CHAPT 11 PRACTICE TEST 1 WHAT IS POLARIZABILITY? THE

CHAPTER 11 OECD AVERAGE AND OECD TOTAL BOX
 CONTENTS PREFACE IX INTRODUCTION 1 REFERENCES 5 CHAPTER
 NRC INSPECTION MANUAL NMSSDWM MANUAL CHAPTER 2401 NEAR‑SURFACE

32 STAKEHOLDER ANALYSIS IN THIS CHAPTER A STAKEHOLDER ANALYSIS
CHAPTER 13 MULTILEVEL ANALYSES BOX 132 STANDARDISATION OF
CHAPTER 6 COMPUTATION OF STANDARD ERRORS BOX 61

Chapt

Chapt. 11 Practice Test

  1. What is polarizability? The ease with which electron density can be distorted


  1. What force(s) of attraction exist between He atoms? Dispersion forces


  1. What type of substance would exhibit both dispersion forces and dipole-dipole forces? A polar substance


  1. What type of force exists between a Ca2+ ion and water? Ion – dipole


  1. True or False: PH3 is capable of hydrogen bonding false


  1. List the properties of molecular compounds Soft, low melting point, poor conductor


  1. List the properties of ionic compounds

Hard, brittle, high melting point, solid form is a poor conductor, aqueous or molten forms will conduct


  1. Which of the following substances should have the highest boiling point? D


A. CH4 B. Cl2 C. Kr D. CH3Cl E. N2


  1. What is the relationship between strength of intermolecular force and

  1. Heat of vaporization stronger forces = greater heat of vaporization

  2. Vapor pressure stronger forces = lower vapor pressure

  3. Boiling point stronger forces = higher boiling point

  4. Viscosity stronger forces = greater viscosity


  1. Which of the following would have the lowest vapor pressure? C, it is capable of forming the most hydrogen bonds

A.CH3OCH3 B. C2H5OH C. HOCH2CH2OH


  1. Each of the following substances is a liquid at 50C. Place these liquids in order of increasing vapor pressure.

dimethyl ether (CH3OCH3), propane (C3H8), ethanol (CH3CH2OH) Answer: B

A. ethanol < propane < dimethyl ether

B. ethanol < dimethyl ether < propane

C. propane < dimethyl ether < ethanol

D. dimethyl ether < ethanol < propane

E. propane < ethanol < dimethyl ether


  1. Which one of the following substances should exhibit hydrogen bonding in the liquid state? Answer: E


A. PH3 B. He C. H2S D. CH4 E. CH3OH


  1. What is surface tension? Give specific examples.

The amount of energy required to stretch or increase the surface of a liquid by a unit area.

Examples: Bug “walking” on water; pin floating on water


  1. Which substance has the highest normal boiling point? D; it can hydrogen bond

    1. CH3Cl

    2. CH3Br

    3. CH3I

    4. CH3OH


  1. When does a liquid boil?

When its vapor pressure reaches or exceeds the external pressure





  1. Water boils at 71˚C on top of Mt. Everest (8848 m above sea level) and at 86˚C on top of Mt. Whitney (4418 m above sea level). Why does water boil at a higher temperature on Mt. Whitney than on Mt. Everest?

At higher altitudes, atmospheric pressure is less than at lower altitudes. Boiling occurs when the vapor pressure of the liquid equals the surrounding atmospheric pressure. Thus, water has a lower vapor pressure and boiling point on Mt. Everest than on Mt. Whitney


  1. List all the different phase changes that can occur and determine whether they are endothermic or exothermic.

Melting = endothermic

Freezing = exothermic

Vaporization = endothermic

Condensation = exothermic

Sublimation = endothermic

Deposition = exothermic


  1. List ALL the types of intermolecular forces that exist between HCl and ICl. Dipersion and dipole-dipole



  1. List ALL the intermolecular forces that exist between HF and H2O. Dispersion, dipole-dipole, and hydrogen bonding


  1. The specific heat capacity of liquid water is 4.184 J/g·C and the molar heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must be provided to convert 2.50 g of liquid water at 45C into 2.50 g of steam at 100C?

  1. Step One: Heat the water to 100.0°C

q= Cm∆T

q= 575.3 J

  1. Convert liquid to steam

  1. First change grams to moles (0.139 mol)

  2. Multiply the molar heat of vaporization (5.65 kJ)

  1. Add steps 1 and 2 together (make sure they are in the same units): = 6.23 kJ


  1. Calculate the amount of heat needed to melt 1.25 kg of iron at its melting point (1,809 K), given that: Hfus = 13.80 kJ/mol.

Convert kg to grams and then to moles

Multiply by the molar heat of fusion

Answer = 308.9 kJ

  1. Explain why water forms a meniscus in a capillary tube.

The water adheres to the wall of the glass tube. These adhesive forces are stronger than the cohesive forces, causing water to rise up the glass tube.






CHAPT 11 PRACTICE TEST 1 WHAT IS POLARIZABILITY? THE

B

C

A

D


  1. What is the normal boiling point of the substance with the phase diagram shown above? 400˚C


  1. What is the temperature and pressure at the triple point? 100˚C, 0.65 atm


  1. Which segment corresponds to the conditions of temperature and pressure under which the solid and liquid are in equilibrium? BD


  1. Which letter corresponds to the critical point? What type of substance exists past the critical point? C; supercritical fluid


  1. If I had a quantity of this substance at a pressure of 1.25 atm and a temperature of 3000 C and lowered the pressure to 0.25 atm, what phase transition(s) would occur? vaporization


  1. What state of matter is this substance in at 300˚C and 1.50 atm? liquid


CONFIGURING USER STATE MANAGEMENT FEATURES 73 CHAPTER 7 IMPLEMENTING
INTERPOLATION 41 CHAPTER 5 INTERPOLATION THIS CHAPTER SUMMARIZES POLYNOMIAL
PREPARING FOR PRODUCTION DEPLOYMENT 219 CHAPTER 4 DESIGNING A


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