Interpretation:
The correct options that depict the periodic table which contain elements that form isoelectronic species should be determined.
Concept Introduction:
Periodic Table: The available chemical elements are arranged considering their
In periodic table the horizontal rows are called periods and the vertical column are called group.
In periodic table the horizontal rows are called periods and the vertical column are called group. There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,
Atomic Number: Atomic number of the element is equal to the number of protons present in the nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the
Atomic radius:
Atomic radius is the distance between the atomic nucleus and outermost electron of an atom. From the atomic radius, the size of atoms can be visualized. But there is no specific distance from nucleus to electron, due to electron cloud around the atom does not have well-defined boundary.
The atomic radius follows the trend that it tends to decrease as we move from left to right as the effective nuclear charge increases and the radius tends to increases from top to bottom of the group since shells gets added to the atom.
Cation: Removal of electron from the atom results to form positively charged ion called cation.
Anion: Addition of electron to atom results to form negatively charged ion called anion.
The net charge present in the element denotes the presence or absence of electrons in the element.
Effective nuclear charge: It is the overall positive charge experienced by the outermost electrons present in the atom from the nucleus of the atom.
Screening Effect: The core electrons present near the nucleus shields the outermost electrons (valence electrons) from the charge of the nucleus.
Isoelectronic species: Two species are considered to isoelectronic species if they have equal number of electrons with them.
Want to see the full answer?
Check out a sample textbook solutionChapter 4 Solutions
CHEMISTRY:ATOMS FIRST-W/ACCESS>CUSTOM<
- Practice by drawing the electron configuration notation and orbital notation of the following elements. Then identify if the element is paramagnetic or diamagnetic. 1. ) Oxygen 2.) Neon 3.) Sodium 4. )Phosphorus Thank you!arrow_forwardChoose the atom or ion using a periodic table. Larger atomic radius, P or Sbarrow_forwardBased on the electron configuration below. Determine the element and/or ion that matches the configuration. *Select all that apply. Can have multiple answers or no answers. 1s22s22p63s23p64s23d104p3 As Se P S Se2- Se+arrow_forward
- According to periodic trends, which of the following statements are TRUE? Select all that apply. (THERE'S ONLY 2) Arsenic is smaller than oxygen Chlorine is larger than fluorine Calcium is less electronegative than copper Copper has a lower ionization energy than silverarrow_forwardWhich is always going to be the highest ionization energy? Group of answer choices All Ionization energies are equal. 1st Ionization energy 3rd Ionization Energy 2nd Ionization Energyarrow_forwardwhat do you think is the reason for a decreasing atomic radius within one period? answer choice below a)decreasing metallic character b)decreasing number of neutrons c)increasing number of protons d)increasing electronegativity which of this answers is correct?arrow_forward
- if a sulfur atom gains two electrons the resulting species is ______ (larger/same size/smaller) than a sulfur atom. the resulting species is an ______(anion/cation) and is isoelectronic with a _______ atom (correct element)arrow_forwardPlease I want answer for this question by typing. Many Thanks Atomic size is one of the most important periodic property of elements in the periodic table. Prepare a report on the effect of atomic size on ionization energy, electron affinity, electronegativity and metallic character of elements. (Word Limit 200)arrow_forwardWhich of the following statements is not true? Group of answer choices Elements in the upper right hand corner of the periodic table have the least metallic character. Noble gases tend to have low ionization energies. Nonmetals tend to have high ionization energies. Elements in the lower left hand corner of the periodic table have the greatest metallic character. Metals tend to have low ionization energies.arrow_forward
- Of the elements magnesium, calcium, and barium, whichforms the ion with the largest radius? The smallest? Whatperiodic trend explains this?arrow_forwardPlease type all work Question 8 Explain the error in the following electron configuration for Sr2+, and provide the correct electron configuration. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2arrow_forwardGive typed explanation Select the incorrect periodic trends. There may be more than ine correct answer. Inorganic Chemistry.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning