General Characteristics of Elements
The general characteristics of elements are determined by their position in the Periodic Table.
These characteristics include physical properties, chemical properties, and periodic trends.
1. **Atomic Radius**:
- The size of an atom, measured as the distance from the nucleus to the outermost electron shell.
- Decreases across a period due to increasing nuclear charge.
- Increases down a group due to the addition of electron shells.
2. **Ionization Enthalpy**:
- The energy required to remove an electron from an atom in its gaseous state.
- Increases across a period due to stronger nuclear attraction.
- Decreases down a group as atomic size increases.
3. **Electronegativity**:
- The tendency of an atom to attract electrons in a chemical bond.
- Increases across a period.
- Decreases down a group.
4. **Electron Affinity**:
- The energy change when an electron is added to a neutral atom.
- Becomes more negative across a period.
- Becomes less negative down a group.
5. **Metallic and Non-Metallic Character**:
- Metallic character decreases across a period and increases down a group.
- Non-metallic character follows the opposite trend.
6. **Reactivity**:
- Metals become more reactive down a group.
- Non-metals become less reactive down a group.
7. **Oxidation States**:
- Elements exhibit variable oxidation states depending on their electronic configurations.
- Transition elements show multiple oxidation states.
The general characteristics of elements are determined by their position in the Periodic Table.
These characteristics include physical properties, chemical properties, and periodic trends.
1. **Atomic Radius**:
- The size of an atom, measured as the distance from the nucleus to the outermost electron shell.
- Decreases across a period due to increasing nuclear charge.
- Increases down a group due to the addition of electron shells.
2. **Ionization Enthalpy**:
- The energy required to remove an electron from an atom in its gaseous state.
- Increases across a period due to stronger nuclear attraction.
- Decreases down a group as atomic size increases.
3. **Electronegativity**:
- The tendency of an atom to attract electrons in a chemical bond.
- Increases across a period.
- Decreases down a group.
4. **Electron Affinity**:
- The energy change when an electron is added to a neutral atom.
- Becomes more negative across a period.
- Becomes less negative down a group.
5. **Metallic and Non-Metallic Character**:
- Metallic character decreases across a period and increases down a group.
- Non-metallic character follows the opposite trend.
6. **Reactivity**:
- Metals become more reactive down a group.
- Non-metals become less reactive down a group.
7. **Oxidation States**:
- Elements exhibit variable oxidation states depending on their electronic configurations.
- Transition elements show multiple oxidation states.
