Question
(c) Calculate the relative formula mass (M_(r)) of magnesium fluoride (MgF_(2)) Relative atomic masses (A_(r)):F=19 Mg=24 Relative formula mass (M_(r))= __ (d)Argon is a noble gas. Explain why no product is formed when magnesium and argon are heated together. __
Answer
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Glynis
Master · Tutor for 5 years
Answer
(c) The relative formula mass (Mr) of magnesium fluoride is 24+19x2= 62(d) No compound is formed when magnesium is heated together with argon because argon is a noble gas with a stable electronic configuration. Hence, it does not react and no product is produced.
Explanation
This question includes two parts:(c) In part (c), the question asks to calculate the relative formula mass (Mr) of magnesium fluoride (MgF2). The relative formula mass (Mr) of a molecule is the sum of the relative atomic masses (Ar) of the atoms in a molecular compound as listed in the periodic table.(d) Part (d) revolves around the properties of the noble gases, specifically argon. The question is asking why no product forms when magnesium and argon are heated together.For (c), as the relative atomic masses are given for Fluorine (F) with 19 and Magnesium (Mg) with 24, we need to calculate the Mr for MgF2. Since there are two atoms of fluorine (F) in magnesium fluoride (MgF2), we need to take this into account before adding the relative atomic masses.Chemically, the metal magnesium (Mg) can easily lose two electrons and form a stable 2+ cation, and Fluorine is one of the elements that needs an electron pair to reach eight electrons in its outermost shell, becoming a stable ionize of 18 electrons. Therefore, magnesium fluoride MgF2 can be formed between them.The likely formula mass of magnesium fluoride (MgF2) is the sum of the relative atomic masses, calculated as (the relative atomic mass of magnesium (Mg) x1 + the relative atomic mass of fluorine x2 = 24x1 + 19*2), which can be computed accordingly.Regarding question (d), Argon falls under the noble gases’ category in the Periodic Table. Noble gases are characteristically chemically inert because their outermost electron orbital is completely full with electrons, fulfilling the octet rule. This completeness renders it unnecessary for them to gain, lose out, or share electrons making them highly stable and indisposed to reacting when heated together with another atom, in this case, magnesium.