons for that atom
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Lewis structure
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The attraction between oppositely charged ions
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Ionic bond
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Consists of a pair of electrons shared between two atoms
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Covalent bond
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A covalent bond between two atoms with differeing electronegativity values, resulting in unequal sharing of bonding electrons
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Polar covalent bond
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The relative attraction that an atom has for a pair of shared electrons in a covalent bond
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Electronegativity
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If the electronegativities are the same, the bond is ________ ________ and the electrons are shared equally
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Nonpolar covalent
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A molecule that is electrically asymmetrical, causing it to be oppositely charged at two points
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Dipole
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When only two pairs of electrons surround a central atom, they should be placed 180 degrees apart to give a _______________
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Linear structure
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When three pairs of electrons surround an atom, they should be placed 120 degrees apart to show the ____________________
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trigonal planar structure
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Wehn four pairs of electrons surround a central atom, they should be placed 109.5 degrees apart to give them a ____________________
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tetrahedral structure
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A group of assumptions used to explain the behavior and properties of gases
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Kinetic-molecular theory (KMT)
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A gas that behaves exactly as outlined by the theory is known as
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Ideal Gas
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1/2mv^2
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KE (Kinetic Energy)
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The ability of two or more gases to mix spontaneously until they form a uniform mixture
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Diffusion
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A process by which gas molecules pass through a very small orifice (opening) from a container at higher pressure to one at lower pressure
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Effusion
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The reates of effusion of two gases at the same temperature and pressure are inversely proportional to the square roots of their densities, or molar masses
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Graham's law of effusion
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Defined as forcer per unit area
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Pressure
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The pressure experienced by objects on Earth as a result of the layer of air surrounding our planet.
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Atmospheric Pressure (ATM)
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A device used to measure atmospheric pressure
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Barometer
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The standard atmospheric pressure, the pressure exerted by a column of mercury 760 mm high at a temperature of 0 C
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1 atmosphere (atm)
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At constant temperature (T) the volume (V) of a fixed mass of gas is inversely proportional to the pressure (P), which may be expressed as:
P₁V₁ = P₂V₂ |
Boyle's law
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-273 Degrees C; this temperature is the zero point on the Kelvin (absolute) temperature scale--the temperature at which the volume of an ideal, or perfect, gas would become zero
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Absolute Zero
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At constant pressure the volume of a fixed mass of any gas is directly proportional to the absolute temperature, which may be expressed as:
V₁/T₁ = V₂/T₂ |
Charle's Law
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The pressure of a fixed mass of a gas, at constant volume, is directly proportional to the Kelvin temperature:
P₁/T₁ = P₂/T₂ |
Gay-Lussac's Law
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0 degress Celcius (273 K) and 1 atm (760 torr)
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Standard Conditions
Standard Temperature and Pressure (STP) |
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The total pressure of a mixture of gases is the sum of the partial pressures exerted by each of the gases in the mixture
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Dalton's law of partial pressures
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The pressure exerted independently by each gas in a mixture of gases
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Partial pressure
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Whem measured at the same temperature and pressure, the ratios of the volumes of reacting gases are small whole numbers
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Gay-Lussac's law of combining volumes
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Equal volumes of different gases at the same temperature and pressure contain the same number of molecules
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Avagadro's law
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he volume of 1 mol of a gas at STP equals 22.4 L/mol
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Molar volume (of a gas)
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Mass/Volume or g/L
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Density
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PV = nRT
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Ideal Gas Equation
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A substance existing in two or more molecular or crystalline forms (example: graphite and diamond are two ______ forms of carbon)
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Allotrope
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The escape of molecules from the liquid state to the gas or vapor state
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Evaporation
Vaporization |
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Solid -------> Vapor
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Sublimination
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The process by which molecules in the gaseous state return to the liquid state
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Condensation
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The pressure exerted by a vapor in equilibrium with its liquid is known as the _____ _______
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Vapor pressure
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A substance that evaporates readily; a liquid with a high vapor pressure and a low boiling point
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Volatile
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The resistance of a liquid to an increase in its surface area is called
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Surface tension
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The spontaneous rising of a liquid in a narrow tube, which results from the cohesive forces within the liquid and the adhesive forces between the liquid and the walls of the container
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Capillary action
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The temperature at which the vapor pressure of a liquid is equal to the external pressure above the liquid
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Boiling point
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The temperature at which the vapor pressure of a liquid equals 1 atm or 760 torr pressure
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Normal boiling point
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A graph generated by plotting the temperature of a liquid on the x-axis and its vapor pressure on the y-axis.
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Vapor-pressure curve
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The temperature at which the solid and liquid states of a substance are in equilibrium
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Freezing or Meling point
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The energy required to change exactly one gram of a solid at its melting point into a liquid is called
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Heat of Fusion
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The energy required to change exactly one gram of liquid to vapor at its normal boiling point
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Heat of Vaporization
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Water is a highly polar molecule. It therefore does not have a ______ ________
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Linear structure
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The intermolecular force acting between molecules that contain hydrogen covalently bonded to the highly electronegative elements, F, O, and N
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Hydrogen bond
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Solids that contain water molecules as part of their crystallin structure are known as
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Hydrates
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Water in a hydrate is known as
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Water of hydration
Water of crystallization |
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"without water"
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Anhydrous
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A system in which one or more substances are homogeneously mixed or dissolved in another substance
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Solution
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The substance that is dissolved--or the lest abundant component--in a solution
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Solute
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The dissolving agent or the most abundant component in a solution
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Solvent
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Describes the amount of one substance (solute) that will dissolve in a specified amount of another substance (solvent) under stated conditions
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Solubility
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Liquids that are capable of mixing and forming a solution
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Miscibile
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Those that do not form solutions or are generally insoluble in each other
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Immiscible
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The quantitative expression of the amount of dissolved solute in a particular quantity of solvent is known
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Concentration of a solution
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A solution containing dissolved solute in equilibrium with undissolved solute
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Saturated solution
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A solution containing less solute per unit volume than its corresponding saturated solution
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Unsaturated solution
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A solution containing more solute than needed for a saturated solution at a particular temperature
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Supersaturated solution
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Describes a solution that contains a relatively small amount of dissolved solute
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Dilute solution
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Contains a relatively large amount of dissolved solute
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Concentrated solution
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g solute/g solute + g solvent X 1,000,000 =
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Parts per million (ppm)
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g solute/ g solute + g solvent X 100 =
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Mass percent
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number of moles of solute
_________________________ = liter of solution |
Molarity (M)
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Properties that depend only on the number of solute particles in a solution and not on the nature of those particles
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Colligative properties
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A membrane that allows the passage of water (solvent) molecules through it in either direction but prevents the passage of larger solute molecules or ions
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Semipermeable membrane
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The diffusion of water, either from a dilute solution or from pure water, through a semipermeable membrane into a solution of higer concentration
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Osmosis
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A solution contains an excess of H⁺ ions
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Arrhenius acid
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A solution contains an excess of OH⁻ ions
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Arrhenis base
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A acid is a proton (H⁺) donor
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Bronsted-Lowry acid
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A base is a proton (H⁺) acceptor
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Bronsted-Lowry base
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The result of a protein combining with a polar water molecule to form a hydrated hydrogen ion, H₃O⁺
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Hydronium ion
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An electron-pair acceptor
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Lewis acid
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An electron-pair donor
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Lewis base
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A substance having properties of both an acid and a base
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Amphoteric
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Substances whose aqueous solutions are conductors of electricity are called
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Electrolytes
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Substances whose solutions are nonconductors are known as
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Nonelectrolytes
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The process by which the ions of a salt separate as the salt dissolves
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Dissociation
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Acids, bases, and salts are __________
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electrolytes
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The formation of ions; it occurs as a result of a chemical reaction of certain substances with water
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Ionization
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Are essentially 100% ionized in solution
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Strong electrolytes
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Are much less ionized (based on comparing 0.1 M solutions)
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Weak electrolytes
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-log[H⁺] =
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pH
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pH < 7.00
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Acidic solution
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pH = 7.00
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Neutral solution
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pH > 7.00
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Basic solution
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The power to which 10 must be raised to give that number
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Logarithm
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The negative logarithm of the H⁺ or H₃O⁺ concentration in moles per liter
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pH
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The reaction of an acid and a base to form a salt and water
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Neutralization
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An ion in solution that does not undergo chemical change during a chemical reaction
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Spectator ions
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The process of measuring the volume of one reagent required to react with a measured mass or volume of another reagent
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Titration
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Compounds are written in their molecular, or formula expressions
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Un-ionized equation
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Compounds are written to show the form in which they are predominantly present; strong electrolytes as ions in solution; and nonelectrolytes, weak electrolytes, precipitates, and gases in their molecular (or un-ionized ) forms
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Total ionic equation
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Only those molecules or ions that have changed are included in the equation; ions are molecules that do not change (the spectators) are omitted
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Net ionic equation
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A dispersion in which the dispersed particles are larger than the solute ions or molecules of a true solution and smaller than the particles of a mechanical suspension
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Colloid
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The random motion of colloidal particles are called
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Brownian movement
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An intense beam of light is clearly visible when passed thourhg a colloidal dispersion, but is not visible when passed through a true solution
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Tyndall effect
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Dissovled solutes can be removed from colloidal dispersions through the use of such a membrane by a process called _____.
The process by which a parchment membrane allows the passage of true solutions, but prevents passage of colloidal dispersions |
Dialysis
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The total mass remains constant during a chemical reaction. What law is this?
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Law of conservation of mass
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All samples of a compound have the same composition; that is, all samples have the same proportions, by mass, of the elements present in the compound. What law is this?
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Law of constant composition
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In two or more compounds of the same elements, the masses of one element that comine with a fixed mass of the second element are in the ratio of small whole number. What law is this?
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Law of multiple proportions
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What has a relative mass of 1, also carries one fundamental unit of positive electric charge, denoted 1+?
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Proton
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What is an electrically neutral particle; it has no charge, has a slightly greater mass than that of the proton?
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Neutron
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What has a mass that is 1/1836 of the mass of a proton, has the same quantity of charge as a proton, but it is a negative charge, denoted as 1-?
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Electron
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Protons and neutrons are densely packed into a tiny, positively charged core of atom known as the _________.
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Nucleus
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What is the number of protons in the nucleus of an atom of a give element?
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Atomic number (Z)
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Atoms that have the same number of protons but different numbers of neutrons are called _______.
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Isotopes
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What is the sum of the numbers of protons and neutrons in an atom, always an integral (whole) number.
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Mass number (A)
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Exactly one-twelth the mass of a carbon-12 atom
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Atomic Mass Unit
|
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1.66054 X 10^-24 g =
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1 amu or u
|
|
What is the weighted average of the masses of the naturally occurring isotopes of that element?
|
Atomic mass
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Mendeleev arranged the elements in order of increasing atomic weight, from left to right in rows and from top to bottom in columns (or groups). Elements that most closely resemble one another in physical and chemical properties tend to fall in the same vertical group. This group similarity recurs periodcially, hence the name __________ ________.
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Periodic Table
|
|
Elements that lack metalic properties, to the right of the stepped line are ________
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Nonmetals
|
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Some of the elements bordering the stepped line resemble metals in some of their properties and nonmetals in other. They are sometimes considered in a special category called semimetals or _________
|
Metalloids
|
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A symbolic representation of the composition of a compound expressed in terms of its constituent elements is a ____________ _________
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Chemical formula
|
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A group of two or more atoms held together in a definite spatial arrangement by forces called covalent bonds
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Molecule
|
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Molecules are the smallest characteristic entites of a ______ ________, and these molecules determine the properties of the substance.
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Molecular compound
|
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The simplest formula we can write for a compound. It lists the elements present and indicates the smallest integral (whole-number) ratio in which atoms of these elements are combined
|
Emperical formula
|
|
Show the differences between compounds with identical empirical formulas by giving the symbol and the actual number of each kind of atom in a molecule
|
Molecular formula
|
|
A chemical formula that shows how atoms are attached to one another
|
Structural formula
|
|
A individual atom or a group of bonded atoms may lose or gain one ore more electrons, thereby acquiring a net electric charge and becoming and _______
|
Ion
|
|
Positively charged ions are called _______
|
Cations
|
|
Negatively charged ions are called ________
|
Anions
|
|
Oppositely charged ions (cations and anions) attract one another and are held together in huge clusters by electrostatic attractions, such clusters are called _________ _________
|
Ionic compounds
|
|
Because ionic compounds do not consist of discrete molecules, we base the chemical formula on the simplest collection of cations and anions that represents an electrically neutral unit. We call this hypothetical collection of ions a _______ ______ of the compound.
|
Formula unit
|
|
A charged group of bonded atoms--for example, NH₄+ or SO₄2-
|
Polyatomic ion
|
|
A ionic compound in which the formula unit includes a fixed number of water molecules associated with the cations and anions
|
Hydrate
|
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Substances that have the following characteristics when dissolved in water:
- Tasts sour if diluted with enough water to be tasted safely - Produce a pricking or stinging sensation on the skin - Turn the color of litmus, an indicator dye, from blue to red - React with many metals to produce ionic compounds and hydrogen gas - React with bases, thereby losing their acidic properties |
Acids
|
|
Are substances that have the following characteristics when dissolved in water:
- Taste bitter if diluted with enough water to be tasted safely - Feel slippery or soapy on the skin - Turn the color of the indicator dye litmus from red to blue - React with acids, thereby losing their basic properties |
Bases
|
|
A molecular compound (such as HBr) that ionizes, or breaks up, in water to form a solution containing H+ cations plus anions (such as Br-)
|
Arrhenius acid
|
|
A compound that ionizes in water to form a solution containing OH- anions and related cations
|
Arrhenius base
|
|
The cation from the base and the anion from the acid make up an ionic compound called a _______
|
Salt
|