Concept explainers
Give the formula of a negative ion that would have the same number of electrons as each of the following positive ions.
a. Na+
b. Ca2+
c. Al3+
d. Rb+
(a)
Interpretation: The formula of negative ions that have the same number of electrons as each of the given positive ions is to be written.
Concept introduction: The ionic compound can be separated into ions. Ions are of two types. Positively charged ions are called cation and negatively charged ions are called anions.
To determine: The formula of negative ions that have the same number of electrons as in
Answer to Problem 49E
Explanation of Solution
The electronic configuration of
It contains 10 electrons.
The atomic number of oxygen
It gains two electrons to get 10 electrons and form
The atomic number of fluorine
It gains an electron to get 10 electrons and form
The atomic number of nitrogen
It gains three electrons to get 10 electrons and form
(b)
Interpretation: The formula of negative ions that have the same number of electrons as each of the given positive ions is to be written.
Concept introduction: The ionic compound can be separated into ions. Ions are of two types. Positively charged ions are called cation and negatively charged ions are called anions.
To determine: The formula of negative ions that have the same number of electrons as in
Answer to Problem 49E
Explanation of Solution
The electronic configuration of
It contains 18 electrons.
The atomic number of chlorine
It gains an electron to get 18 electrons and form
The atomic number of sulfur
It gains two electrons to get 18 electrons and form
The atomic number of phosphorous
It gains three electrons to get 18 electrons and form
(c)
Interpretation: The formula of negative ions that have the same number of electrons as each of the given positive ions is to be written.
Concept introduction: The ionic compound can be separated into ions. Ions are of two types. Positively charged ions are called cation and negatively charged ions are called anions.
To determine: The formula of negative ions that have the same number of electrons as in
Answer to Problem 49E
Explanation of Solution
The electronic configuration of
It contains 10 electrons.
The atomic number of fluorine
It gains an electron to get 10 electrons and form
The atomic number of oxygen
It gains two electrons to get 10 electrons and form
The atomic number of nitrogen
It gains three electrons to get 10 electrons and form
(d)
Interpretation: The formula of negative ions that have the same number of electrons as each of the given positive ions is to be written.
Concept introduction: The ionic compound can be separated into ions. Ions are of two types. Positively charged ions are called cation and negatively charged ions are called anions.
To determine: The formula of negative ions that have the same number of electrons as in
Answer to Problem 49E
Explanation of Solution
The electronic configuration of
It contains 36 electrons.
The atomic number of bromine
It gains an electron to get 36 electrons and form
The atomic number of selenium
It gains two electrons to get 36 electrons and form
The atomic number of arsenic
It gains three electrons to get 36 electrons and form
Want to see more full solutions like this?
Chapter 8 Solutions
CHEMISITRY W/OWL PKG LOOSELEAF
- Use data in this chapter (and Chapter 2) to discuss why MgO is an ionic compound but CO is not an ionic compound.arrow_forwardUsing the bond energies in Table 7.2, determine the approximate enthalpy change for each of the following reactions: (a) Cl2(g)+3F2(g)2ClF3(g) (b) H2C=CH2(g)+H2(g)H3CCH3(g) (c) 2C2H6(g)+7O2(g)4CO2(g)+6H2O(g) .arrow_forwardhat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?arrow_forward
- What main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.arrow_forwardUsing the standard enthalpy of formation data in Appendix G. determine which bond is stronger: the PCl bond in PCl3(g) or in PCl5(g)?arrow_forwardArrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl, KBr (b) MgO, CaO, CaCl2 (c) LiF, BeF2, BeOarrow_forward
- For which of the following substances is the least energy required to convert one mole of the solid into separate ions? (a) MgO (b) SrO (c) KF (d) CsF (e) MgF2arrow_forwardUsing the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulfur double bond in CS2.arrow_forwardDescribe the molecular structure around the indicated atom or atoms: (a) the sulfur atom in sulfuric acid, H2SO4[(HO)2SO2] (b) the chlorine atom in chloric acid, HClO3[HOClO2] (c) the oxygen atom in hydrogen peroxide, HNO3[HONO2] (d) the nitrogen atom in nitric acid, HNO3[HONO2] (e) the oxygen atom in the OH group in nitric acid, HNO3[HONO2] (f) the central oxygen atom in the ozone molecule, O3 (g) each of the carbon atoms in propyne, CH3CCH (h) the carbon atom in Freon, CCl2F2 (i) each of the carbon atoms in aliene, H2CCH2arrow_forward
- Which of the following compounds requires the most energy to convert one mole of the solid into separate ions? (a) MgO (b) SrO (c) KF (d) CsF (e) MgF2arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forwardThe standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are + 278.8, + 79.0, 775, and 1209 kJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 8.5. What conclusions can you draw? c. Why are the Ht0 values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning