gen chem II LG iv - exam 1 review (key)

For a molecule of XeCl3H a) Draw the Lewis structure then predict the shape of the compound and draw the shape of the compound b) Determine if the molecule is polar or nonpolar and explain how you made that determination. If there is a dipole moment, draw it.

Consider the following ion: BrO3 − . a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3 − and briefly explain why your Lewis structure is correct.  c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3 − ? What is its molecular shape?  e) Does BrO3 − have a dipole moment? Briefly justify your answer.  f) On average, would you expect IO3 − to have longer or shorter bonds than BrO3 − ? Briefly explain your answer.  g) Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice.  h) What is the molecular formula for Compound C? What is the empirical formula for Compound C?

Please answer all parts of the question

Which of the following (NBR3, BF3, OF2, IF3) is(are) exempted from the octet rule? Check all that applies. IF3 O NBR3 O BF3 OF2 Question 6 Give the number of lone pairs around the central atom and the geometry of NO3. 0; trigonal planar O 1; tetrahedral O 0; trigonal pyramidal O 2; linear

♥ 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.

- 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 REDS 0, no central atom 2 3 4 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5° 120° 180° none, no central atom 9. Na3P valence e = REDs = shape= bond angles = 10. AI(NO3)3 valence e = REDs = shape = bond angles = sodium phosphide aluminum nitrate For nitrate

For NO3^- provide a Lewis structure, predicted VSEPR molecular geometry, bond angle and indicate whether the compound is polar, non polar or a polyatomic ion

JAINTING Decide whether the Lewis structure proposed for each molecule is reasonable or not. molecule + NH₂2 CO2 Be H₂ proposed Lewis structure H-N=H H]* :0-C=0: H-Be-H 2 No, some atoms have the wrong number of electrons around them. 0 The symbols of the problem atoms are: * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical O Is this a reasonable structure? If not, why not? 787 Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. The correct number is: 27 - ♫ átv © 2023 McGraw Hill LLC.…

The carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]

Draw the bonding pattern for the third resonance structure of the azide ion, N3. Two of the resonance structures are shown below. (Include double/triple bonds and any formal charges.) Edit Drawing eTextbook and Media N=N_N?²- A How many lone pair electrons are on the central nitrogen atom? # of lone pair electrons on the central nitrogen atom: -Ń=N: B How many lone pair electrons are on the each of the other two nitrogen atoms? # of lone pair electrons on each of the other nitrogen atoms: Why do both bonds of the azide ion have the same length? O The bond lengths are the same because the resonance structure you drew was tetrahedral. O The bond lengths are the same because single, double, and triple bonds are always the same length. O The bond lengths are the same because structures A and B are equivalent and therefore make equal contributions to the hybrid.

For the following three Lewis structures, list whether they are correct or incorrect:   alt-text for image above: The first image shows a proposed Lewis structure for Freon-13, CClF3, that has a central carbon singly bonded to a three chlorine atoms and a fluorine atom. Each chlorine and the fluorine have 3 lone pairs of electrons around them. The second image shows a proposed lewis structure for the nitrite ion, NO2-, as a central nitrogen atom between two oxygen atoms. The O atom on the left has three lone pairs of electrons and then a single bond between the N. The right O atom has two lone pairs of electrons and a double bond with the N atom. The N atom has a single lone pair of electrons in addition to the double and single bonds with oxygen atoms. The third image shows diazomethane, CH2N2, and the proposed Lewis structure has a carbon singly bonded to two H atoms, then doubly bonded to a nitrogen. The nitrogen is doubly bonded to the second nitrogen, and the second nitrogen has…