Interpretation:
(a) By using only the valence orbitals of the oxygen atoms an MO diagram for the formation of
Concept Introduction:
Atomic number (Z) = number of protons present in the nucleus of an atom of the element = number of electrons present in a neutral atom of the element
A chemical bond is a force of attraction which holds two atoms together.
MO theory uses linear combination of atomic orbital (LCAO) method to show resulting molecular orbitals.
In MO theory first construct the orbital interaction diagram and then put in the electrons according to the aufbau principle.
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Inorganic Chemistry
- (a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .arrow_forward. Assume that the third-period element phosphorus forms a diatomic molecule, P2, in an analogous way as nitrogen does to form N2. (a) Write the electronic configuration for P2. Use [Ne2] to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?arrow_forwardCompounds such as NaBH4, Al(BH4)3, and LiAlH4 are complexhydrides used as reducing agents in many syntheses.(a) Give the oxidation state of each element in these compounds.(b) Write a Lewis structure for the polyatomic anion in NaBH4, and predict its shape.arrow_forward
- (a) Construct a molecular orbital energy diagram of N₂. (b) Use this diagram to explain why the first ionization of N₂ is greater than that of N. (b) Use this diagram to predict which is more favorable: the first electron affinity of N₂ or that of N.arrow_forwardBorane (BH3) is unstable under normal conditions, but it has been detected at lowpressure.(a) Draw the Lewis structure for borane.(b) Draw a diagram of the bonding in BH3, and label the hybridization of each orbital.(c) Predict the H¬B¬H bond anglearrow_forward(a) What are trihalomethanes (THMs)? (b) Draw the Lewisstructures of two example THMs.arrow_forward
- Describe the molecular structure around the indicated atom or atoms:(a) the sulfur atom in sulfuric acid, H2SO4 [(HO)2SO2](b) the chlorine atom in chloric acid, HClO3 [HOClO2](c) the oxygen atom in hydrogen peroxide, HOOH(d) the nitrogen atom in nitric acid, HNO3 [HONO2](e) the oxygen atom in the OH group in nitric acid, HNO3 [HONO2](f) the central oxygen atom in the ozone molecule, O3(g) each of the carbon atoms in propyne, CH3CCH(h) the carbon atom in Freon, CCl2F2(i) each of the carbon atoms in allene, H2CCCH2arrow_forward1. Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central atom. (a) POF3 (b) XeO₂F3+ (c) BrCl₂ (d) N3 (the central atom is N; two other N's are bonded to it) (e) PF3arrow_forwardThe Lewis structure of BH2Cl (a) Is the molecule polar or nonpolar? (b) What is the hybridization of the carbon atom? (c) What is the geometric shape of the molecule?arrow_forward
- In addition to Al₂Cl₆, aluminum forms other specieswith bridging halide ions to two aluminum atoms. One suchspecies is the ion Al₂Cl₇. The ion is symmetrical, with a 180° Al−Cl−Al bond angle.(a) What orbitals does Al use to bond with the Cl atoms?(b) What is the shape around each Al?(c) What is the hybridization of the central Cl?(d) What do the shape and hybridization suggest about the pres-ence of lone pairs of electrons on the central Cl?arrow_forwardChlorine dioxide gas (ClO2) is used as a commercial bleachingagent. It bleaches materials by oxidizing them. In thecourse of these reactions, the ClO2 is itself reduced. (a)What is the Lewis structure for ClO2? (b) Why do you thinkthat ClO2 is reduced so readily? (c) When a ClO2 moleculegains an electron, the chlorite ion, ClO2-, forms. Draw theLewis structure for ClO2-. (d) Predict the O—Cl—O bondangle in the ClO2- ion. (e) One method of preparing ClO2is by the reaction of chlorine and sodium chlorite:Cl2(g) + 2 NaClO2(s)------>2 ClO2(g) + 2 NaCl(s)If you allow 15.0 g of NaClO2 to react with 2.00 L of chlorinegas at a pressure of 1.50 atm at 21 °C, how many gramsof ClO2 can be prepared?arrow_forwardEach of the following properties shows a regular trend inGroup 1A(1). Predict whether each increases or decreases downthe group: (a) density; (b) ionic size; (c) E−E bond energy; (d) IE₁; (e) magnitude of ΔH(hydr) of E⁺ion.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning