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what type of bonds form lattice structures?
Ionic bonded always. Also giant covalent structures- like diamond and silicon dioxide. It is NOT just ionic compounds!
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.
Is water a giant covalent structure?
No, water is not a giant covalent structure. Water molecules are held together by hydrogen bonds, which are much weaker than the covalent bonds typically found in giant covalent structures like diamond or graphite.
Is mercury has giant structure?
Yes, metallic bonds only ever form giant structures. Mercury is an exception to the rule that giant structures have high melting points.
What is a giant covalent lattice?
Giant covalent, lattice structures contain a lot of non-metal atoms, each joined to adjacent atoms by covalent bonds. The atoms are usually arranged into giant regular lattices. The structure requires an element with very strong bonds between the atoms to create various materials. A couple of examples are (carbon) Diamond and Buckminster Fullerine. Graphite is also one but has weak bonds as well. Silica and molybdenum can also make covalent lattice structures.
When atoms join by covalent bonds they form?
giant molecoule structures
what type of bonds form lattice structures?
Ionic bonded always. Also giant covalent structures- like diamond and silicon dioxide. It is NOT just ionic compounds!
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.
Why are giant covalent structures non conductors of electricity?
Because the electrons are fixed their given bond, and are NOT free to move. When electrons are free to move within a substance then it is conducting electricity. In Diamond , electrons are not free to move. ], because each carbon atom creates four single covalent bonds , with each of its four neighbour carbon atoms, in an Adamantine Structure. However, in Graphite, each carbon atom creates three bonds with neighbour carbon atoms. This leaves a 'spare' electron that can move. Hence graphite conducts electricity,; as in carbon brushes in electrical motors. Diamond and Graphite are two of the three allotropes of carbon. One conducts electricity , but the other resists conduction.
Do ionic bonds always produce giant ionic lattices?
Yes. The nature of an ionic bond is that it is non-directional and therfore compounds form lattices rather than discrete molecules.
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 difference between molecular structures and giant structures?
Molecular structure - just a few atoms bonded together, weak intermolecular forcesGiant molecular structure - covalent bonds, each atom forms a few bonds so there are lots of atoms in each molecule, strong forces between atoms.
Is water a giant covalent structure?
No, water is not a giant covalent structure. Water molecules are held together by hydrogen bonds, which are much weaker than the covalent bonds typically found in giant covalent structures like diamond or graphite.
Is mercury has giant structure?
Yes, metallic bonds only ever form giant structures. Mercury is an exception to the rule that giant structures have high melting points.
What is a giant covalent lattice?
Giant covalent, lattice structures contain a lot of non-metal atoms, each joined to adjacent atoms by covalent bonds. The atoms are usually arranged into giant regular lattices. The structure requires an element with very strong bonds between the atoms to create various materials. A couple of examples are (carbon) Diamond and Buckminster Fullerine. Graphite is also one but has weak bonds as well. Silica and molybdenum can also make covalent lattice structures.
Do substances that usually contain covalent bonds have a giant or simple molecular structure?
Substances that usually contain covalent bonds have a simple molecular structure. Examples include elements like oxygen and compounds like methane. Giant molecular structures are typically found in substances with strong covalent bonds, such as diamond and quartz.
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.
