What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75*10^14 Hz

Explanation:

The computation is shown below:

Data provided in the question

The frequency of the radio wave is f =  

Let us assume the number of photons is N

=

And, h =

Based on the above information, the total energy is

As we know that

E = N h f

We just applied the above formula so that the total energy contained could come i.e by multiplying the three items so that the correct value could come

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.

if you mean hydrogen and oxygen then water is the product