ࡱ>  JLINN'. (bjbjWW == ++{{{4tg"47^!!!!!!!$#=&R "{v" "++!"PPP+8{!P!PP:,c #d& !7"0g"0R&&&{ P " "ng"& : 1 List the intermolecular and intramolecular forces. Why is the term intramolecular sometimes a misnomer? 2 Identify intramolecular and intermolecular forces for each of the following. Predict the order in which they would melt. GeH4 SiH4 SnH4 CH43 A. Identify intramolecular and intermolecular forces for each of the following. The electronegativities of Se, S, and Te are all within 0.5 of each other which is quite small. Predict the order in which they would melt. When these substances melt, are intermolecular or intramolecular forces being broken? H2Te H2S H2O H2Se B. If a mixture contained all four of these substances in the liquid phase, which would be the first to distill? Which would be the last? How does this list compare with your list in part A? Why?4 Does the following diagram best describe a crystalline solid, liquid, or gas? Explain.  EMBED PBrush 5 The following are in order; do they go in order of increasing or decreasing melting points? Use intramolecular and intermolecular forces to thoroughly justify the order. C, BaCl2, HF, CO, Ne, H2 What type of solid would each substance form? Are any solid types not represented? If so, list them and give an example.6 In the Lewis structure shown below, A, D, E, Q, X, and Z represent elements in the first two periods of the periodic table. Identify all six elements and explain how you determined the identity.  EMBED PBrush 7 Which of the following molecules can form hydrogen bonds with other molecules of the same kind? Draw two molecules for each selection and indicate Hydrogen bonding. Circle covalently-bonded hydrogens that cannot H-bond. CH3F CH3NH2 CH3OH CH3Br8 As the intermolecular attractive forces between molecules increase in magnitude, do you expect each of the following to increase or decrease in magnitude? *boiling point, freezing point, viscosity, surface tension, adhesion, cohesion, capillary action, vapor pressure9 What kinds of attractive forces exist between particles in molecular solids, network solids, ionic solids, and metallic solids (discuss electrons)? A white substance melts with some decomposition at 730C. As a solid, it is a nonconductor of electricity, but it dissolves in water to form a conducting solution. Which type of solid might the substance be? How do you know?10 The state of aggregation of solids can be described as belonging to the following four types: (1) ionic (3) network (2) metallic (4) molecular For each of these types of solids, sketch a diagram of the solid and indicate the kinds of particles that occupy the lattice points and identify forces among these particles. How could each type of solid be identified in the laboratory?11 Identify the type of solid the representation below depicts. List all the properties of this solid type that you know. Use features of the diagram to explain why this solid has two properties you listed.  INCLUDEPICTURE "http://www.kentchemistry.com/images/links/bonding/Metalbond5.gif" \* MERGEFORMATINET 12 The diagram uses a polar stationary phase and a nonpolar mobile phase. Given the following solutions, identify which would be A and which would be B. Br2____&NH3_____ CH3Cl___&CH4____ ethane_____ðanol_____ Calculate the Rf values for A and B.13 Lab equipment: beaker, scale, graduated cylinder, weigh boat, volumetric flasks (100mL and 500mL), water, solid NaCl, Erlenmeyer flask A. The equipment above is available to you. Thoroughly explain how to make 100 mL of a 2.5M solution of NaCl. Show any calculations needed. B. Explain how to dilute the solution made in part A into 500mL of 1.0M NaCl solution. Show any calculations needed.14 For practice: For the following: draw the lewis structure (with formal charges), name the shape according to modern bonding theory, identify angles, and indicate polarity and hybridization. Explain similarities and differences. phosphite and phosphate Answers: 1. inter=London dispersion, dipole-dipole, hydrogen bond; intra=covalent, metallic, ionic; intramolecular is a misnomer because only the individual particles of covalent substances are called molecules (formula unit is used for ionic and metallic has no name for individual parts)2. lowest: CH4, SiH4, GeH4,SnH4 (if you assume that the first three are covalent and have only LDF, they increase in molecular weight and therefore increase strength of LDF; the last one is ionic) 3. This one is tricky ;) You need to know that the electronegativities of S, Se, and Te are pretty close to each other. A. lowest: H2S, H2Se, H2Te, H2O (the first three are all dipole-dipole and LDF, but their closeness in electronegativity means that the increasing molar mass makes the larger ones have a higher LDF forces and a higher meting point; H-bonding in water makes it highest), intermolecular forces are being broken when these substances melt. B. H2S would distill first; water would distill last; the order is the same because the forces that hold these in the solid state are the same forces holding them in the liquid state.4. liquid: , no repeating structure like a crystalline solid, not spaced out enough to be a gas (although you could make an argument for gas, liquid is still the best answer) 5. they decrease; lowest: H2, Ne, CO, HF, BaCl2, C (LDF, stronger LDF because it has more electrons, dipole-dipole, H-bond, ionic, network; metallic is missing: Cu, Zn, are examples) ( if two things have the same forces, you must explain why they are different to get full credit6. A is fluorine, D is carbon, E is oxygen, Q is nitrogen, Z/X are hydrogen 7. CH3NH2 and CH3OH can do H-bonding because they have hydrogen attached to N/O/F (see below). Although CH3F has hydrogen and fluorine, they are not attached to each other. CH3Br doesnt have NOF, so it cannot do hydrogen bonding.  8. Everything increases except vapor pressure (which decreases) 9. Molecular (intermolecular), network (covalent, electrons are being shared), ionic (intramolecular electrostatic attractions, electrons are trapped onto ions), metallic (nondirectional covalent, intramolecular, sea of electrons); the unknown is most likely an ionic solid10. USE YOUR FOLDABLE TO CHECK YOUR DRAWINGS. Lattice points are occupied by: -Molecular (covalent compounds or nonmetal atoms) -network (carbon, silicon, or SiC or SiO2) -metallic (the core electrons and nuclei of metal atoms, valence electrons have been removed) -ionic (ions) USE YOUR FOLDABLE TO CHECK YOUR ANSWER TO HOW THESE SUBSTANCES COULD BE IDENTIFIED IN THE LAB.11. The solid is a metal. Metals have low vapor pressures, conduct heat and electricity, and mare malleable/ductile. Good conductor of heat/electricity-The valence electrons are delocalized and relatively free to move Malleable/Ductile-Deforming the solid doesnt change the environment immediately surrounding each metal core 12. Since the mobile phase is nonpolar, nonpolar molecules should travel with the nonpolar solute (where they are more soluble/attracted to) rather than sticking to the polar stationary phase. Br2_A__&NH3_B___ CH3Cl_B_&CH4_A__ ethane__A__ðanol__B__ Rf values:  EMBED PBrush 13. A. First calculate the mass of NaCl needed:  EMBED PBrush  Then, measure 14.61 grams of NaCl using a weigh boat and a scale. Then, place this in a 100mL volumetric flask and fill partially with distilled water. Wait for the solid to completely dissolve. Add water until the bottom of the meniscus meets the line on the neck of the volumetric flask. Stir to combine. B Calculate the volume of the 2.5 Molar solution needed. M1V1=M2V2 (2.5 M) V1 = (1.0 M)(500mL) (if V2 is in mL, V1 will also be; liters could be used as well) V1 = 200 mL Measure 200mL of the 2.5 M NaCl stock solution. Place this in a volumetric flask. Fill partially with distilled water. Stir. Add water until the bottom of the meniscus meets the line on the neck of the volumetric flask. Stir to combine. 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