Reactivity Series of Metals

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to Lesson

Podcast

Play an AI-generated podcast conversation about this lesson
Download our mobile app to listen on the go
Get App

Questions and Answers

What is the primary basis for the reactivity series?

  • The physical properties of metals, such as melting points
  • The metals' ability to lose electrons and form ions (correct)
  • The ability of metals to gain electrons and form ions
  • The chemical properties of metals, such as their reactivity with water

Which of the following metals is most likely to displace copper from its compound?

  • Gold (Au)
  • Iron (Fe) (correct)
  • Zinc (Zn)
  • Silver (Ag)

What is the oxidation reaction in the context of the reactivity series?

  • The reaction between a metal and acid
  • The loss of electrons by a metal to form an ion (correct)
  • The gain of electrons by a metal to form an ion
  • The reaction between a metal and oxygen

Which of the following is a characteristic of the alkaline earth metals?

<p>They lose electrons to form +2 ions (D)</p> Signup and view all the answers

What is the purpose of the reactivity series in predicting the outcome of single displacement reactions?

<p>To predict whether a reaction will occur or not (B)</p> Signup and view all the answers

What is the term for the gain of electrons by an ion to form a metal?

<p>Reduction (D)</p> Signup and view all the answers

Flashcards are hidden until you start studying

Study Notes

Reactivity Series

A reactivity series is a list of metals in order of their reactivity, from most reactive to least reactive.

Key Features

  • The series is based on the metals' ability to lose electrons and form ions.
  • The more reactive a metal, the more easily it loses electrons.
  • The reactivity series is used to predict the outcome of single displacement reactions.

Metals in the Reactivity Series

  1. Alkali Metals:
    • Most reactive
    • Lose electrons easily to form +1 ions
    • Examples: Potassium (K), Sodium (Na), Lithium (Li)
  2. Alkaline Earth Metals:
    • Less reactive than alkali metals
    • Lose electrons to form +2 ions
    • Examples: Calcium (Ca), Magnesium (Mg), Barium (Ba)
  3. Transition Metals:
    • Less reactive than alkaline earth metals
    • Can form ions with different charges
    • Examples: Iron (Fe), Copper (Cu), Zinc (Zn)
  4. Less Reactive Metals:
    • Not very reactive
    • Do not easily lose electrons
    • Examples: Silver (Ag), Gold (Au), Platinum (Pt)

Uses of the Reactivity Series

  • Predicting the outcome of single displacement reactions
  • Identifying the most reactive metals
  • Understanding the properties of metals and their ions

Important Reactions

  • Displacement reaction: a more reactive metal displaces a less reactive metal from its compound.
  • Oxidation: the loss of electrons by a metal to form an ion.
  • Reduction: the gain of electrons by an ion to form a metal.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Quiz Team

More Like This

Reactivity Series of Metals
0 questions
Reactivity Series of Metals
16 questions

Reactivity Series of Metals

VeritableBaritoneSaxophone avatar
VeritableBaritoneSaxophone
Metals and Reactivity Series
40 questions
Use Quizgecko on...
Browser
Browser