EBK CHEMISTRY
8th Edition
ISBN: 9780135216972
Author: Robinson
Publisher: PEARSON CO
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Textbook Question
Chapter 8, Problem 8.96SP
What is the difference in spatial distribution between electrons in a bonding MO and electrons in an anti bonding MO?
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Check out a sample textbook solutionStudents have asked these similar questions
Study the following sketch of a molecular orbital (MO) in a homonuclear diatomic molecule. This MO was formed by combining one 3p atomic orbital from eac
atom.
00
The dark dots in this sketch are the nuclei.
Now use the sketch to complete the table below.
Write the symbol for this Mo.
JT
O*
O bonding
O antibonding
Is this a bonding or antibonding MO?
O higher
O lower
What is the energy of this MO, compared to the
energy of a 3p orbital on one of the separate
atoms?
O the same
not enough information
to decide
Submit Ass
Continue
Complete the table below, which lists information about some diatomic molecules or molecular ions.
In particular:
• Decide whether each molecule is stable or not.
• Decide whether each molecule would be diamagnetic or paramagnetic.
• Calculate each molecule's bond order.
diamagnetic or
paramagnetic?
molecule
stable?
bond order
O yes
O diamagnetic
O no
O paramagnetic
yes
O diamagnetic
Li,
O no
O paramagnetic
yes
O diamagnetic
Ne,
O no
O paramagnetic
olo
이0 이0 이
Complete the table below, which lists information about some diatomic molecules or molecular ions.
In particular:
• Decide whether each molecule is stable or not.
• Decide whether each molecule would be diamagnetic or paramagnetic.
• Calculate each molecule's bond order.
diamagnetic or
paramagnetic?
molecule
stable?
bond order
O yes
diamagnetic
O paramagnetic
no
О yes
diamagnetic
Be,
O paramagnetic
no
О yes
diamagnetic
H,
O no
O paramagnetic
olo
Chapter 8 Solutions
EBK CHEMISTRY
Ch. 8 - Prob. 8.1PCh. 8 - What is the number and geometric arrangement of...Ch. 8 - PRACTICE 8.3 Acetic acid, CH3CO2H , is the main...Ch. 8 - APPLY 8.4 Benzene, C6H6 , is a cyclic molecule in...Ch. 8 - PRACTICE 8.5 Identify the orbitals that overlap to...Ch. 8 - APPLY 8.6 Describe the bonding in propane, C3H8 ,...Ch. 8 - PRACTICE 8.7 Describe the hybridization of the...Ch. 8 - Describe the hybridization of each carbon atom in...Ch. 8 - Which orbitals overlap to form the sigma and pi...Ch. 8 - APPLY 8.10 Describe the hybridization of the...
Ch. 8 - Prob. 8.11PCh. 8 - Conceptual APPLY 8.12 Match the following...Ch. 8 - Prob. 8.13PCh. 8 - Prob. 8.14ACh. 8 - Prob. 8.15PCh. 8 - Prob. 8.16ACh. 8 - Prob. 8.17ACh. 8 - Prob. 8.18ACh. 8 - The B2 molecule has a MO diagram similar to that...Ch. 8 - Prob. 8.20ACh. 8 - PRACTICE 8.23 Draw two resonance structures for...Ch. 8 - APPLY 8.24 Draw two resonance structures for the...Ch. 8 - Prob. 8.23PCh. 8 - Prob. 8.24PCh. 8 - Caffeine is the most widely used stimulant...Ch. 8 - Prob. 8.26PCh. 8 - What is the geometry around the central atom in...Ch. 8 - What is the geometry around the central atom in...Ch. 8 - Three of the following molecular models have a...Ch. 8 - Identify each of the following sets of hybrid...Ch. 8 - The VSEPR model is a simple predictive tool that...Ch. 8 - The following ball-and-stick molecular model is a...Ch. 8 - The following ball-and-stick molecular model is a...Ch. 8 - Prob. 8.34CPCh. 8 - The dipole moment of methanol is =1.70D . Use...Ch. 8 - Methylarnine, CH3NH2 , is responsible for the odor...Ch. 8 - Prob. 8.37CPCh. 8 - Prob. 8.38SPCh. 8 - What shape do you expect for molecules that meet...Ch. 8 - How many charge clouds are there around the...Ch. 8 - Prob. 8.41SPCh. 8 - What shape do you expect for each of the following...Ch. 8 - What shape do you expect for each of the following...Ch. 8 - What shape do you expect for each of the following...Ch. 8 - Prob. 8.45SPCh. 8 - Prob. 8.46SPCh. 8 - What shape do you expect for each of the following...Ch. 8 - What bond angles do you expect for each of the...Ch. 8 - What bond angles do you expect for each of the...Ch. 8 - Acrylonitrile is used as the starting material for...Ch. 8 - Predict values for all bond angles in dimethyl...Ch. 8 - Oceanographers study the mixing of water masses by...Ch. 8 - A potential replacement for the chlorofluorocarbon...Ch. 8 - Explain why cyclohexane, a substance that contains...Ch. 8 - Like cyclohexane (Problem 8.54), benzene also...Ch. 8 - Use VSEPR theory to answer the following...Ch. 8 - Draw an electron-dot structure for each of the...Ch. 8 - What is the difference in spatial distribution...Ch. 8 - The average CC bond dissociation energy (D) is 350...Ch. 8 - What hybridization do you expect for atoms that...Ch. 8 - What spatial arrangement of charge clouds...Ch. 8 - What hybridization would you expect for the...Ch. 8 - What hybridization would you expect for the...Ch. 8 - Oxaloacetic acid is an intermediate involved in...Ch. 8 - The atoms in the amino acid glycine are connected...Ch. 8 - Describe the hybridization of the carbon atom in...Ch. 8 - Describe the hybridization of each carbon atom in...Ch. 8 - Bupropion, marketed as Wellbutr in, is a heavily...Ch. 8 - Efavirenz, marketed as Sustiva, is a medication...Ch. 8 - What is the hybridization of the B and N atoms in...Ch. 8 - Prob. 8.71SPCh. 8 - Aspirin has the following connections among atoms....Ch. 8 - The cation [HCNXeF]+ is entirely linear. Draw an...Ch. 8 - Acrylonitrile (C3H3N) is a molecule that is...Ch. 8 - The odor of cinnamon oil is due to cinnamaldehyde,...Ch. 8 - The following molecular model is a representation...Ch. 8 - Prob. 8.77SPCh. 8 - Which of the following substances would you expect...Ch. 8 - Which of the following substances would you expect...Ch. 8 - Why is the dipole moment of SO2 1.63 D hut that of...Ch. 8 - Prob. 8.81SPCh. 8 - The class of ions PtX42 , where X is a halogen,...Ch. 8 - Prob. 8.83SPCh. 8 - Prob. 8.84SPCh. 8 - Prob. 8.85SPCh. 8 - Prob. 8.86SPCh. 8 - Prob. 8.87SPCh. 8 - What are the most important kinds of...Ch. 8 - Of the substances Xe, CH3Cl , and HF which has:...Ch. 8 - Methanol (CH3OH;bp=65C) boils nearly 230 °C higher...Ch. 8 - Prob. 8.91SPCh. 8 - Prob. 8.92SPCh. 8 - Prob. 8.93SPCh. 8 - A liquid sample contains methylamine (CH3NH2)...Ch. 8 - Prob. 8.95SPCh. 8 - What is the difference in spatial distribution...Ch. 8 - Prob. 8.97SPCh. 8 - Use the MO energy diagram in Figure 8.22b to...Ch. 8 - Use the MO energy diagram in Figure 8.22 a to...Ch. 8 - The C2 molecule can be represented by an MO...Ch. 8 - Prob. 8.101SPCh. 8 - Prob. 8.102SPCh. 8 - Prob. 8.103SPCh. 8 - Draw a molecular orbital energy diagram for Li2 ....Ch. 8 - Calcium carbide, CaC2 , reacts with water to...Ch. 8 - At high temperatures, sulfur vapor is...Ch. 8 - Carbon monoxide is produced by incomplete...Ch. 8 - Make a sketch showing the location and geometry of...Ch. 8 - Make a sketch showing the location and geometry of...Ch. 8 - Prob. 8.110MPCh. 8 - Prob. 8.111MPCh. 8 - Prob. 8.112MPCh. 8 - Prob. 8.113MPCh. 8 - Just as individual bonds in a molecule are often...Ch. 8 - Cyclooctatetraenedian ion, C8H82 , is an organic...
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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
- Compare and contrast the molecular orbital and ionic bonding descriptions of LiF.arrow_forwardIdentify the hybrid orbitals used by antimony in SbCl5 and in SbCl6, the ion formed from the reaction of SbCl5 and Cl. Explain your choices.arrow_forwardComplete the table below, which lists information about some diatomic molecules or molecular ions. In particular: • Decide whether each molecule is stable or not. Decide whether each molecule would be diamagnetic or paramagnetic. Calculate each molecule's bond order. diamagnetic or paramagnetic? molecule stable? bond order O yes O diamagnetic O no O paramagnetic O yes O diamagnetic O no O paramagnetic O yes O diamagnetic 0, O no O paramagnetic O ooooarrow_forward
- Which hybridization scheme allows the formation of at least one 7 bond? sp', sp, sp'd?arrow_forwardA bond arises from "sideways" overlap of two parallel p orbitals. The electron density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals. orbital on C+ References Use the References to access important values if needed for this question. orbital on O What atomic or hybrid orbitals make up the bond between C and O in carbon dioxide, CO2? How many o bonds does C have in CO2? How many bonds does C have? + p-orbital p-orbital atom ₁ atom 2 T bondarrow_forwardComplete the table below, which lists information about some diatomic molecules or molecular ions. In particular: • Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. • Calculate each molecule's bond order. diamagnetic or paramagnetic? molecule stable? bond order 믐 O yes diamagnetic H, ? no paramagnetic yes diamagnetic He, no paramagnetic yes O diamagnetic no paramagneticarrow_forward
- write Orbital diagram to represent electron configurations with hybridization for S in SF2. Please explain.arrow_forwardWhy must non‐bonded electrons be considered in VSEPR?arrow_forwardUsing the MO model to predict bond order and paramagnetism Complete the table below, which lists information about some diatomic molecule In particular: • Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. • Calculate each molecule's bond order. diamagnetic or paramagnetic? molecule stable? bond order Oyes diamagnetic no paramagnetic yes O diamagnetic Be, O paramagnetic no yes O diamagnetic F2 O paramagnetic no Explanation Check Type here to searcharrow_forward
- Consider a heteronuclear diatomic molecule, AB, where A and B are period 2 elements. Using the following pieces of information, provide details on the molecular orbital diagram of AB: Clue 1: The MO diagram of AB does not contain non- bonding electrons. Clue 2: The s and p orbital energies of both atoms are quite close to one another that interactions between different orbital types occur. Clue 3: AB" is more stable than AB, but AB2 is less stable than AB". Clue 4: The potential energies of the atomic orbitals of A are higher than the potential energies of the atomic orbitals of B. Table 1. Atomic orbital energies of period 2 elements. Atom Orbital energy Orbital energy (2s) (2p) Li -5.45 Ве -9.30 B -14.0 -8.30 C -19.5 -10.7 -25.5 -13.1 -32.3 -15.9 F -46.4 -18.7 Ne -48.5 -21.5arrow_forwardUse MO diagrams to place C2-, C2, and C2- in order of (a) increasing bond energy; (b) increasing bond length.arrow_forwardComplete the table below, which lists information about some diatomic molecules or molecular ions. In particular: . Decide whether each molecule is stable or not. Decide whether each molecule would be diamagnetic or paramagnetic. ● Calculate each molecule's bond order. ● molecule H₂ 2 Be2 Li₂ stable? O yes O no O yes O no OO O yes no diamagnetic or paramagnetic? O diamagnetic paramagnetic diamagnetic paramagnetic Odiamagnetic paramagnetic bond order 0 1 0 00arrow_forward
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