ALEKS 360; 18WKS F/ GEN. CHEMISTRY >I<
13th Edition
ISBN: 9781264070077
Author: Chang
Publisher: INTER MCG
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Chapter 10, Problem 10.5QP
Interpretation Introduction
Interpretation:
The reason for a lone pair occupies an equatorial position rather than an axial position in the trigonal bipyramidal arrangement should be explained briefly.
Concept introduction:
- Valence Shell Electron Pair Repulsion (VSEPR) based on the repulsion between lone pairs and bond pairs of electron in the bonded atoms on the central atom or ion.
- There will be a deviation from the regular geometry of a molecule due to the electrostatic repulsion formed. So the bonded electrons tend to move away as far as possible so there is some deviation in regular geometry.
- So in VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom.
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Students have asked these similar questions
What is the molecular structure of a molecule that has a trigonal planar electron-pair geometry and one lone pair on the central atom?
Why double bonds and lone pairs cause deviations from ideal bond angles
Consider an iodine tetrafluoride cation (IF4+):
What is the elemental symbol of its central atom?
How many valence electrons does this molecule contain?
How many lone electron pairs surround the central atom?
How many regions of electron density surround the central atom?
For remaining items in this question, place the appropriate letter in the box:
What is the electron geometry of this molecule?
A = linear
B = trigonal planar
C = tetrahedral
D = trigonal bipyramidal
E = octahedral
What is the molecular shape of this molecule?
A = tetrahedral
B = trigonal pyramid
C = bent or angular
D = T-shape
E = Sawhorse or seesaw
Is this a polar molecule?
A = Yes
B = No
What is the hybridization of the central atom?
A = sp
B = sp2
C = sp3
D = sp3d
E = sp3d2
Chapter 10 Solutions
ALEKS 360; 18WKS F/ GEN. CHEMISTRY >I<
Ch. 10.1 - Use the VSEPR model to predict the geometry of (a)...Ch. 10.1 - What is the molecular geometry of GeCl4?Ch. 10.1 - What is the molecular geometry of BrO3?Ch. 10.1 - Which of the following geometries has a greater...Ch. 10.2 - Does the AlCl3 molecule have a dipole moment?Ch. 10.2 - Predict whether PF5 has a dipole moment.Ch. 10.2 - The molecule CF4 does not have a dipole moment...Ch. 10.2 - Carbon dioxide has a linear geometry and is...Ch. 10.3 - Compare the Lewis theory and the valence bond...Ch. 10.4 - Determine the hybridization state of the...
Ch. 10.4 - Describe the hybridization state of Se in SeF6.Ch. 10.4 - How many orbitals does a set of sp3d hybrid...Ch. 10.4 - What is the hybridization of P in PH4+?Ch. 10.4 - What is the hybridization of Xe in XeF4Ch. 10.5 - Describe the bonding in the hydrogen cyanide...Ch. 10.5 - How many pi bonds are present in CS2?Ch. 10.5 - Which of the following pairs of atomic orbitals on...Ch. 10.6 - One way to account for the fact that an O2...Ch. 10.7 - Which of the following species has a longer bond...Ch. 10.7 - Calculate the bond order of F2+.Ch. 10.7 - Determine if N2+ is diamagnetic or paramagnetic.Ch. 10.7 - Estimate the bond enthalpy (kJ/mol) of the H2+...Ch. 10.8 - Describe the bonding in the nitrate ion (NO3) in...Ch. 10 - How is the geometry of a molecule defined and why...Ch. 10 - Sketch the shape of a linear triatomic molecule, a...Ch. 10 - How many atoms are directly bonded to the central...Ch. 10 - Discuss the basic features of the VSEPR model....Ch. 10 - Prob. 10.5QPCh. 10 - Prob. 10.6QPCh. 10 - Predict the geometries of the following species...Ch. 10 - Predict the geometries of the following species:...Ch. 10 - Predict the geometry of the following molecules...Ch. 10 - Predict the geometry of the following molecules...Ch. 10 - Predict the geometry of the following molecules...Ch. 10 - Predict the geometries of the following ions: (a)...Ch. 10 - Describe the geometry around each of the three...Ch. 10 - Which of the following species are tetrahedral?...Ch. 10 - Prob. 10.15QPCh. 10 - Prob. 10.16QPCh. 10 - Prob. 10.17QPCh. 10 - The bonds in beryllium hydride (BeH2) molecules...Ch. 10 - Referring to Table 10.3, arrange the following...Ch. 10 - The dipole moments of the hydrogen halides...Ch. 10 - List the following molecules in order of...Ch. 10 - Does the molecule OCS have a higher or lower...Ch. 10 - Which of the molecules (a) or (b) has a higher...Ch. 10 - Prob. 10.24QPCh. 10 - What is valence bond theory? How does it differ...Ch. 10 - Use valence bond theory to explain the bonding in...Ch. 10 - Prob. 10.27QPCh. 10 - Prob. 10.28QPCh. 10 - Prob. 10.29QPCh. 10 - What is the angle between the following two hybrid...Ch. 10 - Describe the bonding scheme of the AsH3 molecule...Ch. 10 - What is the hybridization state of Si in SiH4 and...Ch. 10 - Describe the change in hybridization (if any) of...Ch. 10 - Consider the reaction BF3+NH3F3BNH3 Describe the...Ch. 10 - What hybrid orbitals are used by nitrogen atoms in...Ch. 10 - Prob. 10.36QPCh. 10 - Give the formula of a cation comprised of iodine...Ch. 10 - Give the formula of an anion comprised of iodine...Ch. 10 - How would you distinguish between a sigma bond and...Ch. 10 - What are the hybrid orbitals of the carbon atoms...Ch. 10 - Specify which hybrid orbitals are used by carbon...Ch. 10 - Prob. 10.42QPCh. 10 - The allene molecule H2CCCH2 is linear (the three C...Ch. 10 - How many pi bonds and sigma bonds are there in the...Ch. 10 - How many sigma bonds and pi bonds are there in...Ch. 10 - What is molecular orbital theory? How does it...Ch. 10 - Sketch the shapes of the following molecular...Ch. 10 - Explain the significance of bond order. Can bond...Ch. 10 - Explain in molecular orbital terms the changes in...Ch. 10 - The formation of H2 from two H atoms is an...Ch. 10 - Prob. 10.51QPCh. 10 - Arrange the following species in order of...Ch. 10 - Prob. 10.53QPCh. 10 - Which of these species has a longer bond, B2 or...Ch. 10 - Acetylene (C2H2) has a tendency to lose two...Ch. 10 - Compare the Lewis and molecular orbital treatments...Ch. 10 - Explain why the bond order of N2 is greater than...Ch. 10 - Compare the relative stability of the following...Ch. 10 - Use molecular orbital theory to compare the...Ch. 10 - A single bond is almost always a sigma bond, and a...Ch. 10 - In 2009 the ion N23 was isolated. Use a molecular...Ch. 10 - The following potential energy curve represents...Ch. 10 - Prob. 10.63QPCh. 10 - Prob. 10.64QPCh. 10 - Prob. 10.65QPCh. 10 - Explain why the symbol on the left is a better...Ch. 10 - Determine which of these molecules has a more...Ch. 10 - Nitryl fluoride (FNO2) is very reactive...Ch. 10 - Describe the bonding in the nitrate ion NO3 in...Ch. 10 - Prob. 10.70QPCh. 10 - Which of the following species is not likely to...Ch. 10 - Draw the Lewis structure of mercury(II) bromide....Ch. 10 - Sketch the bond moments and resultant dipole...Ch. 10 - Although both carbon and silicon are in Group 4A,...Ch. 10 - Acetaminophen is the active ingredient in Tylenol....Ch. 10 - Caffeine is a stimulant drug present in coffee....Ch. 10 - Predict the geometry of sulfur dichloride (SCl2)...Ch. 10 - Antimony pentafluoride, SbF5, reacts with XeF4 and...Ch. 10 - Draw Lewis structures and give the other...Ch. 10 - Predict the bond angles for the following...Ch. 10 - Briefly compare the VSEPR and hybridization...Ch. 10 - Describe the hybridization state of arsenic in...Ch. 10 - Draw Lewis structures and give the other...Ch. 10 - Which of the following molecules and ions are...Ch. 10 - Prob. 10.85QPCh. 10 - The N2F2 molecule can exist in either of the...Ch. 10 - Cyclopropane (C3H6) has the shape of a triangle in...Ch. 10 - The compound 1,2-dichloroethane (C2H4Cl2) is...Ch. 10 - Does the following molecule have a dipole moment?...Ch. 10 - So-called greenhouse gases, which contribute to...Ch. 10 - The bond angle of SO2 is very close to 120, even...Ch. 10 - 3-azido-3-deoxythymidine, shown here, commonly...Ch. 10 - The following molecules (AX4Y2) all have...Ch. 10 - The compounds carbon tetrachloride (CCl4) and...Ch. 10 - Prob. 10.95QPCh. 10 - What are the hybridization states of the C and N...Ch. 10 - Use molecular orbital theory to explain the...Ch. 10 - Referring to the Chemistry in Action essay...Ch. 10 - Which of the molecules (a)(c) are polar?Ch. 10 - Prob. 10.100QPCh. 10 - The stable allotropic form of phosphorus is P4, in...Ch. 10 - Referring to Table 9.4, explain why the bond...Ch. 10 - Use molecular orbital theory to explain the...Ch. 10 - The ionic character of the bond in a diatomic...Ch. 10 - Prob. 10.105QPCh. 10 - Prob. 10.106QPCh. 10 - Aluminum trichloride (AlCl3) is an...Ch. 10 - The molecules cis-dichloroethylene and...Ch. 10 - Prob. 10.109QPCh. 10 - Prob. 10.110QPCh. 10 - The molecule benzyne (C6H4) is a very reactive...Ch. 10 - Assume that the third-period element phosphorus...Ch. 10 - Consider a N2 molecule in its first excited...Ch. 10 - Prob. 10.114QPCh. 10 - Prob. 10.116QPCh. 10 - Draw the Lewis structure of ketene (C2H2O) and...Ch. 10 - TCDD, or 2,3,7,8-tetrachlorodibenzo-p-dioxin, is a...Ch. 10 - Write the electron configuration of the cyanide...Ch. 10 - Prob. 10.120QPCh. 10 - The geometries discussed in this chapter all lend...Ch. 10 - Prob. 10.122QPCh. 10 - Which of the following ions possess a dipole...Ch. 10 - Given that the order of molecular orbitals for NO...Ch. 10 - Shown here are molecular models of SX4 for X = F,...Ch. 10 - Based on what you have learned from this chapter...Ch. 10 - How many carbon atoms are contained in one square...
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