Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 9, Problem 18PS
For each compound below, decide whether cis and trans isomers are possible. If isomerism is possible, draw the other isomer.
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2. From the models of SF4, BrF3, and XeF4, deduce whether different atom arrangement, called
geometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometry
for each case and suggest a reason for your choice. Indicate which structures have dipole
moments and show their direction,
Preferred
Molecular
Compound
Electron
Dipole
Reason
Geometry
Moment
(Polarity) geometry
SF4
BRF3
XeF4
3. Using the Lewis structure predict the geometrical structures of the following ions and state
the hybridization of the central atom.
Ion
Electron Geometry
Molecular
Formal Charge
Central Atom
Geometry
of Central
Hybridization
Atom
CO32-
NO3-
BF4
Determine the molecule below that contains one or more atoms that violate the
octet rule.
O CH2NCH2CH3
O CHCH3CH2CH3
O CH3CH2
HOCH2CH3
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Chapter 9 Solutions
Chemistry & Chemical Reactivity
Ch. 9.1 - Use valence bond theory to describe the bonding in...Ch. 9.1 - Identify the hybridization of each underlined atom...Ch. 9.1 - Use valence bond theory to describe the bonding in...Ch. 9.2 - What is the electron configuration of the H2+ ion?...Ch. 9.2 - Could the anion Li2 exist? What is the ions bond...Ch. 9.2 - The cations O2+ and N2+ are formed when molecules...Ch. 9.3 - Photoelectron spectroscopy is s1milar to the...Ch. 9.3 - What is the energy of a photon with a wavelength...Ch. 9.3 - Using the accompanying figure, state which...Ch. 9.3 - The kinetic energy of an electron ejected from the...
Ch. 9.3 - The N2+ ions that are formed when electrons with...Ch. 9.3 - What is the empirical formula of Tynan purple?Ch. 9.3 - Butter yellow absorbs light with a wavelength of...Ch. 9.3 - Prob. 2.3ACPCh. 9 - Draw the Lewis structure for chloroform, CHCl3....Ch. 9 - Draw the Lewis structure for NF3. What are its...Ch. 9 - Draw the Lewis structure for hydroxylamine, H2NOH....Ch. 9 - Draw the Lewis structure for 1,...Ch. 9 - Draw the Lewis structure for carbonyl fluoride,...Ch. 9 - Draw the Lewis structure for acetamide, CH3CONH2....Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Specify the electron-pair and molecular geometry...Ch. 9 - Prob. 9PSCh. 9 - What is the hybrid orbital set used by each of the...Ch. 9 - Draw the Lewis structures of the acid HPO2F2 and...Ch. 9 - Draw the Lewis structures of the arid HSO3F and...Ch. 9 - What is the hybridization of the carbon atom in...Ch. 9 - What is the hybridization of the carbon atoms in...Ch. 9 - What is the electron-pair and molecular geometry...Ch. 9 - What is the electron-pair and molecular geometry...Ch. 9 - Prob. 17PSCh. 9 - For each compound below, decide whether cis and...Ch. 9 - Molecular Orbital Theory (See Examples 9.49.6.)...Ch. 9 - Give the electron configurations for the ions Li2+...Ch. 9 - Calcium carbide, CaC2, contains the acetylide ion,...Ch. 9 - Platinum hexafluoride is an extremely strong...Ch. 9 - When sodium and oxygen react, one of the products...Ch. 9 - When potassium and oxygen react, one of the...Ch. 9 - Among the following, which has the shortest bond...Ch. 9 - Consider the following list of small molecules and...Ch. 9 - Prob. 27PSCh. 9 - The nitrosyl ion. NO+, has an interesting...Ch. 9 - These questions are not designated as to type or...Ch. 9 - What is the OSO angle and the hybrid orbital set...Ch. 9 - Sketch the resonance structures for the nitrite...Ch. 9 - Sketch the resonance structures for the nitrate...Ch. 9 - Sketch the resonance structures for the N2O...Ch. 9 - Compare the structure and bonding in CO2 and CO32...Ch. 9 - Numerous molecules are detected in deep space....Ch. 9 - Acrolein, a component of photochemical smog, has a...Ch. 9 - The organic compound below is a member of a class...Ch. 9 - The compound sketched below is acetylsalicylic...Ch. 9 - Phosphoserine is a less-common amino acid. (a)...Ch. 9 - Lactic acid is a natural compound found in sour...Ch. 9 - Cinnamaldehyde ocaus naturally in cinnamon oil....Ch. 9 - The ion Si2 was reported in a laboratory...Ch. 9 - The simple valence bond picture of O2 does not...Ch. 9 - Nitrogen, N2, can ionize to form N2+ or add an...Ch. 9 - Which of the homonuclear, diatomic molecules of...Ch. 9 - Which of the following molecules or ions are...Ch. 9 - Prob. 47GQCh. 9 - The structure of amphetamine, a stimulant, is...Ch. 9 - Menthol is used in soaps, perfumes, and foods. It...Ch. 9 - Prob. 50GQCh. 9 - Suppose you carry out the following reaction of...Ch. 9 - Ethylene oxide is an intermediate in the...Ch. 9 - The sulfamate ion, H2NSO3, can be thought of as...Ch. 9 - The compound whose structure is shown here is...Ch. 9 - Prob. 55ILCh. 9 - Carbon dioxide (CO2), dinitrogen monoxide (N2O),...Ch. 9 - Draw the two resonance structures that describe...Ch. 9 - Draw a Lewis structure for diimide, HNNH. Then,...Ch. 9 - Prob. 59SCQCh. 9 - Consider the three fluorides BF4, SiF4, and SF4....Ch. 9 - When two amino acids react with each other, they...Ch. 9 - What is the connection between bond order, bond...Ch. 9 - When is it desirable to use MO theory rather than...Ch. 9 - Show how valence bond theory and molecular orbital...Ch. 9 - Three of the four molecular orbitals for...Ch. 9 - Lets look more closely at the process of...Ch. 9 - Borax has the molecular formula Na2B4O5(OH)4. The...Ch. 9 - A model of the organic compound allene is shown...Ch. 9 - Prob. 69SCQCh. 9 - Prob. 70SCQCh. 9 - Bromine forms a number of oxides of varying...Ch. 9 - Prob. 72SCQCh. 9 - Urea reacts with malonic acid to produce...
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- 3) Determine whether CH3CI is polar. To do this, you must: draw the 3D structure of the molecule, use arrows to indicate polar bonds, and either use an arrow to indicate the net dipole moment or state that the molecule is non-polar.arrow_forwardThe trans arrangement is favored in N2H2, but the cis arrangement is favored in N2F2. Explain this result?arrow_forwardPlease answer questions 1 2 3 4abcarrow_forward
- ) Bean hexene is an odor compound used in cosmetics and cleaners. It is also known as leguminal. Its formula is: CH3CH2CHCHCH2CH2OCHCH2CH3 | OCH3 Please draw a Lewis structure for this compound with CORRECT GEOMETRY (use dashes and wedges!) Label all pi bonds in the molecule (if there are any) Indicate the bond angles for the red highlighted section of the molecule. (hint: you may want to keep the main carbon chain in-plane with the page for clarity) For this question, you don’t need to draw out the orbitals.arrow_forwardPlease complete answersarrow_forwardresonance structuresarrow_forward
- Draw the correct shape of TcCl2 Are the bonds here polar? If so, draw crossed arrows along them to show the direction of polarity. If not, explain why not. Is the whole molecule polar? If so, draw a crossed arrow through the 3-dimensional structure above to show the direction of polarity. If not, explain why not.arrow_forward● Explain both of the following trends in terms of attractive/repulsive forces and distance:▪ the general upwards trend WITHIN a given column(family)▪ the general downwards trend WITHIN a given period(row)arrow_forwardAnswer the questions in the table below about the shape of the methanone (H₂CO) molecule. How many electron groups are around the central carbon atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central carbon atom? (You may need to use the scrollbar to see all the choices.) (choose one) X Sarrow_forward
- Choose the compound below that contains at least one polar covalent bond, but is nonpolar. SCl2 CH2Cl2 AsCl5 GeH2Br2 All of the above are nonpolar and contain a polar covalent bond.arrow_forwardUnshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs. Use the structural formulas below to determine the number of unshared pairs at each designated atom. Be sure your answers are consistent with the formal charges on the formulas. The number of unshared pairs at atom a is 4 The number of unshared pairs at atom b is 2 H The number of unshared pairs at atom c is 3 The number of unshared pairs at atom a is The number of unshared pairs at atom b is C-NEN а b H The number of unshared pairs at atom c is Submit Answer Retry Entire Group 8 more group attempts remainingarrow_forwardSolve this questionarrow_forward
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