Periodic Table, Atomic Number & Isotopes Why We Use What We Do Periodic Table, Atomic Number & Isotopes

The Periodic Table Mid 1800’s 60 Different Elements were identified 5 were gases at room temperature (all non-metals) H, O, N, F, Cl 2 were liquids Hg (metal) Br (non-metal) The rest were solids

The Periodic Table Construction of The Periodic Table Elements with similar properties were placed near one another. Dimitri Mendeleev In 1869 he published a periodic table

Mendeleev’s Periodic Table

The Periodic Table Mendeleev’s Table arranged by Atomic Weight (Molar Mass) Combining Capacity Chemical Properties NaCl vs CuCl2 Modern Periodic Table arranged by Atomic Number Number of valence electrons Supports Combining Capacity Properties

The Periodic Table Atomic Number Determined by the number of Protons in the nucleus Positive Particles (p+) Each element has its own atomic number Na = 11 protons (p+) Identify every atoms as a particular element by this number.

Molar Mass

The Periodic Table Mass Number Mass # = (p+) + (n0) Does not include (e-) (e-) too small to contribute to the overall mass of the atom. Mass number changes when the number of neutrons change.

The Periodic Table Isotopes: Atoms with the same number of (p+) but a different number of (n0). Atoms of the same element with different mass #’s 14C = Radioactive 12C = Non-radioactive For Example Hydrogen (H with one (p+) but no (n0) ) and Deuterium (H with one (p+) and one (n0) ). ttp://web.visionlearning.com/custom/chemistry/animations/CHE1.3-an-isotopes.shtml

The Periodic Table Why use Atomic Number rather than Molar Mass (atomic weight)? Organization by Molar Mass (atomic weight) works well for small atomic weights but not large ones. Due to many varieties of isotopes

The Periodic Table Vertical arrangement Elements with similar properties were placed in vertical Groups (columns) or Families.

Group Molar Mass

Molar Mass Group

Molar Mass Group

Molar Mass Group

Molar Mass Group Etc.

The Periodic Table Horizontal arrangement Placed by increasing atomic weights in rows called Periods.

Molar Mass Periods

Periods Molar Mass

Periods Molar Mass

Molar Mass Periods

Molar Mass Periods Etc.

Families/Groups Alkali Metals Group 1 – Lithium, Sodium, Potassium, Rubidium, Cesium, Francium 1 electron in valence (outer) shell Very, VERY reactive – not found free in nature Alkali Metal Clip

Family/Group Alkaline Earth Metals Group 2 – Beryllium, Magnesium, Calcium, Strontium, Barium, Radium 2 electron in valence shell Very reactive – not usually found pure in nature

Families/Groups Nobel Gases Group 18 – Helium, Neon, Argon, Krypton, Xenon, Radon Full valence electron shell Very stable (not reactive) Under normal conditions do not form compounds with other elements XeF4 (xenon tetrafluoride) is the first reported stable compound of a noble gas - 1962

Families/Groups Halogens Group 17 – Fluorine, Chlorine, Bromine, Iodine, Astatine 7 electrons in valence shell Halogen means “salt former” Compounds they form are called salts

Families/Groups Transition Metals Groups 3 to 12, periods 4 to 7 1, 2, or 3 electrons in valence electron shell Hard and have a high melting point Often used to form alloys (mixtures of metals)

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