Chemistry--Final Exam 2005

Chemistry--Final Exam 2005

Multiple Choice

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

____ 1. Each row in the periodic table ends with a _____.

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

____ 2. 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

____ 3. 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

____ 4. 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

____ 5. 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

____ 6. 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

____ 7. A metallic ion is _____ its corresponding atom.

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

____ 8. Bromine is a typical nonmetal. A bromide ion is _____ a bromine atom.

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

____ 9. Ionic radii _____ down a group in the periodic table.

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

____ 10. Alkaline earth metals lose _____ electrons to achieve the electron configuration of the noble gas in the preceding period.

a.	one	c.	six
b.	two	d.	seven

____ 11. Alloys of magnesium are commonly used because they are _____.

a.	heavy and strong	c.	lightweight and strong
b.	strong and rigid	d.	reactive

____ 12. Plants need the alkaline earth element _____ in photosynthesis.

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

____ 13. Group 13 elements tend to form _____.

a.	ionic compounds	c.	alloys
b.	covalent compounds	d.	metalloids

____ 14. The most unreactive group of elements is the _____.

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

____ 15. In general, main group elements have _____ melting points and boiling points when compared with transition metals.

a.	higher	c.	much lower
b.	slightly lower	d.	the same

____ 16. Most transition metals have _____ oxidation state(s).

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

____ 17. Because transition metals have similar atomic radii, transition metals have _____ chemical properties.

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

____ 18. 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

____ 19. Which of the following elements is not in the iron triad?

a.	cobalt	c.	nickel
b.	copper	d.	iron

____ 20. Which of the following elements is not a coinage metal?

a.	copper	c.	platinum
b.	gold	d.	silver

____ 21. One physical property of acids is a _____.

a.	slippery feel	c.	sour taste
b.	pink color	d.	presence of hydrogen

____ 22. Acids react with carbonates to produce _____.

a.	hydrogen	c.	a hydronium ion
b.	a base	d.	carbon dioxide

____ 23. The top industrial chemical produced in the United States for many years has been _____.

a.	sulfuric acid	c.	hydrochloric acid
b.	ammonia	d.	oxygen

____ 24. An example of a polyprotic acid is _____.

a.	HCl	c.	H₂SO₄
b.	HC₂H₃O₂	d.	HCN

____ 25. Ammonia is considered to be a base because it _____.

a.	loses hydroxide ions in water	c.	contains hydrogen
b.	contains the hydroxide ion	d.	accepts hydrogen ions

____ 26. A piece of blue litmus paper placed into water through which carbon dioxide gas is bubbled will _____.

a.	turn pink	c.	show no change
b.	remain blue	d.	lose its color

____ 27. Oxides of nitrogen and sulfur are _____.

a.	acids	c.	acidic anhydrides
b.	bases	d.	basic anhydrides

____ 28. The weak acid in the following list is _____.

a.	hydrochloric acid	c.	nitric acid
b.	sulfuric acid	d.	acetic acid

____ 29. An acidic solution would have a pH of _____.

a.	less than 7	c.	7 or above
b.	more than 7	d.	7 or below

____ 30. Conductivity of an acid or a base in water is affected by all of the following except _____.

a.	strength	c.	molarity
b.	an indicator	d.	pH

____ 31. The total number of possible different kinds of acid-base reactions is _____.

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

____ 32. The reaction between an acid and a base always results in the formation of _____.

a.	a salt	c.	a basic anhydride
b.	an acid anhydride	d.	a spectator ion

____ 33. The type of acid-base reaction that always goes to completion is the reaction between _____.

a.	a weak acid and a weak base	c.	a strong acid and a weak base
b.	a weak acid and a strong base	d.	a strong acid and a strong base

____ 34. According to the Bronsted-Lowry definition, an acid is a substance that _____.

a.	releases H⁺ in solution	c.	accepts protons
b.	donates hydrogen atoms	d.	donates protons

____ 35. In the reaction CO₃^2- + H⁺ ® HCO₃^¯, the base is _____.

a.	CO₃^2-	c.	HCO₃^¯
b.	H⁺	d.	not shown

____ 36. The effect of antacid on stomach fluids is to _____.

a.	make them neutral	c.	increase their pH
b.	make them basic	d.	decrease their pH

____ 37. The six extra electrons in a benzene molecule are _____.

a.	arranged in double bonds
b.	arranged in alternate single and double bonds
c.	shared equally by all six carbon atoms
d.	shared equally by all six hydrogen atoms

____ 38. An organic compound that contains a carbon atom bonded to a hydrogen atom and double-bonded to an oxygen atom is an _____.

a.	alkene	c.	aldehyde
b.	alcohol	d.	ether

____ 39. A process that typically yields alcohols is _____.

a.	distillation	c.	polymerization
b.	fermentation	d.	cracking

____ 40. Which pair of reactants listed below could take part in a condensation reaction?

a.	methane and an alcohol	c.	an alkane and an alcohol
b.	water and an alcohol	d.	an amine and a carboxylic acid

____ 41. The burning of gasoline in an automobile engine is an example of a(n) _____.

a.	photosynthesis reaction	c.	exothermic reaction
b.	endothermic reaction	d.	reversible reaction

____ 42. In a chemical change, energy can be _____.

a.	created, but not destroyed	c.	either created or destroyed
b.	destroyed, but not created	d.	neither created nor destroyed

____ 43. An example of a process in which entropy decreases is _____.

a.	melting	c.	boiling
b.	freezing	d.	vaporization

____ 44. The main source of energy for living things on Earth is _____.

a.	combustion of fossil fuels	c.	solar energy
b.	oxidation of dead organisms	d.	geothermal energy

____ 45. The major product formed during the process of photosynthesis is _____.

a.	carbon dioxide	c.	sugar
b.	water	d.	DNA

____ 46. Even in an exothermic reaction, _____ is needed to get the reaction started.

a.	activation energy	c.	an endothermic reaction
b.	a catalyst	d.	an inhibitor

____ 47. If the heat of reaction is negative, the reaction is _____.

a.	endothermic	c.	negative
b.	exothermic	d.	positive

____ 48. When bowling pins at the end of an alley are hit by a bowling ball, the entropy of the pins _____.

a.	decreases	c.	is spontaneous
b.	increases	d.	stays the same

____ 49. A _____ is the heat required to raise the temperature of 1 g of liquid water by 1ºC.

a.	calorie	c.	kilocalorie
b.	Calorie	d.	joule

____ 50. In processes that produce electricity, some of the energy used is wasted as _____ energy.

a.	chemical	c.	kinetic
b.	heat	d.	light