CH3CH2NH2 Practice 17 For the compounds below identify all covalent and all ionic substances NaHCO3 CH,CH,NH, CF₁ CH,COONa • Explain, using one of the covalent compounds as an example, how you came to an inference that it is covalent. Make sure to discuss why it cannot be ionic in terms of the valence electrons each atoms has and how covalent bond allows it to obtain stability. • Explain, using of the ionic compounds above as an example, rationale for your decision that it is ionic. Make sure to discuss how and why atoms become ions and why covalent bond is not possible in this case. . For all covalent compounds above draw Lewis structures showing correct number of bonds and lone pairs for each atom H √" H- 1 H H 1 -C-N-H I I H "" F-C-F • For all ionic compounds determine and show charges of mono and polyatomic ions. Draw Lewis structures for all polyatomic ions. 15

CH3CH2NH2 Practice 17 For the compounds below identify all covalent and all ionic substances NaHCO3 CH,CH,NH, CF₁ CH,COONa • Explain, using one of the covalent compounds as an example, how you came to an inference that it is covalent. Make sure to discuss why it cannot be ionic in terms of the valence electrons each atoms has and how covalent bond allows it to obtain stability. • Explain, using of the ionic compounds above as an example, rationale for your decision that it is ionic. Make sure to discuss how and why atoms become ions and why covalent bond is not possible in this case. . For all covalent compounds above draw Lewis structures showing correct number of bonds and lone pairs for each atom H √" H- 1 H H 1 -C-N-H I I H "" F-C-F • For all ionic compounds determine and show charges of mono and polyatomic ions. Draw Lewis structures for all polyatomic ions. 15

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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From the Lewis structures of the species given, pick all of those in which the central atom obeys the octet rule. :ci: :ci: ci: .. :CI: H-C-H H H-B-H None of the Above HI :o:
Could someone help me?? The answer to this question must look similar to the example attached. Back ground info: Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation. The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron…
Consider the structure of the given ion. Lo What is an appropriate resonance structure of the ion? Select one: H-C - :0:
1 What is the total number of valence electrons in the Lewis structure of BrO4"? electrons 2 Draw a Lewis structure for BrO4 • Do not include overall ion charges or formal charges in your drawing. • If the species contains oxygen, do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. 0- Y **** O. Sn [1 2. Draw Lewis Structures (Octet and Nonoctet): This is group attempt 1 of 5
Number 3 4 and 5 for pratice Lewis for structure and vsepr
O ELECTRONIC STRUCTURE AND CHEMICA... Deciding whether a Lewis... Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure [O=C-H]* :0: : CIC CI: [¤¤-6: 0/5 Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: 0 No, it has the right number of valence electrons but doesn't satisfy the octet rule. 000 The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: 0 Alia V No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* X Ar If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example,…
Question 12 of 21 View Policies Show Attempt History Current Attempt in Progress. Use Lewis symbols to diagram the formation of Cal2 from Ca and I atoms. Ca2+ 2|:: | Ca: 2|:1:| Ca2+ + Ca2+ 2|::| Ca: Ca* + 2[: | eTextbook and Media Hint P Type here to search O a
Show how these elements combine into octet-rule ionic compounds, as in the first example. First, draw atomic Lewis structures for the atoms and their O.R. ions. Show their charges, and use them to find the unit formula, and the name. Then draw atomic Lewis structures for all atoms in the formula unit together, show with arrows how all e s are transferred to make the ions, and draw the Lewis structure of the ionic compound. Unit formula Atoms O.R. ions Name Transfer e s with arrows Lewis Structure LizN le 1e 30 Lithium Li. + •N• Li. •N• Li. Li 30 Li Li Li :N: nitride )le Li. Pb and K and H
=q req Preq Visited F3 To answer the questions, interpret the following Lewis structure for SF6. F4 1. For the central sulfur atom: The number of lone pairs The number of single bonds = The number of double bonds= Submit Answer [References) Use the References to access important values if needed for this a 2. The central sulfur atom % Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support F5 A F6 & F7 * ∞ F8 F9
Use the References to access important values if needed for this question. Please note that "geometry" refers to the molecular or ionic geometry. 3- A. The Lewis diagram for PO4³- is: :0: B. The Lewis diagram for NO3" is: :0: 3- The electron-pair geometry around the P atom in PO4³- is Submit Answer There are lone pair(s) around the central atom, so the geometry of PO4³- is 3- 3- :0: Recall that for predicting geometry, double and triple bonds count as only one electron pair. The electron-pair geometry around the N atom in NO3 is There are lone pair(s) around the central atom, so the geometry of NO3™ is Retry Entire Group 9 more group attempts remaining
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