This shows the in a It is to everythingDIRECTION: Read, and solve the in SHOW YOUR SOLUTIONCan you identify one Scientific ahilit..since it will describe the behavior of electrons and how is it distributed in an element.Let us answer the given problems below.1. List down the n, I, and ml for orbitals in the 4d subshell2. Give the n, I, and ml number of 3p subshell: DIRECTION: Read, in YOUR SOLUTION.1. What are the quantum numbers contained in the third energy level? (n = 3)· 2.Write the quantum numbers if the configuration is 4p°.ROCESSING QUESTION:w will I use the concept of Quantum Numbers to discover the new Scientific abilities I have developed?

Quantum number : n = principal quantum number l = angular momentum quantum number ml = magnetic…

Answered: an you identify one Scientific describe…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 30QAP: Consider the following representation of a set of p orbitals for an atom: mg...

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Similar questions

Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?
6.47 Depict two ways to place electrons in the 2p orbitals for a nitrogen atom. Which depiction is correct according to Hund’s rule?
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?
The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.
Consider the following representation of a set of p orbitals for an atom: mg src=Images/HTML_99425-11-30QAP_image001.jpg alt="" align="top"/> ich of the following statements is(are) true? The areas represented by the p orbitals are positively charged clouds with negatively charged electrons embedded within these clouds. The nucleus is located at the center point of each axis. The electrons move along the elliptical paths as indicated by the p orbitals above. The atom could not be hydrogen because its electron is found in the 1s orbital.
Consider the orbitals shown here in outline. (a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)? (b) How many orbitals of type (x) are found in a shell with n=2? How many of type (y)? How many of type (z)? (c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell with n=4, of an orbital of type (y) in a shell with n=2. Of an orbital of type (z) in a shell with n=3. (d) What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)? (e) What are the possible I and ml values for an orbital of type (x)? Of type (y)? Of type (z)?
The following questions use concepts from this and previous chapters. Why is the radius of Li+ so much smaller than the radius of Li? Why is the radius of F so much larger than the radius of F?
The first ionization energy of helium is 2370kJmol1 , the highest for any element. (a) Define ionization energy and discuss why for helium it should be so high. (b) Which element would you expect to have the highest second ionization energy? Why? (c) Suppose that you wished to ionize some helium by shining electromagnetic radiation on it. What is the maximum wavelength you could use?
Which atom would be expected to have a half-filled 4s subshell?
Without referring to your text, predict the trend of second ionization energies for the elements sodium through argon. Compare your answer with Table 2-5. Explain any differences.
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.

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