For the following - Learnexams

For the following: (a) name the compound, (b) draw the Lewis symbol, (c) if applicable, draw the resonance structure, (d) if applicable calculate the formal charge. a. CCl4 g. FeCl2 b. SeCl3+ c. PCl3 d. V2S5 h. MoS2 i. NiCO3 j. H3PO4 e. ICl3 f. Rb2O

The Correct Answer and Explanation is:

Here’s the breakdown for each compound:

a. CCl4 (Carbon Tetrachloride)

(a) Name: Carbon tetrachloride
(b) Lewis Structure: The carbon atom is at the center, surrounded by four chlorine atoms. Each chlorine atom has three lone pairs of electrons, and carbon shares one pair of electrons with each chlorine.Cl | Cl-C-Cl | Cl
(c) Resonance Structure: There are no resonance structures in CCl4 because all bonds are single, and there are no alternative arrangements of electrons.
(d) Formal Charge: The formal charge on all atoms is zero, as each chlorine atom has 7 valence electrons, and carbon has 4.

b. SeCl3+ (Selenium Trichloride Ion)

(a) Name: Selenium trichloride ion
(b) Lewis Structure: Selenium in the center, with three chlorine atoms. Selenium has a positive charge because it is missing an electron. Cl | Cl-Se-Cl | Cl
(c) Resonance Structure: There are no resonance structures for SeCl3+ because the positive charge is localized on selenium.
(d) Formal Charge: The formal charge on Se is +1, and each Cl atom has a formal charge of 0.

c. PCl3 (Phosphorus Trichloride)

(a) Name: Phosphorus trichloride
(b) Lewis Structure: Phosphorus is the central atom, with three chlorine atoms attached. Each chlorine has three lone pairs. Cl | Cl-P-Cl | Cl
(c) Resonance Structure: There are no resonance structures in PCl3.
(d) Formal Charge: The formal charge is zero on all atoms (P has 5 valence electrons, Cl has 7).

d. V2S5 (Vanadium Pentasulfide)

(a) Name: Vanadium pentasulfide
(b) Lewis Structure: The two vanadium atoms are bonded to five sulfur atoms in a way that each sulfur is connected to a vanadium atom.
(c) Resonance Structure: The structure has no resonance due to the nature of the bonds and the arrangement of the atoms.
(d) Formal Charge: Vanadium has a formal charge of zero, and sulfur atoms have zero formal charge as well.

e. ICl3 (Iodine Trichloride)

(a) Name: Iodine trichloride
(b) Lewis Structure: Iodine is the central atom, surrounded by three chlorine atoms. Iodine has three lone pairs. Cl | Cl-I-Cl | Cl
(c) Resonance Structure: There are no resonance structures for ICl3.
(d) Formal Charge: Iodine has a formal charge of 0, and each chlorine has a formal charge of 0.

f. Rb2O (Rubidium Oxide)

(a) Name: Rubidium oxide
(b) Lewis Structure: The rubidium atoms each donate one electron to bond with oxygen. The oxygen atom has two lone pairs. cssRb-O-Rb
(c) Resonance Structure: No resonance exists in this compound.
(d) Formal Charge: The formal charge on each Rb is +1, and oxygen has a formal charge of -2.

g. FeCl2 (Iron(II) Chloride)

(a) Name: Iron(II) chloride
(b) Lewis Structure: The iron ion (Fe2+) bonds with two chloride ions (Cl-), where each Cl has three lone pairs. Cl-Fe-Cl
(c) Resonance Structure: No resonance structures exist for FeCl2.
(d) Formal Charge: Fe has a formal charge of +2, and each chlorine has a formal charge of -1.

h. MoS2 (Molybdenum Disulfide)

(a) Name: Molybdenum disulfide
(b) Lewis Structure: Molybdenum is at the center, bonded to two sulfur atoms. CopyEdit S-Mo-S
(c) Resonance Structure: No resonance structures exist for MoS2.
(d) Formal Charge: The formal charge on Mo is 0, and each sulfur has a formal charge of 0.

i. NiCO3 (Nickel Carbonate)

(a) Name: Nickel carbonate
(b) Lewis Structure: Nickel is bonded to a carbonate ion (CO3^2-), with carbon at the center of three oxygens. One oxygen has a negative charge. O || O-C-O | Ni
(c) Resonance Structure: The carbonate ion has resonance, where the double bond alternates between the oxygens.
(d) Formal Charge: The formal charge on the carbon is 0, each oxygen has a -1 charge, and nickel has a formal charge of 0.

j. H3PO4 (Phosphoric Acid)

(a) Name: Phosphoric acid
(b) Lewis Structure: Phosphorus is at the center, bonded to three hydroxyl groups (OH) and one double-bonded oxygen. OH | OH-P=O | OH
(c) Resonance Structure: No resonance structures exist for H3PO4.
(d) Formal Charge: The formal charge on phosphorus and the oxygens is 0.

Each compound has a distinct Lewis structure and varying possibilities for resonance and formal charge depending on the electron arrangement and bonding patterns.