History Dmitri Mendeleev 1896 1951 - Seaborg Developed the modern periodic table.

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Presentation transcript:

History Dmitri Mendeleev 1896

Seaborg Developed the modern periodic table

The Whole Periodic table

Groups vs. Periods Need to Know: Halogens Noble Gas Alkali Metals Alkaline Earth Transition Metals Lanthanides Actanides Groups: Up and Down Periods: Left to Right

Periodic Table Atomic Number Atomic Mass Name Symbol **Mass Number can not be found on the periodic table

Element Symbol Symbol Atomic Number Mass Number

Atoms What do we know MUST be in an atom? (3 particles)

Ions How is an ion formed?

If an ion has a charge of -2, what has happened to the atom? Ions If an ion has a charge of +2, what has happened to the atom? The atom has gained two electrons The atom has lost two electrons

Isotopes Count the neutrons and protons Proton Neutron

Natural State of an Element

Questions?

Quiz Time Acceptable Answers Correct Answer

Good Luck You have 7 minutes to complete your quiz. When you are done, hold on to it and wait patiently.

1 copper atom = x kg on average 69.2% of Cu atoms are x kg 30.8% of Cu atoms are x kg 1 copper penny = x kg x kg 1 Cu atom = x atoms x kg Relative Size

Average Atomic Mass Calcs 1 atomic mass unit (amu) = x kg, Mass of an electron = x kg Mass of a proton = x kg Mass of a neutron = x kg **You will NOT need to memorize these numbers. Always given to you. Relative Size

Carbon has 2 common isotopes C and 13 6 C. If the abundance of the two isotopes is 98.89% and 1.11 % respectively, what is the average atomic mass of carbon in amu? Average Atomic Mass Calcs Carbon 12Carbon 13 Neutrons Protons Electrons

12 6 C 6 neutrons x kg1 amu = amu 1 neutron x kg 6 electrons x kg1 amu = amu 1 electron x kg 6 protons x kg1 amu = amu 1 proton x kg amu amu amu = amu

6 protons x kg1 amu = amu 1 proton x kg 7 neutrons x kg1 amu = amu 1 neutron x kg 6 electrons x kg1 amu = amu 1 electron x kg amu amu amu = amu 13 6 C

Putting It All Together What we know: Carbon 12: amu (98.89% abundance) Carbon 13: amu (1.11% abundance) Therefore: ( amu x ) + ( amu x ) amu

Homework *Attempt problem #1 on Average Atomic Mass Calculations WS Read and notes 3.5, 3.7, 3.8