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Chapter 5: Problem 1

Predict the formula of the compound that forms between carbon and chlorine.

Short Answer

Expert verified
The compound that forms between carbon and chlorine is predicted to be Carbon Tetrachloride, with the formula \(CCl_4\). This is because carbon, with 4 valence electrons, can share its electrons with 4 chlorine atoms, each needing 1 electron to achieve a stable state.

Step by step solution

01

Determining the Valency of Carbon (C)

Carbon belongs to group 14 (also known as group IVA) on the periodic table. Elements in this group have 4 valence electrons. Since elements typically strive to achieve a stable state by having a full outer shell (8 electrons, except for hydrogen and helium which have 2), carbon needs to gain, lose, or share 4 electrons to form a stable compound.
02

Determining the Valency of Chlorine (Cl)

Chlorine belongs to group 17 (also known as group VIIA) on the periodic table. Elements in this group have 7 valence electrons. To achieve a stable state, chlorine needs to gain, lose, or share 1 electron.
03

Combining Carbon and Chlorine

Since carbon needs 4 electrons and chlorine needs only 1 electron, carbon can share its 4 valence electrons with 4 chlorine atoms. This way, each chlorine atom will have 8 electrons in its valence shell, achieving a stable state. Carbon will also have access to 8 electrons, with one shared from each of the 4 chlorine atoms. This results in the formation of a compound with 1 carbon atom and 4 chlorine atoms.
04

Writing the Predicted Formula for the Compound

Combining the information about how the carbon and chlorine atoms bond, the predicted formula for the compound formed between carbon and chlorine is: \(C Cl_4\) This compound is called Carbon Tetrachloride.

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Most popular questions from this chapter

Ethers are compounds of \(\mathrm{C}, \mathrm{H}\), and \(\mathrm{O}\) that are often used as solvents. One particular ether molecule has the formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} .\) The structure is such that both carbons are attached to the oxygen atom, and there are no \(\mathrm{O}-\mathrm{H}\) bonds. Starting with dot diagrams for the atoms, draw a dot diagram for this ether molecule. How many bonding pairs does the molecule have? How many lone pairs?

Classify the bonds in each of the following as ionic, covalent, or polar covalent. Explain each choice. (a) \(\mathrm{Br}_{2}\) (b) \(\mathrm{PCl}_{3}\) (c) LiCl (d) ClF (e) \(\mathrm{MgCl}_{2}\)

Give the proper name for the following binary covalent compounds: (a) \(\mathrm{PCl}_{3}\) (b) \(\mathrm{SO}_{2}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{4}\) (d) \(\mathrm{P}_{5} \mathrm{O}_{10}\)

Using only the periodic table, arrange these sets of atoms in order of increasing electronegativity: (a) \(\mathrm{Li}, \mathrm{Be}, \mathrm{K}\) (b) \(\mathrm{O}, \mathrm{Si}, \mathrm{S}\) (c) \(\mathrm{Br}_{t} \mathrm{I}, \mathrm{Te}\)

Draw a dot diagram for the \(\mathrm{NO}_{2}^{+}\) cation.
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