10/4/2011. Tells you the number of protons
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1 Atomic Structure The arrangement of the subatomic particles within the atom determines the chemical properties of the elements How they interact with one another The types of ions and structures that they form The periodic table gives you 2 basic pieces of information Atomic number (upper whole number) Atomic mass (lower decimal number) Atomic number Tells you the number of protons Since the overall charge on the atom is neutral, the number of electrons must equal the number of protons 1
2 Atomic mass Weighted average mass that takes into account the mass and abundance in nature of the isotopes of the element Measured in atomic mass units (amu) Mass number Total number of protons and neutrons Isotopes are indicated by including the mass number with the symbol I.e. C- 14 tells you that the mass of carbon is 14, not the more common 12. Atomic mass This number is the mass of the nuclear particles The nucleus is comprised of protons and neutron so the atomic mass is the sum of the protons and neutrons The mass of the electrons is negligible The atomic mass is not a whole number because it is an average of the isotopes of the element Calculating amu Atomic mass units average atomic mass There are 2 isotopes of element X X-10 has a mass of amu and a relative abundance of 19.91% X-11 has a mass of amu and has a relative abundance of 80.09% X-10; x.1991 = amu X-11; x.8009 = amu Element X = amu 2
3 Vocabulary Ion Charged particle Atom that has lost or gained electrons Isotope Atoms of the same element with different numbers of neutrons Nucleus Contains the nucleons Protons and neutrons Where the mass of the atom is located Has an overall positive charge Subatomic Particles Proton The positively charged particle Found in the nucleus Accounts for the mass of the atom, along with the neutrons Determines the identity of the element 3
4 Neutron The neutrally charged particle Located in the nucleus The number of neutrons determines which isotope of an element is present With the proton, accounts for the mass of the atom Mass of a neutron is relatively equivalent to the mass of a proton Electron The negatively charged particle in the atom Located in orbitals around the nucleus When lost or gained determines the type of ion formed from the atom When an atom loses an electron a positive ion (cation) is formed When an atom gains an electron a negative ion (anion) is formed Interact between atoms to form chemical bonds in compounds Arrangement of Electrons Electrons hold the energy in the atom The energy level of an electron is the region around the nucleus where the electron is likely to be moving Electrons move between energy levels based on the energy they possess The energy it takes to move an electron from one level to the next is a quantum 4
5 Waves and electrons Electromagnetic radiation travels at a speed of 3.0 x 10 8 m/s, in a vacuum Amplitude wave height from the origin to the crest Wavelength ( ) distance between the crests Frequency ( ) number of wave cycles to pass a given point per unit of time Calculations Frequency and wavelength are inversely related and can be calculated l The SI unit of frequency (cycles per second) is hertz (Hz) C = Atomic Emission Spectrum When atoms are excited by an electric current passed through its gas or vapor, they first absorb energy, then lose it as they emit light. The light emitted by an atom will consist of a unique set of lines each corresponding to one exact frequency of light Likewise atoms give off a particular color of light when they are burned. 5
6 Max Planck Father of quantum physics Studied the relationship between energy and frequency Showed that the amount of radiant energy absorbed or emitted is proportional to the frequency of the radiation E = h E = energy H = Plancks constant (6.626 x Js) Previously it was thought that there was no limit to how small of an energy change could be in an atom Albert Einstein Proposed that light could be described as quanta of energy that behave like particles Light quanta are called photons Energy of photons is calculated E = h Energy changes in the Atom When energy is added to an atom, the electrons are excited and move to a higher energy level (excited state) The same amount of energy is emitted as a photon when the electron drops back to a lower level (ground state) Only electrons in transition from higher to lower energy levels will emit light 6
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