Explanation

Orbitals that have the same energy level are called degenerate orbitals.

This concept is important in understanding electron behavior and how they fill atomic orbitals, following principles like the Aufbau principle and Hund's rule.

For example, in a hydrogen atom, all orbitals with the same principal quantum number (n) are degenerate. 

Explanation

GROUP - 11 (I B) [Copper, Silver and Gold]

Copper, Ag, and Au are known as coinage metals

Because they were used to make coins.

All the metals are noble w.r.t. chemical activity.

Explanation

The transition state is the highest energy point along the reaction pathway.

Reactants and products have lower energy compared to this activated complex.

Explanation

Ionic radius decreases with higher positive charge (more protons pull electrons closer).

K⁺ (monovalent) has a much larger radius than Pb³⁺ or Cr³⁺ (trivalent cations).

Explanation

Energy order follows the (n + l) rule: lower (n + l) means lower energy.

For 3p (n + l = 3 + 1 = 4), 4s (n + l = 4 + 0 = 4), 3d (n + l = 3 + 2 = 5).

→ So, 3p < 4s < 3d in energy.

Explanation

Alpha (α) particles consist of 2 protons and 2 neutrons (like a He²⁺ nucleus).

They carry a +2 charge and are emitted in radioactive decay.

Explanation

In a neutralization reaction, acid + base → salt + water.

Thus, the acid and base are neutralized, and a salt is formed.

Explanation

Chlorine has atomic number 17 → 17 electrons in neutral state.

With a –1 charge, it gains 1 more electron → 17 + 1 = 18 electrons.

Explanation

The main chain is butane (4 carbons).

A phenyl group (-C₆H₅) is attached to the 2nd carbon of butane → hence the name 2-phenylbutane.

Explanation

H₂SO₄ reacts with Ba(NO₃)₂ to form a white precipitate of BaSO₄, confirming sulfuric acid.

HCl does not give this reaction, so the test differentiates between the two acids.