Periodic Trends In Properties Of Elements
Chapter Name : Classification Of Elements And Periodicity In Properties |
Sub Topic Code : 102_11_03_07_03 |
Topic Name : Periodic Trends In Properties Of Elements |
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Sub Topic Name : Ionization Enthalpy |
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Introduction
• The energy required to remove an electron from an isolated gaseous atom (X) in its ground state is ionization energy. (measured in kilojoules, kJ) • High ionization energy means the atom has a strong hold on its valence electrons. Low ionization energy means that the atom loses its valence electrons easily. • Ionization enthalpies are always positive. • Ionizations energies are inversely proportional to atomic radius.
Pre-Requisites:
Element, periodic properties, classification, valence shell, Metals, non-metals
Activity:
How magnets attract pieces of metals?
Real Life Question:
How easily can you remove the first outer piece of metal sticking from a magnet?
Key Words / FlashCards
| Key Words | Definitions (pref. in our own words) |
|---|---|
| Ionization enthalpy | The energy required to remove an electron from an isolated gaseous atom (X) in its ground state is ionization energy. |
Learning aids / Gadgets
| Gadgets | How it can be used |
|---|---|
| Magnet | A piece of metal kept far away from a magnet is easier to remove than a piece of metal kept close to it. |
Real life uses :
Ionization enthalpy helps to find out whether an atom would have a positive charge or a negative charge.
Places to visit :
school
Practical examples around us
| Examples | Explainations |
|---|---|
| Magnet | It is easier to remove metal kept a distance away from a magnet than the one kept close to it. |
What you learn in Theory:
• The energy required to remove an electron from an isolated gaseous atom (X) in its ground state is ionization energy. (measured in kilojoules, kJ) • High ionization energy means the atom has a strong hold on its valence electrons. Low ionization energy means that the atom loses its valence electrons easily. • Ionization enthalpies are always positive. • Ionizations energies are inversely proportional to atomic radius.
What you learn in Practice:
Larger ions have smaller ionization enthalpy and vice versa.