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Helga [31]
1 year ago
9

The following combinations are not allowed. If n and ml are correct, change the l value to create an allowable combination:

Chemistry
1 answer:
ololo11 [35]1 year ago
7 0

The allowable combination for the atomic orbital is n=3, l=1 or 2, m_{l}=+1.

<h3>What are the three quantum numbers of an atomic orbital?</h3>

Three quantum numbers specify an atomic orbital:

- The principal quantum number, n, which is a positive integer, describes the relative size of the orbital and its distance from the nucleus.

- l is the angular momentum quantum number that is related to the shape of the orbital; l is an integer from 0 to n-1 (so n limits l ),

- $\boldsymbol{m}_{l}$ is the magnetic quantum number that prescribes the three-dimensional shape of the orbital around the nucleus; m_{l} values are integers from -l to =l(l limits ml)

For n = 3, l can have three values: 0, 1, and 2. Hence, the l value must be lower than 3. Because of m_{l}= +1, the l value must be higher than 0. Two l values are consistent with n and m_{l) values:

l= 1 or 2

Therefore, the allowable condition is n=7, l=1 or 2, m_{l}=+3.

To know more about quantum numbers, visit: brainly.com/question/16979660

#SPJ4

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It takes 495.0 kJ of energy to remove 1 mole of electron from an atom on the surface of sodium metal. How much energy does it ta
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Answer:

\lambda=241.9\ nm

Explanation:

The work function of the sodium= 495.0 kJ/mol

It means that  

1 mole of electrons can be removed by applying of 495.0 kJ of energy.

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1 mole = 6.023\times 10^{23}\ electrons

So,  

6.023\times 10^{23} electrons can be removed by applying of 495.0 kJ of energy.

1 electron can be removed by applying of \frac {495.0}{6.023\times 10^{23}}\ kJ of energy.

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Also,  

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Energy required = 82.18\times 10^{-20}\ J

Also, E=\frac {h\times c}{\lambda}

Where,  

h is Plank's constant having value 6.626\times 10^{-34}\ Js

c is the speed of light having value 3\times 10^8\ m/s

So,  

79.78\times 10^{-20}=\frac {6.626\times 10^{-34}\times 3\times 10^8}{\lambda}

\lambda=\frac{6.626\times 10^{-34}\times 3\times 10^8}{82.18\times 10^{-20}}

\lambda=\frac{10^{-26}\times \:19.878}{10^{-20}\times \:82.18}

\lambda=\frac{19.878}{10^6\times \:82.18}

\lambda=2.4188\times 10^{-7}\ m

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\lambda=241.9\ nm

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