Periodic table mg molar mass'
Magnesium is 1/3rd less dense than aluminium. To extract the Mg, firstly, calcium hydroxide (Ca(OH) 2 ) is added to seawater to form magnesium hydroxide precipitate:īrucite (Magnesium hydroxide, Mg(OH) 2 ) is insoluble in water, can be filtered out and reacted with hydrochloric acid (HCl) to produced concentrated magnesium chloride (MgCl 2 ):įinaly, magnesium produces by electrolysis of magnesium chloride (MgCl 2).įirst Isolation: Humphry Davy (1808) Magnesium Uses Mg (II) is precipitated by hydroxide ions (OH-), and Ammonia (NH 3) will also precipitate Mg (II) as hydroxide, but the precipitation is incomplete: The metal dissolves readily in acids, and forming Mg (II) ions & Hydrogen: Metal Reacts with Cl 2, and forming magnesium chloride: Mg does not react with liquid water at room temperature, but It reacts steam, and forming magnesium hydroxide (Mg(OH) 2), with excess steam & hydrogen gas: The metal reacts with oxygen at room temperature, and forming a passivating layer of MgO, and when Mg ignited, then it reacts with both oxygen & nitrogen forming a mixture of magnesium oxide & Magnesium nitride (Mg 3 N 2 ): Hexagonal Close Packed (HCP) Reactivity of Magnesium Ionization energies: 1st: 737.6 kJ.mol 2nd: 1450.6 kJ/mol 3rd: 7732.6 kJ/molĬrystal structure: Hexagonal close packed The ionization potential of an atom: 7.61 Molar magnetic susceptibility: 0.168×10 -9 m 3/molĭensity: 1.737 g/cm 3 (In solid) 1.585 g/cm 3 (In Liquid at M.P) Mass magnetic susceptibility: 6.9×10 -9 m 3/kg Magnetic susceptibility (x mol): +13.1×10 -6 cm 3/mol Magnesium Electron Configuration Thermal Properties of Magnesiumĭebye temperature: 318 K (44.85 oC, 112.73 oF) World’s Top 3 Reserve holders of Magnesium.Note: Although Na 2CO 3 is an ionic compound and sodium is present in an ionic form, it is a habitual way of referring to an element in these types of calculations. This is the accurate way of rounding off to the correct number of significant figures in multistep calculations. I do it here mainly to save space, but you can keep the numbers in the calculator and round them off at the end. The little inconsistency in the final answer is due to rounding off the intermediate numbers. So, to calculate the moles from a given mass, we make a conversion factor correlating 1 mole with the molar of the given component.įor example, how many moles of sulfur are there in a 16.2 g sample? The molar mass, on the other hand, is a constant number for a given atom or a molecule as it is for a specific amount of it. The given mass is the mass of the sample, and it can be any number, for example, we can have 10 g of salt, 15 g, or 100 g. To calculate the moles from a given mass (m), the molar mass of the component is used. The molecular mass of water is 18.0 amu, and the molar mass is 18.0 g/mol.įor the molar mass, keeping one decimal is usually an acceptable approximation, and for the Avogadro’s number, you can use 6.02 x 10 23. Numerically, the molar mass is equal to the atomic mass of a given atom or a molecule, so we can look up the molar mass of an element in the periodic table.įor example, we can say that the mass of Cu is 63.55 amu or 63.55 g/mol. The mass of one mole of atoms/molecules/ions is called its molar mass (M) expressed in g/mol. One mole of any element contains 6.022 x 10 23 of its atoms, and a mole of a compound contains 6.022 x 10 23 molecules, ions-ions, and in general, 1 mol = 6.022 x 10 23 particles. This is called Avogadro’s number ( N A = 6.022 x 10 23). By definition, a mole is the number of atoms in a 12-g sample of 12C isotope which happens to be 6.022 x 10 23 atoms. The mole is just a number like a dozen, a hundred, or a million.