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.
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Chemistry: Atoms First
- 2-98 Explain how the ionization energy of atoms changes when proceeding down a group of the Periodic Table and explain why this change occurs.arrow_forwardWrite the electron configuration for each of the following ions. (a) Sb3−Write the electron configuration for each of the following ions. (a) Sb^3− (b) Tl+ (c) Se2− (d) Si4+ (e) Cr6+arrow_forwardPick out a pair of species that are isoelectronic. (a) C and N (b) Mg2+ and Ne (c) F and O+ (d) S2- and Parrow_forward
- (b) A new element, "X", is discovered and found to have 2 electrons in its outer level. Is X a metal or non-metal? Predict the formula its ion would have in any ionic compounds it forms.arrow_forwardHow many inner, outer, and valence electrons are present in an atom of each of the following elements?(a) O(b) Sn(c) Ca(d) Fe(e) Searrow_forwardArrange in order of increasing nonmetallic character. (a) the period 4 elements Ga, Ge, Ti (b) the Group 5A elements P, Bi, and Narrow_forward
- Question A11 (a) Write the full electronic configuration of Cu, using s,p,d,f notation. (b) Complete the table below: Atom/Ion 64 Ni2+ 28 Proton Neutrons Electrons (c) Predict whether Na or Cl has the more stable 1s² shell and explain your rationale. (d) What three factors can influence the Ionization energy of group 2 elements?arrow_forwardHow many inner, outer, and valence electrons are present inan atom of each of the following elements?(a) Br(b) Cs(c) Cr(d) Sr(e) Farrow_forwardvi. Answer true or false. (a) Elements in the same column of the Periodic Table have the same outer-shell electron configuration. (b) All Group 1A elements have one electron in their valence shell. (c) All Group 6A elements have six electrons in their valence shell. (d) All Group 8A elements have eight electrons in their valence shell. (e) Period 1 of the Periodic Table has one element, period 2 has two elements, period 3 has three elements, and so forth. (1) Period 2 results from filling the 2s and 2p orbitals and, therefore, there are eight elements in period 2. (g) Period 3 results from filling the 3s, 3p, and 3d orbitals and, therefore, there are nine elements in period 3. (h) The main-group elements are s block and p block elements.arrow_forward
- Predict the larger ion in each of the following pairs. (a) Rb+ or Sr2+ _________rubidium ion or strontium ion (b) Co2+ or Co3+ _________cobalt(II) ion or cobalt(III) ion (c) S- or S2- _________sulfur -1 ion or sulfide ion (d) Br- or I- _________bromide ioniodide ionarrow_forwardQ1. This question is about atomic structure. (a) Write the full electron configuration for each of the following species. CH Fe2+ (b) Write an equation, including state symbols, to represent the process that occurs when the third ionisation energy of manganese is measured. (c) State which of the elements magnesium and aluminium has the lower first ionisation energy Explain your answer. (d) A sample of nickel was analysed in a time of flight (TOF) mass spectrometer. The sample was ionised by electron impact ionisation. The spectrum produced showed three peaks with abundances as set out in the table. m/z Abundance /% 58 61.0 60 29.1 61 9.9 Give the symbol, including mass number, of the ion that would reach the detector first in the sample. Calculate the relative atomic mass of the nickel in the sample. Give your answer to one decimal place. Page 2 of 12 Symbol of ion Relative atomic massarrow_forwardIn which of the following species is the difference betweenthe number of protons and the number of electrons largest?(a) Ti2+ (b) P3- (c) Mn (d) Se 2- (e) Ce4+arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning