2. If you have two beakers of liquid, one containing hexane and one containing water, you...
2. If you have two beakers of liquid, one containing hexane and one containing water, you will notice that one has a smell and the other does not. Explain which one you can smell (using the wafting technique) and why you can smell that one liquid over the other. Discuss the interparticle forces. Use complete sentences. Do not use any abbreviations.
3. For the following pairs, predict which compound would have the higher melting point and explain why by discussing the important types of interparticle forces in each compound. Use complete sentences. Do not use any abbreviations.
a. KI or H2O
b. CCl4 or CH4
4. Both carbon dioxide and diamond contain carbon atoms and also have covalent bonds. Explain why carbon dioxide is a gas at room temperature while diamond is a solid even though they both have covalent bonds. Use complete sentences. Do not use any abbreviations.
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2. If you have two beakers of liquid, one containing hexane and
one containing water, you...
You have two beakers containing acids. Beaker A contains a 0.100 M solution with a pH...
You have two beakers containing acids. Beaker A contains a 0.100 M solution with a pH of 4.5 and beaker B contains a 0.100 M solution with a pH of 3.5. Which acid has the larger equilibrium constant? Why does this have an effect on pH? Explain your answer.
You are performing a simple distillation of roughly 50:50 liquid solution containing two components, hexane and...
You are performing a simple distillation of roughly 50:50 liquid solution containing two components, hexane and nonane You place 15 ml of the mixture in a round bottom flask, and then collect the distillate sequentially as four three ml samples labeled S1, S2, S3, and S4. Pure hexane has a refractive index of 1.375 and pure nonane has a refractive index of 1.407. You measure a refractive index of 1.3964 for one of the four samples. Assuming the refractive index...
Which compound/s (water, acetone, ethanol, hexane, decane, 1-decanol, sodium chloride, and/or iodine) do you think will...
Which compound/s (water, acetone, ethanol, hexane, decane, 1-decanol, sodium chloride, and/or iodine) do you think will be soluble in hexane and explain why. You must discuss intermolecular forces in your explanation.
Which compound (water, acetone, ethanol, hexane, decane, or 1-decanol) do you think will be the least...
Which compound (water, acetone, ethanol, hexane, decane, or 1-decanol) do you think will be the least volatile and explain why. You must discuss intermolecular forces in your explanation.
Chemistry 2 help with lab questions! Intermolecular forces are not chemical bonds. Explain the difference. When...
Chemistry 2 help with lab questions! Intermolecular forces are not chemical bonds. Explain the difference. When answering the rest of the essay questions, use language that clearly distinguishes between chemical bonds and intermolecular forces. Why do compounds with higher intermolecular forces have higher boiling points? Show that you understand why a higher temperature is needed to boil a compound that has stronger intermolecular forces. Which has greater dispersion forces, hexane or pentane? How can you use their molecular formulas to...
PART IV. MISCIBILITY OF TWO LIQUIDS 1. For the first two liquids in Table IV-B (the...
PART IV. MISCIBILITY OF TWO LIQUIDS
1. For the first two liquids in Table IV-B (the solvents in the
miscibility tests), use the molecular structures provided in the
Introduction to identify each liquid as polar or nonpolar. Put an X
in the appropriate column.
2. For the remaining liquids in Table IV-B, determine if they
are primarily polar, primarily nonpolar, or both polar and polar
based on your observations in Table III-A and based on the polarity
of the solvent....
2. Identify the strongest type of intermolecular forces in acetone, ethanol, water and hexane. (Structures listed...
2. Identify the strongest type of intermolecular forces in acetone, ethanol, water and hexane. (Structures listed on page 15.) Experiment 2 Intermolecular Forces There are three general types of intermolecular forces. All substances exhibit London Dispersion Forces (LDF), and they are generally the weakest of the three types. These London forces are due to the attractions between small, temporary dipoles that arise from the constant, random movement of the electrons in a substance. As molar mass increases, the size of...
3. (2 points) Both glucose and water have hydrogen bonds, yet glucose is a solid at...
3. (2 points) Both glucose and water have hydrogen bonds, yet glucose is a solid at room temperature, and water is a liquid. On your work sheet provide, in your own words, a likely explanation for why that is true. Use complete sentences. Glucose is the major free sugar circulating in our blood. It is the source of energy in cell function and is the sugar that is related to diabetes. Its chemical formula is CH,,Oand its structure is shown...
1) Define Lewis structures (2) and present two examples (4 pts) for representations of two compounds...
1) Define Lewis structures (2) and present two examples (4 pts) for representations of two compounds or species where one has 4 carbon and a nitrogen and the other has 4 carbon, a chlorine and an oxygen with two pairs shared with one of the carbons. Complete the structure with the H that is required. 2) Define the electronic pair repulsion model (VSEPR) and apply it to an organic compound of 4 or more carbons that have a double or...
Two beakers of clear colorless liquids sit in front of you on a lab bench. One...
Two beakers of clear colorless liquids sit in front of you on a lab bench. One beaker contains 50 mL of aqueous 0.1 M HBr (hydrobromic acid): HBr (aq) + H20 (1) → H30+ + Br (aq) (aq) and the other beaker contains 50 mL of aqueous 0.1 M HNO2 (nitrous acid): HNO2 (aq) + H2O() H3O+ (aq) + NO2- (aq) Answer the following: 1. Do these two solutions dissociate to produce the same amount of [H*]? 2. Do these...
PART IV. MISCIBILITY OF TWO LIQUIDS
1. For the first two liquids in Table IV-B (the solvents in the
miscibility tests), use the molecular structures provided in the
Introduction to identify each liquid as polar or nonpolar. Put an X
in the appropriate column.
2. For the remaining liquids in Table IV-B, determine if they
are primarily polar, primarily nonpolar, or both polar and polar
based on your observations in Table III-A and based on the polarity
of the solvent....
2. Identify the strongest type of intermolecular forces in acetone, ethanol, water and hexane. (Structures listed on page 15.) Experiment 2 Intermolecular Forces There are three general types of intermolecular forces. All substances exhibit London Dispersion Forces (LDF), and they are generally the weakest of the three types. These London forces are due to the attractions between small, temporary dipoles that arise from the constant, random movement of the electrons in a substance. As molar mass increases, the size of...
3. (2 points) Both glucose and water have hydrogen bonds, yet glucose is a solid at room temperature, and water is a liquid. On your work sheet provide, in your own words, a likely explanation for why that is true. Use complete sentences. Glucose is the major free sugar circulating in our blood. It is the source of energy in cell function and is the sugar that is related to diabetes. Its chemical formula is CH,,Oand its structure is shown...
Two beakers of clear colorless liquids sit in front of you on a lab bench. One beaker contains 50 mL of aqueous 0.1 M HBr (hydrobromic acid): HBr (aq) + H20 (1) → H30+ + Br (aq) (aq) and the other beaker contains 50 mL of aqueous 0.1 M HNO2 (nitrous acid): HNO2 (aq) + H2O() H3O+ (aq) + NO2- (aq) Answer the following: 1. Do these two solutions dissociate to produce the same amount of [H*]? 2. Do these...
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