<span>Moles of solid copper used in reaction, using molar mass:
1 gram Cu @ 63.55 g/mol = 0.0157 moles Cu
(f) Moles of solid silver produced in reaction , using molar mass:
3.395g Ag @ 107.87 g/mol = 0.317 moles of Ag
Write the net ionic equation for the reaction between, using your mole values:
0.0157 Cu (s) & 0.317 Ag+ --> 0.0157 Cu+2 & 0.317 Ag (s)
Convert to whole number ratio, by dividing by the smaller :
0.0157 moles Cu / 0.057 = 1 mole Cu
0.317 moles Ag+ / 0.157 = 2 moles Ag
and rewrite the equation using the whole number ratio:
1 Cu (s) & 2 Ag+ --> 1 Cu+2 & 2 Ag (s)</span>
Answer:
a. There are only 5 electrons in 2p. 2p should be filled with 6 electrons prior to 3s and 3p
b. There are 8 electrons in 2p. 2p should be filled only with 6 electrons (not 8)
Explanation:
The typical electron configuration: 1s2 2s2 2p6 3s2 3p6
a. There are only 5 electrons in 2p
=> should be 1s2 2s2 2p6 3s2 3p2
b. There are 8 electrons in 2p
=> should be 1s2 2s2 2p6 3s2 3p1
-colour
-odour
-texture
-density
-boiling point (sometimes also melting point)
-freezing point
KIO4 is an example of polyatomic ion.
The sum of the oxidation numbers in a polyatomic ion is equal to the charge on the ion.
The charge on this polyatomic ion is 0.
To get the oxidation number of I, we will let x as the oxidation number of I.
We can get the oxidation number of Iodine by solving like this;
KIO4 : (+1) + x + 4(-2) = 0
(+1) + x - 8 = 0
x - 7 = 0
x = +7
Therefore, the oxidation number of iodine atom in KIO4 is +7.