![OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)](https://s3.amazonaws.com/compass-isbn-assets/textbook_empty_images/large_textbook_empty.svg)
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
5th Edition
ISBN: 9781285460420
Author: John W. Moore; Conrad L. Stanitski
Publisher: Cengage Learning US
expand_more
expand_more
format_list_bulleted
Videos
Question
Chapter 7, Problem 58QRT
Interpretation Introduction
Interpretation:
The reason for the solubility of alpha-tocopherol in fat and not in water has to be given.
Concept introduction:
Vitamin: It is an organic molecule which is essential in trace amounts and it cannot be synthesized in the body. It must be obtained from the diet.
According to the solubility, vitamins can be classified into two:
- Water soluble vitamin
- Fat soluble vitamin
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Testosterone is an anabolic steroid. The structure of testosterone is shown below.
What is the idealised bond angle at the indicated atom (ii) ?
Hint: atom (iv) has been completed for you as an example.
(iv) bond angle: 109.5°, geometry of the electron pairs: tetrahedral, shape of the
bonds: tetrahedral
·····|||I
H
····||||I
ii
iv
Suggest some spectroscopic techniques that can be used to determine the structure of Prussian blue.
19 of 44 >
© Macmillan Learning
In the given three-dimensional molecular structure, the
differently colored spheres represent different types of atoms.
Write a molecular formula for this molecule.
molecular formula:
4
R
%
67 68
5
1
SPECIAL
xº
(g)
ΔΣΩ λμπ
X₁ X
()
6
[]
(s)
Y
(1) (aq)
→>>>
MacBook Pro
The
11
7
U
t
CLR
8
K
→>>
9
Rotate X
You
9
Rotate Y
(
0
☐C □H
D
Rotate Z
0
Zoom In
P
O
Zoom Out
Attempt
A
Label Atoms
C
Chapter 7 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
Ch. 7.2 - Identify the electron-region geometry, the...Ch. 7.2 - Based on the discussion so far, identify a...Ch. 7.2 - Prob. 7.2PSPCh. 7.2 - Determine the electron-region geometry and the...Ch. 7.2 - Prob. 7.2CECh. 7.2 - Prob. 7.3ECh. 7.2 - Prob. 7.4PSPCh. 7.4 - Using hybridization and sigma and pi bonding,...Ch. 7.4 - Prob. 7.4CECh. 7.5 - Decide whether each molecule is polar and, if so,...
Ch. 7.5 - Prob. 7.5ECh. 7.6 - Prob. 7.8PSPCh. 7.6 - Prob. 7.7CECh. 7.6 - Prob. 7.9PSPCh. 7.7 - Prob. 7.8CECh. 7.7 - Prob. 7.9CECh. 7 - Write the Lewis structures and give the...Ch. 7 - The structural formula for the open-chain form of...Ch. 7 - Describe the VSEPR model. How is the model used to...Ch. 7 - What is the difference between the electron-region...Ch. 7 - Prob. 3QRTCh. 7 - Prob. 4QRTCh. 7 - If you have three electron regions around a...Ch. 7 - Prob. 6QRTCh. 7 - Prob. 7QRTCh. 7 - Prob. 8QRTCh. 7 - Prob. 9QRTCh. 7 - Prob. 10QRTCh. 7 - Prob. 11QRTCh. 7 - Prob. 12QRTCh. 7 - Prob. 13QRTCh. 7 - Prob. 14QRTCh. 7 - Prob. 15QRTCh. 7 - Prob. 16QRTCh. 7 - Write Lewis structures for XeOF2 and ClOF3. Use...Ch. 7 - Write Lewis structures for HCP and [IOF4]. Use...Ch. 7 - Prob. 19QRTCh. 7 - Prob. 20QRTCh. 7 - Explain why (I3)+ is bent, but (I3) is linear.Ch. 7 - Prob. 22QRTCh. 7 - Prob. 23QRTCh. 7 - Give approximate values for the indicated bond...Ch. 7 - Give approximate values for the indicated bond...Ch. 7 - Prob. 26QRTCh. 7 - Compare the FClF angles in ClF2+ and ClF2. From...Ch. 7 - Prob. 28QRTCh. 7 - Prob. 29QRTCh. 7 - Prob. 30QRTCh. 7 - Prob. 31QRTCh. 7 - Describe the geometry and hybridization of carbon...Ch. 7 - Describe the geometry and hybridization for each C...Ch. 7 - Describe the hybridization around the central atom...Ch. 7 - The hybridization of the two carbon atoms differs...Ch. 7 - The hybridization of the two nitrogen atoms...Ch. 7 - Identify the type of hybridization, approximate...Ch. 7 - Prob. 38QRTCh. 7 - Prob. 39QRTCh. 7 - Prob. 40QRTCh. 7 - Prob. 41QRTCh. 7 - Methylcyanoacrylate is the active ingredient in...Ch. 7 - Prob. 43QRTCh. 7 - Prob. 44QRTCh. 7 - Prob. 45QRTCh. 7 - Prob. 46QRTCh. 7 - Which of these molecules has a net dipole moment?...Ch. 7 - Prob. 48QRTCh. 7 - Use molecular structures and noncovalent...Ch. 7 - Prob. 50QRTCh. 7 - Explain why water “beads up” on a freshly waxed...Ch. 7 - Explain why water will not remove tar from your...Ch. 7 - Prob. 53QRTCh. 7 - Prob. 54QRTCh. 7 - Prob. 55QRTCh. 7 - Prob. 56QRTCh. 7 - The structural formula for vitamin C is Give a...Ch. 7 - Prob. 58QRTCh. 7 - Prob. 59QRTCh. 7 - Prob. 60QRTCh. 7 - Prob. 61QRTCh. 7 - Prob. 62QRTCh. 7 - Prob. 63QRTCh. 7 - Prob. 64QRTCh. 7 - Prob. 65QRTCh. 7 - Prob. 66QRTCh. 7 - Methylcyanoacrylate is the active ingredient in...Ch. 7 - Prob. 68QRTCh. 7 - Prob. 69QRTCh. 7 - Use Lewis structures and VSEPR theory to predict...Ch. 7 - In addition to CO, CO2, and C3O2, there is another...Ch. 7 - Prob. 72QRTCh. 7 - Prob. 73QRTCh. 7 - Prob. 74QRTCh. 7 - Prob. 75QRTCh. 7 - In the gas phase, positive and negative ions form...Ch. 7 - Prob. 77QRTCh. 7 - Prob. 78QRTCh. 7 - Prob. 79QRTCh. 7 - Prob. 80QRTCh. 7 - Prob. 81QRTCh. 7 - Prob. 82QRTCh. 7 - Prob. 83QRTCh. 7 - Prob. 84QRTCh. 7 - Prob. 85QRTCh. 7 - Prob. 86QRTCh. 7 - Prob. 87QRTCh. 7 - Prob. 88QRTCh. 7 - Prob. 89QRTCh. 7 - Prob. 90QRTCh. 7 - Prob. 91QRTCh. 7 - Prob. 92QRTCh. 7 - Prob. 93QRTCh. 7 - Prob. 94QRTCh. 7 - Which of these are examples of hydrogen bonding?Ch. 7 - Prob. 96QRTCh. 7 - Prob. 97QRTCh. 7 - Prob. 98QRTCh. 7 - Halothane, which had been used as an anesthetic,...Ch. 7 - Ketene, C2H2O, is a reactant for synthesizing...Ch. 7 - Gamma hydroxybutyric acid, GHB, infamous as a date...Ch. 7 - There are two compounds with the molecular formula...Ch. 7 - Piperine, the active ingredient in black pepper,...Ch. 7 - Prob. 105QRTCh. 7 - Two compounds have the molecular formula N3H3. One...Ch. 7 - Prob. 108QRTCh. 7 - Prob. 109QRTCh. 7 - Prob. 110QRTCh. 7 - Prob. 111QRTCh. 7 - Prob. 7.ACPCh. 7 - Prob. 7.BCPCh. 7 - Prob. 7.CCPCh. 7 - Prob. 7.DCP
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
- Carbon naturally occurs in two forms: diamond and graphite. Why do these two forms have very different properties? The key difference is that diamonds have other elements bonded within their structure. The differences are explained by the number of covalent and ionic bonds within each substance. The differences are explained by the density: graphite is very high and diamond is much lower. The differences are explained by how the carbon atoms within each substance are covalently bonded together.arrow_forwardUse Born-Mayer equation to calculate the lattice energy for PbS (it crystallizes in theNaCl structure). Then, use the Born–Haber cycle to obtain the value of lattice energy for PbS.You will need the following data following data : ΔH Pb(g) = 196 kJ/mol; ΔHf PbS = –98kJ/mol; electron affinities for S(g)→S- (g) is -201 kJ/mol; ) S- (g) →S2-(g) is 640kJ/mol. Ionizationenergies for Pb are listed in Resource section 2, p.903. Remember that enthalpies of formationare calculated beginning with the elements in their standard states (S8 for sulfur). Diatomicsulfur, S2, is formed from S8 (ΔHf: S2 (g) = 535 kJ/mol. Can you just do the Born-Haber part?arrow_forwardDraw the Lewis structure of the following molecules: Sulfuric acid Sulfur trioxide Sulfurous acid Sulfur dioxide Nitric acid Nitrate Nitrite Nitrogen trioxide Nitrous acid Nitrogen dioxide nitrous oxidearrow_forward
- Iodine is an essential trace element in our diet; it is needed to produce thyroid hormone. Insufficient iodine in the diet can lead to the development of a goiter, an enlargement of the thyroid gland . The addition of small amounts of iodine to table salt (iodized salt) has essentially eliminated this health concern in the United States, but as much as 40% of the world’s population is still at risk of iodine deficiency. The iodine atoms are added as anions, and each has a 1− charge and a mass number of 127. Determine the numbers of protons, neutrons, and electrons in one of these iodine anions.arrow_forwardCalculate the Delta H for the reaction of fluorine gas, F2(g) with H20(I) water to form 2HF(g) and O2(g).arrow_forwardHow many grams of gaseous ammonia will the reaction of 3.0 g hydrogen gas and 3.0 g of nitrogen gas produce?arrow_forward
- Using the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulfur double bond in CS2.arrow_forwardFor many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains 77.55% Xe and 22.45% F by mass.(a) What is the formula of the compound?(b) Write a Lewis structure for the compound.(c) Predict the shape of the molecules of the compound.(d) What hybridization is consistent with the shape you predicted?arrow_forwardConsider the elements Li, K, Cl, C, Ne, and Ar. From this list, select the element that (a) is most electronegative, (b) has the greatest metallic character, (c) most readily forms a positive ion, (d) has the smallest atomic radius, (e) forms p bonds most readily, (f) has multiple allotropes.arrow_forward
- 3 What is the biggest difference between the Lewis and the AO-model in terms of the localisation of electrons in atoms?arrow_forwardDraw all of the Lewis structures of O22- which obey the octet rule and use this Lewis structure or these resonance structures to predict how many covalent bonds connect each oxygen atom in the real structure to the central O atom. Assume that the octet rule is followed for the O atom when you draw your structure(s). Pick the correct statement from the choices below. a) Each oxygen atom is connected to the central O atom with 1 covalent bonds. b) Each oxygen atom is connected to the central O atom with 1.33 covalent bonds. c) Each oxygen atom is connected to the central O atom with 2 covalent bonds. d) Each oxygen atom is connected to the central O atom with 1.67 covalent bonds. e) Each oxygen atom is connected to the central O atom with 1.25 covalent bonds.arrow_forwardFill in the systematic names of the following chemical compounds. Note: for compounds containing hydrogen, you may give the common name instead. molecular formula name of compound Cs, C;S, BI, ВР H,0arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Linear Combination of Atomic Orbitals LCAO; Author: Edmerls;https://www.youtube.com/watch?v=nq1zwrAIr4c;License: Standard YouTube License, CC-BY
Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY