and the ionic formula of the compound formed. Remember metals tend to l electrons and non-metals tend to gain electrons. NUMBER OF VALENCE ELECTRONS NUMBER OF ELECTRONS LOST NUMBER OF ELECTRONS GAINED FORMULA OF ION FORMED FORMULA O COMPOUND F ATOM 1 Mg F Na P 5 2. Complete the following chart: Number of Valence Electrons Number of Electrons Needed for an Octet Number of Bonds Formed Element Boron Carbon 4 Nitrogen Phosphorous Sulphur Neon 3. Draw out the Lewis electron dot structures for the following: a] H3S1+ bl CH3CH3 c] O3 d H2CO 263 LO KN

and the ionic formula of the compound formed. Remember metals tend to l electrons and non-metals tend to gain electrons. NUMBER OF VALENCE ELECTRONS NUMBER OF ELECTRONS LOST NUMBER OF ELECTRONS GAINED FORMULA OF ION FORMED FORMULA O COMPOUND F ATOM 1 Mg F Na P 5 2. Complete the following chart: Number of Valence Electrons Number of Electrons Needed for an Octet Number of Bonds Formed Element Boron Carbon 4 Nitrogen Phosphorous Sulphur Neon 3. Draw out the Lewis electron dot structures for the following: a] H3S1+ bl CH3CH3 c] O3 d H2CO 263 LO KN

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter4: Molecular Structure And Orbitals

Section: Chapter Questions

Problem 123CP: Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron...

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Fill in the blank with the appropriate numbers for bothelectrons and bonds (considering that single bonds arecounted as one, double bonds as two, and triple bonds asthree).(a) Fluorine has valence electrons and makesbond(s) in compounds.(b) Oxygen has valence electrons and makesbond(s) in compounds.(c) Nitrogen has valence electrons and makesbond(s) in compounds.(d) Carbon has valence electrons and makesbond(s) in compounds.
Rank order of the EA of Na, Cl, Cl+, and Cs in order from least exothermic to most exothermic. Explain your ordering in terms of Coulumb forces felt by the electron at issue.
A compound is being tested for use as a rocket propellant. Analysis shows that it contains 18.54% F, 34.61%Cl, and 46.85% O.(a) Determine the empirical formula for this compound.(b) Assuming that the molecular formula is the same asthe empirical formula, draw a Lewis diagram for thismolecule. Review examples elsewhere in this chapterto decide which atom is most likely to lie at thecenter.(c) Use the VSEPR theory to predict the structure of themolecule from part (b).
One scale for electronegativity is based on the concept thatthe electronegativity of any atom is proportional to theionization energy of the atom minus its electron affinity:electronegativity = k1I - EA2, where k is a proportionalityconstant. (a) How does this definition explain why the electronegativityof F is greater than that of Cl, even though Clhas the greater electron affinity? (b) Why are both ionizationenergy and electron affinity relevant to the notion ofelectronegativity? (c) By using data in Chapter 7, determinethe value of k that would lead to an electronegativity of 4.0for F under this definition. (d) Use your result from part (c)to determine the electronegativities of Cl and O using thisscale. (e) Another scale for electronegativity defines electronegativityas the average of an atom’s first ionization energyand its electron affinity. Using this scale, calculate the electronegativitiesfor the halogens, and scale them so that fluorinehas an electronegativity of 4.0. On this…
(a) What is the trend in electronegativity going fromleft to right in a row of the periodic table? (b) How doelectronegativity values generally vary going down a columnin the periodic table? (c) True or false: The most easilyionizable elements are the most electronegative.
8.17 Specify which compound in each of the following pairsof ionic compounds should have the higher latticeenergy: (a) KCl or MgO, (b) LiF or LiBr, (c) Mg3N2 orNaCl. Explain your choice.
Given the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule.a. BF3b. NH3c. BeCl2d. PCl5*e. OF2f. SF4*g. SF6*h. XeF2*i. SnCl4j. H3O+ Set up your own table to the following formatColumn CharacteristicsA Bonding electronsB Sigma-bondsC Nonbonding electron pairsD Hybrid orbitals havingnonbonding electron pairsE Hybrid orbitals used F 3-D structureG Polar (P) or nonpolar (NP) molecule or ion lewis structure A B C D E F G
he formulas of several chemical substances are given in the table below. For each substance in the table, give its chemical name and predict its molecular structure. l> Formula Compound Name Molecular Structure msp;CO2 msp;NH3 msp;SO3 msp;H2O msp;ClO4
Which brand in each of the following pairs has the greater ionic character? msp;a.NaForNaIb.LiClorCsClc.CaSorC0d.MgNorMgP
Mixing SbCl3 and GaCl3 in a 1:1 molar ratio (using liquid sulfur dioxide as a solvent) gives a solid ionic compound of empirical formula GaSbCl6 . A controversy arises over whether this compound is (SbCl2+)(GaCl4) or (GaCl2+)(SbCl4) . (a) Predict the molecular structures of the two anions. (b) It is learned that the cation in the compound has a bent structure. Based on this fact, which formulation is more likely to be correct?
Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron in hemoglobin is the reason that CO is so toxic. The bond carbon monoxide forms to metals is through the carbon atom: MCO a. On the basis of electronegativities, would you expect the carbon atom or the oxgen atom to form bonds to metals? b. Assign formal charges to the atoms in CO. Which atom would you expect to bond to a metal on this basis? c. In the MO model, bonding MOs place more electron density near the more electronegative atom. (See the HF molecule in Figs. 4-54 and 4-55.) Antibonding MOs place more electron density near the less electronegative atom in the diatomic molecule. Use the MO model to predict which atom of carbon monoxide should form bonds to metals.
Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. In an N—O bond. electron density is greater near the O atom. An N—O bond is an example of a polar covalent band. In general, chemical bonds form to minimize energy. The bond in KBr is formed by sharing electrons.