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Unit 4: Chemical Bonding & Intermolecular Forces - Coggle Diagram
Unit 4:
Chemical Bonding & Intermolecular Forces
Ionic Bonds
usually between non-metal and metal
electronegativity difference higher than 2
ionic compounds form crystals (3D until no more pairs are available)
ternary ionic compounds are made of more than 2 elements
polyatomic ion => tightly covalently minded group of atoms that act as a unit to ionically bond with other elements
ammonium is the only positive one
oxyanion => serios of anions containing an element with different numbers of oxygens
when there are only 2 oxyanions, more O has the (-ate) ending
less O has the (-ite) ending
if there are more than 2 (hypo-) less O
(per-) more O
Naming Compounds
Ionic
(-ide) suffix on anion only
use Roman numerals to indicate the charge of the cation
Covalent
use prefixes to dentate how many of each molecule there are
ex.
C4O10 = tetracarbon decaoxide
only use (mono-) prefix on anion
written cation then anion
subscript shows ratio of elements not the number of molecules there are
cation subscript shows charge if it forms more than 1 ion
Covalent Bonds
mostly between non-metal and non-metal
polar
EN difference between .5 and 2
non polar
EN difference between 0 and .5
type of bond that holds the polyatomic ions
Periodic Table
Groups 1A and 2A (plus He)
S subshell
Transition Metals
D subshell
Groups 3A, 4A, 5A, 6A, 7A, and 8A
P subshell
lanthanides/actinides
F subshell
Lewis Structures
one line = 2 electrons
5 molecules: tetrahedral
3 molecules: bent
4 molecules
trigonal planar
trigonal pyramidal
lone pair on center atom
2 molecules: linear
Octet Rule
each element can only have 8 electrons
HONC1234
Hydrogen: 1 bond (2 electrons)
Oxygen: 2 bonds (4 electrons)
Nitrogen: 3 bonds (6 electrons)
Carbon: 4 bonds (8electrons, full octet capability)