why are electrons loosely packed in metals
vishwa23:
because they have that type of nature
because they have to lose electron that's why
Answers
Answered by
1
mark me brainliest answer plsssssss
When electricity flows, the electrons
are considered "free" only because
there are more electrons than there
should be, and because the transition
metals, such as iron, copper, lead,
zinc, aluminum, gold etc. are willing
to transiently accept and give up
electrons from the d -orbitals of their
valence shell.
Transition metals are defined in part
by their stability in a wide range of
"oxidation states"; that is, in several
combinations of having too many or
too few electrons compared to
protons. This is thought to be
because of the d orbital in their
valence shells. Compared to the s and
p orbitals at a particular energy level,
electrons in the d shell are in a
relatively high energy state, and by
that token they have a relatively
"loose" connection with their parent
atom; it doesn't take much additional
energy for these electrons to be
ejected from one atom and go
zooming through the material, usually
to be captured by another atom in the
material (though it is possible for the
electron to leave the wire entirely).
This impetus can be caused by many
things, from mechanical impact to
chemical reactions to electromagnetic
radiation (aka light, though not all of
it visible); antennas work to capture
radio frequencies, because the light at
those frequencies induces an electric
current in the wire of the antenna.
Now, in the absence of a continuous
force keeping the electron in this
higher energy state, the electron (and
the metal atoms) will naturally settle
into a state of equilibrium. Electricity
is generated when just such a force is
acting on the metal, giving energy to
the electrons in the d orbital and
forcing them to move in a certain
direction.
When electricity flows, the electrons
are considered "free" only because
there are more electrons than there
should be, and because the transition
metals, such as iron, copper, lead,
zinc, aluminum, gold etc. are willing
to transiently accept and give up
electrons from the d -orbitals of their
valence shell.
Transition metals are defined in part
by their stability in a wide range of
"oxidation states"; that is, in several
combinations of having too many or
too few electrons compared to
protons. This is thought to be
because of the d orbital in their
valence shells. Compared to the s and
p orbitals at a particular energy level,
electrons in the d shell are in a
relatively high energy state, and by
that token they have a relatively
"loose" connection with their parent
atom; it doesn't take much additional
energy for these electrons to be
ejected from one atom and go
zooming through the material, usually
to be captured by another atom in the
material (though it is possible for the
electron to leave the wire entirely).
This impetus can be caused by many
things, from mechanical impact to
chemical reactions to electromagnetic
radiation (aka light, though not all of
it visible); antennas work to capture
radio frequencies, because the light at
those frequencies induces an electric
current in the wire of the antenna.
Now, in the absence of a continuous
force keeping the electron in this
higher energy state, the electron (and
the metal atoms) will naturally settle
into a state of equilibrium. Electricity
is generated when just such a force is
acting on the metal, giving energy to
the electrons in the d orbital and
forcing them to move in a certain
direction.
Answered by
3
The metals are those elements which have the property of loosing electrons to gain positive charge.Most of the metals have 1,2,3 electrons in their outermost shell.Thus the electrostatic force between the negatively charge electron and positively charged protons in the nucleus is very low.Thus the electrons are loosely packed I metals
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