Cheat Sheet: Chemical Bonding NEET Express Summary

SN	Hybridization	E. Geometry	Molecular Shape	Bond Angle	Key Example
2	sp	Linear	Linear	180°	$CO_{2}$ , $BeCl_{2}$
3+0	$sp^{2}$	Trig. planar	Trig. planar	120°	$BF_{3}$ , $SO_{3}$
3+1	$sp^{2}$	Trig. planar	Bent	~117°	$SO_{2}$ , $O_{3}$
4+0	$sp^{3}$	Tetrahedral	Tetrahedral	109.5°	$CH_{4}$ , $CCl_{4}$
4+1	$sp^{3}$	Tetrahedral	Trig. pyramidal	~107°	$NH_{3}$ , $PCl_{3}$
4+2	$sp^{3}$	Tetrahedral	Bent	~104.5°	$H_{2}O$
5+0	$sp^{3}$ d	TBP	TBP	90°/120°	$PCl_{5}$
5+1	$sp^{3}$ d	TBP	Seesaw	~173°/102°	$SF_{4}$
5+2	$sp^{3}$ d	TBP	T-shaped	~90°	$ClF_{3}$ , $BrF_{3}$
5+3	$sp^{3}$ d	TBP	Linear	180°	$XeF_{2}$ , $I_{3}^{-}$
6+0	$sp^{3}$$d^{2}$	Octahedral	Octahedral	90°	$SF_{6}$
6+1	$sp^{3}$$d^{2}$	Octahedral	Sq. pyramidal	~90°	$BrF_{5}$ , $IF_{5}$
6+2	$sp^{3}$$d^{2}$	Octahedral	Sq. planar	90°	$XeF_{4}$

Species	$e^{-}$	BO	Magnetic	Note
$H_{2}$	2	1	Dia	—
$He_{2}^{+}$	3	0.5	Para	Exists!
$He_{2}$	4	0	—	Doesn't exist
$Li_{2}$	6	1	Dia	Gas phase only
$B_{2}$	10	1	Para	2 unpaired in π2p
$C_{2}$	12	2	Dia	Both π bonds!
$N_{2}$	14	3	Dia	Most stable
$O_{2}$	16	2	Para	2 unpaired in π*2p
$O_{2}^{+}$	15	2.5	Para	—
$O_{2}^{-}$	17	1.5	Para	Superoxide
$O_{2}^{2-}$	18	1	Dia	Peroxide
$F_{2}$	18	1	Dia	—
NO	15	2.5	Para	Odd-electron
$NO^{+}$	14	3	Dia	Isoelectronic with $N_{2}$
CO	14	3	Dia	Isoelectronic with $N_{2}$

$CO_{2}$ (linear), $BF_{3}$ (trig. planar), $CCl_{4}$ (tetrahedral), $SF_{6}$ (octahedral), $XeF_{4}$ (sq. planar), $PCl_{5}$ (TBP, all Cl)

$\Delta Hf$ = −411, $\Delta Hs$ ub = +108, IE = +496, ½ $\Delta Hd$ iss = +121, EA = −349, U = −787 kJ/mol

Small cation + large anion + high cation charge → MORE COVALENT CHARACTER

Z ≤ 7 (B,C,N): π2p BEFORE σ2p. Z > 7 (O,F): σ2p BEFORE π2p.

Higher BO → shorter bond → stronger bond → higher bond energy BO order: $N_{2}$ (3) > $O_{2}$ (2) > $F_{2}$ (1) → length: $N_{2}$ < $O_{2}$ < $F_{2}$