Interpretation: The possible orbitals in an atom should be determined.
Concept Introduction: The distribution of electrons in an atom is described by the use of quantum numbers used by the
The forth quantum number is spin quantum number which is denoted by symbol s and determined the spin of the electron if it is clockwise or anticlockwise.
The all four quantum numbers are explained in detail as follows:
Principal quantum number (n) determines the size of the orbital. The orbital with principal quantum number 2 is larger than the value 1. This also determines the energy of the orbital, as the value of n increases the energy of the orbital increases as its distance from the nucleus increases.
Angular quantum number (l) determined the shape of the orbital. For
The rules for the allowed quantum numbers combinations are as follows:
- All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
- The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
- The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
- The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2
lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.
Here, for s orbital value of
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
EBK BASIC CHEMISTRY
- Consider three elements with the following abbreviatedelectron configurations: (5.4, 5.5, 5.6)X = [Ar]4s23d5 Y = [Ar]4s23d104p1 Z = [Ar]4s23d104p6a. Identify each element as a metal, nonmetal, or metalloid.b. Which element has the smallest atomic size?c. Which element has the highest ionization energy?d. Which element has a half-filled sublevel?arrow_forward(9.3, 9.4)Identify the element with the ground state electron configuration of [Ar]4s23d¹04p³. O antimony iron tin arsenicarrow_forward28. Completely describe the orbitals found in the fourth energy level. How many electrons can be found in a full fourth energy level? Give an example of an element that has its valence electrons in the fourth energy level. (3.3) K/Uarrow_forward
- Discussion 6 - week 6 Electron Configuration, Periodic Trends (4.7, 4.8), and Nuclear Chemistry (5.1) Part 1: Electron Configurations and Orbital Diagrams of Atoms (4.7, 4.8) 1. Write the abbreviated (short-hand) electron configuration and draw the orbital diagrams for the following ground-state (lowest energy) neutral atoms: A. Sodium (Na) B. Sulfur (S) C. Krypton (Kr) D. Vanadium (V)arrow_forwardWrite the abbreviated electron configuration and group numberfor each of the following elements: (5.4)a. Zn b. I c. V d. Srarrow_forward4. If you were given an antique piece of jewelry and you were told that it was made of solid gold, how could you devise a test to indicate that it was actually made of gold? 6,7.5arrow_forward
- 5.96 a. Si b. Se c. Mn d. Sb Write the abbreviated electron configuration and group number for each of the following elements: (5.4) a. Br b. Rh c. Tc d. Raarrow_forward(9.6) Which of the following is in the correct order of increasing atomic radius? O Cs > S > Si Cs > Si > S OS > Si > Cs O Si > S > Csarrow_forwardThe most prevalent isotope of gold is Au-197. (4.5)a. How many protons, neutrons, and electrons are in this isotope?b. What is the atomic symbol of another isotope of gold with 116 neutrons?c. What is the atomic symbol of an atom with an atomic number of 78 and 116 neutrons?arrow_forward
- 4.82 For each of the following, write the symbol and name for X and the number of protons and neutrons. Which are isotopes of each other? (4.4, 4.5) a. 124x A 47 b. 16x 116x 49 C. 50 d. 124x 50 116X e. 48arrow_forward6.9.2 What element is represented by the following electronarrow_forwardMendeleev used chemical reactivity to determine how to organize the elements of the periodic table into groups and periods. Based on this knowledge, explain why his first table did not include the noble gases. (2 pts) Barrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY