How many electrons should appear in the Lewis structure of the following:
Determine the formula change on the following
Lewis electron count:
H3O + : The number of electrons on O are 6.
The number of electrons on H atom are 1.
Number of H atoms bonded to O by covalent bonds are 2.
Number of H atoms bonded to O by co-ordinate covalent bond are 1, this H atom
does donate an electron and hence the total electron count = 8.
SCN- : The number of electrons on C = 4
The number of electrons on S = 6
The number of electrons on N = 5
The negative charge indicates an additional electron
Thus the total electron count = 16.
HCO3- : The number of electrons on C = 4
The number of electrons on H = 1
This solution determines the number of electrons on each element of a molecule as well as their formal charge to show how many electrons should appear in the Lewis Structure. The refractive index and mole fraction is used to determine formula change.
Electron configurations, Redox reactions, Lewis structures
1. Write an electron configuration for N ,and draw the Lewis structure for N.
2. Add single electron dots and/or pairs of dots as appropriate to show the Lewis symbols of the following neutral atoms. As, Se, Br, K, Ca, and Ga
3. If the following elements were involved in redox (electron transfer) reactions, which noble-gas (He, Ne,Ar, and Kr) configuration would they most likely attain? Li, Mg, N, S, K, As, Rb
4. Arrange these substances in order of increasing magnitude of lattice energy. NaF, KCl, BaO, and CaO
5. Draw covalent Lewis structure of diatomic molecule formed from each element (or family of elements). Hydrogen, the halogens, oxygen , and nitrogen
6. Consider the following element combinations. Classify the bonds formed between each pair as ionic, polar covalent, or nonpolar covalent based solely on each element's position on the periodic table. S-S, Sr-O, Al-N, O-Cl, S-I, Cl-Cl, P-F, Cs-Cl
7. Determine the number of bonding electrons and the number of nonbonding electrons in the structure of CS 2 .Enter the number of bonding electrons followed by the number of nonbonding electrons in the dot structure of this molecule separated by a comma (e.g., 1,2).
8. Draw the main Lewis structure of NOF.
9. Determine the number of bonding electrons and the number of nonbonding electrons in the structure of XeF 2 .Enter the number of bonding electrons followed by the number of nonbonding electrons, separated by a comma, in the dot structure of this molecule (e.g., 1,2).
10. Draw the molecule by placing atoms on the grid and connecting them with bonds. Do not identify the charge on each of these species. Include all lone pairs of electrons. CN - and NO 2 -
11. Draw the Lewis structure of PH 3 .NO 2 − .
12. For a molecule of fluorous acid, the atoms are arranged as HOFO . (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.)
13. What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed.
14. Express your answers as charges separated by comma. For example, a positive one charge would be written as +1.