Concept explainers
What is the Lewis structure for the compound that forms between K and S?
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Chapter 10 Solutions
Introductory Chemistry (6th Edition)
- Consider the SO 3 molecule. How many valence electrons does the molecule have? How many lone pairs of electrons are on the central atom? How many lone pairs of electrons in total are on the substituent atoms? How many resonance structures can be drawn for the molecule? If the ion doesn't exhibit resonance, indicate "1" as only one structure can be drawn for the molecule.arrow_forwarda) how many total pairs of electrons does CF4 have? b) How many bonded pairs and how many lone pairs does CF4 have? c) What is the molecular shape and angle of CF4? d) what is the lewis structure for CF4?arrow_forwardWhich of the following compounds would require a Lewis structure that shows electrons were transferred (ionic) instead of being shared (covalent)? A) Al2S3 B) NO2 C) CO2 D) SF6 When drawing a Lewis structure for a covalent compound, you need to know the total number of valence electrons for the compound. How many valence electrons are there for Cl2CO? A) 17 B) 24 C) 28 D) 32 Which of the following molecules have Lewis structures with lone pairs of electrons on the center atom? A) CO2 B) CCl4 C) All of them D) OF2arrow_forward
- A. What is the electron-pair geometry for Sb in SbF3? _______There are ____ lone pair(s) around the central atom, so the geometry of SbF3 is _________.B. What is the electron-pair geometry for B in BCl3? ________There are ____ lone pair(s) around the central atom, so the geometry of BCl3 is _______.arrow_forward1) Discuss the advantages and disadvantages of using the molecular models (ball and stick) as learning aids. Recommend an alternative to using this method for modeling molecules. 2) Build C6H6 as a ring. What do you notice about the placement of the bonds? This is an example of resonance. What is a resonant Lewis structure? 3) Explain how a diminished and expanded octet can be formed.arrow_forwardDetermine the number and type of chemical bonds in silicon tetrachloride (SiCl4) and beryllium sulfide (BeS). 1.) One formula unit of silicon tetrachloride has ___________, (_____________) polar covalent nonpolar covalent ionic bond(s). 2.) One formula unit of beryllium sulfide has ______________, (_____________) polar covalent nonpolar covalent ionic bond(s). Name the following ionic compounds. Example.) ----(a) Cu(ClO)2_______Copper(II) hypochlorite___ (b) Rb3PO3 ____________________(c) Y2Se3______________________arrow_forward
- 1) A) In the Lewis structure for IF2–, how many lone pairs of electrons are around the central iodine atom?a) 0b) 1c) 2d) 3e) 4B) The Cl–Xe–Cl bond angle in XeCl4 is closest toa) 90°b) 120°c) 150°d) 360°e) 109°C) Which of the following atoms cannot exceed the octet rule in a molecule?a) Bb) Snc) Pdd) Ie) All atoms exceed the octet rulearrow_forwardWhich statement is false given the following Lewis structures? Group of answer choices Structure III is a valid structure for PF4 because P can expand its octet. Structure I is a valid structure for BBr3 because B (n=2) needs an octet of electrons. Structure II is a valid structure for SeH2 because H needs a duet of electrons. Structure IV is a valid structure for AsO43- because As can expand its octet.arrow_forward1) A) Describe a polar covalent bond, and give an example B) Describe a nonpolar covalent bond, and give an examplearrow_forward
- 1. In its Lewis dot symbol, which element would have four (4) dots? Select one: a.Si b.F c.N d.S 2. Which compound is expected to be soluble in a polar solvent? Select one: a.CH4 b.NH3 c.None of these. d.BF3 3. Which compound is nonpolar? Select one: a.CO2 b.None of these. c.HCl d.H2O 4. In HCN, the formal charge on nitrogen is Select one: a.+1 b.0 c.–1 d.None of these. 5. For the carbonate anion, CO3–2, the number of contributing equienergetic resonance structures is Select one: a.3 b.4 c.1 d. 2arrow_forwardWhich is the correct Lewis structure for HOCN? Why is it correct and why the other options are incorrect ?arrow_forwardSubstance(s): H2CO, IF2-, O3, N2H4, NH4+, SCl4, NO2-, SO2, C2H2, Cl3PO, HCN, CF2H2, IF4-, XeF2, CI4, I3-, SeF6,H2O2, NF3, CS2. 1.Bonding groups 2.Number of lone pairs 3.Number of electron groups about the central atom 4.Number of resonance structures 5.Hybridization state about the central atom 6.Bond Angles 7.Polarityarrow_forward
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