Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules and ions. Draw a Lewis structure for SF2 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

Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules and ions. Draw a Lewis structure for SF2 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

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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In at least one sentence, explain what happens when a potassium atom becomes a monatomic ion. In your response, answer the following questions: a. How many valence electrons does potassium have? b. How many electrons does it lose or gain to obey the octet rule? C. What noble gas atom has the same number of electrons as the potassium ion? d. Is the potassium ion a cation or an anion?
For each row in the table below, decide whether the pair of elements will form a molecular compound held together by covalent chemical bonds. If the elements will form a molecular compound, check the box and enter the chemical formula and name of the compound. (If the elements will form more than one molecular compound, use the compound with the fewest total number of atoms.) You may assume all chemical bonds are single bonds, not double or triple bonds. element pair will form a molecular compound element #1 element #2 molecular chemical name compound formula calcium chlorine hydrogen iodine sulfur bromine
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= ELECTRONIC STRUCTURE AND CHEMICAL BONDING Counting electron pairs in a Lewis structure with double or tripl... Below is the Lewis structure of the hydrogen cyanide (HCN) molecule. H:C:::N: Count the number of bonding pairs and the number of lone pairs around the carbon atom in this molecule. bonding pairs: lone pairs: 0 X 3/5
Part 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!
Ions: Transfer of Electrons Element Atomic # 1. Electron Configuration of Atom 2. Electron- Dot Symbol 3. Loss or Gain 4. Electron Configuration of Ion 5. Ionic Charge 6.Symbol of Ion 7. Nameof Ion Sodium 11 1+ Na 1+ Sodium ion Nitrogen 7 N Aluminum 13 Al Chlorine 17 Cl Calcium 20 Ca Oxygen 8 O
A. Draw the Lewis Dot Structure of the molecule or ion OF2 B. Find the shape of the molecule or ion OF2 C. Draw the Lewis Dot Structure of the molecule or ion CH2F2 D. Find the shape of the molecule or ion CH2F2 E. Draw the Lewis Dot Structure of the molecule or ion PO3^-3 F. Find the shape of the molecule or ion PO3^-3
이 %%$ . —Br-O Choose a possible Lewis structure for each of the following polyatomic ions. All bonding valence electron pairs are shown as lines and all nonbonding valence electron pairs as dots. a. Bromite ion, BrO₂. ] T 1 b. Perbromate ion, BrO4. 1:0- 0-Br-o :0 Ö-Br-O :0-Br-Ö: o' o-Br .O. O o Br Show Hint o Te importance of... -0. [Review Topics] Untitled document... [References] B Sports Injuries Ant... Previous Next Save and Exit FTSTOF
Discuss the three types of chemical bonds and then create a summary diagram that captures the main ideas of each (include polar covalent somewhere in your drawing). Use your white board first and then transfer your diagram here. -Non polar -Polar covalent -Ionic character
1. Write the Lewis dot (electron dot) symbol for each atom or ion. a. Mg b. Mg+2 C. N d. Br¹ e. He
QUESTION 3 Which of the following have more than one resonance structure? O A. SO42 (hint: there are two double bonds!) O B. CO2 (Only one bond length is observed experimentally) OC. C6H6 (the carbons form a hexagona and have one hydrogen each) O D. H20 O E. N20 (A nitrogen is in the middlel) OF. SO2
To answer the questions, interpret the following Lewis diagram for NHF, . H-N- 1. For the central nitrogen atom: The number of non-bonding electrons The number of bonding electrons The total number of electrons 2. The central nitrogen atom A. obeys the octet rule. B. has more than an octet. C. has less than an octet. I| ||||