1. 1 Chemistry Midterm Review

2. 2 Problem Solving 1. A piece of ice has a mass of 9.2 g and a volume of 10.0 cm 3. a.What is the density of ice? b.Would the ice float in liquid water (d = 1.0 g/mL)? c.Would this ice float in gasoline (d = 0.7 g/mL)? 2. The density of silicon is 2.33 g/cm 3. What is the volume of a piece of silicon that has a mass of 83.8 g? 3. Helium boils at 4 K. What is this temperature in degrees Celsius?

3. 3 The earth’s circumference is 2.4901x10 4 miles. How many centimeters is this? (2.54 cm = 1 in) If you can swim 3 miles per hour, how many seconds will it take for you to swim to England (6000 km from VA Beach)? (1 m = 1.094 yd, 1760 yds = 1 mile)

4. 4 Matter and Change Give three examples of a chemical property. Give three examples of a physical property. List 2 examples of a chemical change paper can undergo. Now list two for paper. Give three examples for each homogeneous and heterogeneous mixtures. How would you separate each mixture? If 34.9 grams of magnesium reacts with 60.4 grams of oxygen, how many grams of magnesium oxide are formed?

5. 5 Atoms Complete the table: Element Number of protons Number of electron Number of neutrons Atomic number Mass number Manganese25 30 1112 Bromine35 45 3989 Arsenic 33 75 Actinum 227

6. 6 How many neutrons are in each atom? – 238 92 U – 81 35 Br The two most abundant isotopes of carbon are carbon-12 (mass=12.0 amu) and carbon-13 (mass=13.0 amu). Their relative abundances are 98.9% and 1.10%, respectively. Calculate the atomic mass of carbon. How many electrons are lost or gained to form: –Fe 3+ –O 2-

7. 7 Define isotope. The most common isotope of carbon is carbon-12 ( 12 6 C). Suggest two isotopes of carbon.

8. 8 List the four quantum numbers and what they mean. Define aufbau principle, Pauli exclusion principle, and Hund’s rule Describe Bohr’s model and the quantum mechanical model of the atom. Give a brief description of the major contributions to atomic theory.

9. 9 How many ORBITALS are in the following sublevels? –4f –6d –7s –4p –3s Write electron configurations for: –Vanadium –Antimony –Barium

10. 10 Write the symbol for alpha, beta, and gamma radiation. 32 P undergoes beta radiation. –Write the equation for this reaction. –The half-life for phosphorus-32 is 27 days. If you start with 43 grams of phosphorus-32, how much will be left after 135 days? (Use correct SF) 230 Th undergoes alpha radiation. –Write the equation for this reaction. –You start with 92 grams and are left with 5.8 g after 3.2x10 5 years. Calculate t 1/2.

11. 11 Nomenclature What types of elements form molecular cmpds? Identify each cmpd as ionic or molecular. Then name them: –NiCl 2 –MnO 2 –SnCl 4 –Li 3 N –N 2 F 2 –PCl 5 –P 4 O 6 –Cl 2 O 7

12. 12 Write the formulas for these cmpds: –Sodium sulfate –Copper (II) hydroxide –Xenon difluoride –Magnesium nitride –Selenium tetrachloride –Iron (III) oxalate –Lithium phosphate

13. 13 Write both the classical and stock names for these cmpds: –Fe 2 O 3 –Cr(NO 2 ) 2 –CuOH –Hg 2 O What are the seven diatomic elements? What does it mean to be diatomic?

14. 14 Moles Calculate the molar mass of C 7 H 12 and NaHCO 3 Calculate the mass in grams of: –8.0 moles lead (II) oxide –1.50x10 -2 mol oxygen (O 2 ) –2.3x10 20 molecules of carbon tetrachloride How many atoms are in 8.0 g of tin? You need to make a solution in the lab. You require 0.0465 mol quinine (C 20 H 24 N 2 O 2 ). What mass should you use? How many moles are in 135 L of ammonia gas at STP?