Sn, because it is metal
Mg is the most metallic in character among the given atoms. It is an alkali earth metal with two valence electrons, making it more likely to lose electrons and exhibit metallic properties. Silicon (Si) and Germanium (Ge) are metalloids with properties between metals and nonmetals, while Iodine (I) is a nonmetal.
Silicon (Si) and Germanium (Ge) are located in the same group (Group 14) of the periodic table, which means they have the same number of valence electrons. As a result, they exhibit similar chemical properties such as forming covalent compounds, sharing electrons, and having the ability to act as semiconductors.
Ga,Ge,Si are few examples for metalloids. They have metal and non metal properties.
Lead (Pb) is more similar to Silicon (Si) because they are both metalloids, while Germanium (Ge) is also a metalloid but has a slightly different atomic structure than Si and Pb. Lead shares more chemical properties with Silicon, such as forming covalent bonds and having similar physical properties.
The elements that are commonly recognized as metalloids or semimetals are boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), and tellurium (Te). These elements exhibit properties of both metals and nonmetals, such as being good conductors of electricity but also brittle and less malleable.
Mg is the most metallic in character among the given atoms. It is an alkali earth metal with two valence electrons, making it more likely to lose electrons and exhibit metallic properties. Silicon (Si) and Germanium (Ge) are metalloids with properties between metals and nonmetals, while Iodine (I) is a nonmetal.
Potassium (K) has a more metallic character compared to Silicon (Si). This is because potassium is an alkali metal with more metallic properties such as high electrical conductivity, luster, and malleability, while silicon is a metalloid with properties that are in between metals and nonmetals.
Silicon (Si) and Germanium (Ge) are located in the same group (Group 14) of the periodic table, which means they have the same number of valence electrons. As a result, they exhibit similar chemical properties such as forming covalent compounds, sharing electrons, and having the ability to act as semiconductors.
Ga,Ge,Si are few examples for metalloids. They have metal and non metal properties.
For Si it is 0.6or 0.7 and for Ge 0.3 or 0.2.Both values correct for both si and ge
Lead (Pb) is more similar to Silicon (Si) because they are both metalloids, while Germanium (Ge) is also a metalloid but has a slightly different atomic structure than Si and Pb. Lead shares more chemical properties with Silicon, such as forming covalent bonds and having similar physical properties.
Ge
In the 3rd row all on the left side do the elements on the right are non-metals. In the 3rd column all the elements represent metallic properties 'cause they are metals.
Si, Ge - column 4A on the periodic table
Ge has higher conductivity than Si. Because at room temperature the electron and hole mobility for Ge is larger than those of Si. Another explanation is the lower band gap of Ge than Si.
the energy required to break covalent bond in si is 1.1ev and in ge is 0.7ev
for germanium it is 0.3 and for silicon it is 0.7