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NTS NAT-IE Chemistry Syllabus
The Chemistry syllabus for NTS NAT-IE in full: 9 chapters and 25 topics, every one listed below, plus 50 Chemistry flashcards with answers.
Chemistry syllabus: all 9 chapters
Expand any chapter to see its topics and sub-topics.
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Fundamentals of Chemistry
3 topics- Atomic Structure
- Mole Concept and Stoichiometry
- Empirical and Molecular Formulas
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States of Matter
3 topics- Gases and Gas Laws
- Liquids and Intermolecular Forces
- Solids and Crystal Structure
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Chemical Bonding
3 topics- Ionic and Covalent Bonding
- Molecular Geometry
- Hydrogen Bonding
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Thermochemistry and Energetics
2 topics- Enthalpy and Heat of Reaction
- Hess's Law
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Chemical Equilibrium
3 topics- Law of Mass Action
- Le Chatelier's Principle
- Acids, Bases and pH
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Reaction Kinetics
3 topics- Rate of Reaction
- Factors Affecting Rate
- Order of Reaction
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Electrochemistry
3 topics- Oxidation and Reduction
- Electrolysis
- Galvanic Cells
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Organic Chemistry
3 topics- Hydrocarbons
- Functional Groups
- Alcohols, Aldehydes and Carboxylic Acids
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Periodic Table and Periodicity
2 topics- Periodic Trends
- s, p and d Block Elements
NTS NAT-IE Chemistry flashcards — 50 questions with answers
Who discovered the electron, and through what experiment?
J.J. Thomson discovered the electron in 1897 using the cathode ray tube experiment, determining its charge-to-mass ratio.
What did Rutherford's gold foil (alpha-scattering) experiment establish about the atom?
It showed the atom has a small, dense, positively charged nucleus with electrons surrounding mostly empty space.
State the four quantum numbers and what each describes.
Principal (n) – energy level/size; Azimuthal (l) – subshell/shape; Magnetic (m_l) – orbital orientation; Spin (m_s) – electron spin (+1/2 or -1/2).
What is the Aufbau principle?
Electrons fill atomic orbitals in order of increasing energy, starting with the lowest-energy orbital first.
State the Pauli Exclusion Principle.
No two electrons in an atom can have the same set of all four quantum numbers; an orbital holds at most two electrons with opposite spins.
State Hund's Rule.
Electrons occupy degenerate (equal-energy) orbitals singly with parallel spins before pairing up.
What is the maximum number of electrons in an energy level n?
2n², where n is the principal quantum number.
How many electrons can s, p, d, and f subshells hold?
s = 2, p = 6, d = 10, f = 14 electrons.
What are isotopes?
Atoms of the same element with the same number of protons but different numbers of neutrons (different mass numbers).
What is Avogadro's number and what does it represent?
6.022 × 10²³ — the number of particles (atoms, molecules, ions) in one mole of a substance.
Define one mole.
The amount of substance containing as many elementary entities as there are atoms in 12 g of carbon-12, i.e., 6.022 × 10²³ particles.
How do you calculate the number of moles from a given mass?
moles = mass (g) ÷ molar mass (g/mol).
What is molar mass?
The mass of one mole of a substance in grams per mole (g/mol), numerically equal to its atomic or molecular mass in amu.
What volume does one mole of any ideal gas occupy at STP?
22.4 litres (at 0 °C and 1 atm).
In stoichiometry, what is a limiting reagent?
The reactant that is completely consumed first and therefore limits the amount of product formed.
How is percentage yield calculated?
Percentage yield = (actual yield ÷ theoretical yield) × 100.
What is an empirical formula?
The simplest whole-number ratio of atoms of each element in a compound.
What is a molecular formula?
The actual number of atoms of each element in one molecule of a compound.
How is the molecular formula related to the empirical formula?
Molecular formula = n × (empirical formula), where n = molar mass ÷ empirical formula mass.
What are the steps to determine an empirical formula from percentage composition?
Divide each element's % by its atomic mass to get moles, then divide all by the smallest value to get the simplest whole-number ratio.
Show the other 30 Chemistry flashcards
State Boyle's Law.
At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure (PV = constant).
State Charles's Law.
At constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature (V/T = constant).
State Avogadro's Law.
Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules (V ∝ n).
Write the ideal gas equation and define each term.
PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant, T = absolute temperature (Kelvin).
State Dalton's Law of Partial Pressures.
The total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of the individual gases.
State Graham's Law of Diffusion.
The rate of diffusion of a gas is inversely proportional to the square root of its density (or molar mass): rate ∝ 1/√M.
What is vapor pressure of a liquid?
The pressure exerted by a vapor in equilibrium with its liquid at a given temperature.
Define the boiling point of a liquid.
The temperature at which the vapor pressure of the liquid equals the external (atmospheric) pressure.
What is surface tension and what causes it?
The force acting along the surface of a liquid that minimizes surface area, caused by unbalanced intermolecular attractions on surface molecules.
Name the three main types of intermolecular forces in order of increasing strength.
London dispersion forces < dipole-dipole forces < hydrogen bonding.
How does viscosity change with temperature for liquids?
Viscosity decreases as temperature increases, because higher kinetic energy overcomes intermolecular attractions.
What is the difference between crystalline and amorphous solids?
Crystalline solids have a regular, repeating long-range atomic arrangement and sharp melting points; amorphous solids lack long-range order and soften over a range.
Name the four main types of crystalline solids based on bonding.
Ionic, covalent (network), metallic, and molecular solids.
What is a unit cell?
The smallest repeating structural unit of a crystal lattice that, when repeated in three dimensions, generates the entire crystal.
What is the coordination number in a crystal?
The number of nearest-neighbor particles immediately surrounding a given particle in the crystal lattice.
How is an ionic bond formed?
By the complete transfer of one or more electrons from a metal to a non-metal, producing oppositely charged ions held by electrostatic attraction.
How is a covalent bond formed?
By the mutual sharing of one or more pairs of electrons between two non-metal atoms.
What is a coordinate (dative) covalent bond?
A covalent bond in which both shared electrons are donated by the same atom.
How do ionic and covalent compounds differ in electrical conductivity?
Ionic compounds conduct when molten or dissolved (mobile ions); covalent compounds generally do not conduct (no free ions or electrons).
What is electronegativity?
The tendency of an atom in a bond to attract the shared pair of electrons toward itself.
What does VSEPR theory predict?
The geometry of a molecule based on minimizing repulsion between electron pairs (bonding and lone) around the central atom.
What is the shape and bond angle of a molecule with four bonding pairs and no lone pairs (e.g., CH₄)?
Tetrahedral, with bond angles of 109.5°.
What is the shape and bond angle of water (H₂O)?
Bent/angular with a bond angle of about 104.5°, due to two lone pairs on oxygen.
What is the shape and bond angle of ammonia (NH₃)?
Trigonal pyramidal with a bond angle of about 107°, due to one lone pair on nitrogen.
What is hydrogen bonding and which atoms make it possible?
A strong dipole-dipole attraction between a hydrogen atom bonded to F, O, or N and a lone pair on an F, O, or N atom of another molecule.
Why does water have an unusually high boiling point compared to similar molecules?
Because of extensive hydrogen bonding between water molecules, which requires extra energy to break.
Define enthalpy of reaction (ΔH).
The heat change of a reaction measured at constant pressure; ΔH = H(products) − H(reactants).
What is the difference between exothermic and endothermic reactions in terms of ΔH?
Exothermic reactions release heat (ΔH negative); endothermic reactions absorb heat (ΔH positive).
State Hess's Law.
The total enthalpy change of a reaction is the same regardless of the route taken, depending only on the initial and final states.
State the Law of Mass Action.
The rate of a chemical reaction is proportional to the product of the molar concentrations of the reactants, each raised to the power of its coefficient in the balanced equation.
NTS NAT-IE Chemistry FAQ
What is in the NTS NAT-IE Chemistry syllabus?
NTS NAT-IE Chemistry is split into 9 chapters: Fundamentals of Chemistry, States of Matter, Chemical Bonding, Thermochemistry and Energetics, Chemical Equilibrium, Reaction Kinetics, Electrochemistry, Organic Chemistry and Periodic Table and Periodicity. Together they contain 25 topics.
How many chapters are in NTS NAT-IE Chemistry?
9 chapters, containing 25 topics. The largest chapter is Fundamentals of Chemistry, with 3 topics.
Are there flashcards for NTS NAT-IE Chemistry?
Yes — a 50-card 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.