Silicon gains 4 electrons.
Se will gain electrons
The silicon chip is in many devices today....ex. mp3 players. It was a major breakthrough because it allowed more technology to be stored in portable or smaller devices. Almost everything has a silicon chip..even your cell phone. Particularly the computer industry it was important to forthe same reasons. The iPad is a computer, so is the iPhone. But they wouldn't be possible without the silicon chip:)
Sorry but that question can not be answer.
Today's computers are many times smaller than DNA computers.
Silicon, its cheap and nearly ideal. Many other things have been tried, but none has really seen widespread use due to one or more difficulties that occurred. Gallium Arsenide is expensive and has mostly been limited to use in high priced supercomputers where the speed improvement justifies the cost. Diamond & graphenes & carbon nanotubes all still have process problems. Silicon-Germanium alloy has seen some use, but not so much in digital devices.
Silicon (Si) can gain or lose 4 electrons. It can either gain 4 electrons to have a stable octet configuration or lose 4 electrons to achieve a stable configuration.
Se will gain electrons
it will lose 3 electrons
Selenium may lose 2, 4 or 6 electrons and may gain 2 electrons.
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It will lose 2 electrons.
Phosphorus wants to gain three electrons to have 8 valence electrons.
5s orbital
Silicon has the atomic no. of 14 and has 4 electrons in its outermost shell. Thus,in order to make bonds it must loose or gain 4 electrons in order to achieve stable configuration but this process requires lot of energy. Therefore, silicon mostly makes bonds by sharing its electrons.
Aluminum will lose 3 electrons to form Al3+ ion.
Phosphorus can gain up to three electrons to achieve a full outer shell and form the phosphide ion (P3-), or lose up to three electrons to achieve a stable electron configuration and form the phosphorus cation (P3+).
Silicon typically gains 4 electrons to achieve a stable octet configuration. This allows it to form stable covalent bonds with neighboring atoms.