English

Draw shapes of 2p orbitals.

Advertisements
Advertisements

Question

Draw shapes of 2p orbitals.

Diagram
Advertisements

Solution


          Shapes of 2p orbitals

shaalaa.com
  Is there an error in this question or solution?
Chapter 4: Structure of Atom - Exercises [Page 54]

APPEARS IN

Balbharati Chemistry [English] Standard 11 Maharashtra State Board
Chapter 4 Structure of Atom
Exercises | Q 6. (M) | Page 54

RELATED QUESTIONS

Choose the correct option.

“No two electrons in the same atoms can have identical set of four quantum numbers”. This statement is known as -


State Heisenberg uncertainty principle.


State and explain Pauli’s exclusion principle.


Explain the anomalous behaviour of chromium.


Write orbital notations for the electron in orbitals with the following quantum numbers.

n = 2, l = 1


Write condensed orbital notation of electronic configuration of the following element:

Lithium (Z = 3)


Write condensed orbital notation of electronic configuration of the following element:

Silicon (Z = 14)


Draw shapes of 2s orbitals.


Write a note on ‘Principal Quantum number.


Indicate the number of unpaired electron in:

Cr (Z = 24)


Which mineral among the following contains vanadium in it?


Which one of the following orders is CORRECT in case of energy of the given subshells?

P: n = 4; l = 3

Q: n = 5; I = 1

R: n = 5; l = 0

S: n = 4; l = 2


How many electrons in 19K have n = 3, l = 1?


The three electrons have the following set of quantum numbers:

X = 6, 1, −1, `+1/2`

Y = 6, 0, 0, `+1/2`

Z = 5, 1, 0, `+1/2`

Identify the CORRECT statement.


Which of the following has a greater number of electrons than neutrons?

(Mass number of Mg, C, O and Na is 24, 12, 16 and 23 respectively).


Which of the following options does not represent ground state electronic configuration of an atom?


Number of angular nodes for 4d orbital is ______.


Total number of orbitals associated with third shell will be ______.


Out of the following pairs of electrons, identify the pairs of electrons present in degenerate orbitals:

(i)  (a) `n = 3, l = 2, m_l = -2, m_s = - 1/2`
  (b) `n = 3, l = 2, m_l = -1, m_s = - 1/2`
   
(ii)  (a) `n = 3, l = 1, m_l = 1, m_s = + 1/2`
  (b) `n = 3, l = 2, m_l = 1, m_s = + 1/2`
   
(iii) (a) `n = 4, l = 1, m_l = 1, m_s = + 1/2`
  (b) `n = 3, l = 2, m_l = 1, m_s = + 1/2`
   
(iv)  (a) `n = 3, l = 2, m_l = +2, m_s = - 1/2`
  (b) `n = 3, l = 2, m_l = +2, m_s = + 1/2`

Which of the following sets of quantum numbers are correct?

  `n` `l` `m_l`
(i) 1 1 +2
(ii) 2 1 +1
(iii) 3 2 –2
(iv) 3 4 –2

In which of the following pairs, the ions are iso-electronic?

(i) \[\ce{Na^{+}, Mg^{2+}}\]

(ii) \[\ce{Al3^{+}, O-}\]

(iii) \[\ce{Na+ , O2-}\]

(iv) \[\ce{N3-, Cl-}\]


The arrangement of orbitals on the basis of energy is based upon their (n + l) value. Lower the value of (n + l), lower is the energy. For orbitals having same values of (n + l), the orbital with lower value of n will have lower energy.

Based upon the above information, arrange the following orbitals in the increasing order of energy.

5p, 4d, 5d, 4f, 6s


The electronic configuration of valence shell of Cu is 3d104s1 and not 3d94s2. How is this configuration explained?


What is the difference between the terms orbit and orbital?


Match the following species with their corresponding ground state electronic configuration.

Atom / Ion Electronic configuration
(i) \[\ce{Cu}\] (a) 1s2 2s2 2p6 3s2 3p6 3d10
(ii) \[\ce{Cu^{2+}}\] (b) 1s2 2s2 2p6 3s2 3p6 3d10 4s2
(iii) \[\ce{Zn^{2+}}\] (c) 1s2 2s2 2p6 3s2 3p6 3d10 4s1
(iv) \[\ce{Cr^{3+}}\] (d) 1s2 2s2 2p6 3s2 3p6 3d9
  (e) 1s2 2s2 2p6 3s2 3p6 3d3

Which of the following is the correct plot for the probability density ψ2 (r) as a function of distance 'r' of the electron from the nucleus for 2s orbitals?


Which one of the following laws will represent the pairing of electrons in a subshell after each orbital is filled with one electron?


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×