IB Chemistry – Assignment #1 Name:_________________
1.
Write the formulas of the following common compounds. *These compounds are encountered throughout IB
Chemistry and MUST be memorized. a) Sulfuric acid b) Sodium hydroxide f) Ethanoic acid g) Copper (II) sulfate c) Nitric acid d) Ammonia e) Hydrochloric acid h) Carbon monoxide
i) Sulphur dioxide
j) Sodium hydrogencarbonate
2.
Write formulas of the following substances: a) Sodium chloride f) Calcium phosphate b) Copper (II) sulphide c) Zinc sulphate g) Hydroiodic acid h) Ammonium carbonate d) Aluminum oxide e) Magnesium nitrate i) Methane j) Phosphorus pentachloride
3.
Insert coefficients, to balance the following equations. Re-write equations. a) CaO + HNO
3
 Ca(NO
3
)
2
+ H
2
O b) NH
3
+ H
2
SO
4
 (NH
4
)
2
SO
4 c) HCl + ZnCO
3
 ZnCl
2
+ H
2
O + CO
2 d) SO
2
+ Mg  S + MgO e) Fe
3
O
4
+ H
2
 Fe + H
2
O f) K + C
2
H
5
OH  KC
2
H
5
O + H
2 g) Fe(OH)
3
 Fe
2
O
3
+ H
2
O h) CH
3
CO
2
H + O
2
 CO
2
+ H
2
O i) Pb(NO
3
)
2
 PbO + NO
2
+ O
2 j) NaMnO
4
+ HCl  NaCl + MnCl
2
+ Cl
2
+H
2
O
4.
Write balanced equations for the following reactions. Do your best to provide state symbols for all entities.
Predict products if required. Identify the type of reaction taking place. a) Copper(II) carbonate forming copper(II) oxide and carbon dioxide. b) Nickel oxide reacting with sulphuric acid to form nickel sulphate and water. c) Iron and bromine reacting to give iron(III) bromide. d) Lead(IV) oxide and carbon monoxide forming lead metal and carbon dioxide. e) Iron(II) chloride reacting with chlorine to form iron(III) chloride. f) Ethanol burning in air to form carbon dioxide and water. g) Silver reacting with nitric acid to form silver nitrate, nitrogen dioxide and water. h) Manganese(IV) oxide reacting with hydrochloric acid to form manganese(II) chloride, chlorine and water. i) Sulfur dioxide reacting with hydrogen sulphide to form sulphur and water. j) Ammonia reacting with oxygen to form nitrogen monoxide and water. k) Sodium and chlorine react to produce sodium chloride l) Magnesium displaces hydrogen from hydrochloric acid. m) Aluminum oxide decomposes into its elements n) Lead(II) iodide precipitates out of solution when potassium iodide and lead(II) nitrate react o) Propane (C
3
H
8
) undergoes complete combustion. p) Propane undergoes incomplete combustion q) Lithium is added to water r) Hydrochloric acid is mixed with magnesium hydroxide s) Ethanoic acid is mixed with sodium hydrogen carbonate(baking soda) t) Copper is added to a solution of silver nitrate u) Copper(II) sulfate solution is mixed with sodium hydroxide solution. v) Lithium oxide decomposes into its elements

5. True or False? If the statement is false, make the necessary modifications to make it true. a) _____A negativity charged particle is called a cation. b) _____The symbol
27
13
Al represents an atom that has 27 protons and 13 neutrons. c) _____Elements that have the same number of valence electrons have similar chemical properties. d) _____The Lewis structure for an atom of neon, Ne, has 8 dots around the element symbol. e) _____The atom has a sharply defined outer boundary. f) _____Elements in the periodic table are arranged according to their atomic mass. g) _____In the periodic table, elements that have similar properties are grouped in horizontal rows. h) _____Of the elements, helium, iron, sulfur, calcium, and potassium, the one that would react in a way that is
most like sodium is calcium. i) _____Neutrons and electrons have nearly identical masses. j) _____In the chemical notation
A
Z
X, A is the atomic symbol and Z is the mass number. k) _____Neutral atoms have equal numbers of protons and electrons. l) _____There is no limit to the number of electrons that can occupy each energy level surrounding an atom. m) _____Given the choice of aluminum, magnesium, oxygen, helium, and hydrogen, the element that is least
reactive is oxygen. n) _____Hydrogen-1, hydrogen-2 (deuterium), and hydrogen-3 (tritium) are isotopes that have the same number
of protons but different numbers of electrons. o) _____The Lewis structure for an element that has an atomic number of 12 would have 2 dots. p) ____The most common fluoride ion has 7 valence electrons.