Thank you!!
1.Explain (not describe) the solubility behavior of table salt in water.
2. Explain (not describe) the behavior of eggshell in water. Do not simply say “it dissolved” (that would be describing), explain why it dissolved.
Do not use the polar/nonpolar” reasoning here. Use the solubility rules of ionic compounds.
With so many restrictions I don't know but here goes.
1. NaCl is an ionic compound. When placed in water the negative oxygen end the positive H end of water is strong enough break the crystal lattice forces of the ionic NaCl so solution takes place.
2. Egg shells don't dissolve in water because the shell is not an ionic compound.
1. Well, when you add table salt to water, it's all like, "Hey water, mind if I join the party?" And the water's all like, "Sure, come on in!" You see, table salt, also known as sodium chloride, is an ionic compound. It's made up of positively charged sodium ions (Na+) and negatively charged chloride ions (Cl-). Now, water is a polar molecule, which means it has a positive end (the hydrogen side) and a negative end (the oxygen side). This polarity helps it separate the sodium and chloride ions in the salt. The water molecule surrounds the ions and pulls them apart, allowing them to dissolve and blend in with the water. So, the solubility behavior of table salt in water is kind of like a friendly team-up between water molecules and salt ions.
2. Ah, the curious case of the eggshell in water! When you put an eggshell in water, it's like a little adventure for the shell. The eggshell is mostly made up of calcium carbonate (CaCO3), which is another ionic compound. Water, being the sociable solvent it is, welcomes the challenge and tries to break those ionic bonds in the shell. You see, water molecules form hydrogen bonds with the carbonate ions (CO3 2-) and calcium ions (Ca2+) present in the shell. These bonds weaken the ionic bonds in the compound, causing the shell to dissolve. So, it's not just a simple dissolve, but a team effort between the water molecules and the ions in the eggshell. It's like a chemistry version of "Finding Nemo" with water and calcium carbonate playing the main roles.
1. To explain the solubility behavior of table salt (sodium chloride) in water, we need to understand the solubility rules of ionic compounds.
When an ionic compound like table salt is added to water, the water molecules surround each ion, forming hydration shells. In the case of table salt, it consists of sodium (Na+) and chloride (Cl-) ions.
The water molecule, being polar, has a partially positive hydrogen end and a partially negative oxygen end. The positive hydrogen in water is attracted to the negatively charged chloride ion (Cl-), and the negative oxygen is attracted to the positively charged sodium ion (Na+). This attraction leads to the process of hydration, where the water molecules pull the ions away from the crystal lattice and into the solution.
The solubility of table salt in water is high because the attractive forces between the ions and water molecules are generally stronger than the forces holding the ions together in the crystal lattice. As a result, the table salt dissolves and forms a homogeneous mixture with the water.
Overall, the solubility behavior of table salt in water can be explained by the strong electrostatic attraction between the polar water molecules and the charged sodium and chloride ions, leading to the dissolution of table salt in water.
2. Now let's explain the behavior of eggshell in water, without using the polar/nonpolar reasoning and instead using the solubility rules of ionic compounds.
Eggshells primarily consist of calcium carbonate (CaCO3), which is an ionic compound. When eggshell is placed in water, the water molecules surround each individual calcium ion (Ca2+) and carbonate ion (CO32-) due to their polarity.
However, unlike table salt, the behavior of eggshell in water is different because calcium carbonate has a lower solubility in water compared to sodium chloride. It means that calcium carbonate does not dissolve easily in water.
The solubility behavior of calcium carbonate can be explained by the solubility rules of ionic compounds. Calcium carbonate is sparingly soluble due to its high lattice enthalpy, which is the energy required to break the crystal lattice structure and separate the ions.
While water is able to surround the ions and pull them away from the crystal lattice, the attractive forces between the calcium and carbonate ions in the lattice are generally stronger than the forces of hydration (attraction to water molecules). Therefore, only a small amount of calcium carbonate dissolves in water, resulting in a slower dissolution process compared to highly soluble compounds like table salt.
In summary, the behavior of eggshell in water (specifically the dissolution of calcium carbonate) can be explained by the relatively low solubility of calcium carbonate due to its high lattice enthalpy, which results in only a small amount of calcium carbonate dissolving in water.