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Elements in Group 14 on the Periodic Table have similar properties to carbon. These elements are carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and flerovium (Fl). Each of these elements has two electrons in the outermost p orbital, the electron configuration ns2np2, and they tend to adopt oxidation sates of +4 (+2 for the heavier elements due to the inert pair effect). Silicon is most similar to carbon.
Each has four valence electrons, but germanium will at a given temperature have more free electrons and a higher conductivity. Silicon is by far the more widely used semiconductor for electronics, partly because it can be used at much higher temperatures than germanium.
Germanium has two forms , each with a formula unit of Ge. One has a structure like diamond, the other is metallic, and only forms at very high pressure and has structure similar to the metallic form of tin.
Carbon, silicon, germanium are all teravalent atoms (4 electrons in the outer shell). Each element becomes heavier, and (because there are more total electrons) is less "pure" in it's chemical (and electrical) responses.
Similar charges will repel each other.
You will have to look it up in a databook to be certain.
Elements in Group 14 on the Periodic Table have similar properties to carbon. These elements are carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and flerovium (Fl). Each of these elements has two electrons in the outermost p orbital, the electron configuration ns2np2, and they tend to adopt oxidation sates of +4 (+2 for the heavier elements due to the inert pair effect). Silicon is most similar to carbon.
Each has four valence electrons, but germanium will at a given temperature have more free electrons and a higher conductivity. Silicon is by far the more widely used semiconductor for electronics, partly because it can be used at much higher temperatures than germanium.
Germanium has two forms , each with a formula unit of Ge. One has a structure like diamond, the other is metallic, and only forms at very high pressure and has structure similar to the metallic form of tin.
Germanium, metalloid with a similar structure to silicon- 4 covalent bonds per germanium atomPhosphorus, the most familiar form is white phosphorus which is molecular, consisting of P4 units, each P atom has 3 covalent bonds, other allotropes are not discrete molecules but all have 3 covalent bonds per P atomSelenium This is molecular in Se8 rings each Se atom has two covalent bondsChlorine this is a diatomic gas with a single covalent bond
Carbon, silicon, germanium are all teravalent atoms (4 electrons in the outer shell). Each element becomes heavier, and (because there are more total electrons) is less "pure" in it's chemical (and electrical) responses.
These elements are the metalloids: arsenic, silicon, germanium, tellurium, boron, antimony.
Yes, a prism is similar to each other.
Similar charges will repel each other.
No, each one is in a three different period from the other two!
when two similar poles are facing each other, they will push away from each other, or repel.
No they can not attract each other.