Messenger_creation_4852507814974550.jpeg

# Advanced Placement Chemistry ## Summer Assignment Welcome to AP Chemistry! I am excited that you have decided to take on the challenges of college-level chemistry. This course will be rigorous and will require dedication and hard work throughout the year. However, if you are willing to put in th...

# Advanced Placement Chemistry ## Summer Assignment Welcome to AP Chemistry! I am excited that you have decided to take on the challenges of college-level chemistry. This course will be rigorous and will require dedication and hard work throughout the year. However, if you are willing to put in the effort, I am confident that you will be successful and gain a deep understanding of chemistry. ### Purpose of this Assignment This summer assignment is designed to help you review some of the fundamental concepts that you learned in your first-year chemistry course. It will ensure that we can hit the ground running when the school year begins. By completing this assignment, you will strengthen your understanding of key topics and develop essential skills that will be utilized throughout the AP Chemistry course. ### Content Covered The assignment covers the following topics: 1. Nomenclature 2. Stoichiometry 3. Solution Chemistry 4. Atomic Structure 5. Periodic Trends ### Expectations * All work must be shown for calculations to receive credit. * The assignment must be completed individually. * The assignment is due on **the first day of class.** Late submissions will not be accepted. ### Grading This summer assignment will count as a grade. It is important to complete the assignment to the best of your ability, as it will provide a foundation for future learning in the course. ### How to Submit The completed assignment should be submitted in class on the first day. Make sure your name is clearly written on the assignment. ### Additional Resources To assist you in completing the assignment, you may find the following resources helpful: * Your chemistry textbook from your first-year chemistry course * Online chemistry resources (e.g., Khan Academy, Chem LibreTexts) * Chemistry videos on YouTube ### Contact Information If you have any questions or need clarification on any of the topics covered in this assignment, please do not hesitate to contact me via email. I will do my best to respond to your inquiries in a timely manner. ### Nomenclature Write the formula for the following compounds: 1. Sodium Sulfide: $Na_2S$ 2. Magnesium Chloride: $MgCl_2$ 3. Aluminum Oxide: $Al_2O_3$ 4. Copper(II) Nitrate: $Cu(NO_3)_2$ 5. Iron(III) Carbonate: $Fe_2(CO_3)_3$ 6. Lead(II) Chromate: $PbCrO_4$ 7. Ammonium Phosphate: $(NH_4)_3PO_4$ 8. Potassium Permanganate: $KMnO_4$ 9. Hydrochloric Acid: $HCl$ 10. Sulfuric Acid: $H_2SO_4$ Write the names for the following compounds: 1. $KBr$: Potassium Bromide 2. $Li_2O$: Lithium Oxide 3. $CaCl_2$: Calcium Chloride 4. $Sn(SO_4)_2$: Tin(IV) Sulfate 5. $FeCl_3$: Iron(III) Chloride 6. $HgO$: Mercury(II) Oxide 7. $Cu(NO_2)_2$: Copper(II) Nitrite 8. $(NH_4)_2CO_3$: Ammonium Carbonate 9. $HNO_3$: Nitric Acid 10. $H_2CO_3$: Carbonic Acid ### Stoichiometry 1. What is the mass of 1 mol of $(NH_4)_2S$? $(14.01 \cdot 2) + (1.01 \cdot 8) + 32.07 = 68.17 \, g/mol$ 2. How many moles are there in 45 grams of $C_6H_{12}$? $C_6H_{12} = (12.01 \cdot 6) + (1.01 \cdot 12) = 84.18 \, g/mol$ $45 \, g \cdot \frac{1 \, mol}{84.18 \, g} = 0.53 \, mol$ 3. How many molecules are there in 28 grams of $CO_2$? $CO_2 = 12.01 + (16.00 \cdot 2) = 44.01 \, g/mol$ $28 \, g \cdot \frac{1 \, mol}{44.01 \, g} \cdot \frac{6.022 \cdot 10^{23} \, molecules}{1 \, mol} = 3.8 \cdot 10^{23} \, molecules$ 4. How many grams of $NaCl$ are there in 5.0 moles? $NaCl = 22.99 + 35.45 = 58.44 \, g/mol$ $5.0 \, mol \cdot \frac{58.44 \, g}{1 \, mol} = 292.2 \, g$ 5. What is the percent composition of copper(II) chloride? $CuCl_2 = 63.55 + (35.45 \cdot 2) = 134.45$ $\%Cu = \frac{63.55}{134.45} \cdot 100 = 47.27 \%$ $\%Cl = \frac{35.45 \cdot 2}{134.45} \cdot 100 = 52.73 \%$ 6. Determine the empirical formula of a compound containing 63.50% silver, 8.25% nitrogen, and the remainder oxygen. $Ag: \frac{63.50}{107.87} = 0.5887 \, mol / 0.5887 = 1$ $N: \frac{8.25}{14.01} = 0.5889 \, mol / 0.5887 = 1$ $O: 100 - 63.50 - 8.25 = 28.25$ $\frac{28.25}{16.00} = 1.766 \, mol / 0.5887 = 3$ $AgNO_3$ 7. Determine the empirical formula of a compound containing 27.29% C, 2.29% H, and 70.42% O. $C: \frac{27.29}{12.01} = 2.272 \, mol / 2.272 = 1$ $H: \frac{2.29}{1.01} = 2.267 \, mol / 2.272 \approx 1$ $O: \frac{70.42}{16.00} = 4.401 \, mol / 2.272 \approx 2$ $CHO_2$ 8. Butane gas ($C_4H_{10}$) reacts with oxygen gas to form carbon dioxide and water. a. Write the balanced chemical equation for this reaction. $2C_4H_{10} + 13O_2 \rightarrow 8CO_2 + 10H_2O$ b. How many grams of $CO_2$ are produced when 5.0 grams of $C_4H_{10}$ reacts with excess oxygen? $C_4H_{10} = (12.01 \cdot 4) + (1.01 \cdot 10) = 58.14 \, g/mol$ $CO_2 = 12.01 + (16.00 \cdot 2) = 44.01 \, g/mol$ $5.0 \, g \, C_4H_{10} \cdot \frac{1 \, mol \, C_4H_{10}}{58.14 \, g \, C_4H_{10}} \cdot \frac{8 \, mol \, CO_2}{2 \, mol \, C_4H_{10}} \cdot \frac{44.01 \, g \, CO_2}{1 \, mol \, CO_2} = 15.14 \, g \, CO_2$ 9. Consider the following reaction: $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$ If 10.0 g of $N_2$ react with 3.0 g of $H_2$, calculate the mass of $NH_3$ produced. $N_2 = 14.01 \cdot 2 = 28.02 \, g/mol$ $H_2 = 1.01 \cdot 2 = 2.02 \, g/mol$ $NH_3 = 14.01 + (1.01 \cdot 3) = 17.04 \, g/mol$ $10.0 \, g \, N_2 \cdot \frac{1 \, mol \, N_2}{28.02 \, g \, N_2} \cdot \frac{2 \, mol \, NH_3}{1 \, mol \, N_2} \cdot \frac{17.04 \, g \, NH_3}{1 \, mol \, NH_3} = 12.16 \, g \, NH_3$ $3.0 \, g \, H_2 \cdot \frac{1 \, mol \, H_2}{2.02 \, g \, H_2} \cdot \frac{2 \, mol \, NH_3}{3 \, mol \, H_2} \cdot \frac{17.04 \, g \, NH_3}{1 \, mol \, NH_3} = 16.87 \, g \, NH_3$ $N_2$ is the limiting reactant, so $12.16 \, g \, NH_3$ is produced. 10. When $KClO_3$ is heated, it decomposes to form $KCl$ and $O_2$. If 20.0 g of $KClO_3$ is heated and produces 6.5 g of $O_2$, what is the percent yield of the reaction? $2KClO_3 \rightarrow 2KCl + 3O_2$ $KClO_3 = 39.10 + 35.45 + (16.00 \cdot 3) = 122.55 \, g/mol$ $O_2 = 16.00 \cdot 2 = 32.00 \, g/mol$ $20.0 \, g \, KClO_3 \cdot \frac{1 \, mol \, KClO_3}{122.55 \, g \, KClO_3} \cdot \frac{3 \, mol \, O_2}{2 \, mol \, KClO_3} \cdot \frac{32.00 \, g \, O_2}{1 \, mol \, O_2} = 7.83 \, g \, O_2$ $\frac{6.5 \, g}{7.83 \, g} \cdot 100 = 83.0 \%$ ### Solution Chemistry 1. What is the molarity if 14 grams of $Cu(NO_3)_2$ is dissolved in 0.35 liters of water? $Cu(NO_3)_2 = 63.55 + (14.01 \cdot 2) + (16.00 \cdot 6) = 187.57 \, g/mol$ $\frac{14 \, g}{0.35 \, L} \cdot \frac{1 \, mol}{187.57 \, g} = 0.21 \, M$ 2. What is the molarity if 1.2 moles of $NaCl$is dissolved in 4600 mL of water? $4600 \, mL = 4.6 \, L$ $\frac{1.2 \, mol}{4.6 \, L} = 0.26 \, M$ 3. How many grams of $CaCl_2$ would be required to make 1.0 liter of a 0.10 M solution? $CaCl_2 = 40.08 + (35.45 \cdot 2) = 110.98 \, g/mol$ $\frac{0.10 \, mol}{1 \, L} \cdot 1 \, L \cdot \frac{110.98 \, g}{1 \, mol} = 11.1 \, g$ 4. What volume of a 0.25 M solution can be made using 5.5 grams of $KCl$? $KCl = 39.10 + 35.45 = 74.55 \, g/mol$ $5.5 \, g \, KCl \cdot \frac{1 \, mol \, KCl}{74.55 \, g \, KCl} = 0.0738 \, mol \, KCl$ $M = \frac{mol}{L} \rightarrow L = \frac{mol}{M}$ $L = \frac{0.0738 \, mol}{0.25 \, M} = 0.295 \, L$ ### Atomic Structure 1. Write the electronic configurations for the following atoms or ions: a. $N$: $1s^22s^22p^3$ b. $Ca$: $1s^22s^22p^63s^23p^64s^2$ c. $Cl^-$: $1s^22s^22p^63s^23p^6$ d. $Fe^{2+}$: $1s^22s^22p^63s^23p^63d^6$ ### Periodic Trends 1. For each of the following pairs, indicate which one has the larger radius: a. Na or Cs: Cs (Cesium) b. Mg or Cl: Mg (Magnesium) c. $K^+$ or $Cl^-$: $Cl^-$ (Chloride) 2. For each of the following pairs, indicate which one has the higher ionization energy: a. Li or K: Li (Lithium) b. $S$ or $Cl$: $Cl$ (Chlorine) c. Mg or P: P (Phosphorus)