Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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Chapter 13, Problem 4ASA
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
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Draw a Lewis structure for BF3 that obeys the octet rule if possible and answer the following questions based on your drawing.
1. For the central boron atom:
- The number of lone pairs = ?
- The number of single bonds = ?
- The number of double bonds = ?
2. The central boron atom is
a. obeys the octet rule.
b. has an incomplete octet.
c. has an expanded octet.
Draw a Lewis structure for SO2 that obeys the octet rule if possible and answer the following questions based on your drawing.
1. For the central sulfur atom:
- The number of lone pairs = ?
- The number of single bonds = ?
- The number of double bonds = ?
2. The central sulfur atom
a. obeys the octet rule.
b. has an incomplete octet.
c. has an expanded octet.
A. State the Octet Rule.B. Write the Lewis symbol of neon. Is the neon atom stable? Does neon exist as atoms in nature? If not, how does neon exist in nature.C. Write the Lewis symbol of nitrogen. Is the nitrogen atom stable? Does nitrogen exist as atoms in nature? If not, how does nitrogen exist in nature.
Chapter 13 Solutions
Chemical Principles in the Laboratory
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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
- In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.arrow_forwardFor three simple molecules of your own choice, apply the rules for writing Lewis structures. Write your discussion as if you are explaining the method to someone who is not familiar with Lewis structures.arrow_forwardOn the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent. msp;a.HOc.HHb.OOd.HClarrow_forward
- Question 39 and 40 are two different questions.arrow_forwardQuestion 82arrow_forward1. Consider the structure shown below and then answer the following questions. a. Complete the structure by adding the missing formal charges. All atoms and lone pairs are explicitly shown. (Hint: Consider the number of bonds neutral atoms have.) :Ö: H ‚H H H b. Draw two more resonance structures of the molecule from part a by adding the missing î bonds, lone pairs, and formal charges. All atoms in both structures should possess an octet. (All atoms and o bonds are drawn for you; remember, only lone pairs and bonds move in resonance structures.) Additional guidelines are given for each structure. All atoms in this structure will be neutral (no formal charges). One oxygen atom has a +1 formal charge and one oxygen atom has a -1 formal charge. H H H H H H H H Harrow_forward
- With regard to resonance structures that are drawn for a real species, which of the following statements is NOT TRUE? Select one: A. Resonance structures differ in the location of their electrons, not the positions of their atoms. B. Resonance structures are only drawings; each structure alone does not represent an existing molecule. O C. Resonance structures are real molecules that co-exist in equilibrium with each other. O D. Resonance structures all have electron localized structures, while the real species that is described by them has delocalized electrons.arrow_forwardThe element sulphur has atomic number 16. Sulphur forms a molecular compound with chloride witha molecular formula SCl2. The atomic number of chlorine is 17.i. Write down the electronic configuration of a sulphur atom and a chlorine atom.ii. Draw a Lewis structure of an SCl2 molecule, by showing the electrons in the outer shells of theatoms.iii. State how many bond pairs and lone pairs of electrons are arranged around the sulphur atomsin SCl2 molecule.iv. Sketch the shape and state the molecular geometry of SCl2 molecule.v. Explain the hybridisation of the central atom in SCl2 molecule.vi. Explain the intermolecular forces exists in SCl2 moleculearrow_forwardAnswer both partsarrow_forward
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