Reactions with Oxygen
Equation
4Na (s) + O2 (g) -> 2Na2O (s)
2Mg (s) + O2 (g) -> 2MgO (s)
4Al (s) + 3O2 (g) -> 2Al2O3 (s)
Rate of reaction
Vigorously
Vigorously
Vigorously
Sl (s) + O2 (g) -> SiO2 (s)
4P (s) + 5O2 (g) -> P4O10 (s)
S (s) +O2 (g) -> 5O2 (g)
Slowly
Vigorously
Gently
Reactions with Chlorine
Equation
2Na (s) + Cl2 (g) -> 2NaCl (s)
Mg (s) + Cl2 (g) -> MgCl2 (s)
2Al (s) + 3Cl2 (g) -> Al2Cl6 (s)
Si (s) + 2Cl (g) -> SiCl4 (s)
2P (s) + 5Cl2 (g) -> 2PCl5 (l)
Rate of reaction
Vigorously
Vigorously
Vigorously
Slowly
Slowly
Reaction of Sodium Magnesium with Water
Equation
2Na (s) + 2H2O (l) -> 2NaOH (aq) + H2 (g)
Mg (s) + 2H2O (l) -> Mg(OH)2 (aq) + H2 (g)
Mg (s) + H2O (g) -> MgO (s) + H2 (g)
Product color
White
Flame color
Yellow
White
Powder (white residue)
White cloud
Yellow/White
Blue
Product color
White
White solid
Pale yellow
Flame color
Bright orange
White
Probably white
White
Probably white
Temperature
Cold
Cold
Hot
Reaction with Water on Oxides and Hydroxides
Equation
Na2O (s) + H2O (l) -> 2NaOH (aq)
MgO (s) + H2O (l) -> Mg(OH)2 (aq)
Al2O3 (s) + 2NaOH (aq) + 3H2O (l) -> 2NaAl(OH)4 (aq)
Al2O3 (s) + 3NaOH (aq) -> Al2(SO4)3 (aq) + 3H2O (l)
P4O10 (s) +CH2O (l) -> 4H3PO4 (aq)
SO3 (g) + H2O (l) -> H2SO4 (aq)
Acid or base
Base (strong)
Base (weak)
Base
Reaction rate
Vigorous
Vigorous
Notes
Oxidation #
+1
+2
+3
+4
+5
Rate of reaction
Quickly
Slowly
Vigorously
Temp.
Melting point
High
High
High
Hot
High
Low
Low
Notes
Giant ionic compound
Giant ionic compound g 2
Simple molecular compound
Simple molecular compound
Simple molecular compound
Notes
pH 14
pH 11
Acid or base
Acid -> Base (strong)
Acid -> Base (weak)
Acid or base
(amphoteric)
Neutral
Acid
Acid
Size
Giant ionic
Giant ionic
Giant ionic
Giant ionic
Small compound
Small compound
Effect of Water on Chlorides chart on pg 172
Everything is acidic basically
Formula
Bonding
+
NaCl (s) -> Na (aq) + Cl (aq)
Structure
Observations
pH
Yellow-sodium
White-aluminum
Phosphorous-yellow/white
Copper- green
Strontium-red/purple
Check up questions
1. a. Br
b. They originally ranged the periodic table by mass, but then arranged it by proton number because there are different ionic
masses. They would not be in the same colomn where they would react similarly to the same elements in the group. Iodine (127) should
be where solarium (128) is and solarium should be where iodine is.
c. The electrons in the s shell and electrons are in the p orbital
Lithium is going to give away its election. Fluorine will take an electron. Fluorine is smaller because it has more electrons and proteins will
pull. Lithium has a wider radius. Greater electrons in the right side.. More electrons -> More protons that shrink the outer shell.
Lithium+ lost an electron so it has gotten smaller. Lithium is larger than lithium+.
Decreases moving left to right. Atomic radius increases to right. Ionic radius decreases to the right. Relative size decreases to the right.
Nuclear charge increases going across the period. Anions decrease in size from phosphorous to chlorine as nuclear charge increases.
Pg 164.
Sulfur is a covalent simple molecular molecule. Silicon is a giant molecular compound. Silicon has more vanderwals forces and a higher
melting point.
Sulfur is S8. It has a higher melting point and it is a covalent compound that is a solid. It has stronger bonds and greater vanderwals
forces. Cl2 is a gas so it has a lower melting point, less strong bonds and weaker vanderwals forces.
Mg vs. Sodium. Both metals with a sea of delocalized electrons. Na +1, Mg +2, magnesium has more electrons to give. For every 2
protons, there are 2 electrons along it to make it a big sea of electrons (if you’re drawing it out)
Aluminum is in the P shell. Mg is in the S shell.
The P orbital of Sulfur would loose its first electron. Phosphorous is more stable so it won’t let that electron go away that quickly. 3p4 3p3
Se is between Sulfur and Oxygen so it has to be lower than 1,000 because it is going to be in the 4px2y1z1 and give its electron away
easily like the sulfur.