1. Periodic Table

2. Memorize these element
names & symbols:
Gases:
H hydrogen He helium Ne neon
N nitrogen O oxygen F fluorine
Cl chlorine Ar argon
Liquids:
Hg mercury
Br bromine

3. Solids:
Li lithium B boron
C carbon Na sodium Mg magnesium
Al aluminum Si silicon P phosphorus
S sulfur K potassium Ca calcium
Cr chromium Mn manganese Fe iron
Co cobalt Ni nickel Sn tin
Cu copper Zn zinc Pb lead
As arsenic I Iodine
Se selenium Ba barium
Ag silver Au gold
Pt platinum U uranium

4. Arrangement of the Elements
Russian, Dmitri Mendeleev
created The first “accepted”
periodic table (1800’s)
1) Increasing atomic number
2) By groups or families:
columns
elements in a column have very similar
properties

5. Ca I Cu 3) periods Rows (across) Identify the element in:
Group 2A, period 4
Group 7A, period 5
Group 1 B, period 4 Ca I Cu

6. 4) Metal, Nonmetal, Metalloid
nonmetals
metalloids
Metals

7. Properties of Metals
high melting pt. (not Hg)
shiny
good conductors of
heat & electricity
malleable & ductile
easily oxidized:
lose e- in chem rxns

8. Properties of Nonmetals
low melting pt. (sol, liq, gas)
xenon
poor conductors
solids are brittle & dull
gain e- in chem rxns
sulfur
carbon
Reduction (easily reduced))

9. Properties of Metalloids
(either side of zig zag line)
Ex: B, Si, Ge, As, Sb
not Al
properties are intermediate between metal and nonmetal
silicon
used in semiconductor
industry (computer chips)

10. Quantum Theory revisited
5) Electron Arrangement
Quantum Theory revisited
Apartment building analogy
atom
apartment building
nucleus
ground floor
energy levels
floors
sublevels
apartments
orbitals
rooms
electrons
people

11. s p d f types of orbitals (one room apt.) spherical dumbell

12. Electron Configuration: The “address” of the e-
Principal
Quantum
Number (n)
energy
level
number of
sublevels
type of sublevels
orbitals
max
number
electrons n2
2n2 1 1 1 1s 1 2
2s 2p 4 8 2 2 2 3 3 3
3s 3p 3d 9 18 4 4 4
4s 4p 4d 4f 16 32
Electron Configuration:
The “address” of the e-
Ex: 1s22s22p6
no. electrons
energy level
sublevel

13. Aufbau Diagram 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14
Energy level
sublevels
max. no. e-

14. 1s1 1s2 1s22s1 N 7 e- 1s2 2s2 2p3 sample electron configurations
H 1 e-
1s1 He
2e-
1s2 Li
3e-
1s22s1 1s 2s N
7 e-
1s2
2s2
2p3 1s 2s 2p

15. Fe
26e-
1s2
2s2
2p6
3s2
3p6
4s2
3d6 3p 4s 1s 2s 2p 3s 3d

16. Sample problem:
Given the electron configuration:
1s22s22p63s23p5
1. How many electrons are unpaired? 1
2. How many electrons are in the outermost energy level ?
s23p5
3. How many energy levels and sublevels are
occupied?
3 energy levels (1, 2, 3)
5 sublevels (1s 2s 2p 3s 3p)
4. What element has this ground state
configuration? Cl

17. As Given the configuration: 1s22s22p63s23p64s23d104p3
this is the config.
of: As
How many electrons are in the outer energy
level?
5, 4s24p3 3
2. How many electrons are unpaired?

18. Short method for e- config.
Use noble gases
Ex: Cl
17 e-
[Ne]
3s2
3p5
1st 10 e-
[Ne]
1st 18 e-
[Ar]
Ex: Ba
56e-
[Xe]
6s2
1st 36 e-
[Kr]
Ex: Zn
30 e-
[Ar]
4s2
3d10
1st 54 e-
[Xe]
1st 86 e-
[Rn] U
92 e-
[Rn]
7s2
5f4 Si
[Ne] 3s23p2 Pd
[Kr] 5s2 4d6
14 e-
46 e-

19. s & p using the periodic table to write electron configurations 1 1s 2
period # (n) 2p 2s 3
period #(n) -1 3s d 3p 4 3d 4s 4p 5 5s 4d 5p 6 6s 5d 6p 7 7s 6d f
Period #(n) -2 6 4f 7 5f

20. Ex: Na
[Ne]
3s1
Ex: P
[Ne]
3s2
3p3
Ex: Co
[Ar]
4s2
3d7
Ex: Sn
[Kr]
5s2
4d10
5p2
Ex: Pu
[Rn]
7s2
4f6
1. calcium
[Ar] 4s2
2. chlorine
[Ne] 3s2 3p5
3. cadmium
[Kr] 5s2 4d10

21. Inner transition metals
Families of Elements
halogens
Noble gases
Transition metals
Alkali metals
Alkaline earth metals
Inner transition metals

22. All have 1 valence electron
Group 1A: Alkali metals Na Li
1s2 2s1
All have 1 valence electron Na
[Ne] 3s1
outer energy level K
[Ar] 4s1 Rb
most reactive metals
always found
combined in nature Cs
react with water producing hydrogen gas Fr

23. Also react w/ water to produce hydrogen gas
Group 2A: Alkaline Earth Metals Be
1s2 2s2
all have 2 valence electrons Mg
[Ne]3s2 Mg Ca
[Ar] 4s2 Sr
quite reactive; always found combined w/ other elements in nature Ba Ra
Also react w/ water to produce hydrogen gas

24. most reactive nonmetalsCl
Group 7A: Halogens F
1s2 2s2 2p5 Cl
[Ne] 3s2 3p5 Br
all have 7 valence e-
[Ar] 4s2 3d10 4p5 I
most reactive nonmetals At
form salts when
combined with
metals; ex: NaCl, KI
always found in compounds

25. filled outer levels makes them stable
Group 8 A: Noble Gases He
1s2 Xe Ne
1s2 2s2 2p6
most have 8 valence e- Ar
[Ne] 3s2 3p6 Kr
chemically inert (unreactive);
don’t form compounds Xe Rn
filled outer levels makes them stable Ar Kr

26. Au Ag Transition Metals (B groups)
unique property: form bright colored compounds
“typical” metals

27. Inner Transition elements many are synthetic (man made)
lanthanide series
actinides series La Ac
many are synthetic (man made)
and radioactive
“yellow cake” uranium oxide

28. Change from left to right across the row
Periodicity
Trend: property that changes
atomic radius, ionization energy, electronegativity
Group trend
change from top to bottom down a group
Periodic trend
Change from left to right across the row

29. I. Atomic Radius
Indicates the size of an atom
Group trend
larger down the group
more energy levels makes the atoms larger
Li: 2 energy levels K:
4 energy levels

30. Periodic trend smaller across
more protons increases nuclear charge; pulls electrons in closer making the atom smaller Li C Ne +3 +6
+10
arrange these atoms from smallest to largest:
Sr, Ne, Ca, S, Al Ne S Al Ca Sr

31. Li K Energy required to remove an e- from an atom
III. Ionization Energy Li K
Group trend
decreases going down
larger atoms hold their valence e- more loosely

32. Increases across; increase in nuclear charge (more p+) causes
electrons to be held more tightly
Periodic trend Na Al Cl
+13
+17
+11
Ex: Which will lose an electron the easiest?
K or Ge ?
Mg or Ba ?
Al or Cs ?

33. gains e- easily; very reactive
Number from 0-4 that indicates an atom’s attraction for e-
IV. Electronegativity
F 4.0
gains e- easily; very reactive
Cs 0.7
loses e-easily;
very reactive
group trend
Increases going across (not noble gases
Periodic trend
decreases going down
Ex: Arrange these atoms from
greatest attraction for e- to least:
P, Al, Sr, O
O, P, Al, Sr

34. trends summary Smallest radius Highest I.E. Highest EN (F) Lowest EN
Lowest I.E.
Largest radius