Chemistry Week 12

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Last updated 7:54 PM on 4/10/26
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8 Terms

1
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Valance Bond Theory

  • States that a covalent bond is just an overlap of atomic orbitals

  • Atoms want to be as close together as possible

- Limited by nuclei pushing each other away

  • Energy slowly decreases as atoms move together, but then skyrockets as they get close enough for nuclei to be repulsive

<ul><li><p>States that a covalent bond is just an overlap of atomic orbitals</p></li><li><p>Atoms want to be as close together as possible </p></li></ul><p>- Limited by nuclei pushing each other away </p><ul><li><p>Energy slowly decreases as atoms move together, but then skyrockets as they get close enough for nuclei to be repulsive </p></li></ul><p></p>
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Sigma Bond

  • Type of overlap of atomic orbitals

  • Happens when two s orbitals, an s and a p orbital, or the end to end overlap of 2 p orbitals occurs

  • Can be the only bond in a pair or the first bond of a multi bond

  • Bonds exist on the bonding access

- Bonds in one straight line of space, only capable of holding one electron pair

<ul><li><p>Type of overlap of atomic orbitals</p></li><li><p>Happens when two s orbitals, an s and a p orbital, or the end to end overlap of 2 p orbitals occurs</p></li><li><p>Can be the only bond in a pair or the first bond of a multi bond</p></li><li><p>Bonds exist on the bonding access </p></li></ul><p>- Bonds in one straight line of space, only capable of holding one electron pair</p><p></p>
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Pi Bond

  • Type of overlap of atomic orbitals

  • Happens when side by side p orbitals overlap

  • Bonds happen above and below the bonding axis

  • Seen as multiple bonds in lewis structures

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Hybrid Orbitals

  • S and P orbitals combine

- Notated as SP^x with x being the number of P orbitals that needed to be used

  • Done when multiple bonds are needed

- 1 Bond for every pair used

<ul><li><p>S and P orbitals combine</p></li></ul><p>- Notated as SP^x with x being the number of P orbitals that needed to be used </p><ul><li><p>Done when multiple bonds are needed </p></li></ul><p>- 1 Bond for every pair used </p><p></p>
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Lewis Structure Short Hand

  • Used in large organic models

  • C and H aren’t draw

- C is implied to be between bonds and at the end of bonds

- Every C is given an octet by adding as many H to it as necessary

<ul><li><p>Used in large organic models</p></li><li><p>C and H aren’t draw</p></li></ul><p>- C is implied to be between bonds and at the end of bonds</p><p>- Every C is given an octet by adding as many H to it as necessary </p>
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Paramagnetism

  • Weak attractions form to externally applied magnetic force

  • Caused by unpaired electrons that exist in molecule

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Diamagnetic

  • Weak repulsion to externally applied magnetic force

  • Caused by all electrons being paired

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Molecular Orbital Theory

  • Describes electron distribution in a molecule using molecular orbitals

- Molecular orbitals formed through combining linear combinations of atomic orbitals (LCAO)