Chemistry: matter and change

Applied Research
research that is directed toward a practical goal or application, research undertaken to solve a specific problem
The scientific study of matter and the changes it undergoes
a judgment based on the information obtained
In an experiment, the standard used for comparison.
Dependent Variable
in an experiment, the variable whose value depends on the independent variable
a set of controlled observations that test the hypothesis
a tentative, testable statement or prediction about what has been observed
Independent Variable
in an experiment, the variable that the experimenter plans to change
a measure of the amount of matter
anything that has mass and takes up space
a visual, verbal, and/or mathematical explanation of data collected from many experiments
Pure Research
a type of scientific investigation that seeks to gain knowledge for the sake of knowledge itself
Qualitative Data
information describing color, odor, shape, or some other physical characteristic
Quantitative Data
numerical information describing how much, how little, how big, how tall, how fast, etc.
Scientific Law
describes a relationship in nature that is supported by many experiments
Scientific Method
a systematic approach used in scientific study that typically includes observation, a hypothesis, experiments, data analysis, and a conclusion
the practical use of scientific information
an explanation supported by many experiments; still subject to new data and can be modified
a measure of the amount of matter and also the effect of Earth’s gravitational pull on the matter
refers to how close a measured value is to an accepted value
base unit
a defined unit in a system of measurement that is based on an object or event in the physical world and is independent of other units
conversion factor
a ratio of equivalent values used to express the same quantity in different units
a ratio that compares the mass of an object to its volume
derived unit
a unit defined by a combination of base unit
dimensional analysis
a problem solving method that focuses on the units that are used to describe matter
a visual representation of information that can reveal patterns in data
the SI base unit of temperature
the SI base unit for mass
the metric unit for volume equal to one cubic decimeter
the SI base unit for length
percent error
the ratio of an error to an accepted value
refers to how close a series of measurements are to one another
scientific notation
expresses numbers as a multiple of two factors – a number between 1 and 10, and 10 raised to a power or exponent
the SI base unit for time
significant figure
the number of all known digits reported in measurements plus one estimated digit
chemical change
a process involving one or more substances changing into new substances
chemical property
the ability or inability of a substance to combine with or change into one or more new substances
a chemical combination of two or more different elements
a pure substance that cannot be broken down into simpler substances
a form of matter that flows to conform to the shape of its container, fills the container’s volume, and is easily compressed
heterogeneous mixture
one that does not have a uniform composition and in which the individual substances remain distinct
homogeneous mixture
one that has a uniform composition throughout and always has a single phase
law of conservation of mass
states that mass is neither created nor destroyed during a chemical reaction but is conserved
law of definite proportions
states that, regardless of the amount, a compound is always composed of the same elements in the same proportion by mass
a form of matter that flows, has constant volume, and takes the shape of its container
a physical blend of two or more pure substances in any proportion in which each substance retains its individual properties; can be separated by physical means
percent by mass
a percentage determined by the ratio of the mass of each element to the total mass of the compound
periodic table
a chart that organizes all known elements into a grid of horizontal rows (periods) and vertical columns (groups) arranged by increasing atomic number
physical change
a type of change that alters the physical properties of a substance but does not change its composition
physical property
a characteristic of matter that can be observed or measured without changing the sample’s composition
a form of matter that has its own definite shape and volume, is incompressible, and expands only slightly when heated
a uniform mixture that may contain solids, liquids, or gases
states of matter
the physical forms in which all matter naturally exists on Earth – most commonly solid, liquid, and gas
a form of matter that has a uniform and unchanging composition
gaseous state of a substance that is a liquid or a solid at room temperature
the height of a wave from the origin to a crest
atomic emission spectrum
the frequencies of light emitted by an element separated into discrete lines
atomic orbital
a 3D region around the nucleus of an atom that describes an electron’s probable location
aufbau principal
states that each electron occupies the lowest energy orbital available
electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space
electromagnetic spectrum
includes all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths
electron configuration
the arrangement of electrons in an atom
electron-dot structure
consists of an element’s symbol (representing the nucleus & inner electrons) that is surrounded by dots representing the atom’s valence electrons
energy sublevel
the energy levels contained within a principle energy level.
the number of waves that pass a given point per second
ground state
the lowest allowable energy state of an atom
Heisenberg uncertainty principle
states that it is not possible to know precisely both the velocity and the position of a particle at the same time
Hund’s rule
single electrons with the same spin must occupy each orbital before additional electrons with opposite spins can occupy the same orbital
Pauli exclusion principle
states that a maximum of two electrons may occupy the same orbital, but only if the electrons have opposite spins
photoelectric effect
the emission of electrons from a metal when light shines on the metal
a particle of electromagnetic radiation with no mass that carries a quantum of energy
Planck’s constant
h, which has a value of 6.6261×10^-34 Js, where J is the symbol for Joules
principal energy levels
the major energy levels of an atom
principal quantum number
n, which in the quantum mechanical model indicates the relative sizes and energies of atomic orbitals
the minimum amount of energy that can be gained or lost by an atom
quantum mechanical model of the atom
an atomic model in which electrons are treated as waves
valence electron
the electrons in an atom’s outermost orbitals
the shortest distance between equivalent points on a continuous wave
alkali metal
group 1A elements, except hydrogen, that are on the left side of the modern periodic table
alkaline earth metal
group 2A elements in the modern periodic table
ability of an atom to attract electrons when the atom is in a compound
a vertical column of elements in the periodic table; also called a family
a highly reactive group 7A element
inner transition metal
a type of group B element that is contained in the f-block of the periodic table
an atom or bonded group of atoms with a positive or negative charge
ionization energy
energy required to remove an electron from an atom
an element that is a solid at room temperature, a good conductor of heat and electricity, and generally shiny
an element, such as silicon or germanium, that has physical and chemical properties of both metals and nonmetals
noble gas
an extremely unreactive group 8A element
elements that are generally gases or dull, brittle solids that are poor conductors of heat and electricity
a horizontal row of elements in the modern periodic table
periodic law
states that when the elements are arranged by increasing atomic number, there is periodic repetition of their chemical and physical properties
representative elements
groups of elements in the modern periodic table that are designated with an A (1A through 8A) and possess a wide range of chemical and physical properties
transition metal
a type of group B element that is contained in the d-block of the periodic table
transition elements
groups of elements in the modern periodic table that are designated with a B(1B through 8B) and are further divided into transition metals and inner transition metals
positive ion; formed by metallic elements
negative ion; mostly formed by nonmetal elements
covalent bond
a bond that results from the sharing of valence electrons
chemical reaction in which a greater amount of energy is required to break the existing bonds in reactants than is released when the new bonds form in product molecules
a chemical reaction in which more energy is released that is required to break bonds in the initial reaction
Lewis structure
a model that uses electron-dot structures to show how electrons are arranged in molecules
forms when two or more atoms covalently bond; usually includes two or more nonmetals
polar covalent
a type of bond that forms when electrons are not shared equally
structural formula
a molecular model that uses symbols and bonds to show relative positions of atoms
VSEPR model
model based on an arrangement that minimizes the repulsion of shared and unshared pairs of electrons around the central atom
a mixture of elements that has metallic properties
chemical bond
the force that holds two atoms together
delocalized electrons
the electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom
formula unit
the simplest ratio of ions represented in an ionic compound
ionic bond
the electrostatic force that holds oppositely charged particles together; usually a nonmetal paired with a metal
metallic bond
the attraction of a metallic cation for delocalized electrons
monatomic ion
ion formed from only one atom
oxidation number
the positive or negative charge of a monatomic ion
polyatomic ion
an ion made up of two or more atoms bonded together that acts as a single unit with a net charge
aqueous solution
a solution in which the solvent is water
chemical equation
a statement using chemical formulas to describe the identities and relative amounts of the reactants and products involved in the chemical reaction
chemical reaction
the process by which the atoms of one or more substances are rearranged to form different substances
the number written in front of a reactant or product in a chemical equation
combustion reaction
a chemical reaction that occurs when a substance reacts with oxygen, releasing energy in the form of heat and light
decomposition reaction
a chemical reaction that occurs when a single compound breaks down into two or more elements
double replacement reaction
a chemical reaction that involves the exchange of positive ions between two compounds and produces either a precipitate, a gas, or water
a solid produced during a chemical reaction in a solution
a substance formed during a chemical reaction
the starting substance in a chemical reaction
single replacement reaction
a chemical reaction that occurs when the atoms of one element replace the atoms of another element in a compound
a substance dissolved in a solution
the substance that dissolves a solute to form a solution
synthesis reaction
a chemical reaction in which two or more substances react to yield a single product
Avagadro’s number
6.02 x 10^23, which represents the number of particles in a mole
empirical formula
a formula that shows the smallest whole number mole ratio of the elements of a compound and may/may not be the same as the actual molecular formula
a compound that has a specific number of water molecules bound to its atoms
molar mass
the mass in grams of one mole of any pure substance
the SI unit used to measure the amount of a substance
molecular formula
a formula that specifies the actual number of atoms of each element in one molecule or formula unit of a substance
percent composition
the percent by mass of each element in a compound
Avogadro’s principle
if temperature and pressure are constant, gases with the same volume will then have the same number of particles
Boyle’s law
if temperature is constant, volume and pressure are inversely proportional
Charles’s law
if pressure is constant, volume and temperature are directly proportional
combined gas law
combines Boyle’s, Charles’s, and Gay-Lussac’s law to show the relationship between pressure, volume, and temperature for a fixed amount of gas
Gay-Lussac’s law
if volume is constant, pressure and temperature are directly proportional
ideal gas constant
an experimentally determined constant whose value in the ideal gas equation depends on the units that are used for pressure
ideal gas law
describes the behavior of an ideal gas in terms of temperature, volume, and pressure, and number of moles of gas present
molar volume
the volume that gas occupies at zero degrees Celsius and 1.0 atmospheres (STP); 22.4L
the amount of heat required to raise the temperature of one gram of pure water by one degree Celsius
an insulated device that is used to measure the amount of heat released or absorbed during a physical or chemical process
chemical potential energy
energy stored in a substance because of its composition
the capacity to do work or produce heat
the heat content of a system at constant pressure
a measure of disorder or randomness of the particles of a system
free energy
energy available to do work
a form of energy that flows from a warmer object to a cooler object
Hess’s law
two or more thermochemical equations can be added to produce a final equation for a reaction
the SI unit for heat
law of conservation of energy
energy may change from one form or another, but is neither created nor destroyed
law of disorder
entropy of the universe must increase as a result of a spontaneous reaction
heat of fusion
the amount of heat required to melt one mole of a solid substance
heat of vaporization
the amount of heat required to evaporate one mole of a liquid
specific heat
amount of heat required to raise the temperature of one gram of a given substance by one degree Celsius
includes everything in the universe except the system
the specific part of the universe containing the reaction or the process being studied
thermochemical equation
a balanced chemical equation that includes the physical states of all the reactants and products and specifies the change in enthalpy
the study of heat changes that accompany chemical reactions and phase changes
the system plus the surrounding
activation energy
the minimum amount of energy required to start a chemical reaction
a substance that initiates or accelerates a chemical reaction without itself being affected
collision theory
states that chemical reactions occur through collisions between molecules or atoms
complex reaction
A chemical reaction that consists of two or more elementary steps.
instantaneous rate
The rate of decomposition at a specific time, calculated from the rate law, the specific rate constant, and the concentrations of all the reactants.
A substance formed in one elementary step of a complex reaction and consumed in another
rate-determining step
the slowest elementary step in a complex reaction
rate law
an equation that relates reaction rate and concentrations of reactants
reaction mechanism
a series of elementary reactions that take place during the course of a complex reaction
reaction order
defines how rate is affected by concentration of that reactant
reaction rate
the change in concentration of reactants or products per unit time as a reaction proceeds
describes how much solute is present in a solution compared to the amount of solvent
the concentration of a solution expressed in moles of solute per kilogram of solvent
concentration measured by the number of moles of solute per liter of solvent
the maximum amount of solute that will dissolve in a given amount of time at a specific temperature and pressure
capable of being dissolved in a given substance
saturated solution
contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure
unsaturated solution
a solution that contains less solute than a saturated solution does and that is able to dissolve additional solute
supersaturated solution
contains more dissolved solute than a saturated solution at the same temperature
the dissolved substance in a solution
a liquid substance capable of dissolving other substances
chemical equilibrium
a chemical reaction and its reverse proceed at equal rates
equilibrium constant
describes the ratio of product concentrations to reactant concentrations raised to the power indicated by the coefficients
Le Chatelier’s Principle
a change in any of the factors determining equlibrium will cause the system to adjust to reduce the effect of the change
reversible reaction
A chemical reaction in which the products re-form the original reactants
acidic solution
a solution whose pH is less than 7
Arrhenius model
An acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution; A base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution
basic solution
a solution whose pH is greater than 7
Bronsted-Lowry model
a model of acids and bases in which an acid is a hydrogen ion donor and a base is a hydrogen ion acceptor
an ionic compound that resists changes in its pH
conjugate acid
the particle formed when a base gains a hydrogen ion
conjugate base
the particle that remains when an acid has donated a hydrogen ion
neutralization reaction
the reaction of an acid and a base to form a neutral solution of water and a salt
the negative logarithm of the hydrogen ion concentration of a solution
the negative logarithm of the hydroxide ion concentration of a solution
strong acid
an acid that ionizes completely in aqueous solution
strong base
A base that dissociates completely into ions in solution.
process in which a solution of known concentration is used to determine the concentration of another solution
weak acid
an acid that is only slightly ionized in aqueous solution
weak base
A base that does not dissociate completely into ions in solution.