Chemistry — Unit 1 — Test 5

AgCl(s) + 2 NH3(aq) ⇌ [Ag(NH3)2]+ + Cl− (right favored)

AgI(s) dissolves readily in NH3 forming a stable ammine complex (right favored).

Both AgI and AgCl dissolve equally in NH3.

AgI(s) + 2 NH3(aq) ⇌ [Ag(NH3)2]+ + I− (left favored)

Ag+ + NH3 → [Ag(NH3)2]+ stronger than Ag+ + I−

Cd2+ + I− weaker than Cd2+ + F−

BH3 + NH3 versus BH3 + SMe2 (choose the harder base for strongest adduct)

AlF3 + F− → [AlF4]−

Bronsted–Lowry is broader than Lewis because all Lewis bases are proton donors.

Bronsted–Lowry: proton transfer; Lewis: electron‑pair transfer; the latter encompasses the former.

Bronsted acids must be neutral molecules; Lewis acids must be cations.

Both definitions are identical for all solvents.

Zn2+ (hard) shows no preference between S2− and O2−.

Hg2+ (hard) prefers F− (hard); HgF2 is less stable than HgI2.

Cu+ (soft) prefers I− (soft) over F− (hard); thus CuI is more stable than CuF.

Mg2+ (hard) prefers I− (soft) over F− (hard); MgI2 is more stable than MgF2.

I− < R2S < PH3 < NH3 < H2O < OH− < F− (soft→hard)

PH3 < NH3 < H2O < OH− < F− < R2S < I− < S2− (hard→soft)

R2S < S2− < I− < PH3 < NH3 < H2O < OH− < F−

F− < OH− < H2O < NH3 < PH3 < I− < S2− < R2S

HClO4 ≈ HNO3 > H2SO4 > H3PO4

H3PO4 > H2SO4 > HNO3 ≈ HClO4

HClO4 < HNO3 because Cl is more electronegative.

H2SO4 is weaker than acetic acid in water.

In water, HClO4 and HCl show different intrinsic acidities because water is a differentiating solvent.

In acetic acid, HCl and HClO4 are both strongly leveled and indistinguishable.

In liquid NH3, strong mineral acids are leveled to the common acid NH4+.

In HF, all bases are leveled to F−.

AlCl3·SMe2 stronger than AlCl3·OEt2

BH3·NH3

BH3·CO

Ag+·PR3 stronger than Ag+·I− in water

All are equally weak bases.

ClO4− and NO3− are much weaker bases than Cl− and HSO4−.

Cl− is the weakest base in the series Cl−, NO3−, HSO4−, ClO4−.

HSO4− is stronger base than NO3−.