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.
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Chemistry: Atoms First
- Question:Consider an atom X with an atomic number of 79, and another atom Y with an atomic number of 78. Identify atoms X and Y and describe their location in the periodic table.What differences would you expect between the two in terms of their periodic properties, such as atomic radius, ionization energy, and electron affinity?Predict and provide a reason for which atom is more likely to form a positive ion.arrow_forwardWhich of the following answers is true to describe the general trend for Ionization Energy for the Periodic Table? Group of answer choices Decreases from top to bottom within a group, Decreases from left to right across a period (row) Decreases from top to bottom within a group, Increases from left to right across a period (row) Increases from top to bottom within a group, Decreases from left to right across a period (row) Increases from top to bottom within a group, Increases from left to right across a period (row)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
- why is there no element to the immediate right of magnesium in the periodic tablearrow_forwardRank the following elements according to their ionization energy. element fluorine tin oxygen tellurium ionization energy X (Choose one) (Choose one) (Choose one) (Choose one) Śarrow_forwardWhich elements would be found in the alkaline earth metals family? [Select all that apply] cesium sodium O zinc O calcium O bariumarrow_forward
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- 56. Refer to the periodic table and write the predicted electron configuration for each of the following elements. (a) B (c) Na (e) Ge (b) Ti (d) O (f) Ba (h) Kr (g) Pdarrow_forwardRank the following elements according to their ionization energy. element bromine arsenic bismuth thallium ionization energy (Choose one) (Choose one) (Choose one) (Choose one) x Śarrow_forwardQuestion:Consider the following elements from the periodic table: element X with atomic number 12 and element Y with atomic number 17. Element X belongs to Group 2, while Element Y belongs to Group 17 (Group 7A). Both elements exist as neutral atoms. Determine the electron configuration of each element and explain why element X is more reactive than element Y.arrow_forward
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