Preparatory Work for Atomic Structure Topic
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1 Preparatory Work for Atomic Structure Topic Use the Atomic Structure PowerPoint at to complete this sheet NOT your GCSE notes You will need to bring to your first lesson: a ring binder A4 folder, a highlighter, a pen, a pencil, lined paper, a ruler, a scientific calculator. Fundamental Particles Relative mass Relative Charge What are atoms like? Atoms are neutral particles they have no overall charge. Complete: In an atom number of protons = number of. This atom is fully represented as Li 3 is called the atomic number (Z) 7 is called the mass number (A) Label the nucleus. Write the (GCSE) electron configuration for this atom Define Atomic number 7 3 Define Mass number How would you calculate the number of neutrons from the atomic number and the mass number? Number of neutrons =
2 Isotopes Examples of isotopes of hydrogen are: 1 H 2 H 3 H Notice there is no need to give the atomic number the element symbol tells you what this is anyway. Define isotopes in terms of numbers of fundamental particles. Another element with isotopes is chlorine (use the Periodic Table to find the number of protons). 35 Cl Number of protons neutrons electrons 37 Cl Write the (GCSE) electron configuration for chlorine. Chlorine is a halogen which group of the periodic table does it belong to? How does the group number relate to the electronic configuration? The CHEMICAL properties of isotopes of the same element like 35 Cl and 37 Cl are always IDENTICAL because... Ions An ion is a.. particle. The number of and are NOT equal. When an atom loses one or more it forms a. charged ion called a.. Give an example.. When an atom gains one or more.it forms a. charged ion called an. Give an example Often ions have electron arrangements with a full outer shell like the..... gases which should be stable.
3 ATOMIC STRUCTURE Complete the atomic structure preparation work using this PowerPoint to help you complete the questions. Bring the completed worksheet to your first chemistry lesson of the A level course when we will go over the answers so that they can form part of your notes on this topic. You should find this piece of work fairly straightforward as it is based on work that you have probably covered at GCSE. Nevertheless the A level examiners do set questions on it. Obviously you can choose when you do the work but we suggest you leave it until you are fairly close to starting your A level Chemistry course.
4 Fundamental Particles Proton Neutron Electron Relative Mass Relative charge The actual masses and charges are very small e.g. a proton is 1.7 x kg NOTE The relative mass of an electron is so small that it is often taken to be ZERO.
5 Fundamental Particles Relative Mass Relative charge Proton 1 +1 Neutron 1 0 Electron The actual masses and charges are very small e.g. a proton is 1.7 x kg NOTE The relative mass of an electron is so small that it is often taken to be ZERO.
6 Atoms An atom is a neutral particle, it has no overall charge. In an atom number of protons = number of electrons
7 An atom of lithium Atoms can be represented as follows: - Mass number 7 Atomic number 3 NUCLEUS Li At GCSE This electronic configuration is written 2,1
8 Atomic Number (Z) The number of protons in the nucleus (of an atom). Mass Number (A) The number of protons plus the number of neutrons in the nucleus (of an atom).
9 Calculating the Number of Neutrons in the Nucleus Mass number = number of protons + number of neutrons Therefore:- Number of neutrons = mass number - atomic number
10 Isotopes Isotopes Atoms with the same number of protons but a different number of neutrons. Examples of isotopes of hydrogen are : 1 H 2 H 3 H Examples of isotopes of chlorine are : 35 Cl 37 Cl Notice there is no need to give the atomic number the element symbol tells you what this is anyway
11 Isotopes Number of protons neutrons electrons Cl = Cl = 20 17
12 Isotopes The electronic arrangement of chlorine is 2, 8, 7 Chlorine is a halogen (Group 7). The number of outer shell electrons is the same as the group number. Why do chlorine-35 and chlorine-37 have identical chemical reactions? See the next slide for the answer.
13 Isotopes The chemical properties of isotopes of the same element like 35 Cl and 37 Cl are identical because they have the same number of electrons. The only differences between isotopes of the same element are physical properties such as rates of diffusion, which depend on the mass of the particles, or nuclear properties such as radioactivity.
14 IONS An ion is a particle. The number of and are NOT equal. When an atom loses one or more it forms a charged ion called a. When an atom gains one or more it forms a charged ion called an. Often ions have electron arrangements with a full outer shell like the gases which should be stable. Use these words once/ more than once or not at all to fill the gaps negatively positively charged Noble Diatomic electrons neutrons protons anion cation
15 An ion is a charged particle. IONS The number of electrons and protons are NOT equal. When an atom loses one or more electrons it forms a positively charged ion called a cation. Example Na + When an atom gains one or more electrons it forms a negatively charged ion called an anion. Example Cl - Often ions have electron arrangements with a full outer shell like the Noble gases which should be stable. Use these words once/ more than once or not at all to fill the gaps negatively positively charged Noble Diatomic electrons neutrons protons anion cation
16 To ensure you are fully prepared to start your A level Chemistry course we recommend that you also sort out and read your chemistry GCSE notes and when you are fairly close to starting in September, work through the tasks below. Go to the BBC GCSE BiteSize website Work through the section on atomic structure (activity first, then revise, then test): _2011/atomic/atomstrucrev1.shtml Work through the section on calculations (both tiers), revise pages 1,2 & 3 (mass number, isotopes, relative atomic mass) and activity up to relative atomic mass: mcalc/
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