Plot graphs of bond dissociation energy for halogens (F2, Cl2, Br2, I2) and boiling points for hydrogen halides (HF, HCl, HBr, HI).

Values (in $\si{kJ.mol^{-1}}$):

$$\begin{align*} \ce{F2}&: && 159~\si{kJ.mol^{-1}} \\ \ce{Cl2}&: && 243~\si{kJ.mol^{-1}} \\ \ce{Br2}&: && 193~\si{kJ.mol^{-1}} \\ \ce{I2}&: && 151~\si{kJ.mol^{-1}} \end{align*}$$

Trend: Plot points at these values. Connect with a line: starts low at $\ce{F2}$ (weak bond due to lone pair repulsion), peaks high at $\ce{Cl2}$, then decreases steadily to $\ce{I2}$ (weaker overlap of large orbitals).

Values (in $^\circ\si{C}$):

$$\begin{align*} \ce{HF}&: && 19.5~^\circ\si{C} \\ \ce{HCl}&: && -85~^\circ\si{C} \\ \ce{HBr}&: && -67~^\circ\si{C} \\ \ce{HI}&: && -35~^\circ\si{C} \end{align*}$$

Trend: Plot points at these values. Connect with a line: sharp drop from $\ce{HF}$ (high due to hydrogen bonding) to $\ce{HCl}$, then gradual increase to $\ce{HI}$ (increasing London dispersion forces with molecular size).

Sketched trends match data points and lines described above.
BDE: low F₂ → peak Cl₂ → ↓ to I₂

BP: high HF → sharp ↓ HCl → gradual ↑ HI