Concept explainers
(a)
Interpretation: The hybridization of the orbitals having unshared pair of electrons in
Concept Introduction: The hybridization is defined as mixing of atomic orbitals. The new hybrid orbitals are formed equal in the number of atomic orbitals involved in the mixing.
(b)
Interpretation: The relative abilities of
Concept Introduction: The hybridization is defined as mixing of atomic orbitals. The new hybrid orbitals are formed equal in the number of atomic orbitals involved in the mixing.
(c)
Interpretation: The given species needs to be ranked in order of the acid strength.
Concept Introduction: The species which can form stable negative charge will be most acidic because it will readily donate hydrogen atom to attain stability.
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Organic Chemistry: Structure and Function
- Identify the hybridization of each underlined atom in the following compounds and ions: (a) B_H4 (b) H2C_=C_HC_H3 (c) BCl3arrow_forward. For each of the diatomic species listed below, sketch an appropriate molecular orbitaldiagram. In your diagram be sure to show all the contributing atomic orbitals, the molecularorbitals generated, and place all necessary electrons. Be sure to calculate the bond orderand indicate whether the species is diamagnetic or paramagnetic.(a) Br2+(b) BC‒(c) NeO(d) OH‒arrow_forwardDichloroethylene (C2H2Cl2) has three forms (isomers), eachof which is a different substance. (a) Draw Lewis structures ofthe three isomers, all of which have a carbon–carbon doublebond. (b) Which of these isomers has a zero dipole moment?(c) How many isomeric forms can chloroethylene, C2H3Cl,have? Would they be expected to have dipole moments?arrow_forward
- 3) Which statement best describe the structure of a carbonate anion C02- ? A) The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are 120°. There is a n-bond formed between a non-hybridized "C" p-orbital overlapping with an "O" p-orbital. C) The electron geometry of carbon in a carbonate anion is trigonal planar with a sp2 hybridization and bond angles are 120°. There is a 7-bond formed between a non-hybridized “C" p-orbital overlapping with an “O" p-orbital.arrow_forwardUse MO diagrams and the bond orders you obtain fromthem to answer: (a) Is O₂⁻ stable? (b) Is O₂⁻ paramagnetic? (c) What is the outer (valence) electron configuration of O₂⁻?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_forward
- Sodium azide is a shock-sensitive compound that releases N2upon physical impact. The compound is used in automobileairbags. The azide ion is N3-. (a) Draw the Lewis structure of theazide ion that minimizes formal charge (it does not form a triangle).Is it linear or bent? (b) State the hybridization of the centralN atom in the azide ion. (c) How many σ bonds and how manyπ bonds does the central nitrogen atom make in the azide ion?arrow_forwardLactic acid is a natural compound found in sour milk. (a) How many π bond occur in lactic acid? How many u bonds? (b) What is the hybridization of atoms 1, 2, and 3? (c) Which CO bond is the shortest in the molecule ? Which CO bond is the strongest? (d) What are the approximate value of the bond angles A, B and C?arrow_forwardButadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths:(a) Predict the bond angles around each of the carbon atomsand sketch the molecule. (b) From left to right, whatis the hybridization of each carbon atom in butadiene?(c) The middle C¬C bond length in butadiene (1.48 Å) isa little shorter than the average C¬C single bond length(1.54 Å). Does this imply that the middle C¬C bond in butadieneis weaker or stronger than the average C¬C singlebond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might supportthe shorter middle C¬C bond.arrow_forward
- (a) State the hybrid orbitals for C1,C2,O1 and O2 (b) state the number of π bonds present (c) State teh number of C atoms with sp2 hybridization.arrow_forward1. Phosphine (PH3) reacts with borane (BH3) as follows: PH3 + BH3 → H3P--BH3 (a) Which of the illustrations below depicts the change, if any, in the orbital hybridization of P during this reaction? (b) Which depicts the change, if any, in the orbital hybridization of B? 2. The illustrations below depict differences in orbital hybridization of some tellurium (Te) fluorides. (a) Which depicts the difference, if any, between TeF6 (left) and TeFs- (right)? (b) Which depicts the difference, if any, between TeF4 (left) and TeF6 (right)? and and and and Darrow_forwardWhich compound in each of the following pairs would you expect to have the greaterdipole moment μ? Why?(a) HF or HCl (d) CHCl3 or CCl3F(b) HF or BF3 (e) CH3NH2 or CH3OH(c) (CH3)3CH or (CH3)3CCl (f) CH3NH2 or CH3NO2arrow_forward
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