Activity Series and Spontaneous Reactions

This video tutorial covers the activity series found in Table J of reference tables, focusing on its application in redox reactions and electrochemistry. It explains how the series ranks metals and nonmetals by reactivity, influencing their likelihood to undergo oxidation or reduction. The tutorial also discusses conditions for spontaneous reactions and provides examples of how to use Table J to solve related questions.

What is the primary use of the activity series in electrochemistry?

• To determine the boiling points of metals

• To measure the electrical conductivity of solutions

• To predict the reactivity of metals and nonmetals

• To calculate the density of elements

Which metals are more likely to be oxidized according to the activity series?

• Metals not listed in the series

• Metals at the top of the series

• Metals in the middle of the series

• Metals at the bottom of the series

What condition must be met for a metal to react spontaneously with another metal ion?

• The metal must not be in the series

• The metal and ion must be at the same level

• The metal must be above the ion in the series

• The metal must be below the ion in the series

Which metal will react spontaneously with a hydrogen ion according to the activity series?

• Gold

• Iron

• Silver

• Copper

Which metal can replace the nickel ion in nickel nitrate?

• Tin

• Chromium

• Lead

• Zinc

Why is chromium able to replace nickel in a compound?

• Chromium is less reactive than nickel

• Chromium is a noble metal

• Chromium has a lower atomic number

• Chromium is higher on the activity series

Which atom-ion pair will oxidize spontaneously under standard conditions?

• Cobalt and zinc ion

• Copper and silver ion

• Iron and copper ion

• Cobalt and nickel ion

What determines if an atom will oxidize spontaneously in a reaction?

• The atom's color

• The atom's atomic mass

• The atom's position above the ion in the series

• The atom's position below the ion in the series

In the context of the activity series, what does it mean for a reaction to be spontaneous?

• The reaction requires external energy

• The reaction occurs without external energy

• The reaction is reversible

• The reaction is endothermic