Chem Final -- First Sem 04

Chem Final -- First Sem 04

Multiple Choice

Identify the letter of the choice that best completes the statement or answers the question.

____ 1. A physical property of zinc metal is _____.

a.	its color	c.	how it reacts with nitrogen gas
b.	whether it burns	d.	whether it changes when placed into acid

____ 2. Which of the following materials cannot be broken down into a simpler form?

a.	compound	c.	mixture
b.	solution	d.	element

____ 3. An example of a pure substance in everyday life is _____.

a.	pond water	c.	a cola drink
b.	sugar	d.	concrete

____ 4. An example of a chemical change is _____.

a.	melting	c.	burning
b.	electrical conductivity	d.	density

____ 5. The density of a material depends on _____.

a.	its mass only	c.	its mass and volume
b.	its volume only	d.	its weight

____ 6. In a list of the densities of common materials, the one density that might not seem reasonable is _____.

a.	35 885 g/mL	c.	2.54 g/mL
b.	0.45 g/mL	d.	1.000 g/mL

____ 7. The structure of matter refers to its _____.

a.	behavior	c.	measurements
b.	composition	d.	reactions

____ 8. Which of the following is not an example of a model?

a.	a floor lamp	c.	a road map
b.	a globe	d.	a wind tunnel

____ 9. Classification based on measurements is said to be _____.

a.	composed	c.	qualitative
b.	observed	d.	quantitative

____ 10. Gold melts at 1064ºC. Melting point is a _____.

a.	chemical change	c.	physical change
b.	chemical property	d.	physical property

____ 11. In ocean water, salt is a(n) _____.

a.	alloy	c.	solution
b.	solute	d.	solvent

____ 12. Sugar, which is a substance, can be broken down into carbon, oxygen, and hydrogen. Sugar is a(n) _____.

a.	compound	c.	mixture
b.	element	d.	solution

____ 13. A 1-g sample of the compound hydrogen chloride was analyzed and found to be 2.74 percent hydrogen and 97.3 percent chlorine. What percentage of hydrogen is present in a 2-g sample of hydrogen chloride?

a.	1.37%	c.	5.48%
b.	2.74%	d.	97.3%

____ 14. How many atoms are present in one unit of sodium sulfate, Na₂SO₄?

a.	1	c.	4
b.	2	d.	7

____ 15. Which of the following has the greatest density?

a.	a rock	c.	oil
b.	oxygen	d.	ice

____ 16. A 26.0-g sample of a liquid was found to have a volume of 13.0 mL. What is the density of the liquid?

a.	0.500 g/mL	c.	39.0 g/mL
b.	2.00 g/mL	d.	338 g/mL

____ 17. Coal burns in a furnace, producing light and heat. This reaction is _____.

a.	a physical change	c.	energetic
b.	endothermic	d.	exothermic

____ 18. The scientific statement that says that compounds always have exactly the same composition by mass is the _____.

a.	atomic theory	c.	law of conservation of matter
b.	matter hypothesis	d.	law of definite proportions

____ 19. When a hypothesis is tested by many experiments, it becomes a(n) _____.

a.	scientific law	c.	theory
b.	revised hypothesis	d.	experimental fact

____ 20. The atomic number of an element whose atoms have 9 protons and 10 neutrons is _____.

a.	9	c.	10
b.	19	d.	18

____ 21. The mass number of an element whose atoms have 12 protons and 13 neutrons is _____.

a.	12	c.	25
b.	13	d.	12.5

____ 22. One isotope of carbon has 6 protons and 6 neutrons. The number of protons and neutrons of a second isotope of carbon would be _____.

a.	7 and 6	c.	7 and 7
b.	6 and 7	d.	6 and 6

____ 23. According to the law of conservation of matter, if 4.0 g of hydrogen react with chlorine to produce 146 g of hydrogen chloride, how many grams of chlorine reacted?

a.	4.0 g	c.	146 g
b.	142 g	d.	150 g

____ 24. If 9.0 g of water contain 1.0 g of hydrogen, what mass of oxygen is contained in 36 g of water?

a.	4.0 g	c.	10.0 g
b.	8.0 g	d.	32 g

____ 25. Which of the following statements is not a main point of Dalton's atomic theory?

a.	All matter is made up of atoms.
b.	Atoms are made up of smaller particles.
c.	Atoms are indestructible.
d.	All atoms of one element are exactly alike, but they are different from atoms of other elements.

____ 26. What is a good comparison of the charge of an electron and the charge of a proton?

a.	They are equal, but opposite.	c.	They are the same.
b.	The charge of the electron is larger.	d.	The charge of the proton is larger.

____ 27. Iodine-131 and iodine-127 are examples of _____.

a.	nuclei	c.	isotopes
b.	isomers	d.	neutrons

____ 28. The discovery of isotopes led to the discovery of _____.

a.	atoms	c.	protons
b.	electrons	d.	neutrons

____ 29. Which of the following are definitely in atoms of the same element?

a.	3 protons, 3 neutrons and 3 protons, 4 neutrons
b.	3 protons, 3 neutrons and 4 protons, 4 neutrons
c.	4 protons, 4 neutrons and 3 protons, 4 neutrons
d.	3 protons, 4 neutrons and 4 protons, 3 neutrons

____ 30. Atomic mass units are based on the mass of an atom of _____.

a.	carbon-12	c.	oxygen-16
b.	carbon-14	d.	nitrogen-14

____ 31. The _____ is where the electron is most likely to be found.

a.	energy level	c.	electron cloud
b.	electron orbit	d.	orbit

____ 32. An atom of iron contains 26 electrons. How many energy levels are needed to contain these electrons?

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

____ 33. In a Lewis dot diagram, the dots represent _____ in the atom.

a.	all the electrons	c.	the protons
b.	the valence electrons	d.	the neutrons

____ 34. Which of the following is an example of periodicity?

a.	eating breakfast	c.	writing a letter
b.	hitting a home run	d.	sneezing

____ 35. Which element is least likely to be used in semiconductors?

a.	silicon	c.	sulfur
b.	phosphorus	d.	boron

____ 36. Chlorine, iodine, and _____ make up the halogen triad.

a.	bromine	c.	sodium
b.	lithium	d.	potassium

____ 37. The second row of the periodic table includes _____ elements.

a.	2	c.	18
b.	8	d.	32

____ 38. Which of the following is a transition element?

a.	gallium	c.	aluminum
b.	nickel	d.	tellurium

____ 39. Which of the following events is periodic?

a.	a basketball game	c.	snowfall
b.	tides	d.	a single flower blooming

____ 40. The blank spaces in Mendeleev's periodic table represented _____.

a.	liquids	c.	nonexistent elements
b.	gases	d.	undiscovered elements

____ 41. Modern periodic law states that properties of elements repeat in a regular pattern when the elements are arranged in order of increasing _____.

a.	density	c.	atomic number
b.	atomic mass	d.	periodicity

____ 42. Horizontal rows of the periodic table are known as _____.

a.	groups	c.	periods
b.	families	d.	columns

____ 43. Columns of the periodic table are known as _____.

a.	groups	c.	similarities
b.	periods	d.	rows

____ 44. Most elements are _____.

a.	metals	c.	metalloids
b.	nonmetals	d.	synthetic

____ 45. Which of the following is not a characteristic of a metal?

a.	lustrous	c.	brittle
b.	conducts heat	d.	flexible

____ 46. Which groups are considered to be transition elements?

a.	1 and 2	c.	1, 2, and 18
b.	3 through 12	d.	13 through 18

____ 47. A certain element is a gas and does not conduct electricity or heat. Which of the following is a possible number of valence electrons for the atoms of this element?

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

____ 48. Most semiconductors are _____.

a.	metals	c.	metalloids
b.	nonmetals	d.	synthetics

____ 49. The properties of a compound are _____ the properties of the elements that form it.

a.	similar to	c.	identical to
b.	different from	d.	derived from

____ 50. A colorless, odorless gas combines with a magnetic, metallic element. What can you predict about the product?

a.	It will also be magnetic.
b.	A gas and a solid produce a liquid.
c.	The compound will be shiny and odorless.
d.	It is impossible to predict its specific properties.

____ 51. Noble gases _____.

a.	form no compounds
b.	form compounds easily
c.	form no compounds that occur naturally in the environment
d.	do not obey the octet rule

____ 52. Oppositely charged ions attract each other, forming a(n) _____ bond.

a.	covalent	c.	ionic
b.	crystal	d.	molecular

____ 53. The strong crystal structure of an ionic compound is one reason ionic compounds have _____ melting points.

a.	high	c.	moderate
b.	low	d.	variable

____ 54. The formula for iron(III) oxide, Fe₂Cl₃, shows that one unit of the compound contains _____ iron atoms.

a.	2	c.	5
b.	3	d.	6

____ 55. Two atoms of bromine react with each other to form a(n) _____ bond.

a.	covalent	c.	crystal
b.	ionic	d.	molecular

____ 56. Electron sharing produces _____.

a.	crystals	c.	molecules
b.	ions	d.	liquids

____ 57. A covalent compound is most likely formed from _____.

a.	two metals	c.	two metalloids
b.	two nonmetals	d.	a metal and a nonmetal

____ 58. Nitrogen atoms each have five valence electrons. How many pairs of electrons must be shared in a molecule of N₂?

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

____ 59. Noble gases are sometimes used to protect valuable documents because they are _____.

a.	molecular	c.	unreactive
b.	totally inert	d.	unstable

____ 60. When reacting with an atom of fluorine, an atom of lithium will lose an electron and become a lithium _____.

a.	compound	c.	ion
b.	crystal	d.	molecule

____ 61. When an atom loses an electron, it becomes a _____ ion.

a.	negative	c.	neutral
b.	positive	d.	polyatomic

____ 62. A tug-of-war in which neither side is able to move the other side could be used to model a(n) _____.

a.	covalent bond	c.	ionic bond
b.	crystal	d.	transfer of electrons

____ 63. A substance will conduct an electric current if it _____.

a.	is wet	c.	is covalent
b.	forms ions in solution	d.	consists of ions in the dry state

____ 64. Which of the following is the correct chemical formula for a formula unit of aluminum bromide?

a.	AlBr₃	c.	Al₃Br₉
b.	Al₂Br₆	d.	Al₄Br₁₂

____ 65. Based on its position in the periodic table, the most likely charge of an iodide ion is _____.

a.	1+	c.	2+
b.	1-	d.	7-

____ 66. Which of the following formulas is incorrect?

a.	Al₂(SO₄)₃	c.	Ca(OH)₂
b.	AlOH₃	d.	(NH₄)₂S

____ 67. The correct name for Fe₂S₃ is _____.

a.	iron(III) sulfide	c.	iron(II) sulfide
b.	iron sulfide	d.	iron(I) sulfide

____ 68. In order to separate two liquids from each other by distillation, they must _____.

a.	evaporate at the same temperature	c.	both be molecular substances
b.	evaporate at different temperatures	d.	both be inorganic compounds

____ 69. Each row in the periodic table ends with a _____.

a.	metal	c.	metalloid
b.	nonmetal	d.	noble gas

____ 70. In going from left to right in any given row in the periodic table, the size of atoms generally _____.

a.	increases	c.	stays the same
b.	decreases	d.	changes randomly

____ 71. Compared to the neutral atom from which it is derived, a negative ion is _____.

a.	always larger
b.	always smaller
c.	larger in some cases and smaller in others
d.	the same size

____ 72. When compared to the main group metals, transition metals have melting and boiling points that are _____.

a.	always lower	c.	about the same
b.	usually higher	d.	usually lower

____ 73. Transition elements, such as chromium, are likely to have _____.

a.	an oxidation number of 1+	c.	multiple oxidation numbers
b.	an oxidation number of 2+	d.	a negative oxidation number

____ 74. The two actinides used as nuclear fuels are uranium and _____.

a.	plutonium	c.	americium
b.	californium	d.	thorium

____ 75. The atoms of an element in Group 2 are _____ atoms of a Group 13 element in the same period.

a.	larger than	c.	the same size as
b.	smaller than	d.	impossible to compare with

____ 76. A metallic ion is _____ its corresponding atom.

a.	larger than	c.	the same size as
b.	smaller than	d.	impossible to compare with

____ 77. Ionic radii _____ down a group in the periodic table.

a.	increase	c.	stay the same
b.	decrease	d.	follow no pattern

____ 78. Plants need the alkaline earth element _____ in photosynthesis.

a.	magnesium	c.	strontium
b.	calcium	d.	barium

____ 79. The most unreactive group of elements is the _____.

a.	halogens	c.	alkali metals
b.	noble gases	d.	transition elements

____ 80. Most transition metals have _____ oxidation state(s).

a.	no	c.	two
b.	only one	d.	multiple

____ 81. Because transition metals have similar atomic radii, transition metals have _____ chemical properties.

a.	similar	c.	definitely different
b.	no	d.	identical

____ 82. Because of its ability to bond with oxygen, _____ is an essential element in the hemoglobin in blood.

a.	tin	c.	copper
b.	iron	d.	manganese

____ 83. An example of a chemical formula is _____.

a.	Na	c.	H₂SO₄
b.	4.5 g/mL	d.	d = 13.6 g/L

____ 84. When ice melts and becomes liquid water, it has undergone a _____.

a.	chemical change	c.	physical change
b.	chemical property	d.	physical property

____ 85. A soft drink is an example of a(n) _____.

a.	compound	c.	heterogeneous mixture
b.	element	d.	homogeneous mixture

Give a balanced chemical equation for each reaction.

86. barium chloride and potassium sulfate:

a. BaCl + KSO₄ ® BaSO₄ + KCl

b. BaCl₂ + K₂SO₄ ® BaSO₄ + KCl

c. BaCl + KSO₄ ® BaSO₄ + KCl

d. BaCl₂ + K₂SO₄ ® BaSO₄ + 2KCl

e. 2BaCl₂ + K₂SO₄ ® 2BaSO₄ + 2KCl

87. magnesium metal and iron(III) chloride:

a. Mg + 2FeCl₃ ® 3MgCl₂ + 2Fe

b. 3Mg + 2FeCl₃ ® 3MgCl₂ + 2Fe

c. 3Mg + FeCl₃ ® 3MgCl₂ + 2Fe

d. 3Mg + 2FeCl₃ ® MgCl₂ + 2Fe

e. 3Mg + 2FeCl ® 3MgCl₂ + Fe

88. propane (C₃H₈) gas:

a. C₃H₈ + O₂ ® CO₂ + H₂O

b. C₃H₈ + 5O₂ ® CO₂ + 4H₂O

c. C₃H₈ + 5O₂ ® 3CO₂ + H₂O

d. C₃H₆ + 4.5O₂ ® 3CO₂ + 3H₂O

e. C₃H₈ + 5O₂ ® 3CO₂ + 4H₂O