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I. Subatomic Particles (p )

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Presentation on theme: "I. Subatomic Particles (p )"— Presentation transcript:

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

2 Subatomic Particle Properties
Symbol Location Charge Relative Mass (amu) Actual Mass (g) e- Electron cloud 1/1840 electron 9.11 x 10-28 approx 0 p+ + proton nucleus 1 1.67 x 10-24 n0 neutron nucleus 1 1.67 x 10-24

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 # n0 = Atomic mass – Atomic number Protons Electrons Protons
Neutrons # n0 = Atomic mass – Atomic number

9 Subatomic Particles equal in a neutral atom #n0 = Atomic mass
NUCLEUS ELECTRONS equal in a neutral atom PROTONS NEUTRONS NEGATIVE CHARGE QUARKS #n0 = Atomic mass - Atomic # Atomic Number equals the # of... POSITIVE CHARGE NEUTRAL CHARGE Most of the atom’s mass.

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

11 Ch. 4.3 - Atomic Structure II. How Atoms Differ (p. 114 - 121)
Mass Number Isotopes Relative Atomic Mass Average Atomic Mass

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

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

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

15 B. Isotopes Isotope notation: Chlorine-37 atomic #: mass #:
# of protons: # of electrons: # of neutrons: 17 37 20

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 12C atom = 1.992 × 10-23 g
atomic mass unit (amu) 1 amu = 1/12 the mass of a 12C atom 1 p = amu 1 n = amu 1 e- = amu © Addison-Wesley Publishing Company, Inc.

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

19 D. Average Atomic Mass EX: Calculate the avg. atomic mass of oxygen if its abundance in nature is 99.76% 16O, 0.04% 17O, and 0.20% 18O. Avg. Atomic Mass 16.00 amu

20 D. Average Atomic Mass EX: Find chlorine’s average atomic mass if approximately 8 of every 10 atoms are chlorine-35 and 2 are chlorine-37. Avg. Atomic Mass 35.40 amu

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