By
Alec “Dr. Bathroom” Levy
Niteesh “The Yellow Dart” Chitturu
Nomenclature
 Cation-Electron-deficient atom/molecule (+ charge)
 Atoms in transition metals, alkalines, alkaline earths
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typically form cations
Ex.: Ca2+ Fe2+ Li+
Transition metals include Roman Numerals except
Zn2+ Ni2+ Ag+
Anion-Electron-surplus atom/molecule (- charge
Form in halogens, chalcogens, pnictogens, and
polyatomic molecules
Ex: F- O2- N3- SO2-
Nomenclature
 Atom-smallest unit of element that retains its
properties, includes mono- and poly Compound-2 different elements bonded together
 Molecule-Covalently bonded atoms
 Salt-Combination of 2 or more ions bonding to form a
neutral compound
 Same thing as a neutral ionic compound, which
consists of a metal cation and nonmetal anion
Acid Nomenclature
 Acids-Contains H+ cation
 -ide hydro_____ic acid
 -ate _____ic acid
 -ite ______ous acid
 Ex: Sulfide=hyrdosulfuric acid
 Ex: Sulfate=sulfuric acid
 Ex: Sulfite=sulfurous acid
Bonding & Formulas
 Covalent compounds-2 or more nonmetals, come first
in formula, except for F and O
 Organic compounds-Hydrocarbons, consists of only C
and H
 Alkanes-Carbon backbone, fills in excess with H, ends
with –ane 1=meth 2=eth 3=prop 4=but 5+=binary
 Alcohols-Adds O to chain, ends in -anol
Common Anions
 1- H- (Hydride ion), F- (Fluoride ion), Cl- (Chloride
Ion), Br- (Bromide ion), I- (Iodide ion), CN- (Cyanide
ion), OH- ( Hydroxide ion), C2H3O2- (Acetate ion),
ClO3- (Chlorate ion) ClO4- (Perchlorate ion), NO3(Nitrate ion), MnO4- (Permanganate ion)
 2- O2- (Oxide ion), O22- (Peroxide ion), S2- (Sulfide
ion), CO32- (Carbonate ion), CrO42- (Chromate ion),
Cr2O72- (Dichromate ion), SO42- (Sulfate ion)
 3- N3- (Nitride ion), PO43- (Phosphate ion)
Atomic Structures
 Angstrom-Å=10-10 meters=size of an atom
 Proton-Subatomic particle with positive charge of 1, in
the nucleus
 Neutron-Subatomic particle with neutral charge, in
the nucleus
 Electron-Subatomic particle with negative charge of 1,
in energy orbitals
 Protons and Neutrons consist of 99.99% of mass
 1 electron=1/1800 proton
Isotopic Notation
A
Z
X
q
 Isotopes have same number of protons but different
number of neutrons and are chemically identical
 A-Mass number=protons+neutrons
 q-Charge=electron+protons
 Z-Atomic number=protons
Isotopic Abundance/Molar Mass
 To calculate isotopic abundance from molar mass
 Ex: Average mass of sample is 1.614 g/mol. Molar mass
of hydrogen-1 is 1.00782, molar mass of deuterium is
2.01410. What is the abundance of the two isotopes?
 Answer: hydrogen-1=39.76%, deuterium=60.24%
Balancing reaction equations
 Given: C24H46O3 + O2CO2 + H2O
 Answer : C24H46O3 + 34O224CO2 + 23H2O
It’s 1.5-glyceride
Isn’t Chemistry pHun?
Mass-mole relationship
 1 mole of a substance is equal to 6.022 x 1023 particle
 1 mole of substance is equal to its amu but in grams
 Poly-atomic substances moles are a sum of its
constituents
 Ex: C24H46O3 has 24 C, 46 H, and 3 O. Thus:
(12.0107 x 24) + (1.00794 x 46) + (15.9994 x 3)=382.62024
g/mol
Empirical formulas/
percent composition
 Given percent composition by mass spectrometry, the
empirical formula of a molecule is what?
 54.50% carbon, 13.72% hydrogen, 31.78% nitrogen
 Assume given values are in grams, then calculate for
moles
 Divide moles by lowest value of moles
 Answer is subscript of empirical formula
 To determine molecular formula, molar mass must be
known Ex: 88.15 g/mol
Limiting/Excess Reactants
 To determine limiting reactant, balance equation and
solve for both reactants
 Lower value is limiting, the higher one is excess
Percent Yield
 Percent Yield=(actual or experimental
value)/(theoretical values determined by limiting
reactant)
Easy? Yes/No?
IT’S A GAS GAS GAS!!!
 Qualitative: pressure, volume, number of moles, and
temperature are at work, along with R, the gas constant
 Boyle’s Law: Volume of gas at constant temperature is
inversely proportional to pressure V=k ∙ 1/p
 Charles’s Law: Volume of gas at constant pressure is
directly proportional to absolute temperature V=k ∙ T
 Avogadro’s Law: Equal volumes of gases at equal
temperature and pressure contains equal number of
molecules, and volume of gas at constant pressure and
temperature is directly proportional to number of moles
V=k ∙ n
Ideal Gas Law
 PV=nRT
 R is the ideal gas constant, equal to 0.08206 L-
atm/mol-K
 Volume of a gas at STP is 22.41 L
 To calculate density, calculate concentration (mol/L)
and convert to g/cm3 (1 mL=1 cm3)
PV=nRT in action…
 Given: pressure is 1020 torr, volume is 1.5 L, and
temperature 37. 4 degrees Celsius, mass of sample is
2.530 g, what is the molar mass?
 1020 torr=1.342 atm
 37.4 degrees Celsius=310.55 degrees Kelvin
 n=PV/RT=.07899 mol
 Molar mass=g/mol=2.530 g/ .07899 mol= 32.03 g/mol
 It’s O2!
Partial Pressure
 Dalton’s law of partial pressures: Total pressure of a
mixture of gases equals the sum of the pressures that
each would exert alone
 Applies only for ideal gases!!!
 Pt = P1 + P2 + P3 …. + Pn
 Mole fraction (X)=Moles of given gas/Total Moles of
gas
 Pn = Xn Pt
Kinetic Molecular Theory
 Gases consist of large amounts of molecules in
continuous random motion
 The molecules have negligible volume compared to the
total volume the gas occupies
 There are negligible attractive or repulsive forces
between those molecules
 The average kinetic energy of the molecules remains
constant (the collisions are perfectly elastic)
 The molecule’s average kinetic energy is proportional
to the absolute temperature
Root Means Square Speed
 Velocity=u=√(3RT/M)
 R=gas constant
 T=absolute temperature
 M=kg/mol
 Lighter molecules move on average faster than heavier
molecules
Graham’s rates of
effusion/diffusion
 Effusion: Gas escaping into a vacuum
 Diffusion: Gas mixing into another gas, going from
high concentration to low concentration
 Rate A escapes/Rate B escapes= ua/ub = √Mb/Ma
Van der Waals’s equation
 Real (non-ideal) gas equation
 Molecules DO occupy space, thus takes up volume
 Molecules DO sometimes attract each other
 Correction factors are needed
 (Preal + a(n/v)2)(Vcontainer – bn)=nRT
 a=attractive coefficient, expressed in atm ∙ L2/mol2
 b=volume coefficient, expressed in L/mol
(Das Good?)
Fin
Dr. Bathroom and the Yellow Dart…Away!?!