a)
Interpretation:
The
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
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.
Quantum numbers: These terms are explained for the distribution of electron density in an atom. They are derived from the mathematical solution of Schrodinger’s equation for the hydrogen atom. The types of quantum numbers are the principal quantum number (n), the
b)
Interpretation:
The total number of s-electrons in
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
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.
Quantum numbers: These terms are explained for the distribution of electron density in an atom. They are derived from the mathematical solution of Schrodinger’s equation for the hydrogen atom. The types of quantum numbers are the principal quantum number (n), the angular momentum quantum number (l), the magnetic quantum number (ml) and the electron spin quantum number (ms). Each atomic orbital in an atom is categorized by a unique set of the quantum numbers.
c)
Interpretation:
The total number of p-electrons in
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
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.
Quantum numbers: These terms are explained for the distribution of electron density in an atom. They are derived from the mathematical solution of Schrodinger’s equation for the hydrogen atom. The types of quantum numbers are the principal quantum number (n), the angular momentum quantum number (l), the magnetic quantum number (ml) and the electron spin quantum number (ms). Each atomic orbital in an atom is categorized by a unique set of the quantum numbers.
d)
Interpretation:
The total number of p-electrons in
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
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.
Quantum numbers: These terms are explained for the distribution of electron density in an atom. They are derived from the mathematical solution of Schrodinger’s equation for the hydrogen atom. The types of quantum numbers are the principal quantum number (n), the angular momentum quantum number (l), the magnetic quantum number (ml) and the electron spin quantum number (ms). Each atomic orbital in an atom is categorized by a unique set of the quantum numbers.
e)
Interpretation:
The element is either a metal, metalloid, or non-metal has to be predicted.
Concept Introduction:
Electronic configuration: The electronic configuration is the distribution of electrons (e-) of an given molecule or respective atoms in atomic or molecular orbital’s.
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.
Quantum numbers: These terms are explained for the distribution of electron density in an atom. They are derived from the mathematical solution of Schrodinger’s equation for the hydrogen atom. The types of quantum numbers are the principal quantum number (n), the angular momentum quantum number (l), the magnetic quantum number (ml) and the electron spin quantum number (ms). Each atomic orbital in an atom is categorized by a unique set of the quantum numbers.
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Chapter 7 Solutions
Bundle: Chemistry & Chemical Reactivity, Loose-Leaf Version, 9th + OWLv2, 4 terms (24 Months) Printed Access Card
- A neutral atom has two electrons with n = 1, eight electrons with n = 2, eight electrons with n = 3, and two electrons with n = 4. Assuming this element is in its ground state, supply the following information:(a) atomic number(b) total number of s electrons(c) total number of p electrons(d) total number of d electrons(e) Is the element a metal, metalloid, or nonmetal?arrow_forwardA neutral atom has two electrons with n = 1, eight electrons with n = 2, eight electrons with n = 3, and two electrons with n = 4. Assuming this element is in its ground state, supply the following information: a.atomic number b.total number of s electrons c.total number of p electrons d.total number of d electrons e.Is the element metal, metalloid, or nonmetal?arrow_forwardGive the number of electrons in the sublevel of 6p in lead?arrow_forward
- The figure attached here is a representationof 50 atoms of a fictitiouselement with the symbol Ntand atomic number 120. Nt hasthree isotopes represented by thefollowing colors: Nt-304 (red),Nt-305 (blue), and Nt-306 (green)arrow_forwardwhat group in the periodic table would an element with atomic number 112 belong?arrow_forwardWhich subatomic particle has a negative (-1) charge?arrow_forward
- Which of the following is False?a. An element is defined by its atomic number.b. Ninety-two elements occur naturally.c. An atom consists of subatomic particles.d. Electron shells increase in energy closer to the nucleus.arrow_forwardThe element with atomic number 38, strontium (Sr), can be found in what period of the periodic table?arrow_forwardHow do I tell if S2- is the most common isotope ? and what are difference between a Bohr-Rutherford diagram and a real anion ?arrow_forward
- Please do question 6a and if you to ptable.com you will see the periodic table… please dont return the questionarrow_forwardWhat is one way to describe the modern understanding of the location of electrons in an atom?arrow_forward7. Which of the following sets of numbers could be used to designate the principal energy levels (shells) in an atom?arrow_forward
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