positive because they shed the electron from their outer shell
Silicon is in Group 4A or 14.
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Silicon is found in group 14 of the periodic table. It has 4 valence electrons in its outer shell.
1. Carbon is a nonmetal. 2. Silicon and germanium are metalloids. 3. Tin and lead and flerovium are metals. 4. The title Group 4a is obsolete and incorrect after IUPAC rules; correct is Group 14.
There's no charge within the atom of each group since there is a same number of electrons (negatively charged) and protons ( positively charged). The charge does not change unless after ionic bonding. The atomic charge changes depending on the reaction.
Silicon is in Group 4A or 14.
4A
4A
Gorup 14 or 4A
group: 14 or IVA (not 4A) period: 2
Well, isn't that a happy little question! A Group 4A cation with 80 electrons would be Lead (Pb). Lead is a versatile element that can form different ions depending on the situation, but in this case, it would likely have a 2+ charge to balance its 80 electrons. Just imagine all those electrons peacefully coexisting in their little lead home, creating a sense of harmony and balance in the world of chemistry.
The elements in Group 4A are called the carbon group elements. This group includes carbon, silicon, germanium, tin, and lead. They share similar chemical properties such as forming covalent compounds and having multiple oxidation states.
1a 4a
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Germanium is in period 4 and group 4A or 14.
Group 4A elements have 4 valence electrons, which allows them to form strong covalent bonds by sharing electrons with other atoms. This sharing of electrons helps them achieve a full outer electron shell, making them more stable. Additionally, group 4A elements are not as electronegative as elements in other groups, making them more likely to form covalent bonds instead of ionic bonds.
Silicon belongs to Group 14 in the periodic table, also known as the Carbon Group. It has 4 valence electrons.