Concept explainers
Interpretation:
The Lewis structure for each of the given ions and molecules is to be explained.
Concept introduction:
The structure used to show the bonding between the atoms and a lone pair of electrons of amolecule is known as Lewis structure.
The rules for drawing the Lewis structure areas follows:
The skeletal structure of the compound is drawn, in which theelement with thelowest electronegativity is placed as thecentral atom, which is surrounded by the substituent atoms.
The total number of valence electrons for the compound is determined.
Subtract two electrons for each bond in the skeletal structure from thetotal number of valence electrons to know the remaining number of electrons.
Complete the octet of each terminal atom by placing a pair of electrons from the remaining electrons.
If any of the electrons are remaining after completing the octets of the terminal atoms, place the remaining electrons as a pair on the central atom.
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
Chemistry
- Part A) Which of the following molecules contain one pi bond? (a) CO (b) N2 (c) C2H4 (d) F2 (e) None of them Part B) According to the octet rule, which of elements listed below will have a tendency to lose 2 electrons? (a) oxygen (b) strontium (c) nitrogen (d) bismuth (e) None of those Part C) Using the following data: reactions DH°rxn (kJ) H2(g) + Cl2(g) → 2HCl(g) -184 H2(g) → 2H(g) 432 Cl2(g) → 2Cl(g) 239calculate the H – Cl bond energy. a) 770 kJ b) 856 kJ c) 518 kJ d) 326 kJ e) 428 kJ(e) None of the above. If so what is your answer?arrow_forwardPRACTICE EXAMPLE A: Write plausible Lewis structures for the following ions: (a) NO*; (b) N₂H; (c) 0². PRACTICE EXAMPLE B: Write plausible Lewis structures for the following ions: (a) BF; (b) NH¸OH*; (c ) NCO.arrow_forwardCyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forward
- Write Lewis structures for the following:(a) O2(b) H2CO(c) AsF3(d) ClNO(e) SiCl4(f) H3O+(g) NH4+(h) BF4−(i) HCCH(j) ClCN(k) C22+arrow_forwardThe sulfate ion, SO4 2-, can be drawn in many ways. If youminimize formal charge on the sulfur, how many S“Odouble bonds should you draw in the Lewis structure?(a) 0 (b) 1 (c) 2 (d) 3 (e) 4arrow_forwardDraw Lewis structures for HFO4, HFO3, HC0O4, HC0O3, HCO2. (These molecules have the halogen atom as the central atom. All O atoms are attached to the halogen. The hydrogen atom is bonded to one of the O atoms.) Use formal charges to determine which molecule is least likely to occur in nature. (A) HFO4 (B) HC(O2 (C) HC!O3 (D) HFO3 (E) HC\O4 DO000arrow_forward
- Determine the formal charge of each element in the following:(a) H3O+(b) SO42−(c) NH3(d) O22−(e) H2O2arrow_forwardWrite the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols of the atom from which they are formed:(a) MgS(b) Al2O3(c) GaCl3(d) K2O(e) Li3N(f) KFarrow_forward19. :O: || :0-N- O: Which of the following statements, if true, would support the claim that the NO3 ion, represented above, has three resonance structures? (A) The NO3 ion is not a polar species. (B) The oxygen-to-nitrogen-to-oxygen bond angles are 90°. (C) One of the bonds in NO3 is longer than the other two. (D) One of the bonds in NO3¯ is shorter than the other two.arrow_forward
- Draw the Lewis structures and determine which of these molecules is least likely to exist. (A) SF B) SeF4 (C) PF3 (D) OF4 (E) SF4 Draw all 5 structures with 1 central atom. All of the other atoms are attached to the central atom.arrow_forwardDetermine the formal charge of each element in the following: (a) H3O+ (b) SO42−SO42− (c) NH3 (d) O22−O22− (e) H2O2arrow_forwardWhich two species have the same number of lone electron pairs in their Lewis structures?(a) H2O and H3O+(b) NH3 and H3O+(c) NH3 and CH4(d) NH3 and NH4+arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY