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The melting point of MGO is higher than that of NAF because the former has more ionic bonds than the latter.
Ionic compounds have higher melting and boiling points, and the ionic crystal melting process of ionic compounds needs to break the ionic bonds, so the melting point of ionic compounds is related to the number of ionic bonds, so the more ionic bonds, the higher the melting point.
At the same time, if the structure is similar and in the ionic crystal with the same number of ions in the chemical formula, the ionic radius is small, and the charge of the ions in the chemical formula is large, the bond energy will be stronger, and the boiling point and melting point will be higher.
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The melting process of ionic crystals requires the destruction of ionic bonds, so the melting point is determined by the strength of ionic bonds. In an ionic crystal with a similar structure and the same number of ions in the chemical formula, the smaller the ionic radius (or the smaller the sum of the anion and cation radius), the greater the charge of the ion, and the higher the melting and boiling point of the stronger the bond energy.
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Magnesium ions and oxygen ions each have a formal charge of two units, and sodium ions and fluoride ions each have a formal charge of one unit. Therefore, the ionic bond in MGO is strong (strictly speaking, it should be the lattice energy of MGO).
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They are both ionic crystals, and the melting and boiling point of ionic crystals is related to the number of charges carried by the ions and the bond length of the ionic bond, the bond length is related to the atomic radius, the smaller the atomic radius, the greater the bond length. As you can see from the periodic table, Mg and O have larger atomic radii than both Na and F, so the melting point of Mgo is higher than that of Naf.
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Ionic compounds have high melting and boiling points, which is related to the large lattice energy of their ionic crystals. The melting point of MGO (2800) is much higher than that of NAF (988) due to Umgo UNAF.
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Because the number of MGO charges is large, the ionic bond is strong, so the melting point is high.
MGO two.
naf one.
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Force: MGO>BAS; Melting Point: MGO>BAS
Because they are ionic crystals, the smaller the ionic radius, the greater the inter-ion force, i.e., the greater the lattice energy. The greater the lattice energy, the higher the melting point of the ionic crystal.
Ionic radius: r(mg2+).
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1. Magnesium oxide is composed of divalent ions, while sodium chloride is composed of monovalent ions; 2. The radius of magnesium ions and sodium ions is about the same, but the radius of oxygen ions is smaller than that of sodium ions, so the ions in magnesium oxide can be closer to each other. In summary, magnesium oxide has stronger ionic bonds and is therefore less prone to liquefaction and gasification than sodium chloride.
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MGO has a high melting point compared to NaCl, the former has a high charge and a large lattice energy.
The factors that determine the lattice energy are, in order:
Ionic charge. Ionic radius.
Electron shell configuration of an ion.
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