The de Broglie wave equation showed that the wavelength of any moving

The de Broglie wave equation showed that the wavelength of any moving object is equal toa. hmb. hmc. hmd. mh2. One of the following statements will not be true if quantum mechanics are used in explanations of particlebehaviora. sub-atomic particles display quantum behaviorb. wave-particle duality must existc. some quantum behavior can be observed visuallyd. discrete energy levels must be shown3. True or False: The Bohr model of the electron clearly explained why atomic energy states were quantized.4. True or False: Electrons can only exist in an atom at specific energies.5. Acceptance of the _____ nature of the electron allowed a new way of understanding how electrons functioned.6. The Heisenberg Uncertainty Principal states that the _______ and __________ of a particle cannot be determinedsimultaneously.7. In an eight-ball pool game, the cue ball can travel 5m/sec. If the cue ball has a mass of 160 g, what is thewavelength it demonstrates?Lesson Objective: Explain the difference between quantum mechanics and classical mechanics.8. All of the following statements about classical mechanics are true except one.a. all objects move with wavelike motionb. objects gain or lose energy in any amountc. the materials demonstrate wave-particle dualityd. size and mass of objects obscures any quantum effects9. The Heisenberg Uncertainty Principle statesa. velocity and position can both be determined at the same timeb. a beam of light can interfere with the path and speed of an electronc. photons do not affect the position of an electrond. the velocity of a car cannot accurately be measured by a radar beam10. True or False: Particles described by quantum theory can only lose or gain energy in discrete units.11. True or False: The Heisenberg Uncertainty Principle says that we can never measure the position and velocityof the moon accurately.12. Particles whose motions are better described by quantum mechanics can only gain or lose energy in discreteunits called _________.13. The study of motion in large objects is called _______ _________ .Lesson Objective: Understand how the Heisenberg uncertainty principle and Schrdinger’s wave equationled to the idea of atomic orbitals.14. Which of the following statements about the Schrdinger wave equation is not true?a. the quantum mechanical model of the electron comes from this equationb. this equation supports the Bohr model of electron orbitsc. solutions to this equation are called wave functionsd. quantization of electron energies is required to solve the equation15. An electron clouda. represents a 50% probability of finding an electronb. has uniform densityc. can be called an orbitald. can only show where the electron is not located16. True or False: An orbital represents a three-dimensional area of space.17. True or False: Electrons travel around the nucleus in circular orbits.18. The electron cloud represents an area of space where there is a _____% probability of finding an electron.19. The ___________ wave equation accurately described the behavior of the electron in a hydrogen atom.Lesson Objective: Know the four quantum numbers and how they are related to the arrangement of electronsin an atom.20. Each electron can be described by ___________ quantum numbers.a. 4b. 3c. 2d. 121. The quantum numbers describe all the characteristics of an electron excepta. velocityb. magnetic spinc. energy leveld. orbital shape22. True or False: The principal quantum number describes the magnetic spin of an electron.23. True or False: The magnetic quantum number describes the orientation of an orbital.24. Each orbital can hold a maximum of ____ electrons.25. The possible values for the spin quantum number are ___ and ____ .Lesson Objective: Describe the interrelationships between principal energy level, sublevel, orbital and electronspin and how they relate to the number of electrons of an atom.26. One of the following is not an allowable sublevel for n = 3a. pb. dc. fd. s27. For n = 2, the number of orbitals per principal energy level isa. 3b. 6c. 1d. 228. True or False: The p orbitals are dumbbell-shaped.29. True or False: All s orbitals have complex shapes.30. The following image represents a _____ orbital.31.32. The total number of allowable orbitals for n = 4 is ________.33. The Heisenberg Uncertainty Principle states that it is impossible to determine simultaneously both the positionand the velocity of a particle. The detection of an electron, for example, would be made by way of itsinteraction with photons of light. Since photons and electrons have nearly the same energy, any attempt tolocate an electron with a photon will knock the electron off course, resulting in uncertainty about where theelectron is headed.34. A running back collides with a defensive tackle and is knocked down. Explain how the Heisenberg UncertaintyPrinciple applies to this situation.


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