Periodic Table and Atomic Properties Quiz

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Questions and Answers

How does electronegativity change across a Period (from left to right) and down a Group in the periodic table?

  • Increases across a Period, increases down a Group
  • Increases across a Period, decreases down a Group (correct)
  • Decreases across a Period, decreases down a Group
  • Decreases across a Period, increases down a Group

Alkali metals are found in their free state in nature due to their low reactivity.

False (B)

What type of compounds do alkali metals typically form when they react with non-metals?

electrovalent compounds

The tendency of an atom in a molecule to attract shared pair of electrons towards itself is known as ______.

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

Match the following properties with their trend in a group (from top to bottom):

<p>Electron Affinity = Decreases Electronegativity = Decreases Metallic Character = Increases Non-metallic Character = Decreases</p> Signup and view all the answers

Which of the following is NOT a typical physical property of alkali metals?

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

Halogens are good conductors of heat and electricity.

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

What happens when alkali metals react with water?

<p>They form hydroxides and release hydrogen gas. (D)</p> Signup and view all the answers

Which of the following statements accurately describes the organization of the Modern Periodic Table?

<p>It consists of 7 Periods and 18 Groups, arranged by increasing atomic number. (D)</p> Signup and view all the answers

In the periodic table, elements within the same period have similar valencies.

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

What is the primary factor that determines the arrangement of elements in the modern periodic table?

<p>atomic number</p> Signup and view all the answers

Elements in Group 18 of the periodic table are also known as ______ gases.

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

Match the following properties with their trends in a period (from left to right):

<p>Atomic Size = Decreases Ionization Potential = Increases Electron Affinity = Increases</p> Signup and view all the answers

Which of the following statements is correct regarding the ionization potential (IP) of elements?

<p>IP decreases down a group and increases across a period. (A)</p> Signup and view all the answers

The energy required to remove the second electron from an atom is less than the energy required to remove the first electron.

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

Explain how the number of electron shells changes as one moves down a group in the periodic table.

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

Flashcards

Periodic Table

A tabular arrangement of elements based on properties and atomic structure.

Modern Periodic Law

States that properties of elements are periodic functions of atomic numbers.

Groups and Periods

There are 18 Groups and 7 Periods in the Modern Periodic Table.

Noble Gases

Elements in Zero Group; known as inert gases.

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Atomic Size

Distance from nucleus to outermost shell, decreases in Periods, increases in Groups.

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Ionization Energy

Energy needed to remove an electron; increases in Periods, decreases in Groups.

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Electron Affinity

Energy released when an electron is added to an atom.

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Valency of Elements

Determined by the number of electrons in the outer shell; same in a Group.

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Electronegativity

The tendency of an atom to attract shared electrons in a bond.

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Metallic Character

The ability of an atom to lose electrons, showing metallic properties.

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Non-metallic Character

The ability of an atom to gain electrons to fill its outer shell.

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Alkali Metals

Elements in Group 1 of the periodic table, highly reactive.

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Physical Properties of Alkali Metals

Soft, metallic luster, good conductors, low melting points.

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Halogens

Elements in Group VIIA, known for forming salts.

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Physical Properties of Halogens

Non-metals, poor conductors, increase in size down the group.

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Study Notes

Periodic Table Summary

  • Periodic Table organizes known elements based on their properties, composition, and atomic structure.
  • Elements arranged in periods (rows) and groups (columns).
  • Modern Periodic Law states elements' properties are periodic functions of their atomic number.
  • Seven periods and eighteen groups.
  • Groups I to VII are divided into subgroups A and B.
  • Zero Group elements are noble/inert gases.

Atomic Size

  • Atomic radius is the distance between the nucleus and outermost shell.
  • Measured in angstroms (Å).
  • Decreases across periods from left to right.
  • Increases down groups from top to bottom

Ionization Energy

  • Amount of energy to remove an electron from an isolated gaseous atom.
  • Measured in electron volts (eV).
  • First ionization potential is the energy to remove the first electron.
  • Second ionization potential is the energy to remove the second electron.
  • Increases from left to right across periods.
  • Decreases down groups from top to bottom.

Electron Affinity

  • Energy released when adding an electron to an isolated gaseous neutral atom.
  • Increases left to right across periods.
  • Decreases down groups.

Electronegativity

  • Tendency of an atom in a molecule to attract shared electrons.
  • Increases left to right across periods.
  • Decreases down groups.

Metallic Character

  • Ability of an atom to lose electrons, becoming electropositive.
  • Decreases left to right across periods.
  • Increases down groups.

Non-metallic Character

  • Ability of an atom to gain electrons, becoming electronegative.
  • Increases left to right across periods.
  • Decreases down groups.

Alkali Metals

  • Group I elements in the periodic table.
  • Soft, metallic lustre.
  • Excellent conductors of heat and electricity.
  • Low melting/boiling points.
  • Highly reactive, not found free in nature.
  • React with water to produce hydrogen and hydroxide.

Halogens

  • Group VII elements in the periodic table.
  • Non-metals.
  • Poor conductors of heat/electricity.
  • Increasing atomic size and decreasing electronegativity/electron affinity down the group.
  • Increasing melting/boiling points down the group.
  • Reactive elements, primarily found as compounds.
  • Strong oxidizing agents.

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