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Chapter 2 Nomenclature. Periodic Table Metals Conductors Lose electrons Malleable and ductile.
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Transcript of Chapter 2 Nomenclature. Periodic Table Metals Conductors Lose electrons Malleable and ductile.
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Chapter 2Nomenclature
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Periodic TablePeriodic Table
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Metals Conductors Lose electrons Malleable and ductile
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Nonmetals Brittle Gain electrons Covalent bonds
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Semi-metals or Metalloids
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Alkali Metals
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Alkaline Earth Metals
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Halogens
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Transition metals
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Noble Gases
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Inner Transition Metals
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+1 +2 -1-2-3
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Periodic Table Periodic table is organized based on the
properties that elements have in common with one another.
Groups: Elements in the same vertical columns are in the same group have similar chemical properties.
Group 1A: Alkali metals: Li, Na, K, Rb, Cs, Fr Group 2A: Alkaline earth metals: Be, Mg, Ca, Sr, Ba,
Ra Group 7A: Halogens: F, Cl, Br, I, At (astatine) Group 8A: Noble gases: He, Ne, Ar, Kr, Xe, Rn (radon)
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Periodic Table Periods: The horizontal rows of elements in the
periodic table are called periods. First period: horizontal row one contains H and He Second period: row two contains Li through Ne Letters in the boxes are the symbols for the
elements Abbreviations are based on the current element
names or the original names. The number above each symbol is the atomic
number (number of protons)
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Periodic Table Most of the elements are metals in the periodic
table. Metals: Conduction of heat and electricity,
malleability, ductility, lustrous, form positive ions
Nonmetals: appear in the upper right hand corner of the periodic table except hydrogen. Nonmetals lack the physical properties that characterize the metal, gain electrons in chemical reaction and form negative ions, form covalent bond to each other.
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Naming Compounds Binary Compounds: Compounds composed of
two elements Binary Ionic Compounds (Type I): contains a
positive ion (cation) always written first in the formula and a negative ion (anion)
Rules: 1. The cation is always named first and the anion
second2. A monatomic (meaning one atom) cation takes its
name from the name of the element3. A monatomic anion is named by taking the root of
the element name and adding –ide
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Naming compounds Two types Ionic - metal and non metal or
polyatomics. Covalent- non-metals.
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Ionic compounds If the cation is monoatomic- Name the
metal (cation) just write the name. If the cation is polyatomic- name it. If the anion is monoatomic- name it but
change the ending to –ide. If the anion is poly atomic- just name it.
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Covalent compounds Two words, with prefixes. Prefixes tell you how many. mono, di, tri, tetra, penta, hexa, hepta, octa,
nona, deca First element whole name with the
appropriate prefix, except mono. Second element, -ide ending with
appropriate prefix.
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Ionic compounds If the cation is monoatomic- Name the
metal (cation) just write the name. If the cation is polyatomic- name it If the anion is monoatomic- name it but
change the ending to -ide If the anion is poly atomic- just name it
from a table.
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Ionic Compounds Have to know what ions they form CaS K2S
AlPO4
K2SO4
FeS CoI3
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Some Polyatomic Ions (Table 2.3)NH4
+ ammonium SO42- sulfate
CO32- carbonate SO3
2- sulfite
HCO3- bicarbonate NO3
- nitrate
ClO3- chlorate NO2
- nitrite
Cr2O72-
dichromate SCN- thiocyanate
CrO42- chromate OH- hydroxide
2.7
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Naming compounds Binary Ionic Compounds (Type II): Metals that
form more than one type of positive ion. Fe2+ and Fe3+
Transition metals form several positive oxidation states
Charge on the metal ion must be specified Roman numeral indicates the charge of the cation.
Iron (II) chloride and iron (III) chloride The ion with the higher charge has a name ending
in –ic and the one with the lower charge has a name ending in –ous; ferrous chloride and ferric chloride
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Naming Compounds
Ionic Compounds with Polyatomic Ions: Need to know the names of the polyatomic ions
(Table 2.5).
NH4+ ammonium, SO4
2- sulfate Na2SO4 Sodium sulfate KH2PO4 Potassium dihydrogen phosphate Fe(NO3)3 Iron(III) nitrate CsClO4 Cesium perchlorate NaOCl sodium hypochlorite Al2(Cr2O7)3 Aluminum dichromate Sr(CN)2 Strontium cyanide
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Naming compoundsBinary Covalent Compounds (Type III):Formed between two nonmetalsRules: The first element in the formula is named first,
using the full element’s name Second element is name as if it were an anion Use prefixes to denote the number of atoms
present Never use mono – prefix for naming the first
element
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Molecular compounds nonmetals OR nonmetals + metalloids common names
H2O, NH3, CH4, C60
element further left in periodic table is 1st
element closest to bottom of group is 1st
if more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom
last element ends in ide
2.7
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CO ==> carbon monoxide, not monocarbon monoxide
P2O5 ==> diphosphorus pentoxide
S2Cl4 ==> disulfur tetrachloride
NO2 ==> nitrogen dioxide
N2O5 ==> dinitrogen penoxide
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Chemical Nomenclature Ionic Compounds
often a metal + nonmetal anion (nonmetal), add “ide” to element name
BaCl2 barium chloride
K2O potassium oxide
Mg(OH)2 magnesium hydroxide
KNO3 potassium nitrate
2.7
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Transition metal ionic compounds indicate charge on metal with Roman numerals
FeCl2 2 Cl- -2 so Fe is +2 iron(II) chloride
FeCl3 3 Cl- -3 so Fe is +3 iron(III) chloride
Cr2S3 3 S-2 -6 so Cr is +3 (6/2) chromium(III) sulfide
2.7
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HI hydrogen iodide
NF3 nitrogen trifluoride
SO2 sulfur dioxide
N2Cl4 dinitrogen tetrachloride
NO2 nitrogen dioxide
N2O dinitrogen monoxide
Molecular Compounds
2.7
TOXIC!
Laughing Gas
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An acid can be defined as a substance that yields hydrogen ions (H+) when dissolved in water.
HCl•Pure substance, hydrogen chloride•Dissolved in water (H+ Cl-), hydrochloric acid
An oxoacid is an acid that contains hydrogen, oxygen, and another element.
HNO3 nitric acid
H2CO3 carbonic acid
H2SO4 sulfuric acid
2.7
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A base can be defined as a substance that yields hydroxide ions (OH-) when dissolved in water.
NaOH sodium hydroxide
KOH potassium hydroxide
Ba(OH)2 barium hydroxide
2.7
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Common Cations and Anions
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Formulas from Names
Name Chemical FormulaDiphosphorus pentasulfide P2S5 (two non metals)
Cesium peroxide Cs2O2 (Cs1+, O22-)
Aluminum fluoride AlF3 (Al3+, F-1)
Vanadium (v) fluoride VF5 (V5+, F-1)
Dioxygen difluoride O2F2 (two non metals)
Gallium oxide Ga2O3 (Ga3+, O2-)
Ammonium dichromate (NH4)2Cr2O7 (NH4+, Cr2O7
2-)
Cupric phosphate Cu3(PO4)2 (Cu2+, PO43-)
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Flowchart for Naming Binary Compounds
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Acids
When dissolved in water produce a solution containing free H+ ions (protons)
An acid is a molecule with one or more H+ ions attached to an anion
If the anion does not contain oxygen, the acid is named with the prefix hydro – and the suffix –ic
HCl Hydrochloric acid
HCN Hydrocyanic acid
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Acids If the anion contains oxygen, the acidic name is
formed from the root name of the anion with the suffix of –ic or –ous depending on the anion
HNO3 Nitric acid (Nitrate anion)
H2SO4 Sulfuric acid (Sulfate anion)
H3PO4 Phosphoric acid (Phosphate anion)
HC2H3O2 Acetic acid (Acetate anion)
H2SO3 Sulfurous acid (sulfite anion)
HNO2 Nitrous acid (nitrite anion)