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🇵🇰 NTS NAT-IE · flashcards
NTS NAT-IE Chemistry Flashcards
50 question-and-answer cards covering Chemistry as it is examined in NTS NAT-IE. 24 of them are printed below, taken from across the deck — no signup, no paywall on the preview.
24 sample cards from the Chemistry deck
Sampled from the end of the deck, so these are different cards from the ones shown on the syllabus page.
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.
What this deck covers
The Chemistry deck follows the NTS NAT-IE Chemistry syllabus — 9 chapters and 25 topics — so questions land on material that is genuinely examinable rather than trivia around it. That works out to roughly 5.6 cards per chapter.
Answers are written to be recallable, not just readable — averaging about 107 characters, which is long enough to carry the reasoning and short enough to say out loud.
A deck like this earns its keep on the second and third pass. Read the syllabus first so you know the shape of the subject, then use the cards to find the specific facts that have not stuck.
Chemistry flashcards FAQ
How many Chemistry flashcards are in this NTS NAT-IE deck?
50 cards. This page previews 24 of them, sampled evenly across the deck so you can judge the difficulty before installing anything.
Are these NTS NAT-IE flashcards free?
Yes. The preview here is free to read with no signup, and the full 50-card deck is free inside the Examius app.
What do the Chemistry cards cover?
They follow the NTS NAT-IE Chemistry syllabus — 9 chapters and 25 topics — so the questions track what is actually examinable.
How should I use these flashcards?
Read the syllabus first so you know the shape of the subject, then drill the deck. Examius schedules each card with spaced repetition, so cards you keep missing come back sooner and ones you know drift further apart.