If you think to the electron configuration of magnesium this is: [Ne]3s2.
If you express your answer as a chemical equation with all forms given, you would get: Mg+(g) + e- -> Mg (g)
Helium (He) is the element that has a negative electron affinity. This means that it is less likely to gain an electron compared to other elements listed (Kr, O, Ca, and Mg) which have positive electron affinities.
na is more electropositive. it is so as electropositivity decreases from left to right across a group
Ar and Cr will not bond. Ar is a noble gas and is already in a stable electron configuration, so it does not readily bond. Cr has a half-filled d orbital, making it stable and less likely to form bonds. Mg, P, and Cl are more likely to form bonds based on their electron configurations.
The Lewis dot structure for magnesium (Mg) shows one dot representing its single valence electron, as Mg is in group 2 of the periodic table. For sulfur (S), the Lewis dot structure displays six dots, representing its six valence electrons since it is in group 16. When these two elements bond, magnesium donates its one electron to sulfur, leading to the formation of Mg²⁺ and S²⁻ ions, which can be represented as Mg²⁺ and S²⁻ in a compound like MgS.
If you express your answer as a chemical equation with all forms given, you would get: Mg+(g) + e- -> Mg (g)
A Mg atom has an equal number of protons and electrons, resulting in a neutral charge, while a Mg^2+ ion has lost two electrons, giving it a positive charge. This difference in electron configuration affects the reactivity and chemical properties of each.
An electron configuration with all electron spins paired would indicate a diamagnetic atom. For example, an electron configuration of 1s2 2s2 2p6 3s2 3p6 would be diamagnetic because all the electron spins are paired.
Mg+2 and Br-1
Helium (He) is the element that has a negative electron affinity. This means that it is less likely to gain an electron compared to other elements listed (Kr, O, Ca, and Mg) which have positive electron affinities.
The electron affinity of magnesium (Mg) is lower than that of potassium (K) because Mg is a smaller atom with a fully-filled valence shell, making it less likely to accept an additional electron. In contrast, potassium is a larger atom with an electron configuration that benefits from gaining an electron to achieve a stable inert gas configuration.
The element with the electron configuration 1s22s22p63s23p5 is fluorine (F).
Magnesium Nitride is Mg3N2. What I think you do is draw it Mg N Mg N Mg and then draw 8 electrons around each Nitrogen so that Mg shares its 2 electrons with Nitrogen and Nitrogen's Pz electron is bumped down into the Px.
Ba has a larger atomic radius than Mg because Ba has more energy levels and electrons than Mg, leading to increased electron-electron repulsion which pushes the outer electrons further apart. This results in a larger atomic radius for Ba compared to Mg.
[Ne]3s2
The electron configuration of magnesium is 1s2 2s2 2p6 3s2. Mg+ has one less electron (electrons have negative charge, so a positive charge is a lack of electrons) so you remove one from the outermost orbital: 1s2 2s2 2p6 3s1, or simply [Ne] 3s1.
The electron gain enthalpies of Mg and P are almost zero because both elements are inherently stable in their neutral state (Mg+ and P-). They have a full valence shell configuration, which makes them reluctant to gain additional electrons and become more stable. This results in low electron affinity values for both elements.