Ch.9 - Molecular Geometry and Bonding Theories

Problem 71b

Chapter 9, Problem 71b

Consider the H2+ ion. (b) How many electrons are there in the H2+ ion?

Verified step by step guidance

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.

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

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.

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.

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.

Recommended video:

Guided course

02:10

Atom Structure

Related Practice

Textbook Question

What hybridization do you expect for the atom indicated in red in each of the following species? (a) CH3CO2-

views

Textbook Question

Which of the following statements about molecular orbitals and hybrid orbitals are true?

a. Molecular orbitals and hybrid orbitals are both created by mathematically mixing the wave functions of atomic orbitals.

b. Molecular orbitals are made by combining atomic orbitals from different atoms.

c. Hybrid orbitals and molecular orbitals are different names for the same things.

d. A hybrid orbital can hold more electrons than can a molecular orbital.

views

Textbook Question

Consider the H2+ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.

886

views

Textbook Question

Consider the H2+ ion. (d) What is the bond order in H2+?

882

views

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?

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 bond order of the ion does not change when an electron is excited, or iii. In the excited state there are more bonding electrons than antibonding electrons?

views