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Chapter 8: Problem 16

(a) Use Lewis symbols to represent the reaction that occurs between Ca and F atoms. (b) What is the chemical formula of the most likely product? (c) How many electrons are transferred? ( \(\mathbf{d} )\) Which atom loses electrons in the reaction?

Short Answer

Expert verified
(a) The reaction between Ca and F using Lewis symbols is represented as: \[ \underset{\displaystyle .}{\text{Ca}} + 2 \underset{\displaystyle :.}{\text{F}} \rightarrow \text{Ca}^{2+} + 2 \text{F}^{-} \] (b) The chemical formula of the most likely product is CaF2. (c) A total of 2 electrons are transferred during the reaction. (d) The Calcium atom (Ca) loses electrons in the reaction.

Step by step solution

01

Determine the Lewis symbols for Ca and F

First, let's determine the Lewis symbols for calcium (Ca) and fluorine (F) atoms. The Lewis symbol of an atom represents its valence electrons as dots surrounding the chemical symbol. Calcium has 2 valence electrons and fluorine has 7 valence electrons. \[ \text{Ca:} \: \: \: \underset{\displaystyle .}{\text{Ca}} \] \[ \text{F:} \: \: \: \underset{\displaystyle :.}{\text{F}} \]
02

Determine the reaction between Ca and F using Lewis symbols

Calcium has 2 valence electrons that can be lost to achieve a stable noble gas configuration, and fluorine needs 1 more electron to achieve a stable noble gas configuration. Therefore, one calcium atom can react with two fluorine atoms to form an ionic compound. In this reaction, calcium loses 2 electrons, and each fluorine atom gains 1 electron. Here's the representation of the reaction using Lewis symbols (the arrows indicate electron transfer): \[ \underset{\displaystyle .}{\text{Ca}} + 2 \underset{\displaystyle :.}{\text{F}} \rightarrow \text{Ca}^{2+} + 2 \text{F}^{-} \] #a)# The representation of the reaction using Lewis symbols is shown above.
03

Determine the chemical formula of the product

The product of this reaction is an ionic compound formed between calcium ion (Ca虏鈦�) and two fluoride ions (2F鈦�). The chemical formula of the product is: \( \text{CaF}_2 \) #b)# The chemical formula of the most likely product is CaF鈧�.
04

Determine the number of electrons transferred

One calcium atom loses 2 electrons, and each of the two fluorine atoms gains 1 electron. Therefore, a total of 2 electrons are transferred during the reaction. #c)# 2 electrons are transferred in the reaction.
05

Identify which atom loses electrons

In this reaction, the calcium atom loses 2 electrons to form the Ca虏鈦� ion. #d)# Calcium (Ca) loses electrons in the reaction.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Bonding
Understanding chemical bonding is fundamental to performing any chemical reaction. Bonds are the connections between atoms that allow the formation of chemical substances that contain two or more atoms. The type of bond mainly depends on the elements involved and their electron configurations.

There are three primary types of chemical bonding:
  • Covalent bonding where atoms share electrons.
  • Ionic bonding which involves the transfer of electrons from one atom to another.
  • Metallic bonding found in metals, where electrons are free to move around.

In our exercise, the focus is on ionic bonding, which occurs when a metal (in this case, calcium) gives up electrons to a non-metal (fluorine), resulting in positively and negatively charged ions that attract each other. This attraction forms the ionic bond and the resulting ionic compound, CaF2.
Ionic Compounds
Ionic compounds are substances composed of ions bound together by electrostatic forces termed ionic bonding. An ion is an atom or molecule that has lost or gained one or more electrons, giving it a net positive or negative charge. Ionic compounds typically form between metals and nonmetals, where metals tend to lose electrons and nonmetals tend to gain electrons.

Characteristics of ionic compounds include:
  • High melting and boiling points due to the strong attraction between cations and anions.
  • Electrical conductivity when dissolved in water or melted, as ions are free to move.
  • Brittle nature, as any displacement of ions can disrupt the crystal lattice, causing the material to break.

The product of the chemical reaction in our example is calcium fluoride, CaF2, an ionic compound where a calcium atom has transferred its two electrons to two fluorine atoms, achieving stable electron configurations for both.
Electron Transfer
Electron transfer is the process of moving electrons from one atom to another during a chemical reaction, transforming the oxidation state of the atoms. This transfer is fundamental in the formation of ionic bonds.

In the given exercise, we've observed that:
  • Calcium (Ca), a metal, is willing to give up its two valence electrons to achieve a noble gas electron configuration.
  • Fluorine (F), a non-metal, is eager to accept one electron to complete its valence shell to also reach a noble gas electron configuration.

With the transfer of two electrons from calcium to the two fluorine atoms:
  • Calcium becomes a cation, Ca2+.
  • Each fluorine atom becomes an anion, F-.

Thus establishing a classic ionic bond through electron transfer. In terms of the number of electrons transferred in our example, a total of two electrons were moved from calcium to the two fluorine atoms鈥攃onfiguring the formula CaF2 for calcium fluoride.

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Most popular questions from this chapter

(a) Describe the molecule xenon trioxide, \(\mathrm{XeO}_{3},\) using four possible Lewis structures, one each with zero, one, two, or three \(\mathrm{Xe}-\mathrm{O}\) double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in part (a) yields the most favorable formal charges for the molecule?

Which of the following statements about electronegativity is false? (a) Electronegativity is the ability of an atom in a molecule to attract electron density toward itself. (b) Electronegativity is the same thing as electron affinity. (c) The numerical values for electronegativity have no units. (d) Fluorine is the most electronegative element. (e) Cesium is the least electronegative element.

The substance chlorine monoxide, ClO(g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of \(1.24 \mathrm{D},\) and the \(\mathrm{Cl}-\) O bond length is 1.60 \(\mathrm{A}\) . (a) Determine the magnitude of the charges on the Cl and O atoms in units of the electronic charge, \(e\) (b) Based on the electronegativities of the elements, which atom would you expect to have a partial negative charge in the Clo molecule? (c) Using formal charges as a guide, propose the dominant Lewis structure for the molecule. (d) The anion \(\mathrm{ClO}^{-}\) exists. What is the formal charge on the Cl for the best Lewis structure for \(\mathrm{ClO}^{-}\) ?

We can define average bond enthalpies and bond lengths for ionic bonds, just like we have for covalent bonds. Which ionic bond is predicted to have the smaller bond enthalpy, Li-F or \(\mathrm{Cs}-\mathrm{F}\) ?

Although \(\mathrm{I}_{3}\) is a known ion, \(\mathrm{F}_{3}^{-}\) is not. (a) Draw the Lewis structure for \(\mathrm{I}_{3}^{-}\) (it is linear, not a triangle). (b) One of your classmates says that \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{Fis}\) too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because it would violate the octet rule. Is this classmate possibly correct? (d) Yet another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too small to make bonds to more than one atom. Is this classmate possibly correct?
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