CHAPTER 3 HW SOLUTIONS: INTERMOLECULAR FORCES
|
|
- Myron Douglas
- 6 years ago
- Views:
Transcription
1 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 each transition state with an asterisk (*). c. Label each intermediate with an I. Rxn coordinate d. Label the activation barrier for each step with a double-headed arrow. 2. The energy diagrams of two reactions are plotted side by side below. a. Which reaction is more exothermic? B (more downhill) b. Assuming equal concentration of reactants and equal temperatures, which reaction would proceed faster? Δ Rxn A Rxn B A (lower activation barrier) Rxn coordinate BND DISSIATIN ENERGIES 3. Given that the bond dissociation energy (BDE) of -F in 3 F is 109 kcal/mol and the BDE of -I in 3 I is 56 kcal/mol, which bond is stronger, -F or -I? Briefly explain. BDE refers to the amount of energy needed to break a bond in half, into radicals. The higher the BDE, the more energy it takes to break the bond. Therefore, -F is a stronger bond, since its BDE is higher. Page 1
2 4. onsult a table of bond dissociation energies, and use them to determine the D for each reaction. Also state whether each reaction is favorable or not (in terms of D ). a. 4 + I 2 à 3 I + I D = [ I-I ] [ I + -I] = [ 4(104) + 36 ] [ 3(104) ] = [ 452 ] [ 439 ] = +13 kcal/mol Unfavorable (positive D and reactant bonds are stronger) + I I I + I b. 2 = 2 + F à 3 2 F + F F D = [ = + F ] [ F] = [ 4(98) ] [ 5(98) ] = [ 680 ] [ 685 ] = -5 kcal/mol Note: these 4 - are the ones listed as 2 =- Somewhat favorable (negative D and product bonds are stronger) c /2 = à 2 == /2 + D = [ /2 = ] [ 4 = ] = [ 6(98) /2(119) ] [ 4(192) + 6(119) ] = = [ ] [ 1482 ] = kcal/mol Very favorable (very negative D and product bonds are stronger) d. Match the previous reactions to each energy diagram below, considering the calculated D and their relative magnitude. Note: energy diagrams are not perfectly to scale, choose the closest option. b c a Page 2
3 FUNTINAL GRUPS 1. Identify the main functional group in each compound below. Structure N 3 3 Funct Gp Aromatic Alkene Alkane Ketone Amide Ester Structure N Funct Gp Ether Alkyne Alcohol Amine Aldehyde arboxylic acid 2. Identify the functional groups in each compound. alkane aromatic ester 3 3 amine N 3 3 ether amide N carboxylic acid aromatic aromatic N amine Ibuprofen (analgesic) Darvon (analgesic) Melatonin (hormone thought to induce sleep) alkene alkyne N amine alkene alcohol alkyne alkene ester three more alkenes ketone istrionicotoxin (poison secreted by S. American frog) Pyrethrin I (potent insecticide from chrysanthemums) Page 3
4 INTERMLEULAR FRES 3. Multiple choice: The electrons pointed to in this water molecule are part of a: a. ovalent bond. b. ydrogen bond. c. Dipole-dipole force. d. Both b+c. 4. Identify the type of intermolecular force (London dispersion force, weak/strong dipole-dipole force, or hydrogen bond) pointed to in each interaction. l l dipole-dipole force (hard to say weak/strong) LDF strong dipole-dipole force hydrogen bond 5. For the substances below, Structure Br N 3 Draw and label the IMF δ+ δ Br Br dipole-dipole force (hard to say weak/strong) δ+ δ δ+ δ+ δ N δ+ hydrogen bond δ N Place d +, d - labels on the appropriate atoms in any polar bonds. Draw two of the same molecules interacting (using dashed lines), to show how the molecules orient relative to one another in the liquid form. Point to and identify the type of intermolecular force present. 6. Describe how a London dispersion force (LDF) arises, and where the force of attraction comes from. An atom s electron cloud is often evenly distributed, but because electrons move, they can at times be lopsided. When lopsided, there is a buildup of electrons on one side, which is a partial negative area (d - ). The other side is a partial positive area (d +). This is a temporary dipole. The temporary dipole causes nearby electron clouds in other molecules to polarize (create temporary d -, d + areas), and the attraction between the temporary dipoles in different molecules is a LDF. Page 4
5 7. Draw a molecular picture of the substances below, showing how the molecules orient relative to one another in the pure liquid form. Draw at least two molecules interacting and use dashed lines to show the strongest type of intermolecular forces (IMF) in each. Structure l 3 N Draw the IMF δ+ δ l δ+ δ l 3 N N 3 Strongest type of IMF Dipole-dipole forces (weak) LDF ydrogen bond Structure Draw the IMF 3 3 δ δ+ δ+ δ δ+ δ δ+ δ 3 Strongest type of IMF Dipole-dipole forces (strong) ydrogen bonds Dipole-dipole forces (strong) Page 5
6 8. Explain why compound A experiences weak dipole-dipole forces in the pure liquid phase while compound B has stronger dipole-dipole forces in the pure liquid phase A Two reasons why B is strong and A is weak: B Trigonal planar geometry in B allows for close contact of the dipoles, and stronger interaction. A has tetrahedral geometry on the atoms that are involved in the dipole and doesn t allow for as close contact. The net dipole is greater in B. In A, the individual dipoles somewhat cancel each other out, leading to a smaller net dipole. In B there is one dipole with nothing counteracting it. 9. In each set, rank the compounds in order of increasing strength of intermolecular forces. Explain your ranking. a. 3 l middle strongest weakest 3 molecules can form -bonds in the pure liquid phase, which are strong. 3 l molecules have weak dipole-dipole forces in the pure liquid phase, which are stronger than the intermolecular forces of 3 3 (which has only weak London dispersion forces). All molecules are of similar size and have similar LDF s. b. 3 Br 3 l 3 I middle weakest strongest These compounds differ in the halogen, and halogen size/mass goes from smallest to biggest l < Br < I. The bigger the atom, the further the electrons are from the nucleus, causing the atom to be more polarizable and able to distort, thus creating stronger LDF s. With this logic, 3 I has the strongest LDF s (and strongest IMF s) of the series. c. strongest middle weakest The compounds are the same with respect to shape and molar mass, meaning they have equivalent LDF s. owever, the first two compound have additional forces, causing them to have stronger forces than the last compound. The first compound can also form -bonds (the strongest IMF), and the second compound can also form strong dipole-dipole forces (stronger than just LDF). Page 6
7 TRENDS IN BILING PINT 10. In each set, rank the compounds in order of increasing boiling point. Explain your ranking. a. I I 3 I middle highest lowest The only difference between these compounds is chain length and therefore size. The largest one (or one with highest mass) has the strongest LDF s, and so has the highest boiling point. This is because as the carbon chain increases there is increased surface area and more potential electron clouds to polarize and create LDF s. b. highest lowest middle These compounds have the same formula ( 7 16 ) and same mass, but differ in their shape caused by branching. Increased surface-to-surface contact between molecules increases the strength of LDF s and raises boiling points. The branched molecules have less surface area than the linear ones, so have weaker LDF s and a lower b.p. c. lowest highest middle f the two hydrocarbons, the first has the lower boiling point as it is more branched so has weaker LDF s. The alkene (far right structure) and ketone (middle structure) both have stronger LDF s with less branching. Their LDF s are roughly equivalent as they have nearly the same mass and surface area (5 ~ 4+). owever, the ketone has the highest boiling point as it also has strong dipole-dipole forces, which are a stronger IMF than only LDF. d. N 3 N 3 3 middle lowest highest The left two compounds have nearly the same mass (5 ~ 4+N) and the same shape, so have the same strength of LDF. The amine (far left) has a dipole, so can participate in weak dipole-dipole forces in the liquid phase, making it have a higher boiling point than the middle compound. The far right amine has the strongest IMF and highest boiling point due to two factors: it has an N bond so can form hydrogen bonds in the liquid phase, and also has a linear structure so has slightly stronger LDF than the other two compounds. Page 7
8 10 continued e. 3 middle highest lowest strong dip-dip hydrogen bonds weak dip-dip Each compound is the same mass and shape, so all 3 compounds have essentially equivalent LDF s. The trend in boiling point follows the strength of the other IMF s present; the stronger the IMF, the higher the boiling point. From weak to strong: weak dip-dip < strong dip-dip < hydrogen bonds. f. lowest middle highest The alcohol (right) forms strong hydrogen bonds in the liquid phase so has the highest b.p. The two ethers each have weak dipole-dipole forces in the liquid phase, so have a lower b.p. but the difference between them is in their branching (their masses are the same). The flatter, longer ether will have more surface contact, so stronger LDF s and a higher b.p. than the other ether. 11. Explain the following statements. a. Propane ( ) is a gas while pentane ( ) is a liquid at room temperature. Propane exists as a gas at room temperature because its boiling point is below room temp. Pentane has a higher boiling point (above room temperature) so exists as a liquid at room temperature. Pentane has a higher b.p. because it is a much longer compound than propane. This causes it to have stronger London dispersion forces (LDF s) due to its higher mass and greater surface area. b. ompound has a lower boiling point than compound D. D Both +D have similar LDF s in the liquid phase because they have the same mass and shape. ompound D has strong hydrogen bonds in the liquid phase, while compound has strong dipoledipole forces. (Remember that compound does NT hydrogen bond with the drawn because that is bound to a carbon and is a nonpolar region.) Since strong dip-dip are weaker than bonds, has a lower b.p. Page 8
9 11 continued c. ompound E has stronger London dispersion forces than compound F. 3 2 E F LDF s arise from the temporary polarization of electron clouds, and are correlated to mass and shape. ompound E has a higher mass than compound F (6 carbons > 2+) so has a greater electron cloud to potentially polarize, and has stronger LDF s. (Note compound F actually has a higher b.p. due to its strong bonding ability, but this is hard to predict when the LDF are inequivalent). d. ompound G has a higher boiling point than compound. G The only IMF s present in the liquid phase of either compound are LDF, since neither G nor is polar (they are hydrocarbons). They have approximately the same molecular formula (6), but G is linear while is branched. The flatter compound G has a greater surface area, and since LDF s increase with surface-to-surface contact, G has a higher b.p. The fact that G has an alkene makes little difference in this analysis. Page 9
10 WATER SLUBILITY 12. Draw each compound as it would exist in a dilute aqueous solution (assuming each dissolves). Label the intermolecular forces. Structure N 2 l Molecular Picture of Aqueous Solution N 2 δ+ δ l δ δ+ Type of IMF ydrogen bonds ydrogen bonds Wk. Dipole-dipole forces Structure l 3 l Molecular Picture of Aqueous Solution δ δ+ δ+ l δ l δ 3 Type of IMF ydrogen bonds Wk. Dipole-dipole forces ydrogen bonds 13. There are two main criteria necessary for a substance to be water soluble. List them below. ( Water soluble can be defined as when greater than 3g of solute dissolves in 100 ml of water.) The compound must be able to hydrogen bond with water. It must also have a small nonpolar region (have fewer than 5 carbon atoms, if there is one polar area). Page 10
11 14. In each set, rank the compounds in order of increasing water solubility. Explain your ranking. a. l middle least most soluble The ketone (right) can form -bonds to water (shown), making it the most water soluble. The other two cannot -bond with water, so are insoluble. The alkyl chloride is slightly more water soluble than the alkane because it has a weak dipole, allowing for a slightly stronger interaction with water than the LDF s experienced between the alkane and water. b. least most soluble middle All three compounds can -bond with water, but the diol (center) can -bond in two regions, so has the most favorable interactions with water and is the most water soluble (most polar). The alcohol (left) has a larger number of carbons than the ketone (right)- 7 versus 5- so the alcohol is less overall polar and less water soluble. c. most soluble middle least The alkene (right) can t -bond with water so is the least water soluble. Both the ether (left) and the alcohol (center) can form -bonds to water through their oxygen atoms, but the ether has fewer carbons so is more overall polar and more water soluble. 15. Predict whether each molecule should be water soluble or insoluble. l l l 3 N Insoluble Soluble Soluble Soluble 3 N 3 3 Insoluble Insoluble Page 11
12 16. T is the active ingredient in marijuana and ethanol is the alcohol in alcoholic beverages. Propose a brief explanation why drug screenings are able to detect the presence of T but not ethanol weeks after these substances have been introduced in the body Ethanol Ethanol is very water soluble (can -bond with water, and has <5, polar) so it is easily excreted by the body in urine. It is hard to detect it after a little while because it doesn t stay in the body long. 3 T has two spots of polarity, but many carbon atoms so is overall 3 T a nonpolar molecule. This causes it to be harder to excrete, and it stays in our fatty tissues longer. This allows for drug screening to detect T weeks after it has been used. 17. Explain the following statements in detail. a. Pentane is completely soluble in benzene. Pentane Benzene When these two substances are mixed, the LDF s the pentane molecules had with each other are replaced with LDF s between pentane and benzene. Since these LDF s have similar strength, there is negligible enthalpy change in the process. owever, there is an increase in entropy during dissolving, as there are more ways to arrange a solution than the pure solvents. D S dominates the D G equation, and the two substances mix because of the favorable change in entropy associated with mixing. b. Ethylene glycol is insoluble in hexane. Ethylene glycol strongly -bonds with itself, and when it theoretically dissolves in hexane, it is not favorable to Ethylene glycol exane replace its bonds with LDF interactions with the hexane. The glycol therefore maintains its -bonds, forming a very ordered, rigid cage around the hexane molecules, which is unfavorable with respect to entropy (it has restricted connections, or is an ordered system). The unfavorable D S prevents the two from mixing. c. Diethyl ether and 1-butanol have similar solubility properties in water, but 1-butanol has a much higher boiling point. Diethyl ether 1-Butanol Both compounds can form -bonds to water through their atoms (shown), and they are of similar size (4+) making their water solubility similar. Boiling point is determined by the strength of IMF s between molecules in the liquid phase: the alcohol can form -bonds between molecules of itself while the ether has weaker dipole-dipole attractions. There is almost no difference in the IMF with water so they have the same water solubility, but there is a big difference in the IMF with themselves, so their b.p. are different. Page 12
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 informationChap 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 information2.26 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 information2.26 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 informationIntermolecular 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 informationAlkanes, Alkenes and Alkynes
Alkanes, Alkenes and Alkynes Hydrocarbons Hydrocarbons generally fall into 2 general groupings, aliphatic hydrocarbons and aromatic hydrocarbons. Aliphatic hydrocarbons contain chains and rings of hydrocarbons,
More informationChapter 2 Structure and Properties of Organic Molecules. Advanced Bonding: Review
hapter 2 Structure and Properties of Organic Molecules hemistry 231 Organic hemistry I Fall 2007 Advanced Bonding: Review Atomic Quantum Mechanics cannot explain how molecules like 4 form: Valence Bond
More informationChapter 25: The Chemistry of Life: Organic and Biological Chemistry
Chemistry: The Central Science Chapter 25: The Chemistry of Life: Organic and Biological Chemistry The study of carbon compounds constitutes a separate branch of chemistry known as organic chemistry The
More information1. Which compound would you expect to have the lowest boiling point? A) NH 2 B) NH 2
MULTIPLE CICE QUESTINS Topic: Intermolecular forces 1. Which compound would you expect to have the lowest boiling point? A) N 2 B) N 2 C) N D) E) N Ans: : N 2 D Topic: Molecular geometry, dipole moment
More informationWave Properties of Electrons. Chapter 2 Structure and Properties of Organic Molecules. Wave Interactions. Sigma Bonding
rganic hemistry, 5 th Edition L. G. Wade, Jr. hapter 2 Structure and Properties of rganic Molecules Jo Blackburn Richland ollege, Dallas, TX Dallas ounty ommunity ollege District 2003, Prentice all Wave
More informationCS 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 informationClasses of Organic Compounds
Unit 1 Functional Groups Depicting Structures of rganic ompounds Lewis Structures ondensed structural formulas Line angle drawings 3-dimensional structures Resonance Structures Acid-Base Reactions urved
More informationLecture 2. The framework to build materials and understand properties
Lecture 2 The framework to build materials and understand properties 1 Trees are made into a solid materials/structures in an environment that consists of small molecules: CO 2, N 2, H 2 0, CH 4 O C 2.58Ǻ
More informationORGANIC - EGE 5E CH. 2 - COVALENT BONDING AND CHEMICAL REACTIVITY
!! www.clutchprep.com CONCEPT: HYBRID ORBITAL THEORY The Aufbau Principle states that electrons fill orbitals in order of increasing energy. If carbon has only two unfilled orbitals, why does it like to
More informationLearning Organic Chemistry
Objective 1 Represent organic molecules with chemical formulas, expanded formulas, Lewis structures, skeletal structures. Determine shape (VSEPR), bond polarity, and molecule polarity. Identify functional
More information2.2.2 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 informationChapter 12 Section 1
hapter 12 Section 1 Kinetic Molecular Description of Liquids and Solids Noncovalent Forces Intermolecular interactions Electrostatic Forces Dispersion Forces -bonding DNA, RNA Mary J. Bojan hem 110 1 What
More informationINTRODUCTION TO ORGANIC CHEMISTRY
INTRODUTION TO ORGANI EMISTRY GENERAL DESRIPTION OF ORGANI EMISTRY The Study of arbon ompounds GENERAL DESRIPTION OF ORGANI EMISTRY The Study of arbon ompounds Organic Man-made Substances Plant or Animal
More informationORGANIC MOLECULES (LIVE) 10 APRIL 2015 Section A: Summary Notes and Examples Naming and Functional Groups
ORGANIC MOLECULES (LIVE) 10 APRIL 2015 Section A: Summary Notes and Examples Naming and Functional Groups Important Features of Carbon There are different allotropes (same element, same phase, different
More informationCHAPTER 2. Structure and Reactivity: Acids and Bases, Polar and Nonpolar Molecules
CHAPTER 2 Structure and Reactivity: Acids and Bases, Polar and Nonpolar Molecules 2-1 Kinetics and Thermodynamics of Simple Chemical Processes Chemical thermodynamics: Is concerned with the extent that
More informationCHAPTER 6 ELECTRONEGATIVITY
EMISTRY 104 elp Sheet #1 hem 103 Review hapters 6 and 7 Do topics appropriate for your lecture Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets: Electronegativity (6.7),
More information[8.5] Melting Points and Boiling Points of Solutions
[8.5] Melting Points and Boiling Points of Solutions Melting and Boiling Points We have talked about melting and boiling points earlier in the semester Now we are going to understand how intermolecular
More informationCHEM 263 Oct 11, Lecture Outline 3: Alcohols, Ethers, Stereochemistry, Ketones, and Aldehydes. Ethanol
CEM 263 ct 11, 2016 Lecture utline 3: Alcohols, Ethers, Stereochemistry, Ketones, and Aldehydes Nomenclature of Alcohols Alcohols are compounds that have a hydroxyl group (-) bonded to a carbon atom (but
More informationCHEM 261 Dec 4, 2017
200 CEM 261 Dec 4, 2017 REVIEW: 1. N 3 2 S 4 1. 2 Al 3 N 2 2. 2 Al 3 2. N 3 2 S 4 N 2 I II For the left hand reaction, I - to create a meta positioned, the first molecule to be subsituted should be N 2,
More informationCHAPTER 2: Structure and Properties of Organic Molecules
1 HAPTER 2: Structure and Properties of Organic Molecules Atomic Orbitals A. What are atomic orbitals? Atomic orbitals are defined by special mathematical functions called wavefunctions-- (x, y, z). Wavefunction,
More informationPolar molecules vs. Nonpolar molecules A molecule with separate centers of positive and negative charge is a polar molecule.
CHM 123 Chapter 8 8.5 8.6 Polar covalent Bonds and Dipole moments Depending on the relative electronegativities of the two atoms sharing electrons, there may be partial transfer of electron density from
More informationWhy does more NaCl dissolve in 100 g of water than in 100 g of gasoline? Chapter 10
I sometimes wonder (because I m a nerd). Why does more NaCl dissolve in 100 g of water than in 100 g of gasoline? Chapter 10 Why does 2O have a higher boiling point than hexane (C3C2C2C2C2C3)? Liquids,
More informationCHAPTER 3: INTERMOLECULAR FORCES
CAPTE 3: ITEMLECULA FCES FUCTIAL GUPS DEFIITI Functional Groups are grouping of atoms with characteristic reactivity and properties. + Br Br + 2 Br + Br + 2 Page 1 GUPIGS ydrocarbons Carbonyl (C=) Containing
More informationCHEMISTRY 110 EXAM 2 Feb 25, 2013 FORM A
EMISTRY 110 EXAM 2 Feb 25, 2013 FORM A 1. ow many valence electrons and lone pairs are in the structure of the ammonium ion? # valence electrons # lone pairs A. 8 0 B. 10 1. 8 1 D. 10 2 E. 12 3 2. Which
More informationChapter 04 Alcohols and Alkyl Halides part 01
hapter 04 Alcohols and Alkyl alides part 01 EM 341: Spring 2012 Prof. Greg ook Functional Groups A functional group is a structural feature in a molecule that has characteristic reactivity. A functional
More informationOne 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 informationLecture 2. The framework to build materials and understand properties
Lecture 2 The framework to build materials and understand properties 1 Trees are made into a solid materials/structures in an environment that consists of small molecules: C 2, N 2, H 2 0, CH 4 C 2.58Ǻ?
More informationWhen 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 informationElectronegativity Scale F > O > Cl, N > Br > C, H
Organic Chem Chapter 12 Alkanes Organic chemistry is the study of carbon compounds. Carbon has several properties that are worth discussing: Tetravalent Always forms 4 bonds Can form multiple bonds (double
More informationIntermolecular 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 informationMolecular Geometry: VSEPR model stand for valence-shell electron-pair repulsion and predicts the 3D shape of molecules that are formed in bonding.
Molecular Geometry: VSEPR model stand for valence-shell electron-pair repulsion and predicts the 3D shape of molecules that are formed in bonding. Sigma and Pi Bonds: All single bonds are sigma(σ), that
More informationHISTORY OF ORGANIC CHEMISTRY
ISTORY OF ORGANI EMISTRY In the early days of chemistry, scientists classified chemical substances into 2 groups: 1. Inorganic: those that were composed of minerals, such as rocks and nonliving matter.
More informationLiquids, 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 informationDefinition: An Ionic bond is the electrostatic force of attraction between oppositely charged ions formed by electron transfer.
3 Bonding Definition An Ionic bond is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form +ve ions. on-metal atoms gain
More informationSolids, 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 informationIntermolecular 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 informationLecture 14: October 4, 2018
CM 223 Organic Chemistry I Prof. Chad Landrie C 3 Ea + O 3 C O 2 reactant intermediate Lecture 14: October 4, 2018 Ch. 6: Section 6.8: Bond Dissociation Energies and Reaction Enthalpy Ch. 17: Sections:
More informationObjectives. Organic molecules. Carbon. Hydrocarbon Properties. Organic Chemistry Introduction. Organic versus Hydrocarbon 1/1/17
Objectives Organic Chemistry Introduction 8.1 To determine the properties of organic molecules and recognize a hydrocarbon. Use table P and Q to write structural and molecular formulas for hydrocarbons.
More informationSUPPLEMENTAL HOMEWORK SOLUTIONS WEEK 10
SUPPLEMENTAL OMEWORK SOLUTIONS WEEK 10 Assignment for Tuesday, March 21 st 9.105 a) ombustion reactions require oxygen (in addition to the hydrocarbon). b) The products are O 2 and 2 O (carbon dioxide
More informationCalifornia State Polytechnic University, Pomona
alifornia State Polytechnic University, Pomona 2-1 Dr. Laurie S. Starkey, rganic hemistry M 314, Wade hapter 2: Structure and Physical Properties of rganic Molecules hapter utline 1) rbitals and Bonding
More informationLondon 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 informationQuick 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 informationChemistry: 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 informationIntermolecular 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 informationORGANIC - BRUICE 8E CH.3 - AN INTRODUCTION TO ORGANIC COMPOUNDS
!! www.clutchprep.com CONCEPT: INDEX OF HYDROGEN DEFICIENCY (STRUCTURAL) A saturated molecule is any molecule that has the maximum number of hydrogens possible for its chemical structure. The rule that
More informationChem 1075 Chapter 19 Organic Chemistry Lecture Outline
Chem 1075 Chapter 19 Organic Chemistry Lecture Outline Slide 2 Introduction Organic chemistry is the study of and its compounds. The major sources of carbon are the fossil fuels: petroleum, natural gas,
More informationChapter 1 Reactions of Organic Compounds. Reactions Involving Hydrocarbons
Chapter 1 Reactions of Organic Compounds Reactions Involving Hydrocarbons Reactions of Alkanes Single bonds (C-C) are strong and very hard to break, therefore these compounds are relatively unreactive
More informationOrganic Chemistry. Introduction to Organic Molecules and Functional Groups
For updated version, please click on http://ocw.ump.edu.my Organic Chemistry Introduction to Organic Molecules and Functional Groups by Dr. Seema Zareen & Dr. Izan Izwan Misnon Faculty Industrial Science
More informationNo Brain Too Small CHEMISTRY AS91390 Demonstrate understanding of thermochemical principles and the properties of particles and substances
COLLATED QUESTIONS Attractive forces between atoms, ions, and molecules. These will include ionic bonds, covalent bonds, and intermolecular attractions due to temporary dipoles and permanent dipoles (including
More informationOrganic and Biochemical Molecules. 1. Compounds composed of carbon and hydrogen are called hydrocarbons.
Organic and Biochemical Molecules 1. Compounds composed of carbon and hydrogen are called hydrocarbons. 2. A compound is said to be saturated if it contains only singly bonded carbons. Such hydrocarbons
More informationPOGIL: 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 informationThe 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 informationChapter 12. Intermolecular Forces: Liquids, Solids, and Phase Changes
Chapter 12 Intermolecular Forces: Liquids, Solids, and Phase Changes There are attractive intermolecular in all solids, liquids (called condensed phases) and gases. Molecules are held together by attractive
More informationChemistry 11 Spring 2013 Examination #3 ANSWER KEY
Chemistry 11 Spring 2013 Examination #3 ASWER KEY 1. (52 pts. total) seltamivir (sold under the trade name Tamiflu ) is a prescription antiviral drug that is used in the treatment of both Influenzavirus
More informatione.g. propan-2-ol ethane-1,1-diol propane-1,2,3-triol H H
Alcohols General The functional group is - The homologous series has general formula n 2n+1 The names end in ol, with a number if needed to indicate where on the carbon skeleton the group is located. When
More informationCarbon Compounds. Chemical Bonding Part 2
Carbon Compounds Chemical Bonding Part 2 Introduction to Functional Groups: Alkanes! Alkanes Compounds that contain only carbons and hydrogens, with no double or triple bonds.! Alkyl Groups A part of a
More informationAP Chemistry Chapter 22 - Organic and Biological Molecules
AP Chemistry Chapter - Organic and Biological Molecules.1 Alkanes: Saturated Hydrocarbons A. Straight-chain Hydrocarbons 1. Straight-chain alkanes have the formula C n H n+. Carbons are sp hybridized The
More informationINTERMEDIATE 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 informationTopic 5: Structure and Shape
Topic 5: Structure and Shape Lewis structures Lewis structures are a means of determining stable electron arrangements in molecules. It considers the valence electrons of an atom only. A stable arrangement
More informationFUNCTIONAL GROUPS Functional Group Suffix Formula Other Info O. Ester. Amide --- R C N R' or R(CO)NR R
EMISTRY 10 elp Sheet # rganic (Part III hapters.7 (condensed, structural drawings, 6.3 (line drawings, 6.9a (benzene, 7.e (hybrid orbitals in organic structures, and Appendix E (functional groups Do topics
More informationChapter 3: Structure and Nomenclature of Organic Compounds Focus on Alkanes
hapter 3: Structure and Nomenclature of rganic ompounds Focus on Alkanes rganic molecules are composed of one or more functional groups attached to one or more hydrocarbon groups (alkyl or groups) I. Functional
More informationPSI AP Chemistry Solutions Practice Problems
PSI AP Chemistry Solutions Practice Problems Name Solutions: Mixtures, Solubility and Concentration Classwork 1. A student determined that there were 0.032 grams of oxygen gas dissolved in a 200.0 ml sample
More informationForce Model Physical basis Energy (kj/ mole) Example
All course materials, including lectures, class notes, quizzes, exams, handouts, presentations, and other materials provided to students for this course are protected intellectual property. As such, the
More informationChapters 2 & 25: Covalent bonds & Organic Chemistry
hapters 2 & 25: ovalent bonds & Organic hemistry Read: BLB 2.6, 2.9; 25.1-25.4 (only nomenclature in Table 25.1, NOT reactions) W: BLB 2:43, 45, 69, 76, 77 BLB 25:11, 12, 25, 40a, c-f Packet Organic:1
More informationChapter #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 informationINTRODUCTION TO ORGANIC CHEMISTRY: ALKANES
P a g e 1 Chapter 12 INTRODUCTION TO ORGANIC CHEMISTRY: ALKANES Organic chemistry: The study of carbon compounds. Carbon is tetravalent; it always forms four bonds. Organic molecules have covalent bonds.
More informationIt is possible for organic molecules with the same molecular formula to have different structures
Isomerism It is possible for organic molecules with the same molecular formula to have different structures Definition- Structural isomers: same molecular formula different structures (or structural formulae)
More informationSolutions and Intermolecular Forces
Solutions and Intermolecular Forces REVIEW Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other
More informationP R A C T I C E T E S T
South Pasadena onors hemistry Name Semester 2 inal Exam Period Date The following information may be helpful. P R A T I E T E S T D = m K = + 273 V M = n V P 1 V 1 P2 V2 T = P V = n R T 1 T R = 0.0821
More informationCovalent Bonding. Chapter 8. Diatomic elements. Covalent bonding. Molecular compounds. 1 and 7
hapter 8 ovalent bonding ovalent Bonding A metal and a nonmetal transfer An ionic bond Two metals just mix and don t react An alloy What do two nonmetals do? Neither one will give away an electron So they
More information2FAMILIES OF CARBON COMPOUNDS:
P1: PBU/VY P2: PBU/VY Q: PBU/VY T1: PBU Printer: Bind Rite JWL338-02 JWL338-Solomons-v1 April 23, 2010 21:49 2AMILIES ARB MPUDS: UTIAL GRUPS, ITERMLEULAR RES, AD IRARED (IR) SPETRSPY SLUTIS T PRBLEMS 2.1
More informationChemistry 122 (Tyvoll) ANSWERS TO PRACTICE EXAMINATION I Fall 2005
hemistry 122 (Tyvoll) ANSWERS T PRATIE EXAMINATIN I Fall 2005 1. Which statement is not correct? 1) A volatile liquid has a high boiling point. 2. Which of the following compounds is predicted to have
More informationvideo 14.4 isomers isomers Isomers have the molecular formula but are rearranged in a structure with different properties. Example: Both C 4 H 10
video 14.4 isomers isomers Isomers have the molecular formula but are rearranged in a structure with different properties. Example: Both C 4 H 10 Butane Methylpropane 1 match the isomers drawing an isomer
More informationName: Date: Period: #: BONDING & INTERMOLECULAR FORCES
BONDING & INTERMOLECULAR FORCES Page 1 INTERMOLECULAR FORCES Intermolecular forces (van der Waals forces) relative weak interactions that occur between molecules. Most of the physical properties of gases,
More informationIntermolecular forces are classified into four major types.
Intermolecular forces are classified into four major types. 1. Ion-dipole: IMF s that occur between neighboring an ion solution and a polar molecule (dipole) also in solution. Na+ 2. Dipole-dipole: IMF
More informationSolids, 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 informationCHEMISTRY 110 EXAM 2 Oct. 11, 2010 FORM A
EMISTRY 110 EXAM 2 Oct. 11, 2010 FORM A --------------------------------------------------------------------------------- 1. What is the empirical formula that corresponds to a compound that contains only
More informationChapter 6 Intermolecular Forces: State Changes, Solubility, and Cell Membranes
Chapter 6 Lecture Chapter Outline General, Organic, and Biological Chemistry: An Integrated Approach Laura Frost, Todd Deal and Karen Timberlake by Richard Triplett Chapter 6 Intermolecular Forces: State
More informationWelcome to C341!! Chapter 1 & 2: Review of General Chemistry
Welcome to C341!! Chapter 1 & 2: Review of General Chemistry What will we do today? 1. Review of the syllabus together. 2. Discuss course structure and textbook. You will use the entire textbook between
More informationHigher Chemistry. Unit 1 Chemical Changes and Structure Summary Notes
Higher Chemistry Unit 1 Chemical Changes and Structure Summary Notes Success Criteria I am confident that I understand this and I can apply this to problems? I have some understanding but I need to revise
More informationPSI AP Chemistry: Solutions Practice Problems
PSI AP Chemistry: Solutions Practice Problems Name Solutions: Mixtures, Solubility and Concentration Classwork 1. A student determined that there were 0.032 grams of oxygen gas dissolved in a 200.0 ml
More informationMOLECULAR REPRESENTATIONS AND INFRARED SPECTROSCOPY
MOLEULAR REPRESENTATIONS AND INFRARED SPETROSOPY A STUDENT SOULD BE ABLE TO: 1. Given a Lewis (dash or dot), condensed, bond-line, or wedge formula of a compound draw the other representations. 2. Give
More informationGeneral Chemistry A
General Chemistry 1140 - A May 5, 2005 (6 Pages, 48 Questions) ame 1. Which of the following properties is a general characteristic of solids? (A) Solids have a rigid shape and fixed volume (B) Solids
More informationName Chemistry Pre-AP. Notes: Solutions
Name Chemistry Pre-AP Notes: Solutions Period I. Intermolecular Forces (IMFs) A. Attractions Between Molecules Attractions between molecules are called and are very important in determining the properties
More informationLecture 15. Polar vs Non-Polar Substances. Professor Hicks Inorganic Chemistry II (CHE151)
Lecture 15 Professor icks Inorganic hemistry II (E151) Polar vs on-polar Substances Ionic compounds Molecules with significant dipole moments (from polar bonds) Molecules with little or no dipole moment,
More informationCh. 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 informationCHAPTER 6 Intermolecular Forces Attractions between Particles
CHAPTER 6 Intermolecular Forces Attractions between Particles Scientists are interested in how matter behaves under unusual circumstances. For example, before the space station could be built, fundamental
More informationWeek 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 informationLecture Notes 1: Physical Equilibria Vapor Pressure
Lecture Notes 1: Physical Equilibria Vapor Pressure Our first exploration of equilibria will examine physical equilibria (no chemical changes) in which the only changes occurring are matter changes phases.
More informationDepartment of Chemistry University of Texas at Austin
Physical Equilibria Unit Activity Thinking Like a Chemist KEY A major goal for this class is for you to learn the concept of macro/micro thinking or Thinking Like a Chemist. Thinking like a chemist is
More informationDIPOLES IN CHEMICAL COMPOUNDS
hapter 2 Polar ovalent Bonds; Acids and Bases DIPLES IN EMIAL MPUNDS Ionic bonding between different elements and covalent bonding between atoms of the same element can be thought of as limits of electron
More informationSection 6.2A Intermolecular Attractions
Section 6.2A Intermolecular Attractions As we know, molecules are held together by covalent bonds, but there are also attractive forces BETWEEN individual molecules (rather than within). These are called
More informationExperiment 14. Intermolecular Forces rev 1/12
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,
More information2. Bonding Ionic Bonding
2. Bonding Ionic Bonding Metal atoms lose electrons to form +ve ions. on-metal atoms gain electrons to form -ve ions. Mg goes from 1s 2 2s 2 2p 6 3s 2 to Mg 2+ 1s 2 2s 2 2p 6 goes from 1s 2 2s 2 2p 4 to
More informationLab 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