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Study guide for chapter 4 1. State the number of protons, electrons and neutrons in the 15 N3-. 7 2. The element vanadium has two isotopes, 50V and 51 V, and a relative atomic mass of 50.94. (5pts) a. Define the term isotope. b. State the number of protons, electrons and neutrons in 50V. c. State and explain which is the more abundant isotope. d. State the name and the number of the isotope relative to which all atomic masses are measured. 3. Describe and explain the operation of a mass spectrometer (5) a. State three factors that affect the degree of deflection of ions in a mass spectrometer b. Calculate the relative atomic mass of strontium to two decimal places from the following data. c. Isotope Percentage abundance Sr-84 .56 Sr 86 9.90 Sr-87 7.00 Sr-88 82.54 4. State a physical property that is different for isotopes of an element. 5. a. Chlorine exists as two isotopes, 35 Cl and 37Cl. The relative atomic mass of chlorine is 35.45. Calculate the percentage abundance of each isotope. 6. A sample of argon exists as a mixture of three isotopes. Calculate the relative abundance of argon. Isotope Ar-36 Ar-38 Ar-40 percent abundance .337 0.0630 99.6 7. State the number of electrons, protons and neutrons in the ion 56Fe. 8. Define the following terms 9. a. Atomic number b. Mass number c. Use the data below to calculate the relative molecular mass of thallium bromide, TiBr3, to two decimal places . Isotope 203 Tl 205 Tl 79 Br 81 Br Percentage abundance 29.52 70.48 50.69 49.31 10. In a sample of gallium, the percentage abundance of 69Ga is 60.4, and 71Ga is 39.6. Determine the relative mass of gallium. b. Describe the difference between a continuous spectrum and a line spectrum. c. On the diagram below draw four lines in the visible line spectrum of hydrogen. Explain how the formation of lines indicates the presence of energy levels. Low energy high energy 11.Which statement is correct about a line emission spectrum? a. b. c. d. Electrons absorb energy as they move from low to high energy levels. Electrons absorb energy as they move from high to low energy levels. Electrons release energy as they move from low to high energy levels. Electrons release energy as they move form high to low energy levels. 12.A sample of the element chromium contains four isotopes, as shown in the table below. Calculate the relative atomic mass of chromium in the sample, giving your answer to two decimal places. Isotope 50 Cr 52 Cr 53 Cr 54 Cr Percentage abundance 4.30 83.8 9.50 2.40 13. How many protons, neutrons and electrons are present in each atom of 31 P? 14.How many protons, neutrons and electrons are present in each atom of 19F? 15.Which statement is correct for the emission spectrum of the hydrogen atom? a. The lines converge at lower energies b. The lines are produced when electrons move from lower to higher energy levels c. The lines in the visible region involve electron transition into the energy level closest to the nucleus. d. The line corresponding to the greatest emission of energy is the ultraviolet region. 16.A certain sample of element Z contains 60% of 69Z and 40% of 71Z. What is the relative atomic mass of element Z in the sample 17.What is the difference between two neutral atoms represented by the symbols 59Co and 59 Ni? 27 28 15. How many electrons are there in on 24 Mg2+ ion? 12 18.Information is given about four different atoms. Which two atoms are isotopes Species W X Y Z Number of protons 9 11 12 13 Number of neutrons 10 12 12 14 Number of electrons 10 11 12 10 19.Tritium, 3 T, is an isotope of hydrogen. a. State the number and type of sub-atomic particles in a tritium atom and the location of each type. 20.Eelctrons are directed into an electric field form left to right as indicated by the arrow in the diagram below. Which path is most probable for these electrons? + 1 2 - 4 3 21.How many neutrons are there in the ion 18 O2-. 22.Which statements are correct for the emission spectrum of the hydrogen atom? I. The lines converge at lower energies II. Electron transitions to n=1 are responsible for lines in the UV region. III. Lines are produced when electrons move from higher to lower energy levels. 23.Which process is responsible for the lines in the visible emission spectrum of hydrogen b. The release of energy by the electron c. The release of energy by the excited nucleus d. The excitation of the electron e. The absorption of energy by the electron