1. . This is just a review of simpler concepts or older material that you should know to be successful. This does not include sample problems, see your study guide for those!

2.  1 mole of NaCl would equal 6.022 x 10 23 atoms. (F…NaCl is compoud) True or False

3.  There are 22.4 Liters of gas in 1 mole of ANY gas at STP.  (T) True or False

4.  In order to find the molar mass of a compound, you need to use the periodic table to look up ATOMIC NUMBERS.  (F…need atomic masses) True or False

5.  1 mole of carbon is equal to 12.011 grams.  (T) True or False

6.  Avogadro’s number is equal to 22.4 L.  (F it is 6.022 * 10 23 ) True or False

7.  1 mole of molecules is equal to Avogadro’s number of molecules  (T) True or False

8.  The mole is a handy conversion factor because it can be equal to so many different things.  (T) True or False

9.  It would be impossible to hold 1 mole of any substance in the palm of your hand.  (F you can hold a mole of H atoms) True or False

10.  The molar mass of Oxygen gas is 16.00 grams  (F…Oxygen gas is diatomic so 32.00 g) True or False

11.  How many sig figs in 12.00?.  (4 sig figs)

12.  How many sig figs in the number 6.022 x 10 23  (4 sig figs)

13.  The formula for Iron (II) Nitride is...  (Fe 3 N 2 )

14.  In order to calculate from mass to moles, you must use Avogadro’s number  (F, you need molar mass) True or False

15.  In order to calculate from moles to liters, you must use the molar mass of the gas.  (F, you need the conversion 22.4L/1mol) True or False

16.  In order to calculate from atoms to moles, you will need to use 6.02 x 10 23.   (T) True or False

17.  How many atoms 1 formula unit of NaOH.   (3)

18.  How many Cl atoms in 1 mole of Carbon Tetrachloride, CCl 4 ? Just show work.  ( 6.022x10 23 x 4)

19.  1 mole of iron atoms is enough for a large building.  (F, it is about the size of ping pong ball) True or False

20.  1 mole of xenon gas will take up much more space than 1 mole of He gas.  (F, 1 mole of all gas = 22.4 L ) True or False

21.  It is impossible to calculate the molar mass of a substance if you do not know its formula.  (T) True or False

22.  Percent composition is found by finding the molar mass of the element and dividing it by the total molar mass of the compound  (T) True or False

23.  C 2 H 2 O is an empirical formula  (T) True or False

24.  H 2 O 2 is an empirical formula  (F) True or False

25.  To find an empirical formula, convert % to g to mole and then find the whole number ratio.  (T) True or False