Chemistry Concepts: Ionization Energy, Electronegativity, Reactivity, and Allotropes

These flashcards cover key concepts about ionization energy, electronegativity, reactivity of elements, and allotropes.

Ionization Energy

The amount of energy needed to remove an electron from an atom.

First Ionization Energy

The energy required to remove the first electron from an atom.

Second Ionization Energy

The energy required to remove the second electron from an atom.

Ionization Energy Trend

Ionization energy increases across a period and decreases down a group.

Electronegativity

A measure of an atom's ability to attract a pair of electrons when bonded to another atom.

Fluorine

The most electronegative element.

Francium

The least electronegative element.

Electronegativity Trend

Electronegativity decreases down a group and increases across a period.

Element Reactivity

Determined based on an element's number of valence electrons and atomic radius.

Alkali Metals

Group 1 elements, most reactive metals, with 1 valence electron.

Alkaline Earth Metals

Group 2 elements, second most reactive metals, with 2 valence electrons.

Transition Metals

Elements in groups 3-12 with varying oxidation states and colored ions.

Halogens

Group 17, most reactive nonmetals with 7 valence electrons.

Noble Gases

Group 18, inert gases that do not form ions and have 8 valence electrons.

Allotropes

Different structural arrangements of the same element leading to different properties.

Carbon Allotropes

Includes diamond and graphite.

Oxygen Allotropes

Includes O2 (oxygen) and O3 (ozone).