Chemistry 113 practice exam | Chemistry homework help

Chemistry 113 Practice Exam 4 Spring 2016                                                                                           

Directions on actual Exam: The exam consists of 2 sections (Chemical Bonding and Geometry and IMFs. Each multiple choice question is worth 4.33 points. You are allowed to use a scientific (nonprogrammable) calculator, periodic table, and VSEPR Theory Table.     

 

Useful information:

ΔH°_rxn  =  Σn×D(bonds broken) – Σn×D(bonds formed)

where Σn represents the sum of the moles of a particular type of bond

D represents bond energy per mole of bond

Chemical Bonding and Geometry

1.	The Lewis dot symbol for the calcium ion is
	A)	2+
	B)	¾Ca¾
	C)	2+
	D)	Ca2+
	E)	Ca

 

2.	The electron dot structure for AsCl3 molecule shows
	A)	a total of 84 electron dots
	B)	three single bonds and 10 lone pairs
	C)	two single bonds, one double bond, and 9 lone pairs
	D)	one single bond, two double bonds, and 8 lone pairs
	E)	three single bonds and one lone pair

 

 

 

3.	The correct Lewis structure for CO2 is: C

A)

 

 

B)

 

 

C)

 

 

D)   

4.	Which of the following Lewis structures is incorrect?
	A)
	B)
	C)
	D)
	E)

 

5.	How many covalent bonds will be formed by bromine in BrO3– for the dot structure that expands the octet to minimize formal charge and places negative formal charges on only the most electronegative atom(s). The Pauling electronegativity values are: Br = 2.8; O = 3.5
	A)	3
	B)	4
	C)	5
	D)	6
	E)	7

 

 

6.	Estimate the enthalpy change for the reaction 2CO + O2 ® 2CO2 given the following bond energies. BE(CºO) = 1074 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol
	A)	+2380 kJ/mol
	B)	+744 kJ/mol
	C)	+1949 kJ/mol
	D)	–561 kJ/mol
	E)	–744 kJ/mol

 

7.	Give the number of lone pairs around the central atom and the molecular shape of the ion ClO3–.
	A)	0 lone pairs, trigonal
	B)	1 lone pair, bent
	C)	1 lone pair, trigonal pyramidal
	D)	2 lone pairs, T-shaped
	E)	2 lone pairs, trigonal

 

8.	Which of the following substances is/are bent? (i)  H2S      (ii).  CO2      (iii)  ClNO     (iv)  NH2–    (v)  O3
	A)	only (iii)
	B)	only (i) and (v)
	C)	only (i), (iii), and (v)
	D)	all are bent except for (iv)
	E)	all are bent except for (ii)

 

 

9.	Which of the following molecules is polar?
	A)	CH4
	B)	SF6
	C)	F2
	D)	CH3F
	E)	CO2

 

10.	Indicate the type of hybrid orbitals used by the central atom in TeF4.
	A)	Sp
	B)	sp2
	C)	sp3
	D)	sp3d
	E)	sp3d2

 

11.	The hybridization of the O atom in CO2 will be
	A)	S
	B)	Sp
	C)	sp2
	D)	sp3
	E)	sp3d

 

12.	The number of pi bonds in the molecule below is
	A)	1
	B)	2
	C)	3
	D)	5
	E)	9

 

IMF’s

13.     Order the forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest .

a)       dipole-dipole, London dispersion, ionic, and hydrogen-bonding

b)       London dispersion, dipole-dipole, hydrogen-bonding, and ionic

c)       hydrogen-bonding, dipole-dipole, London dispersion, and ionic

d)       dipole-dipole, ionic, London dispersion, and hydrogen-bonding

e)       London dispersion, ionic, dipole-dipole, and hydrogen-bonding

 

14.     Which of the following would you expect to have the highest boiling point?

a)       F₂

b)       Cl₂

c)       Br₂

d)       I₂

e)       All of the above have the same boiling point.

 

15.     The molecules in a sample of SO₂ are attracted to each other by a combination of

a)       London forces and H-bonding

b)       H-bonding and ionic bonding

c)       covalent bonding and dipole-dipole interactions

d)       London forces and dipole-dipole interactions

e)       none of these

 

16.     When a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction?

a)       a hydrogen from one molecule and a hydrogen from the other molecule

b)       a hydrogen from one molecule and an oxygen from the other molecule

c)       an oxygen from one molecule and an oxygen from the other molecule

d)       an oxygen and a hydrogen from the same molecule

e)       two hydrogens from one molecule and one hydrogen from the other molecule

 

Chemical Bonding and Geometry

 

17. Which formula is matched with the correct number of valence electrons in the free (not bonded) central atom, bonds, and lone pairs in the molecule for the underlined atom?

            a. SeH₂; 6 valence electrons, 2 bonds, and 1 lone pair

            b. SiCl₄; 4 valence electrons, 4 bonds, and 0 lone pairs

            c. FCl; 1 valence electron, 1 bond, and 0 lone pairs

            d. SCl₂; 6 valence electrons, 2 bonds, and 0 lone pairs

            e. PH₃; 4 valence electrons, 3 bonds, and 1 lone pair

 

18. The electron-dot structure for the species NH₄O⁺ contains

            a. 1 double bond and 4 single bonds

            b. 5 single bonds and 3 lone pairs.

            c. 5 single bonds and 2 lone pairs.

            d. 5 single bonds and 1 lone pair.

            e. 5 single bonds and zero lone pairs.

 

19. What is the hybridization of the carbon atom in CO₂?

            a. sp²

                b. sp³

                c. sp³d

                d. sp³d²

                e. sp

20. Which of the following molecules requires two resonance hybrid Lewis structures to account for the bonding?

a.    SO₂

b.   CO₂

c.    O₂

d.   CH₄

e.    C₂H₄

21. Which of the following is the best electron-dot description for sulfur dioxide, SO₂?

22. Which of the following compounds (or ions) contains an atom that does NOT follow the octet rule?

1. BrF₃
2. CBr₄
3. NO⁺
4. BF₄^–
5. NCl₃

23. What is atom X in the Lewis structure of the following anion?

1. Xe
2. Cl
3. S
4. N
5. C

24.  Which of the following statements is correct?

a. Covalent bonds usually involve two nonmetals and ionic bonds usually involve two metals.

b. Covalent bonds usually involve two metals and ionic bonds usually involve a metal and a nonmetal.

c. Covalent bonds usually involve a metal and a nonmetal and ionic bonds usually involve two nonmetals.

d. Covalent bonds usually involve two nonmetals and ionic bonds usually involve a metal and a nonmetal.

e. Covalent bonds usually involve two metals and ionic bonds involve two nonmetals.

25. The molecular structure of the IO₃^– ion is best described as:

a. bent or angular.

b. trigonal planar.

c. trigonal pyramidal.

d. trigonal bipyramidal.

e. T-shaped.

26. The electron domain geometry of the AsF₆^– ion is octahedral.  The hybrid orbitals used by the As atom for bonding are:

            a. sp²

            b. sp³d

            c. sp

            d. sp³d²

                e. sp³ 

27. The F-B-F bond angle in BF₃ is ____________.

            a. 60°

                b. 90°

                c. 109.5°

                d. 120°

                e. 180°

28. The geometry associated with sp hybridization is:

            a. linear

            b. octahedral

            c. trigonal biplanar

            d. trigonal planar

            e. tetrahedral

29.  Which series of elements is arranged in order of increasing electronegativity?

a. C, Si, P, As, Se

b. O, P, Al, Mg, K

c. Na, Li, B, N, F

d. K, Mg, Be, O, N

e. Li, Be, B, C, Ca

IMF’s

Use the following to answer questions 30-32:

Consider the representations below to answer the next three questions.

(I)

(II)

(III)

30.     How many of the following statements are correct concerning drawing I?

a)       0

b)       1

c)       2

d)       3

e)       4

31.     Which drawing best represents the interactions in a sample of HF?

a)       I

b)       II

c)       III

d)       I, II

e)       all of the above

32.     Which of the following statements are incorrect concerning drawing III?

a)       Electrostatic interactions exist between the molecules.

b)       The molecules find the best compromise between attraction and repulsion.

c)       These molecules exhibit ionic bonding.

d)       CHCl₃ exhibits this type of interaction.

e)       Two of the above statements are incorrect.

33.     Which of the following is the correct order of boiling points for KNO₃, CH₃OH, C₂H₆, Ne?

a)       Ne < CH₃OH < C₂H₆ < KNO₃

b)       KNO₃ < CH₃OH < C₂H₆ < Ne

c)       Ne < C₂H₆ < KNO₃ < CH₃OH

d)       Ne < C₂H₆ < CH₃OH < KNO₃

e)       C₂H₆ < Ne < CH₃OH < KNO₃

34. What is the strongest intermolecular force (IMF) found in a sample of thousands of C₂H₆ molecules?

a.       London          b. dipole dipole          c. nonpolar          d. H bond force        e. polar

35. What is the strongest intermolecular force (IMF) found in a sample of thousands of HBr molecules?

a.London          b. dipole dipole          c. nonpolar          d. H bond force        e. polar

36. What is the strongest intermolecular force (IMF) found in a sample of thousands of He atoms?

a. London          b. dipole dipole          c. nonpolar          d. H bond force        e. polar

37. What holds the N atom to the H atom in a molecule of ammonia, NH₃?

a.Ionic bond          b. polar bond         c. H bond          d. nonpolar bond         e. dipole dipole

38. What holds the molecules together in a sample of ammonia, NH₃?

a.       Dipole dipole forces          b. polar bonds         c. H bond forces         d. London forces

39. What holds the O atoms to each other in a molecule of oxygen gas?

a.       Ionic bond          b. polar bond         c. H bond          d. nonpolar bond         e. dipole dipole

40. As intermolecular forces increase, which of the following decreases?

a.       Surface tension        b. Boiling Point          c. Vapor Pressure          d. Melting Point          e. Viscosity

41.Which is true when comparing samples of C₆H₆(l) (has C-H bonds) to C₂H₅OH(l) (has an O-H bond)?

a    The vapor pressure of C₂H₅OH is higher.

b.      The boiling point of C₆H₆ is higher.

c.       The surface tension of C₂H₅OH is lower.

d.      The melting point of C₂H₅OH is lower.

e.      The viscosity of C₆H₆ is lower.