Concept explainers
(a)
Interpretation:
The most likely charge for ion formed from
Concept Introduction:
The fundamental principles that are followed to write an electronic configuration include three rules as follows:
Electron in a
Hund’s rule suggests electrons are not allowed to be paired up until each degenerate set of orbital has got at least one electron.
Pauli Exclusion Principle states two electrons within the same orbital cannot possess same set for four possible quantum numbers.
In
The convention followed to remove or add electrons is electrons of largest principal quantum number are lost first. In case of subshells of the same
(b)
Interpretation:
The most likely charge for ion formed from
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The most likely charge for ion formed from
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The most likely charge for ion formed from
Concept Introduction:
Refer to part (a).
(e)
Interpretation:
The most likely charge for ion formed from
Concept Introduction:
Refer to part (a).
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Chemical Principles: The Quest for Insight
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- (c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F. 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smalleor going down the halogen group from HF to HI Describe these observationsarrow_forwardDraw Lewis electron dot diagrams for the following species: (a) methane; (b) carbon dioxide; (c) phosphorus trichloride; (d) perchlorate ionarrow_forwardWrite the Lewis symbol for atoms of each of the following elements:(a) Al, (b) Br, (c) Ar, (d) Sr.arrow_forward
- 3. By means of Lewis structures, represent bonding between the following pairs of elements (Your structures should show whether the bonding is essentially ionic or covalent): (a) Cs and Br (b) H and Sb (c) B and Cl (d) Cs and Cl (e) Li and 0 (f) Cl and Iarrow_forwardFor many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains 77.55% Xe and 22.45% F by mass.(a) What is the formula of the compound?(b) Write a Lewis structure for the compound.(c) Predict the shape of the molecules of the compound.(d) What hybridization is consistent with the shape you predicted?arrow_forwardUse Lewis electron-dot symbols to represent the formationof (a) BrF₃ from bromine and fluorine atoms; (b) AlF₃ from alu-minum and fluorine atoms.arrow_forward
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- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning