A solid melts when the available energy in heat exceeds the energy required to break up the solid, which is equal to the extra energy gained by letting the atoms stay always close to one another rather than passing only occasionally near like ships
in the night. The simplest model of metals treats the valence electrons as
a gas around charged cores composed of the atoms minus their valence
electrons. Zn, Cd and Hg all have the same number of valence electrons (2)
and hence the same charge on their cores, *but* the volume each valence
electron has to move around in increases from 8 to 11 to 12 in units of
10^-24 cm^3, that is the gas of valence electrons becomes less dense. When
it is less dense, the electrons interact (favorably) with the oppositely
charged cores less often, so the extra energy gained by having cores and
electrons all close together is less, hence the extra energy of the solid
is less, hence the melting point lower. Why should the valence electron
gas get less dense? Not an easy question to answer, the density is a
delicate competition between the desire of all the electrons to get close
to the cores and their mutual repulsion. Since the Hg core is bigger (it
has more non-valence electrons in it) the electrons are squeezed anyway in
Hg by the core hogging more space, so you might guess the preferred density
might end up a little lower, as it does. This is simply because Mercury has a very low melting point (-38.83°C/234.32K), meaning it is only a solid when it gets cold enough.
Mercury has completely filled d10 electronic configuration. hence the extent of metallic bond formation is less as the orbitals are completely filled. due to weak interatomic forces of attraction, Hg exists as a liquid at room temperature
A solid melts when the available energy in heat exceeds the energy required to break up the solid, which is equal to the extra energy gained by letting the atoms stay always close to one another rather than passing only occasionally near like ships
in the night. The simplest model of metals treats the valence electrons as
a gas around charged cores composed of the atoms minus their valence
electrons. Zn, Cd and Hg all have the same number of valence electrons (2)
and hence the same charge on their cores, *but* the volume each valence
electron has to move around in increases from 8 to 11 to 12 in units of
10^-24 cm^3, that is the gas of valence electrons becomes less dense. When
it is less dense, the electrons interact (favorably) with the oppositely
charged cores less often, so the extra energy gained by having cores and
electrons all close together is less, hence the extra energy of the solid
is less, hence the melting point lower. Why should the valence electron
gas get less dense? Not an easy question to answer, the density is a
delicate competition between the desire of all the electrons to get close
to the cores and their mutual repulsion. Since the Hg core is bigger (it
has more non-valence electrons in it) the electrons are squeezed anyway in
Hg by the core hogging more space, so you might guess the preferred density
might end up a little lower, as it does. This is simply because mercury has a very low melting point (-38.83°C/234.32K), meaning it is only a solid when it gets cold enough.
The first ionization potential value for mercury is very high (partially because of "lanthanide contraction" (mercury is not itself a lanthanoid, but the contraction applies to all elements following lanthanum), but mainly because the 6s electrons in mercury are relativistic, increasing their mass which reduces their average distance from the nucleus which in turn results in an unusually strong attraction to the positively charged nucleus). This makes the metallic bond in mercury weak compared to other metals as the electrons are not as readily delocalizable, and weaker bonding leads to a lower melting point.
Mercury. is the only metal that is liquid at room temperature.
The metallic element Mercury (symbol Hg) is a liquid at standard temperature and pressure, The only other element which is also a liquid under these conditions is the halogen Bromine (symbol Br).
its a metal richardMercury is a liquid metal at room temperature .
There are two elements which are liquid at room temperature and they are Mercury (Hg) and Bromine (Br). Copernicium (Cn) might be liquid at room temperature but chemists are not sure about it.
Mercury
mercury is a liquid at room temperatute At room temperature, mercury is a LIQUID.
Mercury. is the only metal that is liquid at room temperature.
Mercury is a liquid at room temperature.
Mercury is a liquid at room temperature
Mercury is the metal that is liquid at room temperature
Mercury is the only metal to be liquid at room temperature.
Metals are typically solid at room temperature, although mercury is a liquid.
Mercury is a metal element which is liquid at room temperature
The metallic element Mercury (symbol Hg) is a liquid at standard temperature and pressure, The only other element which is also a liquid under these conditions is the halogen Bromine (symbol Br).
Mercury (Hg) is liquid at room temperature.
Mercury (Hg) is the only metal that exists as a liquid at room temperature.
Mercury and bromine are the only two elements liquid at room temperature.