"Application of Periodic Table of Elements and Periodic Law of Elements" Periodic Law of Elements PPT

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"Application of Periodic Table of Elements and Periodic Law of Elements" Periodic Law of Elements PPT

Part One: Goals and Competencies:

1. Know the simple partitioning of the periodic table of elements. (Macroscopic identification)

2. Further understand that the periodic table is a specific manifestation of the periodic law of elements. (Macroscopic identification)

3. Understand the relationship between the atomic structure of elements, their positions in the periodic table and the properties of elements. (Macroscopic identification and microscopic analysis)

4. Understand the guiding significance of the periodic table of elements and the periodic law of elements in scientific research and industrial and agricultural production. (Scientific attitude and social responsibility)

PPT on the application of the periodic table of elements and the periodic law of elements, part 2: independent preview to explore new knowledge

1. Partitions of the periodic table of elements and valence rules of elements

Please fill in the content represented by the serial number in the picture.

①___; ②___; ③___; ④___;

⑤___; ⑥___; ⑦___; ⑧___.

Micro tip: ① The lower left part of the periodic table is the most metallic element (francium), and the upper right part is the most non-metallic element (fluorine). The most alkaline is FrOH, and the most acidic oxygen-containing acid is HClO4.

② Since there is no strict boundary between the metallicity and non-metallicity of elements, elements located near the dividing line can exhibit both certain metallicity and certain non-metallicity.

③The relationship between the valence of an element and its position in the periodic table

The highest positive valence of main group elements is equal to the number of outermost electrons that an atom can lose or shift; the negative valence of non-metals is equal to the number of electrons required to achieve a stable structure of 8 electrons. Therefore, the sum of the absolute value of the highest positive valence of a non-metal element and its negative valence is equal to 8. That is: a. The highest positive valence = group number = the number of electrons in the outermost shell of the atom (except O and F); b. The absolute value of the highest positive valence + the lowest negative valence = 8.

2. Application of the periodic table of elements and the periodic law of elements

1. Determine the ______ (or ______) of the properties of elements based on the gradient of properties of elements in the same period and in the same main group.

2. Applied to mutual inference of elements "______—______—______".

3. Predict new elements

Providing clues for the discovery of new elements and predicting their ______.

4. search for new substances

(1)______ materials can be found at the boundary between metals and non-metals.

(2) Study elements near ____________ to create new pesticides.

(3) Look for catalysts and high-temperature and corrosion-resistant alloy materials in ______.

PPT on the application of the periodic table of elements and the periodic law of elements, part three: core breakthroughs and overcoming difficulties

The "position, structure, and nature" relationship of the same element

The atomic structure of an element determines the position of the element in the periodic table and the main properties of the element. The position of the element in the periodic table reflects the atomic structure of the element and the main properties of the element, so the three can be inferred from each other.

1. The mutual inference of structure and position is the basis for solving problems.

(1) Master the four relational expressions

①Number of electron layers = number of cycles.

②Number of protons = atomic number.

③The number of electrons in the outermost shell of a main group element atom = the main group number.

④The highest positive valence of main group elements = group number, and the lowest negative valence = main group number -8.

(2) Proficient in some special rules in the periodic table

①The number of element types in each period (2, 8, 8, 18, 18, 32, 32 respectively).

②The atomic numbers of rare gas elements (2, 10, 18, 36, 54, 86, 118 respectively) and their periods (one to seven periods respectively).

③The relationship between the atomic numbers of adjacent elements in the same group (the difference is 2, 8, 18, 32, 32).

④The difference in atomic number between group IIA and group IIIA elements in the same period (1, 11, 25, etc.).

2. Interpretation of properties and locations is the key to solving problems

Be familiar with the gradation laws of the properties of elements in the same period and the same main group in the periodic table of elements, which mainly include:

(1) Atomic radius.

(2) The main valence of the element.

(3) Metallic and non-metallic properties of elements.

(4) Oxidizing and reducing properties of elemental substances.

(5) Stability of gaseous hydride.

(6) The highest valence oxide corresponds to the acidity and alkalinity of the hydrate.

(7) How easy it is for metal to replace H2 from H2O or acid.

3. The mutual inference of structure and properties is the key to solving problems

(1) The number of electron shells and the number of electrons in the outermost shell determine the metallicity and non-metallicity of element atoms.

(2) Elements in the same main group have the same number of electrons in their outermost shells and similar chemical properties.

(3) Correctly infer the size and structural characteristics of atomic radius and ionic radius.

(4) Determine the metallicity and non-metallicity of elements.

PPT on the application of the periodic table of elements and the periodic law of elements, part 4: meeting standards in class and improving quality

1. The position of an element in the periodic table reflects its atomic structure and its properties. Which of the following statements is correct ()

A. It is impossible for the same element to exhibit both metallic and non-metallic properties

B． The highest positive valence of an element in the third period is equal to its main group number

C． After short-period elements form ions, the outermost layer reaches an 8-electron stable structure.

D． Atoms of the same main group element have the same number of electrons in the outermost shell and have exactly the same chemical properties.

B [ Elements (such as Al) located on the dividing line between metals and non-metals in the periodic table can exhibit both metallic and non-metallic properties. A is wrong; H+ has no electrons in the outermost layer, H- and Li+ have the most There are only two electrons in the outer shell, C error; atoms of the same main group elements have similar chemical properties, but not exactly the same, D error; the highest positive valence of the elements in the third period is +1 and +2 from groups IA to VIIA respectively. , +3, +4, +5, +6, +7 valence is equal to the main family ordinal number it is in, B is correct. ]

2. Scientists have officially named the element with atomic number 114 as tungsten. Which of the following predictions about its atomic structure and properties is incorrect ()

A. The number of electrons in the outermost shell of an atom of this element is 4

B． Its common valence states are +2, +4

C． It is more metallic than lead

D． Its atomic radius is smaller than that of element 115

D. Based on the atomic number of element 114, it can be inferred that this element is in the seventh period of the periodic table, group IVA. It is the same main group element as carbon. The number of electrons in the outermost shell of this element is 4. There are +2 valence and +4 valence. Items A and B are correct; element 114 is the same main group element as lead. According to the metallicity of the elements in the same main group gradually increasing from top to bottom, it can be seen that the metallicity of this element is stronger than lead. Item C Correct; element No. 114 and element No. 115 are in the same period. According to the gradual decrease of the atomic radius of elements in the same period, it can be seen that the radius of atomic No. 114 is greater than the radius of atomic No. 115. Item D is incorrect. ]

3. The elements of Group IIA from the second period to the sixth period are Be (beryllium), Mg (magnesium), Ca (calcium), Sr (strontium), and Ba (barium). Which of the following predictions about group IIA elements may be correct ()

①At room temperature, elemental beryllium can react violently with water to release H2; ②At room temperature, elemental barium can react violently with water to release H2; ③Be(OH)2 is easily soluble in water; ④Ba(OH)2 is easily soluble in water; ⑤SrCO3 is easily soluble in water

A. ①②③　B． ③⑤ 　C. ②④　D. ①②③④⑤

C [ From top to bottom, the metallicity of the same main group gradually increases, and the reaction with water becomes more and more violent. That is, at room temperature, elemental barium can react violently with water to release H2. ① is wrong, ② is correct; Mg(OH) 2 is hardly soluble in water, Ca(OH)2 is slightly soluble in water, it follows that Be(OH)2 is hardly soluble in water, ③ is wrong; Ba(OH)2 is a strong base that is easily soluble in water, ④ is correct; according to MgCO3, CaCO3 and BaCO3 are difficult to dissolve in water, so SrCO3 is difficult to dissolve in water, ⑤ is wrong. ]

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Update Time: 2024-11-24

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