Virtual Lab - Ionic bond simulator

IONIC BOND FORMATION

Spin the Ions and Form Compounds

Explore how positive and negative ions combine to form ionic compounds.

STUDENT INSTRUCTIONS

1. Spin the positive ion wheel.
2. Spin the negative ion wheel.
3. Observe the selected ions.
4. Click Form Ionic Compound.
5. Observe the compound formula and name.
6. Click Explain Formation to understand charge balancing.
7. Click Listen to hear the correct compound name.

Positive Ions

Selected positive ion

Negative Ions

Selected negative ion

FORMATION OF IONIC COMPOUND

+

−

Select ions from both wheels.

IMPORTANT CHEMISTRY CONCEPTS

Cation

A positively charged ion formed by losing electrons.

Example: Na⁺

Anion

A negatively charged ion formed by gaining electrons.

Example: Cl⁻

Ionic bond

Electrostatic attraction between oppositely charged ions.

Charge balancing

Total positive charge must equal total negative charge.

Polyatomic ions

Groups of atoms carrying an overall charge, such as NO₃⁻ and SO₄²⁻.

Formula writing

Write the simplest whole-number ratio of ions. Use parentheses for multiple polyatomic ions.

TEST YOUR UNDERSTANDING

Score: 0

Interactive Chemistry Learning Laboratory

script async src="https://pagead2.googlesyndication.com/pagead/js/adsbygoogle.js?client=ca-pub-7234129978809365" crossorigin="anonymous">

Read More

Virtual Lab - Place values - Interactive way

🔢 INDIAN PLACE VALUE EXPLORER

Discover the Value of Every Digit!

Interactive Mathematics Learning Simulation

📘 Instructions to Students

1. Enter any whole number in the input box.
2. Click the Show Place Values button.
3. Observe how the digits move into separate boxes.
4. Listen to the sound as each digit enters its box.
5. Click any digit to discover its place and place value.
6. Listen to the audio explanation by clicking the Speak button.
7. Observe the expanded form of the number.
8. Click another digit to explore its place value.

✏️ Enter Your Number

🎯 Digit Place Value Boxes

Click any digit box to explore its place value.

🔍 Explore Your Selected Digit

📚 Indian Number System

Ones Tens Hundreds Thousands Ten Thousands Lakhs Ten Lakhs Crores Ten Crores Arab Ten Arab Kharab

🧠 Expanded Form

Enter a number to see its expanded form.

💡 Remember

Face Value: The digit itself, irrespective of its position.
Place Value: The value of a digit according to its position in a number.

Interactive Learning Resource | Ready To Learn Hub

Read More

Virtual Lab - Double Displacement Reaction

🧪 CHEMISTRY LAB SIMULATION

Formation of Yellow Precipitate – Lead Iodide

1. Select the Concentration

🟦 Potassium Iodide (KI)

Colourless aqueous solution

Concentration: 0.50 M Volume: 20 mL

Not added

🧪 Lead(II) Nitrate

Pb(NO₃)₂ – Colourless aqueous solution

Concentration: 0.50 M Volume: 20 mL

Not added

2. Observe the Experiment

Laboratory apparatus

KI solution

Pb(NO₃)₂

Test tube

Waiting for solutions...

3. Experimental Observation

Add both solutions and click MIX to observe the reaction.

Precipitate: Not formed yet

Limiting reactant: Not calculated

4. Chemical Equation

2KI(aq) + Pb(NO₃)₂(aq)
↓
PbI₂(s) + 2KNO₃(aq)

Net ionic equation

Pb²⁺(aq) + 2I⁻(aq) → PbI₂(s) ↓

Observation: A bright yellow precipitate of lead(II) iodide is formed.

5. Test Your Understanding

Which compound is responsible for the yellow precipitate?

6. Important Safety Note

Lead compounds are toxic. This experiment is intended as a digital simulation. Do not handle lead nitrate or lead-containing waste without appropriate laboratory safety procedures and trained supervision.

Designed for Science Learning | Ready To Learn Hub

Read More

Virtual Lab - Quantum numbers

⚛ QUANTUM NUMBERS LABORATORY

Explore orbitals • Select electrons • Discover all four quantum numbers

🔬 1. Select Your Orbital and Electron

Select Orbital / Subshell 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p

Select Electron Number

Important: Select a subshell first. Then select the electron number in that subshell. The simulation follows Hund's rule and the conventional left-to-right orbital-box order.

🎯 2. Orbital Box Diagram

Select an orbital to begin.

Select an electron to see its position in the orbital.

🌈 3. All Four Quantum Numbers

Principal Quantum Number ? n – Main energy level

Azimuthal Quantum Number ? l – Subshell shape

Magnetic Quantum Number ? mₗ – Orbital orientation

Spin Quantum Number ? mₛ – Electron spin

The four quantum numbers will appear here automatically.

📘 4. Understand the Four Quantum Numbers

Principal quantum number (n)
It indicates the main energy level or shell of an electron. Its values are 1, 2, 3, 4 and so on.

---

Azimuthal quantum number (l)
It indicates the subshell. For s, l = 0; for p, l = 1; for d, l = 2; for f, l = 3.

---

Magnetic quantum number (mₗ)
It indicates the orbital orientation. Its values range from minus l to plus l, including zero.

---

Spin quantum number (mₛ)
It indicates the spin of the electron. Its possible values are plus one-half and minus one-half.

🧠 5. Quantum Number Practice

Test your understanding with automatically generated questions.

📌 6. Important Rules to Remember

Rule 1: The value of n is always a positive integer.
Rule 2: The value of l ranges from 0 to n − 1.
Rule 3: The value of mₗ ranges from −l to +l.
Rule 4: The value of mₛ is either +1/2 or −1/2.
Rule 5: Each orbital can accommodate a maximum of two electrons with opposite spins.
Rule 6: According to Hund's rule, electrons occupy degenerate orbitals singly with parallel spins before pairing.

Interactive Chemistry Learning Laboratory
Learn • Explore • Experiment • Understand

Read More

Virtual Lab - - Electronic configuration

⚛ ELECTRONIC CONFIGURATION VIRTUAL LAB

Explore the First 30 Elements

Discover how electrons occupy atomic orbitals through five colourful interactive simulations. Observe electron filling, spin directions, orbital capacities and electronic configurations.
Learn by watching, listening and experimenting!

SELECT ELEMENT

FIVE INTERACTIVE SIMULATIONS

1. Aufbau Principle

2. Hund's Rule

3. Pauli's Principle

4. Shell Distribution

5. Valence Electrons

AUFBAU PRINCIPLE

ANIMATED ELECTRON FILLING

Blue arrow = Spin up | Red arrow = Spin down

Electrons filled: 0

ELECTRONIC CONFIGURATION

1s⁰

Ground-state electronic configuration

STEP-BY-STEP LEARNING

Select an element and start the simulation.

SHELL-WISE ELECTRON DISTRIBUTION

ELEMENT ANALYSIS

Atomic Number6

Total Electrons6

Valence Electrons4

Occupied Shells2

ORBITAL CAPACITY REFERENCE

s subshell2 electrons

p subshell6 electrons

d subshell10 electrons

f subshell14 electrons

s = 1 orbital | p = 3 orbitals | d = 5 orbitals | f = 7 orbitals

TEST YOUR KNOWLEDGE

SIMULATION COMPLETE

Complete the electron filling to see your result.

Read More

Interactive Simulation -Rules to write Electronic configuration

⚛ ELECTRONIC CONFIGURATION LAB

Aufbau Principle | Hund's Rule | Pauli's Exclusion Principle

Explore how electrons are distributed in different atomic orbitals. Select an element and watch electrons enter the orbitals step by step.

1. Aufbau Principle

Electrons occupy orbitals in the increasing order of their energies. Lower-energy orbitals are filled first.

2. Hund's Rule

Electrons occupy orbitals of equal energy singly with parallel spins before pairing begins.

3. Pauli's Exclusion Principle

An orbital can accommodate a maximum of two electrons, and they must have opposite spins.

SELECT AN ELEMENT

Hydrogen (H) - 1 Helium (He) - 2 Lithium (Li) - 3 Beryllium (Be) - 4 Boron (B) - 5 Carbon (C) - 6 Nitrogen (N) - 7 Oxygen (O) - 8 Fluorine (F) - 9 Neon (Ne) - 10 Sodium (Na) - 11 Magnesium (Mg) - 12 Aluminium (Al) - 13 Silicon (Si) - 14 Phosphorus (P) - 15 Sulphur (S) - 16 Chlorine (Cl) - 17 Argon (Ar) - 18 Potassium (K) - 19 Calcium (Ca) - 20

ELEMENT INFORMATION

Electrons filled: 0

ORBITAL FILLING DIAGRAM

Blue arrow: Spin up (↑) | Red arrow: Spin down (↓)

ELECTRONIC CONFIGURATION

Select START SIMULATION

STEP-BY-STEP EXPLANATION

Start the simulation to observe the electron-filling process.

ENERGY ORDER OF ORBITALS

1s → 2s → 2p → 3s → 3p → 4s

Orbitals are filled in increasing order of energy.

TEST YOUR UNDERSTANDING

Which principle states that lower-energy orbitals fill first?

Read More

Spin and Learn - Elements, Acids, Bases and Salts

Interactive Chemistry Spinning Wheels

Explore chemical elements, acids, bases and salts through colourful spinning wheels. Learn their names, symbols, atomic numbers and uses through audio narration.

How to use: Choose a wheel from the index and press SPIN. Watch the fixed red arrow. The item selected by the arrow will be displayed and narrated after the wheel stops.

INDEX 1 – CHEMICAL ELEMENTS

INDEX 2 – ACIDS, BASES AND SALTS

Read More