Which of the following statements correctly describe the electron configurations of transition metals? - When filling the valance shell orbitals for a d-block element, e-s are usually placed in the (n-1)d orbitals before the ns orbitals - Most d-block elements have a valence-level e- configuration that corresponds ns^2(n-1)d^x. - The f sublevel is included for transition elements of P.5 and 6 - P.4 is the earliest period that contains transition metals.

- P.4 is the earliest period that contains transition metals. - Most d-block elements have a valence-level e- configuration that corresponds ns^2(n-1)d^x.

Which of the following types of substances are classified as acids only under the Lewis definition? Select all that apply. - Weak acids (e.g., HCN) - Small, highly charged metal ions that are hydrated - Molecules that contain a polar multiple bond - Molecules with electron deficient central atoms - Salts that contain the conjugate acid of weak bases (e.g., NH4Cl)

- Molecules that contain a polar multiple bond - Molecules with electron deficient central atoms

Why do many transition metals have an oxidation state of +2? - The ns2 electrons are readily lost. - Electrons are easily added to the (n – 1)d orbitals. - The (n – 1)d electrons are lost before ns2 electrons.

- The ns2 electrons are readily lost.

Why do transition metals have multiple oxidation states? Select all that apply. - Since both filled and half-filled sublevels are especially stable, there are several stable states for most transition metals - The ns and (n – 1)d electrons are close in energy; hence all or most of these can be used in bonding. - Transition metals lose their valence d electrons one at a time and therefore have as many oxidation states as they have d electrons. - Transition metals can either lose or gain electrons to attain a noble gas electron configuration.

- The ns and (n – 1)d electrons are close in energy; hence all or most of these can be used in bonding. - Since both filled and half-filled sublevels are especially stable, there are several stable states for most transition metals

Chem 124 Ch. 18(10), Ch.21(1-3) Flashcards by Jadyn Walton

Match each specie to the correct Lewis acid-base def.
LB-
LA-

E- pair donor
E- pair acceptor

LB- donor
LA- acceptor

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The product of a Lewis acid-base reaction is called a(n) ____, which is a single species containing a new ____.

free radical;H bond
+; ionic bond
LB: e- pairs
adduct; covalent bond

adduct; covalent bond

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Which of the following species are LA?

SO3
-OF2
-Cl-
Cu2+
BF3

Cu2+
BF3
SO3

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T or F: A metal cation behaves as a LA in water to form a hydrated cation adduct.

T
Reason: The LPs on O’s of water act as LB to form new covalent bonds w/ metal cation.

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Many____ metal compounds are colored and paramagnetic, whereas main-group ionic compounds are colorless and ____.

transition; diamagnetic

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Which of the following statements correctly describe the electron configurations of transition metals?

When filling the valance shell orbitals for a d-block element, e-s are usually placed in the (n-1)d orbitals before the ns orbitals
Most d-block elements have a valence-level e- configuration that corresponds ns^2(n-1)d^x.
The f sublevel is included for transition elements of P.5 and 6
P.4 is the earliest period that contains transition metals.

P.4 is the earliest period that contains transition metals.
Most d-block elements have a valence-level e- configuration that corresponds ns^2(n-1)d^x.

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Which of the following is the correct condensed ground state e- configuration for Cr?

[Ar] 4s23d4
[Ar] 4s14d5
[Ar] 3d6
[Ar] 4s13d5

[Ar] 4s1 3d5

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Match each metal, assuming it is neutral and in its ground state, with the correct number of unpaired electrons within the valence d-sublevel. Ti, Cr, Cu, Co, Fe.

4 d e-
2 d e-
none
5 d e-
3 d e-

Ti:2
Cr:5
Cu:0
Co:3
Fe:4

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Which of the following types of substances are classified as acids only under the Lewis definition? Select all that apply.

Weak acids (e.g., HCN)
Small, highly charged metal ions that are hydrated
Molecules that contain a polar multiple bond
Molecules with electron deficient central atoms
Salts that contain the conjugate acid of weak bases (e.g., NH4Cl)

Molecules that contain a polar multiple bond
Molecules with electron deficient central atoms

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Which of the following is the correct condensed ground-state electron configuration for vanadium?

[Ar] 4s2 3d3
[Ar] 4s1 3d4
[Ar] 4s2 3d2
[Ar] 4s2 4d3

[Ar] 4s2 3d3

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Metal cations act like ____ when dissolved in water. The hydrated cation is the ____.

Lewis acids; adduct
Lewis bases; adduct
Lewis acids; Lewis bases
Lewis bases; Lewis acids

Lewis acids; adduct

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Match each type of element to the correct description:
The transition elements->
The main-group elements->
The formation of ionic compounds that are colored and paramagnetic->
The formation of ionic compounds that are colorless and diamagnetic->

include metals and nonmetals
typical of main group elements
typical of transition elements
only metals

The transition elements-> only metals
The main-group elements-> includes metals and nonmetals
The formation of ionic compounds that are colored and paramagnetic-> transition metals
The formation of ionic compounds that are colorless and diamagnetic-> main group

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A transition metal cation is always formed by losing the ____ e- before the ____ e-. Zn2+ will therefore have ____ unpaired e^-s.

ns, (n – 1)d; 0
(n – 1)d, ns; 2
ns, (n – 1)d; 2

ns, (n – 1)d; 0

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In which orbital or group of orbitals would the last electron for each of the following elements be placed? (neutral atom w/ ground-state electron configuration.) Ni, Na, Zr, Br.

Ni: 3d
Na: 3s
Zr: 4d
Br: 4p

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Match each outer electron configuration with the correct element, assuming a neutral atom with ground-state electron configuration. Sc (Z=21), Cr(Z=24), Cu (z=29), Ni (Z=28)

4s2 3d8
4s2 3d1
4s1 3d10
4s1 3d5

Sc: 4s2 3d1
Cr: 4s1 3d5
Cu: 4s1 3d10
Ni: 4s2 3d8

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Why do many transition metals have an oxidation state of +2?

The ns2 electrons are readily lost.
Electrons are easily added to the (n – 1)d orbitals.
The (n – 1)d electrons are lost before ns2 electrons.

The ns2 electrons are readily lost.

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Why do transition metals have multiple oxidation states? Select all that apply.

Since both filled and half-filled sublevels are especially stable, there are several stable states for most transition metals
The ns and (n – 1)d electrons are close in energy; hence all or most of these can be used in bonding.
Transition metals lose their valence d electrons one at a time and therefore have as many oxidation states as they have d electrons.
Transition metals can either lose or gain electrons to attain a noble gas electron configuration.

The ns and (n – 1)d electrons are close in energy; hence all or most of these can be used in bonding.
Since both filled and half-filled sublevels are especially stable, there are several stable states for most transition metals

Which of the following is the correct electron configuration for the Fe3+ ion?

[Ar] 3d6
[Ar] 3d5
[Ar] 4s13d4
[Ar] 4s23d3

[Ar] 3d5

Match each type of transition metal ion with the physical properties of its compounds.
Highly colored and paramagnetic->
Colorless and diamagnetic->

Transition metal ion with either a full or an empty d sublevel
Transition metal ion with a partially filled d sublevel

Highly colored and paramagnetic-> partially
Colorless and diamagnetic-> full/empty

A coordination compound is typically made up of a complex ion and counter ions. The complex ion consists of a central____
cation bonded to molecules and/or____ called____.

metal;anions;ligands

Which of the following options correctly describes the behavior of a coordination complex when it is dissolved in water?

The ligands become associated with the counter ions, releasing the metal cation into solution.
The counter ions, ligands, and central metal cation are all separated from each other.
The ligands are separated from the metal cation, but the cation remains associated with its counter ions.
The complex ion dissociates from the counter ions, but the ligands remain attached to the metal cation.

The complex ion dissociates from the counter ions, but the ligands remain attached to the metal cation.

Which of the following statements correctly describe the oxidation states for transition metals? Select all that apply.

For elements from Groups 3B to 7B, the highest oxidation state observed equals the group number.
Elements in all groups designated 8B have more oxidation states than other transition elements.
A +2 oxidation state is very common among transition elements.
Most transition elements display at least two oxidation states.
The most common oxidation state for elements of Group 8B (8) is +8.

For elements from Groups 3B to 7B, the highest oxidation state observed equals the group number.
A +2 oxidation state is very common among transition elements.
Most transition elements display at least two oxidation states.

Which of the following species will be present in solution when [Cu(NH3)4]Cl2 dissolves in water? Select all that apply.

[Cu(NH3)4]2+
Cu2+
Cl22–
Cl–
NH3

[Cu(NH3)4]2+
Cl–

Which of the following statements correctly describe the composition of a coordination complex? Select all that apply.

The ligands are directly bonded to the central metal cation.
Ligands may be neutral molecules or anions.
The central ion of the complex ion is usually a Group 1A metal.
A coordination complex has a complex ion as the cation or anion.
The counter ions of a coordination complex are also called ligands.

The ligands are directly bonded to the central metal cation.
Ligands may be neutral molecules or anions.
A coordination complex has a complex ion as the cation or anion.

Which of the following statements correctly describe the coordination number of a complex ion? Select all that apply. - A particular metal cation always has the same coordination number. - The coordination number is the number of donor atoms bonded to the central metal ion. - The coordination number is the overall charge of the complex ion. - The coordination number depends on the metal, the oxidation state of the metal, and the specific compound. - The most common coordination number is 6.

- The most common coordination number is 6. - The coordination number is the number of donor atoms bonded to the central metal ion. - The coordination number depends on the metal, the oxidation state of the metal, and the specific compound

The coordination number of the Cr3+ ion in the complex [Cr(NH3)4Cl2]Cl is equal to____ b/c there are____ ligands attached to the central metal ion. There is/are ____ counter ion(s) for the complex ion.

6;6;1

Match each coordination compound with the correct number of ions each produces when dissolved in water. - [Co(NH3)6]Cl3 -> - K2[Fe(CN)4] -> - [Ag(NH3)2]NO3-> - 2 ions - 4 ions - 3 ions

- [Co(NH3)6]Cl3 -> 4 ions - K2[Fe(CN)4] -> 3 ions - [Ag(NH3)2]NO3-> 2 ions

What is the geometry for the complex ion [Co(SO4)(NH3)5]+? - Tetrahedral - Octahedral - Trigonal bipyramidal - Square pyramidal

- Octahedral Reason: Reason: There are 6 ligands; both the NH3 molecules and the SO42– ion are ligands. The shape will be octahedral.

The number of ligand donor atoms bonded directly to the central metal ion in a complex ion is called the ____ number.

coordination

To form a complex ion, each ligand donates a(n) _____ pair of electrons to the metal ion to form a coordinate______ bond.

lone;covalent

A ligand that bonds to the metal through two donor atoms is classified as a(n)_____ ligand. A complex ion containing a ligand with more than one donor atom is called a(n)______ because the ligands seem to hold the metal ion like a pair of claws.

bidentate; chelate

Which of the following ligands can form chelating complexes? Select all that apply. - H2NCH2CH2NH2 - EDTA - SCN– - NH3

- EDTA - H2NCH2CH2NH2

Match each coordination number to the correct geometry of the complex ion. 4-> 2-> 6-> -Octahedral -Linear -Tetrahedral or square planar

4->Tetra 2-> linear 6->octa

Which of the following statements correctly describe the steps required to determine the charge on the central metal ion in the complex [Cr(H2O)5Br]Cl2? Select all that apply. - The charge on the complex ion is +1. - The central metal ion is Cr3+. - The charge on the complex ion is +2. - The central metal ion is Cr2+. -The ligands provide a charge of -6.

- The charge on the complex ion is +2. - The central metal ion is Cr3+.

Which one of the following coordination complex formulas is written correctly? - [PtCl2(NH3)4](NO3)2 - [Co(H2O)5(CN)]Cl2 - Cl[Ag(NH3)2]

- [Co(H2O)5(CN)]Cl2

Match each type of ligand to the correct description. Monodentate-> Bidentate-> Polydentate-> - Ligand bonds through a single donor atom - Ligand has more than 2 donor atoms - Ligand has 2 donor atoms

Monodentate->Ligand bonds through a single donor atom Bidentate->Ligand has 2 donor atoms Polydentate->Ligand has more than 2 donor atoms

Which of the following options classify the given ligand correctly? Select all that apply. - H2NCH2CH2NH2 is a monodentate ligand. -EDTA is a bidentate ligand. - H2O is a bidentate ligand. - Cl– is a monodentate ligand. - C2O42– is a bidentate ligand.

- Cl– is a monodentate ligand. - C2O42– is a bidentate ligand.

Match each component of a coordination complex with the correct rule used when naming the compound. Neutral ligands-> Anionic ligands-> Metal cation-> Anionic complex ion-> - Generally keep the name of the molecule - Name ending changes from -ide to -o - Named after the ligands - Name ending changes to -ate

Neutral ligands-> Generally keep the name of the molecule Anionic ligands-> Name ending changes from -ide to -o Metal cation-> Named after the ligands Anionic complex ion->Name ending changes to -ate

Which of the following complex ions contain Fe with a 3+ charge? Select all that apply. - [Fe(H2O)6]2+ - [Fe(SCN)4]2– - [FeCl4]– - [Fe(NH3)5(SCN)]2+

- [FeCl4]– - [Fe(NH3)5(SCN)]2+

When are the numerical prefixes bis, tris, and tetrakis used for naming coordination complexes? - These prefixes are used to indicate the number of any anionic ligands. - These prefixes are used to indicate the number of any neutral ligands. - These prefixes are used to indicate the number of bidentate ligands. - These prefixes indicate the number of ligands if the ligand name already contains a numerical prefix.

- These prefixes indicate the number of ligands if the ligand name already contains a numerical prefix.

Which of the following options correctly describe how to write the formula for a coordination complex? Select all that apply. - The formula for the whole complex ion is written in square brackets. - The charge of the metal ion is balanced by the charge of the counter ion(s). - The counter ion is always listed at the end of the formula. - The cation is listed first in the formula. - The formulas for neutral ligands are placed before the formulas for anionic ligands.

- The formula for the whole complex ion is written in square brackets. - The cation is listed first in the formula. -The formulas for neutral ligands are placed before the formulas for anionic ligands.

Which of the following statements correctly describe the rules for naming a coordination compound? Select all that apply. - If the complex ion, is an anion its name will end in -ide. - The number of each ligand is indicated by a numerical prefix. - The ligands of the complex ion are named in alphabetical order. - For an anionic ligand, the -ide ending is changed to -o after the root name. - The names of the ligands are listed after the name of the metal ion.

- The number of each ligand is indicated by a numerical prefix. - The ligands of the complex ion are named in alphabetical order. - For an anionic ligand, the -ide ending is changed to -o after the root name.

Chem 124 Ch. 18(10), Ch.21(1-3) Flashcards

Lewis acids, bases. Transition metals. Coordination compounds