Chapter 10 Review Packet

Size: px
Start display at page:

Download "Chapter 10 Review Packet"

Transcription

1 Chapter 10 Review Packet Name 1. If water and carbon dioxide molecules did interact, what major intermolecular force will exist between these molecules? a) Hydrogen bonding b) London dispersion c) Dipole-dipole forces 2. Which of the following molecule pairs are not involved in hydrogen bonding? a) HCOOH, H 2 O b) H 2 O, NH 3 c) CH 3 OH, CH 3 COOH d) H 2 and I 2 3. Arrange the following molecules in order of decreasing intermolecular interaction: SO 2, Cl 2, CH 3 OH, CH 3 NH 2 a) CH 3 OH > CH 3 NH 2 > SO 2 > Cl 2 b) Cl 2 > SO 2 > CH 3 OH > CH 3 NH 2 c) SO 2 > CH 3 NH 2 > CH 3 OH > Cl 2 d) CH 3 NH 2 > CH 3 OH > SO 2 > Cl 2 4. Knowing that solutes with a certain polarity (or absence of it) are best dissolved in solutions with similar polarity, which of the following solvents would be optimal for the solvation of CH 3 COOH? a) CH 4 b) CH 3 OH c) C 2 H 6 d) C 6 H 6 5. Which of the following molecules interact primarily through London-dispersion forces? a) SO 2 b) CCl 4 c) CH 2 Cl 2 d) H 2 S 6. Which of the following has the highest boiling point? a) H 2 O b) HF c) HI d) HBr

2 7. Surface tension is due to the: a) liquid molecules being more attracted to surrounding surface molecules than other liquid molecules b) liquid molecules being as attracted to surrounding molecules as to other liquid molecules c) liquid molecules being more attracted to other liquid molecules than surrounding molecules d) liquid molecules being attracted only to surrounding molecules 8. Which of the following liquids will be the most viscous? a) C 3 H 8 b) C 6 H 6 c) CH 4 d) C 2 H 6 9. In the liquid state, molecules: a) are100% hydrogen bonded to their neighbors. b) are part of a crystal lattice. c) are frozen in space. d) are considerably restricted in movement. 10. Which of the following liquids would show a convex meniscus when placed in a glass tube? a) CH 3 OH(l) b) H 2 O(l) c) CHCl 3 (l) d) BF 3 (l) 11. The smallest repeating unit of the lattice is called: a) unit cell b) unit lattice c) cell d) unit crystal 12. Which of the following types of solids exist as crystals? a) ionic solids b) atomic solids c) molecular solids d) metallic solids 13. The successive packing pattern for an hcp cell is which one of the following? a) ABABAB b) ABAABA c) ABCABC d) ABCCBA

3 14. X-rays with a particular wavelength were used to analyze a crystalline solid. Assuming n = 1, and knowing that the distance between the planes of atoms, producing a diffraction with an angle = 20.0º, is 200 pm, calculate the frequency of the X-rays. a) 365 b) 6.22 x c) d) 2.19 x Conducting electrons in metals are situated in: a) Localized orbitals b) s-orbitals c) Metallic orbitals d) Conduction bands 16. The vapor pressure of 1-propanol at 14.7 C is 10.0 torr. The heat of vaporization is 47.2 kj/mol. Calculate the vapor pressure of 1-propanol at 52.8 C. a) 100. torr b) 20.0 torr c) 200. torr d) 600. torr ln P T1 = ΔH vap 1 1 P T2 R T 2 T 1 ln 10.0 = 47,200 J/mol 1 1 P T J/mol K K ln(10/p T2 ) = /P T2 = P T2 = 100. torr

4 17. The difference between interstitial alloy and substitutional allow is that in substitutional alloys: a) Some atoms of one element are replaced by atoms of another element b) Atoms of one element are inserted in the spaces between the atoms of the other element c) Atoms of one element fuse with the atoms of the other element d) Three elements, rather than two, are combined to form the alloy 18. Which one of the following decreases as the strength of the attractive intermolecular forces increases? a) The heat of vaporization. b) The normal boiling temperature. c) The extent of deviations from the ideal gas law. d) The sublimation temperature of a solid. e) The vapor pressure of a liquid. 19. 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 of solids is higher. c) The compressibility of liquids is higher. d) Liquids have higher vapor pressures. e) The heat of vaporization is less than the heat of fusion. 20. Which of the following is a correct listing in terms of increasing boiling point? a) CH 4 < NH 3 < H 2 O < HF b) CH 4 < NH 3 < HF < H 2 O c) CH 4 < HF < NH 3 < H 2 O d) HF< H 2 O < NH 3 < CH 4 e) CH 4 < HF < H 2 O < NH The boiling points of the halogens increase from F 2 to I 2. What type of intermolecular forces are responsible for this trend? a) permanent dipole b) hydrogen bonding c) ion-ion attraction d) London dispersion forces e) ion-dipole attraction 22. Which of the following statements is true about p-type silicon? a) It is produced by doping Si with P or As. b) Electrons are the mobile charge carriers. c) It does not conduct electricity as well as pure Si. d) All are true. e) None is true. As atomic size increases, LD forces become increasingly more important. a. is incorrect because it produces an n-type semiconductor. b. is incorrect because the charge carriers are holes in a p-type. c. is incorrect because it would conduct better than pure Si.

5 23. Doping Se with As would produce a(n) semiconductor with conductivity compared to pure Se. a) n-type, increased b) n-type, decreased c) p-type, increased d) p-type, decreased e) intrinsic, identical 24. A material is made from Al, Ga, and As. The mole fraction of each element is 0.25, 0.26, and 0.49, respectively. This material would be a) a metallic conductor because Al is present. b) an insulator. c) a p-type semiconductor. d) an n-type semiconductor. e) none of the above 25. Which of the following statements about superconductors is false? a) They conduct electricity without wasting heat energy. b) A class of high-temperature superconductors is called perovskites. c) Good conductivity, efficiency, and ductility are reasons why ceramic materials are used in superconductors. Ceramics are brittle, not ductile. d) High-temperature superconductors contain copper, oxygen, a lanthanide metal, and an alkaline earth metal. e) All of these are true. 26. Which of the following statements about phase changes are true? I. No temperature change is observed during a phase change. II. Vaporization is an exothermic process. EXOTHERMIC III. When a phase change occurs, no energy is transferred to or from the substance. IT TAKES ENERGY TO BREAK IMF S!! IV. When cooling a given amount of a substance, the rate at which cooling occurs is a function of.the mass of the substance and its specific heat. V. The heat of fusion for ice would determine how much energy would be required to change the temperature of a 10-g block of ice from 20 C to 2 C. IT WOULD BE NECESSARY TO KNOW THE SPECIFIC HEAT OF ICE, NOT THE HEAT OF FUSION! a) I and III b) I and IV c) II and III d) II, III, and IV e) IV only As has one less valence electron than Se so the resulting semiconductor would be a p-type. This would increase the conductivity due to holes that the electrons can jump into. Twice as much As would seem that the material was doped with Al and Ga. Because Al and Ga have fewer valence electrons than As, it would make this a p-type.

6 For questions 27 and 28, use the phase diagram for compound X below: 27. The normal boiling point of X is most likely: a) 21 C b) 47 C c) 73 C d) 18 C e) 0 C 28. How will the melting point of X change with increased pressure? a) increase b) decrease c) remain the same d) there is not enough information given e) increase and then decrease 29. How much energy is needed to convert 64.0 grams of ice at 0.00 C to water at 75.0 C? specific heat capacity of water = 4.18 J/g C H vap of water = 2258 J/g specific heat capacity of ice = 2.1 J/g C H fusion of water = 333 J/g a) 10.1 kj b) 20.7 kj c) 31.4 kj d) 41.4 kj e) 65.8 kj Melt water. q = ΔH fus grams q = (333 J/g) (64.0 g) q = 21,300 J = 21.3 kj Heat water from 0 C to 75 C. q = mcδt q = (64.0 g) (4.18 J/g C) (75 C 0 C)) q = 20,100 J = 20.1 kj Add to get the energy needed: 21.3 kj kj = 41.4 kj

7 30. Which of the compounds below is an example of a network solid? a) S 8 (s) b) SiO 2 (s) c) MgO (s) d) NaCl (s) e) C 25 H 52 (s) 31. How much heat is required to change the temperature of a 10.0-gram ice cube from 15 C to 132 C?

8 32. Use the band model to describe differences between insulators and conductors. The band model or molecular orbital (MO) model for metals is a molecular model for metals in which the electrons are assumed to travel around the metal crystal in molecular orbitals formed from the valence atomic orbitals of the metal atoms. In this model, the electrons are assumed to travel around the metal crystal in molecular orbitals formed from the valence atomic orbitals of the metal atoms. When many metal atoms interact, as in a metal crystal, the large number of resulting molecular orbitals become more closely spaced and finally form a virtual continuum of levels, called bands. This existence of empty molecular orbitals close in energy to filled molecular orbitals explains the thermal and electrical conductivity of metal crystals. Metals conduct electricity and heat very efficiently because of the availability of highly mobile electrons. The difference between insulators and conductors comes in the proximity of the molecular orbitals. Metals have MO's that are very close together. The band model is used to explain heat and electrical conduction. In this model, mobile electrons are furnished when electrons in filled molecular orbitals are excited into empty ones. These conduction electrons are free to travel throughout the metal crystal. Nonmetals have a wide gap between its MO's. As a result, their electrons cannot be excited into empty MO's. Therefore, they do not conduct heat and electricity in an appreciable manner. 33. How can an n-type semiconductor be produced from pure germanium? Explain. To produce an n-type semiconductor, dope Ge with a substance that has more than 4 valence electrons, (a group 15 element). Phosphorus or arsenic are a couple of substances which would produce n-type semiconductors when they are doped into germanium. 34. What would be the shape of the meniscus of water in a polyethylene tube? (Polyethylene can be represented as CH 3 (CH 2 ) n CH 3, where n is a large number on the order of 1000.) Justify your answer. Polyethylene is a nonpolar substance. The H 2 O-H 2 O attraction (cohesive force) is stronger than the H 2 O-polyethylene attraction (adhesive force) because of hydrogen bonding in the former and only LDF in the latter. Thus, the meniscus will have a convex shape.

9 35. How much heat is given off when 164 g of steam at 350. C is cooled to ice at 125 C mol H 2 O

10 36. Order the following compounds from largest to smallest enthalpy of fusions: H 2 O, CO 2, MgO (Justify your answer!) H 2 O has hydrogen bonding as well as dipole and LDF. CO 2 has is nonpolar and has only LDF. MgO is ionic. Ionic is the strongest force, then hydrogen bonding, and finally LDF. Thus the order of largest to smallest forces will be MgO, H 2 O, and CO 2. As intermolecular forces decrease, the enthalpy of fusions decrease. Therefore, the order from largest to smallest enthalpy of fusions: MgO, H 2 O, CO How much heat is necessary to melt g of sodium chloride at 801 C? (The heat of fusion of sodium chloride is kj/mole.) kj 1 mol NaCl g NaCl = kj 1 mol NaCl g NaCl Remember: *As IMF's increase, all properties (b.p., m.p., viscosity,...) will also increase EXCEPT vapor pressure which will decrease. *Know how to determine LDF, dipole-dipole, and H-bonding. *LDF's become more important as the SIZE of the atom increases. *Understand cohesive and adhesive forces which produce either a convex meniscus or a concave meniscus. *Know that "normal" means at 1 atmosphere of pressure and 1 atm = 760 mm Hg = kpa *Know that "standard pressure" = 1 atm *Understand the trends in the diagrams of the alkanes and the b.p. s of the hydrogen compounds of Groups *Understand phase diagrams and how to read them. *Understand the trend that density follows during phase changes. *Know the difference between substitutional and interstitial alloys and examples of each. *Know the difference between n-type and p-type semiconductors and how to form each. *Know how to calculate enthalpy changes (Like a 10.0-g ice cube at 15 C to 150. C) *Understand the band model pertaining to thermal and electrical conductivity of metals.

Chapter 10. Liquids and Solids

Chapter 10. Liquids and Solids Chapter 10 Liquids and Solids Chapter 10 Table of Contents 10.1 Intermolecular Forces 10.2 The Liquid State 10.3 An Introduction to Structures and Types of Solids 10.4 Structure and Bonding in Metals 10.5

More information

Chapter 10. Liquids and Solids

Chapter 10. Liquids and Solids Chapter 10 Liquids and Solids Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Metallic bonds Covalent bonds Ionic

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

Chapter 10: Liquids and Solids

Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids *Liquids and solids show many similarities and are strikingly different from their gaseous state. 10.1 Intermolecular Forces Intermolecular

More information

AP* Chapter 10. Liquids and Solids. Friday, November 22, 13

AP* Chapter 10. Liquids and Solids. Friday, November 22, 13 AP* Chapter 10 Liquids and Solids AP Learning Objectives LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses

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

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

Chapter 10 Liquids and Solids. Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, , 113

Chapter 10 Liquids and Solids. Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, , 113 Chapter 10 Liquids and Solids Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, 104-106, 113 Recall: Intermolecular vs. Intramolecular Forces Intramolecular: bonds between

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

Liquids and Solids Chapter 10

Liquids and Solids Chapter 10 Liquids and Solids Chapter 10 Nov 15 9:56 AM Types of Solids Crystalline solids: Solids with highly regular arrangement of their components Amorphous solids: Solids with considerable disorder in their

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

What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction

What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction Liquids and Solids What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction Types of Interparticle Forces Ionic Bonding Occurs between cations and anions Metallic

More information

ก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes

ก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes ก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes ก ก ก ก Mc-Graw Hill 1 Intermolecular Forces: Liquids, Solids, and Phase Changes 12.1 An Overview of Physical States and Phase Changes 12.2

More information

compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due

compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due Liquids and solids They are similar compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due to the molecules being close together in solids

More information

They are similar to each other. Intermolecular forces

They are similar to each other. Intermolecular forces s and solids They are similar to each other Different than gases. They are incompressible. Their density doesn t change much with temperature. These similarities are due to the molecules staying close

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

They are similar to each other

They are similar to each other They are similar to each other Different than gases. They are incompressible. Their density doesn t change much with temperature. These similarities are due to the molecules staying close together in solids

More information

Chapter 12 INTERMOLECULAR FORCES. Covalent Radius and van der Waals Radius. Intraand. Intermolecular Forces. ½ the distance of non-bonded

Chapter 12 INTERMOLECULAR FORCES. Covalent Radius and van der Waals Radius. Intraand. Intermolecular Forces. ½ the distance of non-bonded Chapter 2 INTERMOLECULAR FORCES Intraand Intermolecular Forces Covalent Radius and van der Waals Radius ½ the distance of bonded ½ the distance of non-bonded Dipole Dipole Interactions Covalent and van

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

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

Chapter 11 SOLIDS, LIQUIDS AND GASES Pearson Education, Inc.

Chapter 11 SOLIDS, LIQUIDS AND GASES Pearson Education, Inc. Chapter 11 SOLIDS, LIQUIDS AND GASES States of Matter Because in the solid and liquid states particles are closer together, we refer to them as. The States of Matter The state of matter a substance is

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

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

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

CHAPTER ELEVEN KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS

CHAPTER ELEVEN KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS CHAPTER ELEVEN AND LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS Differences between condensed states and gases? KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS Phase Homogeneous part

More information

Chapter 12 Intermolecular Forces and Liquids

Chapter 12 Intermolecular Forces and Liquids Chapter 12 Intermolecular Forces and Liquids Jeffrey Mack California State University, Sacramento Why? Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature

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

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

CHEM Principles of Chemistry II Chapter 10 - Liquids and Solids

CHEM Principles of Chemistry II Chapter 10 - Liquids and Solids CHEM 1212 - Principles of Chemistry II Chapter 10 - Liquids and Solids 10.1 Intermolecular Forces recall intramolecular (within the molecule) bonding whereby atoms can form stable units called molecules

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids 11.2 Intermolecular Forces Intermolecular forces are much weaker than ionic or covalent bonds (e.g., 16 kj/mol versus 431 kj/mol for HCl). Melting or boiling = broken intermolecular forces Intermolecular

More information

Intermolecular Forces and States of Matter AP Chemistry Lecture Outline

Intermolecular Forces and States of Matter AP Chemistry Lecture Outline Intermolecular Forces and States of Matter AP Chemistry Lecture Outline Name: Chemical properties are related only to chemical composition; physical properties are related to chemical composition AND the

More information

2) Of the following substances, only has London dispersion forces as its only intermolecular force.

2) Of the following substances, only has London dispersion forces as its only intermolecular force. 11.1 Multiple Choice and Bimodal Questions 1) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? A) CH 3CH 2 CH3 B) CH 3OCH3

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 10. Lesson Starter. Why did you not smell the odor of the vapor immediately? Explain this event in terms of the motion of molecules.

Chapter 10. Lesson Starter. Why did you not smell the odor of the vapor immediately? Explain this event in terms of the motion of molecules. Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of Gases Deviations of Real Gases from Ideal Behavior Section 1 The Kinetic-Molecular

More information

States of matter. Chapter 11. Kinetic Molecular Theory of Liquids and Solids. Kinetic Molecular Theory of Solids Intermolecular Forces

States of matter. Chapter 11. Kinetic Molecular Theory of Liquids and Solids. Kinetic Molecular Theory of Solids Intermolecular Forces States of matter Chapter 11 Intermolecular Forces Liquids and Solids By changing the T and P, any matter can exist as solid, liquid or gas. Forces of attraction determine physical state Phase homogeneous

More information

CHEMISTRY The Molecular Nature of Matter and Change

CHEMISTRY The Molecular Nature of Matter and Change CHEMISTRY The Molecular Nature of Matter and Change Third Edition Chapter 12 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 11 INTERMOLECULAR FORCES

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

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

Liquids & Solids. For the condensed states the ave KE is less than the attraction between molecules so they are held together.

Liquids & Solids. For the condensed states the ave KE is less than the attraction between molecules so they are held together. Liquids & Solids Intermolecular Forces Matter exists in 3 states. The state of matter is influenced by the physical properties of a substance. For liquids & solids, the condensed states, many of the physical

More information

Ch. 11: Liquids and Intermolecular Forces

Ch. 11: Liquids and Intermolecular Forces Ch. 11: Liquids and Intermolecular Forces Learning goals and key skills: Identify the intermolecular attractive interactions (dispersion, dipole-dipole, hydrogen bonding, ion-dipole) that exist between

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

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

Chapter 14. Liquids and Solids

Chapter 14. Liquids and Solids Chapter 14 Liquids and Solids Section 14.1 Water and Its Phase Changes Reviewing What We Know Gases Low density Highly compressible Fill container Solids High density Slightly compressible Rigid (keeps

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

Question 2 Identify the phase transition that occurs when CO 2 solid turns to CO 2 gas as it is heated.

Question 2 Identify the phase transition that occurs when CO 2 solid turns to CO 2 gas as it is heated. For answers, send email to: admin@tutor-homework.com. Include file name: Chemistry_Worksheet_0039 Price: $4 (c) 2012 www.tutor-homework.com: Tutoring, homework help, help with online classes. Chapter 11

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids 11.2 Intermolecular Forces Intermolecular forces are much weaker than ionic or covalent bonds (e.g., 16 kj/mol versus 431 kj/mol for HCl). Melting or boiling = broken intermolecular forces Intermolecular

More information

Chap 10 Part 4Ta.notebook December 08, 2017

Chap 10 Part 4Ta.notebook December 08, 2017 Chapter 10 Section 1 Intermolecular Forces the forces between molecules or between ions and molecules in the liquid or solid state Stronger Intermolecular forces cause higher melting points and boiling

More information

CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS. Chemistry 1411 Joanna Sabey

CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS. Chemistry 1411 Joanna Sabey CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS Chemistry 1411 Joanna Sabey Forces Phase: homogeneous part of the system in contact with other parts of the system but separated from them by a

More information

Chapter 9. Liquids and Solids

Chapter 9. Liquids and Solids Chapter 9 Liquids and Solids Chapter 9 Table of Contents (9.1) (9.2) (9.3) (9.4) (9.5) (9.6) (9.7) (9.8) (9.9) (9.10) Intermolecular forces The liquid state An introduction to structures and types of solids

More information

Liquids, Solids, and Phase Changes

Liquids, Solids, and Phase Changes C h a p t e r 10 Liquids, Solids, and Phase Changes KMT of Liquids and Solids 01 Gases have little or no interactions. Liquids and solids have significant interactions. Liquids and solids have well-defined

More information

Chapter 10. The Liquid and Solid States. Introduction. Chapter 10 Topics. Liquid-Gas Phase Changes. Physical State of a Substance

Chapter 10. The Liquid and Solid States. Introduction. Chapter 10 Topics. Liquid-Gas Phase Changes. Physical State of a Substance Introduction Chapter 10 The Liquid and Solid States How do the properties of liquid and solid substances differ? How can we predict properties based on molecular- level structure? Glasses Wires Reshaping

More information

Chem 112 Dr. Kevin Moore

Chem 112 Dr. Kevin Moore Chem 112 Dr. Kevin Moore Gas Liquid Solid Polar Covalent Bond Partial Separation of Charge Electronegativity: H 2.1 Cl 3.0 H Cl δ + δ - Dipole Moment measure of the net polarity in a molecule Q Q magnitude

More information

Chapter 14. Liquids and Solids

Chapter 14. Liquids and Solids Chapter 14 Liquids and Solids Review Solid - Has a definite (fixed) shape and volume (cannot flow). Liquid - Definite volume but takes the shape of its container (flows). Gas Has neither fixed shape nor

More information

Nestor S. Valera Ateneo de Manila. Chapter 12 - Intermolecular Forces

Nestor S. Valera Ateneo de Manila. Chapter 12 - Intermolecular Forces Nestor S. Valera Ateneo de Manila Chapter 12 - Intermolecular Forces 1 A phase is a region that differs in structure and/or composition from another region. 2 Phases Solid phase - ice Liquid phase - water

More information

Chapter 11: Intermolecular Forces. Lecture Outline

Chapter 11: Intermolecular Forces. Lecture Outline Intermolecular Forces, Liquids, and Solids 1 Chapter 11: Intermolecular Forces Lecture Outline 11.1 A Molecular Comparison of Gases, Liquids and Solids Physical properties of substances are understood

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

Chapter 10: Liquids and Solids

Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids STATES OF MATTER: At any temperature above absolute zero, the atoms, molecules, or ions that make up a substance are moving. In the kinetic theory of gases, this motion is

More information

Week 8 Intermolecular Forces

Week 8 Intermolecular Forces NO CALCULATORS MAY BE USED FOR THESE QUESTIONS Questions 1-3 refer to the following list. (A) Cu (B) PH 3 (C) C (D) SO 2 (E) O 2 1. Contains instantaneous dipole moments. 2. Forms covalent network solids.

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

Some Properties of Solids, Liquids, and Gases

Some Properties of Solids, Liquids, and Gases AP Chemistry: Intermolecular Forces, Liquids, and Solids Lecture Outline 11.1 A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These

More information

CHAPTER 10. States of Matter

CHAPTER 10. States of Matter CHAPTER 10 States of Matter Kinetic Molecular Theory Kinetikos - Moving Based on the idea that particles of matter are always in motion The motion has consequences Explains the behavior of Gases, Liquids,

More information

CHAPTER 10. Kinetic Molecular Theory. Five Assumptions of the KMT. Atmospheric Pressure

CHAPTER 10. Kinetic Molecular Theory. Five Assumptions of the KMT. Atmospheric Pressure Kinetic Molecular Theory CHAPTER 10 States of Matter Kinetikos - Moving Based on the idea that particles of matter are always in motion The motion has consequences Explains the behavior of Gases, Liquids,

More information

Ch 9 Liquids & Solids (IMF) Masterson & Hurley

Ch 9 Liquids & Solids (IMF) Masterson & Hurley Ch 9 Liquids & Solids (IMF) Masterson & Hurley Intra- and Intermolecular AP Questions: 2005 Q. 7, 2005 (Form B) Q. 8, 2006 Q. 6, 2007 Q. 2 (d) and (c), Periodic Trends AP Questions: 2001 Q. 8, 2002 Q.

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

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids Sample Exercise 11.1 (p. 450) In which of the following substances is hydrogen bonding likely to play an important role in determining physical properties: methane (CH 4 ), hydrazine (H 2 NNH 2 ), methyl

More information

Ch. 9 Liquids and Solids

Ch. 9 Liquids and Solids Intermolecular Forces I. A note about gases, liquids and gases. A. Gases: very disordered, particles move fast and are far apart. B. Liquid: disordered, particles are close together but can still move.

More information

States of Matter SM VI. Liquids & Solids. Liquids. Description of. Vapor Pressure. if IMF then VP, b.p.

States of Matter SM VI. Liquids & Solids. Liquids. Description of. Vapor Pressure. if IMF then VP, b.p. chem101/3, wi2010 po 20 1 States of Matter SM VI Description of Liquids & Solids chem101/3, wi2010 po 20 2 Liquids molecules slide along in close contact attraction due to various IMF s can diffuse, but

More information

CHE 107 Fall 2017 Exam 1

CHE 107 Fall 2017 Exam 1 CHE 107 Fall 2017 Exam 1 Your Name: Your ID: Question #: 1 Fill in the blanks with the letter corresponding to the correct term. Use each term only once. Your response for each one should be a single letter.

More information

Kinetic Theory (Kinetikos - Moving ) Based on the idea that particles of matter are always in motion

Kinetic Theory (Kinetikos - Moving ) Based on the idea that particles of matter are always in motion Chapter 10 Kinetic Theory (Kinetikos - Moving ) Based on the idea that particles of matter are always in motion The motion has consequences Behavior of Gases Physical Properties of Gases Ideal Gas an imaginary

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

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. Determine the oxidation number of the underlined element in K 2CO 3. a. 1 b. 2 c.

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids Chapter 11. Intermolecular Forces, Liquids, and Solids A Molecular Comparison of Gases, Liquids, and Solids Physical properties of substances are understood in terms of kinetic-molecular theory: Gases

More information

Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces

Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces Exam Accelerated Chemistry Study Sheet Chap12 Solids/Liquids/Intermolecular Forces Name /66 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Intermolecular

More information

Ch 11: Intermolecular Forces, Liquids, and Solids

Ch 11: Intermolecular Forces, Liquids, and Solids AP Chemistry: Intermolecular Forces, Liquids, and Solids Lecture Outline 11.1 A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These

More information

CHAPTER 10. Liquids and solids

CHAPTER 10. Liquids and solids CHAPTER 10 Liquids and solids 10.1 - Forces Solids and Liquids Gases can be compressed because gas particles are far apart. (ideal gases do not interact with one another NO IMF s) Liquid and solids are

More information

HEMISTRY 110 EXAM 3 April 6, 2011 FORM A When the path is blocked, back up and see more of the way. 1. A 250 L vessel is evacuated and then connected to a 50.0 L bulb with compressed nitrogen. The pressure

More information

Week 13 MO Theory, Solids, & metals

Week 13 MO Theory, Solids, & metals Week 13 MO Theory, Solids, & metals Q UEST IO N 1 Using the molecular orbital energy diagrams below, which one of the following diatomic molecules is LEAST likely to exist? A. Li2 B. Be2 C. B2 D. C2 E.

More information

CHEM 10113, Exam 4. All equations must be balanced and show phases for full credit. Significant figures count, and box your answers!

CHEM 10113, Exam 4. All equations must be balanced and show phases for full credit. Significant figures count, and box your answers! CHEM 10113, Exam 4 November 30, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, and box your answers! 1. (10 points) Consider the phase

More information

Honors Chemistry Dr. Kevin D. Moore

Honors Chemistry Dr. Kevin D. Moore Honors Chemistry Dr. Kevin D. Moore Key Properties: Solid is less dense than liquid Water reaches maximum density at 4 C Very high specific heat Dissolves many substances Normal Boiling Point: 100 C Normal

More information

States of Matter; Liquids and Solids. Condensation - change of a gas to either the solid or liquid state

States of Matter; Liquids and Solids. Condensation - change of a gas to either the solid or liquid state States of Matter; Liquids and Solids Phase transitions - a change in substance from one state to another Melting - change from a solid to a liquid state Freezing - change of a liquid to the solid state

More information

a) 1.3 x 10 3 atm b) 2.44 atm c) 8.35 atm d) 4.21 x 10-3 atm e) 86.5 atm

a) 1.3 x 10 3 atm b) 2.44 atm c) 8.35 atm d) 4.21 x 10-3 atm e) 86.5 atm 1. (6 pts) A sample of gas with a volume of 750 ml exerts a pressure of 756 mm Hg at 30.0 0 C. What pressure (atm) will the sample exert when it is compressed to 250 ml and cooled to -25.0 0 C? a) 1.3

More information

Intermolecular forces (IMFs) CONDENSED STATES OF MATTER

Intermolecular forces (IMFs) CONDENSED STATES OF MATTER Intermolecular forces (IMFs) CONDENSED STATES OF MATTER States of Matter: - composed of particles packed closely together with little space between them. Solids maintain a. - any substance that flows.

More information

Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided.

Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided. CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. a. The gas

More information

Notes on Solids and Liquids

Notes on Solids and Liquids THE LIQUID STATE Notes on Solids and Liquids Why do liquids tend to bead up when on a solid surface? The effect of uneven pull on surface molecules draws them into the body of the liquid causing droplet

More information

Properties of Liquids and Solids

Properties of Liquids and Solids Properties of Liquids and Solids World of Chemistry Chapter 14 14.1 Intermolecular Forces Most substances made of small molecules are gases at normal temperature and pressure. ex: oxygen gas, O 2 ; nitrogen

More information

Chem 1A Dr. White Fall 2015 Exam 3 Practice Problems

Chem 1A Dr. White Fall 2015 Exam 3 Practice Problems Exam 3 Practice Problems 1. The face centered cubic cell of copper has an edge length of 0.362 nm. Calculate the density of copper (g/cm 3 ). 2. Consider the following ionic substances and arrange them

More information

Some Properties of Solids, Liquids, and Gases

Some Properties of Solids, Liquids, and Gases AP Chemistry: Intermolecular Forces, Liquids, and Solids Sec 1. A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These are forces

More information

General Chemistry 202 CHM202 General Information. General Chemistry 202 CHM202 Policies. General Chemistry 202 CHM202 Laboratory Guidelines

General Chemistry 202 CHM202 General Information. General Chemistry 202 CHM202 Policies. General Chemistry 202 CHM202 Laboratory Guidelines General Chemistry 202 CHM202 General Information Instructor Meeting times and places Text and recommended materials Website Email Grading Schedule 1 General Chemistry 202 CHM202 Policies Equipment Instruction

More information

9/2/10 TYPES OF INTERMOLECULAR INTERACTIONS

9/2/10 TYPES OF INTERMOLECULAR INTERACTIONS Tro Chpt. 11 Liquids, solids and intermolecular forces Solids, liquids and gases - A Molecular Comparison Intermolecular forces Intermolecular forces in action: surface tension, viscosity and capillary

More information

Chapter 12 Intermolecular Forces of Attraction

Chapter 12 Intermolecular Forces of Attraction Chapter 12 Intermolecular Forces of Attraction Intermolecular Forces Attractive or Repulsive Forces between molecules. Molecule - - - - - - Molecule Intramolecular Forces bonding forces within the molecule.

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 12. Insert picture from First page of chapter. Intermolecular Forces and the Physical Properties of Liquids and Solids

Chapter 12. Insert picture from First page of chapter. Intermolecular Forces and the Physical Properties of Liquids and Solids Chapter 12 Insert picture from First page of chapter Intermolecular Forces and the Physical Properties of Liquids and Solids Copyright McGraw-Hill 2009 1 12.1 Intermolecular Forces Intermolecular forces

More information

Solids, Liquids and Gases

Solids, Liquids and Gases WHY? Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water? Why do snowflakes have 6 sides? Why is I

More information

Chapter 10 Liquids, Solids, and Intermolecular Forces

Chapter 10 Liquids, Solids, and Intermolecular Forces Chapter 10 Liquids, Solids, and Intermolecular Forces The Three Phases of Matter (A Macroscopic Comparison) State of Matter Shape and volume Compressibility Ability to Flow Solid Retains its own shape

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Surveying the Chapter: Page 442 Chapter 11 Intermolecular Forces, Liquids, and Solids We begin with a brief comparison of solids, liquids, and gases from a molecular perspective, which reveals the important

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

Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces

Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces Remember Chapter 12.1 Introduction to Kinetic Molecular Theory and Intermolecular forces 1 To understand properties, we want to connect what we see to what is happening on a molecular level. Start with

More information

Multiple Choice. Multiple Choice

Multiple Choice. Multiple Choice 1. At what temperature in degree Celcius is the value in degree Fahrenheit twice of that in degree Celcius? A) 160 o C B) -24.6 o C C) 6.4 o C D) 22.2 o C E) 32 o C 2. The correct name for NaOCl is, A)

More information

CDO AP Chemistry Unit 7 Review

CDO AP Chemistry Unit 7 Review CDO AP Chemistry Unit 7 Review MULTIPLE CHOICE REVIEW 1. Surface tension in a liquid is due to the fact that a) surface molecules are pulled toward the interior b) liquids tend toward lowest energy c)

More information

Intermolecular Forces

Intermolecular Forces Intermolecular Forces Molecular Compounds The simplest molecule is H 2 : Increased electron density draws nuclei together The pair of shared electrons constitutes a covalent bond. Intermolecular Forces

More information