"Atomic Structure and Element Properties" Periodic Law of Atomic Structure Elements (Lesson 1 Nuclide)

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"Atomic Structure and Element Properties" Periodic Law of Atomic Structure Elements (Lesson 1 Nuclide)

Part 1: Essential knowledge and foundation of literacy

1. Atomic structure

1. Atoms and their constituent particles

For atoms: nuclear charge =_______=___________

2. Mass number

(1) Definition: The mass number is the sum of the number of protons (Z) and the number of neutrons (N) in the nucleus, represented by the symbol A.

(2)Calculation formula: mass number (A)=____.

3. Representation method of atomic composition

Generally represented by symbols, the meanings of letters are as follows:

【Situation·Thinking】

Carbon-14 (), a type of carbon atom retained by organisms during their lifetime, decays after death. Measuring the amount of carbon-14 in relics found at archaeological sites can infer its age.

Do you know what the "14" in carbon-14 means? What are the number of protons, neutrons, and extranuclear electrons of this carbon atom?

Tip: The "14" of carbon-14 means that the mass number of this carbon atom is 14, the number of protons of this carbon atom is 6, the number of neutrons is 8, and the number of electrons outside the nucleus is 6.

2. Elements, nuclides and isotopes

1. Concepts and relationships

2. Several common isotopes

(1) Isotopes of hydrogen element

(2) Isotopes of several other common elements

【Situation·Thinking】

Oxygen isotopes are used as a reference for dating in geography, and are often used to date glaciers. Oxygen isotopes are widely used in earth science to determine the source of rock-forming minerals and the temperature of rock-forming and mineralization. It has broad application prospects in biology and medicine. Oxygen exists in nature in the form of three isotopes: 16O, 17O, and 18O.

3. Classification and characteristics of isotopes

(1)Classification

① Isotopes are divided into _____ isotopes and _______ isotopes.

②Applications of radioactive isotopes: _______ tracer (such as ) and as _______.

(2)Features

①The _____ properties of isotopes are basically the same, but there are certain differences in _____ properties.

②For a naturally occurring element, whether in a combined state or a free state, the percentage of atoms occupied by various isotopes is generally _____.

Atomic structure and element properties PPT, part 2 content: key abilities and quality formation

Knowledge point 1: Atomic structure and the relationship between atomic particles

[Key points to clarify doubts]

1. The composition of atoms: The basic particles that make up atoms are protons, neutrons and electrons. The properties, functions and interactions of the three types of particles are as follows:

2. Relationship between particles

(1) Quality relationship

Mass number (A) = number of protons (Z) + number of neutrons (N).

(2) Electrical relationship

[Error-prone reminder] Several error-prone points about atomic structure

(1) Atoms must contain protons, but not necessarily neutrons, such as 1H.

(2) The mass number of an atom and the relative atomic mass have different meanings, but the mass number of an atom is generally equal to the integer part of the relative atomic mass value of the atom.

(3) When converting the number of electrons to the number of protons in ions, attention should be paid to the difference between cations and anions.

[Knowledge Expansion] Break through the two major relationships of atomic composition

(1) There are two equivalent relationships between the particles that make up atoms.

① An atom is composed of a nucleus and electrons outside the nucleus. The nucleus is positively charged, and the electrons outside the nucleus are negatively charged. The nucleus is composed of protons and neutrons; since neutrons are uncharged, the atom is electrically neutral, so the nuclear charge of the atom = Number of protons in the nucleus = number of electrons outside the nucleus.

② The number of nuclear charges in the atomic structure determines the type of element, and the sum of the number of protons and the number of neutrons determines the relative size of the atomic mass, that is, the mass number (A) = the number of protons (Z) + the number of neutrons (N) .

【Think·Discussion】

(1) Why are atoms electrically neutral? But ions are charged?

Tip: Because the number of positive charges carried by the nucleus is equal to the number of negative charges carried by the electrons outside the nucleus. Ions are formed by atoms gaining and losing electrons. The number of electrons outside the nucleus is no longer equal to the number of protons, so the ions are charged.

(2) What are the main factors that determine atomic mass?

Tip: Because the mass of electrons is very small and can be ignored, it mainly depends on the masses of protons and neutrons.

Knowledge point 2: Comparison of elements, nuclides, isotopes and allotropes

[Key points to clarify doubts]

1.Difference

2.Contact

[Error-prone reminder] Several error-prone points about nuclides

(1) An element can have several nuclides or only one nuclide. There are as many atoms as there are nuclides.

(2) Most elements have isotopes, but some elements do not.

(3) The transformation between different nuclides is not a chemical change, but a nuclear reaction.

[Regular method] Techniques for judging isotopes and allotropes

(1) When judging isotopes and allotropes, the essential differences between various particles should be grasped.

Atoms with the same number of protons are the same element. Atoms with the same number of protons but different numbers of neutrons are isotopes of each other. Different elements formed by the same element are allotropes of each other.

(2) Pay attention to the meaning of numbers in atomic symbols. , as long as Z is the same, it is the same element; if Z and A are the same, they are the same nuclide; if Z is the same but A is different, they are isotopes of each other; if Z is different, regardless of whether A is the same, they are not the same element, let alone isotope.

【Quality Improvement】

The Wangfujing Ancient Human Cultural Sites Museum in Beijing shows the world the remains of "Beijing people" who hunted, burned fire, and made tools. The museum's exhibition hall of more than 300 square meters displays stone anvils, stone hammers, and stone flakes unearthed from the original site, as well as bones of primitive cattle, spotted deer, ostriches, fish and other ancient creatures, as well as bone shovels and bones made by ancient humans. Tools such as tablets. Reproduce the scenes of spotted deer jumping, ostriches jubilant, looking at the mountains and listening to the water, and wild boars living 25,000 years ago.

(1) How is "25,000 years" measured? (Scientific Attitude and Social Responsibility)

Tip: "25,000 years" is inferred by measuring the number of carbon-14 (14C) atoms in the remains.

(2) What are the similarities and differences in the atomic structures between carbon-14 atoms and carbon-12 atoms (12C), which are the relative atomic mass standards? (Macroscopic identification and microscopic analysis)

Tip: 14C atoms and 12C atoms have the same number of protons but different numbers of neutrons.

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Update Time: 2024-10-01

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