General, Organic, and Biological Chemistry (3rd Edition)
3rd Edition
ISBN: 9780134042428
Author: Laura D. Frost, S. Todd Deal
Publisher: PEARSON
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Textbook Question
Chapter 3, Problem 3.113CP
One of the most common compounds used in commercial dry deaning is tetrachloroethylene, which has the molecular formula C2C14.
- a. Draw the Lewis structure of tetrachloroethylene.
- b. Determine the shape and the bond angle around each of the carbon atoms.
- c. Label each of the polar covalent bonds with a dipole moment arrow.
- d. Determine if this compound is polar or nonpolar.
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Students have asked these similar questions
1. The molecule boron trifluoride, BF3, assumes a trigonal planar geometry with boron as the
central atom. Which statement correctly describes the polarity of the B-F bond and the polarity
of the molecule?
A. The B-F bond is polar; the BF3 molecule is nonpolar.
B. The B-F bond is nonpolar; the BF3 molecule is nonpolar.
C. The B-F bond is nonpolar; the BF3 molecule is polar.
D. The B-F bond is polar; the BF3 molecule is polar.
E. The polarity cannot be determined.
2. Which of the following species will exhibit tetrahedral geometry?
A. CCI4
B. CO32 -
C. 03
D. PCI5
E. SF6
3. If a compound has a polar bonds, then
1. It is polar overall.
II. There is an electronegativity difference between the bonded atoms.
III. It is ionic.
IV. It doesn't have resonance.
A. Il only
B. II, IV
C. I, II, IV
D. I, II
E. All of the above statements are correct.
4. Predict the geometry and polarity of the CS2 molecule.
A. linear, nonpolar
B. linear, nonpolar
C. tetrahedral, polar
D. bent, polar
E. bent, nonpolar
TTTTTTTTTTT
Atoms of oxygen can form many different types of covalent chemical bonds. Which
19 covalent bond can atoms of oxygen form?
A. Single bonds only
B. Single bonds & Double bonds
C. Single bonds, Double bonds, & Triple bonds
D. None of the options listed.
Which element's atoms can only form one single bond and no others in a covalent
20 compound?
A. Hydrogen
B. Helium
C. Lithium
D. Beryllium
Which element's atoms can only form one single bond and no others in a covalent
21 compound?
A. Selenium
B. Arsenic
C. Aluminum
D. Bromine
Consider the covalent compound H₂O.
22 How many total valence electrons are in one molecule?
A. 2
C. 8
B. 6
D. 10
Consider the covalent compound H₂O.
23 How many unshared pairs of electrons are in one molecule?
C. 3 pairs
A. 1 pair
B. 2 pairs
D. 4 pairs
Consider the covalent compound NF3.
24 How many total valence electrons are in one molecule?
A. 22
B. 26
C. 28
D. 32
Consider the covalent compound NF3.
25 How many unshared pairs of electrons are in one…
1. How many electrons will an iodine atom donate or accept, based on its number of valence electrons?
A. Donate 7 electrons
B. Donate 1 electron
C. Accept 7 electrons
D. Accept 1 electrons
2.What type of bond is formed between the two nitrogen atoms in diatomic nitrogen, N2?
A. Triple Bond
B. Double Covalent Bond
C. Double Ionic Bond
D. Single Bond
3.Which metal would form a stronger metallic bond?
A. Lithium
B. Sodium
C. Strontium
D. Tungsten
4. What holds the metal ions together in a lattice?
A. Hydrogen Bonds
B. Covalent Bonds
C. Metallic Bonds
D. Ionic Bonds
Chapter 3 Solutions
General, Organic, and Biological Chemistry (3rd Edition)
Ch. 3 - How many electrons are in each energy level of the...Ch. 3 - How many electrons are in each energy level of the...Ch. 3 - How many valence electrons are present in the...Ch. 3 - How many valence electrons are present in the...Ch. 3 - Which of the following elements are stable as...Ch. 3 - Which of the following elements are stable as...Ch. 3 - Prob. 3.7PPCh. 3 - Prob. 3.8PPCh. 3 - Prob. 3.9PPCh. 3 - How are the names of a transition metal atom and...
Ch. 3 - Provide the charge on each element when an ion is...Ch. 3 - Provide the charge on each element when an ion is...Ch. 3 - Prob. 3.13PPCh. 3 - How many protons and electrons are present in the...Ch. 3 - Name the ions in Problem 3.13.Ch. 3 - Prob. 3.16PPCh. 3 - Prob. 3.17PPCh. 3 - Give the name and symbol of the ion with the...Ch. 3 - Prob. 3.19PPCh. 3 - Name the following ions: a. Cu2+ b. SO42 c. HPO42Ch. 3 - Prob. 3.21PPCh. 3 - Prob. 3.22PPCh. 3 - Prob. 3.23PPCh. 3 - Prob. 3.24PPCh. 3 - Prob. 3.25PPCh. 3 - Prob. 3.26PPCh. 3 - Prob. 3.27PPCh. 3 - Prob. 3.28PPCh. 3 - Draw the correct Lewis structure for each of the...Ch. 3 - Draw the correct Lewis structure for each of the...Ch. 3 - Draw the correct Lewis structure for each of the...Ch. 3 - Draw the correct Lewis structure for each of the...Ch. 3 - Determine whether each of the following is a...Ch. 3 - Determine whether each of the following is a...Ch. 3 - Prob. 3.35PPCh. 3 - Prob. 3.36PPCh. 3 - Compare (a) the number of atoms and (b) the number...Ch. 3 - Compare (a) the number of atoms and (b) the number...Ch. 3 - Calculate the following: a. the number of Na atoms...Ch. 3 - Calculate the following: a. the number of S atoms...Ch. 3 - Prob. 3.41PPCh. 3 - Determine the molar mass for the following...Ch. 3 - Prob. 3.43PPCh. 3 - Prob. 3.44PPCh. 3 - For the molecules shown, indicate whether the...Ch. 3 - For the molecules shown, indicate whether the...Ch. 3 - For the molecules in 3.45, determine the shape...Ch. 3 - For the molecules in 3.46, determine the around...Ch. 3 - Prob. 3.49PPCh. 3 - Prob. 3.50PPCh. 3 - Prob. 3.51PPCh. 3 - For each of the following molecules, (1) draw the...Ch. 3 - Prob. 3.53APCh. 3 - Prob. 3.54APCh. 3 - Prob. 3.55APCh. 3 - How many valence electrons are present in the...Ch. 3 - Prob. 3.57APCh. 3 - Prob. 3.58APCh. 3 - Complete the following statements: a. An anion has...Ch. 3 - Prob. 3.60APCh. 3 - Prob. 3.61APCh. 3 - Prob. 3.62APCh. 3 - Prob. 3.63APCh. 3 - Prob. 3.64APCh. 3 - Prob. 3.65APCh. 3 - Prob. 3.66APCh. 3 - Each of the following ions is isoelectronic with a...Ch. 3 - Each of the following ions is isoelectronic with a...Ch. 3 - Prob. 3.69APCh. 3 - Prob. 3.70APCh. 3 - Give the formula for the ionic compound formed by...Ch. 3 - Prob. 3.72APCh. 3 - Prob. 3.73APCh. 3 - Give the formula for each of the following ionic...Ch. 3 - Name the following ionic compounds: a. Na2O b....Ch. 3 - Prob. 3.76APCh. 3 - Prob. 3.77APCh. 3 - Prob. 3.78APCh. 3 - Prob. 3.79APCh. 3 - Prob. 3.80APCh. 3 - Prob. 3.81APCh. 3 - Prob. 3.82APCh. 3 - Prob. 3.83APCh. 3 - Prob. 3.84APCh. 3 - Prob. 3.85APCh. 3 - Explain the difference between a Lewis structure...Ch. 3 - Draw a Lewis structure for each of the following...Ch. 3 - Draw a Lewis structure for each of the following...Ch. 3 - Prob. 3.89APCh. 3 - Give the name of each of the following covalent...Ch. 3 - Explain the difference between an ionic bond and a...Ch. 3 - What are the units of Avogadros number?Ch. 3 - Prob. 3.93APCh. 3 - Prob. 3.94APCh. 3 - What is the mass of 4.00 moles of the following?...Ch. 3 - How many atoms or molecules are in 5.0 moles of...Ch. 3 - A pencil mark (made with graphite, a form of...Ch. 3 - Prob. 3.98APCh. 3 - Prob. 3.99APCh. 3 - Prob. 3.100APCh. 3 - Aspartic acid, a naturally occurring amino acid...Ch. 3 - Cyanoacrylic acid is one of the compounds used to...Ch. 3 - Methyl isocyanate is used in the manufacturing of...Ch. 3 - Vinyl acetate is used in the production of safety...Ch. 3 - Identify the more electronegative atom in each of...Ch. 3 - Identify the more electronegative atom in each of...Ch. 3 - Prob. 3.107APCh. 3 - Prob. 3.108APCh. 3 - Prob. 3.109CPCh. 3 - Prob. 3.110CPCh. 3 - Prob. 3.111CPCh. 3 - Vinyl chloride, C2H3Cl, is used in the production...Ch. 3 - One of the most common compounds used in...Ch. 3 - Prob. 1IA.1QCh. 3 - Prob. 1IA.2QCh. 3 - Prob. 1IA.3QCh. 3 - Prob. 1IA.4QCh. 3 - Prob. 1IA.5QCh. 3 - Prob. 1IA.6QCh. 3 - Prob. 1IA.7QCh. 3 - Prob. 1IA.8QCh. 3 - Prob. 2IA.1QCh. 3 - Complete the following table: Molecular Formula...Ch. 3 - Complete the following table: Molecular Formula...Ch. 3 - Based on the tables in questions 2 and 3, does the...Ch. 3 - Prob. 3IA.1QCh. 3 - Prob. 3IA.2QCh. 3 - Draw the Lewis structure for ammonia. NH3. Show...Ch. 3 - Draw the Lewis structure for H2O. Show the...Ch. 3 - Draw the Lewis structure for carbon dioxide. What...Ch. 3 - Draw the Lewis structure for carbon tetrachloride,...Ch. 3 - Prob. 3IA.7QCh. 3 - Using a dipole moment arrow (), indicate the...Ch. 3 - Find out which cations and anions are important in...
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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
- a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.arrow_forwardHydrogen 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_forwardUse the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a two-atom molecule: (a) Adjust the electronegativity value so the bond dipole is pointing toward B. Then determine what the electronegativity values must be to switch the dipole so that it points toward A. (b) With a partial positive charge on A, turn on the electric field and describe what happens. (c) With a small partial negative charge on A, turn on the electric field and describe what happens. (d) Reset all, and then with a large partial negative charge on A, turn on the electric field and describe what happens.arrow_forward
- 7. What kind of bond is formed when two molecules share electrons to form a molecule? a. Covalent b. Ionic c. Polar ionic d. Metallic 8. Why are transition metals special cases? a. They have two valence shells with complete octets that want to react. b. They have up to 8 electrons in their valence shell. c. They don't react with other elements because they are actually noble gases. d. They have two valence shells with an incomplete octet that want to react. 9. Name the following compound, BrF; a. Bromine pentafluoride b. Bromine fluoride c. Bromine (IV) fluoride d. Monobromine pentafluoride 10. Avron was conducting his science fair project when he came across a bottle of acid whose label read, "HSCN." What is the name of the acid that is contained within the bottle? a. Hydrocyanic acid b. Hydrothiocyanic acid c. Thiocyanic acid d. This acid does not exist 11. What is the chemical formula for copper (II) hydroxide? а. Cu,(ОН) b. CUOH с. CuOН, d. Cu(OH),arrow_forwardPart II Practicing Coordinate Covalent Bonding for Molecular compounds. Example: Given the molecular compound SO, draw the molecular compound using the coordinate covalent bonding model. A. Calculate the total number of electrons. S = 1x 6 = 6 electrons O = 4 x 6 = 24 electrons Charge -2 = 2 electrons Total = 32 electrons B. Determine Center Atom (look for the single element) in this case S. C. Now make a single bond to all other elements to the central atom. You have used 8 electrons of the 32. 0- D. Place electrons around the atoms that are bonded to the central atom so that each will have 8 electrons around them (in this case each oxygen needs 6 more electrons or 3 pairs of electrons). : E. Make sure that the central atom has a full octet (8 electrons). In this case it does, so you are done. If not, one of the lone pairs of electrons from an outer atom will share a second pair of electrons with the center atom. Finally be sure that you have used all your electrons and NO MORE!arrow_forward1-How many total shared electrons are there in the Lewis structure of CS2? a.10 b.6 c.2 d.8 e.4 2-In which bond does the Cl atom have the highest electron density, i.e. it attracts the electrons in the covalent bonds the most? a.N—Cl b.H—Cl c.O—Cl d.S—Cl e.Br—Clarrow_forward
- Which of the following represents a non-polar covalent bond? a. H-O b. C-N c. C-C d. Li-F e. S-O Based on electronegativities, which of the following would you expect to be most ionic? a. N2 b. CaF2 c. CO2 d. CH4 e. CF4 Which element is the least electronegative? a. Calcium b. Cesium c. Iron d. Barium e. Potassiumarrow_forwarda. Predict the formula of thecompound formed from aluminum and fluorine.b. Calculate the electronegativity difference between aluminum and fluorine.c. Is the AlF bond ionic, polar covalent, or nonpolar covalent?d. Write the name of the compound formed from aluminum and fluorine..e. Is this compound ionic, polar covalent, or nonpolar covalent?f. Is this compound water soluble? ( give the all answer with stepwise and type the answer.)arrow_forwardFor each molecule below, a. Draw the lewis structure, using wedges and dashes to indicate the VSEPR shape as necessary. b. Draw the bond dipole for all polar bonds. c. Determine if the overall molecule is polar or nonpolar. first molecule: H₂ second molecule: CO₂ third molecule: H₂Oarrow_forward
- 1. The chemical formula of methane is CH4. The Lewis Structure of methane is shown below. Explain how a chemical formula differs from a Lewis structure. H-C-H H 2. Draw a Lewis structure for the following molecules. Include the total number of valence electrons for each molecule. Show all your work. a.PH3 b.CS2arrow_forward1. Write the Lewis symbol for each atom or ion below. a. carbon b. nitrogen with -3 charge С. C. potassium with +1 charge d. sulfurarrow_forwardUse covalent Lewis structures to explain why each element (or family of elements) occurs as diatomic molecules.a. hydrogen b. the halogens c. oxygen d. nitrogenarrow_forward
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