Explanation of metal bonding
metal bonding
A metal bond
is a chemical bond formed by the use of electrons of valence electrons between
metal atoms. Compounds form by metal bonds are called metals (if all atoms are
equal). For example: In copper, copper atoms of twellef copper (bonded) or
alloy (if there are different atoms)
Formation of
Metal Bonding
Metals have
few valence electrons and have low electronegativity. All kinds of metals. To
generate positive ions / positive atoms / metal cations.
The outer
shell of the metal element is relatively loose (there are many empty spaces) so
the electrons are delocalized, that is a state in which the valence electrons
do not remain in their position on an atom, constantly moving from one atom to
another.
Metal valence
electrons move very quickly around the core and mingle with other valence
electrons in the bonds of the metal to hold up the "cloud" or
"oceans" that make positive ions in them. Free electrons in this
orbit as adhesives or glue. The adjacent metal cations attract each other with
the presence of free electrons as "glue".
The physical
properties of the metal
The physical
properties of the metal are determined by their strong metal bonds, dense
structures, and the contents of free electrons. Some important physical
properties of metals:
Form solids
at room temperature
The metal
atoms are joined by very strong metal bonds of tightly shaped crystalline
structures. This causes the atoms not to have freedom of movement as in the
liquid (his boss is Hg).
Hard and
flexible / not easily broken if forged
Strong metal
bonds and strong metal structures are strong, hard, and tight. Will it be. The
existence of free electrons is not restrained / not easily broken. This is due
to the presence of a stylistic metal, free electrons will move shifted positive
ions. Then, bind again with the atoms next to it. Therefore, the metal can be
forged, bent, or shaped as desired.
Has high
melting and boiling points
This happens
metal atoms bound by strong metal bonds. To overcome these bonds, energy is
needed in large numbers.
Delivers
electricity well
In metal
bonds, there are free electrons that can carry electrical charges. If given a
voltage difference, then these electrons will move from negative pole to
positive pole.
Delivers heat
well
The
free-moving electrons in the metal crystals have kinetic energy. When heated,
the electrons will produce enough kinetic energy to move rapidly. In motion,
these electrons will collide with other electrons. This causes air transfer
energy from the high-temperature part to the low-temperature part.
Has a glossy
level
In metal
bonds, there are free electrons. When light falls on a metal surface, free
electrons absorb the energy of that light. The electrons will release the
energy in the form of electromagnetic radiation with a frequency equal to the
initial light frequency. Because the frequency is the same, then we see it as a
reflection of the coming light. This light reflection provides a glossy
metallic look.
Effect of
photoelectric effect and thermionic effect
When the
electrons are free on enough metal bonds from the outside, then the electrons
can be separated from the metal. The electrons can be pulled out by a positive
potential difference. If the energy produced by free electrons comes from
light, then the phenomenon of electron discharges from metals is called the
photoelectric effect. Whereas if the energy comes from heating, it is called
the thermionic effect.
Examples of
Metal Bonding
The outer
electrons in most metals usually have a close relationship with this because
they are far from the core positive charge. All valence electrons of metals
combine to form a sea of free-moving electrons between nuclei. The free-moving
electrons act as bonds to positively charged ions. The metal bond has no direction.
As a result, the bond is not damaged when the metal is forged.Metal bonding
scheme can be seen in the picture below. The valence electrons become
dissociated with their nuclei and form an ocean of electrons.
Here is my video link about of metal bonding:
https://youtu.be/PV_S8QrZtdo
What is thermal conductivity?
BalasHapusThermal conduction is a transport phenomenon in different temperatures causing the transfer of thermal energy from one of the hot objects to the same region at a lower temperature. Heat transferred from one point to another through one of three methods of conduction, convection, and radiation.
HapusThe form of a metal bonded compound is called a metal (if all atoms are equal). So based on your statement how the characteristics of the metal bond, and give me 2 examples of metal bonds.
BalasHapusMetals or metals possess some common characters of solid form, indicating luster, high density, boiling point and high melting point, good heat or electrical conductors, strong or hard but easily formed for example malleable and ductile.
HapusExamples of bonding elements that have metal bonds are mostly metals such as Cu, Al, Au, Ag, etc. Transition metals such as Fe, Ni, etc. form a mixed bond consisting of covalent bonds (in 3d electrons) and metal bonds.
Explain the theory of ocean electrons found by Drude and Lorentz!
BalasHapusAccording to this theory in metal crystals, each atom releases its valence electrons to form a cloud of electrons and a positively charged cation and is arranged in the cloud of the electron. Positively charged metal ions are located at a certain distance from each other in the crystal. Since valence electrons are not attached to any of the metal ions or metal ion pairs, but are delocalized to all metal ions, the valence electrons are free to move all parts of the metal crystals, as well as gas molecules that can move freely within a given space .
HapusHow many valence electrons are said to bond metal?
BalasHapusValence electrons from 1 to 4
HapusWhy metal bonds can occur?
BalasHapusProcess Occurrence Metal Bond Metal has a few valence electrons and has a low electronegativity. All metals tend to release their outer electrons to form positive ions / positive atoms / metal cations. The outer shell of a relatively loose metal element (there are many empty spaces) so that the electrons are delocalized, ie a state where the valence electrons are not fixed in an atom, but constantly moving from one atom to another. In metals, the electrons that cause the bond between the metal atoms do not only become owned a pair of atoms alone, but being owned all the metal atoms , so the electrons can move freely. Metal valence electrons move very quickly around the core and mingle with other valence electrons in the metal bonds to resemble "clouds" or "oceans" that enclose the positive ions in them. The free electrons in this orbit act as glue or glue. The adjacent metal cations attract each other with the free electrons as the "glue." The metal structure can be imagined to consist of positive ions enclosed by clouds or oceans of valence electrons. Positive ions are in the middle of the "ocean" of free-moving electrons there will be a tug of attraction between the positive ions with the electrons.
Hapus