[Cu(NH3)4]2+ is known to exhibit a blue color due to d-d transitions.

[Cu(H2O)6]2+ is known to exhibit a blue color due to d-d transitions in the presence of water ligands.

[Cu(H2O)6]2+ is typically blue due to the d-d transitions of the copper ion in an octahedral field.

Strontium salts produce a red flame when burned.

Lithium salts produce a red flame when burned.

Potassium dichromate (K2Cr2O7) gives a yellow solution.

The combined gas law is represented by the equation P1V1/T1 = P2V2/T2, which combines Boyle's, Charles's, and Gay-Lussac's laws.

The common difference is found by subtracting any two consecutive terms: 15 - 10 = 5.

The common oxidation state of actinides in their compounds is +4.

Alkali metals have a common oxidation state of +1.

Alkaline earth metals commonly exhibit a +2 oxidation state.

Alkaline earth metals typically exhibit a common oxidation state of +2.

Aluminum commonly exhibits an oxidation state of +3 in its compounds.

Chromium commonly exhibits a +6 oxidation state in chromates (CrO4^2-).

In Cr2O7^2-, chromium has a common oxidation state of +6.

In CrO3, chromium (Cr) has an oxidation state of +6.

Chromium commonly exhibits a +6 oxidation state in compounds such as chromium trioxide (CrO3).

Group 1 elements commonly exhibit an oxidation state of +1.

Group 13 elements commonly exhibit a +3 oxidation state due to the loss of three valence electrons.

Group 17 elements, also known as halogens, commonly exhibit an oxidation state of -1.

In Fe2O3, iron has a common oxidation state of +3.

In FeCl3, iron (Fe) has an oxidation state of +3.

In ammonia, nitrogen has an oxidation state of -3.

In ammonia (NH3), nitrogen has an oxidation state of -3.

In sulfuric acid, sulfur has an oxidation state of +6.

The common oxidation state of group 13 elements, such as Aluminum, is +3.

The common oxidation state of transition metals in the d-block is +2, as they often lose two electrons from their outermost shell.

Transition metals commonly exhibit a +2 oxidation state due to the loss of two 4s electrons.

The common ratio r = 12/4 = 3.

f(g(x)) = f(2x) = 2x + 1.