Properties of Matter and Their Measurement: Complete Guide

 Complete Notes on Matter Properties & Measurement in Physics

Visual explanation of physical properties of matter including mass, volume, density, and temperature using scientific instruments.

- Dr.Sanjaykumar Pawar 

📘 1.3 Properties of Matter and Their Measurement

1.3.1 Physical and Chemical Properties

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🔹 1. What are properties of matter?

• Every substance has its own special characteristics.
• These characteristics are called properties.
• Example:
  • Water is colorless
  • Iron is hard and magnetic

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🔹 2. Types of properties

Properties of substances are divided into two main types:

(A) Physical properties

• Can be seen or measured without changing the substance.
• No new substance is formed.

✳️ Examples:

• Colour (e.g., copper is reddish-brown)
• Odour (smell)
• Melting point (ice → water at 0°C)
• Boiling point (water boils at 100°C)
• Density (mass per unit volume)

⭐ Key point:

✔ Identity of substance remains the same
✔ Only physical form or state may change

📌 Example:

• Ice → Water → Steam (still H₂O, no new substance)

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(B) Chemical properties

• Can be observed only when a chemical change happens
• New substance is formed

✳️ Examples:

• Composition (what elements it contains)
• Combustibility (ability to burn)
• Reaction with acids and bases
• Reactivity with other substances

⭐ Key point:

✔ Identity of substance changes
✔ New substance is formed

📌 Example:

• Iron + Oxygen → Rust (iron oxide)
• Burning of magnesium → white ash (MgO)

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🔹 3. Important difference

Physical Properties	Chemical Properties
No new substance formed	New substance formed
No chemical change	Chemical change occurs
Easy to observe	Requires reaction
Example: melting, boiling	Example: burning, rusting

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🔹 4. Why do we study properties?

• Helps chemists:
  • Identify substances
  • Understand behavior of matter
  • Predict reactions
• Based on careful measurement and experiments

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🔹 5. Final summary (NEET revision line)

• Physical properties → change in form, no change in substance
• Chemical properties → change in substance, new product formed

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Here are line-by-line easy NEET-level notes for the topic 1.3.2 Measurement of Physical Properties:

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Line 1

“Quantitative measurement of properties is required for scientific investigation.”

• In science, we must measure things using numbers.
• This is necessary to do experiments and research properly.
• Without measurement, science cannot be accurate or reliable.

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Line 2

“Many properties of matter, such as length, area, volume, etc., are quantitative in nature.”

• Some properties of matter can be measured in numbers.
• Examples:
  • Length (how long something is)
  • Area (how much surface is covered)
  • Volume (how much space is occupied)
• These are called quantitative properties.

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Line 3

“Any quantitative observation or measurement is represented by a number followed by units in which it is measured.”

• Every measurement has two parts:
  1. A number (how much)
  2. A unit (what type of measurement)
• Example format: Number + Unit

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Line 4

“For example, length of a room can be represented as 6 m; here, 6 is the number and m denotes metre, the unit in which the length is measured.”

• Example: 6 m
  • 6 = numerical value
  • m (metre) = unit of length
• Without unit, the number has no meaning in science.

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Line 5

“Earlier, two different systems of measurement, i.e., the English System and the Metric System were being used in different parts of the world.”

• In the past, there was no single system worldwide.
• Two main systems:
  • English System (used in some countries)
  • Metric System (used in others)
• This caused confusion in science.

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Line 6

“The metric system, which originated in France in late eighteenth century, was more convenient as it was based on the decimal system.”

• Metric system started in France (late 1700s).
• It is easier because it uses base 10 system (decimal system).
• Example:
  • 1 km = 1000 m
  • 1 m = 100 cm

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Line 7

“Later, need of a common standard system was felt by the scientific community.”

• Scientists realized that:
  • Different systems caused confusion in communication
• So, they needed a single universal system.

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Line 8

“Such a system was established in 1960 and is discussed in detail below.”

• In 1960, a common system was introduced:
  • Called SI system (International System of Units)
• This system is now used worldwide in science and NEET exams.

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 1.3.3 The International System of Units (SI):

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📘 1.3.3 The International System of Units (SI)

🔹 What is SI System?

• SI stands for International System of Units.
• In French, it is called Le Système International d’Unités.
• It is the worldwide standard system of measurement used in science.

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🔹 Who established SI system?

• SI system was established by the 11th General Conference on Weights and Measures (CGPM).
• CGPM is a global organization that decides standard units.

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🔹 What is CGPM?

• CGPM = Conférence Générale des Poids et Mesures (French name).
• It is an inter-governmental treaty organization.
• It was formed under the Metre Convention.

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🔹 What is Metre Convention?

• It is an international agreement signed in 1875 in Paris.
• Its purpose is to maintain uniform measurement standards worldwide.

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📘 SI Units System

🔹 Basic idea

• SI system has 7 base units.
• These units represent 7 fundamental physical quantities.
• All other physical quantities are derived from these base units.

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📘 Seven Base Quantities and Units (Very Important for NEET)

Base Physical Quantity	Symbol	SI Unit	Symbol of Unit
Length	l	metre	m
Mass	m	kilogram	kg
Time	t	second	s
Electric current	I	ampere	A
Temperature	T	kelvin	K
Amount of substance	n	mole	mol
Luminous intensity	Iᵥ	candela	cd

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📘 Derived Quantities

• Many physical quantities are derived from base quantities.
• Examples:
  • Speed = distance/time (m/s)
  • Volume = length³ (m³)
  • Density = mass/volume (kg/m³)

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📘 Why SI system is important?

• It is universal (used in all countries).
• It ensures uniformity in scientific measurements.
• It avoids confusion in different unit systems.

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📘 National Standards of Measurement

🔹 Why standards are needed?

• Units can improve with time due to better technology and accuracy.
• So, definitions of units may be updated scientifically.

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🔹 Role of countries

• Every country has a National Metrology Institute (NMI).
• These institutes maintain standard units of measurement.

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🔹 Example in India

• India’s institute is NPL (National Physical Laboratory), New Delhi.
• NPL:
  • Defines and maintains SI base units
  • Conducts experiments to realize units
  • Maintains National Standards of Measurement

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🔹 International comparison

• National standards are compared regularly with other countries.
• Also compared with International Bureau of Weights and Measures (BIPM) in Paris.

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📌 NEET Quick Revision Points

• SI system = international standard system of units.
• Established by CGPM under Metre Convention (1875).
• 7 base quantities = length, mass, time, current, temperature, amount of substance, luminous intensity.
• India’s standard body = NPL (New Delhi).
• Other quantities are derived from base units.

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1.3.4 Mass and Weight (NEET Level Notes – Line by Line, Easy Understanding)

1. Mass of a substance is the amount of matter present in it.

• Mass means how much “stuff” (matter) is inside an object.
• Example: A stone has more matter than a pencil, so it has more mass.

2. Weight is the force exerted by gravity on an object.

• Weight is not matter; it is a force.
• It depends on how strongly Earth (or any planet) pulls the object downward.

3. The mass of a substance is constant.

• Mass never changes anywhere in the universe (Earth, Moon, space).
• Example: If a student has 50 kg mass on Earth, it is still 50 kg on the Moon.

4. Whereas, its weight may vary from one place to another due to change in gravity.

• Weight changes because gravity is different on different planets or places.
• Example: Weight on Moon is less than on Earth because gravity is weaker.

5. You should be careful in using these terms.

• Mass ≠ Weight (very important NEET concept).
• Students often confuse them in exams.

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Measurement of Mass

6. The mass of a substance can be determined accurately in the laboratory by using an analytical balance.

• In labs, mass is measured using a highly precise instrument called an analytical balance.
• It gives very accurate readings for small quantities of chemicals.

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SI Unit of Mass

7. The SI unit of mass is kilogram (kg).

• Standard unit used worldwide for mass.

8. However, its fraction named gram (1 kg = 1000 g) is used in laboratories.

• 1 kilogram = 1000 grams.
• Gram is used in labs because chemical substances are usually small in quantity.

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Key NEET Points (Quick Revision)

• Mass → amount of matter (constant)
• Weight → gravitational force (changes with gravity)
• SI unit of mass → kilogram (kg)
• Lab unit → gram (g)
• Instrument for mass → analytical balance

Here are line-by-line simple NEET-level notes for beginners based on your text:

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1.3.5 Volume – Easy Notes

• Volume means the amount of space occupied by a substance.
• It tells us how much space an object or liquid takes up.

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• Volume is a derived quantity because it depends on length.
• Its unit is (length)³.

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• In the SI system, the unit of volume is cubic metre (m³).

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• In chemistry laboratories, we usually deal with small quantities,
  so smaller units are used instead of m³.

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• Common small units of volume are:
  cubic centimetre (cm³) and cubic decimetre (dm³).

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Litre (L) – Important Unit

• A litre (L) is a commonly used unit for measuring liquids.
• It is not an SI unit, but widely used in chemistry.

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Conversions (Very Important for NEET)

• 1 L = 1000 mL
• 1 L = 1000 cm³
• 1 dm³ = 1 L

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Laboratory Instruments for Measuring Volume

• Graduated cylinder → used to measure volume of liquids approximately.
• Burette → used for accurate measurement in titrations.
• Pipette → used to transfer fixed, accurate volume of liquid.
• Volumetric flask → used to prepare a solution of exact known volume.

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Summary Idea

• Volume = space occupied
• SI unit = m³
• Lab units = cm³, dm³, L
• Instruments depend on accuracy required

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1.3.7 Temperature (NEET Notes)

1. What is Temperature?

• Temperature is the measure of how hot or cold a body is.
• It tells the degree of hotness or coldness of a substance.

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2. Common Temperature Scales

There are three main temperature scales:

• °C (Degree Celsius)
• °F (Degree Fahrenheit)
• K (Kelvin)

👉 These are used to measure temperature in different systems.

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3. SI Unit of Temperature

• The SI unit of temperature is Kelvin (K).
• Kelvin is the standard scientific unit used in physics.

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4. Celsius Scale (°C)

• Most commonly used in daily life and labs.
• Defined using water:
  • 0°C = Freezing point of water
  • 100°C = Boiling point of water
• So, Celsius scale is divided between 0 to 100 degrees for water phase change.

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5. Fahrenheit Scale (°F)

• Used mainly in some countries like the USA.
• Defined using water:
  • 32°F = Freezing point of water
  • 212°F = Boiling point of water
• So, Fahrenheit scale ranges from 32°F to 212°F for water.

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6. Relation between Celsius and Fahrenheit

• Conversion formula:

°C = \frac{5}{9}(°F - 32)

👉 Meaning:

• Subtract 32 from Fahrenheit
• Multiply by 5/9 to get Celsius

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7. Kelvin Scale (K)

• Kelvin is the absolute temperature scale.
• It starts from absolute zero.

Relation with Celsius:

K = °C + 273.15

👉 Meaning:

• Add 273.15 to Celsius to get Kelvin

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8. Important Concept: Negative Temperature

• In Celsius scale, temperature can be negative (e.g., -10°C).
• In Kelvin scale, temperature can NEVER be negative.
  • Because 0 K is the lowest possible temperature (absolute zero).

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9. Key Exam Points (NEET)

• SI unit: Kelvin (K)
• Freezing point:
  • 0°C = 32°F = 273.15 K
• Boiling point:
  • 100°C = 212°F = 373.15 K
• Kelvin scale has no negative values

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CBSE Class 11 complete question bank from “Properties of Matter and their Measurement” with MCQs, VSA, SA, LA, Assertion–Reason, Fill in the blanks, Case study, Statement-based, and Match the following.

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📘 1. MCQs (Multiple Choice Questions)

Q1. SI unit of mass is:

A) gram
B) kilogram
C) pound
D) Newton
✅ Answer: B) kilogram

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Q2. Weight of a body is:

A) Scalar quantity
B) Vector quantity
C) Fundamental quantity
D) Dimensionless
✅ Answer: B) Vector quantity

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Q3. Which is a physical property?

A) Rusting of iron
B) Burning of wood
C) Density
D) Digestion
✅ Answer: C) Density

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Q4. SI unit of temperature is:

A) °C
B) °F
C) Kelvin
D) Joule
✅ Answer: C) Kelvin

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Q5. Density is defined as:

A) mass × volume
B) mass / volume
C) volume / mass
D) force / area
✅ Answer: B) mass / volume

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✏️ 2. Very Short Answer Questions (1 mark)

Q1. What is matter?

Ans: Anything that has mass and occupies space is called matter.

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Q2. Define SI unit.

Ans: The standard unit system used internationally for measurements.

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Q3. What is weight?

Ans: Weight is the force exerted by gravity on a body.

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Q4. SI unit of density?

Ans: kg/m³

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Q5. What is volume?

Ans: Space occupied by a body.

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✏️ 3. Short Answer Questions (2–3 marks)

Q1. Differentiate between mass and weight.

Ans:

• Mass: Amount of matter in a body, SI unit kg, constant everywhere.
• Weight: Gravitational force on body, SI unit Newton, changes with gravity.

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Q2. Define physical and chemical properties.

Ans:

• Physical properties: Can be observed without changing substance (e.g., density, melting point).
• Chemical properties: Show ability to form new substances (e.g., rusting, burning).

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Q3. Write SI units of:

• Mass → kg
• Length → m
• Time → s
• Temperature → K

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Q4. Why is Kelvin scale used in science?

Ans: Because it is an absolute scale and has no negative values.

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📘 4. Long Answer Questions (5 marks)

Q1. Explain physical quantities and their measurement.

Ans:

• Physical quantity is something that can be measured.
• It has numerical value + unit.
• Example: length, mass, time, temperature.
• Measurement involves comparing with a standard unit.
• SI system ensures uniformity in measurement worldwide.

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Q2. Explain density and its importance.

Ans:

• Density = mass/volume
• SI unit = kg/m³
• It tells how tightly matter is packed.
• Helps in identifying substances.
• Example: oil floats on water due to lower density.

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⚖️ 5. Assertion and Reason

Q1.

Assertion (A): Weight of a body changes from place to place.
Reason (R): Gravitational acceleration varies on Earth.
✅ Answer: Both A and R are true, R is correct explanation.

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Q2.

A: Kelvin scale cannot have negative values.
R: Kelvin scale starts from absolute zero.
✅ Answer: Both true, R explains A.

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Q3.

A: Mass changes with location.
R: Mass depends on gravity.
❌ Answer: A is false, R is false.

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📝 6. Fill in the Blanks

Q1. SI unit of mass is ______

✅ kilogram

Q2. Density = ______ / volume

✅ mass

Q3. Kelvin scale starts from ______

✅ absolute zero

Q4. Weight is a ______ quantity

✅ vector

Q5. Temperature is measured in ______

✅ Kelvin

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📊 7. Case Study Based Questions

Case:

A student measures mass of a substance as 100 g and volume as 50 cm³.

Q1. Find density.

Ans: Density = mass/volume = 100/50 = 2 g/cm³

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Q2. SI unit of density?

Ans: kg/m³

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Q3. Is density a scalar or vector?

Ans: Scalar quantity

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Q4. If mass increases, density will:

A) increase
B) decrease
C) remain same
D) become zero
✅ Answer: A (if volume constant)

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📌 8. Statement Based Questions

Q1.

Statement 1: Mass is constant everywhere.
Statement 2: Weight depends on gravity.
✅ Both correct

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Q2.

Statement 1: Density depends on mass and volume.
Statement 2: Density is independent of temperature.
❌ Second is false

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🔗 9. Match the Column

Column A	Column B
Mass	kg
Weight	Newton
Density	kg/m³
Temperature	Kelvin

✅ Answers:

• Mass → kg
• Weight → Newton
• Density → kg/m³
• Temperature → Kelvin

Internal Links the 

/physics/properties-of-matter

/physics/physical-vs-chemical-properties

/physics/si-units-and-measurement

/physics/mass-vs-weight

/physics/density-explained

/physics/temperature-scales

/physics/measurement-of-physical-quantities

/class-11-physics/units-and-measurements

/Chemistry /all Chapter Full Index 

📘 Properties of Matter and their Measurement (NEET Mind Map)

1. Physical and Chemical Properties

• Physical properties: No new substance formed (color, density, melting point)
• Chemical properties: New substance formed (burning, rusting)

2. Measurement of Physical Quantities

• Physical quantities are expressed as Number + Unit
• Example: 6 m (6 = number, m = unit)
• Earlier systems: English & Metric
• Now SI system is used worldwide

3. SI Units

• SI = International System of Units
• Established by CGPM (1960)
• 7 Base quantities:
• Length (m), Mass (kg), Time (s), Temperature (K), Current (A), Mole (mol), Candela (cd)

4. Mass and Weight

• Mass: Amount of matter (constant), SI unit kg
• Weight: Force due to gravity (varies), unit Newton
• Mass measured using analytical balance

5. Volume

• Space occupied by a substance
• SI unit: m³
• Lab units: cm³, dm³, L
• 1 L = 1000 cm³ = 1 dm³
• Instruments: burette, pipette, measuring cylinder

6. Density

• Density = Mass / Volume
• SI unit: kg/m³
• Scalar quantity
• Helps identify substances

7. Temperature

• Measure of hotness or coldness
• SI unit: Kelvin (K)
• Scales: Celsius (°C), Fahrenheit (°F), Kelvin (K)
• Formulas:
• K = °C + 273.15
• °C = 5/9 (°F − 32)
• Kelvin has no negative values

Table 1.2: SI Base Units Definitions

Unit	Definition
Metre (m)	The metre is defined by taking the fixed numerical value of the speed of light in vacuum c to be 299,792,458 m s⁻¹, where the second is defined using the caesium frequency ΔνCs.
Kilogram (kg)	Defined by fixing the Planck constant h to 6.62607015 × 10⁻³⁴ J·s, where J = kg m² s⁻², with metre and second defined via c and ΔνCs.
Second (s)	Defined by the caesium-133 atom frequency ΔνCs = 9,192,631,770 Hz, where Hz = s⁻¹.
Ampere (A)	Defined by fixing the elementary charge e to 1.602176634 × 10⁻¹⁹ C, where C = A·s.
Kelvin (K)	Defined by fixing Boltzmann constant k to 1.380649 × 10⁻²³ J·K⁻¹, relating temperature to energy.
Mole (mol)	Contains exactly 6.02214076 × 10²³ elementary entities (Avogadro constant).
Candela (cd)	Defined by luminous efficacy Kcd = 683 lm·W⁻¹ at frequency 540 × 10¹² Hz.

Table 1.3: SI Prefixes

Multiple	Prefix	Symbol
10⁻²⁴	yocto	y
10⁻²¹	zepto	z
10⁻¹⁸	atto	a
10⁻¹⁵	femto	f
10⁻¹²	pico	p
10⁻⁹	nano	n
10⁻⁶	micro	µ
10⁻³	milli	m
10⁻²	centi	c
10⁻¹	deci	d
10	deca	da
10²	hecto	h
10³	kilo	k
10⁶	mega	M
10⁹	giga	G
10¹²	tera	T
10¹⁵	peta	P
10¹⁸	exa	E
10²¹	zetta	Z
10²⁴	yotta	Y