Final answer:
Compounds CO_2, H_2CO_3, HCO_3-, and CO_3^2- are ranked based on their charge and hydrogen bonding capability with water. CO_2 has the weakest attraction, followed by H_2CO_3, HCO_3-, and CO_3^2-, which has the strongest attraction due to its higher negative charge and ability to form multiple hydrogen bonds.
Step-by-step explanation:
The compounds CO_2, H_2CO_3, HCO_3-, and CO_3^2- can be ranked in order of increasing attraction to water molecules based on their charge and ability to form hydrogen bonds with water. Carbon dioxide (CO_2) is a neutral molecule and exhibits the least attraction to water molecules since it can only interact through weak Van der Waals forces. Next is carbonic acid (H_2CO_3), which, despite being neutral, can form hydrogen bonds due to the presence of -OH groups. Bicarbonate ion (HCO_3-) is a negatively charged ion and is more attracted to water than carbonic acid because of its ability to form both hydrogen bonds and ionic interactions. Carbonate ion (CO_3^2-) has the strongest attraction to water since it can form multiple hydrogen bonds and has a greater negative charge which increases ionic interactions with the polar water molecules.
In the order of increasing attraction to water molecules, the ranking is: CO_2 < H_2CO_3 < HCO_3- < CO_3^2-.