1. Regents Chemistry
Topic 2
The Periodic Table and
Formulas / Equations

2. Regents Chemistry Introduction to the Table Groups and Families
Elements of Metals, Nonmetals and Metalloids

3. Recap The nucleus contains protons and neutrons Nucleus
Electrons surround the
nucleus in a “cloud”
Atomic number is the
number of protons
Atomic mass is the
sum of protons and
neutrons
electrons

4. The Periodic Table
The periodic table is arranged according to Atomic Number
The first table, by Russian chemist Dmitri Mendeleev, was arranged by atomic mass, but this was not accurate
Current arrangement shows many important trends..

5. Rows and Columns

6. Divisions of the Periodic Table
Metals
Alkali metals
Alkaline earth metals
Transition Metals
Metalloids
Nonmetals
Halogens
Nobel gases

7. Periodic Table

9. Physical Properties of Metals
Efficient conduction of heat and electricity
Malleability (they can be hammered into
thin sheets
3. Ductility (they can be pulled into wires)
4. A lustrous (shiny) appearance

12. Natural States of Elements
Most of the matter around us consists of mixtures
Mixtures contain compounds
Atoms of individual elements are not often found in nature in pure form
Some exceptions: gold, platinum and silver
Also noble gases – do not combine readily
Ex; Helium gas in underground deposits

13. Elements after Separation..
After we use a chemical process to separate the elements in a compound, we find the elements to be:
Monoatomic atoms– only (1) atom of the element
Diatomic molecules– (2) atoms bonded together

14. Examples
Argon (noble gas)
Nitrogen and
oxygen

15. Natural Physical States
Metals are solids at 25 C
Noble gases are gas at room 25 C and are individual atoms
Several others are gases and diatomic at 25 C – (H2, N2, O2, F2, Cl2)
Only two elements are liquids at 25 C
Bromine and Mercury

16. Elements can have different forms…
Solid metals differ from solid non-metals
In fact, different forms of the same element can occur
These are called allotropes
Ex: Carbon
Diamond (very hard)
Graphite (soft)
Buckministerfullerene (newly discovered)
End

17. Regents Chemistry Information on the Table Average Atomic Mass
Atomic Number
Isotopes

18. Regents Chemistry
Periodic Table Bingo

19. Regents Chemistry
Ions and Oxidation States

21. **Change ending of parent name to -ide and add word - ion**

22. Cloride Anion

23. ***Keep parent name and add word - ion***

24. Sodium Cation

25. Ionic charges from Periodic Table
See pg. 112

26. Writing out ionic charges
Gain e-
Sodium ion
Lose e-
Magnesium ion

27. Ionic Compounds Combination of cation and anion
Write cation first and anion second
When combining, we must consider electrical charge
Ions combine in such a way to make a zero net charge
Total charge
of cations
Total charge
of anion
Zero net charge + =

28. Examples

29. More Examples... Dissolving Ionic CompoundsVideo Does this work? =
worksheet

30. Regents Chemistry
Chemical Nomenclature

31. Naming Compounds
Common names were originally developed to name compounds
Ex: Epsom salts, milk of magnesia, gypsum and laughing gas
Too many common names..a system had to be developed!

32. Naming Compounds
Binary compounds – compounds that are composed of two elements
We will examine two classes of binary compounds
1. Compounds that contain a metal and a nonmetal
2. Compounds that contain two nonmetals

33. Naming Binary Ionic Compounds
Binary ionic compounds result when a metal combines with a nonmetal
The metal loses electrons as the nonmetal gains electrons
The result is a positive cation (the metal) and a negative anion (the nonmetal)
In naming ionic compounds, we simply name the ions

34. Naming Binary Ionic Compounds
We will learn how to name two types of ionic compounds (polyatomic ion naming will come later)
Type I compounds – The metal is present in only one type of cation - look at periodic table!
Ex: Na+, K+, Ca2+, Al3+
Type II compounds – The metal present can form two (or more) cations that have different charges - look at periodic table!
Ex: Cr2+, Cr3+, Cu+, Cu2+

35. Some Common Examples Cation Name Anion H+ F- Fluoride Li+ Lithium Cl-
Hydrogen F-
Fluoride
Li+
Lithium
Cl-
Chloride K+
Potassium
Br-
Bromide
Ca2+
Calcium I-
Iodide
Ag+
Silver
S2-
Sulfide

36. Naming Rules for Type I Ionic
1. The cation is always named first and the anion second
2. A simple cation (obtained from a single atom) takes its name from the name of the element.
Ex: Na+ Sodium ion
3. A simple anion (obtained from a single atom) is named by taking the first part of the elemental name and adding – ide
Ex: F- Fluoride ion

37. Examples NaCl KI CaS Name the following compounds sodium chloride
CLICK TO REVEAL ANSWERS
sodium chloride
potassium iodide
STOP
worksheet
calcium sulfide

38. Regents Chemistry
Naming Type II Compounds

39. Naming Type II compounds
Type II compounds – The metal present can form two (or more) cations that have different charges - look at periodic table!
Ex: Cr2+, Cr3+, Cu+, Cu2+
We cannot only look at the periodic table to determine the charge…we must determine the charge according to the chemical formula

40. Determing the correct charge
All compounds must be electrically neutral..so
we use the charge of the anion to determine the charge of the cation…and multiply the charges by the number of atoms to determine the overall net charge

41. CuCl Example Cl comes in as Cl- : -1 x 1 Cl ion = -1
Cu must come in as a +1 :+1 x 1 Cu ion = +1
= 0 , the charges balance
Copper (I) Chloride

42. Naming Type II Rules
Use the same system of naming as Type I binary compounds..except
add the following after the cation depending on the cation’s charge
(I) (V) +5
(II) (VI) +6
(III) +3 (VII) +7
(IV) +4

43. Practice
HgO
Fe2O3
Mercury (II) Oxide
Iron (III) Oxide
Worksheet

44. Regents Chemistry Naming Type III Binary Compounds
Non-metal to non-metal

45. Type III Binary Compounds
Type III Binary Compounds - are compounds that contain only nonmetals participating in covalent bonds (sharing of electrons)

46. Rules for Naming Type III
1. The first element in the formula is named first, and the full element name is used
2. The second element is named as though it were an anion (-ide ending)
3. Prefixes are used to denote the numbers of atoms present.
4. The prefix mono is never used for naming the first element

47. Prefixes for Naming Type III
NUMBER INDICATED
mono- 1 di
tri
tetra
penta- 5
hexa
hepta- 7
octa

48. Practice BF3 NO N2O5 carbon tetrachloride CCl4 boron trifluoride
nitrogen monoxide
dinitrogen pentoxide
CCl4
worksheet

49. Regents Chemistry
Polyatomic Ion Compound Nomenclature

50. What’s a polyatomic ion?
A polyatomic ion consists of two or more elements bonded together that posess an overall net charge that can be used to form an ionic bond with a metal cation
We looked at some of these!
SO42-

51. Polyatomic Ion Intro… Polyatomic ions have specific names…
You must be able to recognize polyatomic ions in chemical formulas and chemical names
You reference tables can help!
See the table on the front page

52. Naming Polyatomic Ions…
Some polyatomic ions have general names that are made from modification of the names of the elements involved
Ex: NH4+ Ammonium Ion
CN- Cyanide Ion

53. Naming Oxyanions SO42- SO32-
Oxyanions are polyatomic ions (anions) that contain atoms of an element and different numbers of oxygen atoms
When there are two members in such a series, the anion with the lesser number of oxygen is given the ending –ite and the larger number ends in –ate
Sulfite
Ion
SO42-
Sulfate
Ion
SO32-

54. Naming Oxyanions cont…
If there are more that two in the series, we use the prefix hypo for the member with the fewest oxygen and per for the one with the most oxygen
ClO- hypochlorite ion
ClO2- chlorite ion
ClO3- chlorate ion
ClO4- perchlorate ion

55. Naming Compounds that Contain Polyatomic Ions…
We use the cation name and roman numerals (if needed) and the polyatomic ion’s name
Ex: Na2SO4
2 x
Na+
sodium sulfate
1 x
SO42-

56. Examples iron (III) nitrate Fe(NO3)3 manganese (II) hydroxide Mn(OH)2
copper (II) sulfate
CuSO4

57. Regents Chemistry
Revisiting the Periodic Table
Trends of the Table

58. Properties of Elements
Trends to be familiar with:
Ionization Energy
Atomic Radii
Ionic Radii
Electronegativity
Reactivity of Elements

59. Summary of Trends
Ionization Energy – increases from left to right and up the columns
Atomic Radii – increases from right to left and down columns
Ionic Radii – depends on if the atom looses or gains electrons
Electronegativity – increases from left to right and up the columns
Reactivity – Groups 1,2 and 17 along with oxygen are most reactive

60. Families on the Table
3 – day website project: see handout