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MindMap Gallery Chapter 5 Atomic Structure

Chapter 5 Atomic Structure

This is a mind map about Chapter 5 Atomic Structure. The main contents include: atomic structure and the periodic law of elements, the structure of multi-electron atoms, description of electron orbits within atoms, wave-particle duality of microscopic particles, human beings Understanding of atomic structure models.

Edited at 2024-10-18 19:47:27

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Chapter 5 Atomic Structure

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Outline

Chemistry - Atomic Structure
- 113
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Atomic structure and periodic system of elements
- 38
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structure of atom
- 19
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Basic Overview of Materials Chemistry
- 40
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Atomic structure
- 25
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Chapter 5 Atomic Structure

Human understanding of atomic structure models

Dalton - Atoms are indivisible

Thomson - jujube cake model

Rutherford - The nucleus is in the center and contains all of the atom's positive charge and mass. Electrons move in circles around the nucleus and carry a negative charge.

Planck's quantization theory and Bohr's atomic model - Planck's quantization theory: changes in physical quantities are discontinuous and consist of integer multiples of the smallest unit. Bohr atomic model: The energy of electron orbits in an atom is quantized. Electrons have a certain energy in a fixed energy level orbit. If they absorb or release fixed energy, they will jump in different energy level orbits.

Wave-particle duality of microscopic particles

Einstein's photoelectric effect

Photons have wave-particle duality

de Broglie

In addition to being particles, physical particles also have wave properties.

Davidson and Germer's electron diffraction experiments

A stream of electrons creates a ring-shaped diffraction image

Description of electron orbits within an atom

wave function

n: main quantum number, representing the number of electron layers

l: Angular quantum number, representing sub-layers of different states in the same electron layer

l=0: s spherical

l=1, p dumbbell type

l=3, d petal type

l=4, f multi-petal type

m: magnetic quantum number, representing the number of electrons that can be filled in the same sub-layer

m={-n 1<=m<=n-1}

ms: spin quantum number, representing the orientation of electron rotation

ms= 1\2,-1\2

Electrons are distributed in the form of electron clouds

The structure of a multi-electron atom

shielding effect

drill-through effect

Hundt's rule

Pauli Exclusion Principle

Atomic structure and periodic law of elements

periodic table of elements

The composition of the periodic table of elements

cycle

Divided according to energy level groups, elements in the same period have the same number of energy level groups

clan

According to the outermost electron beam classification, the outermost electron beams of the same family of elements are the same

district

Divided according to the energy levels filled by the outermost electrons

s area

p area

area d

ds area

…

The rules of the periodic table of elements

Ionization energy

The energy required for a ground state gaseous atom of an element to lose one electron and become a monovalent gaseous positive ion

Quantitatively reflects the ability of gaseous atoms of elements to lose electrons and compares the metallicity of elements.

The ionization energies of main group elements in the same period show an increasing trend from left to right, with abnormalities appearing in the second and third main groups and the fifth and sixth main groups.

The ionization energy of elements of the same family increases from top to bottom.

electronegativity

Compare the ease with which gaseous atoms of different elements gain and lose electrons

The periodic table of elements increases from left to right and from bottom to top.

Atomic orbital energy level diagram