Chapter 4 Atoms, Ions, and Compounds. The Composition of Compounds The law of multiple proportions...
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Transcript of Chapter 4 Atoms, Ions, and Compounds. The Composition of Compounds The law of multiple proportions...
![Page 1: Chapter 4 Atoms, Ions, and Compounds. The Composition of Compounds The law of multiple proportions states that the masses of element Y that combine with.](https://reader036.fdocuments.us/reader036/viewer/2022062600/5a4d1b437f8b9ab0599a2046/html5/thumbnails/1.jpg)
Chapter 4Atoms, Ions, and Compounds
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The Composition of Compounds• The law of multiple proportions states
that the masses of element Y that combine with a fixed mass of elements X to form two or more different compounds are in the ratios of small whole numbers.
• Examples: NO, NO2, N2O, N2O5, etc.
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Atomic Structure• J. J. Thomson discovered the subatomic
particle know as the electron.• Thomson used cathode ray tube.
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Mass of An Electron• Robert Millikan
determined the mass of an electron with his oil-droplet experiment.
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Thomson Model of the Atom• J. J. Thomson’s Plum-pudding model of the atom.
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Radioactivity and the Nuclear Atom• Henri Becquerel discovered that some
samples produced invisible radiation.• One type is a steam of beta () particles
(high energy electrons).• A second type consists of alpha ()
particles, which have a +2 charge and a mass equivalent to that of a helium nucleus.
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Rutherford’s Experiment• Rutherford and two of his students
bombarded a thin foil of gold with particles to test Thomson’s model of the atom.
• Theory would predict that the particles would travel through the foil without deflection, but the results didn’t confirm the model.
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Rutherford’s Experiment
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The Nuclear Atom• The nucleus of an atom contains all the
positive charge and nearly all the mass in an atom.
• The nucleus is about 1/10,000 the size of the atom.
• A proton is a positively charged subatomic particle present in the nucleus of an atom.
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The Third Subatomic Particle• A neutron is an electrically neutral or
uncharged subatomic particle found in the nucleus of an atom.
• Atomic Mass Units (amu) comprise a relative scale used to express the masses of atoms and subatomic particles.
• The scale is based on the definition that the mass of 1 atom of carbon with 6 protons and 6 neutrons in its nucleus is exactly 12 amu.
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Aston’s Experiment• Francis W. Aston built a postive-ray analyzer.
• Data from neon gas samples demonstrated that two different kinds of atoms or isotopes existed.
• Isotopes are atoms of an element whose nuclei have the same number of protons but different numbers of neutrons.
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Aston’s Positive-ray Analyzer
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• Elements are pure substances made up of identical atoms.
• There are 115 known kinds of atoms. Each has its own symbol.
• The first character in an atoms symbol is an uppercase letter that corresponds the first letter of the elements name.
• Most elements have a second character in their symbol which is is a lowercase letter usually the second letter of the elements name.
Elements
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Symbol and names for the known atoms are given in Table 2.1.
Elements discovered long ago have names and symbols with Latin or other origins, such as Au for gold (from aurum, meaning “bright dawn”), or Pb for lead (plumbum). Tungsten has a symbol of W, which is the first letter of its German name, wolfram.
Element Names
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The symbol and names for
the known atoms are given
in Table 2.1.
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Symbols of Isotopes• Each element consists of atoms with the
same number of protons in the nucleus. This number is called atomic number (Z).
• Protons and neutrons in atomic nuclei are called nucleons.
• The mass number (A) is the total number nucleons in one atom of an element.
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Writing the Symbol of an Isotope
XAZ
• A is the mass number
• Z is the atomic number
• X is the atomic symbol
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Average Atomic Masses
• A mass spectrometer is an instrument that measures precise masses and relative amounts of ions of atoms and molecule.
• The natural abundance of an isotope is its relative proportion among all the isotopes found a natural sample.
• The average atomic mass of an element is calculated by multiplying the natural abundance of each isotope by its exact mass in atomic mass units and then summing these products.
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ExampleIsotope Mass (amu) Natural abundance (%)
Neon-20 19.9924 90.4838Neon-21 20.99395 0.2696Neon-22 21.9914 9.2465
Neon is found in three isotopes in nature.
19.9924 x 0.904838 = 20.99395 x 0.002696 =21.9914 x 0.092465 =
18.0898323 amu0.056599689 amu2.033434801 amu
20.1797 amu
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Mendeleev’s Periodic Table• Dmitrii I. Mendeleev
arranged elements in the periodic table by their chemical and physical properties.
• He left open spaces in his periodic table to account for elements not yet discovered.
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The Modern Periodic Table• The modern periodic table is also based on a
classification of elements in terms of their physical and chemical properties.
• The horizontal rows are called periods.• Columns contain elements of the same family
or group.• Transition metals are the elements in group 3
through 12 in the periodic table.
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Groups of Elements• Group 1 contains the alkali metals.
• Group 2 contains the alkaline earth metals.
• Group 17 contains the halogens.
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Broad Categories of Elements• Metals are elements on the left-hand side of
the table. Metals are shiny solids that conduct heat and
electricity well and are malleable and ductile.
• Nonmetals have properties opposite to those of the metals and are on the right side of table
• Metalloids are the elements between the metals and nonmetals.
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Continued
• Main group elements or representative elements are the elements in groups 1,2 and 13 through 18.
• The noble gases are the elements in Group 18.
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Kinds of Compounds• Molecular Compounds are composed of
atoms held together by covalent bonds.• Covalent bonds are shared pairs of electrons
that chemically bond atoms together.• Ionic Compounds are composed of positively
and negatively charged ions that are held together by electrostatic attraction.
• Ions with negative charge are called anions.• Ions with positive charge are called cations.
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Continued• Molecular compounds are made of
nonmetals
• Ionic compounds are made of a metal and a nonmetal.
• Metal form cations and nonmetals form anions.
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Terms• Molecular formulas describe the exact
number and type of atoms present in one molecule of a compound.
• An empirical formula gives the simplest whole-number ratio of elements in a compound.
• The formula unit of an ionic compound is the smallest electrically neutral unit within the crystal of the compound.
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Binary means two different elements
Ionic means metal and nonmetal
Step 1First give the name of the metal, followed by thenonmetal name using the “ide” suffix.
Step 2 If the metal is to the right of group IIA, then aRoman numeral is used after the metal to todescribe the charge of the metal. Except Ag,Zn,and Al
ExamplesNaCl Al2O3
FeCl2 FeCl3
NOMENCLATUREI. Binary Ionic compounds
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Binary means two different elements
Ionic means metal and nonmetal
Step 1First give the name of the metal, followed by thenonmetal name using the “ide” suffix.
Step 2 If the metal is to the right of group IIA, then aRoman numeral is used after the metal to todescribe the charge of the metal. Except Ag,Zn,and Al
ExamplesNaCl Sodium chloride Al2O3
FeCl2 FeCl3
NOMENCLATUREI. Binary Ionic compounds
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Binary means two different elements
Ionic means metal and nonmetal
Step 1First give the name of the metal, followed by thenonmetal name using the “ide” suffix.
Step 2 If the metal is to the right of group IIA, then aRoman numeral is used after the metal to todescribe the charge of the metal. Except Ag,Zn,and Al
ExamplesNaCl Sodium chloride Al2O3 Aluminum oxide
FeCl2 FeCl3
NOMENCLATUREI. Binary Ionic compounds
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Binary means two different elements
Ionic means metal and nonmetal
Step 1First give the name of the metal, followed by thenonmetal name using the “ide” suffix.
Step 2 If the metal is to the right of group IIA, then aRoman numeral is used after the metal to todescribe the charge of the metal. Except Ag,Zn,and Al
ExamplesNaCl Sodium chloride Al2O3 Aluminum oxide
FeCl2 Iron(II) chloride FeCl3
NOMENCLATUREI. Binary Ionic compounds
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Binary means two different elements
Ionic means metal and nonmetal
Step 1First give the name of the metal, followed by thenonmetal name using the “ide” suffix.
Step 2 If the metal is to the right of group IIA, then aRoman numeral is used after the metal to todescribe the charge of the metal. Except Ag,Zn,and Al
ExamplesNaCl Sodium chloride Al2O3 Aluminum oxide
FeCl2 Iron(II) chloride FeCl3 iron(III) chloride
NOMENCLATUREI. Binary Ionic compounds
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II. Nonbinary Ionic compoundsNonbinary means more than two different elements
Step 1First give the name of the metal, followed by the memorized polyatomic ion name.
Step 2
If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.
ExamplesNaOH Fe(NO3)3
Fe(SO4)2Zn(C2H3O2)2
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Formula Name Formula NameNH4
+ Ammonium O22- Peroxide
C2H3O2- Acetate NO3
- NitrateCO3
2- Carbonate NO2- Nitrite
HCO31- Hydorgen
carbonateSO4
2- Sulfate
ClO4- Perchlorate SO3
2- SulfiteClO3
- Chlorate PO43- Phosphate
ClO2- Chlorite PO3
3- PhosphiteClO- Hypochlorite CrO4
2- ChromateCN- Cyanide Cr2O7
2- DichromateOH- Hydroxide
Memorized Polyatomic Ion List
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II. Nonbinary Ionic compoundsNonbinary means more than two different elements
Step 1First give the name of the metal, followed by the memorized polyatomic ion name.
Step 2
If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.
ExamplesNaOH Fe(NO3)3
Fe(SO4)2Zn(C2H3O2)2
Sodium hydroxide
CO
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II. Nonbinary Ionic compoundsNonbinary means more than two different elements
Step 1First give the name of the metal, followed by the memorized polyatomic ion name.
Step 2
If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.
ExamplesNaOH Fe(NO3)3
Fe(SO4)2Zn(C2H3O2)2
Sodium hydroxide
Iron(III) nitrate
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II. Nonbinary Ionic compoundsNonbinary means more than two different elements
Step 1First give the name of the metal, followed by the memorized polyatomic ion name.
Step 2
If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.
ExamplesNaOH Fe(NO3)3
Fe(SO4)2Zn(C2H3O2)2
Sodium hydroxide
Iron(III) nitrate
Iron(II) sulfate
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II. Nonbinary Ionic compoundsNonbinary means more than two different elements
Step 1First give the name of the metal, followed by the memorized polyatomic ion name.
Step 2
If the metal is to the right of group IIA, then aRoman numeral is used after the metal to describe the charge of the metal. Except Ag, Zn, and Al.
ExamplesNaOH Fe(NO3)3
Fe(SO4)2Zn(C2H3O2)2
Sodium hydroxide
Iron(III) nitrate
Iron(II) sulfate Iron(II) sulfate
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III. Binary molecular Compounds
Step 1First give the name of the first nonmetal,followed by the nonmetal name using the “ide”
suffix.Step 2
Give each nonmetal a Latin prefix describing the number of atoms present in the compound.
ExamplesCO CO2
P2O5 CCl4
Molecular means nonmetals
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You will need to learn the Greek numerical prefixes (Table 4.6):
Number Prefix1 Mono-*2 Di-3 Tri-4 Tetra-5 Penta-6 Hexa-7 Hepta-8 Octa-9 Nona-
10 Deca-
*Note 1 Compound names never start with mono
Note 2 When adding a prefix two vowls cannot next to each other
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III. Binary Molecular Compounds
Step 1First give the name of the first nonmetal,followed by the nonmetal name using the “ide”
suffix.Step 2
Give each nonmetal a Latin prefix describing the number of atoms present in the compound.
ExamplesCO Carbon monoxide CO2
P2O5 CCl4
Molecular means nonmetals
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III. Binary Molecular Compounds
Step 1First give the name of the first nonmetal,followed by the nonmetal name using the “ide”
suffix.Step 2
Give each nonmetal a Latin prefix describing the number of atoms present in the compound.
ExamplesCO Carbon monoxide CO2 Carbon dioxide
P2O5 CCl4
Molecular means nonmetals
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III. Binary Molecular Compounds
Step 1First give the name of the first nonmetal,followed by the nonmetal name using the “ide”
suffix.Step 2
Give each nonmetal a Latin prefix describing the number of atoms present in the compound.
ExamplesCO Carbon monoxide CO2 Carbon dioxide
P2O5 CCl4
Molecular means nonmetals
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II. Binary Ionic molecular
Step 1First give the name of the first nonmetal,followed by the nonmetal name using the “ide”
suffix.Step 2
Give each nonmetal a Latin prefix describing the number of atoms present in the compound.
ExamplesCO Carbon monoxide CO2 Carbon dioxide
P2O5 Diphosphorus Pentoxide
CCl4
Molecular means combination of nonmetals
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II. Binary Ionic molecular
Step 1First give the name of the first nonmetal,followed by the nonmetal name using the “ide”
suffix.Step 2
Give each nonmetal a Latin prefix describing the number of atoms present in the compound.
ExamplesCO Carbon monoxide CO2 Carbon dioxide
P2O5 Diphosphorus Pentoxide
CCl4 Carbon tetrachloride
Molecular means combination of nonmetals
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III. Nonbinary Molecular Compounds
Step 1Write down the memorized polyatomic ions present in the compound.
Step 2
Look to see if any monatomic ions are present. If so, then cations use the normal name. If it is an anion, then its name comes last with the “ide” suffix.
Examples
NH4Cl
NH4OH
Note: Do not use Latin prefixes
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III. Nonbinary Molecular Compounds
Step 1Write down the memorized polyatomic ions present in the compound.
Step 2
Look to see if any monatomic ions are present. If so, then cations use the normal name. If it is an anion, then its name comes last with the “ide” suffix.
Examples
NH4Cl
NH4OH
Note: Do not use Latin prefixes
Ammonium chloride
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III. Nonbinary Molecular Compounds
Step 1Write down the memorized polyatomic ions present in the compound.
Step 2
Look to see if any monatomic ions are present. If so, then cations use the normal name. If it is an anion, then its name comes last with the “ide” suffix.
Examples
NH4Cl
NH4OH
Note: Do not use Latin prefixes
Ammonium chloride
Ammonium hydroxide
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Compounds that Start with HydrogenCase 1
Case 2
Case 3
Case 4
If the anion ends in “ide” and it is aqueous, then use the prefix hydro and suffix “ic acid”
If the anion ends in “ate” then drop it and add the suffix “ic acid”
If the anion ends in “ite” then drop it and add the suffix “ous acid”
If the anion ends in” ide” and is a gas, or liquid, then leave the name and do not use Latin prefiex
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate nitric acid
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate nitric acid
nitrite
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate nitric acid
nitrite nitrous acid
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate nitric acid
nitrite nitrous acid
oxide
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate nitric acid
nitrite nitrous acid
oxide hydrogen oxide
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate nitric acid
nitrite nitrous acid
oxide hydrogen oxide
chloride
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Compounds that Start with HydrogenExamples
HCl (aq)
HNO3
HNO2
H2O (l)
HCl (aq)
chloride chloric acid hydrochloric acid
nitrate nitric acid
nitrite nitrous acid
oxide hydrogen oxide
chloride hydrogenchloride
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The End