Draw a Lewis structure that obeys the octet rule for each of the following ions. Assign formal...
Question:
Draw a Lewis structure that obeys the octet rule for each of the following ions. Assign formal charges to each atom.
{eq}1.\ ClO_3^-\\ 2.\ ClO_4^-\\ 3.\ NO_3^-\\ 4.\ NH_4^+ {/eq}
Lewis structure:
More than one Lewis structure is possible for a molecule which depends on octet rule and formal charges. If formal charge on atoms is neutral, and if octet rule is satisfied, the structure is stable.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answer
1. For {eq}{\rm{Cl}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}, {/eq} Cl has 7 valence electrons, O has 6 valence electrons. Total valence electrons are 25+1...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Lewis Structures: Single, Double & Triple Bonds
from
Chapter 5 / Lesson 8
70K
Learn to depict molecules and compounds using the Lewis structure. Explore the relationship between the octet rule, valence electron, and the electron dot diagram.
Related to this Question
- Write a Lewis structure that obeys the octet rule for each of the following ions. Assign formal charges to each atom. \\ A.\ NO_3^-\\ B.\ NH_4^+\\ C.\ C
- Draw a Lewis structure for SO2 in which all atoms obey the octet rule. Show formal charges.
- Draw the Lewis structures for each of the following molecules or ions. Which do not obey the octet rule? (a) NO. (b) AlH_3. (c) ICl_2^-. (d) OPBr_3 (the P is the central atom). (e) XeF_4.
- Draw a Lewis structure that obeys the octet rule for each of the following ions. Assign formal charges to each atom. DO NOT use any double bonds in this ion to reduce formal charges. ClO3-
- Draw a Lewis structure for PSBr3 in which the octet rule is satisfied on all atoms and show all non-zero formal charges on all atoms.
- Draw the Lewis structure and indicate whether or not the molecule satisfies the octet rule. BeCl_2.
- Draw a Lewis structure for BrO_4^(-), in which the octet rule is satisfied on all atoms. Show all nonzero formal charges on all atoms. Note that the overall charge on this ion is -1.
- Draw the Lewis structure for NO2 and determine whether or not it satisfies the octet rule.
- Draw a Lewis structure that obeys the octet rule for each of the following ions. Obeying the octet rule may mean that the structure you draw is not the most stable or ideal for the given molecule. Ass
- Draw the Lewis structure and indicate whether or not the molecule satisfies the octet rule. NO^+.
- Draw a Lewis structure for SO2(CH3)2 in which the octet rule is satisfied on all atoms and show all NONZERO formal charges on all atoms.
- Draw a Lewis structure for SO2 in which all atoms obey the octet rule. Show formal charges. Do not consider ringed structures.
- Draw the Lewis structure for the bromate ion BrO3- obeying the octet rule and then draw it when it breaks the octet rule but minimizes formal charges.
- Draw the Lewis structure for AsF5 and determine whether or not it satisfies the octet rule.
- Draw the Lewis structures for BeH2 and determine whether or not it satisfies the octet rule.
- Draw the Lewis structure for the following ion. Be sure to include all lone pair electrons and nonzero formal charges. S_2^2-
- Draw a Lewis structure for BrO3- that obeys the octet rule. Assign oxidation numbers to each atom.
- Draw a Lewis structure for OCS that obeys the octet rule. Assign oxidation numbers to each atom.
- Draw the best Lewis structure for NCCH2C(O)CH2CHO, a neutral molecule. Show all atoms, bonds, lone pairs, and formal charges.
- Draw a Lewis structure for HClO2 that obeys the octet rule. Assign oxidation numbers to each atom.
- Draw the Lewis structure for HBrO2 and assign formal charges to each atom.
- Draw Lewis structures for SeF_6 and include all-electron lone pairs. Is the octet rule satisfied in each case?
- Write Lewis structures that obey the octet rule for each of the following, and assign oxidation number, and formal charges to each atom: (a) OCS, (b) SOCl_2 (S is the central atom), (c) BrO_3^-, (d) HClO_2 (H is bonded to O).
- Draw the Lewis structures for KrF2 that obey the octet rule and show all resonance forms.
- Draw the Lewis structure for CH3O- and determine the formal charge of each atom.
- Draw the Lewis dot structure for acetamide, CH3CONH2, and determine the formal charge of each atom of this molecule.
- Write Lewis structures that obey the octet rule for the following species. Assign the formal charge for each central atom. (a) P O C l 2 (b) S O 2 4 (c) C l O 4 (d) P O 3 4
- Draw the Lewis structure and indicate whether or not the molecule satisfies the octet rule. PF_3
- Draw lewis structures of the ions or molecules whose formulas are given in the answer choices below. Determine whether each of these species follows the octet rule, is octet deficient (central atom works with less than eight electrons in its valence shell
- Draw and explain the Lewis structure for the molecule ICl2-, which does not follow the octet rule.
- Draw and explain the Lewis structure for the molecule BCl3, which does not follow the octet rule.
- Draw and explain the Lewis structure for the molecule XeF4, which does not follow the octet rule.
- Write a Lewis structure for each of the following ions. Assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge. a) PO4^3- b) SO3^2-
- Draw Lewis structures for the following compounds. State the number of valence electrons in each compound.
- Draw Lewis structures for SeF_4 and include all-electron lone pairs. Is the octet rule satisfied in each case?
- Do the following questions. 1) Draw a Lewis structure for a molecule that obeys the octet rule. 2) Recognize a structure that requires an expanded octet. 3) Calculate formal charge for the atoms in
- Draw Lewis structures that obey the octet rule for the following species. Assign the formal charge to each central atom. a. POCl_3. b. SO_4^2-. c. ClO_4^-. d. PO_4^3-. e. SO_2Cl_2. f. XeO_4. g. ClO_3^-. h. NO_4^3-.
- Draw the best Lewis structure (include formal charges) for the following molecule: KBH_3CN.
- Draw a Lewis structure for the following compound. Include all lone pair electrons. PF_3C_2F_4
- Draw a Lewis structure for the following compound. Include all lone pair electrons. SbH_3
- Draw and explain the Lewis structure for the arsonium ion, AsH4+. Assign formal charges to all atoms in the ion.
- Draw Lewis structures of the ions or molecules whose formulas are given in the answer choices below. Determine whether each of these species follows the octet rule, is octet deficient (central atom wo
- Draw a Lewis structure for NHF_2 in which the central N atom obeys the octet rule, and answer the following questions based on your drawing. The number of lone pairs on the central N atom is: _ The c
- Write Lewis structures that obey the octet rule for each of the following molecules and ions. (In each case the first atom listed is the central atom.) a. POCl_3, SO_4^{2-}, XeO_4, PO_4^{3-}, CIO_4^- b. NF_3, SO_3^{2-}, PO_3^{3-}, CIO_3^- c. CIO_2^-, SCl_
- Draw a Lewis dot structure for each of the following elements. Identify what net charge each element would adopt to achieve the valence electron configuration of a noble gas (achieve a stable octet). a. Li b. F c. Mg d. Cl e. K f. S g. Ca
- Draw the Lewis structure for CN- and determine the formal charge of each atom.
- Please write down the Lewis structures for the following. Indicate the formal charge on the atoms and point out the exceptions to octet rule and draw all the possible resonance structures where possib
- Draw Lewis structures for each of the following species. Show the formal charges of all atoms in the correct structure. Include all lone pairs of electrons. A) AsF6^- B) Cl3PO C) IF5
- Draw the Lewis Structure for the following molecules and ions and calculate their formal charge. If there is more than one possible Lewis structure, choose the one most likely preferred. a. NO^+. b. CH_3CH_2O^-. c. CH_2O. d. HCN. e. NCO^-.
- Draw the dominant Lewis structure and calculate the formal charge on each atom. a. CO b. SO_4^- c.NH_4^+
- Draw the Lewis structure for each of the following molecules and ions. (a) ( C H 3 ) 3 S i H (b) S i O 4 4 (c) S i 2 H 6 (d) S i ( O H ) 4 (e) S i F 2 6
- Draw the Lewis structure and indicate whether or not the molecule satisfies the octet rule. NO_2^- (nitrite ion).
- Draw the Lewis structure of the formate ion, HCO_2-. (Assign lone pairs, radical electrons, and atomic charges where appropriate.)
- Draw one valid Lewis structure (including all lone pair electrons and any formal charges) for CH_3NO_2.
- Draw a lewis structure for BrO_4^- in which all atoms have the lowest formal changes. Indicate the values of nonzero formal charges and include lonepair electrons.
- Draw a Lewis structure for each of the following molecules. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons. PH_3, SCl_2, F_2, HI, C_2H_2, C_2H_4, N_2H_2, N_2H_4.
- Draw the Lewis structure for CN^+. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of an electron and nonbonding electrons. Show the formal charges of all nonhydrogen atoms in the correct structure.
- Write a Lewis formula for each of the following, assuming that the octet rule holds for the atoms. Then obtain the formal charges of the atoms. a. O_3. b. CO. c. HNO_3.
- Draw the Lewis structure of SO2 that obeys the octet rule. Which electrons are bonding and which are non-bonding? What is the shape of this molecule?
- (a) Draw the Lewis dot structure for (CH_3)_2S. (b) Does it have 20 valence electrons?
- Draw a Lewis structure for each of the following compounds. Include all lone pair electrons in your structure. (a) CH_4S (b) S_2Cl_2 (c) CHCl_3.
- Draw one valid Lewis structure (including all lone pair electrons and any formal charges) for CH_2N_2. Assume the atoms are arranged as shown below.
- Draw a Lewis structure for each of the following sets. Use formal charge to determine which is best. a) H_3SCH \text{ and } H_3CSH b) 3 structures of phosphate ion (1st with 1 double bond, 2nd with 2 double bonds, 3rd with 3 double bonds)
- Draw the Lewis structure for SO2. Show all lone pairs and locate any formal charges. Determine the number of valence electrons, give the overall shape of the molecule, and indicate whether the molecule is polar or nonpolar.
- Draw the Lewis structure with a formal charge XeF_4.
- Draw the Lewis structure for C_2^{2-} and find the formal charges for each carbon atom.
- Draw one valid Lewis structure (including all lone pair electrons and any formal charges) for Assume the atoms are arranged as shown below.
- Draw the Lewis structure for the sulfur trioxide (SO_3) molecule. Be sure to include all resonance structures that satisfy the octet rule.
- Draw the Lewis structure with the lowest formal charges for the compound below. Include nonzero formal charges and lone pair electrons in the structure. (Image)
- Draw Lewis structures for these molecules that show all of their valence electrons. (a) C2H6 (b) CS2 (c) HCN
- Draw the Lewis structure for the ions in NF4SbF6.
- Write Lewis structures for BrF3, ClF5, and IF7. Identify those in which the octet rule is not obeyed.
- Draw the Lewis structure for CO. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.
- Write a Lewis structure for each atom or ion. Cl Draw the particle atoms on the grid and connecting them with bonds. Including all lone pairs of electrons and nonbonding electrons.
- Draw a Lewis structure for CO^2-_3 in which the central C atom obeys the octet rule, and answer the following questions based on your drawing. The number of unshared pairs (lone pairs) on the central
- Write the Lewis structure for the Formate ion, HCOO^-. Show all valence electrons and all formal charges.
- Draw the Lewis dot structures for each of the following molecules. Show the steps for each including total valence electrons, number of electrons wanted by each atom. a) NOCl b) CH3Br
- Draw all of the Lewis structures of SeO3 that obey the octet rule and use this Lewis structure or these resonance structures to predict how many covalent bonds connect each oxygen atom in the real structure to the central Se atom. Assume that the ...
- Draw the Lewis structure for NH2- and determine the formal charge of each atom.
- Draw the Lewis structure for HCO2- and determine the formal charge of each atom.
- Draw the best Lewis structure for CH3CHC(OH)CH2CO2H, a neutral molecule. Complete the lewis structure in that order and show hydrogen bonds.
- Draw a Lewis structure; fill in any nonbonding electrons for [N3]-(azide ion). Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons and an
- Draw the Lewis structures for each of the following ions or molecules. Give the number of electrons in each species. Remember to enclose ions in square brackets with the charge as a superscript outside the right bracket. (a) POF_3 (P is the central atom)
- Write a Lewis formula for each of the following, assuming that the octet rule holds for the atoms. Then obtain the formal charges of the atoms. a. ClNO. b. POCl_3. c. N_2O (NNO).
- Draw the Lewis structure for OPBr_3. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.
- Draw the Lewis structures and determine which of these molecules has a central atom that unavoidably violates the octet rule. Please note that NO_3 has an odd number of electrons. But you must decide
- Draw the Lewis dot structure for (CH3)4NCl. Show non-bonding electrons and formal charges where appropriate.
- Draw the best Lewis structure of [(CH3)3O]^+); fill in any nonbonding electrons. Calculate the formal charge on each atom other than hydrogen. Draw the molecule by placing atoms on the grid and conne
- Draw a lewis structure for the most important resonance form of the following ion, showing formal charges and oxidation numbers of the atoms, AsO_4^{3-}.
- Draw a Lewis structure for NH_4^+ in which the central N atom obeys the octet rule, and answer the following questions based on your drawing. The number of unshared pairs (lone pairs) on the central...
- Draw the Lewis structure for PCl5 and determine whether or not it satisfies the octet rule.
- Draw a Lewis structure for CH_4 in which the central C atom obeys the octet rule, and answer the following questions based on your drawing. The number of lone pairs on the central C atom is: .......
- Draw a Lewis structure for SO2 in which all atoms have a formal charge of zero.
- A) XeO_4 B) PO_3^(-) C) NO Draw Lewis structures for the formula above. Include any resonance structures. If more than one Lewis structure can be drawn, use formal charges to decide on the most preferred Lewis structure.
- Draw the Lewis structure with a formal charge H_2CO.
- Draw and explain the Lewis structure for the ClO2 molecule, which is an exception to the octet rule.
- Draw a Lewis structure for one important resonance form of HBrO_4\ (HOBrO_3). Include all lone pair electrons in your structure. Do not include formal charges in your structure.
- Draw the Lewis structure for the Ga3+ ion.
- Draw a Lewis structure for each ion. a. CH3O- b. (HC2)- c. (CH3NH3)+ d. (CH3NH)-
Explore our homework questions and answers library
Browse
by subject