86 96, What is the shape of the H;Te molecule?a. lincarb.c.trigonal planarbentd.tetrahedral

The shape of H2Te is the bent shape. option b is correct - bent Reason: because the two Hydrogen…

Answered: 86, What is the shape of the H;Te…

Science

Chemistry

86, What is the shape of the H;Te molecule? lincar c. trigona! planar a. b. bent d. tetrahedral

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 14Q: What modification to the molecular orbital model was made from the experimental evidence that B2 is...

See similar textbooks

Related questions

Q: 6) What is the electron group (EG) and molecular geometry (MG) of an ammonia molecule? A) (EG)…

A: "Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: The molecular structures of both the carbon dioxide and oxygen molecules are well explained by the…

A: Given: The molecular structures of both the carbon dioxide and oxygen molecules are well explained…

Q: ssome foievit DOLI sorie fele Uie 112.6 128.1 111.6 B-? A=?

Q: Explain why hydrogen bonding is more extensive in NH3, H20, and HF than it is in PH3, H2S, and HCl.

A: Hydrogen bonding results /depends on following factor The molecule should contain a electronegative…

Q: See image below....

A: Answer for the first sub-part: The central atom is xenon which contributes 8 electrons. Oxygen atom…

Q: a) Compare and contrast the three-dimensional structure of methane CH4 and ammonia NH3. b) How are…

A: The solution with explanation is given below:

Q: In a typical multiple bond, the o (sigma) bond results from the overlap of from overlap of orbitals…

A: Given Typical Multiple Bond Orbitals from sigma bond are formed = To be determined Orbitals from…

Q: What are the angles a and b in the actual molecule of which this is a Lewis structure? -C EN: Note…

A: In the given structure hybridization of carbon atom is sp and hybridization of O atom is sp3.

Q: The phosphate, use VSPER theory and bond theory to predict 1) orbital hybridization for Phosphorus…

Q: What is the hybridization of chlorine in each of the following: (a) ClO2; (b) ClO3-; (c) ClO4-?

A: The names of the given compounds are: ClO2 - Chlorine dioxide ClO3- - Chlorate ion ClO4- -…

Q: 25) Which of the following figure represents the formation of a o* antibonding molecular orbital? A)…

A: According to concept of Valence bond theory orbitals always overlap with each other when they have…

Q: B. Write the molecular geometry of the following two structures:

A: Molecular geometry is used to represent the molecule in the three-dimensions.

Q: 21) What's the molecualr shape of BCI3 A) trigonal planar B) bent C) linear

Q: hybrid

A: As per the generic Lewis structure, The total number of valence electrons = [Number of bonding…

Q: Elemental sulfur is a yellow solid that consists of S8 molecules. The structure of the S8 molecule…

A: Hey, since you have posted sub-part question, we would answer only first three sub-part. If your…

Q: Bonding and antibonding orbitals as explained in the Molecular Orbital theory of bonding.

Q: The hybridization of nitrogen in the sulfathiazole molecule is

A: We have to find the hybridization of nitrogen atom in the sulfathiazole molecule.

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

A: a.

Q: Consider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N…

A: (a) B in BF3 in SP2 hybridized and N in NH3 is SP3 hybridized.But after F3B -NH3 bonding…

Q: All of the molecules shown here have a tetrahedral geometry. For which molecule is the H-A-H bond…

Q: In molecular orbital theory, a molecular orbital that is lower in energy than the atomic orbitals…

Q: 29. If two sp? hybridized orbitals are going to overlap, what is the expected molecular geometry? A.…

A: Hybridization is process of mixing of atomic orbitals of different energy to give a new set of…

Q: According to Molecular Orbital Theory, the energy of Bonding Molecular Orbital (BMO) is: Equal to…

A: Molecular Orbital Theory was proposed by Hund and Mulliken According to this theory Linear…

Q: 1. A. What is an energy (electron or valence) shell and B. What determines whether it makes an atom…

Q: w. BClg has trigonal planar geometry

Q: Which of the following statement(s) is/are true? According to Molecular Orbital Theory, when two…

Q: Draw a Lewis structure for diimide, H-N=N-H, explain how the Lewis structure is drawn. Then, using…

Q: cO 2 Draw and identify depictions, including shapes and nodes, for atemic, hybrid, and molecular…

A: In NH3 central atom is nitrogen participate in SP3 hybridisation. Preparation of ammonia by Haber…

Q: 24) Predict the molecular geometry of SO3 molecule by VSEPR. A) trigonal planar B) bent C)…

A: VSEPR Theory ( Valence shell electron pair repulsion ) : Valence electron of central atom decide the…

Q: What is the electron pair geometry, lewis structure, molecular geometry, and hybridization of HF? Is…

Q: What is the molecular geometry of PHs? (A) Trigonal planar (B) T-shaped (C) Trigonal pyramidal (D)…

A: Molecular geometry tells about the arrangement of bond pairs and lone pairs of electrons in a…

Q: blltics, B... O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Identifying hybridization in a small…

Q: 20. According to the VSEPR theory, the geometry of the SO, molecule is A. pyramidal. B. distorted…

A: SO3 molecule has one sulfur atom and three oxygen atoms. S contributes 6 electrons. Every O atom…

Q: Specify the hybridization at the atoms labelled a-d. H H H -C a b c=C= -H- H H H. а. b. С. d.

A: these are single bond have sp3 hybridization double bond have sp2 hybridization, but in case of C,…

Q: Draw the Lewis structure for carbonyl fluoride, COF2. What are teh electron-pair geometry and…

Q: Describe the VSEPR Theory?

A: VSEPR theory or valence shell electron pair repulsion theory is a model that is used to predict the…

Q: In addition to Al₂Cl₆, aluminum forms other specieswith bridging halide ions to two aluminum atoms.…

A: Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Q: 83. Which of the following statement(s) concerning valence-bond theory and molecular orbital theory…

A: Valence bond theory describes a covalent bond as a result of the overlap of atomic orbitals,…

Q: Structure of the Bis-( dimethylglyoximato) nickel(II) (write the C.N , geometry type):

Q: Use VESPER theory to predict the shapes molecular iodine, tetramethylammonium iodide (both ions),…

A: Hybridization explains the overlapping of two atomic orbitals which gives the formation of new…

Q: What is the electron pair geometry, lewis structure, molecular geometry, and hybridization of NO? Is…

Q: What hybridization is required for central atoms that have a tetrahedral arrangement ofelectron…

A: The hybridization of the central atom can be related to the geometry of the structure.

Q: A) Explain the molecular orbital diagram of CO and O2 by dependent M.O theory and give the order…

Concept explainers

Stereochemistry and Isomerism

Stereochemistry deals with the three-dimensional structure and properties of molecules. It explains the arrangement of atoms and their manipulation within a molecule in a 3D structure. Stereochemistry can be dealt with all types of molecules. Based on the stereochemistry of a molecule, the physical and chemical properties of the molecules vary.

Question

96, What is the shape of the H;Te molecule?
a. lincar
b.
c.
trigonal planar
bent
d.
tetrahedral

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1- Concept

VIEW

Step 2- Final explanation

VIEW

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

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

Give the expected hybridization of the central atom for the molecules in Exercises 21 and 22.
Give the expected hybridization of the central atom for the molecules or ions in Exercises 81 and 87 from Chapter 3.
Sketch the molecular orbital and label its type ( or , bonding or antibonding) that would be formed when the following atomic orbitals overlap. Explain your labels. a. b. c. d.
Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals: a. Which is the bonding molecular orbital and which is the antibonding molecular orbital? Explain how you can tell by looking at their shapes. b. Which of the two molecular orbitals is lower in energy? Why is this true?
In addition to Al₂Cl₆, aluminum forms other specieswith bridging halide ions to two aluminum atoms. One suchspecies is the ion Al₂Cl₇. The ion is symmetrical, with a 180° Al−Cl−Al bond angle.(a) What orbitals does Al use to bond with the Cl atoms?(b) What is the shape around each Al?(c) What is the hybridization of the central Cl?(d) What do the shape and hybridization suggest about the pres-ence of lone pairs of electrons on the central Cl?
What is the hybrid orbital? What is the molecular arrangement? What is the shape?
Describe the bonding in NO+, NO, and NO, using both the localized electron and molecular orbital models. Account for any discrepancies between the two models.
In the hybrid orbital model, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.
Two variations of the octahedral geometry (see Table 4-1) are illustrated below. Which of the compounds/ions Br3, ClF3, XeF4, SF4, PF5, ClF5, and SF6 have these molecular structures?
What modification to the molecular orbital model was made from the experimental evidence that B2 is paramagnetic?
Give the Lewis structure, molecular structure, and hybridization of the oxygen atom for OF2. Would you expect OF2 to be a strong oxidizing agent like O2F2 discussed in Exercise 61?