Chemical Bonds and Reactions Chapter Exam

Exam Instructions:

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

Page 1

Question 1 1. How do you determine the amount of product made?

Question 2 2. What is a coefficient?

Question 3 3. Which of the following mole ratio is NOT appropriate to the equation 6CO2+ 6H2 O = C6 H12 O6+ 6O2?

Question 4 4. How many moles of Na are needed to produce 15 moles of NaCl in the reaction 2Na + Cl2 = 2NaCl?

Question 5 5. Given a balanced equation involving A and B, which set of conversions must you make to change mass A to mass B?

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Question 6 6. If 4.0 moles of HCl react with 5.0 moles of NaOH to make NaCl and H2 O in the equilibrium reaction HCl+ NaOH = NaCl + H2 O, what is the limiting reactant?

Question 7 7. Which of the following equations is balanced?

Question 8 8. How is a mole ratio used?

Question 9 9. What was the Kinetic Molecular Theory designed to explain?

Question 10 10. Substances in which phase of matter have the most space between particles?

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Question 11 11. Which of the following is TRUE about most gases?

Question 12 12. Determine the percent yield if the theoretical yield is 20 g and the actual yield is 15 g.

Question 13 13. Why would a scientist have difficulty observing the behavior of an ideal gas?

Question 14 14.

Which of the following statements is true?

I. In an ionic bond, electrons move toward the atom that is more electronegative.

II. A cation is a negatively charged atom.

III. A positively charged atom is called an anion.

IV. Under biological conditions, ionic bonds are stronger than covalent bonds.

Question 15 15. Which of the following is TRUE about ideal gas particles?

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Question 16 16. Determine the actual yield if the theoretical yield is 12 g and the percentage yield is 90%.

Question 17 17. Say you take a reactant A and calculate the amount of moles of another reactant B required to use up all of A. How do you know which of two reactants is the limiting one?

Question 18 18. How many moles of N2 are needed to produce 18 moles NH3 in the reaction N2 + 3H2 = 2NH3?

Question 19 19. Two atoms with the same electronegativity would form what kind of bond?

Question 20 20. Select the most suitable definition for stoichiometry.

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Question 21 21. Which of the following atoms is most likely to participate in an ionic bond with chlorine, an atom with 7 valence electrons?

Question 22 22. The starting point of a stoichiometric problem is _____.

Question 23 23. What is the actual yield?

Question 24 24. What is theoretical yield?

Question 25 25. What does it mean when a collision is elastic?

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Question 26 26. A London Dispersion force is:

Question 27 27.

If a carbon atom has four valence electrons, which of the following statements are true?

I. Carbon can form a triple covalent bond with another carbon atom.

II. A carbon atom cannot form two double bonds simultaneously.

III. A carbon atom can form four single covalent bonds simultaneously.

Question 28 28. If 2.5 moles of zinc react with 6.0 moles of hydrochloric acid in the equation Zn + 2HCl = ZnCl2 + H2, what is the limiting reactant?

Question 29 29. 3.9g of potassium reacts with water to produce potassium hydroxide and hydrogen gas. Calculate the mass of potassium hydroxide produced.

Question 30 30. Conservation of matter means that:

Chemical Bonds and Reactions Chapter Exam Instructions

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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