Chemistry For Today: General, Organic, And Biochemistry, Loose-leaf Version
9th Edition
ISBN: 9781305968707
Author: Spencer L. Seager
Publisher: Brooks Cole
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Textbook Question
Chapter 4, Problem 4.57E
Use the periodic table and Table
a. 
b. 
c. 
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What force is NOT taken into account in the formation of a covalent bond?a. repulsion between positively charged nuclei and negatively charged electronsb. repulsion between two positively charged nuclei.c. force of attraction between positively charged nuclei and negatively charged electrons
Which description below correctly describes polar molecules?
a. Have polar bonds present.
b. The polar bonds are arranged so that they do not cancel.
c. Lone pairs on the central atom are arranged so that they do not cancel.
d. Lone pairs on the central atom are arranged so that they can be cancelled out.
1. How many electron groups does a central atom have that has one single bond, one double bond, and one lone pair.
a.1
b. 2
c. 3
d.4
Chapter 4 Solutions
Chemistry For Today: General, Organic, And Biochemistry, Loose-leaf Version
Ch. 4 - Refer to the group numbers of the periodic table...Ch. 4 - Prob. 4.2ECh. 4 - Write abbreviated electronic configurations for...Ch. 4 - Write abbreviated electronic configurations for...Ch. 4 - Draw Lewis structure for the elements given in...Ch. 4 - Draw Lewis structures for the elements given in...Ch. 4 - Prob. 4.7ECh. 4 - Prob. 4.8ECh. 4 - Prob. 4.9ECh. 4 - Prob. 4.10E
Ch. 4 - Use the periodic table and predict the number of...Ch. 4 - Prob. 4.12ECh. 4 - Write a symbol for each of the following ions: a.A...Ch. 4 - Write a symbol for each of the following ions: a.A...Ch. 4 - Prob. 4.15ECh. 4 - Identify the element in period 3 that would form...Ch. 4 - Identify the noble gas that is isoelectronic with...Ch. 4 - Identify the noble gas that is isoelectronic with...Ch. 4 - Write equations to represent positive and negative...Ch. 4 - Prob. 4.20ECh. 4 - Write the formula for the ionic compound formed...Ch. 4 - Prob. 4.22ECh. 4 - Classify each of the following as a binary...Ch. 4 - Prob. 4.24ECh. 4 - Prob. 4.25ECh. 4 - Prob. 4.26ECh. 4 - Prob. 4.27ECh. 4 - Prob. 4.28ECh. 4 - Prob. 4.29ECh. 4 - Name the following binary ionic compounds: a. SrS...Ch. 4 - Name the following binary ionic compounds, using a...Ch. 4 - Name the following binary ionic compounds, using a...Ch. 4 - Prob. 4.33ECh. 4 - Prob. 4.34ECh. 4 - Prob. 4.35ECh. 4 - Write formulas for the following binary ionic...Ch. 4 - Prob. 4.37ECh. 4 - Prob. 4.38ECh. 4 - Identify the ions that would occupy lattice sites...Ch. 4 - Identify the ions that would occupy lattice sites...Ch. 4 - Calculate the mass in grams of positive ions and...Ch. 4 - Calculate the mass in grams of positive ions and...Ch. 4 - Prob. 4.43ECh. 4 - Prob. 4.44ECh. 4 - Represent the following reaction using Lewis...Ch. 4 - Prob. 4.46ECh. 4 - Prob. 4.47ECh. 4 - Represent the following molecules by Lewis...Ch. 4 - Draw Lewis structures for the following polyatomic...Ch. 4 - Prob. 4.50ECh. 4 - Prob. 4.51ECh. 4 - Prob. 4.52ECh. 4 - Predict the shape of each of the following...Ch. 4 - Prob. 4.54ECh. 4 - Prob. 4.55ECh. 4 - Prob. 4.56ECh. 4 - Use the periodic table and Table 4.4 to determine...Ch. 4 - Use Table 4.4 and classify the bonds in the...Ch. 4 - Use Table 4.4 and classify the bonds in the...Ch. 4 - Prob. 4.60ECh. 4 - On the basis of the charge distributions you drew...Ch. 4 - Prob. 4.62ECh. 4 - Prob. 4.63ECh. 4 - Prob. 4.64ECh. 4 - Show the charge distribution in the following...Ch. 4 - Prob. 4.66ECh. 4 - Prob. 4.67ECh. 4 - Prob. 4.68ECh. 4 - Prob. 4.69ECh. 4 - Prob. 4.70ECh. 4 - Prob. 4.71ECh. 4 - Prob. 4.72ECh. 4 - Prob. 4.73ECh. 4 - Prob. 4.74ECh. 4 - Prob. 4.75ECh. 4 - The covalent compounds ethyl alcohol and dimethyl...Ch. 4 - Prob. 4.77ECh. 4 - Prob. 4.78ECh. 4 - Prob. 4.79ECh. 4 - Prob. 4.80ECh. 4 - Prob. 4.81ECh. 4 - Prob. 4.82ECh. 4 - Suppose an element from group II(A)(2) and period...Ch. 4 - What would be the mass in grams of 0.200moles of...Ch. 4 - The ampere unit is used to describe the flow of...Ch. 4 - Prob. 4.86ECh. 4 - Prob. 4.87ECh. 4 - Prob. 4.88ECh. 4 - Prob. 4.89ECh. 4 - Prob. 4.90ECh. 4 - Prob. 4.91ECh. 4 - Prob. 4.92ECh. 4 - Prob. 4.93ECh. 4 - Prob. 4.94ECh. 4 - Prob. 4.95ECh. 4 - Noble gases: a.have low boiling points. b.are all...Ch. 4 - Prob. 4.97ECh. 4 - Name the type of bond that is formed when...Ch. 4 - Prob. 4.99ECh. 4 - A atom becomes an ion that possesses a negative...Ch. 4 - When calcium reacts with chlorine to form calcium...Ch. 4 - Prob. 4.102ECh. 4 - Prob. 4.103ECh. 4 - Which molecule below has a nonpolar bond in which...Ch. 4 - What is the correct formula for bismuth (III)...Ch. 4 - Which of the following species will combine with a...Ch. 4 - What type of bond is created when bromine and...Ch. 4 - The parts of an atom directly involved in ionic...Ch. 4 - In forming an ionic bond with an atom of chlorine,...Ch. 4 - In bonding, what would happen between the...Ch. 4 - Which compound contains a bond with no ionic...Ch. 4 - Prob. 4.112ECh. 4 - Which molecule is nonpolar and contains a nonpolar...Ch. 4 - Which of the following is a nonpolar covalent...Ch. 4 - Prob. 4.115ECh. 4 - Prob. 4.116E
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- Hydrogen gas and oxygen gas react violently to form water. When this occurs, a very loud noise is heard. Draw the Lewis structures for hydrogen gas, oxygen gas, and water. State whether each molecule is polar or nonpolar and why. Explain how the polarity of these molecules is related to hydrogen and oxygen existing in the gas phase at room temperature and water existing in the liquid phase at room temperature. Which is lower in energy for this reaction a mixture of hydrogen and oxygen gases or water? How do you know this is true?arrow_forwardDraw in all the hydrogen atoms and nonbonded electron pairs in each ion. a. b. d. ENHarrow_forward1. The electron pair in a H - Cl bond could be considered... a. closer to H because Hydrogen has a larger radius and thus exerts greater control over the shared electron pair b. closer to Cl because Chlorine has a higher electronegativity than Hydrogen c. closer to H because Hydrogen has a lower electronegativity than Chlorine d. an inadequate model since the bond is ionic 2. It is important to know the geometry of a molecule because the geometry _______. a. will give the Lewis structure of the molecule b. affects the physical and chemical properties of the substance c. will determine whether the molecule is ionic or covalent d. Both B, and Carrow_forward
- The molecular shapes depend on: A. The total number of valence shell electron pairs present around the terminal atoms in the molecule and the number of bonded pairs. B. The total number of lone pairs present around the central atom in the molecule and the number of bonded pairs. C. The total number of valence shell electron pairs present around the central atom in the molecule and the number of lone pairs. D. The total number of valence shell electron pairs present around the central atom in the molecule and the number of bonded pairs.arrow_forwardIn your own words, differentiate polar and nonpolar covalent bond. 1. What is electronegativity and how can it be used in in determining the polarity of molecules? le it possible for a molecule to fiave a polar bond but have an overall polarity of 2. nonpolar? 3. Differentiate bonding and non-bonding electrons.arrow_forwardWhich of the following statements is INCORRECT? a. Polar covalent bonds can be present in a nonpolar molecule.b. Polar covalent bond is present if the electronegativity difference between atoms is equal or less than 0.4.c. Polarity of bond and molecular geometry are the two factors that affect the polarity of molecules. d. Polar bonds forms when electrons are unequally shared by two atoms in a compound.arrow_forward
- If an atom has one valence electron—that is, a single electron in its outer energy level—it will most likely form a. one polar, covalent bond. b. two nonpolar, covalent bonds. c. two covalent bonds. d. an ionic bond.arrow_forwardpick the correct statement a. On the periodic table, atomic size generally increase across a period from left to right b. in VSEPR theory, the lone pair of electrons on the central atom play a role in deciding the molecular geometry c. ionization energy is the measure of the attractive force that on atom in a covalent bond has for the electrons of the bond. d. in chemical bonding, metals gains electronns and non metals lose electronsarrow_forwardIf a molecule requires two or more resonance structures to draw it, which of the following statements is true? Select one: A. The molecule does not have a single structure but dynamically oscillates between the resonance structures drawn for it. B. The molecule has lower energy than the computed energy of any of the resonance structures that are drawn for it. O C. The molecule is less stable than any of the resonance structures drawn for it. D. The molecule's resonance structures coexist in an equilibrium with the lower energy form predominating.arrow_forward
- Why does the octet rule not apply to transition metals? a. the octet rule does apply to transition metals as they are all classified as metals b. transition metals do not form cations or anions c. most transition elements form ions with more than one positive charge d. transition elements cannot be assigned with charges to form ions What do you call the process of positive and negative ions of an ionic compound separating from each other when solubilized in water? a. dissociation b. solubilization c. differentiation d. precipitation Which of the following statements is considered true? a. The size of an atom is determined by the size of the outermost occupied orbital b. Higher ionization energy means that the electron is more difficult to remove c. both are correct d. both are incorrectarrow_forwardIt is a type of bond between a hydrogen atom and a pair of unshared electrons on the electronegative atom of another molecule? a. metallic bond b. sigma bond c. Pi bond d. hydrogen bond ....arrow_forwardCarbons forms a variety of compounds. Which of the following is NOT a valid reason for this observation? a. Organic compounds may have many isomers. b. C can make multiple bonds to O, N, S, or other C. c. C can form single covalent bonds to O, N, S, and halogens. d. C forms a total of four covalent bonds. e. C forms stable covalent bonds to metal atoms.arrow_forward
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