Chemistry I Semester 1 Review: Day 1Student name______

Study previous notes, labs, and assignments from this semester in addition to completing the practice questions on this Exam Review.

Unit 1 – Introduction and Atomic Structure

DIRECTIONS: Use your notes and text to complete the following review sheet.

  1. For the following scientists, describe their experiment, what the model of the atom was before their experiment and what the model of the atom was after their experiment.

Describe experiment and/or discovery / Model
Thomson
Rutherford
Bohr
Schrodinger
  1. Explain how electrons are arranged around the nucleus in the quantum mechanical/Schrodinger’s model of the atom
  1. Using the Bohr model,

a. Draw a model of a hydrogen atom showing the electron going from the ground state to an excited state. / b. Draw another hydrogen atom and show a larger electron jump. / c. Draw two more hydrogen atoms but show the electron falling a different distance in each atom. Be sure to include at least 3 energy levels.
  1. Where is energy being absorbed and where is energy released?
  1. Compare the amount of energy absorbed or released as well.
  1. Explain the evidence that Bohr used to justify his model of the atom
  1. Rank the colors of light from most energy to least energy (orange, blue, yellow, red, purple, green)
  1. Rank the colors from longest wavelength to shortest wavelength
  1. State the relationship between wavelength, energy and frequency of light
  1. Describe the difference between an atomic absorption spectrum and an atomic emission spectrum.

8. View the emission spectra. Which elements (A, B, and/or C) are present are in the unknown?

I I I I I I I
I I I
I I I
I I I I I I

A

B

C

unknown

9. Rubidium has two common isotopes, and . The abundance of is 72.2% and the abundance of is 27.8%. What is the average atomic mass of rubidium?

  1. Hydrogen has 3 naturally occurring isotopes: H-1, H-2, and H-3. Which isotope would you predict is the mostabundant on the earth?
  1. A student measures a small amount of steel wool on a balance and the mass is found to be 2.35 g. The student then predicts that if she burns the steel wool in the Bunsen burner and then finds the mass again the mass will be less. After she burns the steel wool in the flame the mass actually increases to 2.56 g. Her prediction was wrong. What happened? Where did this extra mass come from?
  1. What are the differences between nuclear reactions and chemical reactions.
  1. Compare the penetrating power of alpha, beta, and gamma radiation. What material stops the radiation?
  1. What are the pros and cons of using nuclear energy?
  1. Describe fission and fusion...including their difference.
  1. Complete the following reactions and identify the type of nuclear decay: (Alpha, Beta, or Positron decay)

______ + Type: ______

 + _____Type: ______

 + ______Type: ______

 ______+ Type: ______

_____  + Type: ______

 + ______Type: ______