Poly/mono atomic ions
Polyatomic Ions: ions with more than one Monatomic ions: ions with one single
atom (ex. nitrate has one nitrogen atom atom
and three oxygen)
Acetate – CH3COO-1 Sodium ion – Na+1
Ammonium – NH4+1 Potassium ion – K+1
Bicarbonate – HCO3-1 Calcium ion – Ca+2
Carbonate – CO3-2 Carbon ion – C+4
Chlorate – ClO3-1 Carbide ion – C-4
Hydronium – H3O-1 Chloride ion – Cl-1
Hydroxide – OH-1 Hydrogen ion – H+1
Nitrate – NO3-1 Hydride ion – H-1
Phosphate – PO4-3 Nitride ion – N-3
Sulfate – SO4-2 Phosphide ion – P-3
Sulfide ion – S-2
Non vs spontaneous
- Spontaneous reaction = equilibrium constant > 1.
- ΔG = negative
- Exothermic / Exergonic
- Nonspontaneous reaction = equilibrium constant < 1.
- ΔG = positive
- Endothermic / Endergonic
Mass action expression with Ksp
1. Zn(OH)2(s) ⇌ Zn2+ (aq) + 2OH- (aq)
- Ksp = [Zn2+][OH-]2
[Zn2+] × [OH-]2 [ products ]
Ksp = —————— ————— = K (mass action)
[Zn(OH)2] 1 [ reactants ]
- Solids and pure liquids become 1. Ksp does NOT include solids.
Equilibrium (LeChatelier)
1. increase in pressure = shifts to side with less moles
2. increase in volume = shifts to side with more moles
- 1H3PO4 ⇌ 3H+1 + 1PO4
, - 1 mole ⇌ 3+1=4 moles
Calculate molarity
Molarity = moles of solute/liters of solution
- Convert grams to moles = molar mass
- Convert moles to anything = avogadro’s #
- Low molarity = dilute | high molarity = concentrated
1. Molarity of a 100 mL solution with 0.90g NaCl?
NaCl # of atoms Atomic mass Total mass (g/mol)
Na 1 22.99 58.44 g/mol
Cl 1 35.45
Molarity:
(0.90g NaCl) (1 mole NaCl) 0.90 moles
——————————— = —————— = 0.0154 moles/0.1L = 0.154 M
— 58.44
(58.44g NaCl)
2. Moles of solute in 1.5 liters of 0.70M NaClO?
- 0.70=x/1.5L (M=moles/L)
- x=1.05 (1.1M because 0.70 has two sig figs)
Calculate valence electrons
CH4 # of atoms # of valence total valence
C 1 4e- 8e-
H 4 1e-
Lewis dot
Group A I II III IV V VI VII VIII
elements
# of bonds 1 2 3 4 3 2 1 0
# of lone pairs of 0 0 0 0 1 2 3 4
Polyatomic Ions: ions with more than one Monatomic ions: ions with one single
atom (ex. nitrate has one nitrogen atom atom
and three oxygen)
Acetate – CH3COO-1 Sodium ion – Na+1
Ammonium – NH4+1 Potassium ion – K+1
Bicarbonate – HCO3-1 Calcium ion – Ca+2
Carbonate – CO3-2 Carbon ion – C+4
Chlorate – ClO3-1 Carbide ion – C-4
Hydronium – H3O-1 Chloride ion – Cl-1
Hydroxide – OH-1 Hydrogen ion – H+1
Nitrate – NO3-1 Hydride ion – H-1
Phosphate – PO4-3 Nitride ion – N-3
Sulfate – SO4-2 Phosphide ion – P-3
Sulfide ion – S-2
Non vs spontaneous
- Spontaneous reaction = equilibrium constant > 1.
- ΔG = negative
- Exothermic / Exergonic
- Nonspontaneous reaction = equilibrium constant < 1.
- ΔG = positive
- Endothermic / Endergonic
Mass action expression with Ksp
1. Zn(OH)2(s) ⇌ Zn2+ (aq) + 2OH- (aq)
- Ksp = [Zn2+][OH-]2
[Zn2+] × [OH-]2 [ products ]
Ksp = —————— ————— = K (mass action)
[Zn(OH)2] 1 [ reactants ]
- Solids and pure liquids become 1. Ksp does NOT include solids.
Equilibrium (LeChatelier)
1. increase in pressure = shifts to side with less moles
2. increase in volume = shifts to side with more moles
- 1H3PO4 ⇌ 3H+1 + 1PO4
, - 1 mole ⇌ 3+1=4 moles
Calculate molarity
Molarity = moles of solute/liters of solution
- Convert grams to moles = molar mass
- Convert moles to anything = avogadro’s #
- Low molarity = dilute | high molarity = concentrated
1. Molarity of a 100 mL solution with 0.90g NaCl?
NaCl # of atoms Atomic mass Total mass (g/mol)
Na 1 22.99 58.44 g/mol
Cl 1 35.45
Molarity:
(0.90g NaCl) (1 mole NaCl) 0.90 moles
——————————— = —————— = 0.0154 moles/0.1L = 0.154 M
— 58.44
(58.44g NaCl)
2. Moles of solute in 1.5 liters of 0.70M NaClO?
- 0.70=x/1.5L (M=moles/L)
- x=1.05 (1.1M because 0.70 has two sig figs)
Calculate valence electrons
CH4 # of atoms # of valence total valence
C 1 4e- 8e-
H 4 1e-
Lewis dot
Group A I II III IV V VI VII VIII
elements
# of bonds 1 2 3 4 3 2 1 0
# of lone pairs of 0 0 0 0 1 2 3 4
