Protons, Neutrons, and Electrons

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Presentation transcript:

Protons, Neutrons, and Electrons Structure of the Atom Protons, Neutrons, and Electrons

Subatomic Particles Name Symbol Charge Relative Mass (amu) Actual Mass (kg) proton p+ +1 1 1.67 x 10-27 neutron n0 electron e- -1 1/1840 9.11 x 10-31

Basic Structure of the Atom There are two regions The nucleus With protons and neutrons Positive charge Almost all the mass Electron cloud Most of the volume of an atom The region where the electron can be found

Describing Atoms Atomic Number Mass Number number of protons number of electrons (if atom is neutral) is on the Periodic Table must be the same for atoms of the same element Mass Number number of protons + neutrons is NOT on the Periodic Table can be different for atoms of the same element

Isotopes Atoms of the same element with different mass numbers. For isotopes of the same element: The number of protons stays the same. The number of neutrons varies.

Complete Chemical Symbols Contain the symbol of the element, the mass number and the atomic number. X Mass number Atomic # protons + # neutrons mass number # protons

Br Symbol Practice 80 35 Find the number of protons number of neutrons number of electrons Atomic number Mass number Br 80 35

Isotopes + + Carbon-12 Neutrons 6 Protons 6 Electrons 6 Carbon-14 Nucleus Neutron Proton + Electrons Nucleus Nucleus Neutron Proton + Carbon-12 Neutrons 6 Protons 6 Electrons 6 Electrons Carbon-14 Neutrons 8 Protons 6 Electrons 6 Nucleus

Atomic Mass Atomic mass is a weighted average of the mass of all isotopes of an element. The measurement unit is the atomic mass unit (amu). 1 amu = 1/12 of the mass of a carbon-12 atom. 1 p+ = 1.007276 amu 1 n0 = 1.008665 amu 1 e- = 0.0005486 amu

Calculating Atomic Mass To calculate the atomic mass, you need the mass of each isotope of the element and the relative abundance of each isotope. The relative abundance is usually expressed as a percentage. When using the percentages in atomic mass calculations, you will need to express the percentage in its decimal form. 25% = .25 Then, multiply each isotope’s mass by its relative abundance (in decimal form). Record each result, and then add the results for all of the isotopes. The total is the atomic mass.

Example: Atomic Mass Calculate the atomic mass of magnesium. The three magnesium isotopes have atomic masses and relative abundances of 23.985 amu (78.99%), 24.986 amu (10.00%), and 25.982 amu (11.01%).