Rank the following series of molecules or ions in order of decreasing bond energy using their bond order to predict relative magnitude: fluorine: F2, oxygen: 02, nitrogen: N2 Rank from highest to lowest bond energy. To rank items as equivalent, overlap them. View Available Hint(s) Reset Help nitrogen fluorine охудen Lowest bond energy Highest bond energy The correct ranking cannot be determined.

Rank the following series of molecules or ions in order of decreasing bond energy using their bond order to predict relative magnitude: fluorine: F2, oxygen: 02, nitrogen: N2 Rank from highest to lowest bond energy. To rank items as equivalent, overlap them. View Available Hint(s) Reset Help nitrogen fluorine охудen Lowest bond energy Highest bond energy The correct ranking cannot be determined.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 99AP: A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and...

See similar textbooks

Similar questions

Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.
What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?
Based on the concept of formal charge, what is the central atom in (a) HCN (do not include H as a possibility)? b) NOCI (Cl is always a terminal atom)?
(a) Describe the molecule xenon trioxide, XeO3, usingfour possible Lewis structures, one each with zero, one,two, or three Xe¬O double bonds. (b) Do any of theseresonance structures satisfy the octet rule for every atomin the molecule? (c) Do any of the four Lewis structureshave multiple resonance structures? If so, how many resonancestructures do you find? (d) Which of the Lewisstructures in part (a) yields the most favorable formalcharges for the molecule?
Draw the Lewis structures for each of the following moleculesor ions. Identify instances where the octet rule is notobeyed; state which atom in each compound does not followthe octet rule; and state how many electrons surround theseatoms: (a) NO, (b) BF3, (c) ICl2-, (d) OPBr3 (the P is the centralatom), (e) XeF4.
Using Lewis symbols and Lewis structures, diagram the formationof SiCl4 from Si and Cl atoms, showing valence-shellelectrons. (a) How many valence electrons does Si have initially?(b) How many valence electrons does each Cl haveinitially? (c) How many valence electrons surround the Siin the SiCl4 molecule? (d) How many valence electrons surroundeach Cl in the SiCl4 molecule? (e) How many bondingpairs of electrons are in the SiCl4 molecule?
Calculate the bond energy per mole for breaking all the bonds of oxygen, O2? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HẢ ? kJ AHo; = 410.2 mol Submit Previous Answers X Incorrect; Try Again; One attempt remaining
The dipole moment (u) of HBr (a polar covalent molecule) is 0.824D (debye), and its percent ionic character is 12.2 %. Estimate the bond length of the H-Br bond in picometers. Note that . 1 D 3.34 x 10-30 Cm and in a bond with 100% ionic character, Q=1.6 x 10-19 C. Express your answer to two significant figures and include the appropriate units. View Available Hint(s) r = μA Value 6 O Units ? Inits input for part B
Without consulting tables of data, predict which specieshas the larger bond energy, H+2 or H2.
The CO32- ion has three resonance structures. Predict the molecular shape ofeach of the three resonance structures. What does this result tell you aboutthe importance of considering each resonance structure when determiningthe shape of a molecule?
Examples: Example: H▬N▬H HIN: Examples: :F Н lone pair : -bond pair (2 e-) single bond :F: Non-Polar 8+. H :F: H:Cl: HCl:o is better represented as closer to Cl due to its greater electronegativity. Thus, HCl contains a polar covalent bond. H :0: Polar lone pair 8- :S H -S= :0: 2 bond pairs (4 e-) double bond because the bond electrons are pulled F: Pola