Concept explainers
Interpretation:
The largest and the smallest ion from the given 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
- 2-89 Assume that a new element has been discovered with atomic number 117. Its chemical properties should be similar to those of astatine (At). Predict whether the new element’s ionization energy will be greater than, the same as, or smaller than that of: (a)At (b)Raarrow_forward2-64 Consider the elements B, C, and N. Using only the Periodic Table, predict which of these three elements has: (a) the largest atomic radius. (b) the smallest atomic radius. (c) the largest ionization energy (d) the smallest ionization energyarrow_forward2-59 You are presented with a Lewis dot structure of element X as X.. To which two groups in the Periodic Table might this element belong?arrow_forward
- 2-47 Which element in each pair is more metallic? (a) Silicon or aluminum (b) Arsenic or phosphorus (c) Gallium or germanium (d) Gallium or aluminumarrow_forwardHow many protons(p), neutrons(n), and electrons(e) does the following ion have? P3- Group of answer choices 31p, 15n, 15e 15p, 16n, 18e 15p, 16n, 12e 15p, 16n, 15earrow_forwardWhich of the following contains sets of atoms or ions that are isoelectronic? Answer(s): ________________ a. B+3 , C+4, H+, He b. Na+, Ne, N+3, O-2 c. Mg+2, F-, Na+, O-2 d. Ne, Ar, Xe, Kr e. O-2, S-2, Se-2, Te-2 f. None of the choices.arrow_forward
- I think you made a mistake for all the answers for example in the first paragraph of your answer ,the last sentence ''For example, if the noble gas is helium (He), the configuration would represent the group 13 element nitrogen (B): [He] 2s²2p¹.'' you have mentioned nitrogen as (B) , how is nitrogen be (B). similar clarification is needed for the second paragraph , you mentioned 'chromium (Ga): [Ar] '' and for third paragraph you mentioned '' Vanadium (V): [Ar]''arrow_forwardAre the following statements correct? If not, fix it Barium adopts a “-1” charge in chemical reactionsarrow_forwardWhich of the following has the element and the correct expected charge when its an ion? Element Expected Ion Charge 1. S -2 2. Al -5 3. P +3 4. K +1 Group of answer choices 1 and 4 2 and 3 1 and 3 3 and 4arrow_forward
- what 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_forwardAmong Cl-, Ar, K+, Ca2+, Br-, Kr, Rb+, and Sr2+, which one has the largest radius? Question H:Among Cl-, Ar, K+, Ca2+, Br-, Kr, Rb+, and Sr2+, which one has the largest ionization energy? Question I:When H+(aq) reacts with Fe(s) to produce Fe2+(aq) and hydrogen gas, is H+(aq) an acid, base, oxidizing agent, or reducing agent? Question J:What is the oxidation state of the C atoms in C6H12O3? Question K:arrow_forward2-98 Explain how the ionization energy of atoms changes when proceeding down a group of the Periodic Table and explain why this change occurs.arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co