Activity 2. Strength of IMFA and Physical Properties of Covalent Compounds For each pair of molecules, identify the one with the higher boiling point (BP), melting point (MP), viscosity (VM), surface tension (ST) and vapor pressure (VP). Briefly explain your choice. BP MP V ST VP H. CI H C H. CI C CI jort eo CI Methane, CH. carbon tetrachloride. CCl. н H. H. H. Dihydrogen sulfide, H:S water, H:O H. H. H. сон н с с он H. H. Methanol, CH:OH ethanol. CHCH:OH H O нон н с с OH C C H. H. H. Acetic acid. CH:COOH acetone, CH:OCH: Brief explanation:

Activity 2. Strength of IMFA and Physical Properties of Covalent Compounds For each pair of molecules, identify the one with the higher boiling point (BP), melting point (MP), viscosity (VM), surface tension (ST) and vapor pressure (VP). Briefly explain your choice. BP MP V ST VP H. CI H C H. CI C CI jort eo CI Methane, CH. carbon tetrachloride. CCl. н H. H. H. Dihydrogen sulfide, H:S water, H:O H. H. H. сон н с с он H. H. Methanol, CH:OH ethanol. CHCH:OH H O нон н с с OH C C H. H. H. Acetic acid. CH:COOH acetone, CH:OCH: Brief explanation:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the proper ranking of the following molecules in terms of increasing strength of dispersion forces? H H H. H CC -H H C C C- H- H. H. H. O A
What kinds of attractive forces, including chemical bonds, would be present between the particles in: (d) BrCl(l ) a. dipole-dipole b. London forces c. covalent bonding d. H-bonding e. ionic bonding (e) NaCl(s) a. dipole-dipole b. London forces c. covalent bonding d. H-bonding e. ionic bonding (f) Na2SO4(s) a. dipole-dipole b. London forces c. covalent bonding d. H-bonding e. ionic bonding
11. At the end of a cooking cycle, a pressure cooker contains a mixture of water, steam, and food at a temperature of 120°C and 1.5 atm of pressure. The pressure is valve is opened and the pressure decreases, which alters water's boiling point and causes the contents of the pressure cooker to cool rapidly. Which statement best explains why the contents cooled rapidly after the pressure was released? A. Water lost heat as it vaporized. B. Water absorbed heat as it vaporized. C. Water lost heat as it condensed. D. Water absorbed heat as it condensed.
Select the compound that will have the lower equilibrium vapor pressure based on predicted intermolecular forces. pentane (C5H12) phosphorus tribromide
4. What is the relationship between a liquid's molecular weight and the strength of intermolecular bonds (assume the liquid is only compared to other liquids that lo similar intermolecular bonds)? Use the molecular structures and weights of ethano and methanol, the types of intra- and inter- molecular bonds they make and the observations you made of ethanol and methanol in this investigation to support your answer. What is different about water's molecular structure that makes water not follow this relationship when compared to ethanol and methanol?
Explain why the boiling point of Br2 (59°C) is lower than that of iodine monochloride, ICl (97°C), even though they have nearly the same molar mass.Choose one: A. Br2 is larger than ICl. B. The molar mass is not identical: the molar mass of Br2 is only 159.80 g/mol compared to 162.35 g/mol for ICl. C. ICl is ionic. D. ICl is polar while Br2 is nonpolar. E. It is impossible to say without further information. F. The molar mass dependence of a liquid's boiling point is not an absolute rule, and it should not be applied to all of the compounds.
Mars has a very thin atmosphere with a pressure of 610 Pa, less than 1% of the pressure found on Earth. The atmosphere on Mars is also composed of 95% CO2. Calculate the mass of CO, that would dissolve in 1.0 kg of water on Mars at 0 °C. Data: Henry's Law constant for CO2 at 0 °C is 7.28 x 102 atm 0.44 mg 0.26 mg 19 mg 0.89 mg 7.9 mg
QUESTION 5 Which of the following compounds would be most soluble in carbon tetrachloride, C14 (non-polar molecule)? O A. H20 (polar molecule) O B. C6H6 (non-polar molecule) O C. CH3OH (polar molecule) O D. HCI (polar molecule) O E. NH3 (polar molecule)
8. Identify the substance in each of the following pairs that would have the higher melting point and explain. a. Nacl or HCI b. NH3 or PH3 W DELL DELL
Which of the following statements is correct about the lattice energy and hydration of ionic solids in water? a. The lattice energy of Bas is more exothermic than MgO. b. The lattice energy of NaCl is more exothermic than CsBr. O. The hydration cenergy of BaF2 is more exothermic than CaF2. d. The hydration energy of NaCl is more exothermic than LICI. The lattice energy of KF is more exothermic than CaF). е.
4. Arrange the following in order of increasing melting point: NaCl, H2O, CH4, C6H4(OH)2. A. CH4 < H2O < NaCl < C6H4(OH)2 B. NaCl < H2O < CH4 < C6H4(OH)2 C. CH4 < NaCl < C6H4(OH)2 < H2O D. CH4 < H2O < C6H4(OH)2 < NaCl E. CH4 < C6H4(OH)2 < H2O < NaCl
The strongest intermolecular interactions between pentane (C 5H 12) molecules arise from: O dispersion forces. covalent bond forces. dipole-dipole attraction. hydrogen bonding. ionic interactions. Previous