Subatomic Particles PDF

Subatomic Particles At the end of the lesson, 75% of the students will be able to: 1. identify the subatomic particles associated with mass number; 2. determine the number of protons, neutrons, and electrons in an atom ; and between mass 3. differentiate number and atomic n...

Subatomic Particles At the end of the lesson, 75% of the students will be able to: 1. identify the subatomic particles associated with mass number; 2. determine the number of protons, neutrons, and electrons in an atom ; and between mass 3. differentiate number and atomic number.  In 1869, British chemist and physicist William Crookes invented the Crookes tube, an electrical discharge tube used to study cathode rays. The tube contains a cathode and an anode at the two ends. When electricity is introduced into the tube, a glowing ray is produced, it travels from the cathode to the anode. This ray, called a cathode ray, is electrically negative. The Crookes tube, also known as cathode ray tube, was instrumental in the discovery of the subatomic particles. ELECTRON In 1897, J.J. Thomson studied cathode rays using the Crookes tube. In his experiments, he noticed that the mass of the cathode rays was over 1000 times smaller than that of a hydrogen atom, and that the mass was the same for all ELECTRON Thomson found that the cathode rays were negatively charged particles, which he called corpuscles. These corpuscles are now called electrons. An electron has PROTON German physicist Eugen Goldstein was the first observe the existence of positive particles. In 1886, he conducted an experiment using a modified cathode ray tube made from a metal disk PROTON Goldstein concluded that the canal rays carry a charge opposite to that of the cathode rays. Since cathode rays are negatively charged, the canal rays are positively charged. PROTON Rutherford further studied the nature of the positive particle, which was later called proton. He concluded that the proton is a subatomic particle. The proton has a mass of 1.673x10-24 g and an electric NEUTRON The third subatomic particles is electrically neutral. It has a relative mass of about 1 amu and an actual mass of 1.675x10-24 g, slightly larger than that of a proton. An atomic number is theAtomic number Number that is unique to a given element and it tells the Element Symbol number of protons which is also equal to the number of electrons.  Atomic Mass Element Symbol Protons Neutrons Electrons Number Number Magnesium Mg 12 Argon Ar 18 Cobalt Co 27 Gold Au 79 Tin Sn 50 The sum of the number of protons and number of neutrons in an atom. Mass Number  Atomic Mass Element Symbol Protons Neutrons Electrons Number Number Magnesium Mg 12 24 Argon Ar 18 40 Cobalt Co 27 59 Gold Au 79 197 Tin Sn 50 119 The number of protons of an atom can be identified by its atomic number.  Atomic Mass Element Symbol Protons Neutrons Electrons Number Number Magnesium Mg 12 24 12 Argon Ar 18 40 18 Cobalt Co 27 59 27 Gold Au 197 79 79 Tin Sn 50 119 50 Remember This! Atomic = Number of Number (Z) Protons () The number of neutrons of an atom can be identified by subtracting the mass number to its atomic number. Atomic Number 22 (Z): # of Protons (): 22 Mass Number 48 (A): # of Neutrons (): 26  Atomic Mass Element Symbol Protons Neutrons Electrons Number Number Magnesium Mg 12 24 12 12 Argon Ar 18 40 18 22 Cobalt Co 27 59 32 27 Gold Au 79 197 118 79 50 119 Tin Sn 50 69 The number of proton is the basis for identifying the number of electrons.  47 Atomic Number: # of Protons:47 # of Electrons: 47  Atomic Mass Element Symbol Protons Neutrons Electrons Number Number Magnesium Mg 12 24 12 12 12 Argon Ar 18 40 18 22 18 Cobalt Co 27 59 27 32 27 Gold Au 79 19 118 79 7 79 50 11 Tin Sn 50 69 9 50 Direction: Using the periodic table, complete the information needed on the table.  Atomic Atomic Proton Neutron Element Symbol Numbe Electrons Mass s s r Bromine Br 35 80 35 45 35 Iodine I 127 53 53 53 74 Lead Pb 82 207 82 12 82 5 Barium Ba 56 137 56 81 56 Platinu Pt 78 195 78 11 78 m 3 Nickel Ni 28 59 28 31 28  “APE MAN” Atomic Number = Number of Proton = Number of Electron Mass Number – Atomic Number = Number of Neutron IONS An atom can become an electrically charged particle when it gains or loses one or more electrons while its number of protons remains the same. If an atom gains electrons, it will have more negative particles than positive particles and thus carry a IONS If it loses electrons, it will have more positive particles than negative particles and thus have a net positive charge. An atom that carries a net electrical charge is called an ion. A positively charged ion is called a cation, while a negatively H : a neutral hydrogen atom (1 proton, 1 electron, o neutron) H : a hydrogen cation (1 proton, 0 electron, o neutron H : a hydrogen anion (1 proton, 2 electron, o neutron Neither the number of protons and neutrons changes in any of the ions. Therefore, both the atomic number and the mass number remains the same. ISOTOPES Isotopes are atoms having the same number of protons, but they can have different number of neutrons.  Isotopes of Hydrogen Isotopes Atomic Mass Protons Neutrons Electrons number Number (p+) (n0) (e-) (Z) (A) H-1 (protium) 1 1 1 0 1 H-2 (deuterium) 1 2 1 1 1 H-3 (tritium) 1 3 1 2 1 Isotopes of Carbon Isotopes Atomic Mass Protons Neutrons Electrons number Number (p+) (n0) (e-) (Z) (A) Carbon - 12 6 12 6 0 6 Carbon - 13 6 13 6 7 6 Carbon - 14 6 14 6 8 6 CHEMISTRY BINGO Direction: Using the periodic table, complete the information needed on the table. Isotopes Element Z A p+ n0 e- Name B-11 Boron 5 6 5 11 5 Chlorine 35 18 Cl-35 Mg-24 17 17 12 17 12 Al-27 Magnesium 13 12 24 12 14 S-32 Aluminum 27 11 16 11 Sulfur 16 32 16 16 1. Which of the following subatomic particles determine the identity of an atom? A. protons B. neutrons C. protons plus neutrons D. electrons plus protons 2. An atom of an element is electrically neutral because the number of protons is equal to the number of ___________. A. electrons B. neutrons C. nucleons 3. Which particles have approximately the same size and mass? A. protons and neutrons B. electrons and protons C. neutrons and electrons D. None because all are different in 4. How do we call the protons and neutrons that are found together in the nucleus? A. nuclei B. nucleons C. atomic mass D. mass number 5. Element A has a mass number of 100 while element B has an atomic number of 118. What will be the number of electrons of element B? A. 59 B. 60 C. 118 D. 120 6. What is the atomic mass of an atom of Terbium that has 65 protons, 65 electrons, and 94 neutrons? A. 130 B. 159 C. 172 7. Which of the following statements best describes isotopes? A. Same number of neutrons, different number of protons B. Same number of protons, different number of neutrons C. Same number of protons, different number of electrons D. Same number of neutrons, different number of electrons 8. What is a mass number? A. The sum of the number of protons and number of neutrons in an atom. B. The sum of the number of neutrons and electrons. C. The sum of the number of electrons and protons. D. The sum of the three subatomic 9. What is the number of neutrons in an atom of Germanium that has a mass number of 73, 32 protons, and 32 electrons? A. 32 B. 41 C. 73 D. 105 10. Which of the following statements describe atomic number? A. It can be located above the element symbol and tells the number of neutrons. B. It can be located below the element symbol and tells the number of electrons. C. It can be located above the element symbol and tells the number of protons. D. It can be located below the element symbol and tells the number of neutrons. ASSIGNMENT: Do you know that the human body is approximately 99% comprised of six elements. Oxygen, Hydrogen, Nitrogen, Carbon, Calcium, and Phosphorus. As an assignment, find the number of protons, electrons, neutrons, atomic number, and mass of the above stated elements. CREDITS: This presentation template was created by Slidesgo, including icons by Flaticon, and infographics & images by Freepik