Phương pháp dạy học hóa học bằng tiếng Anh
Áp dụng dạy học chương trình cấu tạo nguyên tử hóa học lớp 10
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- Điều hướng trang này:
- Vocabulary Meaning a
- C. SUMMARY
- II. What is the Structure of an Atom
- Atomic mass unit
- 3. Elemental notation
Áp dụng dạy học chương trình cấu tạo nguyên tử hóa học lớp 10CHAPTER: ATOMIC STRUCTURE A. VOCABULARY
B. SENTENCES - The fundamental unit of matter is the atom: Đơn vị cơ bản của vật chất là nguyên tử. - Since atoms are electrically neutral, the number of protons equal the number of electrons in an atom: Nguyên tử trung hòa về điện, nên số proton bằng số electron. - Chemical reactions: Phản ứng hóa học - The atomic structure (the structure of an atom): Cấu trúc nguyên tử - To be made up of : Được tạo thành - The modern atomic structure: Cấu trúc nguyên tử hiện đại - “planetary” model of the atom: mô hình hành tinh nguyên tử - The extra-nuclear part: Phần ngoài hạt nhân (vỏ nguyên tử) - Tomic mass unit: Đơn vị khối lượng nguyên tử - The size of atom: Kích thước nguyên tử - Isotopes atoms of an element that have the same number of protons but different numbers of neutrons: Các nguyên tử đồng vị của cùng một nguyên tố có cùng số proton nhưng khác nhau số nơtron. - The atomic masses, shown on the periodic table, represent a weighted average of the masses of the naturally occurring isotopes of each element: Nguyên tử khối trong bảng tuần hoàn, được lấy trung bình khối lượng của các đồng vị trong tự nhiên của mỗi nguyên tố - The principal is used to indicate the energy level that the electron is found in: Số lượng tử chính dùng để xác định mức năng lượng của electron tìm thấy. - The value for n will always be a whole number, and the higher the number, the further away from the nucleus the electron described by n tends to be: Giá trị n luôn là số nguyên, n càng lớn thì electron càng ở xa hạt nhân. - The angular momentum quantum number, is used to indicate the type of sublevel that the electron occupies: Số lượng tử phụ xác định kiểu phân lớp mà electron chiếm đóng. - The electrons in the highest energy level, which are called valence electrons: Các electron ở mức năng lượng cao nhất được gọi là các electron hóa trị. - The possible values for l refer to the types of sublevels, each of which contain a certain number of orbitals: Mỗi giá trị l chỉ mỗi phân lớp, mỗi phân lớp chứa một số obitan xác định. - To calculate the total number of electrons that an energy level can hold is to use the formula 2n2: Để tính tổng số electron trong một mức năng lượng ta dùng công thức 2n2 - The superscript of 1s1 shows us that hydrogen has only one electron: Số mũ cho thấy hiđro có 1 electron. - The large number (1 in 1s2) represents the principal quantum number for the electron: Số lớn đại diện số lượng tử chính của electron. - The letter indicates the sublevel that the electron is located in: Chữ cái cho biết phân lớp electron chiếm đóng. - Shorthand electron configuration: Cấu hình electron thu gọn
I. What is an Atom? All substances are made up of matter and the fundamental unit of matter is the atom. The atom constitutes the smallest particle of an element which can take part in chemical reactions and may or may not exist independently. II. What is the Structure of an Atom? The history of the discovery of the atomic structure is outlined below. The concept of “atoms” is believed to have originated in ancient Greece. Democritus and his teacher Leppicutius were supporters of what has been called a discontinuous theory of matter, which means that all matter is made up of tiny particles, which are separated by spaces. This atomic theory didn’t attract too many followers over the next 2,000 years or so. However, in the 1600s and 1700s, early chemists began publishing the results of experiments that they were carrying out. • John Dalton (1808) proposed the Atomic Theory. According to Dalton, matter is made up of tiny particles called atoms. The atom is the smallest particle of matter that takes part in a chemical reaction. Atoms are indivisible and cannot be created or destroyed. Further, atoms of the same element are identical in every respect. • J. J. Thomson (1897) discovered electrons in Cathode Ray experiments. According to Thomson, atoms are divisible. Atoms contain very tiny negatively charged particles called electrons. • E. Goldstein (1900) discovered protons in Anode Ray experiments. According to Goldstein, atoms contain positively charged particles called protons. Since atoms contain negatively charged particles, they must contain positively charged particles for them to be electrically neutral. • E. Rutherford (1911) discovered the nucleus and provided the basis for the modern atomic structure through his alpha particle scattering experiment. According to Rutherford, the atoms is made of two parts: the atom nucleus and the extra-nuclear part. Ernest Rutherford’s famous “gold-foil” experiment showed that most of the atom was empty space, leading to Niels Bohr’s “planetary” model of the atom, where the electrons orbited around the nucleus the way planets do a star.. • N. Bohr (1940) provided the modern concept of the atomic model. According to Bohr, the atom nucleus and the extra-nuclear part. His experiments proved that the atom is largely empty and has a heavy positively-charged body at the center called the nucleus. The central nucleus is positively-charged and the negatively-charged electrons revolve around the nucleus. • James Chadwick (1932) disovered neutrons. According to Chadwick, atoms contain neutral particles called neutrons in their nucleus along with the subatomic particles is made of a central nucleus containing protons (positively-charged) and neutrons (with no charge). The electrons (negatively-charged) revolve around the nucleus in different imaginary paths called orbits or shells. The Structure of an atom: Atoms themselves are made up of even smaller particles. These subatomic particles protons, neutrons, and electrons. Protons and neutrons cluster together to form the central core, or nucleus, of an atom. Fast-moving electrons occupy the space that surrounds the nucleus of the atom. A proton is a positively charged subatomic particle with a mass of approximately 1 atomic mass unit (amu) and a charge of +1. It is the number of protons in the nucleus of an atom, or the nuclear charge, that gives the element its identity. For example, any atom containing only one proton in its nucleus is considered an atom of the element hydrogen, the number of protons in an atom is called the atomic number of that element. So, we can say that the atomic number of hydrogen is 1. A single proton is often represented by the symbol (p+) or (  ). Because a single proton is identical to the nucleus of a form of hydrogen, the symbol (H+), which will we see often when we study acids, also represents a proton.
A neutron(n0) is a neutrally charged subatomic particle, which, as does the proton, has a mass of approximately 1 atomic mass unit (amu). When we add the total number of protons and neutrons in the nucleus of an atom, we get the atom’s mass number. Because the neutron has no charge, it does not affect the atomic number and does not alter the identity of the element. For this reason, it is possible to have two atoms of the same element with differing mass numbers, because they have different numbers of neutrons. Atoms of the same element with different masses are called isotopes. For example, there are three different isotopes of hydrogen. Electrons (e-), which are located outside of the nucleus, have essentially no mass and a charge of -1. Each electron has a charge that is the equal and opposite to the charge of a proton but contains only about 1/1836th of the mass of a proton. Because atoms typically have the same number of electrons as protons, they normally have a net charge of zero and are said to be neutral. For example, if an atom of oxygen has 8 protons (8 × (+1) = +8) and 8 electrons (8 × (-1) = -8, then (+8) + (-8) = 0) the atom of oxygen has a net charge of zero. Properties of Protons, Neutrons, and Electrons
The size of atom: An average atom is about 10−10m in diameter. Such a tiny size is difficult to visualize. If an average atom were the size of a grain of sand, a strand of your hair would be about 60 m in diameter! Atomic mass unit (AMU) = 1/12mass of 12C= 1u 1u=19.9265×10-27kg/12 =1.66×10−27kg III. The Nucleus of an Atom 1. Atomic number (Z) of an element is the number of protons in the nucleus of an atom. Since atoms are electrically neutral, the number of protons equal the number of electrons in an atom. Atomic Number (Z)= of protons in the nucleus = of electrons in an atom Nucleus: protons and neutrons- very little volume but most of the mass 2. Mass number (A) of an element is the sum of the number of protons and neutrons in the nucleus of an atom. A = Z + N For example, an oxygen atom, which has 8 protons and 8 neutrons in its nucleus, has a mass number of 16. A uranium atom, which has 92 protons and 146 neutrons, has a mass number of 238. 3. Elemental notation (Atomic symbol for an element , the atomic symbol is also called the element symbol). When the elemental symbol of an element is combined with additional information, such as the atomic number, mass number, or charge, it is usually called elemental notation. Elemental notation is a simple way of summarizing a good deal of information in a small space. Examples of elemental notation is shown here: 
X: atomic symbol Z: atomic number A: mass number n+: điện tích Each element has a different atomic symbol. For example, consider the element fluorine:  .The mass number (the superscript 19) indicates that fluorine has a total of 19 protons and neutrons. The atomic number (subscript 9) indicates that fluorine has 9 protons. Neither the mass number nor the atomic number tells you how many neutrons fluorine has. You can calculate this value, however, by subtracting the atomic number from the mass number.
Number of neutrons = Mass number − Atomic number = A−Z Thus, for fluorine, Number of neutrons = A−Z =19−9 = 10
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