Unit 3: Periodic Table and Periodicity of Properties

What is the Periodic Table and Periodicity of Properties?

The Periodic Table and Periodicity of Properties delve into the organization and classification of elements based on their chemical and physical properties. This unit examines how elements are arranged in the Periodic Table, understanding periodic trends such as atomic radius, ionization energy, and electronegativity. It explores how these trends recur periodically across different periods and groups, providing insight into the behavior and characteristics of elements.

Key Topics in the Periodic Table and Periodicity of Properties:

• Periodic Table Organization: Understanding the arrangement of elements into periods (rows) and groups (columns) based on atomic structure.
• Periodic Trends: Exploring trends such as atomic size, ionization energy, electron affinity, and electronegativity.
• Element Classification: Studying the categorization of elements into metals, nonmetals, metalloids, and noble gases.
• Periodic Law: Learning how the properties of elements repeat periodically when arranged by increasing atomic number.
• Group and Period Properties: Analyzing how elements in the same group or period exhibit similar properties.

Benefits of Studying the Periodic Table and Periodicity of Properties:

• Element Understanding: Provides a systematic approach to understanding the properties and behavior of elements.
• Predictive Power: Enhances the ability to predict the properties of elements and compounds based on their position in the Periodic Table.
• Scientific Insight: Offers valuable knowledge for advanced studies in Chemistry and other scientific disciplines.

This unit is essential for students to comprehend how elements are organized and how their properties change in a predictable manner. Mastering these concepts lays the foundation for understanding chemical reactions and bonding.

1. The atomic radii of the elements in Periodic Table:

a. increase from left to right in a period
b. increase from top to bottom in a group
c. do not change from left to right in a period
d. decrease from top to bottom in a group

2. The amount of energy given out when an electron is added to an atom is
called:

a. Lattice energy
b. Ionization energy
c. Electronegativity
d. Electron Affinity

3. Mendeleev Periodic Table was based upon the:

a. Electronic configuration
b. Atomic mass
c. Atomic number
d. Completion of a subshell

4. Long form of Periodic Table is constructed on the basis of:

a. Mendeleev Postulate
b. Atomic number
c. Atomic mass
d. Mass number

5. 4^th and 5^th period of the long form of Periodic Table are called:

a. Short periods
b. Normal periods
c. Long periods
d. Very long periods

6. Which one of the following halogen has lowest electronegativity?

a. Fluorine
b. Chlorine
c. Bromine
d. Iodine

7. Along the period, which one of the following decreases:

a. Atomic radius
b. Ionization Energy
c. Electron affinity
d. Electronegativity

8. Transition elements are

a. All gases
b. All metals
c. All non-metals
d. All metalloids

9. Mark the incorrect statement about ionization energy:

a. It is measured in kJmol^-1
b. It is absorption of energy
c. It decreases in a period
d. It decreases in a group

10. Point out the incorrect statement about electron affinity:

a. It is measured in kJmol^-1
b. It involves release of energy
c. It decreases in a period
d. it decreases in a group