| Chem H | Chapter 6 Review

Lattice energy

Energy released when one mold of an ionic compound is formed from gaseous ions.

Bond length

distance between atoms in a chemical bond, nucleus to nucleus

The length of the bond, is shorter when the bond is stronger and when the bond number is higher.

Octet rule

8 valence electrons to be neutral

(except hydrogen, helium , and boron)

Intermolecular force

Forces of attraction between molecules, forces that hold molecules close to eachother in the solid + liquid state

Molecule

Group of covalently bonded atoms, no charge , neutral. Covalent

Formula unit

Smallest particle of an ionic compound. Ionic

Covalent bond

2 atoms sharing some valence electrons

Delta plus and delta minus

Partial positive charge and partial negative charge

Hydrogen bonding

Strongest dipole- dipole force

O-H. N-H. F-H.

Ionic bond

Transfer of valence electrons from metal to nonmetal

Electron sea

Valence e-s move from atom to atom, mobilize e-s , delocalized e-s (

Also a bond between atoms where they share 3 pairs of electrons

Triple bond

Shortest bond and strongest energy

Electronegativity

Measure of the ability of an atom to attract bonding e- s

Polyatomic ion

Group of covalently bonded atoms with a charge

The relationship between bond length and bond energy for single, double , and triple bonds

As the bond every increases, the bonds get shorter

What is meant by resonance structures

Two or more Lewis structures of the same molecule where the atoms stay in the same positions, but the electrons are arranged differently.

Melting point of ionic compounds and molecular compounds

Ionic compounds have higher melting points than molecular compounds because ionic bonds are stronger and require more energy to break

Example of the following type of intermolecular bonding it’s in form: Dipole- Dipole (polar)

HCl

SO₂

H₂S

CH₃Cl

Example of the following type of intermolecular bonding it’s in form: Hydrogen bonding (H attached to N,O, or F)

H₂O

NH₃

HF

CH₃OH

Example of the following type of intermolecular bonding it’s in form: London Dispersion Forces (Nonpolar)

CO₂

CH₄

O₂

N₂

CCl₄

Ionic bond

🔺 greater than 1.7

Polar covalent bond

🔺 0.3-1.7

Non polar covalent bond

🔺0.0 to 0.3

Bond angle of linear geometry

180 degrees

Bong angle of tringonal planar

120 degrees

Bond angle of tetrahedral

109.5