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Chem Do Now

Chem Do Now. Hand me all assignments you are submitting Gather all your materials Find your name on the seating chart on the board up front and move your seat. By the time the timer is up, you should be seated with your notes pages out.

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Chem Do Now

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  1. Chem Do Now • Hand me all assignments you are submitting • Gather all your materials • Find your name on the seating chart on the board up front and move your seat. • By the time the timer is up, you should be seated with your notes pages out. • Anyone not in their assigned seat at the time of the buzzer must go get a late pass. • Talk to me AFTER CLASS if you have an issue, I WILL NOT move you today during class.

  2. Ions

  3. Nuclear Charge • In the nucleus there are protons and neutrons • Protons are positive • Neutrons are neutral • If the nucleus has 3 protons it has a charge of 3+

  4. Neutral Atom In a neutral atom, there are equal numbers of protons and electrons Each positive is cancelled by a negative.

  5. Ions • In an ion, there are unequal numbers of protons and electrons 3 + charge 4 – charge 1 – charge

  6. Ions • In an ion, there are unequal numbers of protons and electrons 3 + charge 2 – charge 1 + charge

  7. What is the charge of an ion that has 12 protons and 13 electrons?

  8. What is the charge of an ion that has 54 protons and 52 electrons?

  9. What is the charge of an ion that has 29 protons and 32 electrons?

  10. What is the charge of a SR ion that loses two electrons?

  11. What is the charge of a Fluorine atom that gains one electron?

  12. What is the charge of an Oxygen ion that gains two electrons?

  13. Now for some practice • Complete the back page of your notes by your self. • When the timer is up, partner up and share your answers. • Work together to make sure you and your partner agree on every answer. • We will go over this as a class

  14. POGIL: Ion Formation • Complete the Ion formation activity with your group members • Hand in your sheet when completed • If you finish early you may work on your homework until time is up.

  15. Chemical Bonding

  16. Electron Review • The electron configuration shows the location of all of the electrons in an atom • Valence electrons are the electrons in the outer most shell • Valence electrons are represented in Lewis Dot Structures • The charge of a particular atom can be found by subtracting the number of electrons (given by the electron configuration) from the number of protons (given by the atomic number)

  17. Noble Gas Configuration • Elements will gain or lose electrons to obtain a noble gas configuration (full outer shell). • Metals tend to lose electrons • Nonmetals tend to gain electrons Current Electron Configuration 2-8-8-1 After losing an electron Nobel gas configuration 2-8-8

  18. Energetically Stable • By achieving the noble gas configuration, the atom becomes more energetically stable (reaches a lower energy state). e-

  19. Gaining or Losing Electrons • When an electron is gained or lost, it isn’t being pulled out of air or released into space. • Electrons are always taken from or given to other atoms.

  20. Bonding • When electrons are transferred, shared or pooled between atoms, a bond is formed. • A bond represents increased stability between two atoms.

  21. Spectrum of Bonding There are many different types of bonding. Ionic Bonding CovalentBonding Electron Transferred Electron Attracted Electron Shared MetallicBonding IntermolecularBonding

  22. Types of Bonding • Ionic Bonding: when electrons are transferred between atoms (Metal and Nonmetal) • Metallic Bonding: when electrons are pooled among atoms (all Metal) • Covalent Bonding: when electrons are shared between two atoms (all Nonmetals) • Intermolecular bonding: When an atom is attracted to electrons in another molecule (between covalent molecules)

  23. Ions Quick Facts • When do ions gain or lose? - 1, 2, or 3 valence electrons will lose those electrons - 5, 6, or 7 valence electrons will gain electrons • Always want to get to a full outer level (usual 8 electrons) • To find overall charge: • 1. Add the number of protons • 2. Add the number of electrons when in balanced state • 3. Add/sub the number of electrons changing by (lose = subtract; gain = add). • Remember: electrons are NEGATIVE • Answer should be: -3, -2, -1, 0, +1, +2, +3. Rarely will you have a charge grater than 3.

  24. Ions Con’t • To write the notation of an ion: 1. write the element symbol 2. in the upper right corner write the charge Practice: Li F O • Atoms that gain electrons are cations • Atoms that lose electrons are anions

  25. Ionic Bonding • In ionic bonding, the electron is completely transferred from one atom to another. • Both atoms become charged ions. - + Na Cl

  26. Ionic Bonding Positive ions will lose all electrons. Negative ions will gain until they have 8. If need be, an atom will give away electrons to many different atoms - Cl + 2 Mg - Cl

  27. Practice Draw Lewis Dot diagrams for each of the following atomic pair and show electrons transferred. Na and F Al and Cl Na and O

  28. Do Now: Update TOC • Ion Formation • POGIL: Ion Formation • Atoms and Ions HW • Chemical Bonding • Chemical bonding con’t • Ionic Bonds Activity • Ionic Bonding Worksheet • Naming Ionic Compounds Notes • POGIL: Naming Ionic Compounds 9-a POGIL Con’t 10. Ionic Bonding Practice 11. Writing Ionic Compounds Guided Practice 12. Bond with a classmate 13. Chemical Bonding

  29. Ionic Formulas • Formulas represent the number of ions that are involved in bonding. • In the formula MgCl2, one magnesium atom is ionically bonded with two atoms of chlorine. • In the formula NaCl, one sodium atom is ionically bonded with one atom of chlorine.

  30. Formula Writing When writing formulas for ionic systems, always write the cation (positively charged ion) first. MgCl2 Cl2Mg

  31. Writing Ionic Compound Formulas Boron Fluoride • Find the two elements (metal and Non-metal) on the periodic table. • Write their oxidation numbers above. • Criss Cross • Reduce 3+ 1- B F BF3

  32. Nature of ionic Bonds • Charged atoms are attracted to opposite charges much like magnets are. • However, nothing more is holding the atoms together. + -

  33. Formula Units • Since no ion is specifically bonded with another ion, we cannot refer to ionic compounds as molecules. • Instead, we refer to ionic compounds as formula units (the ratio of cations to anions in the solid).

  34. Bonding Basics Activity • One group member come get a “white board” • One group member get a marker • One group member get counters • Take out the Bonding Basics Sheet • Wait for further instructions

  35. Completing the chart Completing the Ionic Bonds Step 1- Write the Element Symbols on white boards Step 2- Add counters to create Lewis Structures Step 3- Move the electron to complete the shell Step 3- Draw a model like the one to the right on your paper that represents what you did on the white board Step 4- Write the notation for each ion Step 5- Write the equation for the new compound made by the ionic bond

  36. Naming Ionic Compounds

  37. Binary Compounds • For ionic compounds consisting of two types of atoms… NaCl The anion is given the element name ending in -ide The cation is given the element name Sodium Chloride Chlorine

  38. Common Anions • Sulfur = Sulfide • Oxygen = Oxide • Phosphorus = Phosphide • Nitrogen = Nitride • Fluorine = Fluoride • Chlorine = Chloride • Carbon = Carbide • Arsenic = Arsenide • Sellenium = Selenide • Bromine = Bromide • Iodine = Iodide

  39. What is the name for NaP? • Sodium Phosphorus • Sodium Phosphide • SodidePhosphide • Sodide Phosphorus

  40. What is the name for MgO? • Magnesium Oxygen • Magenide Oxide • Oxygen Magnenide • Magnesium Oxide

  41. Polyatomic Ions • Some ions are composed of multiple atoms covalently bonded together • These groups of ions are called polyatomic ions [OH]- Hydroxide

  42. Polyatomic Ions

  43. What is the formula for Sodium Hydrogen Carbonate? • NaHC • Na2HCO3 • NaHCO3 • NaHCO2

  44. Ions with multiple charge states • Some elements have multiple charge states possible. • To designate the charge of these ions in the formula name, we use roman numerals.

  45. Roman Numerals • 1 = I • 2 = II • 3 = III • 4 = IV • 5 = V • 6 = VI

  46. Examples Consider the following name: Copper (II) Chloride Cu Cl

  47. Practice Consider the following name: Chromium (VI) Oxide Cr O

  48. What is the formula for Iron (II) Oxide? • Fe2O • FeO • FeO2 • Fe2O2

  49. What is the formula for Vanadium (V) Bromide • VBr3 • V3Br • VBr5 • V5Br

  50. Writing Ionic Compounds Beryllium Oxide 2+ 2- Be O BeO SIMPLIFY

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