![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_largeCoverImage.gif)
Concept explainers
Manganese is found as MnO2 in deep ocean deposits.
- (a) Depict the electron configuration of this element using the noble gas notation and an orbital box diagram.
- (b) Using an orbital box diagram, show the electrons beyond those of the preceding noble gas for Mn4+.
- (c) Is Mn4+ paramagnetic?
- (d) How many unpaired electrons does the Mn4+ ion have?
(a)
![Check Mark](/static/check-mark.png)
Interpretation:
The electronic configuration of Manganese has to be depicted using its orbital notation box and noble gas electron filling methods.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.
The important there rules for electronic configuration given below:
Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.
Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.
Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.
Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.
Explanation of Solution
Let us consider the orbital filling method of Manganese (Mn) element
Hence, the electronic configuration of Manganese (Mn) =
(b)
![Check Mark](/static/check-mark.png)
Interpretation:
The electronic configuration of Manganese ion (Mn4+) has to be depicted using its orbital notation box and noble gas electron filling methods.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.
The important there rules for electronic configuration given below:
Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.
Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.
Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.
Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.
Explanation of Solution
Let us consider the orbital filling method of Manganese (Mn4+) element
Than manganese (Mn) atom was oxidized to (Mn4+) ions, it lost for four electrons in outermost (4s and 3d) orbitals.
Hence, the electronic configuration of Manganese (Mn4+) =
(c)
![Check Mark](/static/check-mark.png)
Interpretation:
Mn4+ ion is paramagnetic or not has to be predicted.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.
The important there rules for electronic configuration given below:
Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.
Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.
Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.
Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.
Explanation of Solution
The manganese (Mn4+) ion has three unpaired electrons in (3d) shells. Hence this system completely obeyed for paramagnetic nature, because all unpaired electrons occupying in each single shell, so this (Mn4+) is paramagnetic.
(d)
![Check Mark](/static/check-mark.png)
Interpretation:
The number of unpaired electrons the Mn4+ion possess has to be predicted.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.
The important there rules for electronic configuration given below:
Aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. If consider the 1s shell is filled the 2s subshell is occupied.
Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Pauli exclusion rule: an atomic orbital may describe at most two electrons, each with opposite spin direction.
Paramagnetic: The Paramagnetic properties are due to the presence of some unpaired electrons, and from the realignment of the electron paths caused by the external magnetic field.
Diamagnetic properties: In diamagnetic materials all the electron are paired so there is no permanent net magnetic moment per atom.
Explanation of Solution
The manganese (Mn4+) system having three unpaired electrons, see the above electronic configuration diagram.
Want to see more full solutions like this?
Chapter 7 Solutions
Chemistry & Chemical Reactivity
- rite the proper charges so that an alkali metal, a noble gas, and a halogen have the same electron configurations. What is the number of protons in each“? The number of electrons in each? Arrange them from smallest to largest radii and explain your ordering rationale.arrow_forwardWhat neutral atoms are isoelectronic with the following ions? (a) Pb4+ (b) Br (c) S2 (d) Ni3+arrow_forward2. The ionization energy of an element is defined as the amount of energy required to remove an electron from an individual atom. The following table gives the ionization energy (in units of kilojoules per mole) for five metals, listed in alphabetical order. Locate each of these metals on the periodic table and arrange them in order of rows and columns as in the periodic table. (a) Describe the periodic trend in the ionization energy of elements within a group. (b) Describe the periodic trend in the ionization energy of elements across a period. Metal Calcium Magnesium Potassium Sodium Strontium Ionization Energy 590 738 419 496 549 Materialsarrow_forward
- Consider the isoelectronic series Ca2+, Sc3+, Ti4+, V5+. Arrange these species as follows. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) in order of increasing atomic or ionic radius (b) in order of increasing ionization energyarrow_forwardThe gadolinium +3 ion (Gd3+) has advantageous magnetic properties for Magnetic Resonance Imaging (MRI) applications, specifically a high number of unpaired electrons. In fact, both neutral Gd and Gd3+ have a set of degenerate orbitals with seven unpaired electrons. a) Write the electron configuration for Gd and Gd3+ using the condensed noble gas notation. Identify which orbitals lose electrons to yield the +3 cation based on the above information. Explain your reasoning (2-3 sentences). b) Curium (Cm) is an actinide element named for Marie Curie. Cm is in the same group as Gd and also forms a +3 cation. Write the electron configuration for Cm and Cm3+. c) While +3 is the most common oxidation state for lanthanide elements, some can form +2 ions. Identify an isoelectronic ion to Gd3+ that has a +2 oxidation state and indicate which orbitals lose electrons to form that ion.arrow_forwardBoron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forward
- (1) What is the valence electron configuration for the krypton atom? (2) What is the valence electron configuration for the silicon atom? (1) What is the name of the element with a valence electron configuration of 2s2p4? (2) What is the name of the element with a valence electron configuration of 4s24p°? (1) The element with a valence electron configuration of 2s22p4 is in group and period (2) The element with a valence electron configuration of 3s23p² is in group and period please explain eacharrow_forwardGive the group number and the general valence electron configuration of an element with the following electron-dot symbol. (For example, type ns2 np6 for ns²np°, which is the valence configuration of all group 8A elements.) (a) group number electron configuration (b) group number electron configurationarrow_forwardArrange the following sets of ions in order of decreasing ionic radii. (a) Br,I, S² , Se²- (b) Ba2+, Ca?+ Sr²+arrow_forward
- (1) What is the valence electron configuration for the arsenic atom? (2) What is the valence electron configuration for the fluorine atom?arrow_forwardWrite the complete electron configuration for each of the following ions (a) Ga3+: (b) Mg2+:arrow_forwardWhich of the following elements is expected to have the highest SECOND IONIZATION ENERGY: (A) Be (B) Ca (C) Mg (D) Naarrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337399425/9781337399425_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)