X Chemistry - Tredyffrin/Easttown School District
X Chemistry Name _______________________
Final Review 2014 one/customer
Electrons in Atoms
Summary: Light, electromagnetic spectrum, ground state for an electron, excited state for an electron, Heisenberg Uncertainty Principle, atomic orbital, quantum numbers, electron configurations, valence electrons, electron dot configurations
A. Bohr Model
Describe the differences between a ground state and excited state for an electron.
B. Electron Configurations
Define the following:
Aufbau principle –
Pauli exclusion principle –
Hund’s Rule –
Heisenberg Uncertainty Principle -
Answer the following questions:
1. What are the designations for the 4 sublevels?
_______, _______, ________, and ________
2. How many orbitals does each of the sublevels contain?
a. a s sublevel _______,
b. a p sublevel ________,
c. a d sublevel _______.
d. a f sublevel ________..
3. How many electrons (maximum) can each of the sublevels hold?
s _______, p _______, d _______, and f _______
4. How many electrons (maximum) can each of the following energy levels hold?
1st ______ 2nd _______ 3rd _______ 4th ______
Problems
1. Draw the full electron configurations for the following elements (no abbreviated)
A. N
B. Sr
2. Draw the abbreviated/Noble Gas electron configuration for the following elements.
A. Ca
B. Au
3. Draw the orbital electron configuration for the following elements.
A. P
The Periodic Table and Periodic Law
Summary: the scientists that contributed to the development of the Periodic Table, periodic law, the general organization of the Periodic Table, the basic properties of the groups and families, and the periodic trends of radius, energy and electronegativity
Problems:
What major contribution did each of the following make to the development of the Periodic Table:
Lavoisier:
Newlands:
Mendeleev:
Moseley
Define/describe the following:
Group or family:
Period:
Main group/representative elements:
Metals:
Nonmetals:
Metalloids:
Alkali metals:
Alkaline Earth metals:
Transition metals:
Halogens:
Noble Gases:
Rare Earth Metals:
Valence electrons:
Periodicity:
Atomic radius:
Ionic radius:
Ionization energy:
Electronegativity:
Periodic Trends: the 4 L’s!!!!! Period Group
Atomic Radius
Ionization energy
Electronegativity
Molecular Geometry
Summary: Lewis structures, resonance, expanded octets, VSEPR –shapes and electronegativity and bond type and polarity
Problems:
Define/describe the following:
Lewis dot structure:
Ionic bond:
Covalent bond:
Metallic bond:
Resonance:
Reduced octet
Expanded octet:
VSEPR model:
Complete the following table based on the correct molecular geometry:
|Chemical Formula |Name of Shape |Lewis Dot Structure |Polar or |
| | | |nonpolar? |
|CO2 | | | |
| | | | |
| | | | |
| | | | |
|H2O | | | |
| | | | |
| | | | |
| | | | |
|NH3 | | | |
| | | | |
| | | | |
| | | | |
|CH4 | | | |
| | | | |
| | | | |
| | | | |
| | | | |
| | | | |
|CSCl2 | | | |
| | | | |
| | | | |
| | | | |
| | | | |
| | | | |
|PCl6 | | | |
| | | | |
| | | | |
| | | | |
States of Matter
Summary: the 3 states of matter, kinetic molecular theory, diffusion and effusion, intermolecular forces, general properties of the phases, phase changes, and heating curve
Define/describe the following:
Solid:
Liquid:
Gas:
Kinetic Molecular Theory:
Temperature:
Diffusion:
Effusion:
Atmospheric pressure:
Barometer:
Manometer:
Intermolecular force:
Dispersion:
Dipole-dipole:
Hydrogen bonding:
Melting:
Vaporization:
Sublimation:
Condensation:
Deposition:
Freezing:
Problems:
1. Using the Lewis Dot Structures from the previous section, assign the dominant intermolecular force to each molecule:
CO2 ____________________________________________________
H2O___________________________________
NH3___________________________________
CH4___________________________________
CSCl2__________________________________
PCl6____________________________________
Gases
Summary: the general gas laws, combined gas law and ideal gas law,
relationships between variables
Problems:
1. State the relationship between the following sets (direct or indirect) of variables and briefly explain using the kinetic molecular theory:
a. P and V
b. V and T
c. P and T
2. A gas occupies a volume of 15.25mL when its pressure is 755torr. What will be the pressure if the gas is allowed to expand to a volume of 0.55L, while the temperature remains constant?
3. A gas at a constant pressure occupies a volume of 275ml at 25 oC. To what volume would the gas expand if its temperature were raised to 220.0 °C?
4. A gas at 28.0 °C has a volume of 65.0L and a pressure of 1135torr. Calculate the final temperature of the gas when its volume is 50.0L and its pressure is 1465torr.
5. What is the volume of a 0.031 moles of CO2 gas if it is in a container at 23 °C and 1.11atm?
Solutions
Summary: general information about solutions, the dissolving process, solubility, concentration calculations, and colligative properties, Solubility Curve
Problems:
Define/describe the following:
Solute:
Solvent:
Solution:
Miscible/Immiscible:
Solubility:
Saturated:
Unsaturated:
Supersaturated:
Boiling point elevation:
Freezing point depression:
1. What is the molarity of a solution containing 14.6g of CaSO4 dissolved in a total of 3.5L of solution?
2. How many grams of potassium hydroxide would you need to make 5 liters of a 0.75M solution?
3. How many milliliters of a 12M solution of hydrochloric acid would be required to make 8L of 2.25M hydrochloric acid?
Energy and Chemical Change
Summary: energy forms, calorie and Joule conversions, specific heat problems, transition state diagrams, and enthalpy problems
Problems:
Define/describe the following:
Energy:
Kinetic energy:
Potential energy:
Law of Conservation of Energy:
Chemical Potential Energy:
Heat:
Specific heat:
Endothermic:
Exothermic:
System:
Surroundings:
Universe:
Enthalpy:
1. What is the mass of a chunk of lead if 55,670 Joules of heat are absorbed when its temperature increases from 37°C to 100°C? The specific heat of lead is 0.129 J/g oC.
Reaction Rates and Equilibrium
Summary: reaction rate calculations, collision theory, potential energy diagrams, factors that effect reaction rates, equilibrium and the vocabulary involved, shifting equilibrium based on Le Chatelier’s principle
Problems:
Define/describe the following:
Reaction rate:
Collision theory:
Activated complex:
Activation energy:
Catalyst:
Inhibitor:
Reversible reaction:
Chemical equilibrium:
Dynamic equilibrium:
Equilibrium constant:
Le Chatelier’s Principle:
Stress:
1. Draw and label the potential energy diagram according to the following scenario. The potential energy of the reactants are 250 kcal, the potential energy of the products are 300 kcal, the activation energy without catalysis is 150 kcal and with catalysis is 100 kcal.
a. Is the above reaction endo or exothermic? _______________
b. What is the energy of the activated complex without catalysis? ____________
c. What is the heat of the reaction (ΔH)?__________________
Acids and Bases
Summary: Arrhenius model, acid/base strength, pH, pOH, neutralization, titrations
Problems:
Define/describe the following:
Acid solution
Base solution
Arrhenius model
Polyprotic and monoprotic acids
pH
pOH
neutralization reaction
titrations
equivalence point
acid/base indicator
1. What is the pH of a solution having a [H+] = 1.0 x 10-4 M? the pOH?
2. If the [OH-] was found to be 1.3 x 10-2 M, what is the pH?
3. A 35.0 mL sample of NaOH solution is titrated to an endpoint by 14.76 mL of 0.412 M HBr. What is the molarity of the NaOH solution?
................
................
In order to avoid copyright disputes, this page is only a partial summary.
To fulfill the demand for quickly locating and searching documents.
It is intelligent file search solution for home and business.
Related searches
- wisconsin school district report cards
- university school district jobs
- texas school district report cards
- university place school district jobs
- tea school district report card
- university city school district calendar
- school district of university city
- school district report cards texas
- u city school district employment
- university city school district employment
- university city school district website
- university place school district employment