PRACTICE TEST for EXAM 4: the REACTIONS of MATTER
PRACTICE TEST for EXAM 4: THE REACTIONS OF MATTER
1. Prepare a summary (in the format of your choice) of the study guide for Unit 4.
2. For the reactionHCl (aq) + NaHCO3 (s) NaCl (aq) + CO2 (g) + H2O (l)
a. Identify the reactants and the products.
b. Describe the state of each substance in the equation.
3. Balance each equations in lowest terms and do the stoichiometry problem.
a. C5H12 (l) + O2 (g) CO2 (g) + H2O (l)
How many grams of CO2 form when 0.050 moles of C5H12 react?
b. Br2 (l) + F2 (g) BrF3 (g)
How many moles of BrF3 form when 5.98 g of Br2 react?
c. (NH4)2Cr2O7 (s) H2O (l) + N2 (g) + Cr2O3 (s)
How many grams of (NH4)2Cr2O7 are consumed when 25 g of Cr2O3 form?
d. ZnCl2 (aq) + KOH (aq) Zn(OH)2 (s) + KCl (aq)
How many grams of ZnCl2 will react with 0.168 g KOH?
e. Mg (s) + HCl (aq) MgCl2 (aq) + H2 (g)
How many moles of HCl are needed to react with 0.45 g Mg?
f. Na2CO3 (aq) + CaCl2 (aq) NaCl (aq) + CaCO3 (s)
How many moles of NaCl will form when 0.138 mol CaCO3 are produced?
g. C2H5OH (l) + O2 (g) CO2 (g) + H2O (l)
How many grams of O2 are needed to react with 12.85 g C2H5OH?
h. Br2 (aq) + KI (aq) KBr (aq) + I2 (aq)
How many moles of KBr form when 0.40 moles of Br2 react?
4. Identify each reaction as exothermic or endothermic and do the stoichiometry problem.
a. 2 H2 + O2 2 H2O + 572 kJ
How much energy (in kJ) is released when 3.6 g H2O form?
b. 88 kJ + PCl5 PCl3 + Cl2
How many moles of PCl5 can be decomposed with 460 kJ of energy?
c. 247 kJ + CH4 + CO2 2 CO + 2 H2
How much energy is consumed when 54 g CO are produced?
d. N2H4 + 2 H2O2 N2 + 4 H2O + 818 kJ
How many grams of H2O2 are needed to produce 3500 kJ?
5. a. List the number of protons, neutrons, and electrons in an atom of
i. 3H ii. 63Cu iii. 207Pb
b. Identify each atom and write its symbol
i. 6 protons, 8 neutrons, 6 electrons ii. 53 protons, 78 neutrons, 53 electrons
6. Fill in this description of ions:
A metals tends to ______valence electrons to form a _____ ion, which is called a ______.
(gain, lose) ( +, – ) (cation, anion)
A nonmetal tends to ______valence electrons to form a _____ ion, which is called a ______.
(gain, lose) ( +, – ) (cation, anion)
A cation is ______than its parent atoms, and an anion is ______than its parent atom.
(larger, smaller) (larger, smaller)
7. Draw Lewis dot structures for each of these molecules.
a. CCl4 b. ClO21– c. NO21– d. PH3 e. CH2O
8. a. Compare/contrast the three major types of bonding: covalent, ionic, and metallic
b. Identify the type of bonding in each of these substances:
i. NH3 ii. K2O iii. Fe iv. C6H12O6 v. H2O vi. CuCl2 vii. Au
9. On a blank periodic table, fill in the period numbers, group numbers, and staircase; label the alkali metal, alkaline earth, halogen, and noble gas families; indicate the nonmetal, semi-metal, metal, and transition metal regions; add the trends in atomic size and ionization energy.
Answers to UNIT 4 PRACTICE TEST
2. For the reactionHCl (aq) + NaHCO3 (s) NaCl (aq) + CO2 (g) + H2O (l)
a. The reactants are HCl and NaHCO3. The products are NaCl, CO2 and H2O.
b. NaHCO3 is solid, H2O is liquid, CO2 is a gas, and HCl and NaCl are aqueous (dissolved in water).
3. a. 1, 8, 5, 611 g CO2e. 1, 2, 1, 10.037 mol Mg
b. 1, 3, 20.0748 mol BrF3f. 1, 1, 2, 10.276 mol NaCl
c. 1, 4, 1, 141 g (NH4)2Cr2O7 g. 1, 3, 2, 326.78 g O2
d. 1, 2, 1, 20.204 g ZnCl2 h. 1, 2, 2, 10.80mol KBr
4. a. exothermic, 57 kJ b. endothermic, 5.2 mol c. endothermic, 238 kJ d. exothermic, 290 g
5. a. i. 1, 2, 1 ii. 29, 34, 29 iii. 82, 125, 82b. i. 14C ii. 131I
6. A metal tends to lose valence electrons to form a positive ion, which is called a cation .
A nonmetal tends to gain valence electrons to form a negative ion, which is called an anion .
A cation is smaller than its parent atoms, and an anion is larger than its parent atom.
7. (Draw Lewis dot structures for each of these molecules.) See me for the dot structures.
a. CCl4 b. ClO21– c. NO21– d. PH3 e. CH2O
8a. In covalent bonding, nonmetals share valence electrons with other nonmetals so that each atom is surrounded by 8 (or 2, for H). The atoms stay with their valence e– to form molecules. The molecule has no charge, so it does not conduct electricity in any state.
In ionic bonding, metals transfer e– to nonmetals; as a result, the metals form positive ions (cations) and the nonmetals form negative ions (anions), which stick together because of the attraction of their opposite charges. The ions collect into crystals but do not stay with their own electrons to form molecules. The ions can conduct electricity if they are free to move (liquid or dissolved in water).
In metallic bonding, metal atoms release their valence electrons, forming a lattice of positive ions in a “sea” of mobile electrons that holds the metal cations together. The electrons are free to move, so metals conduct in both the solid and the liquid state.
8b. i. NH3 covalent ii. K2O ionic iii. Fe metallic iv. C6H12O6 covalent v. H2O covalent
vi. CuCl2 ionic vii. Au metallic