Convert the following Lewis structure for the nitrate ion into a line structure that includes the lone pairs. Why does the nitrate ion have a -1 charge?

For SO3^-2 provide a Lewis structure, predicted VSEPR molecular geometry, bond angle and indicate whether the compound is polar, nonpolar, or a polyatomic ion.

Predicting the arrangement of electron groups around the central atom of a molecule.

Diazomethane (CH2N2) is an important reagent for the methylation of some organic molecules. Complete Parts 1 and 2 below about this unique reagent.  Draw the Lewis structure of diazomethane (CH2N2) that contains a formal charge on carbon and nitrogen. Be sure to include all lone pairs of electrons and formal charges.

Decide whether the Lewis structure proposed for each molecule is reasonable or not. proposed Lewis structure Is this a reasonable structure? If not, why not? molecule O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. BeH, Н— Ве —Н The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are:U O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. CO2 :0-C=0: The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: U O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. OF2 F=0=F The correct number is: O No, some atoms have the wrong number of electrons around them. .. 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 symbol for the atom as many times as…

Consider the incomplete structure shown. Draw an alternative Lewis (resonance) structure for the incomplete structure. Show the unshared electron pairs and nonzero formal charges in your structure. Don't use radicals.     Determine the formal charge on the nitrogen atom in the structure. If the atom is formally neutral, indicate a charge of zero.

- 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. Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Types nonpolar covalent polar covalent nonpolar & polar covalent ionic ionic & covalent Type of molecule Nonpolar Polar Ionic 5. C2Cl2 valence e-1 = shape= type of bonds = type of molecule = 6. AICI3 valence e-1 for one Cl-1 = shape= type of bonds = type of molecule = 7. K3PO3 valence e-1 = shape= type of bonds = type of molecule = 8. KH2PO3 valence e-1 = shape at the P= type of bonds = type of molecule = dicarbon dichloride aluminum chloride potassium phosphite potassium dihydrogen phosphite

CO3²- Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons. Show the formal charges of all atoms in the correct structure. To change the symbol of an atom, double-click on the atom, and enter the letter of the new atom.

Draw three resonance structures for N3-. This species has its three atoms bonded sequentially in the following fashion: N-N-N. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Now select the statement from the multiple choices which is true about this most important resonance structure.In the most important resonance structure of N3- : a) The leftmost bond (between N and N) is a single bond.b) The rightmost bond (between N and N) is a single bond.c) The formal charge on the leftmost (N) atom is -1.d) The number of nonbonding pairs (lone pairs) of electrons on the leftmost (N) atom is 4.e) The number of nonbonding (lone) pairs of electrons on the rightmost (N) atom is 4.

Draw a Lewis structure for the following ions/molecules, including any resonance structures and/or formal charges. Place a box around any contributing resonance structures XeO4^-2, BrF5, CHF2CL What is the electron group geometry around the central atom for each of the above ions/molecules? For the above ions/molecules, what is the shape of the entire molecule/ion of the entire ion/molecule? Identify polar bonds with dipole arrows  Indicate whether each of the ions/molecules is POLAR or NON-POLAR