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(a) Predict the geometry of the
(b) The ion
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Chapter 3 Solutions
Principles of Modern Chemistry
- The elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?arrow_forward(a) Which poisonous gas is evolved when white phosphorus is heated with Cone. NaOH solution? Write the chemical equation. (b) Write the formula of first noble gas compound prepared by N. Bartlett. What inspired N. Bartlett to prepare this compound? (c) Fluorine is a stronger oxidising agent than chlorine. Why? (d)Write one use of chlorine gas.arrow_forwardMixing SbCl3 and GaCl3 in a 1:1 molar ratio using liquid sulfur dioxide as a solvent gives a solidionic compound with the empirical formula GaSbCl6. A controversy arose over whether this compoundis [SbCl2]+[GaCl4]− or [GaCl2]+[SbCl4]−.(a) Predict the molecular structure of the two anions from the two choices using VSEPR theory.(b) It is learned that the cation in the compound has a bent structure. Based on this fact, whichformulation is the correct one?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_forward(a) (i) (ii) (iii) With the aid of a simple schematic, explain what covalent bonding is and how it is formed. What are the differences between a covalent bond and an ionic bond? Which type of bond is found in crystalline silicon? At room temperature do you expect an ionic crystal to be a good electrical conductor or a good electrical insulator? Explain why.arrow_forward. For each of the following, draw the Lewis structure, predict the ONO bond angle, and give the hybridization of the nitrogen. You may wish to review the chapters on chemical bonding and advanced theories of covalent bonding for relevant examples. (a) NO2 (b) NO-2arrow_forward
- Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.(a) PH3(b) PH4+(c) P2H4(d) PO43−(e) PF5arrow_forwardDescribe 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_forwardDescribe the molecular shape of the following: (a) NCl2+arrow_forward
- Determine the geometry of the ClF2+ ion using the VSEPR theory. Provide information about the polarity,hybrid type and Bond angle of the structure. (CL:7A,F:7A)arrow_forwardThe Electron pair geometry, molecular geometry and Hybridization for NCl3 is (a) Tetrahedral, Trigonal pyramidal, sp^3 (b) Trigonal planar, Bent, sp^2 (c) Bent, Trigonal planar, sp^2 (d) Nonearrow_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
- 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