Worksheet 1-4d Classification of Matter

In the spaces provided, classify each of the following substances as; an element, a compound, a solution, or a heterogeneous mixture.

1) Carbon Monoxide	2) Helium
3) Gold	4) Water
5) Oxygen	6) Salt Water
7) Carbon Dioxide	8) Lead
Answers: 1) Compound 2) Element 3) Element 4) Compound 5) Element 6) Solution 7) Compound 8) Element

Worksheet 1-4c Classification of Matter

In the spaces provided, classify each of the following substances as; an element, a compound, a solution, or a heterogeneous mixture.

1) Koolaid	2) Sugar water
3) Chocolate Milk	4) Salt water
5) Coffee with milk	6) A cup of tea, with tea leaves floating in it
7) Salt	8) Chocolatechip Cookie
Answers 1) Solution 2) Solution 3) Heterogeneous mixture 4) Solution 5) Heterogeneous mixture 6) Heterogeneous mixture 7) Compound 8) Heterogeneous mixture

Worksheet 1-4b Classification of Matter

In the spaces provided, classify each of the following substances as; an element, a compound, a solution, or a heterogeneous mixture.

1)Raisin Bran	2)Silver
3)Lithium Carbonate	4)Apple Pie
5)Iced Tea(with powder well mixed)	6)Potassium
7)Soda	8)Calcium Nitrate
Answers 1)heterogeneous mixture 2)element 3)compound 4)heterogeneous mixture 5)solution 6)element 7)solution 8)compound

Worksheet 1-4a Classification of Matter

Part I. Classify each of the following substances as; an element, a compound, a solution, or a heterogeneous mixture.

1. Sand	2. Salt	3. Pure Water	4. Soil
5. Soda	6. Pure Air	7. Carbon Dioxide	8. Gold
9. Bronze	10. Oxygen	11. Salad Dressing	12. Salt Water

Part II. In the spaces provided, describe the distinguishing characteristics of the major categories of matter.

13. Element -

14. Compound -

15. Solution -

16. Mixture -

Answers - part I.
1) mixture 2) compound 3) compound 4) mixture 5) solution 6) solution
7) compound 8) element 9) solution 10) element 11) mixture 12) solution

Test Atomic Structure

1. What is the total number of electrons in the 2p sublevel of a chlorine atom in the ground state? (1) 6; (2) 2; (3) 3; (4) 5.
2. Which is the electron configuration of an atom in the excited state? (1) 1s1,2s ; (2) 1s2,2s2,2p1 ; (3) 1s2,2s2,2p; (4) 1s2,2s2,2p2,3s1
3. A Ca (+2) ion differs from a Ca atom in that the Ca (2+) ion has (1) more protons; (2) fewer protons; (3) more electrons; (4) fewer electrons.
4. At the end of 12 days, 1/4 of an original sample of a radioactive element remains. What is the half-life of the element? (1) 24 days; (2) 48 days; (3) 3 days; (4) 6 days.
5. The total number of orbitals in the 4f sublevel is (1) 1; (2) 5; (3) 3; (4) 7.
6. Which electron transition is accompanied by the emission of energy? (1) 1s to 2s; (2) 2s to 2p; (3) 3p to 3s; (4) 3p to 4p.
7. What is the total number of nucleons (protons and neutrons) in an atom of selenium (atomic no.=34, atomic mass= 79)? (1) 34; (2) 45; (3) 79; (4) 113.
8. What is the total number of principal energy levels that are completely filled in an atom of magnesium in the ground state? (1) 1; (2) 2; (3) 3; (4) 4.
9. What is the maximum number of electrons that can occupy the 4d sublevel? (1) 6; (2) 2; (3) 10; (4) 14.
10. Which sublevels are occupied in the outermost principal energy level of an argon atom in the ground state? (1) 3s and 3d; (2) 3s and 3p; (3) 2s and 3p; (4) 2p and 3d.
11. Which electron configuration represents an atom in the excited state? (1) 1s,2s2 ; (2) 1s2,3p1 ; (3) 1s2 ,2s2,2p5 ; (4) 1s2,2s2,2p6.
12. Which element has an atom in the ground state with the most loosely bound electron? (1) He; (2) As; (3) Xe; (4) Cs.
13. The half-life of C-14 is 5730 years. What fraction of a 1 gram sample of C-14 would remain after 17,190 years? (1) 1/2; (2) 1/4; (3) 1/8; (4) 1/16.
14. Isotopes of an element have a different (1) number of electrons; (2) number of protons; (3) atomic number; (4) mass number.
15. A neutral atom of an element has an electron configuration of 2-8-2. What is the total number of p electrons in this atom? (1) 6; (2) 2; (3) 10; (4) 12.
16. A neutral oxygen atom (O) differs from an oxide ion in that the atom has (1) more electrons; (2) fewer electrons; (3) more protons; (4) fewer protons.
17. Which is the electron configuration of a hydrogen atom with an atomic mass of 3 in1the ground state? (1) 1s; (2) 1s2; (3) 1s2,2s1; (4) 1s22,2s.
18. When an electron in an atom of hydrogen moves from the second to the first principal energy level then the result is the emission of (1) a beta particle; (2) an alpha particle; (3) quantized energy; (4) gamma rays.
19. How many occupied sublevels are in an atom of carbon in the ground state? (1) 5; (2) 6; (3) 3; (4) 4.
20. What is the total number of electrons in the 2nd principal energy level of a chlorine atom in the ground state? (1) 5; (2) 7; (3) 8; (4) 17.

Test Acids and Bases

1. The pH of a solution is 2 at 25 °C. What is the pOH of this solution?
   (1) 0; (2) 2:(3) 12; (4) 14.
2. In a solution with a pH of 3 the color of (1) litmus is red; (2) litmus is
   blue;(3) phenolphthalein is red; (4) phenolphthalein is blue.
3. What is the total number of moles of H1+ ions that will neutralize 2.0 moles
   of OH1-ions? (1) 1.0; (2) 2.0; (3) 17; (4) 34.
4. Which salt hydrolyzes in water to form a solution that is acidic? (1) KCl;
   ( 2) NH4Cl;(3) NaCl; (4) LiCl.
5. Which particle is amphiprotic? (1) HNO3 ; (2) NO31- ; (3) NH3 ; (4) NH41+ .
6. As 50. milliliters of 0.1 M HCl is added to 100 milliliters of 0.1 M NaOH the
   pH of theNaOH solution (1) decreases; (2) increases; (3) remains the same.
7. Which compound is an electrolyte? (1) C6H12O6 ; (2) C12H22O11; (3) C2H5OH
   (4) CH3COOH.
8. The hydroxide ion concentration is greater than the hydronium ion concentration in a 0.1 M solution of (1) NaOH; (2) CH3OH; (3) HNO3 ; (4) H2SO4.
9. What is the pH of a solution whose hydronium ion concentration is 0.0001 moles per
   liter? (1) 1; (2) 10; (3) 14; (4) 4.
10. The conjugate base of the bisulfite ion is the (1) sulfide ion; (2) sulfite ion;
    (3) bisulfate ion; (4) sulfate ion.
11. A weak acid (HX) has an equilibrium constant of 1.0 X 10-8. What is the pH of a 1.0
    M solution of this acid? (1) 1; (2) 7; (3) 8; (4) 4.
12. If 6 milliliters of 1M HCl is exactly neutralized by 3 milliliters of KOH then the
    molarity of the KOH is (1) 1M; (2) 2M; (3) 3M; (4) 9M.
13. The pH of 0.001M HCl is (1) 1; (2) 2; (3) 3; (4) 4.
14. NH3 + H2O = NH4 1+ + OH1- Given the above reaction the two Bronsted acids are
    (1) NH3 and H2O; (2) NH3 and OH1- ; (3) NH4 1+ and H2O ; (4) NH4 1+ and OH1- .
15. An organic compound whose water solution turns litmus red is (1) CH3OH; (2) C6H12;(3) CH3COOH; (4) C6H12O6 .
16. Which could act as either a Bronsted acid or a Bronsted base? (1) chloride ion;
    (2) sulfide ion; (3) bisulfide ion; (4) carbonate ion.
17. Which solution will be exactly neutralized by 1.0 liter of 1.0M NaOH? (1) 1.0 liter
    of 0.50M HCl; (2) 1.0 liter of 2.0M HCl; (3) 0.50 liter of 0.50M HCl; (4) 0.50 liter
    of 2.0M HCl.
    17. Which solution will be exactly neutralized by 1.0 liter of 1.0M NaOH? (1) 1.0 liter
    of 0.50M HCl; (2) 1.0 liter of 2.0M HCl; (3) 0.50 liter of 0.50M HCl; (4) 0.50 liter
    of 2.0M HCl.
18. Which pH indicates the highest concentration of hydronium ions? (1) 1; (2) 7;
    (3) 10; (4) 14.
19. Which 0.1M aqueous solution is the poorest conducter of electricity? (1) C2H5OH;
    (2) HCl; (3) H2SO4 ; (4) NH3 .
20. Which of the following 0.1 M solutions is the best conductor of electricity? (1) HNO3
    ; (2) HNO2 ; (3) NH3 ; (4) CH3COOH .
21. Which of the following is the weakest Bronsted acid? (1) HBr; (2) HI; (3) HCl;
    (4) HF.
22. When K2CO3 dissolves in water the resulting solution turn litmus paper (1) red
    and is acidic; (2) blue and is acidic; (3) red and is basic; (4) blue and is basic.
23. A 30 milliliter sample of HCl is completely neutralized by 10. milliliters of a 1.5 M
    NaOH solution. What is the molarity of the HCl solution? (1) 0.25; (2) 0.50;
    (3) 1.5; (4) 4.5.
24. Which could be the pH of a solution whose hydronium ion concentration is less than
    the hydroxide ion concentration? (1) 9; (2) 2; (3) 3; (4) 4.
25. A solution of which metallic ion would have an acid pH? (1) sodium; (2) aluminum;
    (3) potassium; (4) lithium.
26. Which compound is the weakest electrolyte? (1) HCl; (2) HNO3 ; (3) H2S;
    (4) H2SO4 .
27. Which hydrogen ion concentration indicates the most acidic solution? (1) 1 x
    10-11M; (2) 1 x 10-9 M; (3) 1 x 10-7 M; (4) 1 x 10-5 M.
28. Which compound is correctly classified as a salt? (1) KNO3 ; (2) HNO3 ; (3) CH3COOH
    ; (4) C2H5OH .
29. How many milliliters of 2.0 M NaOH are needed to exactly neutralize 50 mL of 2.0
    M HCl? (1) 25; (2) 50; (3) 100; (4) 200.
30. In the reaction H2O + H2O ------> H3O1+ + OH1- water is acting as (1) a Bronsted
    acid only; (2) a Bronsted base only; (3) neither a Bronsted acid nor base; (4) both
    a Bronsted acid and base.
31. Which of the following combinations when dissolved in water would produce an
    acidic buffer? (1) KCl and NaCl; (2) NaOH and HOH; (3) NaCl and HCl;
    (4) CH3COOH and NaCH3COO .
32. When titrating a strong acid and a weak base the stoichiometric point may have a
    pH of (1) 0; (2) 7; (3) 5; (4) 9.
33. Which 0.1 molar aqueous solution contains the highest concentration of OH1- ions?
    (1) CH3OH ; (2) NaOH ; (3) C2H5OH ; (4) NH3 .
34. Red litmus will turn blue when placed in an aqueous solution of (1) HCl; (2) CH3COOH;
    (3) KOH; (4) CH3OH.
35. Which ion is amphiprotic? (1) Cl1- ; (2) HSO41- ; (3) O2- ; (4) NH41+ .
36. A solution at 25 degrees Celsius with a pH of 7 contains (1) more hydronium ions
    than hydroxide ions; (2) fewer hydronium ions than hydroxide ions; (3) an equal
    number of hydronium ions and hydroxide ions; (4) no hydronium ions or hydroxide
    ions.
37. Which acid is almost completely ionized in a dilute solution at 25 °C? (1) CH3COOH;
    (2) H2S; (3) H3PO4 ; (4) HNO3 .
38. A solution of potassium carbonate would have a pH closest to (1) 1; (2) 5; (3) 3;(4) 8.
39. How many liters of 2.5 M HCl are required to exactly neutralize 1.5 liters of 5.0 M
    NaOH? (1) 1.0; (2) 2.0; (3) 3.0; (4) 4.0.
40. What are the Bronsted-Lowry bases in the following reaction:
    H2S + H2O ------> H3O1+ + HS1- ? (1) H2S and H2O; (2) H 2S and H3O1+ ; (3) HS1-and H2O; (4) HS1- and H3O1+ .
41. When additional solid NaCl dissolves in a solution of NaCl in water the pH of the
    solution (1) decreases; (2) increases; (3) remains the same.
42. When hydrochloric acid is neutralized by sodium hydroxide then the salt formed is
    sodium (1) hydrochlorate; (2) chlorate; (3) chloride; (4) perchloride.
43. The ionization constant of 1.8 x 10-5 is for a weak acid. A reasonable pH for a 0.1 M
    solution of this acid would be (1) 1; (2) 9; (3) 3; (4) 14.
44. A 1 molal solution of magnesium chloride has a higher boiling point than a 1 molal
    solution of solution of (1) FeCl3 ; (2) CaCl2 ; (3) BaCl2 ; (4) NaCl.
45. A water solution of which gas contains more hydroxide ions than hydronium ions?
    (1) HCl; (2) NH3 ; (3) CO2 ; (4) SO2 .
46. The following are hydrogen ion concentrations. Which hydrogen ion concentration
    indicates the strongest acid? (1) 1.0 x 10-4; (2) 2.0 x 10-5; (3) 3.0 x 10-6; (4) 4.0 x
    10-7.
47. How many milliliters of 0.200 molar NaOH are needed to neutralize 100 milliliters
    of 0.100 molar HCl? (1) 40.0; (2) 50.0; (3) 100.; (4) 200.
48. Given the following reaction: H2SO4 + H2O ======> HSO41- + H3O1+ . The two
    Bronsted-Lowry acids are (1) H2SO4 and H2O; (2) H2SO4 and H3O1+ ; (3) H2O and
    H3O1+ ; (4) HSO4 1- and H3O1+ .
49. Neutralization of 15 milliliters of a 1.0-molar solution of KOH requires 5 milliliters
    of hydrochloric acid. What is the molarity of the HCl solution? (1) 1.0; (2) 2.0;
    (3) 3.0; (4) 6.0.
50. Which solution is the best conductor of electricity? (1) 1.0 M boric acid; (2) 1.0 M
    carbonic acid; (3) 1.0 M acetic acid; (4) 1.0 M hydrochloric acid.

CRUDE OILS ( MINYAK MENTAH )

Crude oil is the term for "unprocessed" oil, the stuff that comes out of the ground. It is also known as petroleum. Crude oil is a fossil fuel, meaning that it was made natural­ly from decaying plants and animals living in ancient seas millions of years ago -- most places you can find crude oil were once sea beds. Crude oils vary in color, from clear to tar-black, and in viscosity, from water to almost solid.

On average, crude oils are made of the following elements or compounds:
• Carbon - 84%
• Hydrogen - 14%
• Sulfur - 1 to 3% (hydrogen sulfide, sulfides, disulfides, elemental sulfur)
• Nitrogen - less than 1% (basic compounds with amine groups)
• Oxygen - less than 1% (found in organic compounds such as carbon dioxide,
phenols, ketones, carboxylic acids)
• Metals - less than 1% (nickel, iron, vanadium, copper, arsenic)
• Salts - less than 1% (sodium chloride, magnesium chloride, calcium chloride)

Crude oils are such a useful starting point for so many different substances because they contain hydrocarbons. Hydrocarbons are molecules that contain hydrogen and carbon and come in various lengths and structures, from straight chains to branching chains to rings.

There are two things that make hydrocarbons exciting to chemists:

Hydrocarbons contain a lot of energy. Many of the things derived from crude oil like gasoline, diesel fuel, paraffin wax and so on take advantage of this energy.
Hydrocarbons can take on many different forms. The smallest hydrocarbon is methane (CH4), which is a gas that is a lighter than air. Longer chains with 5 or more carbons are liquids. Very long chains are solids like wax or tar. By chemically cross-linking hydrocarbon chains you can get everything from synthetic rubber to nylon to the plastic in tupperware. Hydrocarbon chains are very versatile!