FINAL EXAM REVIEW

Disclaimer this is NOT the official final review. Please do not just use this to study.

1.) Determine which of the following are chemical or physical changes.

a.) Two clear liquids are mixed and a blue color appears C

b.) Cutting your hair P

c.) Burning a tree to form ashes C

d.) bending a piece of metal P

e.) Methanol burning leaving behind a residue C

2.) Complete each of the following conversions:

a.) 0.50 m = ____500_____ mm

b.) 10.0 mm = ____1.00____ cm

c.) 56.4 L = ____56400_____ mL

d.) 456 g = _____0.456____ kg

e.) 5.00 cm = ____0.05____ m

3.) How many protons, neutrons, and electrons does Potassium have?

19 p, 20 n, 19 e

4.) How many protons, neutrons, and electrons does Calcium have?

20 p, 20 n, 20 e

5.) How many protons, neutrons, and electrons does Mg2+ have?

12p, 12n, 10 e

6.) Gallium has two naturally occurring isotopes. The mass of gallium-69 is 68.93 amu and it is 60.11% abundant. The mass of gallium-71 is 70.92 amu and it is 39.89% abundant. Find the atomic mass of gallium.

7.) Antimony has two naturally occurring isotopes. The mass of antimony-121 is 120.91 amu and the mass of antimony-123 is 122.90 amu. Find the abundance of each isotope.

8.) Name the following molecules:

a.) CF Carbon monofluoride

b.) Cl2O Dichlorine monoixide

c.) Na2SO4 Sodium Sulfate

d.) Ba(C2H3O2) Barium Acetate

9.) What is the mass in grams of 2.83 x 1024 sodium atoms?

10.) How many moles of mercury are in 3.36 x 1025 atoms?

11.) What is the empirical formula of a compound that contains 0.783g of Carbon, 0.196g of Hydrogen and 0.521g of Oxygen?

12.) 4 Al + 3 O2 2 Al2O3

We have placed 0.048 moles of aluminum in a container that has 0.030 moles of O2. What is the limiting reactant? How many moles of the excess reactant remain?

13.) what is the molarity of NaOH if it takes 30.0 mL of NaOH to reach the equivalence point in a titration with 50.0 mL of 0.300 M HCl?

14.) What is the net ionic equation for nickel nitrate and sodium hydroxide?

15.) Identify what is being oxidized and reduced in the following:

Cr+ + Sn4+  Cr3+ + Sn2+

16.) A gas occupies 12.3 liters at a pressure of 40.0 mmHg. What is the volume when the pressure increased to 60.0mmHg?

17.) Fluorine gas at 300K occupies a volume of 500mL. To what temperature should it be lowered to bring the volume to 300mL.

18.) If I have an unknown quantity of gas held at a temperature of 119K in a container with a volume of 25 liters and a pressure of 560 atm, how many moles of gas do I have?

19.) A mixture of 2.00 mols oh H2 , 3.00 mols of NH3, 4.00 mols of CO2, and 5.00 mols of N2 exerts a total pressure of 800 torr. What is the partial pressure of each gas?

20.) 5.0 L of an ideal gas is expanded into a vacuum and the new volume is 7.0 L. If 600J of heat flow out of the container, what is the change in the internal energy of the system? Is the work done on the system?

21.) A ‘coffee-cup’ calorimeter contains 150g of water at 24.6 °C. A 110 g block of molybdenum metal is heated to 100 °C and then placed in the water in the calorimeter. The contents of the calorimeter come to an average temperature of 28.0 °C. What is the specific heat capacity of the molybdenum metal if the specific heat capacity of water is assumed to be 4.184 J/°Cg?

22.) Violet light has a wavelength of 4.10 x 10-12m. What is the frequency?

7.31 x 1019

23.) Calculate and wavelength. Ninitial = 4 and Nfinal = 2.

- 1/I^2)

-2.18 x 10-18 () = -4.09 x 10-19 J

…… wl= hc/

= 4.86x10-7 m

J

m

24.)

Energy levels

Sublevel (orbital)

Orientation (orbital)

# of e-

N= 1

0

This refers (s)

0

This tells us the shape which is a sphere

2

N= 2

0 (s)

1 (p)

0

-1, 0, +1

2

6

N= 3

0 (s)

1 (p)

2 (d)

0

-1, 0, +1

-2, -1, 0, +1, +2

2

6

10

N= 4

0 (s)

1 (p)

2 (d)

3 (f)

0

-1, 0, +1

-2, -1, 0, +1, +2

-3, -2, -1, 0, +1, +2, +3

2

6

10

14

25.) what are the electron configurations for the following:

a.) barium _______________________________

b.) tellurium _______________________________

c.) Rubidium ____________________________

26.) Draw two resonance structures for CHO2-.

27.) Draw all the possible Lewis structures for CNO-. Calculate the formal charge of all the atoms in each structure and find which one is more stable.

28.) Estimate the enthalpy change for the reactions using bond energies.

CH4 (g) + 3Cl2 (g) CHCl3 (g) + 3HCl (g)

Bond energies: C-H: 413 kJ/mol, Cl-Cl: 242 kJ/mol, C-Cl: 328 kJ/mol, H-Cl: 431 kJ/mol

29.) What is the molecular geometry for the following? Are they polar or nonpolar?

a.) SO42-

b.) NH3

c.) H2CO

30.) What is the molecular orbital for NO and its bond order?