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Important Graphs of Periodic Properties | Chemistry Class 11 - NEET



Alkali Metals

Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET
Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

 

Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET


Important Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEET


CARBON FAMILY


Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEET


CHALCOGENS


Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

 

 Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET
Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

 
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Important Graphs of Periodic Properties | Chemistry Class 11 - NEETImportant Graphs of Periodic Properties | Chemistry Class 11 - NEET

 

POINTS TO REMEMBER

1. The basis of Mendeleev's periodic table was his periodic law. According to it the physical and chemical properties of the elements are a periodic function of their atomic masses.

2. According to Moseley, that a plot of v (where v is frequency of X-Rays emitted) against atomic number (Z) gave a straight line and not the plot of ~ vs atomic mass. Therefore, he concluded that atomic number (Z) instead of atomic mass was a better fundamental property of an element and atomic number instead of atomic mass should be basis of the classification of the elements.

3. Long form of periodic table contains seven periods (horizontal rows) and eighteen groups (vertical columns).

4. In the modern periodic table, the period indicates the value of principle quantum number.

5. The number of elements in each period is twice the number of atomic orbitals available in the energy level that is being filled. 6. Group consists of a series of elements having similar valence shell electronic configuration.

7. In modern periodic table each block (s, - p, - d - and f -) contains a number of columns equal to the numbers of electrons that can occupy that sub-shell.

8. The 4f - (i.e., actinides) and 5f - (i.e., lanthanides) inner transition series of element are placed separately in the periodic table to maintain its structure and to preserve the principle of classification.

9. Metals comprise more than 78% of all known elements and appear on the left side of the periodic table. Silicon, germanium, arsenic, antimony, selenium and tellurium all are semi - metals or metalloids.

10. The combined effect of attractive force due to nucleus and repulsive force due to intervening electrons, acting on the valence electrons is that the valence - electron experiences less attraction from the nucleus. This is called shielding or screening effect.

11. Covalent radius < metallic or crystal radius < Van der Waal's radius.

12. Species having same number of electrons but different in the magnitude of their nuclear charges are called as isoelectronic species and their size is inversely proportional to their effective nuclear charge.

13. The smaller the ionisation energy, the easier it is for the neutral atom to change in to a positive ions in gaseous state . IE1 < IE2 < IE.........•

14. The greatest increase in ionization enthalpy is experienced on removal of electrons from core noble gas configuration. End of valence electrons is marked by a big jump in ionization enthalpy. 15. Electron gain enthalpy provides a measure of the ease with which an atom adds an electron to form anion:


Important Graphs of Periodic Properties | Chemistry Class 11 - NEET


16. The negative value of electron gain enthalpy of Cℓ > F (similarly S > 0) because there is weak electron electron repulsion in the bigger 3p subshell of Cℓ as compared to compact 2p - subshell of F.

17. Noble gases have larger positive electron gain enthalpies because the electron has to enter the next higher energy level.

18. Addition of 2nd electron to an anion is opposed due to electrostatic repulsion and thus requires the absorption of energy e.g in case of the formation of S2–, O2– etc.

19. The relative reactivity of metals increases with the decrease in their ionisation energies. Similarly the relative reactivity of non-metals increases with increases in the negative value of electron gain enthalpy.

20. According to Pauling, the electronegativity difference between two atoms is equal to 0.208 √Δ  where L is the extra bond energies in K cal mol-1. The acidic character of oxides increases when electronegativity difference decreases between element and oxygen (E - O).


  

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FAQs on Important Graphs of Periodic Properties - Chemistry Class 11 - NEET

1. What are the trends in periodic properties for alkali metals?
Ans. The alkali metals exhibit several trends in their periodic properties. These include: - Atomic radius: The atomic radius of alkali metals increases as you move down the group. This is because there is an increase in the number of electron shells, resulting in a larger atomic size. - Ionization energy: The ionization energy, which is the energy required to remove an electron from an atom, decreases as you move down the group. This is because the outermost electron is further away from the nucleus and experiences less attraction, making it easier to remove. - Reactivity: Alkali metals are highly reactive, and their reactivity increases as you move down the group. This is due to the decreasing ionization energy, which makes it easier for alkali metals to lose their outermost electron and form positive ions.
2. How do the periodic properties of the carbon family vary?
Ans. The carbon family, which includes carbon, silicon, germanium, tin, and lead, exhibits some common trends in their periodic properties. These include: - Atomic radius: The atomic radius generally increases as you move down the group. This is because the number of electron shells increases, leading to a larger atomic size. - Ionization energy: The ionization energy generally decreases as you move down the group. This is because the outermost electron is further away from the nucleus and experiences less attraction, making it easier to remove. - Electronegativity: Electronegativity generally decreases as you move down the group. This is because the larger atomic size and increased shielding from inner electron shells reduce the attraction for electrons.
3. What are the properties of chalcogens in terms of periodic trends?
Ans. The chalcogens, which include oxygen, sulfur, selenium, tellurium, and polonium, exhibit some common trends in their periodic properties. These include: - Atomic radius: The atomic radius generally increases as you move down the group. This is because the number of electron shells increases, leading to a larger atomic size. - Ionization energy: The ionization energy generally decreases as you move down the group. This is because the outermost electron is further away from the nucleus and experiences less attraction, making it easier to remove. - Electronegativity: Electronegativity generally decreases as you move down the group. This is because the larger atomic size and increased shielding from inner electron shells reduce the attraction for electrons.
4. What are some important graphs of periodic properties?
Ans. Some important graphs of periodic properties include: - Atomic radius trend: A graph showing the increase in atomic radius as you move down a group in the periodic table. - Ionization energy trend: A graph showing the decrease in ionization energy as you move down a group in the periodic table. - Electronegativity trend: A graph showing the decrease in electronegativity as you move down a group in the periodic table. - Melting point trend: A graph showing the variation in melting points of elements across periods or groups in the periodic table.
5. What are some frequently asked questions about periodic properties in exams?
Ans. Some frequently asked questions about periodic properties in exams include: - Explain the trend in atomic radius as you move down a group in the periodic table. - Why does ionization energy decrease as you move down a group in the periodic table? - Compare the electronegativity of alkali metals and chalcogens. - Discuss the reactivity trend of alkali metals. - How does the melting point of elements vary across periods in the periodic table?
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