Transcript Chapter one - gen. obc - Swampscott High School

CP 2 Chemistry Final Exam Review
Guide
Chemical Reactions
Symbols and abbreviations
Balancing Reactions
Types of reactions
SRR (Single replacement reaction)Element and a compound producing
different element and a compound
DRR (Double- Replacement reaction) Two compounds producing two different
compounds
Neutralization- Reaction between an
acid and a base producing salt and water
Composition – Reaction between two or
more reactants producing one product
Decomposition-One reactant producing
two or more products
Combustion- Reaction with oxygen
which produces carbon dioxide and water
Molecular composition
Mole Calculations (mol=Mass/F.W)
Formula weight calculations
% composition= (A.W of element/F.W of
compound) x100
% water in hydrated salt (8A-Lab)
Density of solution –mass percent (9 A
Lab)
Concentration and Beer’s Law (9 B Lab)
Gas Laws
What a Gas –Problem Solving and KMT
of gases
Boyle’s Law (p1V1=p2V2)
Charles’s Law (V1/T1 =V2/T2)
Gay- Lussac’s Law (p1/T1=p2/T2)
Avogadro’s Law (n1/V1=n2/V2)
Ideal gas law (pV=nRT, R = 0.08205
atm.L/mol.K)
Dalton’s Law Pt =P1+P2 +…
STP: Standard pressure and temperature
P=1 atm, T=0◦C
Labs: Boyle’s Law, Gas applications,
Hydrogen, Determining the value of R, Air
bag
Liquids and Solids
Properties of liquids and solids (Physical
equations for phase changes)
Heating and Cooling curve (Lab: Cooling
curve of Lauric acid)
Phase diagram Determining of normal
melting, boiling point, critical point, triple
point)
Properties of water (Lab: efflorescence
and deliquescence)
Solutions
Properties of Solutions (Lab: Factors
affecting the rate of dissolving- Heating,
Stirring, Grounding)
Solute- the substance that is
dissolve(lower amount)
Solvent- the substance that does the
dissolving (larger amount)
Solution- a homogeneous mixture
Solubility- maximum amount of a solute
that can be dissolved in 100 g of solvent
Miscible – capable of dissolving
Immiscible –not capable of dissolving
“Like dissolve like” rule – two identical
substances dissolve in each other
Solution and Calorimetery( Lab:
Determining the heat of Neutralization
Reaction)
Determining Hess’s Law: Heat of
formation lab
Concentration Units
Molarity M= mol /V in L
Mass % =( mass of solute /mass of
solution) x100
Dilution: M1V1 = M2V2
Colligative properties (Lowering
freezing point, Increasing Boiling point
and Lowering vapor pressure) Lab: Ice
cream
6. Acids and bases
6.1. Properties of acid and bases
(Explore household acids and basesAvtivity)
* Acid -is any substance that produces
hydrogen ions in water
- changes blue litmus paper to red
- Sour taste
- pH  7
* Base- is any substance that produces
OH- ions in water solution
- changes red litmus paper to blue
- Bitter taste
- pH  7
- feel slippery or soapy to the touch
Both acids and bases can undergo a
neutralization reaction.
Neutralization reaction is a reaction
between acid and base where the
products are salt and water.
6.2. Arrhenius definition
* Acid - is a substance that ionizes in
water to produce H+
* Base - is a substance that dissociate in
water to release OH- ions
6.3. Bronsted - Lowry definition
* Acid - is a substance that donates
hydrogen ions to any other substance
(proton donor).
* Base - is any substance that accept a
hydrogen ion (proton acceptor).
6.4. Acid- base titration
a) Principles of titration’s
measurement of the amount of a solution
of known concentration that is required to
react completely with a measured
amount of a solution of unknown
concentration.
* Standard solution - a solution that
contains a precisely known concentration
of a
solute
* Titration curve - is used to represent
pH data
- Strong acid with the strong base
(upward graph - end point at pH =7).
- Weak acid with a strong base (upward
graph - end point at pH = 8.9)
- Weak base with strong acid (downward
graph - end point at pH = 5.8)
Equivalent point - is the point at which
exactly enough standard solution I s
added to neutralize the unknown solution.
* End point - the point at which the
indicator changes color.
b) Indicators - are weak acids or bases
dyes whose colors are sensitive to pH or
hydronium ion concentration.
Labs: Standardization of NaOH, Titration
using pH meter-Titration curves, Titration
of vinegar 13B, Commercial antacids
Inquiry 13C
7. Equilibrium
7.1. The concept of equilibrium
In chemistry - most chemical reactions
are reversible processes.
a. When the rate of forward reaction is =
to the rate of the reverse reaction chemical equilibrium is
established.
b. Under the same condition, at
equilibrium the concentration of both
reactants and products remain constant.
c. At the same temperature the
equilibrium constant is constant
d. Equilibrium may be approached from
different starting points.
e. At other temperature the value of the
equilibrium constant differs.
7.2. The law of equilibrium
a) Equilibrium constant Keq.
collide in order to react. In successful
collision the existing bonds in a
molecule are broken and new bonds are
formed.
c) Factors affecting the rate of a chemical
reaction
* Collision frequency (depends of
concentration of the molecules and
temperature).
* Collision energy
* Orientation of the molecules
7.3. Reaction profile- shows the energy
of reactants and products during reaction
* Transition state - is the highest point on
the reaction profile where reactant and
products have the same potential
energy.
* Activation energy - the energy require
for the reaction to achieve the transition
state
a) Energy profile for exothermic reaction
b) Energy profile for endothermic reaction
7.4. Types of chemical equilibrium
a) Homogeneous
b) Heterogeneous
dynamic equilibrium is upset by
disturbance, the equilibrium will shift in a
direction to minimize the effect of
disturbance
a. Effect of concentration
b. Effect of temperature
c. Effect of pressure
d. Effect of catalyst
8. Electrochemistry
What kind of chemistry creates electricity
in a battery?-The lemon Battery 15A
An Electrochemical Cell -15 B (How do
batteries store energy?)
Oxidation- Reduction Reactions of metals
and Metal ions