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Alcohols have melting and boiling points higher than most other compounds of similar molar mass due...
The principal source of the difference in the normal boiling points of ICl (97 °C; molar...
The principal source of the difference in the normal boiling points of ICl (97 °C; molar mass 162 g/mol) and Br2 (59 °C; molar mass 160 g/mol) is dipole dipole interactions. London dispersion forces. hydrogen bonding. both hydrogen bonding and dipole - dipole interactions.
Arrange the compounds in order from highest to lowest boiling point.
Arrange the compounds in order from highest to lowest boiling point. Consider how noncovalent interactions would affect the boiling point rather than looking up actual boiling points. Highest boiling point Lowest boiling point Identify the three true statements. Stronger intermolecular forces usually correlate with higher boiling points. Boiling point generally increases with molecular weight due to increased strength of dispersion forces. Hydrocarbons exhibit only dispersion forces. Dipolo-dipole interactions are stronger than dispersion forces and hydrogen bonds. Hydrogen bonds require carbon, hydrogen, and a halogen.
The higher the molar mass, the higher which of these intermolecular forces? A. ion-dipole forces B....
The higher the molar mass, the higher which of these intermolecular forces? A. ion-dipole forces B. London dispersion forces C. dipole-dipole forces D. hydrogen bonding
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...
An ester has a higher boiling point than a carboxylic acid with similar molar mass. True...
An ester has a higher boiling point than a carboxylic acid with similar molar mass. True or False
Which two statements about propene and ethanol are true? Н Н Н, Н—С —С—ОН Н H...
Which two statements about propene and ethanol are true? Н Н Н, Н—С —С—ОН Н H Н Н ethanol propene Ethanol has a lower vapor pressure than propene at a given temperature. and ethanol have London forces and dipole-dipole forces. Both propene Propene has a higher boiling point than ethanol due to its double bond Ethanol forms hydrogen bonds, whereas propene has dipole-dipole interactions Of the two compounds, only ethanol forms hydrogen bonds. о
3. The compounds seen below have similar molar masses, but vary wildly in melting points. Rank...
3. The compounds seen below have similar molar masses, but vary wildly in melting points. Rank the molecules in increasing (low to high) melting point and explain your choices in terms of intermolecular forces. (4 points) OOH NH ного p-Xylene 1,4+dichloro benzene NH2 1,4-phenylene diamine Terephthalic Acid
18. A solid at -40C was heated uniformly until it changed into a gas. What is...
18. A solid at -40C was heated uniformly until it
changed into a gas. What is the melting point of the
?????
-20C
0C
20C
40C
19. In the temperature-time graph, the segment DE
represents the
Gas being warmed
Solid being warmed
Liquid being warmed
Liquid changing to gas
Solid changing to liquid
20. The principle difference in boiling points of ICl
(97C; mass 162 amu) and Br2 (59C; mass 160 amu) is due
to
London-dispersion forces
Dipole-dipole interactions
Hydrogen...
1. The melting points of most metals are higher than most plastics because: lonic bonds are...
1. The melting points of most metals are higher than most plastics because: lonic bonds are weaker than metallic bonds Van der Waals bonds are weaker than metallic bonds lonic and Van der Waals bonds are weaker than metallic bonds None of the above a. b. c. d. 2. A rubber band can stretch more than a metal paper clip because: Covalent bonds along polymer chains can stretch and rotate Covalent bonds along polymer chains can rotate and break Covalent...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding. The...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding. The structure of 3-methylbutyric acid is shown below. Draw a second molecule of 3-methylbutyric acid - oriented in the most stable dimeric configuration with the other molecule of acid-and show the intermolecular hydrogen bonds. To indicate a hydrogen bond, draw a regular single bond between the atoms, then click on the "graded select" tool (the yellow highlighter) and click on the bond. A selected bond...
The higher the molar mass, the higher which of these intermolecular forces? A. ion-dipole forces B. London dispersion forces C. dipole-dipole forces D. hydrogen bonding
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...
Which two statements about propene and ethanol are true? Н Н Н, Н—С —С—ОН Н H Н Н ethanol propene Ethanol has a lower vapor pressure than propene at a given temperature. and ethanol have London forces and dipole-dipole forces. Both propene Propene has a higher boiling point than ethanol due to its double bond Ethanol forms hydrogen bonds, whereas propene has dipole-dipole interactions Of the two compounds, only ethanol forms hydrogen bonds. о
3. The compounds seen below have similar molar masses, but vary wildly in melting points. Rank the molecules in increasing (low to high) melting point and explain your choices in terms of intermolecular forces. (4 points) OOH NH ного p-Xylene 1,4+dichloro benzene NH2 1,4-phenylene diamine Terephthalic Acid
18. A solid at -40C was heated uniformly until it
changed into a gas. What is the melting point of the
?????
-20C
0C
20C
40C
19. In the temperature-time graph, the segment DE
represents the
Gas being warmed
Solid being warmed
Liquid being warmed
Liquid changing to gas
Solid changing to liquid
20. The principle difference in boiling points of ICl
(97C; mass 162 amu) and Br2 (59C; mass 160 amu) is due
to
London-dispersion forces
Dipole-dipole interactions
Hydrogen...
1. The melting points of most metals are higher than most plastics because: lonic bonds are weaker than metallic bonds Van der Waals bonds are weaker than metallic bonds lonic and Van der Waals bonds are weaker than metallic bonds None of the above a. b. c. d. 2. A rubber band can stretch more than a metal paper clip because: Covalent bonds along polymer chains can stretch and rotate Covalent bonds along polymer chains can rotate and break Covalent...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding. The structure of 3-methylbutyric acid is shown below. Draw a second molecule of 3-methylbutyric acid - oriented in the most stable dimeric configuration with the other molecule of acid-and show the intermolecular hydrogen bonds. To indicate a hydrogen bond, draw a regular single bond between the atoms, then click on the "graded select" tool (the yellow highlighter) and click on the bond. A selected bond...
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