IMG_4113

Molecule or lon CIF2 #valence e SbF52- #valence e H3O+ #valence e ICl₂+ #valence Lewis Structure Number of Regions of Electron Density on Central Atom Lone Pairs (LP) Bond Pairs (BP) +Electron Pair Interactions of the Most Stable Configuration L-L L-B B-B L-L L-B B-B L-L L-B B-B L-L L-B B-B Electron Geometry (name only) Molecular Geometry (name only) Sketch Most Stable lon Showing Molecular Geometry (show atoms only!)

Please provide only typed answer solution no handwritten solution needed allowed

Xenon can be the central atom of a molecule by expanding beyond an octet of electrons. Draw Lewis structures for the given xenon compounds. Show all lone pairs. XeF₂ Select Draw Rings S Xe More F Erase Q2Q XeF₂0 Select Draw Rings More G → Xe 0 F Q2 Erase 0

complete #13 & #14, use #15 as an example!

question 4, 5, 6

rd Font Paragraph Styles Edit SO2 NO2 PF3 Sil4 Crude Sketch Calculations (# of valence electrons, # of bonds, etc. Lewis Structure # electron groups, electron group geometry 以 D, Focus 目 目 圈 18 2428 words P Type here to search 梦 。 85°F A O hp

Molecule # 1 ТеОз- Draw the Lewis Structure below Calculate the number of valence electrons Draw the three-dimensional structure of the molecule using the "wedge and dash" notation. The molecular geometry is: This molecule is polar nonpolar (Circle your choice.) Our logic for this choice is: The formal charge on the central Te atom is on the terminal O atom is The hybridization of Te is Estimate O-Te-O bond angle Molecule # 2 CIF.+ Calculate the number of valence electrons Draw the Lewis Structure below Draw the three-dimensional structure of the molecule using the "wedge and dash" notation. The molecular geometry is: This molecule is polar nonpolar (Circle your choice.) Our logic for this choice is: The formal charge on Cl is The formal charge on F is The hybridization of Cl is Estimate F-Cl-F bond angle

v Question Completion Status: QUESTION 2 What is the formal charge on nitrogen in the following structure? H. H-C H. H C=N O 2- QUESTION 3 What is the electronic configuration for the magnesium ion O 1s2 2s2 2p63s2 O 1s2 2s2 2p6 O 1s2 2s22p4

♥ Draw Lewis structures for each of the following. Use the DEN and the number of REDs around thecentral atom to select the type of bonds, the molecular shape, and type of molecule from the lists.♥ Do not put covalent bonds between metals and nonmetals♥ Put brackets around anions to show both charge and quantity.

QUESTION 4 Determine which compound should have a(n) trigonal pyramidal molecular geometry. Key Concept: Lewis structures are drawn from a knowledge of the total number of electrons from all the atoms involved in the structure. The element with the lowest electronegativity is the central atom. Fulfill octet of outside atoms first. Molecular shape depends upon the number of atoms and lone pair electrons around the central atom.   A BrCl3   B IF4+   C BCl3   D NCl3

= Deciding whether a Lewis structure satisfies the octet rule Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure :5: I :Z: H- :0: | U: -C-C-H Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: 0 No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 Yes. No, it has the wrong number of valence electrons. The correct number is: 0 No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many 1/5

QUESTION 5 Determine which compound should have a(n) linear molecular geometry. Key Concept: Lewis structures are drawn from a knowledge of the total number of electrons from all the atoms involved in the structure. The element with the lowest electronegativity is the central atom. Fulfill octet of outside atoms first. Molecular shape depends upon the number of atoms and lone pair electrons around the central atom.   A H3O+   B ClF2+   C IF2-   D AsF5

♥ Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. ♥ Do not put covalent bonds between metals and nonmetals. ♥ Put brackets around anions to show both charge and quantity. 1. HCI hydrogen chloride valence e = REDS = shape= bond angles = 2. CCl4 valence e = REDS = shape bond angles = carbon tetrachloride REDS 0, no central atom 234 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5⁰ 120⁰ 180⁰ none, no central atom

The 3rd box is number of bonds and number of lone pairs around central atom and the 4th box is the Lewis structure.

Many organic compounds belong to a category of molecules called "hydrocarbons", meaning that they only contain hydrogen and carbons. An example of a simple hydrocarbon is shown below. Considering both the VSEPR shape of the molecule and electronegativity values of the elements and state whether you expect this simple hydrocarbon to be polar or nonpolar. Explain your answer. нн H-C-C-H нн