Redox Reactions and Net Ionic Equations

Which half-reaction shows conservation of charge?

• Cu + e^– → Cu⁺

• Cu⁺ → Cu + e^–

• Cu²⁺ + 2e^– → Cu

• Cu²⁺ → Cu + 2e^–

Tags

NGSS.HS-PS1-7

Which half-reaction equation represents the reduction of a potassium ion?

• K⁺ + e^– → K

• K + e^– → K⁺

• K⁺ → K + e^–

• K → K⁺ + e^–

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which statement is true:
Mg → Mg²⁺ + 2e^–

• Mg gains 2 electrons

• Mg_²⁺ loses 2 electrons

• Mg loses 1 electron

• Mg loses 2 electrons

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-7

In the reaction
2Ca(s) + O₂(g) --> 2CaO(s), calcium is __________

• Reduced

• Synthesized

• Oxidized

• None of the above

In the reaction Zn + H₂O --> ZnO₂ + H₂
 which element, if any, is oxidized? 

• Zinc

• Hydrogen

• Oxygen

• None

Cl₂ + 2e- --> 2Cl ^- is an example of:

• a chemical reaction

• redox

• oxidation

• reduction

Oxidation is the loss of electron, meaning, there is an increase of oxidation number

• True

• False

Tags

NGSS.HS-PS1-1

The species that gain electron is _____ and usually the ____ agent

• oxidized;oxidizing

• reduced;reducing

• reduced;oxidizing

• oxidized; reducing

The species that loses electron is _____ and usually _____ agent.

• oxidized;reducing

• reduced;oxidizing

• oxidized;oxidizing

• reduced;reducing

The third step in balancing the redox reaction using oxidation-number-change is

• Check the balancing for both atoms and charge.

• Use coefficients to make the total increase in oxidation number equal to the total decrease in oxidation number.

• Assign oxidation numbers to each of the atoms in the equation and write the numbers above the atom.

• Use a line to connect the atoms that are undergoing a change in oxidation number.