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Chemistry Cumulative Final
Chemistry Cumulative Final
107
Chemistry
Undergraduate 2
04/30/2014
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Term
variables-
 Definition
quantities that have more that one value
Term
density=
 Definition
mass/volume
Term
Precision-
 Definition
how close the measurements in a series are to each other
Term
Accuracy-
 Definition
how close each measurement is to the actual value
Term
Aqueous Solutions:
 Definition
Solutions in which water is the solvent
Term
Precipitation:
 Definition
reactions in which insoluble substances are produced
Term
Acid-Base:
 Definition
reactions between acids and bases
Term
Oxidation-Reduction:
 Definition
reactions which result in a change in oxidation state
Term
Strong Electrolyte:
 Definition
Compounds that completely dissociate in to their ions in H2O
Term
Nonelectrolyte:
 Definition
Compounds that do not dissociate in to their ions in H2O.
Term
Most molecular compounds that dissolve in H2O are ____
 Definition
nonelectrolytes.
Term
Weak Electrolyte:
 Definition
A molecular substance in whose aqueous solution some of the molecules react with H2O to form ions, but where some do not
Term
Acids:
 Definition
A substance that ionizes in water to produce H+ ions.
Term
Bases:
 Definition
A substance that ionizes in water to produce OH- ions.
Term
Titration:
 Definition
one solution of known concentration is used to determine the concentration of another solution through a monitored reaction.
Term
Oxidation Number:
 Definition
The charge of an atom in a molecule or ion
Term
Each element in its pure form has the oxidation number of __
 Definition
0
Term
For monoatomic ions, the oxidation number is =
 Definition
to the charge of the ion.
Sodium ion Na+1, Calcium ion Ca+2
Term
fluorine always has an oxidation number of __
 Definition
-1.
Term
The oxidation number of O is ___
 Definition
-2
Term
Oxidation:
 Definition
Loss of Electrons, oxidation number increases
Term
Reduction:
 Definition
Gain of Electrons, oxidation number decreases (or is reduced)
Term
Oxidizing Agent:
 Definition
Compound responsible for the oxidation, but is itself reduced
Term
Reducing Agent:
 Definition
Compound responsible for the reduction, but is itself oxidized
Term
Combination reactions:
 Definition
two or more reactants form one product:
X + Y à Z
Term
Boyle’s Law:
 Definition
The Compressibility of Gases (when moles and temp are constant)
Term
Pressure is inversely proportional to ___
 Definition
volume
Term
As pressure increases, the volume ____
 Definition
decreases
Term
Boyle’s Law Equation
 Definition
P1V1= P2V2
Term
Charles Law:
 Definition
if a given quantity of gas is held at a constant pressure, its volume is directly proportional to the Kelvin temperature
Term
Volume is proportional to ____
 Definition
temperature
Term
As temperature increases, the volume ___
 Definition
increases
Term
Charles Law Equation
 Definition
V1/ T1 = V2/ T2
Term
General Gas Law or Combined Gas Law Equation
 Definition
P1 V1/ T1 = P2V2 / T2
Term
Avogadro’s Hypothesis:
 Definition
the volume of a gas at a given temperature and pressure is directly proportional to the amount of gas in moles.
Term
Standard molar volume:
 Definition
1 mol of gas occupies 22.414 L
Term
Standard Temperature and Pressure (STP) :
 Definition
0 oC or 273.15 K and 1atm
Term
The Ideal Gas Law Equation
 Definition
PV = nRT
Term
The Density of Gases Equation
 Definition
d= m/v= PM/RT
Term
Partial Pressure:
 Definition
the pressure of each gas in the mixture
Term
Dalton’s Law of Partial Pressure:
 Definition
the pressure of a mixture of ideal gases is the sum of the partial pressures of the different gases in the mixture.
Term
Effusion:
 Definition
the movement of a gas through a tiny opening in a container into another container where the pressure is very low.
Term
Graham’s Law:
 Definition
The rate of effusion of a gas is inversely proportional to the square root of the mass of its particles.
Term
The First Law of Thermodynamics
 Definition
The energy change for a system is the sum of the energy transferred as heat between the system and its surroundings and the energy transferred as work between the system and its surroundings.
Term
The First Law of Thermodynamics Equation
 Definition
ΔE= q + w
Term
ΔE=
 Definition
Change in energy content
Term
q =
 Definition
Energy transferred as heat to or from the system
Term
w =
 Definition
Energy transferred as work to or from the system
Term
Enthalpy:
 Definition
Is the thermodynamic function defined by H. It is equal to the amount of energy transferred as heat at a constant pressure.
Term
If ΔH is negative, energy is transferred as heat from the system to the surroundings.
 Definition
Exothermic.
Term
If ΔH is positive, energy is transferred as heat from the surroundings to the system.
 Definition
Endothermic.
Term
Specific Heat Capacity:
 Definition
The energy transferred as a heat that is required to raise the temperature of 1 grams of a substance by 1 kelvin (when heating or cooling)
Term
Specific Heat Capacity Equation
 Definition
q = C x m x ΔT
Term
C =
 Definition
specific heat capacity, units in J/g*K
Term
m =
 Definition
mass of the substance
Term
ΔT =
 Definition
change in temperature
Term
Thermal Equilibrium:
 Definition
When two objects which were once at different temperatures, reach the same temperature
Term
Calorimetry:
 Definition
The method by which the energy evolved or required as heat in a chemical of physical process is measured.
Term
Calorimetry Equations
 Definition
qr + qsolution = 0
qsolution = Csolution x msolution x ΔT
Term
Standard Molar Enthalpies of Formation ΔfHo :
 Definition
The enthalpy change for the formation of 1 mol of a compound directly from its component elements in their standard states.
Term
Standard Molar Enthalpies of Formation ΔfHo Equation
 Definition
ΔrHo= ∑ ΔfHo(products) - ∑ ΔfHo(reactants)
Term
Electromagnetic Radiation:
 Definition
Characterized by wavelength and frequency and includes light, microwaves, television and radio signals x-rays, and other forms of radiation
Term
Plank:
 Definition
Assumed that the EMR emitted was caused by vibrating atoms called oscilators. And if each oscilator had a frequency, and the emitted radiation had a certain energy, the following eqn could be written.
Term
Plank's Equations
 Definition
E= nhν
E= hν
Term
Plank's Constant
 Definition
h = 6.6260693 x 10 -34 J*s
Term
Einstein:
 Definition
Photoelectric Effect: electrons are ejected when light strikes the surface of a metal.
Term
The 4 visible lines in the spectrum of hydrogen are now known as the_____
 Definition
Balmer series.
Term
If n = 3 the wavelength of the ___ line in the Hydrogen spectrum is obtained
 Definition
red
Term
If n = 4 the wavelength of the ____ line is obtained
 Definition
green
Term
If n = 5 and 6 the wavelength of the ___ lines are obtained
 Definition
blue
Term
deBroglie:
 Definition
Proposed that matter which was normally considered a particle, could also exhibit wave properties. Previously for light in the photoelectric effect.
Term
Bohr Model:
 Definition
That both the energy and the location for the electron in the hydrogen atom can be described accurately
Term
Heisenberg:
 Definition
Determined that for an object such as an electron in an atom, it is impossible to determine accurately both its position and its energy.
Term
Heisenberg Uncertainty Principle:
 Definition
any attempt to determine accurately either the location or the energy will leave the other uncertain.
Term
Schrodinger:
 Definition
Developed quantum mechanics or wave mechanics. Uses mathematical eqns of wave motion to generate wave functions which are used to describe a electrons in the atom.
Term
Paramagnetic:
 Definition
Elements or compounds that have unpaired spins and are attracted to magnets.
Term
Diamagnetic:
 Definition
Substances in which all the electrons are paired (with 2 electrons in each pair, having opposite spins) experience a slight repulsion when subjected to a magnet
Term
Pauli Exlusion Principle:
 Definition
No two electrons can have the same set of quantum numbers. No more than two electrons can be in an atomic orbital.
Term
Aufbau Principle:
 Definition
The procedure in which electrons are assigned to orbitals.
Term
Ionization Energy:
 Definition
The energy required to remove an electron from an atom in the gas phase.
Term
Electron Affinity:
 Definition
The energy change for a process in which an electron is acquired by the atom in the gas phase or “how bad an atom wants an electron.”
Term
Trends in Ion Sizes:
 Definition
The trends are the same down a periodic group as for neutral atoms. Positive and negative ions increase in size, but they are much smaller and larger than the neutral atoms, respectively.
Term
Isoelectronic Ions:
 Definition
Ions that have the same number of electrons (but different number of protons). N-3, O-2, F-, Na+,and Mg+2
Term
Ionic bond:
 Definition
forms when one of more valence electrons is transferred from one atom to another. Produces a positive and negative ion. The “bond” is the attraction between the ions
Term
Covalent bond:
 Definition
forms by the sharing of valence electrons between atoms.
Term
Lattice Energy:
 Definition
D Holattice the enthalpy change that occurs when 1 mol of ionic solid separates into gaseous ions.
Term
Coulombs Law:
 Definition
electrostatic energy between two charges is directly proportional to the product of their magnitudes and inversely proportional to the distance between them.
Term
Electrostatic energy =
 Definition
(Cation charge x Anion charge) / (Cation radius + Anion radius)
Term
Bond Length:
 Definition
the distance between the nuclei of two bonded atoms
Term
Related to the atomic size and the order of the bond.
 Definition
Bond Length
Term
Bond Dissociation Enthalpy:
 Definition
the enthalpy change for breaking a bond in a molecule with the reactants and products in the gas phase
Term
Bond Dissociation Enthalpy Equation
 Definition
ΔrH= ΣΔH(bonds broken)- ΣΔH(bonds formed)
Term
Polar Covalent Bond:
 Definition
When the e- are shared unequally.
Term
If the difference between electronegativities is greater than 1.7, the bond is ____
 Definition
ionic
Term
If the difference between electronegativities is less than 1.7, the bond is ____
 Definition
polar covalent
Term
If the difference between electronegativities is 0.5 or less, the bond is _____
 Definition
covalent (nonpolar)
Term
Octet:
 Definition
An octet of e- surrounding an atom is regarded as a stable configuration.
Term
Bond pair:
 Definition
The e- involved in the covalent bond.
Term
Lone pair:
 Definition
The e- not involved in bonding also called nonbonding e-.
Term
Formal Charge:
 Definition
the charge on an atom in a molecule or polyatomic ion.
Term
Formal charge= group # of the atom- [ LPE + 1/2(BE)]
 Definition
group # of the atom- [ LPE + 1/2(BE)]
Group #= gives the number of valence e- for a particular atom
LPE= number of lone pair e-
BE= number of bonding e- around the atom
Term
Resonance structure:
 Definition
Alternative structures of the same molecule which have identical bonding patterns and equal energy.
Term
Resonance hybrid:
 Definition
The actual structure of the molecule is a composite of the equivalent resonance structures. In the hybrid, the bonds are between a single and double bond in length.
Term
Bond Order:
 Definition
the number of bonding e- pairs shared by two atoms in a molecule.
Term
Bond order=
 Definition
# of Shared pairs in all X-Y bonds / # of X-Y links in the molecule or ion
Term
Dipole/Induced Dipole Forces:
 Definition
polar molecules can induce a dipole in a molecules that do not have a permanent dipole.
Term
London dispersion forces are the only intermolecular forces that allow _____ molecules to interact
 Definition
non- polar
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