Exam 4 and Final Exam Review

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Exam 4 and Final Exam Review General Chemistry I Material Exam 4: Wednesday, Dec 12 th 5:30 6:30 PM Bolton 150 Chapters 1-19 44 multiple choice

1 Exam 4 and Final Exam Review General Chemistry I Material Exam 4: Wednesday, Dec 12 th 5:30 6:30 PM Bolton 150 Chapters multiple choice questions Final Exam: Wednesday, Dec 19 th 3:00-5:00 PM Bolton 150 Chapters 1-19 Two parts, each standardized, each 40 questions (each 55 minutes)

2 Using the review sheet Concept: This is a short name of the concept / will sometimes correspond to title headings in your text or lesson titles in your lecture activity book Example(s): Some descriptions of questions that might fall into these categories or actual numeric problems These are not intended to be comprehensive; rather quick example references to check if this is the category of problems you are struggling with Chapter/pages: Reference in Chang Notes: Use these however you find useful notes to yourself on progress, scheduling, homework problems to check, etc. Strategy: This is what you complete what will you do for this concept Study: most intensive, likely to involve reading portions of the book/working problems in the book or lecture activity book; may need help from outside : need more practice working more problems (you understand it, but you are not very reliable or speedy); working more problems can help Review: you have this concept you just need to review before the test.

3 Chapter 1 1. Iron is more dense than aluminum. A 10.0 g sample of each metal is placed in water. Which metal will displace the most water and why? (A) Aluminum because it will have the largest volume. (B) Aluminum because it will have the smallest volume. (C) Iron because it will have the largest volume. (D) Iron because it will have the smallest volume.

4 2. Which figure depicts a compound? Chapter 1 (A) (C) (B) (D)

5 Chapter 2 3. Which nucleus is an isotope with 2 H? (A) (B) (C) (D) Neutron Proton

6 Chapter 2 4. What describes an ion of silver? (A) The ion has a +1 charge because it has a nuclear charge of 0 and gained 1 electron. (B) The ion has a +1 charge because it has a nuclear charge of 0 and lost 1 electron. (C) The ion has a +1 charge because it has a nuclear charge of +47 and 46 electrons. (D) The ion has a +1 charge because it has a nuclear charge of +47 and 48 electrons.

7 5. Which process determines the percent composition by mass of carbon in g of octane (C 8 H 18 )? Chapter 3 (A) (B) (C) (D) g C 100% g C H g C 8 mol C mol C 100% g C H g C 8 mol C mol C 100% g C 1.01 g H 8 mol C 18 mol H mol C mol H g C 1.01 g H 8 mol C 18 mol H mol C mol H 100% g C 8 mol C mol C

8 Chapter 3 6. The molecules in the reaction vessel react to form NO 2. What is the limiting reactant and what is in excess? (A) (B) 2NO(g) + O 2 (g) 2NO 2 (g) limiting reactant quantity in excess (C) (D)

9 Chapter 4 7. What were the two reactants to produce the reaction shown? (A) K, Cl 2 and Cd(OH) 2 (B) K, O 2, H 2 and CdCl 2 K+ Cl - K+ Cl - Cd(OH) 2 (C) KCl and Cd(OH) 2 (D) KOH and CdCl 2

10 Chapter 4 8. What is the net ionic equation for the reaction of methyl amine (CH 3 NH 2, a weak base) with the strong acid, HCl? (A) H + (aq) + OH (aq) H 2 O(l) (B) CH 3 NH 2 (aq) + H + (aq) CH 3 NH 3+ (aq) (C) CH 3 NH 2 (aq) + HCl(aq) CH 3 NH 3+ (aq) + Cl (aq) (D) CH 3 NH 2 (aq) + H 2 O(l) CH 3 NH 3+ (aq) + OH (aq)

11 Chapter 4 9. What mass (in g) of Molar mass / g mol 1 calcium chloride is needed CaCl to make ml of a M Cl solution? (A) g (C) 1.11 g (B) g (D) 2.22 g

12 Chapter A gas mixture of Ne and CO is shown in the figure. If more CO is added to the container, what will happen? (A) Both X Ne and will P Ne decrease. (B) P Ne will decrease while X Ne will remain constant. (C) X Ne will decrease while P Ne will remain constant. (D) Both X Ne and will P Ne remain constant.

13 Chapter Carbon monoxide will combust in oxygen to produce carbon dioxide. If 2.0 atm of each gas is reacted in a closed rigid container at a constant temperature, what is the total pressure in the container if the reaction yield is 100%? (A) 2.0 atm 2CO(g) + O 2 (g) 2CO 2 (g) (B) 3.0 atm (C) 4.0 atm (D) 6.0 atm

14 Chapter What is the equation for the enthalpy of solution (heat of solution) for methanol (CH 3 OH), a nonelectrolyte? (A) CH 3 OH(l) CH 3 OH(g) (B) CH 3 OH(l) CH 3 OH(aq) (C) CH 3 OH(l) CH 3+ (aq) + OH (aq) (D) CH 3 OH(l) + 3 / 2 O 2 (g) CO 2 (g) + 2H 2 O(l)

15 Chapter What is a possible set of quantum numbers for a ground state electron in beryllium? (A) (1, 0, 1, ½) (B) (1, 1, 0, ½) (C) (2, 0, 0, ½) (D) (2, 1, 0, ½)

16 Chapter What is the ground state electron of Ni 2+? (A) [Ar] 4s 2 3d 8 (B) [Ar] 4s 2 3d 6 (C) [Ar] 4s 2 3d 10 (D) [Ar] 3d 8

17 Chapter What is smaller than Na +? (A) F (B) K + (C) Mg 2+ (D) Na

18 Chapter Which molecule has a non zero formal charge on carbon? (A) (B) (C) H C O O C O O C H (D) H C N

19 Chapter There are two resonance structures for nitrite. What is/are the bond lengths in nitrite? O N O (A) One is a single bond, and one is a double bond. (B) They oscillate between a single bond and a double bond. (C) One bond length that is longer than a single bond but shorter than a double bond. O N O (D) One bond length that is shorter than a single bond but longer than a double bond.

20 Chapter How many sigma and pi bonds are in the molecule shown? (A) 12 σ and 8 π H 3 C (B) 16 σ and 4 π (C) 21 σ and 4 π (D) 25 σ and 4 π O N C O C N CH 3 C C N N CH 3 C H

21 Chapter What is the hybridization of the noted carbons (a and b)? H 2 N (A) C a = sp; C b = sp 2 (B) C a = sp 3 ; C b = sp 2 (C) C a = sp; C b = sp 3 (D) C a = sp 3 ; C b = sp 3 a O b OH

22 Chapter Between NF 3 and NCl 3, which has the highest boiling point and why? (A) NF 3 because it has fewer electrons than NCl 3. (B) NF 3 because it has hydrogen bonding while NCl 3 does not. (C) NCl 3 because it is polar while NF 3 is nonpolar. (D) NCl 3 because it has more electrons than NF 3.

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is