Question

1. sep construct explanations describe and explain the trend in the melting point data for the compounds listed in this table below.

compound	ch₄	c₂h₆	c₄h₁₀	c₅h₁₂	c₆h₁₄	c₇h₁₆	c₈h₁₈	c₉h₂₀

1. sep construct explanations why do you think the melting points of mgo and mgs are significantly higher than the other compounds that contain mg²⁺ as well as the alkali chlorides listed in the table?

1. sep engage in argument from evidence imagine you are a scientist employed by a manufacturer of cookware like pots and pans. which of the materials in the table would you use for a ceramic baking dish, and why?

1. sep analyze data classify electron dot structures for molecules with linear, bent, trigonal planar, trigonal pyramidal, and tetrahedral molecular geometry. explain by valence shell electron pair repulsion (vsepr) theory. write molecular geometry for the following molecules: h₂co, so₂, cf₂h₂, nh₃

Explanation:

4.

As the number of carbon - atoms in the hydrocarbon chain increases (from $CH_4$ to $C_8H_{20}$), the molar mass and the strength of London - dispersion forces increase. London - dispersion forces are weak intermolecular forces, but their magnitude increases with the size and molar mass of the molecules. Higher molar mass leads to more electrons and a larger electron cloud, which can be more easily polarized, resulting in stronger London - dispersion forces. Stronger intermolecular forces require more energy to overcome, thus the melting point increases.

$MgO$ and $MgS$ are ionic compounds with a high - charge density. The $Mg^{2 + }$ ion has a + 2 charge. In $MgO$, the $O^{2 - }$ ion and in $MgS$, the $S^{2 - }$ ion also have a - 2 charge. According to Coulomb's law, the force of attraction between ions ($F=\frac{kq_1q_2}{r^2}$, where $k$ is a constant, $q_1$ and $q_2$ are the charges of the ions, and $r$ is the distance between them) is directly proportional to the product of the charges of the ions. The high - charge ions in $MgO$ and $MgS$ result in strong ionic bonds. Other compounds with $Mg^{2+}$ or alkali chlorides have ions with lower charges or weaker ionic bonds, so $MgO$ and $MgS$ have higher melting points.

For a ceramic baking dish, a material with a high melting point and good heat - resistance is needed. Among the materials in the table (not shown completely here, but generally), materials with high melting points like certain metals or ceramics themselves would be suitable. High - melting - point materials can withstand the high temperatures used in baking without melting or deforming. Also, materials with good thermal conductivity can distribute heat evenly.

Answer:

The melting point of the listed hydrocarbons increases as the number of carbon atoms in the molecule increases due to the increase in molar mass and the strength of London - dispersion forces.

5.