Suppose you have a compound which has an empirical formula of C4H5N2O and molar mass of 194 g/mol. What is the compounds molecular formula?

C₈H₁₀N₄O₂

Explanation:

Step 1: Given data

Step 2: Determine the molar mass of the empirical formula

The molar mass is equal to the sum of the masses of the elements that form it.

M = 4 × C + 5 × H + 2 × N + 1 × O

M = 4 × 12.01 g/mol + 5 × 1.01 g/mol + 2 × 14.0 g/mol + 1 × 16.0 g/mol

M = 97.09 g/mol ≈ 97 g/mol

Step 3: Calculate "n"

n = molar mass of the molecular formula / molar mass of the empirical formula

n = (194 g/mol)/(97 g/mol) = 2

Step 4: Determine the molecular formula

To determine the molecular formula, we have to multiply the empirical formula by "n".

C₄H₅N₂O × 2 = C₈H₁₀N₄O₂

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.

c.

explanation: