Chemistry Exam Vocab

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The study of the composition, structure, and properties of matter and the changes it undergoes

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chemistry

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(type of chem.) the study of most carbon-containing components

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organic chemistry

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(type of chem.)
the study of all substances not classified as organic, mainly those compounds that do not contain carbon

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inorganic chemistry

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(type of chem.)
the study of the properties and changes of matter and their relation to energy

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physical chemistry

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(type of chem.)
the identification of the components and composition of materials

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analytical chemistry

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(type of chem.)
the study of substances and processes occuring in living things

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biochemistry

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(type of chem.)
the use of mathematics and computers to understand the principles behind observed chemical behavior and to design and predict the properties of new compounds

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theoretical chemistry

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any substance that has a definite shape composition

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chemical

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research carried out to solve a problem

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applied research

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development involving the production and use of products that improve our quality of life

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technological development

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research carried out for the sake of increasing knowledge

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basic research

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a measure of the amount of matter

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mass

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anything that has mass and takes up space

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matter

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a substance that is made from the atoms of two or more elements that are chemically bonded

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compound

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properties that depend on the amount of matter that is present

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extensive properties

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properties that do not depend on the amount of matter present

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intensive properties

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a characteristic that can be observed or measured without changing the identtity of the substance

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physical property

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a change in a substnace that does not involve a change in the identity of the substance

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physical change

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a physical change of a substance from one state to another

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change of state

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matter that has a definite volume and definite shape

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solid

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matter that has a definite volumbe but an indefinite shape

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liquid

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matter that has neither definite volume nor defnite shape

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gas

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a high temerature physical state of matter in which atoms lose their electrons

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plasma

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relates to a substnace's ability to undergo changes that trnsform it into different substances

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chemical property

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a change in which one or more substances are conerted into different substances

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chemical change
chemical reaction

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substances that react in a chemical change

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reactants

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substances that are formed by the chemical change

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products

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a blend of two or more kinds of matter, each of which retains its own identity and properties

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mixture

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mixtures that are uniform in composition

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homogeneous/solutions

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mixtures that are not uniform throughout

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heterogeneous

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a substance has a fixed composition and differs from a mixture in the following ways:
1) Every sample of a given pure substance has exactly the same charcteristic properties
2) Every sample of a given pure substance has exactly the same components

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pure substance

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the vertical columns of the periodic table

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groups/families

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the horizontal rows of elements in the periodic table

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periods

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an element that is a good conductor of heat and electricity

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metal

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an element that is a poor conductor of heat and electricity

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nonmetal

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an element that has some characteristics of metals and some characterstics of nonmetals

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metalloid

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a logical approach to solving problems by observing and collecting data, formulating hypotheses, testing hypotheses, and formulating theories that are supported by data

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scientific method

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a testable statement

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hypothesis

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a broad generalization that explains a body of facts or phenomena

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theory

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something that has magnitude, size, or amount

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quantity

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a measure of the gravitational pull on matter

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weight

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the ratio of mass to volume, or mass divided by volume

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density

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the closeness of measurements to the correct or accepted value of the quanity

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accuracy

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the closeness of a set of measurements of the same quantity made in the same way

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precision

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a measurement consisting of all the digits known with certainty plus one final digit, which is somewhat uncertain or estimated

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significant figures

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mass is neither destroyed nor created during ordinary chemical reactions or physical changes

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law of conservation of mass

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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

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law of definite proportions

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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 number

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law of multiple proportions

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the smallest particle of an element that retains the chemical properties of that element

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atom

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short-range proton-neutron, proton-proton, and neutron-neutron froces holding the nuclear particles together

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nuclear forces

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the number of protons in the nucleus of each atom of that element

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atomic number

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atoms of the same element that have different masses

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isotopes

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any isotope of any element

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nuclide

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the total number of protons and neutrons in the nucleus of an isotope

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mass number

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the weighted average of the atomic masses of the naturally occurring isotopes of an element

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average atomic mass

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the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12

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mole

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what is avogadro's number?

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6.022 x 10^23

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the mass of one mole of a pure substance

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molar mass

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form of energy that exhibits wavelike behavior as it travels through space

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electromagnetic radiation

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all the forms of radiation form this

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electromagnetic spectrum

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the distance between corresponding points on adjacent waves

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wavelength

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the number of waves that pass a given point in a specific time

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frequency

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the emission of electrons from a metal when light shines on the metal

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photoelectric effect

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the minimum quantity of energy that can be lost or gained by an atom

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quantum

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a particle of electromagnetic radiation having zero mass and carrying a quantum energy

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photon

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lowest energy state of an atom

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ground state

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a state in which an atom has a higher potential energy than it has in its ground state

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excited state

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E(photon)=

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h x v
(planck's constant, 6.636 x 10^-34)(frequency)

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states that it is impossible to determine simultaneously both the position and velocity of an electron or any other paricle

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Heisenberg uncertainty principle

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describes mathematically the wave properties of electrons and other very small paricles

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quantum theory

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a 3-D region around the nucleus that indicates the probable location of an electron

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orbital

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specify the properties of atomic orbitals and the properties of electrons in orbitals

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quantum numbers

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symbolized by n, indicates the main energy level occupid by an electron

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principal quantum number

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symbolized by l, indicates the shape of the orbital

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angular momentum

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symbolized by m, indicates the orientation of an orbital around the nucleus

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magnetic quantum number

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has only two possible values (+1/2, -1/2) which indicate the two fundamental spin states of an electron in an orbital

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spin quantum number

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the arrangement of electrons in an atom

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electron configuration

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states that an electron occupies the lowest-energy orbital that can recieve it

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Aufbau principle

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states that no tow electrons in the same atom can have the same set of four quantum numbers

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Pauli exclusion principle

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states that orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, all electrons in singly occupied orbitals must have the same spin

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Hund's rule

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The Group 18 elements

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noble gases

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the physical and chemical properties of the elements are periodic functions of their atomic numbers

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periodic law

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the elements of Group 1 of the periodic table

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alkali metals

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the elements of Group 2 of the periodic table

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alkaline-earth metals

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the elements of Group 17 of the periodic table

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halogens

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One-half the distance between the nuclei of idential atoms that are bonded together

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atomic radius

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an atom or group of bonded atoms that has a postitive or negative charge

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ion

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the energy required to remove one electron from a neutral atom of an element

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ionization energy

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the energy change that occurs when an electron is acquired by a neutral atom

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electron affinity

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a positive ion

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cation

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a negative ion

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anion

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the electrons available to be lost, gained, or shared in the formation of chemical compounds

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valence electrons

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a measure of the ablility of an atom in a chemical compound to attract electrons

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electronegativity

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a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

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chemical bond

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chemical bonding that results from the electrical attraction between large numbers of cations and anions

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ionic bonding

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results from the sharing of electron pairs between two atoms

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covalent bonding

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a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge

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nonpolar-covalent bond

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a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons

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polar-covalent bond

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A chemical compound whose simplest units are molecules

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molecular compound

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indicates the relative numbers of atoms of each kindin a chemical compound by using atomic symbols and numerical subscripts

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chemical formula

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shows the types and numbers of atoms combined in a single molecule of a molecular compound

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molecular formula

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a molecule containing only two atoms

BrINClHOF

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diatomic molecule

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the distance between two bonded atoms at their minimum potential energy; the average distance between two bonded atoms

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bond length

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the energy required to break a chemical bond and form neutral isolates atoms

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bond energy

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chemical compounds tend to form so that each atoms, by gaining, losing, or sharing electrons, has an octed of electrons in its highest occupied energy level

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octet rule

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an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol

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electron-dot notation

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a pair of electrons that is not involved in bodning and that belongs exclusively to one atom

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unshared pair/
lone pair

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in a covalent bond produced by the sharing of one pair of electrons between two atoms

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single bond

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in a covalent bond produced by the sharing of two pairs of electrons between two atoms

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double bond

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in a covalent bond produced by the sharing of three pairs of electrons between two atoms

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triple bond

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bonding moleculse or ions that cannot be correctly represented by a single Lewis structure

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resonance

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composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal

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ionic compound

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the energy released when one mole of an ionic crystalline compound is formed from gaseous ions

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lattice energy

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a charged group of covalently bonded atoms

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polyatomic ion

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the chemical bonding that resluts from the attraction between metal atoms and the surrounding sea of electrons

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metallic bonding

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the ablility of a substnace to be hammered or beaten into thin sheets

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malleablitlity

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the ability of a substance to be drawn, pulled, or extruded through a shamll opening to produce a wire

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ductility

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VSEPR

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Valence-Shell Electron-Pair Repulsion

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the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies

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hybridization

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the forces of attraction between molecules

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intermolecular forces

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created by equal but opposite charges that are separated by a short distance

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dipole

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the intermolecular attractions resulting from the constance motion of electrons and the creation of intstantaneous dipoles

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London dispersion forces