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Electrons in bonds remain localized between two atoms Electrons in bonds can become delocalized between more than two atoms?
Wiki User
∙ 12y ago
Electrons in SIGMA bonds remain localized between two atoms, Electrons in PI bonds can become delocalized between more than two atoms?
Wiki User
∙ 12y ago
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What is it called when electrons that move freely in metals?
trueThe free-moving electrons in metals account does hold many of the properties of metals. There are three properties.
Why are the valance electrons of metallic bonds different from other bonds?
In a metal the valence electrons delocalize into the conduction band, becoming an "electron gas" that fills the metal's bulk volume.In covalent bonds the valence electrons are shared between local pairs of atoms.In ionic bonds the valence electrons leave the "metal" and move to the "nonmetal" creating a pair of separate oppositely charged ions.In resonance bonds the valence electrons oscillate between being shared between two nearby local pairs of atoms.etc.To summarize in metals the valence electrons become delocalized, in other bonds the valence electrons stay local.
What is the difference between hydrogen bonds and metallic bonds?
Hydrogen bonding is a form of intermolecular force that occurs in compounds where hydrogen is bonded with a highly electronegative element such as nitrogen, oxygen, or fluorine. In such a molecule, the electronegative atom has a partial negative charge and the hydrogen a partial positive charge. The oppositely charged parts of the molecule strongly attract one another, much like the poles of a magnet. Metallic bonding occurs between atoms of a metal. The outermost electrons of the metal atoms become dislodged or "delocalized." At this point the delocalized electrons do not belong to any particular atom but are shared as a communal "electron pool." The positively charge nuclei of the atoms are all attracted to these electrons, which holds a piece of metal together.
Which electrons are responsible for current in a material?
The conduction band electrons. These are valence electrons that become delocalized in conductors and form an "electron gas" that fills the bulk of the conductor and can flow as a fluid in response to electric fields applied across the conductor.
How many electrons does sulfur gain or lose to become stable?
Sulfur gains 2 electrons to become stable.
What do delocalised valence electrons moving between nuclei do?
Delocalized valence electrons moving between nuclei become detached from their parent atom. The metal is held together by the strong forces of attraction between the delocalized electrons and positive nuclei.
What are the electrons that have high energy levels and are loose in an atom?
conduction band electrons detach themselves from atoms and become delocalized
What does the phrase delocalized electrons mean?
Delocalisation is when electrons are not associated with one atom but are spread over several atoms. So the electrons are not directly bonded with any atoms but effectively 'float' above and below the molecule in electron clouds.
What type of bonding allow elements to be hammered into different shape?
Metallic bond - common in transition metals where electrons become delocalized and move around collective positive nuclei. Thus, since electrons are allowed to slide over each other (not localized = free to move), these metals are flexible (malleable, ductile, etc)
A student asserts that silicon and germanium become good insulators at very low temperatures and good conductors at very high temperatures. Do you agree?
silicon and germanium have 4 valence electrons...they will be bound by covalent bonds at very low temperature..hence there will be no delocalized electrons to conduct electricity..therefore at low temperature these two elements behave like insulators....at high temperature,the energy will be sufficient to break the covalent bond and thus electrons become delocalized....therefore at high temp they behave like conductors
What is it called when electrons that move freely in metals?
trueThe free-moving electrons in metals account does hold many of the properties of metals. There are three properties.
Why are the valance electrons of metallic bonds different from other bonds?
In a metal the valence electrons delocalize into the conduction band, becoming an "electron gas" that fills the metal's bulk volume.In covalent bonds the valence electrons are shared between local pairs of atoms.In ionic bonds the valence electrons leave the "metal" and move to the "nonmetal" creating a pair of separate oppositely charged ions.In resonance bonds the valence electrons oscillate between being shared between two nearby local pairs of atoms.etc.To summarize in metals the valence electrons become delocalized, in other bonds the valence electrons stay local.
What is the difference between hydrogen bonds and metallic bonds?
Hydrogen bonding is a form of intermolecular force that occurs in compounds where hydrogen is bonded with a highly electronegative element such as nitrogen, oxygen, or fluorine. In such a molecule, the electronegative atom has a partial negative charge and the hydrogen a partial positive charge. The oppositely charged parts of the molecule strongly attract one another, much like the poles of a magnet. Metallic bonding occurs between atoms of a metal. The outermost electrons of the metal atoms become dislodged or "delocalized." At this point the delocalized electrons do not belong to any particular atom but are shared as a communal "electron pool." The positively charge nuclei of the atoms are all attracted to these electrons, which holds a piece of metal together.
Which electrons are responsible for current in a material?
The conduction band electrons. These are valence electrons that become delocalized in conductors and form an "electron gas" that fills the bulk of the conductor and can flow as a fluid in response to electric fields applied across the conductor.
Difference between metallic and electrolytic conduction?
Metallic conductance involves the movement of electrons throughout a metal. There are many metal atoms in a sheet of metal such as copper. The outer electrons of these atoms become delocalized (not fixed in one place). They are therefore able to move about the metallic sheet and so conduct electricity. Electrolytic conduction involves the movement of ions (charged species formed when an atom loses or gains electrons) throughout a pure liquid (for example molten NaCl) or solution such as NaCl and water. Main difference - one invloves the movement of electrons and the other involves the movement of ions.
Why are solid metals really good conductors?
Metals are made up of atoms which are joined together tightly in a the solid state. Metals are having free electrons around atoms which are the ones that carry the heat energy or electrical energy for one end to the other.
What must become weaker for the melting point to decrease down the group?
The bonds between the electrons
