13. Liquids, Solids & Intermolecular Forces

Intermolecular Forces

Identifying Intermolecular Forces - Real Chemistry

Would you expect that an anion would be physically closer
to the oxygen or to the hydrogens of water molecules that
surround it in solution?

(c) Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?

Polar Bonds and Molecules

Determine the kinds of intermolecular forces that are present in
each element or compound.
b. NCl3

Intermolecular Forces Example 1

It is common to add Epson salts to bath water when one has been over exercising and has sore muscles. What is the primary intermolecular force that exists between magnesium sulfate, the primary in Epson salts, and the water in the bathtub?

Which type of intermolecular force accounts for each of these differences? (b) Xe is a liquid at atmospheric pressure and 120 K, whereas Ar is a gas under the same conditions. 

(a) Which type of intermolecular attractive force operates between all molecules?

Which of the following intermolecular forces are found in ALL molecules?

Which member in each pair has the greater dispersion forces?(c) SiH4 or GeH4.

CH3CH2CH3

Which of these molecules exhibit the highest number of different intermolecular forces?

Which species is expected to have the largest dispersion forces?

Intermolecular Forces Concept 1

Of the substances Xe, CH3Cl, and HF, which has:
(a) The smallest dipole–dipole forces?

What Are Intermolecular Forces | Properties of Matter | Chemistry | FuseSchool

between molecules and weaker than a chemical bond

between two atoms within a molecule and weaker than a chemical bond

between molecules and stronger than a chemical bond

between two atoms within a molecule and stronger than a chemical bond.

between electrons within an atom and stronger than a chemical bond

A number of salts containing the tetrahedral polyatomic anion, BF4-, are ionic liquids, whereas salts containing the somewhat larger tetrahedral ion SO42 - do not form ionic liquids. Explain this observation.

List the three states of matter in order of (a) increasing molecular disorder

Two isomers of the planar compound 1,2-dichloroethylene
are shown here. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/b931c90e11a95d94-1665671581079.jpg" alt="" /> (a) Which of the two isomers will have the stronger dipole– dipole forces?

What is the difference between London dispersion forces 
and dipole–dipole forces?

(a) How does the average kinetic energy of molecules com- pare with the average energy of attraction between mole- cules in solids, liquids, and gases?

Which member in each pair has the stronger intermolecular dispersion forces? (c) CH3CH2CH2Cl or (CH3)2CHCl

Intermolecular Forces and Boiling Points

Intermolecular Forces Example 2

The dominant forces between molecules (intermolecular forces) are ____ in origin.

The table below shows the normal boiling points of benzene and benzene derivatives. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/95cdb397c6c38390-1665674596236.jpg" alt="" /> (a) How many of these compounds exhibit dispersion in- teractions?

Determine the kinds of intermolecular forces that are present in 
each element or compound. 
d. I2

Propanol (PrOH) and methyl methacrylate (MMA) asso-ciate in solution by an intermolecular force, forming an adduct represented as PrOH•MMA. The equilibrium con- stant for the association reaction is Kc = 0.701 at 298 K. 
(b) Draw a plausible structure for the PrOH • MMA adduct. Use to signify an intermolecular interaction.

Polar Bonds, Polarity and Intermolecular Forces

The DNA base thymine dissolves in water due to hydrogen bonding. 
Which of the following hydrogen bonds drawn between thymine 
and surrounding water molecules are valid? (LO 8.10) 

(a) I and II (b) I, II, IV 
(c) I, II, III (d) III and IV

True or false: (b) For the noble gases the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table.

The critical temperatures and pressures of a series of haloge- nated methanes are as follows: <img src="https://lightcat-files.s3.amazonaws.com/problem_images/7cfe6faee0647565-1665670156584.jpg" alt="" /> (a) List the intermolecular forces that occur for each compound.

Ethanol 1CH CH OH 2 dissolves in hexane 1C H 2. Give the strongest type of intermolecular force between two sol- ute molecules, between two solvent molecules, and between a solute and solvent molecule. (LO 13.1) <TABLE> (a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/6f3041e0b4930bae-1671207545313.jpg" alt="" />

1,3-Propanediol can form intramolecular as well as intermolecular 
hydrogen bonds. Draw a structure of 1,3-propanediol 
showing an intramolecular hydrogen bond.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/b172e9bea90e8d83-1671215024298.jpg" alt="" />

(b) Which type of intermolecular attractive force operates only between polar molecules?

Intermolecular forces are important in creating ordered arrangements in liquid crystals. What types of intermolecu- lar forces exist in a sample of the following compound? <img src="https://lightcat-files.s3.amazonaws.com/problem_images/451e37ef043c35aa-1671139734633.jpg" alt="" />

Hydrogen Bonding

What are Intermolecular Forces?

Which member in each pair has the greater dispersion forces? (a) H2O or H2S,

True or false: (e) The larger the atom, the more polarizable it is.

(b) Which of these kinds of interactions are broken when a liquid is converted to a gas?

Determine the kinds of intermolecular forces that are present in
each element or compound.
a. Kr

Determine the kinds of intermolecular forces that are present in 
each element or compound. 
c. CH3OH

Describe the intermolecular forces that must be overcome to convert these substances from a liquid to a gas: (b) CH3COOH,

When ethyl alcohol, CH3CH2OH, dissolves in water, how many hydrogen bonds are formed between one ethyl alcohol molecule and surrounding water molecules? Sketch the hydro- gen bonding interactions. (Hint: Add lone pairs of electrons to the structure before drawing hydrogen bonds.)

(b) Which of the following molecules can form hydrogen bonds with other molecules of the same kind: CH3F, CH3NH2, CH3OH, CH3Br?

Intermolecular Forces - Hydrogen Bonding, Dipole Dipole Interactions - Boiling Point & Solubility

(a) Which kind of intermolecular attractive force is shown in each case here? (b) Predict which of the four interactions is the weakest. [Section 11.2] (i) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/eb62119f5919c3bb-1665675374272.jpg" alt="" /> (b) <img src="" alt="" /> (c) <img src="" alt="" /> (d) <img src="" alt="" />

Intermolecular Forces Concept 2

Which substance in each of the following pairs would you
expect to have larger dispersion forces?
(b) HCl or HI

Determine the kinds of intermolecular forces that are present in 
each element or compound. 
d. HF

At room temperature, Si is a solid,CCl4 is a liquid, and Ar is a gas. List these substances in order of (a) increasing intermo- lecular energy of attraction and

What types of intermolecular forces exist in a sample of acetone?
(LO 8.8)
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/90f147b6e811686b-1671261734017.jpg" alt="" />
(a) Dispersion forces 
(b) Dispersion forces and dipole–dipole forces 
(c) Dipole–dipole forces 
(d) Dispersion forces, dipole–dipole forces, and hydrogen bonding

List the three states of matter in order of (b) increasing intermolecular attrac- tion.

Determine the kinds of intermolecular forces that are present in
each element or compound.
d. He

Dimethyl ether has the following structure. 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/e13519d90122bf14-1671218627420.jpg" alt="" /> 
(b) Which of the following illustrations depicts the hydrogen 
bonding that occurs between dimethyl ether and water? 
(i) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/eb5228fd4a91848f-1671218288751.jpg" alt="" /> 
(ii) <img src="" alt="" />

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1. Intro to General Chemistry

2. Atoms & Elements

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4. BONUS: Lab Techniques and Procedures

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6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Body Centered Cubic Unit Cell

Body Centered Cubic Unit Cell contains 2 atoms total.

Phase Diagrams

Phase&nbsp;Diagrams show&nbsp;what&nbsp;effect&nbsp;temperature and pressure have&nbsp;on a pure substance in a closed system without any air.

Intermolecular Forces and Physical Properties

Intermolecular forces influence physical properties. &nbsp;We will look at direct and indirect relationships.

Face Centered Cubic Unit Cell

Face Centered Cubic Unit Cell contains 4 atoms in total.

Heating and Cooling Curves

Heating and Cooling Curves represent amount of heat (q) absorbed or released by a substance during phase changes.

Clausius-Clapeyron Equation

The Clausius-Clapeyron Equation establishes a quantitative relationship between vapor pressure and temperature.&nbsp;

Molecular Polarity

Polarity of chemical bonds happen in molecules when there is an unequal sharing of electrons.&nbsp;

Intramolecular Forces are the bonding forces within a molecule. Intermolecular Forces are the attractive forces between 2 molecules.

Simple Cubic Unit Cell

Simple Cubic Unit Cell is the least complex&nbsp;cubic unit cell and contains only 1 atom.

Atomic, Ionic, and Molecular Solids

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Crystalline solids represent structures with well-organized patterns and shapes. Amorphous solids represent structures that lack an organized pattern or shape.&nbsp;</div></div>

Crystalline Solids

Crystalline Solids are composed of unit cells, crystal lattice and lattice point.