(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.
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.
(c)
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.
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemistry In Context
- QUESTION 1 Which of the compounds below is non-polar? Key Concept: Polar molecules occur when an electronegativity differences exists between of atoms involved in the bonding and the molecule is not perfectly symmetric A PBr3 B TeF5- C XeO2F2 D SF6arrow_forwardQuestion 10 Listen ▶ Identify two valid resonance structures for SeO3²¹ In the blank below type in the number of valence electrons you calculated for the structure. A valence electrons.arrow_forwardPart A Directions: Determine the type of bond that will form between each pair of atoms in the table below. Use the Electronegativity Chart and Bond Type Chart to help you. Bond Type (Nonpolar Covalent (NPC), Moderately Polar Covalent (MPC), Very Polar Covalent (VPC), or lonic (1)) Electronegativity Difference (AEN) Atom 1 Atom 2 Arsenic Sulfur Cobalt Bromine Germanium Selenium Silicon Fluorine Potassium Nitrogen Nickel Oxygen Barium Tin Hydrogen Oxygenarrow_forward
- Reflection 3 1. Why are Lewis structures important? 2. An atom becomes stable when bonded with other atoms, how will you relate this in human relationship? 3. What type of bond do you have with the people around you?arrow_forwardDrawing Bonds Practice 1. For each of the following ionic bonds: Write the symbols for each element. Draw a Lewis Dot structure for the valence shell of each element. Draw an arrow (or more if needed) to show the transfer of electrons to the new element. • Write the charges on the ions. Write the resulting chemical formula. a) Sodium + Chlorine b) Magnesium + lodine c) Sodium + Oxygen 2. For each of the following covalent bonds: Write the symbols for each element. Draw a Lewis Dot structure for the valence shell of each element. Rearrange the electrons to pair up electrons from each atom. Draw circles to show the sharing of electrons between each pair of atoms Draw the bond structure using chemical symbols and lines. Use one line for each pair of electrons that is shared. Write the chemical formula for each molecule. a) Carbon + Hydrogen b) Chlorine + Chlorine c) Hydrogen + Chlorinearrow_forwardLearning Goal: When covalent compounds, such as water (H₂O), form covalent Donds, they share valence electrons. A Lewis dot structure or electron dot structure is a drawing that represents chemical bonds between atoms as shared or transferred electrons, where the valence electrons are represented as dots. For example, notice the Lewis structure of NC13 (Figure 1). When a pair of a bond. electrons is shared between two atoms, a line is drawn to indicate tab Figure s lock Resolving host... :C—N—C: :C1: esc control alt F1 option Z 2 W S X H command # 1 of 1 3 20 F3 $ 10809009 4 E D C How to draw a Lewis dot structure To draw a Lewis dot structure, follow these steps: skeletal structure of water is shown here: H O H. 1. Draw the skeletal structure of the molecule. The skeletal structure shows how the atoms of the molecule should be connected. For example, t 2. Determine the number of electrons for the Lewis structure by summing the valence electrons of each atom the molecule. .3.…arrow_forward
- Draw 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_forwardQuestion 14 Photo 15: [NO2]- Lewis Structure and VSEPR Model m Question 15 III Photo 16: SO2 Lewis Structure and VSEPR Model Question 16 + m + Upload an image Photo 17: OF2 Lewis Structure and VSEPR Model + Upload an image Upload an image fo fo M Need Help?arrow_forwardVälues if needed for this question. To answer the questions, interpret the following Lewis diagram for NO,F. 1. For the central nitrogen atom: The number of non-bonding electrons = The number of bonding electrons The total number of electrons 2. The central nitrogen atom A. obeys the octet rule. B. has less than an octet. C. has more than an octet. Submit Answer Try Another Version 2 item attempts remaining »t pt pt Previous Nextarrow_forward
- Expert Q&A Done 1. Lewis bonding theory emphasizes the importance of valence electrons true or false ? 2. Electronegativity measures the pull an atom has on bonding electrons true or false ?arrow_forwardQuestion 11 Photo 12: NF3 Lewis Structure and VSEPR Model III Question 12 Question 13 + Photo 13: NH3 Lewis Structure and VSEPR Model Upload an image 11 Upload an image Photo 14: [NH4]+ Lewis Structure and VSEPR Model Upload an image fo 2 fo M M Need Help?arrow_forwardTo answer the questions, interpret the following Lewis diagram for SeBr,0. :0-Se-Br: 1. For the central selenium atom: The number of non-bonding electrons The number of bonding electrons %3D The total number of electrons 2. The central selenium atom A. obeys the octet rule. B. has more than an octet. C. has less than an octet. Submit Answer Try Another Version 1 item attempt remaining %3Darrow_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