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- a) b) c)a) Draw all the possible Lewis structures for the following ions: SeCl4 PO43- BrO3 b) Assign formal charges to each atom in each resonance structure (Show all your work on paper) c) indicate the most plausible Lewis structure. (Show all your work on paper) d) Indicate the approximate bond angles for each ion. (e) determine the names for the molecular geometry. (Show all your work on paper) (d) determine if the molecule is polar or non-polar;4. Which of the following Lewis structures is INCORRECT? A) B) C) D) 1 H H 4 H N-H ["%" ] " H H :0: H
- The Lewis dot symbol .X. might possibly represent a neutral atom of a) nitrogen b) boron c) oxygenWhy is the ability to draw a Lewis structure considered a core chemistry skill?Boranes are a class of chemical compounds that undergo combustion reactions that are very similar to the reactions of hydrocarbons but they release more heat. If they were not so expensive, they would be considered for rocket fuel. The structure of diborane is shown below. It “breaks rules” in terms of its Lewis structure. The “rule breaking” part is referred to as a “banana bond”. a) Explain why it breaks rules. b) Using the combustion of a hydrocarbon as your guide, predict the equation for the combustion of diborane. Balance the equation you predict.
- In a polar covalent bond, A) both atoms in the bond have the same level of electronegativity. B) one atom in the bond must have higher electronegativity than the other atom. C) one atom must be a H atom. D) both atoms in the bond must be metals.Choose only ONE of the following covalently bonded structures listed below and complete all parts I) sulfite, SO3²- OR II) sulfur tetrafluoride, SF4 A) Draw the complete Lewis structure. Show your work. B) Identify the molecule as being either polar, nonpolar or ionic. C) Name and draw the VSEPR shape for this structure. E) Identify how many sigma (o) and pi (π) bonds are present within the structure. F) List all intermolecular forces present within a crystal containing particles with this structure.To answer the questions, interpret the following Lewis diagram for NHF2 . 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 fill in the blank 4 ... A. obeys the octet rule. B. has more than an octet. C. has less than an octet.
- 1a) Which of the following statmenst regarding bond polarity is true? and why? a) electrons are shared equally in polar bonds b) Atoms of elements with small differences in electronegativity form ionic bonds c) atoms of elements with small differences in electronegativity form nonpolar covalent bonds d) electrons are shared unequally in nonpolar bonds e) electrons in polar bonds are transferred from one atom to another 1b)Which of the following bonds is least polar and why? a) H--C b)H--O c)H--N d) H--Cl e)H--F(2) Write the preliminary Lewis structure for C2H2 (Figure 35). Place one pair of electron dots between each pair of bonded atomic cores. Figure 35 (3) What is the total number of valence electrons remaining? answerIonic Bonding 1. Show the transfer of electrons with ↓ notation in the reactions between the following pairs of elements to create an ionic compound. Show the elements as atoms, even though they may exist as diatomic or polyatomic species. (a) Ba and F (b) K and I (c) Cs and S (d) Ca and As (e) Li and N (f) Rb and Se (g) Sr and P (h) Al and Br 2. Write Lewis dot structures for atoms and ions of each of the reactants and products in Exercise 1.
