Chemistry 11 Review
Unit 1: Safety
• Safety Equipment in the classroom
– Fume Hood
– Broken Glass Container
– Fire Blanket
– Emergency Shower
– Eye Wash Station
– ETC ETC
Unit 1: Safety
• First Aid Personnel
– Mr. Chio
– Mr. Ngo (next door teacher)
– Office
– Safe School Liason
Unit 1: Safety
• Common Hazards
– Broken Glass
– Fire
– Chemical Spill
– Fumes in the air
– Chemical in eye
– ETC ETC
Unit 1: Measurement
• SI Units (g, L, m)
• SI Unit conversion between base unit and
prefixes (mg, g, kg, mL, L, kL, mm, m, km)
• Precision vs Accuracy
• Sig Figs
• Calculations involving sig figs
• Scientific Notation
Unit 1: Unit Conversion
• What you want is always on the “top” or
“bottom”
• Always remember your conversions for SI
units
– 1kg = 1000g
– 1mg = 0.001g
• Calculate at the very end!
Unit 2: Matter
• What is matter?
– Anything that has mass and takes up volume
• Hypothesis vs Theory vs Law
• Physical vs Chemical properties
– Physical = any property that uses 5 senses
– Chemical = reactivity properties
• Matter
– Solid, Liquid, Gas
Unit 2: Matter
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Classification of Matter
Homogeneous vs Heterogeneous
Pure Substance vs Solution
Mixtures
Mechanical Mixtures vs Homogeneous
Mixtures
Unit 2: Matter
• Intensive Properties
– Doesn’t matter about how much
• Extensive Properties
– Matters about how much you have
• Quantitative vs Qualitative
• Kinetic Molecular Theory
– Bouncey Balls that do not lose energy
Unit 2: Matter
• Physical vs Chemical change
– Physical Change = no new substance is formed
– Chemical Change = new substance is formed
Unit 2: Matter
• Types of Separations
– Hand Separation
– Filtration
– Evaporation
– Distillation
– Solvent Extraction
– Recrystallization
– Gravity Separation
– Chromatography
Unit 2: Nomenclature
• Second element ends in IDE!
• Ionic Compounds
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Criss Cross method
Reduce
Never write 1
Multi-valents use roman numerals
• Use the non-metals charge that never changes to find its charge
– Polyatomics are grouped together and carry a charge
• Covalent follows the same rule, except no charge
– Their names have pre-fixes
• Hydrates are water molecules at the end, use prefixes
to say how many
Unit 2: Nomenclature
• Acids start with H
• Ionic acids that end in
– IDE turns into IC
– ATE turns into IC and drops the hydro
– ITE turns into OUS
Unit 3: Mole Concept
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Everything combines in whole ratios
Avogadro's number
Molecules vs Atom #
How to find atomic mass
STP!
– Only for gases at STP
– 22.4L/mol
Unit 3: Mole Concept
• Molecular vs Empirical Formula
– Percent composition
• How to find
• Make percent = g
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Percent to mass
Mass to moles
Divide by smallest
Multiply til whole!
– Molecular formula needs molar mass
Unit 3: Mole Concept
• Mol/L
• Can use density and molar mass to find
concentration
• Dilution
– C1V1 = C2V2
– If mixing two of the same solution. You add the
concentration at the end!
Unit 4: Chemical Reaction
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Reactants to Products
Coefficient = # of moles
Conservation Laws
Closed vs Open Systems
Balancing chemicals
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Solve metals first
Balance all elements that are with the metals
Balance O and H last
Balance polyatomics as 1 unit
Use fractions
Multiply til whole
• States of matter!
Unit 4: Chemical Reactions
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Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
Acid/Base Neutralization
Unit 4: Chemical Reactions
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Synthesis = exothermic
Decomposition = endothermic
Exothermic vs endothermic
Enthalpy is the heat of a reaction
Page 122 has a summary aid for energy
Unit 4: Stoichiometry
• Cross the mole bridge!
• Convert to moles first
• Molar concentration
– Convert to moles first!
• Titration
– Balance and know that the moles of acid = moles
of base at equivalence point
Unit 4: Stoichiometry
• Limiting Reagent
– Determines how much product you will form
• Percent Yield
– Determines how much yield you will get
– Actual/theoretical
• Percent Purity
– Determines how much yield you will get based on
how pure your substance is
Unit 5: Atomic Theory
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Democritus (matter/atoms)
Aristotle (ancient elements)
Dalton (atoms)
Thomson (electrons)
Rutherford (protons and nucleus)
Bohr (orbitals)
Unit 5: Atomic Theory
• Subatomic Particles
– Electrons
– Protons
– Neutrons
• Atomic number vs Atomic Mass
• Isotopes
– Different neutrons so different mass
• Average atomic mass
– Multiply percentage by mass and add
Unit 5: Atomic Theory
• Mendeleev developed the periodic table from the
reaction with oxygen
• Arranged them by mass
• Periodic Trends
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Your periodic table
EN
IE
Radii
Reactivity
Metallic properties
Unit 5: Atomic Theory
• Electron Configuration
– Orbitals
• Core Notation
– Noble gases need to be written by previous rows
noble gases
• Half and Full filled d-orbitals
• Predicting Valence Electrons
– Only s and p orbitals
Unit 5: Atomic Theory
• Ionization Energy and Electronegativity
• Ionic Bonds
• Covalent Bonds
– Polar vs Non-polar
• Metallic Bonds
• London Forces vs Dipole-Dipole forces
Unit 5: Atomic Theory
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Lewis Structures
8 x #atoms (except hydrogen = 2)
Valence electrons
Substance the two to find bonds
– Exceptions are B, Be, and Al
• Octet rules still apply!
• PCl5 can have more than 4 bonds
Unit 6: Solution Chemistry
• Solutions are homogeneous mixtures
– Solvents
– Solutes
• Solubility
– The amount of substance in mass dissolved in
100mL of water
• Saturated vs Unsaturated
• Like dissolves like
Unit 6: Solution Chemistry
• Polar and Non-polar solvents
• Dissolving which one?
– Polar dissolves ionic
– Non-polar cannot dissolve ionic
• Solvation = hydrating an ionic solid
Unit 6: Solution Chemistry
• Conductivity
– Metals
– Ionic solutions
– Acids or bases
• Covalent and organic compounds do not
conduct
• Solids do not conduct unless they are metal
Unit 6: Solution Chemistry
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Ions have concentration too
Must balance the dissociation equation
Follow the mole conversion
If mixtures, dilute first and add common ions
Good Luck!