![]() The radius of the unknown atom is _ Å.Į) Insufficient data is given. The length of the unit cell edge is 2.85 Å. T 1) Molecular solids consist of atoms or molecules held together by _.ĭ) London dispersion forces and hydrogen bonds onlyĮ) dipole-dipole forces, London dispersion forces, and/or hydrogen bonds E An unknown metal crystallizes in a primitive cubic unit cell. (iv) Molecules in covalent-network solids are connected via a network of covalent bondsĪ) (i) B) (ii) C) (iii) D) (iv) E) none B) ii What portion of the volume of each atom or ion on the face of a unit cell is actually within the unit cell?Į) none of it C A metallic material that is composed of two or more elements is called a(n) _.Į) pure metal A If the electronic structure of a solid substance consists of a valence band that is completely filled with electrons and there is a large energy gap to the next set of orbitals, then this substance will be a(n) _.Į) insulator E The process of _ can produce an n-type semiconductor, which can greatly increase intrinsic conductivity.Į) doping E T/F? Many metals are ductile, which means that they can be drawn into thin wires. (iii) Ionic solids have formula units in the point of the crystal lattice. (ii) Metallic solids have atoms in the points of the crystal lattice. (i) Molecules or atoms in molecular solids are held together via ionic bonds. A) molecularĮ) covalent network D All of the following can form a solid with a lattice structure similar to that of sodium chloride except _.Į) NaF B Consider the following statements about crystalline solids: This is a(n) _ solid.Į) metallic A All of the following are a type of solid except _. Substance, Molecular Mass (amu), Dipole MomentĪcetonitrile, CH3CN 41 3.9 CH3CN Crystalline solids _.ī) have their particles arranged randomlyĮ) are usually very soft C In liquids, the attractive intermolecular forces are _.Ī) strong enough to keep the molecules confined to vibrating about their fixed lattice pointsī) not strong enough to keep molecules from moving past each otherĬ) strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each otherĭ) very weak compared with kinetic energies of the moleculesĮ) strong enough to hold molecules relatively close together C Which molecule has hydrogen bonding as the predominant intermolecular force?Į) C4H10 A Which species has London dispersion forces as the only intermolecular force?Į) KBr B What types of intermolecular forces exist between NH3 and H2O?ī) dispersion forces, hydrogen bonds, and ion-dipole forcesĬ) dispersion forces and ion-dipole forcesĭ) dispersion forces, dipole-dipole forces, and hydrogen bondsĮ) dispersion forces D _ is the energy required to expand the surface area of a liquid by a unit amount of area.Į) Surface tension E Based on the following information, which compound has the strongest intermolecular forces? Substance ΔHvap (kJ/mol)Ī) Water B) Methane C) Benzene D) Argon E) Ethanol A A volatile liquid is one that _.Į) readily evaporates E A solid has a very high melting point, great hardness, and poor electrical conduction. ![]() T T/TF? Heats of vaporization are greater than heats of fusion T T/F? Under ordinary conditions, a substance will sublime rather than melt if its triple point occurs at a pressure above atmospheric pressure T Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? ![]() increase T/F? The boiling points of normal hydrocarbons are higher than those of branched hydrocarbons of similar molecular weight because the London-dispersion forces between normal hydrocarbons are greater than those between branched hydrocarbons. melting London Dispersion Forces tend to _ in strength with increasing molecular weight. The conversion of 50.0 mol of ice at 0.00 C to water at 0.00 requires _ kj of heat.ĭ) 17.2 C Of the following, _ is the most volatileĮ) C2F6 B) C2H6 Which molecule is the least volatile?Į) CH3Br B) CH3I The conversion of a solid to a liquid is called _. In the example given, Q 1 = +1(1.6022 × 10 −19 C) and Q 2 = −1(1.The enthalpy change for converting 1 mol of ice at -25 C to water at 50 C is_ kJ.Į) 8.83 A) The enthalpy change for converting 10.0 mol of ice at -50 C to water at 50 C is _ kJ.ĭ) 17.2 B The heat of fusion of water is 6.01 kJ/mol. In this case, the proportionality constant, k, equals 8.999 × 109 J The equation can also be written using the charge of each ion, expressed in coulombs (C), incorporated in the constant. This value of k includes the charge of a single electron (1.6022 × 10 −19 C) for each ion. The proportionality constant k is equal to 2.31 × 10 −28 J Where each ion’s charge is represented by the symbol Q.
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