(a)
Interpretation:
The bond length of
Concept Introduction:
The dissociation energy is a parameter that allows one to estimate the strength of bond formed. It is essentially the energy required to cleave and separate two atoms. It varies with several factors such as size, multiplicity, and number of unshared electron pairs. If the size of atoms is large bond strength is weak, consequently bond length is more compared to bond formed between smaller atoms. If bond is higher-order as in case of double or triple
(b)
Interpretation:
The bond length of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The bond length of
Concept Introduction:
Refer to part (a).
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Chapter 2 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM
- Like several other bonds, carbon-oxygen bonds havelengths and strengths that depend on the bond order. Draw Lewis structures for the following species, and arrange them in order of increasing carbon-oxygen bond length and then by increasing carbon-oxygen bond strength: (a) CO; (b) CO₃²⁻; (c) H₂CO;(d) CH₄O; (e) HCO₃(H attached to O).arrow_forwardNitrogen trifluoride (NF3) is used in the electronics industry to clean surfaces. NF3 is also a potent greenhouse gas. (A) Draw the Lewis structure of NF3 and determine its molecular geometry. (B) BF3 and NF3 both have three covalently bonded fluorine atoms around a central atom. Do they have the same dipole moment? (C) Could BF3 also behave as a greenhouse gas? Explain why or why not.arrow_forwardWrite Lewis structures for the following: (c) C2F6 (contains a C¬C bond), (d) AsO3 3 -, (e) H2SO3 (H is bonded to O), (f) NH2Cl.. Arrange the bonds in each of the following sets in order of increasing polarity: (a) C¬F, O¬F, Be¬F; (b) O¬Cl, S¬Br, C¬P; (c) C¬S, B¬F, N¬O. What is the Lewis symbol for each of the following atoms or ions? (a) K, (b) As, (c) Sn2 + , (d) N3 Write electron configurations for the following ions and determine which have noble-gas configurations: (a) Cd2+, (b) P3-, (c) Zr4+arrow_forward
- (a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forward1. Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central atom. (a) POF3 (b) XeO₂F3+ (c) BrCl₂ (d) N3 (the central atom is N; two other N's are bonded to it) (e) PF3arrow_forward. Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?arrow_forward
- a) Methane 1CH42 and the perchlorate ion 1ClO4- 2 are both described as tetrahedral. What does this indicate about their bond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forwardFrom their Lewis structures, determine the number of sand π bonds in each of the following molecules or ions:(a) CO2; (b) cyanogen,(CN2); (c) formaldehyde, H2CO;(d) formic acid, HCOOH, which has one H and two O atomsattached to C.arrow_forward(a) Find the angle u between adjacent nearest-neighbor bonds in the silicon lattice. Recall that each silicon atom is bonded to four of its nearest neighbors.The four neighbors form a regular tetrahedron— a pyramid whose sides and base are equilateral triangles. (b) Find the bond length, given that the atoms at the corners of the tetrahedron are 388 pm apart.arrow_forward
- (a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe—O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in (a) yields the most favorable formal charges for the molecule?arrow_forwardConsider the following molecular shapes:a) Match each shape with one of the following species: XeF₃,SbBr₃, GaCl₃. (b) Which, if any, is polar? (c) Which has the most valence electrons around the cental atom?arrow_forward(b) The Murchison meteorite that landed in Australia in 1969 contained 92 different amino acids, including 21 found in Earth organism A skeleton structure (single bond only) of one of these extraterrestrial amino acids is shown below. Draw a Lewis structure, and identify any atoms having a nonzero formal charge. H3N. C ČH2 ČH3 (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 smaller going down the halogen group from HF to HI Describe these observationsarrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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