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According to ( n + l) rule after complet...

According to `( n + l)` rule after completing 'np' level the electron enters into

A

`(n-1)d`

B

`(n+1)s`

C

`nd`

D

`(n+1)p`

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To solve the question "According to (n + l) rule after completing 'np' level the electron enters into", we can follow these steps: ### Step-by-Step Solution: 1. **Understand the (n + l) Rule**: The (n + l) rule helps determine the order in which electrons fill atomic orbitals. Here, 'n' is the principal quantum number and 'l' is the azimuthal quantum number. The lower the value of (n + l), the earlier the orbital is filled. 2. **Identify the Current Orbital**: The question specifies that we are considering the 'np' level. The 'n' in 'np' represents the principal quantum number of the p orbital. 3. **Determine the Next Orbital**: According to the (n + l) rule, after filling the 'np' orbital, the next electrons will fill the orbital with the next lowest (n + l) value. - For the 'np' orbital, 'n' is the principal quantum number and 'l' for p is 1. - Therefore, the (n + l) value for 'np' is (n + 1). 4. **Identify the Next Orbital Based on n**: After completing the 'np' level, the next orbital to be filled will be the (n + 1)s orbital. - For example, if n = 3 (3p), after completing the 3p level, the next orbital will be 4s (where n = 4). 5. **Conclusion**: Thus, after completing the 'np' level, the electron enters into the (n + 1)s orbital. ### Final Answer: After completing the 'np' level, the electron enters into the **(n + 1)s** orbital. ---
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According to Octed Rule, each atom gains or loses electrons to complete its outermost shell. As a result, molecules are formed. Each contributing element has 8 electrons in the outermost shell, but there are some limitations to this rule in which central atom of some molecules has more han 8 electrons. Some molecules like NO and NO_(2) don't satisfy octet rule as they have add electrons in them. On the basis of above paragraph, answer the following : (i) Writer the Lewis structurre of N_(2) molecule. (ii) How the structure of SF_(6) cannot be explained on the basis of octet rule ?

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Knowledge Check

  • According to (n + l) rule, after np level is filled with electrons, the next electron will enter into

    A
    `(n + 1) p`
    B
    `(n +1) s`
    C
    `(n -1) d`
    D
    `nd`

  • According to Slater's rule, correct order of Z_(eff) on valence shell electron is:

    A
    `Fe gt Fe^(2+) gt Fe^(3+)`
    B
    `N^(3-) lt O^(2-) lt F^(-)`
    C
    `Na^(+) lt Mg^(2+) lt Al^(3+)`
    D
    `Tl^(2+) lt V^(3+) lt Mn^(5+)`

  • When 4 d orbital is complete, the newly entering electrons goes in to -

    A
    5f
    B
    5s
    C
    5p
    D
    6d Orbital

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    According to Huckl rule, the number of pi electrons in naphthanlene is:

    In an orbital electrons are filled according to Aufbau principle, Pauli's exclusion principle and Hund's rule of maximum muliplicity . According to Aufbau principal the orbital are filled in order to their increasing energies . In the order of increase of energy of orbitals cna be calculated from ( n + l ) rule. Lower the value of ( n + l ) for an orbital the lowest energy hence orbital are filled in order of increasing ( n + l ) value. If two orbitals have same ( n + l ) value, the orbital with lower value of 'n' has lower energy hence it is filled first. According to Pauli's exclusion principle, an orbital can have maximum two electrons with opposite spin. According to Hunds rule pairing of electron in degenerate orbitals of the same sub shell does not take place until each orbital belonging to that sub shell has got one electron each i.e., singly occupied. If n=4, how many element are possible?

    After filling the 4d-orbitals, an electron will enter in:

    In an orbital electrons are filled according to Aufbau principle, Pauli's exclusion principle and Hund's rule of maximum muliplicity . According to Aufbau principal the orbital are filled in order to their increasing energies . In the order of increase of energy of orbitals cna be calculated from ( n + l ) rule. Lower the value of ( n + l ) for an orbital the lowest energy hence orbital are filled in order of increasing ( n + l ) value. If two orbitals have same ( n + l ) value, the orbital with lower value of 'n' has lower energy hence it is filled first. According to Pauli's exclusion principle, an orbital can have maximum two electrons with opposite spin. According to Hunds rule pairing of electron in degenerate orbitals of the same sub shell does not take place until each orbital belonging to that sub shell has got one electron each i.e., singly occupied. The electron identified by quantum number n & l (i) n = 4, l = 1 (ii) n = 4, l = 0 ( iii) n = 3, l = 2 (iv) n = 3, l = 1 can be placed in order of increasing energy from the lowest to the highest as

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