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Periodic Properties Of Elements

Home > PowerPoint Slides > Periodic Properties Of Elements
Published in: Chemistry
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Discussion about some property trends

Suranjana M / Aurangabad

19 years of teaching experience

Qualification: M.Tech (IIT,Kharagpur - 2000)

Teaches: Science, Chemistry

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  1. PERIODIC PROPERTIES OF ELEMENTS Prepared by Ms. Suranjana mandal Ms. Shilpa kodgire Maharashtra institute of technology, A ad, M.S
  2. PERIODIC PROPERTIES Periodic law = elements arranged by atomic number gives physical and chemical properties varying periodically. We will study the following periodic trends: Atomic radii Metallic and Non metallic character • Ionization energy Electron affinity Electronegativity Melting point
  3. ATOMIC RADIUS Li Be 6.94 9.01 Atomic radii actually decrease across a row in the periodic table. Due to an increase in the effective nuclear charge. Within each group (vertical column), the atomic radius tends to increase with the period number. INCREASING ATOMIC RADIUS 3 o
  4. METALLIC AND NON METALLIC CHARACTER z z P. U 'N i P" JAM Cm, Ot CtlU INCREASING METALLIC CHARACTER 16 s 34 Cl 2 as Ar 11 19 20 22 2B 27 30 3 33 K ca sc Ti V Cr Mn Fe co Ni cu Ga Ge As Metallic characteristics decrease from left to right across a period. This is caused by the decrease in radius of the atom that allows the outer electrons to ionize more readily. Metallic characteristics increase down a group. Electron shielding causes the atomic radius to increase thus the outer electrons ionizes more readily than electrons in smaller atoms. Metallic character relates to the ability to lose electrons, and nonmetallic character relates to the ability to gain electrons.
  5. HELIUM IONIZATION ENERGY 4 s NEON 6 7 8 10 11 12 13 ATOMIC NUMBER 1 Mg 2 3 INCREASING IONIZATION ENERGY 14 2 z z Ionization energy required to remove an electron from a neutral atom in its gaseous phase. Conceptually, ionization energy is the opposite of electronegativity. The lower this energy is, the more readily the atom becomes a cation. Therefore, the higher this energy is, the more unlikely it is the atom becomes a cation. Generally, elements on the right side of the periodic table have a higher ionization energy because their valence shell is nearly filled. Elements on the left side of the periodic table have low ionization energies because of their willingness to lose electrons and become cations. Hence,ionization energy increases from left to right on the periodic table. The ionization energy of the elements within a period generally increases from left to right. This is due to valence shell stability. The ionization energy of the elements within a group generally decreases from top to bottom. This is due to electron shielding. The noble gases possess very high ionization energies because of their full valence shells as indicated in the graph. Note that helium has the highest ionization energy of all the elements.
  6. ELECTRON AFFINITY Electron affinity is the ability of an atom to accept an electron. Electron affinity is a quantitative measurement of the energy change that occurs when an electron is added to a neutral gas atom. The more negative the electron affinity value, the higher an atom's affinity for electrons. INCREASING ELECTRON AFFINITY 2 S.nv;• z z z
  7. ELECTRONEGATIVITY INCREASING ELECTRONEGATIVITY 2 13 DAI Si Mg 19 20 22 23 -24 26 27 30 34 K ca se Ti V Cr Mn Fe co Ni cu zo Ga Ge As se Br Kr z Electronegativity can be understood as a chemical property describing an atom's ability to attract and bind with electrons Electronegativity is a qualitative property, there is no standardized for method electronegativity. Electronegativity element can be periodic tables. calculating values for each found on certain
  8. MELTING POINT 4000 3500 3000 2500 z 2000 1500 z 1000 soo H He -soo The melting points is the amount of energy required to break a bond(s) to change the solid phase of a substance to a liquid. The stronger the bond between the atoms of an element, the more energy required to break that bond. As temperature is directly proportional to energy, a high bond dissociation energy correlates to a high temperature. Melting points are varied and do not generally form a distinguishable trend across the periodic table. However, certain conclusions can be drawn from the graph below. Metals generally possess a high melting point. Most non-metals possess low melting points. The non-metal carbon possesses the highest boiling point of all the elements. The semi-metal boron also possesses a high melting point.
  9. REFERENCES https://chem.libretexts.org/Core/Inorganic Chemistry/ Descriptive Chemistry/ Pe riodic Trends of Elemental Properties/ Periodic Trends https://VNNLkhanacademy.org/science/ap-chemistry/periodic-table-ap https://smmn.youtube.com/

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