I. Subatomic Particles (p.113 - 114). ParticleSymbolLocationChargeRelative Mass (amu) Actual Mass (g) electron proton neutron e-e- p+p+ n0n0 Electron.

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Presentation transcript:

I. Subatomic Particles (p )

ParticleSymbolLocationChargeRelative Mass (amu) Actual Mass (g) electron proton neutron e-e- p+p+ n0n0 Electron cloud nucleus – + 0 1/ x x approx 0

 Elements are listed by their chemical symbols  Symbols are usually either one capital letter like C for Carbon, or one capital and one lowercase letter like Ne for Neon

 The periodic table gives much information we need to learn more about the atom of each element

 Atomic number = # of protons in an atom  Whole number shown on periodic table  Periodic table is arranged by atomic number

 The average atomic mass is the number at the bottom of this square  Found by averaging the natural abundances of its isotopes  Weighted average

Atomic Number Symbol Element Name Atomic Mass

Protons Electrons ProtonsNeutrons # n 0 = Atomic mass – Atomic number

Most of the atom’s mass. NUCLEUS ELECTRONS PROTONS NEUTRONS NEGATIVE CHARGE POSITIVE CHARGE NEUTRAL CHARGE ATOM QUARKS #n 0 = Atomic mass - Atomic # equal in a neutral atom Atomic Number equals the # of...

 Quarks ◦ component of protons & neutrons ◦ 6 types  3 quarks = 1 proton or 1 neutron He

II. How Atoms Differ (p )  Mass Number  Isotopes  Relative Atomic Mass  Average Atomic Mass

 mass # = protons + neutrons always a whole number NOT on the Periodic Table! © Addison-Wesley Publishing Company, Inc.

 Atoms of the same element with different numbers of neutrons Mass # Atomic # Isotope notation: Isotope name: carbon-12 Element name Mass #

© Addison-Wesley Publishing Company, Inc.

 Chlorine-37 ◦ atomic #: ◦ mass #: ◦ # of protons: ◦ # of electrons: ◦ # of neutrons: Isotope notation:

 Most elements are found as mixtures of isotopes  Relative abundance of each isotope is the same in each source

 12 C atom = × g 1 p= amu 1 n = amu 1 e - = amu © Addison-Wesley Publishing Company, Inc. atomic mass unit (amu) 1 amu= 1 / 12 the mass of a 12 C atom

 weighted average of all isotopes  on the Periodic Table  round to 2 decimal places Avg. Atomic Mass

Avg. Atomic Mass  EX: Calculate the avg. atomic mass of oxygen if its abundance in nature is 99.76% 16 O, 0.04% 17 O, and 0.20% 18 O amu

Avg. Atomic Mass  EX: Find chlorine’s average atomic mass if approximately 8 of every 10 atoms are chlorine-35 and 2 are chlorine amu