6. Which one of the following is the strongest intermolecular force experienced
ID: 996027 • Letter: 6
Question
6. Which one of the following is the strongest intermolecular force experienced by noble gases? a) London dispersion forces b) Dipole-dipole interactions c) Hydrogen bonding d) lon-ion interactions 7. Methane (CH) is a gas, but carbon tetrachloride (CCla) is a liquid at room conditions. Which of the following explains this phenomenon? a) CCl4 is a polar molecule and CH4 is not b) CCl4 and CH4 have different geometries and shapes. c) CH4 exhibits hydrogen bonding and CCl4 does not. d) Cl is more electronegative than H e) None of these 8. Which of the following species exhibits the strongest intermolecular forces? a) CH b) H20 c) N2 d) Co e)He 9. When a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction? molecule molecule molecule water molecule a) A hydrogen atom from one water molecule and a hydrogen atom from the other water b) An oxygen atom from one water molecule and an oxygen atom from the other water c) A hydrogen atom from one water molecule and an oxygen atom from the other water d) Two hydrogen atoms from one water molecule and one hydrogen atom from the other e) A hydrogen atom and an oxygen atom from the same water molecule. 10. Which intermolecular force is the strongest? a) Dipole-dipole b) London dispersion c) Hydrogen bonding d) lon-ion interactions 11. Which of the following would you expect to have the lowest vapor pressure? a) CHOCH) CH.CH,CHCH b) CH CH20H a) CH3OCH c) CHCH2 e) H20 12. Which of the following is the correct order of boiling points for KNOs, CH3OH, CaHo, and Ne? b) CH3OHExplanation / Answer
6) London dispersion force
7)E: none of these.
The reason is that CCl4 is held together with an ionic bond, a strong bond which results in high melting and boiling points. CH4 is held together with weaker covalent bonds, meaning it has a low melting and boiling point. The stronger bonds that hold CCl4 together allow it to exist as a liquid at room temperature. Methane's boiling point is so low (far below zero), that it cannot exist as anything but a gas at room temperature.
8)b) H2O
Water exhibits hydrogen bonding. Methane (CH4), N2, and He exhibit London dispersion forces. Carbon monoxide (CO) exhibits dipole–dipole interactions
9)C, one hydrogen from one molecule and one oxygen from the other molecule. The partial negative charge of the oxygen, and partial positive charge of the hydrogen attract one another, forming a weak bond.
10)D)
The intermolecular forces increase with increasing polarization of bonds. Strength of forces (and therefore impact on boiling points) is ionic > hydrogen bonding >dipole dipole > dispersion
11)e )H20
The substance with the highest boiling point should have the lowest vapor pressure at room temperature
12)
d) Ne < C2H6 < CH3OH < KNO3
The boiling points are determined by size and intermolecular forces. Ne has the lowest boiling point because it is the smallest and has only London dispersion forces. C2H6 is next; it has only London dispersion forces. CH3OH is next; it has dipole–dipole forces. KNO3 has the highest boiling point, because it has ionic forces.
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