Download Practice Test C Electron Configurations and Periodic Trends File

NAME_________________________
Electron Configurations and Periodic Trends
Chapter 13 and 14
Practice Test C
Round 2 Testing
Objective 1: Summarize the development of atomic theory.
Directions: Identify the correct scientist to the clues as related to atomic theory history.
1. The atom was considered an indivisible mass.
2. Discover of the nucleus, showing that the atom’s mass is concentrated in a small,
positively charged region.
3. Modern atomic theory that describes the electronic structure of the atom as the
probability of finding electrons within certain regions of space.
4. The discoverer of the electron, proposed the plum-pudding model.
5. Electrons travel in definite orbits around the nucleus, similar to a solar system.
Answers:
1. ________________________________
2. ________________________________
3. ________________________________
4. ________________________________
5. ________________________________
Score: ________________/10
Objective 2: Apply the Aufbau principle, the Pauli Exclusion Principle, and Hund’s
Rule in writing electron configurations and orbital diagrams of atoms.
Directions: Write the complete electron configurations and orbital diagrams for the
following elements:
1. Manganese
2. Magnesium
3. Potassium
4. Yttrium
5. Krypton
Score: _________________/15
Objective 3: Using Kernel Structures, write the electron configuration and orbital
diagrams for the following elements:
1. Indium
2. Cobalt
3. Iodine
4. Strontium
5. Sodium
Score: _________________/15
Objective 4: Interpret group and periodic trends in atomic radii, ionic radii,
ionization energies, and electronegativities.
1. Of the following atoms, which has the smallest FIRST ionization energy?
Mg, K, N, Ge, Br
_______________
2. Which element would have the lowest electronegativity value?
O, Cs, Al, Ca, P
__________________
3. Which of the following has the largest Second ionization energy?
Pb, F, K, Mg, N
_______________
4. List the following in the correct order of increasing atomic radius (smallest to biggest):
Mg, Na, S, P, Al
_______________________________________________________________
5. Which ion has the smallest radius?
Calcium Ion, Iodide Ion, Oxide Ion, Potassium Ion, Sulfide Ion
_________________
Score: _______________/15
Objective 5: Radiant Energy (3 points each)
1.
What is the frequency of radiation that has a wavelength of 392 mm?
2. What is the wavelength of radiation that has a frequency of 1.67 x 10 14 s-1?
3. What is the frequency of radiation whose wavelength is 15.0 Angstroms?
4. A nitrogen ion laser emits light at 337 nm. What is the frequency of this radiation?
Score: ______________/12
Objective 6: Quantized Energy and Photons (3 points each)
1. Calculate the smallest increment of energy (a quantum) that can be emitted or absorbed at
a wavelength of 522 nm.
2. Calculate the energy of a photon of frequency of 5.76 x 10 12 s-1.
3. What wavelength of radiation has photons of energy 7.82 x 10-18 J?
4. The energy from radiation can be used to cause the rupture of chemical bonds. A
minimum energy of 193 kJ/mol is required to break the bromine-bromine bond in
molecular bromine. What is the longest wavelength of radiation that possesses the
necessary energy to break the bond? What type of electromagnetic radiation is this?
5. It requires a photon with a minimum energy of 1.44 x 10-19 J to emit electrons from
sodium metal.
a. What is the minimum frequency of light necessary to emit electrons from sodium
via the photoelectric effect?
b. What is the wavelength of this light?
c. If sodium is irradiated with light of 340 nm, what is the maximum possible
kinetic energy of the emitted electrons?
d. What is the maximum number of electrons that can be freed by a burst of light
whose total energy is 3.00 mJ?
Score: ___________________/24
Objective 7: Bohr’s Model & Matter Waves (3 points each)
1. For each of the following electronic transitions in the hydrogen atom, calculate the
energy, frequency, and wavelength of the associated radiation, and determine whether the
radiation is emitted or absorbed during the transition: (this is a 4 part answer for each
section)
a. From n=6 to n=2
Energy:
Frequency:
Wavelength:
Radiation emitted or absorbed?
2. Use the de Broglie relationship to determine the wavelengths of the following objects:
a. An 58 kg person skiing at 45 km/hr.
b. A lithium atom moving at 5.2 x 105 m/s.
Score: __________________/18
Objective 8: Distributed Practice:
1. Solid zinc metal is place into a solution of silver nitrate causing a single – replacement
reaction to occur.
a. Write the balanced equation.
b. If the mass of the zinc was 2.0 grams and it was placed into 2.50 grams of the
silver nitrate solution, how many grams of solid silver are formed?
c. How much excess reagent, in grams, is left over at the end of
this reaction?
2. A 7.0 Liter flask at 26 C contains 9.5 grams of sulfur dioxide and 12.0 grams
of chlorine gas.
a. What is the partial pressure of each gas contained in this flask? (answer in
atmospheres of pressure)
b. What is the total pressure in this flask?
3. How many kilojoules of heat are required to raise 60 grams of water from 15 °C
to 125 °C. The specific heats of ice, liquid water, and steam are 2.1 J/g-K, 4.184 J/gK, and 1.84 J/g-K respectively. The heat of fusion for water is 6.01 kJ/mol and
the heat of vaporization for water is 40.7 kJ/mol. DRAW A PHASE DIAGRAM!
SCORE: _________________________/45