(a)
Interpretation:
The reason for the
(a)
Explanation of Solution
Electron affinity is the energy required to add an electron to the neutral atom.
The electronic configuration of neutral selenium and selenium anion is written as follows:
The electronic configuration of neutral bromine and bromine anion is written as follows:
Addition of one electron to bromine gives a noble gas configuration. Hence, it is very stable. So, selenium has lower electron affinity than bromine.
(b)
Interpretation:
The reason for the first ionization energy of aluminum being lower than that of magnesium has to be explained using electron configurations.
(b)
Explanation of Solution
The ionization energy is the energy required to remove the outermost electron in an atom.
The electronic configuration of neutral aluminum and aluminum cation is written as follows:
The electronic configuration of neutral magnesium and magnesium cation is written as follows:
The magnesium atom has all subshells filled. So, removing an electron requires more energy. Hence, aluminum has lower first ionization energy than magnesium.
(c)
Interpretation:
The reason for the first ionization energy of sulfur being lower than that of phosphorus has to be explained using electron configurations.
(c)
Explanation of Solution
The ionization energy is the energy required to remove the outermost electron in an atom.
The electronic configuration of neutral sulfur and sulfur cation is written as follows:
The electronic configuration of neutral phosphorus and phosphorus cation is written as follows:
The phosphorus atom has half-filledp-subshell. So, removing an electron requires more energy. Hence, sulfur has lower first ionization energy than phosphorus.
(d)
Interpretation:
The reason for the first ionization energy of bromine being lower than that of chlorine has to be explained using electron configurations.
(d)
Explanation of Solution
The ionization energy is the energy required to remove the outermost electron in an atom.
The electronic configuration of neutral bromine and bromine cation is written as follows:
The electronic configuration of neutral chlorine and chlorine cation is written as follows:
The electron removed from chlorine is from
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Chapter 5 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- (a) Describe the trends of atomic size and ionization energy, respectively, in the Periodic Table: (1) from left to right across a period, and (ii) from top to bottom down a group. (b) Rank the following elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization energy, and (iii) reactivity. (c) Rank the following elements: F, CI, Br and I, in increasing order of: (i) atomic size; (ii) electron affinity, (iii) electronegativity, and (iv) reactivity.arrow_forwardIdentify each statement as true or false: (a) Ionization energiesare always negative quantities. (b) Oxygen has a larger firstionization energy than fluorine. (c) The second ionization energy of an atom is always greater than its first ionizationenergy. (d) The third ionization energy is the energy neededto ionize three electrons from a neutral atom.arrow_forward(a) Identify the number of electrons in the ground-state outer shell of atomic oxygen (atomic number 8).(b) How many electrons are in the ground-state outer shell of fluorine?arrow_forward
- Identify each statement as true or false: (a) Ionization energiesare always negative quantities. (b) Oxygen has a larger firstionization energy than fluorine. (c) The second ionizationenergy of an atom is always greater than its first ionizationenergy. (d) The third ionization energy is the energy neededto ionize three electrons from a neutral atom.arrow_forwardGive the shell electron configuration for the following. (For example, the shell electron configuration of lithium is written 2,1.) (a) argon (b) magnesiumarrow_forwardArrange in order of increasing atomic size. (a) the period 3 elements Cl, Na, and Ar (b) the Group 2A elements Ca, Be, and Mgarrow_forward
- Which of the following chemical equations is connected tothe definitions of (a) the first ionization energy of oxygen,(b) the second ionization energy of oxygen, and (c) the electronaffinity of oxygen?(i) O(g) + e------>O-(g) (ii) O(g)---->O+(g) + e-(iii) O(g) + 2 e------->O2-(g) (iv) O(g)----->O2+(g) + 2 e-(v) O+(g)----->O2+(g) + e-arrow_forwardIdentify the true statements concerning the atoms andions of the group 6A elements. (a) The ionic radii are larger than the atomic radii becausethe ions have more electrons than their correspondingatoms.(b) Atomic radii increase going down the group because ofincreasing nuclear charge.(c) The ionic radii increase going down the group becauseof the increase in the principal quantum number ofoutermost electrons.(d) Of these ions, Se2- is the strongest base in water becauseit is largest.arrow_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_forward
- (a) Rank elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization energy, and (iii) reactivity. (b) Explain why atomic size decreases from left to right, but increases from top to bottom; (c) Explain why ionization energy increases from left to right, but decreases from top to bottom; (d) Explain why the reactivity of alkali metals (Group-1) increases from top to bottom, where as the reactivity of halogen (Group-17) decreases from top to bottom.arrow_forwardchoose three . What are the characteristerses of a metal like element? (a) they try to get additional electrons (b) they are melleable. (c) they are lightly to give away or share electrons. (d) they are good conductors of electricityarrow_forward(a) Why do successive IEs of a given element always increase? (b) When the difference between successive IEs of a given element is exceptionally large (for example, between IE1 and IE2 of K), what do we learn about its electron configuration? (c) The bars represent the relative magnitudes of the first five ionization energies of an atom: Identify the element and write its complete electron config uration, assuming it comes from (a) Period 2; (b) Period 3; (c) Period 4.arrow_forward
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