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Chemistry Bell Work Assignments

A series of chemistry bell work exercises covering types of bonding, molecular structure, ideal gas law, partial pressures, and more. Ideal for students to practice key concepts in chemistry.

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Chemistry Bell Work Assignments

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  1. Bell Work 1 / Types of Bonding What are the three types of bonds? List 4 characteristics of a Ionic bond. 3. What is the difference between a substitutional alloy and Interstitial Alloy?

  2. Bell Work 2 / Semiconductors • Explain how a semiconductor works. 2. Explain the difference between n-doping and p-doping.

  3. Bell Work 3 / Covalent bonds • List the 7 diatomic gases. 2. Describe what it means if an element or compound is paramagnetic or dimagnetic

  4. Bell Work 4 / Formal Charges 1. Predict the molecular structure, bond angles, and hybridization for the following: a. SeO3 b. SeO2 2. Determine the formal charge on each element in the compounds from problem number 1.

  5. Bell Work 5 / Molecular Structure 1. Draw the Lewis dot structure for the following compounds. Then, determine if the bond is dipole and if the molecule is dipole. a. SO4 -2 b. SO3-2 c. ClO3-1

  6. Bell work 6 / IMF’s • What are the three IMF’s? 2. Which has the most influence on physical properties? 3. Which of the following compounds would have the highest boiling point and explain why? a. CH4 or H2S  b. pure water or table salt  c. HF or HCl d. NH3 or PH3e. Water or CH4

  7. Bell Work 7 / Combined Gas Law Ideal Gas Law • A balloon filled with gas at a pressure of 102.3 kPa and a temperature of 45.5o C. Its volume under these conditions is 12.5 L. The balloon is then taken into a decompression chamber and brought to STP what is the volume of the balloon in the chamber? 2. Find the number of grams of CO2 that exert a pressure of 785 torr at a volume of 32.5 L and a temperature of 32 C. 3. What is the density of NH3 at 720. torr and 25 C? (Density = R ∙ Temp / molar mass ∙ Pressure

  8. Bell Work 8 / Ideal Gas Law 1. Find the number of grams of CO2 that exert a pressure of 785 torr at a volume of 32.5 L and a temperature of 32 C. 2. What is the density of NH3 at 720. torr and 25 C? (Density = R ∙ Temp / molar mass ∙ Pressure

  9. Bell Work 9/ Partial Pressures • A container of gases consists of the following mixture of gases: 2.0 moles of helium, 6.0 moles of carbon dioxide, 10.0 moles of neon, and 12.0 moles of xenon. If the total pressure is 900.0 mm of Hg, determine the partial pressure of each gas. 2. Nitrogen is collected over water at 21.5C. What is the partial pressure of nitrogen if the atmospheric pressure is 99.4 kPa? 3. Argon is collected over water at 30C. Find the pressure of the dry gas if the barometric pressure is 0.975 atm.

  10. Bell Work 10 / Gas Laws A sample containing 15.0 grams of dry ice (CO2(s)) is put into a balloon and allowed to sublime according to the following reaction: CO2 (s)  CO2 (g). 1. How big will the balloon be at 22 °C and 1.04 atm after all the dry ice has sublimed?

  11. Bell Work 10 / Gas Laws A sample containing 15.0 grams of dry ice (CO2(s)) is put into a balloon and allowed to sublime according to the following reaction: CO2(s)  CO2 (g). 1. How big will the balloon be at 22 °C and 1.04 atm after all the dry ice has sublimed? 15g CO2 x 1 mole = 0.341 moles 44.0 grams PV = nRT (1.04atm) V = (0.341 moles) (0.0821) (295) V = 7.94 Liters

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