CHEMISTRY THE CENTRAL SCIENCE 14TH EDI
14th Edition
ISBN: 9780134863016
Author: Brown
Publisher: PEARSON
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Textbook Question
Chapter 8, Problem 45E
In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound:
- SiF4 and LaF3,
- FeCl2 and ReCl6,
- PbCl4 and RbCl.
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Part II: Binary Covalent Compounds
Covalent compounds are produces by nonmetals bonding with one another. You can use the valence
electrons for each element to determine the simplest formula that exists between two elements. For
example, H has 1 valence electron and needs one more to obey the Octet Rule, so it will only make 1
bond when found in a compound. Oxygen has 6 valence electrons and needs two more to obey the
Octet Rule, so it typically makes 2 bonds when found in a compound. Since hydrogen needs just one
electron while oxygen needs two, the correct formula for the simplest compound would be H20.
However, there are often other combinations possible in addition to the simplest formula. For
example, hydrogen and oxygen can also form, H2O2, which is known as hydrogen peroxide. To work
with all the possible combinations, some rules have been developed for naming binary covalent
compounds. The rules are stated below:
1. The least metallic element will always end in the suffix…
Naming Ionic Compounds
ACTIVITY 2: Give the name of the ions expected from the following compounds,
then, give the correct names of the ionic compounds. Further classify the
compounds as BINARYor TERNARY.
Chemical
Positive Ion Negative Ion
Name of Ionic
Binary or
Ternary
Formula
Compound
ZnCl2
Cu(NO3)2
Вао
Ni(OH)2
ACTIVITY 3: Write the formula of the ions expected from the following compounds.
Write the chemical formulas and classify them further as BINARY or TERNARY.
Name of Ionic
Positive Ion Negative Ion
Chemical
Binary or
Ternary
Compound
Formula
Calcium sulfate
Lead (II) iodide
Sodium carbonate
Tin (IV) oxide
Strontium chromate
6. Which of the following do not accurately represent stable binary ionic compounds?
Why? Mgl, Al(OH)2, InF2, CO4 , RÜC12 , CsS, Be;0.
Chapter 8 Solutions
CHEMISTRY THE CENTRAL SCIENCE 14TH EDI
Ch. 8.2 - Which of the these elements is most likely to from...Ch. 8.2 - Prob. 8.1.2PECh. 8.2 - Which of the following bond is the most polar? H-F...Ch. 8.2 - Prob. 8.2.2PECh. 8.3 - Prob. 8.3.1PECh. 8.3 - Prob. 8.3.2PECh. 8.4 - Which of the following bonds is the most polar? a....Ch. 8.4 - Which of the following bonds is most polar: S-Cl,...Ch. 8.4 - Prob. 8.5.1PECh. 8.4 - The dipole moment of chlorine monofluoride,...
Ch. 8.5 - Which of the these molecules has a Lewis structure...Ch. 8.5 -
How many valence electrons should appear in the...Ch. 8.5 - Compare the lewis symbol for neon the structure...Ch. 8.5 - Prob. 8.7.2PECh. 8.5 - Prob. 8.8.1PECh. 8.5 - Prob. 8.8.2PECh. 8.5 - Prob. 8.9.1PECh. 8.5 - Prob. 8.9.2PECh. 8.6 - Which of the statements about resonance is true?...Ch. 8.6 - Prob. 8.10.2PECh. 8.7 - Prob. 8.11.1PECh. 8.7 - Prob. 8.11.2PECh. 8 - Prob. 1DECh. 8 - Prob. 1ECh. 8 - Prob. 2ECh. 8 - A portion of a two-dimensional "slab" of NaCl(s)...Ch. 8 - Prob. 4ECh. 8 - Prob. 5ECh. 8 - Incomplete Lewis structures for the nitrous acid...Ch. 8 - Prob. 7ECh. 8 - Prob. 8ECh. 8 - Prob. 9ECh. 8 - True or false: The hydrogen atom is most stable...Ch. 8 - Consider the element silicon, Si. Write its...Ch. 8 - Write the electron configuration for the element...Ch. 8 - Prob. 13ECh. 8 - What is the Lewis symbol for each of the following...Ch. 8 - Using Lewis symbols, diagram the reaction between...Ch. 8 - Use Lewis symbols to represent the reaction that...Ch. 8 - Predict the chemical formula of the ionic compound...Ch. 8 - Prob. 18ECh. 8 - Prob. 19ECh. 8 - Prob. 20ECh. 8 - Is lattice energy usually endothermic or...Ch. 8 - NaCI and KF have the same crystal structure. The...Ch. 8 - Prob. 23ECh. 8 - Prob. 24ECh. 8 - Consider the ionic compounds KF, NaCl, NaBr, and...Ch. 8 - Which of the following trends in lattice energy is...Ch. 8 - Energy is required to remove two electrons from Ca...Ch. 8 - Prob. 28ECh. 8 - Use data from Appendix C, Figure 7.10, and Figure...Ch. 8 - Prob. 30ECh. 8 - Prob. 31ECh. 8 - Prob. 32ECh. 8 - Using Lewis symbols and Lewis structures, diagram...Ch. 8 - Use Lewis symbols and Lewis structures to diagram...Ch. 8 - Prob. 35ECh. 8 - Prob. 36ECh. 8 - Prob. 37ECh. 8 - What is the trend in electronegativity going from...Ch. 8 - Prob. 39ECh. 8 - By referring only to the periodic table, select...Ch. 8 - which of the following bonds are polar? B-F,...Ch. 8 - Arrange the bonds in each of the following sets in...Ch. 8 - Prob. 43ECh. 8 - Prob. 44ECh. 8 - In the following pairs of binary compounds,...Ch. 8 - Prob. 46ECh. 8 - Prob. 47ECh. 8 - Write Lewis structures for the following: H2CO...Ch. 8 - Prob. 49ECh. 8 - Draw the dominant Lewis structure for the...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Prob. 52ECh. 8 - Prob. 53ECh. 8 - Prob. 54ECh. 8 - Prob. 55ECh. 8 - Prob. 56ECh. 8 - Prob. 57ECh. 8 - Prob. 58ECh. 8 - Prob. 59ECh. 8 - Prob. 60ECh. 8 - Prob. 61ECh. 8 - 8.62 For Group 3A-7A elements in the third row of...Ch. 8 - Draw the Lewis structures for each of the...Ch. 8 - Prob. 64ECh. 8 - In the vapor phase, BeCl2exists as a discrete...Ch. 8 -
8.66
Describe the molecule xenon trioxide, XeO3,...Ch. 8 -
8.67 There are many Lewis structures you could...Ch. 8 - Prob. 68ECh. 8 - Using Table 8.3, estimate H for each of the...Ch. 8 - Using Table 8.3, estimate H for the following...Ch. 8 - State whether each of these statements is true or...Ch. 8 - Prob. 72ECh. 8 - Prob. 73ECh. 8 - Prob. 74ECh. 8 - Prob. 75ECh. 8 - Prob. 76ECh. 8 - A new compound is made that has a C-C bond length...Ch. 8 - A new compound is made that has an N-N bond length...Ch. 8 - Prob. 79AECh. 8 - Prob. 80AECh. 8 - An ionic substance of formula MX has a lattice...Ch. 8 - Prob. 82AECh. 8 - Prob. 83AECh. 8 - Prob. 84AECh. 8 - Consider the collection of nonmetallic elements 0,...Ch. 8 - The substance chlorine monoxide, CIO(g), is...Ch. 8 -
[8.87]
a. using the electronegativities of Br...Ch. 8 - Prob. 88AECh. 8 - Although I3- is a known ion, F3- is not. a. Draw...Ch. 8 - Calculate the formal charge on the indicated atom...Ch. 8 - The hypochlorite ion, CIO- , is the active...Ch. 8 - Prob. 92AECh. 8 - a. Triazine, C3 H3N3, is like benzene except that...Ch. 8 - Prob. 94IECh. 8 - Prob. 95IECh. 8 - Prob. 96IECh. 8 - Prob. 97IECh. 8 - Prob. 98IECh. 8 - Prob. 99IECh. 8 - Prob. 100IECh. 8 - Prob. 101IECh. 8 - Prob. 102IECh. 8 -
8.103 The compound chloral hydrate, known in...Ch. 8 - Barium azide is 62.04% Ba and 37.96% N. Each azide...Ch. 8 - Acetylene (C2H2) and nitrogen (N2) both contain a...Ch. 8 - Prob. 106IECh. 8 - Prob. 107IECh. 8 -
8.108 Formic acid has the chemical formula...Ch. 8 - Prob. 109IECh. 8 - Prob. 110IE
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- Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?arrow_forwardFrom the following ions and their radii (in pm), choose a pair that gives the strongest ionic bonding and a pair that givesthe weakest: Mg²⁺72; K⁺138; Rb⁺152; Ba²⁺135; Cl⁻181;O²⁻140; I⁻220arrow_forwardCompounds such as Freon® 112 (referred to as chlorofluorocarbons, or CFCs) were used as refrigerants for many years, but they were phased out because of their harmful effects on Earth's atmosphere. Write the molecular and empirical formulas for Freon 112. The Lewis dot structure of Freon 112. There are two central carbon atoms bonded together through a single bond. Each carbon atom is bonded to two chlorine atoms and one fluorine atom through single bonds. Each chlorine atom has 3 lone pairs. Each fluorine atom has 3 lone pairs.arrow_forward
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