General Chemistry - MOOC Cheat Sheet

A Education › Chemistry cheat sheet in English by dswelam

Basic High School Chemistry

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PRs

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:
Ptotal = Pgas1 + Pgas2 + Pgas3 + 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

Density Equation

Density

= (m/v) g/mL ³

Energy

4184J	= 4.184kJ	= 1 kcal	=1000 cal
Kinetic Energy	= (1/2) mv²
Kelvin	= C^o + 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.

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)

Reactions of Alkenes

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.

Hydrocarbon Alkanes

Functional Groups List

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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