Chem 124/125: Chapter 23 - Transition Elements and Their Coord Cmpds: Properties, Nome

What is the geometry for the complex ion [Co(SO4)(NH3)5]+?

Octahedral

Which of the following statements correctly describe the electron configurations of transition metals? Select all that apply.

Period 4 is the earliest period that contains transition metals. Most d-block elements have a valence-level electron configuration that corresponds to ns2(n - 1)dx.

Which of the following statements correctly describe a pair of optical isomers? Select all that apply.

-Optical isomers have identical melting and boiling points. -Optical isomers rotate plane polarized light in opposite directions. -Optical isomers are mirror-image compounds that cannot be superimposed.

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 +2. -The central metal ion is Cr3+.

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

-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 coordination number is the number of donor atoms bonded to the central metal ion.

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 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 lanthanides? Select all that apply.

-The properties of the lanthanides are very similar. -The lanthanides are known as the rare earth elements. -Most lanthanides have an empty valence d sublevel.

Which of the following metals will reduce Mn2+? Select all that apply.

-V -Ti

Which of the following complex ions contain Fe with a 3+ charge? Select all that apply.

-[Fe(NH3)5(SCN)]2+ -[FeCl4]-

Which of the following complex ions can exist as a pair of cis-trans isomers? Select all that apply.

-[Pt(NH3)4Br2]2+ -[Pd(CN)2(OH)2]2-

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

6; 6; 1

Match each geometric isomer in the image shown to the correct designation.

A -cis-diamminetetraaquairon(II) B -trans-diamminetetraaquairon(II)

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

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.

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

The ns2 electrons are readily lost.

Match each type of element to the correct description.

The transition elements -include only metals. The main-group elements -include both metals and nonmetals. The formation of ionic compounds that are colored and paramagnetic -is typical of transition elements. The formation of ionic compounds that are colorless and diamagnetic -is typical of main-group elements.

True or false: In general, reducing strength will decrease across each period for the transition metal series.

True

Match each type of transition metal ion with the physical properties of its compounds. Instructions

Highly colored and paramagnetic -Transition metal ion with a partially filled d sublevel Colorless and diamagnetic -Transition metal ion with either a full or an empty d sublevel

Which one of the following coordination complex formulas is written correctly?

[Co(H2O)5(CN)]Cl2

Which of the following electron configurations is that of a lanthanide?

[Xe] 6s24f15d1

Match each complex ion with the correct coordination number.

[Zn(OH)4]2- 4 [Co(NH3)3(H2O)3]3+ 6 [Fe(OH)(H2O)4]2+ 5 [AgCl2]- 2

In which orbital or group of orbitals would the last electron for each of the following elements be placed? (Assume a neutral atom with a ground-state electron configuration.)

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

Atomic sizes for transition metals within the same period __________ from left to right at first but then remain fairly constant, increasing only slightly compared to the trend found among the main-group elements. The reason for this trend is because the d orbitals are ___________ orbitals and thus they shield outer electrons very efficiently.

decrease, inner

Reducing strength, in general, will across each period for the transition metal series. Thus cobalt has a reducing strength than nickel.

decrease; greater

Isomers that have the same skeleton but differ in the spatial arrangement of their atoms are called _____, whereas isomers that have different skeletons are called _____ isomers.

stereoisomers; constitutional isomers

Transition metals exhibit multiple oxidation states because ______.

their ns and (n - 1)d electrons are very close in energy so all or most of these electrons can behave like valence electrons

Many __________ metal compounds are colored and paramagnetic, whereas main-group ionic compounds are colorless and ___________.

transition, diamagnetic

Transition metals exhibit less metallic behavior in their higher oxidation states due to a modified ability to attract electron density, called ______.

valence-state electronegativity

Transition metals exhibit less metallic behavior in their higher oxidation states due to a modified ability to attract electron density, called ________.

valence-state electronegativity

The lanthanides generally form ions with a _________ charge.

+3

Consider the following iron compounds, Fe2O3 and FeO. What is the oxidation state of iron in each of these two compounds?

+3 in Fe2O3, +2 in FeO

Match each element correctly to its highest possible oxidation state.

+6 -Chromium +7 -Manganese +5 -Vanadium +3 -Scandium

Which of the following statements correctly describe the physical appearance and properties of transition metal compounds? Select all that apply.

- Transition metal ions with a d0 configuration will be colorless. - If a transition metal compound is colored, it will also be paramagnetic. - Transition metal ions with unpaired d electrons will form colored compounds.

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

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

Which of the following statements correctly describe geometric isomers of coordination compounds? Select all that apply.

-A coordination compound may have geometric isomers if the ligands can be arranged differently in space relative to the central metal ion. -The isomer that has identical ligands adjacent to each other is called the cis isomer. -Geometric isomers are different compounds and have different physical properties.

Which of the following statements correctly describe the actinides? Select all that apply.

-Actinides form highly colored compounds. -All actinides are radioactive. -The actinides have similar outer-electron configurations to the lanthanides.

Which of the following metals are lanthanides? Select all that apply.

-Cerium -Gadolinium -Neodymium

Which of the following statements correctly describe the two types of constitutional (structural) isomers exhibited by coordination compounds? Select all that apply.

-Coordination isomers have different complex ions. -Linkage isomers are possible if a ligand has more than one donor atom. -Coordination isomers can result when a compound contains more than one complex ion.

Which of the following metals will reduce Zn2+? Select all that apply.

-Manganese -Chromium -Vanadium

Match each coordination number to the correct geometry of the complex ion.

Four -Tetrahedral or square planar Two -Linear Six -Octahedral

Match each type of isomer to the correct description.

Constitutional isomers -Have the same molecular formula but different skeletons Stereoisomers -Have the same molecular formula and skeleton, but differ in the spatial arrangement of their atoms

Coordination complexes exhibit different types of constitutional (structural) isomers. Match each type of isomer with the correct description.

Coordination isomers -Differ in the composition of the complex ion but have the same overall molecular formula Linkage isomers -Have the same formula and complex ion composition, but differ in the attachment of the ligand

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

Most transition elements display at least two oxidation states. 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.

Both ionization energy and electronegativity remain relatively __________ as you move from left to right across a period of transition metals. This is due to effective __________ by the inner d electrons.

constant, shielding

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

coordination

Two coordination compounds that have the same ligands arranged differently in space around the central metal ion, but are not mirror images of one another, are called __________ isomers. If the identical ligands are next to each other, the isomer is described as __________ while the isomer with identical ligands across from each other is the ___________ isomer.

geometric; cis; trans

A transition metal in a lower oxidation state will form a compound higher in _____ character, whereas a transition metal in a higher oxidation state will form a compound that is more _____ in character.

ionic; covalent

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

Transition metal oxides become _____ covalent and _____ basic as the oxidation state of the metal increases.

more; less

If two compounds are mirror images of one another, but are not superimposable, they are called _________ isomers or enantiomers. These isomers have _________ physical properties except for the direction in which each rotates the plane of polarized light.

optical; identical

Valence-state electronegativity is an effective electronegativity that depends on the __________ state of an element. The higher the oxidation state of a transition metal, the ___________ its attraction for bonded electrons and the ___________ its valence-state electronegativity.

oxidation; greater; higher