(a)
Interpretation:
The atomic orbital for
Concept Introduction:
Hund’s rule: Each orbital must be singly occupied before any orbital is occupied. All the electrons in singly occupied orbitals have same spin.
(b)
Interpretation:
The atomic orbital for
Concept Introduction:
Hund’s rule: Each orbital must be singly occupied before any orbital is occupied. All the electrons in singly occupied orbitals have same spin.
(c)
Interpretation:
The atomic orbital for
Concept Introduction:
Hund’s rule: Each orbital must be singly occupied before any orbital is occupied. All the electrons in singly occupied orbitals have same spin.
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
Chemistry: The Molecular Science
- (a) Use orbital diagrams to illustrate what happens when anoxygen atom gains two electrons. (b) Why does O3 - not exist?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_forward7. Use an orbital diagram to describe the electron configuration of the valence shell of each of the following atoms: (a) N (b) Si (c) Fearrow_forward
- (1) What is the valence electron configuration for the arsenic atom? (2) What is the valence electron configuration for the fluorine atom?arrow_forwardThe orbital diagram that follows shows the valence electronsfor a 2+ ion of an element. (a) What is the element?(b) What is the electron configuration of an atom of this element?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_forward
- (c) Silicon (Si) is the most common chemical element in today's semiconductor industry. It has an atomic number of 14 and belongs to the Group IV (4) of the periodic table with its most common isotope being Si-29. (i) (ii) (iii) Explain what an isotope is. How many protons and how many neutrons are in the nucleus of this Silicon isotope? What is the electron configuration of Si?arrow_forwardWhen a nonmetal oxide reacts with water, it forms an oxoacid with the same oxidation number as the nonmetal. Give the name and formula of the oxide used to prepare each of these oxoacids: (a) hypochlorous acid; (b) chlorous acid; (c) chloric acid; (d) perchloric acid; (e) sulfuric acid; (f ) sulfurous acid; (g) nitric acid; (h) nitrous acid; (i) carbonic acid; ( j) phosphoric acid.arrow_forwardUsing complete subshell notation (1s^22s^22p^6, and so forth), predict the electron configurations of the following ions. (a) N3– (b) Ca2+ (c) S– (d) Cs2+ (e) Cr2+ (f) Gd3+arrow_forward
- (a) Write the electron configuration for silicon, element 14, in its ground state. (b) How many unpaired electrons does a ground-state silicon atom possess?arrow_forwardFor each pair, identify the orbital in which an electron possesses more energy. (a) 4s or 5s; (b) 5p or 5darrow_forward11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning