What is the correct order of boiling points for CH3OH, KNO3, Ne, C2H6?
Ne < C2H6 < CHOH. KNO3 is a solid. First it must be melted and then it can boil. Ionic compounds have a very high boiling point assuming they don't decompose before boiling.
Well, it seems like you've got quite the lineup here! Let's put these compounds in order, from highest to lowest boiling point, like contestants in a "Boiling Point Beauty Pageant":
1. KNO3: This compound is like a beauty queen with stellar performance. It forms strong ionic bonds, which require a lot of energy to break. So, it takes the crown for having the highest boiling point.
2. CH3OH: Next up, we have good ol' CH3OH, also known as methanol. Although not as hot as KNO3, methanol still has some sizzling characteristics. It forms hydrogen bonds, which add a little extra stability and raise its boiling point.
3. C2H6: Here comes C2H6, or ethane, strutting its stuff. It's a simple hydrocarbon with only van der Waals forces to hold it together, which aren't as strong as those in KNO3 or CH3OH. So, it's not a boiling point superstar, but it still earns a place on the podium.
4. Ne: Last but certainly not least, we have our noble gas, Ne. Poor Ne, it doesn't even have any boiling point to speak of! It prefers to stay a gas at any temperature, showing us that sometimes, it's cool to be different.
So, to summarize the "Boiling Point Beauty Pageant" lineup: It's KNO3, CH3OH, C2H6, and Ne (or, as we say in the humor business, "KNO3, methanol, ethane, and Ne-gligible").
To determine the correct order of boiling points for CH3OH, KNO3, Ne, and C2H6, we need to examine their chemical properties and intermolecular forces.
1. Ne (Neon) is a noble gas that exists as individual atoms. It has very weak London dispersion forces between its atoms. Since it is a non-polar molecule, it has the lowest boiling point.
So, the correct order so far is: Ne < (unknown order for CH3OH, KNO3, and C2H6)
2. CH3OH (Methanol) is a covalent compound. It has intermolecular hydrogen bonding due to the presence of hydrogen atoms bonded to an electronegative oxygen atom. Hydrogen bonding is a strong intermolecular force, so CH3OH has a relatively higher boiling point compared to Ne.
So, the correct order so far is: Ne < CH3OH < (unknown order for KNO3 and C2H6)
3. C2H6 (Ethane) is a covalent compound that only has London dispersion forces. It has relatively larger and more compact molecules compared to CH3OH, so it has slightly stronger London dispersion forces. Thus, C2H6 has a higher boiling point than CH3OH.
So, the correct order so far is: Ne < CH3OH < C2H6 < (unknown order for KNO3)
4. KNO3 (Potassium Nitrate) is an ionic compound composed of potassium cations (K+) and nitrate anions (NO3-). Ionic compounds have strong electrostatic forces of attraction between oppositely charged ions. These forces are known as ionic bonds. When KNO3 is heated, these ionic bonds need to be broken, resulting in a relatively high boiling point compared to the previous compounds.
So, the final correct order is: Ne < CH3OH < C2H6 < KNO3
Final order of boiling points:
1. Neon (Ne)
2. Methanol (CH3OH)
3. Ethane (C2H6)
4. Potassium Nitrate (KNO3)
To determine the correct order of boiling points for CH3OH, KNO3, Ne, and C2H6, we need to consider the intermolecular forces between the molecules.
Boiling points generally increase with increasing molecular size and intermolecular forces. The stronger the intermolecular forces, the higher the boiling point.
Let's analyze each compound one by one:
1. Ne (neon): Neon is a noble gas with a monatomic structure. Since noble gases have weak van der Waals forces, the boiling point of Ne is very low and remains as a gas at all temperatures. Therefore, Ne has the lowest boiling point.
2. CH3OH (methanol): Methanol is a polar molecule with a bent shape, which gives rise to dipole-dipole interactions. It also has hydrogen bonding due to the presence of a hydrogen atom bonded directly to an oxygen atom. Both dipole-dipole interactions and hydrogen bonding contribute to stronger intermolecular forces than van der Waals forces. Thus, methanol has a higher boiling point than Ne.
3. C2H6 (ethane): Ethane is a nonpolar molecule composed of only carbon and hydrogen atoms. It can exhibit weak van der Waals forces, such as London dispersion forces. However, the boiling point of ethane is lower than that of methanol because it lacks dipole-dipole interactions or hydrogen bonding.
4. KNO3 (potassium nitrate): Potassium nitrate is an ionic compound composed of potassium ions (K+) and nitrate ions (NO3-). Ionic compounds have strong electrostatic forces of attraction between ions, known as ion-ion interactions. These interactions are significantly stronger than the intermolecular forces found in the other compounds mentioned. As a result, KNO3 has the highest boiling point among the given compounds.
Therefore, the correct order of boiling points from lowest to highest is: Ne, C2H6, CH3OH, KNO3.