FINAL - Chapter 2 Bonding Flashcards
(13 cards)
Which atoms can satisfy octets with fewer than 8 electrons?
Carbon, boron, and berelliym
Guideline’s for Lewis structure
- Negative FC on most electronegative atom and positive FC on least electronegative atom
- Fewest and smallest formal charges
VESPR Steric Number 2
(including degrees)
1) AX2
2) AXE
1) Linear
2) Linear
180 degrees
VESPR Steric Number 3
(including degrees)
1) AX3
2) AX2E
1) Trigonal Planar
2) Bent
120 degrees
VESPR Steric Number 4
(including degrees)
1) AX4
2) AX3E
3) AX2E2
1) Tetrahedral (109.5)
2) Trigonal pyrimdinal (106.7)
3) Bent (104.5)
VESPR Steric Number 5
1) AX5
2) AX4E
3) AX3E2
1) Trigonal bipyrmidal
2) Seesaw
3) T-shaped
VESPR Steric Number 6
1) AX6
2) AX5E
3) AX4E2
1) Octaheddral
2) Square pyramidal
3) Square planar
Which casue greater repulsion: electron lone pairs or bonding pairs?
Electron lone pairs
Define electronegativity
Ability of atom in molecule to attract e- in bonding pair to itself
Draw Lewis Structure for CN- (two resonsance forms)
In one triple bond in between with lone pair on each
In other one double bond, C has one lone pair and n has two lone pairs
How do you draw the 3D version of NH3?
N with two lone pairs at the top, 3 H’s spread out in teh bottom half, one with solid bond, one with dash and one with wedge
Why do lone pairs repel stronger than bonding pairs?
Lone pairs are not shared so more tightly bond to central atom, more repulse to neighboring electrons.
Bonding pairs are shared so electron density is more spread out
Why does VESPR incorrectly predict bond angles in OF2 and OH2
Assumes that bonding pairs and lone pairs cause same amount of repulsion but disregards that lone pairs exert more repulsion on neighboring electrons becuase electron density is more concentrate
