(a)
Interpretation:
The electron configuration for elements with single unpaired electrons and with an
Concept Introduction:
The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of
Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:
Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.
(a)
Explanation of Solution
The electronic configuration for elements with an atomic number less than 10 is as follows:
According to Hund’s rule, initially each orbital is singly occupied and then pairing occurs in the filling of an electron in the same subshell.
Therefore, the single unpaired electrons are present in elements with atomic numbers 1, 3, 5, and 9.
(b)
Interpretation:
The electron configuration for the element with completely filled subshells and with an atomic number less than 10 has to be determined.
Concept Introduction:
Refer to part (a).
(b)
Explanation of Solution
The electronic configuration for elements with an atomic number less than 10 is as follows:
Therefore, the fulfilled subshell electron configuration is present in elements that have atomic numbers 2, 4, and 10.
(c)
Interpretation:
The electron configuration for elements with two unpaired electrons and with an atomic number less than 10 has to be determined.
Concept Introduction:
Refer to part (a).
(c)
Explanation of Solution
The electronic configuration for elements with an atomic number less than 10 is as follows:
According to Hund’s rule, initially each orbital is singly occupied and then pairing occurs in the filling of an electron in the same subshell.
Therefore, the two unpaired electrons are present in
Want to see more full solutions like this?
Chapter 7 Solutions
Chemistry
- In the second row of the periodic table, Be, N, and Ne all have positive (unfavorable) electron affinities, whereas the other second-row elements have negative (favorable) electron affinities. Rationalize why Be, N, and Ne have unfavorable electron affinities.arrow_forwardLight with a wavelength of 405 nm fell on a strontium surface, and electrons were ejected. If the speed of an ejected electron is 3.36 105 m/s, what energy was expended in removing the electron from the metal? Express the answer in joules (per electron) and in kilojoules per mole (of electrons).arrow_forwardThe energy emitted when an electron moves from a higher energy state to a lower energy state in any atom can be observed as electromagnetic radiation. (a) Which involves the emission of less energy in the H atom, an electron moving from n = 4 to n = 2 or an electron moving from n = 3 to n = 2? (b) Which involves the emission of more energy in the H atom, an electron moving from n = 4 to n = 1 or an electron moving from n = 5 to n = 2? Explain fully.arrow_forward
- Give the possible values of a. the principal quantum number, b. the angular momentum quantum number, c. the magnetic quantum number, and d. the spin quantum number.arrow_forwardA bright violet line occurs at 435.8 nm in the emission spectrum of mercury vapor. What amount of energy, in joules, must be released by an electron in a mercury atom to produce a photon of this light?arrow_forwardWhich of the following statements is (are) true? I. The product of wavelength and frequency of light is a constant. II. As the energy of electromagnetic radiation increases, its frequency decreases. III. As the wavelength of light increases, its frequency increases. a I only b II only c III only d I and III only e II and III onlyarrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning