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2 allotropes of carbon

graphite; diamond

3 forms of C (carbon)

graphite (2-D network solid)
diamond (3-D network solid)
coke (highly carbonaceous amorphic solid)

Ag (type)

metallic solid


different structural modifications of an element; bonding is different


molecular solid

coke (type)

amorphous solid

Diamond (structure)

tetrahedral network

Diamond (type)

Network solid (3-D)

Fe (type)

metallic solid

glass (type)

amorphous solid

Graphite (description of structure)

layered, planar; can be described as a 2-dimensional lattice because covalent bonds occur only within sheets (planes) called graphenes; in each layer C atoms are arranged in a honeycomb-like lattice

Graphite (structure)

Graphenes (layers) are weakly held together by LDFs. As far as LDFs go they are strong because graphene layers are flat and large.

Graphite (type)

2-D network solid

Graphite (unit cell)

H₂O (type)

molecular solid

H₂ (type)

molecular solid


group 18 solid (aka atomic solid)


a regular, repeating array of atoms or ions

NaCl (structure)

NaCl (type)

ionic solid

NH₃ (type)

molecular solid

Pb (type)

metallic solid


different forms of crystal structure for the same solid material

SiC (structure)

tetrahedral network

SiC (type)

Network solid (3-D)

Silica (description of structure)

has more polymorphs than almost any other structure


Silicon dioxide, (aka) silica, (most commonly found in nature as) quartz

SiO₂ (type)

Network Solid (3-D)

Si (structure)

tetrahedral network

Si (type)

Network solid (3-D)

Si (unit cell)

unit cell

The smallest building block of a crystal, consisting of atoms, ions, or molecules, whose geometric arrangement defines a crystal's characteristic symmetry and whose repetition in space produces a crystal lattice.

U (type)

metallic solid


The most common form of silica (SiO₂) in nature.


Formed from α-quartz at 846K.

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