He and Ar are both noble gases, are nonpolar, and experience only London dispersion forces (LDF's). Which one has the higher boiling point and why?

Ar has more electrons and is therefore more polarizable.

He has more electrons and is therefore more polarizable.

He has fewer electrons and is therefore not as polarizable.

Ar has fewer electrons and is therefore not as polarizable.

Methane is CH 4 , and carbon tetrachloride is CCl 4 . They are both nonpolar and therefore only experience London dispersion forces (LDF's). Which one has the higher boiling point and why?

CCl 4 because it has more electrons and is therefore more polarizable.

CH 4 because it has more electrons and is therefore more polarizable.

CH 4 because it has fewer electrons and is therefore not as polarizable.

CCl 4 because it has fewer electrons and is therefore not as polarizable.

Which statement explains why Cl 2 is a gas and Br 2 is a liquid at 25 °C and 1 atm?

Br 2 has stronger intermolecular forces than Cl 2 , making it a liquid.

Cl 2 has a higher molecular weight than Br 2 , making it a gas.

Cl 2 is more reactive than Br 2 , which determines its state.

Br 2 has a lower boiling point than Cl 2 .

Explain why H 2 is a gas and I 2 is a solid at 25 °C and 1 atm.

I 2 has more electrons than H 2 and therefore experiences stronger IMF's, keeping it a solid at room temperature.

Because of their molecular structures and electronegativities

Due to their positions in the periodic table.

Because of their atomic masses.

Due to the difference in their electron configurations.

Which of the following best explains why propane, C 3 H 8 , melts at -306.4 °F and decane, C 10 H 22 , melts at 345.4 °F?

Decane has more electrons than propane, leading to stronger London dispersion forces.

Propane has a higher molecular weight than decane.

Propane is a gas at room temperature, while decane is a liquid.

Decane has a lower boiling point than propane.

The structures for ethanal, C 2 H 4 O, and methanol, CH 3 OH, are shown. Identify the types of IMF's that exist in pure samples of each. Ethanal experiences Methanol experiences

LDF's, dipole-dipole, and H-bonding

Honors Chem Chapter 9

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Honors Chem Chapter 9

Quiz

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Chemistry

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10th Grade

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Practice Problem

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Easy

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NGSS

HS-PS1-7, HS-PS1-3, HS-PS3-2

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Abbey Zaepfel

Used 6+ times

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65 questions

Show all answers

FILL IN THE BLANK QUESTION

5 mins • 1 pt

Convert the following pressure: 1650 torr to atm.

FILL IN THE BLANK QUESTION

5 mins • 1 pt

Convert the following pressure: 3.50 x 10^5 atm to mmHg.

FILL IN THE BLANK QUESTION

5 mins • 1 pt

Convert the following pressure: 185 mmHg to atm.

FILL IN THE BLANK QUESTION

5 mins • 1 pt

Convert the following pressures: 5.65 kPa to atm.

FILL IN THE BLANK QUESTION

5 mins • 1 pt

Convert the following pressures: 190 mmHg to torr.

FILL IN THE BLANK QUESTION

5 mins • 1 pt

Convert the following pressure: 85.0 mmHg to kPa.

FILL IN THE BLANK QUESTION

5 mins • 1 pt

Convert the following pressure: 20.2 inHg to mmHg.

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Honors Chem Chapter 9

65 questions

Convert the following pressure: 1650 torr to atm.

Convert the following pressure: 3.50 x 10^5 atm to mmHg.

Convert the following pressure: 185 mmHg to atm.

Convert the following pressures: 5.65 kPa to atm.

Convert the following pressures: 190 mmHg to torr.

Convert the following pressure: 85.0 mmHg to kPa.

Convert the following pressure: 20.2 inHg to mmHg.

Convert the following pressures: 0.025 atm to mmHg.

Convert 37.0°C to Kelvin.

Convert -27°C to Kelvin.

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