Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 7, Problem 7.78PAE
Interpretation Introduction
Interpretation:
The reason of lone pair occupying at equatorial position should be described.
Concept introduction:
The electrons involved in bond formation for any compound are known as bond pair and the electrons remained unused in bonding are known as lone pairs.
As per the VSEPR theory, any molecule should have minimum energy and minimum repulsion states.
It means that, the bonds should be arranged in such manner which could minimize the electronic repulsion and stabilize the molecules.
Further, the axial positions are the positions parallel to the axes and the equitorial positions are perpendicular to the axes and lie on the equator.
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There is an instrument in Johnson 334 that measures total-reflectance x-ray fluorescence (TXRF) to do elemental analysis (i.e., determine what elements are present in a sample). A researcher is preparing a to measure calcium content in a series of well water samples by TXRF with an internal standard of vanadium (atomic symbol: V). She has prepared a series of standard solutions to ensure a linear instrument response over the expected Ca concentration range of 40-80 ppm. The concentrations of Ca and V (ppm) and the instrument response (peak area, arbitrary units) are shown below. Also included is a sample spectrum. Equation 1 describes the response factor, K, relating the analyte signal (SA) and the standard signal (SIS) to their respective concentrations (CA and CIS).
Ca, ppm
V, ppm
SCa, arb. units
SV, arb. units
20.0
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14375.11
14261.02
40.0
10.0
36182.15
17997.10
60.0
10.0
39275.74
12988.01
80.0
10.0
57530.75
14268.54
100.0…
A mixture of 0.568 M H₂O, 0.438 M Cl₂O, and 0.710 M HClO are enclosed in a vessel at 25 °C.
H₂O(g) + C₁₂O(g) = 2 HOCl(g)
K = 0.0900 at 25°C
с
Calculate the equilibrium concentrations of each gas at 25 °C.
[H₂O]=
[C₁₂O]=
[HOCI]=
M
Σ
M
Chapter 7 Solutions
Chemistry for Engineering Students
Ch. 7 - List some factors influencing the biocompatibility...Ch. 7 - • use electron configurations to explain why...Ch. 7 - • describe die energy changes in the formation of...Ch. 7 - • define electronegativity and state how...Ch. 7 - • identify or predict polar, nonpolar, and ionic...Ch. 7 - • write Lewis electron structures for molecules or...Ch. 7 - • describe chemical bonding using a model based on...Ch. 7 - • explain how hybridization reconciles observed...Ch. 7 - • predict the geometry of a molecule from its,...Ch. 7 - • use models (real or software) to help visualize...
Ch. 7 - • explain the formation of multiple bonds in terms...Ch. 7 - • identify sigma and pi bonds in a molecule and...Ch. 7 - Define the term biocompatibility.Ch. 7 - List some properties associated with biomaterials...Ch. 7 - Prob. 7.3PAECh. 7 - Prob. 7.4PAECh. 7 - Prob. 7.5PAECh. 7 - Prob. 7.6PAECh. 7 - Why is the ion not found in nature?Ch. 7 - Why do nonmetals tend to form anions rather than...Ch. 7 - Prob. 7.9PAECh. 7 - 7.10 Arrange the members of each of the following...Ch. 7 - 7.11 Arrange the following sets of anions in order...Ch. 7 - 7.12 Which pair will form a compound with the...Ch. 7 - In a lattice, a positive ion is often surrounded...Ch. 7 - Use the concept of lattice energy to rationalize...Ch. 7 - 7.13 Figure 7-2 depicts the interactions of an ion...Ch. 7 - Mat type of bond is likely to form between one...Ch. 7 - 7.14 Describe the difference between a covalent...Ch. 7 - Prob. 7.18PAECh. 7 - Sketch a graph of the potential energy of two...Ch. 7 - Prob. 7.20PAECh. 7 - 7.17 Coulombic forces are often used to explain...Ch. 7 - 7.18 In terms of the strengths of the covalent...Ch. 7 - 7.19 If the formation of chemical bonds always...Ch. 7 - 7.20 Draw the Lewis dot symbol for each of the...Ch. 7 - 7.21 Theoretical models for the structure of...Ch. 7 - 7.22 Use Lewis dot symbols to explain why chlorine...Ch. 7 - 7.23 Define the term lone pair.Ch. 7 - 7.24 How many electrons are shared between two...Ch. 7 - 7.25 How does the bond energy of a double bond...Ch. 7 - 7.26 How is electronegativity defined?Ch. 7 - 7.27 Distinguish between electron affinity and...Ch. 7 - 7.28 Certain elements in the periodic table shown...Ch. 7 - 7.29 When two atoms with different...Ch. 7 - 7.30 The bond in HF is said to be polar, with the...Ch. 7 - 7.31 Why is a bond between two atoms with...Ch. 7 - Prob. 7.36PAECh. 7 - 7.33 In each group of three bonds, which bond is...Ch. 7 - Prob. 7.38PAECh. 7 - Prob. 7.39PAECh. 7 - 7.35 Which one of the following contains botb...Ch. 7 - Prob. 7.41PAECh. 7 - Prob. 7.42PAECh. 7 - 7.37 Draw the Lewis structure for each of the...Ch. 7 - 7.38 Draw a Lewis structure for each of the...Ch. 7 - Prob. 7.45PAECh. 7 - 7.40 Why is it impossible for hydrogen to be the...Ch. 7 - Prob. 7.47PAECh. 7 - 7.42 Draw resonance structure for (a) (b) and (c)Ch. 7 - Prob. 7.49PAECh. 7 - Prob. 7.50PAECh. 7 - Prob. 7.51PAECh. 7 - 7.46 Consider the nitrogen-oxygen bond lengths in...Ch. 7 - 7.47 Which of the species listed has a Lewis...Ch. 7 - 7.48 Identify what is incorrect in the Lewis...Ch. 7 - 7.49 Identify what is incorrect in the Lewis...Ch. 7 - 7.50 Chemical species are said to be isoelectronic...Ch. 7 - 7.51 Explain the concept of wave interference in...Ch. 7 - Distinguish between constructive and destructive...Ch. 7 - How is the concept of orbital overlap related to...Ch. 7 - 7.52 How does orbital overlap explain the buildup...Ch. 7 - 7.53 How do sigma and pi bonds differ? How are...Ch. 7 - 7.54 CO , CO2 , CH3OH , and CO32 , all contain...Ch. 7 - 7.55 Draw the Lewis dot structure of the following...Ch. 7 - 7.56 Draw the Lewis dot structures of the...Ch. 7 - 7.57 What observation about molecules compels us...Ch. 7 - Prob. 7.66PAECh. 7 - 7.59 What type of hybrid orbital is generated by...Ch. 7 - Considering only s and p atomic orbitals, list all...Ch. 7 - 7.61 What hybrid orbitals would be expected for...Ch. 7 - 7.62 What type of hybridization would you expect...Ch. 7 - 7.63 What physical concept forms the premise of...Ch. 7 - 7.64 Predict the geometry of the following...Ch. 7 - Prob. 7.73PAECh. 7 - Prob. 7.74PAECh. 7 - Prob. 7.75PAECh. 7 - 7.68 Give approximate values for the indicated...Ch. 7 - 7.69 Propene has the chemical formula Describe the...Ch. 7 - Prob. 7.78PAECh. 7 - Describe what happens to the shape about the...Ch. 7 - Prob. 7.80PAECh. 7 - Prob. 7.81PAECh. 7 - 7.72 How does an MSN differ from amorphous silica...Ch. 7 - Prob. 7.83PAECh. 7 - Prob. 7.84PAECh. 7 - Prob. 7.85PAECh. 7 - Prob. 7.86PAECh. 7 - 7.91 A Lewis structure for the oxalate ion is...Ch. 7 - Prob. 7.88PAECh. 7 - 7.93 An unknown metal M forms a chloride with the...Ch. 7 - Prob. 7.90PAECh. 7 - Prob. 7.91PAECh. 7 - 7.96 Consider the hydrocarbons whose structures...Ch. 7 - 7.97 Consider the structure shown below for as...Ch. 7 - Prob. 7.94PAECh. 7 - Prob. 7.95PAECh. 7 - Prob. 7.96PAECh. 7 - 7.101 Lead selenide nanocrystals may provide a...Ch. 7 - Prob. 7.98PAECh. 7 - Prob. 7.99PAECh. 7 - 7.104 Hydrogen azide, HN3 , is a liquid that...Ch. 7 - Prob. 7.101PAECh. 7 - Prob. 7.102PAECh. 7 - 7.107 How do the Lewis symbols for C, Si, and Ge...Ch. 7 - Prob. 7.104PAECh. 7 - Prob. 7.105PAE
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