Textbook Question
(a) If you combine two atomic orbitals on two different atomsto make a new orbital, is this a hybrid orbital or a molecularorbital?
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 71b
Consider the H2+ ion. (b) How many electrons are there in the H2+ ion?
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Identify the composition of a neutral hydrogen molecule (H2). A neutral H2 molecule consists of two hydrogen atoms.
Recognize that each hydrogen atom in its neutral state has one electron. Therefore, a neutral H2 molecule has a total of two electrons.
Understand that the '+' sign in H2+ indicates the loss of one electron from the neutral H2 molecule.
Subtract one electron from the total number of electrons in the neutral H2 molecule to account for the positive charge in H2+.
Conclude that the H2+ ion, having lost one electron, contains one electron.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Ions
Molecular ions are charged species formed when molecules gain or lose electrons. In the case of H2+, the ion is formed from two hydrogen atoms (H) that share a pair of electrons, but one electron is removed, resulting in a positive charge. Understanding how molecular ions are formed is crucial for determining their electron count.
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Ion Formation
Electron Count in Ions
The electron count in an ion is determined by the number of electrons present in the neutral atom or molecule minus the number of electrons lost or plus the number gained. For H2+, which is derived from two neutral hydrogen atoms (each having one electron), the removal of one electron leads to a total of one electron remaining in the ion.
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Atomic Structure of Hydrogen
Hydrogen is the simplest element, consisting of one proton and one electron in its neutral state. When considering the H2+ ion, it is essential to recognize that each hydrogen atom contributes one electron, and the overall structure of the ion is influenced by the interactions between the two hydrogen nuclei and the remaining electron. This understanding aids in visualizing the ion's formation and electron configuration.
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Related Practice
Textbook Question
(b) If you combine two atomic orbitals on one atom to make a new orbital, is this a hybrid orbital or a molecular orbital?
Textbook Question
Consider the H2+ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.
Textbook Question
Consider the H2+ ion. (c) Write the electron configuration of the ion in terms of its MOs. (d) What is the bond order in H2+?
Textbook Question
Consider the H2+ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H2+ ion to be stable or to fall apart?
Textbook Question
Consider the H2+ ion. (f) Which of the following statements about part (e) is correct: (i) The light excites an electron from a bonding orbital to an antibonding orbital, (ii) The light excites an electron from an antibonding orbital to a bonding orbital, or (iii) In the excited state there are more bonding electrons than antibonding electrons?