Classifying Periodic Elements
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Questions and Answers

Which group of elements typically has characteristics of being malleable and ductile with high electrical and thermal conductivity?

  • Alkaline Earth Metals
  • Noble Gases
  • Nonmetals
  • Metals (correct)

Ionisation enthalpy decreases from left to right across a period.

False (B)

What is the characteristic of noble gases that contributes to their lack of reactivity?

Full outer energy level

Cations are ______ than parent atoms.

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

Match the following properties to their respective trend:

<p>Decreases from left to right across a period = Atomic Radii Increases down a group = Electron Gain Enthalpy Increases from left to right across a period = Electronegativity</p> Signup and view all the answers

Study Notes

Classifications of Periodic Elements

Metals

  • Typically found on the left side and center of the periodic table
  • Characteristics:
    • High electrical and thermal conductivity
    • Malleable and ductile
    • High density
    • React with nonmetals to form ionic compounds
    • Tend to lose electrons to form cations
  • Examples: sodium (Na), iron (Fe), copper (Cu)

Nonmetals

  • Typically found on the right side of the periodic table
  • Characteristics:
    • Low electrical and thermal conductivity
    • Brittle and non-ductile
    • Low density
    • React with metals to form ionic compounds
    • Tend to gain electrons to form anions
  • Examples: carbon (C), nitrogen (N), oxygen (O)

Alkaline Earth Metals

  • Group 2 elements
  • Characteristics:
    • Less reactive than alkali metals
    • Tend to lose two electrons to form a +2 cation
    • High melting and boiling points
    • React with nonmetals to form ionic compounds
  • Examples: magnesium (Mg), calcium (Ca), strontium (Sr)

Noble Gases

  • Group 18 elements
  • Characteristics:
    • Unreactive due to full outer energy level
    • Low melting and boiling points
    • Low reactivity
    • Do not react with other elements to form compounds
  • Examples: helium (He), neon (Ne), argon (Ar)

Ionisation Enthalpy

  • Energy required to remove an electron from an atom
  • Increases from left to right across a period
  • Decreases down a group
  • Important in determining chemical reactivity

Electron Gain Enthalpy

  • Energy released when an electron is gained by an atom
  • Increases from left to right across a period
  • Decreases down a group
  • Important in determining chemical reactivity

Atomic Radii

  • Distance from the nucleus to the outermost electron
  • Decreases from left to right across a period
  • Increases down a group
  • Affects chemical reactivity and bonding

Ionic Radii

  • Distance from the nucleus to the outermost electron in an ion
  • Cations (positive ions) are smaller than parent atoms
  • Anions (negative ions) are larger than parent atoms
  • Affects chemical reactivity and bonding

Electronegativity

  • Ability of an atom to attract electrons in a covalent bond
  • Increases from left to right across a period
  • Decreases down a group
  • Affects chemical reactivity and bonding
  • Important in determining polarity of molecules

Characteristics of Periodic Elements

Metals

  • Found on the left side and center of the periodic table
  • Have high electrical and thermal conductivity
  • Are malleable and ductile
  • Have high density
  • React with nonmetals to form ionic compounds
  • Tend to lose electrons to form cations
  • Examples: sodium (Na), iron (Fe), copper (Cu)

Nonmetals

  • Found on the right side of the periodic table
  • Have low electrical and thermal conductivity
  • Are brittle and non-ductile
  • Have low density
  • React with metals to form ionic compounds
  • Tend to gain electrons to form anions
  • Examples: carbon (C), nitrogen (N), oxygen (O)

Alkaline Earth Metals

  • Are Group 2 elements
  • Are less reactive than alkali metals
  • Tend to lose two electrons to form a +2 cation
  • Have high melting and boiling points
  • React with nonmetals to form ionic compounds
  • Examples: magnesium (Mg), calcium (Ca), strontium (Sr)

Noble Gases

  • Are Group 18 elements
  • Are unreactive due to full outer energy level
  • Have low melting and boiling points
  • Have low reactivity
  • Do not react with other elements to form compounds
  • Examples: helium (He), neon (Ne), argon (Ar)

Ionisation Enthalpy

  • Is the energy required to remove an electron from an atom
  • Increases from left to right across a period
  • Decreases down a group
  • Is important in determining chemical reactivity

Electron Gain Enthalpy

  • Is the energy released when an electron is gained by an atom
  • Increases from left to right across a period
  • Decreases down a group
  • Is important in determining chemical reactivity

Atomic and Ionic Radii

  • Atomic radii decrease from left to right across a period
  • Atomic radii increase down a group
  • Ionic radii: cations are smaller than parent atoms, anions are larger than parent atoms
  • Affect chemical reactivity and bonding

Electronegativity

  • Is the ability of an atom to attract electrons in a covalent bond
  • Increases from left to right across a period
  • Decreases down a group
  • Affects chemical reactivity and bonding
  • Is important in determining polarity of molecules

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Learn about the characteristics and examples of metals and nonmetals in the periodic table.

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