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

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Presentation on theme: "Regents Chemistry Topic 2 The Periodic Table and Formulas / Equations."— Presentation transcript:

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

8

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

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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

20

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


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