PRE-AP CHEMISTRY EQUATIONS AND CONSTANTS
PRE-AP CHEMISTRY
REFERENCE PACKET
Includes:
Equations & Constants
Periodic Table
Common Oxidation Numbers
Naming Flow Chart
Elements to Memorize
Polyatomic Ions to Memorize
Electronegativity Values
Solubility Rules
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PRE-AP CHEMISTRY EQUATIONS AND CONSTANTS
ATOMIC STRUCTURE
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BEHAVIOR OF GASES
Ptotal = P1 + P2 + P3 + …
PV = nRT
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SOLUTIONS
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V1M1 = V2M2
Kw = [H+][OH–]
pH = – log [H+]
pOH = – log [OH–]
[H+] = 10 – pH
[OH–] = 10 – pOH
pH + pOH = 14
THERMOCHEMISTRY
Q = mCΔT (also known as “ΔH”)
ΔH = moles x Hfus/vap
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OTHER FORMULAS
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EQUILIBRIUM
For aA + bB ↔ cC + dD:
[pic] Rate = k[A]x[B]y
CONSTANTS AND CONVERSIONS
Avogadro’s Number = 6.022 x 1023 particles per mole
h = Planck’s Constant = 6.63 x 10-34 J·s
c = Speed of Light = 3.0 x 108 m/s
Kw = ionization constant of water = 1 x 10–14 (mol/L)2
STP = 0 °C and 1 atm
0°C = 273 K
Volume of Ideal Gas at STP = 22.4 L/mol
1 atm = 760 mm Hg = 760 torr = 101.33 kPa = 14.7 psi
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1 cm3 = 1 mL
1 calorie (cal) = 4.18 joules (J)
1000 calories (cal) = 1 Calorie (Cal) = 1 kilocalorie (kcal)
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Naming Flow Chart
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NAMES/SYMBOLS OF ELEMENTS TO MEMORIZE!
|NAME |SYMBOL |NAME |SYMBOL |NAME |SYMBOL |
|antimony |Sb |fluorine |F |phosphorus |P |
|argon |Ar |gold |Au |platinum |Pt |
|arsenic |As |helium |He |potassium |K |
|barium |Ba |hydrogen |H |radon |Rn |
|beryllium |Be |iodine |I |selenium |Se |
|bismuth |Bi |iron |Fe |silicon |Si |
|boron |B |krypton |Kr |silver |Ag |
|bromine |Br |lead |Pb |sodium |Na |
|cadmium |Cd |lithium |Li |strontium |Sr |
|calcium |Ca |magnesium |Mg |sulfur |S |
|carbon |C |manganese |Mn |tin |Sn |
|cesium |Cs |mercury |Hg |tungsten |W |
|chlorine |Cl |neon |Ne |uranium |U |
|chromium |Cr |nickel |Ni |xenon |Xe |
|cobalt |Co |nitrogen |N |zinc |Zn |
RULES: (1) 1st letter PRINTED uppercase, 2nd letter PRINTED lowercase (2) spelling counts! (3) NO cursive!
QUIZ ONE: 1st column QUIZ TWO: 1st and 2nd column QUIZ THREE: 1st, 2nd and 3rd column
Electronegativity Values
|H | | | |
|2.1 | | | |
|xxx |PO4—3 |PO3—3 |xxx |
| |phosphate |phosphite | |
|xxx |SO4—2 |SO3—2 |SO2—2 |
| |sulfate |sulfite |hyposulfite |
|xxx |CO3—2 |xxx |xxx |
| |carbonate | | |
|xxx |NO3—1 |NO2—1 |xxx |
| |nitrate |nitrite | |
|ClO4—1 |ClO3—1 |ClO2—1 |ClO—1 |
|perchlorate |chlorate |chlorite |hypochlorite |
|BrO4—1 |BrO3—1 |BrO2—1 |BrO—1 |
|perbromate |bromate |bromite |hypobromite |
|IO4—1 |IO3—1 |IO2—1 |IO—1 |
|periodate |iodate |iodite |hypoiodite |
per___ate: has one more oxygen than “ATE”
___ate: most common form
___ite: one less oxygen than the “ate”
hypo__ite: two less oxygens than the “ate”
___ide: no oxygens, not a polyatomic
OTHERS:
|MnO4—1 |permanganate |
|C2H3O2—1 |acetate |
|HCO3—1 |hydrogen carbonate (bicarbonate) |
|CrO4—2 |chromate |
|Cr2O7—2 |dichromate |
|OH—1 |hydroxide |
|CN—1 |cyanide |
|NH4+1 (note positive charge) |ammonium |
NOTE: The charge can be shown either before or after the number… both are correct. Also, if a charge is either +1 or –1, you may show just the sign (+ or –). The 1 is not required to be shown.
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