Yes. actinides show higher OS than lanthanides. This is because of the low energy difference of 5f, 6d and 7s orbitals.

Yes, actinides show higher oxidation states than lanthanides.

Actinides and lanthanides are two series of elements that are located in the f-block of the periodic table. While they have similar properties, there is a key difference between them when it comes to their oxidation states.

1. Electronic Configuration:
- Actinides: The actinide series begins with the element actinium (Ac) and ends with lawrencium (Lr). The general electronic configuration of actinides is [Rn] 5f₁-¹⁴ 6d₀-² 7s².
- Lanthanides: The lanthanide series begins with the element lanthanum (La) and ends with lutetium (Lu). The general electronic configuration of lanthanides is [Xe] 4f¹-¹⁴ 5d₀-² 6s².

2. Shielding Effect:
The lanthanides have a larger number of electrons in the 4f subshell, which provides better shielding for the outer electrons. This shielding effect reduces the effective nuclear charge experienced by the outermost electrons, making it harder to remove them and achieve higher oxidation states.

On the other hand, the actinides have a smaller number of electrons in the 5f subshell, leading to less effective shielding. This results in a stronger attraction between the outer electrons and the nucleus, making it easier for actinides to achieve higher oxidation states.

3. Energy Difference:
The energy difference between the 5f and 6d subshells is relatively small for actinides, allowing for greater participation of the 5f electrons in chemical reactions. This availability of 5f electrons contributes to the ability of actinides to exhibit higher oxidation states.

In contrast, the energy difference between the 4f and 5d subshells is larger for lanthanides, resulting in less participation of the 4f electrons in chemical reactions. This limits the ability of lanthanides to show higher oxidation states.

4. Oxidation States:
Actinides can exhibit a wide range of oxidation states, including +3, +4, +5, +6, and even higher states such as +7 or +8 in some cases. This variation in oxidation states is due to the availability of the 5f electrons for bonding.

Lanthanides, on the other hand, primarily exhibit an oxidation state of +3 due to the limited participation of the 4f electrons in chemical reactions.

Conclusion:
In conclusion, actinides show higher oxidation states than lanthanides. This is mainly due to the smaller number of electrons in the 5f subshell of actinides, which leads to weaker shielding and stronger attraction between the outer electrons and the nucleus. Additionally, the smaller energy difference between the 5f and 6d subshells allows for greater participation of the 5f electrons in chemical reactions, enabling actinides to exhibit a wider range of oxidation states.