Selected chlorides have the following melting points: NaCl (801 °C), MgCl 2 (714 °C), PCl 3 (-94 °C), SCl 2 (-121 °C) (a) For each compound, indicate what type its solid form is (molecular, metallic, ionic, or covalent-network).

Everyone who asked classify the following floor rides based on their melting points, recall that compounds with low melting points are gonna be molecular in compounds with high melting points are gonna be ionic. We have c. F four and this has a low melting point. So this is gonna be a molecular for n a f. This has a high melting point, so that's gonna be ionic N F three. This has a low melting point, so this is molecular, And for M. G.F. this has a high melting point. So this is ionic. Thanks for watching my video, and I hope it was helpful.

Ch.12 - Solids and Modern Materials

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Brown 14th Edition

Ch.12 - Solids and Modern Materials

Problem 103a

Chapter 12, Problem 103a

Selected chlorides have the following melting points: NaCl (801 °C), MgCl₂ (714 °C), PCl₃ (-94 °C), SCl₂ (-121 °C) (a) For each compound, indicate what type its solid form is (molecular, metallic, ionic, or covalent-network).

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Identify the type of bonding present in each compound based on the elements involved.

NaCl is composed of a metal (Na) and a non-metal (Cl), indicating it is an ionic compound.

MgCl2 is also composed of a metal (Mg) and a non-metal (Cl), indicating it is an ionic compound.

PCl3 consists of non-metals (P and Cl), suggesting it is a molecular compound with covalent bonds.

SCl2 consists of non-metals (S and Cl), suggesting it is a molecular compound with covalent bonds.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionic Compounds

Ionic compounds are formed from the electrostatic attraction between positively and negatively charged ions. They typically consist of a metal and a non-metal, resulting in a crystalline structure that exhibits high melting points due to strong ionic bonds. Examples include NaCl and MgCl2, which are solid at room temperature and have high melting points.

Molecular Compounds

Molecular compounds are formed when two or more non-metals share electrons through covalent bonds. These compounds usually have lower melting and boiling points compared to ionic compounds and can exist as gases, liquids, or solids at room temperature. PCl3 and SCl2 are examples of molecular compounds, characterized by their discrete molecular units.

Melting Points and Bonding Types

The melting point of a substance is influenced by the type of bonding present. Ionic compounds generally have high melting points due to the strong forces between ions, while molecular compounds have lower melting points due to weaker van der Waals forces. Understanding the relationship between bonding types and melting points helps in classifying compounds accurately.

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Imagine the primitive cubic lattice. Now imagine pushing on top of it, straight down. Next, stretch another face by pulling it to the right. All angles remain 90°. What kind of primitive lattice have you made?

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Pure iron crystallizes in a body-centered cubic structure, shown in the figure. but small amounts of impurities can stabilize a facecentered cubic structure. Which form of iron has a higher density?

Selected chlorides have the following melting points: NaCl (801 °C), MgCl2 (714 °C), PCl3 (-94 °C), SCl2 (-121 °C) (a) For each compound, indicate what type its solid form is (molecular, metallic, ionic, or covalent-network).

Verified video answer for a similar problem:

Key Concepts

Ionic Compounds

Molecular Compounds

Melting Points and Bonding Types

Selected chlorides have the following melting points: NaCl (801 °C), MgCl₂ (714 °C), PCl₃ (-94 °C), SCl₂ (-121 °C) (a) For each compound, indicate what type its solid form is (molecular, metallic, ionic, or covalent-network).