Chapter 1
Chapter 1
STUDY NOTES IN CHEMISTRY One Ionic and Covalent Bonding, Lewis Structures, Polarity, VSEPR, and Intermolecular Forces (Week Seven - Eleven)
POINTS TO MEMORIZE
One. NaCl is ionic.
Two. CO2 is covalent.
Three. Ionic bonding involves electron transfer.
Four. Covalent bonding involves electron sharing.
Five. Metal plus nonmetal usually result in ionic.
Six. Nonmetal plus nonmetal usually result in covalent.
Seven. CaCO3 has ionic attraction between Ca two plus and CO3 two minus, with covalent bonds within CO3 two minus.
Eight. The octet rule involves achieving a stable valence-shell arrangement.
Nine. CO2 is written O equals C equals O.
Ten. NH3 has three bonds plus one lone pair.
Eleven. H2O has two bonds plus two lone pairs.
Twelve. CO2 is linear and nonpolar.
Thirteen. H2O is bent and polar.
Fourteen. NH3 is trigonal pyramidal and polar.
Fifteen. VSEPR is based on repulsion between electron domains.
Sixteen. London dispersion forces occur in all atoms and molecules.
Seventeen. HCl experiences dipole-dipole attractions.
Eighteen. H2O can form hydrogen bonds.
Nineteen. Stronger intermolecular forces generally mean higher boiling point.
Twenty. Boiling generally overcomes intermolecular forces, not the covalent bonds within the molecules.
IONIC AND COVALENT COMPOUNDS
IONIC AND COVALENT COMPOUNDS
A. Ionic Compounds What is an ionic compound?
An ionic compound forms when electrons are generally transferred from one atom to another, producing oppositely charged ions.
Metal loses electrons positive ion (cation)
Nonmetal gains electrons negative ion (anion)
The oppositely charged ions attract through electrostatic forces.
Example: NaCl
Na loses one electron.
Sodium loses one electron.
Cl gains one electron.
Chlorine gains one electron.
Therefore: Na plus Cl minus equals NaCl