hmmm speed run

lattices

PE diagram

bonds form when minimun PE

blond length is the distance of the lowest point on the curve

geometry

Molecular Geometry & Bond Angles (VSEPR)

• Bond Angles:

  • Linear = 180°

  • Trigonal planar = 120°

  • Tetrahedral = 109.5°

  • Trigonal pyramidal ≈ 107°

  • Bent ≈ 104.5°

hybridization changes during a reaction

Addition reaction: C=C double bond (sp²) → becomes sp³.

lone pairs push bonds close tg

decreasing angles

bond length is shorter w 

strong bonds

ionic 

lattices of alternating cation and anion 

high mp 

hard

free floating = yes 2 conductivity

solid = none

molecular

molecular hmph - imf

held by IMF, dipole dipole

low mp

soft

dont conduct

covalent solids (bonds = nonmetals)

hella high

atoms = covalently bonded

high mp

hard

dont conduct - molecular

metalic

metalicsea

metal cations in a sea of electrons

mp depend on metal

ductile

good conducters

polar lewis structure

central atoms have lone pair = polar

If the outer atoms are different (for example, COCl₂ with O and Cl attached to the same C)

electronegativity difference

polar bonds arragned sym cancel dipoles out 

The particle must be a cation because the negative end of each water molecule is pointed toward it.

the Br—F molecule is the most polar

larger electronegativity difference (so the larger bond dipole), making it the most polar.

Propanoic acid — because it can form intermolecular hydrogen bonds strongly

intermolec force from temp dipoles

trans isomer = dipole dipole interaction

cisometer = london

brittle water

london disp in cl4

The carbon atoms in C₂H₂ are sp hybridized (triple bond), and in C₂H₃Cl₂ they change to sp³ hybridization (single bonds), so answer b is correct.

smallest O-S-O bond angle at approximately 109.5° in its tetrahedral structure

The Cl-Cl bond is stronger than the Br-Br bond because chlorine atoms are smaller, allowing for better orbital overlap and a stronger covalent bond, making answer d correct.