1. Do Now!!!
Two highly reactive elements in Period 4 are the metal potassium and the:
Metalloid arsenic
Nonmetal selenium
Nonmetal bromine
Nonmetal krypton

2. Do Now!!!
Two highly reactive elements in Period 4 are the metal potassium and the:
Metalloid arsenic
Nonmetal selenium
C. Nonmetal bromine
Nonmetal krypton

3. Objectives Recognize stable electron configurations.
Predict an element’s chemical properties using number of valence electrons and electron dot diagrams.
Describe how an ionic bond forms and how ionization energy affects the process.

4. Chapter 6
Chemical Bonds

5. Stable Electron Configurations
When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react.

6. Electron Dot Diagram
A diagram of an atom, ion or molecule in which each dot represents a valence electron.

7. Ionic Bonds A bond between a metal and a nonmetal.
Some elements achieve stable electron configurations through the transfer of electrons between atoms.
A bond between a metal and a nonmetal.

9. Do Now!!!
In an ionic compound, the attractions between cations and _____________ hold the compound together.
anions

10. Do Now!!!
What is the name of CoCl2?
Cobalt (II) chloride

11. Objectives Recognize stable electron configurations.
Predict an element’s chemical properties using number of valence electrons and electron dot diagrams.
Describe how an ionic bond forms and how ionization energy affects the process.

12. Na (sodium) loses 1 electron Cl (chlorine) gains 1 electron
Transfer of Electrons
Na (sodium) loses 1 electron
Cl (chlorine) gains 1 electron

13. Ion
An atom or group of atoms that has a positive or negative charge.

14. Anion An ion with a negative charge. Examples: Cl- (chloride ion)
O2- (oxide ion)

15. Cation Examples: Na+ (sodium ion) Mg2+ (magnesium ion)
An ion with a positive charge.
Examples:
Na+ (sodium ion)
Mg2+ (magnesium ion)

16. Chemical Bond
The force that holds atoms or ions together as a unit.

17. Ionic Bond
The force that holds cations and anions together.

18. Ionization Energy

19. Ionization Energy
The amount of energy needed to remove an electron from an atom.
The lower the ionization energy, the easier it is to remove an electron from an atom.

20. Chemical Formula Examples: NaCl (sodium chloride)
Notation that shows what elements a compound contains and the ratio of the atoms or ions of these elements in the compound.
Examples:
NaCl (sodium chloride)
MgCl2 (magnesium chloride)

21. Crystals Sodium Chloride (salt) Crystal
Solids whose particles are arranged in a lattice structure.
Sodium Chloride (salt) Crystal

22. Properties of Ionic Compounds
The properties of an ionic compound can be explained by the strong attractions among ions within a crystal lattice.

23. Do Now!!!
The chemical formula for calcium chloride, CaCl2, shows that the compound contains two _____________ ions for every _____________ ion.
chloride
calcium

24. Objectives
Describe how covalent bonds form and the attractions that keep atoms together in molecules.
Compare polar and nonpolar bonds, and demonstrate how polar bonds affect the polarity of a molecule.
Compare the attractions between polar and nonpolar molecules.

25. Covalent Bond A bond between a nonmetal and a nonmetal.
A chemical bond in which two atoms share a pair of valence electrons.
A bond between a nonmetal and a nonmetal.

26. Molecule
A neutral group of atoms that are joined together by one or more covalent bonds.

27. Molecule Examples: HCl (hydrogen chloride)
The attractions between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond.
Examples:
H2 (diatomic hydrogen)
HCl (hydrogen chloride)

28. Covalent Bonds Double bond – share 4 electrons between 2 atoms
Single bond – share only 2 electrons between 2 atoms
Double bond – share 4 electrons between atoms
Triple bond – share 6 electrons between atoms

29. Polar Covalent Bond
A covalent bond in which electrons are not shared equally.
When atoms form a polar covalent bond, the atom with the greater attraction for electrons has a partial negative charge. The other atom has a partial positive charge.

30. Polar and Nonpolar Molecules
The type of atoms in a molecule and its shape are factors that determine whether a molecule is polar or nonpolar.

31. Attraction Between Molecules
Attractions between polar molecules are stronger than attractions between nonpolar molecules.

32. Do Now!!!
In an electron dot diagram, each dot represents a(an) _____________.
electron

33. Objectives
Recognize and describe binary ionic compounds, metals with multiple ions, and polyatomic ions.
Name and determine chemical formulas for ionic and molecular compounds.

34. Describing Ionic Compounds
The name of an ionic compound must distinguish the compound from other ionic compounds containing the same elements. The formula of an ionic compound describes the ratio of the ions in the compounds.

35. Nomenclature Group 1 and 2 metals and Al with non-metals
1. Metal name first
2. Non-metal name 2nd with the -ide ending

36. Nomenclature Examples: CaCl2 = calcium chloride K2S
= potassium sulfide

37. Metals With Multiple Ions (P. 172)
Many transitions metals form more than one type of ion.

38. Polyatomic Ion (P. 173)
A covalently bonded group of atoms that has a positive or negative charge and acts as a unit.
Name
Formula
Ammonium
Hydroxide
Nitrate
Sulfate
Sulfite
Phosphate
Chromate
Silicate
Cyanide
Chlorate
NH4+
OH-
NO3-
SO42-
SO32-
PO43-
CrO42-
SiO32-
CN-
ClO3-
Acetate
Peroxide
Permanganate
Hydrogen sulfate
Hydrogen carbonate
Hydrogen phosphate
Dichromate
Hypochlorite
Carbonate
Perchlorate
C2H3O2-
O22-
MnO4-
HSO4-
HCO3-
HPO42-
Cr2O72-
OCl-
CO32-
ClO4-

39. Metals with Polyatomic Ions
Examples:
Na2SO4
= Sodium sulfate
Fe(NO3)3
= Iron(III) nitrate

40. Do Now!!! The name copper(II) indicates that a compound contains:
copper ions with a 11+ charge.
copper ions with a 2+ charge.
copper ions with a negative charge.
two types of copper ions.

41. Do Now!!! The name copper(II) indicates that a compound contains:
copper ions with a 11+ charge.
B. copper ions with a 2+ charge.
copper ions with a negative charge.
two types of copper ions.

42. Objectives
Recognize and describe binary ionic compounds, metals with multiple ions, and polyatomic ions.
Name and determine chemical formulas for ionic and molecular compounds.

43. Non-metals with non-metals (P. 175)
Most electropositive element first
2. First element has a prefix indicating number and the name of the element
EXCEPTION: Mono prefix (not used for first element)
Second element has prefix indicating number and the “-ide” ending.
NOTE: 2nd o is eliminated for oxides
(e.g., monoxide not monooxide)

44. Non-metals with non-metals
Examples:
CO2
= Carbon dioxide
BrF3
= Bromine trifluoride

45. Do Now!!! What is the name of TiO2?
What is the formula of sodium phosphate?
Titanium (IV) oxide
Na3PO4

46. Objectives
Recognize and describe binary ionic compounds, metals with multiple ions, and polyatomic ions.
Name and determine chemical formulas for ionic and molecular compounds.

47. Metallic Bond
The attraction between a metal cation and the shared electrons that surround it.

48. Metallic Bond
The cations in a metal form a lattice that is held in place by strong metallic bonds between the cations and the surrounding valence electrons.

49. Properties of Metals
The mobility of electrons within a metal lattice explains some of the properties of metals.

50. Manganese (III) cyanide
Do Now!!!
What is the name of Mn(CN)3?
What is the formula of diboron trioxide?
What is the formula of (NH4)2S?
Manganese (III) cyanide
B2O3
Ammonium sulfide

51. Do Now!!! An alloy that contains mainly copper and tin is:
A. Sterling silver B. Brass
C. Stainless steel D. Bronze

52. Do Now!!! An alloy that contains mainly copper and tin is:
A. Sterling silver B. Brass
C. Stainless steel D. Bronze

53. Objective
Define an alloy and demonstrate how the composition of an alloy affects its properties.

54. Alloy
A mixture of two or more elements, at least one of which is a metal, that has the characteristic properties of a metal.

55. Examples Brass: Copper and zinc Steel: Iron and carbon
Bronze: Tin and copper
Brass: Copper and zinc
Steel: Iron and carbon
Stainless Steel: Iron, carbon, and chromium

56. Objectives
Predict the composition of an ionic compound from its chemical formula.
Relate the properties of ionic compounds to the structure of crystal lattices.

57. Objectives
Describe how covalent bonds form and the attractions that keep atoms together in molecules.
Compare polar and nonpolar bonds, and demonstrate how polar bonds affect the polarity of a molecule.
Compare the attractions between polar and nonpolar molecules.

58. Objectives Describe the structure and strength of bonds in metals.
Relate the properties of metals to their structure.
Define an alloy and demonstrate how the composition of an alloy affects its properties.