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AP Chemistry > Atomic Structure and Electrons > Flashcards

Atomic Structure and Electrons Flashcards

1
Q

Coulomb’s law

Force

A
  • (k x q1 x q2)/r^2
  • q = charges
  • Repulsion Force = (+)
  • Attraction Force = (-)
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2
Q

Coulomb’s law

Energy

A
  • (k x q1 x q2)/r
  • q = charges
  • E released or required to make bond
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3
Q

Lattice Energy

Lattice Energy

A
  • Energy required to seperate 1 mole of an ionic solid into gaseous ions
  • Higher LE ==> Higher Ionic Bond Strength
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4
Q

Lattice Energy

Lattice Energy Calculations

A
  • Born-Haber Cycle = Applying Hess’ Law to its maximum
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5
Q

Lewis Structures

Lewis Structures

A
  • Used to explain that atoms combined to acheieve more stable electrong configuration
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6
Q

Lewis Structures

Ions

A
  • = [ ] + charge
  • Ex) .Cä. –> [Ca] 2+
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7
Q

Lewis Structures

Coordinate Covalent Bond

A
  • Electrons donated from one atom to another
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8
Q

Formal Charge

What are Formal Charges used for?

A
  • Determines most possible lewis structure
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9
Q

Formal Charge

Formal Charge Equation

A
  • FC= V.E. - (non-bonding e-) - (# of bonds)
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10
Q

Formal Charge

Formal Charge Rules

A
  1. FC= 0 for neutral or Ion FC= Ion charge
  2. FC = 0 more favorable than FC >/< 0
  3. Less FC > Greater FC
  4. Best strucure = Lewis Structure with FCs similar to ENs
    * Increased EN = Increased - FC
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11
Q

Resonance

Resonance Theory

A
  • Molecule/ Ions with 2+ plausible Lewis Structures with diff e- distribution
  • Hybrids joined with double-headed arrows
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12
Q

Delocalized Electrons (Again)

A
  • bonding electrons spread out over several atoms
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13
Q

Exceptions to the Octet Rule

Expanded Octet

A
  • More than 8 electrons
  • Happens in elelments that have n > 2
  • Have s–>d sublevels
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14
Q

Valence Bond Theory

Sigma (𝞂) Bond

A
  • 1 covalent bond where orbitals overlap
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15
Q

Valence Bond Theory

Domain of Double Bond

A
  • 1
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16
Q

Valence Bond Theory

Hybridization

A
  • Promotion of electrons and mixing of orbitals
  • Only central atoms
17
Q

Valence Bond Theory

Pi (𝛑) bond

A
  • For bonds after single bonds
  • ex) Double or Triple
  • Bonding pairs are parallel to each other
18
Q

Resonance Strutures

Relation to delocalized atoms

A
  • Having them makes a structure more stable and the more you have the more stable because the lectrons are able to spread out over a larger volume

AP Chemistry (9 decks)

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