UPCAT Chemistry — Matter, Mixtures & MeasurementCheat Sheet
A printable cheat sheet for Matter, Mixtures & Measurement, built for UPCAT reviewers who want one go-to reference in the final stretch. Covers formulas, key definitions, common question types, and the University of the Philippines-specific twists you will see on UPCAT day.
Exam context
On the UPCAT 2026, the Chemistry subtest carries a "Core" weight in University of the Philippines's pattern. Matter, Mixtures & Measurement lands at position 1st out of 7 in the standard review order. Target score is UPG ≤ 2.2 typical, and roughly 20 items come from Chemistry on a typical UPCAT paper.
Matter, Mixtures & Measurement - Cheat sheet
Your last-minute revision companion for Matter, Mixtures & Measurement - covering all essential concepts, formulas, and definitions for UPCAT and other college entrance exams.
Sections
Section Title
Matter Classification
Important Facts
- Elements cannot be broken down by chemical means
- Compounds have fixed ratios of elements
- Mixtures have variable compositions
- Pure substances have constant properties throughout
Key Definitions
Term
Matter
Example
Water, air, rocks, living organisms
Definition
Anything that has mass and occupies space (volume)
Term
Pure Substance
Example
Pure water (H₂O), pure gold (Au)
Definition
Matter with definite composition and distinct properties
Term
Element
Example
Hydrogen (H), Carbon (C), Oxygen (O)
Definition
Pure substance composed of the same type of atoms; cannot be broken down chemically
Term
Compound
Example
Water (H₂O), Carbon dioxide (CO₂)
Definition
Pure substance made of two or more different elements chemically combined
Term
Mixture
Example
Salt water, air, concrete
Definition
Combination of two or more substances physically combined; can be separated mechanically
Diagrams To Know
- Classification tree of matter
- Particle arrangement in elements vs compounds
Section Title
Types of Mixtures
Important Facts
- Solutions are transparent and do not scatter light
- Colloids scatter light (Tyndall Effect) but do not settle
- Suspensions settle over time and can be filtered
- Particle size: Solution < Colloid < Suspension
Key Definitions
Term
Homogeneous Mixture
Example
Salt water, air, brass
Definition
Uniform mixture where components are evenly distributed
Term
Heterogeneous Mixture
Example
Oil and water, sand and water
Definition
Non-uniform mixture where components are not evenly distributed
Term
Solution
Example
Sugar in water, vinegar
Definition
Homogeneous mixture where solute dissolves in solvent
Term
Colloid
Example
Milk, mayonnaise, fog
Definition
Mixture with particles too large to dissolve but too small to settle; shows Tyndall Effect
Term
Suspension
Example
Sand in water, muddy water
Definition
Mixture with large particles that settle at the bottom
Term
Tyndall Effect
Example
Light beam through milk or fog
Definition
Scattering of light by colloidal particles
Diagrams To Know
- Particle size comparison diagram
- Tyndall Effect demonstration
Section Title
States of Matter
Important Facts
- All states have definite mass
- Solids are incompressible and have strong intermolecular forces
- Liquids are slightly compressible with moderate intermolecular forces
- Gases are highly compressible with weak intermolecular forces
- Plasma is the most abundant state in the universe
Key Definitions
Term
Solid
Example
Ice, metals, crystals
Definition
State with definite shape and volume; molecules vibrate in fixed positions
Term
Liquid
Example
Water, oil, mercury
Definition
State with definite volume but indefinite shape; molecules move past each other
Term
Gas
Example
Air, steam, carbon dioxide
Definition
State with indefinite shape and volume; molecules move freely
Term
Plasma
Example
Stars, lightning, neon signs
Definition
Superheated matter containing charged ions and electrons
Diagrams To Know
- Particle arrangement in different states
- Phase transition diagram
Common Values
Value
0°C or 273.15 K
Symbol
mp
Quantity
Melting point of ice
Value
100°C or 373.15 K at 1 atm
Symbol
bp
Quantity
Boiling point of water
Section Title
Phase Transitions
Important Facts
- All phase transitions are physical changes
- Energy is absorbed during melting, evaporation, and sublimation
- Energy is released during freezing, condensation, and deposition
- Phase transitions occur at specific temperatures and pressures
Key Definitions
Term
Melting
Example
Ice melting to water
Definition
Solid to liquid transition
Term
Freezing
Example
Water freezing to ice
Definition
Liquid to solid transition
Term
Evaporation
Example
Water evaporating from a puddle
Definition
Liquid to gas transition at surface
Term
Boiling
Example
Water boiling at 100°C
Definition
Liquid to gas transition throughout the liquid
Term
Condensation
Example
Steam condensing on a cold surface
Definition
Gas to liquid transition
Term
Sublimation
Example
Dry ice subliming to CO₂ gas
Definition
Direct solid to gas transition
Term
Deposition
Example
Frost formation
Definition
Direct gas to solid transition
Diagrams To Know
- Phase transition diagram with arrows
- Heating/cooling curve
Section Title
Chemical vs Physical Changes
Important Facts
- Physical changes are usually reversible
- Chemical changes often involve energy changes
- Signs of chemical change: color change, gas production, heat/light emission
- Mass is conserved in both physical and chemical changes
Key Definitions
Term
Physical Change
Example
Melting ice, cutting paper
Definition
Change in form without altering chemical composition
Term
Chemical Change
Example
Burning wood, rusting iron
Definition
Change where new substances with different properties are formed
Term
Physical Property
Example
Color, density, melting point
Definition
Property observed without changing chemical composition
Term
Chemical Property
Example
Flammability, reactivity with acids
Definition
Property related to ability to undergo chemical reactions
Diagrams To Know
- Examples of physical vs chemical changes
Section Title
Separation Techniques
Important Facts
- Choose method based on physical properties of components
- Filtration works for insoluble solids in liquids
- Distillation requires significant boiling point differences
- Chromatography separates based on solubility and molecular size
Key Definitions
Term
Filtration
Example
Separating sand from water
Definition
Separates solids from liquids using filter paper
Term
Distillation
Example
Separating water from salt solution
Definition
Separates liquids based on different boiling points
Term
Decantation
Example
Separating oil from water
Definition
Separates liquids with different densities by pouring off top layer
Term
Chromatography
Example
Separating ink dyes
Definition
Separates components based on different travel speeds through medium
Term
Magnetism
Example
Separating iron filings from sand
Definition
Separates magnetic materials from non-magnetic ones
Diagrams To Know
- Simple distillation setup
- Filtration apparatus
- Chromatography setup
Section Title
Laws of Chemical Combination
Important Facts
- These laws led to atomic theory development
- Mass ratios are always constant for pure compounds
- Laws apply to all chemical reactions and compounds
Key Definitions
Term
Law of Conservation of Mass
Example
Total mass of reactants = Total mass of products
Definition
Mass cannot be created or destroyed in chemical reactions
Term
Law of Definite Composition
Example
Water always contains H and O in 1:8 mass ratio
Definition
Chemical compounds contain elements in fixed mass ratios
Term
Law of Multiple Proportions
Example
CO and CO₂ have C:O ratios of 1:1 and 1:2
Definition
When elements form multiple compounds, mass ratios are simple whole numbers
Formulas
Formula
Density = mass/volume or ρ = m/V
Meaning
ρ = density, m = mass, V = volume
Watch Out
Units must be consistent (g/mL or kg/m³)
When To Use
When calculating density from mass and volume measurements
Common Values
Value
1.00 g/mL or 1000 kg/m³
Symbol
ρ
Quantity
Density of water
Section Title
Measurement and Significant Figures
Important Facts
- All non-zero digits are significant
- Zeros between non-zero digits are significant
- Leading zeros are not significant
- Trailing zeros after decimal point are significant
- In calculations, round to least precise measurement
Key Definitions
Term
Significant Figures
Example
12.30 has 4 significant figures
Definition
Digits in a measurement that carry meaningful information
Term
Accuracy
Example
Measuring 9.8 m/s² for gravity (true = 9.81)
Definition
How close a measurement is to the true value
Term
Precision
Example
Three measurements: 9.7, 9.8, 9.7 m/s²
Definition
How close repeated measurements are to each other
Diagrams To Know
- Accuracy vs precision target diagrams
Must Remember
- Matter = anything with mass and volume
- Pure substances have fixed composition; mixtures have variable composition
- Elements cannot be broken down chemically; compounds can be
- Homogeneous mixtures are uniform; heterogeneous are not uniform
- Tyndall Effect distinguishes colloids from solutions
- Phase transitions are physical changes, not chemical
- Law of Conservation of Mass: mass is neither created nor destroyed
- Density = mass/volume (ρ = m/V)
- Significant figures rules for measurements and calculations
- Separation methods depend on physical property differences
Last Minute Tips
- Remember the particle size order: Solution < Colloid < Suspension
- For phase transitions, energy is absorbed going up (solid→liquid→gas), released going down
- In density problems, watch your units - convert to match before calculating
- Tyndall Effect = light scattering = colloid (think of car headlights in fog)
- Law of Definite Composition means same compound always has same mass ratios everywhere
Comparison Tables
Rows
Values
- Fixed/Definite
- Variable
Property
Composition
Values
- Constant throughout
- May vary in different parts
Property
Properties
Values
- Only by chemical means
- By physical means
Property
Separation
Values
- H₂O, NaCl, Au
- Salt water, air, soil
Property
Examples
Columns
- Property
- Pure Substance
- Mixture
Table Title
Pure Substances vs Mixtures
Rows
Values
- Definite
- Indefinite
- Indefinite
Property
Shape
Values
- Definite
- Definite
- Indefinite
Property
Volume
Values
- Incompressible
- Slightly compressible
- Highly compressible
Property
Compressibility
Values
- Vibration only
- Move past each other
- Free movement
Property
Molecular Motion
Columns
- Property
- Solid
- Liquid
- Gas
Table Title
States of Matter Properties
Rows
Values
- < 1 nm
- 1-1000 nm
- > 1000 nm
Property
Particle Size
Values
- No
- Yes
- Yes
Property
Tyndall Effect
Values
- No
- No
- Yes
Property
Settling
Values
- Cannot filter
- Cannot filter
- Can filter
Property
Filtration
Columns
- Property
- Solution
- Colloid
- Suspension
Table Title
Solution vs Colloid vs Suspension
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