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| the scientific study of the composition, structure, and properties of matter and the changes that matter undergoes |
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| an explanation that is based on prior scientific research or observations and that can be tested |
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| a measure of the amount of matter in an object |
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| a measure of the gravitational force exerted on an object |
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| the ratio of the mass of a substance to the volume of the substance |
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| carried out for the sake of increasing knowledge |
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| carried out to solve a problem |
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| focuses on most carbon-containing compounds |
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| focuses on non-organic substances |
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| focuses on processes occuring in living things |
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| focuses on composition of materials |
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| meter-length; kilogram-mass; second-time; kelvin-temperature; mole-amount of substance; ampere-electrical current; candela-luminous intensity |
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| a description of how close a measurement is to the true value of the quantity measured |
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| the exactness of a measurement |
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| any digit of a number that is known with certainty |
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| in between significant numbers and final zeros after the decimal point |
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45,600,000=4.56x10^8
.00000526=5.26x10^-7 |
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| anything that has mass and takes up space |
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| a substance that cannot be separated or broken down into simpler substances by chemical means |
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| a substance made up of atoms of two or more different elements joined by chemical bonds |
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| a combination of two or more substances that are not chemically combined |
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| matter and energy are conserved |
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| energy is transformed into another so it's never destroyed. matter can be changed into energy so it can continue to exist in other forms |
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| solid, liquid, gas, and plasma |
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| definite volume and shape |
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| definite volume but indefinite shape |
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| neither definite volume nor shape |
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| high temperature, atoms lose most of their electrons |
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| a change of matter from one form to another |
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| a change that occurs when one or more substances change into new substances with different properties |
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| the smalles unit of an element that maintains the chemical properties of that element |
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| the positively-charged dense center of an atom |
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| an atom, radical, or molecule that has gained or lost one or more electrons and has a negative or positive charge |
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| an atom that has the same number of protons as other atoms of the same element but different number of neutrons |
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| the number of protons in the nucleus of an atom |
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| the mass of an atom of a chemical element expressed in atomic mass units |
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| protons, neutrons, and electrons |
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| in the nucleus with a positive charge (same as atomic number) |
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| in the nucleus with a neutral charge (same as protons) |
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| in the electron cloud with a negative charge (protons+electrons/2) |
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| same as atomic mass . g/mol |
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| the number of waves produced in a given amount of time |
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| the distance from any point on a wave to an identical point on the next wave |
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| the height of a wave from its trough or crest to its midpoint |
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| electromagnetic radiation |
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| the radiation associated with an electric and magnetic field |
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| the basic unit of electromagnetic energy |
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| a unit or quantum of light |
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| the lowest energy state of a quantized system |
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| red, orange, yellow, green, indigo, violet |
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| speed of light (3x10^8 m/s) |
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60.626x10^-3 x wavelength
Max Planck |
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| refers to the emission of electrons from a metal when light shines on the metal |
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| the energy level denoted by the principal quantum number |
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| a part of a level which can hold a different number of electrons |
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| a region in an atom where there is a high probability of finding electrons |
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| s=1(2), p=3(6), d=5(10), f=7(14) |
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| an electron occupies the lowest-energy orbital that can receive it |
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| Pauli Exclusion Principle |
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| no two electrons in the same atom can have the same set of four quantum numbers |
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| orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron and all electrons in singly occupied orbitals must have the same spin state |
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| 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 4f 5d 6s 6p |
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| an arrangement of the elements in order of their atomic numbers |
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| a horizontal row of elements in the periodic table |
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| a vertical column of elements in the periodic table |
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| electrons that are found in the outermost shell of an atom |
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| atoms tend to gain, lose, or share electrons to have eight electrons in the outer shell |
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| elements that are shiny and conduct heat and electricity well |
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| elements that conduct heat and electricity poorly |
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| credited for developing the modern periodic table |
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| transition metals&d block |
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| lanthanides and actinides&f block |
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| one-half of the distance between the center of identical atoms that are not bonded together |
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| the energy required to remove an electron from an atom or ion |
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| the energy needed to remove an electron from a negative ion to form a neutral atom or molecule |
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| a measure of the ability of an atom in a chemical compound to attract electrons |
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| a force that attracts electrons from one atom to another which transforms neutral to ions |
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| a bond formed when atoms share one or more pairs of electrons |
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| a covalent bond in which a pair of electrons shared by two atoms is held more closely by one atom |
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| a covalent bond in which the bonding electrons are equally attracted to both bonded atoms |
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| the smallest unit of a substance that keeps all the physical and chemical properties of that substance |
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| the number of electrons that must be added to or removed from an atom in a combined state to convert the atom into the elemental form |
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| NH4 +, OH-, NO3 -, C2H3O2 -, SO4 2-, PO4 3- |
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| ions made up of two or more elements covalently-bonded |
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| to become stable compounds |
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| why do atoms bond to form compounds? |
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| predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other (linear, bent, trigonal planar&pyramidal, tetrahedral) |
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| atoms connected together in a straight line; bond angle=180 degrees; occurs in compounds consisting of only two atoms and three if middle has no unshared electrons |
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| atoms connected in an angled fashion; bond angle=105 degrees; occurs in compounds consisting of three atoms if the central atoms has unshared electrons |
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| trigonal planar&pyramidal |
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| occurs in compounds consisting of four atoms bonded together |
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| occurs in compounds consisting of five atoms bonded together; no unshared electrons; bond angle=109.5 degrees |
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| an orbital formed by the combination of multiple atomic orbitals on the same atom |
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| different polarities which attract each other |
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| same polarities which repel each other |
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| repulsion between atoms, dipole-dipole, induced dipole |
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| non-chemical combinations of elements or compounds; no chemical change that occurs among the combining materials |
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| have different amounts of substances dispersed; don't totally dissolve; maintain their original states; will separate over time |
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| have the same amount throughout; one substance becomes completely dissolved in another; dissolved substance takes on the state of what it is dissolved in; mixed substances stay together |
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| substance that gets dissolved |
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| substance that does the dissolving |
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| solid/liquid/gas dissolved in a solid |
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| solid/liquid/gas dissolved in a liquid |
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| solid/liquid/gas dissolved in a gas |
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| a solution made of two or more metals mixed together |
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| have properties in between those of suspensions and solutions |
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| solute that when dissolved, makes its solvent more conductive to electricity; solutes that when dissolved, break up into ions |
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| process of a solute being dissolved by a solvent; has to be able to "pull apart" the solute |
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| nature of the solute and solvent "like dissoves like"; temperature of the solution; pressure; heat of the solution |
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| raising the temperature of a solution witha solid solute.. |
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| raising the temperature of a solution with a gaseous solute.. |
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| does not change solubility |
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| raising the temperature of a solution with a liquid solute.. |
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| changes in this will affect solubility only when the solute is a gas |
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| pressure above a gas is directly proportional to the solubility of the gas |
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| has an increase in solubility when the temperature increases |
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| has a decrease in solubility when the temperature increases |
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| amount of energy produced or consumed by the formation of the solution |
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| a solution with the max amount of solute that can be dissolved |
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| a solution with less than the max amount of solute that can be dissolved |
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| a solution with more than the max amount of solute |
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| the larger available for dissolving, the faster the solute will dissolve |
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| puts more solute particles into contact with solvent, therefore increasing rate of dissolving |
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| ionic compounds that dissolve will actually be separated into the ions that make them up |
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| some ionic compounds don't dissolve at all in water |
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| process of solids forming in a solution |
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| ions that don't take part in a chemical reaction |
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| formation of ions in solution from molecules |
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| measure of how much solute is dissolved in a solution |
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| change as a result of the concentration of solute particles but are independent of the nature of the solute |
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| freezing point depression |
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| a colligative property that drops in freezing point of a solution when a solute is added |
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