Chapter 3 and 4 review. 1. List the types of electromagnetic radiation in order from smallest to highest wavelength:
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1 Chapter 3 and 4 review Name 1. List the types of electromagnetic radiation in order from smallest to highest wavelength: 2. When placed in the above order, is the frequency increasing or decreasing? 3. When placed in the above order, is the energy increasing or decreasing? 4. Energy and frequency are proportional 5. Frequency and wavelength are proportional 6. Energy and wavelength are proportional 7. Answer the following questions regarding the Bohr model of the atom a. This model was trying to explain the bright line spectrum of which element? b. An electron in its lowest energy state is in the state c. The movement of an electron from the excited state back to the ground state is always accompanied by the emission of d. The picture below is the bright line spectrum of hydrogen, answer the following questions about it the wavelength range is listed below the picture: 300 nm A B C D E 700 nm i. Which line represents longest wavelength? The shortest? ii. Which line represents the lowest frequency? The highest? iii. Which line represents the greatest Energy difference between the excited and ground state? The least energy difference?
2 Use the following Choices to match the scientist to his/her contribution to atomic theory a. Dalton f.chadwick b. Democritus g. Thomson c. Proust h.rutherford d. Lavoisier i. Heisenberg e. Millikan 8.. Stated that an atom is the smallest particle of an element 9. Determined the mass of an electron 10. Law of Multiple Proportions 11. First to state that all things are composed of atoms 12. Gold Foil 13. Cathode ray is negatively charged 14. Law of Conservation of mass 15. proposed Plum pudding model 16. Refuted plum pudding model 17. Cannot know both the speed and location of an electron 18. The Moving paddlewheel showed that a cathode ray is made of particles 19. Law of Definite Composition 20. He used her experiments to discover neutrons 21. Stated that all atoms of an element are identical, but atoms of differe nt elements are different 22. The results of her experiments were used in the discovery of the neutron 23. The positive charges of an atom are clustered into a tiny, densely packed nucleus 24. Cathode rays are attracted to the positive pole of a magnet 25. Write the following laws: Conservation of mass Definite Composition Multiple Proportions 26. Write the names, masses and number of neutrons in the three isotopes of hydrogen
3 27. Fill in the following chart symbol Atomic Atomic Mass name number mass number protons neutrons electron Carbon-14 Mg +2 Br -1 Answer the following questions about Quantum Theory : 28. Fill in the following chart: Energy level (n) Total # sublevels (list them) # orbitals of electrons 29. Which is the next highest energy orbital after 5p? 30. Which element has an electron configuration of 1s 2 2s 2 2p 5? 31. An electron for which n=3 has more than an electron in which n=2
4 32. The third energy level of an atom with n=2 contains how many different sublevels 33. The diagonal arrow chart used to determine when electrons are placed into specific orbitals illustrates which law/principle 34. states that no 2 electrons in the same atom have the same 4 quantum numbers 35. states that for orbitals of equal energy, one electron must be placed into each before a second electron is placed into any of these orbitals. 36. An electron is in the 2s orbital: What is its principle quantum number : What is its second quantum number (l) 37. An orbital is where there is a high of finding an electron. 38. How many different s orbitals are there in an s sublevel? 39. How many different p orbitals are there in an p sublevel? 40. How many different d orbitals are there in an d sublevel? 41. How many different f orbitals are there in an f sublevel? 42. How many electrons fit in tan s sublevel? p? d? f? 43. How many total electrons fill in the 1 st energy level? 2 nd? 3 rd? 4 th? 44. What is the first energy level to have an f orbital? d? p? s? 45. Which orbital is filled before the 4f? after the 4f?
5 46. for helium, how does the electron configuration for all of the noble gases end? 47. Neon has the electron configuration 1s 2 2s 2 2p 6. What do the underlined numbers refer to: 1s 2 2s 2 2p 6 What do the letters refer to? What do the superscripts(exponents) refer to? 3. An element has two isotopes. One of its isotores has a mass of amu and a percent abundance of 69.17%. The other isotope has a percent abundance of % and a mass of amu What is the average atomic mass of this element? What is the identity of this element? 3. You are accidentally exposed to electromagnetic radiation with a wavelength of 535 nm. a. What is the frequency of this radiation? b. What is the energy of this radiation 4. Write the orbital notation for silicon: 5. Write the electron configuration notation for Br Write the shorthand notation for mercury:
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