1. Ionic Bonding

2. Stable Electron Configuration When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react. goal is to achieve an octet in outer shell Electron dot diagram model of an atom in which each dot represents a valence electron symbol in the center represents the nucleus and all the other electrons in the atom F

3. Stable Electron Configurations

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

13. Ionic Bonds Ionic bonds are one way that elements can achieve stable electron configurations Occurs between metals and nonmetals 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.

14. Ionic Bonds When an atom gains or loses an electron, the number of protons is no longer equal to the number of electrons. The atom is not neutral. An atom that has a net positive or negative electric charge is called an ion. The charge on an ion is represented by a plus or a minus sign.

15. Ionic Bonds The ion that forms when a chlorine atom gains an electron has 17 protons and 18 electrons. This ion has a charge of 1– The symbol for the ion is written 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.

16. Ionic Bonds A sodium ion has 11 protons and 10 electrons. The sodium ion has a charge of 1+ The symbol for the ion is written Na 1+, or Na + for short An ion with a positive charge is a cation A cation uses the element name, as in the sodium ion

17. Ionic Bonds Scientists use atomic radii to compare the sizes of atoms of different elements. The radius of a sphere is the distance from the center of the sphere to its outer edge–half the diameter of the sphere. Atomic radii are extremely small. They are expressed in units of picometers (pm). There are one billion (10 9 ) picometers in a millimeter.

18. Ionic Bonds This table shows the atomic radius and ionic radius for six metals and six nonmetals.

19. Ionic Bonds 1. Within a period, what happens to the atomic radius as the atomic number of the elements increases?

20. Ionic Bonds 2. Within Groups 1A, 2A, 6A, and 7A, what happens to the atomic radius of elements as the atomic number increases?

21. Ionic Bonds 3. How does adding an occupied energy level affect the atomic radius? (Hint: Lithium is a Period 2 element and sodium is a Period 3 element.)

22. Ionic Bonds 4. Compare the atomic and ionic radii for potassium (K), and for bromine (Br).

23. Ionic Bonds 5. What happens to the radius of an atom when the atom loses electrons? When the atom gains electrons?

24. Ionic Bonds 6. Explain the difference in size between a metal atom and its cation.

25. Formation of Ionic Bonds A negatively charged particle will attract a positively charged particle chemical bond - force that holds atoms or ions together as a unit ionic bond - the force that holds cations and anions together forms when electrons are transferred from one atom to another

26. Ionization Energy 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 Group 1 has very low ionization energy Group 7 has a very high ionization energy

27. Ionization Energy Trend

28. Chemical Formula notation that shows what elements a compound contains shows the ratio of the atoms or ions of those elements in the compound NaCl

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

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

31. Ionic Bonding All the electrons must be accounted for! CaP

32. Ionic Bonding CaP

33. Ionic Bonding Ca +2 P

34. Ionic Bonding Ca +2 P Ca

35. Ionic Bonding Ca +2 P -3 Ca

36. Ionic Bonding Ca +2 P -3 Ca P

37. Ionic Bonding Ca +2 P -3 Ca +2 P

38. Ionic Bonding Ca +2 P -3 Ca +2 P Ca

39. Ionic Bonding Ca +2 P -3 Ca +2 P Ca

40. Ionic Bonding Ca +2 P -3 Ca +2 P -3 Ca +2

41. Ionic Bonding Ca 3 P 2 Formula Unit Ca 2+ P 3- Ca 2+ P 3- Ca 2+ P 3- Ca 2+

42. Crystal Lattices a regular, repeating arrangement of ions in the solid chemical formula shows ratio of the ions in a compound, but not how the ions are arranged classified into groups based on the shape of their crystals

43. Crystal Lattice Ions 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.

44. 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.

45. Properties of Ionic Compounds 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.

46. Properties of Ionic Compounds 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.