2. By Alec “Dr. Bathroom” Levy Niteesh “The Yellow Dart” Chitturu

3. Nomenclature Cation-Electron-deficient atom/molecule (+ charge) Atoms in transition metals, alkalines, alkaline earths typically form cations Ex.: Ca 2+ Fe 2+ Li + Transition metals include Roman Numerals except Zn 2+ Ni 2+ Ag + Anion-Electron-surplus atom/molecule (- charge Form in halogens, chalcogens, pnictogens, and polyatomic molecules Ex: F - O 2- N 3- SO 2-

4. 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

5. 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

6. 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

7. Common Anions 1 -  H - (Hydride ion), F - (Fluoride ion), Cl - (Chloride Ion), Br - (Bromide ion), I - (Iodide ion), CN - (Cyanide ion), OH - ( Hydroxide ion), C 2 H 3 O 2 - (Acetate ion), ClO 3 - (Chlorate ion) ClO 4 - (Perchlorate ion), NO 3 - (Nitrate ion), MnO 4 - (Permanganate ion) 2 -  O 2- (Oxide ion), O 2 2- (Peroxide ion), S 2- (Sulfide ion), CO 3 2- (Carbonate ion), CrO 4 2- (Chromate ion), Cr 2 O 7 2- (Dichromate ion), SO 4 2- (Sulfate ion) 3 -  N 3- (Nitride ion), PO 4 3- (Phosphate ion)

8. 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

9. Isotopic Notation 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 X A Z q

10. 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%

11. Balancing reaction equations Given: C 24 H 46 O 3 + O 2  CO 2 + H 2 O Answer : C 24 H 46 O 3 + 34O 2  24CO 2 + 23H 2 O It’s 1.5-glyceride Isn’t Chemistry pHun?

12. Mass-mole relationship 1 mole of a substance is equal to 6.022 x 10 23 particle 1 mole of substance is equal to its amu but in grams Poly-atomic substances moles are a sum of its constituents Ex: C 24 H 46 O 3 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

13. 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

14. Limiting/Excess Reactants To determine limiting reactant, balance equation and solve for both reactants Lower value is limiting, the higher one is excess

15. Percent Yield Percent Yield=(actual or experimental value)/(theoretical values determined by limiting reactant) Easy? Yes/No?

16. 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

17. 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/cm 3 (1 mL=1 cm 3 )

18. 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 O 2 !

19. 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!!! P t = P 1 + P 2 + P 3 …. + P n Mole fraction (X)=Moles of given gas/Total Moles of gas P n = X n P t

20. 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

21. 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

22. 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= u a /u b = √M b /M a

23. 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 (P real + a(n/v) 2 )(V container – bn)=nRT a=attractive coefficient, expressed in atm ∙ L 2 /mol 2 b=volume coefficient, expressed in L/mol (Das Good?)

24. Fin Dr. Bathroom and the Yellow Dart…Away!?!