Midterm 2 Flashcards
Ionic Bonding
- Metals + non-metals
- Complete transfer of electrons
- form extended structures not molecules (lattice/ crystals)
Strength of ionic bond depends on
- ionic size (the smaller the stronger the bond)
- Magnitude of charges (the bigger the stronger the bond)
Covalent
- Share electrons
- Non-metal + non-metal
- Form molecule
- High IE very negative EA
Metallic Bonding
metal + metal
delocalized sea of electrons (extended structure)
Electronegativity
The ability of an atom bonded in a molecule to attract shared electrons to itself
Ax2
molecular: linear
Electron group geometry: linear
Ideal bond angle: 180
Ax3
molecular: Trigonal Planar
Electron group: Trigonal Planar
Ideal bond angle: 120
Ax2E
molecular: Trigonal Planar
Electron group: Bent
Ideal bond angle: 120
Actual angle: less than ideal
Ax4
molecular: Tetrahedral
Electron group: Tetrahedral
Ideal bond angle: 109.5
Ax3E
molecular: Tetrahedral
Electron group: Trigonal pyramidal
Ideal bond angle: 109.5
Actual bond angle: less than ideal
Ax2E2
molecular: Tetrahedral
EG: Bent
Ideal: 109.5
Actual: very less
Ax5
M: Trigonal bipyramidal (two axial, 3 equatorial)
EG: Trigonal bipyramidal
Ideal: 90 and 120
Ax4E
M: Trigonal bipyramidal (two axial, 3 equatorial)
EG: Seesaw
Ideal: 90 and 120
actual: less than
Ax3E2
M: Trigonal bipyramidal
EG: T-shaped
ideal: 90 and 120
Actual: axial-equatorial bond are less than 90
Ax2E3
M: Trigonal bipyramidal
EG: Linear
Ideal: 90 and 120
Actual two axial bonding pairs are 180 apart
