Organizing the Elements: The Periodic Table (PT)
Development of the Periodic Table
from Steven Hawkings’ Universe: Cosmic Alchemy
a) As you view the video segment on the periodic table, jot down the answers to the following questions. Short answers only.
1) Where and when was Mendeleev born?______
______
2) What sparked Mendeleev interest in chemistry?______
______
3) What properties of the elements did Mendeleev list before he began to organize the elements?______
4) Explain the process Mendeleev used to help design the first periodic table. ______
5) How was Mendeleev able to predict properties of the yet to be discovered elements?
______
6) How is the modern Periodic Table organized? ______
______
b) Overview of the Periodic Table
Developed by Russian scientist Dimitri Mendeleev (1869)
Revised based on the work of Henry Mosley (1913) and Glenn Seaborg (1940’s)
Revised or Modern Periodic Law: The properties of the elements are periodic function of their atomic number. This means that the
- Elements are arranged by INCREASING atomic number.
- Predictable & repeating pattern to the elements’ properties (characteristics)
- Elements in the same horizontal row (PERIOD) have the same number of energy levels (where the electrons are found). The PERIOD Number on the side of the PT is the same as the number of energy levels.
- Period 1: ______energy level
- Period 4: ______energy levels
- Elements in the same vertical column (GROUP) have similar chemical properties due to the same number of electrons in outermost energy level. In the electron configuration, the number of electrons in the outermost energy level is the number on the right in the configuration for the ‘tall’ groups (exception: He in group 18)
- Group 1: _____ electron in the outermost energy level
- Group 2: _____ electrons in the outermost energy level
- Group 14: _____ electrons in the outermost energy level
- Group 17: _____ electrons in the outermost energy level
Four Basic types of Elements:
1 / 2 / 3 / 4 / 5 / 6 / 7 / 8 / 9 / 10 / 11 / 12 / 13 / 14 / 15 / 16 / 17 / 181 / H / He
2 / Li / Be / B / C / N / O / F / Ne
3 / Na / Mg / Al / Si / P / S / Cl / Ar
4 / K / Ca / Sc / Ti / V / Cr / Mn / Fe / Co / Ni / Cu / Zn / Ga / Ge / As / Se / Br / Kr
5 / Rb / Sr / Y / Zr / Nb / Mo / Tc / Ru / Rh / Pd / Ag / Cd / In / Sn / Sb / Te / I / Xe
6 / Cs / Ba / La-Lu / Hf / Ta / W / Re / Os / Ir / Pt / Au / Hg / Tl / Pb / Bi / Po / At / Rn
7 / Fr / Ra / Ac-Lr / Rf / Db / Sg / Bh / Hs / Mt
Key: Each type of element has certain properties associated with it.
Metal / Metalloid / Nonmetal / Noble gasThe most active metal and nonmetal on the PT are the two F’s in opposite corners! ___&___
Special Names of Groups on the Periodic Table:
Group 1: ______
Group 2: ______(2 names= group 2)
Groups 1& 2 are so active/ reactive (unstable), these elements are always found in compounds and never alone.
Groups 3- 11 ______
Solutions of compounds containing these elements are usually colorful.
- CuSO4 (aq) : ______
- CoCl2 (aq) : ______
Group 17: ______Has elements which are found in all three phases of matter, (s, l & g)
Group 18: ______Very stable (non-reactive, inert) due to having 8 electrons in outermost energy level except for Helium (He), which has 2 electrons.
c) Color Coding the PT on your Reference Tables- use your notes and the PTs around the room to help you
1) On the left side, copy the following to remind yourself that vertical columns are called GROUPS and horizontal rows are called PERIODS:
G
P E R I O D
O
U
P
2) Using a brown pencil, color lightly the elements, which are liquids.
3) Using a yellow pencil, color lightly the elements, which are gases.
4) Using an orange pencil, add two stripes to the Noble gases to remind yourself that they are found alone as Monatomic molecules.
5) Using apurple pencil, color over lightly the elements’ symbols, which always come in pairs, The “BrINClHOF” or “GEN-INE”. You should be able to still see the symbol!
6) Using a green pencil, lightly color the metalloids. Remember Al and Po are metals and NOT metalloids. Metalloids touch one full side along the dark “crack” on the right side of the PT.
7) Using a red pencil, lightly color groups 1 & 2 to remind yourself that these elements are so reactive that they are never found alone in nature, only in compounds.
8) Using a blue pencil, lightly color groups 3 to 11, the Transition elements/metals, to remind you, that these elements often form colorful compounds and solutions.
9) Using an arrow to help, label the groups 1, 2, 17 & 18 with their special names.
10) Use a bracket ( { ) to help label groups 3 & 11, the Transition elements/ metals.
11) At the top of the PT, label the left side metals and the right side NONMETALS.
12) Under Groups #1, #2, #13, #14, #15, #16, #17 & #18 draw the electron dot diagram, using “X” to represent the kernel. (Remember elements in the same vertical group have the same number of valence electrons so they have the same electron dot diagram. They will also have similar chemical properties because of the valence electrons)
d) Properties of Element Types
Element Type / Physical Properties / Chemical PropertiesMetal
Side of PT:
______
about 2/3 of all
elements / - Malleable (aluminum foil)
- Ductile (copper wire)
- Luster (aluminized glass = a mirror!)
- Excellent conductors of heat and electricity (wires + toasters)
- Large atomic radius (big atoms)
- Phase @ 25oC: ______
except: ______
- Silver in color except for: / - Low electronegativity
- Lose electrons when forming bonds
- Form + charged ions (called CATIONS)
- Low ionization energy
- Tend to tarnish or rust or form a patina (oxide coating) in the presence of oxygen
- Group 1 and 2 metals react violently with water
Nonmetal
Side of PT:
______
about 1/3 of all
elements / - Brittle (sulfur can be crushed to a powder)
- Dull (don’t reflect light well)
- Poor conductors of heat and electricity (except for certain forms of carbon)
- Small atomic radius (small atoms)
- Phase @ 25oC: ______
______
Only Liquid: ______
Gases:
- Come in a variety of colors & colorless / - High electronegativity
- Gain electrons when forming bonds with metals to form ionic bonds
- Form – charged ions (called ANIONS)
- Share electrons with other nonmetals to form covalent bonds
- Form molecules when bonded to other nonmetals
- Group 17 nonmetals (halogens) are
extremely corrosive
- High ionization energy
Metalloid-
Found along the crack in the PT, except for Al & Po (dog food),
which are metals
a full side must touch the crack / - Sometimes conduct electricity
(semiconductors)
- Used to make computer microchips
- Some have Luster (like metals)
- Brittle (like nonmetals)
- Photovoltaic (produce electricity from light)
- Used to make solar energy panels
- Phase @ 25oC: ______/ - Gain electrons from metals
- Lose electrons to nonmetals
Noble Gas-
Group 18 / - Low boiling points
- All gases at room temperature
- Poor conductors of heat and electricity / - Completely chemically nonreactive
- No electronegativity (no bonds form)
- Extremely high ionization energy
Metallic and Nonmetallic Character
1) Metallic Character: metals lose electrons due to low ionization energy. The element with the least ionization energy (Fr) is the most metallic, because it will lose electrons more easily than any other metal. When comparing metals, the lower the ionization energy, the more metallic character the element has. You can find ionization energy values on Reference Table S.
Example: Ca has an ionization energy of 590 kJ/mol, and K has an ionization energy of 419 kJ/mol. If you heat both metals up, K will lose its electron first, as it requires less energy. K has more metallic character than Ca.
Note: The total quantity of Francium on this planet (Earth) has been estimated to be just enough to fit inside a small pen cap. Being so rare, we will not be using Fr during this course for any other reason than as the most metallic element.
2) Nonmetallic Character: nonmetals tend to gain electrons due to high electronegativity. The element with the highest electronegativity (F) is the most nonmetallic, because it will gain electrons more easily than any other nonmetal. When comparing nonmetals, the higher the electronegativity, the more nonmetallic character the element has. You can find electronegativity values on Reference Table S.
Example: O has an electronegativity of 3.5 and Cl has an electronegativity of 3.2. Since O has a greater attraction to electrons than Cl does, it is more likely to gain electrons from a metal than Cl is. O has greater nonmetallic character than Cl.
e) Common Element Names and Symbols (based on Reference Table S)
Symbol / Name / Significance/Use / Symbol / Name / Significance/UseH / Hydrogen / Lightest element, flammable / Co / Cobalt / Magnetic alloys
He / Helium / Balloons, radioactivity / Ni / Nickel / Coins, alloys
Li / Lithium / Battery technology / Cu / Copper / Wires, pipes, alloys
C / Carbon / Life, plastics, energy / Zn / Zinc / Galvanized steel, batteries
N / Nitrogen / Life, atmosphere / Br / Bromine / Cleaning properties
O / Oxygen / Life, atmosphere, oxides / Kr / Krypton / Headlamps
F / Fluorine / Most nonmetallic element / Ag / Silver / Jewelry, alloys
Ne / Neon / Advertising signs / Sn / Tin / Alloys, toxic heavy metal
Na / Sodium / Explosive metal, makes salt / I / Iodine / Disinfectant
Mg / Magnesium / Lightweight metal, flares / Xe / Xenon / Flashbulbs
Al / Aluminum / Structural lightweight metal / Ba / Barium / Radiocontrast for X-rays
Si / Silicon / Microchip technology / W / Tungsten / Light bulb filaments
P / Phosphorous / Life, incendiary devices / Au / Gold / Jewelry, conductor, alloys
S / Sulfur / Matches, gunpowder / Hg / Mercury / Amalgams, thermostats
Cl / Chlorine / Cleaning properties / Pb / Lead / X-ray blankets, toxic
Ar / Argon / Gas in windows / Fr / Francium / Most metallic element
K / Potassium / Nutrition, explosive metal / Rn / Radon / Carcinogenic gas
Ca / Calcium / Bones, minerals (limestone) / U / Uranium / Nuclear reactor fuel
f) Important Definitions to Know for Periodic Table Unit
PERIODIC TABLE: PROPERTIES OF ELEMENTS and TRENDS
Electronegativity: ______
______
- found on Reference Table S
- For Metals (left side of PT) it tends to be ______
- For Nonmetals (right side of PT) it tends to be ______
Ionization Energy: ______
______
- found on Reference Table S
- For Metals (left side of PT) it tends to be ______
- For Nonmetals (right side of PT) it tends to be ______
Atomic Radii:______
______
- found on Reference Table S
- radii ______as you go across the Periodic Table Left Right
- radii ______as you go down Periodic Table
Reactivity:
As a metal: ______
Most reactive Metal = ______
As a nonmetal: ______
Most reactive Nonmetal = ______
g) Trends in an “atomic shell” instead of a nutshell!
Trend / Down A Group (top to bottom) / Reason for Trend / Across a Period(L R) / Reason for Trend
Atomic Number
Number of Valence Electrons
Atomic Radius
Metallic Characteristics (Reactivity/Activity as a metal loses electrons)
Non-Metallic Characteristics (Reactivity/Activity as a non-metal gains electrons)
Electronegativity (EN)
Ionization Energy (IE)
h) Forming Ions: An ionic bond forms when a metal loses valence electrons to a nonmetal forming a positive ion and the nonmetal, which gained the electrons, forms a negative ion. These oppositely charged ions then attract to each other. By losing or gaining electrons, each ion formed gets 8 valence electrons.
Metals:lose valence electrons when forming positive ions called: ______# electrons lost = ______This is known as oxidation.
For lithium (Li)
Bohr Model of the neutral atom Bohr Model of the “+ ion”
What happens to the size of the metal atom when it forms an + ion? ______
This is known as the ionic radius. Ionic radius of a metal ion is ______then its neutral atom.
(Memory hook- lose weight, get a smaller waist; lose electrons get ______)
Nonmetals:gain valence electrons when forming negative ions called: ______# electrons gained = ______This is known as reduction.
For fluorine (F):
Bohr Model of the neutral atom Bohr Model of the ion “-ion”
What happens to the size of the nonmetal atom when it forms an - ion? ______This is known as the ionic radius. Ionic radius of a nonmetal ion is ______then its neutral atom.
(Memory hook- gain weight, get a larger waist; gain electrons get ______)
I) PERIODIC TABLE WORKSHEET
I. Determine the Principle Energy Level (PEL) and the number of valence electrons for the following elements. (PEL = Period #)
Element / PEL / # Valence ElectronsLi
Mg
Al
Ge
N
Se
Cl
Kr
II. Use the trend for atomic radii to III. Use the trend for electronegativity
determine the larger atom of the pair. (EN)to determine which atom of the pair
Circle the larger element (You can look hasthe higher electronegativity.Circle
up the radii on Reference Table S also) theelement with the higher EN (You
1) O or S2) N or O
3) Mg or P
4) Cl or I
5) P or N
can look up the EN on Ref. Table S also)
1) N or O2) O or S
3) P or As
4) Mg or Na
5) Li or Be
IV. Using the periodic table, determine the charge of the ion formed from the element listed and indicate if the radiusof the ion is Larger (L) or Smaller (S) than the neutral atom. Remember to use the FIRST charge listed for nonmetals.
ELEMENT / CHARGE / Size: L or S / ELEMENT / CHARGE / Size: L or S1) Mg / 5) Br
2) Na / 6) O
3) S / 7) Sc
4) H / 8) N
Periodic Table in Review:
1)Which two elements are the only liquids?______and ______
2)Which group, name and number, exists as monatomic molecules of gas?
Group #: ______Name: ______
3) Which group, name and number, contains elements, which are solids, liquids and gases? Group #: ______Name: ______
4)Which elements exist as diatomic molecules? ______
5)Which elements are gases on the periodic table? ______
6)Which elements are metalloids and where are they found? ______
______
7)Which element is the most reactive metal? ______reactive nonmetal? ______
8)Even though iodine’s mass is less than tellurium, why was iodine (I) placed in group 17, after tellurium (Te)? ______
9)Why is hydrogen (H) placed on top of Group 1 metals when H is not a metal?
______
10)Which elements form compounds whose aqueous solutions are colorful?
______
11)Which metal groups are so reactive, they are never found alone, only in compounds?
Group #: ___Name: ______
Group #: ____Name: ______
12) Metals form ______charge ions by (losing or gaining) electrons, whose size is ______then the neutral atom. Loss of electrons is known as (oxidation or reduction). [circle the correct term in the ( )]
13) Nonmetals form ______charge ionsby (losing or gaining) electrons, whose size is ______then the neutral atom. Gain of electrons is known as (oxidation or reduction). [circle the correct term in the ( )]
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