Concept explainers
(a)
Interpretation:
Using VSEPR theory, the geometry of the hydronium ion
Concept Information:
The shape of a molecule is predicted using Lewis structure and VSEPR (valence-shell electron-pair repulsion) model.
The shape of the molecule depends on the number of electron domains available for the central atom of the molecule.
The VSEPR model predicts that because these electron domains repel one another, they will arrange themselves to be as far apart as possible, thus minimizing the repulsive interactions between them.
For a molecule of type
To Predict: The geometry of hydronium ion
(b)
Interpretation:
The reason why the species
Concept Information:
The shape of a molecule is predicted using Lewis structure and VSEPR (valence-shell electron-pair repulsion) model.
The shape of the molecule depends on the number of electron domains available for the central atom of the molecule.
The VSEPR model predicts that because these electron domains repel one another, they will arrange themselves to be as far apart as possible, thus minimizing the repulsive interactions between them.
For a molecule of type
To Explain: The reason why the species
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Chemistry: Atoms First
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- Both aluminum and iodine form chlorides, Al₂Cl₆ and I₂Cl₆ ,with “bridging” Cl atoms. The Lewis structures are (a) What is the formal charge on each atom? (b) Which of these molecules has a planar shape? Explain.arrow_forwardAcetylene (C2H2) and nitrogen (N2) both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) By referring 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 N2O5(g) and of acetylene to formCO2(g) and H2O(g). (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O5(g) 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(a) Determine the formal charge of oxygen in the following structure. If the atom is formally neutral, indicate a charge of zero. (b) Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge on O 0arrow_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_forwardEthylene, C₂H₄, and tetrafluoroethylene, C₂F₄, are used tomake the polymers polyethylene and polytetrafluoroethylene(Teflon), respectively.(a) Draw the Lewis structures for C₂H₄ and C₂F₄, and give theideal H-C-H and F-C-F bond angles.(b) The actual H-C-H and F-C-F bond angles are 117.4and 112.4, respectively. Explain these deviations.arrow_forward(a) Construct a Lewis structure for O2 in which each atomachieves an octet of electrons. (b) How many bondingelectrons are in the structure? (c) Would you expect theO¬O bond in O2 to be shorter or longer than the O¬Obond in compounds that contain an O¬O single bond?Explain.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning