Skip to main content
Pearson+ LogoPearson+ Logo
Ch.8 - Basic Concepts of Chemical Bonding
All textbooksBrown 14th EditionCh.8 - Basic Concepts of Chemical BondingProblem 98c
Chapter 8, Problem 98c

The Ti2+ ion is isoelectronic with the Ca atom. (c) What charge would Ti have to be isoelectronic with Ca2+ ?

Verified step by step guidance
1
Identify the number of electrons in a neutral calcium (Ca) atom. Since calcium is element number 20 on the periodic table, a neutral Ca atom has 20 electrons.
Understand that Ca2+ indicates a calcium ion with a charge of +2, meaning it has lost two electrons compared to the neutral atom. Therefore, Ca2+ has 18 electrons.
Recognize that the Ti2+ ion, having a charge of +2, implies it has lost two electrons from its neutral state. Titanium (Ti) is element number 22 on the periodic table, so a neutral Ti atom has 22 electrons. Thus, Ti2+ has 20 electrons.
To find the charge Ti needs to have the same number of electrons as Ca2+ (18 electrons), calculate how many electrons need to be lost from a neutral Ti atom (22 electrons) to reach 18 electrons.
Determine the charge on the titanium ion when it has lost the calculated number of electrons. This charge will make it isoelectronic with Ca2+.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
3m
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons, resulting in identical electron configurations. For example, the Ti<sup>2+</sup> ion and Ca atom both have 20 electrons, making them isoelectronic. Understanding this concept is crucial for comparing the electronic structures of different elements and ions.
Recommended video:
Guided course
03:03
Amphoteric Species

Charge of Ions

The charge of an ion is determined by the loss or gain of electrons relative to its neutral atom. A positive charge indicates the loss of electrons, while a negative charge indicates the gain. In the case of titanium (Ti), to become isoelectronic with Ca<sup>2+</sup>, which has lost two electrons, Ti must also lose electrons to match the electron count.
Recommended video:
Guided course
01:39
Polyatomic Ion Charges

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For Ti, the neutral atom has an electron configuration of [Ar] 4s<sup>2</sup> 3d<sup>2</sup>. When forming ions, the configuration changes based on the number of electrons lost or gained, which is essential for determining how many electrons Ti must lose to be isoelectronic with Ca<sup>2+</sup>.
Recommended video:
Guided course
01:33
Electron Configuration Example
Related Practice
Textbook Question

An important reaction for the conversion of natural gas to other useful hydrocarbons is the conversion of methane to ethane. 2 CH4(g) → C2H6(g) + H2(g) In practice, this reaction is carried out in the presence of oxygen, which converts the hydrogen produced into water. 2 CH4(g) + 12 O2(g) → C2H6(g) + H2O(g) Use Table 8.3 to estimate H for these two reactions. Why is the conversion of methane to ethane more favorable when oxygen is used? Why is the conversion of methane to ethane more favorable when oxygen is used?

Textbook Question

Two compounds are isomers if they have the same chemical formula but different arrangements of atoms. Use Table 8.3 to estimate H for each of the following gas-phase isomerization reactions and indicate which isomer has the lower enthalpy. (d) Methyl isocyanide → Acetonitrile

Textbook Question

The Ti2 + ion is isoelectronic with the Ca atom. (b) Calculate the number of unpaired electrons for Ca and for Ti2+.

Textbook Question

Consider the molecule C4H5N, which has the connectivity shown below. (a) After the Lewis structure for the molecule is completed, how many s and how many p bonds are there in this molecule?

Textbook Question

(c) Hydrogen peroxide is sold commercially as an aqueous solution in brown bottles to protect it from light. Calculate the longest wavelength of light that has sufficient energy to break the weakest bond in hydrogen peroxide.

Textbook Question

The electron affinity of oxygen is -141 kJ/mol, corresponding to the reaction O(g) + e- → O-(g). The lattice energy of K2O(s) is 2238 kJ/mol. Use these data along with data in Appendix C and Figure 7.10 to calculate the 'second electron affinity' of oxygen, corresponding to the reaction O-(g) + e- → O2-(g)