(a)
Interpretation: The Lewis structure of
Concept Introduction:
Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.
Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.
Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.
- Ø Lone-pair electrons are valence electrons that are not used in bonding.
- Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.
- Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).
- Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.
(b)
Interpretation: The Lewis structure of
Concept Introduction:
Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.
Geometry: The spatial arrangement of atoms or group of atoms around the central atom defines the geometry of the compound. The geometry can be determined by constructing Lewis structure and VSEPR model.
Hybridization: The concept of mixing atomic orbitals into new hybrid orbitals that possess different shapes, size, and energy than the constituent atomic orbitals.
- Ø Lone-pair electrons are valence electrons that are not used in bonding.
- Ø A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.
- Ø Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).
- Ø Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.
- Ø
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemistry In Context
- QUESTION 5 Draw the lewis dot structure of BF 3. How many lone-pairs of electrons (first) and bonding pairs of electrons exist on the molecule BF 3? 0,3 11,3 2,3 9, 3 Click Save and Submit to save and submit. Click Save All Answers to save all answers. W tv MacBook Pro * $ % & 3 4 5 6. 7 8 向 * 00arrow_forwardDraw the Lewis structures for each of the following compounds as they would appear if one hydrogen (H) was added to the appropriate central atom and the resulting molecule was neutral. Which of your Lewis structures would represent nonpolar molecules (select all that apply)? 1. NH2 2. CC13 3. H 4. CH3 5. OH 6. C₂H3 01 02 3 4 05 06arrow_forward◄ Search 10:39 AM Wed Oct 5 Question 17 Photo 18: H2S Lewis Structure and VSEPR Model m Question 18 m Question 19 + Photo 19: SF6 Lewis Structure and VSEPR Model 111 myhol.holscience.com + Upload an image + Photo 20: IC15 Lewis Structure and VSEPR Model Upload an image Upload an image Submit Your Data fo 2 100% Need Help?arrow_forward
- Which of these molecules would have a linear molecular shape? (Select all that apply.) Cl20 CSez KIF2 Which have lone pairs around the central atom? (Select all that apply.) Cl20 KIF2arrow_forwardQUESTION 29 A compound has an elemental analysis of 48.2% C, 8.2% H, and 43.2% O by mass. What is the empirical formula? OA.C6H05 OB. C2H602 OC.CH30 ⒸD.C3H602 OE. C3H60 QUESTION 30 How many lone pairs answer as a number)? and bonding pairs does the lewis structure of SF4 have around the central atom (enter yourarrow_forwardPART 2 Practice Problems ☆回の Last edit was seconds ago ols Add-ons Help Itim 28 BIUA + 三 2. |I16 | 7 | 8 9. Chemical Formula: Practice Problem 5. TeO Draw the Lewis Dot Structure of the molecule in the space below using the formula given at the top of the slide and complete the chart at the bottom of the slide. :fe::ö: Type of Bond in the Molecule # of PAIRS of valence electrons TOTAL # of Valence Electrons in this Molecule shared between atoms 困arrow_forward
- Identifying Bond Type Lab Write up Choose one of the substances that you tested. Then, answer all the following questions. Your answer should include at least five complete sentences. Which substance did you choose and what bond type did it have? Which properties helped you identify its bond type? Which properties did not help you to identify its bond type? Did you predict the bond type correctly? Why or why not? Metalic Bond Ionic Bobd Covalent Bondarrow_forwardWhich of these molecules would have a linear molecular shape? (Select all that apply.) O CS2 □ XeCl₂ O Br₂ S Which have lone pairs around the central atom? (Select all that apply.) CS₂ O XeCl₂ Br₂Sarrow_forwardQuestion 1 Select which molecules have polar bonds, which molecules are polar, and what type of intermolecular forces they have. You may need to consult the Electronegativity.pdf table. a) C₂H5F Polar bonds? [Select] Polar molecule? [Select] Intermolecular Forces? [Select] b) (CH3)2CH Polar bonds? [Select] Polar molecule? [Select] Intermolecular Forces? [Select] c) PO4³- Polar bonds? [Select] Polar molecule? [Select] Intermolecular Forces? [Select] d) PF3 Polar bonds? [Select] Polar molecule? [Select] Intermolecular Forces? [Select] ✪ ✪ ✪ ✪ ✪ ✪ ✪ ✪ Oarrow_forward
- Which of the following atoms do NOT have 5 valence electrons? Select all that applyarrow_forwardExercise 8 i. Draw Lewis structures for: (a) SiCl,; (b) PF3; (c) PH3; and (d) SCl,. ii. Draw Lewis structures for: (a) carbon disulfide and (b) cyanide ion. iii. Draw the Lewis structure for HCIO4. Assign formal charges to the atoms. iv. Decide which of the following bonds is least polar: C-O or C-N.arrow_forwardUse this condensed chemica structure to complete the table below. I| CH, C 0 C CH, The condensed chemical structure of acetic anhydride Some facts about the acetic anhydride molecule: number of carbon-carbon single (C - C) bonds: number of carbon-hydrogen single (C - H) bonds: number of lone pairs: Explanation Check 2022 McGraw Hill LLC. All Rights Reserved. Te DELLarrow_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