Periodic Trends in Chemistry
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Questions and Answers

Which of the following describes ionization energy?

  • The size of the electron cloud around an atom
  • The energy needed to remove an electron from an atom (correct)
  • The ability of an atom to attract electrons
  • The distance from the nucleus to the outermost shell

The ionic radius increases from left to right across a period.

False (B)

Which element has the largest atomic radius?

Francium

The ionic radius of a cation is usually _____ than the ionic radius of its neutral atom.

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

Match the following terms with their definitions:

<p>Atomic radius = Distance from the nucleus to the outermost shell Cation = Positively charged ion Anion = Negatively charged ion Electron affinity = Energy change when an electron is added to an atom</p> Signup and view all the answers

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

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

Electronegativity increases as you move from left to right across a period.

<p>True (A)</p> Signup and view all the answers

What occurs to the ionic radius when an atom gains an electron?

<p>It increases</p> Signup and view all the answers

What happens to ionization energy as you move from left to right across a period?

<p>It increases (C)</p> Signup and view all the answers

Electronegativity increases as you move from top to bottom in a group.

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

What is the main characteristic of a non-metal in terms of atomic radius?

<p>Small atomic radius</p> Signup and view all the answers

When an atom accepts an electron to form an anion, the energy __________ is released.

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

Match the following properties to their corresponding types:

<p>Big atomic radius = Metallic property High ionization energy = Non-metallic property Good conductor = Metallic property Low electronegativity = Metallic property</p> Signup and view all the answers

Which property tends to increase as you move from top to bottom on the periodic table?

<p>Atomic size (A)</p> Signup and view all the answers

It is easier for an atom with more valence electrons to accept an electron.

<p>True (A)</p> Signup and view all the answers

What element is known to be the most electronegative?

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

Flashcards

Atomic Radius Trend

Atomic radius increases down a group and decreases across a period.

Atomic Radius Definition

Distance from nucleus to outer electron shell in a neutral atom.

Ionization Energy Trend

Ionization energy increases across a period and generally decreases down a group.

Ionization Energy Definition

Energy needed to remove an electron from an atom.

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Ionic Radius Trend (Cations)

Ionic radius decreases when forming a cation. Same charge across the table.

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Ionic Radius Trend (Anions)

Ionic radius increases when gaining electrons. (Same charge across the table)

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Periodic Law

Properties of elements vary periodically with increasing atomic number.

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Cation vs. Anion

Cations are positively charged (lose electrons). Anions are negatively charged (gain electrons).

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Electron Affinity Trend

Electron affinity increases across a period (left to right) and decreases down a group (top to bottom) on the periodic table.

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Electronegativity Trend

Electronegativity increases across a period (left to right) and decreases down a group (top to bottom) on the periodic table.

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Metallic Property Trend

Metallic properties increase down a group (top to bottom) and decrease across a period (left to right) on the periodic table.

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Nonmetallic Property Trend

Nonmetallic properties decrease down a group (top to bottom) and increase across a period (left to right) on the periodic table.

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Atomic Radius Trend (Size)

Atomic radius increases down a group (top to bottom) and decreases across a period (left to right) on the periodic table.

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Ion Size Trend

Cations are smaller than their parent atoms and anions are larger.

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Periodic Trends

Predictable patterns of change in properties of elements across periods or down groups on the periodic table.

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Study Notes

  • Periodic Law: Elements' physical and chemical properties vary periodically with increasing atomic number.

Atomic Radius

  • Defined as the distance from the nucleus to the outermost electron shell in a neutral atom.
  • Trend: Increases down a group (top to bottom) due to higher energy levels further from the nucleus. Decreases across a period (left to right) due to increasing nuclear attraction, pulling electrons closer.
  • Example: Francium is the largest, fluorine the smallest.

Ionic Radius

  • The distance from the nucleus to the outermost electron orbital of an ion.
  • Cations: Positively charged ions. Losing electrons leads to a smaller radius as repulsion decreases and nuclear attraction increases.
  • Anions: Negatively charged ions. Gaining electrons increases electron repulsion, expanding the electron cloud and increasing the radius.
  • Trend: Increases down a group, decreases across a period. Ions with the same charge will follow this same trend, but a cation will generally be smaller than its corresponding anion.

Ionization Energy

  • The energy required to remove an electron from an atom. First ionization energy is for the first electron, and subsequent ionization energies follow.
  • Trend: Increases across a period (left to right) due to greater nuclear attraction. Decreases down a group (top to bottom) due to greater distance from the nucleus.
  • Relationship to Atomic Radius: Higher ionization energy corresponds to a smaller atomic radius.

Electron Affinity

  • Energy released when an atom accepts an electron to form an anion in the gaseous state.
  • Trend: Increases across a period (left to right) as atoms that are closer to a stable configuration (noble gases) readily accept electrons. Decreases down a group (top to bottom) as outer electrons are further from the nucleus.

Electronegativity

  • An atom's ability to attract electrons and gain a negative charge.
  • Trend: Increases across a period (left to right) as atomic structure approaches a stable configuration. Decreases down a group due to increasing distance and shielding of nuclear attraction.
  • Example: Fluorine is the most electronegative element.

Metallic and Nonmetallic Properties

  • Metallic Properties: Large atomic radius, low ionization energy, low electronegativity, low electron affinity, good conductors. Increase down a group, decrease across a period.
  • Nonmetallic Properties: Small atomic radius, high ionization energy, high electronegativity, high electron affinity, good insulators. Increase across a period, decrease down a group.

  • Down a group: Atomic radius, ionic radius, and metallic properties increase; electron affinity and ionization energy decrease.

  • Across a period: Atomic radius and metallic properties decrease; ionization energy, electron affinity, and electronegativity increase.

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Description

Explore the periodic law and trends in atomic and ionic radii. Understand how these properties change across periods and down groups in the periodic table. This quiz covers definitions, trends, and examples of atomic and ionic radii.

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