MindMap Gallery Atomic structure and periodic system of elements
A general overview of atomic structure and the periodic system of elements, including the periodicity of atomic structure and element properties, the arrangement of electrons outside the nucleus, etc.
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This is a mind map about bacteria, and its main contents include: overview, morphology, types, structure, reproduction, distribution, application, and expansion. The summary is comprehensive and meticulous, suitable as review materials.
This is a mind map about plant asexual reproduction, and its main contents include: concept, spore reproduction, vegetative reproduction, tissue culture, and buds. The summary is comprehensive and meticulous, suitable as review materials.
This is a mind map about the reproductive development of animals, and its main contents include: insects, frogs, birds, sexual reproduction, and asexual reproduction. The summary is comprehensive and meticulous, suitable as review materials.
Atomic structure and periodic system of elements
Periodicity of atomic structure and elemental properties
1. Effective nuclear charge
·The same period: the larger z is, the more significant the increase in effective nuclear charge is.
·Same family: from top to bottom, the increase decreases
2. Radius
·The same period: the effective nuclear charge increases, the number of electron layers remains unchanged, and the radius becomes smaller
·Same family: from top to bottom, the radius increases
3. Ionization energy
·Definition: The energy consumed (absorbed) when a gaseous atom of an element loses an electron in its ground state and becomes a monovalent gaseous positive ion.
·Influencing factors: atomic radius, effective nuclear charge, outer nuclear electron layer structure
·Change rules
The same cycle: from left to right, ionization energy increases
Same family: from top to bottom, ionization energy decreases
4. Electron affinity
·Definition: The energy released when a gaseous atom of an element acquires an electron in its ground state and becomes a monovalent negative ion.
·Influencing factors: atomic radius, effective nuclear charge, outer nuclear electron layer structure
·Change rules
In the same cycle: from left to right, electron affinity increases
Homologous group: from top to bottom, electron affinity decreases
5. Electronegativity
·The same cycle: from left to right, electronegativity increases
·Same family: from top to bottom, electronegativity decreases
6. Metallic and non-metallic properties of elements
·Metallicity of an element: The smaller the electronegativity or the smaller the ionization energy, the stronger the metallicity.
·Non-metallic property of an element: The greater the electronegativity or the greater the electron affinity, the stronger the non-metallic property.
The arrangement of electrons outside the nucleus
1. Energy level diagram
2. Electronic arrangement rules outside the nucleus
·The principle of minimum energy
·Pauli Exclusion Principle
·Hunt Rules
·Supplementary rules to Hundt’s rules
3. Representation of electron configuration outside the nucleus
·Electronic layout
·Valence shell electron configuration table
·Atomic real expressions
Characteristics of electron movement
1.Quantization
2. Uncertainty
3. Statistical
Modern description of electron motion outside the nucleus
1.Schrödinger equation
2. Wave function and atomic orbitals
·Atomic orbital angle distribution diagram
3. Probability density and electron cloud
·Probability density: The probability of an electron appearing in a unit volume somewhere outside the nucleus is called the probability density there.
·Shell probability: probability density at r*shell volume
·Electron cloud angle distribution map
four quantum numbers (Note: Three quantum numbers result in a wave function)
·Principal quantum number (n): the main factor that determines the energy of electrons
·Angular quantum number (l)
·Magnetic quantum number (m): describes the extension direction of atomic orbitals in space
·Spin quantum number (ms)
bohr theory
1. Layered distribution of electrons within atoms
2 Energy discontinuity between energy levels (quantization)
3. Energy changes occur only when energy levels transition.