Concept explainers
(a)
Interpretation:Themolecular orbital for the bonding between atoms in
Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. Based on energy and stability these molecular orbitals can be further classified in three types:
- Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.
- Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.
- Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.
Molecular orbital diagrams represent the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.
(b)
Interpretation:The molecular orbital for the bonding between atoms in
Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. Based on energy and stability these molecular orbitals can be further classified in three types:
- Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.
- Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.
- Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.
Molecular orbital diagrams represent the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.
(c)
Interpretation:The molecular orbital for the bonding between atoms in
Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:
- Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.
- Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.
- Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.
Molecular orbital diagrams represent the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.
(d)
Interpretation:The molecular orbital for the bonding between atoms in
Concept Introduction: Molecular orbital theory explained the bonding, magnetic and spectral properties of molecule. It is based on the formation of molecular orbitals by the combination of atomic orbitals. On the basis of energy and stability these molecular orbitals can be further classified in three types:
- Bonding molecular orbitals (BMO): They have lesser energy than atomic orbital therefore more stable compare to atomic orbital.
- Antibonding molecular orbitals (ABMO): They have higher energy than atomic orbital therefore less stable compare to atomic orbital.
- Non-bonding molecular orbitals (NBMO): They have same energy as atomic orbital.
Molecular orbital diagrams represent the distribution of electrons in different molecular orbitals in increasing order of their energy. Hence lower energy molecular orbitals occupy first then only electron moves in higher energy orbitals.
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Organic Chemistry: Structure and Function
- 2. Consider the structure of glycine, the simplest amino acid: (Lone pairs are not drawn in.) H || H2N-C-C-OH H What is the total number of t bonds in the molecule? A) 0 В) 1/2 С) 1 D) 2 E) More information is needed.arrow_forwardXeH2 has geometry and the central atom has lone pairs O Bent (Angular), 3 Trigonal Planar, 2 O Linear , 3 Bent (Angular), 4 then X=arrow_forwardSection 3: Worksheet (continued) 4. H;0 |Total number of valence electrons: Lewis structure: 3D sketch: | Molecular shape / bond angle Polar or nonpolar?arrow_forward
- What is the magnitude of the partial positive and partial negative charges in the HI molecule? (1D = 3.36 x 10¬30 c m; 1e¯ = 1.6022 x 10-19 C; bond length HI = 1.61 angstroms; dipole moment HI = 0.44 D)arrow_forwardConstruct the molecular orbital diagram for SrCl. Would yo u expect the bond length of SrCl+ to be longer or shorter than that of SrCl? Explain and elaborate.arrow_forwardPredict the molecular shape of these compounds. ammonia, NH3 H- linear trigonal pyramidal tetrahedral -H trigonal planar (120°) bent beryllium fluoride, BeF₂ bent linear Be- -F: trigonal planar (120°) trigonal pyramidal tetrahedral ammonium, NH4+ + linear trigonal pyramidal bent trigonal planar (120°) tetrahedral hydrogen sulfide, H₂S HSH trigonal planar (120°) bent trigonal pyramidal tetrahedral lineararrow_forward
- What is the molecular shape of SC3 ^6-?arrow_forward(a) State whether or not the bonding in each substance islikely to be covalent: (i) iron, (ii) sodium chloride, (iii) water,(iv) oxygen, (v) argon. (b) A substance XY, formed from twodifferent elements, boils at -33 °C. Is XY likely to be a covalentor an ionic substance?arrow_forwardPredict the molecular shape of these compounds. ammonia, NH3 ammonium, NH4+ H H- -H bent trigonal pyramidal linear tetrahedral trigonal pyramidal linear tetrahedral trigonal planar (120°) trigonal planar (120°) bent beryllium fluoride, BeF2 hydrogen sulfide, H2S -Be: H- tetrahedral linear trigonal planar (120°) tetrahedral bent trigonal pyramidal trigonal pyramidal trigonal planar (120°) linear bent ООО О O O Oarrow_forward
- 23. Given AH+ [(NF3(g)] = -132 kJ mol-¹ and the bond enthalpy (D) data, D(N₂) = 946 kJ mol-¹ and D(F2) = 159 kJ mol-, which of the following statements is/are FALSE? The average N-F bond enthalpy in NF3 is 281 kJ mol-¹. AH+ [(NF3(g)] > AH+ [(NF3(1)] AH+ [(F(8)] = 159 kJ mol-¹ CEEarrow_forwardDetermine the approximate bond angles in the following ions and molecules approx. 180 аpprox. 120 No Answers Chosen No Answers Chosen approx. 109.5 аpprax, 90 No Answers Chosen No Answers Chosen mix of 120 and 9o No Answers Chosen Possible answers | (SCNJ- (C: central atom) I (NO3)- (N: central atom) I (PO3]3- (P: central atom) I SF4 (S: central atom)arrow_forwardThe N - N - H bond angles in hydrazine N2H4 are 112°. What is the hybridization of the nitrogen orbitals predicted by valence bond theory? How many non- bonding pairs of electrons are found on each of the N centers? How many bonding pairs of electrons are there for each N-center? Use the karet symbol (^) to indicate the superscript and answer in numeric.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning