The atomic number of the element Radium (Ra) is 88. It is an alkaline earth metal. Electronic configuration of Radium (Ra) will be ![[Rn]7s^{2}](https://tex.z-dn.net/?f=%5BRn%5D7s%5E%7B2%7D)
It belongs to the group IIA of the periodic table. Alkaline earth metals that belong to the group IIA of the periodic table lose the valence electrons to form a +2 ion.
Therefore, Radium with an electronic configuration of will lose the two 7s electrons to form the cation with +2 charge.
The substance would be sodium nitrate, to figure this out all you need to do is read each sentence carefully and see if whatever the lab technician notices happening to the substance does it match with any of the substances listed in the table, if it does not match, any one description we can eliminate that compound as a choice. Carry this method of elimination basically until you come to the last sentence. Since the substance melts at temperature above the melting point, it can't be potassium chromate as it would change state at a temperature of 974 degrees Celsius, not high of temperature for the change, as the oven is at 450 degrees Celsius only.
<span>Alkaline Earths hope this helps
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Answer: It will be produced 276,3 mg of product
Explanation: The reaction of anthracene (C14H10) and maleic anhydride (C4H2O3) produce a compound named 9,10-dihydroanthracene-9,10-α,β-succinic anhydride (C18H12O3), as described below:
C14H10 + C4H2O3 → C18H12O3
The reaction is already balanced, which means to produce 1 mol of C18H12O3 is necessary 1 mol of anthracene and 1 mol of maleic anhydride.
1 mol of C14H10 equals 178,23 g. As it is used 180 mg of that reagent, we have 0,001 mol of anthracene. With it, the reaction produces 0,001 mol of C18H12O3.
As 1 mol of C18H12O3 equals 276,3 g, the mass produced is 276,3 mg.
