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Chapter 7 Ionic Bonding

Chapter 7 Ionic Bonding. Bellringer. Define a cation and an anion. Give one example of each. Cations Anions. Ions. Remember: Cations – positively charged atoms that have lost electrons Anions – negatively charged atoms that have gained electrons

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Chapter 7 Ionic Bonding

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  1. Chapter 7Ionic Bonding

  2. Bellringer • Define a cation and an anion. Give one example of each. Cations Anions

  3. Ions • Remember: • Cations – positively charged atoms that have lost electrons • Anions – negatively charged atoms that have gained electrons • Valence Electrons – electrons in the highest occupied energy level of an atom • Octet Rule – all atoms want to be like noble gases and have 8 electrons

  4. Vocabulary Activity • Valence electrons • Electron dot structures • Octet rule • Halide ions • Cations • Anions • Ionic compounds • Ionic Bonds • Chemical Formula • Formula Unit • Coordination Number • Metallic Bonds • Alloys • Ionization Energy • Electronegativity • Atomic Radii • Alkali Metals • Alkaline Earth Metals • Halogens • Noble Gases • Transition Metals

  5. Ionic Bond Formation • Ionic Bond – form between a metal cation and nonmetal anion • To follow the octet rule, the cation gives up an electron(s) to the anion, which bonds the two ions together. • When the two ions bond, they become a neutrally charged compound.

  6. Electron Dot Diagrams • Electron dot diagrams can be used to illustrate how many valence electrons an atom has. • Examples:

  7. Fixed Charge Ionic Compounds Formula to Name • Steps (MgS) • The cation always comes first in the name (magnesium) • The anion comes second in the name, and the suffix “-ide” is added to the stem of the anion name (sulfide) Final name: Magnesium sulfide

  8. Fixed Charge Ionic Compounds Name to Formula • Steps (Aluminum oxide) • Write down the charge and symbol of the cation (Al3+) • Write down the charge and symbol of the anion (O2-) • Remember that ionic compounds are neutral. Use the necessary number of cations and anions to balance the charges. (2 Al and 3 O) Final formula: Al2O3

  9. Polyatomic Ion Nomenclature: Formula to Name • Rules Fe(NO3)2 • Decide if the cation shows variable change. If it does, you will have to use a Roman numeral to denote the charge. (Iron (II)) • Determine the name of the polyatomic ion. (Nitrate) Final name: Iron (II) nitrate Ca(ClO3)2 • If the cation does not show variable change, you do not need a Roman numeral (calcium) • Determine the name of the polyatomic ion (chlorate). Final name: Calcium chlorate

  10. Polyatomic Ion Nomenclature: Name to Formula • Rules (copper (II) chlorate) • The first word provides the symbol of the cation (Cu). • The Roman numeral provides the charge of the cation (+2). • The second word provides the symbol of the anion (ClO3-). • Remember the charges need to balance out, so provide the correct number of ions needed to gain a neutral charge. Final name: Cu(ClO3)2

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