Exam 2 Flashcards
Electron Configuration
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p
Electron Configuration
- S, P, D, F
s = 2 p = 6 d = 10 f = 14
Ionic Bonding
transfer of electrons (lattices) - metals + non metals
Covalent Bonding
sharing of electrons (non-metals)
Representation
HF - H —-> F
Cl2 - Cl –> Cl
Valences Electrons. How many does each group have?
G1 - 1 valence electron
G2 - 2 valence electrons
G13 - 3 valence electrons
G14 - 4 valence electrons
How is an ionic compound formed?
By the transfer of electrons
Lewis
Na *
Ions
chemical units with number of protons (P+) - different number of electrons
Cation
positive charge - only metals can form this charge
Anion
negative charge (non-metals) F = 9 electrons
Cations and their charges …
G1 - charge +1
G2 - charge +2
G13 - (metals) +3
Cations and their charges rule (G15, G16, G17)
the G number - 18
Ex; Group 15 - 18 = -3
the rules for G15, G16, G17
G15 - 18 = -3
G16 - 18 = -2
G17 - 18 = -1 or just (-)
Naming Binary Ionic Compounds
cation (metal) + anion
Ex; Oxygen = Oxide
Potassium = Nitride
Sulfer = Sulfide
