Bonding Flashcards
Trigonal pyramid
107 degrees
tetrahedral
109.5 degrees
trigonal planar
120 degrees
Y-X-Y
Linear
180 degrees
square planar
90 degrees
octahedral
90 degrees
trigonal bipyramidal
120 and 90 degrees
V-shaped
104.5 degrees
Hydrogen bonding
NOF are very electronegative so pull electron pair strongly
this makes the H+ very delta positive
in diagram show all the partial charges lone pairs and H bond with dashes
permanent dipole dipole
Between polar molecules
difference in electronegativity
attraction between delta positive on one molecule and delta negative on the next
Van der Waals forces, how they arise and what affects them
non polar molecules
-electrons constantly moving
-temporary dipole formed
-induces temporary dipole in the next molecule
-attraction between delta + and delta - on different molecule
-all simple molecules have these
size/ Mr and surface area contact all affect van der waals
electron repulsion theory
pairs repel each other and causes the molecule to adopt a shape with the least repulsion
LP>BP-LP>BP-BP
Metallic bonding meaning and factors and properties
Strong electrostatic force of attraction between positive metal ions and the sea of delocalised electrons
factors
-charge
-number of electrons
-atomic radius
properties
-good conductors from free electrons
-high melting point
-malleable and ductile as they have layers
properties of ionic compounds and strength factors
- Solids at room temperature from giant lattice
- high melting/ boiling points
- don’t conduct when solid
strength
-higher charge=stronger
smaller ionic radius = stronger
electronegativity meaning and how it increases
power of an atom to attract the pair of electrons in a covalent bond
increases across period and up the group
