4.3 Atomic Number Atomic Number What makes one element different from another? 4.3 Atomic Number Elements are different because they contain different numbers of protons. The atomic number of an element is the number of protons in the nucleus of an atom of that element. 4.3 Atomic Number for Conceptual Problem 4.1 4.3 Mass Number Mass Number How do you find the number of neutrons in an atom? 4.3 Mass Number The total number of protons and neutrons in an atom is called the mass number. The number of neutrons in an atom is the difference between the mass number and atomic number. 4.3 Mass Number Au is the chemical symbol for gold. 4.1 for Sample Problem 4.1 4.3 Isotopes Isotopes How do isotopes of an element differ? 4.3 Isotopes Isotopes are atoms that have the same number of protons but different numbers of neutrons. Because isotopes of an element have different numbers of neutrons, they also have different mass numbers. 4.3 Isotopes Despite these differences, isotopes are chemically alike because they have identical numbers of protons and electrons. for Conceptual Problem 4.2 4.3 Atomic Mass Atomic Mass How do you calculate the atomic mass of an element? 4.3 Atomic Mass It is useful to compare the relative masses of atoms to a standard reference isotope. Carbon-12 is the standard reference isotope. Cabon-12 has a mass of exactly 12 atomic mass units. An atomic mass unit (amu) is defined as one twelfth of the mass of a carbon-12 atom. It is based on the mass of a proton or neutron. 1 gram = 6.02 x 1023 amu’s (Avagadro’s number) 1 amu = 1.67 x 10-24 grams 4.3 Atomic Mass Some Elements and Their Isotopes 4.3 Atomic Mass The atomic mass of an element is a weighted average mass of the atoms in a naturally occurring sample of the element. A weighted average mass reflects both the mass and the relative abundance of the isotopes as they occur in nature. 4.3 Atomic Mass Weighted Average Mass of a Chlorine Atom for Conceptual Problem 4.3 for Conceptual Problem 4.3 4.3 Atomic Mass To calculate the atomic mass of an element, multiply the mass of each isotope by its percent relative abundance, expressed as a decimal, and then add the products. 4.3 Atomic Mass For example, carbon has two stable isotopes: • Carbon-12, which has a relative abundance of 98.89%, and • Carbon-13, which has a relative abundance of 1.11%. 4.3 The Periodic Table—A Preview The Periodic Table—A Preview Why is a periodic table useful? 4.3 The Periodic Table—A Preview A periodic table is an arrangement of elements in which the elements are separated into groups based on a set of repeating properties. A periodic table allows you to easily compare the properties of one element (or a group of elements) to another element (or group of elements). 4.3 The Periodic Table The Periodic Table—A Preview 4.3 The Periodic Table—A Preview • Each horizontal row of the periodic table is called a period. • Within a given period, the properties of the elements vary as you move across it from element to element. 4.3 A Period The Periodic Table—A Preview 4.3 The Periodic Table—A Preview • Each vertical column of the periodic table is called a group, or family. • Elements within a group have similar chemical and physical properties. 4.3 A Group or Family The Periodic Table—A Preview 4.3 Section Quiz 1. Isotopes of an element have a. the same mass number. b. different atomic numbers. c. the same number of protons but different numbers of neutrons. d. the same number of protons but different numbers of electrons. 4.3 Section Quiz 2. How many neutrons are in sulfur-33? a. 16 neutrons b. 33 neutrons c. 17 neutrons d. 32.06 neutrons 4.3 Section Quiz 3. If sulfur contained 90.0% sulfur-32 and 10.0% sulfur-34, its atomic mass would be a. 32.2 amu. b. 32.4 amu. c. 33.0 amu. d. 35.4 amu. END OF SHOW