Chemistry EOY Vocab
Name
________________________________________
Specific heat 1. the heat required to raise the temperature of the unit mass of a given substance by a given
amount (usually one degree).
mass
Kinetic
molecular theory
a coherent, typically large body of matter with no definite shape
1. Gases are composed of a large number of particles that behave like hard, spherical
objects in a state of constant, random motion.
2. These particles move in a straight line until they collide with another particle or the
walls of the container.
3. These particles are much smaller than the distance between particles. Most of the
volume of a gas is therefore empty space.
4. There is no force of attraction between gas particles or between the particles and
the walls of the container.
5. Collisions between gas particles or collisions with the walls of the container are
perfectly elastic. None of the energy of a gas particle is lost when it collides with
another particle or with the walls of the container.
6. The average kinetic energy of a collection of gas particles depends on the
temperature of the gas and nothing else.
Properties of
1) they are easy to compress, (2) they expand to fill their containers, and (3) they occupy
gasses
far more space than the liquids or solids from which they form
Boyles law
a gas law, stating that the pressure and volume of a gas have an inverse relationship,
when temperature is held constant.
Charles law
Charles's Law is an ideal gas law where at constant pressure, the volume of an ideal gas is directly
proportional to its absolute temperature.
Vi/Ti = Vf/Tf -Where Vi = initial pressureTi = initial temperatureVf = final pressureTf = final
temperature
Gay-Lussac
Gay-Lussac’s Law is a special case of the ideal gas law. This law only applies to ideal gases held at a
constant volume allowing only the pressure and temperature to change.Answer: Gay-Lussac’s Law is
expressed as: Pi/Ti = Pf/Tf
Ideal gas law
An ideal gas is a gas whose pressure P, volume V, and temperature T are related by the ideal gas
lawPV = nRT,where n is the number of moles of the gas and R is the ideal gas constant. Ideal gases
are defined as having molecules with negligible size with an average molar kinetic energy dependent
only on temperature. At low temperature, most gases behave enough like ideal gases that the ideal
gas law can be applied to them. Also Known As: perfect gas
Redox
a process in which one substance or molecule is reduced and another oxidized; oxidation
and reduction considered together as complimentary processes.
Acid base
reaction
Synthesis
Single
replacement
Double
replacement
1. The universal aqueous acid–base definition of the Arrhenius concept is described as the
formation of a water molecule from a proton and hydroxide ion. This leads to
the definition that in Arrhenius acid–base reactions, a salt and water are formed from
the reaction between anacid and a base.
the production of chemical compounds by reaction from simpler materials
1. A single-displacement reaction, also namedsingle-replacement reaction, is a type of
oxidation-reduction chemical reaction when an element or ion moves out of one compound
and into another - that is, one element is replaced by another in a compound.
1. Double Replacement Reactions. Ax + BY --> AY + BX. A double replacement reaction
(also known as an exchange reaction or precipitation reaction) takes place when two
compounds interchange elements to form two new compounds.
Decomposition
the state or process of rotting; decay
combustion
the process of burning something
Electronegativity Electronegativity is a measure of the tendency of an atom to attract a bonding pair of
electrons. The Pauling scale is the most commonly used.
Lewis dot
diagrams
Ionization
energy
1. Lewis structures (also known as Lewis dot diagrams,electron dot diagrams, Lewis
dot formulas, Lewis dot structures, and electron dot structures) arediagrams that show
the bonding between atoms of a molecule and the lone pairs of electrons that may exist in
the molecule.
1. The ionization energy (IE) of an atom or molecule describes the minimum amount
ofenergy required to remove an electron (to infinity) from the atom or molecule in the
gaseous state.
Atomic radius 1. The atomic radius of a chemical element is a measure of the size of its atoms, usually the
mean or typical distance from the center of the nucleus to the boundary of the surrounding
cloud of electrons.
Protons
1. a stable subatomic particle occurring in all atomic nuclei, with a positive electric charge
equal in magnitude to that of an electron, but of opposite sign.
Neutrons
1. a subatomic particle of about the same mass as a proton but without an electric charge,
present in all atomic nuclei except those of ordinary hydrogen.
Electrons
1. a stable subatomic particle with a charge of negative electricity, found in all atoms and
acting as the primary carrier of electricity in solids.
Structure of
Atoms are the basic units of matter and the defining structure of elements. Atoms are
atoms
made up of three particles: protons, neutrons and electrons. Protons and neutrons are
heavier than electrons and reside in the center of the atom, which is called the nucleus
isotope
1. each of two or more forms of the same element that contain equal numbers of protons but
different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not
in chemical properties; in particular, a radioactive form of an element.
Ground state
A ground state configuration is an arrangement of electrons (orbitals occupied, spins states) associated with
configuration
the lowest potential energy for an atom
Physical
properties
Chemical
properties
Elements
1. A physical property is any property that is measurable whose value describes a state of
a physical system. The changes in the physical properties of a system can be used to
describe its transformations or evolutions between its momentary states.
1. a property or characteristic of a substance that is observed during a reaction in which
the chemical composition or identity of the substance is changed: Combustibility is an
important chemical property to consider when choosing building materials.
each of more than one hundred substances that cannot be chemically interconverted or
broken down into simpler substances and are primary constituents of matter. Each element
is distinguished by its atomic number, i.e., the number of protons in the nuclei of its atoms.
Compounds
a thing that is composed of two or more separate elements; a mixture.
Mixtures
a substance made by mixing other substances together.
Homogeneous
any combination of substances that has uniform composition and properties; a mixture that is uniform
mixtures
throughout
Heterogeneous 1. A heterogeneous mixture is made of different substances that remain physically
separate. Heterogeneous mixtures always have more than one phase (regions with
mixtures
uniform composition and properties). A mixtureof sand and sugar is a heterogeneous
mixture.
pH scale
A pH scale is a measure of how acidic or basic a substance is. While the pH scale formally
measures the activity of hydrogen ions in a substance or solution, it is typically
approximated as the concentration of hydrogen ions.
Arhenius
As defined by Arrhenius, acid-base reactions are characterized byacids, which dissociate
acid/bases
in aqueous solution to form hydrogen ions (H+) and bases, which form hydroxide (OH−)
ions. Acids are defined as a compound or element that releases hydrogen (H+) ions into
the solution
Bronsted-Lowry
The Bronsted-Lowry concept is based on the transfer of a proton from one substance to
acid / bases
another. The ionization of HCl in water can be viewed as a Bronsted-Lowry acidbase reaction with HCl behaving as the acid(H1+ ion donor) and water serving as
the base (H1+ ion acceptor).
pH equation
To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion
in moles per liter (molarity). The pH is then calculated using the expression:
pH = - log [H3O+].
Example: Find the pH of a 0.0025 M HCl solution. The HCl is a strong acid and is 100% ionized in
water. The hydronium ion concentration is 0.0025 M. Thus:
pH = - log (0.0025) = - ( - 2.60) = 2.60
pOH equation
To calculate the pOH of a solution you need to know the concentration of the hydroxide ion in moles
per liter (molarity). The pOH is then calculated using the expression:
pOH = - log [OH-]
Example: What is the pOH of a solution that has a hydroxide ion concentration of 4.82 x 10-5 M?
Catalyst (what
does it do to
activation
energy?)
Wavelength
A catalyst is something that will speed up the rate of a chemical reaction.
Lowers activation energy
the distance between successive crests of a wave, especially points in a sound wave or
electromagnetic wave
Frequency
the rate at which a vibration occurs that constitutes a wave, either in a material (as in sound waves),
or in an electromagnetic field (as in radio waves and light), usually measured per second.
Relationship
between
wavelength and
frequency
“exciting”
electrons (how
does this
produce
different colors
of light?)
Endothermic
reactions (be
able to tell these
on a graph)
As you see from what is shown above, wavelength varies inversely with frequency. That means as frequency get
larger, the wavelength gets proportionally smaller
When electrons become excited they enter an excited state, these can relax back to the ground state by
releasing a photon proportional to the energy between these two quantum states. The higher the difference
between these states, the higher the energy, the shorter the wavelength of emission.
the triangle is the uppercase greek letter, delta (Δ) . It means "change" in ΔH is means change in enthalpy. On a
graph, when the reactants are higher than the products, then energy is released, hence exothermic, viceversa,
when the reactants are lower on the graph, then energy was absorbed, thus endothermic
Exothermic
Exothermic reaction is a reaction in which heat/energy is given off
reactions (be
able to tell these
on a graph)
How do you
To balance equations make both elemnts equals on the both sides
balance
equations? (what
do you change?)
Limiting
reactants
1. The limiting reagent (or limiting reactant) in a chemical reaction is the substance which is
totally consumed when the chemical reaction is complete. The amount of product formed is
limited by this reagent since the reaction cannot proceed further without it.
Excess reactants
Limiting Reactant - The reactant in a chemical reaction that limits the amount of product
that can be formed. The reaction will stop when all of the limiting reactant is
consumed. Excess Reactant - The reactant in a chemical reaction that remains when a
reaction stops when the limitingreactant is completely consumed
Percent yield
The percentage yield (or fractional yield or relative yield), which serves to measure the
effectiveness of a synthetic procedure, is calculated by dividing the amount of the desired
product obtained by the theoretical yield(the unit of measure for both must be the same
Le Chatlier’s
Principle
(concentration
does what?)
Label the following graphs as endothermic or exothermic:
1. How do you name covalent compounds?
2. How do you name ionic compounds?
3. How do the following change the rate of a reaction?
a. Temperature
b. Pressure
c. Concentration
d. Surface area
e. catalyst
4. Period run (circle one) up and down or left and right on the periodic table.
5. Groups run (circle one) up and down or left and right on the periodic table.
6. How do you find the molar mass?
7. How do you convert between mass and moles?