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Quizzes > Science > Chemistry

Ready to Ace States of Matter & Intermolecular Forces? Take the Quiz!

Explore hydrogen fluoride IMF, HF dipole-dipole forces, CF4 interactions, and more - challenge yourself now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art style intermolecular forces quiz header with CH3OH and HF molecules on yellow background

This quiz helps you master intermolecular forces in CH3OH by spotting hydrogen bonding in methanol, deciding if HF has dipole - dipole forces, and comparing CF4 with HF. Get instant scoring to find gaps before the exam, and keep practicing with a short IMF quiz or a quick molecular structure quiz .

What is the strongest intermolecular force present in CH3OH?
Ion - dipole interactions
London dispersion forces
Dipole - dipole interactions
Hydrogen bonding
Methanol has an -OH group which forms hydrogen bonds between molecules, making this the strongest intermolecular force present. Dipole - dipole and London dispersion forces also exist but are weaker than hydrogen bonds. Ion - dipole interactions require ions, which are not present in pure methanol.
Which of the following intermolecular forces are present in liquid methanol?
London dispersion, dipole - dipole, and hydrogen bonding
Only hydrogen bonding
Only London dispersion forces
Only dipole - dipole interactions
Methanol molecules exhibit London dispersion forces due to instantaneous dipoles, permanent dipole - dipole interactions because of the polar C - O and O - H bonds, and hydrogen bonding via the O - H group. All three act together to determine its physical properties.
Which atom in a methanol molecule acts as the primary hydrogen bond acceptor?
Carbon
Hydrogen in the hydroxyl group
Hydrogen in the methyl group
Oxygen
The oxygen atom in methanol has two lone pairs that can accept hydrogen bonds from neighboring O - H groups. Carbon does not carry lone pairs, and hydrogens cannot accept hydrogen bonds.
Methanol is miscible with water primarily because of which intermolecular interaction?
Dipole - dipole interactions
Hydrogen bonding
Ionic interactions
London dispersion forces
Methanol and water both have O - H groups capable of forming strong hydrogen bonds with each other, leading to complete miscibility. While dispersion and dipole - dipole interactions also occur, hydrogen bonding is the driving force. Ionic interactions are not relevant in neutral methanol and water.
What is the dominant intermolecular force in hydrogen fluoride (HF)?
London dispersion forces
Hydrogen bonding
Dipole - dipole interactions
Ion - dipole interactions
HF molecules engage in strong hydrogen bonding because fluorine is highly electronegative, attracting the hydrogen of a neighboring HF. This hydrogen bonding dominates over dispersion and dipole - dipole forces.
Why is hydrogen fluoride a liquid at room temperature while hydrogen chloride is a gas?
HF has a higher molar mass
HCl molecules are ionic
HCl has only dispersion forces
HF molecules form hydrogen bonds
HF forms strong hydrogen bonds between molecules, raising its boiling point to above room temperature. HCl lacks hydrogen bonding and only has dipole - dipole and dispersion forces, so it remains a gas.
Which compound has a higher boiling point: CH3OH or CH4?
CH3OH
Insufficient data
CH4
They have the same boiling point
Methanol (CH3OH) exhibits hydrogen bonding in addition to dipole - dipole and dispersion forces, while methane (CH4) only has weak dispersion forces. This makes CH3OH boil at 64.7 °C versus CH4 at - 161.5 °C.
Which part of the methanol molecule contributes most to London dispersion forces?
The O - H group
The hydrogen in the hydroxyl group
The C - O bond
The C - H bonds in the methyl group
London dispersion arises from fluctuations in the electron cloud; the methyl group ( - CH3) has several C - H bonds and a larger electron cloud, contributing most to dispersion in methanol. The O - H bond is more polar and involved in hydrogen bonding.
What type of intermolecular force is primarily responsible for the surface tension of liquid methanol?
Hydrogen bonding
Dipole - induced dipole interactions
Covalent bonds
Ion - dipole interactions
Surface tension in methanol is largely due to hydrogen bonding among O - H groups at the liquid surface. These bonds create a cohesive 'skin' requiring extra energy to increase surface area. Other forces are present but weaker.
Which of the following correctly ranks boiling points from lowest to highest: CH4, CH3OH, H2O?
CH4 < CH3OH < H2O
H2O < CH3OH < CH4
CH3OH < CH4 < H2O
CH4 < H2O < CH3OH
Methane (CH4) has only dispersion forces, so it boils at - 161.5 °C. Methanol (CH3OH) boils at 64.7 °C due to hydrogen bonding, and water (H2O) boils at 100 °C with even stronger hydrogen bonding network.
How many hydrogen bonds can one methanol molecule donate and accept simultaneously?
Donate 1, accept 1
Donate 2, accept 2
Donate 2, accept 1
Donate 1, accept 2
Methanol has one hydroxyl hydrogen (can donate one hydrogen bond) and an oxygen with two lone pairs (can accept two hydrogen bonds). This geometry allows a 1:2 donor - acceptor ratio.
Which factor does NOT significantly affect the strength of London dispersion forces?
Electronegativity of bonded atoms
Molecular size (polarizability)
Electron correlation
Shape and surface area
Dispersion forces depend on polarizability, size, shape, and electron cloud fluctuations. Electronegativity affects bond polarity but does not directly control instantaneous dipole strength.
What primarily explains the large boiling point difference between CH3OH (65 °C) and CH3Cl ( - 24 °C)?
Greater molecular weight of CH3OH
Stronger dispersion in CH3Cl
Hydrogen bonding in CH3OH
Ionic character of CH3OH
Methanol's O - H group allows hydrogen bonding, greatly increasing its boiling point. CH3Cl lacks hydrogen bonding and only has dipole - dipole and dispersion interactions.
Which of these molecules exhibits dipole - dipole interactions but cannot form hydrogen bonds?
HCl
NH3
HF
CH3OH
HCl is polar and exhibits dipole - dipole interactions, but chlorine is not electronegative enough to enable hydrogen bonding with hydrogen. CH3OH, NH3, and HF all can hydrogen bond.
When HF dissolves in methanol, which intermolecular interaction is formed between the two species?
Dipole - dipole between HF and C - H
Hydrogen bonding between HF hydrogen and methanol oxygen
Ion - dipole between F - and CH3OH
London dispersion between HF and the methyl group
HF can donate a hydrogen bond to the lone pairs on the oxygen of methanol, creating HF···O - CH3 interactions. These hydrogen bonds stabilize the mixed solution.
Which liquid is more viscous at room temperature: water or methanol?
Methanol
Water
They have the same viscosity
Insufficient data
Water has stronger hydrogen bonding networks than methanol, leading to higher resistance to flow and thus higher viscosity. Methanol's viscosity is lower because it has only one O - H donor per molecule.
Between NH3 and CH3OH, which compound exhibits stronger hydrogen bonding and why?
They are equal, both form three bonds
NH3, because it has three N - H bonds
Neither forms hydrogen bonds
CH3OH, because the O - H bond is more polar than N - H
The O - H bond in methanol is more polar than the N - H bond in ammonia, resulting in stronger hydrogen bonds per interaction in CH3OH. Ammonia's hydrogen bonds are weaker comparatively.
Which of the following species will NOT form hydrogen bonds with itself under normal conditions?
HF
NH3
CH3OH
CH4
Methane (CH4) lacks sufficiently electronegative atoms bonded to hydrogen and has no lone pairs to accept hydrogen bonds, so it cannot hydrogen bond. The others all have X - H groups with lone pairs on X = O, N, or F.
Which molecule is more polarizable: CH3OH or H2O?
CH3OH
H2O
They are equally polarizable
Polarizability cannot be compared
Methanol has a larger electron cloud due to the methyl group, making it more polarizable than water. Higher polarizability enhances London dispersion forces.
Why does increasing the carbon chain length in alcohols lead to higher boiling points?
Greater molecular symmetry
Increased London dispersion forces
Formation of ion - dipole bonds
Stronger hydrogen bonds with water
Longer carbon chains increase surface area and electron cloud size, strengthening London dispersion forces. This raises boiling points even though hydrogen bonding sites remain the same.
Among methanol, ethanol, 1-propanol, and isopropanol, which has the highest boiling point?
Methanol
1-Propanol
Isopropanol
Ethanol
1-Propanol has the longest unbranched carbon chain among these, leading to the greatest London dispersion forces while still hydrogen bonding. Isopropanol is branched, reducing its dispersion compared to 1-propanol.
Which compound exhibits stronger individual hydrogen bonds: HF or CH3OH?
They are the same strength
Neither forms hydrogen bonds
CH3OH
HF
The H - F bond is highly polar due to fluorine's electronegativity, producing individual hydrogen bonds stronger than those in methanol. However, bulk boiling point also depends on dispersion and network effects.
When methanol is mixed with acetone, what is the primary intermolecular interaction formed?
Dipole - induced dipole between acetone and CH3
Hydrogen bonding between the methanol O - H and the acetone C=O
London dispersion between methyl groups
Ion - dipole between CH3OH and acetone
The oxygen in acetone has a lone pair that can accept a hydrogen bond from the O - H group of methanol. This specific H-bond stabilizes the mixture more than dispersion alone.
Which type of interactions must be overcome when methanol vaporizes?
Only dipole - dipole forces
Only covalent bonds within molecules
Ion - dipole and ionic bonds
Intermolecular hydrogen bonds and London dispersion forces
Vaporization requires breaking the noncovalent interactions between molecules - primarily hydrogen bonds and London dispersion forces - while covalent bonds remain intact.
What structural motif do HF molecules adopt in the solid state?
Layered sheets
Zigzag chain via hydrogen bonds
Discrete monomers
Branched network
Solid HF forms zigzag chains of HF molecules linked by hydrogen bonds, with each molecule acting as both donor and acceptor. This linear chain structure is energetically favorable.
Why do branched alcohols like tert-butanol have lower boiling points than their straight-chain isomers?
Increased ionization of branched alcohols
Lower molar mass of branched alcohols
Reduced surface area decreases London forces
Stronger hydrogen bonding in branched alcohols
Branching reduces the effective surface area available for London dispersion forces, weakening overall intermolecular attractions and lowering the boiling point relative to straight-chain isomers.
Which factor contributes most to phenol having a higher boiling point than methanol?
Phenol cannot hydrogen bond
The aromatic ring increases London dispersion forces
Ionic character of phenol
Phenol is nonpolar
Phenol can hydrogen bond like methanol but also has a bulky aromatic ring that increases London dispersion forces, raising its boiling point above that of methanol.
Which description best defines cooperative hydrogen bonding in methanol clusters?
Each hydrogen bond weakens the next one
The formation of one hydrogen bond enhances the strength of adjacent bonds
Hydrogen bonds form only in isolation
Hydrogen bonds become purely electrostatic
Cooperative hydrogen bonding refers to the phenomenon where one hydrogen bond strengthens neighboring hydrogen bonds via electronic redistribution, leading to a network of enhanced interactions. This is observed in methanol clusters and water networks.
In IR spectroscopy of liquid methanol versus gas-phase methanol, the O - H stretching band shifts from about 3600 cm?¹ to ~3300 cm?¹. What does this red shift indicate?
Ionization of methanol in liquid
Stronger O - H covalent bonds in liquid
Reduced mass of O - H oscillator in liquid
Intermolecular hydrogen bonding weakens the O - H bond
The red shift and broadening of the O - H stretch in the IR spectrum of liquid methanol indicates hydrogen bond formation, which lengthens and weakens the O - H covalent bond relative to the gas phase.
In ab initio modeling of methanol dimers, which basis set feature is most critical for accurately predicting hydrogen bond energy?
Extended core electron functions
Exclusion of polarization functions
Diffuse functions to describe electron delocalization
Minimal STO-3G description
Diffuse functions in the basis set are essential for accurately modeling the electron density in the hydrogen bond region, capturing long-range interactions. Without them, H-bond energies are severely underestimated. https://en.wikipedia.org/wiki/Basis_set_(chemistry)#Diffuse_and_polarization_functions
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Study Outcomes

  1. Understand Intermolecular Forces in CH3OH -

    Learn to identify and explain hydrogen bonding, dipole - dipole interactions, and London dispersion forces in methanol molecules.

  2. Analyze Hydrogen Fluoride IMFs -

    Determine the types of intermolecular forces in HF, including whether HF exhibits dipole - dipole interactions and hydrogen bonding.

  3. Compare IMFs in Different Molecules -

    Contrast the intermolecular forces of CH3OH, HF, and CF4 to understand how molecular structure affects force strength.

  4. Apply IMFs to Predict Physical Properties -

    Use knowledge of intermolecular forces to predict boiling points, solubility, and other properties of various compounds.

  5. Evaluate Quiz Performance -

    Assess your understanding by reviewing quiz answers and explanations to identify areas for improvement in intermolecular forces.

Cheat Sheet

  1. Hydrogen Bonding in CH₃OH -

    Methanol exhibits strong hydrogen bonding due to the O - H group, which raises its boiling point significantly above similarly sized molecules (Chemguide, University of Cambridge). These interactions are the primary intermolecular forces in CH₃OH, making it more cohesive and giving it a higher heat of vaporization.

  2. Polarity and Hydrogen Fluoride IMFs -

    HF is a highly polar molecule because of the large electronegativity difference between H and F, so it forms both strong hydrogen bonds and dipole - dipole interactions (American Chemical Society). This combination explains HF's anomalously high boiling point compared to other hydrogen halides.

  3. Does HF Have Dipole - Dipole Forces? -

    Yes - in addition to hydrogen bonding, HF has classic dipole - dipole attractions as the H - F bond generates a permanent dipole moment (IUPAC Gold Book). These forces work alongside hydrogen bonds to stabilize liquid HF and contribute to its unique physical properties.

  4. Intermolecular Force of CF₄ -

    Carbon tetrafluoride is nonpolar and lacks any dipole or hydrogen bonds, so its only intermolecular attractions are London dispersion forces (Journal of Chemical Education). These weak, temporary dipoles explain CF₄'s low boiling and melting points despite its tetrahedral symmetry.

  5. Comparing IMF Strengths: CH₃OH, HF, and CF₄ -

    Ranked by strength: HF (strongest due to hydrogen bonding + dipole - dipole) > CH₃OH (hydrogen bonding) > CF₄ (dispersion only). Remember the mnemonic "HDL" (Hydrogen & Dipole > Liquid dispersion) to recall why HF outweighs methanol, with CF₄ trailing.

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