NEET Chemistry Mock Test – 1

The empirical formula is the simplest ratio of elements. For glucose, it is $\text{CH}_2\text{O}$.

Manganese loses two $4s$ electrons in $\text{Mn}^{2+}$ state, leaving five unpaired $3d$ electrons.

This is the complete combustion equation for methane.

Azimuthal quantum number determines the shape ($s$, $p$, $d$, $f$) of the orbital.

The molar mass of $\text{CaCO}_3$ is $40 + 12 + 48 = 100\ \text{g/mol}$.

$\text{HCl}$ has a polar covalent bond due to different electronegativities of H and Cl.

The carbon in methane undergoes $sp^3$ hybridization.

The rate for a first-order reaction is directly proportional to $[A]$.

Osmotic pressure is given by $\Pi = iCRT$ where $i$ is the van‘t Hoff factor.

Strong acids completely ionize in solution. Hydrochloric acid is one of them.

In $\text{H}_2\text{SO}_4$, sulfur has an oxidation state of +6.

Chromium has an anomalous electron configuration to achieve extra stability.

No real gas behaves ideally at all temperatures and pressures; deviations occur at high pressures and low temperatures.

$\text{NH}_3$ has a trigonal pyramidal geometry due to the lone pair of electrons on nitrogen.

A redox reaction involves both reduction and oxidation.

An ionic bond forms when the difference in electronegativity is high (typically > 1.7).

HCl is a strong acid and fully dissociates in solution. pH = -log[H+].

Helium has the highest ionization energy due to its stable electronic configuration.

Tollen’s reagent gives a silver mirror with aldehydes but not with ketones.

In $\text{BF}_3$, boron undergoes $sp^2$ hybridization, forming a trigonal planar shape.