Recognising solid type from its formula

1	2
							1H										2He
3 Li	4 Be											5 B	6 C	7 N	8 O	9 F	10 Ne
11 Na	12 Mg											13 Al	14 Si	15 P	16 S	17 Cl	18 Ar
19 K	20 Ca	21 Sc	22 Ti	23 V	24 Cr	25 Mn	26 Fe	27 Co	28 Ni	29 Cu	30 Zn	31 Ga	32 Ge	33 As	34 Se	35 Br	36 Kr
37 Rb	38 Sr	39 Y	40 Zr	41 Nb	42 Mo	43 Tc	44 Ru	45 Rh	46 Pd	47 Ag	48 Cd	49 In	50 Sn	51 Sb	52 Te	53 I	54 Xe
55 Cs	56 Ba	71 Lu	72 Hf	73 Ta	74 W	75 Re	76 Os	77 Ir	78 Pt	79 Au	80 Hg	81 Tl	82 Pb	83 Bi	84 Po	85 At

Metallic solids
A metal lattice is represented by the symbol for the metallic element.
Metallic elements are in the blue squares in the periodic table.
Example: Cu (lattice shown), Na, Mg C

Ionic solids
Substances existing as Ionic solids are always compounds
For ionic solids having only two elements, one is a metal and one is a nonmetal.
Nonmetallic elements are in green boxes in the periodic table.
Examples: NaCl (lattice shown), CaF₂, MgO.

Molecular solids
Both elements and compounds may exist as molecules (groups of atoms).
All elements in molecular solids are non-metals.
Examples: O₂, H₂O (molecule shown), CCl₄, SCl₂

Network solids
The common network solids involve either silicon (Si) with oxygen or carbon OR the elemental forms of carbon.
Note that carbon and silicon are from the center of the periodic table.
Examples: C(graphite), C(diamond), SiO₂ (lattice shown)