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Understanding the Periodic Table: Groups, Periods, and Chemical Properties

This resource explores the periodic table, focusing on its structure with groups and periods. It covers main-group elements, including noble gases, halogens, alkali metals, and alkaline-earth metals, detailing their valence electrons and chemical properties. Readers will learn about trends like atomic size, ionization energy, electronegativity, and electron affinity. The text also discusses filling electron orbitals, general rules for electron configurations, and shorthand notation for electron configurations, making complex topics accessible for learners.

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Understanding the Periodic Table: Groups, Periods, and Chemical Properties

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  1. Mr. Nelson Chemistry The Periodic Table

  2. Periodic Table • Group – Vertical columns on PT • Period – Horizontal rows on PT

  3. Main-Group Elements • Groups 1, 2, and 13-18

  4. Main-Group Elements • The chemical properties of the main-group elements depends on their number of valence electrons • Valence electrons are the outermost electrons involved in chemical bonding

  5. Valence Electrons & Chemical Properties • Each group of the main-group elements has the same number of valence electrons • Each element wants to be as stable as possible • All main-group elements want a full shell of electrons, which is 8 valence electrons

  6. Valence Electrons & Chemical Properties • Each group forms ions based on the easiest way to obtain this full shell • Also known as the octet rule

  7. Family Groups • Noble Gases (Group 18) • Examples: Ne, Xe • Description: stable, unreactive group of gases • Number of Valence Electrons: 8 • Forms NO ions

  8. Family Groups • Halogens (Group 17) • Examples: F, Cl • Description: Highly reactive group of gases • Number of Valence Electrons: 7 • Forms 1- ions

  9. Family Groups • Alkali Metals (Group 1) • Examples: Na, K (not H) • Description: Highly reactive group of metals • Number of Valence Electrons: 1 • Forms 1+ ions

  10. Brainiac Movie

  11. Family Groups • Alkaline-Earth Metals (Group 2) • Examples: Be, Mg • Description: Slightly less reactive group than alkali metals • Number of Valence Electrons: 2 • Forms 2+ ions

  12. Family Groups • Transition Metals (Group 3 – 12) • Examples: Fe, Au, Ag • Description: Fairly stable group of metals • Forms multiple ions

  13. Family Groups • Lanthanides & Actinides • Location: Bottom 2 periods of PT • Description: Heavy metals, synthetics, radioactive

  14. States of Matter • Metals and Nonmetals (Staircase)

  15. Periodic Table Trends • Atomic Size • Definition: The volume occupied by the electrons around a nucleus • Period Trend • Caused by: Increasing Effective Nuclear Charge

  16. Atomic Size • Effective nuclear charge is the amount of charge felt by outer electrons in an atom • Group trend • Caused by: Increasing electron energy levels

  17. Ionization Energy • Definition: The amount of energy required to remove one electron • Period trend • Caused by: Inc. Effective Nuclear Charge

  18. Ionization Energy • Group trend • Caused by: Electron shielding • Electron shielding occurs when inner electrons shield outer electrons from the pull of the nucleus

  19. Electron Affinity • Definition: The attraction of an atom for an electron • Period Trend • Caused by: Inc. Eff. Nuclear Charge

  20. Electron Affinity • Group trend • Caused by: Inc. electron shielding

  21. Electronegativity • Definition: How much an atom in a chemical bond attracts electrons • Period trend • Caused by: Inc. Eff. Nuclear Charge

  22. Electronegativity • Group trend • Caused by: Electron shielding/Inc. electron energy levels

  23. Filling Electron Orbitals • Orbitals are the area in space where electrons are found • Each individual orbital holds 2 electrons • There are four main shapes which hold a different number of electrons

  24. Shapes of Orbitals • The four shapes are s, p, d, and f

  25. Shapes of the Orbitals • Each shape holds a different number of orbitals • s has 1 orbital, p has 3 orbitals, and d has 5 orbitals • www.ptable.com

  26. Energy Levels • Each period is a new energy level • Like an elevator, electrons cannot exist between energy levels!

  27. General Rules • Aufbau Principle – Electrons fill lowest energy level first • Analogy: Lazy Tenant Rule

  28. General Rules • Pauli Exclusion Principle – Electrons must have opposite spin (up/down) when in the same orbital • Analogy: Yin and Yang Rule

  29. General Rules • Hund’s Rule – Electrons in equal energy orbits fill orbitals with parallel spin • Analogy: Empty Bus Seat Rule

  30. Orbital Notation • Specific order for filling electrons – based on periodic table • Examples • Beryllium • Oxygen

  31. Orbital Notation • Examples • O2- • Titanium

  32. Electron Configuration • Examples • Silicon • Selenium • Manganese

  33. Shorthand Electron Config • Shorter version of writing electron configurations • Noble Gas Core – inner core of electrons not involved in chemical bonding

  34. Shorthand Electron Config

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