What is the molarity of an aqueous solution that contains 0.072 g C2H6O2 per gram of solution? The density of the solution is 1.40 g/mL.

1.626 M

Explanation:

Let's start by calculating how many grams of C₂H₆O₂ are there per mL of solution:

So the C₂H₆O₂ concentration can be expressed as 0.1008 g/mL.

Now we convert g/mL to molarity, using the molar mass of C₂H₆O₂:

(1 mL = 0.001 L)

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.