Concept explainers
(a)
Interpretation:
Lewis structure for
Concept Introduction:
Lewis structures are diagrams that represent the
Electron geometry is the shape of a molecule predicted by considering both bond electron pairs and lone pair of electrons.
Molecular geometry is the shape of a molecule predicted by considering only bond pair of electrons
Geometry of different type of molecules with respect to the number of electron pairs are mentioned below,
(b)
Interpretation:
Hybridisation of each carbon atom in
Concept Introduction:
Refer to (a).
(c)
Interpretation:
Whether croconate ion is planar or not has to be determined.
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OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
- (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_forwardConsider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.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_forward
- (a) Triazine, C3 H3 N3, is like benzene except that in triazineevery other C¬H group is replaced by a nitrogen atom.Draw the Lewis structure(s) for the triazine molecule. (b) Estimatethe carbon–nitrogen bond distances in the ring.arrow_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) 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
- Chloral (Cl₃C—CH=O) forms a monohydrate, chloralhydrate, the sleep-inducing depressant called “knockout drops”in old movies. (a) Write two possible structures for chloral hy-drate, one involving hydrogen bonding and one that is a Lewis adduct. (b) What spectroscopic method could be used to identify the real structure? Explain.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_forwardWe have just arrived at a bonding description for the formaldehydemolecule. Which of the following statements about themolecule is or are true?(i) Two of the electrons in the molecule are used to make the pbond in the molecule.(ii) Six of the electrons in the molecule are used to make the sbonds in the molecule.(iii) The C¬O bond length in formaldehyde should be shorterthan that in methanol, H3COH.(a) Only one of the statements is true.(b) Statements (i) and (ii) are true.(c) Statements (i) and (iii) are true.(d) Statements (ii) and (iii) are true.(e) All three statements are true.arrow_forward
- Propylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is given. (a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make σ bonds in the molecule? (c) How many valenceelectrons are used to make π bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?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_forwardAcetylene 1C2H22 and nitrogen 1N22 both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) Byreferring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O51g2 and of acetylene to formCO21g2 and H2O1g2. (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O51g2 is 11.30 kJ>mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning