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WorksheetsElectron & Solids Review
Total questions: 22
Worksheet time: 1hrs 11mins
1s22s22p63s23p64s23d10
1s22s22p63s2
how many electrons are present?
7
2
6
8
how many electrons are present?
7
4
6
8
how many electrons are present?
1
3
2
8
Define crystalline solid
A solid in which the atoms CANNOT be changed.
A regular repeating, three-dimensional structure of atoms that form a crystal lattice.
A pure solid that can conduct electricity.
A pure solid that has a defined melting and boiling point.
One major difference between crystalline and amorphous solids is that
crystalline solids have a true melting point, while amorphous solids do not.
amorphous solids have a lattice structure.
amorphous solids always behave consistently and uniformly.
crystalline solids break unpredictably and can produce curved fragments.
Which is an example of an ionic crystal?
Graphite (lead in a lead pencil)
Sodium Chloride (NaCl)
Ammonia (NH3)
Iron (Fe)
Which type of solid has very strong covalent bonds between neighboring atoms?
Ionic Crystal
Covalent Molecular Crystal
Metallic Crystal
Covalent Network Crystal
Identify the metallic crystal.
Graphite (carbon)
NaCl
Ammonia (NH3)
Iron (Fe)
High melting points, good conductors of electricity in the solid state, does not dissolve in water.
Ionic
Metallic
Covalent Network
Covalent Molecular
Identify the property that gives metallic solids the ability to conduct electricity well, but not covalent network solids.
Electrons in metallic solids are strongly bound in place
Electrons in covalent network solids are freely moving around
Covalent network solids are not bound to other atoms
Metallic solids have a sea of electrons that are not bound and can move about the solid freely.
KCl is
a metallic network
an ionic substances
a polar covalent substances
a non polar covalent substances
Which of the following is an example of covalent network solid.
Diamond (carbon)
Graphite (carbon in a lead pencil)
copper
silver chloride
