Chemistry Chapter 5 WS #1 (first four pages)Complete the worksheet while viewing the power point. Use your textbook to answer remaining questions after the power point. Some information repeats itself. Consider this the important concepts in the chapter.Name of chapter:5.1 The Development of Atomic Models1. Rutherford’s atomic model could not explaina. why _________________________________give off characteristic colors when heatedb. why objects ___________________________ first glow dull red, then yellow, then white.c. his model could not explain ____________________________________.The Bohr Model2. Bohr proposed that an electron is found only in specific circular paths, or _________, aroundthe nucleus.3. Each possible electron orbit in Bohr’s model has a fixed energy called ____________.4. A quantum of energy is the amount of energy required to move an electron_______________________________________________________________________.The Quantum Mechanical Model5. Erwin Shrodinger used math to propose the ___________________________ model.6. The quantum mechanical model determines the allowed energies an electron can have and how likely it is ___________________________________________________________________________________________________________________________.Atomic Orbitals7. An _______________________ is often thought of as a region of space in which there is a high probability of finding an electron. The s orbitals are _____________ shaped, and p orbitals are __________________ shaped.5.2 Electron Configurations8. The ways in which electrons are arranged in various orbitals around the nuclei of atoms are called ________________________.9. Aufbau principle: electrons occupy the orbitals of _________ energy first.Pauli exclusion principle: an atomic orbital may describe at most ____________. To occupy the same orbital, two electrons must have ______________; that is, the electron spins must be paired. Hund’s rule: electrons occupy orbitals of the ______________ in a way that makes the number of electrons with the _____________ direction as large as possible.Some actual electron configurations differ from those assigned using the aufbau principle because __________sublevels are not as stable as _________ sublevels, but they are more stable than other configurations.Exceptions to the aufbau principle are due to ___________________________________ in orbitals with very similar energies.5.3 Physics and the Quantum Mechanical Model—Light10. The __________________ of a wave is the wave’s height from zero to the crest. The______________________, represented by _________, is the distance between the crests. The _________________, represented by _______, is the number of wave cycles to pass a given point per unit of time. The SI unit for cycles per second is the ___________. The speed of light is _________________. Draw a picture of a wave and label the parts.11. ___________________________________ include radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays.12. When sunlight passes through a prism, the different frequencies separate into a______________ of colors. The lowest frequency and longest wavelength is _____________. The other colors in order are _____________________________________________________. Atomic Spectra and Explanation of Atomic Spectra13. When atoms absorb energy, __________ move into higher energy levels. These electrons then lose energy by ________________ when they return to lower energy levels.14. The frequencies of light emitted by an element separate into discrete lines to give the_____________________ of the element.15. When the electron has its lowest possible energy, the atom is in its _______________.16. Excitation of the electron by absorbing energy raises the atom from the ground state to an______________.17. A quantum of energy in the form of light (photon) is emitted when the electron drops back toa ___________________.18. The light emitted by an electron moving from a higher to a lower energy level has a frequency __________ proportional to the energy change of the electron.Quantum Mechanics19. Einstein proposed that light could be described as quanta of energy called ______________. The quanta behave as if they were ____________________, resulting in a dual wave-particle behavior.20. In 1924, De Broglie developed an equation that predicts that all moving objects have___________________ behavior.21. The older theory of classical mechanics, adequately describes __________________________________________________________, while the newer theory of quantum mechanics describes ___________________________________________________________________. 22. The ___________________ uncertainty principle states that it is impossible to know exactly both the velocity and the position of a particle at the same time. The very act of measuring the position of an electron changes it velocity, and makes its velocity uncertain.Review…5.2 Electron Configurations (pages 133–135)1. The ways in which electrons are arranged around the nuclei of atoms arecalled ___________________________________________ .2. In the shorthand method for writing an electron configuration, what does asuperscript stand for? What do the sum of the superscripts equal?5.3 Light (pages 138–140)1. Match each term describing waves to its definition._______ amplitude a. the distance between two crests_______ wavelength b. the wave’s height from the origin to the crest_______ frequency c. the number of wave cycles to pass a given point per unit of time Atomic Spectra (page 141)4. What happens when an electric current is passed through the gas or vapor ofan element?5. Is the following sentence true or false? Explain. The emission spectrum of an elementcan be the same as the emission spectrum of another element.An Explanation of Atomic Spectra (pages 142–143)6. What is the lowest possible energy of an electron called?7. Only electrons moving from ______________________ to______________________ energy levels lose energy and emit light.WS #2 (last two pages)Chemistry—Ch. 5 textbook problems p. 149-151 (22-26, 30, 34-35, 40, 43, 61-65, 68)22. What was inadequate about Rutherford’s model of the atom? Which subatomic particles didThomson include in the plum-pudding model of the atom?23. What did Bohr assume about the motion of electrons?24. Describe Rutherford’s model of the atom and compare it with the model proposed by hisstudent Niels Bohr.25. What is the significance of the boundary of an electron cloud?26. What is an atomic orbital?30. How many electrons are in the highest occupied energy level of these atoms?c)barium b) sodium c) aluminum d) oxygen34. Give electron configurations for atoms of these elements:a) Na b) S c) Mgd) Ne e) K35. Which of these orbital designations are invalid?a)4s b) 2d c) 3f d) 3d40. List the colors of the visible spectrum in order of increasing wavelength.43. Explain the difference between the energy lost or gained by an atom according to the laws ofclassical physics and according to the quantum model of an atom.61. Pieces of energy are known asa) isotopes b) particles c) quanta d) line spectra62. The lowest sublevel in each principal energy level is represented by the symbola) f b) p c) s d) d63. Which electron transition results in the emission of energy?a)3p to 3s b) 3p to 4p c) 2s to 2p d) 1s to 2s64. Which is the ground state configuration of a magnesium atom?a) 1s22s22p63s2b) 1s22s22p63s1 c) 1s22s23s22p6 d) 1s22s22p43s265. Explain the difference between an orbit in the Bohr model and an orbital in the quantum mechanical model of the atom.68. Orbital diagrams for the ground states of two elements are shown below. Each diagramshows something that is incorrect. Identify the error in each diagram and then draw thecorrect diagram.a. Nitrogenb. MagnesiumCh. 4 review questions_______________ discovered the electron in 1897. He sealed gases in a tube and put electricity through the tube. The result was a glowing beam, or________________ ray. By using a magnet, he showed that there were tiny_______________ charged particles moving at high speeds (corpuscles or electrons). He found that the charge-to-mass ratio of electrons did not depend on the kind of gas used or type of metal plates. Thus, electrons must be part of the atoms of all elements.Thomson’s ___________________ model suggested that atoms were a_______________ mass with _______________ charged particles within similarto a plum pudding. His student, ___________________, disproved this theory by his ____________________ experiment. He found that most alpha particles went straight through showing that an atom is mostly _______________ space. He also concluded that there is a small, dense, positively charged _______________ at the center of the atom.Ch. 5 concept questionOuter _______________ gain a quantum of energy from high temperature or high _______________ and move from the ground state to an excited state. The_______________ are not stable in this higher energy level, so they emit energy called _______________ and move back to the lower energy, or ground state. We see colors because the energy emitted is in our _______________ spectrum, which is between ________ nm and __________nm. The colors in this spectrum from lowest energy are _________________________________________________________________________________________________________________.。
