NAME______

Electron Configurations

and

Periodic Trends

Chapter 13 and 14

Practice Test A

Objective 1: Summarize the development of atomic theory.

Identify the correct scientist to the clues as related to atomic theory history.

  1. Modern atomic theory that describes the electronic structure of the atom as the probability of finding electrons within certain regions of space.
  2. The atom was considered an indivisible mass.
  3. The discoverer of the electron, proposed the plum-pudding model.
  4. Electrons travel in definite orbits around the nucleus, similar to a solar system.
  5. Discover of the nucleus, showing that the atom’s mass is concentrated in a small, positively charged region.

Answers:

  1. ______
  1. ______
  1. ______
  1. ______
  1. ______

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. Silicon
  1. Nickel
  1. Strontium
  1. Sulfur
  1. Germanium

Score: ______/15

Objective 3: Using Kernel Structures, write the electron configuration and orbital diagrams for the following elements:

  1. Rhodium
  1. Mercury
  1. Iodine
  1. Barium
  1. Francium

Score: ______/15

Objective 4: Interpret group and periodic trends in atomic radii, ionic radii, ionization energies, and electronegativities.

  1. List the following in the correct order of decreasing atomic radius:

Mg, Na, P, Si, and Ar.

  1. Of the following atoms, which has the largest FIRST ionization energy?

I, O, C, P, Br

______

  1. Which of the following has the largest SECOND ionization energy?

P, Si, Al, Mg, Na

______

  1. Which ion has the largest radius?

Sodium Ion, Fluoride Ion, Potassium Ion, Bromide Ion, Chloride Ion

______

  1. Which element would have the highest electronegativity value?

Cs, Ge, Al, O, F

______

Score: ______/15

Objective 5: Radiant Energy (3 points each)

  1. What is the frequency of radiation that has a wavelength of 955 mm?
  1. What is the wavelength of radiation that has a frequency of 5.5 x 10 14 s-1?
  1. What is the frequency of radiation whose wavelength is 10.0 Angstroms?
  1. An argon ion laser emits light at 489 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 438 nm.
  1. Calculate the energy of a photon of frequency of 6.75 x 10 12 s-1.
  1. What wavelength of radiation do photons with 2.87 x 10-18 J of energy have?
  1. The energy from radiation can be used to cause the rupture of chemical bonds. A minimum energy of 941 kJ/mol is required to break the nitrogen-nitrogen bond in molecular nitrogen. What is the longest wavelength of radiation that possesses the necessary energy to break the bond? What type of electromagnetic radiation is this?
  1. It requires a photon with a minimum energy of 4.41 x 10-19 J to emit electrons from sodium metal.
  2. What is the minimum frequency of light necessary to emit electrons from sodium via the photoelectric effect?
  1. What is the wavelength of this light?
  1. If sodium is irradiated with light of 439 nm, what is the maximum possible kinetic energy of the emitted electrons?
  1. What is the maximum number of electrons that can be freed by a burst of light whose total energy is 1.00 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)
  2. From n=4 to n=1

Energy:

Frequency:

Wavelength:

Radiation emitted or absorbed?

  1. Use the de Broglie relationship to determine the wavelengths of the following objects:
  2. An 85 kg person skiing at 50 km/hr.
  1. A lithium atom moving at 2.5 x 105 m/s.

Score: ______/18

Objective 8: Distributed Practice:

1. The reaction of fluorine gas with ammonia gas produces dinitrogen tetrafluoride

gas and hydrogen fluoride gas.

  1. Write the balanced equation. (3 pts)
  1. How many liters of dinitrogen tetrafluoride gas can be produced from 15 grams of fluorine gas and 1.15 x 1022 molecules of ammonia gas? (7 points)
  1. How much excess reagent, in grams, is left over at the end of this reaction? (10 points)
  1. A 2.00 Liter flask at 27 C contains 4.40 grams of carbon dioxide and 2.00 grams of nitrogen gas.
  2. What is the partial pressure of each gas contained in this flask? (answer in atmospheres of pressure) (6 points)
  1. What is the total pressure in this flask? (4 points)
  1. How many kilojoules of heat are required to raise 40.0 grams of water from -12 C to 120 C The specific heats of ice, liquid water, and steam are 2.1 J/g-K, 4.184 J/g-K, 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! (15 points)

SCORE: ______/45 points

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