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.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.

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.
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

Chemistry Ch 7 Vocab

#LCA #Chemistry #Chapter7

Valence Bond Theory The concept that covalent bonds are formed when orbital of different a toms overlap; also called the localized electron theory
Sigma bond A hybrid bond in which an s and p orbital overlap end to end
Pi bond A bond in which there is a side-by-side overlap of the orbitals
resonance A molecular property where instead of oscillating between two different bond regions, the bonds take o n an intermediate character
molecular orbital theory A bonding theory that suggests that the orgbitals of a molecule's atoms are replaced by totally new orbitals when a molecule forms. These orbitals, both bonding and non-bonding, are linear combinations o f the atomic orbitals.
VSEPR (valence shell electron pair repulsion) A theory stating that because of electron-electron repulsion, the electron orbitals in molecules are arranged so that they are as far apart as possible around the central atom
tetrahedral A structural arrangement in which four areas of electron density surround a central atom are oriented toward the corners of a four-sided pyramid
trigonal planar A structural arrangement in which three particles surrounding a central particle are oriented toward the corners of a flat triangle
linear a structural arrangement in which particles are positioned in a straight line
hybridization The process of forming new kinds of orbitals with equal energies from a combination of orbitals of different energies
pyramidal a structural arrangement in which three particles and an unshared electron pair surrounding a central particle are oriented toward the corners of a four sided pyramid
bent A structural arrangement in which two particles are bonded to a central particle nonlinearly
polar covalent bond A chemical bond that has partially positive and partially negative ends because of unevenly shared electrons. All bonds between nonidentical atoms are polar
dipole moment The vector sum of the distance between charges and the strength of the charges; a measure of all bond polarities that exist within a molecule
Created by: IcanDance