Experiment 14. Intermolecular Forces rev 1/12

Size: px
Start display at page:

Download "Experiment 14. Intermolecular Forces rev 1/12"

Transcription

1 Experiment 14 Intermolecular Forces rev 1/12 GAL: We will examine connections between molecular structure, intermolecular forces, and physical properties. BAKGRUND: Physical properties such as solubility, melting point, and boiling point are determined by a substance s intermolecular forces. Non-polar molecules have the weak intermolecular forces known as London dispersion forces caused by slight, temporary asymmetries in their electron clouds. Although London dispersion forces are relatively weak, as the number of electrons in a molecule increases so does the strength of the London dispersion forces. So, if we are comparing several non-polar molecules to each other, we expect the largest ones (with the most electrons) to have strongest London dispersion forces. Polar molecules have London dispersion forces in addition to dipole forces. Dipole forces are attractions between + and - charges on the molecules. Dipole forces are generally stronger than London dispersion forces because the charges are permanent, not temporary, and the charges are stronger. Both dipole forces and London dispersion forces figure into the total strength of intermolecular forces for polar compounds. Suppose we had two molecules with very similar London dispersion forces but one was polar and one was not. The presence of the dipole forces will give the polar molecule stronger intermolecular forces overall. - + ydrogen bonds are the strongest intermolecular forces found in covalent compounds. They are formed by the attraction between a hydrogen atom on one molecule and a nonbonding pair of electrons on a second molecule. ydrogen bonds are found only in molecules where a hydrogen atom is bonded to fluorine, oxygen, or nitrogen. These molecules also have dipole and London dispersion forces, and all three types of forces contribute to the total strength of intermolecular forces. The presence of hydrogen bonding makes the total intermolecular forces very strong and leads to high melting and boiling points. aving multiple groups capable of hydrogen bonding makes melting points even higher. Two molecules with exactly the same types of intermolecular forces may still differ from each other in the strength and impact of these forces due to general molecule shape or the placement of hydrogen bonding groups which are very particular about geometry. Linear and planar molecules often exhibit stronger intermolecular forces because their shape allows the molecules to pack closely and maximize the interactions. The combined effects of all intermolecular forces determine physical properties. The stronger the intermolecular forces a compound has, the more energy will be required to overcome those attractions. Thus, strong intermolecular forces correspond to high boiling points and less volatile compounds, i.e., ones that will evaporate less. In Part 1, you will observe several liquids as they evaporate. All liquids 2012 Intermolecular Forces 15-1

2 cool as they evaporate because they must use energy to overcome intermolecular forces and move into the gas phase. The liquids that show the most cooling have lost the most molecules due to evaporation. This indicates a compound with weaker intermolecular forces. In Part 2, you will measure the melting points of several compounds. In Part 3, you ll also use Spartan Student to calculate their dipole moments (polarities). In Part 4, you will use physical models to look at intermolecular forces in water and aqueous solutions. Table 1: Names and Structures of rganic ompounds Used in this Experiment Name Structure Name Structure methanol ethanol 1-propanol 1-butanol pentane hexane benzoic acid 2-hydroxybenzoic acid or o-salicylic acid 4-hydroxybenzoic acid or p-salicylic acid naphthalene 15-2 Intermolecular Forces 2012

3 PRE-LAB ASSIGNMENT: Two of the molecules you will study this week are methanol and ethanol. The structures of these molecules are given on page opy the structures in your notebook. List all the types of intermolecular forces these molecules have. AZARDS: Several of the liquids that you will be working with are highly flammable, so no flames are allowed in the lab. While none of the chemicals used in this experiment pose unusual health hazards, your hands may be exposed to these chemicals. Wear disposable gloves to limit your exposure. Keep the test tubes containing the liquids closed when not in use. Part 1 is done in the hood. Look up the MSDS for methanol ( or Trexler 464). Record the following information in your notebook hazards section: appearance, odor, and boiling point (see Physical & hemical Properties) a summary of potential health effects (see azards Identification) a summary of potential effects if released to the environment (see Ecological Information) LABRATRY DATA AND BSERVATINS: The in-lab portion of this experiment will be done in teams of two students, but the lab reports will be done separately. This means each student will need a full set of notebook entries. Note the name of your in-lab partner in your lab notebook. Remember to record both what you do and what you observe in your notebook. The four parts of this experiment may be done in any order. Your lab instructor will assign you to start with a given part in order to avoid congestion. PART 1 PREDURE: Evaporation 1. Your numerical data for Part 1 will be most easily recorded in a table with four columns labeled: liquid, maximum temperature, minimum temperature, and. You will need one line for each of the six liquids tested. 2. Use one of the computers that are set up in a hood. If it has not already been done for you, prepare the computer for data collection by opening Experiment 13 from the Roanoke Experiments folder in Logger Pro. n the Graph window, the vertical axis has temperature scaled from 5 to 30 o. The horizontal axis has time scaled from 0 to 250 seconds. 3. Wrap Probe 1 and Probe 2 with square pieces of filter paper secured by wire. Roll the filter paper around the probe tip in the shape of a cylinder. The paper should be even with the probe end. 4. You will be testing 6 liquids. The four alcohols are methanol, ethanol, 1-propanol, and 1-butanol. The two alkanes are pentane and hexane. These have been pre-measured into test tubes. You may do the liquids in any order. Get two liquids at a time. When finished, return the liquids to the supply bench so that others may use them. Keep the liquids stoppered when they are not in use Intermolecular Forces 15-3

4 5. Wear gloves for the rest of Part 1. Stand Probe 1 in the first liquid container and Probe 2 in the second liquid container. Record which probe goes into which liquid. Make sure the containers do not tip over. 6. Prepare 2 pieces of masking tape, each about 10-cm long, to be used to tape the probes in position during Step After the probes have been in the liquids for at least 30 seconds, begin data collection by clicking. Monitor the temperature for 15 seconds to establish the initial (maximum) temperature of each liquid. Then simultaneously remove the probes from the liquids and tape them to the metal flashing at the front edge of the hood so that the probe tips extend 5 cm over the edge and into the hood. The probe tip should not touch the working surface of the hood. Pull the hood sash down as far as you can. Stopper the test tubes to minimize the loss of these liquids. 8. When both temperatures have reached minimums and have begun to increase, click to end data collection. Two statistics boxes should appear on the screen. You may need to drag the boxes apart since the computer sometimes places them on top of each other. Record the maximum and minimum values for Temperature Probe 1 (first liquid) and Temperature Probe 2 (second liquid) in your notebook. 9. For each liquid, subtract the minimum temperature from the maximum temperature to determine T, the temperature change during evaporation. Record this in your table. 10. Roll the rubber band up the probe shaft and dispose of the filter paper in the waste container in the hood. 11. Return your first two liquids to the supply bench. Be sure they are stoppered. Get two different liquids. When you choose ollect for your second set of liquids, you will be prompted to discard your prior set of data. Discard it. Repeat the procedure above first for liquids 3 & 4, and then for liquids 5 & Be sure that both you and your lab partner have a full set of data before leaving lab. Remember that you will write up your reports separately. PART 2 PREDURE: Melting points of organic solids 1. ne member of your team should prepare melting point capillaries of benzoic acid and naphthalene. The other team member should prepare melting point capillaries of 2- hydroxybenzoic acid (or o-salicylic acid) and 4-hydroxybenzoic acid (or p-salicylic acid). Remember that you need just one crystal of each in your capillary. Set each capillary on a labeled piece of paper so that you don t mix them up. 2. Measure the melting point range of each solid, starting with the temperature where you first see softening to the temperature where the entire sample has melted. Put both capillaries in the MelTemp at the same time. Make sure you know which is which. You will heat rapidly until you near the melting point for each compound and then slow the rate of heating to just 1 o every seconds Intermolecular Forces 2012

5 3. If you are doing the benzoic acid/naphthalene set, heat quickly to 70 o then adjust so that temperature increases just 1 o every seconds until your first solid melts. Now heat quickly to 110 o and then again adjust so that temperature increases just 1 o every seconds until your second solid melts. For each solid, you should record a melting point range of just a degree or two in which the solid softened and melted. 4. If you are doing the 2-hydroxybenzoic acid/4-hydroxybenzoic set, heat quickly to 145 o then adjust so that temperature increases just 1 o every seconds until your first solid melts. Now heat quickly to 205 o and then again adjust so that temperature increases just 1 o every seconds until your second solid melts. For each solid, you should record a melting point range of just a degree or two in which the solid softened and melted. 5. As soon as your second solid melts, get the apparatus cooling back down using the compressed air. Dispose of the capillaries in the broken glass box. PART 3 PREDURE: Using Spartan Student to calculate dipole moments of organic solids 1. Use Spartan Student to draw models of the four molecules from Part 2: benzoic acid, 2- hydroxybenzoic acid, 4-hydroxybenzoic acid, and naphthalene. Follow the structures which are shown on page 2. ave these drawings handy to follow. Recall that you used Spartan Student for Exp 11 in EM 111. Begin by opening Spartan Student on one of the lab computers. 2. pen a new file by clicking the button. n the righthand side of the screen, you should see a collection of molecular fragments that you can use to build the molecules. 3. Start by building benzoic acid. Add a benzene ring to the main drawing area. Now click on the Groups dropdown menu. hoose arboxylic Acid. Add this to an open bond in your drawing. 4. Spartan should recognize your drawing as benzoic acid. Look at the bottom right of the screen. lick the up arrow next to the name. hoose Replace. 5. Now click View: lick and drag to rotate the molecule. 6. From the dropdown menu at the top of the screen, choose Display, Properties. Record the displayed dipole moment in your notebook. 7. You can easily modify this benzoic acid structure into 2-hydroxybenzoic acid, also known as salicylic acid. lick Add Fragment: 8. hoose the molecular fragment at right that is an oxygen atom with two single bonds. Add this to the appropriate place on your molecule. Spartan should recognize your molecule. Follow steps 4-6 above to find your dipole moment. 9. Again modify your structure, this time to form 4-hydroxybenzoic acid. lick on Add Fragment as in Step 7. Now delete the group from your molecule using the Delete Button: Switch back to Add Fragment, and add the new group on the correct spot Intermolecular Forces 15-5

6 10. Again, Spartan should recognize your molecule as p-salicylic acid. Follow steps similar to Steps 4-6 above to find the dipole moment. 11. The last molecule you need to make is naphthalene. It is sufficiently different from the others that you should close this file and open a new one using the buttons across the top of the screen. You do not need to save a copy of the current file. 12. nce you have a blank drawing area, choose the Rings dropdown menu and select Naphthalene. You do not need to modify this structure! Simply follow Steps 4-6 above to record the dipole moment. 13. nce you have dipole moments for your four compounds, simply use the lose File button but leave the software open for the next group of students. PART 4 PREDURE: Intermolecular forces in water and aqueous solutions 1. Spread out your up of Water models. You should have 12 2 molecules, one Na 1+ ion, one l 1- ion, one hydroxyl group, and one 2 6 (ethane) molecule. Small magnets in the models will help us simulate intermolecular forces. Record observations in your notebook as you follow the instructions below. 2. Select two 2 molecules. ow are they most attracted to each other: to, to, to, or some combination of these? Which two types of intermolecular forces are being represented here? Record your observations. 3. hoose one 2 molecule to be your central molecule. ow many other water molecules can you attach directly to this one central molecule? Draw a structure similar to the one of water molecules on page 13-1 but showing how all the molecules attach to the central water molecule. 4. In solid 2 (ice), the water molecules arrange themselves so that each water molecule can hydrogen bond with as many others as possible. Arrange all 12 of your water molecules in the most compact structure that also maximizes hydrogen bonding. Use a sketch and written description to record this structure in your notebook. Describe how much open space is trapped inside your solid structure. 5. In liquid 2, the water molecules are constantly forming and breaking intermolecular hydrogen bonds as the individual molecules move. Take your model of solid ice in your hands and compact it like you would a snow ball to simulate this. When compared to your solid structure before, how much open space is now trapped inside the liquid structure? 6. Now let s consider how solutes interact with water molecules. Find the Nal. The smaller ion is Na 1+. Note the strength of its attraction for a l 1- ion. ow many l 1- could fit around a single Na 1+? 7. Examine the Nal model on the instructor s bench. Use a sketch and written description to record this structure in your notebook Intermolecular Forces 2012

7 8. ow are water molecules attracted to the Na 1+ : through the or through the? Fit the maximum number of water molecules on the Na 1+ possible. Use a sketch and written description to record this structure in your notebook. 9. ow are water molecules attracted to the l 1- : through the or through the? Fit the maximum number of water molecules on the l 1- possible. Use a sketch and written description to record this structure in your notebook. 10. You should now have a Na 1+ surrounded by water molecules and a l 1- surrounded by water molecules. This is how they actually exit in water. We say that each ion is surrounded by a hydration sphere. old the hydrated Na 1+ next to the hydrated l 1-. With the hydration spheres intact, will the ions stick together? 11. Pull the water off the ions and examine the attraction between the water molecules and the ethane ( 2 6 ) molecule. ow strong is its attraction for water? Does it form a hydration sphere? 12. ne of the hydrogen atoms on the ethane molecule is marked with a small colored spot and small raised dots on the carbon atom at its base. arefully remove this hydrogen and set it aside in a safe place. Insert the, hydroxyl group, in its place. You now have 2 5, ethanol. ow strong is its attraction for water? Use a sketch and written description to record the structure/interaction between ethanol and water. 13. Remove the from your ethanol and replace the that you previously set aside. arefully count the models as you return them to the original cup. Be sure that you have 12 2 molecules, one Na 1+ ion, one l 1- ion, and one hydroxyl group, and one 2 6 ethane molecule. RESULTS: For Part 1, prepare a Results table with 6 columns: liquid name, formula, structure, molar mass, intermolecular forces, and T. Structures for the liquids are given in the Introduction. List all the intermolecular forces expected for each compound. The Introduction or your textbook will provide help. ombine Parts 2 and 3, preparing a Results table with 7 columns: compound name, structure, molar mass, experimental melting point, literature melting point, dipole moment, and intermolecular forces. Structures for the compounds are given in the Introduction (draw them in by hand). Experimental melting points are the ones you found in lab. Literature melting points are accepted values that you find in chemical literature. Look up your compounds in either the R (see the Table of Physical Properties of rganic ompounds) or the Merck Index. List the source of your data just below your Results table. In the final column, list all the intermolecular forces expected for each compound. QUESTINS: Questions 1-4 refer to Part 1 only: 1. Which of the alcohols studied in Part 1 has the strongest intermolecular forces of attraction? The weakest intermolecular forces? Explain how the results of this experiment show this. Explain how this result could be predicted from looking at the structures or formulas Intermolecular Forces 15-7

8 2. Which of the alkanes studied in Part 1 has the stronger intermolecular forces of attraction? The weaker intermolecular forces? Explain how the results of this experiment show this. Explain how this result could be predicted from looking at the structures or formulas. 3. Two of the liquids, pentane (an alkane) and 1-butanol (an alcohol), have nearly the same molar masses, but significantly different t values. Explain the difference in t values of these substances, based on their intermolecular forces. 4. Diethyl ether ( ) has a molar mass similar to that of pentane and 1-butanol (see Question 3). Draw the Lewis structure of diethyl ether. Is it polar or non-polar? What types of intermolecular forces are expected in diethyl ether? What t do you predict for diethyl ether? (Think about the t you measured for pentane and 1-butanol) Explain your reasoning. Questions 5-9 refer to Parts 2 and 3 only: 5. ow well do your experimental melting points correspond to the literature melting points? What might cause an experimental melting point to deviate from an accepted value? 6. Rank your four compounds in order of increasing molar mass. Do your melting points correlate well with molar mass (that is, does increasing molar mass always cause a similarly sized increase in melting point)? ite examples from your data to support your statement. 7. Rank your four compounds in order of increasing dipole moment. Do your melting points correlate well with dipole moment (that is, does increasing dipole moment always cause a similarly sized increase in melting point)? ite examples from your data to support your statement. 8. What general connection should exist between melting points and the strength of intermolecular forces? Give a general explanation of why this is true. (Talk about changes that happen when a solid melts.) See the Introduction or your textbook for help. 9. Polar molecules should have a measurable dipole moment. Do the dipole moments that Spartan calculated correspond to your polarity predictions from just looking at the structures? ite examples from your data to support your statement. Questions refer to Part 4 only: 10. List all the types of intermolecular forces present in a sample of pure water. Describe each in a sentence or two. Which of these were simulated by our models? 11. Use what you observed about the structures of solid and liquid water to explain why ice floats on liquid water. (int: think about the effect of that open space you noticed) 12. Nal dissolves well in water. Describe what you observed with the models to explain why and how it dissolves. 13. Describe the interactions between water and the two related molecules of ethane and ethanol. Which will be more soluble in water? Why? 15-8 Intermolecular Forces 2012

Evaporation and Intermolecular Attractions

Evaporation and Intermolecular Attractions Evaporation and Intermolecular Attractions BACKGROUND A substance absorbs energy from its surroundings as it changes from the liquid to the gas phase. The absorption of heat by the evaporating substance

More information

Evaporation and Intermolecular Attractions

Evaporation and Intermolecular Attractions Name Partners: Evaporation and Intermolecular Attractions Experiment 1 In this experiment, Temperature Probes are placed in various liquids. Evaporation occurs when the probe is removed from the liquid

More information

Evaporation and Intermolecular Forces

Evaporation and Intermolecular Forces Evaporation and Intermolecular Forces In this experiment, temperature probes are placed in various liquids. Evaporation occurs when the probe is removed from the liquid's container. This evaporation is

More information

EVAPORATION AND INTERMOLECULAR ATTRACTIONS From Chemistry with Vernier, Vernier Software and Technology LABQUEST 9

EVAPORATION AND INTERMOLECULAR ATTRACTIONS From Chemistry with Vernier, Vernier Software and Technology LABQUEST 9 EVAPORATION AND INTERMOLECULAR ATTRACTIONS From Chemistry with Vernier, Vernier Software and Technology LABQUEST 9 Westminster College In this experiment, Temperature Probes are placed in various liquids.

More information

Intermolecular and Ionic Forces

Intermolecular and Ionic Forces Intermolecular and Ionic Forces Comparing IMF Using Percent Evaporation: This lab will explore changing masses during evaporation of organic liquids. The decrease in mass is related to the strength of

More information

Experiment 13: EFFECT OF STRUCTURE ON PHYSICAL PROPERTIES

Experiment 13: EFFECT OF STRUCTURE ON PHYSICAL PROPERTIES Experiment 13: EFFET F STRUTURE N PYSIAL PRPERTIES Purpose: The relationships between the structures of molecules and their physical properties, such as volatility, viscosity, and solubility are examined.

More information

2.26 Intermolecular Forces

2.26 Intermolecular Forces 2.26 Intermolecular Forces Intermolecular forces are the relatively weak forces that exist between molecules. These govern the physical properties such as boiling point, melting point, solubility in solvents

More information

Lab #20: Observing the Behavior of Electrons

Lab #20: Observing the Behavior of Electrons Lab #20: Observing the Behavior of Electrons Background: In today s lab we will examine the attractive forces that hold molecules together and the disruptive forces that break them apart. The forces between

More information

May the Force Be with You

May the Force Be with You hemistry May the Force Be with You Exploring Evaporation and Intermolecular Forces MATERIALS AND RESOURES EA GROUP aprons data collection device filter paper, any size goggles paper towels 2 sensors, temperature,

More information

Intermolecular Forces in Solids, Liquids, and Gases What Do You See?

Intermolecular Forces in Solids, Liquids, and Gases What Do You See? Section 2 Intermolecular Forces in Solids, Liquids, and Gases What Do You See? Learning Outcomes In this section you will Describe how the size and shape of molecules affect their physical state. Classify

More information

Chemistry: A Molecular Approach, 1 st Ed. Nivaldo Tro

Chemistry: A Molecular Approach, 1 st Ed. Nivaldo Tro hemistry: A Molecular Approach, 1 st Ed. Nivaldo Tro Roy Kennedy Massachusetts Bay ommunity ollege Wellesley ills, MA 2008, Prentice all omparisons of the States of Matter the solid and liquid states have

More information

2.26 Intermolecular Forces

2.26 Intermolecular Forces 2.26 Intermolecular Forces Intermolecular forces are the relatively weak forces that exist between molecules. These govern the physical properties such as boiling point, melting point, solubility in solvents

More information

Intermolecular Forces I

Intermolecular Forces I I How does the arrangement of atoms differ in the 3 phases of matter (solid, liquid, gas)? Why doesn t ice just evaporate into a gas? Why does liquid water exist at all? There must be some force between

More information

2.2.2 Bonding and Structure

2.2.2 Bonding and Structure 2.2.2 Bonding and Structure Ionic Bonding Definition: Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form

More information

Ashes to Ashes: Using evaporation rate to identify an unknown liquid

Ashes to Ashes: Using evaporation rate to identify an unknown liquid Case File 11 Ashes to Ashes: Using evaporation rate to identify an unknown liquid Measure and compare the cooling rates of unknown liquids, and identify the probable arsonist. PROBABLE ARSON Investigator:

More information

9. Solubilities of Ionic and Molecular Substances

9. Solubilities of Ionic and Molecular Substances 9. Solubilities of Ionic and Molecular Substances What you will accomplish in this experiment You ll investigate the like dissolves like rule for predicting the ability of a solute to dissolve in a given

More information

CHM Salicylic Acid Properties (r16) 1/11

CHM Salicylic Acid Properties (r16) 1/11 CHM 111 - Salicylic Acid Properties (r16) 1/11 Purpose In this lab, you will perform several tests to attempt to confirm the identity and assess the purity of the substance you synthesized in last week's

More information

CHAPTER 3 HW SOLUTIONS: INTERMOLECULAR FORCES

CHAPTER 3 HW SOLUTIONS: INTERMOLECULAR FORCES APTER 3 W SLUTINS: INTERMLEULAR FRES ENERGY DIAGRAMS 1. Label and answer questions about the following energy diagram. Energy * I * I * small E a3 a. ow many steps are in the overall reaction? 3 b. Label

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

One Q partial negative, the other partial negative Ø H- bonding particularly strong. Abby Carroll 2

One Q partial negative, the other partial negative Ø H- bonding particularly strong. Abby Carroll 2 Chemistry Notes v Polarity Experiment Ø Things involved Polarity Solubility Dispersion Ø Polarity Shaving cream has soap steric acid Water is polar Food coloring is polar/ionic because dissolved Like dissolves

More information

Intermolecular Forces

Intermolecular Forces Intermolecular Forces H covalent bond (stronger) Cl H Cl intermolecular attraction (weaker) The attractions between molecules are not nearly as strong as the covalent bonds that hold atoms together. They

More information

Intermolecular Forces of Attraction

Intermolecular Forces of Attraction Name Unit Title: Covalent Bonding and Nomenclature Text Reference: Pages 189-193 Date Intermolecular Forces of Attraction Intramolecular vs. Intermolecular So far in our discussion of covalent bonding,

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

What determines whether a substance will be a solid, liquid, or gas? Thursday, April 24, 14

What determines whether a substance will be a solid, liquid, or gas? Thursday, April 24, 14 What determines whether a substance will be a solid, liquid, or gas? Answer: The attractive forces that exists between its particles. Answer: The attractive forces that exists between its particles. For

More information

Ch. 10 in- Class Exercise

Ch. 10 in- Class Exercise Chemistry 123/125 Ch. 10 in- Class Exercise In a liquid, the molecules are very close to one another and are constantly moving and colliding. Molecules attract each other, and the force of attraction is

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

Intermolecular Forces

Intermolecular Forces Intermolecular Forces 5/14/12 Do now: find a piece of metal at your table and describe three properties about it Work on bonding types Homework: work on pg 209 1-7 Due Wednesday Blazertime: finish organic

More information

Chemistry II Unit 5b Practice Test

Chemistry II Unit 5b Practice Test Practice for Unit 5b Exam 2013 1 Unit5Practicetest2013.odt Chemistry II Unit 5b Practice Test Reading: This material is covered in chapter 5 and chapter 12 in your book. Your notes and your molecular drawings

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

WKS Name Intermolecular Forces Period Date

WKS Name Intermolecular Forces Period Date WKS Name Intermolecular orces Period Date Introduction: Substances exist in three states of matter: solids, liquids and gases. We know that molecules are... (a) far apart in gases; (b) close together,

More information

Honors Unit 9: Liquids and Solids

Honors Unit 9: Liquids and Solids Name: Honors Unit 9: Liquids and Solids Objectives: 1. Students will be able to describe particles in the solid, liquid, and gas phases, and to explain what happens during phase transitions in terms of

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

The Phase Change Lab: Freezing and Melting of Water

The Phase Change Lab: Freezing and Melting of Water The Phase Change Lab: Freezing and Melting of Water Experiment 3 Freezing temperature is the temperature at which a substance turns from a liquid to a solid. Melting temperature is the temperature at which

More information

What biological molecules have shapes and structures that depend on intermolecular forces?

What biological molecules have shapes and structures that depend on intermolecular forces? Chapter 11 Reading Guide Intermolecular Forces Dr. Baxley Tro 3 rd edition 1 Section 11.1: How do geckos stick to walls? What biological molecules have shapes and structures that depend on intermolecular

More information

What factors affect whether something is a solid, liquid or gas? What actually happens (breaks) when you melt various types of solids?

What factors affect whether something is a solid, liquid or gas? What actually happens (breaks) when you melt various types of solids? States of Mattter What factors affect whether something is a solid, liquid or gas? What actually happens (breaks) when you melt various types of solids? What external factors affect whether something is

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

HYDROCARBONS: STRUCTURE & PROPERTIES

HYDROCARBONS: STRUCTURE & PROPERTIES YDROARBONS: STRUTURE & PROPERTIES PURPOSE: To discover the physical and chemical properties of alkanes, alkenes, and aromatic hydrocarbons. To identify an unknown hydrocarbon by comparing it to known samples.

More information

Comparing Ionic and Covalent Compounds

Comparing Ionic and Covalent Compounds Comparing Ionic and Covalent Compounds It takes energy to overcome the forces holding particles together. Thus, it takes energy to cause a substance to go from the liquid to the gaseous state. The boiling

More information

Name: Hour: Teacher: ROZEMA / CHEMISTRY. Molecular Attractions

Name: Hour: Teacher: ROZEMA / CHEMISTRY. Molecular Attractions Name: Hour: Teacher: ROZEMA / CHEMISTRY Molecular Attractions Name: Hour: Teacher: Ms. Rozema Starter Questions Grading: 2 pts = Date and full question written, question answered. 1 pt. = one requirement

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

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

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

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: Background

Intermolecular forces: Background Intermolecular forces: Background Electrostatics Up until now, we have just discussed attractions between molecules in the area of the covalent bond. Here, atoms within a molecule are attracted to one

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

Quick Review. 1. Hybridization. 2. Delocalization. 3. We will not be talking about Molecular Orbital Model.

Quick Review. 1. Hybridization. 2. Delocalization. 3. We will not be talking about Molecular Orbital Model. Quick Review 1. ybridization. 2. Delocalization. 3. We will not be talking about Molecular Orbital Model. **OUR EXAM II IS TURSDAY April 2 nd at 7pm** *BQ5, BQ6 and BQM are in 66 Library *BQ1, BQ2, BQ3,

More information

EXPERIMENT 15. USING CONDUCTIVITY TO LOOK AT SOLUTIONS: DO WE HAVE CHARGED IONS OR NEUTRAL MOLECULES? rev 7/09

EXPERIMENT 15. USING CONDUCTIVITY TO LOOK AT SOLUTIONS: DO WE HAVE CHARGED IONS OR NEUTRAL MOLECULES? rev 7/09 EXPERIMENT 15 USING CONDUCTIVITY TO LOOK AT SOLUTIONS: DO WE AVE CARGED IONS OR NEUTRAL MOLECULES? rev 7/09 GOAL After you complete this experiment, you should have a better understanding of aqueous solutions

More information

Empirical Gas Laws (Parts 1 and 2) Pressure-volume and pressure-temperature relationships in gases

Empirical Gas Laws (Parts 1 and 2) Pressure-volume and pressure-temperature relationships in gases Empirical Gas Laws (Parts 1 and 2) Pressure-volume and pressure-temperature relationships in gases Some of the earliest experiments in chemistry and physics involved the study of gases. The invention of

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 OR WHY IS WATER SPECIAL?

Intermolecular Forces OR WHY IS WATER SPECIAL? Intermolecular Forces OR WHY IS WATER SPECIAL? Define the prefixes Inter Between, as internet, interstate Intra Inside, as intramural Intermolecular Forces (2) Forces between covalent molecules These are

More information

EXPERIMENT 7 - Distillation Separation of a Mixture

EXPERIMENT 7 - Distillation Separation of a Mixture EXPERIMENT 7 - Distillation Separation of a Mixture Purpose: a) To purify a compound by separating it from a non-volatile or less-volatile material. b) To separate a mixture of two miscible liquids (liquids

More information

This activity has been used in an introductory chemistry course (prep chemistry or GOB course) Learning Goals: Prerequisite knowledge

This activity has been used in an introductory chemistry course (prep chemistry or GOB course) Learning Goals: Prerequisite knowledge This activity has been used in an introductory chemistry course (prep chemistry or GOB course) Learning Goals: Name phase changes Identify phase changes at molecular (particulate) level Name intermolecular

More information

CHEMISTRY Matter and Change. Chapter 12: States of Matter

CHEMISTRY Matter and Change. Chapter 12: States of Matter CHEMISTRY Matter and Change Chapter 12: States of Matter CHAPTER 12 States of Matter Section 12.1 Section 12.2 Section 12.3 Section 12.4 Gases Forces of Attraction Liquids and Solids Phase Changes Click

More information

The dative covalent bond acts like an ordinary covalent bond when thinking about shape so in NH 4. the shape is tetrahedral

The dative covalent bond acts like an ordinary covalent bond when thinking about shape so in NH 4. the shape is tetrahedral 1.3 Bonding Definition Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form ve ions. Non-metal atoms gain

More information

Physical States of Matter

Physical States of Matter Intermolecular forces Chapter 5 Physical States of Matter Section 12.3 Physical States of Matter Three phases of matter solid Definite shape and volume solid liquid liquid Definite volume, shape of container

More information

Chapter 8 H H H H. Molecular Compounds & Covalent Bonding. Why do covalent bonds form? 8.1 Molecular Compounds. Properties of Molecular Compounds

Chapter 8 H H H H. Molecular Compounds & Covalent Bonding. Why do covalent bonds form? 8.1 Molecular Compounds. Properties of Molecular Compounds Chapter 8 Molecular Compounds & Covalent Bonding Why do covalent bonds form? If only group 5A, 6A, 7A atoms existed, ionic bonds can t form. NNMETALS Each atom needs electrons so they are not willing to

More information

GRIGNARD REACTION Synthesis of Benzoic Acid

GRIGNARD REACTION Synthesis of Benzoic Acid 1 GRIGNARD REACTION Synthesis of Benzoic Acid In the 1920 s, the first survey of the acceleration of chemical transformations by ultrasound was published. Since then, many more applications of ultrasound

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

CS 2, HCN, BeF 2 Trigonal planar. Cl 120 BF 3, AlCl 3, SO 3, NO 3-, CO NCl 3,PF 3,ClO 3,H 3 O + ...

CS 2, HCN, BeF 2 Trigonal planar. Cl 120 BF 3, AlCl 3, SO 3, NO 3-, CO NCl 3,PF 3,ClO 3,H 3 O + ... Shape of molecules Name No bonding pairs No lone pairs Diagram Bond angle Examples linear 2 0 l Be l 180 2, S 2, N, Be 2 Trigonal planar 3 0 l l 120 B 3, All 3, S 3, N 3-, 2-3 B Tetrahedral 4 0 109.5 Sil

More information

MIXTURES, COMPOUNDS, & SOLUTIONS

MIXTURES, COMPOUNDS, & SOLUTIONS MIXTURES, COMPOUNDS, & SOLUTIONS As with elements, few compounds are found pure in nature and usually found as mixtures with other compounds. A mixture is a combination of two or more substances that are

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

States of Matter. We can explain the properties that we observe in the various states of matter with these postulates.

States of Matter. We can explain the properties that we observe in the various states of matter with these postulates. States of Matter Kinetic Molecular Theory When discussing the properties of matter, it is not enough just to classify them. We must also create a model that helps to explain the properties that we see.

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

Ask the Professor. Michael Patrick, Ph.D. University of Wisconsin - Madison. Mary Gruhl, Ph.D. University of Wisconsin - Milwaukee

Ask the Professor. Michael Patrick, Ph.D. University of Wisconsin - Madison. Mary Gruhl, Ph.D. University of Wisconsin - Milwaukee Ask the Professor If you have questions about water or other molecules, be sure to contact us through our Ask the Professor link on the Water Resource pages of the 3D Molecular Designs website 3dmoleculardesigns.com.

More information

Chapter #16 Liquids and Solids

Chapter #16 Liquids and Solids Chapter #16 Liquids and Solids 16.1 Intermolecular Forces 16.2 The Liquid State 16.3 An Introduction to Structures and Types of Solids 16.4 Structure and Bonding of Metals 16.5 Carbon and Silicon: Network

More information

Experiment 7 Aldehydes, Ketones, and Carboxylic Acids

Experiment 7 Aldehydes, Ketones, and Carboxylic Acids Experiment 7 Aldehydes, Ketones, and arboxylic Acids Aldehydes and ketones are molecules that contain a carbonyl group, which is an oxygen atom with a double bond to a carbon atom. In an aldehyde, the

More information

2. What is meant by Chemical State?. 3. Changing states of matter is about changing,,, and other.

2. What is meant by Chemical State?. 3. Changing states of matter is about changing,,, and other. Name: Date: Period: Matter Mania! Online Computer Activity (3 pages) Part I: Go to http://www.chem4kids.com/ and answer the following questions in complete sentences. a. Click on MATTER (written in yellow)

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

Chemistry A: States of Matter Packet Name: Hour: Page!1. Chemistry A States of Matter Packet

Chemistry A: States of Matter Packet Name: Hour: Page!1. Chemistry A States of Matter Packet Chemistry A: States of Matter Packet Name: Hour: Page!1 Chemistry A States of Matter Packet Chemistry A: States of Matter Packet Name: Hour: Page!2 Worksheet #1: States of Matter In this packet we will

More information

Molecular Modeling and Conformational Analysis with PC Spartan

Molecular Modeling and Conformational Analysis with PC Spartan Molecular Modeling and Conformational Analysis with PC Spartan Introduction Molecular modeling can be done in a variety of ways, from using simple hand-held models to doing sophisticated calculations on

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

Chapter 5, Lesson 1: Water is a Polar Molecule

Chapter 5, Lesson 1: Water is a Polar Molecule Chapter 5, Lesson 1: Water is a Polar Molecule Key Concepts The water molecule, as a whole, has 10 protons and 10 electrons, so it is neutral. In a water molecule, the oxygen atom and hydrogen atoms share

More information

Lab 3: Solubility of Organic Compounds

Lab 3: Solubility of Organic Compounds Lab 3: Solubility of rganic Compounds bjectives: - Understanding the relative solubility of organic compounds in various solvents. - Exploration of the effect of polar groups on a nonpolar hydrocarbon

More information

Chapter 15 Gases, Liquids, and Solids

Chapter 15 Gases, Liquids, and Solids Free Study Guide for Cracolice Peters Introductory Chemistry: An Active Learning Approach Second Edition www.brookscole.com/chemistry Chapter 15 Gases, Liquids, and Solids Chapter 15 Assignment A: Forces

More information

Evaporation Rates of Liquids. Sarah Byce

Evaporation Rates of Liquids. Sarah Byce Evaporation Rates of Liquids Sarah Byce Herrington CHM 201-10 8 October 2012 Byce 2 Statement of Question How do evaporation rates relate to molecular structure? Based on the information given (Appendix:

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

Unit 4:Chemical Bonding Practice Packet

Unit 4:Chemical Bonding Practice Packet Name: KEY Unit 4:Chemical Bonding Practice Packet 1. I can state the three types of chemical bonds. 2. I can state the number of valence electrons that an atom attains to be most stable. 3. I can state

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

POGIL: Intermolecular Forces and Boiling Points

POGIL: Intermolecular Forces and Boiling Points Name Date Block POGIL: Intermolecular Forces and Boiling Points Model 1: Intermolecular Forces in Liquids and Gases Molecules attract each other, and the intermolecular force increases rapidly as the distance

More information

States of Matter. Intermolecular Forces. The States of Matter. Intermolecular Forces. Intermolecular Forces

States of Matter. Intermolecular Forces. The States of Matter. Intermolecular Forces. Intermolecular Forces Intermolecular Forces Have studied INTRAmolecular forces the forces holding atoms together to form compounds. Now turn to forces between molecules INTERmolecular forces. Forces between molecules, between

More information

Substances and Mixtures:Separating a Mixture into Its Components

Substances and Mixtures:Separating a Mixture into Its Components MiraCosta College Introductory Chemistry Laboratory Substances and Mixtures:Separating a Mixture into Its Components EXPERIMENTAL TASK To separate a mixture of calcium carbonate, iron and sodium chloride

More information

Polarity. Q

Polarity.  Q Unit 6 Polarity Polarity Reflect: Hydrogen has a very low affinity for electrons, while oxygen has a very high affinity. What do you think the bond between the two is like? Polarity http://www.youtube.com/watch?v=kj3o0xvhvq

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

CHM 130LL: Molecular Models

CHM 130LL: Molecular Models CM 130LL: Molecular Models In this lab, you will study covalently bonded molecules i.e., molecules where nonmetal atoms are held together because they share one or more pairs of electrons. In this experiment,

More information

Evaluation copy. The Molar Mass of a Volatile Liquid. computer OBJECTIVES MATERIALS

Evaluation copy. The Molar Mass of a Volatile Liquid. computer OBJECTIVES MATERIALS The Molar Mass of a Volatile Liquid Computer 3 One of the properties that helps characterize a substance is its molar mass. If the substance in question is a volatile liquid, a common method to determine

More information

Intermolecular Forces and Physical Properties

Intermolecular Forces and Physical Properties Intermolecular Forces and Physical Properties Attractive Forces Particles are attracted to each other by electrostatic forces. The strength of the attractive forces depends on the kind(s) of particles.

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 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

Chemistry A: States of Matter Packet Name: Hour: Page 1. Chemistry A States of Matter Packet

Chemistry A: States of Matter Packet Name: Hour: Page 1. Chemistry A States of Matter Packet Chemistry A: States of Matter Packet Name: Hour: Page 1 Chemistry A States of Matter Packet Chemistry A: States of Matter Packet Name: Hour: Page 2 Worksheet #1: States of Matter In this packet we will

More information

Experiment 6 Alcohols and Phenols

Experiment 6 Alcohols and Phenols Experiment 6 Alcohols and Phenols Alcohols are organic molecules that contain a hydroxyl (-) group. Phenols are molecules that contain an group that is directly attached to a benzene ring. Alcohols can

More information

Salt vs. Sugar. 1. Ionic Compounds. 2. Molecular Compounds (Cont.) 12/18/2014. What is this Compound You Speak Of? Sodium Chloride Dissolving in Water

Salt vs. Sugar. 1. Ionic Compounds. 2. Molecular Compounds (Cont.) 12/18/2014. What is this Compound You Speak Of? Sodium Chloride Dissolving in Water Salt vs. Sugar Unit 7: Chemical Compounds & Formulas Lesson#7.1: Types of Compounds What is this Compound You Speak Of? Compound: Any substance that is formed by the chemical bonding of atoms. We classify

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

Liquids and Solids. H fus (Heat of fusion) H vap (Heat of vaporization) H sub (Heat of sublimation)

Liquids and Solids. H fus (Heat of fusion) H vap (Heat of vaporization) H sub (Heat of sublimation) Liquids and Solids Phase Transitions All elements and compounds undergo some sort of phase transition as their temperature is increase from 0 K. The points at which these phase transitions occur depend

More information

When intermolecular forces are strong, the atoms, molecules, or ions are strongly attracted to each other, and draw closer together.

When intermolecular forces are strong, the atoms, molecules, or ions are strongly attracted to each other, and draw closer together. INTERMOLECULAR FORCES: THE FORCE BEHIND VARIOUS PROPERTIES WHY? Intermolecular forces are largely responsible for the properties of affinity, solubility, volatility, melting/ boiling point, and viscosity.

More information

Intermolecular forces

Intermolecular forces Intermolecular forces World of Chemistry, 2000 Updated: August 29, 2013 The attractions of molecules to each other are known as intermolecular forces to distinguish them from intramolecular forces, such

More information

R R CH. Some reactions of alcohols vary depending on their classification as 1º, 2º, or 3º alcohols.

R R CH. Some reactions of alcohols vary depending on their classification as 1º, 2º, or 3º alcohols. Experiment: Alcohol Reactions Alcohols are important organic molecules characterized by an alkyl group covalently bonded to a hydroxyl group. They may be classified as primary, secondary, or tertiary,

More information

INTERMEDIATE BONDING AND INTERMOLECULAR FORCES. Electronegativity

INTERMEDIATE BONDING AND INTERMOLECULAR FORCES. Electronegativity INTERMEDIATE BNDING AND INTERMLECULAR FRCES Electronegativity is defined as follows Electronegativity Electronegativity is the ability of an atom within a covalent bond to attract the bonding pair of electrons.

More information

Determination of the Equivalent Weight and the K a or K b for a Weak Acid or Base

Determination of the Equivalent Weight and the K a or K b for a Weak Acid or Base INTRODUCTION Determination of the Equivalent Weight and the K a or K b for a Weak Acid or Base Chemists frequently make use of the equivalent weight (eq. wt.) as the basis for volumetric calculations.

More information

Liquids and Intermolecular Forces. Course Learning Outcomes for Unit I. Reading Assignment. Unit Lesson UNIT I STUDY GUIDE

Liquids and Intermolecular Forces. Course Learning Outcomes for Unit I. Reading Assignment. Unit Lesson UNIT I STUDY GUIDE UNIT I STUDY GUIDE Liquids and Intermolecular Forces Course Learning Outcomes for Unit I Upon completion of this unit, students should be able to: 1. Identify the intermolecular attractive interactions

More information

Q. What happens when you boil (melt) a compound?

Q. What happens when you boil (melt) a compound? Intermolecular Forces (MHR Text p. 202 206) Molecular compounds are: 1) made up of molecules 2) are made up of two or more nonmetallic atoms 3) held together by covalent bonds (sharing e ) Q. But what

More information