LMS

The increasing order of sizeAnion > Neutral > CationN–3 > O–2 > F–1 > Na+Greater the negative charge greater the size of ion.

Left to right effective nuclear charge increase. So atomic size decrease.

Cation is always smaller than neutral atom and anion is always larger than neutral atom 

Size of parent atom is always greater than its positive ion

Ionization energy value is related to the all of thesea. Higher the I.E more stable it isb. Lesser the value of ionization energy greater will be the metalic characterc. The difference between I.E values help us to predict number of electrons in valence shell of an atom.

Mg belongs to IIA while Al  belongs to IIIA order of I.E IA < IIA > IIIA < IVA < VA > VIA < VIIA < VIII A

The order of electron affinity for group VII group is Cl>F>Br>I due to smaller size and greater repulsion

IE across the period does not depend upon Shielding effect because it will remain same from left to right.

ionization energy does not depend upon nature of orbital in the group because all the elements in the group have same orbital

In period number of shell and shielding effect will remain constant 

The valence shell is the highest energy level occupied by electrons 

Na atom after losing 1 electron and O- atom after gaining 2 electrons have given electronic configuration  

If electronegativity difference between two atoms is 1.7 units. The bond is roughly 50% ionic and 50% covalent

Only noble gases in periodic table which have complete outermost shell.

BF₃  does not follow octet rule, it forms stable compounds with six electron.

NH3 have one lone pair of electron which is responsible for the formation of coordinate covalent bond

The bond between NH ₃  and H ⁺  dative in NH₄⁺¹   ion

Due to high electronegativity difference

Total bonds in PH₄⁺¹  = 4Total covalent bonds in PH₄⁺¹  = 3Total dative bonds in PH₄⁺¹  = 1%age covalent character = (total covalent bonds / total bonds) × 100 = (3 / 4) × 100 = 75%

NF ₃  has three covalent bonds or six bonding electrons

Total bonds in NH₄⁺¹  = 4Total covalent bonds in NH₄⁺¹  = 3Total dative bonds in NH₄⁺¹  = 1%age coordinate covalent = (total dative bonds / total bonds) × 100 = (1 / 4) × 100 = 25%

Hydrogen sulphide has bent structure with two lone pairs of electron at the central atom and the angles is 92o S has greater size and comparatively smaller E.N.

Number of lone pair of electrons on central atom is inversely related to the bond angle

In NF₃ , the strong polarity of N-F bond pulls the lone pair of N atom closer to its nucleus and the angle shrinks to 102o

NH₃  has lone pair of electron on N atom & angle decrease to 107.5o remaining all other have 120° bond angle

Alkane are also called paraffins and have bond angle of 109.5°

It is AB₃ L type, so its shape or structure is trigonal pyramidal

The shape of sulphate ion is tetrahedral

VSEPR theory describe the geometry of covalent molecules.

Shape of water is angular or bent.

Pi(π) bond is formed by overlap of p-orbitals perpendicular to the two nuclei. Sigma bond is formed by axial overlapping of orbitals. Hydrogen bond and dative bond(coordinate covalent bond) are formed by donating electron pair to empty orbital of an atom through linear combination.

Hybridization is the extended form of Valence bond theory, which was given to solve some problems and limitations of VBT 

There are 3 sigma bonds therefore 3×2=6 sigma electrons

Bond length  and s character have inverse relation, sp hybridizsed orbital having maximum s-character, so shorter the bond length  

CH₂=CH-CH=CH₂  in this structure all carbon are double bonded so are sp2 hybridized.

In H₂ O sp³   and in H₃ O+ = sp³ 

sp²   = SnCl₂ sp³  = NF₃, SO₄^2-     and  H₂S

sp3 hybrid orbitals are used for bonding in triangular pyramidal molecule

There are 12 sigma bonds and 6 pi delocalized electrons are there in benzene resonance structure

Bond length is directly proportional to the size of atom.HF has smallest bond length.

Extent of overlapping is maximum in case of P – P overlapping 

smaller the size stronger the bond Bond energy kJ/mol H–H =  436,     C–C =  348,           F–F = 154,                 N–N = 163

Na-F is ionic bond while others are covalent bond but the strongest is H – Cl because H has smallest atomic size and polarity also. 

Greater the bond order shorter the bond length

N ≡ N has non polar nature while among other, C ≡ O has polarity as well as smaller size of O atom.

Greater the dipole moment greater the %age ionic character 

Boron have no lone pair and regular geometry but N have one lone pair and irregular geometry

CH₃ F is most polar due to its higher dipole moment.

NH₃   is pyramidal (irregular shape) while BF₃  is trigonal planar (regular shape)