Unit: Final Exam Review

Chemistry

Unit: Final Exam Review

1. Using the word bank determine the uses of the following.

1. Use to measure 100 mL of water: ______

1. Use to measure 100.5 mL of water:______

1. Use to test a solution: ______

1. Use to heat and evaporate liquids: ______

1. Using the following diagram determine the amount of liquid in the graduated cylinder. ______mL

1. What is the equation used to determine density?

1. Determine the density of a liquid by using the following information:

Graduated cylinder with liquid: 55 g

Empty graduated cylinder: 50 g

Volume of a liquid in cylinder: 5 mL

1. What do the following Isotopes have in common?

1. Explain Rutherford’s Theory of the atom.

1. An atom that has a mass number of 20 has 10 protons, 10 electrons and how many neutrons?

Using the periodic table answer questions 8-12

1. Determine the electron configuration of the following:

1. He: ______

1. Cl: ______

1. K: ______

1. Which pair has the same electron configuration?

1. Ar and S2-
2. Ar and S
3. Cl and S2-
4. Cl and S

1. Determine the number of valence electrons for each of the following groups on the periodic table.

1. Noble gases: ______

1. Halogens: ______

1. Alkali metals: ______

1. Alkaline earth metals: ______

1. Define the following parts of the periodic table:

1. Families:______

1. Periods: ______

1. Groups: ______

1. Transition metals: ______

1. Which group of elements would be expected to have similar chemical properties?

1. F, Cl, Br
2. B, C, N
3. Ne, Ar, F
4. Al, Si, As, Se

Using the periodic table below answer questions 13-16

1. Which of the following is most likely to be an ionic compound?

1. J and U
2. J and R
3. R and K
4. L and I

1. Which of the following is the most reactive nonmetal?

1. Z
2. Y
3. U
4. L

1. Which element has the lowest electronegavitiy?

1. W
2. K
3. L
4. Z

1. Which of the following has the largest atomic radius?

1. L
2. Y
3. Z
4. R

1. Define Chemical Bonding: ______

1. Determine the shapes and polarity of the following:

1. Determine the number of atoms in each of the following compounds:

1. Ca(OH)2: ______

1. Ca(C2H3O2)2: ______

1. Fe(OH)3: ______

1. Name the following compounds:

1. Fe(OH)2: ______

1. Ca(OH)2: ______

1. KOH: ______

1. H2SO4: ______

1. HCl:______

1. H3PO4: ______

1. Define the following:

1. Endothermic reaction: ______

1. Exothermic reaction: ______

1. Determine which reaction the following graph represents (endo or exo).

1. Determine the products of this chemical reaction:

1. Which of these changes is proof that a chemical reaction has occurred?

1. Formation of a precipitate
2. Change in temperature
3. Disappearance of a solid

1. What are the products of a combustion reaction?

1. Balance the following equation:

1. P4O10 + _____ H2O → _____ H3PO4

1. _____ I2 + ____ NH3 → N2I4 + ____ HI

1. Define the following:

1. Physical change: ______

Example: ______

1. Double replacement: ______

Example: ______

1. Decomposition reaction: ______

Example: ______

1. Using the following equation answer the questions below:

N2(g) + 3H2 2NH3(g)

1. If 16.0 g of nitrogen reacts with excess hydrogen, what mass of ammonia is produced?

1. If 25.0 g of hydrogen reacts with excess nitrogen, what volume of ammonia is produced?

1. A 200 g sample of methane (CH4) contains how many molecules?

1. A compound contains 25% carbon and 75% H by mass. What is the empirical formula of this compound?

1. Using the following information determine the percent error and the source of error:

A student reacts 20.00g of NaHCO3 with excess HCl to produce NaCl, H2O, and CO2.

• The CO2 bubbles.
• Excess H2O and HCl are evaporated by heat, leaving dry NaCl.
• The theoretical yield of NaCl is 13.92 g.
• The student’s experimental yield is 12.00 g.

Percent error: ______

Source of error: ______

1. Define the movement of the following:

1. Solid: ______

1. Liquid: ______

1. Gas: ______

1. True or False: If a capped soda bottle sits in the hot sun the pressure inside the bottle increases because molecules are hitting the walls of the bottle more frequently? ______

1. Which graph below represents the relationship b/w pressure and volume at a constant temperature? ______

1. Which of the graphs below represent the temperature as a function of time for a pure substance as it is heated and changes from a solid to a liquid? ______

1. A gas has a volume of 100 mL at STP. If the pressure remains constant, to what new temperature must the gas be raised to increase the volume to 125 mL?

1. Define the following:

1. Saturated: ______

1. Supersaturated: ______

1. Unsaturated: ______

1. True of False: If you seen a bottle with the following label 0.2 M CaCl2 does it mean that CaCl2 is a solute, and H2O is the solvent? ______

1. Determine the molarity of a 10 g sample of NaCl that dissolves in 1000 mL of solution.

1. Define electrolytes.

1. When NaOH dissolves in water it conducts electricity. NaOH is

1. An electrolyte dissolving as ions
2. A non-electrolyte dissolving as ions

1. What type of compound turns red litmus paper blue? ______

1. Circle any compound below that will turn red litmus paper blue?

1. NaOH
2. HCl
3. KOH
4. H2SO4

1. Which compound below can be a product of a neutralization reaction?

1. NaOH
2. HCl
3. NaCl

1. What volume of 5.00 M KOH is needed to neutralize 0.100 L of 10.00 M HCl?

1. What is the pH of 0.01 M HCl?

1. What is a catalyst and how does it affect a chemical reaction?

1. Define the Law of Conservation of Mass.

1. Give an example where mass is conserved.

1. Using the following ground state electron configuration 1s22s22p63s2

1. Write the correct symbol for the element. ______

1. Identify the element as a metal or nonmetal. ______

1. Write the electron configuration of the most commonly formed ion of the element. ______

1. Predict the elements formula if it bonded with H. ______

1. Draw the Lewis dot structure for this compound (D).

1. Identify the shape of a molecule of this compound (E). ______

1. The complete combustion of ethanol produces carbon dioxide and water according to the following chemical equation:

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l)

1. How many moles of oxygen are necessary to produce 18.0 moles of carbon dioxide?

1. How many grams of carbon dioxide are produced when 1.2 moles of water are produced?

1. How many grams of water are produced in the complete combustion of 100.0 grams of ethanol?

1. An antacid neutralizes excess stomach acid. Students compared the pH of a standard dose of several antacids. Tablets were dissolved in deionized water. The volume of HCl needed to neutralize the recommended dose of each antacid was determined by titration. The results are given in the data table below.

Antacid Brand / pH / Volume of HCl needed to neutralize the antacid (mL)
Mylanta (l) / 9 / 3.0
Mylanta (s) / 7 / 2.0
Pepto-Bismol (s) / 7 / 2.0
Pepto-Bismol (l) / 8 / 2.5
Temp (s) / 7 / 2.0
Rolaids (s) / 7 / 1.7
Maalox (l) / 10 / 3.4
Alka-Seltzer (s) / 6 / 0.0
l = liquid
s = solid

1. Which antacid is best? Explain.

1. Is a liquid or a tablet a better antacid? Explain.

1. Which antacid has the highest hydroxide ion [OH-] concentration? Explain.