Reactions of Metals (HSC SSCE Chemistry): Flashcards
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Most reactive group of metals
Most reactive group of metals
Group 1 metals (e.g., potassium, sodium, lithium)
Metal reactivity trend across a period (left to right)
Metal reactivity trend across a period (left to right)
Decreases from left to right
Metal reactivity trend down Groups 1 and 2
Metal reactivity trend down Groups 1 and 2
Increases from top to bottom
First ionisation energy definition
First ionisation energy definition
Energy needed to remove an electron from an atom
Ionisation energy vs metal reactivity relationship
Ionisation energy vs metal reactivity relationship
As ionisation energy decreases, reactivity increases
K ionisation energy vs Au
K ionisation energy vs Au
K: kJ/mol (reactive), Au: kJ/mol (unreactive)
Atomic radius effect on reactivity within a group
Atomic radius effect on reactivity within a group
Larger radius = higher reactivity
Why larger atomic radius increases reactivity
Why larger atomic radius increases reactivity
Weaker electrostatic force; electrons more easily lost
Electronegativity vs reactivity correlation
Electronegativity vs reactivity correlation
Inverse relationship (opposite trends)
Why electronegativity and reactivity inversely related
Why electronegativity and reactivity inversely related
One measures electron loss, other measures electron gain