VI. Assessment Write the longhand electron configuration, short-hand electron configuration for the following elements. a. Sulfur 16e- (longhand) = 1s2 2s2 2p6 3s2 3p4 S 16e- (shorthand) = 3s2 3p4 %3D b. Argon 18e- (longhand) = 1s2 2s2 2p6 3s2 3p6. %3D Ar 18e- (shorthand) = 3s2 3p6_ c. Calcium 20e- (longhand) = %3D Ca 20e- (shorthand) : %3D d. Potassium 19e- (longhand) K 19e- (shorthand) = e. Titanium 22e- (longhand) = Ti 22e- (shorthand) = %3D

VI. Assessment Write the longhand electron configuration, short-hand electron configuration for the following elements. a. Sulfur 16e- (longhand) = 1s2 2s2 2p6 3s2 3p4 S 16e- (shorthand) = 3s2 3p4 %3D b. Argon 18e- (longhand) = 1s2 2s2 2p6 3s2 3p6. %3D Ar 18e- (shorthand) = 3s2 3p6_ c. Calcium 20e- (longhand) = %3D Ca 20e- (shorthand) : %3D d. Potassium 19e- (longhand) K 19e- (shorthand) = e. Titanium 22e- (longhand) = Ti 22e- (shorthand) = %3D

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 12ALQ

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Similar questions

We can represent both probability and radial probability versus distance from the nucleus for a hydrogen ls orbital as depicted below. What does each graph tell us about the electron in a hydrogen 1s orbital?
The periodic table consists of four blocks of elements that correspond to s, p, d, and f orbitals being filled. After f orbitals come g and h orbitals In theory, if a g block and an h block of elements existed, bow long would the rows of g and h elements be in this theoretical periodic table?
Explain in your own words what is meant by (a) the Pauli exclusion principle. (b) Hund's rule. (c) a line in an atomic spectrum. (d) the principal quantum number.
The following are orbital diagrams for presumed ground-state atoms. Several, though, violate Paulis principle or Hunds rule Which of the these follow both Paulis principle and Hunds rule, and which violate one or the other (state whether Paulis principle or Hunds rule is violated)? a b c d e
Your text describes the probability map for an s orbital using an analogy to the earth’s atmosphere. Explain this analogy.
Is the following statement true or false? The hydrogen atom has a 3s orbital. Explain.
(a) The nitrogen atom has one electron in each of the 2px , 2py , and 2pz orbitals. By using the form of the angular wave functions, show that the total electron density, 2(2px)+2(2py)+2(2pz) , is spherically symmetric (that is, it is independent of the angles and ). The neon atom, which has two electrons in each 2p orbital, is also spherically symmetric. (b) The same result as in part (a) applies to d orbitals, thus a filled or half-filled subshell of d orbitals is spherically symmetric. Identify the spherically symmetric atoms or ions among the following: F , Na, Si, S2,Ar+ , Ni, Cu, Mo, Rh, Sb, W, Au.
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?
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)?

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