In which of these molecules or ions do es the presence ofnonbonding electron pairs produce an effect on molecularshape? (a) SiH4, (b) PF3, (c) HBr, (d) HCN, (e) SO2.f tho fallorr:-

In VSEPR theory, both the lone pair and the bonded pair are together considered as electron domain…

Answered: In which of these molecules or ions do…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 16QRT

See similar textbooks

Similar questions

10. The following Lewis structures for (a) HCN, (b) C3H;, (c) SnOz, (d) BF3, (e)HOF are incorrect. Explain what is wrong with each one and give a correct structure for the molecule. (Relative positions of atoms are shown correctly.) (a) H-ëN (b) HCC-H (c) 0-Sn-0 (d) :F B :F: (e) H-O-F:
Thionyl chloride (SOCl₂) is a sulfur oxohalide used indus-trially to dehydrate metal halide hydrates. (a) Write a balancedequation for its reaction with magnesium chloride hexahydrate,in which SO₂ and HCl form along with the metal halide. (b) Drawa Lewis structure of SOCl₂ with minimal formal charges.
By referring only to the periodic table, select (a) the most electronegativeelement in group 6A; (b) the least electronegativeelement in the group Al, Si, P; (c) the most electronegative elementin the group Ga, P, Cl, Na; (d) the element in the group K,C, Zn, F that is most likely to form an ionic compound with Ba.
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.
The bond between carbon and hydrogen is one of the most important typesof bonds in chemistry. The length of an H¬C bond is approximately 1.1 Å.Based on this distance and differences in electronegativity, do you expect thedipole moment of an individual H¬C bond to be larger or smaller than that ofan H¬I bond?
Which of the following bonds is the most polar (a) H¬F (b) H¬I (c) Se¬F (d) N¬P (e) Ga¬C?
Which substance in each of the following pairs would you expect to have the higher boiling point? (a) Ne or Xe, (b) CO, or CSz, (e) CH4 or C, (d) Fz or LiF, (e) NH; or PH, O (a) Xe; (b) CS2: (e) Cl; (d) F2; (e) NH3 O (a) Xe; (b) CS;; (c) Ch; (d) LiF; (e) PH3 O (a) Xe; (b) CS2; (c) Ch; (d) LiF; (e) NH3 O (a) Ne; (b) CS2; (c) CH; (d) F2; (e) NH3 O (a) Xe; (b) CO2: (e) CH4: (d) LiF: (e) PH3
From 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.
For the Lewis structure of C2O42-, are the C --> O bonds the same strengths or different strengths? I calculated the bond strength as being 7/5 or 1.4, all the same, but not sure.
The percent ionic character of the bonds in several interhalogen Molecules (as estimated from their measured dipole moments and bond lengths) are ClF (11%), BrF(15%), BrCl (5.6%), ICl(5.8%), and IBr (10%). Estimate the percent ionic characters for each of these molecules, using the equation in Problem 37, and compare them with the given values.
The bond energy for a CH bond is about 413 kJ/mol in CH4 but 380 kJ/mol in CHBr3. Although these values are relatively close in magnitude, they are different. Explain why they are different. Does the fact that the bond energy is lower in CHBr3, make any sense? Why?
9. The following figure shows the potential energy as a function of the distance between two hydrogen atoms. (a) Label the axes (include reasonable units!) and indicate the equilibrium bond distance. (b) What is the energy when the atoms are infinitely far apart? (c) On the same plot, sketch what you think the potential energy of the anion H; might look like. Consider where you would put the equilibrium bond distance and how deep the potential energy dips down.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

In which of these molecules or ions do es the presence of nonbonding electron pairs produce an effect on molecular shape? (a) SiH4, (b) PF3, (c) HBr, (d) HCN, (e) SO2. f tho fallorr:-