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COMEDK UGET Chemistry - Inorganic Chemistry Syllabus

The Chemistry - Inorganic Chemistry syllabus for COMEDK UGET in full: 4 chapters, 12 topics and 29 sub-topics, every one listed below, plus 51 Chemistry - Inorganic Chemistry flashcards with answers.

4Chapters
12Topics
29Sub-topics
51Flashcards

Chemistry - Inorganic Chemistry syllabus: all 4 chapters

Expand any chapter to see its topics and sub-topics.

  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. 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. 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. 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

COMEDK UGET Chemistry - Inorganic Chemistry flashcards — 51 questions with 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.

Show the other 31 Chemistry - Inorganic Chemistry flashcards

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

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

  2. 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).

  3. 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.

  4. 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).

  5. 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.

  6. What is the diagonal relationship and which pairs show it?

    Similarity between an element and the element diagonally placed to its lower right due to similar size/charge ratio. Pairs: Li-Mg, Be-Al, B-Si.

  7. Describe the Solvay (ammonia-soda) process product and why it cannot be used for potassium carbonate.

    It produces Na2CO3 (washing soda) via NaHCO3. It fails for K2CO3 because KHCO3 is too soluble to be precipitated out.

  8. Why is BeO amphoteric while the oxides of other alkaline earth metals are basic?

    Be is small with high charge density and significant covalent character, so BeO reacts with both acids and bases; the larger metals form purely ionic, basic oxides.

  9. What is the cause of Be's anomalous behaviour among alkaline earth metals?

    Its small size, high ionization enthalpy, high electronegativity, absence of d-orbitals, and high charge/size ratio give it largely covalent compounds (diagonal relation with Al).

  10. What is gypsum, plaster of Paris, and the reaction connecting them?

    Gypsum is CaSO4.2H2O; heating it to ~393 K gives plaster of Paris, CaSO4.(1/2)H2O, which re-sets to gypsum on adding water.

  11. State the inert pair effect and its relevance in Group 13/14.

    The reluctance of the ns2 electrons to participate in bonding, increasing down the group. It makes lower oxidation states more stable (e.g., Tl+ over Tl3+, Pb2+ over Pb4+).

  12. Why is BCl3 a Lewis acid while it is electron deficient?

    Boron in BCl3 has only six valence electrons (incomplete octet), so it accepts an electron pair, behaving as a Lewis acid.

  13. What are the three allotropes/forms of carbon and a structural feature of each?

    Diamond (sp3, 3D tetrahedral network, hardest), graphite (sp2 layers, conducts, slippery), and fullerene (e.g., C60, cage-like spherical molecule).

  14. Why does carbon show catenation more than silicon?

    The C-C bond is much stronger than the Si-Si bond, so carbon forms long, stable chains and rings far more readily than silicon.

  15. What are silicones and one of their properties?

    Synthetic organosilicon polymers with (R2SiO)n backbone, made by hydrolysis of alkyl/aryl chlorosilanes. They are water-repellent, thermally stable, and chemically inert.

  16. Explain why N2 is exceptionally unreactive.

    N2 has a very strong triple bond (bond dissociation enthalpy ~941 kJ/mol), making it kinetically inert at ordinary temperatures.

  17. Why does nitrogen not form pentahalides like phosphorus?

    Nitrogen lacks d-orbitals in its valence shell, so it cannot expand its octet; phosphorus has accessible 3d orbitals and forms PCl5, etc.

  18. Describe the structures of the white and red allotropes of phosphorus.

    White phosphorus consists of discrete tetrahedral P4 molecules (reactive, toxic); red phosphorus is a polymeric chain of P4 units (less reactive, stable).

  19. State the trend in stability of the +6 and +4 oxidation states down Group 16.

    Stability of +6 decreases and +4 increases down the group due to the inert pair effect (e.g., SO3 vs PoO2).

  20. Outline the Contact process for manufacturing sulphuric acid.

    S/SO2 is oxidized to SO3 over V2O5 catalyst (2SO2 + O2 -> 2SO3), SO3 is absorbed in conc. H2SO4 to form oleum (H2S2O7), which is diluted to give H2SO4.

  21. Why does ozone act as a powerful oxidizing agent?

    Ozone (O3) readily decomposes to give nascent oxygen (O3 -> O2 + [O]), which is a strong oxidant.

  22. State the trend in oxidizing power and bond dissociation enthalpy in Group 17.

    Oxidizing power decreases F2 > Cl2 > Br2 > I2. Bond dissociation enthalpy order: Cl2 > Br2 > F2 > I2 (F2 anomalously low due to small size/lone-pair repulsion).

  23. Why is HF a weaker acid than HCl, HBr, and HI?

    The H-F bond is the strongest of the hydrogen halides (small F, high bond enthalpy), so it ionizes least readily, making HF the weakest acid in the series.

  24. Why are noble gases (Group 18) chemically inert and which forms most compounds?

    They have stable, completely filled valence shells (ns2np6) and very high ionization enthalpies. Xenon, being largest with lowest IE, forms the most compounds (e.g., XeF2, XeF4, XeF6).

  25. Give the hybridization and shape of XeF4.

    sp3d2 hybridization with two lone pairs; square planar shape.

  26. Define transition elements and explain why Zn, Cd, Hg are often excluded.

    Elements with partially filled d-orbitals in atom or common ions. Zn, Cd, Hg have completely filled d10 configurations in their common ions, so they are not typical transition metals.

  27. Why do transition metals show variable oxidation states?

    Because their (n-1)d and ns orbitals have similar energies, electrons from both can participate in bonding, allowing many oxidation states.

  28. Why are most transition metal compounds coloured?

    Due to d-d electronic transitions: an electron absorbs visible light to jump between split d-orbitals, and the complementary colour is observed.

  29. State Werner's coordination theory key idea, defining primary and secondary valencies.

    Metals show two valencies: primary valency (ionizable, satisfied by anions, = oxidation state) and secondary valency (non-ionizable, fixed in number, = coordination number, gives geometry).

  30. Define ligand, coordination number, and denticity with an example of a bidentate ligand.

    Ligand: an ion/molecule donating an electron pair to the metal. Coordination number: number of donor atoms bonded to the metal. Denticity: number of donor sites; ethylenediamine (en) is bidentate.

  31. Name the principal steps in the metallurgical extraction of a metal from its ore.

    Concentration/dressing of ore, conversion to oxide (roasting/calcination), reduction of oxide to metal, and refining/purification of the crude metal.

COMEDK UGET Chemistry - Inorganic Chemistry FAQ

What is in the COMEDK UGET Chemistry - Inorganic Chemistry syllabus?

COMEDK UGET Chemistry - Inorganic Chemistry is split into 4 chapters: Periodicity and Chemical Bonding, Hydrogen and s-Block Elements, p-Block Elements and Transition Elements and Coordination Compounds. Together they contain 12 topics and 29 sub-topics.

How many chapters are in COMEDK UGET Chemistry - Inorganic Chemistry?

4 chapters, containing 12 topics and 29 sub-topics. The largest chapter is Periodicity and Chemical Bonding, with 3 topics.

Are there flashcards for COMEDK UGET Chemistry - Inorganic Chemistry?

Yes — a 51-card Chemistry - Inorganic Chemistry deck, printed in full in the flashcards section of this page and available in the Examius app with spaced repetition. The free plan covers one exam of your choice, including its flashcards; Examius Pro, a one-time purchase, unlocks every other exam and deck.