che 106 prof. j. t. spencer 1 chapter seven: periodicity v periodic table - organizes many...
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CHE 106 Prof. J. T. Spencer 1
Chapter Seven: PeriodicityChapter Seven: PeriodicityChapter Seven: PeriodicityChapter Seven: Periodicity
Periodic Table - Organizes Periodic Table - Organizes many “facts” and trends in many “facts” and trends in chemical reactivitychemical reactivity
Based upon electronic Based upon electronic configurations of the elementsconfigurations of the elements
Similarities in electronic Similarities in electronic properties leads to similarities properties leads to similarities in chemical reactivity and in chemical reactivity and structurestructure
Copyright J. T. Spencer 1995 - 1997
CHE 106 Prof. J. T. Spencer 2
Chapter Seven: PeriodicityChapter Seven: PeriodicityChapter Seven: PeriodicityChapter Seven: Periodicity
Element - Element - a substance that cannot be a substance that cannot be decomposed into simpler substances decomposed into simpler substances by chemical or physical meansby chemical or physical means..
Most elements not found in nature in Most elements not found in nature in “elemental” form but in combination “elemental” form but in combination with other elements (particularly H with other elements (particularly H or O) in the form of mineralsor O) in the form of minerals
Prior to 1800, 31 elements known Prior to 1800, 31 elements known (mostly those that were found in (mostly those that were found in elemental form in nature (i.e., gold, elemental form in nature (i.e., gold, silver, nitrogen, etc...).silver, nitrogen, etc...).
CHE 106 Prof. J. T. Spencer 3
Periodic Table Periodic Table DevelopmentDevelopmentPeriodic Table Periodic Table DevelopmentDevelopment
Between 1800 and 1865, 32 more were Between 1800 and 1865, 32 more were isolated by improved chemical techniques.isolated by improved chemical techniques.
Dmitri Mendeleev - noted that chemical and Dmitri Mendeleev - noted that chemical and physical properties recur periodically when physical properties recur periodically when the elements are arranged in order of the elements are arranged in order of increasing atomic weight. (atomic number increasing atomic weight. (atomic number not known then although atomic weights not known then although atomic weights generally follow atomic number sequence)generally follow atomic number sequence)
When he created the table, he was forced When he created the table, he was forced to leave blank spaces for “undiscovered” to leave blank spaces for “undiscovered” elements but he correctly predicted many elements but he correctly predicted many of their properties by use of his table.of their properties by use of his table.
CHE 106 Prof. J. T. Spencer 4
Mendeleev’s GuessesMendeleev’s GuessesMendeleev’s GuessesMendeleev’s Guesses
Mendeleev’s guesses Mendeleev’s guesses Observed Observed for Ge (1871) for Ge (1871)
properties properties for Ge (1886)for Ge (1886)
Atomic WeightAtomic Weight 7272 72.5972.59DensityDensity 5.55.5 5.355.35Specific Heat (J/gK)Specific Heat (J/gK) 0.3050.305 0.3090.309Melting Point (°C)Melting Point (°C) HighHigh 947947Oxide FormulaOxide Formula XOXO22 GeOGeO22
Density of Oxide Density of Oxide 4.7 g/cm4.7 g/cm33 4.70 4.70 g/cmg/cm33
Chloride FormulaChloride Formula XClXCl44 GeClGeCl44
Chloride b.p. (°C)Chloride b.p. (°C) <100<100 8484
Guesses for Ge based upon Periodic TrendsGuesses for Ge based upon Periodic Trends
Table in TEXT
CHE 106 Prof. J. T. Spencer 5
Mendeleev’s GuessesMendeleev’s GuessesMendeleev’s GuessesMendeleev’s Guesses
Mendeleev’s guesses Mendeleev’s guesses Observed Observed for Ge (1871) for Ge (1871)
properties properties for Ge (1886)for Ge (1886)
Atomic WeightAtomic Weight 7272 72.5972.59DensityDensity 5.55.5 5.355.35Specific Heat (J/gK)Specific Heat (J/gK) 0.3050.305 0.3090.309Melting Point (°C)Melting Point (°C) HighHigh 947947Oxide FormulaOxide Formula XOXO22 GeOGeO22
Density of Oxide Density of Oxide 4.7 g/cm4.7 g/cm33 4.70 4.70 g/cmg/cm33
Chloride FormulaChloride Formula XClXCl44 GeClGeCl44
Chloride b.p. (°C)Chloride b.p. (°C) <100<100 8484
Guesses for Ge based upon Periodic TrendsGuesses for Ge based upon Periodic Trends
Table in TEXT
CHE 106 Prof. J. T. Spencer 6
Periodic DevelopmentPeriodic DevelopmentPeriodic DevelopmentPeriodic Development
Moseley (1887-1915) discovered Moseley (1887-1915) discovered atomic number concept (atomic atomic number concept (atomic number = number or protons and number = number or protons and electrons in an atom) from assigning electrons in an atom) from assigning X-ray from the elements.X-ray from the elements.
Periodic Table:Periodic Table:– column or column or groupsgroups (increasing n, (increasing n,
principal quantum numberprincipal quantum number, on , on descendingdescending
GGrroouupp
PeriodPeriod
CHE 106 Prof. J. T. Spencer 7
Periodic TablePeriodic TablePeriodic TablePeriodic Table
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1H 2He
3Li 4Be 5B 6C 7N 8O 9F 10Ne
11Na 12Mg 13Al 14Si 15P 16S 17Cl 18Ar
19K 20Ca 21Sc 22Ti 23V 24Cr 25Mn 26Fe 27Co 28Ni 29Cu 30Zn 31Ga 32Ge 33As 34Se 35Br 36Kr
37Rb 38Sr 39Y 40Zr 41Nb 42Mo 43Tc 44Ru 45Rh 46Pd 47Ag 48Cd 49In 50Sn 51Sb 52Te 53I 54Xe
55Cs 56Ba 57La 72Hf 73Ta 74W 75Re 76Os 77Ir 78Pt 79Au 80Hg 81Tl 82Pb 83Bi 84Po 85At 86Rn
87Fr 88Ra 89Ac 104Unq 105Unp 106Unh 107Ns 108Hs 109Mt
58Ce 59Pr 60Nd 61Pm 62Sm 63Eu 64Gd 65Tb 66Dy 67Ho 68Er 69Tm 70Yb 71Lu
90Th 91Pa 92U 93Np 94Pu 95Am 96Cm 97Bk 98Cf 99Es 100Fm 101Md 102No 103Lr
s orbitalss orbitals
p orbitalsp orbitals
d orbitalsd orbitals
f orbitalsf orbitals
closed shellclosed shell
3d3d3d3d
4d4d4d4d
5d5d5d5d
6d6d6d6d
2s2s2s2s
3s3s3s3s
4s4s4s4s
5s5s5s5s
6s6s6s6s
7s7s7s7s
2p2p2p2p
3p3p3p3p
4p4p4p4p
5p5p5p5p
6p6p6p6p
4f4f4f4f
5f5f5f5f
CHE 106 Prof. J. T. Spencer 8
““Electron Shells”Electron Shells”““Electron Shells”Electron Shells”
Electrons with same principal energy value are in Electrons with same principal energy value are in the same “shell”.the same “shell”.
Why is the Ar n = 1 closer than n = 1 Ne or He? Why is the Ar n = 1 closer than n = 1 Ne or He? SCREENINGSCREENING!!
22 (rad)(rad)
Distance from NucleusDistance from Nucleus
ArAr
NeNe
HeHe
Helium showed 1 shell (n = 1)Helium showed 1 shell (n = 1)Neon showed 2 shells (n = 1,2)Neon showed 2 shells (n = 1,2)
Argon showed 3 shells ( n= 1,2,3)Argon showed 3 shells ( n= 1,2,3)
CHE 106 Prof. J. T. Spencer 9
In many electron atoms, electron-electron In many electron atoms, electron-electron repulsions become more important than repulsions become more important than electron-nuclear attractions.electron-nuclear attractions.
Estimate the energy of an electron in an orbital Estimate the energy of an electron in an orbital by considering how it, on the average, interacts by considering how it, on the average, interacts with its electronic environment (treat electrons with its electronic environment (treat electrons individually).individually).
The net attractive force that an electron will feel The net attractive force that an electron will feel is the is the effective nuclear chargeeffective nuclear charge (Z (Zeffeff).).
ZZeffeff = Z - S = Z - S Screening is the average number of other Screening is the average number of other
electrons that are between the electron and the electrons that are between the electron and the nucleus.nucleus.
Screening (Shielding)Screening (Shielding)Screening (Shielding)Screening (Shielding)
Z = nuclear chargeS = screening valueZ = nuclear chargeS = screening value
CHE 106 Prof. J. T. Spencer 10
Screening (Shielding)Screening (Shielding)Screening (Shielding)Screening (Shielding)
rr
Average electronic charge (S) between the nucleus and the electron of interest
Electrons outside of sphere of radius r have very little effect
on the effective nuclear charge experienced by the electron at
radius r
Zeff = Z - S
ZZ
The larger The larger the Zthe Zeffeff an an
electron electron feels leads feels leads to a lower to a lower energy for energy for
the electronthe electron
CHE 106 Prof. J. T. Spencer 11
Atomic SizesAtomic SizesAtomic SizesAtomic Sizes
Atoms as hard spheres vs. quantum Atoms as hard spheres vs. quantum mechanical picture without sharply mechanical picture without sharply defined boundaries. (electron defined boundaries. (electron density does not abruptly stop)density does not abruptly stop)
Estimate atomic radii by assuming Estimate atomic radii by assuming that atoms are spheres that “touch” that atoms are spheres that “touch” when bonded together in molecules. when bonded together in molecules.
Atomic radii are approx. constant Atomic radii are approx. constant when an atom is bonded in many when an atom is bonded in many compounds.compounds.
CHE 106 Prof. J. T. Spencer 12
Atomic RadiiAtomic RadiiAtomic RadiiAtomic Radii
Periodic TablePeriodic Table
Radius IncreasesRadius Increases
2r2r
1. Radii 1. Radii increase increase
from top to from top to bottom within a bottom within a
groupgroup2. Radii 2. Radii
increase in increase in moving R to L moving R to L
within a periodwithin a period
Molecule Bond Distance (pm)H2 74 pmF2 272 pmC-C 154 pmCH 114 pmCF 213 pm
CHE 106 Prof. J. T. Spencer 13
For Outer electron:For Outer electron:Boron; ZBoron; Zeffeff (approx.) = 5 - 4 = 1 nuclear charge (approx.) = 5 - 4 = 1 nuclear charge
Carbon; ZCarbon; Zeffeff (approx.) = 6 - 4 = 2 nuclear charges (approx.) = 6 - 4 = 2 nuclear charges
Nitrogen; ZNitrogen; Zeffeff (approx.) = 7 - 4 = 3 nuclear charges (approx.) = 7 - 4 = 3 nuclear charges
Fluorine; ZFluorine; Zeffeff (approx.) = 9 - 4 = 5 nuclear charges (approx.) = 9 - 4 = 5 nuclear charges
Why does radius decrease across a Why does radius decrease across a group?group?– Nuclear charge increases while Nuclear charge increases while
screening does not increase.screening does not increase.
Atomic SizesAtomic SizesAtomic SizesAtomic Sizes
Periodic TablePeriodic Table
Radius IncreasesRadius Increases 2p electrons DO NOT 2p electrons DO NOT screen each other screen each other while the 2s very while the 2s very effectively screen the effectively screen the 2p, also each element 2p, also each element to right adds +1 to to right adds +1 to nucleus.nucleus.
CHE 106 Prof. J. T. Spencer 14
Atomic SizesAtomic SizesAtomic SizesAtomic Sizes
Li < Na < K < Rb < Cs, due to increasing n Li < Na < K < Rb < Cs, due to increasing n values.values.
Li > F because of ZLi > F because of Zeffeff changes. changes.
LiLiNaNa
KKRbRb
FF ClCl BrBr II
AtomicAtomicRadiusRadius
(Å)(Å)
Atomic NumberAtomic Number
TransitionMetals
TransitionMetals
1010 20 20 30 30 40 40 50 50
CHE 106 Prof. J. T. Spencer 15
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Fe Fe (232 pm)(232 pm)
FeFe+2 +2
(152 pm)(152 pm)FeFe+3 +3
(128 pm)(128 pm)
FF(128 pm)(128 pm)
F F -1 -1
(272 pm)(272 pm)Li Li
(304 pm)(304 pm)LiLi++
(120 pm)(120 pm)
CHE 106 Prof. J. T. Spencer 16
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Sample exercise: Predict which will be greater, the P-Br bond length in PBr3 or the As-Cl bond length in AsCl3.
CHE 106 Prof. J. T. Spencer 17
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Sample exercise: Predict which will be greater, the P-Br bond length in PBr3 or the As-Cl bond length in AsCl3.
PBr3 P - 1.06Br - 1.14
Length: 2.20
CHE 106 Prof. J. T. Spencer 18
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Sample exercise: Predict which will be greater, the P-Br bond length in PBr3 or the As-Cl bond length in AsCl3.
PBr3 P - 1.06Br - 1.14
Length: 2.20
AsCl3 As - 1.19Cl - 0.99
Length: 2.18
CHE 106 Prof. J. T. Spencer 19
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Sample exercise: Arrange the following atoms in order of increasing atomic radius: Na, Be, Mg
CHE 106 Prof. J. T. Spencer 20
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Sample exercise: Arrange the following atoms in order of increasing atomic radius: Na, Be, Mg
- radius decreases as you go across the period, increases as you go down the group.
CHE 106 Prof. J. T. Spencer 21
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Sample exercise: Arrange the following atoms in order of increasing atomic radius: Na, Be, Mg
- radius decreases as you go across the period, increases as you go down the group.
CHE 106 Prof. J. T. Spencer 22
Atomic Sizes: Charge Atomic Sizes: Charge EffectsEffectsAtomic Sizes: Charge Atomic Sizes: Charge EffectsEffects
Sample exercise: Arrange the following atoms in order of increasing atomic radius: Na, Be, Mg
- radius decreases as you go across the period, increases as you go down the group.
Be < Mg < Na
CHE 106 Prof. J. T. Spencer 23
Ionization Energy (IE)Ionization Energy (IE)Ionization Energy (IE)Ionization Energy (IE)
Electrons are “exchanged” in many chemical Electrons are “exchanged” in many chemical reactions. [i.e., A gives electron(s) to B]reactions. [i.e., A gives electron(s) to B]
Ionization EnergyIonization Energy (IE) measures how strongly an (IE) measures how strongly an atom holds on to its electrons (atom holds on to its electrons (the minimum energy the minimum energy necessary to remove an electron from the ground necessary to remove an electron from the ground state of an isolated gaseous atomstate of an isolated gaseous atom).).
Higher ionization processes are possible:Higher ionization processes are possible:
– first IE - remove 1st electron; first IE - remove 1st electron; AA AA+1+1 + e + e--
– second IE - remove 2nd electron;second IE - remove 2nd electron; AA+1+1
AA+2+2 + e + e--
– third IE - remove 3rd electron;third IE - remove 3rd electron; AA+2+2 AA+3+3 + e + e--
E(g)E(g) EE+1+1(g) + 1 e(g) + 1 e--
CHE 106 Prof. J. T. Spencer 24
Ionization EnergiesIonization EnergiesIonization EnergiesIonization Energies II11 < I < I22 < I < I33 (increasing positive charge on atom). (increasing positive charge on atom). Very sharp increase in IE when an inner shell Very sharp increase in IE when an inner shell
(core) electron is removed.(core) electron is removed. Within each period, IWithin each period, I11, generally increases with , generally increases with
increasing atomic number (increasing Zincreasing atomic number (increasing Zeffeff).). Within each group, IE generally decreases with Within each group, IE generally decreases with
increasing atomic number (“bigger” atoms).increasing atomic number (“bigger” atoms).
Periodic TablePeriodic Table
1st IE Increases1st IE Increases
CHE 106 Prof. J. T. Spencer 25
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
HH (1s (1s11))
HeHe (1s (1s22))
Atomic NumberAtomic Number
1st IE1st IE(kJ/mol)(kJ/mol)
CHE 106 Prof. J. T. Spencer 26
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
HH (1s (1s11))
HeHe (1s (1s22))
Li Li (1s(1s222s2s11))
Atomic NumberAtomic Number
1st IE1st IE(kJ/mol)(kJ/mol)
CHE 106 Prof. J. T. Spencer 27
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
HH (1s (1s11))
HeHe (1s (1s22))
Li Li (1s(1s222s2s11))
Atomic NumberAtomic Number
1st IE1st IE(kJ/mol)(kJ/mol) BeBe (1s (1s222s2s22))
CHE 106 Prof. J. T. Spencer 28
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
HH (1s (1s11))
HeHe (1s (1s22)) (1s(1s222s2s222p2p66) ) NeNe
Li Li (1s(1s222s2s11))
Atomic NumberAtomic Number
1st IE1st IE(kJ/mol)(kJ/mol) BeBe (1s (1s222s2s22))
BB (1s (1s222s2s222p2p11))
C C (1s(1s222s2s222p2p22))
(1s(1s222s2s222p2p33) ) NN
O O (1s(1s222s2s222p2p44))
F F (1s(1s222s2s222p2p55))
1s 2s 2p 2p 2p1s 2s 2p 2p 2p
CHE 106 Prof. J. T. Spencer 29
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
HH
HeHe NeNe
LiLi
Atomic NumberAtomic Number
1st IE1st IE(kJ/mol)(kJ/mol) BeBe
BB
CC
NN O O
FF
ZZeffeff = 1 to 2 = 1 to 2
ZZeffeff = 1 to 2 = 1 to 2
ZZeffeff = 2 to 3 = 2 to 3
ZZeffeff = 1 to 2 = 1 to 2
ZZeffeff = 4 to 5 = 4 to 5
ZZeffeff = 5 to 6 = 5 to 6
Screening and increasing Zeff
2s to 2p2s to 2p
CHE 106 Prof. J. T. Spencer 30
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
HH
HeHe NeNe
LiLi
Atomic NumberAtomic Number
1st IE1st IE(kJ/mol)(kJ/mol) BeBe
BB
CC
NN O O
FF
88OO1s 2s 2p 2p 2p1s 2s 2p 2p 2p
n = 1 to 2n = 1 to 2
pairing energypairing energy
increasing n andpairing energy
CHE 106 Prof. J. T. Spencer 31
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
HH
HeHe
NeNe
ArArKrKr
LiLi NaNa KK RbRb
Atomic NumberAtomic Number
1st IE1st IE(kJ/mol)(kJ/mol)
24002400
18001800
12001200
600600
Trends recur throughout periodic tableTrends recur throughout periodic table
CHE 106 Prof. J. T. Spencer 32
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
Elem.Elem. Elec. Config.Elec. Config. I I11 I I22 I I33 I I44 I I55 I I66
NaNa [Ne]3s[Ne]3s11 496496 45604560
MgMg [Ne]3s[Ne]3s22 738738 14501450 77307730
AlAl [Ne]3s[Ne]3s223p3p11 577577 18161816 27442744 1160011600
SiSi [Ne]3s[Ne]3s223p3p22 786786 15771577 32283228 43544354 1610016100
PP [Ne]3s[Ne]3s223p3p33 10601060 18901890 29052905 49504950 627062702120021200
SS [Ne]3s[Ne]3s223p3p44 999999 22602260 33753375 45654565 6950695084908490
Core ElectronsCore ElectronsBeing RemovedBeing Removed
CHE 106 Prof. J. T. Spencer 33
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
Sample exercise: Based on the Sample exercise: Based on the trends discussed in this section, trends discussed in this section, predict which of the following atoms, predict which of the following atoms, B, Al, C, or Si - has the lowest first B, Al, C, or Si - has the lowest first ionization energy.ionization energy.
CHE 106 Prof. J. T. Spencer 34
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
Sample exercise: Based on the Sample exercise: Based on the trends discussed in this section, trends discussed in this section, predict which of the following atoms, predict which of the following atoms, B, Al, C, or Si - has the lowest first B, Al, C, or Si - has the lowest first ionization energy.ionization energy.
As atoms get smaller, the ionization energy gets As atoms get smaller, the ionization energy gets larger, so the lowest ionization energy belongs to larger, so the lowest ionization energy belongs to the largest atom.the largest atom.
CHE 106 Prof. J. T. Spencer 35
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
Sample exercise: Based on the Sample exercise: Based on the trends discussed in this section, trends discussed in this section, predict which of the following atoms, predict which of the following atoms, B, Al, C, or Si - has the lowest first B, Al, C, or Si - has the lowest first ionization energy.ionization energy.
As atoms get smaller, the ionization energy gets As atoms get smaller, the ionization energy gets larger, so the lowest ionization energy belongs to larger, so the lowest ionization energy belongs to the largest atom.the largest atom.
Size decreases as you go across the period, so Size decreases as you go across the period, so the left-most atom is the largest.the left-most atom is the largest.
CHE 106 Prof. J. T. Spencer 36
Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)Ionization Energies (IE)
Sample exercise: Based on the Sample exercise: Based on the trends discussed in this section, trends discussed in this section, predict which of the following atoms, predict which of the following atoms, B, Al, C, or Si - has the lowest first B, Al, C, or Si - has the lowest first ionization energy.ionization energy.
As atoms get smaller, the ionization energy gets As atoms get smaller, the ionization energy gets larger, so the lowest ionization energy belongs to larger, so the lowest ionization energy belongs to the largest atom.the largest atom.
Size decreases as you go across the period, so Size decreases as you go across the period, so the left-most atom is the largest.the left-most atom is the largest.
AlAl
CHE 106 Prof. J. T. Spencer 37
Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)
Electron Affinity - Electron Affinity - the energy associated with the energy associated with adding an electron to a gaseous atomadding an electron to a gaseous atom..
E(g) + eE(g) + e-1-1 E E--
11(g)(g) Signs;Signs;
– Negative (exothermic) when energy is Negative (exothermic) when energy is released upon adding an electron.released upon adding an electron.
– Positive (endothermic) when energy is Positive (endothermic) when energy is required to add an electron.required to add an electron.
– Most neutral atoms and all ions (cations) Most neutral atoms and all ions (cations) have negative (exothermic) EA’s.have negative (exothermic) EA’s.
CHE 106 Prof. J. T. Spencer 38
Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)
200200
100100
00
-100-100
-200-200
-300-300
-400-400
EAEA(kJ/mol)(kJ/mol)
Atomic NumberAtomic Number
HH
HeHe
LiLi
BeBe
BB
CC
NN
OO
FF
NeNe
NaNa
MgMg
AlAl
SiSi
PP
SS
ClCl
ArAr
KK
CsCs
CHE 106 Prof. J. T. Spencer 39
Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)
00EAEA
(kJ/mol)(kJ/mol)
Atomic NumberAtomic Number
HeHe
LiLi
BeBe
FF
NeNe
NaNa
MgMg
ClCl
ArAr
KK
CsCsFilled Filled Shell Shell
AlreadyAlready
ns to npns to np
npnp55 to to Filled Filled Shell Shell
nsns11 to to
nsns22
CHE 106 Prof. J. T. Spencer 40
Summary of General Observations:Summary of General Observations:– Neutral atoms and cations, EA exothermic (neg).Neutral atoms and cations, EA exothermic (neg).
– EA becomes more negative across period (ZEA becomes more negative across period (Zeffeff increases).increases).
– Group 2 EA positive because of nsGroup 2 EA positive because of ns22 to ns to ns22npnp11 addition.addition.
– Gp 18 has filled shell (no need to gain electrons).Gp 18 has filled shell (no need to gain electrons).– Gp 15 has significant electron-electron Gp 15 has significant electron-electron
repulsions (pairing electrons going from nsrepulsions (pairing electrons going from ns22npnp33 to to nsns22npnp44).).
– EA’s do not range significantly down group EA’s do not range significantly down group (because decreased nuclear attraction (Z(because decreased nuclear attraction (Zeffeff) is ) is offset by decreased electron-electron repulsions).offset by decreased electron-electron repulsions).
Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)Electron Affinities (EA)
CHE 106 Prof. J. T. Spencer 41
Trends and Group Trends and Group PropertiesPropertiesTrends and Group Trends and Group PropertiesProperties
Trends of radius, IE, EA, etc. are useful in Trends of radius, IE, EA, etc. are useful in predicting chemical behaviorpredicting chemical behavior
radius, IE, etc.. are ATOMIC properties radius, IE, etc.. are ATOMIC properties (individual atoms) which only noble gases exist (individual atoms) which only noble gases exist as isolated atoms in nature.as isolated atoms in nature.
Trends and properties of groups of atoms (and Trends and properties of groups of atoms (and atoms in compounds) are also useful (i.e., atoms in compounds) are also useful (i.e., metal, non-metal, conductor, insulator, etc...).metal, non-metal, conductor, insulator, etc...).
Periodic TablePeriodic Table
Non metal characterNon metal characterincreasesincreases
CHE 106 Prof. J. T. Spencer 42
Metals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloidsMetals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloids
metalsmetals non-metalsnon-metals
GoldGold GraphiteGraphite
CHE 106 Prof. J. T. Spencer 43
Metals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloidsMetals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloids
metalsmetals non-metalsnon-metalsconductorsconductors insulatorsinsulators
shinyshiny dulldull
high thermal conductivityhigh thermal conductivitythermal insulatorsthermal insulators
solids at RTsolids at RT (except Hg) (except Hg) freq. non-solids at RTfreq. non-solids at RT
ductile and malleableductile and malleable brittlebrittle
Metalloids (along line in table) have properties between metals and non-metals
CHE 106 Prof. J. T. Spencer 44
Metals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloidsMetals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloids
metalsmetals non-metalsnon-metalsLow Ionization EnergiesLow Ionization Energies High IEHigh IE
tend to form cationstend to form cations tend to form anions tend to form anions
TM’s form multiple + statesTM’s form multiple + states Tend to form single Tend to form single (-) (-) states states
Basic OxidesBasic Oxides Acidic OxidesAcidic Oxides
Metalloids (along line in table) have properties between metals and non-metals
CHE 106 Prof. J. T. Spencer 45
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1H 2He
3Li 4Be 5B 6C 7N 8O 9F 10Ne
11Na 12Mg 13Al 14Si 15P 16S 17Cl 18Ar
19K 20Ca 21Sc 22Ti 23V 24Cr 25Mn 26Fe 27Co 28Ni 29Cu 30Zn 31Ga 32Ge 33As 34Se 35Br 36Kr
37Rb 38Sr 39Y 40Zr 41Nb 42Mo 43Tc 44Ru 45Rh 46Pd 47Ag 48Cd 49In 50Sn 51Sb 52Te 53I 54Xe
55Cs 56Ba 57La 72Hf 73Ta 74W 75Re 76Os 77Ir 78Pt 79Au 80Hg 81Tl 82Pb 83Bi 84Po 85At 86Rn
87Fr 88Ra 89Ac 104Unq 105Unp 106Unh 107Ns 108Hs 109Mt
58Ce 59Pr 60Nd 61Pm 62Sm 63Eu 64Gd 65Tb 66Dy 67Ho 68Er 69Tm 70Yb 71Lu
90Th 91Pa 92U 93Np 94Pu 95Am 96Cm 97Bk 98Cf 99Es 100Fm 101Md 102No 103Lr
metalsmetals
metalloidsmetalloids
non-metalsnon-metals
Metals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloidsMetals, Nonmetals and Metals, Nonmetals and MetalloidsMetalloids
Metallic Metallic PropertiesPropertiesIncreaseIncrease
NonmetalliNonmetallic c
PropertiesPropertiesIncreaseIncrease
CHE 106 Prof. J. T. Spencer 46
Compounds of metals and nonmetals tend to be Compounds of metals and nonmetals tend to be ionic.ionic.
Metal Oxides are basic;Metal Oxides are basic; Metal Oxide + WaterMetal Oxide + WaterMetal Hydroxide Metal Hydroxide NaNa22O(s) + HO(s) + H22O(l)O(l)2 NaOH(aq)2 NaOH(aq) KK22O(s) + HO(s) + H22O(l)O(l) 2 2 KOH(aq)KOH(aq) MgO(s) + HMgO(s) + H22O(l)O(l)Mg(OH)Mg(OH)22(aq)(aq) Metal Oxide + AcidMetal Oxide + AcidSalt + WaterSalt + Water MgO(s) + 2 HCl(aq)MgO(s) + 2 HCl(aq)MgClMgCl22(aq) + H(aq) + H22O(l)O(l) FeFe22OO33(s) + 3HNO(s) + 3HNO33(aq)(aq)Fe(NOFe(NO33))33(aq) + 3H(aq) + 3H22O(l)O(l) CuO(s) + HCuO(s) + H22SOSO44(aq)(aq)CuSOCuSO44(aq) + H(aq) + H22O(l)O(l)
Metal Compounds : Metal Metal Compounds : Metal OxidesOxidesMetal Compounds : Metal Metal Compounds : Metal OxidesOxides
CHE 106 Prof. J. T. Spencer 47
Nonmetals reacting with metals give salts Nonmetals reacting with metals give salts (electron receivers)(electron receivers)
Non metal oxides are acidic;Non metal oxides are acidic;Nonmetal oxide + waterNonmetal oxide + water
acidacid PP44OO1010(s) + 6 H(s) + 6 H22O(l)O(l)4 H4 H33POPO44(aq)(aq) BB22OO33(s) + 3 H(s) + 3 H22O(l)O(l)2 H2 H33BOBO33(aq)(aq) SOSO33(g) + H(g) + H22O(l)O(l)HH22SOSO44(aq)(aq) Nonmetal oxide + baseNonmetal oxide + base
salt + watersalt + waterCOCO22(g) + 2NaOH(aq)(g) + 2NaOH(aq)
NaNa22COCO33(aq) + H(aq) + H22O(l) BO(l) B22OO33(s) + 6NaOH(s) + 6NaOH2NaBO2NaBO33(aq) + 6H(aq) + 6H22O(l)O(l)
Non-metal CompoundsNon-metal CompoundsNon-metal CompoundsNon-metal Compounds
CHE 106 Prof. J. T. Spencer 48
COCO22 Nonmetal Chemistry Nonmetal ChemistryCOCO22 Nonmetal Chemistry Nonmetal Chemistry
Carbon dioxide (COCarbon dioxide (CO22) is a “typical” non-metal ) is a “typical” non-metal
and dissolves in water to form an acidic and dissolves in water to form an acidic solution:solution:
COCO22(s) + H(s) + H22O(l)O(l) HH22COCO33(aq)(aq)
HH22COCO33(aq) + H(aq) + H22O(l)O(l) HH33OO++(aq) + (aq) +
HCOHCO33--(aq)(aq) HCOHCO33
--(aq) + H(aq) + H22O(l)O(l) HH33OO++(aq) + (aq) +
COCO33-2-2(aq)(aq)
pH - measure of the acidity of a solution.pH - measure of the acidity of a solution.
Indicators - display different colors depending Indicators - display different colors depending upon the pH of the solution.upon the pH of the solution.
Demonstration 6.2
Nonmetal oxides are acidicNonmetal oxides are acidic
CHE 106 Prof. J. T. Spencer 49
Along Diagonal Line in Periodic TableAlong Diagonal Line in Periodic Table
Have properties between metals and Have properties between metals and nonmetalsnonmetals
Metalloid oxides - AMPHOTERIC -Metalloid oxides - AMPHOTERIC -
–As bases:As bases:AlAl22OO33 + 6H + 6H++ 2Al2Al+3+3 + 3 H + 3 H22OO
–As Acids:As Acids: AlAl22OO33
+ 2OH+ 2OH-- + 3 H + 3 H22OO 2 Al(OH) 2 Al(OH)44--
MetalloidsMetalloidsMetalloidsMetalloids
CHE 106 Prof. J. T. Spencer 50
Group Trends: Group I Group Trends: Group I (1A)(1A)Group Trends: Group I Group Trends: Group I (1A)(1A)
33LiLi77
1111NaNa2323
1919KK3939
3737RbRb8585
5555CsCs133133
8787FrFr223223
Alkali MetalsAlkali Metals
MOST REACTIVEMOST REACTIVE
LiLi NaNa K K
CHE 106 Prof. J. T. Spencer 51
Group Trends: Group I Group Trends: Group I (1A)(1A)Group Trends: Group I Group Trends: Group I (1A)(1A)
33LiLi77
1111NaNa2323
1919KK3939
3737RbRb8585
5555CsCs133133
8787FrFr223223
Alkali MetalsAlkali Metals
1st IE 1st IE decreasedecrease
ss
Radius Radius increaseincrease
ss
mp/bp mp/bp decreasedecrease
ss
electron electron sharing dec. sharing dec. (covalency)(covalency)
MOST REACTIVEMOST REACTIVE
CHE 106 Prof. J. T. Spencer 52
Group Trends: Group I Group Trends: Group I (1A)(1A)Group Trends: Group I Group Trends: Group I (1A)(1A)
Soft, metallic solids.Soft, metallic solids. Low first ionization energies (electron Low first ionization energies (electron
donors); form +1 ions. Form pure metals donors); form +1 ions. Form pure metals by electrolysis (passing electrical current by electrolysis (passing electrical current through a molten salt).through a molten salt).
2Na2Na++ + 2e + 2e-- 2 Na2 Na 2Cl2Cl--
ClCl22 + 2 e + 2 e--
Reactions dominated by 1 electron loss Reactions dominated by 1 electron loss (to 1+) [i.e., Rx with hydrogen = MH; Rx (to 1+) [i.e., Rx with hydrogen = MH; Rx with S = Mwith S = M22S,etc...].S,etc...].
MH are hydride compounds (HMH are hydride compounds (H-1-1 not H not H++).).
33LiLi77
1111NaNa2323
1919KK3939
3737RbRb8585
5555CsCs133133
8787FrFr223223
CHE 106 Prof. J. T. Spencer 53
Group Trends: Group I Group Trends: Group I (1A)(1A)Group Trends: Group I Group Trends: Group I (1A)(1A)
Oxides:Oxides:Li + OLi + O22 2Li 2Li22OO lithium lithium
oxide [O]oxide [O]2-2- 2Na + O2Na + O22 Na Na22OO22 sodium peroxide [Osodium peroxide [O22]]2-2-K + OK + O22
KO KO22 pot. superoxide [Opot. superoxide [O22]]--
React with water to form React with water to form hydroxides;hydroxides; 2M + 2 H2M + 2 H22OO
2 MOH(aq) + H2 MOH(aq) + H22
HH22O O reactivity; Li - v. slowly; Na - reactivity; Li - v. slowly; Na - vigorously; K - inflames; Rb & Cs - vigorously; K - inflames; Rb & Cs - explodeexplode
React Flame Tests - elements React Flame Tests - elements excited to higher state by the excited to higher state by the flame and then emit light as they flame and then emit light as they return to the ground state (Na - return to the ground state (Na - yellow, 3p to 3s).yellow, 3p to 3s).
33LiLi77
1111NaNa2323
1919KK3939
3737RbRb8585
5555CsCs133133
8787FrFr223223
CHE 106 Prof. J. T. Spencer 54
Flame TestsFlame TestsFlame TestsFlame Tests
CHE 106 Prof. J. T. Spencer 55
Group Trends: Group 2 Group Trends: Group 2 (2A)(2A)Group Trends: Group 2 Group Trends: Group 2 (2A)(2A)
44BeBe99
1212MgMg2424
2020CaCa4040
3838SrSr8787
5656BaBa137137
8888RaRa226226
Alkaline Earth MetalsAlkaline Earth Metals
MOST REACTIVEMOST REACTIVE
MgMg Ca Ca
CHE 106 Prof. J. T. Spencer 56
Group Trends: Group 2 Group Trends: Group 2 (2A)(2A)Group Trends: Group 2 Group Trends: Group 2 (2A)(2A)
44BeBe99
1212MgMg2424
2020CaCa4040
3838SrSr8787
5656BaBa137137
8888RaRa226226
Alkaline Earth MetalsAlkaline Earth Metals
1st IE 1st IE decreasedecrease
ss
Radius Radius increaseincrease
ss
mp/bp mp/bp decreasedecrease
ss
electron electron sharing decr. sharing decr. (covalency)(covalency)
MOST REACTIVEMOST REACTIVE
CHE 106 Prof. J. T. Spencer 57
Tendency to lose two electrons to form Tendency to lose two electrons to form MM+2 +2 cations (achieves noble gas electron cations (achieves noble gas electron config.).config.).
Mg(s) + ClMg(s) + Cl22(g)(g) MgClMgCl22(s) and (s) and MgCl(s)MgCl(s)
Flame Tests: Ca - brick red; strontium - Flame Tests: Ca - brick red; strontium - crimson red (in fireworks); barium - crimson red (in fireworks); barium - green.green.
In nature;In nature; berylberyl BeBe33AlAl22(SiO(SiO33))66
dolomitedolomite CaCOCaCO33MgCOMgCO33
limestonelimestone CaCOCaCO33
Group Trends: Group 2 Group Trends: Group 2 (2A)(2A)Group Trends: Group 2 Group Trends: Group 2 (2A)(2A)
44BeBe99
1212MgMg2424
2020CaCa4040
3838SrSr8787
5656BaBa137137
8888RaRa226226
Alkaline Earth MetalsAlkaline Earth Metals
CHE 106 Prof. J. T. Spencer 58
Group Trends: Group 13 Group Trends: Group 13 (3A)(3A)Group Trends: Group 13 Group Trends: Group 13 (3A)(3A)
55BB1111
1313AlAl2727
3131GaGa7070
4949InIn115115
8181TlTl204204
Radius Radius increaseincrease
ss
mp/bp mp/bp decreasedecrease
ss
1st IE 1st IE decreasedecrease
ss
electron electron sharing decr. sharing decr. (covalency)(covalency)+3 Ox. State
+1 Ox. State
CHE 106 Prof. J. T. Spencer 59
Boron Compounds; Boron Compounds;
Numerous Polyhedral Compounds (covalent)Numerous Polyhedral Compounds (covalent)
Boron Neutron Capture TherapyBoron Neutron Capture Therapy Aluminum;Aluminum;
2Al + Fe2Al + Fe22OO33 AlAl22OO33 + 2Fe + 2Fe
THERMITE REACTIONTHERMITE REACTION
Gemstones; AlGemstones; Al22OO33 (Alumina) (Alumina)
trace Crtrace Cr+3 +3 = ruby= ruby
trace Fetrace Fe+2+2, Fe, Fe+3+3, Ti, Ti+3 +3 = blue sapphire= blue sapphire
Group Trends: Group 13 Group Trends: Group 13 (3A)(3A)Group Trends: Group 13 Group Trends: Group 13 (3A)(3A)
55BB1111
1313AlAl2727
3131GaGa7070
4949InIn115115
8181TlTl204204
CHE 106 Prof. J. T. Spencer 60
• Dictionary - “A number of things held together”.Dictionary - “A number of things held together”.• Earliest Man-made Polyhedra: Neolithic Scots Earliest Man-made Polyhedra: Neolithic Scots • Plato : Five “Platonic” Bodies: All Triangular Face (Its Plato : Five “Platonic” Bodies: All Triangular Face (Its
not what you discover but who publishes not what you discover but who publishes FirstFirst))• tetrahedrontetrahedron trigonal trigonal octahedronoctahedron dodecahedrondodecahedron icosahedronicosahedron
bipyramidbipyramid
• Archimedes Archimedes : Thirteen Semi-Regular Polyhedra Derived : Thirteen Semi-Regular Polyhedra Derived from the Platonic Solidsfrom the Platonic Solids
Clusters??Clusters??Clusters??Clusters??
CHE 106 Prof. J. T. Spencer 61
Boron Neutron Capture Boron Neutron Capture Therapy (BNCT)Therapy (BNCT)Boron Neutron Capture Boron Neutron Capture Therapy (BNCT)Therapy (BNCT)
thermal neutron
thermal neutron
10B 11B* 7Li + + 2.4 MeV
to Cells CELL
CHE 106 Prof. J. T. Spencer 62
Group Trends: Group 16 Group Trends: Group 16 (6A)(6A)Group Trends: Group 16 Group Trends: Group 16 (6A)(6A)
88OO1616
1616SS3232
3434SeSe7979
5252TeTe128128
8484PoPo209209
ChalcogensChalcogens
1st IE 1st IE decreasedecrease
ss
Radius Radius increaseincrease
ss
mp/bp mp/bp increaseincrease
ss
electron electron sharing decr. sharing decr. (covalency)(covalency)
CHE 106 Prof. J. T. Spencer 63
Oxygen - two allotropes Oxygen - two allotropes (allotropes - different form of (allotropes - different form of the same element) - Othe same element) - O22 and O and O33..
Great tendency to gain Great tendency to gain electrons (oxidize other electrons (oxidize other elements)elements)
Most common OMost common O-2-2.. S reacts similarly to oxygenS reacts similarly to oxygen
Group Trends: Group 16 Group Trends: Group 16 (6A)(6A)Group Trends: Group 16 Group Trends: Group 16 (6A)(6A)
88OO1616
1616SS3232
3434SeSe7979
5252TeTe128128
8484PoPo209209
ChalcogensChalcogens
CHE 106 Prof. J. T. Spencer 64
99FF1919
1717ClCl3535
3535BrBr8080
5353II127127
8585AtAt210210
1st IE 1st IE decreasedecrease
ss
Radius Radius increaseincrease
ss
mp/bp mp/bp increaseincrease
ss
electron electron sharing decr. sharing decr. (covalency)(covalency)
Group Trends: Group 17 Group Trends: Group 17 (7A)(7A)Group Trends: Group 17 Group Trends: Group 17 (7A)(7A)
HalogensHalogens
CHE 106 Prof. J. T. Spencer 65
Greek for “salt formers”.Greek for “salt formers”. Diatomic in elemental state (FDiatomic in elemental state (F22, Cl, Cl22, Br, Br22, ,
etc...).etc...). Highest electron affinities - form EHighest electron affinities - form E-1-1 anions. anions.
–F removes electrons from almost F removes electrons from almost everything else.everything else.
–Reacts with most metals directly to form Reacts with most metals directly to form salts.salts.
–Reacts with hydrogen to form hydrogen Reacts with hydrogen to form hydrogen halides which dissolve in water to form halides which dissolve in water to form acids (all except HF are strong acids).acids (all except HF are strong acids).
99FF1919
1717ClCl3535
3535BrBr8080
5353II127127
8585AtAt210210
Group Trends: Group 17 Group Trends: Group 17 (7A)(7A)Group Trends: Group 17 Group Trends: Group 17 (7A)(7A)
CHE 106 Prof. J. T. Spencer 66
Group Trends: Group I8 Group Trends: Group I8 (8A)(8A)Group Trends: Group I8 Group Trends: Group I8 (8A)(8A)
22HeHe44
1010NeNe2020
1818ArAr4040
3636KrKr8383
5454XeXe131131
8686RnRn222222
1st IE 1st IE decreasedecrease
ss
Radius Radius increaseincrease
ss
mp/bp mp/bp increaseincrease
ss
electron electron sharing decr. sharing decr. (covalency)(covalency)
Noble GasesNoble Gases
CHE 106 Prof. J. T. Spencer 67
Very unreactive and have closed shell Very unreactive and have closed shell electronic configurations [called noble or electronic configurations [called noble or inert gases].inert gases].
All are monoatomic in native state.All are monoatomic in native state. 1962, Bartlett noticed that Xe has a similar 1962, Bartlett noticed that Xe has a similar
ionization energy to oxygen and could ionization energy to oxygen and could possible form compounds with Xe.possible form compounds with Xe.– Reacted Xe with very strong oxidizer Reacted Xe with very strong oxidizer
(remover of electrons) F and O to form (remover of electrons) F and O to form XeFXeF22, XeF, XeF44, XeF, XeF66, XeO, XeO33, etc..., etc...
– No compounds of He, Ne or Ar are known No compounds of He, Ne or Ar are known and only one compound is known for Kr and only one compound is known for Kr (KrF(KrF22).).
Group Trends: Group I8 Group Trends: Group I8 (8A)(8A)Group Trends: Group I8 Group Trends: Group I8 (8A)(8A)
22HeHe44
1010NeNe2020
1818ArAr4040
3636KrKr8383
5454XeXe131131
8686RnRn222222
Noble GasesNoble Gases
CHE 106 Prof. J. T. Spencer 68Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequations
Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequationsSample exercise: Predict the Sample exercise: Predict the
formula of the compound formula of the compound formed by Rb and Se.formed by Rb and Se.
CHE 106 Prof. J. T. Spencer 69Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequations
Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequationsSample exercise: Predict the Sample exercise: Predict the
formula of the compound formula of the compound formed by Rb and Se.formed by Rb and Se.
RbRb1+1+ SeSe2-2-
CHE 106 Prof. J. T. Spencer 70Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequations
Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequationsSample exercise: Predict the Sample exercise: Predict the
formula of the compound formula of the compound formed by Rb and Se.formed by Rb and Se.
RbRb1+1+ SeSe2-2-
RbRb22SeSe
CHE 106 Prof. J. T. Spencer 71Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequations
Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequationsSample exercise: Write the Sample exercise: Write the
balanced chemical equation balanced chemical equation for the reaction between for the reaction between copper II oxide and sulfuric copper II oxide and sulfuric acid.acid.
CHE 106 Prof. J. T. Spencer 72Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequations
Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequationsSample exercise: Write the Sample exercise: Write the
balanced chemical equation balanced chemical equation for the reaction between for the reaction between copper II oxide and sulfuric copper II oxide and sulfuric acid.acid.
CuCu2+2+ O O2-2-
CHE 106 Prof. J. T. Spencer 73Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequations
Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequationsSample exercise: Write the Sample exercise: Write the
balanced chemical equation balanced chemical equation for the reaction between for the reaction between copper II oxide and sulfuric copper II oxide and sulfuric acid.acid.
CuCu2+2+ O O2-2-
CuO + HCuO + H22SOSO44
CHE 106 Prof. J. T. Spencer 74Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequations
Setting up ionic Setting up ionic compounds, molecular compounds, molecular compounds, and chemical compounds, and chemical equationsequationsSample exercise: Write the Sample exercise: Write the
balanced chemical equation balanced chemical equation for the reaction between for the reaction between copper II oxide and sulfuric copper II oxide and sulfuric acid.acid.
CuCu2+2+ O O2-2-
CuO + HCuO + H22SOSO44 CuSO CuSO44 + H + H22OO
CHE 106 Prof. J. T. Spencer 75
Chapter SevenChapter SevenChapter SevenChapter Seven
Periodic Table Trends and Periodic Table Trends and GeneralizationsGeneralizations
Electron ShellsElectron Shells Atomic Radii and screening (shielding)Atomic Radii and screening (shielding) Ionization EnergyIonization Energy Electron AffinitiesElectron Affinities Metals, Nonmetals and MetalloidsMetals, Nonmetals and Metalloids Group I, 2, 16, 17 and 18 Chemistry - Group I, 2, 16, 17 and 18 Chemistry -
Examples of above concepts and Examples of above concepts and trendstrends