Unit 3: Atomic Structure. A. Subatomic Particles Most of the atom’s mass (Mass Number) NUCLEUS ELECTRON CLOUD PROTONS NEUTRONS ELECTRONS POSITIVE CHARGE.

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Presentation transcript:

Unit 3: Atomic Structure

A. Subatomic Particles Most of the atom’s mass (Mass Number) NUCLEUS ELECTRON CLOUD PROTONS NEUTRONS ELECTRONS POSITIVE CHARGE NEUTRAL CHARGE ATOM Atomic Number equals the # of... equal in a neutral atom NEGATIVE CHARGE

A. Subatomic Particles 19 K Potassium ATOMIC NUMBER # of protons Identifies the element # of electrons in neutral atoms AVERAGE ATOMIC MASS mass of protons + neutrons

B. Mass Number 19 K Potassium MASS NUMBER = protons + neutrons round off the average atomic mass always a whole number NOT on the periodic table!!!!! 39 WHAT IS THE MASS NUMBER FOR POTASSIUM?

B. Mass Number © Addison-Wesley Publishing Company, Inc. Q: Carbon has 6 protons & 6 neutrons.What is it’s mass number? A: 12 (Carbon-12)

C. Isotopes  Atoms of the same element with different mass numbers (This means they have different # of neutrons. Mass # Atomic #  Nuclear symbol:  Hyphen notation: Iron-56 Fe 56 26

© Addison-Wesley Publishing Company, Inc. HOW DO THESE ELEMENTS DIFFER? SAME ELEMENT, BUT DIFFERENT # OF NEUTRONS  ISOTOPES

C. Isotopes  To find # of neutrons: Mass # Atomic # # of Neutrons = 6 mass number - atomic number

Example  Chlorine-37 atomic #: mass #: # of protons: # of electrons: # of neutrons:

D. Ions  Atoms with a (+) or (-) charge due to a gain or loss of electron(s) Positive Ion: loss of e- Ex: Ca 2+ Lost 2 e- Negative Ion: gain of e- Ex: Cl - Gained 1 e-

Examples  Br – __________  Al 3+ _________  Mg 2+ ________  Na + _________  O 2- __________  I - ____________ Gains 1 e- Loses 3 e- Loses 2 e- Loses 1 e- Gains 2 e- Gains 1 e-

E. Relative Atomic Mass  Carbon-12 atom has a mass of = × g (very small number)  1 p+ = amu 1 n = amu 1 e - = amu  So we use atomic mass unit (amu)  1 amu= 1 / 12 the mass of a 12 C atom

F. Average Atomic Mass  A weighted average of all isotopes  Given on the Periodic Table  round to 2 decimal places Avg. Atomic Mass

Avg. Atomic Mass F. 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

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