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 = (-)
2
Q
Coulomb’s law
Energy
A
- (k x q1 x q2)/r
- q = charges
- E released or required to make bond
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
4
Q
Lattice Energy
Lattice Energy Calculations
A
- Born-Haber Cycle = Applying Hess’ Law to its maximum
5
Q
Lewis Structures
Lewis Structures
A
- Used to explain that atoms combined to acheieve more stable electrong configuration
6
Q
Lewis Structures
Ions
A
- = [ ] + charge
- Ex) .Cä. –> [Ca] 2+
7
Q
Lewis Structures
Coordinate Covalent Bond
A
- Electrons donated from one atom to another
8
Q
Formal Charge
What are Formal Charges used for?
A
- Determines most possible lewis structure
9
Q
Formal Charge
Formal Charge Equation
A
- FC= V.E. - (non-bonding e-) - (# of bonds)
10
Q
Formal Charge
Formal Charge Rules
A
- FC= 0 for neutral or Ion FC= Ion charge
- FC = 0 more favorable than FC >/< 0
- Less FC > Greater FC
- Best strucure = Lewis Structure with FCs similar to ENs
* Increased EN = Increased - FC
11
Q
Resonance
Resonance Theory
A
- Molecule/ Ions with 2+ plausible Lewis Structures with diff e- distribution
- Hybrids joined with double-headed arrows
12
Q
Delocalized Electrons (Again)
A
- bonding electrons spread out over several atoms
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
14
Q
Valence Bond Theory
Sigma (𝞂) Bond
A
- 1 covalent bond where orbitals overlap
15
Q
Valence Bond Theory
Domain of Double Bond
A
- 1
