menu
bartleby
search
close search
Hit Return to see all results
close solutoin list

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?

BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

Solutions

Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 7, Problem 41GQ
Textbook Problem
381 views

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:

  1. (a) atomic number
  2. (b) total number of s electrons
  3. (c) total number of p electrons
  4. (d) total number of d electrons
  5. (e) Is the element a metal, metalloid, or nonmetal?

a)

Interpretation Introduction

Interpretation:

The atomic number for n =1, 2, and 4 has to be determined.

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.

Explanation of Solution

Given: Presence of (n) shells having 18 electrons in each shells

The term ‘n’ indicates the principle quantum number.

  • For n =1, the first principle shell contains only s-orbital represented as 1s and the orbital contains given two electrons that represented as 1s2.
  • For n = 2, the second principle shell contains both s-orbital and p-orbital represented as 2s and 2p the orbital contains given eight electrons that represented as 2s22p6.
  •  For n =3, the third principle shell contains s-orbital p-orbital and d-orbital represented as 3s, 3p and 3d ; the orbital contains given eight electrons that represented as 3s23p63d0

b)

Interpretation Introduction

Interpretation:

The total number of s-electrons in 1s22s22p63s23p64s2 has to be determined.

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 Introduction

Interpretation:

The total number of p-electrons in 1s22s22p63s23p64s2 has to be determined.

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 Introduction

Interpretation:

The total number of p-electrons in 1s22s22p63s23p64s2 has to be determined.

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 Introduction

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.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Chapter 7 Solutions

Chemistry & Chemical Reactivity
Show all chapter solutions
add
Ch. 7.4 - 2. Which of the following ions has the largest...Ch. 7.4 - Which of the following species is most...Ch. 7.5 - Without looking at the figures for the periodic...Ch. 7.5 - What is the trend in sizes of the ions K+, S2, and...Ch. 7.5 - Locate the elements C, N, Si, and P in the...Ch. 7.6 - Give the electron configurations for iron and the...Ch. 7.6 - In hemoglobin, iron can be in the iron(II) or...Ch. 7.6 - Why are copper atoms (radius = 128 pm) slightly...Ch. 7.6 - In hemoglobin, the iron is enclosed by the...Ch. 7.6 - 1. Which of the following is an incorrect...Ch. 7.6 - 2. Which of the following is not the formula for a...Ch. 7.6 - The most common oxidation state of a rare earth...Ch. 7.6 - This textbook places lanthanum directly below...Ch. 7.6 - Gadolinium has eight unpaired electrons, the...Ch. 7.6 - Use the atomic radii of scandium, yttrium,...Ch. 7.6 - Europium oxide (Eu2O3) is used in the production...Ch. 7.6 - Neodymium is commonly used in magnets, usually as...Ch. 7 - Write the electron configurations for P and CI...Ch. 7 - Write the electron configurations for Mg and Ar...Ch. 7 - Using spdf notation, write the electron...Ch. 7 - Using spdf notation, give the electron...Ch. 7 - Depict the electron configuration for each of the...Ch. 7 - Using spdf and noble gas notations, write electron...Ch. 7 - Use noble gas and spdf notations to depict...Ch. 7 - The lanthanides, once called the rare earth...Ch. 7 - Americium, Am, is a radioactive element isolated...Ch. 7 - Predict electron configurations for the following...Ch. 7 - What is the maximum number of electrons that can...Ch. 7 - What is the maximum number of electrons that can...Ch. 7 - Depict the electron configuration for magnesium...Ch. 7 - Depict the electron configuration for phosphorus...Ch. 7 - Using an orbital box diagram and noble gas...Ch. 7 - Using an orbital box diagram and noble gas...Ch. 7 - Using orbital box diagrams, depict an electron...Ch. 7 - Using orbital box diagrams, depict an electron...Ch. 7 - Using orbital box diagrams and noble gas notation,...Ch. 7 - Using orbital box diagrams and noble gas notation,...Ch. 7 - Manganese is found as MnO2 in deep ocean deposits....Ch. 7 - One compound found in alkaline batteries is NiOOH,...Ch. 7 - Arrange the following elements in order of...Ch. 7 - Arrange the following elements in order of...Ch. 7 - Select the atom or ion in each pair that has the...Ch. 7 - Select the atom or ion in each pair that has the...Ch. 7 - Which of the following groups of elements is...Ch. 7 - Arrange the following atoms in order of increasing...Ch. 7 - Compare the elements Na, Mg, O, and P. (a) Which...Ch. 7 - Compare the elements B. Al, C, and Si. (a) Which...Ch. 7 - Explain each answer briefly. (a) Place the...Ch. 7 - Explain each answer briefly. (a) Rank the...Ch. 7 - Identify the element that corresponds to each of...Ch. 7 - Identify the element that corresponds to each of...Ch. 7 - Explain why the photoelectron spectra of hydrogen...Ch. 7 - Sketch the major features (number of peaks and...Ch. 7 - These questions are not designated as to type or...Ch. 7 - The deep blue color of sapphires comes from the...Ch. 7 - Using an orbital box diagram and noble gas...Ch. 7 - The rare earth elements, or lanthanides, commonly...Ch. 7 - A neutral atom has two electrons with n = 1, eight...Ch. 7 - Element 109, now named meitnerium (in honor of the...Ch. 7 - Which of the following is not an allowable set of...Ch. 7 - A possible excited state for the H atom has an...Ch. 7 - The magnet in the following photo is made from...Ch. 7 - Name the element corresponding to each...Ch. 7 - Arrange the following atoms in order of increasing...Ch. 7 - Rank the following in order of increasing...Ch. 7 - Answer the questions below about the elements A...Ch. 7 - Answer (he following questions about the elements...Ch. 7 - Which of the following ions are unlikely to be...Ch. 7 - Place the following ions in order of decreasing...Ch. 7 - Answer each of the following questions: (a) Of the...Ch. 7 - The following are isoelectronic species: Cl, K+,...Ch. 7 - Compare the elements Na. B. Al, and C with regard...Ch. 7 - Two elements in the second transition series (Y...Ch. 7 - The configuration for an element is given here....Ch. 7 - The configuration of an element is given here. (a)...Ch. 7 - Answer the questions below about the elements A...Ch. 7 - Answer the questions below concerning ground state...Ch. 7 - Nickel(II) formate [Ni(HCO2)2] is widely used as a...Ch. 7 - Spinets are solids with the general formula M2+...Ch. 7 - The following questions use concepts from this and...Ch. 7 - Which ions in the following list are not likely to...Ch. 7 - Answer the following questions about first...Ch. 7 - The ionization of the hydrogen atom can be...Ch. 7 - Compare the configurations below with two...Ch. 7 - The bond lengths in Cl2, Br2, and I2 are 200, 228,...Ch. 7 - Write electron configurations to show the first...Ch. 7 - What is the trend in ionization energy when...Ch. 7 - (a) Explain why the sizes of atoms change when...Ch. 7 - Which of the following elements has the greatest...Ch. 7 - What arguments would you use to convince another...Ch. 7 - Explain why the first ionization energy of Ca is...Ch. 7 - The energies of the orbitals in many elements have...Ch. 7 - The ionization energies for the removal of the...Ch. 7 - Using your knowledge of the trends in element...Ch. 7 - The densities (in g/cm3) of elements in Croups 6B,...Ch. 7 - The discovery of two new elements (atomic numbers...Ch. 7 - Explain why the reaction of calcium and fluorine...Ch. 7 - Thionyl chloride. SOCl2, is an important...Ch. 7 - Sodium metal reacts readily with chlorine gas to...Ch. 7 - Slaters rules are a way to estimate the effective...

Additional Science Textbook Solutions

Find more solutions based on key concepts
Show solutions add
B vitamins often act as: a. antioxidants. b. blood clotting factors. c. coenzymes. d. none of the above.

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

2. Describe an atom.

Chemistry In Focus

What does the oceans density stratification have to do with biogeochemical cycles?

Oceanography: An Invitation To Marine Science, Loose-leaf Versin

Two 2.00 103-kg cars both traveling at 20.0 m/s LLU undergo a head-on collision and stick together. Find the c...

Physics for Scientists and Engineers, Technology Update (No access codes included)