1. Bellwork Monday, 10/28
To the right is a label from a popular food item. Name five elements that are found on this food label.

2. CHEMICAL NAMES AND FORMULAS
CHEMISTY I CHAPTER 6
CHEMICAL NAMES AND FORMULAS

3. Molecule- the smallest electrically neutral unit of a substance that still has the properties of that substance -made up of two or more atoms that act as a unit Ex.
CH4 O2
H2O
CO2 O3

4. Molecular compound- -usually composed of molecules -Have low melting & boiling points -Are usually made up of two or more NONMETALS
Sugar, a compound made of carbon, hydrogen and oxygen, melts easily in a hot pan.

5. Which of the following is molecular and which is ionic?
NaCl
H2O
CaCO3 CO
Al2Cl3
CF4 O3

6. diatomic molecule –consists of two atoms of the same element (O2 and H2)

7. triatomic molecule- contain three atoms of the same element (O3, ozone)

8. Molecular Compounds and Acids
Binary Molecular Compounds
When naming binary molecular compounds, prefixes are used to tell how many of each atom is in the formula.
CO2 carbon dioxide
N2O4 dinitrogen tetroxide

9. The prefix mono- is never used with the first element
The prefix mono- is never used with the first element. The prefix list in on page 159.
hexa
mono di
hepta
tri
octa
nona
tetra
penta
deca

10. Example: PBr3 ICl3 P2O5 Sulfur hexafluoride tetraarsenic hexoxide
phosphorous tribromide
iodine trichloride
diphosphorous pentoxide
SF6
As4O6

11. Acids and Bases hydrochloric acid sulfuric acid nitric acid
You need to know the names and formulas of these most common acids:
HCl
H2SO4
HNO3
HC2H3O2
H3PO4
hydrochloric acid
sulfuric acid
nitric acid
acetic acid
phosphoric acid

12. Covalent
Two Nonmetals
Example:
Rule:
Use _________ to tell the _________ of each element.
_____________
Note: A prefix is NOT needed on the first element if there is only 1.
1= =
2= =
3= =
4= =
5= =
Acids: contain the element ________ at the left of the formula
Need to know:
HCl:
H2SO4:
HNO3:
HC2H3O2:
H3PO4:

13. Bellwork, Tuesday How many protons, neutrons and electrons are in this atom? Based on what you know about the charge of a proton and an electron, what is the overall charge of this atom? What element is this atom?
Red =protons
Yellow=neutrons
Black=electrons

14. Ions- atoms or groups of atoms that have a positive or negative charge
Ions- atoms or groups of atoms that have a positive or negative charge. Ions are formed when one or more electrons are lost or gained.

15. Let’s Practice!
Sodium loses an electron Na  __________
Magnesium loses two electrons Mg  __________
Chlorine gains one electron Cl  __________
Phosphorus gains three electrons P  __________

16. We are positive about metal cats!
Cation- -positively charged ion -electrons were lost -metals tend to form cations -name of monatomic cation is the same as the element
We are positive about metal cats!

17. Examples: Na  Na+ + e- Ca  Ca2+ + 2e- Fe  Fe3+ + 3e-

18. We feel negatively about ants!
Anion - negatively charged ion -electrons were gained -nonmetals tend to form anions -name of monatomic anion ends in –ide
We feel negatively about ants!
Examples:

19. Ionic compound- -composed of cations and anions -usually metal & nonmetal -electrically neutral -mostly solids at room temperature -high melting points -the more positive element always comes first -Ex NaCl, NaF, CaCl2

21. Monatomic Ions The charge of a monatomic ion can often be determined by the element’s position on the periodic table:
Group 1A: Ex. Na+ Group 2A: Ex. Ca2+ Group 3A: Ex. Al3+ Group 5A: Ex. N3- Group 6A: Ex. O2- Group 7A: Ex. F- See Table 6-2 (pg 143)

22. The noble gasses have no charge and are inert
Alkali metals have a charge of +1
The halogens have a charge of -1
The oxygen family has a charge of -2
The carbon family has a charge of + or -4
The boron family has a charge of +3
Alkaline Earth metals have a charge of +2
The nitrogen family has a charge of -3
Transition metal charges will need to be memorized!

23. Elements in Group 0 (8) do not form ions
Elements in Group 0 (8) do not form ions. Elements in Group 4 rarely form ions. They tend to react by sharing electrons (forming covalent compounds) instead of transferring electrons. Group 8 Electron configuration = s2p6 Group 4 Electron configuration = s2p2

24. What causes the charges for each group on the periodic table?
The charges indicate how many electrons an atom will gain or lose.
If it loses 2, the charge will be +2. If it gains 2, the charge will be -2. Remember that electrons are NEGATIVE!

25. Octet Rule and Stability
The goal of an atom is to become stable. An atom will gain, lose, or share electrons in order for that stability to be attained.
Stability is determined by the octet rule:
Most atoms want 8 valence (outer shell) electrons in order to become stable.

26. Ex: Potassium (and all of group 1) has 1 valence electron, so it will lose 1 electron making its charge +1. Remember that electrons are NEGATIVE!

27. Examples: O P F Na Mg Al Sr 2- 3- 1- 1+ 2+ 3+ 2+

28. Transition Metal ions (See Table 6-3 pg 144): Most transition metals form more than one ion. They are stable losing varying numbers of electrons. The possible charges must be memorized.

29. Exceptions: Zinc and Cadmium will always be 2+ and Silver will always be 1+.

30. What is the formula for the following transition metals as ions?
Copper (I)
Iron (III)
Lead (II)
Manganese (III)

31. The mercury(I) ion is unique
The mercury(I) ion is unique. It only exists in pairs of mercury(I) ions (like Siamese twins). Its symbol is Hg22+.

32. Quick Check Quiz: Have you been studying your ions
Quick Check Quiz: Have you been studying your ions? sodium _______ chromous ________ selenide _______ tin(IV) ________
Na+
Cr2+
Se2-
Sn4+

33. Rubidium loses one electron _____ Silver loses one electron _____
Wednesday Bellwork
Write the ion that forms.
Rubidium loses one electron _____
Silver loses one electron _____
Arsenic gains three electrons _____
Sulfur gains two electrons _____
Lithium loses one electron _____

34. Wednesday Bellwork
Name the following compounds or write the formulas, as appropriate.
CCl4
P4O10
N2O7
XeF4

35. Thursday Bellwork
Practice your ions! Write the symbol and charge for the following ions.
Nitride
Oxide
Magnesium ion
Rubidium ion
Fluoride

36. Friday Bellwork Match the following ions with their names.
___NO3- A. nitride
___CN- B. silver ion
___Ag+ C. cyanide
___NH4+ D. ammonium
___N3- E. chloride
___Cl- F. nitrate

37. Polyatomic Ions (Table 6-4, pg 147): -tightly bound groups of atoms that behave as a unit and carry a charge -atoms are bound together by shared electrons

38. The only positively charged polyatomic ion that we need to memorize is ammonium, NH4+.

39. Ions that end in –ite or –ate contain oxygen
Ions that end in –ite or –ate contain oxygen. In a series such as sulfate and sulfite, the –ite ending has one less oxygen than the –ate ending.
Sulfite SO32-
Sulfate SO42-

40. SO32- sulfite SO42- sulfate NO2- nitrite NO3- nitrate
EXAMPLES
SO sulfite SO sulfate NO nitrite NO nitrate

41. Writing Formulas
Binary compounds- 2 elements Binary ionic compounds- 1 metal + 1 nonmetal Binary molecular compounds- 2 nonmetals

42. Examples: NaCl NaF nonmetal metal CaCl2
**The more positive element (metal) always comes first.

43. When naming ionic compounds, simply name the ions as they appear in the formula.
When naming ionic compounds containing a transition metal, include the Roman numeral representing the charge.

44. Ionic Metal and Nonmetal _____VALENT METAL means:
_____________
Metals in group _____, _______, & these 4: __________________
Ex:
Rule:
Name the __________
then the __________ ending in ________.
_____VALENT METAL means: ___________________________
Located in ________ & under the __________________.
Same as mono- BUT use a ______________ to tell the metal’s __________.

45. Contains a polyatomic ion:
Ionic
Contains a polyatomic ion:
Ex:
Rule:
Follow the same mono- or multi- valent metal rules; use the polyatomic ion’s name.

46. Example: aluminum chloride AlCl3 KBr FeCl2 FeCl3 potassium bromide
iron(II) chloride
iron(III) chloride

47. When writing the formula for an ionic compound, the charges of the ions must cancel out to give the compound a neutral charge.

48. Example:
sodium chloride
Na+ Cl- 1 1
Na1Cl1 =
NaCl

49. magnesium iodide
Mg2+ I- 2 1
Mg1I2 =
MgI2

50. magnesium nitride
Mg 2+ N3- 2 3
Mg3N2

51. strontium selenide
Sr2+ Se2- 2 2 =
Sr2Se2
SrSe

52. rubidium iodide
Rb+ I-
RbI
aluminum oxide
Al3+ O2-
Al2O3

53. When writing formulas containing polyatomic ions, use parentheses around multiple polyatomic ions.
ammonium carbonate
NH4+ CO32- 2 1
(NH4)2CO3

54. strontium hydroxide
Sr2+ OH- 1 2
Sr(OH)2

55. calcium nitrate
Ca2+ NO3- 1 2
Ca(NO3)2

56. aluminum phosphate
Al3+ PO43- 3 3
AlPO4

57. Monday Bellwork Practice this ion quiz: NO3- _______________________
Mercury (II) _______________________
Ag+ _______________________
CN- _______________________
Potassium _______________________
Bromide _______________________
Ba2+ _______________________

58. When naming ionic compounds containing a transition metal, don’t forget to include the Roman numeral for the charge. Ex. FeCl2 iron(II) chloride FeCl3 iron(III) chloride

59. Distinguish Between the two types of compounds!
Molecular
Ionic
Two or more nonmetals
Low melting point
Low boiling point
Example CO2
Metal and nonmetals
High melting point
High boiling point
Solid at room temperature
Electrically neutral
Example NaCl

60. Which of the following is molecular and which is ionic?
NaBr
CO2 O3 NO
KCl
AlBr3
Ionic
Molecular
Molecular
Molecular
Ionic
Ionic

61. Molecular formula- chemical formula written for a molecule
Chemical formula- shows the number and kinds of atoms in the smallest representative unit of the substance.
Molecular formula- chemical formula written for a molecule
Ex. CO2 O2 or H2O2
The formula for this compound would be C5H12O

62. Formula unit- chemical formula written for an ionic compound
Formula unit- chemical formula written for an ionic compound. -lowest whole-number ratio of ions in the compound

63. Tuesday Bellwork Name the following compounds.
NaBr _____________________________
Al(OH)3 ___________________________
NH4F _____________________________
Li2SO3 ____________________________
CaBr2 ____________________________
KMnO4 ___________________________
Fe(NO3)2__________________________
LiOH _____________________________

64. Law of Definite Proportions- In all samples of any chemical compound, the elements are always combined in the same proportion by mass. Ex. Water is always 88.9%O and 11.1%H by mass

65. Law of Multiple Proportions- Whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers.

66. Formula Naming: A Summary

67. Wednesday Bellwork
Using the food label shown, write two compounds in this food.

68. Thursday Bellwork Write the formulas for these compounds.
Potassium chlorite
Calcium hydrogen carbonate
Dichlorine heptoxide
Trisilicon tetranitride
Sodium dihydrogen phosphate
Phosphorus pentabromide
Carbon tetrachloride

69. Friday Bellwork
Study for your all ion quiz!