Hydrogen atom:
The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as
`E_(n)=-(R_(H)Z^(2))/(n^(2))` where `R_(H)= "Rydberg constant," n= "principal quantum number"`
The energy in Joule of an electron in the second orbit of H- atom is:

Answer

To find the energy in Joules of an electron in the second orbit of a hydrogen atom, we can follow these steps:

### Step 1: Identify the values for Z and n
For a hydrogen atom:
- The atomic number (Z) = 1
- The principal quantum number (n) for the second orbit = 2

### Step 2: Use the energy formula for hydrogen-like species
The energy of an electron in a hydrogen-like atom can be calculated using the formula:
\[ E_n = -\frac{R_H Z^2}{n^2} \]
where:
- \( R_H \) is the Rydberg constant, approximately \( 1312 \, \text{kJ/mol} \) for hydrogen.

### Step 3: Substitute the values into the formula
Substituting \( Z = 1 \) and \( n = 2 \) into the formula:
\[ E_2 = -\frac{1312 \times 1^2}{2^2} \]
\[ E_2 = -\frac{1312}{4} \]

### Step 4: Calculate the energy
Now, performing the calculation:
\[ E_2 = -328 \, \text{kJ/mol} \]

### Step 5: Convert kilojoules to joules
To convert kilojoules to joules, we multiply by \( 1000 \):
\[ E_2 = -328 \times 10^3 \, \text{J} \]
Thus, the energy of the electron in the second orbit of a hydrogen atom is:
\[ E_2 = -328000 \, \text{J} \]

### Final Answer
The energy in Joules of an electron in the second orbit of a hydrogen atom is \( -328000 \, \text{J} \).

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