Single Choice

What happens when both of the orbitals in a molecule are in phase, either both positive or both negative and the electrons in the bonds are at their lowest energy level?

ABonding takes place.
Correct Answer
BThe chemicals don't react.
CThe atoms don't bond.
DBonding doesn't take place.

Solution

When both of the orbitals in a molecule are in phase, either both positive or both negative, and the electrons in the bonds are at their lowest energy level, bonding takes place. The electron density between two nuclei increases and in other places, the electron density decreases.

SIMILAR QUESTIONS

Atomic Structure

The atomic number at which filling of a g-orbital is likely to begin is:

Atomic Structure

Which one of the following sequences with regard to the energy content of different orbitals, is correct?

Atomic Structure

Not considering the electronic spin, the degeneracy of the second excited state $$\left(n=3\right)$$ of $$H$$-atom is $$9$$, while the degeneracy of the second excited state of $${H}^{-}$$ is _______.

Atomic Structure

The electronic configuration, $$1s^22s^22p^63s^23p^63d^9$$, represents a:

Atomic Structure

The $$71^{st}$$ electron of an element $$X$$ with an atomic number of $$71$$ enters into the orbital:

Atomic Structure

If the principle quantum number n = 6, the correct sequence of filling of electron will be :

Atomic Structure

Which of the following electronic configurations has maximum energy ?

Atomic Structure

Using the Hund rules, write the spectral symbol of the basic term of the atom whose only partially filled subshell (a) is filled by $$1/3$$, and $$ S = 1$$; (b) is filled by $$70\%$$, and $$S = 3/2$$.

Atomic Structure

Match the atomic numbers among, $$4,8,10,15$$ and $$19$$ with An element with $$4$$ shells.

Atomic Structure

Match the atomic numbers, $$4,8,10,15$$ and $$19$$ with: Element which does not form ion.

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