CP Chemistry Midterm REVIEW GUIDE Units 1-6 (do on another piece of paper)
____ 1. Which of the following is a chemical change?
a. / Evaporation / c. / rustingb. / Freezing / d. / Boiling
____ 2. The diameter of a sulfur atom is 0.000 000 00 293 L. What is this number expressed in scientific notation?
____ 3. How many significant figures are in the measurement 361.98 grams?
____ 4. What is the measurement 2039 L rounded off to three significant digits?
____ 5. What is the temperature of absolute zero measured in C?
____ 6. All atoms of the same element have the same ____.
a. / number of neutrons / c. / mass numbersb. / number of protons / d. / mass
____ 7. Which of the following sets of symbols represents isotopes of the same element?
a. / C C C / c. / E E Eb. / H H H / d. / M M M
____ 8. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements? (KNOW YOUR SCIENTITSTS!!!)
____ 9. In looking at the periodic table, which are there more of? Metals or Nonmetals?
____ 10. Of the elements Ti, Ag, K, and He, which is a nonmetal?
____ 11. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p, 4s?
____ 12. What is the number of electrons in the outermost energy level of a nitrogen atom?
____ 13. What is the electron configuration of calcium?
____ 14. How many electrons does fluorine gain in order to achieve a noble-gas electron configuration?
____ 15. Know the difference between an ionic bond and a covalent bond.
____ 16. What is the shape of the water molecule? What is the shape of CO2?
____ 17. Which atom in a water molecule has the greatest electronegativity? (The oxygen atom or the hydrogen atoms?)
____ 18. Name the following polyatomic ions? HCO, CO, NO, SO, CrO, CrO
____ 19. Create the proper ionic compounds with the ions in a – d. (REMEMBER THE “CRISS CROSS” METHOD WE DID WITH THE ION DICE!!)
a. / Ca2+, F =(write the formula of the compound here) ______/ c. / Ba, O =
(write the formula of the compound here) ______
b. / Na, Cl =
(write the formula of the compound here) ______/ d. / Pb, O =
(write the formula of the compound here) ______
____ 20. Write the correct formula for the ionic compound in a – d.
a. / iron(III) sulfide / c. / tin(II) nitrideb. / aluminum fluoride / d. / potassium bromide
____ 21. Which set of chemical name and chemical formula for the same compound is correct?
a. / ammonium sulfite, (NH)S / c. / lithium carbonate, LiCOb. / iron(III) phosphate, FePO / d. / magnesium dichromate, MgCrO
____ 22. What is the formula for sulfurous acid?
____ 23. List the 7 diatomic molecules?
____ 24. How many moles of copper are in 4.8 10 atoms of copper?
____ 25. How many molecules are in 2.10 mol SO?
____ 26. What is the molar mass of AgBr3?
____ 27. What is the volume (in liters) of one mole of a gas under STP conditions?
____ 28. What is the percent by mass of hydrogen in acetone, CHO?
____ 29. What is the empirical formula of C8H24O64?
____ 30. What is the empirical formula of a substance that is 52.2% C, 17.4% H, and 30.4% N by weight?
____ 31. Balance the following chemical equation?
CuCl + KOH Cu(OH) KCl
____ 32. In order for the reaction 2Fe 6HCl 2FeCl 3H to occur, which of the following must be true?
a. / Fe must be above Cl on the activity series.b. / Fe must be above H on the activity series.
c. / Heat must be supplied for the reaction.
d. / A precipitate must be formed.
____ 33. Which of the following is a balanced equation representing the decomposition of tin (IV) oxide?
a. / SnO Sn 2O / c. / SnO 2Sn Ob. / SnO Sn O / d. / SnO Sn O
____ 34. A double-replacement reaction takes place when aqueous NaCO reacts with aqueous Sn(NO). What are the 2 products in this reaction?
____ 35. The equation Mg(s) 2HCl(aq) MgCl(aq) H(g) is an example of which type of reaction? (YOU MUST KNOW THE 5 TYPES OF CHEMICAL REACTIONS!)
____ 36. Balance the following equation and determine what type of reaction this is:
S(s) + O(g) ® SO(g)
____ 37. Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 13.2 mol of aluminum?
2Al(s) + 3HSO(aq) ® Al(SO)(aq) + 3H(g)
____ 38. The equation below shows the decomposition of lead (II) nitrate. How many grams of oxygen are produced when 12.7 g NO is formed?
____ 39. How many liters of NH are needed to react completely with 21.4 L of NO (at STP)?
4NH(g) + 6NO(g) 5N(g) + 6HO(g)
____ 40. Which of the following is NOT true about limiting and excess reagents?
a. / The amount of product obtained is determined by the limiting reagent.b. / A balanced equation is necessary to determine which reactant is the limiting reagent.
c. / Some of the excess reagent is left over after the reaction is complete.
d. / The reactant that has the smallest given mass is the limiting reagent.
____ 41. How many liters of fluorine gas can be produced when 0.98 L of HF react with excess O at STP? 4HF(g) + O(g) 2F(g) + 2HO(g)
____ 42. Identify the limiting reagent and the volume of NO formed when 11 L NS reacts with 18 L O to produce NO gas and SO gas at STP.
NS(g) + 3O(g) NO(g) + 2SO(g)