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Ch. 4.2 - Atomic Structure I. Subatomic Particles (p.113 - 114)

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Presentation on theme: "Ch. 4.2 - Atomic Structure I. Subatomic Particles (p.113 - 114)"— Presentation transcript:

1 Ch Atomic Structure I. Subatomic Particles (p )

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

3 Symbols 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

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

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

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

7 Atom Math Atomic Number Symbol Element Name Atomic Mass

8 Atom Math Protons Electrons ProtonsNeutrons # n 0 = Atomic mass – Atomic number

9 Subatomic Particles Most of the atoms 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...

10 Subatomic Particles Quarks component of protons & neutrons 6 types 3 quarks = 1 proton or 1 neutron He

11 Ch Atomic Structure II. How Atoms Differ (p ) Mass Number Isotopes Relative Atomic Mass Average Atomic Mass

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

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

14 B. Isotopes © Addison-Wesley Publishing Company, Inc.

15 B. Isotopes Chlorine-37 atomic #: mass #: # of protons: # of electrons: # of neutrons: Isotope notation:

16 Natural Abundances of Isotopes Most elements are found as mixtures of isotopes Relative abundance of each isotope is the same in each source

17 C. Relative Atomic Mass 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

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

19 Avg. Atomic Mass D. Average 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

20 Avg. Atomic Mass D. Average Atomic Mass EX: Find chlorines average atomic mass if approximately 8 of every 10 atoms are chlorine- 35 and 2 are chlorine amu

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