Chapter 12: Problem 13
Indicate the type of solid (molecular, metallic, ionic, or covalent-network)
for each compound: (a)
Short Answer
Expert verified
The types of solids for the given compounds are:
(a) :
(b) :
(c) :
(d) (table sugar):
(e) (benzene):
(f) :
Step by step solution
01
Recognizing Compound Type
Since calcium is a metal, and carbonate (CO3) is polyatomic ion, this is an ionic compound, as it is formed by the transfer of electrons between the metal and non-metal.
02
Solution
For , the type of solid is:
(b)
03
Recognizing Element Type
Platinum (Pt) is a metal, and metallic solids are formed when metal atoms are closely packed and held together by metallic bonds.
04
Solution
For , the type of solid is:
(c)
05
Recognizing Compound Type
Zirconium (Zr) is a metal, and Oxygen (O) is a non-metal, which means this is a compound with ionic bonding between the metal and non-metal.
06
Solution
For , the type of solid is:
(d)
07
Recognizing Compound Type
The molecule is composed only of non-metal atoms, which means it forms a molecular solid. Molecular solids are formed by individual molecules held together by weaker van der Waals forces or hydrogen bonds.
08
Solution
For table sugar , the type of solid is:
(e)
09
Recognizing Compound Type
Benzene, similar to table sugar, is composed only of non-metal atoms. The molecules are held together by weaker van der Waals forces in a molecular solid.
10
Solution
For benzene , the type of solid is:
(f)
11
Recognizing Element Type
Iodine (I) is a non-metal that exists as diatomic molecules composed of two iodine atoms, which are held together by van der Waals forces in molecular solids.
12
Solution
For , the type of solid is:
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Molecular Solids
Molecular solids are an interesting type of solid where the key components are molecules rather than atoms or ions. These molecules are held together by relatively weak forces, primarily van der Waals forces or hydrogen bonds. These intermolecular forces are much weaker compared to ionic or covalent bonds, which is why molecular solids tend to have lower melting points.
Here are some key points about molecular solids:
Here are some key points about molecular solids:
- They have low melting and boiling points compared to other types of solids.
- Their structures are usually soft and more easily disrupted.
- Common examples include substances like dry ice ( CO_2), iodine ( I_2), and table sugar ( C_{12}H_{22}O_{11}).
- They are often poor conductors of electricity due to the absence of free electrons or ions.
Ionic Solids
Ionic solids are fascinating due to the strong electrostatic forces between their ions. These solids form when positive and negative ions come together in a lattice structure, each type of ion being attracted to its oppositely charged neighbors. Because of these strong attractions, ionic solids are incredibly stable and usually have high melting points.
Notable features of ionic solids include:
Notable features of ionic solids include:
- Possessing high melting and boiling points due to the strength of ionic bonds.
- Lattice structures that are rigid and well-organized.
- Typically hard but brittle due to the slipping of planes of ions past each other.
- In their solid state, they don't conduct electricity. However, when dissolved in water or molten, they become excellent conductors as the ions are free to move.
- Common examples include sodium chloride (salt, NaCl) and calcium carbonate ( CaCO_3).
Metallic Solids
Metallic solids stand out due to their unique bonding and structural properties. Composed entirely of metallic atoms, these solids are characterized by a "sea of electrons" that move freely among a lattice of metal cations. This delocalization of electrons explains many of the distinctive physical properties of metals.
Key characteristics of metallic solids include:
Key characteristics of metallic solids include:
- They are excellent conductors of electricity and heat due to the mobility of the electrons.
- Metallic solids are typically ductile and malleable, meaning they can be drawn into wires and hammered into sheets.
- They often exhibit luster, giving them a shiny appearance.
- They vary in hardness and melting points, though many have moderately high melting points.
- Examples include pure metals like platinum ( Pt) and alloys.