Question

differenciate between ionic solid, covalent solid and molecular solid

Answer 1

Ionic crystals -- The ionic crystal structure consists of alternating positively-charged cations and negatively-charged anions (see figure below). The ions may either be monatomic or polyatomic. Generally, ionic crystals form from a combination of Group 1 or 2 metals and Group 16 or 17 nonmetals or nonmetallic polyatomic ions. Ionic crystals are hard and brittle and have high melting points. Ionic compounds do not conduct electricity as solids, but do conduct when molten or in aqueous solution.


Metallic crystal -- Metallic crystals consist of metal cations surrounded by a "sea" of mobile valence electrons (see figure below). These electrons, also referred to as delocalized electrons, do not belong to any one atom, but are capable of moving through the entire crystal. As a result, metals are good conductors of electricity. As seen in the table above, the melting points of metallic crystals span a wide range.


Covalent network crystals -- A covalent network crystal consists of atoms at the lattice points of the crystal, with each atom being covalently bonded to its nearest neighbor atoms (see figure below). The covalently bonded network is three-dimensional and contains a very large number of atoms. Network solids include diamond, quartz, many metalloids, and oxides of transition metals and metalloids. Network solids are hard and brittle, with extremely high melting and boiling points. Being composed of atoms rather than ions, they do not conduct electricity in any state


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Answer 2

Hey !! ✌️

✨Ionic solid - Ionic solids are solid compounds composed of oppositely charged ions held together by electrostatic attractions. 

Examples of ionic solids are: NaCl, CsCl and ZnS. 


✨Covalent Solid - Covalent Solids are solids that are held together by covalent bonds.

Examples include ice (solid water), dry ice (solid CO2), solid iodine and naptholene.


✨Molecular Solid - A molecular solid is a type of solid in which molecules are held together by van der Waals forces rather than by ionic or covalent bonds.

Examples of molecular solids include  sugar, fullerenes, sulfur, and solid carbon dioxide.