Class 9 Chemistry Periodic Table And periodicity Of Properties 7. Why and how are elements arranged in 4^{\text {th }} period?
Change the way you learn with Maqsad's classes. Local examples, engaging animations, and instant video solutions keep you on your toes and make learning fun like never before!
7. Why and how are elements arranged in 4^{\text {th }} period?
Explain the contributions of Mendeleev for the arrangement of elements in his Periodic Table.
Justify the statement bigger size atoms have more shielding effect thus low ionization energy.
6. According to Mosely the chemical properties of elements are the periodic function of their :(a) Atomic Size(b). Atomic Mass(c) Atomic Radius(d). Atomic Number
4. Determine the location of families on periodic table.
What do you mean by blocks in a periodic table and why elements were placed in blocks?
4. Justify that periodicity of properties dependent upon number of protons in ar atom?
![3. Identify the electronic configuration of the following elements.\[\mathrm{Na} \mathrm{Ca} \mathrm{F} \mathrm{Si}\]](/_next/image?url=https%3A%2F%2Fmaq-website-bucket-release.s3.ap-southeast-1.amazonaws.com%2Fdoubtsolve%2Fthumbnail-DS_S_IX_3_LQ3.png&w=640&q=75)
3. Identify the electronic configuration of the following elements.\[\mathrm{Na} \mathrm{Ca} \mathrm{F} \mathrm{Si}\]
9. In group electron affinity values decreases from top to bottom because:(a) Atomic size normal(b) Atomic size increases(c) Atomic size decreases(d) Atomic size same
9. Mark the incorrect statement about ionization energy: (a) it is measured in \mathrm{kJmol}^{-1} (b) it is absorption of energy(c) it decreases in a period(d) it decreases in a group
5. The elements of VIIA group are known as:(a) Lanthanides(b). Actinides(c) Halogens(d). Nobel Gases
7. Why and how are elements arranged in 4^{\text {th }} period?
5. What is the difference between Mendeleevs periodic law and modern periodic law?
2. The amount of energy given out when an electron is added to an atom is called:(a) lattice energy(b) ionization energy(b) electronegativity(d) electron affinity
4. Why shielding effect of electrons makes cation formation easy?
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
10. All Transition Elements are :(a) Gases(b) Metals(c) Nonmetals(d) Metalloids
8. The ability to attract shared pair of electron is called:(a) Electron Affinity(b). Electronegativity(c) lonization Energy(d). Shielding Effect
2. The periodic table divided into S P d and f block based on.(a) Atomic Radius(b). Electronic Configuration(c) Ionization Energy(d). Electron Affinity
7. The shielding effect across the period:(a) Increases(b). Decrease(c) Moderate(d). Same
9. Give the trend of ionization energy in a period.
6. Which one of the following halogen has lowest electronegativity?(a) fluorine(b) chlorine(c) bromine(d) iodine
3. How is periodicity of properties dependent upon number of protons in an atom?
Describe the trends of electronegativity in a period and in a group.
1. Discuss in detail the long form of periodic table.
5. 4^{\text {th }} and 5^{\text {th }} period of the long form of Periodic Table are called:(a) short periods(b) normal periods(c) long periods(d) very long periods
4. Which one of the following decreases along the period?(a) lonization Energy(b). Atomic Radius(c) Electronegativity(d). Electron Affinity
2. Determine the demarcation of periodic table in to s p d and f blocks.
8. Why the size of atom does not decrease regularly in a period?
