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Chapter 3: Problem 112

Write the formula for each of the following compounds: a. diboron trioxide b. arsenic pentafluoride c. dinitrogen monoxide d. sulfur hexachloride

Short Answer

Expert verified
The chemical formulas for the given compounds are: a. Diboron trioxide: \(B_2O_3\) b. Arsenic pentafluoride: \(AsF_5\) c. Dinitrogen monoxide: \(N_2O\) d. Sulfur hexachloride: \(SF_6\)

Step by step solution

01

a. Diboron trioxide

1. Identify the elements: In the compound "diboron trioxide," we have two elements - boron (B) and oxygen (O). 2. Identify the prefixes: In our compound name, we have the prefix "di" for boron, which means 2 atoms of boron, and "tri" for oxygen, which means 3 atoms of oxygen. 3. Write the formula: Combine the elements with their respective prefixes. So, diboron trioxide has a chemical formula of \(B_2O_3\).
02

b. Arsenic pentafluoride

1. Identify the elements: In the compound "arsenic pentafluoride," we have two elements - arsenic (As) and fluorine (F). 2. Identify the prefixes: For arsenic, no prefix is provided, which means 1 atom of arsenic is present. For fluorine, we have the prefix "penta," which means 5 atoms of fluorine. 3. Write the formula: Combine the elements with their respective prefixes. So, arsenic pentafluoride has a chemical formula of \(AsF_5\).
03

c. Dinitrogen monoxide

1. Identify the elements: In the compound "dinitrogen monoxide," we have two elements - nitrogen (N) and oxygen (O). 2. Identify the prefixes: For nitrogen, we have the prefix "di," which means 2 atoms of nitrogen, and for oxygen, we have the prefix "mono," which means 1 atom of oxygen. 3. Write the formula: Combine the elements with their respective prefixes. So, dinitrogen monoxide has a chemical formula of \(N_2O\).
04

d. Sulfur hexachloride

1. Identify the elements: In the compound "sulfur hexachloride," we have two elements - sulfur (S) and chlorine (Cl). 2. Identify the prefixes: For sulfur, no prefix is provided, which means 1 atom of sulfur is present. For chlorine, we have the prefix "hexa," which means 6 atoms of chlorine. 3. Write the formula: Combine the elements with their respective prefixes. So, sulfur hexachloride has a chemical formula of \(SF_6\).

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Most popular questions from this chapter

Write the formula for each of the following compounds: a. zinc chloride b. \(\operatorname{tin}(1 \mathrm{V})\) fluoride c. calcium nitride d. aluminum sulfide e. mercury(I) selenide f. silver iodide

Use the following data to estimate \(\Delta E\) for the reaction: $$\mathrm{Ba}(s)+\mathrm{Br}_{2}(g) \longrightarrow \mathrm{BaBr}_{2}(s) \quad \Delta E=?$$ Lattice energy First ionization energy of Ba Second ionization energy of Ba Electron affinity of Br Bond energy of \(\mathrm{Br}_{2}\) Enthalpy of sublimation of Ba \(-1985 \mathrm{kJ} / \mathrm{mol}\) \(503 \mathrm{kJ} / \mathrm{mol}\) \(965 \mathrm{kJ} / \mathrm{mol}\) -325 kJ/mol \(193 \mathrm{kJ} / \mathrm{mol}\) \(178 \mathrm{kJ} / \mathrm{mol}\)

Lewis structures can be used to understand why some molecules react in certain ways. Write the Lewis structures for the reactants and products in the reactions described below. a. Nitrogen dioxide dimerizes to produce dinitrogen tetroxide. b. Boron trihydride accepts a pair of electrons from ammonia, forming \(\mathrm{BH}_{3} \mathrm{NH}_{3}\) Give a possible explanation for why these two reactions occur.

Write the formula for each of the following compounds: a. sodium oxide b. sodium peroxide c. potassium cyanide d. copper(II) nitrate e. selenium tetrabromide f. iodous acid g. lead(IV) sulfide h. copper(I) chloride I. gallium arsenide J. cadmium selenide k. zinc sulfide I. nitrous acid m. diphosphorus pentoxide

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