Indicate the strongest force holding the crystals together in the following substances by putting a check on the appropriate box. The first five substances were done for you. TYPES OF CRYSTAL Molecular Metallic lonic Covalent Network Substance Dispersio Dipole- dipole Hydroge n bonds Metallic bonds lonic Covalent n bonds Network forces attraction 1 Kr HF 3 NO 4 Al K.S NH, 7 HCI KMNO, so, co, Si 8 10 11 Sio, Coreonite CH,OH Ag 12 13 14 15 16 Ba(OH) 17 Сао 18 Pb 19 20 Cu

Indicate the strongest force holding the crystals together in the following substances by putting a check on the appropriate box. The first five substances were done for you. TYPES OF CRYSTAL Molecular Metallic lonic Covalent Network Substance Dispersio Dipole- dipole Hydroge n bonds Metallic bonds lonic Covalent n bonds Network forces attraction 1 Kr HF 3 NO 4 Al K.S NH, 7 HCI KMNO, so, co, Si 8 10 11 Sio, Coreonite CH,OH Ag 12 13 14 15 16 Ba(OH) 17 Сао 18 Pb 19 20 Cu

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter21: Structure And Bonding In Solids

Section: Chapter Questions

Problem 54AP

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B. Indicate the strongest force holding the crystals together in the following substances by putting a check on the appropriate box. The first five substances were done for you. TYPES OF CRYSTAL 1 2 3 4 5 6 7 8 9 Substance Kr HF NO Al K₂S NH3 HC1 KMnO4 SO₂ CO₂ Si SiO₂ 10 11 12 13 14 15 Ag 16 17 18 19 12 20 Cgraphite CH3OH Ba(OH)2 CaO PH Cu Dispersion forces Molecular Dipole- dipole attraction Hydrogen bonds Metallic Ionic Metallic bonds Ionic bonds Covalent Network Covalent bonds
The melting point of TiCl4 (-24°C) lies below those ofTiF4 (284°C) and TiBr4 (38°C). Explain why by considering the covalent-ionic nature of these compounds and theintermolecular forces in each case.
Quartz crystals are made of silicon dioxide. What is the molecular geometry of silicon dioxide? (*hint* sketch the molecule before answering) O Linear O Bent O Trigonal Pyramidal O Tetrahedral
Why don’t metals cleave in the waydepicted here for ionic substances?
Explain the term crystal radii?
12. Which best explains why an aluminum can may be crushed without it breaking into pieces? (A) Aluminum has ionic bonds that are not easily broken. (B) Aluminum has covalent bonds that are not easily broken. (C) Aluminum has localized valence electrons with direc- tional bonding. (D) Aluminum has delocalized valence electrons with nondi- rectional bonding. 13. Which of the following is true for a solid with a structure as shown in the diagram below? 6+ 8-6+ 8-6+ 8-6+ 8-6+ 8-6+ 8- 8- 6+68+68+68+68+68+ 6+ 8-6+ 8-6+ 8-6+ 8-6+ 8-6+ 8- 8-88-8+68+68+68+68+ (A) It is an atomic solid and consists of atoms with electro- static attractions. (B) It is an ionic solid and consists of ions held together by electrostatic attractions. (C) It is a molecular solid and consists of polar molecules with dipole-dipole attractions. (D) It is a molecular solid and consists of nonpolar mol- ecules with intermolecular forces. 14. Which of these correctly matches the molecular compound with the most important…
Given the following thermodynamic data, calculate the lattice energy of LiCl:ΔH°f[LiCl(s)] = -409 kJ/molΔH°sublimation [Li] = 161 kJ/molBond energy [Cl-Cl] = 243 kJ/molIE1 (Li) = 520 kJ/molEA1 (Cl) = -349 kJ/mol -1682 kJ/mol -984 kJ/mol -1560 kJ/mol -862 kJ/mol -1213 kJ/mol
3 4 5 6 7 8 9 10 11 12 13 14 15 uestion 1 2 The bonds between particles in a solid are very weak. O True O False 多

What are the network covalent atomic solids are composed of?
Describe the fourteen Bravais lattices
7. During a lab, a student filled in the following table regarding three unknown substances that could be jonic, molecular/covalent or metallic. Determine the type of bond based on the data: Appearance at room temperature Fine white solid crystals Conductivity of aqueous solution Melting point (high or low) Solubility in Conductivity of solid Type of Bond in substance Unknown water Non- A Soluble conductive High conductive Non- White solid shiny crystals Dull hard grey solid strip with shiny interior. Malleable. Non- B. Soluble Low conductive conductive Non- High insoluble high conductive conductivity
A paper published in the research Journal Science in 2007 (S. Vallina and R. Simo, Science, Vol. 315, p. 506, January 26, 2007) reported studies of dimethylsulfide (DMS), an important green-house gas that is released by marine phytoplankton. This gas represents the largest natural source of atmospheric sulfur and a major precursor of hygroscopic (i.e., cloud-forming) particles in clean air over the remote oceans, thereby acting to reduce the amount of solar radiation that crosses the atmosphere and is absorbed by the ocean. (a) Sketch the Lewis structure of dimethylsulfide, CH3SCH3, and list the bond angles in the molecule. (b) Use electronegativities to decide where the positive and negative charges lie in the molecule. Is the molecule polar? (c) The mean seawater concentration of DMS in the ocean in the region between 15 north latitude and 15 south latitude is 2.7 nM (nanomolar). How many molecules of DMS are present in 1.0 m3 of seawater?