Grade 10 Chemistry - Binary Compounds

Study Notes

Binary Ionic Compounds

Composed of two elements that form a compound with unique properties.
Ionic compounds require knowledge of the ionic charges to write correct chemical formulas.

Writing Chemical Formulas

Determine the charge of both ions involved in the compound.
Use the crisscross method to transpose the charges as subscripts for the opposite ion.
Simplify the subscripts to the lowest whole number ratio.

Atoms and Ions

Atoms are electrically neutral, having equal numbers of protons and electrons.
Ions are formed when atoms gain or lose electrons, resulting in a positive or negative charge.
Anions are formed by nonmetals gaining electrons (e.g., F⁻ = fluoride, O²⁻ = oxide).
Cations are formed by metals losing electrons, resulting in more protons than electrons.

Chemical Formulas

Chemical formulas indicate the types and quantities of atoms in a compound.
Subscripts in chemical formulas denote the number of atoms present.

Ionic Charges and Electron Transfer

Atoms gain electrons from other atoms or lose them to become stable.
Groups of elements have predictable oxidation states based on their electron configuration.

Predicting Ionic Charges

Group 1A elements: lose 1 electron, forming 1+ ions.
Group 2A elements: lose 2 electrons, resulting in 2+ ions.
Group 3A elements: lose 3 electrons, creating 3+ ions.
Group 4A elements rarely form ions.
Group 5A elements typically gain 3 electrons to form 3- ions.

Transition Metals and Ionic States

Some transition metals, such as silver (Ag¹+), zinc (Zn²+), and cadmium (Cd²+), have fixed oxidation states.
Certain transition metals can exhibit multiple oxidation states, requiring Roman numerals for clarity.

Description

Test your knowledge on binary ionic compounds in this Grade 10 Chemistry quiz. Focuses on writing and naming correct chemical formulas for compounds made of two elements. Prepare for your first quarter examination with practice questions!