Who has a lesson plan for high school chemistry elective 3?

Or teaching objectives, the specific content of the lesson plan includes the following ten items. (2) Teaching a new lesson 1 Choose different teaching methods for different teaching contents, which include the following steps: 1. Topic (explain the name of the lesson) 2. Teaching purpose (or teaching requirements, concise generalization, and explain the tools used in auxiliary teaching methods) in the process of writing the lesson plan.

3 Ask questions about the students and have density: (1) Introduce a new lesson 1 The design is novel and lively, and explain the teaching tasks to be completed in this lesson) 3 Lesson type (explain that it is a new teaching, the teaching process is the key, there are levels, and explain the content and ability of teaching, or a review class) is hidden 4 Lesson time (explain the number of lesson hours) 5 Teaching focus (explain the key problems that must be solved in this lesson) 6 Teaching difficulties (explain the knowledge points that are prone to difficulties and obstacles in the learning of this lesson) 7 Teaching process (or classroom structure, Method steps) 9 board book design (explain the content to be written on the blackboard during class) 10 teaching aids (or teaching aids preparation, to consider the expansion of knowledge, how much time is needed, etc., there is a slope. (3) Consolidation Exercise 1 The exercise is well-designed.

4) Summarize and (5) Arrange and assign those contents of the assignment.

The three knowledge points of high school chemistry elective three are atomic structure and properties, molecular structure and properties, crystal structure and properties, atomic structure and properties of elements, molecular crystals and atomic crystals, and the three-dimensional structure of molecules.

Chapter 1 Atomic Structure and Properties.

Section 1 Atomic Structure.

Section 2 Atomic Structure and Properties of Elements.

Chapter 2 Molecular Structure and Properties.

Section 1 Covalent bonds.

Section 2 Three-dimensional structure of molecules.

Section 3 Destruction of the nature of the molecule.

Chapter 3 Crystal Structure and Properties.

Section 1 Common sense of crystals.

Section 2 Molecular Crystals and Atomic Crystals.

Section 3 Metal Crystals.

Section 4 Ionic crystals.

Ion coexistence, ion sorting, ion coexistence is actually very easy to do, precipitation, gas, double hydrolysis, weak electrolyte, complexes, redox, whether there is color, pH, these few sieves can be selected in a circle, if you are not proficient, it can only mean that the question is not enough (no way, this piece is more brushed to brush the question is familiar), this piece is really simple. Ion coexistence is simple, but ion sorting is a big problem, and it can be said to be one of the most difficult knowledge points to understand in the whole high school.

I don't think I understand this, at least not as well as the school teachers. All I can say is that you must make good use of the three conservations, which can solve almost all the problems of ion concentration sequencing. Also, we must have a vague idea of the approximate concentration.

What do you mean? Let's say you have ammonia, the pH is about 11, and now if you want to rank the particles in the solution, you first have to think about the concentration of each substance.

NH3·H2O is weakly electrolytically retarded, so the concentration is slightly less, pH is 11, so OH- is, the difference between the two is 100 times, and then NH3·H2O>OH->NH4+>H+ can be written by using charge conservation. Why build a concept of approximate concentration? Because when there is some inaccurate order, you can roughly judge by this.

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.