COMEDK UGET Chemistry - Inorganic Chemistry Syllabus

Chemistry - Inorganic Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry - Inorganic Chemistry in COMEDK UGET, not a summary of it.

1. 1

   Periodicity and Chemical Bonding

   3 topics

   • Classification of Elements and Periodicity
     • Modern periodic law
     • Periodic trends in atomic and ionic radii
     • Ionisation enthalpy and electronegativity
   • Chemical Bonding and Molecular Structure
     • Ionic and covalent bonding
     • VSEPR theory and shapes
     • Hybridisation and molecular orbital theory
     • Hydrogen bonding
   • Valence and Bond Parameters
     • Bond length, bond angle and bond order
     • Resonance and polarity of bonds
2. 2

   Hydrogen and s-Block Elements

   3 topics

   • Hydrogen
     • Position in periodic table and isotopes
     • Water, hydrogen peroxide and hydrides
   • Alkali Metals
     • General characteristics and trends
     • Important compounds of sodium
   • Alkaline Earth Metals
     • General characteristics and trends
     • Important compounds of calcium
3. 3

   p-Block Elements

   3 topics

   • Groups 13 and 14
     • Boron family trends and compounds
     • Carbon family trends and compounds
   • Groups 15 and 16
     • Nitrogen family and oxoacids
     • Oxygen family and oxides
   • Groups 17 and 18
     • Halogens and interhalogen compounds
     • Noble gases and their compounds
4. 4

   Transition Elements and Coordination Compounds

   3 topics

   • d- and f-Block Elements
     • Transition metal properties
     • Lanthanoids and actinoids
     • Important compounds: KMnO4, K2Cr2O7
   • Coordination Compounds
     • Werner's theory and nomenclature
     • Isomerism in complexes
     • Valence bond and crystal field theory
   • Metallurgy
     • Principles and methods of extraction
     • Thermodynamic and electrochemical principles

Chemistry - Inorganic Chemistry flashcards for COMEDK UGET

25 of 51 cards from the Chemistry - Inorganic Chemistry deck — real questions with worked answers.

1. State the modern periodic law.

   The physical and chemical properties of elements are a periodic function of their atomic numbers (not atomic masses).

2. How are elements classified into blocks based on the subshell receiving the last electron?

   s-block (last electron in s), p-block (in p), d-block/transition (in d), and f-block/inner-transition (in f).

3. Define ionization enthalpy and state its general trends across a period and down a group.

   Energy required to remove the most loosely bound electron from an isolated gaseous atom. It increases across a period and decreases down a group.

4. Why is the first ionization enthalpy of nitrogen higher than that of oxygen?

   Nitrogen has a half-filled, extra-stable 2p3 configuration, so removing an electron requires more energy than from oxygen's 2p4.

5. Define electron gain enthalpy and explain why chlorine has a more negative value than fluorine.

   Energy change when an electron is added to a neutral gaseous atom. Cl is more negative because F's small size causes high inter-electronic repulsion in its compact 2p subshell.

6. What is the lanthanoid contraction and one of its consequences?

   The steady decrease in atomic/ionic size across the lanthanoid series due to poor shielding by 4f electrons. Consequence: Zr and Hf have nearly identical sizes.

7. Arrange the trend in metallic and non-metallic character across a period and down a group.

   Metallic character decreases across a period and increases down a group; non-metallic character shows the opposite trend.

8. State the octet rule and one major limitation.

   Atoms tend to gain, lose, or share electrons to achieve eight electrons in their valence shell. Limitation: it fails for species like BF3, PCl5, SF6, and odd-electron molecules (NO).

9. What does VSEPR theory predict and on what basis?

   It predicts molecular geometry based on minimizing repulsion among electron pairs (bonding and lone) around the central atom; repulsion order: lp-lp > lp-bp > bp-bp.

10. Give the hybridization, shape, and bond angle of CH4, NH3, and H2O.

    All sp3. CH4: tetrahedral, 109.5 degrees; NH3: pyramidal, ~107 degrees; H2O: bent, ~104.5 degrees (angles decrease due to lone pairs).

11. Define a coordinate (dative) bond and give an example.

    A covalent bond in which both shared electrons are donated by one atom. Example: NH4+ (N donates the lone pair to H+) or H3N->BF3.

12. State the key postulates of valence bond theory (VBT).

    A covalent bond forms by overlap of half-filled atomic orbitals; greater overlap gives a stronger bond; the shared electrons have opposite spins and the bond lies along the line of maximum overlap.

13. Differentiate sigma and pi bonds.

    Sigma: end-to-end (axial) overlap, stronger, allows free rotation. Pi: sideways (lateral) overlap of p/d orbitals, weaker, restricts rotation.

14. Write the molecular orbital electronic configuration and bond order of O2.

    KK sigma2s2 sigma*2s2 sigma2pz2 pi2px2=pi2py2 pi*2px1=pi*2py1; bond order = (8-4)/2 = 2; paramagnetic (two unpaired electrons).

15. How is bond order calculated in MO theory and what does it indicate?

    Bond order = (Nb - Na)/2, where Nb and Na are electrons in bonding and antibonding MOs. Higher bond order means greater bond strength and shorter bond length.

16. Define dipole moment and give its unit.

    Dipole moment (mu) = charge x distance of separation; a measure of bond/molecular polarity. Unit: debye (D), where 1 D = 3.33564 x 10^-30 C m.

17. Why does CO2 have zero dipole moment while H2O has a non-zero value?

    CO2 is linear and symmetric, so bond dipoles cancel; H2O is bent, so its bond dipoles do not cancel, giving a net dipole moment.

18. State Fajans' rules for the development of covalent character in an ionic bond.

    Covalent character increases with: small cation, large anion, high charge on either ion, and a cation with a pseudo-noble-gas (d-electron) configuration.

19. What is hydrogen bonding and how does it affect boiling points?

    An electrostatic attraction between H bonded to a highly electronegative atom (F, O, N) and a lone pair on another such atom. It raises boiling points (e.g., H2O > H2S).

20. Explain the position of hydrogen in the periodic table.

    Hydrogen resembles alkali metals (1 valence electron, forms H+) and halogens (1 electron short of noble gas, forms H-), so it has an anomalous position, usually placed in Group 1.

21. Name the three types of hydrides with an example of each.

    Ionic/saline (NaH), covalent/molecular (CH4, H2O), and metallic/interstitial (LaH2, TiH1.7).

22. What is the difference between temporary and permanent hardness of water and how is each removed?

    Temporary hardness is due to bicarbonates of Ca/Mg (removed by boiling or Clark's method with lime). Permanent hardness is due to chlorides/sulphates of Ca/Mg (removed by washing soda or ion-exchange).

23. What is heavy water and one of its uses?

    Heavy water is D2O (deuterium oxide). It is used as a moderator in nuclear reactors and in the preparation of deuterated compounds.

24. Why are alkali metals strong reducing agents, strongest in solution being Li?

    They have low ionization enthalpies and readily lose their single valence electron. In aqueous solution Li is the strongest reducing agent due to its very high hydration enthalpy (most negative E0).

25. What colors do Li, Na, and K impart to a flame and why?

    Li: crimson red, Na: golden yellow, K: lilac/violet. Heat excites the valence electron, which emits visible light on returning to the ground state.

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