The state of aggregation of solids can be described as belonging to the following four types: ionic, metallic, covalent network, and molecular. For each of these types of solids, indicate the kinds of particles that occupy the lattice points and identify forces among the particles. How could each type of solid be identified in the laboratory.
I suggest you make a table and write the properties of each kind of aggregate state. That will tell you how they might be identified in the laboratory as well as the forces between those particles. I'm not sure what the problem is asking with regard to the kinds of particles that occupy the lattice points unless the question means ion, or atom.
State the elementary particles
To determine the type of solid in the laboratory, we need to consider the types of particles that occupy the lattice points and the forces among these particles. Let's break it down for each type of solid:
1. Ionic Solids:
- Particles: The lattice points in ionic solids are occupied by positively charged metal cations and negatively charged non-metal anions.
- Forces: The forces between these particles are strong electrostatic forces due to the attraction between opposite charges.
- Identification: In the laboratory, ionic solids can be identified by their high melting and boiling points, as well as their ability to conduct electricity when melted or dissolved in water.
2. Metallic Solids:
- Particles: In metallic solids, lattice points are occupied by positively charged metal cations, arranged in a closely packed array, surrounded by a "sea" of mobile valence electrons.
- Forces: The forces between the metal cations and valence electrons are metallic bonds, which are a combination of electrostatic attraction and delocalization of electrons.
- Identification: Metallic solids can be identified by their high electrical and thermal conductivity, malleability, and ductility.
3. Covalent Network Solids:
- Particles: Covalent network solids consist of an extended three-dimensional network of atoms, where each atom is bonded to its neighboring atoms by strong covalent bonds.
- Forces: The forces between the atoms are covalent bonds, which are very strong and require a significant amount of energy to break.
- Identification: Covalent network solids can be identified in the laboratory by their high melting and boiling points, extreme hardness, and lack of electrical conductivity (except for a few exceptions like graphite).
4. Molecular Solids:
- Particles: In molecular solids, the lattice points are occupied by discrete molecules held together by weak intermolecular forces (such as London dispersion forces, dipole-dipole forces, or hydrogen bonding).
- Forces: The forces between these molecules are relatively weak compared to the other types of solids.
- Identification: Molecular solids can be identified by their relatively low melting and boiling points, as well as their poor electrical conductivity.
In the laboratory, several methods can be used to identify the type of solid. These include observing the physical properties like melting and boiling points, conducting electrical conductivity tests, analyzing crystal structures using X-ray diffraction, and studying spectroscopic properties.