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[23] [24] [25] It forms crystals of the AlCl 3 type, with monoclinic crystals and the point group C2/m. [26] Erbium(III) chloride hexahydrate also forms monoclinic crystals with the point group of P2/n (P2/c) - C 4 2h. In this compound, erbium is octa-coordinated to form [Er(H 2 O) 6 Cl 2] + ions with the isolated Cl − completing the ...
Magnesium nitrate reacts with alkali metal hydroxide to form the corresponding nitrate: Mg(NO 3) 2 + 2 NaOH → Mg(OH) 2 + 2 NaNO 3.. Since magnesium nitrate has a high affinity for water, heating the hexahydrate does not result in the dehydration of the salt, but rather its decomposition into magnesium oxide, oxygen, and nitrogen oxides:
CaC 2 + 2H 2 O → Ca(OH) 2 + C 2 H 2 Mg 2 C 3 + 4H 2 O → 2Mg(OH) 2 + C 3 H 4. Reaction with nitrogen. Only Be and Mg form nitrides directly. 3Be + N 2 → Be 3 N 2 3Mg + N 2 → Mg 3 N 2. Reaction with hydrogen. Alkaline earth metals react with hydrogen to generate saline hydride that are unstable in water. Ca + H 2 → CaH 2. Reaction with ...
Electron affinity can be defined in two equivalent ways. First, as the energy that is released by adding an electron to an isolated gaseous atom. The second (reverse) definition is that electron affinity is the energy required to remove an electron from a singly charged gaseous negative ion.
Gadolinium isotopes have four metastable isomers, with the most stable being 143m Gd (t 1/2 = 110 seconds), 145m Gd (t 1/2 = 85 seconds) and 141m Gd (t 1/2 = 24.5 seconds). The isotopes with atomic masses lower than the most abundant stable isotope, 158 Gd, primarily decay by electron capture to isotopes of europium .
Although dibromine is a strong oxidising agent with a high first ionisation energy, very strong oxidisers such as peroxydisulfuryl fluoride (S 2 O 6 F 2) can oxidise it to form the cherry-red Br + 2 cation. A few other bromine cations are known, namely the brown Br + 3 and dark brown Br + 5. [8] The tribromide anion, Br −
See also: Electronegativities of the elements (data page) There are no reliable sources for Pm, Eu and Yb other than the range of 1.1–1.2; see Pauling, Linus (1960).
The mass number (symbol A, from the German word: Atomgewicht, "atomic weight"), [1] also called atomic mass number or nucleon number, is the total number of protons and neutrons (together known as nucleons) in an atomic nucleus. It is approximately equal to the atomic (also known as isotopic) mass of the atom expressed in atomic mass units.