Counting bonding and nonbonding electron pairs in a Lewis...Below is the Lewis structure of the peroxide:0:0le (0₂-) ion.Count the number of bonding pairs and the number of lone pairs around the right oxygen atom.bonding pairs:lone pairs:X50/5

Peroxides are compounds that contain the peroxide ion(O22), which is a molecule of two oxygen…

Answered: Below is the Lewis structure of the…

Below is the Lewis structure of the peroxide (02-) ion. [0:0] Count the number of bonding pairs and the number of lone pairs around the right oxygen atom. bonding pairs: lone pairs: X

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 98QRT

See similar textbooks

Related questions

Q: For each of the following two substances NOCl and SF6 answer the following questions: Draw Lewis…

A: Lewis structure is a method of showing bonding pattern in the molecule. in this , we demonstrate…

Q: Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving…

A: LEWIS STRUCTURE FOR OH free radical Total number of the valence electron in OH free radical =…

Q: Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure :Z: I :Z:…

A: We have to complete the table below using the octet rule.

Q: H-0-F: Draw the correct Lewis structure for HOF, including all lone pairs of electrons.

Q: P ed Lewis structure -C-C- – H H-C [H_H_O_H]* N_o_a -a: Is the proposed Lewis structure reasonable?…

A: Lewis structures are the diagrams in which the total valence electrons of the molecule are depicted…

Q: cide whether the Lewis structure proposed for each molecule is reasonable or not. molecule 13 BH₂…

Q: following fashion: N-N-O. Draw your resonance structures so that the atoms in them are bonded…

Q: Formula SO3 HCN NO₂ AsCl5 #VES Lewis Structure Resonance? (Y/N) Show Electron Group & Bond Angle…

Q: Indicate the direction of polarity of each of the covalent bonds by placing the appropriate delta…

A: This question based upon the concept of Electronegativity : It is defined as the tendency of an atom…

Q: Draw Lewis structures for each of the following. Use the DEN and the number of REDs around the…

A: Lewis Structure is a very simple representation of the valence shell electrons in a molecule.

Q: least polar bond using electronegativities. F - 4.0

A: Given, F - 4.0 O - 3.5 N - 3.0 Cl - 3.0 S - 2.5 I - 2.5 P - 2.1 Li - 1.0 Na - 0.9

Q: How many lone pairs are there on the central C atom in the Lewis structure for CH4 ? How many lone…

A: We have been given a molecule CH4. We have been asked number of lone pairs present on central C atom…

Q: I am not sure if I'm right on the answers I did. Thanks for helping.

Q: Draw regular Lewis structures (no need to use dashed lines and wedges) of the following ions and…

A: Draw lewis structure, electronic geometry and molecular geometry

Q: H3C. H3C CH3

A: Rules for determining the important/stable resonance structure: 1. Uncharged structure is more…

Q: c1

A: Lewis structure is a method of representing bonding pattern in a molecule. It tells us how…

Q: Below is the Lewis structure of the peroxide (O2−2) ion. Count the number of bonding pairs and the…

A: Definition of lewis structure : A Lewis Structure is simple representation of the valence shell…

Concept explainers

Types of Chemical Bonds

The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds. 

Polarizability In Organic Chemistry

Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.

Coordinate Covalent Bonds

A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.

Question

Counting bonding and nonbonding electron pairs in a Lewis...
Below is the Lewis structure of the peroxide
:0:0
le (0₂-) ion.
Count the number of bonding pairs and the number of lone pairs around the right oxygen atom.
bonding pairs:
lone pairs:
X
5
0/5

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Introduction to peroxide ion

VIEW

Step 2: Counting bonding and non-bonding electron pairs

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

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

Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?
Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
Draw the bonding pattern for the third resonance structure of the azide ion, N3. Two of the resonance structures are shown below. (Include double/triple bonds and any formal charges.) Edit Drawing eTextbook and Media N=N_N?²- A How many lone pair electrons are on the central nitrogen atom? # of lone pair electrons on the central nitrogen atom: -Ń=N: B How many lone pair electrons are on the each of the other two nitrogen atoms? # of lone pair electrons on each of the other nitrogen atoms: Why do both bonds of the azide ion have the same length? O The bond lengths are the same because the resonance structure you drew was tetrahedral. O The bond lengths are the same because single, double, and triple bonds are always the same length. O The bond lengths are the same because structures A and B are equivalent and therefore make equal contributions to the hybrid.
molecule OF 2 AlCl3 SF 3 proposed Lewis structure || : 0: :F: || : Cl: : Cl Al - Cl: :F: Is this a reasonable structure? If not, why not? Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: Yes, it's a reasonable structure. 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: Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are:
= O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Counting bonding and nonbonding electron pairs in a Lewis... Below is the Lewis structure of the methoxide H H:C:O: H e (CH₂O) ion. Count the number of bonding pairs and the number of lone pairs around the carbon atom. bonding pairs: lone pairs: X Ś 1/5
Draw the bonding pattern for the third resonance structure of the azide ion, N3. Two of the resonance structures are shown below. (Include double/triple bonds and any formal charges.) Edit Drawing eTextbook and Media NEN-N: A How many lone pair electrons are on the central nitrogen atom? # of lone pair electrons on the central nitrogen atom: 0 2-:N-N=N: B How many lone pair electrons are on the each of the other two nitrogen atoms? # of lone pair electrons on each of the other nitrogen atoms: 4 Why do both bonds of the azide ion have the same length? O The bond lengths are the same because the resonance structure you drew was tetrahedral. O The bond lengths are the same because single, double, and triple bonds are always the same length. The bond lengths are the same because structures A and B are equivalent and therefore make equal contributions to the hybrid.
Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure .. :Z: || :Z: H = Br N101 C1: O оо Is the proposed Lewis structure reasonable? O 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:* Yes. No, it has the wrong number of valence electrons. The correct number is: O 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:* No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * 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,0".
?deploymentid=5735112480241329813180832311&eISBN=9781305862883&id=1774598910&snapshotl... The enthalpy change for the following reaction is 66.4 kJ. N₂(g) + 2 O₂(g) →→→2 NO₂(g) ck a To analyze the reaction, first draw Lewis structures for all reactant and product molecules. O • Draw the reaction using separate sketchers for each species. Separate multiple reactants and/or products using the + sign from the drop-down arrow. • Separate reactants from products using the symbol from the drop-down menu. • Remember to include nonbonding valence electrons in your Lewis structures. C Submit Answer 8 //-000- [F ChemDoodle b Estimate the N=O bond energy in NO₂(g), using tabulated bond energies (linked above) for the remaining bonds. N=O bond energy = remove kJ/mol alculate Bond Energy from Enthalpy of Reaction - Draw Lewis: This is group attempt 1 of 10 Autosaved at 9:11 PM
What possible error(s) exist in the Lewis structure (assume we are trying to represent the best possible Lewis structure for the NO₂S ion knowing N is the central atom in this polyatomic ion)? [:ö==S: N= CO :O: The best structure would have double bond and two lone pairs on each oxygen atom and a single bond with three lone pairs on the sulfur. There are no errors. This is the best possible structure. The Lewis structure above does not minimize formal charges, thus is the not the best possible structure. The nitrogen atom has an expanded octet, and this structure is impossible. The Lewis structure contains the wrong number of electrons, thus this structure is impossible.
Decide whether the Lewis structure proposed for each molecule is reasonable or not. Note: 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 necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.
Below is the Lewis structure of the methoxide H H H:C:O: Count the number of bonding pairs and the number of lone pairs around the carbon atom. bonding pairs: lone pairs: (CH₂O¯) ion. X