Hydrogen peroxide, in the pure state, is:

We begin with the formula of hydrogen peroxide, which is written as $$\mathrm{H_2O_2}$$. Each oxygen atom in this molecule possesses two lone pairs of electrons in addition to the two bonds it forms (one $$\mathrm{O\!-\!O}$$ bond and one $$\mathrm{O\!-\!H}$$ bond). Because a total of four regions of electron density surround every oxygen, we invoke the VSEPR (Valence Shell Electron Pair Repulsion) principle, which tells us that

$$$\text{four electron pairs} \;\Longrightarrow\; \text{approximately tetrahedral electron-pair geometry}.$$$

Now, in such a tetrahedral arrangement, the two lone pairs occupy positions that push the bonding pairs away, creating bond angles smaller than the ideal $$109.5^{\circ}$$. Importantly, the two $$\mathrm{O\!-\!H}$$ bonds do not lie in the same plane as the $$\mathrm{O\!-\!O}$$ bond; instead they fold out of the plane, giving the entire $$\mathrm{H_2O_2}$$ molecule a twisted “open-book” shape. Experimental measurements show that the dihedral angle between the two $$\mathrm{HO\!-\!O}$$ planes is about $$94^{\circ}$$. Because the four atoms $$\mathrm{H-O-O-H}$$ cannot be placed in a single plane simultaneously, we say the molecule is non-planar (and certainly not linear).

Next, we consider its appearance. Absolutely pure hydrogen peroxide is a very pale blue, syrup-like liquid. However, the blue tint is so faint that in ordinary laboratory samples—or in thin layers—it looks essentially colorless to the naked eye. Chemists therefore describe the substance as “almost colorless.”

Putting these two points together:

• Geometry   ⇒   non-planar (definitely not linear).
• Colour       ⇒   almost colorless (not appreciably blue to normal vision).

These two characteristics match exactly with Option A.

Hence, the correct answer is Option A.