GRE Exam > GRE Videos > Chemistry for GRE Paper II > Periodicity in Properties
Periodicity in Properties Video Lecture | Chemistry for GRE Paper II
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FAQs on Periodicity in Properties Video Lecture - Chemistry for GRE Paper II
| 1. What is periodicity in properties? |  |
Periodicity in properties refers to the recurring pattern or trend observed in the properties of elements across the periodic table. It means that certain properties of elements, such as atomic radius, ionization energy, and electronegativity, follow a consistent pattern as you move from left to right or from top to bottom in the periodic table.
| 2. Why is periodicity important in chemistry? | |
Periodicity is important in chemistry because it helps us understand and predict the behavior of elements and compounds. By recognizing the patterns in properties, we can make predictions about an element's reactivity, its ability to gain or lose electrons, and its chemical bonding tendencies. This knowledge is crucial for various applications in fields like materials science, pharmaceuticals, and environmental studies.
| 3. How is atomic radius related to periodicity? | |
Atomic radius refers to the size of an atom, and it follows a periodic trend. As you move from left to right across a period in the periodic table, the atomic radius generally decreases. This is because the increasing number of protons in the nucleus exerts a stronger pull on the electrons, causing the electron cloud to be pulled closer to the nucleus. On the other hand, as you move down a group, the atomic radius tends to increase due to the addition of new energy levels.
| 4. Explain the periodic trend in ionization energy. | |
Ionization energy is the energy required to remove an electron from an atom or ion. The ionization energy generally increases across a period from left to right in the periodic table. This is because the effective nuclear charge, which is the positive charge experienced by the valence electrons, increases. As a result, the valence electrons are held more tightly, making it more difficult to remove them. Conversely, ionization energy tends to decrease down a group due to the increased distance between the valence electrons and the nucleus.
| 5. How does periodicity affect the electronegativity of elements? | |
Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. It follows a periodic trend similar to atomic radius. Electronegativity generally increases across a period from left to right in the periodic table because the effective nuclear charge increases, making the atom more attractive to electrons. Down a group, electronegativity tends to decrease due to the increasing atomic radius and shielding effect, which reduce the attraction for electrons.
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Nov 22, 2024 Last updated |
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