(a)
Interpretation:
The expected ground-state electron configuration in
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 expected ground-state electron configuration of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The expected ground-state electron configuration of
Concept Introduction:
Refer to part (a).
(b)
Interpretation:
The expected ground-state electron configuration of
Concept Introduction:
Refer to part (a).
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Chemical Principles: The Quest for Insight
- (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 a Lewis electron-dot symbol for (a) As; (b) Se; (c) Ga.arrow_forwardDefine the following phenomena with reference to main group compounds: (d) multicenter electron deficient bondingarrow_forward
- Write condensed electron configurations for the following: (a) Zr; (b) V3+; (c) Mo3+.arrow_forwardChemical species are said to be isoelectronic if they have the same Lewis structure (regardless of charge). Consider these ions and write a Lewis structure for a neutral molecule that is isoelectronic with them. (a) CN–, (b) NH4+ (c) CO3 2–arrow_forwardConsider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule?arrow_forward
- Consider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule? [Section 7.3]arrow_forward(b) List some properties of Group 1 elements which indicate they are all metals. (c) What valence do all Group 1 elements exhibit in their compounds? (a) Write the names and symbols of the elements of Group 2.arrow_forwardCyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forward
- If an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? I know that group 3A atoms are elctron deficient, and that period 3 elements and below, except for group 3A elements like Aluminum, can expand their octet because of their available d-orbital, which may not be relevant to this problem. I don't understand this question, or why the answer would be 5A. Is it because 5A have odd valence electrons, and can form free radicals, like NO?arrow_forward8D.4. Benzene, a common solvent, is a covalent molecular compound which contains only carbon and hydrogen. Its simplest (empirical) formula is CH, and its molecular weight is 78 g/mol to 2 significant digits. What is its molecular formula? 8D.5. Draw the Lewis Dot Structure of (a) phosphorus pentafluoride. What is the formal charge on all atoms? (b) the perchlorate ion- in this case expand the octet for the chlorine atom in order to optimize the formal charges.arrow_forwardIn addition to ammonia, nitrogen forms three other hy-drides: hydrazine (N₂H₄), diazene (N₂H₂), and tetrazene (N₄H₄).(a) Use Lewis structures to compare the strength, length, and or-der of nitrogen-nitrogen bonds in hydrazine, diazene, and N₂.(b) Tetrazene (atom sequence H₂NNNNH₂) decomposes above 0°C to hydrazine and nitrogen gas. Draw a Lewis structure fortetrazene, and calculate ΔH°ᵣₓₙ for this decomposition.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning