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What properties make a functional group or hydrocarbon a good conductor of electricity?
Functional groups or hydrocarbons with delocalized electrons, such as aromatic rings in benzene or double bonds in alkenes, can act as good conductors of electricity because the electrons are free to move and carry an electric charge. In contrast, functional groups with fully saturated bonds do not conduct electricity well because the electrons are localized and not free to move.
Do giant covalent bonds conduct electricity when solid?
No, because the molecules are neutral so therefore there are no charged particles to carry a current.
Are electrons in non-polar covalent molecules localised or delocalised amd mobile?
Either one is possible. In benzene, the twelve electrons in the six carbon-hydrogen bonds are localized and the remainder of the electrons are delocalized and can move freely around the benzene ring.
Why are metallic bonds called non directional bonds?
Metallic bonds are called non-directional because the electrons in a metallic bond are free to move throughout the entire structure rather than being localized between two specific atoms. This allows for the strong bonding between metal atoms in all directions, resulting in the characteristic properties of metals such as malleability and ductility.
Why graphite conduct eletricity as it has covant bond?
Graphite can conduct electricity due to the presence of delocalized electrons within its structure. These free electrons are able to move freely between the layers of carbon atoms in graphite, allowing for the conduction of electricity. Despite having covalent bonds within each layer, the delocalized electrons are not localized to any specific bond and are free to move.
What properties make a functional group or hydrocarbon a good conductor of electricity?
Functional groups or hydrocarbons with delocalized electrons, such as aromatic rings in benzene or double bonds in alkenes, can act as good conductors of electricity because the electrons are free to move and carry an electric charge. In contrast, functional groups with fully saturated bonds do not conduct electricity well because the electrons are localized and not free to move.
Do giant covalent bonds conduct electricity when solid?
No, because the molecules are neutral so therefore there are no charged particles to carry a current.
Are electrons in non-polar covalent molecules localised or delocalised amd mobile?
Either one is possible. In benzene, the twelve electrons in the six carbon-hydrogen bonds are localized and the remainder of the electrons are delocalized and can move freely around the benzene ring.
Why are metallic bonds called non directional bonds?
Metallic bonds are called non-directional because the electrons in a metallic bond are free to move throughout the entire structure rather than being localized between two specific atoms. This allows for the strong bonding between metal atoms in all directions, resulting in the characteristic properties of metals such as malleability and ductility.
Why graphite conduct eletricity as it has covant bond?
Graphite can conduct electricity due to the presence of delocalized electrons within its structure. These free electrons are able to move freely between the layers of carbon atoms in graphite, allowing for the conduction of electricity. Despite having covalent bonds within each layer, the delocalized electrons are not localized to any specific bond and are free to move.
Which type of bond occurs between atoms in which the electrons are able to move around?
Metallic bonds and delocalised covalent bonds. Electrons move around in all types of bonds, its a question of degree. In straightforward covalent bonds with an electron pair- the electron moves in a small volume along the bond axis. In delocalised covalent bonds such as that in sheet graphene electrons are free to move along the plane. In metallic bonds electrons are free to move around the lattice. This ability to move is associated with electrical conductivity.
Is graphite is a good conductor of electricity?
Yes it is.
How are metallic bonds different to covalent bonds?
Metallic bonds are bonds between metals. They consist of valence electrons in delocalized bonds covering the whole crystal. These electrons can move freely and are responsible for the special properties of metals such as electrical conductivity. Covalent bonds are electrons being shared and are usually between non-metals. They are localized to the atoms which are sharing them, resulting in individual molecules.
What happens to electrons when bonds are formed?
They disappear... Nothing in this world dies out and disappears. Everything goes from one form of energy to another form. when electrons bond, they form, if I'm correct, a covalent bond.
Why graphite conduct electricity and diamond not?
In graphite,the bonds are often depicted as alternating single and double bonds. This is not quite accurate as the bonds are actually somewhat in between these two structures. This means that in the case of graphite the electrons are delocalized throughout the entire structure, and are free to move to produce an electric current. In diamond all the bonds are single bonds, so the electrons must stay in essentially the same area. This makes them nearly impossible to move without destroying the structure of the diamond.
Why are the valence electrons found in metallic bonds different from other bonds because of what?
their valence electrons are free-roaming they allow for the conductivity of electricity APEX :) <3 JAmie
You will notice there are several double bonds contained in a phospholipid What is a double bond and how does it relate to electron activity?
Since there are double bonds contained in phospholipid, the double bond in a phospholipid a covalent bond and there fore the atoms and the particles, the electrons move together in units. This relates to electron activity because when the electrons move fritfully in side way units, as well as vertically and horizontally like in parabola, the electron activity is very harsh and it creates a double double bond. This double double bond, known as a superior covalent vena cava, relates to the electrons. This is why there is a double bond in phospholipid.
