All substances are made of tiny particles called "ATOM"
Electrons
Negatively charge subatomic particles
Electrons
J. J. Thomson was the first person to accurately calculate the mass and the charge of an electron
Protons
Positively charge subatomic particles
Protons
Discovery of protons is credited to Earnest Rutherford
Neutrons
Neutrally charged subatomic particles
Neutrons
Discovered by James Chadwick in 1932
Quantum Mechanical Model
Louie de Broglie (1924) proposed that the electron could also be thought of as a wave
Quantum Mechanical Model
Erwin Schrodinger used the wave idea to develop a mathematical equation to describe the hydrogen atom
Quantum Mechanical Model
Werner Karl Heisenberg discovered that for a very small particle like the electron, its location cannot be exactly known and how it is moving
Uncertainty Principle
It is impossible to locate the exact position of an electron at any given time (too small, too fast)
Atomic orbital
The volume or region of space around the nucleus where the electron is most likely to be found
Electron Orbit Model
Electrons were thought to orbit around the nucleus in defined paths
Electron Cloud Model
Discovered that electrons move in waves in a defined space called an electron cloud
Quantum Numbers
Principal quantum number
Angular momentum quantum number
Magnetic Quantum Number
Electron Configuration
The electron configuration of a certain element consists of three Quantum Numbers
Octet Rule | Valence Electron | Lewis Dot Structure (LDS)
Chemical Bonding
Chemical bonding refers to the formation of a chemical bond between two or more atoms, molecules, or ions to give rise to a chemical compound
Ionic Bonding
Formed between Metal and a Nonmetal
Covalent Bonding
Bonding is common between two nonmetals
Ions
Uneven numbers of protons and electrons which results in an overall positive or negative charge
Types of Ions
Cation (positive charge)
Anion (negative charge)
Octet Rule
It refers to the tendency of atoms to prefer to have eight electrons in the valence shell
Valence Electron
Electrons in the outermost (valence) principal energy level of an atom that can participate in the formation of chemical bonds with other atoms
Periodic Table Groups
Group 1 (I) -alkali metals
Group 2 (II) - alkaline earth metals & He
Group 3-12 (transition metals)
Group 13 (III) - boron group
Group 14 (IV) - carbon group
Group 15 (V) - nitrogen group
Group 16 (VI) - oxygen group
Group 17 (VII) - halogen
Group 18 (VIII) - noble gases except Helium
Lewis Dot Structure (LDS)
Lewis dot structures (LDS) are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule
Covalent Bonding
The formation of compound also involves sharing of electrons, thus resulting in a covalent bonding
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Atom
Tiny particles that all substances are made of
Electrons
Negatively charged subatomic particles
J.J. Thomson was the first to accurately calculate the mass and charge of an electron
Protons
Positively charged subatomic particles
Discovery of protons is credited to Ernest Rutherford
Neutrons
Neutrally charged subatomic particles
Discovered by James Chadwick in 1932
Quantum Mechanical Model
Model of the atom where the electron can be thought of as a wave (proposed by Louis de Broglie)
Erwin Schrodinger developed a mathematical equation to describe the hydrogen atom
Werner Heisenberg discovered the Uncertainty Principle - the exact position and motion of an electron cannot be known
Atomic Orbital
The volume or region of space around the nucleus where the electron is most likely to be found
Electron Orbit Model
Electrons were thought to orbit around the nucleus in defined paths
Electron Cloud Model
Electrons move in waves in a defined space called an electron cloud
Quantum Numbers
Principal quantum number
Angular momentum quantum number
Magnetic quantum number
Electron Configuration
The arrangement of electrons in an atom's orbitals
Chemical Bonding
The formation of a chemical bond between two or more atoms, molecules, or ions to give rise to a chemical compound
Octet Rule
The tendency of atoms to prefer to have eight electrons in the valence shell