The-Subatomic-Particles.pptx

The Subatomic Particles General Chemistry 1  Lesson Objectiv Identify and describe the three primary es subatomic particles: protons, neutrons, and electrons, including their charges, masses, and locations within an atom. Calculate the atomic number, mass num...

The Subatomic Particles General Chemistry 1  Lesson Objectiv Identify and describe the three primary es subatomic particles: protons, neutrons, and electrons, including their charges, masses, and locations within an atom. Calculate the atomic number, mass number, and number of neutrons in an atom given its number of protons and neutrons or its atomic number and mass number. Define isotopes and explain how they differ in the number of neutrons while having the same number of protons and electrons.  Subatomic A Subatomic particle Particles is nothing but a particle which is smaller than an atom in size. Typically, an atom can be broken down. into three subatomic particles, namely: protons, electrons, and neutrons. Subatomic Particles  Atom its An atom is the basic unit of matter and the smallest are made and Structure particle of an element that retains its properties. Atoms up of three types of subatomic particles: protons, neutrons, and electrons. Proton Neutron Electron Protons are Neutrons are Electrons are positively neutrally charged negatively charged particles particles also charged located in the located in the particles that nucleus (center) nucleus. orbit around the  Atom its and Structure In perspective, if we imagine an atom The nucleus of an atom is actually were the size of a stadium, the nucleus about 100,000 times smaller than the would be smaller than a grain of sand. overall size of the atom.  Electrons Electrons were discovered by Sir John Joseph Thomson in 1897. After many experiments involving cathode rays, J.J. Thomson demonstrated the ratio of mass to electric charge of cathode rays. Electrons are subatomic particles that revolve around the nucleus of an atom. number of protons = number of electrons  Protons Protons were discovered by Ernest Rutherford in the year 1919. He projected alpha particles (helium nuclei) at gold foil, and the positive alpha particles were deflected. He concluded that protons exist in a nucleus and have a positive nuclear charge. The atomic number or proton number is the number of protons present in an atom. The atomic number determines an element. number of protons = atomic number of element  Neutrons Neutrons were discovered by James Chadwick in 1932. Neutrons are located in the nucleus with the protons. Along with protons, they make up almost all of the mass of the atom. the proton number from the atomic mass number.. Number of protons + number of neutrons= mass number of an element  Fundamental facts Regarding the Structure of an atom 1.Atoms consists of a very small positive nucleus surrounded by negative electrons moving at high speeds. 2.The nucleus consists of protons and neutrons while electrons are found outside the nucleus. 3. The relative mass and charge of protons, neutrons and electrons are: Atomic Numbe Atomic number of an element represents the number of protons in its nucleus. r and Atomic Number=Number of Protons=Number of Electrons Mass The number of protons= Number of Electrons Numbe The Mass Number indicates the total number of protons and neutrons; it is an estimate of the elements atomic mass. r Mass Number=Number of Protons+Number of Neutrons Isotopes  Are atoms of an element having the same atomic number but different mass number. ISOTO The existence of isotopes was shown PES by mass spectroscopy experiments, wherein elements were found to be composed of several types of atoms, each with ISOTOPES OF CARBON ISOTOPES Of HYDROGEN  Write the atomic symbol for each situation. A. 7 protons and 8 neutrons B. 11 protons and 13 neutrons C. atomic number of 14 with 15 neutrons D. 9 protons and mass number of 10  Uses of Isotopes in our daily life Cobalt-60 Iodine-131 Carbon-11 Technetium-99 1.The atomic number is equal to the number of protons. TRUE OR FALSE 2.The mass number is the sum of the number of protons and neutrons 3.Isotopes are composed of the same elements 4.Isotopes have the same atomic number 5.Isotopes share the same mass number 6.Isotopes have the same number of neutrons 7.Isotopes differ in the number of protons 8.Isotopes possess different chemical properties 9.Isotopes possess different nuclear properties. Prepared by: GLORY MAE FERRER- RAMIREZ,RN,MAN,LPT