Exam 4 Chem

This set of flashcards covers: electron geometry, molecular geometry, electronegativity difference range (ionic, polar covalent, covalent), .....and more. :) Note: Mostly ionic = ionic. Same for mostly covalent. Just following what the book says yo.

2 electron domains, 0 lone pairs

Linear

Ideal Bond Angle for Linear

180

3 electron domains, 0 lone pairs

Trigonal Planar

3 electron domains, 1 lone pair

Bent/V-shaped

Ideal Bond Angle for Trigonal Planar

120

4 electron domains, 0 lone pairs

Tetrahedral

Ideal Bond Angle for Tetrahedral

109.5

4 electron domains, 1 lone pair

Trigonal Pyramidal

4 electron domains, 2 lone pairs

Bent/V-shaped

5 electron domains, 0 lone pairs

Trigonal Bipyramidal

Ideal AXIAL Bond Angle for Trigonal Bipyramidal

90

Ideal EQUATORIAL Bond Angle for Trigonal Bipyramidal

120

5 electron domains, 1 lone pair

Seesaw

5 electron domains, 2 lone pairs

T-shaped

5 electron domains, 3 lone pairs

Linear

6 electron domains, 0 lone pairs

Octahedral

Ideal Bond Angle for Octahedral

90

6 electron domains, 1 lone pair

Square Pyramidal

6 electron domains, 2 lone pairs

Square Planar

ΔEN: 0.0

Nonpolar

ΔEN: 0.1 - 0.4

Mostly Nonpolar Covalent

ΔEN: 0.5 - 1.7

Polar Covalent

ΔEN: 1.7 - 3.3

Mostly Ionic

Formal Charge =

# of valence electrons - unshared electrons - (1/2 x shared electrons)

Oxidation Number =

# of valence electrons - (#of shared electrons + # of unshared electrons)

Bond Angle of T-shaped

Bond Angle of Square Pyramidal

Bond Angle of Square Planar

90

Hybrid Orbitals formed: Linear

two sp orbitals

Hybrid Orbitals formed: Trigonal Planar

three sp² orbitals

Hybrid Orbitals formed: Tetrahedral

four sp³ orbitals

Hybrid Orbitals formed: Trigonal Bipyramidal

five sp³d

Hybrid Orbitals formed: Octahedral

six sp³d²

Born Haber Cycle Equation (Rearrange to solve for specific variable)

Heat of Formation = Enthalpy of Atomization + Dissociation Energy + Sum of Ionization Energies + Sum of Electron Affinities + Lattice Energy

As charge ____, lattice energy increases.

Increases

Lattice energy ____, as atomic size increases.

Decreases

Properties of Ionic Compounds

-Hard (doesn't dent)
-Brittle (doesn't bend)
-Rigid (cracks w/o deforming)
-Do NOT conduct electricity unless melted or dissolved
-High melting/boiling points

Properties of Covalent Compounds

-Strong INTRAmolecular forces
-Weak INTERmolecular forces
-Generally low melting/boiling points
-Poor electric conductors
-Soft solid form

Properties of Metallic Bonding

-Good conductors of electricity in solid and liquid state
-Good conductors of heat
-Moderate to high melting points, higher boiling points
-Dent and bend when struck by a hammer
-Mobile valence electrons

Metallic Bonding VS Ionic Bonding

No anions present and metal ions are not held as tightly

Metallic Bonding vs Covalent Bonding

No particular pair of metal atoms is bonded through a localized electron pair

Octet Rule Exceptions: Underfilled

B and Be

Octet Rule Exceptions: Overfilled

Nonmetals in period 3 or higher

Octet Rule Exceptions: Free radical

Odd number of valence electrons

Relationship between Bond Order, Bond Length, & Bond Energy

Bond Order ↑ Bond Length ↓ Bond Energy ↑

Polar molecule

-Asymmetric charge/electron distribution
-Odd number of lone pairs on central atom
-Dipole moments do not cancel

Non polar molecule

Symmetrical charge/electron distribution
-No lone pairs on central atom OR are evenly distributed on the molecule (check the shape)
-Dipole moments cancel