For sodium to become stable, it must lose one electron to achieve a full outer electron shell. This typically occurs through the formation of an ionic bond with another atom that can accept this extra electron, such as chlorine. Once sodium loses its electron and forms a stable bond, it becomes a stable compound.
Sodium is a highly reactive metal and is not considered durable in its pure form. It readily reacts with water and air, leading to its degradation. Special precautions must be taken to handle and store sodium due to its reactivity.
Oxygen must bond twice to become stable. In its stable form, oxygen molecules have a double bond (O=O), with each oxygen atom sharing two electrons.
It keeps its neutrons but loses one electron. Protons and neutrons do not move in a chemical reaction. Sodium, being in group one, must lose one electron to have a complete outer electron shell and thus be stable.
Sodium must lose one electron to achieve a stable octet configuration since it has 11 protons and would complete its outer shell to achieve the stable electron configuration of the nearest noble gas, neon, with 10 electrons.
For fluorine to become stable, it needs to gain one electron to attain a full valence shell, similar to the electron configuration of neon. Fluorine has seven valence electrons in its outer shell, so gaining one electron would fill its outer shell and make it stable with a full octet like neon.
Nothing. Krypton is already just about as stable as it's possible for an element to get.
For potassium to become stable, it must have a full outer electron shell, typically with eight electrons (like a noble gas). This can be achieved by losing one electron to become a positively charged ion, as potassium tends to do in chemical reactions.
Beryllium is a stable element.
Fluorine becomes stable when it gains one electron to achieve a full outer shell of electrons, containing 8 electrons in total. This allows fluorine to attain a stable electron configuration similar to that of a noble gas.
Sodium is a highly reactive metal and is not considered durable in its pure form. It readily reacts with water and air, leading to its degradation. Special precautions must be taken to handle and store sodium due to its reactivity.
Oxygen must bond twice to become stable. In its stable form, oxygen molecules have a double bond (O=O), with each oxygen atom sharing two electrons.
It keeps its neutrons but loses one electron. Protons and neutrons do not move in a chemical reaction. Sodium, being in group one, must lose one electron to have a complete outer electron shell and thus be stable.
A neutral sodium atom must lose one electron to have the electron configuration of neon, which has a stable electron configuration with a full outer shell. Sodium typically forms a +1 cation by losing this one electron to achieve a stable configuration like neon.
It must melt.
Sodium must lose one electron to achieve a stable octet configuration since it has 11 protons and would complete its outer shell to achieve the stable electron configuration of the nearest noble gas, neon, with 10 electrons.
The Hypothesis Must Be Supported In Order For It To Become A Theory
For fluorine to become stable, it needs to gain one electron to attain a full valence shell, similar to the electron configuration of neon. Fluorine has seven valence electrons in its outer shell, so gaining one electron would fill its outer shell and make it stable with a full octet like neon.