General Chemistry A

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "General Chemistry A"

Transcription

1 General Chemistry A May 6, 2004 (6 Pages, 43 Parts) Name Each of the 40 multiple choice questions counts 2 point. Give the letter of the correct answer Crystalline solids differ from amorphous solids in that: (A) All crystalline solid contain anions and cations. (B) All crystalline solids have a long range order while all amorphous solids do not. (C) All crystalline solids conduct electricity while all amorphous solids do not. (D) All crystalline solids are hard and strong while all amorphous solids are soft and brittle. (E) All of the above. (F) None of the above. Which of the following properties is a general characteristic of solids? (A) Solids have a rigid shape and fixed volume (B) Solids can have crystalline or noncrystalline structures (C) Solids do not compress or expand significantly (D) A substance is usually more dense as a solid than a liquid (E) All of the above 3. Which of the following is not an example of a molecular crystalline solid? (A) halite, NaCl (D) sucrose, C 12 H (B) iodine, I 2 (E) urea, C (NH 2 ) 2 (C) phosphorus, P Which of the following explains why ice floats in water? (A) Molecules in ice are closer together. (B) The unit cell of ice has holes in it. (C) Ice has a smaller specific heat than water. (D) All of the above (E) None of the above Which of the following types of crystalline solids is hard and brittle, has a high melting point, and conducts electricity only when melted? (A) ionic (D) all of the above (B) molecular (C) metallic Which of the following types of crystalline solids is malleable, ductile, and a conductor of electricity? (A) ionic (D) all of the above (B) molecular (C) metallic Which of the following types of crystalline solids has a low melting point, is generally insoluble in water, and is a nonconductor of electricity? (A) ionic (D) all of the above (B) molecular (C) metallic

2 8. Consider the five pictures below. Each circle represents one carbon dioxide molecule. Which picture is the most realistic representation of solid C 2? (A) A (B) B (C) C (D) D (E) E A B C D E 9. Consider the five pictures above. Which is the most realistic representation of liquid H 2? (A) A (B) B (C) C (D) D (E) E 10. What is the term for the heat required to convert a solid to a liquid at its melting point? (A) heat of crystallization (D) specific heat (B) heat of fusion (C) heat of vaporization 11. Which of the following properties is a general characteristic of liquids? (A) liquids have a variable shape and fixed volume (B) liquids flow readily (C) liquids do not compress or expand significantly (D) a substance is much more dense as a liquid than a gas (F) None of the above 12. Which of the following properties is a general characteristic of liquids? (A) liquids have a fixed shape and variable volume (B) liquids compress and expand significantly (C) a substance is much less dense as a liquid than a gas (D) liquids that are soluble form heterogeneous mixtures 13. Water beads up on a freshly waxed automobile. This phenomenon is an example of: (A) Cohesive forces being weaker than adhesive forces. (B) Adhesive forces being stronger than cohesive forces. (C) Cohesive forces being stronger than adhesive forces. (D) Both a and b. 14. What is the term for the temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure? (A) absolute zero (D) vapor point (B) boiling point (C) critical point 15. Which of the following explains why a needle can float on water? (A) The density of the water is greater than the needle. (B) The molar mass of the water is greater than the needle. (C) The surface tension of the water supports the needle. (D) The vapor pressure of the water supports the needle. (E) The viscosity of the water supports the needle.

3 16. Which statement is correct about the cooling curve at the right? (A) A is cooling of the solid (D) F is freezing of the liquid (B) B is freezing of the liquid (E) E is boiling of the liquid (C) After D, solid starts to form below the freezing point Temp. A B C D Time E F 17. List the three compounds below in order of increasing boiling point: A H B CH 3 C CH 3 (A) A, B, C (B) A, C, B (C) B, A, C (D) B, C, A (E) C, B, A 18. What is the common term for the pressure exerted by vapor molecules above a liquid in a closed container when the rates of evaporation and condensation are equal? (A) atmospheric pressure (D) vapor pressure (B) equilibrium pressure (C) gas pressure 19. If the molecules in a liquid have a strong attraction for each other, which of the following properties has a relatively low value? (A) boiling point (D) viscosity (B) surface tension (C) vapor pressure 20. What is the term for the tendency of a liquid to form spherical droplets? (A) dipole attraction (D) surface tension (B) dispersion forces (E) viscosity (C) intermolecular attraction 21. What is the strongest intermolecular force in dimethyl ether, CH 3 --CH 3? (A) ion-ion attraction (D) hydrogen bond (B) dipole-dipole attraction (E) metallic bond (C) dispersion force 22. What is the term for an attraction between two molecules with temporary dipoles? (A) covalent bond (D) hydrogen bond (B) dipole force (E) intermolecular bond (C) dispersion force 23. What is the term for an attraction between molecules that contain a hydrogen atom bonded to a highly electronegative atom such as oxygen or nitrogen? (A) dipole force (D) intermolecular bond (B) dispersion force (E) polar covalent bond (C) hydrogen bond 24. What is the strongest intermolecular force in a liquid having molecules with H- bonds? (A) covalent bonds (D) hydrogen bonds (B) dipole forces (C) dispersion forces

4 25. Which of the following is true of the intermolecular attraction in liquids? (A) Nonpolar molecules can be attracted by dispersion forces. (B) Polar molecules can be attracted by temporary dipole forces. (C) Polar molecules can be attracted by permanent dipole forces. (D) Polar molecules can be attracted by hydrogen bonds. 26. Which of the following properties of water would you predict to be unusually high? (A) melting point (D) heat of vaporization (B) boiling point (C) heat of fusion 27. What is the term that refers to two liquids that are soluble in one another in all proportions? (A) immiscible (D) Tyndall effect (B) equal vapor pressure (C) miscible 28. What is the term for the general principle that solubility is greatest when the polarity of the solute is similar to that of the solvent? (A) like dissolves like rule (D) solution principle (B) polarity principle (E) solvent principle (C) solute principle 29. What is the term for a solution that contains the maximum amount of solute that will dissolve at a given temperature at equilibrium? (A) colloid (D) solubility (B) concentrated (E) supersaturated (C) saturated 30. What is the term for a solution that contains more solute than is ordinarily soluble at a given temperature? (A) colloid (D) supersaturated (B) concentrated (E) unsaturated (C) saturated 31. Which of the following liquids is miscible with water. (A) chloroform, CHCl 3 (D) pentane, C 5 H 12 (B) cyclohexane, C 6 H 12 (E) toluene, C 6 H 5 CH 3 (C) glycerin, C 3 H 5 (H) Sodium chloride, NaCl, dissolves in water because: (A) It takes very little energy to separate water molecules from water molecules. (B) It takes very little energy to separate sodium ions from chloride ions. (C) The solution has a more entropy than the separated sodium chloride and water. (D) All of the above. (E) None of the above. 33. Carbon tertrachloride, CCl 4, dissolves in hexane, C 6 H 14, because: (A) It takes very little energy to separate CCl 4 molecules from CCl 4 molecules. (B) It takes very little energy to separate C 6 H 14 molecules from C 6 H 14 molecules. (C) The solution has a more entropy than the separated CCl 4 and C 6 H 14. (D) All of the above. (E) None of the above.

5 34. A colligative property is one that: (A) Depends largely on the number of solute particles and not the nature of the solute particles. (B) Depends largely on the nature of the solute particles and not the number of solute particles. (C) Depends largely on both the number of solute particles and the nature of the solute particles. (D) Depends largely on factors other than the number of solute particles and the nature of the solute particles. 35. In osmosis: (A) Solute particles pass through a semipermeable membrane from low to high concentration of solute. (B) Solute particles pass through a semipermeable membrane from high to low concentration of solute. (C) Solvent particles pass through a semipermeable membrane from low to high concentration of solute. (D) Solvent particles pass through a semipermeable membrane from high to low concentration of solute. 36. If a bacterium is placed in solid salt, the bacterium will: (A) Explode due to rupturing the cell membrane. (B) Shrivel up like a raisin. (C) None of the above since salt cannot readily pass through the cell membrane. 37. If a bacterium is placed in pure water, the bacterium will: (A) Explode due to rupturing the cell membrane. (B) Shrivel up like a raisin. (C) None of the above since water cannot readily pass through the cell membrane. 38. For the solvent water, substances can be hydrophobic, hydrophilic, or duel-nature. Which substance is hydrophobic? (A) ethanol (B) gasoline (C) soap 39. Which of the following molecules would be a suitable surfactant? (A) only 1 1. (B) only 2 (C) only 3 (D) only 4 2. (E) 1 and 2 (F) 1 and 3 3. (G) 1 and 4 (H) 2 and 4 (I) all Dacron is a polyester with the structure at the right. The structure of the monomer containing the phenyl group (benzene ring) used to make this copolymer is: S 3 SH NH 3 [ ] A H H B C H H D H H E H H

6 41. (8%) Place the letter of the structure on the right in front of the compound on the left: An anhydride An ester Benzene Butanal 1-Butanol 2-Butanol Cyclohexane Decane 3-Decene Hexanal Hexanoic acid 2-Hexanone 3-Hexanone Hexyl amine ctane Pentane A D H K L H P M B I E NH 2 F H H N C H G J S Not Given Above H 42. (5%) Four separate solutions were prepared by dissolving exactly one mole of each of the following in exactly one kilogram of water. The melting points of each solution then was obtained. The melting points of these solutions and the melting point of pure water are listed on the left. The various samples are listed on the right. Answer the question by placing the letter of the sample on the right in front of the melting point of its solution on the left. The freezing point depression constant for water is 1.86 o /m or 1.86 o /c m. a o b o c o d o e o A. Ammonium hydroxide B. Calcium nitrate C. Ethanol D. Pure water E. Sodium chloride 43. (7%) A 3.40 g sample of an unknown compound was dissolved in g of benzene. The melting point of the solution was 4.86 o. Determine the molar mass (molecular weight) of the unknown compound. Show work for credit! The melting point of pure benzene is 5.54 o. The freezing point depression constant for benzene is 5.12 o /m or 5.12 o /c m.

General Chemistry A

General Chemistry A General Chemistry 1140 - A May 5, 2005 (6 Pages, 48 Questions) ame 1. Which of the following properties is a general characteristic of solids? (A) Solids have a rigid shape and fixed volume (B) Solids

More information

RW Session ID = MSTCHEM1 Intermolecular Forces

RW Session ID = MSTCHEM1 Intermolecular Forces RW Session ID = MSTCHEM1 Intermolecular Forces Sections 9.4, 11.3-11.4 Intermolecular Forces Attractive forces between molecules due to charges, partial charges, and temporary charges Higher charge, stronger

More information

Chem 1075 Chapter 13 Liquids and Solids Lecture Outline

Chem 1075 Chapter 13 Liquids and Solids Lecture Outline Chem 1075 Chapter 13 Liquids and Solids Lecture Outline Slide 2-3 Properties of Liquids Unlike gases, liquids respond dramatically to temperature and pressure changes. We can study the liquid state and

More information

Aqueous Solutions (When water is the solvent)

Aqueous Solutions (When water is the solvent) Aqueous Solutions (When water is the solvent) Solvent= the dissolving medium (what the particles are put in ) Solute= dissolved portion (what we put in the solvent to make a solution) Because water is

More information

Intermolecular forces Liquids and Solids

Intermolecular forces Liquids and Solids Intermolecular forces Liquids and Solids Chapter objectives Understand the three intermolecular forces in pure liquid in relation to molecular structure/polarity Understand the physical properties of liquids

More information

CHAPTER 6 Intermolecular Forces Attractions between Particles

CHAPTER 6 Intermolecular Forces Attractions between Particles CHAPTER 6 Intermolecular Forces Attractions between Particles Scientists are interested in how matter behaves under unusual circumstances. For example, before the space station could be built, fundamental

More information

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules?

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules? Polar Bonds and Polar Molecules Chapter 10 Liquids, Solids, and Phase Changes Draw Lewis Structures for CCl 4 and CH 3 Cl. What s the same? What s different? 1 Polar Covalent Bonds and Dipole Moments Bonds

More information

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO Lecture Presentation Chapter 11 Liquids and Intermolecular Forces John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Gases, Liquids, and Solids State Volume Shape of State Density

More information

Unit 10: Part 1: Polarity and Intermolecular Forces

Unit 10: Part 1: Polarity and Intermolecular Forces Unit 10: Part 1: Polarity and Intermolecular Forces Name: Block: Intermolecular Forces of Attraction and Phase Changes Intramolecular Bonding: attractive forces that occur between atoms WITHIN a molecule;

More information

Mixtures and Solutions

Mixtures and Solutions Mixtures and Solutions Section 14.1 Heterogeneous and Homogeneous Mixtures In your textbook, read about suspensions and colloids. For each statement below, write true or false. 1. A solution is a mixture

More information

- intermolecular forces forces that exist between molecules

- intermolecular forces forces that exist between molecules Chapter 11: Intermolecular Forces, Liquids, and Solids - intermolecular forces forces that exist between molecules 11.1 A Molecular Comparison of Liquids and Solids - gases - average kinetic energy of

More information

Name: Class: Date: ID: A

Name: Class: Date: ID: A Name: Class: _ Date: _ CH11 1. Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest. A) dipole-dipole, London dispersion, ionic, and

More information

London Dispersion Forces (LDFs) Intermolecular Forces Attractions BETWEEN molecules. London Dispersion Forces (LDFs) London Dispersion Forces (LDFs)

London Dispersion Forces (LDFs) Intermolecular Forces Attractions BETWEEN molecules. London Dispersion Forces (LDFs) London Dispersion Forces (LDFs) LIQUIDS / SOLIDS / IMFs Intermolecular Forces (IMFs) Attractions BETWEEN molecules NOT within molecules NOT true bonds weaker attractions Represented by dashed lines Physical properties (melting points,

More information

Chemistry 101 Chapter 14 Liquids & Solids

Chemistry 101 Chapter 14 Liquids & Solids Chemistry 101 Chapter 14 Liquids & Solids States of matter: the physical state of matter depends on a balance between the kinetic energy of particles, which tends to keep them apart, and the attractive

More information

Liquids, Solids and Phase Changes

Liquids, Solids and Phase Changes Chapter 10 Liquids, Solids and Phase Changes Chapter 10 1 KMT of Liquids and Solids Gas molecules have little or no interactions. Molecules in the Liquid or solid state have significant interactions. Liquids

More information

Water & Solutions Chapter 17 & 18 Assignment & Problem Set

Water & Solutions Chapter 17 & 18 Assignment & Problem Set Water & Solutions Chapter 17 & 18 Assignment & Problem Set Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Water & Solutions 2 Vocabulary (know

More information

Properties of Solutions

Properties of Solutions Properties of Solutions The States of Matter The state a substance is in at a particular temperature and pressure depends on two antagonistic entities: The kinetic energy of the particles The strength

More information

Chapter 13 States of Matter Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes

Chapter 13 States of Matter Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes Chapter 13 States of Matter 13.2 Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes I. Forces of Attraction (13.2) Intramolecular forces? (forces within) Covalent Bonds, Ionic Bonds, and metallic

More information

The Liquid and Solid States

The Liquid and Solid States : The Liquid and Solid States 10-1 10.1 Changes of State How do solids, liquids and gases differ? Figure 10.4 10-2 1 10.1 Changes of State : transitions between physical states Vaporization/Condensation

More information

A) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance.

A) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance. PX0411-1112 1. Which of the following statements concerning liquids is incorrect? A) The volume of a liquid changes very little with pressure. B) Liquids are relatively incompressible. C) Liquid molecules

More information

Advanced Chemistry Liquid & Solids Test

Advanced Chemistry Liquid & Solids Test Advanced Chemistry Liquid & Solids Test Name: Multiple Choice 1) Which one of the following statements about liquids and solids is generally false? a) The rate of diffusion is lower in solids b) The density

More information

Unit 5: Bonding Covalent & Intermolecular

Unit 5: Bonding Covalent & Intermolecular Name Unit 5: Bonding Covalent & Intermolecular Date Part 2 Questions 1. Ozone, O3 (g), is produced from oxygen, O2 (g) by electrical discharge during thunderstorms. The unbalanced equation below represents

More information

CHEMISTRY Ch. 14 Notes: Mixtures and Solutions NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

CHEMISTRY Ch. 14 Notes: Mixtures and Solutions NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. CHEMISTRY Ch. 14 Notes: Mixtures and Solutions NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 14.1 notes I. Types of mixtures (mixture a physical blend of substances)

More information

Ch. 14/15 Prep-Test. Multiple Choice Identify the choice that best completes the statement or answers the question.

Ch. 14/15 Prep-Test. Multiple Choice Identify the choice that best completes the statement or answers the question. Ch. 14/15 Prep-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The intermolecular forces between particles in a liquid can involve all of the following

More information

Name Chemistry Pre-AP. Notes: Solutions

Name Chemistry Pre-AP. Notes: Solutions Name Chemistry Pre-AP Notes: Solutions Period I. Intermolecular Forces (IMFs) A. Attractions Between Molecules Attractions between molecules are called and are very important in determining the properties

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 A phase is a homogeneous part of the system in contact

More information

(for tutoring, homework help, or help with online classes)

(for tutoring, homework help, or help with online classes) www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. Elemental iodine (I 2 ) is a solid at room temperature. What is the major attractive force that exists among different

More information

Heat Capacity of Water A) heat capacity amount of heat required to change a substance s temperature by exactly 1 C

Heat Capacity of Water A) heat capacity amount of heat required to change a substance s temperature by exactly 1 C CHEMISTRY Ch. 13 Notes: Water and Its Solutions NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 13.1 Notes I. Water Molecule Characteristics POLAR molecule (a

More information

CHM151 Quiz Pts Fall 2013 Name: Due at time of final exam. Provide explanations for your answers.

CHM151 Quiz Pts Fall 2013 Name: Due at time of final exam. Provide explanations for your answers. CHM151 Quiz 12 100 Pts Fall 2013 Name: Due at time of final exam. Provide explanations for your answers. 1. Which one of the following substances is expected to have the lowest melting point? A) BrI B)

More information

Intermolecular Forces and Liquids and Solids Chapter 11

Intermolecular Forces and Liquids and Solids Chapter 11 Intermolecular Forces and Liquids and Solids Chapter 11 A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well defined boundary. Phases

More information

Liquids & Solids. Mr. Hollister Holliday Legacy High School Regular & Honors Chemistry

Liquids & Solids. Mr. Hollister Holliday Legacy High School Regular & Honors Chemistry Liquids & Solids Mr. Hollister Holliday Legacy High School Regular & Honors Chemistry 1 Liquids 2 Properties of the States of Matter: Liquids High densities compared to gases. Fluid. The material exhibits

More information

CHEMISTRY XL-14A PHYSICAL EQUILIBRIUM. August 13, 2011 Robert Iafe

CHEMISTRY XL-14A PHYSICAL EQUILIBRIUM. August 13, 2011 Robert Iafe CHEMISTRY XL-14A PHYSICAL EQUILIBRIUM August 13, 2011 Robert Iafe Chapter Overview 2 Phases and Phase Transitions Solubility Colligative Properties Binary Liquid Mixtures Phases and Phase Transitions 3

More information

Solution Formation. Copyright Houghton Mifflin Company.All rights reserved. Presentation of Lecture Outlines, 12 2

Solution Formation. Copyright Houghton Mifflin Company.All rights reserved. Presentation of Lecture Outlines, 12 2 Solutions Solution Formation A solution is a homogeneous mixture of two or more substances, consisting of ions or molecules. (See Animation: Solution Equilibrium). A colloid, although it also appears to

More information

Solutions. Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility

Solutions. Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility Solutions Solutions Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility Colligative Properties - Ways of Expressing Concentration

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 A phase is a homogeneous part of the system in contact

More information

Review Topic 8: Phases of Matter and Mixtures

Review Topic 8: Phases of Matter and Mixtures Name: Score: 24 / 24 points (100%) Review Topic 8: Phases of Matter and Mixtures Multiple Choice Identify the choice that best completes the statement or answers the question. C 1. Soda water is a solution

More information

UNIT 14 IMFs, LIQUIDS, SOLIDS PACKET. Name: Date: Period: #: BONDING & INTERMOLECULAR FORCES

UNIT 14 IMFs, LIQUIDS, SOLIDS PACKET. Name: Date: Period: #: BONDING & INTERMOLECULAR FORCES Name: Date: Period: #: BONDING & INTERMOLECULAR FORCES p. 1 Name: Date: Period: #: IMF NOTES van der Waals forces: weak attractive forces between molecules. There are 3 types: 1. London Dispersion Forces

More information

Elemental iodine (I 2 ) is a solid at room temperature. What is the major attractive force that exists among different I 2 molecules in the solid?

Elemental iodine (I 2 ) is a solid at room temperature. What is the major attractive force that exists among different I 2 molecules in the solid? For answers, send email to: admin@tutor-homework.com. Include file name: Chemistry_Worksheet_0106 Price: $3 (c) 2012 www.tutor-homework.com: Tutoring, homework help, help with online classes. 1. Elemental

More information

CfE Higher Chemistry. Unit 1: Chemical Changes and Structure. Intermolecular forces

CfE Higher Chemistry. Unit 1: Chemical Changes and Structure. Intermolecular forces CfE Higher Chemistry Unit 1: Chemical Changes and Structure Intermolecular forces 05/09/2017 Van der Waal s Forces and London Dispersion Forces 05/09/2017 Learning Outcomes : I can explain the difference

More information

General Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 15-May-2009

General Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 15-May-2009 Chem 1046 General Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 15-May-2009 Chapter 12 SOLUTIONS These Notes are to SUPPLIMENT the Text, They do

More information

Chapter 17: Phenomena

Chapter 17: Phenomena Chapter 17: Phenomena Phenomena: Different masses of solute were added to 1 kg of either H 2 O or C 6 H 6. The boiling and freezing points of the solutions were then measured. Examine the data to determine

More information

Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions

Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions 1 Chapter 12 :Solutions Tentative Outline 1. Introduction to solutions. 2. Types of Solutions 3. Solubility and the Solution Process: Saturated,

More information

Lecture Presentation. Chapter 12. Solutions. Sherril Soman, Grand Valley State University Pearson Education, Inc.

Lecture Presentation. Chapter 12. Solutions. Sherril Soman, Grand Valley State University Pearson Education, Inc. Lecture Presentation Chapter 12 Solutions Sherril Soman, Grand Valley State University Thirsty Seawater Drinking seawater can cause dehydration. Seawater Is a homogeneous mixture of salts with water Contains

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A phase is a homogeneous part of the system in contact

More information

Chapter 11. Freedom of Motion. Comparisons of the States of Matter. Liquids, Solids, and Intermolecular Forces

Chapter 11. Freedom of Motion. Comparisons of the States of Matter. Liquids, Solids, and Intermolecular Forces Liquids, Solids, and Intermolecular Forces Chapter 11 Comparisons of the States of Matter The solid and liquid states have a much higher density than the gas state The solid and liquid states have similar

More information

The Liquid and Solid States

The Liquid and Solid States : The Liquid and Solid States 10-1 10.1 Changes of State How do solids, liquids and gases differ? Figure 10.4 10-2 10.1 Changes of State : transitions between physical states Vaporization/Condensation

More information

Ch 10 -Ch 10 Notes Assign: -HW 1, HW 2, HW 3 Blk 1 Ch 10 Lab

Ch 10 -Ch 10 Notes Assign: -HW 1, HW 2, HW 3 Blk 1 Ch 10 Lab Advanced Placement Chemistry Chapters 10 11 Syllabus As you work through each chapter, you should be able to: Chapter 10 Solids and Liquids 1. Differentiate between the various types of intermolecular

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 A phase is a homogeneous part of the system in contact

More information

Chapter 13. Properties of Solutions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO

Chapter 13. Properties of Solutions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO Lecture Presentation Chapter 13 Properties of John D. Bookstaver St. Charles Community College Cottleville, MO are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed

More information

Chapter 10: Liquids, Solids, and Phase Changes

Chapter 10: Liquids, Solids, and Phase Changes Chapter 10: Liquids, Solids, and Phase Changes In-chapter exercises: 10.1 10.6, 10.11; End-of-chapter Problems: 10.26, 10.31, 10.32, 10.33, 10.34, 10.35, 10.36, 10.39, 10.40, 10.42, 10.44, 10.45, 10.66,

More information

Intermolecular Forces and Liquids and Solids. Chapter 11. Copyright The McGraw Hill Companies, Inc. Permission required for

Intermolecular Forces and Liquids and Solids. Chapter 11. Copyright The McGraw Hill Companies, Inc. Permission required for Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw Hill Companies, Inc. Permission required for 1 A phase is a homogeneous part of the system in contact with other parts of the

More information

13.1 States of Matter: A Review 13.2 Properties of Liquids A. Evaporation B. Vapor Pressure C. Surface Tension 13.3 Boiling Point and Melting Point

13.1 States of Matter: A Review 13.2 Properties of Liquids A. Evaporation B. Vapor Pressure C. Surface Tension 13.3 Boiling Point and Melting Point 13.1 States of Matter: A Review 13.2 Properties of Liquids A. Evaporation B. Vapor Pressure C. Surface Tension 13.3 Boiling Point and Melting Point 13.4 Changes of State 13.5 Intermolecular Forces 13.6

More information

Chapter 12. Physical Properties of Solutions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill

Chapter 12. Physical Properties of Solutions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chapter 12 Physical Properties of Solutions Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department of Chemistry

More information

Physical Properties of Solutions

Physical Properties of Solutions Physical Properties of Solutions Physical Properties of Solutions Types of Solutions (13.1) A Molecular View of the Solution Process (13.2) Concentration Units (13.3) Effect of Temperature on Solubility

More information

- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)

- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar) 68 HOW THINGS DISSOLVE - Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)... what happens? - Water molecules pull the sugar molecules out of

More information

Solids, liquids and gases

Solids, liquids and gases Solids, liquids and gases Solids, liquids, and gases are held together by intermolecular forces. Intermolecular forces occur between molecules, not within molecules (as in bonding). When a molecule changes

More information

An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is g/ml Find: molality, mole fraction, molarity.

An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is g/ml Find: molality, mole fraction, molarity. 66 An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is 1.024 g/ml Find: molality, mole fraction, molarity. Find molality: mass percent molality Assuming 100 g solution,

More information

Intermolecular Forces, Liquids, & Solids

Intermolecular Forces, Liquids, & Solids , Liquids, & Solids Mr. Matthew Totaro Legacy High School AP Chemistry States of Matter The fundamental difference between states of matter is the distance between particles. States of Matter Because in

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids PowerPoint Lecture Presentation by J. David Robertson University of Missouri Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction

More information

Chapter 11. Liquids and Intermolecular Forces

Chapter 11. Liquids and Intermolecular Forces Chapter 11 Liquids and Intermolecular Forces States of Matter The three states of matter are 1) Solid Definite shape Definite volume 2) Liquid Indefinite shape Definite volume 3) Gas Indefinite shape Indefinite

More information

Molecules have to move past one another to flow, and stronger attractions between molecules make that more difficult!

Molecules have to move past one another to flow, and stronger attractions between molecules make that more difficult! 40 VISCOSITY - viscosity can also be explained (at least partially) by looking at INTERMOLECULAR FORCES! - For a liquid to FLOW, its molecules must move past one another. This means that some of the molecules

More information

Chapters 11 and 12: Intermolecular Forces of Liquids and Solids

Chapters 11 and 12: Intermolecular Forces of Liquids and Solids 1 Chapters 11 and 12: Intermolecular Forces of Liquids and Solids 11.1 A Molecular Comparison of Liquids and Solids The state of matter (Gas, liquid or solid) at a particular temperature and pressure depends

More information

Properties of Solutions. Chapter 13

Properties of Solutions. Chapter 13 Properties of Solutions Chapter 13 Sodium acetate crystals rapidly form when a seed crystal is added to a supersaturated solution of sodium acetate. Saturated solution: contains the maximum amount of a

More information

Chem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.

Chem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question. Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. An open-tube manometer is used to measure the pressure in a flask. The atmospheric

More information

Unit Five: Intermolecular Forces MC Question Practice April 14, 2017

Unit Five: Intermolecular Forces MC Question Practice April 14, 2017 Unit Five: Intermolecular Forces Name MC Question Practice April 14, 2017 1. Which of the following should have the highest surface tension at a given temperature? 2. The triple point of compound X occurs

More information

Unit 6 Solids, Liquids and Solutions

Unit 6 Solids, Liquids and Solutions Unit 6 Solids, Liquids and Solutions 12-1 Liquids I. Properties of Liquids and the Kinetic Molecular Theory A. Fluids 1. Substances that can flow and therefore take the shape of their container B. Relative

More information

LONDON DISPERSION FORCES. - often called "London forces" for short. - London forces occur in all molecules, polar or nonpolar.

LONDON DISPERSION FORCES. - often called London forces for short. - London forces occur in all molecules, polar or nonpolar. 43 LONDON DISPERSION FORCES - often called "London forces" for short. - occurs because electron density is - at any given point in time - likely to be uneven across a molecule due to the simple fact that

More information

Calderglen High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding. Page 1 of 21

Calderglen High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding. Page 1 of 21 Calderglen High School CfE Higher Chemistry Chemical Changes & Structure Structure and Bonding Page 1 of 21 No. Learning Outcome Understanding? 1 2 The bonding types of the first twenty elements; metallic

More information

Ionic Compounds and Ionic Bonding

Ionic Compounds and Ionic Bonding Ionic Compounds and Ionic Bonding Definitions Review: Crystal Lattice - 3D continuous repeating pattern of positive and negative ions in an ionic solid Formula Unit- smallest possible neutral unit of an

More information

- "Intermolecular forces" is a generic term. It refers to any number of forces that exist between molecules!

- Intermolecular forces is a generic term. It refers to any number of forces that exist between molecules! 41 INTERMOLECULAR FORCES IN LIQUIDS - "Intermolecular forces" is a generic term. It refers to any number of forces that exist between molecules! - In liquids, there are three main types of intermolecular

More information

Solutions are HOMOGENEOUS mixtures and can be gases, liquids, or solids.

Solutions are HOMOGENEOUS mixtures and can be gases, liquids, or solids. UNIT 4 Solutions and Solubility Chapter 8 Solutions and Concentration Types of Solutions The simplest solutions contain 2 substances: 1. SOLVENT o any substance that has another substance o dissolved in

More information

11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 4 Physical Properties of Solutions

11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy.   Chapter 4 Physical Properties of Solutions General Chemistry CHEM 11 (3+1+) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 4 Physical Properties of Solutions 1 Types of Solutions A solution is a homogenous mixture of 2 or more substances.

More information

Chemistry: The Central Science

Chemistry: The Central Science Chemistry: The Central Science Fourteenth Edition Chapter 11 Liquids and Intermolecular Forces Intermolecular Forces The attractions between molecules are not nearly as strong as the intramolecular attractions

More information

Chapter 11 Properties of Solutions

Chapter 11 Properties of Solutions Chapter 11 Properties of Solutions Solutions Homogeneous mixtures of two or more substances Composition is uniform throughout the sample No chemical reaction between the components of the mixture Solvents

More information

Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 13 Properties of Solutions

Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 13 Properties of Solutions Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 13 Properties of Dr. Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville,

More information

Solutions Definition and Characteristics

Solutions Definition and Characteristics Solutions Solutions Definition and Characteristics Homogeneous mixtures of two or more substances Appear to be pure substances Transparency Separation by filtration is not possible Uniform distribution

More information

11) What thermodynamic pressure encourages solution formation of two nonpolar substances?

11) What thermodynamic pressure encourages solution formation of two nonpolar substances? AP Chemistry Test (Chapter 11) Class Set Multiple Choice (54%) Please use the following choices to answer questions 1-10. A) London dispersion forces (temporary dipole attractions) B) Ion-ion attractions

More information

Chapter 11 Solutions and Colloids 645

Chapter 11 Solutions and Colloids 645 Chapter 11 Solutions and Colloids 645 11.5 Colloids Colloids are mixtures in which one or more substances are dispersed as relatively large solid particles or liquid droplets throughout a solid, liquid,

More information

Bonds & IMAFs in Liquids, Solids, and Solutions

Bonds & IMAFs in Liquids, Solids, and Solutions Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Unit 5 (Chp 11,13) Bonds & IMAFs in Liquids, Solids, and Solutions John D. Bookstaver St. Charles

More information

Liquids, Solids, and Intermolecular Forces or. Why your Water Evaporates and your Cheerios Don t. Why are molecules attracted to each other?

Liquids, Solids, and Intermolecular Forces or. Why your Water Evaporates and your Cheerios Don t. Why are molecules attracted to each other? Liquids, Solids, and Intermolecular Forces or Why your Water Evaporates and your heerios Don t Why are molecules attracted to each other? 1 Intermolecular attractions determine how tightly liquids and

More information

Name Practice IMFs and VP

Name Practice IMFs and VP Name Practice IMFs and VP Date 5916. Which formula represents a nonpolar molecule containing polar covalent bonds? A) NH3 B) H2 C) CCl4 D) H2O 408. In substances that sublime, the forces of attraction

More information

3) Accounts for strands of DNA being held together into a double helix. 7) Accounts for the cohesive nature of water and its high surface tension

3) Accounts for strands of DNA being held together into a double helix. 7) Accounts for the cohesive nature of water and its high surface tension AP Chemistry Test (Chapter 11) Multiple Choice (50%) Please use the following choices to answer questions 1-7. A) London dispersion forces B) Ion-ion attractions C) Dipole-dipole attractions D) Dipole-ion

More information

Find molality: mass percent. molality Assume a basis of 100g solution, then find moles ammonium chloride: Find mass water: So molality is:

Find molality: mass percent. molality Assume a basis of 100g solution, then find moles ammonium chloride: Find mass water: So molality is: 66 An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is 1.024 g/ml Find: molality, mole fraction, molarity. Find molality: mass percent molality Assume a basis of 100g

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces Chapter 11, Liquids, and Solids States of Matter The fundamental difference between states of matter is the distance between particles. States of Matter Because in the solid and liquid states particles

More information

Chapter 11. Intermolecular Forces and Liquids & Solids

Chapter 11. Intermolecular Forces and Liquids & Solids Chapter 11 Intermolecular Forces and Liquids & Solids The Kinetic Molecular Theory of Liquids & Solids Gases vs. Liquids & Solids difference is distance between molecules Liquids Molecules close together;

More information

Solutions: Multiple Choice Review PSI AP Chemistry. 1. Which of the following would be FALSE regarding mixtures?

Solutions: Multiple Choice Review PSI AP Chemistry. 1. Which of the following would be FALSE regarding mixtures? Solutions: Multiple Choice Review PSI AP Chemistry Name Part A: Mixtures, Solubility, and Concentration 1. Which of the following would be FALSE regarding mixtures? (A) Mixtures do not obey the law of

More information

Chapter 12. Properties of Solutions

Chapter 12. Properties of Solutions Chapter 12. Properties of Solutions What we will learn: Types of solutions Solution process Interactions in solution Types of concentration Concentration units Solubility and temperature Solubility and

More information

Chapter 10: States of Matter. Concept Base: Chapter 1: Properties of Matter Chapter 2: Density Chapter 6: Covalent and Ionic Bonding

Chapter 10: States of Matter. Concept Base: Chapter 1: Properties of Matter Chapter 2: Density Chapter 6: Covalent and Ionic Bonding Chapter 10: States of Matter Concept Base: Chapter 1: Properties of Matter Chapter 2: Density Chapter 6: Covalent and Ionic Bonding Pressure standard pressure the pressure exerted at sea level in dry air

More information

H 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point

H 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point Unit 9: Solutions H 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point Water is a polar molecule. It experiences hydrogen

More information

Useful Information Provided on Exam 1. Sections Covered on Exam , 10.2, 10.8,

Useful Information Provided on Exam 1. Sections Covered on Exam , 10.2, 10.8, Chem 101B Exam 1 Study Questions Name: Chapters 10(partial), 11 & 12(partial) Review Tuesday 2/7/2017 Due on Exam Thursday 2/9/2017 (Exam 1 date) This is a homework assignment. Please show your work for

More information

Scientists learned that elements in same group on PT react in a similar way. Why?

Scientists learned that elements in same group on PT react in a similar way. Why? Unit 5: Bonding Scientists learned that elements in same group on PT react in a similar way Why? They all have the same number of valence electrons.which are electrons in the highest occupied energy level

More information

Name: Date: Period: #: BONDING & INTERMOLECULAR FORCES

Name: Date: Period: #: BONDING & INTERMOLECULAR FORCES BONDING & INTERMOLECULAR FORCES Page 1 INTERMOLECULAR FORCES Intermolecular forces (van der Waals forces) relative weak interactions that occur between molecules. Most of the physical properties of gases,

More information

Chapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments

Chapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments P a g e 1 Unit 3: Chapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments Liquids and solids are quite different from gases due to their attractive forces

More information

Kirkcaldy High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding

Kirkcaldy High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding Kirkcaldy High School CfE Higher Chemistry Chemical Changes & Structure Structure and Bonding Page 1 of 26 No. Learning Outcome Understanding? The bonding types of the first twenty elements; metallic (Li,

More information