atoms, molecules, and ions chapter 2. democritus 460 bc 460 bc first to propose atomic nature of...
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Atoms, Molecules, Atoms, Molecules, and Ionsand Ions
Chapter 2Chapter 2
DemocritusDemocritus
460 BC460 BC First to propose First to propose
atomic nature of atomic nature of mattermatter
““atomos” - atomos” - indivisibleindivisible
DaltonDalton
Studied Studied experiments experiments from other from other scientistsscientists
Law of multiple Law of multiple proportionsproportions
First Modern First Modern Atomic TheoryAtomic Theory
Dalton’s PostulatesDalton’s Postulates
Each element is composed of tiny Each element is composed of tiny particlesparticles
All atoms of an element are identicalAll atoms of an element are identical Atoms of an element are not Atoms of an element are not
changed into different types of changed into different types of atoms in a chem rxnatoms in a chem rxn
Compounds form when 2 or more Compounds form when 2 or more atoms combineatoms combine
J.J. ThomsonJ.J. Thomson
Cathode ray expeCathode ray experimentsriments
Discovered Discovered electrons and electrons and their charge-to-their charge-to-mass ratiomass ratio
Plum Pudding Plum Pudding Model of AtomModel of Atom
Plum Pudding ModelPlum Pudding Model
JJ ThomsonJJ Thomson 18971897 Electrons float in Electrons float in
a positively a positively charged ooze.charged ooze.
No nucleusNo nucleus
electrons
Positively charged ooze
MillikanMillikan
Oil drop experimOil drop experimentent
Determined the Determined the charge of the charge of the electron as -1electron as -1
RutherfordRutherford
1911 - Gold foil exp1911 - Gold foil experimenteriment
Discovered that the Discovered that the atom was mostly atom was mostly empty space with a empty space with a small dense small dense positively charged positively charged core he called the core he called the nucleusnucleus
Also discovered Also discovered protons in 1919protons in 1919
The Nuclear ModelThe Nuclear Model
19111911 RutherfordRutherford *Nucleus: *Nucleus:
positively positively charged centercharged center
Electrons orbit Electrons orbit the nucleusthe nucleus
*Atom is mostly *Atom is mostly empty space.empty space.
ChadwickChadwick
Discovered neutrDiscovered neutron in 1932on in 1932
Neutrons are Neutrons are about the same about the same size as a proton, size as a proton, but have no but have no charge.charge.
Found in nucleusFound in nucleus
BohrBohr
Planetary model Planetary model of atom in 1913of atom in 1913
Wavelengths of Wavelengths of emissions of emissions of hydrogen hydrogen spectrumspectrum
Bohr’s ModelBohr’s Model
19131913 Electrons orbit the Electrons orbit the
nucleus in specific nucleus in specific energy levelsenergy levels
Electrons can jump Electrons can jump between energy between energy levelslevels
Each energy level Each energy level holds a specific holds a specific number of electronsnumber of electrons
nucleus
Energy levels
n=1
n=2
Electron cloud modelElectron cloud model SchrodingerSchrodinger 19261926 We now know that We now know that
electrons move electrons move very fast around very fast around the nucleus.the nucleus.
This fast movement This fast movement causes the causes the electrons to form a electrons to form a “cloud” around the “cloud” around the nucleus.nucleus.
The cloud is a The cloud is a mathematical mathematical probability of where probability of where the electrons are in the electrons are in orbit.orbit.
Marie CurieMarie Curie
RadiationRadiation Discovered Discovered
radium and radium and poloniumpolonium
Used X-ray Used X-ray machines in WWImachines in WWI
BecquerelBecquerel
Discovered Discovered radiationradiation
Worked with Worked with CuriesCuries
Discovery of Atomic Discovery of Atomic StructureStructure
What is it?What is it? characteristicscharacteristics
Alpha Alpha particles particles ((αα))
Helium nucleus Helium nucleus ((44He)He)
2 protons, 2 2 protons, 2 neutrons, positive neutrons, positive chargecharge
WeakestWeakest
Beta Beta particles particles ((ββ))
High speed eHigh speed e-- emitted from emitted from nucleus at time nucleus at time of creationof creation
-1 charge-1 charge
Weak Weak
Gamma Gamma particles particles ((γγ))
High energy X-High energy X-rayray
StrongestStrongest
Cause and cure Cause and cure cancercancer
Modern View of Atomic Modern View of Atomic StructureStructure
ProtonProtonss
NeutronNeutronss
Electrons Electrons
LocatioLocationn
NucleuNucleuss
NucleusNucleus Moving very fast in Moving very fast in energy levels around energy levels around nucleusnucleus
RelativRelative sizee size
LargeLarge LargeLarge Extremely tinyExtremely tiny
ChargeCharge +1+1 00 -1-1
Symbol Symbol pp+ + nn00 ee--
Atomic Mass - based on #s of Atomic Mass - based on #s of protons, neutrons, and electrons in protons, neutrons, and electrons in the atomthe atom
protons and neutrons have about protons and neutrons have about thethesame mass and size; found in thesame mass and size; found in thenucleus; make up almost ALL of thenucleus; make up almost ALL of themass of the atommass of the atom
electrons are extremely tiny, haveelectrons are extremely tiny, havealmost NO massalmost NO mass
on periodic table, atomic mass ison periodic table, atomic mass isAVERAGE atomic massAVERAGE atomic mass
IsotopesIsotopes
isotopes - atoms of an isotopes - atoms of an element that have different element that have different massesmasses
same # of p+, differentsame # of p+, different# of n# of n
Some symbols, Some symbols, formulas, and termsformulas, and terms A = mass number = protons + A = mass number = protons +
neutronsneutrons Z = atomic number = protons Z = atomic number = protons
= electron (neutral atom)= electron (neutral atom) number of neutrons = mass # number of neutrons = mass #
- protons = A-Z- protons = A-Z
Isotopic notationIsotopic notation
Element-AElement-A AAXX X-AX-A
Neon - 20Neon - 20 2020NeNe Ne-20Ne-20
Cobalt - 60Cobalt - 60 6060CoCo Co-60Co-60
Average Atomic MassAverage Atomic Mass
Average of all the isotopes found Average of all the isotopes found in naturein nature
Naturally occurring chlorine is Naturally occurring chlorine is 75.78% 75.78% 3535Cl, which has an atomic Cl, which has an atomic mass of 34.969amu and 24.22% mass of 34.969amu and 24.22% 3737Cl, which has a mass of 36.966 Cl, which has a mass of 36.966 amu. Calculate the average amu. Calculate the average atomic mass.atomic mass.
Practice problem on page 46.Practice problem on page 46.
DevelopmentDevelopment
DobereinerDobereiner– Triads – groups of 3 based on similar Triads – groups of 3 based on similar
propertiesproperties NewlandsNewlands
– Law of octaves – same properties Law of octaves – same properties repeat every 8repeat every 8thth element element
– 7 rows of 7 elements each7 rows of 7 elements each
MendeleevMendeleev
Father of the Periodic TableFather of the Periodic Table Elements were put into columns Elements were put into columns
according to properties and according to properties and increasing atomic mass.increasing atomic mass.
Rows varied in length.Rows varied in length. LEFT BLANK SPOTS FOR LEFT BLANK SPOTS FOR
UNDISCOVERED ELEMENTS.UNDISCOVERED ELEMENTS. Properties of the elements Properties of the elements
depends on atomic mass.depends on atomic mass.
MoseleyMoseley
Used X-rays to study protons in Used X-rays to study protons in the atomsthe atoms
He noticed that atomic number He noticed that atomic number increased according to increased according to Mendeleev’s chart.Mendeleev’s chart.
Led to modern periodic lawLed to modern periodic law
Periodic Law, based on Periodic Law, based on Moseley’s WorkMoseley’s Work
The properties of the elements The properties of the elements are a periodic function of their are a periodic function of their atomic number.atomic number.
That is, the properties of the That is, the properties of the elements depends on the atomic elements depends on the atomic #.#.
OrganizationOrganization
MendeleevMendeleev Elements are arranged according to Elements are arranged according to
their properties.their properties. Each group or family (vertical columns) Each group or family (vertical columns)
have similar properties.have similar properties. Each horizontal row is called a period.Each horizontal row is called a period. The A groups (columns 1,2,13-18) are The A groups (columns 1,2,13-18) are
representative elements.representative elements. The B groups (columns 3-12) are The B groups (columns 3-12) are
transition elements.transition elements.
Family NamesFamily Names
Group IA (1) – Alkali MetalsGroup IA (1) – Alkali Metals Group IIA (2) – Alkaline Earth MetalsGroup IIA (2) – Alkaline Earth Metals Group VIA (16) – ChalcogensGroup VIA (16) – Chalcogens Group VIIA (17) – HalogensGroup VIIA (17) – Halogens Group VIIIA (18) – Noble GasesGroup VIIIA (18) – Noble Gases Groups 3-12 – Transition MetalsGroups 3-12 – Transition Metals Top Row – LanthanidesTop Row – Lanthanides Bottom Row - ActinidesBottom Row - Actinides
Valence ElectronsValence Electrons
Electrons in the outermost energy Electrons in the outermost energy level of the atom.level of the atom.
Electrons most responsible for Electrons most responsible for atom behavior.atom behavior.
Valence ElectronsValence Electrons
Alkali Metals – 1Alkali Metals – 1 Alkaline Earth Metals – 2Alkaline Earth Metals – 2 Boron Group (13) – 3Boron Group (13) – 3 Carbon Group (14) – 4Carbon Group (14) – 4 Nitrogen Group (15) – 5Nitrogen Group (15) – 5 Chalcogens – 6Chalcogens – 6 Halogens – 7Halogens – 7 Noble Gases - 8Noble Gases - 8
StabilityStability
Ultimate goal: to become stableUltimate goal: to become stable Octet rule: 8 valence electrons make an Octet rule: 8 valence electrons make an
atom stable because that completes the atom stable because that completes the outer energy level; full = stableouter energy level; full = stable
Atoms want to achieve a noble gas Atoms want to achieve a noble gas electron configuration – isoelectronic.electron configuration – isoelectronic.
Some exceptions: a full or half-full Some exceptions: a full or half-full sublevel will also make an atom sublevel will also make an atom relatively stablerelatively stable
Properties of MetalsProperties of Metals
Good conductors of heat & Good conductors of heat & electricityelectricity
Malleable (pounded into sheets)Malleable (pounded into sheets) Ductile (stretched into wires)Ductile (stretched into wires) Hard, shiny appearanceHard, shiny appearance 3 or less valence electrons 3 or less valence electrons Lose electrons to form compoundsLose electrons to form compounds Left side of PTLeft side of PT
Properties of Properties of NonmetalsNonmetals Poor conductors of heat & electricityPoor conductors of heat & electricity Good insulatorsGood insulators Solids are dull and brittle.Solids are dull and brittle. Most are gases at room Most are gases at room
temperature.temperature. 5 or more valence electrons5 or more valence electrons Gain electrons to form compoundsGain electrons to form compounds Right side of PTRight side of PT
Properties of Properties of MetalloidsMetalloids SemiconductorsSemiconductors Share electrons to form Share electrons to form
compoundscompounds Both metallic and nonmetallic Both metallic and nonmetallic
propertiesproperties Follow stair-step lineFollow stair-step line
Molecules - Molecules - Two or more Two or more atoms tightly bound atoms tightly bound togethertogether Chemical formulasChemical formulas
– HH22OO
– CaCa33(PO(PO44))22
Diatomic moleculesDiatomic molecules– BrBr22II22NN22ClCl22HH22OO22FF22
Molecular compoundsMolecular compounds– Composed of molecules and contain Composed of molecules and contain
more than one type of atommore than one type of atom Most contain only nonmetalsMost contain only nonmetals
Molecular formulaMolecular formula– Actual numbers and types of atomsActual numbers and types of atoms– HH22O; CO; C66HH66
Empirical formulaEmpirical formula– Only gives the ratio of atomsOnly gives the ratio of atoms– HH22O; CHO; CH
Structural formulaStructural formula– Shows how atoms are bondedShows how atoms are bonded
Ions and Ionic Ions and Ionic CompoundsCompounds Ion – charged particleIon – charged particle Cation – positive ionCation – positive ion Anion – negative ionAnion – negative ion Polyatomic ions – atoms joined in Polyatomic ions – atoms joined in
a molecule, but with an overall a molecule, but with an overall chargecharge
Charges (Oxidation Charges (Oxidation numbers)numbers) Pattern on PTPattern on PT Transition metals varyTransition metals vary
– Can be determined from formulaCan be determined from formula CuClCuCl22
– Are denoted with roman numeralsAre denoted with roman numerals Iron (III) nitrateIron (III) nitrate
Writing FormulasWriting Formulas
MUST HAVE CHARGES TO WRITE MUST HAVE CHARGES TO WRITE FORMULAS!!!FORMULAS!!!
Sodium chlorideSodium chloride Barium bromideBarium bromide Copper (II) sulfateCopper (II) sulfate Iron (III) nitrateIron (III) nitrate Magnesium phosphateMagnesium phosphate
Binary CompoundsBinary Compounds
Metal-nonmetal compound Metal-nonmetal compound consisting of 2 elementsconsisting of 2 elements– Name the cation.Name the cation.– Name the anion by changing the Name the anion by changing the
ending to –ide.ending to –ide. Example: NaCl – sodium chlorExample: NaCl – sodium chlorideide Example: LiExample: Li22S – lithium sulfS – lithium sulfideide
Naming Compounds Naming Compounds Containing Polyatomic Containing Polyatomic IonsIons 1. Name the cation.1. Name the cation. 2. Name the anion. Do NOT change the 2. Name the anion. Do NOT change the
ending of a polyatomic ion.ending of a polyatomic ion. Example: NaSCN – sodium thiocyanateExample: NaSCN – sodium thiocyanate Example: CaCOExample: CaCO33 – calcium carbonate – calcium carbonate
Example: NHExample: NH44Cl – ammonium chlorideCl – ammonium chloride
Transition Metals (except Transition Metals (except AgAg++, Zn, Zn+2+2, Cd, Cd+2+2))
Determine charge of cation by Determine charge of cation by looking at the formula and the anion.looking at the formula and the anion.
Name the cation, indicating charge Name the cation, indicating charge using Roman numerals in using Roman numerals in parentheses.parentheses.
Name the anion.Name the anion. Example: FeClExample: FeCl33 – iron (III) chloride – iron (III) chloride
Example: PbSOExample: PbSO44 – lead (II) sulfate – lead (II) sulfate
AcidsAcids
If the compound has an H as a If the compound has an H as a cation, it is usually an acid.cation, it is usually an acid.
HCl, HBr, HI, HCl, HBr, HI, HNOHNO33, , HClOHClO44, H, H22SOSO44 – Know these 6 strong acidsKnow these 6 strong acids
Naming acids Naming acids containing H and a containing H and a nonmetalnonmetal 1. Determine the root of the 1. Determine the root of the
nonmetal.nonmetal. 2. Place the prefix “hydro” in front of 2. Place the prefix “hydro” in front of
the base.the base. 3. Change the ending to –ic and add 3. Change the ending to –ic and add
the word “acid”the word “acid” Example: HCl: hydroExample: HCl: hydrochlorchloric acidic acid Example: Example: HBrHBr: hydrobromic acid: hydrobromic acid Example: HI: hydroiodic acidExample: HI: hydroiodic acid
Naming Acids Naming Acids containing polyatomic containing polyatomic ionsions Name the polyatomic ion, Name the polyatomic ion,
changing the ending as follows:changing the ending as follows:– -ate -ate -ic acid -ic acid– -ite -ite -ous acid -ous acid
Example: Example: HNOHNO33: nitric acid: nitric acid
Example: Example: HNOHNO22: nitrous acid: nitrous acid
Naming compounds Naming compounds containing 2 containing 2 nonmetalsnonmetals
Name the compound following the rules Name the compound following the rules for binary compounds and add prefixes for binary compounds and add prefixes to indicate the number of each atom in to indicate the number of each atom in the compound. the compound.
Prefixes:Prefixes:– Mono – 1Mono – 1 hexa - 6hexa - 6– Di- 2Di- 2 hepta - 7hepta - 7– Tri – 3Tri – 3 octa - 8octa - 8– Tetra – 4Tetra – 4 nona - 9nona - 9– Penta – 5Penta – 5 deca - 10deca - 10
Naming compounds Naming compounds containing 2 nonmetalscontaining 2 nonmetals
Example: Example: SS22OO88 : disulfur octoxide : disulfur octoxide
Example: Example: PP33NN55 : triphosphorous : triphosphorous
pentanitridepentanitride Example: CO: carbon monoxideExample: CO: carbon monoxide Example: CO2: carbon dioxideExample: CO2: carbon dioxide
Polyatomic IonsPolyatomic Ions Ions that consist of more than one atomIons that consist of more than one atom Know the ones for the quiz; list for othersKnow the ones for the quiz; list for others Naming of Pis with ONaming of Pis with O
– Most common form –Most common form –ate; ate; ClOClO33-- chlorate chlorate
– One less O: -One less O: -ite; ite; ClOClO22-- chlorite chlorite
– Two less O: Two less O: hypo<hypo<root>root>ite; ite; ClOClO-- hypochlorite hypochlorite
– One more O: One more O: perper<root><root>ate; ate; ClOClO44-- perchlorate perchlorate