The family of 'noble' (= inert) gasses in group (column) 18 of the Periodic Table. Their valence shell is completely filled up with s2 and p6 electrons.
False. Alkali metals lose one electron to form a stable electron configuration with a full outer shell of electrons, which is the stable electron configuration for these elements.
A duplet electron configuration is considered stable, as it corresponds to having two electrons in the outer energy level, which is the most stable configuration for elements in the first period. Elements like helium achieve a duplet electron configuration and are relatively stable due to their full outermost energy level.
Yes, that's correct. Noble gases have full valence electron shells, meaning they have achieved the most stable electron configuration. This stable configuration makes them chemically inert and less likely to form chemical bonds with other elements.
Potassium can lose one electron from its outer shell to achieve a stable electron configuration similar to argon. Fluorine can gain one electron to fill its outer shell and attain a stable electron configuration like neon. In both cases, the atoms are trying to achieve a full valence shell and become stable like the nearest noble gas.
The electron configuration of Cu+1 is [Ar] 3d10 4s1. When copper loses one electron to become a +1 ion, it loses the 4s electron first, followed by one of the 3d electrons to attain a stable electron configuration.
The electron configuration of copper is: [Ar]4s13d10. It isn't 4s23d9 because Cu is able to obtain a more stable electron configuration when it takes an electron from the 4s and adds it to 3d. A half filled 4s and a completely filled 3d is more stable.
Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.
What symbol would represent a chlorine ion that has ionized to have a stable electron 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. 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.
The group of elements that have a stable electron configuration are the noble gases.
False. Alkali metals lose one electron to form a stable electron configuration with a full outer shell of electrons, which is the stable electron configuration for these elements.
The noble gas configuration for fermium (Fm) is [Rn] 5f12 7s2. It represents the electron configuration of fermium in a stable state, where it mimics the electron arrangement of the noble gas radon (Rn) to achieve a more stable configuration.
A duplet electron configuration is considered stable, as it corresponds to having two electrons in the outer energy level, which is the most stable configuration for elements in the first period. Elements like helium achieve a duplet electron configuration and are relatively stable due to their full outermost energy level.
The electron configuration of boron is 1s2 2s2 2p1. When boron becomes an ion, it typically loses its outer electron to achieve a stable electron configuration. Therefore, the electron configuration of a boron ion is typically 1s2 2s2.
Yes, that's correct. Noble gases have full valence electron shells, meaning they have achieved the most stable electron configuration. This stable configuration makes them chemically inert and less likely to form chemical bonds with other elements.
A stable electron configuration for a chlorine ion can be achieved by gaining one electron. This would give the chlorine ion a full outer shell of electrons. The symbol for a stable chlorine ion with an extra electron would be Cl-.
The most stable oxidation state of francium is +1. Francium readily loses its single valence electron to attain a stable electron configuration similar to the noble gas configuration of cesium.