One Of The Test

Front 1

The density of gasoline is 0.7025 g/mL at 20°C. When gasoline is added to water:

Back 1

a. It will float on top.
b. It will sink to the bottom.
c. It will mix so, you can't see it.
d. The mixture will improve the running of the motor.
e. None of these things will happen.

Front 2

1. Which of the following metric relationships is incorrect?

Back 2

a. 1 microliter = 10–6 liters
b. 1 gram = 103 kilograms
c. 103 milliliters = 1 liter
d. 1 gram = 102 centigrams
e. 10 decimeters = 1 meter

Front 3

2. For which pair is the SI prefix not matched correctly with its meaning?

Back 3

a. mega = 106
b. kilo = 1000
c. deci = 10
d. nano = 10–9
e. centi = 0.01

Front 4

3. A metric unit for length is

Back 4

a. gram
b. milliliter
c. yard
d. kilometer
e. pound

Front 5

4. Order the four metric prefixes from smallest to largest.

Back 5

a. nano- < milli- < centi- < kilob.
milli- < nano- < centi- < kiloc.
kilo- < centi- < nano- < millid.
kilo- < centi- < milli- < nanoe.
centi- < nano- < kilo- < milli-

Front 6

5. 9.16 seconds contain this many nanoseconds.

Back 6

a. 9.16 ´ 107
b. 9.16 ´ 109
c. 9.16 ´ 1012
d. 9.16 ´ 1010
e. 9.16 ´ 108

Front 7

6. Consider the numbers 23.68 and 4.12. The sum of these numbers has _4___ significant figures, and the product of these numbers has _3_ significant figures.

Back 7

a. 3, 3
b. 4, 4
c. 3, 4
d. 4, 3
e. none of these

Front 8

7. How many significant figures should be reported for the difference between 18.6150 mL and 18.57 mL?

Back 8

a. 1
b. 2
c. 3
d. 4
e. 6

Front 9

8. Express the volume 622.6 cm3 in liters.

Back 9

a. 622.6 L
b. 62.26 L
c. 6.226 L
d. 0.6226 L
e. 0.06226 L

Front 10

9. The melting point of a certain element is 346°C. What is this on the Fahrenheit scale?

Back 10

a. 465 °F
b. 224 °F
c. 896 °F
d. 655 °F
e. 591 °F

Front 11

11. The state of matter for an object that has a definite volume but not a definite shape is

Back 11

a. solid state
b. liquid state
c. gaseous state
d. elemental state
e. mixed state

Front 12

12. An example of a pure substance is

Back 12

a. an element
b. a compound
c. pure water
d. carbon dioxide
e. all of these

Front 13

13. Which of the following statements is false?

Back 13

a. Solutions are always homogeneous mixtures.
b. The terms “atom” and “element” can have different meanings.
c. Elements can exist as atoms or molecules.
d. Compounds can exist as atoms or molecules.
e. At least two of the above statements (A-D) are false.

Front 14

14. Which best represents a homogeneous mixture of an element and a compound?

Back 14

a. option a
b. option b
c. option c
d. option d
e. option e

Front 15

15. Which best represents a heterogeneous mixture of two elements?

Back 15

a. option a
b. option b
c. option c
d. option d
e. option e

Front 16

16. The scientist who discovered the law of conservation of mass and is also called the father of modern chemistry is

Back 16

a. Proust
b. Boyle
c. Priestly
d. Bauer
e. Lavoisier

Front 17

17. Which of the following pairs can be used to illustrate the law of multiple proportions?

Back 17

a. SO and SO2
b. CO and CaCO3
c. H2O and C12H22O11
d. H2SO4 and H2S
e. KCl and KClO2

Front 18

18. According to the law of multiple proportions:

Back 18

a. If the same two elements form two different compounds, they do so in the same ratio.
b. It is not possible for the same two elements to form more than one compound.
c. The ratio of the masses of the elements in a compound is always the same.
d. The total mass after a chemical change is the same as before the change.
e. None of these.

Front 19

19. A sample of chemical X is found to contain 5.0 grams of oxygen, 10.0 grams of carbon, and 20.0 grams of nitrogen. The law of definite proportion would predict that a 67 gram sample of chemical X should contain how many grams of carbon?

Back 19

a. 5.0 grams
b. 6.7 grams
c. 10. grams
d. 15 grams
e. 19 grams

Front 20

20. Which of the following statements from Dalton's atomic theory is no longer true, according to modern atomic theory?

Back 20

a. Elements are made up of tiny particles called atoms.
b. Atoms are not created or destroyed in chemical reactions.
c. All atoms of a given element are identical.
d. Atoms are indivisible in chemical reactions.
e. All of these statements are true according to modern atomic theory.

Front 21

21. Many classic experiments have given us indirect evidence of the nature of the atom. Which of the experiments listed below DID NOT give the results described?

Back 21

a. The Rutherford experiment proved the Thomson "plum-pudding" model of the atom to be essentially correct.
b. The Rutherford experiment was useful in determining the presence of nucleus in the atom.
c. Millikan's oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the
electron.
d. The cathode-ray tube proved that electrons have a negative charge.
e. All of the above experiments gave the results described.

Front 22

22. Bromine exists naturally as a mixture of bromine-79 and bromine-81 isotopes. An atom of bromine-79 contains

Back 22

a. 35 protons, 44 neutrons, 35 electrons
b. 34 protons and 35 electrons, only
c. 44 protons, 44 electrons, and 35 neutrons
d. 35 protons, 79 neutrons, and 35 electrons
e. 79 protons, 79 electrons, and 35 neutrons

Front 23

23. Which among the following represent a set of isotopes? Atomic nuclei containing:
I. 20 protons and 20 neutrons
II. 21 protons and 19 neutrons
III. 22 protons and 18 neutrons
IV. 20 protons and 22 neutrons
V. 21 protons and 20 neutrons

Back 23

a. I, II, III
b. III, IV
c. I, V
d. I, IV and II, V
e. No isotopes are indicated.

Front 24

24. An isotope, X, of a particular element has an atomic number of 15 and a mass number of 31. Therefore:

Back 24

a. X is an isotope of phosphorus.
b. X has 16 neutrons per atom.
c. X has an atomic mass of 30.973.
d. A and B.
e. A, B, and C.

Front 25

25. Which of the following statements is (are) true?

Back 25

a. 18 8O and 19 9F have the same number of neutrons.
b. 14 6C and 14 7N are isotopes of each other because their mass numbers are the same.
c. 18 28O - has the same number of electrons as 20
10Ne .
d. A and B
e. A and C

Front 26

26. A species with 12 protons and 10 electrons is

Back 26

a. Ne2+
b. Ti2+
c. Mg2+
d. Mg
e. Ne2–

Front 27

27. An ion is formed

Back 27

a. By either adding or subtracting protons from the atom.
b. By either adding or subtracting electrons from the atom.
c. By either adding or subtracting neutrons from the atom.
d. All of the above are true.
e. Two of the above are true.

Front 28

28. The formula of water, H2O, suggests:

Back 28

a. There is twice as much mass of hydrogen as oxygen in each molecule.
b. There are two hydrogen atoms and one oxygen atom per water molecule.
c. There is twice as much mass of oxygen as hydrogen in each molecule.
d. There are two oxygen atoms and one hydrogen atom per water molecule.
e. None of these.

Front 29

29. All of the following are true except:

Back 29

a. Ions are formed by adding electrons to a neutral atom.
b. Ions are formed by changing the number of protons in an atom's nucleus.
c. Ions are formed by removing electrons from a neutral atom.
d. An ion has a positive or negative charge.
e. Metals tend to form positive ions.

Front 30

30. Which of the following are incorrectly paired?

Back 30

a. K, alkali metal
b. Ba, alkaline earth metal
c. O, halogen
d. Ne, noble gas
e. Ni, transition metal

Front 31

31. All of the following are characteristics of nonmetals except:

Back 31

a. poor conductors of electricity
b. often bond to each other by forming covalent bonds
c. tend to form negative ions in chemical reactions with metals
d. appear in the upper left-hand corner of the periodic table
e. do not have a shiny (lustrous) appearance

Front 32

32. Which of the following has 61 neutrons, 47 protons, and 46 electrons?

Back 32

a. 80
61
Pm
b. 108
47
Ag+
c. 108
46
Pd–
d. 108
47
Cd+
e. 108
47
Ag

Front 33

33. Which of the following statements are true of uranium-238 (238U)?
I. Its chemical properties will be exactly like those of uranium-235.
II. Its mass will be slightly different from that of an atom of uranium-235.
III. It will contain a different number of protons than an atom of uranium-235.
IV. It is more abundant in nature than uranium-235.

Back 33

a. III, IV
b. I, II, III
c. I, II, IV
d. II, III, IV
e. all of these

Front 34

34. You are given a compound with the formula MCl3, in which M is a metal. You are told that the metal ion has 10 electrons. What is the identity of the metal?

Back 34

a. Mn
b. Al
c. Cu
d. Fe
e. Co

Front 35

35. Which of the following names is incorrect?

Back 35

a. cobalt(II) chloride
b. magnesium oxide
c. aluminum(III) oxide
d. diphosphorus pentoxide
e. All of the above names are correct.

Front 36

36. Which of the following pairs is incorrect?

Back 36

a. iodine trichloride, ICl3
b. phosphorus pentoxide, P2O5
c. ammonia, NH3
d. sulfur hexafluoride, SF6
e. All of the above pairs are correct.

Front 37

The correct name for Ca2+ is

Back 37

a. calcium
b. calcium(II) ion
c. calcium ion
d. calcium(I) ion
e. monocalcium ion

Front 38

38. The correct name for N3– is

Back 38

a. nitride ion
b. nitrogen ion
c. nitrogen(III) ion
d. nitro(III) ion
e. nitrite

Front 39

39. Which of the following is incorrectly named?

Back 39

a. Ba(NO3)2, barium nitrate
b. NH4ClO4, ammonium perchlorate
c. PO4
3–, phosphate ion
d. Mg(OH)2, magnesium hydroxide
e. NO3–, nitrite ion

Front 40

40. All of the following are in aqueous solution. Which is incorrectly named?

Back 40

a. H2SO4, sulfuric acid
b. H2CO3, carbonic acid
c. H3PO4, phosphoric acid
d. HCN, cyanic acid
e. HCl, hydrochloric acid

Front 41

41. Which of the following is incorrectly named?

Back 41

a. SO3
2–, sulfite ion
b. Cr2O7
2–, dichromate ion
c. PO4
3–, phosphate ion
d. ClO2
–, chlorate ion
e. CN–, cyanide ion

Front 42

42. The compound K2SO3 is named:

Back 42

a. Calcium sulfate
b. Potassium sulfate
c. Potassium sulfite
d. Krypton sulfur trioxide
e. Dipotassium sulfite

Front 43

43. The compound Cu(ClO3)2 is named:

Back 43

a. Copper(II) perchlorate
b. Cobalt chlorine trioxide
c. Copper(II) chlorate
d. Copper(II) chloride
e. Copper dichlorate

Front 44

44. The compound lithium dichromate has the formula:

Back 44

a. LiCrO4
b. Li2CrO4
c. Li2Cr2O7
d. LaCrO4
e. Li(CrO4)2

Front 45

45. Methane has the formula:

Back 45

a. NH3
b. CCl4
c. CH4
d. H2O
e. Mn

Front 46

All physical changes are accompanied by chemical changes

Back 46

(F)

Front 47

The number of neutrons in an atom is the same for all neutral atoms of that element.

Back 47

(F)

Front 48

The number of electrons in an atom is the same for all neutral atoms of that element.

Back 48

T

Front 49

A binary compound formed by a metal and a non-metal is always ionic.

Back 49

T

Front 50

Sodium hydride is an ionic compound.

Back 50

T