Gas Laws & Conditions
760 Torrs = 760 mmHg = 1 atm
P = pressure V = volume
T = temperature n = moles
Boyle's Law (P⇅V): P₁V₁ = P₂V₂
Charles' Law (T⇈V): (V₁/T₁) = (V₂/T₂)
Avogadro's Law (M⇈V): (V₁/n₁) = (V₂/n₂)
Static Conditions:
PV = nRT R = 0.0821 L⁎atm/mol⁎K
note: units should be L, K, atm, & mol
Dalton's Law Pressure:
P total
= P gas1
+ P gas2
+ P gas3
+ P... |
Types of Branches
Alkyl Branches: named based on # of carbon contained
have a -yl ending
CH₃ methyl branch
CH₂CH₃ ethyl branch
CH₂CH₂CH₃ propyl branch
Halogen Branches: from group 17 of periodic table
F - fluoro
Cl - chloro
Br - bromo
I - iodo |
Units of Conversion
100 centimeters |
= 1 meter |
1,000 millimeters |
= 1 meter |
10,000 micrometers |
= 1 meter |
1,000,000 nanometers |
= 1 meter |
1,000 meters |
= 1 kilometer |
Energy
4184J |
= 4.184kJ |
= 1 kcal |
=1000 cal |
Kinetic Energy |
= (1/2) mv2 |
Kelvin |
= Co + 273.15 |
Specific Heat (q) |
= ms△T |
(△ change in temp.) |
Fats |
= 9 kcal/g |
Carbs |
= 4 kcal/g |
Proteins |
= 4 kcal/g |
Liquid ⟶ Solid |
= freezing |
Solid ⟶ Gas |
= sublimation |
Gas ⟶ Liquid |
= condensation |
Solid⟶ Liquid |
= melting |
Liquid ⟶ Gas |
= deposition |
Gas ⟶ Solid |
= vaporization |
Molarity & Concentration
Molarity = moles ÷ L |
Dilution: M₁V₁ = M₂V₂ |
Acids & Bases
Arrhenius Acids |
increase H⁺ / increases protons / increases H₃O⁺ |
Arrhenius Bases |
increase OH- (hydroxide) |
Simple Acids |
H + element off periodic table (e.g. HCl) |
Oxoacid |
H + polyatomic ion (e.g. HNO₃) |
Naming Acids: Drop the ending in simple acids and add "-ic acid" ex: Hydrochloric Acid
If the polyatomic ion ends in "-ite", change to "-ous acid" ex: Chlorous Acid
Note: Strong acids and strong bases dissociate completely.
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pH & Relative Acidity
Calculating Hydroxide: 1x10-14=[H₃O+][OH-] |
pH Equation: pH = - log[H+] |
Finding pH from Hydroxide Equation: solve for H₃O+, then solve for pH. |
Intermolecular Attractive Forces
Hydrogen Bonding - Strongest of the three. Requires an H to be directly bonded to an N, O, or F within a molecule.
Dipole-Dipole - During the next two sections of this module we’ll learn to ID molecules with this IMF. Molecules with dipole-dipole forces have a permanent positive and negative “sidedness” or polarity.
Dispersion Forces - Weakest of the three. All molecules have dispersion forces, but they’re the primary (strongest) forces for nonpolar molecules.
IMF Strength: (lowest)
D ➠ D-D ➠ HB (highest)
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Calculating Abundance
(mass x abundance %) + (mass x abundance %) |
Note:abundance must be calculated by a decimal (moving decimal place two times to the front)
Molecular Prefixes
1 = mono |
2 = di |
3 = tri |
4 = tetra |
5 = penta |
6 = hexa |
7 = hepta |
8 = octa |
9 = nona |
10 = deca |
Note: Ending of last element is replaced by -ide.
Example: CO₂ - carbon dioxide SF₆ - sulfur hexafluoride
Percent Yield
PY = (Actual Yield (g) x 100) ÷ (Theoretical Yield (g)) |
Ionic Compounds
Acetate ⟶ (C₃H₃O₂)-1 |
Nitrate ⟶ (NO₃)-1 |
Chlorate ⟶ (ClO₃)-1 |
Chlorate ⟶ (ClO₄)-1 |
Ammonium ⟶ (NH₄)+1 |
Hydronium ⟶ (H₃O)-1 |
Carbonate ⟶ (CO₃)-2 |
Phosphate ⟶ (PO₄)-3 |
Hydroxide ⟶ (OH)-1 |
Sulfate ⟶ (SO₄)-2 |
Contains : a metal and/or a polyatomic ion
Note: Cations come first (+) and Anions come last (-)
Ion Charges (exceptions): Al ⟶ +3 Zn⟶ +2
Writing Formulas: Cation keeps the name off periodic table while anion ends in -ide.
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Relating IMF Strength
As IMF strength increases:
➀ Boiling point (B.P.) will require higher temperature to boil.
➁ Melting point (M.P.) will require higher temperature to melt.
➂ Solubility in water will increase (like dissolves like, and water exhibits H-bonding, a strong IMF)
➃ Volatility, how readily a substance will go to the gas phase, will decrease.
IMF ⤊ B.P. ⤊ M.P. ⤊ Solubility in Water ⤋ Volatility |
Types of Reactions
Decomposition Reaction |
ex: 2HgO(s)→2Hg(l)+O₂(g) |
Combustion Reaction |
ex: C₃H₇(g)+5O₂(g)→3CO₂(g)+4H₂O(g) |
Single-Replacement Reaction |
ex: Zn(s)+2HCl(aq)→ZnCl₂(aq)+H₂(g) |
Double-Replacement Reaction |
ex: Na₂S(aq)+2HCl(aq)→2NaCl(aq)+H₂S(g) |
Combination Reaction |
ex: 2Na(s)+Cl₂(g)→2NaCl(s) |
Note: ∆⟶ reaction is heated up
hλ ⟶ energy is added in form of light
Strong Acids
HCl |
HBr |
HClO₃ |
HI |
HNO₃ |
HClO₄ |
H₂SO₄ |
Notes: Molecular substances act as nonelectrolytes. Soluble Ionic substances make for strong electrolytes.
Balanced equations with double-sided arrows (⟷) rules an electrolyte is weak because it dissociates and recombines.
Conversion Roadmap
mass ⟶ moles (use molar mass) |
moles ⟶ molecules (use Avogadro's number) |
molecules ⟶ atoms (use chemical formula) |
Note: Avogadro's Number 6.022x1023
Stoichiometry
Step #1: Balance Equation
Step #2: Given mass, convert with moles
Step #3: Perform Stoichiometry, convert back to mass at the end if needed. |
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