What are the important knowledge points of Chemistry Option 3?

Elective three, newly added, seems complicated, but it is not difficult, say ideals, say results, look forward to students, and work hard.

Large**, atomic, a small amount of helium, a large amount of hydrogen, atoms, see electrons, energy difference, divided into seven layers, energy layer, energy levels, number orbitals, electron addition, Pauli, two anti, Hunt rule, separate occupation, tectonic theory, electron discharge, chromium and copper, all not from, one and a half, one full, for the exception, low energy, excited state, variable ground state, electron migration, light presentation, spectrometer, absorption and discharge, new element, old element, electronic line, irregular, electron cloud, is probability, one hundred and ninety, different shape, s ball, p dumbbell.

Basis atom, electron row, de-0 group, valence electricity, valence electrons, look at the law, periodic table, divided into five regions, ds, d close together, s p, keep both sides, f block, unimportant, contain lanthanum actinium, need to know, periodic law, look at change, ionization energy, electronegativity, specific radius, two factors, energy layer, charge number.

covalent bonds, junction molecules, electron pairs, for sharing, electron clouds, ball dumbbells, according to overlapping, split bond type, sigma, head meeting, overlapping large, bond stable, p p, shoulder to shoulder, to appear, bond two three, bond parameters, can long angle, stable or unstable, can size, the longer the bond, the smaller it can be, molecular shape, look at the bond angle, valence primitive, isoelectric, similar in nature, new principle.

There are many molecules, different shapes, valence layer repulsion, seeking stability, a b n, looking at the central plain, bond holland, n definitive, intramolecular, hybridization, lone electric pairs, sigma, complexes, new bonds, concentrated and dilute, color change, ligands, metals, few main groups, and abundant transitions.

Soluble or insoluble, look at polarity, non-polarity, electric centering, intermolecular, force on both sides, van der Waals, and hydrogen bonds, chiral carbon, four bonds, all different, starting with, oxygen-containing acid, specific acidic, non-hydroxyxyl, oxygen hydrogen reduction.

Amorphous, very small, glass, and rubber, crystals, three pathways, crystallization, two kinds of condensation, self-norm, polyhedron, diffraction, anisotropy, polymorphic, hexahedron, need to be juxtaposed, and no gaps.

Molecular crystals, very common, mostly gas, five types of judgment, high coordination, dense packing, small hardness, low melting.

Atomic, covalent bond, high melting and boiling, good hardness.

Electronic gas, metal crystal, thermoelectric, malleable, simple vertical, and k-type, densely packed, mg and cu.

Mixed crystal, graphite, carbon profile, and triadic.

Ionic crystals, lattice energy, look at charge, specific radius, one geometry, two charges, two factors, coordination number.

Ride the long wind, break the waves, accumulate steps, on the peak, those who have aspirations, things can be done, learn and think, and be persistent.

Chemistry Elective 3 is the structure of matter, which involves the knowledge of inorganic chemistry in college, mainly the atomic structure, energy layer, energy level, electron Echizen, etc., and the principles involved are the principle of energy minimum, Hunt's rule and Pauli's principle.

Elective 3 Chapter 1 Atomic Structure and Properties.

This chapter explains. Section 1 Atomic Structure.

Section 2 Atomic Structure and Properties of Elements.

Teaching Resources 1 Teaching Resources 2

Chapter 2 Molecular Structure and Property Units.

This chapter explains. Section 1 Covalent bonds.

Section 2 Three-dimensional structure of molecules.

Section 3 Properties of Molecules.

Teaching Resources 1 Teaching Resources 2

Teaching Resource 3 Chapter 3 Crystal Structure and Properties.

This chapter explains. Section 1 Common sense of crystals.

Section 2 Molecular Crystals and Atomic Crystals.

Section 3 Metal Crystals.

Section 4 Ionic crystals.

Teaching Resources 1 Teaching Resources 2

Chapter 1 Atomic Structure and Properties.

This chapter explains. Section 1 Atomic Structure.

Section 2 Atomic Structure and Properties of Elements.

Teaching Resources 1 Teaching Resources 2

Chapter 2 Molecular Structure and Property Units.

This chapter explains. Section 1 Covalent bonds.

Section 2 Three-dimensional structure of molecules.

Section 3 Properties of Molecules.

Teaching Resources 1 Teaching Resources 2

Teaching Resource 3 Chapter 3 Crystal Structure and Properties.

This chapter explains. Section 1 Common sense of crystals.

Section 2 Molecular Crystals and Atomic Crystals.

Section 3 Metal Crystals.

Section 4 Ionic crystals.

Section 1 Atomic Structure and Properties.

Test Center 1: Electron Configuration Law and Representation Method Outside the NucleusTest Point 2: Atomic Structure and Periodic Table.

Test Center 3: Periodic Law of Elements.

Section 2 Molecular Structure and Properties.

Test Center 1 Covalent bonds.

Test Center 2: Three-dimensional configuration of molecules.

Test 3 Properties of molecules.

Test site 4: Bonding and spatial structure of common molecular compounds.

Section 3 Crystal Structure and Properties.

Test Center 1 Several typical crystal models.

Test Center 2 Determination of crystal type and comparison of melting and boiling point Test point 3 Calculation of the number of particles in the unit cell.

Test Center 4: Comparison of several groups of typical unit cell structures.

From the ionization equation, it can be seen that both the Al element and the F element appear as a whole.

From the perspective of crystal structure, since yin and yang must be alternating structures, they must be cations.

In the crystal structure, the number of · is taken from the vertex and the center of the face, then there is a total of: 8 +6 = 4.

The number of in the crystal structure: take the midpoint of the prism and take the point of the center of the body as 1, then there is a total: 12 + 8 1 = 12.

Since the number of · = 1 3, ·is, is na+.

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<> the basic knowledge of this question, the question is too poor, the blank is ambiguous, I barely wrote it, there should be mistakes, the exam will not test you like this.