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Concept explainers
Interpretation: Thebond length of
Concept Introduction:
Molecular orbital theory explained the bonding, magnetic and spectral properties of the 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 the 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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Chapter 3 Solutions
Bundle: Principles of Modern Chemistry, 8th + OWLv2, 1 term (6 months) Printed Access Card
- If a C-O bond length is 1.66 pm and a C=O bond length is 1.52 pm, how long would the carbon oxygen bonds in the carbonate ion be?arrow_forwardCovalent bonds: H―HC―HO―HO═O C≡O Bond energy (kJ/mol):4364154654981080Calculate the enthalpy change (H, in kJ/mol) for the following reaction and indicate whether the reaction is exothermic or endothermic.(*BE for C═Oin CO2)(a) CH4(g)+ H2O(g)CO(g)+ 3H2(g);arrow_forwardPredict whether the bonds in the following compounds are ionic or covalent: (a) NaI (sodium iodide); (b) H 2O 2 (hydrogen peroxide).arrow_forward
- Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forwardCalculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forwardCompounds (1) C4H6Cl2 and (2) AlCl3. Explain the difference between them using the following categories. Types of bonding? The number of chlorine atom of each one?arrow_forward
- Except for nitrogen, the elements of Group 5A(15) all form pentafluorides and most form pentachlorides. The chlorine atoms of PCI5 can be replaced with fluorine atoms one at a time to give, successively, PCI4F, PCI3F2, ..., PF5. (a) Given the relative sizes of F and Cl, would you expect the first two F substitutions to be at axial or equatorial positions? О axial O equatorial This answer has not been graded yet. (b) Which of the five fluorine-containing molecules have no dipole moment? (Select all that apply.) O PCI3F2 O PCI2F3 O PCIF4 O PF5 O PCI4Farrow_forward2) Using bond energies, verify that the complete combustion of ethene gas, C2 H4 (g) (H2C = CH2), to gaseous carbon dioxide and the water is an exothermic reaction.arrow_forwardChoose the best Lewis structure for C2H30¯. (It will help to work out the missing formal charges for the atoms in these different structures) [Image description: Lewis structure A two C atoms doubly bound to each other. One C has two other single bonds to H atoms. The other C has one more single bond to a H atom and one more single bond to a O atom. There are three electron pairs on O. Lewis structure B has a C atom and a O atom doubly bound to each other. The C has two other single bonds to H atoms. The O has one more single bond to a H atom and one more single bond to a C atom. There are three electron pairs on this C. Lewis structure C has a O atom and a C atom doubly bound to each other. The O has two other single bonds to H atoms. The C has one more single bond to a H atom and one more single bond to another C atom. There are three electron pairs on this C. Lewis structure D has two C atoms singly bound to each other. One C has an electron pair plus two more single bonds to H…arrow_forward
- Acetylene (C2H2) and nitrogen (N2) both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O5(g) and of acetylene to formCO2(g) and H2O(g). (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O5(g) is 11.30 kJ/mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forwardPhosphorus forms a number of oxohalides, X3PO, in which X may be a F, Cl, or Br atom. The most common of these, phosphoryl chloride, is obtained through the reaction 2 PC1₂(g) + O₂(g) → 2 Cl₂PO(g) Draw the Lewis structure for phosphoryl chloride (Cl3PO). Optimize formal charges. Select / |||||| Draw P Cl O Templates More Erasearrow_forwardFor each of the following covalent bonds: (a) use the symbols δ+ and δ- to indicate the direction of polarity (if any).(a) C-F; (b) N-Br; (c) B-C; (d) Si-H(b) Rank the following covalent bonds in order of increasing polarity. (i) C-H, O-H, N-H; (ii) C-N, C-O, B-O; (iii) C-P, C-S, C-Narrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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