How Atoms Differ.

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Presentation transcript:

How Atoms Differ

Properties of Subatomic Particles Symbol Location Relative Charge Relative mass Actual mass (g) Electron e- or In the space surrounding the nucleus 1- 1 1840 9.11 x 10-28 Proton p+ or In the nucleus 1+ 1.673 x 10-24 Neutron n0 or 1.675

II. Atomic Number the number of protons in an atom Identifies element each atom has unique # # never changes

III. Mass Number represents the total number of protons and neutrons in the nucleus # of neutrons = mass number – atomic number

IV. Isotopes Atoms of the same element but have a different # of neutrons Ex: 3 isotopes of carbon:

All elements have isotopes (some 2, some 3, etc.) Some isotopes are naturally radioactive. Ex: Plutonium

V. Representing Isotopes In Ag-107, the 107 represents the mass number (neutrons + protons) the 47 represents the number of protons

Practice: 1. What is the mass number for Co-59? 2. What is the mass number for 59 7

VI. Atomic Mass The standard is the atomic mass unit (amu): defined as 1/12 of the mass of a carbon-12 atom the weighted average of the isotopes of that element. Formula: Atomic mass of an element = ( % abundance of Isotope #1 x mass Isotope #1 ) + Isotope #2 …

Practice 3 Silver has two naturally occurring isotopes. Ag-107 has an abundance of 51.82% and mass of 106.9 amu. Ag-109 has a relative abundance of 48.18% and a mass of 108.9 amu. Calculate the atomic mass of silver.

Practice 4 Rubidium is a soft, silvery-white metal that has two common isotopes, Rb and Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium? 85 37 87 37

Vocabulary to Know Atomic #- same # of protons & electrons Mass #-protons + neutrons written 2 ways: Carbon-14 or C Isotopes-same # of protons, different # of neutrons Atomic mass-weighted average mass 14 6