Questions And Answers On Molecular Orbital Theory Pdf

questions and answers on molecular orbital theory pdf

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Give the formal charge and oxidation number for each atom. Write the Lewis dot structure for the following species: a chlorine dioxide; b perchlorate ion; c permanganate ion. Give the formal charge and the oxidation number for each atom in each species.

It depends on the number of electrons in the bonding and antibonding orbitals. Which of the following statements is true about it?

Molecular Orbitals in Inorganic Chemistry L1-L4 Course information: All the information you need for this course will be accessible from this site. Need some help! Molloy, Harwood Publishing, Chichester, Tutorials and homework form part of this course and are examinable. Extra reading material is associated with each lecture, this is entirely optional!

9.1: Bond Types and Molecular Orbital Theory (Problems)

It depends on the number of electrons in the bonding and antibonding orbitals. Which of the following statements is true about it? A Can have a negative quantity done clear. B Has always an integral value done clear. C Can assume any positive or integral or fractional value including zero done clear.

D Is a nonzero quantity done clear. A 1 done clear. B 2 done clear. D 3 done clear. A One molecular orbital done clear. B Two molecular orbital done clear. C Three molecular orbital done clear. D Four molecular orbital done clear. CET ]. A Pauling done clear. B Pauling and Slater done clear.

C Mulliken done clear. D Thomson done clear. A The difference between the number of electrons in bonding and antibonding orbitals done clear. B Total number of electrons in bonding and antibonding orbitals done clear. C Twice the difference between the number of electrons in bonding and antibonding electrons done clear. D Half the difference between the number of electrons in bonding and antibonding electrons done clear.

A Bonding electrons are more than antibonding electrons done clear. B Contains unpaired electrons done clear. C Bonding electrons are less than antibonding electrons done clear.

D Bonding electrons are equal to antibonding electrons done clear. C Both A and B done clear. A Chlorine done clear. B Nitrogen done clear. C Oxygen done clear. D Hydrogen done clear. A Valence bond theory done clear.

B Resonance done clear. C Molecular orbital theory done clear. D Hybridization done clear. B H2 done clear. C 3 done clear. D 4 done clear. A Greater than that of separate atoms done clear. B Equal to that of separate atoms done clear. C Lower than that of separate atoms done clear.

D None of the above statement is correct done clear. A One done clear. B Two done clear. C Between 1 and 2 done clear. D One and two alternately done clear. A Nitrogen has no vacant d-orbitals done clear. C Nitrogen atom is much smaller done clear. D Nitrogen is highly inert done clear. A Not attracted into a magnetic field done clear. B Containing only paired electrons done clear. C Carrying a positive charge done clear. D Containing unpaired electrons done clear. A 16 shared and 8 unshared electrons done clear.

B 8 shared and 16 unshared electrons done clear. C 12 shared and 12 unshared electrons done clear. D 18 shared and 6 unshared electrons done clear. A 2 done clear. B 3 done clear. C 4 done clear. A Oxygen and nitric oxide molecules are both paramagnetic because both contain unpaired electrons done clear.

B Oxygen and nitric oxide molecules are both diamagnetic because both contain no unpaired electrons done clear. C Oxygen is paramagnetic because it contains unpaired electrons, while nitric oxide is diamagnetic because it contains no unpaired electrons done clear.

D Oxygen is diamagnetic because it contains no unpaired electrons, while nitric oxide is paramagnetic because it contains an unpaired electron done clear. A 0 done clear. B 1 done clear. C 2 done clear.

A 3 done clear. D 1 done clear. A Bond energy done clear. B Activation energy done clear. C Stabilization energy done clear. D Destabilization energy done clear. A Zero done clear. B One done clear.

C Two done clear. D Three done clear. The element shows [CPMT ]. A Ferromagnetism done clear. B Diamagnetism done clear. C Paramagnetism done clear. D None of these done clear. PMT ]. A Remains unaltered done clear. B Decreases done clear. C Increases done clear. A 4 done clear. D 5 done clear. A Copper crystals done clear.

A 3s done clear. B 1p, 2s done clear. C 2p, 1s done clear. D 3p done clear. C CO done clear. A 6 done clear. B 12 done clear.

D 8 done clear. D 2 done clear. B 4 done clear.

MOs in Inorganic Chemistry

Navigate to the page 3. These five hybrid orbitals will adopt a trigonal bipyramidal geometry in order to get as far from each other as possible. Be sure to show how the energy levels for the atomic orbitals of the two atoms are different. Formation of Molecular Orbitals from Atomic Orbitals Use pictorials to describe the linear combination of atomic orbitals that form molecular orbitals. Run-on Sentences - Worksheet to practice correcting run-on sentences.

Vedantu academic counsellor will be calling you shortly for your Online Counselling session. Related Questions. Answer Verified. Hint: In MO theory, molecular orbitals form by the overlap of atomic orbitals. Atomic orbital energy correlates with electronegativity, as electronegative atoms hold electrons more tightly, lowering their energies. MO modelling is only valid when the atomic orbitals have comparable energy; when the energies differ greatly, the bonding mode becomes ionic. A second condition for overlapping atomic orbitals is that they have identical symmetry.


MULTIPLE CHOICE QUESTIONS (MCQ). CHAPTER 1. MOLECULAR ORBITAL THEORY. Q1) Choose the correct option from following and write in right side.


Explain with the help of Molecular Orbital Theory why the $H{{e}_{2}}$ molecule does not exist.

Direction Q. B 2 10 electrons MO electronic configuration is. Species with zero bond order will not exist. Electrons in orbital.

Test: Molecular Orbital Theory

Exercises are short focused sets of practice questions that can be printed and used as worksheets. Each Exercise focuses on a single concept or skill. You should complete Exercises immediately after the concept or skill is discussed in class to ensure that you fully understand it so that you do not fall behind.

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