Learning Goal:When covalent compounds, such as water (H₂O), form covalentDonds, they share valence electrons. A Lewis dot structure orelectron dot structure is a drawing that represents chemicalbonds between atoms as shared or transferred electrons, wherethe valence electrons are represented as dots. For example,notice the Lewis structure of NC13 (Figure 1). When a pair ofa bond.electrons is shared between two atoms, a line is drawn to indicatetabFigures lockResolving host...:C—N—C::C1:esccontrolaltF1optionZ2WSXHcommand#1 of 1320 F3$108090094EDCHow to draw a Lewis dot structureTo draw a Lewis dot structure, follow these steps:skeletal structure of water is shown here: H O H.1. Draw the skeletal structure of the molecule. The skeletal structure shows how the atoms of the molecule should be connected. For example, t2. Determine the number of electrons for the Lewis structure by summing the valence electrons of each atom the molecule..3. Distribute the electrons among the atoms, giving octets (or duets for hydrogen) to as many atoms as possible. According to the octet rule, atomtransfer or share electrons to obtain an outer shell that contains eight electrons. It is important to note that some atoms, including hydrogen, dofollow the octet rule. Hydrogen is stable when it contains two electrons.4. If any atoms lack an octet, form double or triple bonds as necessary to give them octets.Part AFor neutral molecules, which statements about covalent Lewis structures are true?Drag each item to the appropriate bin.View Available Hint(s)F4RTrueF%5For a neutral molecule, thenumber of electrons in theLewis structure is the sum of thevalence electrons for the atoms.VHydrogen atoms are often thecentral atom of a Lewis structure.F5TGBMacBook AirYH&Electrons of covalent compoundsmay be shared between atoms.7Each atom of a Lewis structuremust have eight electrons.FalseJNJ*00Reset8MкHelpF9VLF10command88{PF11. VReview I Constants IaltoptionF12Gdele

For neutral molecules, the following statement is correct about the Lewis Structure:

Part A For neutral molecules, which statements about covalent Lewis structures are true? Drag each item to the appropriate bin. View Available Hint(s) True For a neutral molecule, the number of electrons in the Lewis structure is the sum of the valence electrons for the atoms. Hydrogen atoms are often the central atom of a Lewis structure. Reset Help Electrons of covalent compounds may be shared between atoms. Each atom of a Lewis structure must have eight electrons. False

Part A For neutral molecules, which statements about covalent Lewis structures are true? Drag each item to the appropriate bin. View Available Hint(s) True For a neutral molecule, the number of electrons in the Lewis structure is the sum of the valence electrons for the atoms. Hydrogen atoms are often the central atom of a Lewis structure. Reset Help Electrons of covalent compounds may be shared between atoms. Each atom of a Lewis structure must have eight electrons. False

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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Predict the shape of CCl2H2based on VSEPR theory. Show your work using Lewis dot structure. Central atom is in Bold. After drawing the Lewis structures answer the following. CCl2H2 Central atom Number of bonds to the central atom Nonbonding pairs on the central atom Total bonds + nonbonding pairs Shape of the molecule
Hydrogen is in Group 1 of the periodic table. Which kind of bond would form between two hydrogens? O An ionic bond would form because both atoms are nonmetals. A covalent bond would form because the electron would be shared so both hydrogens have a fullI, stable shell. An ionic bond would form because one hydrogen would transfer its valence electron to the other hydroger make a full shell. O A metallic bond would form because both atoms are metals. P Type here to search の近

Part A For each formula, fill in the eight items listed in the instructions. The Lewis models (at least) should be completed before coming to lab. Be sure to consider the Lewis dot model and the ball-and-stick model as two separate items. The Lewis model should not attempt to indicate geometry. The ball-and-stick model does not need to show multiple bonds or the positions of lone pairs of electrons but should depict molecular geometry. Since ions have a net charge, the issue of polarity is usually unimportant for them. You can skip the polarity analysis for the ions. Fill in the all blanks!
Consider the resonance structures of formate. Select the true statements about the resonance structures. Each carbon-oxygen bond is somewhere between a single and double bond. Each oxygen atom has a double bond 50% of the time. The actual structure of formate is an average of the two resonance forms. The actual structure of formate switches back and forth between the two resonance forms. Incorrect
Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure Is the proposed Lewis structure reasonable? Yes. :0: No, it has the wrong number of valence electrons. | The correct number is: 0 : Cl - C Cl: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 Yes. No, it has the wrong number of valence electrons. The correct number is: H-O- H No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 O Yes. O No, it has the wrong number of valence electrons. JFRZ The correct number is: 0 N No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 * 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, if two oxygen atoms don't satisfy the octet rule, enter "0,0". :ܘ:…
To draw a Lewis Structure, start with the atomic symbol in the middle, then put dots around the symbol until all of the valence electrons are represented. Try to envision a box around the atom symbol, and the electrons on each side of the box. The valence electrons should be drawn around the element symbol one on each side before pairing the electrons up. The maximum number of electrons that could be on one side of a Lewis Structure is two, and the maximum number of electrons around an element symbol is eight. To figure out how many valence electrons each element has, use the Periodic Table. Remember, the number of valance electrons for Group A elements is equal to the Group A number the element is in on the Periodic Table. Use the data you collected in Table 1 to a draw Lewis structure model to show the formation of any one of the compounds you assembled, then explain the model you drew. Remember, you should be explaining and supporting your answers by referencing and citing the…
What it the main difference between an ionic and a covalent bond? Group of answer choices Both bonds are the same, but named different to describe different atoms involved. One is the sharing of a pair of electrons, the other is the transfer of at least one electron. The electrons are traded between the two atoms and this keeps the atoms close. One involves electrons, the other does not involve any electrons. The electrons in both types of bonding undergo an exchange.
Decide whether the Lewis structure proposed for each molecule is reasonable or not. proposed Lewis structure Is this a reasonable structure? If not, why not? molecule O Yes, it's a reasonable structure. :F: No, the total number of valence electrons is wrong. BF, The correct number is:| :F-B -F: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: L Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is:| O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: U O Yes, it's a reasonable structure. :F: No, the total number of valence electrons is wrong. CIF, The correct number is:| .. Cl –F: No, some atoms have the wrong number of electrons around them. : F The symbols of the problem atoms are:U * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as…
Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure fä=ö:] H- Br: |[H-H-Ö-H]" Is the proposed Lewis structure reasonable? 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:* 0 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:* 0 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:* 0 *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, if two oxygen atoms don't satisfy the octet rule, enter "O,O".
Write the electron dot structure for hydrogen monofluoride, HFa. What is the total number of available valence electrons?_______b. In the space below, write the atomic symbols, then add the bonding electron pair. Finally distribute the non-bonding electron pairs.
Identify the errors in each of the following Lewis structures and draw the correct formula. Draw the correct Lewis structure of this molecule by placing atoms on the canvas and connecting them with bonds. Include all hydrogen atoms and lone pairs of electrons.
Octet rule For elements in neutral molecules, the number of bonds needed to achieve an octet follows a trend by group, as shown in the following table: Group 4A 5A 6A 7A Number of bonds 4 3 2 1 Number of lone pairs 0 1 2 3 Part A Draw the Lewis structure for SiCl2 Br2. To add the element Si, either double click on any atom and type the element symbol, or access a periodic table of elements from the More button. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.