Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
8th Edition
ISBN: 9781285199030
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Question
Book Icon
Chapter 12, Problem 45CR

(a)

Interpretation Introduction

Interpretation:

The formula of simple binary compound formed by Al and F should be determined.

Concept Introduction :

A binary compound is formed by two different elements usually a metal and a non-metal. A metal atom has the tendency to lose electrons and form positive cations. A non-metal atom has the tendency to gain electrons and form negative anions. Oppositely charged ions are held together by a strong electrostatic force of attraction to form binary compounds.

(a)

Expert Solution
Check Mark

Answer to Problem 45CR

The formula of the binary compound formed by Al and F is AlF3 .

Explanation of Solution

The electronic configuration of aluminum with atomic number 13 is 1s22s22p63s23p1 . Aluminum atom has the tendency to lose three electrons from the valence shell to obtain stable electronic configuration like the nearest inert gas neon. For this reason, aluminum atom loses 3 electrons to form aluminum ion (Al3+) .

The electronic configuration of fluorine with atomic number 9 is 1s22s22p5 . Fluorine atom has the tendency to gain one electron to obtain stable octet structure. For this reason, fluorine atom gains 1 electron to form fluoride ion (F) .

Three fluoride ions combine with one aluminum ion to balance the charge and form a neutral binary compound AlF3 .

(b)

Interpretation Introduction

Interpretation:

The formula of simple binary compound formed by Li and N should be determined.

Concept Introduction :

A binary compound is formed by two different elements usually a metal and a non-metal. A metal atom has the tendency to lose electrons and form positive cations. A non-metal atom has the tendency to gain electrons and form negative anions. Oppositely charged ions are held together by a strong electrostatic force of attraction to form binary compounds.

(b)

Expert Solution
Check Mark

Answer to Problem 45CR

The formula of the binary compound formed by Li and N is Li3N .

Explanation of Solution

The electronic configuration of lithium with atomic number 3 is 1s22s1 . Lithium atom has the tendency to lose one electron from the valence shell to obtain stable electronic configuration like the nearest inert gas helium. For this reason, lithium atom loses 1 electron to form lithium ion (Li+) .

The electronic configuration of nitrogen with atomic number 7 is 1s22s22p3 . Nitrogen atom has the tendency to gain three electrons to obtain stable octet structure. For this reason, nitrogen atom gains 3 electrons to form nitride ion (N3) .

Three lithium ions combine with one nitride ion to balance the charge and form a neutral binary compound Li3N .

(c)

Interpretation Introduction

Interpretation:

The formula of simple binary compound formed by Ca and S should be determined.

Concept Introduction :

A binary compound is formed by two different elements usually a metal and a non-metal. A metal atom has the tendency to lose electrons and form positive cations. A non-metal atom has the tendency to gain electrons and form negative anions. Oppositely charged ions are held together by a strong electrostatic force of attraction to form binary compounds.

(c)

Expert Solution
Check Mark

Answer to Problem 45CR

The formula of the binary compound formed by Ca and S is CaS .

Explanation of Solution

The electronic configuration of calcium with atomic number 20 is 1s22s22p63s23p64s2 . Calcium atom has the tendency to lose two electrons from the valence shell to obtain stable electronic configuration like the nearest inert gas argon. For this reason, calcium atom loses 2 electrons to form calcium ion (Ca2+) .

The electronic configuration of sulfur with atomic number 16 is 1s22s22p63s23p4 . Sulfur atom has the tendency to gain two electrons to obtain stable octet structure. For this reason, sulfur atom gains 2 electrons to form sulfide ion (S2) .

One calcium ion combines with one sulfide ion to balance the charge and form a neutral binary compound CaS .

(d)

Interpretation Introduction

Interpretation:

The formula of simple binary compound formed by Mg and P should be determined.

Concept Introduction :

A binary compound is formed by two different elements usually a metal and a non-metal. A metal atom has the tendency to lose electrons and form positive cations. A non-metal atom has the tendency to gain electrons and form negative anions. Oppositely charged ions are held together by a strong electrostatic force of attraction to form binary compounds.

(d)

Expert Solution
Check Mark

Answer to Problem 45CR

The formula of the binary compound formed by Mg and P is Mg3P2 .

Explanation of Solution

The electronic configuration of magnesium with atomic number 12 is 1s22s22p63s2 . Magnesium atom has the tendency to lose two electrons from the valence shell to obtain stable electronic configuration like the nearest inert gas neon. For this reason, magnesium atom loses 2 electrons to form magnesium ion (Mg2+) .

The electronic configuration of phosphorus with atomic number 15 is 1s22s22p63s23p3 . Phosphorus atom has the tendency to gain three electrons to obtain stable octet structure. For this reason, phosphorus atom gains 3 electrons to form phosphide ion (P3) .

Three magnesium ions combine with two phosphide ions to balance the charge and form a neutral binary compound Mg3P2 .

(e)

Interpretation Introduction

Interpretation:

The formula of simple binary compound formed by Al and O should be determined.

Concept Introduction :

A binary compound is formed by two different elements usually a metal and a non-metal. A metal atom has the tendency to lose electrons and form positive cations. A non-metal atom has the tendency to gain electrons and form negative anions. Oppositely charged ions are held together by a strong electrostatic force of attraction to form binary compounds.

(e)

Expert Solution
Check Mark

Answer to Problem 45CR

The formula of the binary compound formed by Al and O is Al2O3 .

Explanation of Solution

The electronic configuration of aluminum with atomic number 13 is 1s22s22p63s23p1 . Aluminum atom has the tendency to lose three electrons from the valence shell to obtain stable electronic configuration like the nearest inert gas neon. For this reason, aluminum atom loses 3 electrons to form aluminum ion (Al3+) .

The electronic configuration of oxygen with atomic number 8 is 1s22s22p4 . Oxygen atom has the tendency to gain two electrons to obtain stable octet structure. For this reason, oxygen atom gains 2 electrons to form oxide ion (O2) .

Two aluminum ions combine with three oxide ions to balance the charge and form a neutral binary compound Al2O3 .

(f)

Interpretation Introduction

Interpretation:

The formula of simple binary compound formed by K and S should be determined.

Concept Introduction :

A binary compound is formed by two different elements usually a metal and a non-metal. A metal atom has the tendency to lose electrons and form positive cations. A non-metal atom has the tendency to gain electrons and form negative anions. Oppositely charged ions are held together by a strong electrostatic force of attraction to form binary compounds.

(f)

Expert Solution
Check Mark

Answer to Problem 45CR

The formula of the binary compound formed by K and S is K2S .

Explanation of Solution

The electronic configuration of potassium with atomic number 19 is 1s22s22p63s23p64s1 . Potassium atom has the tendency to lose one electron from the valence shell to obtain stable electronic configuration like the nearest inert gas argon. For this reason, potassium atom loses 1 electron to form potassium ion (K+) .

The electronic configuration of sulfur with atomic number 16 is 1s22s22p63s23p4 . Sulfur atom has the tendency to gain two electrons to obtain stable octet structure. For this reason, sulfur atom gains 2 electrons to form sulfide ion (S2) .

Two potassium ions combine with one sulfide ion to balance the charge and form a neutral binary compound K2S .

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 12 Solutions

Introductory Chemistry: A Foundation

Ch. 12 - hat is meant by a chemical bond?Ch. 12 - hy do atoms form bonds with one another? What can...Ch. 12 - ow does a bond between Naand Cldiffer from a bond...Ch. 12 - n your own words, what is meant by the term...Ch. 12 - xplain the difference between ionic bonding and...Ch. 12 - rue or false? In general, a larger atom has a...Ch. 12 - hy is there an octet rule (and what does actet...Ch. 12 - Does a Lewis structure tell which electrons came...Ch. 12 - If lithium and fluorine react, which has more...Ch. 12 - In a bond between fluorine and iodine, which has...Ch. 12 - We use differences in electronegative to account...Ch. 12 - Prob. 14ALQCh. 12 - Why do we only the consider the valence electrons...Ch. 12 - How do we determine the total number of valence...Ch. 12 - What is the main idea in the valence shell...Ch. 12 - The molecules NH3andBF3have the same general...Ch. 12 - How do we deal with multiple bonds in VSEPR...Ch. 12 - In Section 12.10 of your text, the term “effective...Ch. 12 - Prob. 21ALQCh. 12 - Prob. 22ALQCh. 12 - Prob. 1QAPCh. 12 - Prob. 2QAPCh. 12 - hat sorts of elements react to form ionic...Ch. 12 - n general terms, what is a covalent bond?Ch. 12 - escribe the type of bonding that exists in the...Ch. 12 - Prob. 6QAPCh. 12 - he relative ability of an atom in a molecule to...Ch. 12 - hat does it mean to say that a bond is polar? Give...Ch. 12 - Prob. 9QAPCh. 12 - What factor determines the relative level of...Ch. 12 - In each of the following groups, which element is...Ch. 12 - In each of the following groups. which element is...Ch. 12 - On the basis. of the electronegativity values...Ch. 12 - On the basis of the electronegativity values given...Ch. 12 - Which of the following molecules contain polar...Ch. 12 - Which of the following molecules contain polar...Ch. 12 - On the basis of the electronegativity values given...Ch. 12 - On the basis of the electronegativity values given...Ch. 12 - Which brand in each of the following pairs has the...Ch. 12 - Which hand in each of the following pairs has less...Ch. 12 - What is a dipole moment? Give four examples of...Ch. 12 - Why is the presence of a dipole moment in the...Ch. 12 - In each of the following diatomic molecules, which...Ch. 12 - In each of the following diatomic molecules. which...Ch. 12 - For each of the following bonds, draw a figure...Ch. 12 - For each of the following bonds, draw a figure...Ch. 12 - For each of the following bonds, draw a figure...Ch. 12 - For each of the following bonds, draw a figure...Ch. 12 - What does it mean when we say that in forming...Ch. 12 - Prob. 30QAPCh. 12 - Nonmetals form negative ions by (losing/gaining)...Ch. 12 - Explain how the atoms in covalent molecules...Ch. 12 - Which simple ion would each of the following...Ch. 12 - Which simple ion would each of the following...Ch. 12 - For each of the following numbers of electrons,...Ch. 12 - Give the formula of a negative ion that would have...Ch. 12 - On the basis of their electron configurations,...Ch. 12 - On the basis of their electron configurations,...Ch. 12 - Name the noble gas atom that has the same electron...Ch. 12 - Atoms form ions so as to achieve electron...Ch. 12 - Prob. 41QAPCh. 12 - Describe in general terms the structure of ionic...Ch. 12 - Why are cations always smaller than the atoms from...Ch. 12 - Why are anions always larger than the atoms from...Ch. 12 - For each of the following pairs, indicate which...Ch. 12 - Prob. 46QAPCh. 12 - Prob. 47QAPCh. 12 - For each of the following pairs, indicate which is...Ch. 12 - Why are the valence electrons of an atom the only...Ch. 12 - Explain what the “duet" and “octet” rules are and...Ch. 12 - What type of structure must each atom in a...Ch. 12 - When elements in the second and third periods...Ch. 12 - How many electrons are involved when two atoms in...Ch. 12 - Prob. 54QAPCh. 12 - Write the simple Lewis structure for each of the...Ch. 12 - Write the simple Lewis structure for each of the...Ch. 12 - Give the total number of valence electrons in each...Ch. 12 - Give the total number of valence electrons in each...Ch. 12 - Write a Lewis structure for each of the following...Ch. 12 - Write a Lewis structure for each of the following...Ch. 12 - Write a Lewis structure for each of the following...Ch. 12 - Prob. 62QAPCh. 12 - The “Chemistry in Focus“ segment Broccoli—Miracle...Ch. 12 - The “Chemistry in Focus" segment Hiding Carbon...Ch. 12 - Write a Lewis structure for each of the following...Ch. 12 - Write a Lewis structure for each of the following...Ch. 12 - Write a Lewis structure for each of the following...Ch. 12 - Write a Lewis structure for each of the following...Ch. 12 - What is the geometric structure of the water...Ch. 12 - What is the geometric sanctum of the ammonia...Ch. 12 - What is the geometric structure of the boron...Ch. 12 - What is the geometric structure of the...Ch. 12 - Why is the geometric structure of a molecule...Ch. 12 - Prob. 74QAPCh. 12 - How is the structure around a given atom related...Ch. 12 - Why are all diatomic molecules linear, regardless...Ch. 12 - Although the valence electron pairs in ammonia...Ch. 12 - Although both the BF3and NF3molecules contain the...Ch. 12 - For the indicated atom in each of the following...Ch. 12 - Prob. 80QAPCh. 12 - Using the VSEPR theory, predict the molecular...Ch. 12 - Prob. 82QAPCh. 12 - Using the VSEPR theory, predict the molecular...Ch. 12 - Using the VSEPR theory, predict the molecular...Ch. 12 - For each of the following molecules or ions,...Ch. 12 - For each of the following molecules or ion....Ch. 12 - The “Chemistry in Focus" segment Taste—It's the...Ch. 12 - Prob. 88QAPCh. 12 - What is resonance? Give three examples of...Ch. 12 - Prob. 90APCh. 12 - The geometric arrangement of electron pairs around...Ch. 12 - Choose the bond that is the least polar. Explain...Ch. 12 - Prob. 93APCh. 12 - Prob. 94APCh. 12 - Prob. 95APCh. 12 - For each of the following pairs of elements,...Ch. 12 - On the basis of the electronegativity values given...Ch. 12 - Which of the following molecules contain polar...Ch. 12 - Prob. 99APCh. 12 - Prob. 100APCh. 12 - or each of the following bonds, draw a figure...Ch. 12 - Prob. 102APCh. 12 - Prob. 103APCh. 12 - Prob. 104APCh. 12 - hich noble gas has the same electron configuration...Ch. 12 - Prob. 106APCh. 12 - rite the Lewis structure for each of the following...Ch. 12 - Prob. 108APCh. 12 - rite a Lewis structure for each of the following...Ch. 12 - Prob. 110APCh. 12 - rite a Lewis structure for each of the following...Ch. 12 - Prob. 112APCh. 12 - hy is the molecular structure of H2Ononlinear,...Ch. 12 - Prob. 114APCh. 12 - sing the VSEPR theory, predict the molecular...Ch. 12 - Prob. 116APCh. 12 - or each of the following molecules, indicate the...Ch. 12 - Prob. 118APCh. 12 - Prob. 119APCh. 12 - Prob. 120APCh. 12 - Prob. 121APCh. 12 - Classify the bonding in each of the following...Ch. 12 - ompare the electronegativities of each pair of...Ch. 12 - Prob. 124CPCh. 12 - rrange the atoms and/or ions in the following...Ch. 12 - Prob. 126CPCh. 12 - Prob. 127CPCh. 12 - he formulas of several chemical substances are...Ch. 12 - Prob. 1CRCh. 12 - hat does temperature measure? Are the molecules in...Ch. 12 - Prob. 3CRCh. 12 - Prob. 4CRCh. 12 - Prob. 5CRCh. 12 - hat is the enthalpy change for a process? Is...Ch. 12 - Prob. 7CRCh. 12 - Prob. 8CRCh. 12 - Prob. 9CRCh. 12 - What is a driving force? Name two common and...Ch. 12 - Prob. 11CRCh. 12 - Methane, CH4, is the major component of natural...Ch. 12 - What is electronegative radiation? Give some...Ch. 12 - Prob. 14CRCh. 12 - Do atoms in excited states emit radiation...Ch. 12 - Prob. 16CRCh. 12 - Schrodinger and de Broglie suggested a...Ch. 12 - Describe the general characteristics of the first...Ch. 12 - Prob. 19CRCh. 12 - Describe the sublevels and orbitals that...Ch. 12 - Describe electron spin. How does electron spin...Ch. 12 - Prob. 22CRCh. 12 - List the order in which the orbitals are filled as...Ch. 12 - Prob. 24CRCh. 12 - Prob. 25CRCh. 12 - Prob. 26CRCh. 12 - What are the representative elements? In what...Ch. 12 - Prob. 28CRCh. 12 - Prob. 29CRCh. 12 - Prob. 30CRCh. 12 - Prob. 31CRCh. 12 - Prob. 32CRCh. 12 - Prob. 33CRCh. 12 - Prob. 34CRCh. 12 - Give evidence that ionic bonds are very strong....Ch. 12 - Prob. 36CRCh. 12 - Prob. 37CRCh. 12 - For three simple molecules of your own choice,...Ch. 12 - Prob. 39CRCh. 12 - Prob. 40CRCh. 12 - Prob. 41CRCh. 12 - Prob. 42CRCh. 12 - Prob. 43CRCh. 12 - Prob. 44CRCh. 12 - Prob. 45CRCh. 12 - Prob. 46CR
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Text book image
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Text book image
General, Organic, and Biological Chemistry
Chemistry
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:Cengage Learning
Text book image
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Types of bonds; Author: Edspira;https://www.youtube.com/watch?v=Jj0V01Arebk;License: Standard YouTube License, CC-BY