Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 8, Problem 36E
Can a molecule with an even number of electrons ever be paramagnetic? Explain why or why not.
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Why oxygen molecules are considered to be paramagnetic?
Explain the difference between a paramagnetic species and a diamagnetic one.
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
yes
diamagnetic
N.
2
no
paramagnetic
yes
diamagnetic
H
2
no
paramagnetic
diamagnetic
Li,
+
yes
no
paramagnetic
OO O
Chapter 8 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 8 - Explain how and bonds are similar and how they...Ch. 8 - Draw a curve that describes the energy of a system...Ch. 8 - Explain why bonds occur at specific average bond...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - How many and bonds are present in the molecule...Ch. 8 - A friend tells you N2 has three bonds due to...Ch. 8 - Draw the Lewis structures for CO2 and CO, and...Ch. 8 - Why is the concept of hybridization required in...Ch. 8 - Give the shape that describes each hybrid orbital...
Ch. 8 - Explain why a carbon atom cannot form five bonds...Ch. 8 - What is the hybridization of the central atom in...Ch. 8 - A molecule with the formula AB3 could have one of...Ch. 8 - Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino...Ch. 8 - Sulfuric acid is manufactured by a series of...Ch. 8 - Two important industrial chemicals, ethene, C2H4,...Ch. 8 - For many years after they were discovered, it was...Ch. 8 - Consider nitrous acid, HNO2 (HONO). (a) Write a...Ch. 8 - Strike-anywhere matches contain a layer of KClO3...Ch. 8 - Identify the hybridization of each carbon atom in...Ch. 8 - Write Lewis structures for NF3 and PP5. On the...Ch. 8 - In addition to NF3, two other fluoro derivatives...Ch. 8 - The bond energy of a C—C single bond averages 347...Ch. 8 - For the carbonate ion, CO32, draw all of the...Ch. 8 - A useful solvent that will dissolve salts as well...Ch. 8 - For the molecule allene, H2C=C=CH2, give the...Ch. 8 - Identify the hybridization of the central atom in...Ch. 8 - Describe the molecular geometry and hybridization...Ch. 8 - For each of the following molecules, indicate the...Ch. 8 - For each of the following structures, determine...Ch. 8 - Draw the orbital diagram for carbon in CO2 showing...Ch. 8 - Sketch the distribution of electron density in the...Ch. 8 - How are the following similar, and how do they...Ch. 8 - If molecular orbitals are created by combining...Ch. 8 - Can a molecule with an odd number of electrons...Ch. 8 - Can a molecule with an even number of electrons...Ch. 8 - Why are bonding molecular orbitals lower in energy...Ch. 8 - Calculate the bond order for an ion with this...Ch. 8 - Explain why an electron in the bonding molecular...Ch. 8 - Predict the valence electron molecular orbital...Ch. 8 - Determine the bond order of each member of the...Ch. 8 - For the first ionization energy for an N2...Ch. 8 - Compare the atomic and molecular orbital diagrams...Ch. 8 - Which of the period 2 homonuclear diatomic...Ch. 8 - A friend tells you that the 2s orbital for...Ch. 8 - True or false: Boron contains 2s22p1 valence...Ch. 8 - What charge would be needed on F2 to generate an...Ch. 8 - Predict whether the MO diagram S2 would show s-p...Ch. 8 - Explain why N22+ is diamagnetic, while O24+, which...Ch. 8 - Using the MO diagrams, predict the bond order for...
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- Which of the period 2 homonuclear diatomic molecules are predicted to be paramagnetic?arrow_forwardIn each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.arrow_forwardDistinguish between nonbonding and bonding atomic radii within a molecule?arrow_forward
- 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 Oyes diamagnetic H, no paramagnetic yes diamagnetic B, no paramagnetic yes diamagnetic He, no paramagneticarrow_forward3 2 4 5 Consider the following second-period heteronuclear diatomic molecule. Combining the valence orbitals (2px, 2py, 2pz, and 2s) of each of the two atoms creates eight new orbitals (one 02s*, one 02s, one 02p, one 02p, two л₂p, and two л₂p) that span the entire molecule and explain it's electronic properties. Those eight new orbitals exist at six energy levels. Rank the molecular orbitals of a F2 molecule from lowest (1) to highest (6) energy. Fatom 6- highest 1- lowest F2 molecule [Choose ] [Choose ] [Choose ] [Choose ] [Choose ] [Choose ] F atomarrow_forwardAre CH3+ and CH3 ̄ symmetrical or unsymmetrical molecules? Explain your reasoning.arrow_forward
- 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 oloarrow_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 Oyes diamagnetic Li, no paramagnetic yes diamagnetic B. no paramagnetic + yes diamagnetic Be, no paramagnetic O Oarrow_forwardWhy are Lewis dot structures used to predict the three dimensional shape of molecules?arrow_forward
- FF Xe FF wireframe labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many F atoms are bonded to the central Xe atom? [ Do all of the atoms in XeF4 lie on a plane? [yes A molecule with square planar geometry would result if two of the outer atoms were removed from an octahedral molecule. Does it matter which two of the outer atoms are removed?[ If two adjacent outer atoms were removed from an octahedral molecule, the resulting geometry would most closely resemble a geometry. Are all of the outer atoms geometrically equivalent in a square planar molecule or are there two types? [ What approximate angle at the Xe atom does an F atom make with an F atom that is adjacent to it? [ What approximate angle at the Xe atom does an F atom make with an F atom that is opposite from it? For practice, type in the name of the geometry of the molecule: [ degrees. degrees.arrow_forwardIs it possible for a molecule with polar bonds to be non-polar? Why or why not?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
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