Unit 9 Review - gbschemphysgbschemphys.com/honchem/reviews/U9Review.pdfUnit 9 Review Ionic and...

Unit 9 Review

Ionic and Covalent Bonding

1. Which of the following is a covalent compound composed of nonpolar covalent bonds?

a. NaF b. H2O c. H

2 d . CF

4 e. CH

4

2. Which of the following bonds is the most polar?

a. C -- C b. C -- F c. C -- O d . C -- N e. F – F

3. Which of the following occur when two atoms of d ifferent elements bond together? Bubble in all

that apply.

a. A compound is formed.

b. New elements with d ifferent numbers of protons are formed.

c. The ind ividual atoms become more stable.

d . The potential energy of the atoms is lowered .

e. Protons and neutrons are re-arranged .

4. Which one of the following families of elements are characterized by atoms which alread y have a

full octet of outer electrons?

a. alkali metals b. noble gases c. alkali earth metals

d . halogens e. transition metals

5. Most main-block elements become more stable by _____.

a. losing all their electrons b. gaining more electrons

c. gaining more protons d . achieving an octet of ou ter shell electrons

e. filling their d orbitals with electrons ab. emptying their d orbitals of electrons

6. Most elements become more stable by achieving an electron configuration which is similar to _____.

a. some other element b. a noble gas

c. a transition metal d . a halogen

e. a non-rad ioactive element.

7. Consider the element w ith the electron configuration shown at the right.

This element would be expected to

a. gain 1 more electron b. gain 2 more electrons

c. gain 5 more electrons d . gain 7 more electrons

e. lose 1 electron ab. lose 2 electrons

ac. lose 5 electrons ad . lose 7 electrons

ae. lose 9 electrons bc. ...nonsense! Elements are not that pred ictable.

8. Which of the following atoms would be expected to be stable? Bubble in all that apply .

9. The element represented by the orbital d iagram shown at the

right would be expected to _____ in order to achieve a stable

octet.

a. gain 1 more electron

b. gain 3 more electrons

c. gain 5 more electrons

d . gain 8 more electrons

e. lose 1 electron

ab. lose 5 electrons

ac. lose 7 electrons

ad . lose 8 electrons

ae. ... nonsense! It alread y has a stable octet.

10. If a neutral atom gains 2 electrons, then it acquires a _____.

a. +2 charge b. -2 charge c. … nonsense! Not enough information to tell

11. If a neutral atom loses three electrons, then it acquires a _____.

a. +3 charge b. -3 charge c. … nonsense! Not enough information to tell

12. The orbital d iagram of a neutral atom is shown at the right.

This atom will either gain or lose electrons in order to become

stable. As such it would become an ion. This atom would be

expected to become a _____.

a. +2 ion b. +3 ion c. +5 ion

d . +7 ion e. -1 ion ab. -3 ion ac. -5 ion

13. If a particle is an ion, then one can be certain that _____.

a. the number of protons is greater than the number of neutrons

b. the number of electrons is greater than the number of neutrons

c. the number of protons is greater than the number of electrons

d . the number of electrons is greater than the number of protons

e. the number of protons is not equal to the number of neutrons

ab. the number of electrons is not equal to the number of neutrons

ac. the number of protons is not equal to the number of electrons

14. Based on the orbital shell d iagram shown at the right, one would

reason that this particle would _______ in order to become stable.

a. gain 1 electron b. gain 2 electrons c. gain 7 electrons

d . gain 8 electrons e. lose 1 electron ab. lose 2 electrons

ac. lose 7 electrons ad . lose 8 electrons

ae. ... nonsense! This particle is already stable.

15. There is a whole category of elements which are characterized by atoms which typ ically lose 1

electron in order to become stable. Identify the category.

a. Halogens b. Transition metals c. Alkaline earth metals

d . Noble Gases e. Alkali metals ab. None of these.

16. There is a whole category of elements which are characterized by atoms which typ ically gain 2

electrons in order to become stable. Identify the category .



17. There is a whole category of elements which are characterized by atoms which always form stable

+2 ions. Identify the category.



18. There is a whole category of elements which are characterized by atoms which always form stable -1

ions. Identify the category.



19. Iod ine (I) atoms would be likely to ______ (gain, lose) ____ electrons and become a ______ ion.

a. gain, 1, +1 b. gain, 1, -1 c. gain, 2, +2 d . gain, 2, -2

e. lose, 1, +1 ab. lose, 1, -1 ac. lose, 2, +2 ad . lose, 2, -2

ae. none of the above

20. Based on their electron arrangements, which of the following particles could be expected to be

stable? Bubble in all that apply.

21. Based on their electron arrangements, which of the following particles could be expected to be


a. F+ ion b. Cl

_ ion c. S

2- ion d . Al atom e. O

2- ion

22. Based on their electron arrangements, which of the followin g particles could be expected to be


23. When the element Li and the element O form an ionic bond , _____.

a. one Li atom transfers 1 electron to one O atom

b. one O atom transfers 1 electron to one Li atom

c. one O atom transfers 2 electrons to one Li atom

d . one Li atom transfers 2 electrons to one O atom

e. each of two Li atoms transfers 1 electron to one O atom

ab. each of two O atoms transfers 1 electron to one Li atom

ac. one O atom transfers 2 electrons, one to each of two Li atoms

ad . one Li atom transfers 2 electrons, one to each of two O atoms

24. Atoms of element A want to lose 1 electron. Atoms of element B want to gain 2 electrons. If these

two elements were to form an ionic compound, then there wou ld be _________ in each formula unit.

a. one atom of A and one atom of B b. one atom of A and two atoms of B

c. two atoms of A and one atom of B d . two atoms of A and two atoms of B

e. none of the above

25. The main d istinction between an ionic and a covalent bond is that ionic bonds involve

_____________ and covalent bonds involve ___________.

a. electron sharing (ionic), electron transfer (covalent)

b. electron transfer (ionic), electron sharing (covalent)

c. formation of a compound (ionic), destru ction of a compound (covalent)

d . formation of a compound (ionic), destruction of a compound (covalent)

e. none of these

ab. More than two of the above are true.

26. In a covalent bond between two atoms, the force which holds the bonded atoms togethe r is the

result of _____.

a. the protons in the nucleus of one atom attracting the protons of the other atom

b. the protons in the nucleus of one atom repelling the protons of the other atom

c. the electrons in the outer shell of one atom attracting the electrons of the other atom

d . the electrons in the outer shell of one atom repelling the electrons of the other atom

e. the protons in the nucleus of one atom attracting the electrons of the other atom

ab. the protons in the nucleus of one atom repelling the electrons of the other atom

ac. the cation and the anion attracting each other

27. Consider the d iagram below when answering the following question.

The two atoms are most stable when the d istance between them corresponds to point _____ on t he

graph.

a. A b. B c. C d . D

e. A and D f. none of these

28. Consider the d iagram below when answering the following question.

The fact that the energy at point B on the graph is low can be best attributed to the idea that

___________ between the two atoms are "intense" (strong) at this d istance.

a. electron-electron repu lsions b. electron-electron attractions

c. proton-proton repulsions d . proton-proton attractions

e. electron-proton repulsions ab. electron-proton attractions

Bond Polarity

Table of Electronegativities

H

2.1

Li

1.0

Be

1.5

B

2.0

C

2.5

N

3.0

O

3.5

F

4.0

Na

0.9

Mg

1.2

Al

1.5

Si

1.8

P

2.1

S

2.5

Cl

3.0

K

0.8

Ca

1.0

Sc

1.3

Ti

1.5

V

1.6

Cr

1.6

Mn

1.5

Fe

1.8

Co

1.9

Ni

1.9

Cu

1.9

Zn

1.6

Ga

1.6

Ge

1.8

As

2.0

Se

2.4

Br

2.8

Rb

0.8

Sr

1.0

Y

1.2

Zr

1.4

Nb

1.6

Mo

1.8

Tc

1.9

Ru2

.2

Rh

2.2

Pd

2.2

Ag

1.9

Cd

1.7

In

1.7

Sn

1.8

Sb

1.9

Te

2.1

I

2.5

Cs

0.7

Ba

0.9

La

1.0

Hf

1.3

Ta

1.5

W

1.7

Re

1.9

Os

2.2

Ir

2.2

Pt

2.2

Au

2.4

Hg

1.9

Tl

1.8

Pb

1.9

Bi

1.9

Po

2.0

At

2.2

Fr

0.7

Ra

0.9

Ac

1.1

Th

1.3

Pa

1.4

U

1.4

Np

1.4

29. A dipole moment vector is often used to ind icate the centers of positive and negative partial charge

within a polar covalent bond . Consider the d ipole moment vectors sh own below. Which d iagrams

correctly ind icate the d irection of the d ipole vector? Bubble in all that apply.

30. The greater the electronegativity of an element, the more likely that atoms of that element will _____.

a. attract electrons in a bond tow ards itself. b. be an electrical conductor

c. give its electrons away to form a bond . d . form nonpolar covalent bonds

31. Use the table of electronegativities to identify the most polar bond:

a. B-O b. H-B c. H-C d . S-P

32. Use the table of electronegativities to identify the least polar bond:

a. B-P b. P-Cl c. N-O d . F-O

33. The greater the d ifference in electronegativity between two bonded atoms, the _____.

a. more evenly d istributed which electrons will be in the bond

b. more likely the electrons will be equally shared

c. more polar that the bond is

34. An element with a high electronegativity _____.

a. bond s with many atoms b. bonds with very few atoms

c. has a high attraction for electrons d . has a low attraction for electrons

e. is very stable ab. is very unstable

Se Br S F Cl I H N

Diagram A Diagram B Diagram C Diagram D

35. A covalent bond can be polar covalent or nonpolar covalent. The d istinction has to do with _____.

a. the strength of the bond which results

b. the likelihood that the bond will break

c. the tendency of the bond to store energy

d . the degree to which bonded atoms share electrons equally

36. Use an electronegativity chart to classify the following bond as being ionic, polar covalent, or

nonpolar covalent. The bond formed between chlorine (Cl) and cesium (Cs) is _____.

a. ionic. b. polar covalent. c. nonpolar covalent.

Lewis Electron Dot Structure

37. How many electrons are available for bonding in phosphate ion, PO4

3-?

a. 30 b. 31 c. 32 d . 36 e. 50

38. Which of the following is not a correct Lewis structure?

a. NO2 b. NO

2

- c. NO d . N

2O

e. All of the above are correct structures.

39. How many possible resonance structures exist for su lfur trioxide?

a. 3 b. 4 c. 5 d . 6

40. Which of the following Lewis structures are resonance structures of thiocyanate ion?

a. (1) and (3) b. (2), (3), and (4) c. (1), (3), and (5)

d . (1), (3), and (4) e. (2), (4), and (5)

41. A sulfur (S) atom has ______ valence electron(s).

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

e. approximately 32 ab. none of these.

42. The Lewis structure shown at the right for the given compound is incorrectly

d rawn. Which of the following statements describes something that is

wrong with the structure? (NOTE: 'v.e.' stands for valence electrons).

Bubble in all that apply.

a. The d iagram shows too few v.e.

b. The d iagram shows too many v.e.

c. There are too many v.e. around one or mor of the O atoms.

d . A structure can be drawn with only 8 v.e. around the S atom.

e. The central atom would not be S.

ab. Nonsense! The d iagram is correctly d rawn.

N N OO N O O N O

(NO2) (NO2-)

-

(NO) (N2O)

N O

S C N

(1)

S C N

(2)

S C N

(3)

S C N

(4)

S C N

(5)

- - - - -


d rawn. Which of the following statements describes something that is wrong

with the structure? (NOTE: 'v.e.' stand s for valence electrons). Bubble in all

that apply.



c. There are too many v.e. around the left O atom.

d . There are too few v.e. around the right O atom.

e. There are too many v.e. around the C atom.



d rawn. Which of the following statements describes something that is

wrong with the structure? (NOTE: 'v.e.' stands for valence electrons).

Bubble in all that apply.



c. There are too few v.e. around one or more of the O atoms.

c. There are too many v.e. around one or more of the O atoms.

e. There are too many v.e. around the N atom.


VSEPR, Molecular Shape, Molecular Polarity and Hybridization

45. Which of the following species has a Lewis structure with a molecu lar geometry similar to SO3?

a. NH3

b. ICl3

c. CO3

2- d . SO

3

2- e. PCl

3

46. Use VSEPR theory to pred ict the molecular geometry of ICl3.

a. triangular planar b. octahedral c. triangular pyramid al

d . t-shaped e. triangular bipyramidal

47. Which of the following species have the same molecular geometry: XeF4, ClF

4

+, SF

4, PO

4

3-?

a. XeF4 and SF

4 b. ClF

4

+, and SF

4 c. ClF

4

+ and PO

4

3-

d . XeF4 and ClF

4

+ e. XeF

4, SF

4, and PO

4

3-

48. What is the hybrid ization of the central atom in XeF4?

a. sp b. sp2 c. sp

3 d . sp

3d e. sp

3d

2

49. What hybrid ization change does the carbon atom undergo in the combustion of methane?

CH4(g) + 2O

2(g) CO

2(g) + 2H

2O(g)

a. sp sp2 b. sp

2 sp

3 c. sp

3 sp d . sp

2 sp e. none

50. The shape of the CH 4 molecule is most similar to the shape of a molecule of _____.

a. H2O b. N2H4 c. SiH4 d . C2H4

51. Which one of the following is NOT a true statement about VSEPR theory?

a. Pairs of electrons within a molecule will orient themselves as far apart as possible.

b. The electron pair geometry of a molecule is dependent upon the number of electron clouds

surrounding the central atom.

c. Pairs of electrons will spatially orient themselves in such a way as to reduce the total amount of

repulsions.

d . Electron pair geometry is based on the location of electron clouds whereas molecular shape is

based on the location of atoms in the molecu le.

e. The electron pair geometry and the molecular shape of a molecule are always the same.

52. TRUE or FALSE:

If two molecules to have the same number of atoms and similar formula

(e.g., carbon d ioxide - CS2 - and su lfu r d ioxide - SO2 -molecules each have 3

atoms), then they will have the same molecu lar shapes.

a. TRUE b. FALSE

53. TRUE or FALSE?

Molecular shape describes the location and geometric arrangement of the

electron clouds surrounding the the central atom of a molecule.

a. TRUE b. FALSE

54. Given the Lewis electron dot structure shown at the right, one would expect

the electron pair geometry for this molecule to be _____.

a. bent b. linear c. trigonal pyramid al

d . tetrahedral e. trigonal planar ab. … nonsense! None of these.

55. Given the Lewis electron dot structure shown at the right, one would expect

the molecular geometry for this molecu le to be _____.

a. bent b. linear c. trigonal pyramid al

d . tetrahedral e. trigonal planar ab. … nonsense! None of these.

56. Consider a molecu le whose central atom contains four single bonds and no unshared electron pairs.

Accord ing to hybrid ized bonding theory, the central atom would assume a _____ hybrid ization.

a. sp b. sp2 c. sp

3 d . sp

3d e. sp

3d

2

57. Consider a molecu le whose central atom contains two single bonds and two unshared electron pairs.

Accord ing to hybrid ized bonding theory, the central atom would assume a _____ hybrid ization.

a. sp b. sp2 c. sp

3 d . sp

3d e. sp

3d

2

58. Consider a molecu le whose central atom contains two single bonds, one d ouble bond and no

unshared electron pairs. Accord ing to hybrid ized bond ing theory, the central atom would assume a

_____ hybrid ization.

a. sp b. sp2 c. sp

3 d . sp

3d e. sp

3d

2

59. AXE notation is often used to describe the arrangement of electrons about the central atom in a

molecule. Accord ing to the notation - frequently abbreviated as AXiE

j - i represents the number of

atoms bonded to the central atom and j represents the number of unshared electron p airs on the

central atom. A molecule whose central atom is AX3 will have a molecu lar geometry that is _____.

a. trigonal planar b. T-shaped c. bent d . trigonal bipyramid al

e. linear ab. tetrahedral ac. seesaw ad . trigonal pyramidal

ae. square planar bc. octahedral bd . square pyramid al

60. AXE notation is often used to describe the arrangement of electrons about the central atom in a

molecule. Accord ing to the notation - frequently abbreviated as AXiE

j - i represents the number of

atoms bonded to the central atom and j represents the number of unshared electron pairs on the

central atom. A molecule whose central atom is AX4E

1 will have a molecular geometry that is _____.

a. trigonal planar b. T-shaped c. bent d . trigonal bipyramid al

e. linear ab. tetrahedral ac. seesaw ad . trigonal pyramidal

ae. square planar bc. octahedral bd . square pyramid al

For Questions #61 - #68: Complete the table for the following compounds. Your Lewis structure must be

clear. If necessary, redraw the d iagram at the bottom of the page or on the back.

61. CO2 62. ClO

3

-

# valence e- = ____________ # valence e- = ____________



Molecular Geometry: (Clearly circle)

linear tetrahedral trigonal planar

see saw T-shaped bent octahedral

trigonal pyramid al square pyramid al

trigonal bipyramidal square planar






This molecule is … (Clearly circle)

Polar Non-Polar


Polar Non-Polar

The hybridization of the central atom is … (Clearly circle)

sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2


sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2

63. CS2 64. SOCl

2 (S is central atom)















Polar Non-Polar


Polar Non-Polar


sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2


sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2

65. XeF4 66. XeO

4















Polar Non-Polar


Polar Non-Polar


sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2


sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2

67. AsF5 68. XeF

6















Polar Non-Polar


Polar Non-Polar


sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2


sp s2p sp

2 sp

3

sp4

s2p

2 sp

3d

sp

3d

2

Intermolecular Forces and Polarity

69. Which of the following statements concerning hydrogen bond ing is NOT correct?

a. Water is less dense in the solid phase than the liquid phase due to hydrogen bonding.

b. Hydrogen bond ing occurs in molecu les with N -H, O-H, and F-H bonds.

c. Hydrogen bond ing in water results in lower than expected melting points.

d . The unusually high boiling points of water, ammonia, and hydrogen fluoride are the result of

hydrogen bonding.

e. Hydrogen bonding is an unusually strong d ipole force.

70. What intermolecular forces are present in solid CO2?

a. d ispersion forces b. d ipole forces c. hydrogen bonding

d . answers a and b e. answers a, b, and c

71. Arrange NH3, CH

4, and PH

3 in order from lowest to highest boiling points.

a. CH4 < PH

3 < NH

3 b. CH

4 < NH

3 < PH

3

c. PH3 < NH

3 < CH

4 d . NH

3 < CH

4 < PH

3

e. PH3 < CH

4 < NH

3

72. Which of the following substances will exhibit d ipole forces?

a. SO3

b. H2S c. CH

4 d . SF

6 e. N

2

73. Which one of the following properties would not be affected by the strength of the intermolecular

forces between particles.

a. boiling point b. vapor pressure c. mass

d . melting point e. viscosity

74. What types of intermolecular forces would exist between molecules of methanol (CH3OH)?

a. Lond on d ispersion forces b. Hydrogen-bond ing forces

c. Dipole-d ipole forces

75. Which of the following substances are capable of undergoing hydrogen bonding? Bubble in all that

apply.

a. H2 b. HF c. NaF d . H

2O e. CH

4

76. Which of the following descriptors appropriately characterize Lond on d ispersion forces? Bubble in

all that apply.

a. They are temporary, short-lived forces.

b. They result when a temporary d ipole induces a d ipole in a neighboring particle.

c. They are considerably weaker than hydrogen bonding but stronger than d ipole -d ipole forces.

d . They are permanent forces which persist as long as the sample is not d isturbed .

e. They are forces acting between oppositely charged ions.

77. Pred ict which compound below would have the strongest intermolecular forces.

a. CH3—CH

2—PH

2 b. CH

3—CH

2—H c. CH

3—CH

2—S—H

d . CH3—CH

2—Se—H e. CH

3—CH

2—O—H

Unit 9 Review - gbschemphysgbschemphys.com/honchem/reviews/U9Review.pdfUnit 9 Review Ionic and...

Documents

Transcript of Unit 9 Review - gbschemphysgbschemphys.com/honchem/reviews/U9Review.pdfUnit 9 Review Ionic and...