Bonding Flashcards
Linear
2 bond pairs
180°
Trigonal planar
3 bond pairs
120°
V shaped
2 bond pairs 2 lone pairs
104.5 °
Square planar
4 bond pairs 2 lone pairs
90°
Trigonal pyramid
3 bond pairs 1 lone pair
107°
Trigonal bipyramid
5 bond pairs
120° and 90°
Tetrahedral
4 bond pairs
109.5°
Octahedral
6 bond pairs
90°
See saw
4 bond pairs 1 lone pair
120° and 90°
T - shaped
3 bond pairs 2 lone pairs
90°
How do hydrogen bonds occur?
Polar molecule which has N, O or F bonded to H
Big difference in electronegativity
Pair of electrons in the bond to the hydrogen and (N,O,F)
How do Van Der Waals occur
Temporary dipole forms
Induces dipole in surrounding molecules
Attraction between delta + on one molecule and delta - on another
How do permanent dipole forces occur
Attraction between delta + on one molecule and delta - on another
Ionic bonding
Strong electrostatic force of attraction between oppositely charged ions
Metallic bonding
Strong electrostatic force of attraction between positive metal ions and delocalised electrons
Electronegativity
Power of an atom to attract a pair of electrons in a covalent bond
What is electronegativity dependent on?
Nuclear charge if atom
Atomic radius
Number of principle energy levels
Why are metals good conductors of heat and electricity?
Delocalised electrons are free to move and carry charge throughout the structure
How does bond shape occur?
Electron pairs repel equally
X bonding pairs no lone pairs
Electron pairs repel
lone pair repulsion/ lone pair bond pair repulsion is greater than bond pair repulsion
Bond angle reduced to X°
X bond pairs X lone pairs
