Master this deck with 210 terms through effective study methods.
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A substance that has the same composition and properties wherever it is found
The study of the composition, structure, properties, and reactions of matter
An explanation of an observation that has been validated by repeated experiments that support a hypothesis
A procedure that tests the validity of a hypothesis
An unverified explanation of a natural phenomenon
Information determined by noting and recording a natural phenomenon
The process of making observations, proposing a hypothesis, testing the hypothesis, and making a conclusion as to the validity of the hypothesis
A form of writing large and small numbers using a coefficient that is at least 1 but less than 10, followed by a power of 10
A relationship between two units that measure the same quantity
A system of measurement used by scientists and in most countries
A relationship between the density of a substance and the density of water. sp gr = density of sample/ density of water
The formation of bubbles of gas throughout a liquid
The amount of heat energy that raises the temperature of exactly 1g of water by exactly 1 C
The transformation of one state of matter to another for example, solid to liquid, liquid to solid, liquid to gas
The properties that indicate the ability of a substance to change into a new substance
A pure substance consisting of two or more elements with a definite composition, that can be broken down into simpler substances only by chemical methods
The change of state from a gas to a liquid
A diagram that illustrates temperature changes and changes of state for a substance as heat is removed
The change of a gas directly into a solid; the reverse of sublimation
A pure substance containing only one type of matter, which cannot be broken down by chemical methods
The kilocalories (or kilojoules) obtained per gram of the food types: carbohydrates, fat, and protein
The temperature at which a liquid changes to a solid (freezes), a solid changes to a liquid (melts)
A state of matter that does not have a definite shape or volume
The energy associated with the motion of particles in a substance
The energy required to vaporize exactly 1 g go a substance at its boiling point. For water, 540 cal (2260 J) is needed to vaporize 1 g of liquid; 1 g of steam gives off 540 cal (2260 J) when it condenses
A diagram that illustrates the temperature changes and changes of state of a substance as it is heated
The SI unit of heat energy; 4.184 J = 1 cal
The energy of moving particles
A state of matter that takes the shape of its container but has a definite volume
The material that makes up a substance and has mass and occupies space
The change of state from a solid to a liquid
The physical combination of two or more substances that does not change the identities of the mixed substances
A change in which the physical properties of a substance change but its identity stays the same
The properties that can be observed or measured without affecting the identity of a substance
A type of energy related to position or composition of a substance
A type of matter that has a definite composition
A state of matter that has its own shape and volume
A quantity of heat that changes the temperature of exactly 1 g of a substance by exactly 1 C
Three forms of matter: solid, liquid, and gas
The change of state in which a solid is transformed directly to a gas without forming a liquid first
An element in Group 1A (1), except hydrogen, that is a soft, shiny metal with one electron in its outermost energy level
An element in Group 2A (2) that has two electrons in its outermost energy level
The smallest particle of an element that retains the characteristics of the element
The weighted average mass of all the naturally occurring isotopes of an element
A small mass unit used to describe the mass of extremely small particles such as atoms and subatomic particles; 1 amu is equal to one-twelfth the mass of a C-12 atom
A number that is equal to the number of protons in an atom
The distance between the outermost electrons and the nucleus
An abbreviation used to indicate the mass number and atomic number of an isotope
An abbreviation that represents the name of an element
The block of ten elements from Groups 3B (3) to 2B (12) in which electrons fill the five d orbitals in the d sub levels
A negatively charged subatomic particle having a minute mass that is usually ignored in mass calculations; its symbol is e⁻
A list of the number of electrons in each sub level within an atom, arranged by increasing energy
A group of electrons with similar energy
The block of 14 elements in the rows at the bottom of the periodic table in which electrons fill the seven f orbitals in the 4f and 5f sub levels
A vertical column in the periodic table that contains elements having similar physical and chemical properties
A number that appears at the top of each vertical column (group) in the periodic table and indicates the number of electrons in the outermost energy level
An element in Group 7A (7)- fluorine, chlorine, bromine, iodine, and astatine- that has seven electrons in its outermost energy level
The energy needed to remove the last tightly bound electron from the outermost energy level of an atom
An atom that differs only in mass number from another atom of the same element. Isotopes have the same atomic number (number of protons), but different numbers of neutrons
The representation of an atom that shows valence electrons as dots around the symbol of the element
The total number of protons and neutrons in the nucleus of an atom
An element that is shiny, malleable, ductile, and a good conductor of heat and electricity. The metals are located to the left of the heavy zigzag line on the periodic table
A measure of how easily an element loses a valence electron
Elements with properties of both metals and nonmetals located along the heavy zigzag line on the periodic table
A neutral subatomic particle having a mass of about 1 amu and found in the nucleus of an atom; its symbol is n or n⁰
An element in Group 8A (18) of the periodic table, generally unreactive and seldom found in combination with other elements that has eight electrons (helium has two electrons) in its outermost energy level
An element with little or no luster that is a poor conductor of heat and electricity. The nonmetals are located to the right of the heavy zigzag line on the periodic table
The compact, extremely dense center of an atom, containing the protons and neutrons of the atom
The region around the nucleus where electrons of a certain energy are more likely to be found. The s orbitals are spherical, the p orbitals have two lobes
A diagram that shows the distribution of electrons in the orbitals of the energy levels
The elements in Groups 3A (13) to 8A (18) in which electrons fill the p orbitals in the p sub levels
A horizontal row of elements in the periodic table
An arrangement of elements by increasing atomic number such that elements having similar chemical behavior are grouped in vertical columns
A positively charged subatomic particle having a mass of about 1 amu and found in the nucleus of an atom; its symbol is p or p⁺
An element in the first two columns on the left of the periodic table and the last six columns on the right that has a group number of 1A through 8A or 1, 2 and 13 through 18
The elements in Groups 1A (1) and 2A (2) in which electrons fill the s orbitals
A particle within an atom; protons, neutrons, and electrons are subatomic particles
A group of orbitals of equal energy with an energy level. The number of sub levels in each energy level is the same as the principal quantum number (n)
An element in the center of the periodic table that is designated with the letter "B" or the group number of 3 through 12
Electrons in the highest energy level of an atom
A nuclear particle identical to a helium nucleus, symbol α or He²⁺
A unit of activity of a radioactive sample equal to one disintegration per second
A particle identical to an electron, symbol β, that forms in the nucleus when a neutron changes to a proton and an electron
A fission reaction that will continue once it has been initiated by a high-energy neutron bombarding a heavy nucleus such as uranium-235
A unit of activity of a radioactive sample equal to 3.7 x 10^10 disintegrations/s
A diagram of the decay of a radioactive element
The measure of biological damage from an absorbed dose that has been adjusted for the type of radiation
A process in which large nuclei are split into smaller pieces, releasing large amounts of energy
A reaction in which large amounts of energy are released when small nuclei combine to form larger nuclei
High-energy radiation emitted by an unstable nucleus
A unit of absorbed dose equal to 100 rad
The length of time it takes for one-half of a radioactive sample to decay
A particle of radiation with no mass and a positive charge produced when a proton is transformed into a neutron and a positron
A measure of an amount of radiation absorbed by the body
The process by which an unstable nucleus breaks down with the release of high energy radiation
A radioactive atom of an element
A measure of the biological damage caused by the various kinds of radiation (rad x biological factor)
A unit of biological damage (equivalent dose) equal to 100 rem
A negatively charged ion
The group of symbols and subscripts that represents the atoms or ions in a compound
The separation of positive and negative charges in a polar bond indicated by an arrow that is drawn from the more positive atom to the more negative atom
Attractive forces between oppositely charged ends of polar molecules
Weak dipole bonding that results from a momentary polarization of non-polar molecules
The relative ability of an element to attract electrons in a bond
An atom or group of atoms having an electrical charge because of a loss or gain of electrons
The difference between the number of protons (positive) and the number of electrons (negative) written in the upper right corner of the symbol for the element or polyatomic ion
A compound of positive and negative ions held together by ionic bonds
A representation of a molecule or ion that shows valence electrons
A combination of atoms in which stable electron configurations are attained by sharing electrons
The smallest unit of two or more atoms held together by covalent bonds
A covalent bond in which the electrons are shared equally between atoms
A molecule that has only non polar bonds or in which the bond dipoles cancel
A set of eight valence electrons
Elements in Groups 1A-7A (1, 2, 13-17) react with other elements by forming ionic or covalent bonds to produce a stable electron configuration, usually eight electrons in the outer shell
A covalent bond in which the electrons are shared unequally between atoms
A molecule containing bond dipoles that do not cancel
A measure of the unequal sharing of electrons indicated by the difference in electronegativities
A group of covalently bonded nonmetal atoms that has an overall electrical charge
A sharing of three pairs of electrons by two atoms
A theory that predicts the shape of a molecule by placing the electron pairs on a central atom as far apart as possible to minimize the mutual repulsion of the electrons
The actual amount of product produced by a reaction
The number of items in one mole, equal to 6.02 x 10^23
The final form of a chemical equation that shows the same number of atoms of each element in the reactants and products
A shorthand way to represent a chemical reaction using chemical formulas to indicate the reactants and products and coefficients to show reacting ratios
Whole numbers placed in front of the formulas to balance the number of atoms or moles of atoms of each element on both sides of an equation
A chemical reaction in which reactants combine to form a single product
A chemical reaction in which a fuel containing carbon and hydrogen reacts with oxygen to produce CO2, H2O, and energy
A reaction in which a single reactant splits into two or more simpler substances
A reaction in which parts of two different reactants exchange places
A reaction that requires heat; the energy of the products is higher than the energy of the reactants
A reaction that releases heat; the energy of the products is lower than there energy of the reactants
The group of ions represented by the formula of an ionic compound
The heat (symbol ΔH) absorbed or released when a reaction takes place at constant pressure
The reactant used up during a chemical reaction, which limits the amount of product that can form
The mass in grams of 1 mole of an element equal numerically to its atomic mass. The molar mass of a compound is equal to the sum of the masses of the elements multiplied by their subscripts in the formula
A group of atoms, molecules, or formula units that contains 6.02 x 10^23 of these items
A conversion factor that relates the number of moles of two compounds derived from the coefficients in an equation
The loss of electrons by a substance. Biological oxidation may involve the addition of oxygen or the loss of hydrogen
A reaction in which the oxidation of one reactant is always accompanied by the reduction of another reactant
The ratio of the actual yield for a reaction to the theoretical field possible for the reaction
The substances formed as a result of a chemical reaction
The initial substances that undergo change in a chemical reaction
The gain of electrons by a substance. Biological reduction may involve the loss of oxygen or the gain of hydrogen
A reaction in which an element replaces a different element in a compound
The maximum amount of product that a reaction can produce from a given amount of reactant q
A unit equal to pressure exerted by a column of mercury 760 mm high
The pressure exerted by the atmosphere
A gas law stating that the volume of a gas is directly related to the number of moles of gas when pressure and temperature do not change
A gas law stating that the pressure of a gas is inversely related to the volume when temperature and moles of the gas do not change
A gas law stating that the volume of a gas changes directly with a change in Kelvin temperature when pressure and moles of the gas do not change
A relationship that combines several gas laws relating pressure, volume, and temperature when the amount of gas does not change
A gas law stating that the total pressure exerted by a mixture of gases in a container is the sum of the partial pressures that each gas would exert
A gas law stating that the pressure of a gas changes directly with a change in the Kelvin temperature when the number of moles of a gas and its volume do not change
A numerical value that relates the quantities P, V, n and T in the ideal gas law, PV= nRT
A model used to explain the behavior of gases
A volume of 22.4 L occupied by 1 mole of a gas at STP conditions of 0 °C (273 K) and 1 atm
The force exerted by gas particles that hit the walls of a container
The pressure exerted by the particles of vapor above a liquid
A mixture having particles that are moderately large. Colloids pass through filters but cannot pass through semipermeable membranes
A measure of the amount of solute that is dissolved in a specified amount of solution
The shriveling of a cell because water leaves the cell when the cell is placed in a hypertonic solution
A process in which water and small solute particles pass through a semipermeable membrane
A process by which water (solvent) is added to a solution to increase the volume and decrease (dilute) the concentration of the solute
A substance that produces ions when dissolved in water; its solution conducts electricity
The amount of a positive or negative ion that supplies 1 mole of electrical charge
A swelling and bursting of red blood cells in a hypotonic solution because of an increase in fluid volume
The solubility of a gas in a liquid is directly related to the pressure of that gas above the liquid
The process of surrounding dissolved ions by water molecules
A solution that has higher particle concentration and higher osmotic pressure than the cells of the body
A solution that has a lower particle concentration and lower osmotic pressure than the cells of the body
A solution that has the same particle concentration and osmotic pressure as that of the cells of the body
The grams of solute in exactly 100 mL of solution
A substance that dissolves in eater as molecules; its solution does not conduct an electrical current
The pressure that prevents the low of water into the more concentrated solution
A solution containing the maximum amount of solute that can dissolve at a given temperature. Any additional solute will remain undissolved in the container
The maximum amount of solute that can dissolve in exactly 100 g of solvent, usually water, at a given temperature
The component in a solution that is present in the lesser amount
The substance in which the solute dissolves; usually the component present in greater amount
A mixture in which the solute particles are large enough and heavy enough to settle out and be retained by both filters and semipermeable membranes
A solution that contains less solute than can be dissolved
A percent concentration that relates the volume of the solute in exactly 100 mL of solution
The energy that must be provided by a collision to break apart the bonds of the reacting molecules
A substance that increases the rate of reaction by lowering the activation energy
The point at which the rate of forward and reverse reactions are equal so that no further change in concentrations of reactants and products take place
A model for a chemical reaction stating that molecules must collide with sufficient energy and proper orientation to form products
Th numerical value obtained by substituting the equilibrium concentrations of the components into the equilibrium constant expression
The ratio of the concentrations of products to the concentrations of reactants, with each component raised to an exponent equal to the coefficient of that compound in the balanced chemical equation
When a stress is placed on a system at equilibrium, the equilibrium shifts to relieve that stress
The speed at which reactants are used to form product(s)
A reaction in which a forward reaction occurs from reactants to products, and a reverse reaction occurs from products back to reactants
A substance that dissolves in water and produces hydrogen ions (H+), according to the Arrhenius theory. All acids are hydrogen ion donors, according to the Broasted-Lowry theory
The numerical value of the product of ions from the dissociation of a weak acid divided by the concentration of the weak acid
Substances that can act as either an acid or a base in water
The numerical value of the product of the ions from the dissociation of a weak base divided by the concentration of the weak base
An acid is a hydrogen ion donor; a base is a hydrogen ion acceptor
A solution of a weak acid and its conjugate base or a weak base and its conjugate acid that maintains the pH y neutralizing added acid or base
An acid and a base that differ by one H+. When an acid donates a hydrogen ion, the product is its conjugate base, which is capable of accepting a hydrogen ion in the reverse reaction
The separation of an acid or a base into ions in water
The ion formed by the attraction of a hydrogen ion, H+, to a water molecule
A substance added to a titration sample that changes color when the pH of the solution changes
The term that describes a solution with equal concentrations of [H3O+] and [OH-]
A reaction between an acid and a base to form water
A measure of the [H3O+] in a solution; pH = -log[H3O+]
An ionic compound that contains a metal ion or NH4+ and a nonmetal or polyatomic ion other than OH-
An acid that completely dissociates in water
A base that completely dissociates in water
The addition of base to an acid sample to determine the concentration of the acid
The product of [H3O+] and [OH-] in a solution; Kw = [H3O+][OH-]
An acid that is a poor donor of H+ and dissociates only slightly in water
A base that is a poor acceptor of H+ and produces only a small number of ions in water