Atomic Structure + Theory Flashcards
Describe ionic bonding
- transfer of electrons
- generally metal to non-metal
Describe covalent bonds
- involves sharing electrons
- often 2 non metals
- bonds depicted by a line in diagrams
Define electronegativity
An atoms ability to compete for electrons in a bond
Increasing across a period and up a group
Use Pauling scale to measure ( 4.0 highest)
Different classifications of bond polarity
PURE COVALENT - EN difference < 0.5 (equal sharing of e)
POLAR COVALENT “ 0.5-1.9 (unequal sharing e)
IONIC “ > 1.9 (higher EN atom pulls e. Doesn’t share at all)
What are electrostatic potential maps?
Diagrams that are useful to visualize bond polarity.
Red means negative extreme (positive ion/partial charge)
Blue means positive extreme (negative ion/partial charge)
Explain the steps to make a Lewis structure diagram
1) total electron count
2) draw skeletal structure
3) fill octet for terminal elements
4) calculate if there’s any remaining e and add them to centre element
5) Calculate formal charges (FC = VE-bonds-lone e)
6) minimize Charges
7) make sure all element have proper e count
* ** F O N C must obey octet rule, only Be and group 13 allowed to have less e than an octet
Rate repulsion from lowest to highest: Lone pair - LP Bonded pair - BP LP - BP what about double bonds?
BP BP
LP BP
LP LP
* double bonds take up more space than bonded pairs because they have stronger repulsion*
Formula for VSEPR classification
AXnEn
A is central atom
X is atoms bonded to central atom
E is lone pairs on central atom
Name all different types of electron group geometry (main classifications)
Linear Trigonal planar Tetrahedral Trigonal bipyramidal Octahedral
Name the different types of isomers in VSPER geometry
Cis - same side Trans - opposite side Fac - same face Mer - different faces Equatorial and axial positions
