CHEM2 Chemistry in Your World 2nd Edition by Hogg - Test Bank

CHEM2 Chemistry in Your World 2nd Edition by Hogg – Test Bank

 

Instant Download – Complete Test Bank With Answers

 

 

Sample Questions Are Posted Below

 

MULTIPLE CHOICE

 

1. Magnesium nitride is made up of magnesium ions and nitride ions. What is the expected formula of magnesium nitride?

a.	MgN
b.	Mg2N3
c.	MgN2
d.	Mg3N2

 

 

ANS:  D

 

2. Which is not true about the ionic compound sodium chloride (NaCl)?

a.	It is electrically neutral.
b.	It was formed when electrons were shared.
c.	It has properties different from the atoms from which it is formed.
d.	It is a white crystalline solid.

 

 

ANS:  B

 

3. Which one of the following shows the possible ions for iron?

a.	Fe2+ and Fe4+
b.	Fe+ and Fe2+
c.	Fe2+ and Fe3+
d.	Fe3+ and Fe+

 

 

ANS:  C

 

4. The compound between calcium and chlorine is calcium chloride and has which of the following formulas?

a.	Cl2Ca3
b.	Ca2Cl
c.	CaCl2
d.	ClCa2

 

 

ANS:  C

 

5. Washing soda, soda ash, and baking soda all contain which of the following groupings?

a.	OH–
b.	CO32–
c.	PO43–
d.	NO3–

 

 

ANS:  B

 

6. Which is expected to form a negative ion?

a.	K
b.	Ne
c.	Na
d.	F

 

 

ANS:  D

 

7. Which of the following would be used to recognize an unsaturated hydrocarbon in its structural formula?

a.	presence of a lone pair of electrons
b.	multiple covalent bond
c.	presence of carbon and hydrogen
d.	fits the general formula CnH2n+2

 

 

ANS:  B

 

8. How many nonbonding electrons are in the water molecule?

a.	0
b.	2
c.	4
d.	6

 

 

ANS:  C

 

9. Of the following, which is the strongest bond?

a.	C:C, single bond
b.	C::C, double bond
c.	C:::C, triple bond
d.	All are of equal strength.

 

 

ANS:  C

 

10. If you take three balloons, blow them up and assemble them together, the shape you are most likely to observe is

a.	linear.
b.	tetrahedral.
c.	pyramidal.
d.	trigonal planar.

 

 

ANS:  D

 

11. Which is not a property of ionic compounds?

a.	many are liquids at room temperature
b.	high melting point
c.	crystalline solid
d.	melted ionic materials are conductors of electricity

 

 

ANS:  A

 

12. An ion contains 16 protons, 16 neutrons, and 18 electrons. Its charge is

a.	0.
b.	+2.
c.	–2.
d.	–18.

 

 

ANS:  C

 

 

13. What ion is likely to be formed by magnesium (Mg) in chemical reactions?

a.	Mg+
b.	Mg2+
c.	Mg–
d.	Mg2–

 

 

ANS:  B

 

14. Which of the following substances has polar covalent bonds?

a.	CaF2
b.	KBr
c.	NH3
d.	CH4

 

 

ANS:  C

 

15. Which substance has ionic bonds between atoms?

a.	Na2O
b.	NCl3
c.	H2S
d.	CO2

 

 

ANS:  A

 

16. The shape of CH₄ and CCl₄ are best described as

a.	tetrahedral.
b.	pyramidal.
c.	hexagonal.
d.	octahedral.

 

 

ANS:  A

 

17. Which substance is most likely to have covalent bonds between atoms?

a.	AlCl3
b.	KBr
c.	MgF2
d.	PCl3

 

 

ANS:  D

 

18. A new element has the symbol Y and seven valence electrons. What is the maximum number of hydrogen atoms that can bond to Y?

a.	1
b.	4
c.	3
d.	7

 

 

ANS:  A

 

 

19. Which of the following pairs of atoms share electrons equally?

a.	Cl and H
b.	Mg and Cl
c.	C and C
d.	S and F

 

 

ANS:  C

 

20. Which of the following pairs of atoms form the most polar bond?

a.	C and C
b.	C and F
c.	C and H
d.	C and O

 

 

ANS:  B

 

21. An atom has an electronic arrangement of 2-8-8-2. This atom is most likely to

a.	form a +2 ion
b.	bond covalently to nonmetals
c.	form a –2 ion
d.	bond covalently to metals

 

 

ANS:  A

 

22. A neutral atom can be converted to a negative ion if it

a.	gains electrons.
b.	loses electrons.
c.	gains protons.
d.	loses protons.

 

 

ANS:  A

 

23. What particles make up the crystal in a grain of table salt (sodium chloride)?

a.	atoms of sodium and chlorine
b.	molecules of sodium and chlorine
c.	sodium ions and chloride ions
d.	molecules of sodium chloride

 

 

ANS:  C

 

24. Which of the following has bond a angle of 180° between atoms?

a.	CH4
b.	SO3
c.	H2O
d.	CO2

 

 

ANS:  D

 

 

25. There are ____  electrons in the covalent bond between C and O in CO.

a.	2
b.	4
c.	6
d.	8

 

 

ANS:  C

 

26. Which of the following molecules has a double bond?

a.	CH2CH2
b.	NH3
c.	CH3CH3
d.	H2O

 

 

ANS:  A

 

27. When an ionic solid such as NaCl dissolves in water,

a.	the Na+ and Cl– are changed to atoms.
b.	the Na+ ions gather on one side of the container and the Cl– ions gather on the other side of the container.
c.	Na+ and Cl– ions are evenly dispersed.
d.	the beaker containing the solution becomes charged.

 

 

ANS:  C

 

28. How do aqueous electrolytes conduct electricity?

a.	Dissolved positive ions move to positive electrodes.
b.	Electrons migrate from one electrode to the other electrode.
c.	Ions pass electrons from ion to ion.
d.	Dissolved ions move to oppositely charged electrodes.

 

 

ANS:  D

 

29. Particles in the ____ state are in direct contact but are free to move.

a.	gas
b.	solid
c.	liquid
d.	plasma

 

 

ANS:  C

 

30. Liquids have a

a.	fixed volume and no definite shape.
b.	fixed shape and no volume.
c.	no definite shape and no volume.
d.	fixed shape and fixed volume.

 

 

ANS:  A

 

 

31. Gases

a.	exert a pressure.
b.	are compressible.
c.	are miscible, they mix with other gases in any proportion.
d.	all of these

 

 

ANS:  D

 

32. Sublimation is the process where a

a.	solid changes into a gas.
b.	solid changes into a liquid.
c.	liquid changes into a gas.
d.	liquid changes into a solid.

 

 

ANS:  A

 

33. The relation between gas pressure and volume was discovered by

a.	Robert Boyle.
b.	G. N. Lewis.
c.	Marie Curie.
d.	Rutherford.

 

 

ANS:  A

 

34. The dispersal of odors is partially due to a property of gases known as

a.	diffusion.
b.	miscibility.
c.	expansion.
d.	volatility.

 

 

ANS:  A

 

35. When enough gas molecules stick together to form small droplets of liquid, the process is called

a.	sublimation.
b.	condensation.
c.	deposition.
d.	compression.

 

 

ANS:  B

 

36. Most substances that have molecules with approximately the same weight as water molecules are gases at room temperature. Water is a liquid at room temperature because of

a.	extensive hydrogen bonding between water molecules.
b.	ionic bonding between hydrogen ions and oxide ions.
c.	covalent bonding between hydrogen atoms and oxygen atoms.
d.	the lack of motion of water molecules.

 

 

ANS:  A

 

 

37. The cooling effect that occurs when water evaporates from moist skin is a consequence of this property of water

a.	heat capacity.
b.	surface tension.
c.	heat of vaporization.
d.	vapor pressure.

 

 

ANS:  C

 

38. Surface tension of water is illustrated by this phenomenon

a.	moderating influence of lakes and oceans on climate.
b.	cooling effect that occurs when water evaporates from moist skin.
c.	beading of water droplets on the clean surface of a car’s hood and roof.
d.	expansion of water when it freezes.

 

 

ANS:  C

 

39. When a spoonful of sugar is added to a glass of iced tea, it quickly dissolves. If no solid settles to the bottom, the resulting solution is

a.	saturated.
b.	unsaturated.
c.	ionic.
d.	normal.

 

 

ANS:  B

 

40. Which statement is true about a glass of iced tea flavored with sugar and lemon juice?

a.	Sugar is a solute.
b.	Water is a solvent.
c.	Lemon juice is a solute.
d.	all of these are true

 

 

ANS:  D

 

41. Which is not characteristic of liquids?

a.	freezing point
b.	crystallization
c.	boiling point
d.	All of these are characteristic of liquids.

 

 

ANS:  D

 

42. What is the maximum number of hydrogen bonds that one water molecule can form to its neighbors in an ice crystal?

a.	0
b.	2
c.	4
d.	infinite number

 

 

ANS:  C

 

 

43. Which factor causes more gas to dissolve in a liquid?

a.	size of the container opening
b.	nature of the container (that is, glass versus metal)
c.	increasing the pressure
d.	increasing the temperature

 

 

ANS:  C

 

44. Which of the states of matter has particles in fixed positions and touching one another?

a.	solid
b.	liquid
c.	plasma
d.	gas

 

 

ANS:  A

 

45. Which molecule would be expected to exhibit the least hydrogen bonding?

a.	H—F
b.	H—O—H
c.	NH3
d.	CH4

 

 

ANS:  D

 

46. The normal boiling point of a liquid is

a.	high for volatile liquids.
b.	high for nonvolatile liquids.
c.	low for nonvolatile liquids.
d.	The same for all liquids, that is what normal means.

 

 

ANS:  B

 

47. The normal boiling point of water is

a.	what you measure in a laboratory.
b.	independent of atmospheric pressure.
c.	the one measured at 760 mm pressure (1 atm).
d.	273 K.

 

 

ANS:  C

 

48. Which of the following molecules has only single bonds?

a.	CH2CH2
b.	CH3CH3
c.	CO2
d.	CHCH

 

 

ANS:  B

 

 

49. Which is not a physical property of water?

a.	solid is less dense than liquid at normal freezing point
b.	relatively high heat capacity per unit of weight
c.	relatively low heat of vaporization
d.	relatively large surface tension

 

 

ANS:  C

 

50. Which element has the highest electronegativity?

a.	H
b.	O
c.	N
d.	C

 

 

ANS:  B

 

51. What is the expected formula for a reaction between aluminum and oxygen?

a.	AlO
b.	Al2O3
c.	AlO2
d.	Al3O2

 

 

ANS:  B

 

52. Which of the following elements can form a cation?

a.	K
b.	Ne
c.	O
d.	F

 

 

ANS:  A

 

53. Which of the following is an ionic compound?

a.	CO2
b.	NH3
c.	CaO
d.	C3H8

 

 

ANS:  C

 

54. How many nonbonding electrons are found on the central atom of sulfur dioxide?

a.	0
b.	2
c.	4
d.	6

 

 

ANS:  C

 

 

55. What is name of the following compound NH₄NO₃?

a.	ammonia nitrite
b.	ammonium nitrite
c.	nitrogen hydride nitrite
d.	ammonium nitrate

 

 

ANS:  D

 

56. What is the charge on an ion with 7 protons, 7 neutrons, and 10 electrons?

a.	0
b.	+3
c.	–3
d.	–7

 

 

ANS:  C

 

57. Which atom exists as a diatomic molecule in nature?

a.	carbon
b.	bromine
c.	sulfur
d.	phosphorous

 

 

ANS:  B

 

58. Identify the saturated hydrocarbon listed below.

a.	C3H8
b.	C4H8
c.	C2H4
d.	C6H6

 

 

ANS:  A

 

59. How many resonance structures can be drawn for a nitrate ion?

a.	0
b.	1
c.	2
d.	3

 

 

ANS:  D

 

60. What is the electron pair geometry for silicon dioxide?

a.	linear
b.	bent
c.	trigonal pyramidal
d.	tetrahedral

 

 

ANS:  A

 

 

61. What is the molecular geometry of carbon tetrachloride?

a.	tetrahedral
b.	trigonal pyramidal
c.	bent
d.	trigonal planar

 

 

ANS:  A

 

62. Which of the following is a nonpolar molecule with a polar covalent bond?

a.	HCl
b.	NH3
c.	H2O
d.	CO2

 

 

ANS:  D

 

63. How much heat is required to melt 1 kg of water (heat of melting = 80 cal/g)

a.	–80 cal
b.	+80 cal
c.	–80000 cal
d.	+80000 cal

 

 

ANS:  D

 

64. Which of the following molecules has a triple bond?

a.	CO2
b.	NH3
c.	Cl2
d.	N2

 

 

ANS:  D

 

65. What is the solvent in a solution of sodium chloride?

a.	sodium chloride
b.	sodium
c.	oxygen
d.	water

 

 

ANS:  D

 

 

66. The following image shows two molecules of sulfur dioxide.

 

 

Which of the following describes the type of bonding present?

a.	ionic bonding
b.	polar covalent bonding
c.	nonpolar covalent bonding
d.	hydrogen bonding

 

 

ANS:  B

 

67. Consider the following Lewis dot structure for ozone, O₃.

 

Based on these structures,  what is the shape of this molecule?

a.	linear
b.	bent
c.	tetrahedral
d.	trigonal planar
e.	trigonal pyramidal

 

 

ANS:  B

 

68. Consider the following image.

 

What shape is represented?

a.	linear
b.	bent
c.	tetrahedral
d.	trigonal planar
e.	trigonal pyramidal

 

 

ANS:  D

 

 

69. Choose the statement that best explains why the boiling point of ICl (97 °C) is higher than the boiling point of Br₂ (59 °C),

a.	ICl is an ionic compound,  while Br2 is a covalent compound.
b.	There is hydrogen bonding in ICl, but not in Br2.
c.	ICl is polar while Br2 is nonpolar.
d.	ICl has a bent shape while Br2 is linear.

 

 

ANS:  C

 

70. Which of the following molecules might have the shape shown below?

 

 

a.	AlCl3
b.	CCl4
c.	SO3
d.	TiCl4

 

 

ANS:  B

 

TRUE/FALSE

 

1. Positive ions are smaller than the atoms for which they form.

 

ANS:  T

 

2. Negative ions are approximately the same size as the atoms from which they form.

 

ANS:  F

 

3. A binary ionic compound generally consists of a metal and a nonmetal combination.

 

ANS:  T

 

4. Phosphorus has 3 valence electrons.

 

ANS:  F

 

5. When Na and O combine the bonding will be ionic,  while when O combines with S the bonding will be covalent.

 

ANS:  T

 

 

6. The dotted line in the following images shows the formation of hydrogen bonds.

 

ANS:  F

 

7. Consider the following two Lewis dot structures for ozone.   These two structures are termed resonance structures.

 

 

ANS:  T

 

8. The following images represent the process termed freezing.

 

 

changes to

 

 

 

ANS:  F

 

 

COMPLETION

 

Consider the image below which shows a model of the compound known as hexane.  The large spheres represent carbon and the smaller spheres represent hydrogen.

 

 

1. The total number of valence electrons in hexane is_________.

 

ANS:

38

thirty eight

 

 

2. The total number of single bonds in hexane is__________.

 

ANS:

19

nineteen

 

3. The total number of bonding electron pairs in hexane is____________.

 

ANS:

19

nineteen

 

 

MATCHING

 

Consider the following terms.  Use these to answer the questions given below.

a.	boiling
b.	melting
c.	condensation
d.	sublimation
e.	melting
f.	freezing

 

 

1. What term is given to the following process?

 

 

2. What term describes solid carbon dioxide changing to gaseous carbon dioxide?

 

3. Which process occurs when water droplets form on the outside of a glass of ice water?

 

4. For water,  which process occurs at 100 °C?

 

1. ANS:  B

 

2. ANS:  D

 

3. ANS:  C

 

4. ANS:  A

 

Consider the image given below which depicts bonds formed between two generic elements, X and Y.

 

a.	1
b.	2
c.	3

 

 

5. If X was the element K and Y the element O,  which type of bond would form?

 

6. Which bond type would represent that found in I₂?

 

7. The H—N bond in ammonia, NH₃,  would be best represented by which bond?

 

8. Which type of bond would be found in hydrochloric acid,  HCl?

 

5. ANS:  C

 

6. ANS:  A

 

7. ANS:  B

 

8. ANS:  B