New Semester
Started
Get
50% OFF
Study Help!
--h --m --s
Claim Now
Question Answers
Textbooks
Find textbooks, questions and answers
Oops, something went wrong!
Change your search query and then try again
S
Books
FREE
Study Help
Expert Questions
Accounting
General Management
Mathematics
Finance
Organizational Behaviour
Law
Physics
Operating System
Management Leadership
Sociology
Programming
Marketing
Database
Computer Network
Economics
Textbooks Solutions
Accounting
Managerial Accounting
Management Leadership
Cost Accounting
Statistics
Business Law
Corporate Finance
Finance
Economics
Auditing
Tutors
Online Tutors
Find a Tutor
Hire a Tutor
Become a Tutor
AI Tutor
AI Study Planner
NEW
Sell Books
Search
Search
Sign In
Register
study help
sciences
chemistry principles and practice
Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions
How many sigma bonds and how many pi bonds are there in each of the following molecules? | || | (a) H=C=C=C=C | H (c) :N=C H c=c H ic H H (b) H-C-C H T H (c) CHCHCHOCHCH3
Sketch the bonds in H2CNH, label the type of orbital from which each bond forms, and indicate whether the bond is a π or a bond.
Identify the orbitals on each of the atoms that form the bonds in H3CCN. How many π bonds and bonds form?
Identify the orbitals on each of the atoms that form the bonds in propylene (shown below); then indicate whether each bond is a π or a bond. H C=C H H C
If the z axis is defined as the bond axis, draw a picture that shows the overlap of each of the following pairs of orbitals; then indicate whether a π or bond forms.(a) px, px(b) s, pz(c) sp2 hybrid formed from px, pz, and s orbitals, s
If the z axis is defi ned as the bond axis, draw a picture that shows the overlap of each of the following pairs of orbitals; then indicate whether a π or bond forms.(a) pz, pz(b) py, py(c) sp hybrid formed from pz and s orbitals, pz
Indicate the hybridization on each central atom in the molecules with the following Lewis structures. (a) :: T H=C=C=C-H | (b) T H=C=C=N: H
Indicate the hybridization on each central atom in the molecules with the following Lewis structures. (a) H :C: H-C-0-N-CI: 1 H (b) H T H-C=C-P-H
Nitrous acid has the skeleton structure HONO. What are the hybrid orbitals on the nitrogen atom and the central oxygen atom?
What orbitals on selenium and fluorine form the bonds in SeF4? What orbital holds the lone pair on selenium?
Give the hybrid orbital set used by each of the red atoms in the following molecules. : | || | (2) H-N-C-N-H (b) H,C=C=C=C=0 | | (c) H=C=C=C=N:
Identify all the orbitals that form the bonds and hold the lone pairs on the central atom in the following molecules.(a) OF2 (b) NH3 (c) BCl3
Identify the hybrid orbitals on the oxygen atoms that form the bonds in the following species.(a) H3O (b) H3COH (c) Cl2O
Identify the hybrid orbitals on the carbon atoms that form the σ bonds in the following molecules.(a) C2H6 (b) C2H4 (c) CBr4
Identify the hybrid orbitals on the carbon atoms that form the σ bonds in the following species.(a)CO2−3 (b) CH2F2 (c) H2CO
Identify the types of hybrid orbitals on the central atom that form the σ bonds in the following molecules.(a) ClF3 (b) BBr3(c) BeF2 (d) ONCl
Identify the hybrid orbitals on the central atom that form the σ bonds in the following species.(a) N2O (b) SnCl2(c) I−3 (d) SeO2
Identify the hybrid orbitals on the central atom that form the bonds in the following species.(a) NF3 (b) SCl2 (c) H3O(d) IF5 (e) SCl4
Identify the hybrid orbitals on the central atom that form the bonds in the following species.(a) CF4(b) SbCl−6 (c) AsF5(d) SiH4 (e) NH4
Following are drawings of two isomers of C6H4Cl2 (benzene rings are frequently pictured as hexagons, without the letter for the carbon atom at each vertex). Indicate whether each is polar or nonpolar. Explain your answer. H. H H H H 2 H Cl H H (a) (b)
Following are drawings of two derivatives of acetylene.Indicate whether each is polar or nonpolar, and explain your answer. (a) F-C=C-F (b) H-C=C-F
Indicate which of the following molecules are polar. Draw the molecular structure of each polar molecule, including the arrows that indicate the bond dipoles and the molecular dipole moment.(a) BCl3 (b) OF2 (c) SF6
Indicate which of the following molecules are polar. Draw the molecular structure of each polar molecule, including the arrows that indicate the bond dipoles and the molecular dipole moment.(a) SiH4 (b) PCl3 (c) IF5
Indicate which of the following molecules are polar. Draw the molecular structure of each polar molecule, including the arrows that indicate the bond dipoles and the molecular dipole moment.(a) HCN (b) I2 (c) NO
Indicate which molecules are polar and which are nonpolar.(a) SF2 (b) PCl5 (c) AlCl3
Consider the following molecules:(a) CH4 (b) NH2Cl (c) BF3 (d) CS2(i) Which compound has the most polar bonds?(ii) Which compounds in the list are not polar?
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly. (a) F-0-0-F (b) CI CI | | C-C | | CI CI
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly. (a) (b) |||| H-C-C-C-C-H H 1 H T C-C-C-H (c) Cl T P-Cl Cl
Use the VSEPR model to predict the bond angles around each central atom in the following Lewis structures (benzene rings are frequently pictured as hexagons, without the letter for the carbon atom at each vertex). Note that the drawings do not necessarily depict the bond angles correctly. (a) H-0-
Use the VSEPR model to predict the bond angles around each central atom in the following Lewis structures (left). Note that the drawings do not necessarily depict the bond angles correctly. H :N-0-H I | | | H-C-N-C-H T T
Write a Lewis structure for each of the following species.Indicate all of the bond angles as predicted by the VSEPR model. Deduce the skeleton structure from the way each formula is written.(a) SO2 (b) ClO3- (c) SCN
Write a Lewis structure for each of the following molecules. Indicate all of the bond angles as predicted by the VSEPR model. Deduce the skeleton structure from the way each formula is written.(a) ClC(O)NH2 (oxygen bonded only to the carbon atom)(b) HOCH2CH2OH(c) NCCN
Write a Lewis structure for each of the following molecules. Indicate all of the bond angles as predicted by the VSEPR model. Deduce the skeleton structure from the way each formula is written.(a) H3CCCH(b) Br2CCH2(c) H3CNH2
Indicate which species of each pair has the smaller bond angles. Explain your answer(a) BF3 or AsCl+4 (b) CS2 or AsCl3
Indicate which species of each pair has the smaller bond angles. Explain your answer.(a) Cl2NH or NH+4(b) SF2 or IF−4
Indicate which species of each pair has the smaller bond angles. Explain your answer.(a) SO2−4or AlBr3 (b) CCl4 or BeI2
Give the bonded-atom lone-pair arrangement and the molecular shape of the following species.(a) SeO2(b) N2O (N is the central atom)(c) H3O(d) IF5(e) SCl4
Use the VSEPR model to predict the shape of the following species.(a) CF4 (b) CS2 (c) AsF5(d) F2CO (e) NH+4
Give the bonded-atom lone-pair arrangement expected for a central atom that has(a) Three bonded atoms and no lone pairs.(b) Two bonded atoms and two lone pairs.(c) Four bonded atoms and no lone pairs.(d) Four bonded atoms and one lone pair.
Compare and contrast the molecular orbital and ionic bonding descriptions of LiF.
Identify the hybrid orbitals used by antimony in SbCl5 and in SbCl−6, the ion formed from the reaction of SbCl5 and Cl-. Explain your choices. CI Sb CI Sb
Draw the energy-level diagram for the bonding and antibonding molecular orbitals for H2. Indicate their relative energies with respect to the 1s atomic orbitals of isolated hydrogen atoms.
Make a table that shows the hybridization needed to explain bonds at angles of 180, 120, and 109.5 degrees. 10.17 Define a σ bond and a π bond. Show how p orbitals overlap in a σ bond and in a bond.
Explain why the molecular shape of HCl provides no information about the hybridization of the chlorine atom.
Why are hybrid orbitals needed to explain the bonding in CH4?
Identify the hybrid orbitals used by boron in BCl3 and in BCl−4 , the ion formed from the reaction of BCl3 and Cl-. Explain your choices.
Which atomic orbitals overlap to form the bonds in ClF?
Which atomic orbitals overlap to form the bonds in HI?
Give the valence-bond-theory description of how chemical bonds form.
Indicate which molecule of each pair has the smaller bond angles. Explain your answer.(a) BCl3 or NCl3 (b) OF2 or SF6
Explain why SF6 is nonpolar even though it contains polar S–F bonds.
Give an example of a nonpolar molecule that contains polar bonds. Show the polarity of the bonds with arrows, and show how these bond dipoles cancel.
Draw the three possible arrangements of the fluorine atoms about the xenon atom in XeF2. Choose the shape predicted by VSEPR theory, and explain why this arrangement is favored.
Draw the three possible arrangements of the fluorine atoms about the iodine atom in IF3. Choose the shape predicted by VSEPR theory, and explain why this arrangement is favored.
How does the VSEPR model explain the fact that the measured H–O–H bond angle is 104.5 degrees, less than the predicted value of 109.5 degrees?
Give an example of a molecule in which a central carbon atom makes four bonds but has a trigonal planar bonded atom lone-pair arrangement. Give an example of a molecule in which a central carbon atom makes four bonds but has a linear bonded-atom lone-pair arrangement.
State how the bonded-atom lone-pair arrangement is determined.
What is the basic premise of the VSEPR model?
What is the bonded-atom lone-pair arrangement for phosphorus, and what are the Cl–P–Cl bond angles in PCl5?
If the hypothetical molecule SF2Cl2Br2 is nonpolar, what is its shape? What is the arrangement of the atoms?
Identify the atomic orbitals that form the covalent bond in HCl and the atomic orbitals that hold the lone pairs.
Write the molecular orbital electron configuration and give the bond order of NO-. Is the species diamagnetic or paramagnetic?
Write the molecular orbital electron configuration and give the bond order of CN-.StrategyUse the diagram in Figure 10.47, adding electrons as appropriate to the lowest energy orbitals.Figure 10.47 Energy Atomic orbitals 12p 111 1 2s Natom Molecular orbitals 111 111 11 TC₂ 02p 12p 2s 02s 14 NO
Write the molecular orbital diagram and the electron configuration for(a) Be2 (b) B2.Predict the bond order and the number of unpaired electrons for each molecule.StrategyUse the diagram in Figure 10.40, adding electrons as appropriate to the lowest energy orbitals.Figure 10.40 Energy Atomic
Use molecular orbital theory to predict the bond order and the number of unpaired electrons for C2.
Write the electron configuration for then calculate the bond order. Predict whether this species will be stable.StrategyWrite the molecular orbital diagram, place the correct number of electrons in the diagram, and then calculate the bond order. Any molecule with a positive bond order should be
Write the electron configuration for and calculate the bond order. Will this species be stable? Η ,
Describe the bonds in propylene, CH3CH=CH2. Identify the hybridization of each central atom and the type (σ or π) of each bond.StrategyUse the steric numbers determined from the Lewis structure to assign the hybridization of each central atom. The hybrid orbitals will form the sigma bonds; any
Identify the orbitals that overlap to form the bonds in HCN. HIS- C 5/3 C C
Identify the hybridization of the central atom and the orbitals used for each bond in IF5.StrategyThe steric number, determined from the Lewis structure, defines the hybrid orbitals needed for a central atom. Use the electron configuration of the peripheral atoms to determine which orbital is
Describe the bonding in SF4.
Identify the hybridization of the central atom in(a) BCl3 and(b) CH2F2.StrategyIdentify the hybridization on the central atom from the steric number, determined from the Lewis structure.
What hybrid oxygen orbitals form the bonds in OF2?
Identify the atomic orbitals that are used to form the covalent bond in Cl2 and the atomic orbitals that are occupied by the lone pairs.StrategyDetermine the occupancy of the valence orbitals. The bonds are made by orbitals that contain one electron.
An experiment shows that the molecule PF2Cl3 is nonpolar. What is the molecular shape, and what is the arrangement of the atoms in that shape?StrategyWrite the Lewis structure and determine the bonded-atom lone-pair arrangement. Place the two types of atoms in positions such that the bond dipoles
Predict which of the following molecules are polar and which are nonpolar:(a) CH4,(b) HCN,(c) H2O,(d) XeF4.StrategyWrite the Lewis structure of each, determine the steric number, and assign the bonded-atom lone-pair arrangement. With only a few exceptions, a molecule will be polar unless all
Is PF3 polar or nonpolar?
What is the geometry about each carbon atom in acetylene, HC=CH?
What are the bond angles around each carbon atom in ethylene, C2H4?StrategyUse the Lewis structure to assign separately the steric number of both central atoms. These steric numbers determine the bonded-atom lone-pair arrangements, each of which has characteristic bond angles.
What are the bonded-atom lone-pair arrangements, the bond angles, and the shapes of(a) BrF5,(b) ClNO,(c) ?StrategyObtain the steric numbers of each central atom from the Lewis structures and use them to assign the bonded-atom lone-pair arrangement, which determines the bond angles. The shapes
What are the bonded-atom lone-pair arrangement, the shape, and the Cl–I–Cl bond angles in the [ICl4]- ion?
What is the bonded-atom lone-pair arrangement about the central carbon atom, and what are the angles between the bonds in the molecules(a) CCl4 and(b) CO2?StrategyDetermine the steric number from the Lewis structure, then use that number to assign the bonded-atom lone-pair arrangement.
Natural gas is mostly methane, CH4. Homes that are heated by natural gas obtain the energy from the combustion reaction(a) Balance the reaction.(b) Is this a redox reaction? Defend your answer.(c) Determine the enthalpy change of this reaction using the enthalpy of formation data in the Appendix
Predict whether the bonds between the following atoms should be nonpolar covalent, polar covalent, or ionic.(a) Li and O(b) F and Cl(c) S and S(d) Na and I
Predict whether the bonds between the following atoms should be nonpolar covalent, polar covalent, or ionic.(a) C and H(b) K and F(c) O and O(d) Be and F
The compound ClF3 reacts with solid uranium to produce the volatile compounds UF6 and ClF. ClF3 can be used to separate uranium from plutonium, because plutonium reacts with ClF3 to form the nonvolatile compounds PuF4 and ClF.(a) Write equations for these two reactions.(b) Draw the Lewis
The reaction of XeF6 with a limited amount of H2O yields XeOF4 and HF. Write the equation for this reaction; then draw the Lewis structures of the expanded valence shell molecules in the equation.
Draw the Lewis structures of N2O and NO2. Based on these structures, predict which has the shorter N–O bond. Does either of these molecules contain unpaired electrons?
Match the following three lattice energies with the three compounds LiF, KCl, and CsI. Explain your answer. 715 kJ/mol 582 kJ/mol 1036 kJ/mol
Calculate an approximate enthalpy change for the following reaction: HCN(g) + 2H₂(g) → H3CNH₂(g)
Phosgene, Cl2CO, is an extremely toxic gas that can be prepared by the reaction of CO with Cl2. Using data from Table 9.4, calculate the approximate enthalpy change for this reaction.Table 9.4 TABLE 9.4 Bond Energies (kJ/mol)* Single
The molecule nitrosyl chloride, NOCl, has a skeleton structure of O-N-Cl. Two resonance forms can be written; write them both. Use the formal charge stability rules to predict which form is more stable.
Draw the Lewis structure of BrNO. Which is the more polar bond in the molecule?
Draw the Lewis structure and calculate the energy needed to break all of the bonds in 1 mol of CH3NH2.
A compound related to the new greenhouse gas in the previous exercise is FCSF3, where again the carbon and sulfur atoms are bonded together and act as central atoms. What is the Lewis structure of this compound? Do both central atoms follow the octet rule?
In the gas phase, the oxide N2O5 has a structure with an N - O - N core, with the other four oxygen atoms in terminal positions. In contrast, in the solid phase, the stable form is [NO2]+[NO3]-. Draw one Lewis structure of the molecular form (with N–O–N single bonds) and all possible resonance
Acrolein has the formula CH2C(H)C(O)H. Draw its skeleton structure and Lewis structure.
The compound CF3SF5 was recently identified in Earth’s atmosphere and is a potential greenhouse gas. If the carbon atom and sulfur atom are bonded together, what is the Lewis structure of this compound? Do both central atoms follow the octet rule?
The compound SF4CH2 has an unusually short SC distance of 155 pm. Use the Lewis structure to explain this short distance.
Consider the nitrogen–oxygen bond lengths in In which ion is the bond predicted to be longest? In which is it predicted to be the shortest? Explain briefly. NOŽ,
Showing 1500 - 1600
of 2906
First
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
Last
Step by Step Answers
Get 50% OFF
Claim Now
