Compound Names and Formulas of Chemical Equations Problems

 

 

Topics: Stock notation, polyatomic ions, compound names and formulas, chemical equations, balancing chemical equations, moles, molar mass (MM), mass to mole conversions, mole to mass conversions, stoichiometry problems = chemical math, patterns of reactions, classes of reactions, chemical bonding, Lewis dot theory, Lewis dot ions, Lewis dot structures of molecules.

Purpose: To review concepts learned in lecture and to demonstrate understanding of the topics listed above. Chemical equations are symbolic representations of chemical reactions (changes). It is possible to calculate the amounts of products that could be formed in a reaction (like pharmaceutical drugs or dyes), or calculate the amounts of reactants needed. To explain the shape and functions of molecules like proteins and illicit drugs, bonding theories like Lewis bonding theory with the octet rule are important.

Tasks: Fill out the boxes or write the ion symbol or formula as specified in each question. Follow the model below.

Model example to answer the homework questions.
E.g. Q100. Based on Johll textbook page 127, Chapter 4, problem 49, b
. (4.6, 4.9) Fill out the table. Look up polyatomic ions as needed. Parentheses needed if 2 or more polyatomic groups, else dropped.
Potassium sulfate + lead(II) nitrate ? + ?


Cation symbols = _
K+___ and ___Pb2+___


Anion symbols = __
SO42-___ and ___NO3___

Product 1 name = ____Potassium nitrate__


Product 2 name = ___
lead(II) sulfate___

Convert names into compound symbols for a chemical equation (unbalanced):

__K2SO4_ + ____Pb(NO3)2____ ___KNO3___ + ____PbSO4____

Write the balanced chemical equation:

K2SO4 + Pb(NO3)2 2 KNO3 + PbSO4

Criteria: Points are specified for each question. Deductions will be made for missing, incomplete, or incorrect responses in 0.5-point increments.

Q1. (3 points) Johll textbook page 127, Chapter 4, question 54, (a) and (c) only. (4.7) Complete the calculations for the moles of each substance. Use units and proper significant digits. See problem 53.

Molar mass of CuNO3 = ______________ g/mol; m = ______ g

Moles, _______________ mol

Molar mass of O2 = ______________ g/mol; m = 21.0 g

Moles, _______________ mol

Q2. (2 points) Johll textbook page 156, Chapter 5, problem 24, all. (5.2) Draw the Lewis structures for atoms. See problem 23.

(a)
Ca

(b)
Rb

(c)
F

(d)
B

Q3. (3 points) Based on Johll textbook page 127, Chapter 4, problem 50, a. (4.6, 4.9) Fill out the table. Look up polyatomic ions as needed. Parentheses needed if 2 or more polyatomic groups, else dropped. See Problem 49.
Cobalt(II) nitrate + sodium hydroxide ? + ?


Cation symbols = ________ and ________


Anion symbols = ________ and ________

Product 1 name = ____________________________


Product 2 name = ____________________

Convert names into compound symbols for a chemical equation (unbalanced):

___________ + ________________ _____________ + _______________

Write the balanced chemical equation:

 

Q4. (4 points) Johll textbook page 127, Chapter 4, problem 60. (4.8). Do the stoichiometry problem for the combustion equation: C3H8(g) + 3 O2(g) 3 CO2(g) + 4 H2O(g) + heat. Complete the calculation templates and find the answers. See Problem 59.

MM of propane = ____ . _______ g/mol

MM of water = ____ . ________ g/mol

Step 1: Mass of water to moles:

_____________ mol H2O

Step 2: Convert to moles of propane:
_____________ mol C3H8

Step 3: Getting the mass of propane (show calculation here):

Q5. (2 points) Johll textbook page 156, Chapter 5, problem 26, (b) and (d). (5.2) Draw the ions in each compound using Lewis dot structures (don’t forget square brackets and charges). See Problem 25.

(b) CaS

(d) K2O

Q6. (2 points) Johll textbook page 128, Chapter 4, problem 62, all. (4.9) Identify the reaction class (type of reaction, not pattern). See Problem 63.

Description

Reaction class (type)

(a) The explosion last night at the railroad terminal was linked to a small leak in the tanker carrying diesel fuel.

 

(b) If the swimming pool pH is greater than 8.0, add muriatic acid to lower the pH.

 

(c) Carbon dioxide from the atmosphere will react with the concentrated sodium hydroxide solution to form an insoluble carbonate.

 

(d) Warning: The whitewall tire cleaner should not be used on metal because it contains hydrofluoric acid.

 

Q7. (4 points) Based on Johll textbook page 157, Chapter 5, problem 32, (a) and (c). (5.2) Draw the Lewis structures in steps by filling out the table. Follow the general strategy as outlined in CHEM 100 lectures, and stick to the octet rule (warning: you will get other bonding structures for SO3 on the web based on more advanced theories using formal charge concepts and non-octet structures). See Problem 31.

(a) H2S
Total valence electrons = ______

(c) SO3
Total valence electrons = _____

Single bond network:

Valence electrons left = _____

Single bond network:

Valence electrons left = ____

Structure after completing outside octets:

Valence electrons left = _____

Structure after completing outside octets:

Valence electrons left = _____

Final structure

Final resonance structures:

(1)

(2)

(3)

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