Concept explainers
(a)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(b)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(c)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(d)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(e)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(f)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(g)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(h)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(i)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
(j)
Interpretation:
Lewis dot symbol for
Concept Introduction:
Lewis dot symbol represents the number of valence electrons of an atom or constituent atoms bonded in a molecule. Each dot corresponds to one electron.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Chemistry
- (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 compounds: CaCl 2 , CaI 2 , and MgCl 2 . Answer the following questions based on expected periodic trends: (a) Which is expected to have t he shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forwardA resident expert on electronegativity comes up to visit with you. He makes two claims (seen below) about electronegativity with relation to covalent bonding. Is the expert correct or can you refute him with your knowledge of electronegativity? (a) If a diatomic molecule is made up of atoms X and Y, which have different electronegativities, the molecule must be polar. (b) The farther two atoms are apart in a bond, the larger the dipole moment will be.arrow_forward
- One of the following pictures(Figure 1) represents NaCl and one represents MgO. Which is which? (a) is NaCl and (b) is MgO (b) is NaCl and (a) is MgO Which has the larger lattice energy? NaCl MgOarrow_forwardNa+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (The ionic compound as a whole, not just OCN-) (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forwardWrite the Lewis symbol for atoms of each of the following elements: a) Te, b) Si, c) Kr, d) P.arrow_forward
- Write Lewis dot symbols for (a) Ca2+, (b) N3−, and (c) I −.arrow_forwardIn each case, tell whether the bond is ionic, polar cova- lent, or nonpolar covalent. (a) Br, (e) SiH, (d) SrF, (c) HCl (g) N, (b) BrCl 2 (f) CO (h) CsCl 4.arrow_forwardConsider the formate ion, HCO2", which is the anion formed when formic acid loses an H* ion. The H and the two O atoms are bonded to the central C atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? Explain briefly (c) Would you predict that the C-O bond lengths in the formate ion would be longer or shorter relative to those in CO2? Explain brieflyarrow_forward
- Na+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forward(a) The 03 molecule has a central oxygen atom bonded to two outer oxygen atoms that are another. In the box below, draw the Lewis electron-dot diagram of the 03 molecule. Include all valid resonance structures. 0 - 0 = 0 (b) Based on the diagram you drew in part (a), what is the shape of the ozone molecule? and trigonal Bent Ozone decomposes according to the reaction represented below. 2 03(g) → 3 0₂(8) (c) The bond enthalpy of the oxygen-oxygen bond in O₂ is 498 kJ/mol. Based on the enthalpy of the reaction represented above, what is the average bond enthalpy, in kJ/mol, of an oxygen-oxygen bond in 03 ? Ozone can oxidize HSO3(aq), as represented by the equation below. [0] 1.0 x 10-5. <-> 00: HSO3(aq) + O3(aq) → HSO4 (aq) + O₂(8) A solution is prepared in which the initial concentration of HSO₂ (aq) (6.4 × 10+ M) is much larger than that of O3(aq) (1.0 × 10-5 M). The concentration of O3(aq) is monitored as the reaction proceeds, and the data are plotted in the graph below. 8.0 x…arrow_forwardIn which of the following compounds does hydrogen bear a partial negative charge: (a) CH4, (b) NH3, (c) H2O, (d) SiH4 or (e) H2S?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY