electron energy levels
DESCRIPTION
Atomic Symbols Each element is assigned a unique symbol Nitrogen Hydrogen Bromine Nickel Aluminum Each element is assigned a unique symbol 1-2 letters; 1st is capitalizedTRANSCRIPT
2 - 1CH104
Chapter 4: Atoms
Elements & Symbols
The Periodic Table
Atomic Structure
Isotopes
Electron Energy LevelsPeriodic Trends
2 - 2CH104
Each element is assigned a unique symbol1-2 letters; 1st is capitalized
Atomic Symbols
BromineNickelHydrogen Nitrogen
Aluminum
2 - 4CH104
Atomic Symbols
The original name is often of Latin or Greek origin
Potassium (Kalium)
Lead (Plumbum)
Sodium (Natrium)
Iron(Ferrum)
Silver (Argentum)Gold (Aurum)
2 - 6CH104
Elements with same starting letter, get second letter added to the symbol
Atomic Symbols
ChlorineChromiumCalcium
CarbonCobalt Copper (Cu)
2 - 8CH104
Modern periodic table
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa
He
RnAtPoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
I A II A III A IV A V A VI A VIIA VIIIA
III B IVB V B VIB VIIB VIII B IB IIB
1
2
3
4
5
6
7 Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
The periodic tablehelps us understand
• behavior, • reactions• properties
of the elements.
Mendeleev, 1871“Properties of the elements
vary in a periodic manner.”
2 - 9CH104
A row or period
He
Rn
XeI
KrBrSe
ArClS
NeFO
P
NC
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa PoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In SbSn
Ga Ge
Al
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
At
Te
As
Si
B
1
2
3
4
5
6
7
Periods areassigned numbers
2 - 10CH104
Common group names
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa
He
RnAtPoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
I A
III B IVB V B VIB VIIB VIII B IB IIB
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
Alkali Metals
Alkaline Earth MetalsHalogens
Noble gases
III A IV A V A VI A VIIA
VIIIA
II A
Transition Metals
Lanthanides
Actinides
Chalcogens
2 - 11CH104
Why do we have thoserows on the bottom?
H
Li
Na
Cs
Rb
K
LaBa
Fr
Be
Mg
Sr
Ca
Y
AcRa
Sc
TlHgAuHf PtIrOsReWTa
He
RnAtPoBiPb
CdAgZr PdRhRuTcMoNb
ZnCuTi NiCoFeMnCrV
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
This arrangement takes toomuch space and is hard to read.
2 - 12CH104
Names & Symbols
He
Rn
XeI
KrBrSe
ArClS
NeFO
P
NC
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa PoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In SbSn
Ga Ge
Al
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
At
Te
As
Si
B
1
2
3
4
5
6
7
Know the names & symbols
2 - 13CH104
At
Te
As
Si
B
He
Rn
XeI
KrBrSe
ArClS
NeFO
P
NC
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa PoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In SbSn
Ga Ge
Al
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
Metals Lustrous, malleable and ductile.Conductors (heat & electricity)Solids at room temp (except Hg)
Lose electrons to non-metals.
2 - 14CH104
He
Rn
XeI
KrBrSe
ArClS
NeFO
P
NC
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa PoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In SbSn
Ga Ge
Al
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
At
Te
As
Si
B
Non-metals
Gas, liquid, solid (dull, brittle)Poor conductors = InsulatorsMany are diatomic molecules.Gain e’s from metals Share e’s with other non-metals
2 - 15CH104
He
Rn
XeI
KrBrSe
ArClS
NeFO
P
NC
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa PoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In SbSn
Ga Ge
Al
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
At
Te
As
Si
B
3 - 11
Metaloids
Intermediate propertiesSemi conductors
2 - 16CH104
H
Li
Na
Cs
Rb
K
TlHgAuHfLaBa
Fr
PtIrOsReWTa PoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In Sn
Ga
Al
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
He
Rn
XeI
KrBrSe
ArClS
NeFO
P
NC
Sb
Ge
At
Te
As
Si
B
Metaloids
Metals Non-metals
2 - 18CH104
A model of matterAtom - The smallest unit of an
element that is still that element.
Molecule -The smallest unit of a pure substance that is still that substance.
May contain > 1 atom or element.
ie. Aluminum (Al)
ie. Water (H2O)
2 - 19CH104
Structure of the atom Nucleus Small, dense, + charge in the center of
an atom.
contains protons
& neutrons
++
+++ +
2 - 20CH104
Rutherford’s Gold-Foil Experiment 99% of + particles aimed at gold went straight through. A few were deflected. A few bounced back
Conclusion: Atoms are mostly empty space. Atoms have a small, dense nucleus with + charge.
2 - 21CH104
Structure of the atom Nucleus (+)
Electrons - charged particles that surround the nucleus.
Electrons moved around nucleus in orbitals.
2 - 22CH104
Structure of the atom
The nucleus is a small part of an atom.
If the nucleus was the sizeof a marble, the atom wouldfill a football stadium.
The nucleus would weighover 10,000 tons.
2 - 23CH104
Z = Atomic number = # protons = # electrons
The atomic symbol
XA
Z
A = Atomic mass (amu) = # protons + # neutrons
++
+++ +
-
-
---
-
2 - 24CH104
A = Atomic mass = # p + # n
The atomic symbol
XA
Z
C
#
Z = Atomic # # p = # e
C = Charge = + or - values
# = Number of atoms in a formula.
2 - 25CH104
The atomic symbol
X12
6
A = Atomic mass = # protons + # neutrons
Z = Atomic number = # protons = # electrons
++
+++ +
-
-
---
-
6 6
2 - 26CH104
The atomic symbol
C12
6
A = Atomic mass = # protons + # neutrons
Z = Atomic number = # protons = # electrons
++
+++ +
-
-
---
-
2 - 27CH104
The atomic symbol
Na23
11
1+
A = Atomic mass = p + n = 23
Z = Atomic # = p = 11
C = Charge = +1
# = 1 atom in formula.
Sodium
11 12
2 - 28CH104
Ag107.87
Silver47 Atomic number
Name of the element
Elemental Symbol
Atomic mass (weight)
Atomic weight = The average, relative mass of an atom in an element.
Why is the atomic weight on the tables not a whole #?
2 - 29CH104
Isotopes of HydrogenIsotopes = Atoms of the same element but
having different masses.11
21
31
+
H H H
-+
-+
-
Protium99.99%
Deuterium0.01%
TritiumTrace %
2 - 30CH104
Isotopes of HydrogenIsotopes = Atoms of the same element but
having different masses.11
21
31
+
H H H
-+
-+
-
Average Atomic weight of Hydrogen = 1.00794 amu
2 - 31CH104
++
+++ +
Isotopes of Carbon
-
Average Atomic weight of C= 12.011 amu
98.89%
C612 C6
13 C614
++
+++ +
-
1.11%
++
+++ +
-
Trace %
-
--
-- -
-
- -
-
-
-
--
-
2 - 32CH104
Radioactive Isotopes
C614
zzz++
+++ +
-
-
-
--
-31 H
+
-
Nucleus is unstableSo falls apart (decays)
Giving radioactive particles
H-3 C-14
2 - 33CH104
Average Atomic Mass
Cl1737Cl17
35
(75.8)35
75.8% 24.2%
+ (24.2)37
= 35.45 amu100
2 - 35CH104
Symbol Atomic#
Mass Protons Neutrons Electrons
Atomic Structure
Be
1414 1428 14Si
17201717 37Cl
44 9 4 5
Complete the table:
2 - 36CH104
Electronic arrangement
A new layer isadded for each row or period in the table.
2 - 37CH104
Electron arrangement
28
1832
Electronsfill layers
around nucleusLow High
Shells = Energy levels
2412Mg
2 - 38CH104
11H
73Li
42He
IA IIA
94Be
2, 1 2, 2
2 - 39CH104
115 B
11H
73Li
IA IIA IIIA
94Be
2, 1 2, 2 2, 3
2 - 40CH104
115 B 12
6 C137 N
IIIA IVA VA
2, 3 2, 4 2, 5
2 - 41CH104
94Be
11H
73Li
42He
2010Ne
2311Na
2412Mg 40
18Ar
IA IIA VIIIA
2, 1 2, 2
2, 8, 1 2, 8, 2
2, 8
2, 8, 8
2 - 42CH104
3
2412Mg
11H
73Li
2311Na
94Be 11
5 B
2713Al
Valence electronsWhere most chemical
Reactions occur.
1
2
2, 1 2, 2
2, 8, 1 2, 8, 2
2, 3
2, 8, 3
2 - 43CH104
11H
73Li
42He
94Be 20
10Ne
2311Na
2412Mg 40
18Ar
81
2
2, 1 2, 2 2, 8
2, 8, 1 2, 8, 2 2, 8, 8
Octet Rule
2 - 45CH104
An atom is like an inverted pyramid. As you get farther from the nucleus, there is more room for electrons.
1st level holds 2 e’s.2nd level holds 8 e’s.3rd level holds 18 e’s.4th level holds 32 e’s.etc....
Rules for electron Placement
2 e-
8 e-
18 e-
32 e-
++
+
+ ++
2 - 46CH104
Hotel Model
s
s
p
s
p
d
s
p
d
f
n = 4 (4th floor)
n = 3 (3rd floor)
n = 2 (2nd floor)
n = 1 (1st floor)
Each shell (floor of the Hotel) Has subshells (s,p,d,f)
++
+
+ ++
2 - 47CH104
Orbitals
p (3)s (1) d (5)
Each subshell contains orbitals which can hold a maximum of two electrons
f (7)
2 - 48CH104
s
s
ps
pd
sp
df
n = 4
n = 3
n = 2
n = 1
The Aufbau principleElectrons fill from the low high.fill n = 1 before n = 2 , fill s before p ...
Electrons don’t share same orbital unless they need to.
(i.e. no pairing until each orbital of the set has an electron)
Hund’s Rule+
++
+ ++
2 - 49CH104
5d
5s
5p
4d
4f
4s
4p
3d
3s
3p
2s
2p
1s
Major trends in electron filling
Exceptions to Hotel Model:Fill 4s before 3dFill 5d before 4 fFill 5s before 4dFill 6d before 5 f
This is why transition metals are assigned as B group elements.
2 - 54CH104
1s __2s __
2p __ __ __3s __
3p __ __ __4s __ 3d __ __ __ __ __
5s __4p __ __ __
4d __ __ __ __ __ 5p __ __ __
6s __ 5d __ __ __ __ __ 4f __ __ __ __ __ __ __
73Li
1s22s1
Electron Configuration
2 - 55CH104
1s __2s __
2p __ __ __3s __
3p __ __ __4s __ 3d __ __ __ __ __
5s __4p __ __ __
4d __ __ __ __ __ 5p __ __ __
6s __ 5d __ __ __ __ __ 4f __ __ __ __ __ __ __
1s22s22p4
16 8 O
Electron Configuration
2 - 56CH104
1s __2s __
2p __ __ __3s __
3p __ __ __4s __ 3d __ __ __ __ __
5s __4p __ __ __
4d __ __ __ __ __ 5p __ __ __
6s __ 5d __ __ __ __ __ 4f __ __ __ __ __ __ __
1s22s22p63s23p64s23d10
30Zn
[Ar] 4s23d10
[Ar] 3d104s2
Electron Configuration
2 - 57CH104
Classification by sublevels
H
Li
Na
Cs
Rb
K
TlHgAuLsBa
Fr
PtIrOsReWTa
He
RnAtPoBiPb
Be
Mg
Sr
Ca
CdAgY PdRhRuTcMoNb
AcRa
ZnCu
Hf
Zr
TiSc NiCoFeMnCrV
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es f
s
d
p
3 - 25
2 - 58CH104
Using the periodic tableto find sublevels
Tl RnAtPoBiPb
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es
s
23
45
H
Li
Na
Cs
Rb
K
Ba
Fr
He
Be
Mg
Sr
Ca
Ra
6
7
1
23
4
5HgAuHfLa PtIrOsReWTa
CdAgZrY PdRhRuTcMoNb
Ac
ZnCuTiSc NiCoFeMnCrV345
6
d
6
p
f45
2 - 59CH104
Inner vs. valence electrons
Valence electronsWhere most reactionsoccur.
Inner electronsNot much happenshere under normalconditions.
2 - 60CH104
The Continuous SpectrumWhen sunlight (white light) is passed thru a prism, a continuous rainbow of colors is observed.
There appears to be light of every color in sunlight.
2 - 61CH104
Electromagetic SpectrumThe Continuous Spectrum
2 - 63CH104
The Discrete Spectrum !But when light from elements is passed thru a prism, a continuous spectrum is not observed.
From the red glow of hydrogen, 4 lines emerged.
2 - 64CH104
1 _____
2 _____
3 _____
4 _____
5 _____
6 _____ 11H
Excitation of electrons
Add Energy to kick e- to higher level
1 _____
2 _____
3 _____
4 _____
5 _____
6 _____
E
Energy is given back when e- falls back to lower level
656 nm
486 nm
434 nm
410 nm
Some of these discrete Quantities (Quanta) of Energy appear as colors
2 - 65CH104
Emission Spectrum of Hydrogen
https://www.khanacademy.org/science/chemistry/electronic-structure-of-atoms/bohr-model-hydrogen/v/emission-spectrum-of-hydrogen
Explanation of 4 line spectrum of Hydrogen: (10:49min)
2 - 66CH104
The Discrete Spectrum !
H
Hg
Ne
2 - 68CH104
Group Numbers & Valence Electrons
H
Li
Na
Cs
Rb
K
TlHgAuHfLsBa
Fr
PtIrOsReWTa
He
RnAtPoBiPb
Be
Mg
Sr
Ca
CdAgZrY PdRhRuTcMoNb
AcRa
ZnCuTiSc NiCoFeMnCrV
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
Gd
Cm
Tb
Bk
Sm
Pu
Eu
Am
Nd
U
Pm
Np
Ce
Th
Pr
Pa
Yb
No
Lu
Lr
Er
Fm
Tm
Md
Dy
Cf
Ho
Es4 - 6
1
2 3 4 5 6 7Representative Elements 8
Periodic trends
2 - 69CH104
11H
73Li
2311Na
Electron-Dot Symbols(Lewis Symbols)
Show only Valence
Electrons
H
Li
Na
K
2 - 70CH104
H
Li
Na
K
He
Be B C O F NeN
Mg
Ca
Al
Ga
Si
Ge
P
As
S
Se
Cl
Br
Ar
Kr
1
2 3 4 5 6 7
8Electron-Dot SymbolsPeriodic trends
2 - 71CH104
Atomic Size
Ba
Sr
Ca
Mg
Be
Tl
In
Ga
Al
B
Pb
Sn
Ge
Si
C
Cs
Rb
K
Na
Li
Bi
Sb
As
P
N
Te
Se
S
C
I
Br
Cl
FH
Atomsgetlargeras you go down a group.
Periodic trendsAtoms get smaller as you go across a period.
2 - 73CH104
At
I
Br
Cl
Po
Te
Se
S
Bi
Sb
As
P
Pb
Sn
Ge
Si
FON
Tl
Na
Cs
Rb
K
Ba
Mg
Sr
Ca
In
Ga
Al
H
Li Be B C
First ionization energyThe energy required to remove the first electron from a neutral atom.
4 - 50© Chemeketa Community College: Chemistry for Allied Health
Periodic trends
2 - 75CH104
ElectronegativityRelative ability of atoms to attract electrons
when they form bonds.
At
I
Br
Cl
Po
Te
Se
S
Bi
Sb
As
P
Pb
Sn
Ge
Si
FON
Tl
Na
Cs
Rb
K
Ba
Mg
Sr
Ca
In
Ga
Al
H
Li Be B C
4 - 50© Chemeketa Community College: Chemistry for Allied Health
Periodic trends
2 - 76CH104
Summary of trends.As atomic size decreasesFirst ionization energy increases.Electrons are harder to remove.Adding more electrons is easier.
SummaryMetals are larger so tend to lose electrons.
Non-metals are smaller so tend to gain electrons.
Periodic trends