Busy. Please wait.

show password
Forgot Password?

Don't have an account?  Sign up 

Username is available taken
show password


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.

By signing up, I agree to StudyStack's Terms of Service and Privacy Policy.

Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.

Remove ads
Don't know
remaining cards
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
restart all cards

Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how


Intermolecular Forces

Intermolecular Forces forces between seperate molecules, WEAKLY hold together two different
Intramolecular Forces ionic and covalent bonds, they are STRONG and hold compounds and molecules together
intra inside
inter in-between
What do we mainly use intermolecular forces for? covalent not as much for ionic
Phase Changes when a substance changes from solid to liquid to gas, the molecules remain intact
What are the changes in state due to? changes in the forces among molecules rather than in those within the molecules
How many intermolecular forces are there? 4, but right now were only leaning three
Types Of Intermolecular Forces hydrogen bonding, dipole-dipole, London dispersion
What does every polar molecule have? a dipole
Hydrogen Bond 1. bound to a highly electronegative atom N,O, and F 2. special dipole-dipole interaction which is the strongest IMF
Dipole-Dipole 1. interactions between two polar molecules 2. polar molecules line up so that the positive and negative ends are close to each other
London Dispersion (van der Waals Forces) 1. occurs in ALL molecules 2. higher molar mass, more electrons, more polarizable, stronger LDF 3. attractive forces created by the motion of electrons making temporary dipoles induced in atoms or molecules
What is dipole induced significant in? large atoms/molecules, strength increases with mass of the molecule
What does a stronger IMF mean? 1. higher melting and boiling point 2. higher viscosity 3. higher surface tension 4. less volatile( evaporates less easily)
Surface Tension the amount of energy required to stretch or increase the surface of a liquid by a unit area
Cohesion the intermolecular attraction between LIKE molecules
Adhesion an attraction between UNLIKE molecules
Viscosity a measure of a fluid's resistance to flow
How can you tell if a molecule is polar? contain polar bonds that contain form dipoles, look at the electronegativity of the bond, if the difference in electronegativities is between 0.4 and 1.7 then it is polar
Why are the properties of molecular compounds so diverse? the strengths of intermolecular attractions vary widely
How do dispersion forces compare to dipole interactions? both involve an electrical attraction between molecules, but dispersion forces are much weaker and temporary
What is thought to cause the dispersion forces? motion of electrons
What causes dipole interactions? attraction between polar molecules
What causes hydrogen bonding? bonding of a covalently bonded hydrogen atom with an unshared electron pair
A hydroxide group (-OH) is a component of most bases
Created by: jordinlevy