The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. We can draw three inequivalent Lewis structures for the sulfite ion, SO32. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. Formal Charge S 0₁ 0₂ 03 A :0: 2. The best Lewis structure for SO3²- is A . B –8: • Previous Next

Draw Lewis structure(s) for the carbonate lon (CO₂). If there are equivalent resonance structures, draw all of them. n D co₂2: 0 . Draw one structure per sketcher box, and separate added sketcher boxes with the symbol. Do not include overall lon charges or formal charges in your drawing. Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. ● 6 # H Ⓒ CH, CHO: 0 Y Chemic b Draw Lewis structure(s) for the acetaldehyde molecule (CH₂CHO). If there are equivalent resonance structures, draw all of the POLICE 81 MEDITE HARA (4) Y Draw one structure per sketcher box, and separate added sketcher boxes with the symbol. Do not include overall ion charges or formal charges in your drawing. Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. ARQQA 000-ZIF www HEADING Chartlkoodn MES DE A V Ja remove 000-n [ MacBook Air

Draw three resonance structures for N3-. This species has its three atoms bonded sequentially in the following fashion: N-N-N. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Now select the statement from the multiple choices which is true about this most important resonance structure.In the most important resonance structure of N3- : a) The leftmost bond (between N and N) is a single bond.b) The rightmost bond (between N and N) is a single bond.c) The formal charge on the leftmost (N) atom is -1.d) The number of nonbonding pairs (lone pairs) of electrons on the leftmost (N) atom is 4.e) The number of nonbonding (lone) pairs of electrons on the rightmost (N) atom is 4.

Use the figure to find the electronegativity difference between each of the following pairs of elements, then use the table below to classify the bonds that occur between them as pure covalent, polar covalent, or ionic.   Electronegativity Difference (ΔENΔEN) Bond Type Example zero (0−0.40−0.4) pure covalent Cl2Cl2 intermediate (0.4−2.00.4−2.0) polar covalent HFHF large (2.0+2.0+) ionic NaClNaCl   Find the electronegativity difference between K and Cl. Express your answer using two significant figures.

Draw the best Lewis Structure for ClO4– based on overall formal charges.  Answer the questions below based on that structure.  How many (total) bonding electron pairs are in the molecule?    _______ How many (total) non-bonding electron pairs are in the molecule? _______ How many non-bonding electron pairs are on the central atom? _______

9. Draw all the possible resonance structures for the iodate ion. How many resonance structures can you have in total for iodate?

A newly discovered element Lm has 3 valence electrons. How many total valence electrons are in LmF3 molecule, a molecule that Lm forms with fluorine?  Draw a valid Lewis Structure for the molecule LmF3 that Lm forms with fluorine and use your Lewis structure to determine the number of lone pairs of electrons around the central Lm atom in this molecule.  What is the formal charge of Lm in LmF3? (Number and sign of formal charge) What is the hybridization of Lm according to the hybrid orbital model?

The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. Use the References to access important values if needed for this question. We can draw three inequivalent Lewis structures for dinitrogen monoxide, N₂O . The concepts of formal charge and electronegativity can help us choose the structure that is the most significant representation. 1. Assign formal charges to the elements in each of the structures below. Formal Charge N₁ N₂ :N,=N,-O: || A N=N,=Ô N-N,=O: C 2. The structure that contributes most significantly to the overall electronic structure of N₂O is ↑ Formal Charge

ng and lear X G The element in period 5 that has X C Solved The following Lewis diagr. X nt/takeCovalentActivity.do?locator-assignment-take The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. Formal Charge 01 We can draw three inequivalent Lewis structures for carbon dioxide, CO₂. The concepts of formal charge and electronegativity can help us choose the structure that is the most significant representation. 1. Assign formal charges to the elements in each of the structures below. C [Review Topics] [References] Use the References to access important values if needed for this question. 02 :0₁-C=0₂: A 0,=C=0₂ :0,=C-0₂: + B 999 C *** 2. The structure that contributes most significantly to the overall electronic structure of CO₂ is. AG ENG neme Next 11:52 AM 11/28/2022 [

a. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of XeO4. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: b. Write a Lewis structure that obeys the octet rule for the following species. Assign the formal charge for the central atom of clO3¯. If multiple resonance structures exist, use one that does not involve an expanded valence. Formal charge: