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How does ionic bonding in compounds determine high MP high BP being brittle and have high electrical conductivity?
Ionic bonding in compounds results from the electrostatic attraction between positively and negatively charged ions, leading to a strong, rigid lattice structure. This strong bonding contributes to high melting and boiling points, as significant energy is required to break these interactions. Additionally, while ionic compounds are generally brittle due to the alignment of ions in the lattice, when stressed, similar charges can align and repel each other, causing the structure to shatter. Ionic compounds conduct electricity when dissolved in water or melted, as the ions become free to move and carry an electric current.
What else can I help you with?
Do molecular compound has high electrical conductivity?
Some are, but not usually. They are typically insulators (exceptions are large polymers with conjugated bonding, but these are quite unique and not commonly found).
Bonding between elements in middle of periodic table tend to bewhat kind of chemical bonding?
Bonding between elements in the middle of the periodic table tend to be metallic bonding. In metallic bonding, outer electrons are delocalized and free to move, creating a "sea of electrons" that holds the metal ions together. This leads to properties such as high electrical and thermal conductivity in metals.
Does metallic bonding involve free-floating electrons?
Yes, metallic bonding involves free-floating electrons that are delocalized and are able to move freely throughout the metal structure. These mobile electrons are responsible for many properties of metals, such as electrical conductivity and malleability.
What is responsible for the good electrical conductivity of metals?
The good electrical conductivity of metals is due to their loosely held electrons, which are free to move throughout the metal structure when a voltage is applied. This movement of electrons allows for the flow of electric current with little resistance.
Compounds of unequal distribution of bonding electrons are said to be?
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What are the advantages and limitations of metallic bonding?
Advantages of metallic bonding include high thermal and electrical conductivity, malleability, and ductility. Limitations include lower melting and boiling points compared to ionic compounds, and weakened bonding in alloys due to the presence of different metal atoms.
Is responsible for the good electrical conductivity of metals?
The metallic bonding which is basically a "sea" or cloud of electrons.
Which type of bonding is characteristic of a substance that has a high melting point and electrical conductivity only in the liquid phase?
The substance would likely exhibit metallic bonding. Metallic bonding is responsible for high melting points due to strong bonding between metal atoms. Electrical conductivity in the liquid phase occurs because the metal atoms are mobile and able to carry electrical charges.
How could you test an unknown compound to determine if it was ionic or covalent?
One way to test the compound is to measure its conductivity in solution. Ionic compounds typically conduct electricity in solution due to the presence of free ions, while covalent compounds do not conduct. Additionally, analyzing the compound's physical properties like melting point and solubility in water can also provide clues about its bonding nature. Finally, conducting a chemical reaction with known ionic and covalent compounds and observing the reaction products can help determine the type of bonding in the unknown compound.
Is there Exceptions for low conductivity in covalent bonding?
Yes. Graphite is covalently bonded but is moderately conductive, as are some poly-aromatic compounds.
Is aluminium ionic covalent or metalic bonding?
Aluminium typically displays metallic bonding due to its structure, where the outer electrons are delocalized across the metal lattice, leading to good electrical and thermal conductivity. However, in certain compounds such as aluminium oxide (Al2O3), it exhibits predominantly ionic bonding due to the transfer of electrons between aluminium and oxygen atoms.
Why conductivity of diamond is highest being a nonmetal?
It would help if you specify whether you are talking about thermal conductivity, or electrical conductivity. Diamond certainly doesn't has the highest electrical conductivity. Its thermal conductivity is one of the highest known, and - if a synthetic diamond is made from pure (99.9%) C-12, it is indeed the highest. The Wikipedia article attributes this to a strong covalent bonding.
What type of chemical bonding is in solid copper?
Metal or atomic bonding: electrons are not shared but pooled together in the "conductivity sea" of electrons
Is Fe a covalent ionic or metallic bond?
Fe forms metallic bonds. In its solid state, iron (Fe) atoms share electrons with each other to create a sea of delocalized electrons, leading to its characteristic metallic properties such as high electrical conductivity and malleability.
Is metallic bonding metals or nonmetals?
Metallic bonding occurs in metals, not in nonmetals. It is characterized by the delocalization of electrons throughout a lattice of metal atoms, leading to high electrical and thermal conductivity, as well as malleability and ductility. Nonmetals typically form covalent or ionic bonds.
Do molecular compound has high electrical conductivity?
Some are, but not usually. They are typically insulators (exceptions are large polymers with conjugated bonding, but these are quite unique and not commonly found).
How can bonding determine the properties of a compound?
The type of bonding in a compound (ionic, covalent, metallic) affects properties such as melting point, conductivity, and solubility. For example, compounds with ionic bonds tend to have high melting points and conduct electricity when dissolved in water, while covalent compounds tend to have lower melting points and may not conduct electricity. The strength and nature of the bonds between atoms influence the overall properties of the compound.
