1. “DHMO Investigation Standards Test”

2. I. Graphic Organizer
Fill in the missing parts of the Graphic Organizer. Then use the information to answer other parts of the test. (1 pt. each= 17 pts. total)

3. II. Fill in the chart describing the characteristics of the different types of bonds. (1 pt. each= 10 points total)
Covalent Bond
________ Bond
_________ Bond
Make up
Nonmetals only
Metals and nonmetals
Electron behavior
Share
Transfer
Free flow
Physical Properties
Melting/Boiling Point
Mid- High
Conductivity
Solubility
Not soluble

4. III. Determine the following information about each neutral element
III. Determine the following information about each neutral element. (1 pt. each = 15 points)
Element Name
Atomic #
Mass
p+ #
e- #
n= #
Oxid. #
Cation or Anion?
Calcium
40.08 20 2+ 13
Cation 9

5. IV. Determine the following information about each compound. (1 pts
IV. Determine the following information about each compound. (1 pts. each= 10 points total)
Type of Bond
Compound Formula
Compound Name
Dot Diagrams
Ionic
CaCl2
carbon dioxide
magnesium
calcium
carbonate

6. V. Choose the best answer for each question
V. Choose the best answer for each question. Remember to use the Graphic Organizer and information throughout the test to assist you with each question. (2 pts. each= 60 points total)

7. 1. What has occurred when bubbles form in a liquid that is being heated?
a. Oxygen is absorbed from the air.
b. Heat is radiating in the liquid.
c. The boiling point has been reached.
d. Molecular stability in the liquid is increasing.

8. 2. Which atomic symbol represents an isotope of sulfur with 17 neutrons?
a. 16X b. 33X c. 17X d. 49X

9. 3. Anita heats a beaker containing water
3. Anita heats a beaker containing water. As the temperature of the water increases, which change to the water molecules occurs?
a. The molecules move at a faster rate.
b. The molecules become more massive.
c. The molecules expand and become wider.
d. The molecules separate into atoms of hydrogen and
oxygen.

10. 4. An investigation was conducted using Pure Substance X which was cooled at a constant rate over time. The graph below shows the phase changes of the substance over time as it cools.
According to the curve, how long does it take for Pure Substance X to freeze completely?
a. 5 min. b. 10 min. c. 15 min d. 20 min.

11. 5. Which is the electronic configuration of calcium?
a. 1s22s22p63s23p8
b. 1s22s22p63s23p64s2
c. 1s22s22p63s23p63d2
d. 1s22s22p83s23p6

12. 6. Name the compound with the chemical formula of NO2.
a. nitrogen oxide b. nitrogen dioxide
c. mononitrogen dioxide d. nitrogen trioxide

13. 7. How many particles are in Sodium that also gives the element its identity?
a. 13 electrons
b. 23 protons
c. 11 protons
d. 11 neutrons

14. 8. An electron in an atom of hydrogen goes from energy level 6 to energy level 2. What is the wavelength of the electromagnetic radiation emitted?
a. 410 nm b. 434 nm c. 486 nm d. 656 nm

15. 9. The diagram shows the
changes that occur when an
ice cube changes from solid
state to steam.
What does the constant
temperature in Leg 4 indicate in
terms of energy loss or gain?
a. Heat change cannot be predicted using given data.
b. Heat is gained to change the water to steam.
c. Heat is gained as the ice melts.
d. Heat is lost during this part of the reaction.

16. 10. The half-life of a radioactive isotope is 20 minutes
10. The half-life of a radioactive isotope is 20 minutes. What is the total amount of 1.00g of sample of this isotope remaining after 1 hour?
a g b g c g d g

17. 11. Ionic compounds have which set of properties:
a. mid- level melting and boiling points
b. low conductivity
c. dissolves in alcohol
d. not soluble in water

18. 12. You have a substance that reacts to acid, highly conductive, and is a pure substance. What type of bond is this substance?
a. Ionic Bond
b. Metallic Bond
c. Covalent Bond
d. Polyatomic Bond

19. The graph shows a heating curve for water
The graph shows a heating curve for water. Use this graph to answer questions 13 and 14.
13. Which point on the graph indicates that all of the liquid water has been converted to water vapor?
a b c. 3 d. 4
14. Which point on the graph indicates the most energy in the water molecules?
a b c d. 4

20. 15. An ionic compound does which of the following:
a. transfers electrons, has low melting point
b. flows electrons, has high boiling point
c. transfers electrons, has high boiling point
d. shares electrons, has low condensation point

21. 16. Which statement describes the compound formed between sodium and oxygen?
a. It is NaO2, which is ionic.
b. It is NaO2, which is covalent.
c. It is Na2O, which is ionic.
d. It is Na2O, which is covalent.

22. 17. What is the IUPAC, the naming system, name for the compound represented by the formula Mg(OH)2?
a. Magnesium hydroxide
b. Magnesium dihydroxide
c. Magnesium (II) hydroxide
d. Magnesium (II) dihydroxide

23. 18. Which atom has the largest radius?
a. Bromine
b. Chlorine
c. Selenium
d. Sulfur

24. Based on these results, what is the unknown substance?
19. An unknown substance is tested in the laboratory. The physical test results are listed below.
Nonconductor of electricity
Insoluble in water
Soluble in oil
Low melting point
Based on these results, what is the unknown substance?
a. ionic and polar b. ionic and nonpolar
c. covalent and polar d. covalent and nonpolar

25. 20. The nucleus of an atom is shown.
8p+
9n=
Which statement describes the element?
a. It is a nonmetal in group 2.
b. It is a nonmetal in group 16.
c. It is a metal in group 2.
d. It is a nonmetal in group 17.

26. 21. Arrange the following elements in order of increasing electronegativity, from the lowest to highest: F, K, Si, and S.
a. F<K<S<Si
b. K<Si<S<F
c. Si<F<K<S
d. S<Si<F<K

27. 22. How many electrons are in the outermost energy level of an electrically neutral atom of aluminum?
a b c d. 2

28. 23. When aluminum and sulfur react, which compound is produced?
a. Al2S b. Al3S c. AlS d. AlS

29. 24. The nuclear equation below represents the alpha decay of 222Rn:
222Rn  4He + X
What is the mass number of the element represented by X?
a. It is 88, because element X gains 2 protons.
b. It is 218, because element X loses 2 protons and 2 neutrons.
c. It is 220, because element X loses 2 neutrons.
d. It is 226, because element X gains 2 protons and 2 neutrons.

30. 25. What best compares the properties of ionic and metallic substances?
a. The bonds of metallic substances are composed of
delocalized electrons, and the bonds of ionic substances
are composed of transferred electrons.
b. The bonds of metallic substances are composed of
isolated electrons, and the bonds of ionic substances are
composed of shared electrons.
c. A metallic substance insulates heat and electricity, and
solid ionic substances conduct heat and electricity.
d. A metallic substance has a low melting point, and an ionic
substance has a low melting point.

31. 26. Which combination of elements would most likely form an ionic compound?
a. hydrogen and oxygen
b. carbon and chlorine
c. sodium and fluorine
d. silicon and sulfur

32. 27. Which represents the formula for iron (III) chromate?
a. Fe2(CrO4) b. Fe2(CrO4)2
c. Fe3(CrO4) d. Fe3(CrO4)3

33. 28. An atom of which element has the strongest attraction for electrons?
a. Ba b. Cs c. O d. F

34. 29. Which of the following is the correct oxidation number for O?
a b c d. 6+

35. 30. Which is an accurate comparison of the bonds that can occur between carbon and atoms in terms of bond length and strength?
a. Double bonds are shorter than single bonds, but single
bonds are stronger than triple bonds.
b. Triple bonds are shorter than double bonds, and double
bonds are stronger than single bonds.
c. Double bonds are both shorter and stronger than triple bonds.
d. Triple bonds are the longest and strongest.

36. VI. Answer the following questions fully and completely
VI. Answer the following questions fully and completely. Be sure to include all relevant information from the test and Graphic Organizer to assist in gaining full credit. (28 points total)

37. 1. Using magnesium complete the following tasks (8 pts total):
a. Lewis Dot Structure
b. Oxidation number
c. The formula if combined with Chlorine
d Electron configuration

38. 2. Calculate the electron configuration for an element with 15 electrons (2 pts. total).

39. 3. A substance is in a gas phase at room temperature
(6 pts. total).
a. Describe what type of intermolecular force this could
have between the compounds.
b. Predict what type of bond this gas could be and why.
c. Discuss the attraction, pressure, and temperature of
those molecules.

40. 4. Answer the following questions using the compound dihydrogen monoxide (2 pts. each, 12 pts. total).
a. What is the common name and formula of this compound?
b. Give 4 properties of this compound.
c. What type of bond is this compound?
d. Is this compound a polar or nonpolar molecule? Or does it
apply to this compound?
e. Complete the Lewis Dot Structure for this compound.
f. What do the electrons do in this compound? (Electron
behavior)

41. The End Look over your test. Check your answers!
Make sure you used your G.O. and the test to
assist with answering the questions.