Principles of Chemistry Review: Nomenclature, Solubility Rules, Lattice Energy, and Redox

Practice flashcards covering polyatomic ion nomenclature, acid naming rules, 7 strong acids, detailed solubility rules, lattice energy trends, and basic redox concepts from the lecture notes.

What prefix or suffix convention distinguishes an oxyanion with more oxygen atoms from one with one less oxygen atom?

The suffix -ate is used for the oxyanion with more oxygen atoms, and the suffix -ite is used for the oxyanion with one less oxygen atom.

What is the chemical formula and oxygen count for the nitrate ion?

The formula is $NO_3^-$ and it contains 3 oxygens.

What is the chemical formula and oxygen count for the nitrite ion?

The formula is $NO_2^-$ and it contains 2 oxygens.

What is the chemical formula and oxygen count for the sulfate ion?

The formula is $SO_4^{2-}$ and it contains 4 oxygens.

What is the chemical formula and oxygen count for the sulfite ion?

The formula is $SO_3^{2-}$ and it contains 3 oxygens.

What is the chemical formula and oxygen count for the phosphate ion?

The formula is $PO_4^{3-}$ and it contains 4 oxygens.

What is the chemical formula and oxygen count for the phosphite ion?

The formula is $PO_3^{3-}$ and it contains 3 oxygens.

What is the chemical formula and oxygen count for the chlorate ion?

The formula is $ClO_3^-$ and it contains 3 oxygens.

What is the chemical formula and oxygen count for the chlorite ion?

The formula is $ClO_2^-$ and it contains 2 oxygens.

How does an anion ending in -ate change its suffix when naming its corresponding acid?

An -ate ion changes to an -ic acid.

What acid is formed from the nitrate ion ($NO_3^-$)?

Nitric acid ($HNO_3$).

How does an anion ending in -ite change its suffix when naming its corresponding acid?

An -ite ion changes to an -ous acid.

What acid is formed from the nitrite ion ($NO_2^-$)?

Nitrous acid ($HNO_2$).

What memory trick is provided for remembering acid naming connections?

"I ate something ic-ky, but it was sulfur-ous and delicious-ite." (or simply: -ate $\rightarrow$ -ic, -ite $\rightarrow$ -ous).

What are the 7 strong acids to memorize for dissolution and ionization questions?

$HCl$, $HBr$, $HI$, $HNO_3$, $H_2SO_4$, $HClO_4$, and $HClO_3$.

Why is $HF$ classified as a weak acid rather than a strong acid?

Because the $H-F$ bond/attraction is too strong to dissociate fully.

For what specific types of questions do you need to know the 7 strong electrolytes/acids?

Dissolution and ionization questions.

Which cations are generally soluble without exceptions according to the solubility rules?

Group 1 cations ($Li^+$, $Na^+$, $K^+$, etc.) and $NH_4^+$.

Which polyatomic anions are generally soluble with no listed insoluble exceptions?

Nitrates ($NO_3^-$), acetates ($C_2H_3O_2^-$), chlorates ($ClO_3^-$), and bicarbonates ($HCO_3^-$).

Which halide ions are generally soluble?

$Cl^-$, $Br^-$, and $I^-$.

What are the insoluble exceptions for halide ions ($Cl^-$, $Br^-$, $I^-$)?

$Ag^+$, $Hg_2^{2+}$, and $Pb^{2+}$.

What are the insoluble exceptions for sulfate ions ($SO_4^{2-}$)?

$Ag^+$, $Ba^{2+}$, $Ca^{2+}$, $Hg_2^{2+}$, $Pb^{2+}$, and $Sr^{2+}$.

Which five anion groups are listed as generally insoluble?

Carbonates ($CO_3^{2-}$), phosphates ($PO_4^{3-}$), chromates ($CrO_4^{2-}$), sulfides ($S^{2-}$), and hydroxides ($OH^-$).

What makes generally insoluble anions (like $CO_3^{2-}$, $PO_4^{3-}$, $CrO_4^{2-}$, $S^{2-}$, $OH^-$) soluble?

When they are paired with Group 1 cations or $NH_4^+$.

Which metal hydroxide is soluble in addition to those paired with Group 1 cations or $NH_4^+$?

Hydroxides with $Ba^{2+}$.

According to lattice energy trends, how does ionic charge affect lattice energy and solubility?

Higher ionic charges lead to higher lattice energy and lower solubility.

Why are sulfides and phosphates with $+2/-2$ or $+3/-3$ charges mostly insoluble?

Because higher ionic charges result in higher lattice energy, which leads to lower solubility.

According to lattice energy trends, how does the size difference between a cation and anion affect solubility?

A larger size difference between the cation and anion raises solubility.

Based on the size difference effect, why is $CsF$ more soluble than $LiF$?

Because $CsF$ has a larger size difference between its cation ($Cs^+$) and anion ($F^-$) than $LiF$ does.

What is the rule for assigning oxidation states to free elements in their natural state?

Free elements in their natural state always have an oxidation state of $0$.

What examples of free elements in their natural state are given in the basic rules for oxidation states?

$Cr(s)$, $Sn(s)$, $O_2$, and $H_2$.

What is the oxidation state of a monatomic ion?

An oxidation state equal to its charge (such as $+2$, $+3$, etc.).

What examples of monatomic ions are given in the basic rules for oxidation states?

$Sn^{2+}$ and $Cr^{3+}$.

What does the mnemonic OIL stand for in redox reactions?

Oxidation Is Loss of electrons (oxidation state becomes more positive).

What does the mnemonic RIG stand for in redox reactions?

Reduction Is Gain of electrons (oxidation state becomes more negative/less positive).

How does an element's oxidation state change during oxidation?

It becomes more positive.

How does an element's oxidation state change during reduction?

It becomes more negative (or less positive).

What is the reducing agent in a redox reaction?

The species that gets oxidized (it causes the other species to be reduced).

What is the oxidizing agent in a redox reaction?

The species that gets reduced (it causes the other species to be oxidized).

What chemical reaction equation is presented for Problem 3 Part a in the notes?

$Cr(s) + Sn^{2+}(aq) \rightarrow Cr^{3+}(aq) + Sn(s)$.

In the reaction $Cr(s) + Sn^{2+}(aq) \rightarrow Cr^{3+}(aq) + Sn(s)$, what is the initial oxidation state of $Cr(s)$?

$0$.

In the reaction $Cr(s) + Sn^{2+}(aq) \rightarrow Cr^{3+}(aq) + Sn(s)$, what is the initial oxidation state of $Sn^{2+}(aq)$?

$+2$.

In the reaction $Cr(s) + Sn^{2+}(aq) \rightarrow Cr^{3+}(aq) + Sn(s)$, which species undergoes oxidation?

$Cr(s)$ undergoes oxidation (its oxidation state increases from $0$ to $+3$).

In the reaction $Cr(s) + Sn^{2+}(aq) \rightarrow Cr^{3+}(aq) + Sn(s)$, which species undergoes reduction?

$Sn^{2+}(aq)$ undergoes reduction (its oxidation state decreases from $+2$ to $0$).

In the reaction $Cr(s) + Sn^{2+}(aq) \rightarrow Cr^{3+}(aq) + Sn(s)$, which species acts as the reducing agent?

$Cr(s)$.

In the reaction $Cr(s) + Sn^{2+}(aq) \rightarrow Cr^{3+}(aq) + Sn(s)$, which species acts as the oxidizing agent?

$Sn^{2+}(aq)$.