Chem 11 Final Review!

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Chem 11 Final Review!

• Fun!

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Unit 2

• Unit conversions
• Use conversion factors

Conversion factor
3

• Top part bottom part

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• Cross out units to get the unit you want.
• Find the initial amount, the unknown amount, and
  the conversion factor for every question

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Metric units

• Need to memorize!

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• Derived quantity Number made by combining two or
  more other values. (i.e. molar concentration)
• Derived unit made by combining two or more
  units. (i.e. the units for molar concentration
  mol/L)

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Density

• dm/v
• Less dense liquids/objects float on more dense
  liquids.

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Accuracy/Precision???
Precise but not accurate

• Accuracy measurement close to the
  correct/accepted value.
• Precision how reproducible the measurement is.
  More sigfigs more precise.

Accurate but not precise
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Reading scales
5.92
6.06

• i) 5.925

• ii) 6.064

• iii) 6.000

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Experimental uncertainty

• Estimated amount by which a measurement migth be
  in error.
• 45.56 0.44 mL

Uncertainty. Same number of decimal places as
the actual number.
Certain digits
Uncertain digit
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Range

• 45.56 0.44 mL
• The actual value will lie within the range of
• 46.00mL 45.12 mL

• If given only the range, to figure out the
  experimental uncertainty i.e. 22.1-22.7 mL
• (1/2)(22.122.7) (1/2) (22.7-22.1)
• 22.4 0.3 mL

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Sigfig Rules

• Leading zeroes are not significant
• 0.00043 --gt 2
• Trailing zeros are all significant
• 350.00 ? 5 3500 ? 2 3500. ? 4
• When multiplying/dividing answer least number
  of sig figs used in the calculation.
• 2300 x 5.00 11500 1.2x104
• When adding/subtracting, use least number of
  decimals for answer.
• 13.00 2.0 15.0

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• 1.234x106 4.568x107 ?
• Change them to be both the SAME exponential
  value.
• i.e. 0.1234x107 4.568x107

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Unit 3

• Qualitative (non-numerical) versus quantitative
  (numerical)
• Height
• Weight
• Appearance

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Know your definitions!

• Observation, Interpretation, Description, Data,
  Experiment, Hypothesis, Theory, law
• Physical property (i.e. colour, density),
  chemical property (i.e. flammability)
• Extensive property (mass, volume), intensive
  property (density, melting point)
• Differences between solid/liquid/gas
• Hardness, malleability, ductility, lustre,
  viscosity, diffusion
• Vapour, vapour pressure
• Boiling, melting temperature

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Classification of Matter
Phase
System
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A. Matter Flowchart
MATTER
yes
no
Can it be physically separated?
Heterogeneous
Homogeneous
Compound
Element
Mechanical mixture
Solution
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Solvent/Solutes

• Solution solvent solute
• Solvent MORE
• Solute LESS

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Immiscible/miscible
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Physical separation of substances- study chart
on p58 -

• Hand separation
• Filtration
• Evaporation
• Distillation
• Solvent extraction
• Recrystallization
• Gravity Separation
• Paper, column, thin layer chromatography (dont
  need to know details)

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Phase Changes

• Chemical changes new substances formed
  (irreversible)
• Physical changes (reversible) no new chemicals
  involved

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Boiling
Condensing
Melting
Freezing
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Kinetic energy

• Rotational energy
• Vibrational energy
• Translational energy

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• Phase changes are usually due to the fact that
  translational energy reaches a critical value and
  causes molecules to break out of their original
  phases.

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Unit 4
Non-Metal
Metal
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Group/ Family
Period
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• Cations versus anions
• Cations positive ions Anions negative ions
• Monoatomic, diatomic, triatomic, polyatomic
• Ne, H2, H2O, PO43-

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Naming

• Ionic compounds
• (multivalent metals use roman numerals)
• Covalent compounds use prefixes
• Polyatomic compounds (PO43- , SO42- , OH- )
• Hydrates (FeBr32H2O)

• Iron (III) bromide dihydrate

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Unit 5 the Mole!

• Unit used to measure amount of substance.
• Molar mass mass of
• one mole of particles.
• Si3 (SO4)2

28.1 (3) (32.1) (2) 16.0(8) 276.5 g/mol
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Molar conversions
20 molecules of H2O ?? Atoms One molecule H2O
3 atoms Conversion factor 3 atoms 1
molec H2O 20 molecules x 3 atoms 60 atoms
1 molec H2O
x subscript
MM
X 6.022x1023
Mole (mol)
Molecule (molec)
of Atoms
Mass (g)
MM
subscript
6.022x1023
22.4
22.4
Volume (L)
Can only use 22.4L at STP!
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Percentage Composition

• Percentage of each species in a chemical formula.
• (p90)

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Empirical and molecular formulae

• Empirical formula the simplest formula
• P91

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Molar concentration

• When have only one solution
• M mol (solute)/L (solvent)
• When have two solutions (i.e. dilution problems
  or mixing problems)
• Use M1V1 M2V2

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V1
M1

• What is the molarity of 250.0mL of 0.500M
  solution A after it is diluted with 400.0mL of
  water?
• Use M1V1 M2V2

V2 400.0mL 250.0mL
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Unit 8 Chemical Reactions
Coefficients

• 3Sn(NO2)4 4K3PO4 ---gt 12KNO2
  Sn3(PO4)4

Product
Reactant
Law of Conservation of Mass of reactants
of products
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Open/Closed Systems
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• Write the phases in the equations
• ggas s solid l liquid
• aq aqueous (mixed with water)

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Diatomic elements
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Types of chemical reactions

• 6 types
• Synthesis
• Decomposition
• Single Replacement
• Double Replacement
• Acid-Base
• Combustion

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1) Synthesis
A B ? AB
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2) Decomposition
AB ? A B
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3) Single Replacement
A CD ? AD C
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4) Double Replacement
AB CD ? AD BC
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5) Neutralization
Acid Base ? Salt Water
HA BOH ? AB HOH (H2O)
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6) Combustion

• CxHy O2 ? CO2 H2O

Hydrocarbon
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Energy Changes

• Endothermic

Exothermic
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Unit 7 Stoichiometry

• Mole bridge

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• 4 Mol Al(OH)3 ? ?? mol H2O
• Use mole bridge.
• 4 mol Al(OH)3 x 6 H2O 12 mol H2O
• 2 Al(OH)3

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• Stoichiometry of excess quantities and percentage
  yield.

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Unit 8 The Atom
Democritus
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Thomsons Plum Pudding Model
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Bohr Rutherford
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Energy Level Diagrams

• Aluminum 13 electrons

Orbital
Shell
Subshell
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• Aluminum 13 electrons

1s22s22p63s23p1
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Core Notation use the noble gas that is right
BEFORE the element.
Ne10
Al -
3s23p1
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Ions

• Negative ions add the electrons just like if it
  was a neutral atom.
• Positive ions
• P is removed before s, s is removed before d

V - Ar18 4s23d3
V4 - Ar18 4s23d3
1
V4 - Ar18 3d1
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Valance electrons

• All the electrons in s and p shells not included
  in the noble gas core.
• Filled D f electrons are NOT valence electrons.
• Unfilled D and F electrons ARE valence electrons.

V - Ar18 4s23d3
Ge - Ar18 4s23d104p2
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Electrostatic rules

• Opposites attract
• Likes repel
• Shorter the distance, greater the attraction
• Greater the charges of the two particles, greater
  the attraction

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Periodic Trends

• Metallic trend
• Atomic radius
• Ionization Energy
• Electronegativity

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IE increases
IE decreases
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EN increases
EN decreases
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Know how to draw Lewis compounds

• Covalent and Ionic
• Double/Triple bonds.
• Remember atoms all just want to be stable!
  (have 8 electrons around it)

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• Electron-deficient molecules (H, Be, B, Al)
• Can have less than 8 electrons to be full
• Be 4
• B 6
• Al 6
• H 2
• Expanded octet
• Can have more than 8.
• Any element in the third and fourth periods.