any time there are as many electrons and protons and they fill each orbital optimally.
The noble gases have stable electron configurations.
1s22s2, [He]2s2, 2-2
The nuclear structure is more important because the nuclei of actinides are unstable and spontaneously break apart
when a neutral atom loses an electron it becomes a positive ion. it now has a stable outer most shell.
A hydrogen atom is only a proton and an electron. Beyond that the neutron seems to keep the nucleus together and stable. Maybe a better question is, "What is the difference between a hydrogen atom without an electron and a proton?"
Molybdenum's electon configuration is [Kr] 5s1 4d5 this is because all elements want to be half-full or full. so the 2nd electron in the 5s2 moves to make the 4d4 complete so it turns to 5s1 4d5....making Mo half-full and stable.
Yes. Helium, Xenon, and Neon have stable electron numbers (octette rule).
6
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.
electrons
protons
completely filled valence shells
flourine must gain one electron
Many atoms have electron configurations that are unstable. By sharing electrons with one or more other atoms, new, more stable electron configurations form.
Solutions are mixtures of one or more solutes dissolved in a solvent. They do not have electron configurations. Only atoms and ions have electron configurations.
The most stable number of valence electrons is 2 for hydrogen and helium, which have only one electron shell in the shell model for atomic electron configurations, and 8 for all other elements.
filled energy sublevels
All of the representative elements (s and p block) have predictable electron configurations. However, many of the transition elements have electron configurations that are not predicted by the rules for determining electron configuration.