chem review isaacson entire
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Jeff_Wendling on December 11, 2009
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147 terms
Terms | Definitions |
|---|---|
 chemical | any substance that has a definite composition |
| chemistry | the science of matter |
| atom | the smallest unit of an element that maintains the properties of that element |
| change of state | a physical change of a substance from one state to another |
| chemical change | a change in which one or more substances are converted into different substances |
| chemical property | the ability of a substance to undergo a change that transforms it into a different substance |
| chemical reaction | the process by which one or more substances change to produce one or more different substances |
| compound | a substance made up of atoms of two or more different elements joined by chemical bonds |
| element | a pure substance made of only one kind of atom |
| extensive property | a property that depends on the amount of matter present |
| gas | a state of matter that has no definite shape or volume |
| heterogeneous | not uniform throughout |
| homogeneous | uniform in composition |
| intensive property | a property that does not depend on the amount of matter present |
| liquid | a substance in the fluid state of matter having no fixed shape but a fixed volume |
| mass | a measure of the amount of matter in an object |
| matter | anything that has mass and takes up space |
| mixture | a blend of two or more kinds of matter, each of which retains its own identity and properties |
| physical change | a change in a substance that does not involve a change in the identity of the substance |
| physical property | a characteristic that can be observed or measured without changing the identity of the substance |
| plasma | high temperature physical state of matter in which atoms lose their electrons |
| pure substance | a substance that has a fixed composition and differs from a mixture in that every sample of a given pure substance has exactly the same characteristic properties and composition |
| reactant | the substances that react in a chemical change |
| solid | the state in which matter has a definite shape and volume |
| solution | A homogeneous mixture of two or more substances |
| family | Elements in the same vertical column of the periodic table; also called a group |
| group | Vertical column of elements in the periodic table |
| metal | an element that is a good conductor of heat and electricity |
| metalloid | an element that has some characteristics of metals and some characteristics of nonmetals |
| nonmetal | an element that is a poor conductor of heat and electricity |
| period | a horizontal row of elements in the periodic table |
| hypothesis | testable statement |
| model | An explanation or representation of something that cannot be seen |
| scientific method | a logical procedure for gathering information about the natural world, in which experimentation and observation are used to test hypotheses. |
| system | a specific portion of matter in a given region of space that has been selected for study during an experiment or observation |
| theory | a broad generalization that explains a body of facts or phenomena |
| conversion factor | a ratio derived from the equality between two different units that can be used to convert from one unit to the other. |
| density | the ratio of the mass of a substance to the volume of the substance |
| derived unit | Unit of measurement obtained by combining SI units (density= mass/volume) |
| quantity | something that has magnitude, size, or amount |
| SI | Le Système International d'Unités, or the International System of Units, which is the measurement system that is accepted worldwide |
| volume | the amount of space occupied by an object |
| weight | The measure of the force of gravity on an object |
| accuracy | the closeness of measurements to the correct or accepted value of the quantity measured |
| directly proportional | two quantities that give a constant value when one is divided by the other. |
| indirectly proportional | xy=K |
| percent error | a value calculated by subtracting the experimental value from the accepted value, dividing the difference by the accepted value, and then multiplying by 100 |
| precision | closeness of a set of measurements of the same quantity made in the same way |
| scientific notation | numbers are written in the form M x 10^n, where the factor M is a number greater than or equal to 1 but less than 10 and n is a whole number |
| significant figures | any digit in a measurement that is known with certainty plus one final digit,which is somewhat uncertain or is estimated. |
| law of conservation of mass | Mass is neither destroyed nor created during ordinary chemical reactions or physical changes |
| law of definite proportions | a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound |
| law of multiple proportions | if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers |
| atom | the smallest unit of an element that maintains the properties of that element |
| nuclear forces | short-range proton-neutron, proton-proton, and neutron-neutron forces hold the nuclear particles together |
| atomic mass | number of protons |
| atomic numbers | the number of protons in the nucleus of an atom |
| average atomic mass | the weighted average of the atomic masses of the naturally occurring isotopes of an element |
| avogadro's number | 6.02x10^23 |
| isotopes | atoms of the same element that have different masses |
| mass number | the total number of protons and neutrons in an atom |
| molar mass | the mass of one mole of a pure substance |
| mole | the amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12 |
| nuclide | The general term for any isotope of any element; another term for an atom that is identified by the number of protons and neutrons in its nucleus |
| continuous spectrum | the emission of a continuous range of frequencies of electromagnetic radiation |
| electromagnetic radiation | a form of energy that exhibits wavelike behavior as it travels through space |
| electromagnetic spectrum | All of the frequencies or wavelengths of electromagnetic radiation |
| excited state | a state in which an atom has a higher potential energy than it has in its ground state |
| frequency | the number of waves that pass a given point in a specific time, usually one second |
| ground state | the lowest energy state of an atom |
| line-emission spectrum | series of specific wavelengths of emitted light created when the visible portion of light from excited atoms in shined through a prism |
| photoelectric effect | The emission of electrons from a metal when light shines on the metal |
| photon | a particle of electromagnetic radiation having zero mass and carrying a quantum of energy |
| quantum | the minimum quantity of energy that can be lost or gained by an atom |
| wavelength | The distance between corresponding points on adjacent waves |
| angular momentum quantum number | the quantum number that indicates the shape of the orbital |
| Heisenberg uncertainty principle | it is impossible to determine simultaneously both the position and velocity of an electron or any other particle |
| magnetic quantum number | the quantum number that indicates the orientation of an orbital around the nucleus |
| hund's rule | 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 |
| inner shell electrons | an electron that is not in the highest occupied energy level |
| noble gases | helium, neon, argon, krypton, xenon, and radon |
| noble gas configuration | An outer main energy level fully occupied, in most cases, by eight electrons |
| pauli exclusion principle | no two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers |
| orbital | a three dimensional region around the nucleus that indicates the probable location of an electron |
| quantum numbers | numbers that specify the properties of atomic orbitals and of their electrons |
| quantum theory | a mathematical description of the wave properties of electrons and other very small particles |
| spin quantum number | The quantum number that has only two possible values, +1/2 and -1/2, which indicate the two fundamental spin states of an electron in an orbital |
| aubau principle | an electron occupies the lowest-energy level that can receive it |
| electron configuration | arrangement of electrons in an atom |
| highest occupied energy level | the electron-containing main energy level with the highest principal quantum number |
| actinide | one of the 14 elements with atomic numbers from 90 (thorium, Th) through 103 (lawrencium, Lr) |
| lanthanide | one of the 14 elements with atomic numbers from 58 (cerium, Ce) to 71 (lutetium, Lu) |
| periodic law | the physical and chemical properties of the elements are periodic functions of their atomic numbers |
| periodic table | an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group |
| alkali metals | the elements of Group 1 of the periodic table (lithium, sodium, potassium, rubidium, cesium, and francium) |
| alkaline earth metals | The Group 2 elements (Be, Mg, Ca, Sr, Ba, Ra) |
| halogens | the elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine) |
| main group elements | Those elements occupying the s and p blocks of the periodic table. |
| transition elements | one of the d-block elements that is a metal with typical metalic properties |
| anion | negative ion |
| atomic radius | one-half of the distance between the center of identical atoms that are not bonded together. |
| cation | a positively charged ion |
| electron affinity | the energy change that occurs when an electron is acquired by a neutral atom |
| electronegativity | a measure of the ability of an atom in a chemical compound to attract electrons |
| ionization | the formation of ions from solute molecules by the action of the solvent; any process that results in the formation of an ion |
| ion | an atom or group of bonded atoms that has a positive or negative charge |
| ionization energy | the energy required to remove one electron from a neutral atom of an element |
| valence electrons | an electron that is available to be lost gained or shared in the formation of chemical compounds |
| chemical bond | a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
| ionic bonding | chemical bonding that results from the electrical attraction between large numbers of cations and anions |
| nonpolar covalent bond | A covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge |
| polar | having an uneven distribution of charge |
| polar covalent bond | a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons |
| bond energy | energy required to break a chemical bond and form neutral isolated atoms |
| bond length | the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms |
| chemical formula | A formula that indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts |
| diatomic molecule | a molecule consisting of two atoms |
| double bond | a covalent bond in which two pairs of electrons are shared between two atoms |
| electron dot notation | an electron configuration notation in which only thevalence electrons of an atom of a particular element are shown, indicated by dotsplaced around the element's symbol |
| lewis structures | formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron paris in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons |
| lone pair | A pair of electrons that is not involved in bonding and that belongs exclusively to one atom. |
| molecular compound | a chemical compound whose simplest units are molecules |
| molecular formula | a chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound |
| molecule | a neutral group of atoms held together by covalent bonds |
| multiple bond | a double or triple bond |
| octet rule | chemical compounds tend to form so that each atom, by gaining,losing, or sharing electrons, has an octet of electrons in its highest occupied energy level |
| resonance | the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
| single bond | a covalent bond produced by the sharing of one pair of electrons between two atoms |
| structural formula | a formula that indicates the location of the atoms, groups, or ions relative to one another in a molecule and that indicates the number and location of chemical bonds |
| triple bond | a covalent bond in which two atoms share three pairs of electrons |
| unshared pair | a pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
| formula unit | the simplest collection of atoms from which an ionic compound's formula can be established |
| ionic compound | composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal |
| lattice energy | the energy released when one mole of an ionic crystalline compound is formed from gaseous ions |
| polyatomic ion | a charged group of covalently bonded atoms |
| ductility | the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire |
| malleability | the property of a metal that indicates that it can be bent and rolled into sheets |
| dipole | created by equal but opposite charges that are separated by a short distance |
| dipole dipole forces | polar molecules orient themselves so that oppositely charged ends are near eachother |
| hybrid orbitals | orbitals of equal energy produced by the combination of two or more orbitals on the same atom |
| hybridization | the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies |
| hydrogen bonding | the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule |
| intermolecular forces | forces of attraction between molecules |
| london dispersion forces | intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles |
| molecular polarity | the uneven distribution of molecular charge |
| VSEPR theory | repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible |
| metallic bonding | chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons |
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