Examining Atomic Structure (2.2.2) Flashcards
• Isotopes of an element have the same number of protons, but different numbers of neutrons.
• Isotopes of an element have the same number of protons, but different numbers of neutrons.
• The atomic mass unit (amu) is a convenient unit for describing the masses of atoms.
• The atomic mass unit (amu) is a convenient unit for describing the masses of atoms.
• The relative atomic mass expresses the weighted average of the masses of all naturally occurring isotopes of an element.
• The relative atomic mass expresses the weighted average of the masses of all naturally occurring isotopes of an element.
• The difference in mass between a nucleus and its constituent nucleons is released as the binding energy, E = mc2.
• The difference in mass between a nucleus and its constituent nucleons is released as the binding energy, E = mc2.
Isotopes of an element have the same number of
protons, but different numbers of neutrons.
The number of protons in the nucleus of an atom
determines the type of element. For example, every
isotope of carbon has 6 protons in the nucleus. The
number of protons is designated by a subscript
number before the element symbol.
The total number of protons and neutrons (the
number of nucleons) in the nucleus of an atom is
designated by a superscripted number before the
element symbol. For example, carbon-12 (12C) has
a total of 12 nucleons. Since 6 of these are protons,
the other 6 have to be neutrons. Similarly, carbon-
13 (13C) has a total of 13 nucleons—6 protons and 7
neutrons.
Isotopes of an element have the same number of
protons, but different numbers of neutrons.
The number of protons in the nucleus of an atom
determines the type of element. For example, every
isotope of carbon has 6 protons in the nucleus. The
number of protons is designated by a subscript
number before the element symbol.
The total number of protons and neutrons (the
number of nucleons) in the nucleus of an atom is
designated by a superscripted number before the
element symbol. For example, carbon-12 (12C) has
a total of 12 nucleons. Since 6 of these are protons,
the other 6 have to be neutrons. Similarly, carbon-
13 (13C) has a total of 13 nucleons—6 protons and 7
neutrons.
Mass Number
The total number of nucleons in an atom
Atomic Number
The number of protons in an atom
Relative Atomic Mass
The weighted average of the masses of the isotopes of an element.
Binding Energy
The energy required to break a nucleus apart into protons and neutrons.
