7. 8. 9. In bonding orbital theory, a carbon-carbon triple bond consists of a. 3 pi bonds d. 1 sigma bonds + 4 pi bonds e. 3 sigma bonds b. 1 sigma bond + 2 pi bonds c. 2 sigma bond + 3 pi bonds A substance is a brittle crystal that conducts electricity in molten liquid state only. Which type of substance is it? a. metallic crystal b. ionic crystal c. covalent crystal d. molecular crystal e. frozen gas Four pairs of covalently-bonded electrons surrounding a central atom will be arranged a. pyramidally b. spherically c. tetrahedrally d. linearly e. trigonally

7. 8. 9. In bonding orbital theory, a carbon-carbon triple bond consists of a. 3 pi bonds d. 1 sigma bonds + 4 pi bonds e. 3 sigma bonds b. 1 sigma bond + 2 pi bonds c. 2 sigma bond + 3 pi bonds A substance is a brittle crystal that conducts electricity in molten liquid state only. Which type of substance is it? a. metallic crystal b. ionic crystal c. covalent crystal d. molecular crystal e. frozen gas Four pairs of covalently-bonded electrons surrounding a central atom will be arranged a. pyramidally b. spherically c. tetrahedrally d. linearly e. trigonally

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 26Q: Which of the following statements is(are) true? Correct the false statements. a.The molecules SeS3,...

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The features of polar bonds can be illustrated by considering HF. The general form of the molecular orbital is y = GHY + GỰF, where y, is an H1s orbital and ựe is an F2p, orbital (with z along the internuclear axis, the convention for linear mol- ecules). The relevant data are leV Egglev H 13.6 0.75 F 17.4 3.40 Calculate the energies and coefficients of the bonding and antibonding orbitals made from this combination of atomic orbitals in HF.
11.14 The illustrations below depict differences in orbital hybridiza- tion of some tellurium (Te) fluorides. (a) Which depicts the difference, if any, between TeF, (left) and TeF3 (right)? (b) Which depicts the difference, if any, between TeF, (left) and TeF, (right)? and and A B and and D
Which of the following statements is(are) true? Correct the false statements. a.The molecules SeS3, SeS2, PCl5, TeCl4, ICl3, and XeCl2 all exhibit at least one bond angle, which is approximately 120. b.The bond angle in SO2 should be similar to the bond angle in CS2 or SCl2. c.Of the compounds CF4, KrF4, and SeF4, only SeF4 exhibits an overall dipole moment (is polar). d.Central atoms in a molecule adopt a geometry of the bonded atoms and lone pairs about the central atom in order to maximize electron repulsions.
1a)Identify the molecules below that contains 2-sigma bonding orbitals and 2-pi bonding orbitals? why? a. ethane b. methanol c.ethene d. carbon dioxide 1b) What of the following polyatomic ions contains the fewest valence electrons? why? a. Chlorate b. Chlorite c. hypochlorite d. bicrabonate
Give the electron configurations for the ions Lig* and Liz in molecular orbital terms. Compare the Li-Li bond order in these ions with the bond order in Li2. Electron configuration for Lig + Electron configuration for Liz Bond order of Liz is than that of either of its ions. Drag and drop your selection from the following list to complete the answer: 1 2 1 2 16) (02)² (019) (oʻ1s)" (020)" * * (01s) (o 1s (01s) (o 1s O 2s O 2s O 1s
The first of the two AXmEn type molecules is sp3d and the second has the sp3 hybrid. Accordingly, what values cannot m and n take in the first and second molecules, respectively? A. m = 4 and n = 1, m = 3 and n = 1 B. m = 2 and n = 3, m = 2 and n = 1 C. m = 2 and n = 3, m = 2 and n = 2 D. m = 3 and n = 2, m = 2 and n = 2 E. m = 4 and n = 1, m = 2 and n = 2
I am having trouble with the following chemistry questions, please advise :) 1. For which of the following atoms is the 2+ ion diamagnetic in the ground state? A. Ni B. Fe C. Zn D. Mn E. Cu 2. The dipole moment of BrF is 1.29 D, and its bond length is 178 pm. What is the percent ionic character of the Br-F bond? A. 3.9% B. 8.5% C. 15% D. 33% E. None of these 3. Which of the following reactions correctly describe the formation of NaF(s)? A. Na(s) + F(g) → NaF(s)B. 2 Na(s) + F2(g) → 2 NaF(s)C. Na(s) + 1/2 F2(g) → NaF(s)D. Na(s) + 1/2 F2(s) → NaF(s)E. None of the above
A learningcatalytics.com b My Questions | bartleby O MasteringChemistry le Multiple Choice Question Crayfish learning|catalytics Caitlyn Kelenske | Log out Session 53588886 1 3 4 5 6 7 8 9 10 Jump to V multiple choice question Refer to the MO diagram for 02 for question 3. What is the bond order ( question a) for 02 as calculated from the MO diagram? А. 1 В. С. D. < Join another session O Send a message to the instructor PEARSON ALWAYS LEÀRNING
Consider the following molecule: H2NCH=CH,. Which atomic orbitals overlap to form the nitrogen-carbon sigma bonding orbitals of this molecule? (Best to use my easy method to draw the structure.) skeleton H H H. N CC H. H. O Csp and Nsp O Csp? and C2p O Csp? and Csp? O Csp and N2p O Csp and Csp³ O C2p and C2p O Csp² and Csp O Nsp and Csp
If a molecule demonstrates paramagnetism, then: I. I. The substance can have both paired and unpaired electrons. The bond order is not a whole number. It can be determined by drawing a Lewis structure. It must be an ion. II. IV. O A. I, II O B.I, II, IV OC.II, II O D.I only E. All of the above are correct.
Match the Lewis dot structures with their molecular geometry names: : B - :F: •Br :: .. :: Br: : H-J-H 1. octahedral 2. trigonal bipyramidal 3. see-saw 4. t-shaped 5. linear 6. square planar 7. square pyramidal 8. trigonal planar 9. trigonal pyramidal 10. bent with 120° angles 11. tetrahedral 12. bent with <109.5° angles
The first of the two AXmEn type molecules is sp3d and the second has the sp3 hybrid. Accordingly, what values cannot m and n take in the first and second molecules, respectively? A. m=3 ve n=2, m=2 ve n=2 B. m=4 ve n=1, m=3 ve n=1 C. m=2 ve n=3, m=2 ve n=1 D. m=4 ve n=1, m=2 ve n=2 E. m=2 ve n=3, m=2 ve n=2