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Atomic Structure and Chemical Bonding — Concept Maps
ICSE · Class 9 · Chemistry
4 concept maps of Atomic Structure and Chemical Bonding for ICSE Class 9 Chemistry, each also written out as a text outline.
42 questions44 flashcards4 formulas & key relations5 concepts
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4 Concept Maps
Atomic Structure and Chemical Bonding — Complete Concept Map
The map in words
- Atomic Structure and Bonding
- Sub-Atomic Particles
- Electron
- Charge minus 1
- Mass 1/1840 amu
- Outside nucleus
- Discovered by Thomson
- Proton
- Charge plus 1
- Mass 1 amu
- In nucleus
- Discovered by Goldstein
- Neutron
- Charge zero
- Mass 1 amu
- In nucleus
- Discovered by Chadwick
- Electron
- Atomic Models
- Thomson Plum Pudding
- Positive sphere
- Electrons embedded
- Rutherford Nuclear Model
- Dense positive nucleus
- Electrons orbit around
- Alpha scattering experiment
- Bohr Model 1913
- Fixed energy shells
- K L M N shells
- 2n squared rule
- Thomson Plum Pudding
- Key Numbers
- Atomic Number Z
- Equals protons
- Equals electrons
- Mass Number A
- Protons plus neutrons
- Neutrons
- Equals A minus Z
- Atomic Number Z
- Isotopes
- Same Z different A
- Hydrogen 3 isotopes
- Protium 0 neutrons
- Deuterium 1 neutron
- Tritium 2 neutrons
- Chlorine 2 isotopes
- Cl-35 ratio 75 percent
- Cl-37 ratio 25 percent
- Average mass of Cl = 35.5
- Chemical Bonding
- Octet Rule
- 8 electrons outermost shell
- Noble gas configuration
- Duplet Rule
- 2 electrons for H and He
- Ionic Bond
- Electron transfer
- Metal plus Non-metal
- NaCl MgCl2 CaO
- Covalent Bond
- Electron sharing
- Non-metal plus Non-metal
- Single Double Triple
- Octet Rule
- Sub-Atomic Particles
Atomic Structure — Complete Overview
The map in words
- Atomic Structure
- History
- Kanada 6th BC
- Paramanu concept
- Democritus 460 BC
- Atom meaning indivisible
- Dalton 1808
- First scientific theory
- Kanada 6th BC
- Sub-atomic Particles
- Electron
- Negative charge minus 1
- Mass 1 over 1840 amu
- Outside nucleus
- Thomson cathode rays
- Proton
- Positive charge plus 1
- Mass 1 amu
- Inside nucleus
- Goldstein canal rays
- Neutron
- No charge zero
- Mass 1 amu
- Inside nucleus
- Chadwick 1932
- Electron
- Atomic Models
- Thomson
- Plum pudding
- Rutherford 1911
- Dense nucleus
- Electrons orbit
- Cannot explain stability
- Bohr 1913
- Fixed energy shells KLMN
- No energy loss in orbit
- Explains stability
- Thomson
- Atomic Numbers
- Atomic number Z
- Protons equals electrons
- Mass number A
- Protons plus neutrons
- Neutrons equals A minus Z
- Atomic number Z
- Electronic Configuration
- Rule 2n squared
- K shell 2 max
- L shell 8 max
- M shell 18 max but outermost max 8
- Isotopes
- Same Z different A
- Same chemical properties
- Different physical properties
- Examples H C Cl
- History
Complete Chapter Concept Map: Atomic Structure and Chemical Bonding
The map in words
- root（（Atomic Structure
- and Chemical Bonding））
- Sub-atomic Particles
- Electron
- Discovered by Thomson
- Charge minus 1
- Mass 1 by 1840 amu
- Proton
- Discovered by Goldstein
- Charge plus 1
- Mass 1 amu
- Neutron
- Discovered by Chadwick
- No charge
- Mass 1 amu
- Electron
- Atomic Models
- Dalton Model
- Indivisible atom
- Thomson Model
- Plum Pudding
- Rutherford Model
- Nuclear Model
- Electrons in orbits
- Bohr Model
- Fixed energy shells
- K L M N shells
- Dalton Model
- Atomic Number and Mass Number
- Atomic Number Z
- Number of protons
- Number of electrons
- Mass Number A
- Protons plus neutrons
- Neutrons
- A minus Z
- Atomic Number Z
- Electronic Configuration
- 2n squared rule
- Shell capacities
- Bohr Bury Scheme
- Valence electrons
- Octet Rule
- Noble gases stable
- 8 electrons in valence shell
- Duplet for H and He
- Drives chemical bonding
- Isotopes
- Same Z different A
- Differ in neutrons
- Hydrogen isotopes
- Protium
- Deuterium
- Tritium
- Carbon isotopes
- C 12 C 13 C 14
- Chlorine isotopes
- Cl 35 Cl 37
- Fractional atomic mass
- Chemical Bonding
- Electrovalent Bond
- Electron transfer
- Metal to non-metal
- Cation formed
- Anion formed
- NaCl MgCl2 CaO
- Covalent Bond
- Electron sharing
- Non-metal to non-metal
- Single bond
- H2 HCl CH4
- Double bond
- O2
- Triple bond
- N2
- Non-polar molecules
- H2 Cl2 CCl4
- Polar molecules
- HCl H2O NH3
- Electrovalent Bond
- Sub-atomic Particles
Atoms form the basis of matter, and chemical bonding explains how atoms combine to become stable
The map in words
- Atoms form the basis of matter, and chemical bonding explains how atoms combine to become stable
- Historical ideas about matter
- Sub-atomic particles
- Discovery of particles
- Atomic models
- Atomic number and mass number
- Electron distribution
- Valence electrons and valency
- Octet and duplet rule
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Explore DiagramsFrequently Asked Questions
What are the important topics in Atomic Structure and Chemical Bonding for ICSE Class 9 Chemistry?
Key topics in Atomic Structure and Chemical Bonding include Early ideas and discovery of subatomic particles, Structure of the atom, Fundamental particles of the atom, Atomic models and discovery of nucleus. Study these first, then practise questions on each for Class 9 exams.
What do the concept maps for Atomic Structure and Chemical Bonding show?
The 4 maps show how the ideas in Atomic Structure and Chemical Bonding connect: Atomic Structure and Chemical Bonding — Complete Concept Map; Atomic Structure — Complete Overview. Each map is also written out as an outline on this page.
How should I revise Atomic Structure and Chemical Bonding for Class 9 exams?
Learn the core ideas first, then work through the 42 practice questions on Atomic Structure and Chemical Bonding. Revise definitions regularly and use flashcards for quick recall before the exam.
Sources & Official References
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Practice Quiz
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Important Questions
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Revision Notes
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Formula Sheet
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Chapter Summary
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Study Plan
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Flashcards
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Syllabus
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