1. The handle of this titanium mug was joined to the body by welding. At the welding temperature, titanium reacts with oxygen in the air, forming an oxide. The oxide makes the weld more brittle. Chemical properties, such as reactivity, depend on an element’s electron configuration.

2.  When their highest (outermost) energy level is filled H & He=2valence electrons  H & He = 2 valence electrons All other atoms= 8 valence electrons (OCTET RULE)  All other atoms = 8 valence electrons (OCTET RULE)

3. STABILITY OF ATOMS: Determined by valence electrons When ELECTRON ARRANGEMENT is UNSTABLE substances change chemically CHEMICAL CHANGE: the formation of one or more new substances.

4. The chemical properties of an element depend on the number of valence electrons. An electron dot diagram is a model of an atom in which each dot represents a valence electron. The symbol in the center represents the nucleus and all the other electrons in the atom. Stable Electron Configurations

5. How Do We Show if Highest Energy Level is Filled? ELECTRON DOT DIAGRAM: model of the atom that SHOWS VALENCE e - ONLY, NOT every e-

6. Stable Electron Configurations

7. Noble gases are the most stable elements. The highest occupied energy level of a noble gas atom is completely filled. Noble gases have stable electron configurations with eight valence electrons (two electrons in the case of helium). Elements react to achieve electron configurations similar to those of noble gases. Stable Electron Configurations

8. REACTIVITY: If the HIGHEST ENERGY LEVEL is FILLED with e - the substance will PROBABLY NOT REACT. EX: (NOBLE GASES: 8 valence e - ).If the HIGHEST ENERGY LEVEL is FILLED with e - the substance will PROBABLY NOT REACT. EX: (NOBLE GASES: 8 valence e - ). If the HIGHEST ENERGY LEVEL is NOT FILLED with e- the substance will PROBABLY REACT.If the HIGHEST ENERGY LEVEL is NOT FILLED with e- the substance will PROBABLY REACT. EX: (ALKALI METALS: 1 valence e-) EX: (ALKALI METALS: 1 valence e-)

9. What Happens When Substances React? if substances react, e - get transferred.if substances react, e - get transferred. When e - are transferred, atoms are NOT NEUTRAL.When e - are transferred, atoms are NOT NEUTRAL.

10. ION: an atom with charge. ANION: GAINS one or more e - ANION: GAINS one or more e - NEGATIVE charge (A Negative ION) CATION: LOSES one or more e - CATION: LOSES one or more e - POSITIVE charge

11. What is one way in which elements can achieve stable electron configurations? Ionic Bonds Some elements achieve stable electron configurations through the transfer of electrons between atoms.

12. Transfer of Electrons Chlorine has one electron fewer than an argon atom.  Adding one electron gives chlorine a stable configuration. Sodium has one more electron than a neon atom.  Removing one electron gives sodium a stable configuration. Ionic Bonds

13. When sodium reacts with chlorine,. ? Ionic Bonds

14. When sodium reacts with chlorine, an electron is transferred from each sodium atom to a chlorine atom Ionic Bonds

15. When sodium reacts with chlorine, an electron is transferred from each sodium atom to a chlorine atom. Each atom ends up with a more stable electron arrangement than it had before the transfer. Ionic Bonds

16. Formation of Ions When an atom gains or loses an electron, the number of protons is no longer equal to the number of electrons. The charge on the atom is not balanced, and the atom is not neutral. An atom that has a net positive or negative electric charge is called an ion. Charge on an ion is represented by a plus or a minus sign Cl - or Na + Ionic Bonds

17. When chlorine atom gains an electron, it has 17 protons and 18 electrons. Ion has a charge of 1–. Written as Cl 1–, or Cl – for short. An ion with a negative charge is an anion. Anions like the Cl – ion are named by using part of the element name plus the suffix –ide. Thus, Cl – is called a chloride ion. Ionic Bonds

18. A sodium ion has 11 protons and 10 electrons. The sodium ion has a charge of 1+. Written Na 1+, or Na + for short. An ion with a positive charge is a cation. Ionic Bonds

19. Formation of Ionic Bonds A particle with a negative charge will attract a particle with a positive charge. A chemical bond is the force that holds atoms or ions together as a unit. An ionic bond is the force that holds cations and anions together. An ionic bond forms when electrons are transferred from one atom to another. Ionic Bonds

20.  What will take less energy?  Gaining electrons to have a full shell  Losing electrons to have an empty shell

21. ION EXAMPLES ANION: Chlorine (Cl - ) gains one e - to become more stable forming a chloride ion. ANION: Chlorine (Cl - ) gains one e - to become more stable forming a chloride ion. CATION: Sodium (Na + ) loses one e - to become more stable forming a sodium ion. CATION: Sodium (Na + ) loses one e - to become more stable forming a sodium ion.

22. IONIZATION ENERGY: AMOUNT OF ENERGY used to REMOVE AN e - from an atom. AMOUNT OF ENERGY used to REMOVE AN e - from an atom. lower ionization energy = easier to remove e- lower ionization energy = easier to remove e- INCREASES from LEFT TO RIGHT INCREASES from LEFT TO RIGHT DECREASES from TOP TO BOTTOM DECREASES from TOP TO BOTTOM

23. Ionization Energy Cations form when electrons gain enough energy to escape from atoms. The energy allows electrons to overcome the attraction of the protons in the nucleus. The amount of energy used to remove an electron is called ionization energy. The lower the ionization energy, the easier it is to remove an electron from an atom. Ionic Bonds

24. This figure shows two trends for ionization energy. Ionic Bonds

25. Compounds that contain ionic bonds are ionic compounds, which can be represented by chemical formulas. A chemical formula is a notation that shows what elements a compound contains and the ratio of the atoms or ions of those elements in the compound. The chemical formula for sodium chloride, NaCl, indicates one sodium ion for each chloride ion in sodium chloride. Ionic Compounds

26. What is the chemical formula for magnesium chloride? Ionic Compounds

27. What is the chemical formula for magnesium chloride? Ionic Compounds

28. What is the chemical formula for magnesium chloride? Ionic Compounds

29. What is the chemical formula for magnesium chloride? A magnesium atom cannot reach a stable electron configuration by reacting with just one chlorine atom. It must transfer electrons to two chlorine atoms. After the transfer, the charge on the magnesium ion is 2+ and its symbol is Mg2+. Ionic Compounds

30. The formula for magnesium chloride is MgCl 2. The 2 written to the right and slightly below the symbol for chlorine is used to show the relative numbers of atoms of the elements present. Magnesium chloride is used to control dust on unpaved roads. Ionic Compounds

31. Crystal Lattices A chemical formula for an ionic compound tells you the ratio of the ions in the compound, but not how the ions are arranged. If you looked at a sample of sodium chloride with a hand lens or microscope, you would be able to see that the pieces of salt are shaped like cubes. The crystal shape is a clue to how the sodium and chloride ions are arranged in the compound. Ionic Compounds

32. I ons in sodium chloride are arranged in an orderly, three-dimensional structure. Each chloride ion is surrounded by six sodium ions, and each sodium ion is surrounded by six chloride ions. Each ion is attracted to all the neighboring ions with an opposite charge. This set of attractions keeps the ions in fixed positions in a rigid framework, or lattice. Ionic Compounds

33. The structure and shape of a crystal are related: A In a sodium chloride crystal, each ion is surrounded by six oppositely charged ions. B Sodium chloride crystals are shaped like cubes Ionic Compounds

34. The shape of an ionic crystal, for example, the cubic shape of a sodium chloride crystal, depends on the arrangement of ions in its lattice. The arrangement of the ions depends on the ratio of ions and their relative sizes. Crystals are classified into groups based on the shape of their crystals. Ionic Compounds

35. Properties of Ionic Compounds The properties of sodium chloride are typical of ionic compounds. Sodium chloride has a high melting point (801°C). Solid sodium chloride is a poor conductor of electric current. When melted, it is a good conductor of electric current. Sodium chloride crystals shatter when struck with a hammer. Ionic Compounds

36. The arrangement of particles in a substance is the result of two opposing factors: the attractions among particles in the substance and the kinetic energy of the particles. The stronger the attractions among the particles, the more kinetic energy the particles must have before they can separate. Ionic compounds have strong attractions between particles and high melting points. Ionic Compounds

37. For an electric current to flow, charged particles must be able to move from one location to another. Ions in a solid crystal lattice have fixed positions. Solid sodium chloride is a poor conductor of electric current. When the solid melts, the lattice breaks apart, and the ions are free to flow. Molten sodium chloride is an excellent conductor of electric current. Ionic Compounds

38. When an ionic crystal is struck, ions are moved from their fixed positions. Ions with the same charge repel one another and the crystal shatters. Ionic Compounds Hammer strikes crystal Ionic crystal shatters when struck.

39. Assessment Questions 1. When is an atom stable? a. when its electrons are evenly distributed through its energy levels b. when its lowest occupied energy level is filled with electrons c. when its highest unoccupied energy level is filled with electrons d. when its highest occupied energy level is filled with electrons

40. Assessment Questions 1. When is an atom stable? a. when its electrons are evenly distributed through its energy levels b. when its lowest occupied energy level is filled with electrons c. when its highest unoccupied energy level is filled with electrons d. when its highest occupied energy level is filled with electrons ANS:D

41. Assessment Questions 2. Which description applies to an element that has two valence electrons? a. reactive metal b. nonreactive metal c. reactive nonmetal d. nonreactive nonmetal

42. Assessment Questions 2. Which description applies to an element that has two valence electrons? a. reactive metal b. nonreactive metal c. reactive nonmetal d. nonreactive nonmetal ANS: A

43. Assessment Questions 3. How do sodium and chlorine both achieve stable electron configurations when they react? a. An electron is transferred from the sodium atom to the chlorine atom. b. An electron is transferred from the chlorine atom to the sodium atom. c. Both atoms gain one electron. d. Both atoms lose one electron.

44. Assessment Questions 3. How do sodium and chlorine both achieve stable electron configurations when they react? a. An electron is transferred from the sodium atom to the chlorine atom. b. An electron is transferred from the chlorine atom to the sodium atom. c. Both atoms gain one electron. d. Both atoms lose one electron. ANS:A

45. Assessment Questions 4. Why do ionic compounds tend to have high melting points? a. Ionic compounds contain more than one element, which causes a high melting point. b. Ionic compounds cannot absorb energy efficiently because they contain ions. c. An ionic compound contains metal atoms that raise its melting point. d. A strong electrical attraction means ions require a lot of energy to move apart.

46. Assessment Questions 4. Why do ionic compounds tend to have high melting points? a. Ionic compounds contain more than one element, which causes a high melting point. b. Ionic compounds cannot absorb energy efficiently because they contain ions. c. An ionic compound contains metal atoms that raise its melting point. d. A strong electrical attraction means ions require a lot of energy to move apart. ANS:D

47. Assessment Questions 1. The ratio of aluminum ions to chloride ions in aluminum chloride (AlC13) is 3:1. True False

48. Assessment Questions 1. The ratio of aluminum ions to chloride ions in aluminum chloride (AlC13) is 3:1. True False ANS:F, 1:3