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Understanding Valence Electrons and Group Properties of the Periodic Table

This chapter delves into the concept of valence electrons, which are critical for understanding an atom's chemical behavior. It covers the key groups of elements in the periodic table, including alkali metals, alkaline earth metals, and the transition through various families like boron, carbon, nitrogen, oxygen, halogens, and noble gases. Emphasis is placed on their valence electrons, reactivity, and notable characteristics. The role of these elements in everyday life and their importance in chemical reactions is also explored, providing a comprehensive overview of elemental behavior based on their group classifications.

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Understanding Valence Electrons and Group Properties of the Periodic Table

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  1. Chapter 5 Write the notes that are underlined.

  2. Valence Electrons • Electrons that are in the highest occupied energy level of an atom • Important to chemical reactions • The reason elements in a group have similar properties

  3. Alkali Metals • Group 1A (Li, Na, K, Rb, Cs, Fr) • 1 valence electron • Extremely reactive • Reactivity increases from top to bottom of group

  4. Alkaline Earth Metals • Group 2A (Be, Mg, Ca, Sr, Ba, Ra) • 2 valence electrons • Reactivity increases going down the group • Examples: • Magnesium: in chlorophyll (where plants produce energy from sunlight), makes metals stronger • Calcium: in bones for strength

  5. Boron Family • Group 3A (B, Al, Ga, In, Tl) • 3 valence electrons • Al is the most abundant metal in Earth’s crust • Recycling Al uses 5% of the energy needed to originally extract it from the Earth

  6. Carbon Family • Group 4A (C, Si, Ge, Sn, Pb) • 4 valence electrons • Metallic nature increases down the group • What does that say about conductivity? • Life on Earth is carbon based • Silicon is the 2nd most abundant element in Earth’s crust

  7. Nitrogen Family • Group 5A (N, P, As, Sb, Bi) • 5 valence electrons • N and P are found in fertilizers

  8. Oxygen Family • Group 6A (O, S, Se, Te, Po) • 6 valence electrons • O is the most abundant element in Earth’s crust

  9. Halogens • Group 7A (F, Cl, Br, I, At) • 7 valence electrons • F and Cl are gases • Br evaporates quickly • I sublimes (solid to gas without liquid phase)

  10. Noble Gases • Group 8A (He, Ne, Ar, Kr, Xe, Rn) • He has 2 valence electrons • Other 5 have 8 valence electrons • Colorless • Odorless • Extremely un-reactive

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