Chem 1127 – Final Exam – Flashcards
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| Wavelength |
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| the distance between 2 consecutive crests or troughs often measured in meters or nanometers |
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| crest |
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| rise above midline |
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| trough |
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| sink below midline |
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| frequency |
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| the number of wave cycles that pass a given point in unit time often measured in hertz |
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| wave cycles |
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| successive crests or troughs |
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| ? |
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| wavelength |
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| v |
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| frequency |
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| c |
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| speed of light |
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| speed of light |
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| 2.998E8 m/s |
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| light visible to the eye |
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| 400-700nm |
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| photons |
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| stream of particles that generates light |
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| unit of energy |
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| joule (J) |
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| E |
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| hv |
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| energy |
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| inversely related to wavelength |
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| h |
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| planck's constant |
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| 1nm |
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| 10^-9m |
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| h |
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| 6.626E-34Js |
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| 1kj |
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| 10^3J |
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| En |
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| enery of the electron |
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| -Rh |
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| 2.180E-18J |
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| n^2 |
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| the principle quantum number |
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| the point at which the proton and electron are completely separated |
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| zero |
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| ground state |
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| lowest energy state for which n=1 |
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| excited state |
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| when an electron absorbs enough energy it moves to this |
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| hv |
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| enery of the photon |
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| v=RH/h [1/(nlo)^2 - 1/(nhi)^2] |
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| used to find the frequency or wavelength of any of the lines in the H spectrum |
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| kinetic energy of an electron |
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| inversely related to the volume of the region to which it is confined |
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| orbital |
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| probability is independent of direction |
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| quantum numbers |
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| n, l, m(under)l |
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| ? |
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| wave function |
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| from ? |
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| we can deduce the relative energy of that orbital, its shape, and orientation in space |
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| principle energy levels |
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| primary importance in determining the energy of an electron |
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| energy of H atom |
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| depends only on n |
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| as n increases |
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| the energy of the electron increases and on average is found farther out from nucleus |
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| sublevels of second quantum number |
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| s, p, d, f |
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| second quantum number |
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| l |
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| l determines |
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| general shape of electron cloud associated with an electron |
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| larger values of l = |
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| more complex shapes |
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| if n=1 |
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| l has to be 0 |
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| in the nth principal level |
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| there are n levels |
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| for atoms containing more than one electron |
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| the energy is dependent on l and n |
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| orbitals |
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| differ from one another in the value assigned to the third quantum number, m(under)l |
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| m(under)l |
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| determines the direction in space of the electron cloud surrounding the nucleus |
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| all orbitals in a given d or f sublevel |
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| have the same energy |
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| electron spin |
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| associated with the fourth quantum number, m(under)s |
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| m(under)s |
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| not related to n, l, or m(under)l |
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| parallel spins |
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| electrons that have the same value of m(under)s (i.e. both +1/2 or both -1/2) |
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| opposed spins |
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| electrons that have different m(under)s values (i.e. one +1/2 and one -1/2) |
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| Pauli Exclusion Principle |
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| requires that no two electrons in an atom can have the same set of four quantum numbers |
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| capacity for electrons in an s sublevel |
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| 2e- |
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| capacity for electrons in a p sublevel |
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| 6e- |
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capacity for electrons in a f sublevel |
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| 14e- |
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| total capacity for electrons in the fourth principal level |
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| 32e- |
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| s sublevel |
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| spherical |
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| p sublevel |
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| two lobes along an axis |
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| electron configuration |
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| shows the number of electrons indicated by a superscript in each sublevel |
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| electrons enter the available sublevels |
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| in order of increasing sublevel energy |
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| orbital diagrams |
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| shows how electrons are distributed among orbitals |
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| Hund's Rule |
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| when several orbitals of equal energy are available, as in a given sublevel, electrons enter singly with parallel spins |
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| paramagnetic |
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| if there are unpaired electrons present, the solid will be attracted into the field |
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| diamagnetic |
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| if the atoms in the solid contain only paired electrons, it is slightly repelled by the field |
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| when a monatomic ion is formed from an atom |
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| electrons are added to or removed from sublevels in the highest principal energy level |
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| isoelectronic |
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| having the same electron configuration |
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| all transition metals form cations by |
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| loss of outer s electrons |
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| atomic radii decreases |
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| left to right |
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| atomic radii increases |
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| up to down |
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| ionization energy |
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| a measure of how difficult it is to remove an electron from a gaseous atom |
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| to bring about ionization, energy must be |
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| absorbed |
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| ionization energies are always |
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| positive quantities |
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| ionization energy increases |
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| across the periodic table from left to right |
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| ionization energy decreases |
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| moving down the periodic table |
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| electronegativity |
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| measures the ability of an atom to attract to itself the electron pair forming a covalent bond |
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| the greater the electronegativity of an atom |
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| the greater its attraction for electrons |
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| electronegativity increases |
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| moving from left to right across the periodic table |
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| electronegativity decreases |
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| moving down a group in the periodic table |
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| valence electrons |
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| outermost principal energy level |
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| core electrongs |
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| fill the principal level n=1 |
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| covalent bond |
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| a pair of electrons shared between two atoms |
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| lone pair |
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| an unshared pair of electrons, owned entirely by one atom |
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| single bond |
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| a single electron pair shared between two bonded atoms |
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| octet rule |
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| nonmetals, except for H, achieve a noble-gas structure by sharing in an octet of electrons |
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| resonance hybrid |
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| the actual structure as an intermediate between the two resonant forms |
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| formal charge |
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| the difference between the number of VE in the free atom and the number assigned to that atom in the Lewis structure |
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| free radicals |
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| molecules containing an odd number of VE |
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| molecular geometry can be predicted on the basis of |
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| electron-pair repulsion |
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| VSEPR model |
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| the VE pairs surrounding an atom repel one another so orbitals containing those electron pairs are oriented to be as far apart as possible |
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| trigonal planar |
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| 120 |
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| tetrahedron |
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| 109.5 AX4 |
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| trigonal bipyramid |
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| AX5 |
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| octahedral |
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| AX6 |
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| polar |
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| as a result of an unsymmetrical distribution of electrons, the bond or molecule contains a positive and a negative pole |
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| dipole |
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| contains a positive and a negative pole |
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| nonpolar |
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| a symmetrical distribution of electrons leads to a bond or molecule with no positive or negative poles |
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| nonpolar bonds |
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| formed whenever the two atoms joined are identical |
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| polar bonds |
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| bonds in which the electron density is unsymmetrical |
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| matter |
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| anything that has mass and occupies space |
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| the three phases of matter |
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| solid |
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| fixed shape and volume |
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| liquid |
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| fixed volume but is not rigid in shape |
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| gas |
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| has neither a fixed volume nor shape |
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| pure substances |
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| fixed composition and a unique set of properties |
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| mixtures |
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| composed of two or more substances |
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| element |
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| a type of matter that cannot be broken down into two or more pure substances |
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| compound |
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| a pure substance that contains more than one element |
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| electrolysis |
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| involves passing an electric current through a compound, usually in the liquid state |
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| mixture |
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| contains two or more substances combined in such a way that each substance retains its chemical identity |
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| homogeneous |
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| or uniform mixtures are ones in which the composition is the same throughout (aka solution) |
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| solution |
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| made up of a solvent, usually taken to be the substance present in largest amount, and one or more solutes |
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| heterogeneous |
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| or nonuniform mixtures are those in which the composition varies throughout |
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| filtration |
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| used to separate a heterogeneous solid-liquid mixture |
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| distillation |
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| used to resolve a homogeneous solid-liquid mixture |
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| mega |
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| 10^6 |
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| kilo |
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| 10^3 |
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| deci |
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| 10^-1 |
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| centi |
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| 10^-2 |
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| milli |
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| 10^-3 |
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| micro |
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| 10^-6 |
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| nano |
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| 10^-9 |
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| pico |
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| 10^-12 |
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| mass |
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| a measure of the amount of matter in an object |
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| weight |
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| a measure of the gravitational force acting on an object |
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| temperature |
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| the factor that determines the direction of heat flow |
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| significant figures |
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| the meaningful digits obtained in a measurement |
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| 1 km |
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| 10^3m |
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| 1cm |
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| 10^-2m |
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| 1mm |
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| 10^-3m |
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| 1nm |
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| 10^-9m |
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| 1m^3 |
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| 10^6cm^3 |
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| 1cm^3 |
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| 1mL |
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| 10^-3L |
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| 1cm^3 |
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| 1kg |
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| 10^3g |
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| 1mg |
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| 10^-3g |
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| 1 mile |
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| 5280ft |
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| intensive |
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| independent of amount |
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| extensive |
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| depend on amount |
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| chemical properties |
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| observed when the substance takes part in a chemical reaction |
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| physical properties |
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| observed without changing the chemical identity of a substance |
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| melting point |
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| the temperature at which a substance changes from the solid to liquid state |
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| boiling point |
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| the temperature at which bubbles filled with vapor form within a liquid |
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| Z |
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| atomic number |
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| A |
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| mass number |
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| atomic number |
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| number of protons |
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| mass number |
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| number of prootons +number of neutrons |
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| theoretical yield |
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| the maximum quanityt that can be obtained under such conditions, assuming the reaction goes to completion and no product is lost |
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| simplest formula |
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| gives the simplest whole number ratio of atoms present |
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| percent composition |
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| the mass percents of the elements present |
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| strong electrolytes |
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| the solution conducts an electric current |
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| nonelectrolytes |
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| the solution does not conduct electricity |
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| polyatomic ion |
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| containing more than one atom |
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| "charged molecule" |
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| polyatomic ion |
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| monatomic ion |
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| derived from a single atom by the loss or gain of electrons |
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| metals |
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| have high electrical conductivities |
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| metalloids |
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| have electrical conductivities that are intermediate between those of metals and nonmetals |
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| molecular formulas |
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| represents molecular substances |
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| structural formulas |
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| represent the structures of molecules |
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| condensed structural formula |
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| suggests the bonding pattern in the molecule and highlights the presence of a reactive group of atoms within a molecule |
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| atomic mass |
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| atomic weight |
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| nuclear symbol |
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| shows the composition of a nucleus |
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| acid |
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| a species that produces H+ ions in water solutions |
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| base |
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| a species that produces OH- ions in water solution |
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| strong acids |
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| ionize completely, forming H+ ions and anions |
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| strong base |
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| is completely ionized to OH- ions and cations in water solution |
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| weak acid |
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| molecules containing an ionizable hydrogen atom (i.e. only partially ionized to H+ ions in water) |
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| weak bases |
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| react with H20 molecules, acquiring H+ ions and leaving OH- ions behind |
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| amines |
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| derivatives of ammonia in which one or more hydrogen atoms have been replaced by hydrocarbon groups |
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| a common class of weak bases of the organic molecules |
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| amines |
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| strong acids and bases |
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| are completely ionized in water |
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| weak acids and bases |
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| do not react completely |
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| neutralization |
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| when the H+ ions and OH- ions react with eachother to form H20 molecules |
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| titration |
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| measuring the volume of a standard solution required to react with a measured amount of sample |
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| standard solution |
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| a solution of known concentration |
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| equivalence point |
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| the point at which the reaction is complete |
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| redox reaction |
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| a reaction in aqueous solution that involves a transfer of electrons between two species |
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| oxidation |
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| an increase in oxidation number |
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| reduction |
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| a decrease in oxidation number |
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| oxidizing agent |
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| the ion or molecule that accepts electrons |
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| reducing agent |
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| the species that donates electrons |
