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Chapter 13 – Review Electrons in Atoms

Chapter 13 – Review Electrons in Atoms. Milbank High School. Chapter 13 - Review. What scientist developed an atomic theory in the early 1800s? Who discovered the electron? How does the energy of an electron change when the electron moves closer to the nucleus?. Chapter 13 - Review.

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Chapter 13 – Review Electrons in Atoms

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  1. Chapter 13 – ReviewElectrons in Atoms Milbank High School

  2. Chapter 13 - Review • What scientist developed an atomic theory in the early 1800s? • Who discovered the electron? • How does the energy of an electron change when the electron moves closer to the nucleus?

  3. Chapter 13 - Review • What scientist developed the quantum mechanical model of the atom? • How many energy sublevels are there in the second principal energy level? • What is the maximum number of d orbitals in a principal energy level?

  4. Chapter 13 - Review • What is the maximum number of orbitals in the p sublevel? • What is the maximum number of electrons in the second principal energy level?

  5. Chapter 13 - Review • When an electron moves from a lower to a higher energy level, the electron ____ a quantum of energy. • What did Rutherford’s experiment demonstrate? • The quantum mechanical model exactly predicts which characteristic of electrons in an atom?

  6. Chapter 13 - Review • What is the probability of finding an electron within the region indicated by the drawn electron cloud? • What types of atomic orbitals are in the third principal energy level?

  7. Chapter 13 - Review • Which of the following energy levels has the lowest energy? 3d or 4s • If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?

  8. Chapter 13 - Review • What is the next atomic orbital in the series: 1s, 2s, 2p, 3s, 3p, _?_ • How many unpaired electrons are there in a sulfur atom? (atomic number =16)

  9. Chapter 13 - Review • What is the number of electrons in the outermost energy level of an oxygen atom? • How many half-filled orbitals are there in a bromine atom? • What is the electron configuration of potassium?

  10. Chapter 13 - Review • What statement says that no more than two electrons can occupy an atomic orbital, and that two electrons in the same orbital have opposite spins?

  11. Chapter 13 - Review • In order to occupy the same orbital, two electrons must have _____. • According to the Aufbau principle, electrons enter orbitals of _____ energy first.

  12. Chapter 13 - Review • Which of the following electron configurations is the most stable? 4d55s1 or 4d45s2 • Stable electron configurations are likely to contain _____.

  13. Chapter 13 - Review • Which color of visible light has the shortest wavelength? • What are quanta of light called? • Who predicted that all matter can behave as waves as well as particles?

  14. Chapter 13 - Review • The amplitude of a wave is the measure of the ______. • What is the wavelength of an electromagnetic wave that travels at 3 x 108 m/s and has a frequency of 60 Hz? • What is the approximate energy of a photon having a frequency of 4 x 107 Hz? (h = 6.6 x 10-34 J.s)

  15. Chapter 13 - Review • What is the approximate frequency of a photon having an energy of 5 x 10-24 J? (h = 6.6 x 10-34 J.s)

  16. Chapter 13 - Review • The lowest energy state of an atom is called the ______. • What is the approximate mass of a particle having a wavelength of 1 x 10-7 m, and a speed of 1 m/s? (h = 6.6 x 10-34 J.s)

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