Periodic Table Trends Quiz
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Questions and Answers

What is the periodic trend for atomic radius as you go from left to right across the periodic table?

The atomic radius decreases.

What happens to atomic radius as you go down a group in the periodic table?

The atomic radius increases.

What is ionization energy?

The energy required to remove the loosely held outer electron from an atom.

How does ionization energy change as you go from left to right across the periodic table?

<p>Ionization energy increases.</p> Signup and view all the answers

What is electronegativity?

<p>A measure of the ability of an atom in a chemical compound to attract electrons to itself.</p> Signup and view all the answers

What is the trend for electronegativity as you go across from left to right in the periodic table?

<p>Electronegativity increases.</p> Signup and view all the answers

How does electronegativity change as you go down a group in the periodic table?

<p>Electronegativity decreases.</p> Signup and view all the answers

The ionic radius of a cation is smaller than its atomic radius because there are fewer ______.

<p>electrons</p> Signup and view all the answers

The ionic radius of an anion is bigger than its atomic radius because added electrons ______ each other.

<p>repel</p> Signup and view all the answers

The atomic structure diagrams show a sodium atom gaining an electron.

<p>False (B)</p> Signup and view all the answers

Flashcards

Atomic Radius

One half the distance between the nuclei of two atoms of the same element.

Ionization Energy

Energy needed to remove an electron from an atom.

Atomic Radius - Period Trend

Atomic radius decreases as you move across a period (left to right) on the periodic table.

Atomic Radius - Group Trend

Atomic radius increases as you move down a group (top to bottom) on the periodic table.

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Ionization Energy - Period Trend

Ionization energy increases as you move across a period (left to right).

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Ionization Energy - Group Trend

Ionization energy decreases as you move down a group (top to bottom).

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Cation

A positively charged ion.

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Anion

A negatively charged ion.

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Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons towards itself.

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Valence Electrons

Electrons in the outermost shell of an atom.

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Study Notes

  • Periodic trends describe patterns in the properties of elements across the periodic table.
  • Atomic radius: Half the distance between the nuclei of two atoms of the same element.
    • Trend: Decreases as you go from left to right across the periodic table.
      • Reason: As electrons are added across a period, the electrons are pulled closer to the positive nucleus.
    • Trend: Increases as you go down a group.
      • Reason: As electrons occupy energy levels that are farther from the nucleus, there is less pull between the outer shell electrons and the positive nucleus.
  • Ionization energy: The energy required to remove an electron from an atom.
    • Trend: Increases as you go from left to right across the periodic table.
      • Reason: As the electrons increase, the attraction for the outer level of electrons also increases, requiring more energy to remove an electron.
    • Trend: Decreases as you go down a group.
      • Reason: As you go down a group, the positive nuclear charge increases, but the outer electrons are farther from the nucleus resulting in a decrease in ionization energy.

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Description

Test your knowledge on the trends of the periodic table, including atomic radius and ionization energy. Explore how these properties change across periods and groups. This quiz will challenge your understanding of these fundamental concepts in chemistry.

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