Types of Solid
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Not all solids are the same
Solid substances have a wide range of melting points
Some solids are conductive, others are not
In this activity, we will look at four types of solids, the substances in each category, and their properties
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Four types of solids illustrated in Model 1: Metall-Solids, Ionic Solids, Molecular Solids, Network Covalent Solids
Complete columns A-C in the table by referring to the examples in Model 1
Complete columns D and E in the table by referring to the examples in Model 1
Four possible forces of attraction in a solid: covalent bonds, ionic bonds, metallic bonds, and intermolecular forces
Discuss the type of attractive forces in each type of solid
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Identify the type of attractive forces broken upon melting for each type of solid in Model 1
Match descriptions with the four types of solids
Discuss the effect of strong attractive forces on the melting point of a solid
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Compare the substances listed in Model 2 with those in Model 1
Identify the type of solid with the lowest melting points
Identify the type of solid with the lowest enthalpies of fusion
Rank the remaining three types of solids based on their attractive forces
Use concepts learned to predict the type of solid for given substances
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Properties other than melting point and enthalpy of fusion can be helpful in determining the structure of a solid.
Conductivity and solubility are examples of such properties.
For a substance to be soluble in water, it must be charged or polar.
For a substance to be conductive, there must be charged particles in a state that allows them to complete a circuit.
Model 3 shows the solubility and conductivity of various solids.
Model 3 - Solubility and Conductivity of Solids
Iron(II) sulfide (FeS)
Insoluble in water
Not conductive as a solid
Conductive as a liquid
Calcium bromide (CaBr2)
Very soluble in water
Not conductive as a solid
Conductive as a liquid and in aqueous solution
Sodium chloride (NaCl)
Very soluble in water
Not conductive as a solid
Conductive as a liquid and in aqueous solution
Nitrogen (N2)
Slightly soluble in water
Not conductive in any state
Water (H2O)
Not applicable (N/A) for solubility and conductivity
Carbon dioxide (CO2)
Slightly soluble in water
Not conductive in any state
Diamond (C)
Insoluble in water
Not conductive in any state
Silica (SiO)
Insoluble in water
Not conductive in any state
Platinum (Pt)
Insoluble in water
Conductive as a solid and in aqueous solution
Brass (Cu and Zn)
Insoluble in water
Conductive as a solid and in aqueous solution
Nickel (Ni)
Insoluble in water
Conductive as a solid and in aqueous solution
Questions:
Which type(s) of solid is generally very soluble in water?
Ionic solids are generally very soluble in water.
Which type(s) of solid is least soluble in water?
Metals and network covalent solids are least soluble in water.
Which type of solid is most conductive in the solid state?
Metals are most conductive in the solid state.
Why do some substances in Model 3 have N/A entries for conductivity in aqueous solutions?
Conductivity data for those substances would not exist because they cannot form in aqueous solutions or they do not dissolve in water.
What properties of metallic solids make them well suited for tools and electrical circuits?
Metallic solids are not brittle and are resistant to breaking into pieces, making them well suited for tools.
Metallic solids are good conductors of electricity, making them useful in electrical circuits.
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Extension Questions
Give two reasons why conductivity data for some substances in Model 3 would not exist.
Conductivity data would not exist because these substances cannot form in aqueous solutions or they do not dissolve in water.
What properties of metallic solids make them well suited for tools and electrical circuits?
Metallic solids are not brittle and are resistant to breaking into pieces, making them well suited for tools.
Metallic solids are good conductors of electricity, making