Covalent bonds and Lewis formulas

The final step can be summarized as: $\ce{3NO2(g) + H2O(l) -> 2HNO3(aq) + NO(g)}$ $\Delta H^\ominus = -138\ \mathrm{kJ\,mol^{-1}}$ Describe the types of bonding found in the concentrated aqueous nitric acid product.

Nitric acid, $\ce{HNO3}$, is strong, while nitrous acid, $\ce{HNO2}$, is weak. (i) Outline the difference between a strong and a weak acid. (ii) Deduce the Lewis formula and the molecular geometry for the nitrite ion, $\ce{NO2-}$.

(i) Write the equation for the reaction of Rb with water, $\ce{H2O}$, including state symbols. (ii) Describe the type of bonding in $\ce{Rb}$ and in $\ce{H2O}$, and explain how the valence electrons in each produce that type of bond.

At room temperature hydrogen cyanide is a liquid that evaporates readily, whereas ethyne, $\ce{C2H2}$, which has almost the same molar mass, is a gas that boils at −84 °C. (i) Draw the Lewis formula of the hydrogen cyanide molecule, showing all valence…

Both ionic and covalent bonding are present in sodium ethanedioate, $\ce{Na2C2O4}$. (i) Describe the two types of bonding. Ionic bonding: Covalent bonding: (ii) Deduce a Lewis formula of the ethanedioate ion, $\ce{C2O4^2-}$. (iii) State the geometry of the…

(i) State the electron configuration of a nitrogen atom. (ii) Draw the Lewis formula of ammonia. (iii) Deduce the electron domain geometry and the molecular geometry of the ammonia molecule. (iv) Explain why the ammonia molecule is polar.

For which of these molecules is the octet rule satisfied by every atom? I. $\ce{SiCl4}$ II. $\ce{NCl3}$ III. $\ce{BCl3}$ A. I and II only B. I and III only C. II and III only D. I, II and III

Simple bonding theory expects every atom in a covalent molecule to end up with eight valence electrons. Two stable gas-phase molecules, $\ce{BF3(g)}$ and $\ce{BeF2(g)}$, do not fit this picture. Which adaptation of the bonding model was needed to explain…

Another hydride of sulfur is hydrogen sulfide, $\ce{H2S}$; it forms a sulfonium ion, $\ce{H3S+}$. State the types of bonds present in the sulfonium ion, $\ce{H3S+}$, and explain how these bonds are formed.

Sulfur forms a dichloride, $\ce{SCl2}$. Deduce the Lewis formula of $\ce{SCl2}$.

(i) Deduce the condensed electron configuration of chlorine. (ii) Describe the bonding in a molecule of chlorine in terms of valence electrons. (iii) Explain why chlorine has a much lower boiling point than bromine, although both exist as simple diatomic…

Sodium peroxide, $\ce{Na2O2}$, contains the peroxide ion. Draw the Lewis formula of this anion.