AP Chem Chapter 8 test bank

34) For resonance forms of a molecule or ion, __________. A) one always corresponds to the observed structure B) all the resonance structures are observed in various proportions C) the observed structure is an average of the resonance forms D) the same atoms need not be bonded to each other in all resonance forms E) there cannot be more than two resonance structures for a given species

C) the observed structure is an average of the resonance forms

10) The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively. A) 7, 4, and 6 B) 1, 5, and 7 C) 8, 2, and 3 D) 7, 1, and 2 E) 2, 7, and 4

D) 7, 1, and 2

10) The electron configuration [Kr]4d10 represents __________. A) Sr+2 B) Sn+2 C) Te+2 D) Ag+1 E) Rb+1

D) Ag+1

13) Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br A) Br B) Sr C) Na D) O, Se E) Sr, O, Se

D) O, Se

20) The formula of palladium(IV) sulfide is __________. A) Pd2S4 B) PdS4 C) Pd4S D) PdS2 E) Pd2S2

D) PdS2

41) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) PO4^3- B) SiF4 C) CF4 D) SeF4 E) NF3

D) SeF4

52) As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________. A) increases, increases B) decreases, decreases C) increases, decreases D) decreases, increases E) is unpredictable

D) decreases, increases

55) Dynamite consists of nitroglycerine mixed with __________. A) potassium nitrate B) damp KOH C) TNT D) diatomaceous earth or cellulose E) solid carbon

D) diatomaceous earth or cellulose

7) In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii __________. A) increases, decrease, increase B) increases, increase, increase C) decreases, increase, increase D) increases, increase, decrease E) increases, decrease, decrease

D) increases, increase, decrease

6) Lattice energy is __________. A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase B) the energy given off when gaseous ions combine to form one mole of an ionic solid C) the energy required to produce one mole of an ionic compound from its constituent elements in their standard states D) the sum of ionization energies of the components in an ionic solid E) the sum of electron affinities of the components in an ionic solid

A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase

41) The formal charge on sulfur in SO4^2- is __________, where the Lewis structure of the ion is: A) -2 B) 0 C) +2 D) +4 E) -4

B) 0

42) In the Lewis structure of ClF, the formal charge on Cl is __________ and the formal charge on F is __________. A) -1, -1 B) 0, 0 C) 0, -1 D) +1, -1 E) -1, +1

B) 0, 0

23) The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e) of the negative charge on I in HI? A) 1.6 x 10^-19 B) 0.057 C) 9.1 D) 1 E) 0.22

B) 0.057

36) The Lewis structure of shows __________ nonbonding electron pair(s) on As. A) 0 B) 1 C) 2 D) 3 E) This cannot be determined from the data given.

B) 1

37) The Lewis structure of shows that the central phosphorus atom has __________ nonbonding and __________ bonding electron pairs. A) 2, 2 B) 1, 3 C) 3, 1 D) 1, 2 E) 3, 3

B) 1, 3

26) A double bond consists of __________ pairs of electrons shared between two atoms. A) 1 B) 2 C) 3 D) 4 E) 6

B) 2

45) How many equivalent resonance forms can be drawn for without expanding octet on the sulfur atom (sulfur is the central atom)? A) 0 B) 2 C) 3 D) 4 E) 1

B) 2

23) How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell? A) 3 B) 4 C) 1 D) 2 E) 0

B) 4

28) In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons. A) 2, 2 B) 4, 2 C) 2, 4 D) 0, 6 E) 5, 1

B) 4, 2

1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be2+ C) B2+ D) C2- E) N2-

B) Be2+

46) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) NF3 B) BeH2 C) SO2 D) CF4 E) SO3 ^2-

B) BeH2

16) Of the atoms below, __________ is the most electronegative. A) Si B) Cl C) Rb D) Ca E) S

B) Cl

17) Which one of the following species has the electron configuration [Ar] 3d^4? A) Mn2+ B) Cr2+ C) V^3+ D) Fe3+ E) K+

B) Cr2+

29) In the molecule below, which atom has the largest partial negative charge __________? A) Cl B) F C) Br D) I E) C

B) F

14) In which of the molecules below is the carbon-carbon distance the shortest? A) H2C=CH2 B) H--C=C--H C) H3C--CH3 D) H2C=C=CH2 E) H3C=CH2=CH3

B) H--C=C--H

38) The Lewis structure of HCN (H bonded to C) shows that __________ has __________ nonbonding electron pairs. A) C, 1 B) N, 1 C) H, 1 D) N, 2 E) C, 2

B) N, 1

21) Which of the following has the bonds correctly arranged in order of increasing polarity? A) Be--F, Mg--F, N --F, O--F B) O --F, N--F, Be--F, Mg--F C) O--F, Be--F, Mg--F, N--F D) N--F, Be--F, Mg--F, O--F E) M--gF, Be--F, N--F, O--F

B) O --F, N--F, Be--F, Mg--F

20) Of the bonds below, __________ is the least polar. A) Na, S B) P, S C) C, F D) Si, Cl E) Na, Cl

B) P, S

4) Based on the octet rule, phosphorus most likely forms a __________ ion. A) P3+ B) P3- C) P5+ D) P5- E) P+

B) P3-

12) Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br A) O, Se B) Sr C) Na D) Br E) Sr, O, Se

B) Sr

18) What is the electron configuration for the ion? A) [Ar] 4s^1 3d^6 B) [Ar] 4s^0 3d^7 C) [Ar] 4s^0 3d^5 D) [Ar] 4s^2 3d^9 E) [Ne] 3s^2 3p^10

B) [Ar] 4s^0 3d^7

36) In which of the ions do all X-O bonds (X indicates the central atom) have the same length? A) none B) all C) (i) and (ii) D) (iii) and (v) E) (iii), (iv), and (v)

B) all

21) Elements from opposite sides of the periodic table tend to form __________. A) covalent compounds B) ionic compounds C) compounds that are gaseous at room temperature D) homonuclear diatomic compounds E) covalent compounds that are gaseous at room temperature

B) ionic compounds

47) How many different types of resonance structures can be drawn for SO3^2- the ion where all atoms satisfy the octet rule? A) 1 B) 2 C) 3 D) 4 E) 5

A) 1

50) Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform is __________ kJ/mol. A) 1241 B) 689 C) -689 D) 1378 E) -1378

A) 1241

44) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) ClF3 B) PCl3 C) SO3 D) CCl4 E) CO2

A) ClF3

3) Based on the octet rule, magnesium most likely forms a __________ ion. A) Mg2+ B) Mg2- C) Mg6- D) Mg6+ E) Mg-

A) Mg2+

22) Which two bonds are most similar in polarity? A) O--F and C--F B) B--F and Cl--F C) Al--Cl and I--Br D) I--Br and Si-Cr E) Cl--Cl and Be--Cl

A) O--F and C--F

17) Of the atoms below, __________ is the least electronegative. A) Rb B) F C) Si D) Cl E) Ca

A) Rb

47) Why don't we draw double bonds between the Be atom and the Cl atoms in ? A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. B) There aren't enough electrons. C) That would result in more than eight electrons around beryllium. D) That would result in more than eight electrons around each chlorine atom. E) That would result in the formal charges not adding up to zero.

A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom.

19) What is the electron configuration for the Fe2+ ion? A) [Ar]4s^0 3d^6 B) [Ar] 4s^2 3d^4 C) [Ar] 3s^0 3d^8 D) [Ar] 4s^2 3d^8 E) [Ar] 4s^6 3d^2

A) [Ar]4s^0 3d^6

49) Bond enthalpy is __________. A) always positive B) always negative C) sometimes positive, sometimes negative D) always zero E) unpredictable

A) always positive

14) For a given arrangement of ions, the lattice energy increases as ionic radius __________ and as ionic charge __________. A) decreases, increases B) increases, decreases C) increases, increases D) decreases, decreases E) This cannot be predicted.

A) decreases, increases

24) A __________ covalent bond between the same two atoms is the longest. A) single B) double C) triple D) They are all the same length. E) strong

A) single

40) The formal charge on nitrogen in NO3- is __________. A) -1 B) 0 C) +1 D) +2 E) -2

C) +1

32) The oxidation number of phosphorus in PF3 is __________. A) -2 B) +1 C) +3 D) +2 E) -3

C) +3

6) There are __________ unpaired electrons in the Lewis symbol for an oxygen atom. A) 0 B) 1 C) 2 D) 4 E) 3

C) 2

1) There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom. A) 4, 2 B) 2, 4 C) 2, 3 D) 4, 3 E) 0, 3

C) 2, 3

44) How many equivalent resonance forms can be drawn for - (carbon is the central atom)? A) 1 B) 2 C) 3 D) 4 E) 0

C) 3

34) The ion ICL4- has __________ valence electrons. A) 34 B) 35 C) 36 D) 28 E) 8

C) 36

39) Based on the octet rule, boron will most likely form a __________ ion. A) B3- B) B1+ C) B3+ D) B2+ E) B2-

C) B3+

43) The central atom in __________ violates the octet rule. A) NH3 B) SeF2 C) BF3 D) AsF3 E) CF4

C) BF3

42) The central atom in __________ does not violate the octet rule. A) SF6 B) KrF2 C) CF4 D) XeF4 E) ICl4

C) CF4

11) The only noble gas without eight valence electrons is __________. A) Ar B) Ne C) He D) Kr E) All noble gases have eight valence electrons.

C) He

37) Of the following, __________ cannot accommodate more than an octet of electrons. A) P B) As C) O D) S E) I

C) O

31) Given the electronegativities below, which covalent single bond is most polar? Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5 A) C-H B) N-H C) O-H D) O-C E) O-N

C) O-H

11) Fe+2 ions are represented by __________. A) [Ar]3d1 B) [Ar]3d4 C) [Ar]3d6 D) [Ar]3d104s1 E) [Ar]3d3

C) [Ar]3d6

26) The Lewis structure of N2H2 shows __________. A) a nitrogen-nitrogen triple bond B) a nitrogen-nitrogen single bond C) each nitrogen has one nonbonding electron pair D) each nitrogen has two nonbonding electron pairs E) each hydrogen has one nonbonding electron pair

C) each nitrogen has one nonbonding electron pair

30) The ability of an atom in a molecule to attract electrons is best quantified by the __________. A) paramagnetism B) diamagnetism C) electronegativity D) electron change-to-mass ratio E) first ionization potential

C) electronegativity

32) Electronegativity __________ from left to right within a period and __________ from top to bottom within a group. A) decreases, increases B) increases, increases C) increases, decreases D) stays the same, increases E) increases, stays the same

C) increases, decreases

13) The type of compound that is most likely to contain a covalent bond is __________. A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table B) a solid metal C) one that is composed of only nonmetals D) held together by the electrostatic forces between oppositely charged ions E) There is no general rule to predict covalency in bonds.

C) one that is composed of only nonmetals

27) What is the maximum number of double bonds that a hydrogen atom can form? A) 0 B) 1 C) 2 D) 3 E) 4

A) 0

16) The principal quantum number of the electrons that are lost when tungsten forms a cation is __________. A) 6 B) 5 C) 4 D) 3 E) 2

A) 6

38) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) NF3 B) IF3 C) PF3 D) SbF3 E) So4^2-

B) IF3

25) Which of the following names is/are correct for the compound ? A) tin (II) chloride and tin (IV) chloride B) tin tetrachloride and tin (IV) chloride C) tin (IV) tetrachloride D) tin chloride E) tin chloride and tin (II) tetrachloride

B) tin tetrachloride and tin (IV) chloride

45) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) NI3 B) SO2 C) ICL5 D) SiF4 E) CO2

C) ICL5

28) What is the maximum number of double bonds that a carbon atom can form? A) 4 B) 1 C) 0 D) 2 E) 3

D) 2

27) There are __________ valence electrons in the Lewis structure of CH3CH2Cl. A) 14 B) 12 C) 18 D) 20 E) 10

D) 20

9) Which energy change corresponds to the first ionization energy of potassium? A) 2 B) 5 C) 4 D) 3 E) 6

D) 3

25) How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? A) 1 B) 2 C) 3 D) 4 E) 5

D) 4

2) In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons. A) 4, 2 B) 4,1 C) 2, 5 D) 6, 1 E) 0, 5

D) 6, 1

19) Of the molecules below, the bond in __________ is the most polar. A) HBr B) HI C) HCl D) HF E) H2

D) HF

22) Determining lattice energy from Born-Haber cycle data requires the use of __________. A) the octet rule B) Coulomb's law C) Periodic law D) Hess's law E) Avogadro's number

D) Hess's law

18) Which of the elements below has the largest electronegativity? A) Si B) Mg C) P D) S E) Na

D) S

15) The electron configuration of the S2- ion is __________. A) [Ar]3S23P6 B) [Ar]3S^2 3P^2 C) [Ne]3S^2 3P^2 D) [Ne] 3s^2 3p^6 E) [Kr] 3s^2 2p^-6

D) [Ne] 3s^2 3p^6

53) Of the possible bonds between carbon atoms (single, double, and triple), __________. A) a triple bond is longer than a single bond B) a double bond is stronger than a triple bond C) a single bond is stronger than a triple bond D) a double bond is longer than a triple bond E) a single bond is stronger than a double bond

D) a double bond is longer than a triple bond

51) Of the bonds , and , the bond is __________. A) strongest/shortest B) strongest/longest C) weakest/shortest D) weakest/longest E) intermediate in both strength and length

D) weakest/longest

53) Using the table of bond dissociation energies, the for the following reaction is __________ kJ. A) -359 B) -223 C) 359 D) 223 E) 208

A) -359

39) The formal charge on carbon in the molecule below is __________. A) 0 B) +1 C) +2 D) +3 E) -1

A) 0

7) How many unpaired electrons are there in the Lewis structures of N3- a ion? A) 0 B) 1 C) 2 D) 3 E) This cannot be predicted.

A) 0

8) How many unpaired electrons are there in an O2- ion? A) 0 B) 1 C) 2 D) 3 E) This cannot be predicted.

A) 0

4) Which of the following does not have eight valence electrons? A) Ca B) Rb+ C) Xe D) Br- E) All of the above have eight valence electrons.

A) Ca

24) Which of the following names is/are correct for the compound ? A) titanium dioxide and titanium (IV) oxide B) titanium (IV) dioxide C) titanium oxide D) titanium oxide and titanium (IV) dioxide E) titanium (II) oxide

A) titanium dioxide and titanium (IV) oxide

43) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is __________. A) 0 B) +1 C) -1 D) +2 E) -2

B) +1

17) Which one of the following species has the electron configuration [Ar]3d^4 ? A) Mn 2+ B) Cr^2+ C) V^3+ D) Fe^3+ E) K+

B) Cr^2+

33) To convert from one resonance structure to another, __________. A) only atoms can be moved B) electrons and atoms can both be moved C) only electrons can be moved D) neither electrons nor atoms can be moved E) electrons must be added

C) only electrons can be moved

(i) (ii) (iii) (iv) (v) 35) There can be four equivalent best resonance structures of __________. A) (ii) B) (iii) C) (i) D) (iv) E) (v)

D) (iv)

15) Of the atoms below, __________ is the most electronegative. A) Br B) O C) Cl D) N E) F

E) F

35) The ion NO- has __________ valence electrons. A) 15 B) 14 C) 16 D) 10 E) 12

E) 12

46) How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom? A) 5 B) 2 C) 1 D) 4 E) 3

E) 3

48) Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet? A) N B) C C) H D) O E) B

E) B

2) Of the ions below, only __________ has a noble gas electron configuration. A) S3+ B) O2+ C) I+ D) K+ E) Cl-

E) Cl-

5) Based on the octet rule, iodine most likely forms an __________ ion. A) I 2+ B) I 4+ C) I 4- D) I + E) I --

E) I --

40) Which of the following does not have eight valence electrons? A) Cl- B) Xe C) Ti+4 D) Rb+1 E) Sr+1

E) Sr+1

9) The electron configuration of the phosphide ion ( P^3-) is __________. A) [Ne]3s^2 B) [Ne]3s^23p^1 C) [Ne]3s^2 3p^3 D) [Ne]3p^2 E) [Ne]3s^2 3p^6

E) [Ne]3s^2 3p^6

3) Which of the following has eight valence electrons? A) Ti4+ B) Kr C) Cl- D) Na+ E) all of the above

E) all of the above

56) Dynamite __________. A) was invented by Alfred Nobel B) is made of nitroglycerine and an absorbent such as diatomaceous earth C) is a much safer explosive than pure nitroglycerine D) is an explosive E) all of the above

E) all of the above

54) Most explosives are compounds that decompose rapidly to produce __________ products and a great deal of __________. A) gaseous, gases B) liquid, heat C) soluble, heat D) solid, gas E) gaseous, heat

E) gaseous, heat

33) A nonpolar bond will form between two __________ atoms of __________ electronegativity. A) different, opposite B) identical, different C) different, different D) similar, different E) identical, equal

E) identical, equal

31) Resonance structures differ by __________. A) number and placement of electrons B) number of electrons only C) placement of atoms only D) number of atoms only E) placement of electrons only

E) placement of electrons only