Definition: A displacement reaction occurs when a more reactive element displaces (pushes out) a less reactive element from its compound.

Example: Iron + Copper Sulfate → Iron Sulfate + Copper demonstrates a successful displacement reaction where iron displaces copper.

Highlight: The reactivity series orders metals from most reactive (potassium) to least reactive (gold), helping predict displacement reactions.

Vocabulary: Reactivity series includes metals in descending order: potassium, sodium, lithium, calcium, magnesium, zinc, iron, lead, copper, silver, and gold.

Highlight: Displacement reactions only occur when the displacing metal is more reactive than the metal being displaced.

Example: Iron + Magnesium Sulfate reaction fails because iron is less reactive than magnesium.

Vocabulary: Successful reactions include Zinc + Silver Nitrate → Zinc Nitrate + Silver, while unsuccessful reactions include Lead + Iron Sulfate.

Definition: The success of a displacement reaction depends on the relative positions of metals in the reactivity series.

Definition: A halogen is a chemical element that forms a salt when it reacts with a metal.

Vocabulary: Group 7 elements include Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At), and Tennessine (Ts).

Highlight: Physical states vary down the group - Chlorine is a green gas, Bromine is a brown liquid, and Iodine is a black solid.

Example: The melting points of halogens increase as you move down Group 7 of the periodic table.