Isotopes and Ions of Atoms

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Presentation transcript:

Isotopes and Ions of Atoms Unit 3.3

Mass of Atoms Nucleus- contains most of the mass of an atom Protons & Neutrons contains most of an atom’s mass Electrons- 1/2000th of the mass of a proton or neutron Grams are not used to measure mass of atoms because atoms are too small Amu is used instead Amu = atomic mass unit Mass of proton = mass of neutron = 1amu

Masses of Atoms Protons- determine the type of element the atom is Atomic number- tells us the number of protons and located at the top of the periodic table Average atomic mass-total number of protons & neutrons and is located underneath the name of the element # of neutrons = mass # - atomic #

Masses of Atoms How many neutrons are in an atom of gold (Au)?

Answer: 118 Neutrons (197-79=118)

Masses of Atoms Isotope- Atoms of the same element with different numbers of neutrons To indicate the identity of an isotope, write the element name – mass # Copper-34, Copper-35 Average atomic mass- a weighted average of the masses of the isotopes of an element Example: Copper Av. Atomic Mass: 63.55 Atomic Number: 29 Number of Neutrons: 34.55?

Charges of Atoms Charges of atoms- indicates # of electrons gained or lost by an element Ion- an element that is positively or negatively charged Cation- ion with a positive charge- lost electrons Ex: Na +, Ba 2+ Anion- ion with a negative charge- gained electrons Ex: Cl -, O 2- Ex. NaCl Sodium chloride, or table salt, when dissolved becomes Na+ and Cl- (ionization)