pls make sure it’s correct b. 3s3. The orbital diagram to the right representsan electron configuration for:a.A transition metalAn alkali metalAn alkaline earth metalA lanthanideAn actinides nou jof. A non-metalนาน 101111.11 0.411110МИТНИ 3P13125P

The orbital diagram for a particular element represents the electron distribution and the electron…

3. The orbital diagram to the right represents an electron configuration for: A transition metal a. 4 An alkali metal An alkaline earth metal A lanthanide An actinide f. A non-metal Energy level 119% 11111 115 ИМИНИР 113 НИТИВ RAD 1311411 1125 P

3. The orbital diagram to the right represents an electron configuration for: A transition metal a. 4 An alkali metal An alkaline earth metal A lanthanide An actinide f. A non-metal Energy level 119% 11111 115 ИМИНИР 113 НИТИВ RAD 1311411 1125 P

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 115AP

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Similar questions

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?
What does wave-particle duality mean? What are its implications in our modem view of atomic structure?
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?
The work function is the energy required to remove an electron from an atom on the surface of a metal. How does this definition differ from that for ionization energy?
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.
Which atom would be expected to have a half-filled 4s subshell?
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.
Answer the following questions as a summary quiz on this chapter. (a) The quantum number n describes the ________ of an atomic orbital, and the quantum number describes its ________. (b) When n = 3, the possible values of are _________. (c) What type of orbital corresponds to = 3? ________ (d) For a 4d orbital, the value of n is _______, the value of is ________, and a possible value of m is _________. (e) Each of the following drawings represents a type of atomic orbital. Give the letter designation for the orbital, give its value of , and specify the number of planar nodes. Letter = ______ ______ value = ______ ______ Planar nodes = _______ ______ (f) An atomic orbital with three planar nodes through the nucleus is a(n) ______ orbital. (g) Which of the following orbitals cannot exist according to modem quantum theory: 2s, 3p, 2d, 3f, 5p, 6p? (h) Which of the following is not a valid set of quantum numbers? (i) What is the maximum number of orbitals that can be associated with each of the following sets of quantum numbers? (One possible answer is none. ) (i) n = 2 and =1 (ii) n = 3 (iii) n = 3 and = 3 (iv) n = 2, = 1, and m = 0
A given orbital has a magnetic quantum number of m = 1. This could not be a(n) (a) f orbital (b) d orbital (c) p orbital (d) s orbital
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the probability of finding an electron in that region?
Valence electrons are those electrons in the outermost principal quantum level (highest n level) of an atom in its ground state. Groups lA to 8A have from 1 to 8 valence electrons. For each group of the representative elements (1A-8A). give the number of valence electrons, the general valence electron configuration, a sample element in that group, and the specific valence electron configuration for that element.

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