Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall

En = –2.18 x 10–18 J(1/n2)

a. 3.08 x 1015/s
b. 1.03 x 108/s
c. 2.06 x 1014/s
d. 1.35 x 10–51/s
e. 8.22 x 1014/s

The frequency of the light is

Explanation:

The equation used to calculate the energy for a transition, we use the equation:

where,

n = principal energy level

Calculating the energy difference:

To calculate the energy of the light for a given frequency, we use the equation given by Planck, which is:

where,

E = energy of the light  =

h = Planck's constant =

= frequency of the light = ?

Putting values in above equation, we get:

Hence, the frequency of the light is

your answer would be a. 12.5 kg

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.