Concept explainers
(a)
Interpretation:
Whether
Concept Introduction:
Molecular orbital diagram is a linear combination of atomic orbitals of similar energy and similar symmetry. It is formed by the proper overlap of the atomic orbitals.
There are 3 types of molecular orbitals as follows:
1. Bonding molecular orbital: They are formed by the constructive interference of atomic orbitals and electrons in it stabilize the molecule and are of lesser in energy.
2. Antibonding molecular orbital: This type of orbitals increases the energy of molecule and destabilizes it and weakens the bond between the atoms.
3. Non-bonding molecular orbital: These types of orbitals have energy similar to atomic orbitals that is addition or removal of electron does not change the energy of molecule.
The order of energy in molecular orbital follows two rules as follows:
1. For
2. For atomic number more than 14 order of energy is,
Species with number of unpaired electrons in its subshell is called paramagnetic species.
(b)
Interpretation:
Whether
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Whether
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Chemical Principles: The Quest for Insight
- (i) What is the covalency of N in N2O5 ?(ii) Explain why phosphorus forms pentachloride whereas nitrogen andbismuth do not?arrow_forwardWrite expressions for Ksp for each of the ionic compounds: • • BaSO4 Mn(OH)2arrow_forward(a) Why do stable xenon fluorides have an even number of F atoms? (b) Why do the ionic species XeF₃⁺ and XeF₇⁻ have odd numbers of F atoms? (c) Predict the shape of XeF₃⁺ .arrow_forward
- Which is more reactive, Fe2+ or Fe3+, and why?arrow_forwardTestosterone is an anabolic steroid. The structure of testosterone is shown below. What is the idealised bond angle at the indicated atom (ii) ? Hint: atom (iv) has been completed for you as an example. (iv) bond angle: 109.5°, geometry of the electron pairs: tetrahedral, shape of the bonds: tetrahedral ·····|||I H ····||||I ii ivarrow_forwardConsider the elements O, Ba, Co, Be, Br, and Se. From this list,select the element that (a) is most electronegative, (b) exhibitsa maximum oxidation state of +7, (c) loses an electronmost readily, (d) forms π bonds most readily, (e) is a transitionmetal, (f) is a liquid at room temperature and pressure.arrow_forward
- Which species below will require the most energy for the removal of a valenceelectron?(A) Na+(B) Mg+(C) Ne(D) Al2+arrow_forwardThe first three ionization energies of an element X are 900, 1745, and 14912 kJ·mol–1. What is the most likely formula for the stable ion of X?arrow_forwardGive the electron configuration and the number of unpaired electrons for (a) Sc³⁺; (b) Cu²⁺; (c) Fe³⁺; (d) Nb³⁺arrow_forward
- what is the difference between fe(s) and fe3+ at the atomic level?arrow_forward5. Use Periodic table to answer the following: (a) Which has higher ionization potential Cs or Li? Why? (b) Arrange the following elements in increasing order of valence electrons, Ca, Rb, Br and Xe.arrow_forwardrank the following ions in the order of increasing strength as oxidizing agents: NO3 -1aq2, Ag+1aq2, Cr2O7 2-1aq2.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning