MHT-CET Inorganic Chemistry Review

Flashcards covering key concepts in MHT-CET Inorganic Chemistry.

Boiling point order of Group 16 hydrides

H₂O > H₂Te > H₂Se > H₂S due to Hydrogen bonding.

Boiling point order of Group 17 hydrides

HF > HCl > HBr > HI due to increasing molecular weight and dispersion forces.

Solubility of Group 1 salts in water

Generally soluble; exception for Li⁺ with some phosphates.

Acidic strength of oxoacids in Group 16

H₂SO₄ > H₂SeO₄ > H₂TeO₄ due to electronegativity and oxidation state.

Electronegativity trend in Period 2 and 3

Increases across a period, decreases down a group.

Coordination number of common transition metal complexes

Typically 4 or 6; exception for Ag⁺ with 2.

Color of transition metal complexes in the d-block

Depends on d-electron configuration; e.g. Cu²⁺ is blue due to d-d transitions.

Oxidation states of manganese in compounds

Common states are +2, +4, +6, +7; +3 is less stable.

Melting point trend in Group 14 elements

C > Si > Ge > Sn > Pb due to greater covalent bonding in carbon.

Electron affinity trend in Group 15

Decreases down the group; exception for nitrogen due to stable half-filled p-orbitals.

Stability of peroxides

Increases from Na₂O₂ to BaO₂ due to cation size influence.

Bond angles in hydrides of Group 15

NH₃ > PH₃ due to lone pair-bond pair repulsion.

Trends in ionic radii down a group

Increases down a group due to added electron shells.

Hardness trend in cations

Transition metals are harder, alkali metals softer.

Common oxidation state of chromium

Most common is +6; +3 is stable due to lower energy.

Color of Ni²⁺ complex ions

Green due to d-d transitions.

Hydration energy trend in cations

Higher for smaller, highly charged ions.

Fluorine's unique properties in Group 17

Small size leads to high electronegativity and reactivity.

Stability of iodides vs. chlorides

Iodides are less stable due to larger ion size and weaker bonds.

Hybridization of carbon in organics

sp³ in alkanes, sp² in alkenes, sp in alkynes.

Noble gas stability reason

Full valence shell leads to low reactivity.

Acid-base strength in carboxylic acids

Strength increases with electron-withdrawing groups.

Reduction potential trend in transition metals

Increases as d-electron count decreases.

Boiling point of alcohols vs. ethers

Alcohols higher due to hydrogen bonding; ethers lower.

Exception in Group 2 reactivity

Be reacts less vigorously due to higher ionization energy.

Formation of complex ions with ligands

Strong field ligands create low-spin complexes.

Bond dissociation energy trend in oxides

Increases across a period due to stronger covalent character.

Effect of charge on atomic radius

Positively charged ions are smaller due to increased nuclear attraction.

Stability of halogens

Fluorine is less stable than chlorine due to high electronegativity leading to instability.