Interpretation:
Among
Concept Introduction:
Molecular orbital diagram is a linear combination of atomic orbitals of similar energy and similar symmetry. It is formed by the proper overlap of the atomic orbitals.
There are 3 types of molecular orbitals as follows:
1. Bonding molecular orbital: They are formed by the constructive interference of atomic orbitals and electrons in it stabilize the molecule and are of lesser in energy.
2. Antibonding molecular orbital: This type of orbitals increases the energy of molecule and destabilizes it and weakens the bond between the atoms.
3. Non-bonding molecular orbital: These types of orbitals have energy similar to atomic orbitals that is addition or removal of electron does not change the energy of molecule.
The order of energy in molecular orbital follows two rules as follows:
1. For
2. For atomic number more than 14 order of energy is,
Electron affinity is the energy released when electron is added to gaseous atom or molecule to give negative ion.
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Chapter 2 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 1TERM
- The length of a covalent bond depends upon the size of the atoms and the bond order. For each pair of covalently bonded atoms, choose the one expected to have the shortest bond length.(A) C≡O(B) C-O ...... (A,B) fill in the blank 1(C) N=N(D) N≡N ...... (C,D) fill in the blank 2arrow_forwardSome chemical reactions proceed by the in it ial loss or transfer of an electron to a diatomic species. Which of the molecules N2, NO. O2, C2, F2, and CN would you expect to be stabil ized by (a) the addit ion of an electron to form AB-. (b) the removal of an electron to form AB+?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
- 8D.4. Benzene, a common solvent, is a covalent molecular compound which contains only carbon and hydrogen. Its simplest (empirical) formula is CH, and its molecular weight is 78 g/mol to 2 significant digits. What is its molecular formula? 8D.5. Draw the Lewis Dot Structure of (a) phosphorus pentafluoride. What is the formal charge on all atoms? (b) the perchlorate ion- in this case expand the octet for the chlorine atom in order to optimize the formal charges.arrow_forwardQUESTION 5 (31 MARKS) (a) (i) Draw a pz orbital and a d?-y² orbital. (4) (ii) What are the differences between a 5pz orbital and a 4d,- orbital in the H atom? (6) (b) (i) Draw the Lewis structure of methanol, CH3OH(8). (3) (ii) Show with a simple diagram how methanol dissolves in water. Explain. (2) (c) How does the energy and length of the carbon-oxygen bond in CH3OH(e) compare with the carbon-oxygen distance in carbon monoxide? Explain. (5) (d) Chemical bonds can be classified as polar covalent, according to and (3) (e) Chemical bonds can also be classified as single or number of according to the (2) (f) Draw the Lewis structure(s) for SO3F. Explain the structure which you have drawn. (6)arrow_forward(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe—O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in (a) yields the most favorable formal charges for the molecule?arrow_forward
- Write Lewis structures for the following: (c) C2F6 (contains a C¬C bond), (d) AsO3 3 -, (e) H2SO3 (H is bonded to O), (f) NH2Cl.. Arrange the bonds in each of the following sets in order of increasing polarity: (a) C¬F, O¬F, Be¬F; (b) O¬Cl, S¬Br, C¬P; (c) C¬S, B¬F, N¬O. What is the Lewis symbol for each of the following atoms or ions? (a) K, (b) As, (c) Sn2 + , (d) N3 Write electron configurations for the following ions and determine which have noble-gas configurations: (a) Cd2+, (b) P3-, (c) Zr4+arrow_forwardDraw Lewis electron dot diagrams for the following species: (a) methane; (b) carbon dioxide; (c) phosphorus trichloride; (d) perchlorate ionarrow_forwardDraw Lewis structures of all the important resonance forms of (a) N3₃⁻; (b) NO₂⁻.arrow_forward
- Common exceptions to the octet rule are compounds and polyatomic ions with central atoms having more than 8 electrons around them. Phosphorus pentafluoride, PF5; sulfur tetrafluoride, SF4; xenon tetrafluoride, XeF4; and tri-iodide ion, I3, are all examples of exceptions to the octet rule. (a) Draw the Lewis structures of these substances.(b) For which elements in these substances can theatoms have more than 8 electrons around them?(c) How can the atoms of the elements youidentified in Part (b) be surrounded by morethan 8 electrons?arrow_forwardIf an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? I know that group 3A atoms are elctron deficient, and that period 3 elements and below, except for group 3A elements like Aluminum, can expand their octet because of their available d-orbital, which may not be relevant to this problem. I don't understand this question, or why the answer would be 5A. Is it because 5A have odd valence electrons, and can form free radicals, like NO?arrow_forwardThere are two main types of covalent bond breakage. In ho-molytic breakage , each atom in the bond gets one of the shared electrons. In some cases, the electronega-tivity of adjacent atoms affects the bond energy. In heterolytic breakage, one atom gets both electrons and the other gets none;thus, a cation and an anion form. (a) Why is the C−C bond in H₃C−CF₃(423 kJ/mol) strongerthan that in H₃C−CH₃(376 kJ/mol)?(b) Use bond energy and any other data to calculate the heat ofreaction for the heterolytic cleavage of O₂.arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
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