Yes, eg Na+ and Cl- ions produce an endless, three-dimensional matrix of salt.
Note the ions in a giant ionic structure are closely packed together
Ionic bonded always. Also giant covalent structures- like diamond and silicon dioxide. It is NOT just ionic compounds!
Yes, metallic bonds only ever form giant structures. Mercury is an exception to the rule that giant structures have high melting points.
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.
This is because they have extremely strong covalent bonds that operate in 3D and firmly hold together all the atoms in the lattice structure. Why the bonds are so strong? Probably (and don't quote me here) because the bonds are extremely stable as a result of hybridisation. Consequently, a lot of energy is required to break or even weaken these bonds, hence the exceptionally high melting and boiling points,
Indeed they can. A common example of Carbon covalently bonding with carbon is in what we refer to as Giant Covalent Structures, which are multiple of an atom bonded together in a set, lattice-like shape. Examples of giant covalent structures made from carbon are diamond where the atoms are arranged in a pyramid shape, and graphite, where they are arranged in flat layers.
Ionic bonded always. Also giant covalent structures- like diamond and silicon dioxide. It is NOT just ionic compounds!
Yes, metallic bonds only ever form giant structures. Mercury is an exception to the rule that giant structures have high melting points.
giant molecoule 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.
Yes. The nature of an ionic bond is that it is non-directional and therfore compounds form lattices rather than discrete molecules.
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.
This is because they have extremely strong covalent bonds that operate in 3D and firmly hold together all the atoms in the lattice structure. Why the bonds are so strong? Probably (and don't quote me here) because the bonds are extremely stable as a result of hybridisation. Consequently, a lot of energy is required to break or even weaken these bonds, hence the exceptionally high melting and boiling points,
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.
Giant crystalline lattices in the solid state. Metallic bonding nvolves delocalisation of electrons acoss many atoms. Note that molten metals also conduct electricity- the metallic bonds persist in the molten state.
COVALENT
Indeed they can. A common example of Carbon covalently bonding with carbon is in what we refer to as Giant Covalent Structures, which are multiple of an atom bonded together in a set, lattice-like shape. Examples of giant covalent structures made from carbon are diamond where the atoms are arranged in a pyramid shape, and graphite, where they are arranged in flat layers.
carbon in solid form, forms 4 covalent strong bonds with other carbons (giant lattice structure) these bonds require a high amount of energy to break them.