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Central Science: Chapter 23

front 1

Chalcocite, chalcopyrite, and malachite are sources of which metal?
A) manganese
B) copper
C) titanium
D) iron
E) zinc

back 1

B

front 2

Which mineral contains titanium?
A) pyrolusite
B) chalcopyrite
C) galena
D) rutile
E) sphalerite

back 2

D

front 3

A mineral is ________.
A) a solid inorganic compound that contains one or more metals
B) a vitamin
C) metal in its elemental form
D) a transition metal ion
E) a source of carbon

back 3

A

front 4

What two oxidation states are more frequently observed in the first transition series than in the third?
A) +3 and +7
B) +2 and +3
C) +2 and +7
D) +5 and +6
E) +3 and +5

back 4

B

front 5

A substance with unpaired electrons will be ________.
A) slightly attracted to a magnet
B) slightly repelled by a magnet
C) permanently magnetic
D) brightly colored
E) nonmetallic

back 5

A

front 6

The lanthanide contraction is responsible for the fact that ________.
A) Zr and Y have about the same radius
B) Zr and Nb have similar oxidation states
C) Zr and Hf have about the same radius
D) Zr and Zn have similar oxidation states
E) Zr and Hf have the same oxidation states

back 6

C

front 7

Which one of the following is not true about transition metals?
A) They frequently have more than one common oxidation state.
B) Their compounds are frequently colored.
C) Their compounds frequently exhibit magnetic properties.
D) They are found in the d-block of the periodic table.
E) They typically have low melting points.

back 7

E

front 8

Which one of the following species is paramagnetic?
A) Fe3+
B) Cu+
C) Zn
D) Mg
E) Au+

back 8

A

front 9

Paramagnetic solids ________.
A) have atoms with one or more unpaired electrons
B) show very slight magnetic character when placed in a magnetic field
C) have atoms with randomly oriented magnetic moments
D) have atoms with strongly aligned electrons when placed in a magnetic field
E) both A and D

back 9

E

front 10

Formation of a complex species of Mn+ metal ion with ligands often ________.
A) "masks" original chemical properties of both the Mn+ ion and the ligands
B) reduces availability of the free Mn+ ions in solution
C) may cause changes in the ease with which Mn+ is reduced or oxidized
D) alters original physical properties of Mn+
E) all of the above

back 10

E

front 11

What is the most common geometry found in four-coordinate complexes?
A) square planar
B) octahedral
C) tetrahedral
D) icosahedral
E) trigonal bipyramidal

back 11

C

front 12

The minimum number of unshared valence electron pairs in the ligands of a coordination compound is ________.
A) 1
B) 2
C) 3
D) 4
E) 5

back 12

A

front 13

The coordination number of cobalt in CoCl3 ∙ 6NH3 is ________.
A) 2
B) 3
C) 4
D) 6
E) 8

back 13

D

front 14

What is the oxidation number of Fe in [Fe(CN)5]3-?
A) 1+
B) 2+
C) 3+
D) 4+
E) 5+

back 14

B

front 15

Changes in the coordination sphere of a complex compound may lead to changes in ________.
A) color
B) physical properties
C) chemical properties
D) stability
E) all of the above

back 15

E

front 16

In the compound, CaNa[Fe(CN)6], what ligands are in the coordination sphere?
A) Ca2+
B) Na+
C) CN-
D) H2O
E) none of the above

back 16

C

front 17

What are the respective central-metal oxidation state, coordination number, and overall charge on the complex ion in

Na2[Cr(NH3)2 (NCS)4]?

A) +3; 6; -1
B) +3; 6; +1
C) +2; 6; -2
D) +2; 4; -1
E) +1; 6; -2

back 17

C

front 18

Which of the following complexes has a coordination number of 6?
A) [Co(NH3)2Cl2]
B) [Co(NH3)4]2+
C) [Co(en)3]3+
D) [Co(NH3)2]3+
E) None of these complexes has coordination number 6.

back 18

C

front 19

How many ligands are there in the coordination sphere of [Co(en)2Cl2]+?
A) 3
B) 6
C) 4
D) 1
E) 0

back 19

C

front 20

What is the charge on the complex ion in Ca2[Fe(CN)6]?
A) 3-
B) 2+
C) 2-
D) 1-
E) 4-

back 20

E

front 21

A ligand with a single donor atom is called ________.
A) a chelon
B) a chelate
C) polydentate
D) monodentate
E) bidentate

back 21

D

front 22

Which of the following is not a chelating agent?
A) chloride anion
B) EDTA
C) porphine
D) ethylenediamine
E) oxalate anion

back 22

A

front 23

What is the purpose of adding EDTA to prepared foods?
A) to keep ions such as Ca2+ in solution so the foods look good
B) to complex trace metal ions that catalyze decomposition reactions
C) to complex iron (III) ions so they can catalyze protein decomposition on cooking
D) to aid in browning of the surface during cooking
E) to prevent dissolution of the container in the food when stored for long periods of time

back 23

B

front 24

In humans, what percent of absorbed iron is found in blood?
A) 15
B) 25
C) 40
D) 60
E) 75

back 24

E

front 25

The coordination number and oxidation number of the central atom in [Fe(H2O)4Cl2] are ________ and ________, respectively.
A) 4, +1
B) 6, +1
C) 6, +2
D) 5, +2
E) 4, +2

back 25

C

front 26

What are the donor atoms in a porphine molecule?
A) N
B) O
C) S
D) Br
E) F

back 26

A

front 27

What metal is complexed in chlorophyll?
A) iron
B) chromium
C) manganese
D) vanadium
E) magnesium

back 27

E

front 28

What form of hemoglobin is purplish-red?
A) myoglobin
B) deoxyhemoglobin
C) heme
D) oxyhemoglobin
E) none of the above

back 28

B

front 29

How many bonds can ethylenediamine form to a metal ion?
A) 1
B) 2
C) 3
D) 4
E) 6

back 29

B

front 30

Based on entropy considerations alone, which homogeneous aqueous equilibrium would be expected to lie to the right?
A) AgI2- + 2Br- ⇔ AgBr2- + 2I-
B) Ni(H2NC2H4NH2)32+ + 6NH3 ⇔ Ni(NH3)62+ + 3H2NC2H4NH2
C) CoCl42+ + 6H2O ⇔ Co(H2O)62+ + 4Cl-
D) Fe(NH3)62+ + C20H10N42- ⇔ Fe(NH3)2(C20H10N4) + 4NH3
E) Cu(NH3)42+ + 6H2O ⇔ Cu(H2O)62+ + 4NH3

back 30

D

front 31

The chelate effect is best attributed to considerations of which type?
A) hydration
B) enthalpy
C) entropy
D) hydrogen bonding
E) resonance

back 31

C

front 32

Which one of the following species is a potential polydentate ligand (chelating agent)?
A) NH3
B) Cl-
C) CN-
D) H2O
E) C2O42-

back 32

E

front 33

What are the donor atoms in ferrichrome and how many of them are in one molecule?
A) Cr, 5
B) N, 4
C) O, 6
D) Fe, 4
E) S, 6

back 33

C

front 34

Which of the following is a polydentate ligand?
A) ammonia
B) oxalate ion
C) chloride ion
D) water
E) hydroxide ion

back 34

B

front 35

A complex of correctly written formula [Pt(NH3)3Br]Br ∙ H2O has which set of ligands in its inner coordination sphere?
A) 3 NH3
B) 3 NH3 and 2 Br-
C) 3 NH3 and 1 Br-
D) 3 NH3, 1 Br-, and 1 H2O
E) 3 NH3, 2 Br-, and 1 H2O

back 35

C

front 36

Which one of the following is the correct formula for potassium diaquatetrachloromolybdate (III)?
A) K2[Mo(H2O)2Cl4]
B) K[Mo(H2O)2Cl2]Cl2
C) K[Mo(H2O)2Cl4]
D) Mo[K(H2O)2]Cl4
E) K3[Mo(H2O)2Cl4]

back 36

C

front 37

Does either or both cis- or trans-[Mn(en)2Br2] have optical isomers?
A) cis only
B) trans only
C) both cis and trans
D) neither cis nor trans
E) [Mn(en)2Br2] does not exhibit cis-trans isomerism.

back 37

A

front 38

Linkage isomerism would most likely occur when which of the following ligands is present?
A) H2O
B) NH3
C) Cl-
D) PF3
E) NCS-

back 38

E

front 39

Isomers whose ligands can bind directly to a metal or be outside the lattice are called ________.
A) linkage isomers
B) rotational isomers
C) coordination sphere isomers
D) geometric isomers
E) optical isomers

back 39

C

front 40

Which of the following will display optical isomerism?
A) square-planar [Rh(CO)2Cl2]-
B) square-planar [Pt(H2NC2H4NH2)2]2+
C) octahedral [Co(NH3)6]3+
D) octahedral [Co(NH3)5Cl]2+
E) octahedral [Co(H2NC2H4NH2)3]3+

back 40

E

front 41

Which one of the following complexes would most likely have tetrahedral geometry?
A) [NiCl4]2-
B) [Co(H2O)6]2+
C) [Cr(NH3)6]3+
D) [Fe(CN)6]3+
E) [Pt(NH3)2Cl2]

back 41

A

front 42

Which one of the following complexes can exhibit geometrical isomerism?
A) [Pt(NH3)2Cl2] (square planar)
B) [Zn(NH3)2Cl2] (tetrahedral)
C) [Cu(NH3)4]2+ (square planar)
D) [Cu(NH3)5Cl]2+ (octahedral)
E) All of the above can exhibit geometrical isomerism.

back 42

A

front 43

Coordination sphere isomers ________.
A) have the same molecular formula and coordination number
B) have the same molecular formula but different coordination numbers
C) have different molecular formulas but the same coordination number
D) have different molecular formulas and different coordination numbers
E) are the same as resonance structures

back 43

A

front 44

A racemic mixture is ________.
A) an equal mixture of both enantiomers of an optically active species
B) a mixture of an optically active species with an optically inactive species
C) an equal mixture of cis- and trans-isomers
D) a mixture of metal ions and ligands in equilibrium
E) a mixture of structural isomers

back 44

A

front 45

Which compound is most likely white/colorless?
A) [Cu(H2O)4]2+
B) [Ni(H2O)6]2+
C) [Cr(H2O)5Cl]2+
D) [Cd(H2O)4]2+
E) [Co(H2O)6]2+

back 45

D

front 46

A complex that absorbs light at 700 nm will appear ________.
A) red
B) green
C) yellow
D) orange
E) violet

back 46

B

front 47

A metal complex absorbs light mainly at 420 nm. What is the color of the complex?
A) green
B) yellow
C) red
D) orange
E) purple

back 47

B

front 48

Which one of the following substances has three unpaired d electrons?
A) [Zn(NH3)4]2+
B) [V(H2O)6]4+
C) [Ag(NH3)2]+
D) [Cu(NH3)4]2+
E) [Cr(CN)6]3-

back 48

E

front 49

Which one of the following complex ions will be paramagnetic?
A) [Fe(H2O)6]2+ (low spin)
B) [Fe(H2O)6]3+ (low spin)
C) [Co(H2O)6]3+ (low spin)
D) [Zn(H2O)4]2+
E) [Zn(NH3)4]2+

back 49

B

front 50

Complexes containing metals with d10 electron configurations are typically white/colorless because ________.
A) there is no d electron that can be promoted via the absorption of visible light
B) the empty d orbitals absorb all of the visible wavelengths
C) there are no d electrons to form bonds to ligands
D) a complex must be charged to be colored
E) d electrons must be emitted by the complex in order for it to appear colored

back 50

A

front 51

Complexes containing metals with d10 electron configurations are typically ________.
A) violet
B) blue
C) green
D) yellow
E) white/colorless

back 51

E

front 52

Complexes containing metals with which one of the following electron configurations are usually white/colorless?
A) d2
B) d1
C) d5
D) d8
E) d10

back 52

E

front 53

Consider a complex in which manganese (III) is bonded to six identical ligands. Which one of the following ligands will result in the smallest value of Δ?
A) Cl-
B) NH3
C) H2O
D) F-
E) CN-

back 53

A

front 54

Based on the crystal-field strengths F- < CH2CN < NH3 < NO2- < CN-, which Co (III) complex is most likely high-spin?
A) [Co(NH3)6]3+
B) [Co(NO2)6]3-
C) [Co(CN)6]3-
D) [CoF6]3-
E) [Co(CH3CN)6]3+

back 54

D

front 55

The attraction of a metal to a neutral ligand is due to ________ bonding.
A) ionic
B) covalent
C) ion-dipole
D) dipole-dipole
E) hydrophobic

back 55

C

front 56

Which of the following statements is (are) false?
A) The greater the energy gap in a metal complex, the shorter the wavelength of light the complex will absorb.
B) Complex color depends on both the metal and the ligand.
C) Metal complexes with an ammonia ligand have a larger energy gap than the corresponding fluoride complexes.
D) Strong field ligands are associated with low energy gaps.
E) Both A and C

back 56

D

front 57

Based on the crystal-field strengths Cl- < F- < H2O < NH3 < H2NC2H4NH2, which octahedral Ti (III) complex below has its d-d electronic transition at shortest wavelength?
A) [Ti(NH3)6]3+
B) [Ti(H2NC2H4NH2)3]3+
C) [Ti(H2O)6]3+
D) [TiCl6]3-
E) [TiF6]3-

back 57

B

front 58

Which of the following ions can form both a high spin and a low spin octahedral complexes?
A) Fe3+ and Co2+ only
B) Fe3+, Mn3+, and Co2+
C) Cr3+ only
D) Fe3+, Cr3+, and Co2+
E) Mn3+, Cr3+, and Co2+

back 58

B

front 59

Using the following abbreviated spectrochemical series, determine which complex ion is most likely to absorb light in the red region of the visible spectrum.

small splitting Cl- < H2O < NH3 < CN- large splitting

A) [CuCl4]2-
B) [Cu(H2O)4]2+
C) [Cu(NH3)4]2+
D) [Cu(CN)4]2-
E) not enough information given to determine

back 59

A

front 60

Which of the following cannot form both high- and low-spin octahedral complexes?
A) Mn2+
B) V2+
C) Co3+
D) Cr2+
E) All of the above can form both high- and low-spin complexes.

back 60

B

front 61

Which of the following can form both high- and low-spin octahedral complexes?
A) Cr2+
B) Cr3+
C) Zn2+
D) Cu+
E) All of the above can form either high- or low-spin complexes.

back 61

A

front 62

How many d electrons are associated with the metal ion in [Cr(NH3)3+?
A) 1
B) 2
C) 3
D) 4
E) 5

back 62

C

front 63

The coordination numbers of cobalt (III) and of chromium (III) in their complexes are always ________.
A) 4
B) 5
C) 2
D) 3
E) 6

back 63

E

front 64

The coordination number of platinum in complexes is always ________.
A) 4
B) 5
C) 2
D) 3
E) 6

back 64

A

front 65

During the formation of a coordination compound, the ________ acts as a Lewis acid.
A) metal
B) ligand

back 65

A

front 66

During the formation of a coordination compound, the ________ acts as a Lewis base.
A) metal
B) ligand

back 66

B

front 67

The coordination sphere of a complex consists of ________.
A) the central metal ion only
B) the ligands
C) the central metal ion and the ligands bonded to it
D) the primary and secondary valencies
E) coordination and steric numbers

back 67

C

front 68

In the following reaction, Ni2+ is acting as a(n) ________.

Ni2+ (g) + 6H2O (l) → Ni(H2O)62+ (aq)

A) oxidizing agent
B) Lewis acid
C) precipitating agent
D) solvent
E) ligand

back 68

B

front 69

How many d electrons are in the iron ion of K3[Fe(CN)6]?
A) 3
B) 5
C) 6
D) 7
E) 4

back 69

B

front 70

What is the charge on the complex ion in Mg2[FeCl6]?
A) 2-
B) 2+
C) 3-
D) 3+
E) 4-

back 70

E

front 71

What is the oxidation number of chromium in Cr[(NH3)4Cl2]Cl?
A) -3
B) +3
C) +2
D) -2
E) 0

back 71

B

front 72

What is the ligand in Ca3[Fe(CN)6]2?
A) Ca2+
B) Fe3+
C) CN-
D) Fe(CN)63-
E) Fe2+

back 72

C

front 73

What is the charge of the central metal ion in Ca3[Fe(CN)6]2?
A) 0
B) 1+
C) 2+
D) 3+
E) 6+

back 73

D

front 74

What is the oxidation number of cobalt in [Co(NH3)4F2]?
A) -3
B) +2
C) +1
D) +3
E) +6

back 74

B

front 75

The charge of the complex ion in [Zn(H2O)3Cl]Cl ________.
A) 0
B) 1-
C) 2+
D) 1+
E) 2-

back 75

D

front 76

The coordination number for [Zn(H2O)3Cl]Cl is ________.
A) 5
B) 4
C) 2
D) 1
E) 6

back 76

B

front 77

What is the oxidation state of iron in CaNa[Fe(CN)6]?
A) 0
B) +2
C) +3
D) +4
E) +6

back 77

C

front 78

What is the oxidation state of iron in K3[Fe(CN)6]?
A) 0
B) +2
C) +3
D) +4
E) +6

back 78

C

front 79

What is the coordination number of iron in CaNa[Fe(CN)6]?
A) 2
B) 8
C) 4
D) 6
E) 12

back 79

D

front 80

What is the coordination number of cobalt in [Co(NH3)5Cl](NO3)2?
A) 12
B) 8
C) 4
D) 2
E) 6

back 80

E

front 81

What is the oxidation state of cobalt in [Co(NH3)5Cl](NO3)2?
A) 0
B) 2
C) 3
D) 4
E) 6

back 81

C

front 82

What is the oxidation state of chromium in [Cr(H2O)4Cl2]+?
A) 0
B) +2
C) +3
D) -2
E) -3

back 82

C

front 83

What is the coordination number of chromium in [Cr(H2O)4Cl2]+?
A) 8
B) 6
C) 4
D) 2
E) 12

back 83

B

front 84

The "dentation" of a ligand is defined by ________.
A) how many "dents" or "deceptions" there are in the coordination sphere of a complex species it forms
B) how many electron donor atoms it utilizes to form coordinate bonds to the central metal ion
C) the total number of lone pairs of electrons it possesses
D) how many metal ions it can sequester from solution
E) none of the above

back 84

B

front 85

EDTA is ________-dantate ligand.
A) mono
B) bi
C) tri
D) tetra
E) hexa

back 85

E

front 86

What is the metal ion in the porphyrin of heme?
A) iron
B) calcium
C) molybdenum
D) magnesium
E) chlorophyll

back 86

E

front 87

How many iron atoms are coordinated in a hemoglobin molecule?
A) 1
B) 2
C) 3
D) 4
E) 5

back 87

D

front 88

The correct name for [Ni(NH3)6](NO3)3 ________.
A) dinitrohexaamminenickel (II)
B) hexaamminenickel (III) trinitrate
C) dinitrohexaamminenickelate (III)
D) hexaamminenickel (II) nitrate
E) hexaamminenickel (III) nitrate

back 88

E

front 89

The correct name for [Cu(NH3)4(H2O)2]2+ is ________.
A) diwaterquatraamminecopper (II)
B) tetraamminediaquacopper (II)
C) diaquatetraammoniumcopper (II)
D) tetraamminecopper (II) dihydrate
E) copper (II) tetraamminediaqueous

back 89

B

front 90

The correct name for [Al(H2O)2(OH-)4]- is ________.
A) diwaterquatrahydroxyaluminum
B) tetrahydroxydiaquaaluminum (III)
C) diaquatetrahydroxoaluminate
D) aluminum (IV) hydroxide dihydrate
E) aluminumdihydratetetrahydroxide

back 90

C

front 91

The correct name for [Fe(NH3)5]Cl3 is ________.
A) pentaamineiron (II) chloride
B) pentaamineiron (I) chloride
C) pentaamineiron (III) chloride
D) pentaamineiron (IV) chloride
E) pentaamineiron (0) chloride

back 91

C

front 92

The names of complex anions end in ________.
A) -o
B) -ium
C) -ate
D) -ous
E) -ic

back 92

C

front 93

The correct name for Na3[CoF6] is ________.
A) trisodium hexakisfluorocobalt (III)
B) trisodium hexakisfluorocobalt (II)
C) trisodium hexakisfluorocobalt (IV)
D) sodium hexafluorocobaltate (III)
E) sodium hexafluorocobaltate (IV)

back 93

D

front 94

Triphenylphosphine is often given the abbreviated formula PPh3. The correct name for Rh(PPh3)3Cl is ________.
A) chlorotriphenylphosphinerhodium
B) chlorotriphenylphosphinerhodium (I)
C) tris(triphenylphosphine)chlororhodium (I)
D) chlorotris(triphenylphosphine)rhodium (I)
E) chlorotris(triphenylphosphine)rhodate (I)

back 94

D

front 95

In ________, the bonds are the same but the spatial arrangement of the atoms is different.
A) structural isomers
B) linkage isomers
C) coordination-sphere isomers
D) stereoisomers
E) resonance structures

back 95

D

front 96

A geometrical isomer with like groups located on opposite sides of the metal atom is denoted with the prefix ________.
A) cis-
B) trans-
C) bis-
D) tetrakis-
E) d-

back 96

B

front 97

The complex [Zn(NH3)2Cl2]2+ does not exhibit cis-trans isomerism. The geometry of this complex must be ________.
A) tetrahedral
B) trigonal bipyramidal
C) octahedral
D) square planar
E) either tetrahedral or square planar

back 97

A

front 98

How many isomers exist for the octahedral complex ion [Co(NH3)4F2]+?
A) 1
B) 2
C) 3
D) 4
E) 5

back 98

B

front 99

Trans-[Fe(H2O)2Cl4]2- must be ________.
A) tetrahedral
B) octahedral
C) square planar
D) trigonal bipyramidal
E) linear

back 99

B

front 100

Linkage isomerism can only occur ________.
A) in cis-isomers of octahedral complexes
B) with cobalt complexes
C) with coordination number 6
D) with tetrahedral complexes
E) with ligands that have more than one possible donor atom

back 100

E

front 101

Metals with ________ electron configurations characteristically form diamagnetic, square planar complexes.
A) d0
B) d9
C) d6
D) d8
E) d10

back 101

D

front 102

Which mineral contains mercury?
A) cinnabar
B) sphalerite
C) rutile
D) chromite
E) cassiterite

back 102

A

front 103

Which one of the following species is paramagnetic?
A) Cu
B) Ne
C) Y3+
D) Ra
E) Zn2+

back 103

A

front 104

Which element has the largest bonding atomic radius?
A) scandium
B) titanium
C) vanadium
D) chromium
E) manganese

back 104

A

front 105

What is the most common geometry found in five-coordinate complexes?
A) trigonal bipyramidal
B) octahedral
C) tetrahedral
D) linear
E) icosahedral

back 105

A

front 106

The coordination number of cobalt in CoCl3 ∙ 6NH3 is ________.
A) 6
B) 7
C) 8
D) 1
E) 2

back 106

A

front 107

What is the oxidation number of Ni in [Ni(CN)4]2-?
A) +2
B) +1
C) 0
D) +3
E) +4

back 107

A

front 108

Which ion shown below does not exist?
A) Y4+
B) Y2+
C) Y+
D) Zr4+
E) Nb3+

back 108

A

front 109

Which ion shown has empty 5s orbitals?
A) Mo2+
B) Y3+
C) Zr4+
D) Nb2+
E) All choices have empty 5s orbitals.

back 109

E

front 110

Which ion shown has empty 4d orbitals?
A) Y3+
B) Zr2+
C) Nb+
D) Mo3+
E) Zr3+

back 110

A

front 111

A ligand with a single donor atom is called ________.
A) monodentate
B) bidentate
C) polydentate
D) a chelate
E) a chelon

back 111

A

front 112

Which of the following is not a chelating agent?
A) water
B) ethylenediamine
C) ortho-phenanthroline
D) carbonate ion
E) triphosphate ion

back 112

A

front 113

How many bonds can carbonate ion form to a metal ion?
A) 2
B) 3
C) 4
D) 1
E) 5

back 113

A

front 114

Which of the following is a polydentate ligand?
A) ethylenediamine
B) water
C) cyanide ion
D) nitrite ion
E) ammonia

back 114

A

front 115

The ligand with the formula Br– is named ________ in complexes with transition metals.
A) bromo
B) bromide
C) fluoro
D) carbonato
E) azido

back 115

A

front 116

The ligand with the name aqua when used in complexes with transition metals has the formula ________.
A) H2O
B) H2O2
C) HO-
D) N3-
E) H3O+

back 116

A

front 117

Which one of the following is the correct formula for pentaamminechlorocobalt (III) chloride?
A) [Co(NH3)5Cl]Cl2
B) [Co(NH3)4Cl]Cl2
C) [Co(NH3)6Cl]Cl2
D) [Co(NH3)5]Cl4
E) [Cl(NH3)5Co]Co2

back 117

A

front 118

Which of the following can form both high- and low-spin octahedral complexes?
A) Ru2+
B) Cr3+
C) Cr4+
D) Zr
E) Ag+

back 118

A

front 119

How many d electrons are associated with the metal ion in [Cr(NH3)6]3+?
A) 3
B) 4
C) 2
D) 1
E) 0

back 119

A

front 120

Draw a diagram of the short-hand ground state electron configuration of zinc.

back 120

front 121

Most transition metal ions contain partially occupied ________ subshells.

back 121

d

front 122

A substance is ________ if its ions or atoms have zero unpaired electrons.

back 122

diamagnetic

front 123

The two more common oxidation states of lead are ________ and ________.

back 123

2+, 4+

front 124

________ arises when the unpaired electrons of the atoms or ions in a solid are influenced by the orientations of the electrons of their neighbors.

back 124

Ferromagnetism

front 125

What is the oxidation state of the central atom in CaK[Co(CN)6]?

back 125

+3

front 126

The most common coordination numbers are ________.

back 126

4 and 6

front 127

What is the coordination number of the iron atom in CaNa[Fe(CN)6]?

back 127

6

front 128

Six-coordinate complexes generally have ________ geometry.

back 128

octahedral

front 129

The number of "free" chloride ions in an ionic coordination compound can be determined by treating the compound with ________.

back 129

AgNO3

front 130

The secondary valence in metal ion complexes is called the ________.

back 130

coordination number

front 131

Werner's theory of primary and secondary valences for transition metal complexes has given us the concepts of ________ and ________.

back 131

oxidation state, coordination number

front 132

Transition metal ions with empty valence orbitals act as ________.

back 132

Lewis acids

front 133

What is the oxidation number of the central metal in [Mo(H2O)5NO3]Cl2

back 133

+3

front 134

Define the chelate effect.

back 134

Chelate effect = an increased stability of complex compounds formed with chelating (polydentate) ligands compared to those formed with monodentate ligands.

front 135

The chelate effect is enhanced by polydentate ligand binding because of the change in ________.

back 135

entropy

front 136

List three of the ten transition metals required for human life.

back 136

Co, Cu, Cr, Fe, Mn, V, Zn, Ni, Mo, Cd

front 137

Myoglobin has ________ heme group(s) that bind(s) ________.

back 137

1,oxygen

front 138

In photosynthesis, ________ moles of photons are required to form one mole of ________.

back 138

48, glucose

front 139

In the leaves of plants, visible light is absorbed by a compound known as ________, and is aided by a ________ ion bonded to a porphyrin ring.

back 139

chlorophyll, Mg

front 140

What is the mechanism used in humans to combat blood bacterial growth via deprivation of iron?

back 140

fever

front 141

A large difference in formation constant (Kf) of a poly- versus monodentate ligand is called ________.

back 141

chelate effect

front 142

A compound that can occupy two coordination sites is a (an) ________.

back 142

bidentate ligand

front 143

The porphyrin compound that contains Mg (II) is called ________.

back 143

chlorophyll

front 144

The transport of iron into bacteria is facilitated by the formation of the complex ________.

back 144

ferrichrome

front 145

Name the compound: K2[Cr(H2O)4(CO3)2].

back 145

potassium tetraaquadicarbonatochromate (II)

front 146

Name Na [Ru(H2O)2 (C2O4)2].

back 146

sodium diaquadioxalatoruthenate (III)

front 147

Two compounds have the same formula and contain an ligand. In one compound the ligand is bonded to the metal atom via the N atom and in the other it is bonded via the S atom. These two compounds are examples of ________ isomers.

back 147

linkage

front 148

Non superimposable isomers are ________ isomers.

back 148

optical, chiral, enantiomeric

front 149

How can high-spin and low-spin transition metal complexes be distinguished from each other?

back 149

Magnetic properties and absorption spectra can be compared.

front 150

If chloride is a ligand to a transition metal, it will not be precipitated by silver nitrate.

back 150

true

front 151

The chelate effect must always occur with positive enthalpy change.

back 151

false

front 152

The color of hemoglobin changes from purple to red when water displaces oxygen on the molecule.

back 152

false

front 153

The heme unit of myoglobin is bound to the protein via a nitrogen-containing ligand.

back 153

true

front 154

To separate racemic mixtures, the isomers must be in a chiral environment.

back 154

true

front 155

Green and orange are complementary colors.

back 155

false

front 156

The energy of a metal ligand complex is higher than the energy of the separated components.

back 156

false

front 157

What is the purpose of adding sodium tripolyphosphate to a detergent?

back 157

to sequester the metal ions in hard water to prevent their interference with the action of the detergent

front 158

What colors of light does chlorophyll-a absorb?

back 158

red and blue

front 159

How does an elevated body temperature deprive some bacteria in the body of iron?

back 159

In some bacteria, siderophore production decreases as temperature increases.

front 160

What is a siderophore?

back 160

a ligand that forms an extremely stable water-soluble complex, such as ferrichrome, with iron

front 161

What is meant by the prefix tetrakis-, and when is it used?

back 161

It means 4 and is used when there are 4 of a ligand whose name includes a Greek prefix.

front 162

Name the compound, Ca[AlH4]2.

back 162

calcium tetrahydroaluminate

front 163

Name the compound, [Os(en)3]2 [NiCl2Br2]3.

back 163

tris(ethylenediamine)osmium(III) dibromodichloronickelate(II)

front 164

Name the compound, Cu(H2O)42+.

back 164

tetraaquacopper(II)

front 165

In what two ways can an object appear blue?

back 165

absorb all wavelengths except blue and reflect or transmit only blue, or absorb the complementary color of blue and reflect or transmit all others