Section 2: The Structure of Atoms

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Presentation transcript:

Section 2: The Structure of Atoms

What is in an atom? The three main subatomic particles are distinguished by mass, charge, and location in the atom: electrons, protons and neutrons Proton is a subatomic particle that has a positive charge and that is located in the nucleus of an atom Neutron is a subatomic particle that has no charge and that is located in the nucleus of an atom

What is in an atom? Each element has a unique number of protons An element is defined by the number of protons Unreacted atoms have no overall charge A charged atom is called a ion The electric force holds the atom together

Atomic Number and Mass Number Atoms of each element have the same number of protons, but they can have different numbers of neutrons The atomic number equals the number of protons The mass number equals the total number of subatomic particles in the nucleus Video

Isotopes An isotope is an atom that has the same number of protons as other atoms of the same element do but that has a different number of neutrons Isotopes of an element vary in mass because their numbers of neutrons differ The number of neutrons can be calculated: Neutrons = Mass number (A) – Atomic number (Z)

Atomic Masses Because working with such tiny masses is difficult, atomic masses are usually expressed in unified atomic mass units (u) Average atomic mass is a weighted average

Atomic Masses The mole is used for counting small particles 1 mol = 602,213,670,000,000,000,000,000 particles Avogadro’s number: 6.022 x 1023 Video: What is a mole?

Atomic Masses Moles and grams are related, you can convert between moles and grams

Atomic Masses Examples:

Atomic Mass Compounds also have molar masses Video: Atomic Mass To find the molar mass of a compound, you can add up the molar masses of all of the atoms in the molecules of the compounds Video: Atomic Mass