Classification of Elements and Periodicity in Properties NEET Questions: Dowload pdf
Classification of Elements and Periodicity in Properties is a core subject matter in NEET, covering how factors are organized based totally on atomic shape and ordinary houses. Key areas encompass the periodic desk’s layout, tendencies in atomic radius, ionization power, electronegativity, and electron affinity. Understanding these traits helps predict element reactivity and bonding behavior, which is essential for fixing chemistry troubles in NEET. This topic bureaucracy the basis for gaining knowledge of chemical conduct, reactivity, and periodic relationships amongst elements.
- Introduction to Classification of Elements and Periodicity in Properties
- Download: Classification of Elements and Periodicity in Properties
- The Modern Periodic Table: Classification of Elements and Periodicity in Properties
- Periodic Trends: Classification of Elements and Periodicity in Properties
- Periodic Properties: Classification of Elements and Periodicity in Properties
- Classification of Elements into Blocks
- Group and Period Characteristics
- Application of Periodic Trends in Chemical Reactions
- Important NEET Questions on Classification of Elements and Periodicity in Properties
- FAQs about Classification of Elements and Periodicity in Properties
Introduction to Classification of Elements and Periodicity in Properties
Classification of Elements and Periodicity in Properties is a essential topic for NEET aspirants, protecting the structure and enterprise of elements in the periodic table. This subject matter explores the type of elements based on atomic quantity, electron configurations, and routine chemical residences. Understanding periodic developments—such as atomic radius, ionization electricity, electronegativity, and electron affinity—is important for predicting an element’s reactivity and bonding behavior. NEET questions about this subject matter regularly take a look at conceptual readability and application, difficult students to investigate these trends and their implications on chemical reactions. Mastery of this difficulty helps build a solid foundation in chemistry, making ready college students for advanced hassle-fixing in aggressive tests like NEET.
History and Development of the Periodic Table
The periodic table, as we are aware of it these days, is the culmination of centuries of clinical inquiry and discovery. Here are a few key milestones in its development:
- Dobereiner’s Triads: Johann Dobereiner observed that sure factors can be grouped into triads, wherein the atomic weight of the middle detail was about the common of the alternative two.
- Newlands’ Law of Octaves: John Newlands proposed that once factors had been organized in order of growing atomic weight, every 8th detail had comparable homes, like the octaves in music.
- Mendeleev’s Periodic Law: Dmitri Mendeleev, taken into consideration the daddy of the periodic desk, organized factors in order of increasing atomic weight, recognizing that houses repeated periodically. He even left gaps for undiscovered factors, which have been later filled.
- Modern Periodic Law: Henry Moseley determined that the properties of factors are a periodic function in their atomic wide variety, which is the wide variety of protons within the nucleus. This led to the modern-day periodic table, in which factors are arranged so as of increasing atomic range.
Download: Classification of Elements and Periodicity in Properties
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| Classification of Elements and Periodicity in Properties NEET Questions with Answer | Click |
The Modern Periodic Table: Classification of Elements and Periodicity in Properties
Classification of Elements into Groups and Periods |
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| Groups | Periods | Properties |
|---|---|---|
| 18 Groups (Vertical columns) | 7 Periods (Horizontal rows) | Elements in the same group have similar chemical properties. As we move across a period, properties change gradually. |
| Group 1: Alkali Metals | Period 1: 2 Elements (H, He) | Alkali metals are highly reactive and form basic hydroxides with water. |
| Group 17: Halogens | Period 2-7: 7 Elements each (e.g., Li to Fr, Na to Cs) | Halogens are reactive non-metals, forming salts when combined with metals. |
| Group 18: Noble Gases | Noble gases are inert, non-reactive gases under standard conditions. | |
Types of Elements |
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| Metals | Non-Metals | Metalloids |
| Found on the left side of the periodic table. Good conductors of heat and electricity. Examples: Iron (Fe), Copper (Cu). | Found on the right side. Poor conductors of heat and electricity. Examples: Oxygen (O), Carbon (C). | Elements with properties between metals and non-metals. Examples: Silicon (Si), Boron (B). |
| Generally have high melting and boiling points. | Low melting and boiling points. | Have semi-conductive properties and are used in electronics. |
| Form cations (positive ions) in reactions. | Form anions (negative ions) in reactions. | Can form both cations and anions depending on the reaction. |
Periodic Trends: Classification of Elements and Periodicity in Properties
Explanation of Trends
Atomic Radius:
- Across a Period: As we move throughout a length, the range of protons will increase, leading to a more potent nuclear pull at the electrons. This reasons the atomic size to lower.
- Down a Group: As we pass down a set, new electron shells are brought, growing the atomic length.
Ionization Energy:
- Across a Period: The increasing nuclear rate makes it more difficult to put off an electron, so ionization energy increases.
- Down a Group: The growing distance between the nucleus and the outermost electrons makes it less complicated to dispose of an electron, so ionization power decreases.
Electron Affinity:
- General Trend: Generally, electron affinity increases across a length as atoms become more stable via gaining electrons.
- Exceptions: Some elements, like noble gases, have complete valence shells and feature little tendency to advantage electrons, main to bad electron affinities.
Electronegativity:
- Across a Period: Increasing nuclear fee draws electrons greater strongly, so electronegativity increases.
- Down a Group: Increasing atomic length reduces the enchantment between the nucleus and valence electrons, so electronegativity decreases.
Metallic and Non-metallic Character:
- Metallic Character: Metals tend to lose electrons, while non-metals tend to gain electrons. As we pass across a duration, metal character decreases, and non-metallic man or woman increases. Conversely, down a set, steel individual will increase, and non-steel character decreases.
| Property | Trend Across a Period | Trend Down a Group |
|---|---|---|
| Atomic Radius | Decreases | Increases |
| Ionization Energy | Increases | Decreases |
| Electron Affinity | Generally increases (with exceptions) | Generally decreases |
| Electronegativity | Increases | Decreases |
| Metallic Character | Decreases | Increases |
| Non-metallic Character | Increases | Decreases |
Periodic Properties: Classification of Elements and Periodicity in Properties
| Property | Definition | Trend Across a Period | Trend Down a Group |
|---|---|---|---|
| Effective Nuclear Charge (Zeff) | The net positive charge experienced by an electron in an atom. It’s calculated as: Zeff = Z – S, where Z is the atomic number and S is the screening constant (number of core electrons). | Increases | Increases slightly |
| Shielding Effect | The reduction in the attractive force between the nucleus and valence electrons due to the presence of inner electrons. | Remains relatively constant | Increases |
Trends in the Periodic Table Influenced by Zeff and Shielding Effect
| Property | Trend | Explanation |
|---|---|---|
| Atomic Radius | Decreases across a period, increases down a group | Zeff increases across a period, pulling electrons closer to the nucleus, while shielding effect increases down a group, pushing valence electrons further from the nucleus. |
| Ionization Energy | Increases across a period, decreases down a group | Higher Zeff makes it harder to remove electrons across a period, while lower Zeff and increased shielding effect make it easier to remove electrons down a group. |
| Electron Affinity | Generally increases across a period, decreases down a group (with exceptions) | Higher Zeff makes it easier to add electrons across a period, while lower Zeff and increased shielding effect make it less favorable to add electrons down a group. |
| Electronegativity | Increases across a period, decreases down a group | Higher Zeff makes atoms more attractive to electrons across a period, while lower Zeff and increased shielding effect make atoms less attractive to electrons down a group. |
Classification of Elements into Blocks
Classification of Elements into Blocks
The current periodic table is divided into 4 blocks based on the orbital into which the last electron enters:
- S-Block Elements:
- Last electron enters: s-orbital
- Groups: 1 and 2
- Characteristics:
- Highly reactive metals
- Low ionization energies
- Form ionic compounds
- Examples: Sodium (Na), Potassium (K), Magnesium (Mg), Calcium (Ca)
- P-Block Elements:
- Last electron enters: p-orbital
- Groups: 13 to 18
- Characteristics:
- Diverse properties, such as metals, non-metals, and metalloids
- Form covalent compounds
- Examples: Carbon (C), Nitrogen (N), Oxygen (O), Fluorine (F), Chlorine (Cl), Silicon (Si)
- D-Block Elements:
- Last electron enters: d-orbital
- Groups: 3 to 12
- Characteristics:
- Transition metals
- Variable oxidation states
- Form colored compounds
- Good conductors of heat and electricity
- Catalytic properties
- Examples: Iron (Fe), Copper (Cu), Zinc (Zn), Silver (Ag), Gold (Au)
- F-Block Elements:
- Last electron enters: f-orbital
- Lanthanides (4f series) and Actinides (5f series)
- Characteristics:
- Similar properties within each series
- Mostly form compounds with 3 oxidation states
- Used in various applications, such as magnets, catalysts, and nuclear power
- Examples: Lanthanum (La), Cerium (Ce), Uranium (U), Plutonium (Pu)
Group and Period Characteristics
| Group | Name | General Properties |
|---|---|---|
| 1 | Alkali Metals | Soft, silvery metals, highly reactive, low melting and boiling points, form +1 ions |
| 2 | Alkaline Earth Metals | Harder, denser metals, less reactive than alkali metals, form +2 ions |
| 17 | Halogens | Highly reactive nonmetals, exist as diatomic molecules, form -1 ions |
| 18 | Noble Gases | Colorless, odorless gases, very unreactive, exist as single atoms |
Application of Periodic Trends in Chemical Reactions
Periodic trends are the predictable variations in properties of elements across a period (row) or down a group (column) of the periodic table. Understanding these trends allows us to make predictions about the reactivity of elements and their behavior in chemical reactions.
Reactivity of Elements
Ionization Energy
- Definition: The energy required to remove an electron from an atom.
- Trend: Increases across a period, decreases down a group.
- Reactivity: Elements with lower ionization energies tend to lose electrons more readily, making them more reactive.
Electron Affinity
- Definition: The energy change associated with gaining an electron.
- Trend: Generally increases across a period, decreases down a group (with exceptions).
- Reactivity: Elements with higher electron affinities tend to gain electrons more easily, making them more reactive in reactions involving electron gain.
Electronegativity
- Definition: The ability of an atom to attract electrons toward itself in a chemical bond.
- Trend: Increases across a period, decreases down a group.
- Reactivity: Elements with higher electronegativities tend to form stronger bonds and participate in more diverse chemical reactions.
Trends in Acid-Base Behavior
Oxides
- Metallic oxides: Tend to be basic. As we move down a group, the metallic character increases, leading to more basic oxides.
- Non-metallic oxides: Tend to be acidic. As we move across a period, the non-metallic character increases, leading to more acidic oxides.
Hydroxides
- Group 1 and 2 hydroxides: Strongly basic.
- Group 13-16 hydroxides: Amphoteric (can act as both acids and bases).
- Group 17 hydroxides: Strongly acidic.
Important NEET Questions on Classification of Elements and Periodicity in Properties
| Question Type | Question |
|---|---|
| Conceptual Questions | Which of the following elements has the highest first ionization energy? a) Na b) Mg c) Al d) SiWhich of the following elements has the highest electronegativity? a) F b) Cl c) Br d) I Which of the following oxides is most acidic? Which of the following elements shows the maximum number of oxidation states? Which of the following pairs of elements have similar chemical properties? |
| Numerical Problems | The first ionization energy of Na is 5.1 eV. What is the energy required to remove an electron from the second orbit of Na⁺? a) 13.6 eV b) 16.2 eV c) 21.8 eV d) 30.6 eVThe ionic radii of Na⁺, Mg²⁺, Al³⁺, and Si⁴⁺ are in the order: a) Na⁺ > Mg²⁺ > Al³⁺ > Si⁴⁺ b) Na⁺ > Al³⁺ > Mg²⁺ > Si⁴⁺ c) Si⁴⁺ > Al³⁺ > Mg²⁺ > Na⁺ d) Al³⁺ > Si⁴⁺ > Mg²⁺ > Na⁺ |
| Statement-Based Questions | Statement 1: The atomic radius of Cl is less than that of F. Statement 2: The effective nuclear charge of Cl is greater than that of F. a) Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1. b) Both Statement 1 and Statement 2 are correct but Statement 2 is not the correct explanation of Statement 1. c) Statement 1 is correct but Statement 2 is incorrect. d) Statement 1 is incorrect but Statement 2 is correct.Statement 1: The ionization energy of N is higher than that of O. Statement 2: The electronic configuration of N is more stable than that of O. a) Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1. b) Both Statement 1 and Statement 2 are correct but Statement 2 is not the correct explanation of Statement 1. c) Statement 1 is correct but Statement 2 is incorrect. d) Statement 1 is incorrect but Statement 2 is correct. |
FAQs about Classification of Elements and Periodicity in Properties
1. What is the periodic desk?
Ans: The periodic desk is a scientific arrangement of factors primarily based on their atomic numbers, electron configurations, and ordinary chemical houses.
2. What are intervals inside the periodic desk?
Ans: Periods are horizontal rows in the periodic table. There are 7 durations, and as you pass across a period, atomic quantity increases, and factors exchange from metals to non-metals.
3. What are groups within the periodic desk?
Ans: Groups are vertical columns within the periodic desk. There are 18 businesses, and elements within the same group share comparable chemical houses due to comparable electron configurations.
4. What is periodicity in residences?
Ans: Periodicity refers back to the habitual developments or styles inside the properties of factors as you circulate throughout durations or down organizations inside the periodic table, together with atomic size, ionization energy, and electronegativity.
5. What is atomic radius?
Ans: The atomic radius is the gap from the nucleus of an atom to the outermost electron. It decreases throughout a length and increases down a collection.