Regents Chemistry

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

• Introduction to the Table
• Groups and Families
• Elements of Metals, Nonmetals and Metalloids

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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
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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..

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Rows and Columns
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Divisions of the Periodic Table

• Metals
• Alkali metals
• Alkaline earth metals
• Transition Metals
• Metalloids
• Nonmetals
• Halogens
• Nobel gases

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Periodic Table
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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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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

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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

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Examples

• Argon (noble gas)
• Nitrogen and
• oxygen

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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

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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
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Regents Chemistry

• Information on the Table
• Average Atomic Mass
• Atomic Number
• Isotopes

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Regents Chemistry

• Periodic Table Bingo

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Regents Chemistry

• Ions and Oxidation States

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Change ending of parent name to -ide and add
word - ion
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Cloride Anion
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Keep parent name and add word - ion
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Sodium Cation
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Ionic charges from Periodic Table
See pg. 112
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Writing out ionic charges
Gain e-
Sodium ion
Lose e-
Magnesium ion
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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


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Examples
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More Examples...
Dissolving Ionic CompoundsVideo
Does this work?

worksheet
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Regents Chemistry

• Chemical Nomenclature

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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!

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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

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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

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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

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

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Examples

• Name the following compounds
• NaCl
• KI
• CaS

CLICK TO REVEAL ANSWERS
sodium chloride
potassium iodide
STOP worksheet
calcium sulfide
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Regents Chemistry

• Naming Type II Compounds

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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 chargewe must determine the charge
  according to the chemical formula

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Determing the correct charge

• All compounds must be electrically neutral..so
• we use the charge of the anion to determine the
  charge of the cationand multiply the charges by
  the number of atoms to determine the overall net
  charge

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Example
CuCl
Cl comes in as Cl- -1 x 1 Cl ion -1
Cu must come in as a 1 1 x 1 Cu ion 1
-1 1 0 , the charges balance
Copper (I) Chloride
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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 cations charge

(I) 1 (V) 5 (II) 2 (VI) 6 (III)
3 (VII) 7 (IV) 4
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Practice

• HgO
• Fe2O3

Mercury (II) Oxide
Iron (III) Oxide
Worksheet
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Regents Chemistry

• Naming Type III Binary Compounds

Non-metal to non-metal
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Type III Binary Compounds

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

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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

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Prefixes for Naming Type III
PREFIX
NUMBER INDICATED
mono- 1 di- 2 tri- 3 tetra- 4 penta
- 5 hexa- 6 hepta- 7 octa- 8
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Practice

• BF3
• NO
• N2O5
• carbon tetrachloride

boron trifluoride
nitrogen monoxide
dinitrogen pentoxide
CCl4
worksheet
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Regents Chemistry

• Polyatomic Ion Compound Nomenclature

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Whats 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-

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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

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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

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Naming Oxyanions

• 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

SO42-
Sulfite Ion
Sulfate Ion
SO32-
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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
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Naming Compounds that Contain Polyatomic Ions

• We use the cation name and roman numerals (if
  needed) and the polyatomic ions name
• Ex Na2SO4

Na
2 x
sodium sulfate
SO42-
1 x
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Examples
iron (III) nitrate
Fe(NO3)3
manganese (II) hydroxide
Mn(OH)2
copper (II) sulfate
CuSO4
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Regents Chemistry

• Revisiting the Periodic Table
• Trends of the Table

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Properties of Elements

• Trends to be familiar with
• Ionization Energy
• Atomic Radii
• Ionic Radii
• Electronegativity
• Reactivity of Elements

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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

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Families on the Table

• 3 day website project see handout