(a) Explain why BrF4- is square planar, whereas BF4- is tetrahedral.(b) How would you expect the H¬X¬H bond angle tovary in the series H2O, H2S, H2Se? Explain. (Hint: The size ofan electron pair domain depends in part on the electronegativityof the central atom.)

(a) Explain why BrF4- is square planar, whereas BF4- is tetrahedral.(b) How would you expect the H¬X¬H bond angle tovary in the series H2O, H2S, H2Se? Explain. (Hint: The size ofan electron pair domain depends in part on the electronegativityof the central atom.)

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 3RQ: Describe the bonding in H2S, CH4, H2CO and HCN using the localized electron model.

See similar textbooks

Related questions

Q: The VSEPR model was developed before any xenon com-pounds had been prepared. Thus, these compounds…

A: The shapes of XeF₂, XeF₄, and XeF₆ has to be predicted.

Q: According to Huckel theory, what is the difference in total energy between the anion (C6H6) and the…

A: See below. In anion their is a 8 electron because in ring present 6 e- and 2come from anion. For…

Q: 1. The following are the two possible Lewis structures for C2H2F2. Will both have the same dipole…

A: Dipole moment is the multiplication of charge and distance

Q: The following is part of a molecular orbital energy-level diagramfor MOs constructed from 1s atomic…

A: The overlapping of two atomic orbitals having equivalent energy give rise to a hybrid orbital known…

Q: Construct the molecular orbital diagram for SrCl. Would yo u expect the bond length of SrCl+ to be…

A: We have been aaked to draw the molecular orbital of SrCl for which we need to know the atomic…

Q: provide the following information including the lewis structucre and 3D sketch for SeO3^2- and HNO3

A: Lewis dot structure is the structure that tells about the valence electrons of an atom in the…

Q: the

A: O2-1 is a superoxide ion it is formed from Oxygen gas. In the Oxygen gas ( O2 ) having two unpaired…

Q: With the help of the Lewis structure of XeF4, answer to the following questions. i) Calculate the…

Q: In contrast to the cyanate ion (NCO-), which is stable and found in many compounds, the fulminate…

A: In contrast to the cyanate ion (NCO-), which is stable and found in many compounds, the fulminate…

Q: For the carbonate ion, CO32-, draw all the resonanc structures. Identify which orbitals overlap to…

A: Resonance comes into play when it is possible to draw more than one Lewis structure of a given…

Q: The bond angles in the nitrite ion, nitrogen dioxide, and thenitronium ion (NO₂⁺) are 115°, 134°,…

A: The Lewis electron dot structure for given molecules are determined by first drawing the skeletal…

Q: (b) Arrange the following in decreasing order of bond length and bond angle with explanation C2H6,…

A: The given compounds have to be arranged in the order of decreasing bond length and bond angle,

Q: In the methoxide anion (CH3O-), is it possible for a double bond to exist between C and O, given…

Q: A 0.325 g sample of a gaseous hydrocarbon (compound containing carbon and hydrogen only) occupies a…

A: Given: The given mass of, (m)=0.325 g The volume ,(V)= 193 mL=0.193 L. The temperature,…

Q: Draw the Lewis structure for each of the following moleculesor ions, and predict their…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: 4. Describe the location of the maximumelectron density of o- and n-bonds. How is the difference in…

A: Sigma bonds They are the type of covalent bonds, which differ in the overlapping of atomic orbitals.…

Q: Predict, on the basis of valence bond theory, whether you would expect SO2 to be linear or bent.

A: The arrangement of atoms in a molecule have the tendency to minimize the repulsion between electron…

Q: It has been suggested that a compound of formulaC12B24N24 might exist and have a structure similar…

Q: (a) Write a single Lewis structure for SO3, and determine thehybridization at the S atom. (b) Are…

A: a.

Q: What are the SALCS made up ðf o oroltaIS nloved in forming P-F bonds in PF,?

A: Solution -

Q: Provide the hybridization for the following atoms in the compound below.

A: Since we know that hybridization is the phenomenon of intermixing of atomic orbital of atoms which…

Q: Xenon tetrafluoride reacts with antimony pentafluoride toform the following ionic complex:…

A: (a) Given that Xenon tetrafluoride reacts with antimony pentaflouride. The shape of Xenon…

Q: Defi ne bond dissociation energy and describe its relationship to bond strength.

A: Bond dissociation energy is the amount of energy needed to break a bond.

Q: Give the Lewis-structure of a molecule containing both a σp-p and a πp-p overlap of orbitals. Then…

A: given σp-p and πp-p overlap orbital we need to indicate the lweis structure σ and π bonds in the…

Q: Explain the followings for the anions present magnesiumfloride and sodiumperoxide. i) Molecular…

Q: 2p 2p 2s 2s 1s 1s Energía

Q: What is the molecular shape of SC3 ^6-?

A: The question is based on the concept of chemical bonding. we have to determine the molecular shape…

Q: Arrange the lollowing compounds in the increasing order of vc=c : Provide justification of the…

A: Absorption frequency of internal double bond in cyclic compound is very sensitive to ring size

Q: en trifluoride (NF3) consists of + sigma bonds and * pi bonds. Idehyde (OCH2) consists of A sigma…

A: A) NF3 has 3 sigma and 0 pi bond. B) it has 3 sigma and 1 pi bond.

Q: Q1- Define each of the following with examples: 1- Electronegativity 2- Isoelectronic 3- Electron…

A: Hello. Since your question has multiple parts, and each part has multiple sub-parts, we will solve…

Q: A substance has the molecular formula (d) C4H,N. Is there any likelihood that this material contains…

Q: (b) Arrange the following in decreasing order of bond length and bond angle with explanation C,H.…

A: given molecules are C2H6 = ethane C2H4 = ethene C2H2 = ethyne "Angle of molecules depends upon the…

Q: Which of the foriowing chemica bonds is considered to be polart L-Br NaF Seiect one O Nene of them…

A: Polar bond Polar bond is a bond which is formed by mutual sharing of electrons of atoms having…

Q: A) Explain why BrF4 with a negative charge on top is square planar, whereas BF4 with negative charge…

A: VSEPR theory: VSEPR theory means valence shell electron pair repulsion. Valence shell electrons are…

Q: Considerthese following ions: 02 -, N -, Li2 + and O -

A: Molecular orbital (MO) theory describes the behavior of electrons in a molecule in terms of…

Q: The compound SF3N has been synthesized.(a) Draw the Lewis diagram of this molecule, supposingthat…

A: (a)

Q: (C) Draw and label the molecular orbital energy diagram for SeBr- and populate it with electrons.

A: Molecular orbital energy level diagram is a tool which explains the chemical bonding in the…

Q: What is the central atom of SiSe2, how many lone pairs does it have, and how many single and double…

Q: The N20 molecule is linear and polar. a. On the basis of this experimental evidence, which…

A: N2O is a linear and polar molecule.

Q: Which hybirdization(s) can form sigma bonds?

A: The blending of two atomic orbitals with a similar vitality levels so as to shape deteriorated new…

Q: Considering the Method of Constructing Moleculor Orbitals from Lineor Combinations of Atomic…

Q: Write the electronic configuration of the molecular ion I2+, what is the bond order?

A: Step : 1 Write the electronic configuration of the molecular ion I2+, what is the bond…

Q: A benzene molecule can be modeled as six carbon atoms arrangedin a regular hexagon in a plane. At…

Q: For each of the following molecules: draw Lewis structures showing resonance structures and formal…

A: Lewis structure : Lewis dot structures maintaing octet rule is shown in image. Formal charge : It…

Q: All the following statements are true about sigma bond EXCE O The electron density is high in the…

A: Sigma bond : It is the strongest covalent bond formed by head on overlapping of atomic orbitals.

Q: From models of SF4, BrF3, and XeF4, deduce whether differentatom arrangements, called geometrical…

A: Molecular geometry is the 3-D representation of the molecule in space. As the Lewis model is not…

Q: Give the molecular geometry and total number of electron groups for XeF2

A: The electronic configuration of xenon is = [Kr] 4d¹⁰ 5s² 5p⁶ 6d0 When xenon forms a compound with…

Question

(a) Explain why BrF₄^- is square planar, whereas BF₄^- is tetrahedral.
(b) How would you expect the H¬X¬H bond angle to
vary in the series H₂O, H₂S, H₂Se? Explain. (Hint: The size of
an electron pair domain depends in part on the electronegativity
of the central atom.)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Quantum Mechanical Treatment of Molecular Orbital Theory

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Benzene is commonly regarded as a resonance hybrid ofthe two Kekule structures. but other possible structures canalso contribute. Draw three other structures in which thereare only covalent n bonds (al lowing for bonding betweensome non-adjacent C atoms) and two structures in whichthere is one ionic bond. Why may these structures be ignoredin simple descriptions of the molecule?
Is the electron density consistentwith equal contributions from the tworesonance structures for O3? Explain.
Describe the bonding in H2S, CH4, H2CO and HCN using the localized electron model.
The wavelength at which the O2 molecule most stronglyabsorbs light is approximately 145 nm. (a) In which regionof the electromagnetic spectrum does this light fall?(b) Would a photon whose wavelength is 145 nm haveenough energy to photodissociate O2 whose bond energy is495 kJ/mol? Would it have enough energy to photoionize O2?
5b) i) Discuss the bonding and extra.stability of benzene,ii) Using suitable examples, compare the reactivity of benzene and ethane,
The sulfate ion can be represented with four S—O bonds orwith two S—O and two S=O bonds. (a) Which representation is better from the stand point of formal charges? (b) What is theshape of the sulfate ion, and what hybrid orbitals of S are postu-lated for the σ bonding? (c) In view of the answer to part (b),what orbitals of S must be used for the π bonds? What orbitalsof O? (d) Draw a diagram to show how one atomic orbital fromS and one from O overlap to form a π bond.
Describe the lewis structure od H2SO4 and H2S4O6 and HNO3 in detail ?
High-resolution photoelectron spectroscopy has provided information on the energy levels and bond distance in the ion. Prepare a molecular orbital energy level diagram for this ion Ar2+. How would you expect the bond distance in to compare with 198.8 pm, the bond distance in Cl2
Draw the Lewis structure for each of the following moleculesor ions, and predict their electron-domain and moleculargeometries: (a) AsF3, (b) CH3+, (c) BrF3, (d) ClO3-, (e) XeF2,(f) BrO2-.
If an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? I know that group 3A atoms are elctron deficient, and that period 3 elements and below, except for group 3A elements like Aluminum, can expand their octet because of their available d-orbital, which may not be relevant to this problem. I don't understand this question, or why the answer would be 5A. Is it because 5A have odd valence electrons, and can form free radicals, like NO?
(a) Compare the bond enthalpies (Table 8.3) of the carbon–carbon single, double, and triple bonds to deduce an averageπ -bond contribution to the enthalpy. What fraction ofa single bond does this quantity represent? (b) Make a similarcomparison of nitrogen–nitrogen bonds. What do youobserve? (c) Write Lewis structures of N2H4, N2H2, and N2,and determine the hybridization around nitrogen in eachcase. (d) Propose a reason for the large difference in yourobservations of parts (a) and (b).
β-Carotene is the compound responsiblefor the orange color of carrots and is theprecursor to vitamin A. Judging from theLewis structure shown here, how many πbonds does β-carotene have?