Homework Answers
first question (part A)
the answer there are more hydrogen bonds between water molecules than between alcohol molecules
explanation: water molecule has two hydrogen molecule attached to oxygen, whereas methanol has only one hydrogen attached to oxygen, therefore, water molecule will form more hydrogen bonding compare to methanol. therefore water will have greater boiling point
the second question (part B)
the answer is unlike water molecule, ammonia cannot engage in hydrogen bonding
explanation: water has two lone pair for hydrogen bonding whereas ammonia has only one lone for hydrogen bonding
item 31
answer is only one hydrogen of HF molecule can engage in hydrogen bonding, while both hydrogen atom of water molecule can engage in hydrogen bonding
explanation: water molecule has two hydrogen molecule attached to oxygen, whereas HF has only one hydrogen attached to oxygen, therefore, water molecule will form more hydrogen bonding compare to HF. therefore water will have greater boiling point
part D (fourth question
the answer is hydrogen bond formed by HF is stronger since fluorine is more electronegative than nitrogen
explanation: when atom has greater electonegativity then hydrogen bonding will be stronger
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Part A H,0 (100°C) has a higher boiling point than CH, OH (65°C). There are more...
C The boiling point of H,O is much higher than the boiling point of HS. H2O...
C The boiling point of H,O is much higher than the boiling point of HS. H2O is a molecular compound, while HS is an ionic compound. H2O is a polar molecule, so the attractions between the molecules are stronger than those between nonpolar H2S molecules. H2O has strong hydrogen bonds between its molecules, and HS molecules cannot form hydrogen bonds. The dispersion forces between the H2O molecules are much stronger. d The boiling point of CH,O is much higher than...
Why does benzene have a much higher boiling point (80。c) than hexane (69。c), even though they...
Why does benzene have a much higher boiling point (80。c) than hexane (69。c), even though they have the same number of carbons? A) Benzene is much more polar than hexane which enhances the attractive forces between molecules and raises the boiling point. B) Benzene has fewer hydrogens than hexane. C) Benzene is planar and has delocalized electron density which increases the attractive forces between molecules and raises the boiling point. D) Benzene can covalently bond to another benzene molecule which...
3) The temperature of evaporation is much higher for water than for alcohol. Without knowing more...
3) The temperature of evaporation is much higher for water than for alcohol. Without knowing more about the chemistry of alcohol, which of the following is the most logical chemical explanation for this phenomenon A) Fewer hydrogen bonds form between alcohol molecules. As a result, less heat is needed for alcohol molecules to break away from solution and enter the air. B) Alcohol has a higher surface tension than water. This means that alcohol molecules can easily break away from...
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C...
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C vs. -85°C), even though HF has a lower molecular weight
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C vs. -85°C), even though HF has a lower molecular weight
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...
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C...
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C vs. -85°C), even though HF has a lower molecular weight
show me the work in a clear hand writing so i can understand please Intermolecular Forces...
show me the work in a clear hand writing so i can understand
please
Intermolecular Forces and Boiling Point (3 pts) Formaldehyde (CH2O) appeared in your exam. (a) Use Lewis structures to show a molecule of formaldehyde forming hydrogen bonding attractions with a molecule of water. CLEARLY identify the donor and acceptor in this drawing. (b) Referring to your drawing above, briefly explain why two formaldehyde molecules can't form hydrogen bonding attractions between each other. (c) Formaldehyde molecules are twice...
2) Which of the following compounds has the higher boiling point: butane, butanol, butanoic acid, and...
2) Which of the following compounds has the higher boiling point: butane, butanol, butanoic acid, and methyl ethanoate? Briefly explain why. Batanoic acold Because of molecula weight and long a strong hydrogen bonding 3) From the compounds of previous question, which is more soluble in water? Briefly explain why. 4) Give the name of the carboxylic acid and alcohol used to prepare the ester methyl benzoate - Esterification 5) Write the reaction of acid hydrolysis between methyl ethanoate and water.
Which has Part A the higher boiling point: 1-bromopentane or 1-bromohexane? 1-bromopentane 1-bromohexane Request Answer Submit...
Which has Part A the higher boiling point: 1-bromopentane or 1-bromohexane? 1-bromopentane 1-bromohexane Request Answer Submit Part B the higher boiling point: pentyl chloride or isopentyl chloride? pentyl chloride isopentyl chloride Submit Request Answer Part C the greater solubility in water: 1-pentanol or 1-hexanol? 1-pentanol
2 Why is the boiling point of ammonia higher than the boiling point of ethane? What...
2 Why is the boiling point of ammonia higher than the boiling point of ethane? What type of interaction is responsible for sodium chloride's very high melting point? A 5. What type of interaction is responsible for water's high boiling point? 4 A gaseous sample of a compound has a gas density of 0.647 g/L at 694 torr and 20 °C. What is the molar mass of this compound? If this compound contains only nitrogen and hydrogen, and is 82.2%...
C The boiling point of H,O is much higher than the boiling point of HS. H2O is a molecular compound, while HS is an ionic compound. H2O is a polar molecule, so the attractions between the molecules are stronger than those between nonpolar H2S molecules. H2O has strong hydrogen bonds between its molecules, and HS molecules cannot form hydrogen bonds. The dispersion forces between the H2O molecules are much stronger. d The boiling point of CH,O is much higher than...
3) The temperature of evaporation is much higher for water than for alcohol. Without knowing more about the chemistry of alcohol, which of the following is the most logical chemical explanation for this phenomenon A) Fewer hydrogen bonds form between alcohol molecules. As a result, less heat is needed for alcohol molecules to break away from solution and enter the air. B) Alcohol has a higher surface tension than water. This means that alcohol molecules can easily break away from...
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C vs. -85°C), even though HF has a lower molecular weight
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C vs. -85°C), even though HF has a lower molecular weight
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...
2.21 Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCI) (19.4°C vs. -85°C), even though HF has a lower molecular weight
show me the work in a clear hand writing so i can understand
please
Intermolecular Forces and Boiling Point (3 pts) Formaldehyde (CH2O) appeared in your exam. (a) Use Lewis structures to show a molecule of formaldehyde forming hydrogen bonding attractions with a molecule of water. CLEARLY identify the donor and acceptor in this drawing. (b) Referring to your drawing above, briefly explain why two formaldehyde molecules can't form hydrogen bonding attractions between each other. (c) Formaldehyde molecules are twice...
2) Which of the following compounds has the higher boiling point: butane, butanol, butanoic acid, and methyl ethanoate? Briefly explain why. Batanoic acold Because of molecula weight and long a strong hydrogen bonding 3) From the compounds of previous question, which is more soluble in water? Briefly explain why. 4) Give the name of the carboxylic acid and alcohol used to prepare the ester methyl benzoate - Esterification 5) Write the reaction of acid hydrolysis between methyl ethanoate and water.
Which has Part A the higher boiling point: 1-bromopentane or 1-bromohexane? 1-bromopentane 1-bromohexane Request Answer Submit Part B the higher boiling point: pentyl chloride or isopentyl chloride? pentyl chloride isopentyl chloride Submit Request Answer Part C the greater solubility in water: 1-pentanol or 1-hexanol? 1-pentanol
2 Why is the boiling point of ammonia higher than the boiling point of ethane? What type of interaction is responsible for sodium chloride's very high melting point? A 5. What type of interaction is responsible for water's high boiling point? 4 A gaseous sample of a compound has a gas density of 0.647 g/L at 694 torr and 20 °C. What is the molar mass of this compound? If this compound contains only nitrogen and hydrogen, and is 82.2%...
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