Presentation on theme: " Determines the element Number of protons CANNOT change for an element Common charge notation is +1 Mass (g) = 1.673 x 10 -24 Mass (amu)= 1.0073."— Presentation transcript:
Determines the element Number of protons CANNOT change for an element Common charge notation is +1 Mass (g) = 1.673 x 10 -24 Mass (amu)= 1.0073 = 1
Common charge notation is 0. No charge! Mass (g) 1.675 x 10 -24 (same mass as proton) Mass (amu)= 1.0082 = 1 Number of neutrons CAN change for an element ISOTOPES Stabilizes nucleus by nuclear force
Common Charge notation is -1 Mass (g) of e- = 9.109 x 10 -28 Mass (amu)=.0006 = 0 Number of electrons CAN change for an element IONS Responsible for chemical reactivity, forms bonds
ProtonNeutronElectron LocationNucleus Outside of nucleus Common charge+0_ Mass, g1.673x10 -24 1.675 x 10 -24 9.109 x 10 -24 Mass, amu110
Which subatomic particle can NOT change for an element and gives it’s identity? Which subatomic particle stabilizes the nucleus?
Atomic Number: The number of protons in each atom of that element. Unique to EACH element, never changes!! Neutral atoms: proton #= electron # Example: 1. How many protons does Beryllium (Be) have? How many electrons? 2. How many protons does Gold (Au) have?
Isotopes: Are atoms that have different number of neutrons So masses are different Example of isotopes:
Mass Number: The total number of protons and neutrons in the nucleus
Element- Mass number What is the hyphen notation of lithium if the mass number is 4?
Common isotopes of carbon Carbon-12 Carbon-13 Carbon-14 How many protons do all the carbon isotopes have? How many neutrons do each of the carbon isotopes have?
Atoms are Neutral because they have the same number of electrons and protons You will assume this unless indicated otherwise
Ions :are when the electron number and proton number are different leading to a net charge. What charge would Aluminum have 13 protons and 10 electrons? NOTE: YOU WILL ALWAYS ASSUME ATOMS ARE NEUTRAL (protons = electrons) UNLESS TOLD OTHERWISE
Atomic #= Proton #= Electron # (because we assume atoms are neutral) Mass #= Atomic # + Neutron #
Number of protons= Atomic number Number of electrons = Number of protons (in a neutral atom) Number of neutrons = Mass number– Atomic number SymbolAtomic # Mass ## of protons # of electrons # of neutrons Na11 1531
Average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element This number appears below the element symbol on the periodic table.