Question 1

Which of the following best describes a complete ionic equation?

Accepted Answer

An equation showing all aqueous compounds as dissociated ions.

Question 2

Which type of compound will NOT break up into ions in a complete ionic equation?

Accepted Answer

Solids, liquids, and gases

Question 3

Given the balanced molecular equation: $$3 \ce{CaBr2} (aq) + 2 \ce{Li3PO4} (aq) \rightarrow 6 \ce{LiBr} (aq) + 1 \ce{Ca3(PO4)2} (s)$$, which of the following is the correct complete ionic equation?

Accepted Answer

$$3 \ce{Ca$$^{2+}$$} (aq) + 6 \ce{Br^-} (aq) + 6 \ce{Li^+} (aq) + 2 \ce{PO4$$^{3-}$$} (aq) \rightarrow 6 \ce{Li^+} (aq) + 6 \ce{Br^-} (aq) + \ce{Ca3(PO4)2} (s)$$

Question 4

What is a spectator ion in a chemical reaction?

Accepted Answer

An ion that is present in both reactants and products but does not participate in the reaction.

Question 5

Given the reaction: $$\ce{(NH4)2SO4} (aq) + \ce{CaCl2} (aq) \rightarrow$$ products, which ions are spectator ions?

Accepted Answer

$$\ce{NH4^+}$$ and $$\ce{Cl^-}$$

Question 6

Which of the following steps is necessary to write a net ionic equation?

Accepted Answer

Write the balanced molecular equation and break up all aqueous compounds into their respective ions.

Question 7

When copper(II) bromide and lithium hydroxide are mixed in aqueous solution, what is the net ionic equation?

Accepted Answer

$$\ce{Cu$$^{2+}$$} (aq) + 2 \ce{OH^-} (aq) \rightarrow \ce{Cu(OH)2} (s)$$

Question 8

Which reagent could be used to separate the two anions from a solution containing magnesium nitrate and cesium hydroxide?

Accepted Answer

$$\ce{NH4CN}$$

Question 9

Which reagent could be used to separate the two cations from a solution containing lead(IV) acetate and cesium permanganate?

Accepted Answer

$$\ce{Sr(NO3)2}$$

Question 10

In the process of writing a net ionic equation, why are spectator ions removed?

Accepted Answer

Because they do not participate in the chemical change.

Question 11

A student mixes $$\ce{AgNO3} (aq) $$and $$\ce{NaCl} (aq). $$What is the net ionic equation for the reaction?

Accepted Answer

$$\ce{Ag^+} (aq) + \ce{Cl^-} (aq) \rightarrow \ce{AgCl} (s)$$

Question 12

Which of the following is TRUE about net ionic equations?

Accepted Answer

They show only the ions and molecules directly involved in the chemical change.

Question 13

If a compound is labeled as (aq) in a chemical equation, what does this indicate?

Accepted Answer

The compound is dissolved in water and exists as ions.

Question 14

Which of the following is the correct sequence of steps to write a balanced net ionic equation?

Accepted Answer

Write the balanced molecular equation, break up aqueous compounds into ions, cancel spectator ions, and write the net ionic equation.

Question 15

A solution contains $$\ce{Ba$$^{2+}$$}$$ and $$\ce{SO4$$^{2-}$$}$$ ions. What will happen when these ions are mixed?

Accepted Answer

A precipitate of $$\ce{BaSO4}$$ will form.

Question 16

Which of the following compounds would NOT be written as ions in a complete ionic equation?

Accepted Answer

$$\ce{AgCl} (s)$$

Question 17

A patient is given a solution containing $$\ce{K^+}$$ and $$\ce{Cl^-}$$ ions. Which reagent could be added to precipitate the $$\ce{Cl^-}$$ ions?

Accepted Answer

$$\ce{AgNO3}$$

Question 18

Which of the following best explains why $$\ce{Na^+}$$ and $$\ce{NO3^-}$$ are often spectator ions in precipitation reactions?

Accepted Answer

Because sodium and nitrate salts are highly soluble in water.

Question 19

A student writes the following net ionic equation: $$\ce{Pb$$^{2+}$$} (aq) + 2 \ce{I^-} (aq) \rightarrow \ce{PbI2} (s). $$Which type of reaction does this represent?

Accepted Answer

Precipitation reaction

Complete and Net Ionic Equations in GOB Chemistry

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