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Chemistry 2045 Chapter 2 Part 1 Notes

by: Zayd Alasadi

Chemistry 2045 Chapter 2 Part 1 Notes CHM 2045

Marketplace > University of South Florida > CHM 2045 > Chemistry 2045 Chapter 2 Part 1 Notes
Zayd Alasadi
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About this Document

These notes cover the first part of the chapter 2 lecture.
General Chemistry I
Dr. Bryant
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This 3 page Class Notes was uploaded by Zayd Alasadi on Thursday August 25, 2016. The Class Notes belongs to CHM 2045 at University of South Florida taught by Dr. Bryant in Fall 2016. Since its upload, it has received 64 views.


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Date Created: 08/25/16
Chapter 2 Notes (part 1) Learning Objective 1: Describe the structure of the atom in terms of the of the placement and charge of protons, neutrons, and electrons. Nucleus- a small core in an atom Contains two different particles: Protons- positively charged particles (+) Neutrons- neutral particles with no charge Electrons- negatively charged particles (-) Orbit around the nucleus (not in the nucleus) An atom is mainly made up of empty space. Learning Objective 2: Describe the structure of the atom in terms of the number of protons, neutrons and electrons given mass number and chemical identity or atomic number. Define isotopes and ions in terms of the structure of the atom. Protons and Neutrons have nearly identical masses however protons are positively charged while neutrons have no charge. The charge of a Proton and Electron are equal in magnitude but opposite in sign. Proton- +1.6022 x10^-19 Electron- -1.6022 x 10^-19 The number of protons will tell you which element it is on the periodic table. Example: If an atom has 4 protons, it has to be Beryllium. Atomic Number (Z)- The number of protons in an atom’s nucleus. Each element has its own symbol. Example: Beryllium’s symbol is “Be” while Oxygen’s symbol is “O”. Isotopes are atoms of the same element. The differences in these atoms is that they have a different number of neutrons. They have different masses yet they have the same chemical behavior Example: Carbon-12 and Carbon-13. These two atoms are both considered Carbon. However, Carbon-12 has 6 protons and 6 neutrons while Carbon-13 has 6 protons and 7 neutrons. Therefore they have different masses but still have the same chemical behavior. Mass Number (A)- The number of protons + the number of neutrons in an atom’s nucleus. This is where isotopes can have a different value. Example: Carbon-12 and Carbon-13 have different mass numbers. Carbon-12 has 6 protons and 6 neutrons which gives a value of 12 for the mass number. Carbon-13 has 6 protons and 7 neutrons which gives a value of 13 for the mass number. Isotope Notation- a way you show how many protons, neutrons, and electrons an atom has. Using isotope notation can help you figure out mass number, atomic number, and chemical symbol. Example: The mass number (A) goes on the top left of the chemical symbol and the atomic number (Z) goes on the bottom left of the chemical symbol. Ions- charged particles formed when neutral atoms lose or gain electrons. NeutralAtoms- atoms that have the same number of protons and electrons. Cation- positively charged ions (losing negatively charged electrons) Anion- negatively charged ions (gaining negatively charged electrons) Example: Cr = 3e- + Cr^ 3+ Example: F- = F + 1e-


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