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Ions

• Metals and Nonmetals

  • Metals lose electrons, allowing nonmetals to gain electrons.

  • Nonmetals, upon gaining electrons, become negatively charged.

Ionic Compounds

• Formed when a metal and a non-metal combine.

• Metal Atoms

  • Lose electrons to form positive ions.

  • When all electrons are lost, the remaining electrons in the inner orbit become full, stabilizing the metal.

• Nonmetals

  • Gain one or more electrons to fill their outer shell and achieve stability.

• Most ionic compounds are soluble in water.

Naming Ionic Compounds

• Steps to Name Ionic Compounds:

  1. Write the name of the metal.

  2. Write the name of the non-metal, changing the end to ‘–ide.’

Writing Ionic Compound Formulas

• Identify the number of bonds atoms can make (refer to the periodic table).

• Number the groups on the periodic table from 1-3 (excluding transition metals) to determine charge.

• Cross over the charges to the opposite atom and remove the sign.

Multivalent Compounds

• Involves transition metals.

• Larger atoms have a more complex atomic structure, leading to different numbers of valence electrons in different situations.

Roman Numerals in Multivalent Compounds

• Distinguish between different ion forms using Roman numerals.

• To determine which Roman numeral to use:

  • Reverse the Crisscross method.

  • Use the subscript as the charge for the other symbol.

  • Place the charge for the metal in brackets.

Fun Facts

• Silver (Ag) always has a charge of +1.

• Zinc (Zn) always has a charge of +2.

• Be cautious when determining the Roman numeral given a formula (e.g., CuS).

  • Verify the charge of the anion is correct (for CuS, it appears as -1 on the formula but is -2 on the periodic table).

  • To find the appropriate charge, reference the periodic table and multiply the other charge. This leads to identifying it as copper(II) sulfide.