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Class 11 Chemistry Chapter 3 Notes – Classification of Elements and Periodicity in Properties Notes PDF Download

Class 11 Chemistry Chapter 3 Notes – Classification of Elements and Periodicity in Properties Notes PDF Download

Class 11 Chemistry Chapter 3 Notes:- Chemistry chapter 3 i.e. classification of elements and periodicity in properties is one of the most important chapters of the NCERT book. As 11th class does not involve a board exam so most people ignore this time consuming but important chapter. To make your learning easier, we have made the classification of elements and periodicity in properties class 11 notes for you guys. These practical class 11 chemistry chapter 3 notes to come up in a very easy to understand language and helpful examples.

Chemistry in science is proposed with the “Focal Science” as it has connectivity and relation with geography, science, inherent science, and genuine science. Our class 11 chemistry chapter 3 notes are very helpful for students who are preparing for the Class 11 Chemistry exams. By reading these notes, they can learn the basic concepts which help them to obtain high marks in the final examination. Students must read these class 11 chemistry chapter 3 notes for their efficient exam preparation.

Class 11 Chemistry Chapter 3 Notes

A few ideas have been asked more than once throughout the long term –, for example, Ionic Bond, Van-der Waals power, Structure of Atom, and redox responses. Thus, students must focus and concentrate on these subjects completely with the assistance of CBSE Notes Class 11 Chemistry Notes. The CBSE Notes for Class 11 Chemistry are intended to assist students with getting a handle on ideas easily.

Gathering of Elements and Periodicity in Properties

In this segment, we will look at the improvement of a periodic table and the discontinuous law. The game-plan of parts in the state-of-the-art incidental table is composed of eight vertical portions (get-togethers) and seven even lines (periods) considering their atomic number.

Considering the electronic plan, parts can be assembled into four sorts in the irregular table, viz s-block, p-block, f-square, and d-block parts. More than 70-80% of the acknowledged parts are metals. Parts arranged at the most noteworthy mark of the irregular table are nonmetals and are under 20. In a social event, as the atomic number extends, the metallic individual augmentations. In a period, there is a decrease in the metallic individual from left to right. Also, the substance, similar to its real properties, changes with its atomic number. Parts of a comparative social occasion show equivalent compound properties because of the tantamount valence shell electronic plan.

S-Block Elements

The parts of Group 1 and Group 2 of the high-level incidental table are called S-block parts. 

S-block incorporates 14 parts be explicit hydrogen (H), lithium (Li), helium (He), sodium (Na), beryllium (Be), potassium (K), magnesium (Mg), rubidium (Rb), calcium (Ca), caesium (Cs), strontium (Sr), francium (Fr), barium (Ba), and radium (Ra).

What is S-Block Element?

The s-block parts having quite recently a solitary electron in their s-orbital are called pack one or salt metals while the s block parts having two electrons filling their s-orbital are called bundle two or dissolvable earth metals.

The electrons present in a particle include distinctive sub-orbitals of available energy levels in the solicitation for growing energy. The last electron of a molecule may end up in both of the s, p, d, and f subshells. Moreover, the parts of the particle winning no matter what their last valence electron present in the s-suborbital are known as the s block parts.

Electronic Configuration of S-Block Elements

The electronic game plan of S-block parts is explained under,

The salt parts in the s-block include a lone valence electron in their outermost shell. This farthest electron is roughly held which makes these metals especially electropositive. Due to which they are not available in the free state in nature.

The generally electronic plans of s block parts – Group 1 are shown under:       

ElementSymbolElectronic configuration

The electronic configurations of s block elements -Group 2 are given below:

ElementSymbolElectronic configuration

Properties of S-Block Elements

 Both antacid and basic earth components show a standard degree in their properties among their separate gathering components. Be that as it may, the fundamental person from both S block parts, specifically, Lithium and Beryllium contrast much from the rest of their people but, they take after extra with the inclining part present in the accompanying area.

The irregularity of these S-block parts is relied upon to:

  • Low atomic and ionic size
  • Greater charge thickness (charge/volume of the molecule)
  • Greater polarization
  • Absence of d-orbitals.

More critical polarization of s block parts makes the foremost part more covalent and isolates them from the rest which is ionic.

The closeness in size and charge thickness makes them appear as though the part cockeyed is situated in the accompanying social occasion (corner to corner relationship).

It is seen that the physical and compound properties of these ‘s’ block parts change in a particular example as the atomic number of the parts increases.

Engineered Properties of S-Block Elements

Atomic and Ionic Radii

Exactly when the s block parts of the state-of-the-art infrequent table are seen it is seen that the size of the stomach settling agent metals is greater diverged from various parts in a particular period. As the atomic number extends the hard and fast number of electrons increases close by the extension of shells.

On dropping down the social event the atomic number augmentations. Thus, the atomic and ionic range of the acid neutralizer metals increases.

Real Properties of S-Block parts

  • In the S block parts, the thickness of the salt metals increases down the get-together. Exception case: the thickness of potassium isn’t, by and large, the thickness of sodium.
  • The salt metals have a low relaxing and edge of bubbling over given the feeble metallic holding.
  • Alkali metals and their specific salts can give tone to the oxidizing fire due to the hotness made from the fire which strengthens the valence electrons beginning with one energy level then onto the following energy level. This helps in distinguishing proof of solvent base metals during the fire test.

What is the P-Block Element?

P block elements are the last electron entering any of the three p-orbitals. Since a p-subshell has three savage p-orbitals all of which can oblige two electrons, in like manner in all there are six social events of p-block elements.

P block elements are shining and by and large a good transmitter of force and hotness as they will in general lose an electron. You will find some staggering properties of parts in a P-block element like gallium. A metal can break up in the palm of your hand. Silicon is also one of the most critical metalloids of the p-block bundle as it is a huge piece of glass.

P block elements involve 6 families such as Boron family, Fluorine family, Neon family, Oxygen family, Nitrogen family, and Carbon family.

Traits of P-Block Elements

  • The general electronic plan of p-block parts is ns2np1-6 (except He). However, the internal focus electronic game plan may differentiate. Significantly, there are changes in both the physical and compound properties of the elements.
  • The oxidation state of elements in p – block is most noteworthy when it is identical to an outright number of valence electrons i.e., the measure of S and P electrons. One of the most entrancing real factors about the p-block elements is that it contains both nonmetals and metalloids.

The foremost person from the p block elements contrasts from various parts in two huge respects:

  • First is the size and every property which depends on the size.
  • The second difference applies just to the p block element, which rises out of the effects of d-orbitals in the valence shell of heavier elements.

What are F Block Elements?

Elements whose f orbital getting finished off by electrons are called f block elements. These elements have electrons, (1 to 14) in the f orbital, (0 to 1) in the d orbital of the penultimate energy level, and the uttermost orbital.

The request of F Block Elements

The elements having a spot with the f block are furthermore isolated into:

  • The first series of elements are called lanthanides and consolidate elements with atomic numbers beginning from 57 and completing at 71. Here elements are non-radioactive (only radioactive is promethium).
  • The second series of elements are called actinides and join elements with atomic numbers beginning from 89 and completing at 103. Since the f orbital lies much inside than the d orbital, compared to the change metals naming, f block elements are called internal advancement parts.

Properties of F block Elements

  • Have electrons added to the ‘f’ sub-orbitals of (n-2) level
  • Are set between (n-1) d and ns block elements.
  • Properties resemble d-block elements.

Properties of Lanthanides

  • Lanthanides are fragile metals with a shining white tone.
  • Their tone dulls and their quality reduces rapidly when introduced to the air.
  • They have mellowing centers going from 1000K to 1200K (Except Samarium, 1623K).
  • Lanthanides are OK channels of hotness and force.
  • They are non-radioactive except for Promethium.
  • A decrease in atomic and ionic radii from lanthanum to lutetium is taken note of. This is known as the lanthanoid pressure.

Properties of Actinides

  • The Actinide elements have every one of the reserves of being sparkling.
  • These parts of elements have a radioactive nature.
  • These metals are significantly responsive and their reactivity increases when they are finely divided.
  • A decrease in atomic and ionic radii from Actinium to Lawrencium is taken note of. This is known as actinoid tightening.
  • They generally show an oxidation state of +3. Nevertheless, elements having a spot with the essential piece of the series are known to show higher oxidation states periodically.

Qualification among Lanthanides and Actinides

  • Lanthanoids are related with the filling of 4f-orbitals however actinoids are related with the filling of 5f-orbitals. The restricting energy of 4f electrons is almost not that of 5f-electrons. The protecting effect of 5f-electrons is less fruitful when diverged from that of 4f-electrons.
  • The paramagnetic properties of lanthanoids can be conveniently explained at this point this explanation is problematic of actinoids.
  • Lanthanides are non-radioactive besides promethium however all actinide series parts are radioactive.
  • Lanthanides will not in general shape oxo-cations, yet a couple of oxo-cations of actinide series exist. The combinations molded by lanthanides are less key of course the combinations of actinides are significantly fundamental.

Comparable qualities among Lanthanides and Actinides

The elements of the lanthanide and actinide series are depicted by filling of (n-2) f subshell. They have similar fringe electronic courses of action hence have practically identical properties. Following are the basic comparable qualities:

  • Both have an observable oxidation state of +3.
  • They are locked in with the filling of (n-2) f orbitals.
  • They are significantly electropositive and very responsive.
  • With an augmentation in atomic number, there is a decrease in atomic and ionic size.
  • Both show alluring properties.

Infrequent Trends in Properties of Elements

  • Atomic sizes – With the augmentation in atomic number the atomic radii in the social event will augment. On the other hand, the atomic radii decay from left to decidedly in a period.
  • Ionization Enthalpies – Decreases down in groups yet increases across a period.
  • Electron Gain Enthalpies – Tends to end up being more negative across a period.
  • Electronegativity – Electronegativity reduces down a get-together anyway increases across a period.
  • Chemical Reactivity – Chemical reactivity is generally insignificant in the center and is generally important at the two furthest reaches of a period.

Also Read:- CBSE Class 11 Chemistry Syllabus

CBSE Class 11 Chemistry Chapter 3 Notes PDF Download

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 To Conclude

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