Name: ______

Final Exam Review

Your final exam is on ______in room ______.

Bring your text book, calculator, #2 pencils, and your review materials.

Multiple Choice Section

1.  Define intensive and extensive properties and provide 3 examples of each.

2.  Define physical and chemical properties and provide 3 examples of each.

3.  Define physical and chemical changes and provide 3 examples of each.

4.  Describe the speed, motion, volume, and shape for the 3 phases of matter.

5.  Describe heterogeneous mixtures, homogeneous mixtures, compounds and elements and provide 3 examples of each.

6.  Give an example of a mixture that has more than one phase

7.  Define reactants and products.

8.  List the 4 signs of a chemical change and describe how you know for certain that a chemical change has definitely occurred.

9.  Write 5 large numbers in both standard notation and then write them in scientific notation (include correct significant digits).

10.  Write 5 small numbers (numbers that start 0.______) in both standard and scientific notation (include correct significant digits).

11.  Define and differentiate between accuracy and precision.

12.  How many significant figures are there in 400? 400.0? 0.004? 0.0040?

13.  How do you determine how many significant digits should be in the sum or difference between a series of numbers?

14.  How do you determine how many significant digits should be in the product or quotient of a series of numbers?

15.  Define and differentiate between weight and mass.

16.  What is the formula for density? If a substance has a volume of 4.5 ml and a mass of 0.02lative to its volume1 g, what is its density?

17.  As the density of a substance increases, what happens to its mass relative to its volume?

18.  Describe the mass, charge, and location for the three subatomic particles.

19.  Which subatomic particle is responsible for determining the identity of an atom?

20.  Which subatomic particle is responsible for determining the properties of an atom?

21.  Describe Dalton’s Atomic Theory.

22.  Describe J. J. Thomson’s experiment and contribution to the concept of the atom.

23.  Describe Ernest Rutherford’s experiment and contribution to the concept of the atom.

24.  Describe Chadwick’s experiment and contribution to the concept of the atom.

25.  Describe Bohr’s contribution to the concept of the atom.

26.  As the frequency of light increases, what happens to its wavelength? What happens to its energy?

27.  Which of the following(wavelength, frequency and energy) are directly proportional? Inversely proportional?

28.  Which color of visible light has the longest wavelength? Shortest?

29.  Which type of electromagnetic radiation has the lowest frequency? Highest?

30.  According to the Bohr Model of the atom, what happens when an electron drops down from a higher energy orbit to one of lower energy?

31.  What is atomic number and what information does it provide?

32.  What is mass number and what information does it provide?

33.  What are isotopes?

34.  Define the quantum mechanical model of an atom

35.  What is the Aufbau Principle?

36.  How many electrons can an s sublevel hold? p sublevel? d sublevel ? fsublevel?

37.  What is the maximum number of electrons found in the first energy level? 2nd? 3rd? 4th?

38.  What element would have an electron configuration of 1s22s22p3?

39.  Why is light emitted from an atom?

40.  What was Dmitri Mendeleev’s contribution to the periodic table?

41.  What was Henry Moseley’s contribution to the periodic table?

42.  Describe the properties of metals, nonmetals, metalloids, and noble gases.

43.  Define atomic radius, shielding effect, ionization energy, electronegativity, and electron affinity and describe their trends both down a group and across the periodic table.

44.  Define cations and anions.

45.  Describe how the properties of ionic compounds are different from molecular (covalent) compounds

46.  What is the shape of a water molecule? Why isn’t it linear?

47.  Draw the lewis structure of C2H2. What shape is it?

48.  Define hydrogen bonding. Between what types of molecules does it occur

49.  What are the properties of an acid base reaction? List three properties of an acid

50.  What is the Arrhenius definition of an acid

51.  Define Avogadro’s number

52.  In 10.09 grams of nitric acid, how many grams of oxygen are there?

53.  At STP, one mole of a gas = ______liters

54.  What happens to the temperature of a gas as it expands? As it is compressed?

55.  What happens to the speed of molecules of a gas as you increase the temperature/

56.  List 4 differences between real and ideal gases

57.  Define diffusion

1.  A sample of sodium sulfate weighs 3.32 g. Calculate the mass of sodium in the sample in both grams and ounces (there are 28.35 g in 1 ounce).

2.  Draw the Lewis structure for CS2. Indicate its shape, whether it is polar or nonpolar, the type of intermolecular force that it would exhibit, if that intermolecular force is weak, strong, or very strong, whether the boiling point would be relatively high or low, and predict if it would tend to be a liquid or a gas at room temperature.

a.  Lewis Structure

b.  Shape

c.  Polar or Nonpolar ______

d.  Intermolecular force ______

e.  Weak, strong, very strong intermolecular force ______

f.  High Boiling Point or Low Boiling Point ______

g.  Liquid or Gas ______

3.  a. Indicate the shapes for the following molecules:

NH3 ______SF6 ______

PCl5 ______SBr2______

SiCl4 ______AB2E2 ______

4. Ascorbic acid contains 40.92% C, 4.58% H and 54.50 %O by mass. What is its empirical formula? If its molecular mass is 176.2, what is its molecular formula?

4.  5.00 L of a gas at 45 oC and 5.05 atm is heated to 60 oC and the pressure is reduced to 2.55 atm. Calculate the new volume.

5.  15.00 g of C3H8 is combined with 40.00 g of O2 in a combustion reaction. What are the limiting reagent and excess reagents? How much water will be produced? How much excess excess reagent is left?

Limiting Reagent: ______

Excess Reagent: ______

Water Produced: ______

Excess reagent remaining: ______

6.  Write and balance the following equations. Indicate if the reaction does not occur.

a.  Zinc and phosphoric acid

______

b.  C6H14 + O2

______

c.  Plumbic carbonate and ammonium hydroxide

______

d.  Ba3N2

______

e.  H2O + Mg

______

f.  nitrous acid and lithiumhydroxide

______

g.  copper and silver nitrate

______

h.  magnesium and ferric chlorate

______

i.  stannous fluoride and sodium nitrate

______