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a)
Interpretation: The molecular electronic configuration of
Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.
Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.
Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.
In sigma
In pi
In pi
b)
Interpretation: The bond order of
Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.
Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.
Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.
In sigma
In pi
In pi
c)
Interpretation: The species that is paramagnetic should be determined.
Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.
Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.
Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.
In sigma
In pi
In pi
d)
Interpretation: The ion that has high
Concept introduction: Two or more than two atomic orbitals overlap to form bond, these orbitals are called molecular orbitals. Count of molecular orbital obtained is same as count of atomic orbitals mixed.
Two forms of molecular orbital are obtained. These are bonding and antibonding orbital.
Bonding orbitals are those in that electrons are in between nucleus of two atom. Antibonding orbitals are those in which electrons are away from nucleus of two-atom. Also, electrons in antibonding orbital have energy high as compared to bonding orbital.
In sigma
In pi
In pi
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Chapter 6 Solutions
Bundle: Principles of Modern Chemistry, 8th + OWLv2, 1 term (6 months) Printed Access Card
- In 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_forwardWhat are the relationships among bond order, bond energy, and bond length? Which of these quantities can be measured?arrow_forwardNitrogen trifluoride (NF3) is used in the electronics industry to clean surfaces. NF3 is also a potent greenhouse gas. (A) Draw the Lewis structure of NF3 and determine its molecular geometry. (B) BF3 and NF3 both have three covalently bonded fluorine atoms around a central atom. Do they have the same dipole moment? (C) Could BF3 also behave as a greenhouse gas? Explain why or why not.arrow_forward
- Determine the electron configurations for CN+, CN, andCN-. (a) Which species has the strongest C¬N bond?(b) Which species, if any, has unpaired electrons?arrow_forwardThe structure of caffeine is shown below. (a) Complete the Lewis structure. (b) How many pi bonds are present in caffeine? How many sigma bonds? (c) Identify the hybridization of the carbon atoms. (d) What is the value of the O-C-N angle?arrow_forwardThe lactic acid molecule, CH3CH(OH)COOH, gives sourmilk its unpleasant, sour taste. (a) Draw the Lewis structurefor the molecule, assuming that carbon always forms fourbonds in its stable compounds. (b) How many π and howmany σ bonds are in the molecule? (c) Which CO bond isshortest in the molecule? (d) What is the hybridization ofatomic orbitals around the carbon atom associated withthat short bond? (e) What are the approximate bond anglesaround each carbon atom in the molecule?arrow_forward
- 7. Nitrogen is the central atom in each of the species given. (a) Draw the Lewis electron-dot structure for each of the species. + NO₂ NO₂ NO₂ (b) List the species in order of increasing bond angle. Justify your answer. (c) For NO₂ and NO₂, give the hybridization of the nitrogen atom in it. (d) Identify the only one of the species that dimerizes and explain what causes it to do so.arrow_forwardButadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths: (a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.arrow_forward(a) How does a polar molecule differ from a nonpolar one? (b) Atoms X and Y have different electronegativities. Will the diatomic molecule X—Y necessarily be polar? Explain. (c) What factors affect the size of the dipole moment of a diatomic molecule?arrow_forward
- (a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?arrow_forwardA useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers.(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds.(c) Describe the atomic orbitals that form the π bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.arrow_forwardUse valence bond theory to explain the bonding in F2, HF, and ClBr. (a) F2 This molecule is symmetrical. The single bond present in this molecule is derived from the overlap of two (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbitals contributed by each of the F atoms. (b) HF This molecule is asymmetrical. The single bond present in this molecule is derived from the overlap of one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the H atom and one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the F atom. (c) ClBr This molecule is also asymmetrical. The single bond present in this molecule is derived from the overlap of one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the Cl atom and one (1s, 2s, 2p, 3s, 3d, 3p, 4s, 4d, 4p) orbital contributed by the Br atom. Sketch the overlap of the atomic orbitals involved in the bonds.arrow_forward
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