Which of the following statements is false?

$\stackrel{\mathrm{Be} \mathrm{Mg} \mathrm{Ca} \mathrm{Sr} \mathrm{Ba}}{\to }$As the size increases, metallic nature increases, reactivity with water increases, therefore “Sr” decomposes water readily than Be.

Option - 1 correct

Melting Points order

$\stackrel{{\mathrm{BeCO}}_3<{\mathrm{MgCO}}_3<{\mathrm{CaCO}}_3<{\mathrm{SrCO}}_3<{\mathrm{BaCO}}_3}{\to }$ As the size  [Molecular weight] of carbonates increases, surface area increases, inter molecular attraction increases and hence melting point increases

Option -2 is correct

solubility order

$\stackrel{\mathrm{Be}{\left(\mathrm{OH}\right)}_2<\mathrm{Mg}{\left(\mathrm{OH}\right)}_2<\mathrm{Ca}{\left(\mathrm{OH}\right)}_2<\mathrm{Sr}{\left(\mathrm{OH}\right)}_2<\mathrm{Ba}{\left(\mathrm{OH}\right)}_2}{\to }$ If anion size is smaller [F^- , OH^- ] then solubility depends on lattice energy 
As L.E decreases from Be(OH)₂ to Ba(OH)₂ ,solubility increases.
So option 3 also correct.

Basic strength Order:

$\stackrel{\mathrm{Be}{\left(\mathrm{OH}\right)}_2<\mathrm{Mg}{\left(\mathrm{OH}\right)}_2<\mathrm{Ca}{\left(\mathrm{OH}\right)}_2<\mathrm{Sr}{\left(\mathrm{OH}\right)}_2<\mathrm{Ba}{\left(\mathrm{OH}\right)}_2}{\to }$
As the size of metal increases, metallic nature increases, ionisation of M-OH bond increases, release of OH^- ion increases
Basic strength increases

So Option -4 Incorrect