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?

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