Explanation:
Cadmium, nickel, chromium, and silver are sometimes used as protective platings. Metals have a wide range of corrosion resistance. The most active metals (i.e., those that tend to lose electrons easily)--such as magnesium and aluminum--corrode easily and are listed at the top of Table 2-1.
Answer : 0.0392 grams of Zn metal would be required to completely reduced the vanadium.
Explanation :
Let us rewrite the given equations again.
On adding above equations, we get the following combined equation.
We have 12.1 mL of 0.033 M solution of VO₂⁺.
Let us find the moles of VO₂⁺ from this information.
From the combined equation, we can see that the mole ratio of VO₂⁺ to Zn is 2:3.
Let us use this as a conversion factor to find the moles of Zn.
Let us convert the moles of Zn to grams of Zn using molar mass of Zn.
Molar mass of Zn is 65.38 g/mol.
We need 0.0392 grams of Zn metal to completely reduce vanadium.
The most likely formula for an oxide formed between group 1a atom X and oxygen would be
X2O. - X is group 1a atom.
Answer:
Explanation:
Elements on the right side of the periodic table are very likely to form negative ions -- all of those except elements in the 8th or 18th column (depending on how your periodic table is numbered).
K and Mg are on the left side, so they will not form negative ions.
They give up 1 (for K) electron and 2 (for Mg) electrons which will leave plus charges for the ions.
On the other hand S and I are on the right side of the periodic table. They will take on electrons and hence be charged with a minus.
