BS Nursing Entry Test Chemistry Syllabus

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 in BS Nursing Entry Test, not a summary of it.

1. 1

   Atomic Structure

   3 topics

   • Subatomic Particles
   • Electronic Configuration
   • Isotopes
2. 2

   Periodic Table and Periodicity

   3 topics

   • Periodic Law
   • Periodic Trends
   • Groups and Periods
3. 3

   Chemical Bonding

   4 topics

   • Ionic Bonding
   • Covalent Bonding
   • Hydrogen Bonding
   • Molecular Geometry
4. 4

   States of Matter

   3 topics

   • Gaseous State
   • Liquid State
   • Solid State
5. 5

   Chemical Thermodynamics

   3 topics

   • Enthalpy and Energy Changes
   • Hess's Law
   • Exothermic and Endothermic Reactions
6. 6

   Chemical Equilibrium

   3 topics

   • Reversible Reactions
   • Le Chatelier's Principle
   • Equilibrium Constant
7. 7

   Acids, Bases and Salts

   4 topics

   • Theories of Acids and Bases
   • pH and pOH
   • Buffers
   • Salt Hydrolysis
8. 8

   Reaction Kinetics

   3 topics

   • Rate of Reaction
   • Factors Affecting Reaction Rate
   • Catalysis
9. 9

   Organic Chemistry

   3 topics

   • Hydrocarbons
   • Functional Groups
   • Isomerism
10. 10

    Biochemistry

    4 topics

    • Carbohydrates
    • Proteins and Amino Acids
    • Lipids
    • Vitamins and Enzymes

Chemistry flashcards for BS Nursing Entry Test

21 of 50 cards from the Chemistry deck — real questions with worked answers.

1. What are the three subatomic particles, and what is the relative charge of each?

   Proton (+1), neutron (0, neutral), and electron (-1).

2. Compare the relative masses of a proton, neutron, and electron.

   Proton and neutron each have a relative mass of about 1 amu. The electron is much lighter, about 1/1836 amu (negligible).

3. Where in the atom are protons, neutrons, and electrons located?

   Protons and neutrons are in the nucleus; electrons move around the nucleus in shells/orbitals.

4. What does the atomic number (Z) of an element represent?

   The number of protons in the nucleus (which also equals the number of electrons in a neutral atom).

5. What does the mass number (A) of an atom represent, and how is it calculated?

   The total number of protons and neutrons in the nucleus. A = number of protons + number of neutrons.

6. How do you calculate the number of neutrons in an atom?

   Number of neutrons = Mass number (A) - Atomic number (Z).

7. What is the maximum number of electrons a shell can hold according to the 2n² rule?

   2n², where n is the shell number: 1st shell = 2, 2nd = 8, 3rd = 18, 4th = 32.

8. State the order of filling for the first four subshells by increasing energy (Aufbau).

   1s, 2s, 2p, 3s (following the Aufbau principle of filling lowest energy levels first).

9. What is the maximum number of electrons in s, p, d, and f subshells?

   s = 2, p = 6, d = 10, f = 14.

10. Write the electronic configuration of a neutral sodium atom (Z = 11).

    1s² 2s² 2p⁶ 3s¹ (or 2, 8, 1).

11. State the Pauli Exclusion Principle.

    No two electrons in an atom can have the same set of four quantum numbers; an orbital holds at most 2 electrons with opposite spins.

12. State Hund's Rule of maximum multiplicity.

    Electrons fill degenerate orbitals singly first, all with parallel spins, before pairing up.

13. What are isotopes?

    Atoms of the same element having the same atomic number (protons) but different mass numbers (different numbers of neutrons).

14. Do isotopes of an element have the same chemical properties? Why?

    Yes, because they have the same number of protons and electrons, so the same electronic configuration. They differ only in physical properties related to mass.

15. Name the three isotopes of hydrogen and their mass numbers.

    Protium (¹H, 0 neutrons), Deuterium (²H, 1 neutron), and Tritium (³H, 2 neutrons).

16. How is the relative atomic mass of an element with isotopes calculated?

    It is the weighted average of the masses of its isotopes based on their natural relative abundances.

17. State the Modern Periodic Law.

    The physical and chemical properties of elements are a periodic function of their atomic numbers.

18. On what basis did Mendeleev originally arrange elements, and how does it differ from the modern table?

    Mendeleev arranged elements by increasing atomic mass; the modern periodic table arranges them by increasing atomic number.

19. How does atomic radius change across a period (left to right) and down a group?

    Atomic radius decreases across a period (increasing nuclear charge) and increases down a group (additional shells).

20. How does ionization energy change across a period and down a group?

    Ionization energy increases across a period and decreases down a group.

21. What is ionization energy?

    The minimum energy required to remove the most loosely bound (outermost) electron from a gaseous atom.

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