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(a)
Interpretation:
The number of unpaired electrons that is associated with electronic configuration
Concept Introduction:
Electronic configuration of an atom describes how many electrons are present in the shell. Many orbitals are present about the nucleus of an atom. In these orbitals the electrons do not occupy randomly. There are three rules for assigning the electrons to various shells, subshells, and orbitals. They are,
- The subshells are filled in increasing order of energy.
- In a subshell, the electrons occupy the orbital singly first in all orbitals before pairing up by the second electron. All the electrons that are in singly occupied orbitals have same spin.
- In a given orbital there cannot be more than two electrons and they have opposite spins.
Electronic configuration of an element is the one that gives information about how many electrons are present in each electron subshell of an atom. The electrons are added to the subshells in increasing order of energy. Electronic configurations are written in shorthand notation which uses a number‑letter combination. The shell is indicated by the number and subshell is indicated by the letter. Superscript that follows the subshell tells how many electrons are present in the subshell.
The order of filling up the electrons in the subshell is done as shown in the given figure below.
Orbital diagram is the one that gives information about the number of electrons present in the electron orbitals of an atom. The difference between electronic configuration and orbital diagram is that electronic configuration deals with the electrons occupancy in the subshell while orbital diagram deals with the electrons occupancy in the electron orbital. Electrons are paired up in the orbital only when all the orbitals in the subshell are singly filled.
(b)
Interpretation:
The number of unpaired electrons that is associated with electronic configuration
Concept Introduction:
Electronic configuration of an atom describes how many electrons are present in the shell. Many orbitals are present about the nucleus of an atom. In these orbitals the electrons do not occupy randomly. There are three rules for assigning the electrons to various shells, subshells, and orbitals. They are,
- The subshells are filled in increasing order of energy.
- In a subshell, the electrons occupy the orbital singly first in all orbitals before pairing up by the second electron. All the electrons that are in singly occupied orbitals have same spin.
- In a given orbital there cannot be more than two electrons and they have opposite spins.
Electronic configuration of an element is the one that gives information about how many electrons are present in each electron subshell of an atom. The electrons are added to the subshells in increasing order of energy. Electronic configurations are written in shorthand notation which uses a number‑letter combination. The shell is indicated by the number and subshell is indicated by the letter. Superscript that follows the subshell tells how many electrons are present in the subshell.
The order of filling up the electrons in the subshell is done as shown in the given figure below.
Orbital diagram is the one that gives information about the number of electrons present in the electron orbitals of an atom. The difference between electronic configuration and orbital diagram is that electronic configuration deals with the electrons occupancy in the subshell while orbital diagram deals with the electrons occupancy in the electron orbital. Electrons are paired up in the orbital only when all the orbitals in the subshell are singly filled.
(c)
Interpretation:
The number of unpaired electrons that is associated with electronic configuration
Concept Introduction:
Electronic configuration of an atom describes how many electrons are present in the shell. Many orbitals are present about the nucleus of an atom. In these orbitals the electrons do not occupy randomly. There are three rules for assigning the electrons to various shells, subshells, and orbitals. They are,
- The subshells are filled in increasing order of energy.
- In a subshell, the electrons occupy the orbital singly first in all orbitals before pairing up by the second electron. All the electrons that are in singly occupied orbitals have same spin.
- In a given orbital there cannot be more than two electrons and they have opposite spins.
Electronic configuration of an element is the one that gives information about how many electrons are present in each electron subshell of an atom. The electrons are added to the subshells in increasing order of energy. Electronic configurations are written in shorthand notation which uses a number‑letter combination. The shell is indicated by the number and subshell is indicated by the letter. Superscript that follows the subshell tells how many electrons are present in the subshell.
The order of filling up the electrons in the subshell is done as shown in the given figure below.
Orbital diagram is the one that gives information about the number of electrons present in the electron orbitals of an atom. The difference between electronic configuration and orbital diagram is that electronic configuration deals with the electrons occupancy in the subshell while orbital diagram deals with the electrons occupancy in the electron orbital. Electrons are paired up in the orbital only when all the orbitals in the subshell are singly filled.
(d)
Interpretation:
The number of unpaired electrons that is associated with electronic configuration
Concept Introduction:
Electronic configuration of an atom describes how many electrons are present in the shell. Many orbitals are present about the nucleus of an atom. In these orbitals the electrons do not occupy randomly. There are three rules for assigning the electrons to various shells, subshells, and orbitals. They are,
- The subshells are filled in increasing order of energy.
- In a subshell, the electrons occupy the orbital singly first in all orbitals before pairing up by the second electron. All the electrons that are in singly occupied orbitals have same spin.
- In a given orbital there cannot be more than two electrons and they have opposite spins.
Electronic configuration of an element is the one that gives information about how many electrons are present in each electron subshell of an atom. The electrons are added to the subshells in increasing order of energy. Electronic configurations are written in shorthand notation which uses a number‑letter combination. The shell is indicated by the number and subshell is indicated by the letter. Superscript that follows the subshell tells how many electrons are present in the subshell.
The order of filling up the electrons in the subshell is done as shown in the given figure below.
Orbital diagram is the one that gives information about the number of electrons present in the electron orbitals of an atom. The difference between electronic configuration and orbital diagram is that electronic configuration deals with the electrons occupancy in the subshell while orbital diagram deals with the electrons occupancy in the electron orbital. Electrons are paired up in the orbital only when all the orbitals in the subshell are singly filled.
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Chapter 3 Solutions
General, Organic, and Biological Chemistry
- Comparing two means. Horvat and co-workers used atomic absorption spectroscopy to determine the concentration of Hg in coal fly ash. Of particular interest to the authors was developing an appropriate procedure for digesting samples and releasing the Hg for analysis. As part of their study they tested several reagents for digesting samples. Their results using HNO3 and using a 1+3 mixture of HNO3 and HCl are shown here. All concentrations are given as ppb Hg sample. HNO3: 161, 165, 160, 167, 166 1+3 HNO3–HCl: 159, 145, 140, 147, 143, 156 Determine whether there is a significant difference between these methods at the 95% confidence interval.arrow_forwardComparison of experimental data to “known” value. Monna and co-workers used radioactive isotopes to date sediments from lakes and estuaries.21 To verify this method they analyzed a 208Po standard known to have an activity of 77.5 decays/min, obtaining the following results. 77.09, 75.37, 72.42, 76.84, 77.84, 76.69, 78.03, 74.96, 77.54, 76.09, 81.12, 75.75 Do the results differ from the expected results at the 95% confidence interval?arrow_forwardExplain the difference between the propagated uncertainty and the standard deviation. Which number would you use to describe the uncertainty in the measurement? if the standard deviation is 0.01 and the propagated uncertainty is 0.03arrow_forward
- Propagation of uncertainty. Find the absolute and percent relative uncertainty assuming the ±-values are random error. 7.65±0.04 + 5.28±0.02 – 1.12±0.01 85.6±0.9 × 50.2±0.7 ÷ 13.8±0.5 [4.88±0.07 + 3.22±0.05] / 1.53±0.02arrow_forwardExplain the difference between the propagated uncertainty and the standard deviation. Which number would you use to describe the uncertainty in the measurement?arrow_forwardCircle the compound in each pair where the indicated bond vibrates at higher frequency. WHY IS THIS? Provide thorough explanation to tie topic.arrow_forward
- How can you distinguish between each pair of compounds below using IR? Cite a bond and frequency that can be used to distinguish. Provide thorough steps and explanation.arrow_forwardPropagation of uncertainty. Find the absolute and percent relative uncertainty assuming the ±-values are random error. 65±0.04 + 5.28±0.02 – 1.12±0.01 6±0.9 × 50.2±0.7 ÷ 13.8±0.5 [4.88±0.07 + 3.22±0.05] / 1.53±0.02arrow_forwardMatch to correct spectrum and explain the bonds and frequencies used to tell what spectrum connected to the given option. Thanks.arrow_forward
- Draw the virtual orbitals for the planar and pyramidal forms of CH3 and for the linear and bent forms of CH2arrow_forwardQ2: Draw the molecules based on the provided nomenclatures below: (2R,3S)-2-chloro-3-methylpentane: (2S, 2R)-2-hydroxyl-3,6-dimethylheptane:arrow_forwardQ3: Describes the relationship (identical, constitutional isomers, enantiomers or diastereomers) of each pair of compounds below. ག H CH3 OH OH CH3 H3C OH OH OH ////////// C CH3 CH3 CH3 CH3 H3C CH 3 C/III..... Physics & Astronomy www.physics.northweste COOH H нош..... H 2 OH HO CH3 HOOC H CH3 CH3 CH3 Br. H H Br and H H H Harrow_forward
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