Oxidation States and Electrochemistry

An oxidizing agent will

• increase in mass

• lose electrons

• be reduced

• increase in oxidation number

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

In a redox reaction, the species that loses electrons

• is called the cathode

• is oxidized

• gains mass at the electrode

• decreases in oxidation number

Tags

NGSS.HS-PS1-2

The reaction 2NaCl → 2Na + Cl₂ is an example of

• a reduction reaction, only

• both an oxidation and reduction reaction

• an oxidation reaction, only

• neither an oxidation nor a reduction reaction

Tags

NGSS.HS-PS1-2

As an element is oxidized, its oxidation number

• decreases as electrons are lost

• increases as electrons are lost

• decreases as electrons are gained

• increases as electrons are gained

Tags

NGSS.HS-PS1-2

Oxidation-reduction reactions occur because of the competition between particles for

• electrons

• positrons

• protons

• neutrons

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Mg + PbCl₂ → MgCl₂ + Pb

Which statement correctly describes the oxidation and reduction that occur?

• Mg is oxidized and Pb⁺² is reduced

• Mg is oxidized and Cl^- is reduced

• Mg is reduced and Cl^- is oxidized

• Mg is reduced and Pb⁺² is oxidized

Tags

NGSS.HS-PS1-2

In the reactions

Sn⁺² + 2Fe⁺³ --> Sn⁺⁴ + 2Fe⁺²,

the reducing agent is

• Fe⁺³

• Sn⁺²

• Sn⁺⁴

• Fe⁺²

Tags

NGSS.HS-PS1-2

Pb + 2Ag⁺ → Pb⁺² + 2Ag

The chemical species being reduced is

• Ag

• Pb

• Pb⁺²

• Ag⁺

Tags

NGSS.HS-PS1-2

In the reactions

Sn⁺² + 2Fe⁺³ → Sn⁺⁴ + 2Fe⁺²

the oxidizing agent is

• Sn⁺⁴

• Sn⁺²

• Fe⁺³

• Fe⁺²

Tags

NGSS.HS-PS1-2

Galvanic cells convert

• mechanical energy in to electrical energy

• potential energy in to electrical energy

• electrical energy in to chemical energy

• chemical energy in to electrical energy

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-3