1. Consider the molecule NHCl₂. a. Draw Lewis Dot diagrams for each atom in this molecule to properly show the number of valence electrons around the atoms before bonding occurs. e.g. for carbon: .c. N H Cl Cl b. How many total valence electrons are in NHCl₂? 2. The Lewis structure for NHCl2 is shown here. -N- CIN CI: the H a. How many total electrons are shown in this structure? b. How many total bonding and nonbonding electrons are around the H atom? C. How many total bonding and nonbonding electrons are around the N atom? d. How many total bonding and nonbonding electrons are around each Cl atom?

1. Consider the molecule NHCl₂. a. Draw Lewis Dot diagrams for each atom in this molecule to properly show the number of valence electrons around the atoms before bonding occurs. e.g. for carbon: .c. N H Cl Cl b. How many total valence electrons are in NHCl₂? 2. The Lewis structure for NHCl2 is shown here. -N- CIN CI: the H a. How many total electrons are shown in this structure? b. How many total bonding and nonbonding electrons are around the H atom? C. How many total bonding and nonbonding electrons are around the N atom? d. How many total bonding and nonbonding electrons are around each Cl atom?

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 3STP

See similar textbooks

Similar questions

1. Which is the formula of the compound formed by barium and phosphorus? a. BaP3b. Ba2P Ba3P2c. Ba3Pd. Ba2P 2. The bond between Br atoms in a Br2 molecule is _______ and is formed by the _________ of two valence electrons. a. covalent ; sharingb. covalent; transferc. ionic ; transferd. ionic ; sharing
The molecule H2O2 (H-O-O-H) has: A. 4 bonding pairs and 3 lone pair. B. 3 bonding pairs and 2 lone pairs. C. 3 bonding pairs and 3 lone pairs. D. 3 bonding pairs and 4 lone pair. E. some number of lone and bond pairs not described in 1-4.
6. Refer to the periodic table. Which pair of elements can combine to form ionit bonds. S and Sr a. b. H and N C. H and CI d. Xe and F
1. Which of the following paired atoms 1 point is non-polar? * a. Br-F b. H-CI c. H-F d. H-P 2. Which of the following bonds has the highest polarity? * a. N-H b. C-H c. N-H d. C-O 3. Which of the following bonds has the lowest polarity? * a. N-H b. C-O c. C-H d. O-H 4. Which of the following is the correct decreasing electronegativity values? * a. F, O, N, C b. CI, S, Si, P c. As, Se, Br, F Od. H, Si, P, S 5. Which molecule has an ionic bond? а. Н-F b. Na-F c. F-F d. Cl-F 6. Which best describe the shape and 1 point polarity of CH4? * a. Tetrahedral polar b. Linear non-polar c. Tetrahedral non-polar d. Linear polar 7. Which statement is true about the non-polar molecules? * a. They are symmetric. b. They are asymmetric. c. They have lone pair on the central atom. d. They have charges 8. If a molecule has this symbol -, it means a. Negative b. Neutral C. Positive d. Cancel out 9. If a molecule has this symbol +, it means a. Charge b. Positive c. Negative d. Neutral 10. If a molecule…
Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules land ions. Draw a Lewis structure for CH4 and answer the following questions based on your drawing. 1. For the central carbon atom: The number of lone pairs The number of single bonds The number of double bonds= 2. The central carbon atom î A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet. = | =
To answer the questions, interpret the following Lewis diagram for XeO3. :0–Xe–6: I :0: .. 1. For the central xenon atom: The number of non-bonding electrons = The number of bonding electrons The total number of electrons 2. The central xenon atom A. obeys the octet rule. B. has more than an octet. C. has less than an octet. = =
To answer the questions, interpret the following Lewis diagram for SO42- . 1. For the central sulfur atom: ... The number of non-bonding electrons = The number of bonding electrons = The total number of electrons = 2. The central sulfur atom fill in the blank 4 ... A. obeys the octet rule. B. has more than an octet. C. has less than an octet.
Please note that "geometry" refers to the molecular or ionic geometry. :Br: A. The Lewis diagram for AIBR3 is: AI Br. Br The electron-pair geometry around the Al atom in AlIBr3 is There are | lone pair(s) around the central atom, so the geometry of AlBr3 is B. The Lewis diagram for BeCl, is: Ci-Be-ci: The electron-pair geometry around the Be atom in BeCl, is There are lone pair(s) around the central atom, so the geometry of BeCl, is |
1. The electron pair in a H - Cl bond could be considered... a. closer to H because Hydrogen has a larger radius and thus exerts greater control over the shared electron pair b. closer to Cl because Chlorine has a higher electronegativity than Hydrogen c. closer to H because Hydrogen has a lower electronegativity than Chlorine d. an inadequate model since the bond is ionic 2. It is important to know the geometry of a molecule because the geometry _______. a. will give the Lewis structure of the molecule b. affects the physical and chemical properties of the substance c. will determine whether the molecule is ionic or covalent d. Both B, and C
Which is true of Lewis structures? a. They do not show details regarding the shape of molecules. b. They show details regarding the shape of molecules.
Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules and ions. Draw a Lewis structure for NH,* and answer the following questions based on your drawing. 1. For the central nitrogen atom: The number of lone pairs The number of single bonds = The number of double bonds= 2. The central nitrogen atom A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet.
1-What is the formal charge of the nitrogen atom in hydrogen cyanide (HCN)? a.5 b.−1 c.0 d.1 e.2 2-Which of the following diatomic molecules has the least number of valence electrons? a.N2 b.F2 c.O2 d.Cl2 e.NO