1 3 Identify specifically the type of bonding in each of the three substances as either ionic, polar covalent, or non-polar covalent. Justify each choice with a supporting statement related to the evidence provided in the table. Criteria: I can describe the general properties of ionic and molecular compounds and explain how these properties are a result of the forces between particles with accuracy, clarity, and logic. Substance State at Room Melting Point Boiling point Temperature Solubility in Water Type of Bonding -20 78 soluble liquid solid 725 1025 soluble -10 -63 gas insoluble

1 3 Identify specifically the type of bonding in each of the three substances as either ionic, polar covalent, or non-polar covalent. Justify each choice with a supporting statement related to the evidence provided in the table. Criteria: I can describe the general properties of ionic and molecular compounds and explain how these properties are a result of the forces between particles with accuracy, clarity, and logic. Substance State at Room Melting Point Boiling point Temperature Solubility in Water Type of Bonding -20 78 soluble liquid solid 725 1025 soluble -10 -63 gas insoluble

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.95PAE

See similar textbooks

Similar questions

Predict the arrangement of the atoms about the sulfuratom in F4SPO, assuming that double-bonded atomsrequire more space than single-bonded atoms.
The VSEPR model was developed before any xenon com-pounds had been prepared. Thus, these compounds provided anexcellent test of the model’s predictive power. What would youhave predicted for the shapes of XeF₂, XeF₄, and XeF₆?
The compound gallium arsenide is a commonly used semiconductor,having an energy gap Eg of 1.43 eV. Its crystal structureis like that of silicon, except that half the silicon atoms are replacedby gallium atoms and half by arsenic atoms. Draw a flattened-outsketch of the gallium arsenide lattice, following the pattern.What is the net charge of the (a) gallium and (b) arsenic ioncore? (c) How many electrons per bond are there? (Hint: Consultthe periodic table in Appendix G.)
Draw a molecular level picture and use it to describe the model(s) of bonding present in each substance.CopperGraphiteDiamond
(a) Using the electronegativities of Br and Cl, estimate thepartial charges on the atoms in the Br¬Cl molecule. (b) Usingthese partial charges and the atomic radii given in Figure7.8, estimate the dipole moment of the molecule. (c) Themeasured dipole moment of BrCl is 0.57 D. If you assume thebond length in BrCl is the sum of the atomic radii, what arethe partial charges on the atoms in BrCl using the experimentaldipole moment?
A non-bonding like oxoygen, O, forms both ionic and covalent bonds, depending on the identy of the elementto which it donds. What type of bonding is observed in CaO and CO? Expain why two different types of bonding are observed.
1) Answer the following questions using principles of chemical bonding and molecular structure. (a) Consider the carbon dioxide molecule, CO2, and the carbonate ion, CO32– (i) Draw the complete Lewis electron-dot structure for each species. (ii) Account for the fact at the carbon-oxygen bond length in CO32– is greater than the carbon-oxygen bond length in CO2. 2) Explain the following in terms of the electronic structure and bonding of the compounds considered. (a) Liquid oxygen is attracted to a strong magnet, whereas liquid nitrogen is not. (b) The SO2 molecule has a dipole moment, whereas the CO2 molecule has no dipole moment. Include the Lewis (electron-dot) structures in your explanation. 3) Answer the following questions using principles of chemical bonding and molecular structure: (a) Consider the molecules CF4 and SF4. (i) Draw the complete Lewis electron-dot structure for each molecule. (ii) In terms of molecular geometry, account for the fact that the…
The percent ionic character of a bond between elements A and B may be approximated by the expression %IN = 100[1 - e^(-1/4(XA - XB))], where XA and XB are the electronegavities for the respective elements. What is the the percent ionic character of the interatomic bonds for Fe2O3? What type of bonding would you expect in Fe2O3? Note: Use 1.8 for the electronegativity for Fe and 3.5 for the electronegativity for O.
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.
Draw the Lewis electron dot structures for these molecules, including resonance structures where appropriate: (a) CS32 (b) CS2 (c) CS (d) predict the molecular shapes for CS32 and CS2 and explain how you arrived at your predictions
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.
7.56 Draw the Lewis dot structures of the following compounds and identify the number of pi bonds in each. (a) Cl2O , (b) H2CCH2 , (c) HCCCN , (d) SiO2