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1. The element X has three naturally occurring isotopes, 24X, 25X, and 2%X. Isotope 24X Isotopic mass, amu Relative abundance (%) 78.99 10.00 23.985042 25X 24.985837 26X 25.982593 11.01 Calculate average atomic mass of element X.

1. The element X has three naturally occurring isotopes, 24X, 25X, and 2%X. Isotope 24X Isotopic mass, amu Relative abundance (%) 78.99 10.00 23.985042 25X 24.985837 26X 25.982593 11.01 Calculate average atomic mass of element X.

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter5: Stoichiometry
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1. The element X has three naturally occurring isotopes, 24X, 25X, and 26X. Isotope Isotopic mass, amu Relative abundance (%) 24X 23.985042 78.99 25X 24.985837 10.00 | 26X 25.982593 11.01 Calculate average atomic mass of element X. 2. The yellow light given off by a sodium vapour lamp used for public lighting has a wavelength of 589 nm. What is the frequency and energy of this radiation? 3. Consider a transition of the electron in the hydrogen atom from n= 6 to the n = 3. a. Determine the wavelength (in nm and m) of light associated with this transition? b. What is the energy associated with this transition? c. Will the light be absorbed or emitted? 4. An electron falls to the n= 2 energy level (nr= 2) during a transition in a hydrogen atom. The wavelength of this visible radiation is 656.3 nm. Calculate the energy level that the electron fell from (ni). 5. Give the allowable combinations of quantum numbers for each of the following electrons: a. a 3s electron b. a 4d electron с. а 5pelectron 6. What type of orbital is designated by combination given below: n = 4, 1= 3 a. b. n=3,1=0 с. n=2,1=2 7. For n = 3, what are the possible values of m. For 1=3, what are the possible values of m. 8. Write the electronic configuration for the following a. S in NazSO4 b. Cr in NazCrO4 c. Mn in KMNO4 d. O in H2O2 9. Arrange the following ions in order of increasing size: Sr²“, Rb“, Se², As², Br. Give reasons for your order of arrangement. 10. With the aid of orbital filling diagrams, explain why electron affinity of C is more negative than N? 11. Explain with the aid of orbital diagrams why the first ionization energy of magnesium is greater than that of aluminum and sulfur is less than that of phosphorous.
Transcribed Image Text:1. The element X has three naturally occurring isotopes, 24X, 25X, and 26X. Isotope Isotopic mass, amu Relative abundance (%) 24X 23.985042 78.99 25X 24.985837 10.00 | 26X 25.982593 11.01 Calculate average atomic mass of element X. 2. The yellow light given off by a sodium vapour lamp used for public lighting has a wavelength of 589 nm. What is the frequency and energy of this radiation? 3. Consider a transition of the electron in the hydrogen atom from n= 6 to the n = 3. a. Determine the wavelength (in nm and m) of light associated with this transition? b. What is the energy associated with this transition? c. Will the light be absorbed or emitted? 4. An electron falls to the n= 2 energy level (nr= 2) during a transition in a hydrogen atom. The wavelength of this visible radiation is 656.3 nm. Calculate the energy level that the electron fell from (ni). 5. Give the allowable combinations of quantum numbers for each of the following electrons: a. a 3s electron b. a 4d electron с. а 5pelectron 6. What type of orbital is designated by combination given below: n = 4, 1= 3 a. b. n=3,1=0 с. n=2,1=2 7. For n = 3, what are the possible values of m. For 1=3, what are the possible values of m. 8. Write the electronic configuration for the following a. S in NazSO4 b. Cr in NazCrO4 c. Mn in KMNO4 d. O in H2O2 9. Arrange the following ions in order of increasing size: Sr²“, Rb“, Se², As², Br. Give reasons for your order of arrangement. 10. With the aid of orbital filling diagrams, explain why electron affinity of C is more negative than N? 11. Explain with the aid of orbital diagrams why the first ionization energy of magnesium is greater than that of aluminum and sulfur is less than that of phosphorous.
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