Login

The Kinetic Molecular Theory: Properties of Solids and Liquids

An error occurred trying to load this video.

Try refreshing the page, or contact customer support.

Coming up next: Phase Diagrams: Critical Point, Triple Point and Phase Equilibrium Boundaries

You're on a roll. Keep up the good work!

Take Quiz Watch Next Lesson
 Replay
Your next lesson will play in 10 seconds
  • 0:03 Kinetic Molecular Theory
  • 1:23 KMT and Properties of Liquids
  • 2:49 KMT and Solids
  • 3:54 Intermolecular Forces
  • 6:17 Phase Changes
  • 7:09 Lesson Summary
Add to Add to Add to

Want to watch this again later?

Log in or sign up to add this lesson to a Custom Course.

Login or Sign up

Timeline
Autoplay
Autoplay
Create an account to start this course today
Try it free for 5 days!
Create An Account

Recommended Lessons and Courses for You

Lesson Transcript
Instructor: Elizabeth (Nikki) Wyman

Nikki has a master's degree in teaching chemistry and has taught high school chemistry, biology and astronomy.

This lesson explores the kinetic molecular theory and how it pertains to the properties of solids and liquids. You'll learn the properties of solids and liquids, discover the types of intermolecular attractions that occur between them and gain an understanding how phase changes happen.

Kinetic Molecular Theory

Take a glass of water. Drop a few drops of red food coloring in it. What happens? The red food coloring drops should make their way down the glass of water slowly, spread out and finally tint all of the water a reddish color. Why does this happen? It happens because both substances are made out of molecules that are constantly moving. These molecules have energy; one of the fundamental principles of the kinetic molecular theory.

The Kinetic Molecular Theory (KMT) is a model used to explain the behavior of matter. It is based on a series of postulates.

Some of the postulates of KMT are as follows:

  • Matter is made of particles that are constantly in motion. This energy in motion is called kinetic energy.
  • The amount of kinetic energy in a substance is related to its temperature.
  • There is space between particles. The amount of space in between particles is related to the substance's state of matter.
  • Phase changes happen when the temperature of the substance changes sufficiently.
  • There are attractive forces in between particles called intermolecular forces. The strength of these forces increase as particles get closer together.

In this lesson, we will focus on how KMT can be used to explain the properties of liquids and solids.

KMT and Properties of Liquid

Check out these two pictures of liquid water:

Water in pool and at molecular level
pool and molecular structure of water

One is a photo of water in a swimming pool; the other is of liquid water on the molecular level. What properties of liquids are evident in these two pictures?

One of the most notable properties of liquids is that they are fluid and they can flow. Liquids have definite volume, but not a definite shape. Liquids are said to have low compressibility; in other words, it's hard to pack liquid particles closer together. Compared to gases, there is relatively little space between particles. Compared to solids, however, liquids have some space between particles. This, in tandem with the fact that liquid particles also have relatively more energy than solid particles, is what allows liquids to flow. On the molecular level, these two factors give liquids the look of being disorganized.

The types of intermolecular forces in a liquid depend on the chemical make up of the liquid itself. Strength of intermolecular force is related to the type of intermolecular force, but it is also affected by the amount of kinetic energy in the substance. The more kinetic energy, the weaker the intermolecular forces. Liquids have more kinetic energy than solids, so the intermolecular forces between liquid particles tend to be weaker. We will discuss types of intermolecular forces later.

KMT and Solids

Now, let's check out some solids:

Pyrite crystals and phosphorus trioxide molecular structure
pyrite crystals and phosphorus trioxide

One of these images is of pyrite crystals in their naturally occurring cubic form; the other is the structure of phosphorus trioxide on the molecular scale. What properties of solids do you notice?

Solid substances have definite shapes and volumes. Solid particles do move, but not very far! Solid particles have relatively little kinetic energy and vibrate in place. Because of this, they can't flow like liquids. Most solids are arranged in a tightly packed crystalline structure. The crystalline structure is an orderly, repeating arrangement of particles called a crystal lattice. The shape of the crystal shows the arrangement of the particles in the solid.

Some solids aren't crystalline-shaped. The ones that aren't are called amorphous solids. Amorphous solids don't have orderly internal structures. Examples of amorphous solids include rubber, plastic and glass. Wax is also an amorphous solid. It can be molded into any shape and remolded anytime it is warmed up a bit.

Intermolecular Forces

As previously noted, intermolecular forces are the attractive forces between particles. They are distinctly different from the bonds that occur within particles. The type of intermolecular forces present depends on the type of particles present.

Hydrogen bonds occur between polar molecules that contain an oxygen, nitrogen or fluorine atom covalently bonded to a hydrogen atom. The intermolecular attraction happens between the partially negatively charged oxygen, fluorine or nitrogen and the partially positively charged hydrogen of a neighboring molecule. Hydrogen bonds are relatively strong intermolecular forces.

Ion-dipole forces occur between an ion and a polar molecule. An ion will form an attraction with an oppositely charged pole of a neighboring molecule. Salt water is loaded with ion-dipole attractions. Positive sodium ions are attracted to the negative poles of water molecules. Negatively charged chloride ions are attracted to the positive poles of water molecules.

Dipole-dipole forces occur between the oppositely charged poles of polar molecules.

To unlock this lesson you must be a Study.com Member.
Create your account

Register for a free trial

Are you a student or a teacher?
I am a teacher
What is your educational goal?
 Back

Unlock Your Education

See for yourself why 10 million people use Study.com

Become a Study.com member and start learning now.
Become a Member  Back

Earning College Credit

Did you know… We have over 95 college courses that prepare you to earn credit by exam that is accepted by over 2,000 colleges and universities. You can test out of the first two years of college and save thousands off your degree. Anyone can earn credit-by-exam regardless of age or education level.

To learn more, visit our Earning Credit Page

Transferring credit to the school of your choice

Not sure what college you want to attend yet? Study.com has thousands of articles about every imaginable degree, area of study and career path that can help you find the school that's right for you.

Create an account to start this course today
Try it free for 5 days!
Create An Account
Support