Methane (CH4) is a gas, but carbon tetrachloride (CC14) is a liquid at room temperature and standard pressure conditions. Which one of the following is the best explanation for this? The London dispersion forces in CH4 are stronger than the London dispersion forces in CCl4, so even though the two have the same bp, CCl4 is a liquid. O CCl4 is more polarizeable than CH4 and therefore has a higher bp. Cl is more electronegative than H, so the dipole-dipole forces in CCl4 are stronger than in CH4. CH4 exhibits hydrogen bonding, but CCl4 does not, therefore the bp of CCl4 is higher. O CCl4 is a polar molecule and CH4 is nonpolar, therefore CCl4 has a lower bp.

Methane (CH4) is a gas, but carbon tetrachloride (CC14) is a liquid at room temperature and standard pressure conditions. Which one of the following is the best explanation for this? The London dispersion forces in CH4 are stronger than the London dispersion forces in CCl4, so even though the two have the same bp, CCl4 is a liquid. O CCl4 is more polarizeable than CH4 and therefore has a higher bp. Cl is more electronegative than H, so the dipole-dipole forces in CCl4 are stronger than in CH4. CH4 exhibits hydrogen bonding, but CCl4 does not, therefore the bp of CCl4 is higher. O CCl4 is a polar molecule and CH4 is nonpolar, therefore CCl4 has a lower bp.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 1RQ: What are intermolecular forces? How do they differ from intramolecular forces? What are...

See similar textbooks

Related questions

Q: Solve the problems given on the handouts you can find in content area -IR handouts- make sure you…

A: The sharp peaks at 2900 to 3000 cm-1 indicates the presence of the SP3 C-H bond . Sharp peak at…

Q: a common preservative used in hematology and blood bank

A: Different types of preservatives are used as per the laboratory requirement. Preservatives used in…

Q: what does happen in hydrolysis of soap and synthetic detergent?

A: Hydrolysis is the process in which water molecule is used for the reaction, in which large molecule…

Q: Choose your answer on the words/terms written inside the box. Note: answers may repeat Preservatives…

Q: Solution Concentration of FeSCN2+ (M) Absorbance 1 0.0000491…

A: According to Beer Lambert law, the absorbance of any solution is directly proportional to the…

Q: The local anesthetic novocaine is the hudrogen chioride salt

A: The overall reaction is: Calculation of Ka of novocaine:

Q: The pharmacist must prepare a dilute solution of an oral antiseptic of cetylpyridinium chloride,…

Q: Identify the possible product(s) for the reactions below. A Br₂. FeBr3 8 Br₂, heat B

A: Bromination is a process by which a Br atom substitutes another atom present in a compound.Aromatic…

Q: Where does ammonia separate from water?

Q: 2. What is the use of each apparatus employed for the preparation of Calamine Lotion? Ingredient…

A: Solution is made up of solute and solvent. Solute is present in small amount and solvent is present…

Q: when are surfactants used In seperation techniques

A: Surfactants are substances that lower the surface tension of water, making the molecules slipperier…

Concept explainers

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

Question

Please don't provide handwriting solution

Methane (CH4) is a gas, but carbon tetrachloride (CCl4) is a liquid at room temperature and
standard pressure conditions. Which one of the following is the best explanation for this?
The London dispersion forces in CH4 are stronger than the London dispersion forces in CCl4, so even
though the two have the same bp, CCl4 is a liquid.
CCl4 is more polarizeable than CH4 and therefore has a higher bp.
Cl is more electronegative than H, so the dipole-dipole forces in CCl4 are stronger than in CH4.
CH4 exhibits hydrogen bonding, but CCl4 does not, therefore the bp of CCl4 is higher.
O CCl4 is a polar molecule and CH4 is nonpolar, therefore CCl4 has a lower bp.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Step - 1

VIEW

Step 2: Step - 2

VIEW

Solution

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What are intermolecular forces? How do they differ from intramolecular forces? What are dipole-dipole forces? How do typical dipole-dipole forces differ from hydrogen bonding interactions? In what ways are they similar? What are London dispersion forces? How do typical London dispersion forces differ from dipole-dipole forces? In what ways are they similar? Describe the relationship between molecular size and strength of London dispersion forces. Place the major types of intermolecular forces in order of increasing strength. Is there some overlap? That is, can the strongest London dispersion forces be greater than some dipole-dipole forces? Give an example of such an instance.
Diethyl ether (CH3CH2OCH2CH3) was one of the first chemicals used as an anesthetic. At 34.6C, diethyl ether has a vapor pressure of 760. torr, and at 17.9C, it has a vapor pressure of 400. torr. What is the H of vaporization for diethyl ether?
The compounds ethanol (C2H5OH) and dimethyl ether (CH3OCH3) have the same molecular formula. Which is expected to have the higher surface tension? Why?
For each of the following pairs, choose the member with the lower boiling point. Explain your reason in each case. (a) NaCl or PCl3 (b) NH3 or AsH3 (c) C3H7OH or C2H5OCH3 (d) HI(g) or HCl(g)
Arrange the following substances in order of increasing strength of crystal forces: CO2, KCl, H2O, N2, CaO.
Which of the following compounds would you expect to exhibit only London forces? a potassium chloride, KCl b c silicon tetrafluoride, SiF4 d phosphorus pentachloride, PCl5
The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.
Referring to Figure 9.7, state what phase(s) is/are present at (a) 1 atm, 100C. (b) 0.5 atm, 100C.(c) 0.8 atm. 50C.
8.39 Under what circumstances are ion-dipole forces important?
8.43 Identify the kinds of intermolecular forces (London dispersion, dipoledipole, or hydrogen bonding) that are the most important in each of the following substances. (a) methane (CH4) , (b) methanol (CH4OH) , (c) chloroform (CHCl3) , (d) benzene (C6H6) , (e) ammonia (NH3) , (f) sulfur dioxide (SO2)
Silane SiH4, phosphine (PH3), and hydrogen sulfide (H2S) melt at 185 C, 133 C, and 85 C, respectively. What does this suggest about the polar character and intermolecular attractions of the three compounds?
The types of intermolecular forces in a substance are identical whether it is a solid, a liquid, or a gas. Why then does a substance change phase from a gas to a liquid or to a solid?