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

3 forms of C (carbon)

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

SiO₂ (type)

Network Solid (3-D)

Graphite (type)

2-D network solid

2 allotropes of carbon

graphite; diamond

Diamond (type)

Network solid (3-D)

Graphite (unit cell)

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

Silica (description of structure)

has more polymorphs than almost any other structure


different forms of crystal structure for the same solid material


different structural modifications of an element; bonding is different


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


Formed from α-quartz at 846K.

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.

Diamond (structure)

tetrahedral network

Si (structure)

tetrahedral network

Fe (type)

metallic solid

H₂ (type)

molecular solid

Ag (type)

metallic solid

Si (unit cell)

Pb (type)

metallic solid

H₂O (type)

molecular solid

SiC (structure)

tetrahedral network

SiC (type)

Network solid (3-D)

Si (type)

Network solid (3-D)


molecular solid


group 18 solid (aka atomic solid)


a regular, repeating array of atoms or ions

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.

glass (type)

amorphous solid

NH₃ (type)

molecular solid

U (type)

metallic solid

coke (type)

amorphous solid

NaCl (type)

ionic solid

NaCl (structure)

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