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Why do metals giant covalent structures not conduct electricity?
Metals have a sea of delocalized electrons that can move freely throughout the structure, allowing them to conduct electricity. In contrast, giant covalent structures like diamond and silicon have electrons localized in strong covalent bonds, making them insulators and unable to conduct electricity.
Do giant covalent structures contain charged ions?
No, giant covalent structures do not contain charged ions. They are formed by a network of covalent bonds between atoms, where electrons are shared between them rather than transferred to form charged ions. Examples of giant covalent structures include diamond and graphite.
What is the boiling point of giant covalent?
Giant covalent structures, such as diamond and graphite, do not have a specific boiling point because their atoms are held together by strong covalent bonds that require high temperatures to break. These structures do not boil in the traditional sense like molecular substances but rather decompose or undergo phase transitions at extremely high temperatures.
Properties of compounds with giant ionic structures?
Compounds with giant ionic structures have high melting and boiling points due to the strong electrostatic forces holding the ions together. They are usually hard and brittle solids. These compounds are good conductors of electricity when molten or in aqueous solution, but not as solids.
What do giant covalent structures look like in a gas state?
Giant covalent structures do not exist in a gas state because they have strong covalent bonds that hold their structure together. In a gas state, molecules are moving freely and not in a fixed, rigid structure like giant covalent structures, such as diamond or graphite.
Can giant covalent structures conduct electricity when molten?
Yes, giant covalent structures can conduct electricity when molten because the atoms are free to move and carry charge. This allows for the formation of a continuous pathway for the flow of electricity. Examples of giant covalent structures that can conduct electricity when molten include graphite and silicon.
Why do metals giant covalent structures not conduct electricity?
Metals have a sea of delocalized electrons that can move freely throughout the structure, allowing them to conduct electricity. In contrast, giant covalent structures like diamond and silicon have electrons localized in strong covalent bonds, making them insulators and unable to conduct electricity.
What giant covalent structure is often used in semi conductors?
Silica
Do giant covalent structures contain charged ions?
No, giant covalent structures do not contain charged ions. They are formed by a network of covalent bonds between atoms, where electrons are shared between them rather than transferred to form charged ions. Examples of giant covalent structures include diamond and graphite.
When atoms join by covalent bonds they form?
giant molecoule structures
What is the boiling point of giant covalent?
Giant covalent structures, such as diamond and graphite, do not have a specific boiling point because their atoms are held together by strong covalent bonds that require high temperatures to break. These structures do not boil in the traditional sense like molecular substances but rather decompose or undergo phase transitions at extremely high temperatures.
What is (covalent) compound?
COVALENT
Why does silicon can form giant structures?
Silicon (like carbon) can form covalent bonds, it forms a giant molecule with the diamond structure. Silicon dioxide is also a giant structure with polar covalent bonds. Silica reacts with basic oxides to form silicates- and these are generally giant structures, polar covalent bonds again, that form a very large proportion of the minerals in the earths crust.
Properties of compounds with giant ionic structures?
Compounds with giant ionic structures have high melting and boiling points due to the strong electrostatic forces holding the ions together. They are usually hard and brittle solids. These compounds are good conductors of electricity when molten or in aqueous solution, but not as solids.
What do giant covalent structures look like in a gas state?
Giant covalent structures do not exist in a gas state because they have strong covalent bonds that hold their structure together. In a gas state, molecules are moving freely and not in a fixed, rigid structure like giant covalent structures, such as diamond or graphite.
Does covalent structures have high or low boiling points?
It depends on the type of structure; simple covalent structures (like water) generally have low boiling points, while giant covalent structures (like diamond) have high boiling points.
What properties do giant covalent structures have?
A giant covalent structure is an element made with very strong bonds between the atoms too create various materials. A couple of examples are Diamond and Buckminster Fullerine. Graphite is also one but has weak bonds aswell. like...
