Download Periodic Table Student Outline

Periodic Table
Homework Due: _________________
Text Book: Read pages 63-69
Exam Dates: _____________________________
Periodic Table Student Outline
 Names and symbols of elements on Table S
 Periodic law
 Period is a horizontal row across the periodic table
 Group / family is a vertical column down the periodic table
Group 1 – Alkali metals
Group 2 – Alkaline earth metals
Group 17 - Halogens
Group18 – Noble Gases
Groups 3 - 11 Transition metals
 Reactivity of elements is dependent on valence electrons
 Characteristics of metals, non metals and metalloids
Metals
non metals
left of stairs
right of stairs
few valence electrons
close to 8 valence electrons
lose valence electrons
gain valence electrons
solids except for Hg
solids, liquids and gases
become positive ions
become negative ions
solids
if solid, brittle and dull
conductor of electricity
non conductors
malleable
ductile
shiny/have luster







Transition metals
o Multiple oxidation states
o Can lose electrons from outermost 2 principle energy levels (PEL)
o Colored ions in solution
o Can form multiple compounds with the same element
Atomic radius
Ionic radius
If an atom gains electrons its ion will be ….a negative ANION (-) and is larger than the atom
If an atom loses electrons its ion will be …. a positive CATION (+) and is smaller than the atom
To find the charge of an atom’s ion look it up on the reference table under “Selected Oxidation States”
Periodic trends can be looked up in reference table S and the Periodic Table
Periodic trend
Atomic radius
Ionization energy
Electronegativity
Metallic character
Valence electrons
# of occupied energy levels
Atomic #


metalloids( semi-metals)
Seven Semimetals: on stairs
characteristics of both metals and
non- metals
semi-conductors
include B, Si, Ge, As, Sb, Te, At
Across a period
decrease
increase
increase
Down a group
increase
decrease
decrease
decrease
increase
remains the same
increases
increase
changes
remains the same
increase by 1
Changes in periodic trends are due to …
 Number of PELs
 Nuclear hold (holding strength of the nucleus by the protons)
 Shielding effect ( the PELs between the nucleus and the valence electrons
Identifying phases of elements at room temperature
 Predicting group locations from chemical formulas
GROUP
1
2
13
14
Charge in compounds
+1
+2
+3
+4 or -4
15
-3
16
-2
17
-1
18
0
What you can find out from the periodic table:
1. Atomic mass of any element  which is equal to the mass, in grams, of 1 mole of that substance.
2. Atomic number of any element which
 is equal to the number of protons in the nucleus =
(nuclear charge of the atom)
 and the number of electrons in the energy levels of an atom.
 Protons = electrons = atomic # …in any atom
3. Electron configuration of an atom – placement of electrons in the energy levels, sublevels and
orbitals….determine half filled, occupied and filled.
4. Symbols of the elements and names on table S
5. Valence electrons ( all e- in outer most PEL… or “the trick” group its in)
6. Determine the kernel of the atom ( all parts except the valence e-)
7. The valence PEL is the period #
8. Group names: alkali (I), alkaline earth (II), transition metals, halogens (17), noble/ inert gases (18)
9. Location of the metals, non- metals and metalloids
10. Most metallic properties or most non- metallic properties
11. Radioactive elements … stable radioisotopes
12. Basis of the atomic masses ~~ carbon – 12 and the average of the most abundant isotopes of that element
13. Noble gases have a full outer (valence) shell , therefore not reactive … does not give or take electrons
14. Formation of ions from the atoms . metals = + (lose e- … become smaller)
…
non metals = - (gain e- … become larger)
15. Atomic mass = # of protons + # of neutrons… different mass represents an isotope (change in mass only)
16. Atomic # represents the atom or element .. the atomic # or the number of protons CANNOT change.
17. Determine the ground state and excited state of an atom
18. Can determine the electron dot diagrams from the # of valence e19. Determining the oxidation states (electrons lost or gained) by an atom.
20. Characteristics of transition elements: can lose e- from 2 outermost PEL’s , can form more that one type of
compound formula, form colored solutions.
21. Locating the diatomic elements on the table (Br I N Cl H O F) most diatomics in group 17 ~ the halogens
22. Locating the phases of matter on the periodic table … (halogens have elements in all three phases)
 gases = (O, N, Cl, F , H, and Noble Gases/Group 18),
 liquids Hg (at STP, the only liquid metal) and Br (at STP, the only liquid nonmetal)
 solids (most elements on periodic table).
23. Elements are arranged on the periodic table according to atomic number (# of protons) not atomic mass
24. Period (horizontal row) – tells the valence shell, # of occupied PEL’s , # of e- increases from left to right.
25. Group /family vertical column with similar properties, same # of valence electrons, blocks tell the sublevels
being filled
 Group 1 Alkali metals very reactive … become more reactive as you go down the group …
always occur combined with nonmetals in nature
 Group 2 Alkaline Earth Metals also reactive (not as reactive as group 1)
 Group 17 Halogens- all diatomic, contain elements in all 3 phases of matter.
 Group18 Noble Gases / Inert Gases -rarely bond except for Xe and Kr which can combine with F at
high P and T
 (see periodic table for oxidation states) are unreactive  have
either 8 valence electrons or a filled outer shell (remember about He)
 Groups 3 - 12 transition elements … colored ions and multiple oxidation
states, can lose electrons from inner and outermost energy levels. (Can form
more than one compound when bonding because of multiple oxidation
states)
26. Reactivity of elements …
 lower left = most reactive metals (greatest metallic character) They contain one or two valence
electrons and as you move down the group there are more shells (lower down the group = most
reactive) …
 upper right are the most reactive non metals (greatest nonmetallic character) (group 17; close to
having 8 valence electrons or a full (stable) outermost shell)..These active elements do not occur
alone/uncombined in nature.
27.
28.
29.
30.
Characteristics of metals , non metals and metalloids
The Periodic law – properties of the elements are periodic according to their atomic numbers
Who arranged the periodic Table – Dimitri Mendeleev
How is the periodic table arranged. According to atomic number …. Used to be according to atomic mass
(notice discrepancies (example Cobalt and Nickel) … reorganized by atomic number … the number of
protons in an atom)
33. Determining the Radii of atoms:
 Across a period the radii gets smaller due to greater nuclear charge, pulling the same # of shells closer
together Nuclear hold (# of protons in nucleus) or
 Down a group the radii gets larger due to more shells in the atom Shielding effect ( # of shells between
nucleus and valence electrons)
34. Ionic radius – produced when an atom forms an ion ( loses or gains electrons)
 If an atom gains electrons (becomes - , typically non metals) its ion will be larger than the atom
 If an atom loses electrons (becomes +, typically metals) its ion will be smaller than its atom
35. Periodic trends all can be looked up in the reference tables
Periodic Table Homework
A) Page 82
Introduction to Periodic Table
31)
32)
33)
34)
36)
38)
39)
a ___________
b ___________
c ___________
d ___________
e ___________
f ___________
g ___________
40)
a _________________________________
b _________________________________
c _________________________________
d _________________________________
e _________________________________
B page 356
Atomic properties and the periodic table
48)
49)
50)
51)
52)
53)
54)
55)
a ___________
b ___________
c ___________
d ___________
56)
a ___________
b ___________
c ___________
d ___________
57)
a ______________________
b ______________________
c ______________________
C Complete the Following:
1. Who organized the periodic table? __________________________________________________
1. How many rows are on the current periodic table? _________________________
2. How many columns (groups) are on the current periodic table? _________________________
3. How is the periodic table arranged? _________________________
4. What are the two rows below the main body of the periodic table called? ____________________
5. Where are the nonmetals located on the periodic table? _________________________
6. Where are the metals located on the periodic table? _________________________
7. Where are the metalloids located on the periodic table? _________________________
8. Which columns contain transition metals? _________________________
9. Which column contains elements with completely filled p orbitals? _________________________
10. Which column contains elements whose electron configurations end with a d orbital? ___________
11. Where are the most active metals located on the periodic table? _________________________
12. Where are the most active nonmetals located on the periodic table? _________________________
13. Which is the most active nonmetal on the periodic table? _________________________
14. What happens to the ATOMIC RADIUS as you move across a period from left to right? ________
Why does this radius change? _________________________
15. What happens to the ATOMIC RADIUS as you move down a group from top to bottom? ________
Why does this change in radius occur? _________________________
16. When an atom becomes a negative ion, the original atom is
(smaller OR larger ) than the ion formed? _________________________
17. When an atom becomes a positive ion, the original atom is
(smaller OR larger ) than the ion formed? _________________________
18. What happens to the ionization energy as you move across a period from left to right? __________
Explain why? _________________________
19. What happens to the ionization energy as you move down a group from top to bottom? _________
Explain why? _________________________
20. What are the names of the following groups?

Group 1 _______________________________________________________

Group 2 _______________________________________________________

Groups 3-12 _______________________________________________________

Group 17 _______________________________________________________

Group 18 _______________________________________________________
21. Elements within a group have the same number of _____________________________________
22. Elements within a period have the same number of _________________________
23. What are the “special” characteristics of transition elements?

_________________________

_________________________

_________________________
24. What happens to the metallic character as you go down a group? _________________________
25. What happens to metallic character as you go across a period? _________________________
26. The majority of the elements on the periodic table are ( metals/nonmetals/metalloids) ___________
27. The majority of the elements on the periodic table are ( solids/liquids/gases) __________________
28. Elements on the periodic table are organized according to their_________________________
29. An element with properties of both metals and nonmetals is called_________________________
30. Why do group 18 elements have higher ionization energies and
NO electronegativity values? __________________________________________________
31. The vertical columns of the periodic table are called? _________________________
32. The horizontal rows of the periodic are called? ________________________
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
I
F
G
B
C
E
H
A
J
Place the letter from the periodic table above next to the description that best matches that element:
a) an alkali metal
e) an alkaline earth metal
b) an inactive gas
f) an active nonmetal
c) a semimetal
g) a metal with 3 valence electrons
d) a metal with more than one bonding possibility
h) a nonmetal with 1 valence electron
20 facts you didn’t know about the Periodic table
1
2
3
4
5
6
7
8
9
10
11
12
13
14
~ Adapted online from Lawrence Berkeley National Lab
You’ll never guess its real purpose: It’s a giant cheat sheet.
The table has served chemistry students since 1869, when it was created by Dmitry Mendeleev, a cranky professor at the
University of St. Petersburg.
With a publisher’s deadline looming, Mendeleyev didn’t have time to describe all 63 then-known elements. So he turned to a
data set of atomic weights meticulously gathered by others.
To determine those weights, scientists had passed currents through various solutions to break them up into their constituent
atoms. Responding to a battery’s polarity, the atoms of one element would go this away, the atoms of another that away. The
atoms were collected in separate containers and then weighed.
From this process, chemists determined relative weights—which were all Mendeleyev needed to establish a useful ranking.
Fond of card games, he wrote the weight for each element on a separate index card and sorted them as in solitaire. Elements
with similar properties formed a “suit” that he placed in columns ordered by ascending atomic weight.
Now he had a new Periodic Law (“Elements arranged according to the value of their atomic weights present a clear
periodicity of properties”) that described one pattern for all 63 elements.
Where Mendeleeev’s table had blank spaces, he correctly predicted the weights and chemical behaviors of some missing
elements—gallium, scandium, and germanium.
But when argon was discovered in 1894, it didn’t fit into any of Mendeleeev’s columns, so he denied its existence—as he did
for helium, neon, krypton, xenon, and radon.
In 1902 he acknowledged he had not anticipated the existence of these overlooked, incredibly unreactive elements—the noble
gases—which now constitute the entire eighth group of the table.
Now we sort elements by their number of protons, or “atomic number,” which determines an atom’s configuration of
oppositely charged electrons and hence its chemical properties.
Noble gases (far right on the periodic table) have closed shells of electrons, which is why they are nearly inert.
Atomic love: Take a modern periodic table, cut out the complicated middle columns, and fold it once along the middle of the
Group 4 elements. The groups that kiss have complementary electron structures and will combine with each other.
Sodium touches chlorine—table salt! You can predict other common compounds like potassium chloride, used in very large
doses as part of a lethal injection.
15 The Group 4 elements (shown as IVA above) in the middle bond readily with each other and with themselves. Silicon +
silicon + silicon ad infinitum links up into crystalline lattices, used to make semiconductors for computers.
16 Carbon atoms—also Group 4—bond in long chains and sugars. The chemical flexibility of carbon is what makes it the key
molecule of life.
17 Mendeleyev wrongly assumed that all elements are unchanging. But radioactive atoms have unstable nuclei, meaning they
can move around the chart. For example, uranium (element 92) gradually decays into a whole series of lighter elements,
ending with lead (element 82).
18 Beyond the edge: Atoms with atomic numbers higher than 92 do not exist naturally, but they can be created by bombarding
elements with other elements or pieces of them.
19 The two newest members of the periodic table, still-unnamed elements 114 and 116, were officially recognized last June.
Number 116 decays and disappears in milliseconds. (Three elements, 110 to 112, were also officially named earlier this
month.)
20 Physicist Richard Feynman once predicted that number 137 defines the table’s outer limit; adding any more protons would
produce an energy that could be quantified only by an imaginary number, rendering element 138 and higher impossible.
Maybe.
Questions:
1. State 2 facts from the periodic table you did not know
2. what group of elements did Medeleev overlook until the early 1900’s
3. How did Mendeleev organize the periodic table?
4. Above what atomic number do elements not exist naturally?