10:55Hybridization of Atomic Orbitals - Sigma & Pi Bonds - Sp Sp2 Sp3The Organic Chemistry Tutor970views
Multiple ChoiceHow many of the following molecules have sp3d2 hybridization on the central atom? SeCl6 XeCl4 IF5 AsCl51514views5rank1comments
Open QuestionDraw and determine the hybridization and unhybridized orbitals for the following covalent compound. KrBr4 Hybridization: Unhybridized Orbitals:1721views7rank
Multiple ChoiceDetermine the geometry around the central oxygen atom and the molecular polarity of dimethyl ether:300views
Textbook QuestionWhich of the following molecules has a central atom with sp3 hybridization? (LO 8.4) (a) PCl5 (b) OF2 (c) CO2 (d) SF41245views
Textbook QuestionThe orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. (b) What type of hybrid orbital is produced in this hybridization?658views
Textbook QuestionThe connections between atoms in the amino acid histidine are shown. Complete the electron-dot structure by adding multiple bonds and lone pairs of electrons. Give the hybridization on the numbered carbon and nitrogen atoms. (LO 8.4) (a) N1 = sp2, N2 = sp, C1 = sp2, C2 = sp3 (b) N1 = sp2, N2 = sp2, C1 = sp3, C2 = sp2 (c) N1 = sp3, N2 = sp, C1 = sp2, C2 = sp3 (d) N1 = sp3, N2 = sp2, C1 = sp2, C2 = sp3658views
Textbook QuestionIn the hydrocarbon (a) What is the hybridization at each carbon atom in the molecule?589views
Textbook QuestionUse the chemical structure for Tagamet, a drug used to treat peptic ulcers and heartburn, to answer questions 8 and 9. Which orbitals overlap to form bond 1? (LO 8.5) (a) s bond: N 1sp22 with C 1sp22; p bond: N (p) with C (p) (b) N 1sp22 with C 1sp22 (c) s bond: N 1sp22 with C 1sp22; p bond: N 1sp22 with C 1sp22 (d) s bond: N (sp) with C 1sp22; p bond: N (p) with C (p)465views
Textbook QuestionThe drawing below shows the overlap of two hybrid orbitals to form a bond in a hydrocarbon. (b) Which of the following could be the identity of the hydrocarbon: (i) CH4, (ii) C2H6, (iii) C2H4, or (iv) C2H2? 758views
Textbook QuestionUse the chemical structure for Tagamet, a drug used to treat peptic ulcers and heartburn, to answer questions 8 and 9. Which orbitals overlap to form bond 2? (LO 8.5) (a) C (sp) with C (sp) (b) C (sp) with C 1sp22 (c) C 1sp22 with C 1sp22 (d) C 1sp32 with C 1sp22285views
Textbook QuestionThe molecule shown below is called furan. It is represented in typical shorthand way for organic molecules, with hydrogen atoms not shown, and each of the 4 vertices representing a carbon atom. (e) The C¬C¬C bond angles in furan are much smaller than those in benzene. The likely reason is which of the following: (i) The hybridization of the carbon atoms in furan is different from that in benzene, (ii) Furan does not have another resonance structure equivalent to the one above, or (iii) The atoms in a five-membered ring are forced to adopt smaller angles than in a six-membered ring.937views
Textbook QuestionThe VSEPR model is a simple predictive tool that is usually, but not always, correct. Take urea, for instance, a waste product excreted in animal urine: What hybridization would you expect for the C and N atoms in urea according to the VSEPR model, and what approximate values would you expect for the various bond angles? What are the actual hybridizations and bond angles based on the molecular model shown? 1Red = O, gray = C, blue = N, ivory = H.2640views
Textbook QuestionFor each statement, indicate whether it is true or false. (d) Nonbonding electron pairs cannot occupy a hybrid orbital.514views
Textbook QuestionConsider the molecule BF3. (c) What hybrid orbitals should be constructed on the B atom to make the B–F bonds in BF3?980views
Textbook QuestionConsider the SCl2 molecule.(d) What valence orbitals, if any, remain unhybridized on the S atom in SCl2?781views
Textbook QuestionConsider the SCl2 molecule. (c) What hybrid orbitals should be constructed on the S atom to make the S-Cl bonds in SCl2?799views
Textbook QuestionShown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle. (a) (b) (c) 739views
Textbook QuestionThe valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? c. F 2s22p5527views
Textbook QuestionThe valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? b. P 3s23p3623views
Textbook QuestionThe valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? a. Be 2s21593views
Textbook Question(c) Write the formulas for the analogous species of the elements of period 3;871views
Textbook QuestionThe valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? c. O 2s22p4424views
Textbook QuestionThe valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? a. B 2s22p14031views1rank
Textbook QuestionWrite orbital diagrams (boxes with arrows in them) to represent the electron configuration of carbon before and after sp3 hybridization.1960views
Textbook QuestionWrite orbital diagrams (boxes with arrows in them) to represent the electron configurations of carbon before and after sp hybridization.1042views
Textbook QuestionWhich hybridization scheme allows the formation of at least one p bond? sp3, sp2, sp3d22266views2rank
Textbook QuestionWhat hybridization do you expect for atoms that have the following numbers of charge clouds? (c) 4592views
Textbook QuestionWhich hybridization scheme allows the central atom to form more than four bonds? sp3, sp3d, sp21608views
Textbook QuestionBenzaldehyde, C7H6O, is a fragrant substance responsible for the aroma of almonds. Its Lewis structure is (a) What is the hybridization at each of the carbon atoms of the molecule?704views
Textbook QuestionWhat spatial arrangement of charge clouds corresponds to each of the following kinds of hybridization? (a) sp3480views
Textbook QuestionConsider the Lewis structure for acetic acid, which is known as vinegar: (a) What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?588views
Textbook QuestionConsider the Lewis structure for acetic acid, which is known as vinegar: (b) What are the hybridizations of the orbitals on the two oxygen atoms, and what are the approximate bond angles at the oxygen that is connected to carbon and hydrogen? What are the hybridizations of the orbitals on the two oxygen atoms?957views
Textbook QuestionWrite a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. c. OF2581views
Textbook QuestionWrite a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. b. NH3520views
Textbook QuestionWrite a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. CCl4936views
Textbook QuestionWrite a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. d. I3-1298views1rank
Textbook QuestionWrite a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. COCl2 (carbon is the central atom)2282views1rank
Textbook QuestionWrite a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. SO32 -714views
Textbook QuestionDescribe the hybridization of the carbon atom in the poisonous gas phosgene, Cl2CO, and make a rough sketch of the molecule showing its hybrid orbitals and p bonds.908views
Textbook QuestionWrite a hybridization and bonding scheme for each molecule that contains more than one interior atom. Indicate the hybridization about each interior atom. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. c. C2H6 (skeletal structure H3CCH3)1283views
Textbook QuestionConsider the structure of the amino acid alanine. Indicate the hybridization about each interior atom. 2227views
Textbook QuestionWhat hybridization do you expect for the atom that is underlined in each of the following species? (a) IO2-570views
Textbook QuestionConsider the structure of the amino acid aspartic acid. Indicate the hybridization about each interior atom.1316views
Textbook QuestionWhat is the hybridization of the B and N atoms in borazine, what are the values of the B¬N¬B and N¬B¬N bond angles, and what is the overall shape of the molecule?654views
Textbook Question(a) If you combine two atomic orbitals on two different atoms to make a new orbital, is this a hybrid orbital or a molecular orbital?968views1comments
Textbook QuestionBenzyne, C6H4, is a highly energetic and reactive molecule. What hybridization do you expect for the two triply bonded carbon atoms? What are the 'theoretical' values for the C¬C‚C bond angles? Why do you suppose benzyne is so reactive? 1396views
Textbook QuestionAspirin has the following connections among atoms. Complete the electron-dot structure for aspirin, tell how many s bonds and how many p bonds the molecule contains, and tell the hybridization of each carbon atom. 706views
Textbook QuestionDraw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (b) How many p bonds can the two sets of 2p orbitals make with each other?639views
Textbook QuestionThe odor of cinnamon oil is due to cinnamaldehyde, C9H8O. What is the hybridization of each carbon atom in cinnamaldehyde? How many s and how many p bonds does cinnamaldehyde have? 762views
Textbook QuestionThe following molecular model is a representation of caffeine. Identify the position(s) of multiple bonds in caffeine, and tell the hybridization of each carbon atom. 1Red = O, blue = N, gray = C, ivory = H.2 784views
Textbook QuestionThe genetic code is based on four different bases with the structures shown here. Assign a geometry and hybridization to each interior atom in these four bases. d. guanine 738views
Textbook QuestionAlthough I3- is a known ion, F3- is not. (d) Yet another classmate says F3- does not exist because F is too small to make bonds to more than one atom. Is this classmate possibly correct?1317views1rank
Textbook QuestionWhich of the following statements about hybrid orbitals is or are true? (i) After an atom undergoes sp hybridization, there is one unhybridized p orbital on the atom, (ii) Under sp2 hybridization, the large lobes point to the vertices of an equilateral triangle, and (iii) The angle between the large lobes of sp3 hybrids is 109.5°.1856views
Textbook QuestionHow many types of hybrid orbitals do we use to describe each molecule? b. C2H5NO (four C ¬ H bonds and one O ¬H bond)798views
Textbook QuestionHow many types of hybrid orbitals do we use to describe each molecule? a. N2O51154views
Textbook QuestionIndicate which orbitals overlap to form the s bonds in each compound. a. BeBr2 b. HgCl2 c. ICN1893views2comments
Textbook QuestionSodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3-. (b) State the hybridization of the central N atom in the azide ion.716views
Textbook QuestionButadiene, C4H6, is a planar molecule that has the following carbon–carbon bond lengths: (b) From left to right, what is the hybridization of each carbon atom in butadiene?845views
Textbook QuestionThe structure of borazine, B3N3H6, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar. (e) What are the hybridizations at the B and N atoms in the Lewis structures from parts (a) and (b)? Would you expect the molecule to be planar for both Lewis structures? Would you expect the molecule to be planar for both Lewis structures?1731views
Textbook QuestionAzo dyes are organic dyes that are used for many applications, such as the coloring of fabrics. Many azo dyes are derivatives of the organic substance azobenzene, C12H10N2. A closely related substance is hydrazobenzene, C12H12N2. The Lewis structures of these two substances are (Recall the shorthand notation used for benzene.) (b) How many unhybridized atomic orbitals are there on the N and the C atoms in each of the substances? How many unhybridized atomic orbitals are there on the N and the C atoms in hydrazobenzene?671views
Textbook QuestionIn the cyanate ion, OCN-, carbon is the central atom. (d) Which hybrid orbitals are used by the C atom, and how many p bonds does the C atom form?998views
Textbook QuestionCyclooctatetraene dianion, C8H8 2-, is an organic ion with the structure shown. Considering only the p bonds and not the s bonds, cyclooctatetraene dianion can be described by the following energy diagrams of its p molecular orbitals: (a) What is the hybridization of the 8 carbon atoms?1060views
Textbook QuestionMany primary amines, RNH2, where R is a carboncontaining fragment such as CH3, CH3CH2, and so on, undergo reactions where the transition state is tetrahedral. (a) Draw a hybrid orbital picture to visualize the bonding at the nitrogen in a primary amine (just use a C atom for 'R').754views
Textbook Question(c) What atomic orbitals are involved in the stacking of graphite sheets with each other?536views
Textbook QuestionAlthough polyethylene can twist and turn in random ways, the most stable form is a linear one with the carbon backbone oriented as shown in the following figure: The solid wedges in the figure indicate bonds from carbon that come out of the plane of the page; the dashed wedges indicate bonds that lie behind the plane of the page. (a) What is the hybridization of orbitals at each carbon atom? What angles do you expect between the bonds?347views
Textbook QuestionThe equilibrium constant Kc for the gas-phase thermal decom-position of cyclopropane to propene is 1.0 * 105 at 500 K: (e) Why is cyclopropane so reactive? (Hint: Consider the hybrid orbitals used by the C atoms.)289views
Open QuestionConsider the structure of the amino acid alanine. Indicate the hybridization about each interior atom.157views
Open QuestionWhat is the hybridization of the central atom of each of the following molecules?241views
Open QuestionWhich of the following hybridization schemes allows the formation of at least one π bond?238views
Open QuestionIdentify which types of orbitals overlap to form the bonds between the atoms in a benzene molecule.935views1rank
Open QuestionBy examining electron domain geometry, one can determine that the ammonia molecule (NH3) has201views
Open QuestionPredict the molecular shape and the hybridization of the central atom for: AsCl4-1, SeO4-2, BiF5-2191views
Open QuestionFluorine has 7 valence electrons. Which of the following is true of a fluorine molecule (F2)?130views
Open Questiondraw the lewis structure of azide (n₃⁻) and then determine the hybridization of the central atom.151views
Open QuestionMolecule with 3 atoms bonded to a central atom with 2 unshared pairs of electrons, such as ClF3.134views
Open QuestionDraw the lewis structure of azide (N3-) and then determine the hybridization of the central atom.213views
Open QuestionDraw the lewis structure of SCl2 and then determine the hybridization of the central atom.218views
Open QuestionJudging by the electron domain geometry, which type of hybrid orbitals does this molecule have?134views
Open QuestionHow many of the following molecules have sp2 hybridization on the central atom? HCN SO2 OCl2 XeCl2144views