0
In a ring double bonds are free to move about They do not stay localized?
Wiki User
∙ 9y ago
In a ring double bonds are free to move about. They do not stay localized. This is a property of resonance.
Wiki User
∙ 9y ago
Add your answer:
Earn +20 pts
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.
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.
Can covalents conduct elec?
Usually no. Molecular covalent bonded compounds do not conduct electricity. When the bonding is covalent and the bonds are sigma bonds the electrons are not free to move. HOWEVER. Take graphite covalently bonded and a relatively poor conductor of electricity- because of its free electrons. There are conductive organic polymers, these have free delocalised electrons.
Are protons free to drift in metals?
In metals protons are free to move btw atoms throughout the piece of metal.
How are metalic bonds different from ionic and covalent bonds?
The difference is that metallic bonds have the electrons fully delocalised, spread throughout the metal lattice and they are free to move. In ionic bonds the electrons are all localised onto the anions and cations. In covalent bonds, generally the electrons are shared and generally not delocalised although there are exceptions of course graphite is a reasonable conductor of electricity
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.
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.
Is graphite is a good conductor of electricity?
Yes it is.
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.
Can tetrachloromethane conduct electricity?
No because it forms covalent bonds and electrons are not free to move in covalent bonds. Therefore, electricity (the flow of electrons) cannot happen. - Ch
Do hydrocarbons consist of atoms linked by single or double bonds?
Yes, an aromatic hydrocarbon is a six-carbon ring with alternating single and double bonds. The cool part about an aromatic ring is that the double bonds seem to move between starting at carbons 1, 3 and 5 to starting at 2,4 and 6 then flip back. This makes the ring very stable.
What occurs when a liquid boils?
The particle bonds are broken and the particles are free to move whereever unless they hit each other
What makes solids melt?
When we heat a solid, the energy is transferred to the molecules, and to the bonds between the molecules. Eventually, the bonds become broken and the molecules become free to move about. Just as in a liquid.
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.
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.
Benzoic acid is unsaturated or saturated compound?
Benzoic acid is unsaturated because it has double- double carbon bonds and due to resonance those bonds can be easily move around , that's what makes benzoic acid unique. All compounds containing a benzene ring are actually unsaturated.
Can covalents conduct elec?
Usually no. Molecular covalent bonded compounds do not conduct electricity. When the bonding is covalent and the bonds are sigma bonds the electrons are not free to move. HOWEVER. Take graphite covalently bonded and a relatively poor conductor of electricity- because of its free electrons. There are conductive organic polymers, these have free delocalised electrons.
