[2] Answer the next five questions using the subshell notation: 5d 1) How many atomic orbitals are found in this subshell? 2) What are the possible values for the spin quantum numbers for this subshell? 3) What is the value of the principle quantum number? 4) How many electrons can be placed in this subshell? 5) What is the shape of an atomic orbital that belongs to this subshell?

[2] Answer the next five questions using the subshell notation: 5d 1) How many atomic orbitals are found in this subshell? 2) What are the possible values for the spin quantum numbers for this subshell? 3) What is the value of the principle quantum number? 4) How many electrons can be placed in this subshell? 5) What is the shape of an atomic orbital that belongs to this subshell?

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter6: The Structure Of Atoms

Section: Chapter Questions

Problem 67GQ: Answer the following questions as a summary quiz on the chapter. (a) The quantum number n describes...

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2. How many orbitals are in the n = 4 shell? 1 4 9 16
What is the maximum number of electrons that can occupy a f subshell (l = 3)?
Give electron configurations according to the Bohr model for each of the following elements. Try to not use Figure 3.11, but instead determine the configuration based on your knowledge of the number of electrons in each atom and the maximum number of electrons in each Bohr orbit. Indicate which of these elements you expect to be the most reactive and the least reactive. a. B b. Si c. Ca d. F e. Ar
How many unpaired electrons are there in an atom of (a) phosphorus? (b) potassium? (c) plutonium (Pu)?
The “Chemistry in Focus" segment Fireworks discusses some of the chemicals that give rise to the colors of fireworks. How do these colors support the existence of quantized energy levels in atoms?
Consider a 2+ ion that has six 3d electrons; which ion is it? Which 2+ ion would have only three 3d electrons?
Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
An excited atom can release some or all of its excess energy by emitting a(n) and thus move to a lower energy state.
Arrange these elements in order of increasing atomic size: Ca, Rb, P, Ge, Sr. (Try arranging these without looking at Figure 5.25 and then check yourself by looking up the necessary atomic radii.)
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?
How many electrons in an atom can have the following quantum designation? (a) 1s (b) 4d, m l =0(c) n=5,l=2
Which atom would be expected to have a half-filled 6p subshell?

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