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It is an ionic solid.
The intra and inter molecular forces will help to determine the higher boiling.Intra molecular forces are Polar/Non-polar covalent bonds and ionic bonds. Covalent bonds are stronger than ionic bonds.Polar covalent bonds will have a higher boiling point because non-polar covalent bonds are only affected by London forces.Intermolecular forces are hydrogen bonding, diapole-diapole and London. All molecules have London forces.Also the higher the electro-negativity the higher the boiling point.If all of the intra and inter molecular forces are the same, refer to the electro-negativity and size. The greater the electro-negativity and size, the higher the boiling point.
Whilst lithium is a metal and would be expected to form simple salts containing the Li+ ion- the very small size of this ion leads to it polarising the electron clouds of other ions and leading to covalent character of the bond. This is illustrated by the unusually high solubilities of Li halides in organic polar solvents. this phenomenon is explained by "fajan's rules".
The smaller size of cation (as Li+) and larger size of anion (as I-) is the main cause for the covalent character in ionic compound.
You cannot tell from a formula whether an compound is ionic or molecular. The distinction is arbitrary at best, and there are actually very few purely ionic compounds. Al2S3 will be somewhere between ionic and covalent. Depending what level you are at and wherer you are taught different classifications of aluminium sulfide are given. See link for one view. Al2S3 is a colorless high melting compound, the aluminium atoms are in tetrahedral coordination in the most stable forms. This is line with the size difference between S and Al. The electronegativity difference between Al and S is ony 0.97. These are factors that need to be taken into account when making a decision. My view is partially covalent partially ionic!
It is an ionic solid.
Transition metals are more likely to form covalent bonds because of their small size. Ionic bonds are preferred, but depending on circumstances (electronegativity differences, atomic size, etc.) they can form polar covalent bonds.
The intra and inter molecular forces will help to determine the higher boiling.Intra molecular forces are Polar/Non-polar covalent bonds and ionic bonds. Covalent bonds are stronger than ionic bonds.Polar covalent bonds will have a higher boiling point because non-polar covalent bonds are only affected by London forces.Intermolecular forces are hydrogen bonding, diapole-diapole and London. All molecules have London forces.Also the higher the electro-negativity the higher the boiling point.If all of the intra and inter molecular forces are the same, refer to the electro-negativity and size. The greater the electro-negativity and size, the higher the boiling point.
Whilst lithium is a metal and would be expected to form simple salts containing the Li+ ion- the very small size of this ion leads to it polarising the electron clouds of other ions and leading to covalent character of the bond. This is illustrated by the unusually high solubilities of Li halides in organic polar solvents. this phenomenon is explained by "fajan's rules".
The smaller size of cation (as Li+) and larger size of anion (as I-) is the main cause for the covalent character in ionic compound.
You cannot tell from a formula whether an compound is ionic or molecular. The distinction is arbitrary at best, and there are actually very few purely ionic compounds. Al2S3 will be somewhere between ionic and covalent. Depending what level you are at and wherer you are taught different classifications of aluminium sulfide are given. See link for one view. Al2S3 is a colorless high melting compound, the aluminium atoms are in tetrahedral coordination in the most stable forms. This is line with the size difference between S and Al. The electronegativity difference between Al and S is ony 0.97. These are factors that need to be taken into account when making a decision. My view is partially covalent partially ionic!
The most important distinction you have to make is that when thinking of covalent bonds, think shared electrons. When thinking of ionic bonds, think transfered electrons. Covalent bonds happen between a non-metal and a non-metal. Ionic bonds happen between a metal and a non-metal. Because a molecule may have different atoms with different sizes, electrons are shared unequally in a covalent bond. The different size atoms means that they have a different electronegitivity charge. So in a covalent bond, electrons will spend more time around one or more atoms than others. If a there is a covalent bond between two atoms with different electronegitivities, then the bond is also polar. Whether the entire molecule is polar is a different matter. Ionic bonds happen between a metal and a non-metal, which have very different electronegitivites. Usually in a ionic bond, the metal will have a low electronegitivity and the nonmetal a high electronegitivity. Because of the disparity in the charges, the non-metal will steal electrons rather than sharing them (hence transfer of electrons). Like with covalent bonds, unequal sharing of electrons causes polar charges. But a ionic bond is so much polar than a covalent bond because instead of unequal sharing there is uneqal transfering. The saying with ionic bonds in chemistry is: the bond is so polar that it's ionic.
Only the value for the covalent radius is known now: 260 pm.
silicon alwayus forms the 4 covalent bonds just like carbon. but its pi bonding is not stable due to larger atomic size....
Network solids are held together by covalent bonds to each other. They're usually very hard and have high melting points, and are also poor heat and electrical conductors. Think of diamond and graphite. These are covalent network solids. Molecular solids, on the other hand, are molecules held together by weak intermolecular forces (such as dipole-dipole, ion-dipole, or London dispersion forces). These are usually soft with low melting points, and are also poor conductors of heat and electricity. Some examples of molecular solids would be carbon dioxide and benzene. The way I think about it, to help it make more sense to me, is that in covalent network solids, each atom is BONDED to all the other atoms around it. In molecular solids, you have completely separate molecules that are just weakly held together by intermolecular forces, they're not actually bonded to each other.
Aluminum chloride is an ionic compound because aluminum is a metal and chlorine is a nonmetal. When a metal and a nonmetal are combined they make up an ionic compound. Incorrect. Aluminium Chloride is covalent.
An ionic bond is one in which electrons are gained/lost, ions are formed, and they attract, forming an ionic compound (e.g., HCl, H2SO4,Li2O) A covalent bond is one in which electrons are shared, and depending on the size of the atoms involved, could be polar (H2O) or nonpolar (N2).