Electrons in Atoms Outline
Chapter 5: Electrons In Atoms
A. Models of the atom
i. The Development of Atomic Models
Protons and neutrons make up a nucleus surrounded by electrons
Rutherford’s model or theory ( figured electrons move around the nucleus)
His theory didn’t explain why metals or compounds of medals give off characteristics of colors when heated.
Also didn’t explain why the atomic model could not explain the chemical properties of elements ii. The Bhor Model
Bohr proposed that an electron is found in specific circular path, or orbits, around the nucleus.
Fixed energy’s (energy levels) lowest leval means the lowest level of energy.
Electrons can jump from one energy level to another(but when it jumps must gain or lose energy)
Quantum of energy is the amount of energy required to move an electron from one energy level to another.
The amount of energy an electron gains or loses ina na atom is not always the same.
The higher the energy level occupied by an electron, the less energy it takes to move from that energy level to the next higher energy level. iii. The Quantum Mechanical Model
The quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
There is no specific place where you can find an electron, they move around. iv. Atomic Orbits
An atomic orbit is often thought of as a region of space in which there is a high probability of finding an electron
For each principal energy level, there may be several orbits with different shapes and at different energy levels.
Each energy sublevel corresponds to an orbital of a different shape which describes where the electron is likely to be found
S orbital are spherical (circle), and p orbitals are dumbbell-shaped.
D orbitals have four clover leaf shapes.
# and kinds of atomic orbitals depends on the energy sublevel.
B. Electron Arrangement in Atom
i. Electron Configurations
The way in which electrons are
A. Models of the atom
i. The Development of Atomic Models
Protons and neutrons make up a nucleus surrounded by electrons
Rutherford’s model or theory ( figured electrons move around the nucleus)
His theory didn’t explain why metals or compounds of medals give off characteristics of colors when heated.
Also didn’t explain why the atomic model could not explain the chemical properties of elements ii. The Bhor Model
Bohr proposed that an electron is found in specific circular path, or orbits, around the nucleus.
Fixed energy’s (energy levels) lowest leval means the lowest level of energy.
Electrons can jump from one energy level to another(but when it jumps must gain or lose energy)
Quantum of energy is the amount of energy required to move an electron from one energy level to another.
The amount of energy an electron gains or loses ina na atom is not always the same.
The higher the energy level occupied by an electron, the less energy it takes to move from that energy level to the next higher energy level. iii. The Quantum Mechanical Model
The quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus
There is no specific place where you can find an electron, they move around. iv. Atomic Orbits
An atomic orbit is often thought of as a region of space in which there is a high probability of finding an electron
For each principal energy level, there may be several orbits with different shapes and at different energy levels.
Each energy sublevel corresponds to an orbital of a different shape which describes where the electron is likely to be found
S orbital are spherical (circle), and p orbitals are dumbbell-shaped.
D orbitals have four clover leaf shapes.
# and kinds of atomic orbitals depends on the energy sublevel.
B. Electron Arrangement in Atom
i. Electron Configurations
The way in which electrons are