Chapter 3. Atomic Number. Atomic Number. Section 3. Atoms of different elements have different numbers of protons.
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1 Section 3 Atomic Number Atoms of different elements have different numbers of protons. Atoms of the same element all have the same number of protons. The atomic number (Z) of an element is the number of protons of each atom of that element. Visual Concepts Atomic Number 1
2 Isotopes Isotopes are atoms of the same element that have different masses. The isotopes of a particular element all have the same number of protons and electrons but different numbers of neutrons. Most of the elements consist of mixtures of isotopes. Mass Number The mass number is the total number of protons and neutrons that make up the nucleus of an isotope. Designating Isotopes Hyphen notation: The mass number is written with a hyphen after the name of the element. uranium-235 Nuclear symbol: The superscript indicates the mass number and the subscript indicates the atomic number. 235 U 92 2
3 Designating Isotopes The number of neutrons is found by subtracting the atomic number from the mass number. mass number atomic number = number of neutrons 235 (protons + neutrons) 92 protons = 143 neutrons Nuclide is a general term for a specific isotope of an element. Visual Concepts Isotopes and Nuclides Average Atomic Masses of Elements Average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element. Calculating Average Atomic Mass The average atomic mass of an element depends on both the mass and the relative abundance of each of the element s isotopes. 3
4 Average Atomic Masses of Elements Calculating Average Atomic Mass Copper consists of 69.15% copper-63, which has an atomic mass of amu, and 30.85% copper-65, which has an atomic mass of amu. The average atomic mass of copper can be calculated by multiplying the atomic mass of each isotope by its relative abundance (expressed in decimal form) and adding the results. Average Atomic Masses of Elements Calculating Average Atomic Mass ( amu) + ( amu) = amu The calculated average atomic mass of naturally occurring copper is amu. Relating Mass to Numbers of Atoms The Mole The mole is the SI unit for amount of substance. A mole (abbreviated mol) is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12. Avogadro s Number Avogadro s number is the number of particles in exactly one mole of a pure substance. 4
5 Relating Mass to Numbers of Atoms Molar Mass The mass of one mole of a pure substance is called the molar mass of that substance. Molar mass is usually written in units of g/mol. The molar mass of an element is numerically equal to the atomic mass of the element in atomic mass units. Relating Mass to Numbers of Atoms Gram/Mole Conversions Chemists use molar mass as a conversion factor in chemical calculations. For example, the molar mass of helium is 4.00 g He/mol He. To find how many grams of helium there are in two moles of helium, multiply by the molar mass g He 2.00 mol He = 8.00 g He 1 mol He Relating Mass to Numbers of Atoms Conversions with Avogadro s Number Avogadro s number can be used to find the number of atoms of an element from the amount in moles or to find the amount of an element in moles from the number of atoms. In these calculations, Avogadro s number is expressed in units of atoms per mole. 5
6 Solving Mole Problems Determining the Mass from the Amount in Moles 6
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