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Practice problems: Periodic Properties Video Lecture | Crash Course for IIT JAM Chemistry
FAQs on Practice problems: Periodic Properties Video Lecture - Crash Course for IIT JAM Chemistry
| 1. What are periodic properties in chemistry? |  |
Periodic properties in chemistry refer to the trends and patterns in the physical and chemical properties of elements that are observed when they are arranged in order of increasing atomic number. These properties include atomic radius, ionization energy, electron affinity, electronegativity, and metallic character.
| 2. How are atomic radius and ionization energy related? | |
Atomic radius and ionization energy are inversely related. As you move across a period from left to right, the atomic radius decreases and the ionization energy increases. This is because the increasing number of protons in the nucleus pulls the electrons closer, making it harder to remove an electron and increasing the ionization energy.
| 3. What is electronegativity and how does it vary across the periodic table? | |
Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Electronegativity generally increases from left to right across a period and decreases from top to bottom within a group. This trend is due to the increasing nuclear charge and decreasing atomic size as you move across a period or down a group.
| 4. How does electron affinity change across the periodic table? | |
Electron affinity is the energy change that occurs when an atom gains an electron to form a negative ion. Electron affinity generally increases from left to right across a period and decreases from top to bottom within a group. This trend is influenced by factors such as atomic size, effective nuclear charge, and electron shielding.
| 5. What is metallic character and how does it vary across the periodic table? | |
Metallic character refers to the extent to which an element exhibits metallic properties, such as conductivity and malleability. Metallic character generally increases from right to left across a period and from top to bottom within a group. This trend is due to the decreasing ionization energy and increasing atomic radius as you move towards the left and bottom of the periodic table.
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