Chemistry: Periodic Table and Properties of Metals and Nonmetals

Periodic Table

• A tabular arrangement of elements, organized by their atomic number (number of protons in the nucleus)
• Elements with similar properties and electron configurations are placed in the same group (vertical column)
• Elements with the same number of electron shells are placed in the same period (horizontal row)

Metals and Nonmetals

• Metals:
  • Typically shiny, malleable, and good conductors of electricity
  • Tend to lose electrons to form cations (positive ions)
  • Examples: sodium, iron, copper
• Nonmetals:
  • Typically dull, brittle, and poor conductors of electricity
  • Tend to gain electrons to form anions (negative ions)
  • Examples: carbon, nitrogen, oxygen

Halogens

• A group of highly reactive nonmetals
• Found in Group 17 of the periodic table
• Examples: fluorine, chlorine, bromine, iodine, astatine
• Tend to gain electrons to form anions (negative ions)

Alkali and Alkaline Earth Metals

• Alkali Metals:
  • Found in Group 1 of the periodic table
  • Highly reactive and tend to lose one electron to form a cation
  • Examples: lithium, sodium, potassium, rubidium, cesium
• Alkaline Earth Metals:
  • Found in Group 2 of the periodic table
  • Less reactive than alkali metals and tend to lose two electrons to form a cation
  • Examples: magnesium, calcium, strontium, barium, radium

Noble Gases

• A group of unreactive gases
• Found in Group 18 of the periodic table
• Examples: helium, neon, argon, krypton, xenon, radon
• Tend to have full outer energy levels, making them unreactive

Chemical Reactivity

• The ability of an element to react with other elements to form compounds
• Influenced by the element's position in the periodic table and its electron configuration
• Increases from left to right across a period and decreases from top to bottom within a group

Block of Elements

• A horizontal row of elements in the periodic table
• Elements in the same block have similar electron configurations and chemical properties
• Blocks are named based on the subshell being filled:
  • s-block (first two columns)
  • p-block (next six columns)
  • d-block (next ten columns)
  • f-block (inner transition metals)

Periodic Table

• Organized by atomic number (number of protons in the nucleus)
• Elements with similar properties and electron configurations are placed in the same group (vertical column)
• Elements with the same number of electron shells are placed in the same period (horizontal row)

Metals and Nonmetals

• Metals: shiny, malleable, good conductors of electricity, tend to lose electrons to form cations
• Examples of metals: sodium, iron, copper
• Nonmetals: dull, brittle, poor conductors of electricity, tend to gain electrons to form anions
• Examples of nonmetals: carbon, nitrogen, oxygen

Halogens

• Highly reactive nonmetals
• Found in Group 17 of the periodic table
• Examples: fluorine, chlorine, bromine, iodine, astatine
• Tend to gain electrons to form anions (negative ions)

Alkali and Alkaline Earth Metals

• Alkali metals: found in Group 1, highly reactive, tend to lose one electron to form a cation
• Examples of alkali metals: lithium, sodium, potassium, rubidium, cesium
• Alkaline earth metals: found in Group 2, less reactive, tend to lose two electrons to form a cation
• Examples of alkaline earth metals: magnesium, calcium, strontium, barium, radium

Noble Gases

• Unreactive gases
• Found in Group 18 of the periodic table
• Examples: helium, neon, argon, krypton, xenon, radon
• Tend to have full outer energy levels, making them unreactive

Chemical Reactivity

• Influenced by the element's position in the periodic table and its electron configuration
• Increases from left to right across a period and decreases from top to bottom within a group

Block of Elements

• Named based on the subshell being filled
• s-block: first two columns
• p-block: next six columns
• d-block: next ten columns
• f-block: inner transition metals