chemistry lesson

Credit on the topic "non-Metals" - SUBSTANCES AND their PROPERTIES - LESSON PLANS for CHEMISTRY 11 class - lesson plans-lesson plans-author's lessons-plan-lesson summary - chemistry

Lesson objectives: test your knowledge and skills on the topic "non-Metals".

Equipment: task cards with two options.

Lesson progress

I. Organizational moment

Instructing students about the progress of the test tasks. Recommendation to the teacher

At the time of completing the test, the teacher checks the performance of homework in workbooks, setting grades.

II. Performing credit cards-tasks with two options

Answers to test questions

Option I

At the external energy level, there are seven electrons, three pairs of paired ones and one pair of unpaired ones. The level is close to completion, one electron is taken until stability; chlorine shows a C. o. -1, +1 in the ground state. At the chlorine atom, it is possible to open a 3d sublevel in the state of excitation. It is possible to steam 3P_x, 3P_y, 3s-electrons. Chlorine exhibits:

S. O. +3 (first excitement);

S. O. +5 (second excitement);

C. O. +7 (the third initiation).

2. In ascending order of nemetallicheskie I, Br, Cl, F. These are elements of group VII, the main subgroup. Nonmetallicity increases to the beginning of the group, the main subgroup, because the radius of the atom decreases the number of electrons at the external energy level does not change.

3. Boron, hydrogen, and iodine are covalent nonpolar bonds. Boron is an atomic crystal lattice. Hydrogen, iodine-a molecular crystal lattice.

4. Chlorine has an impossible allotrope, as the chlorine atom single unpaired electron.

A carbon atom has four unpaired electrons in its excited state. Allotropy is possible in the form of: diamond-SP³-hybridization, graphite-SP²-hybridization, carbine-sp-hybridization.

6. a) HCl and H₂S — hydrogen compounds of elements of the III period of hydrogen compounds, the acidic properties are enhanced by the end of the period

HCl as an acid is stronger than H₂S.

b) S⁺⁴O₂and S⁺⁶O₃-salt-forming oxides. S. o. at sulfur in SO₂+4, at sulfur in SO₃+6; the higher the PH, the more pronounced the acidic properties of the oxide. Thus, the acidic properties of SO₃are stronger than the acidic properties of SO₂.

C) H₂S⁺⁶About₄and NSl⁺⁷About₄oxygen-containing acids are formed by elements-nonmetals located in the III period. The strength of oxygen-containing acids increases towards the end of the period.

NSl⁺⁷O₄is stronger than H₂S⁺⁶O₄. C. O. Sl⁺⁷is greater than C. O. S⁺⁶, the radius of the ion CL⁺⁷is less than the radius of the ion S⁺⁶.

7. the Main properties of NH₃are more pronounced than H₂O, since the dorsal joints are formed by elements N and Olocated in the II period. The main properties weaken by the end of the period, because the COC increases and the radius of the nonmetal ion decreases.

Option II

At the external energy level, there are six electrons, two pairs of paired and two pairs of unpaired ones. The level is close to completion, two electrons are taken before stability. Sulfur shows C. O. in the basic state -2; +2.

At the sulfur atom, it is possible to open a 3d sublevel, and in the state of excitation, it is possible to steam 3P_x, 3s electrons. Sulfur manifests:

S. O. +4 (first excitement); S. O. +6 (second excitement).

2. In descending order of nemetallicheskie P, S, Cl, Si. These are elements of the third period. By the end of the period nemetallicheskie is enhanced, and the beginning of the period decreases, increasing atomic radius decreases as the nuclear charge of the atom decreases the number of electrons in the outer energy level.

the decrease of nemetallicheskie

3. Diamond, bromine, oxygen-covalent nonpolar bond.

Diamond is an atomic crystal lattice.

Bromine, oxygen-a molecular crystal lattice.

4. phosphorus can have allotropy, because in the ground state in the phosphorus atom there are three unpaired electrons: P-red, P₄— white.

In the bromine atom there is one unpaired electron, allotropy is impossible.

6. a) HCl and HF are hydrogen compounds of elements of group VII, the main subgroup. Acidic properties of hydrogen compounds are enhanced by the end of the group, the main subgroup, because the radius of the ion increases, and the PH does not change. HCl as an acid is stronger than HF.

b) CL₂⁺¹O and CL₂⁺⁷O_{7 are salt}-forming oxides.₂O +1, in CL₂O₇+7. The greater the PH of the element, the more pronounced the acidic properties are. The acidic properties of CL₂O₇are stronger than those of CL₂O.

C) Hcl⁺⁷O₄and HBr⁺⁷O₄are oxygen-containing acids. They are formed by elements of group VII, the main subgroup. The strength of oxygen-containing acids weakens towards the end of the group, since the element's C. S. O. does not change, and the ion radius increases towards the end of the group._{NSLO 4 acid}is stronger_{than Nvgo 4 acid .}.

7. the Main properties of NH₃are more pronounced than the main properties of PH₃. Hydrogen compounds are formed by elements of one V group, the main subgroup. By the end of the group, the acidic properties of hydrogen compounds are enhanced, the main properties are weakened, because the ion radius increases, and the SR does not change.

SiH₄is the simplest formula. M_SiH3= 32 g/mol;