Periodic Table
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Transcript of Periodic Table
Dmitri Mendeleev organized the known elements into a table called the periodic table.
He organized them by their increasing atomic masses.
Today we organize the elements by their
increasing Atomic Number.
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Rows on the periodic table are called periods. All the elements listed in a row belong to the same period. There are 7 (seven) periods.
Columns in the periodic table are called groups or families. All elements in a group have similar properties.
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The columns have been given an Arabic number. The columns are numbered 1 – 18 starting at the left and moving to the right. Please make sure that your periodic table has them numbered like this.
The outer most energy level is usually not full or complete .
Valence electrons are important because they determine how an element will react with other substance.
These electrons in the outer energy level are called Valence electrons.
Valence Electrons
Group 1 and 2 the number of Valence electrons in the outer energy level will match the group number.
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Groups 3 through 12 do not follow any particular rule to determine the number of Valence electrons.
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Group 13 to 18 – The Valence electrons for each of these is the group number less 10. For example Group 14 – 10 = 4 Valence electrons.
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Elements whose atoms gain, lose or share
electrons are reactive and they combine to form the many compounds we use
in our daily lives.
Elements are categorized as metals, nonmetals or
metalloids.
Metals: An element that has luster, is malleable and ductile, and is said to be a good conductor of heat and electricity.
Luster describes the way a surface reflects light…therefore metallic luster would be shiny like a metal object.
Malleable means to be able to press or pound the substance into sheets or different shapes.
What is luster, malleable and ductile?
Ductile means that the substance can be drawn out into thin wires.
Elements are categorized as metals, nonmetals or metalloids (cont’).
Nonmetals: an element that is usually a gas or a brittle solid at room temperature. It is a poor conductor of heat and electricity.
Elements are categorized as metals, nonmetals or metalloids (cont’).
Metalloid: an element that shares some characteristics or properties with both metals and nonmetals.
Group 1 and 2 Elements:
These elements are so reactive that they are only found combined with other
elements in nature.
3
LiLithium6.941
11Na
Sodium22.990
19K
Potassium39.098
37Rb
Rubidium85.468
55Cs
Cesium132.905
87Fr
Francium223.020
Group 1: Alkali Metals
• Soft – can be cut with a knife• Shiny and silver colored• Low Density (some will even float)
• Most reactive of the metals
• Valence electrons = 1• Reacts violently with water
forming a hydrogen gas
• Compounds from these are very useful such as NaCl
4Be
Beryllium9.012
12Mg
Magnesium24.305
20Ca
Calcium40.078
38Sr
Strontium87.62
56Ba
barium137.327
88Ra
Radium226
Group 2: Alkaline- Earth Metals
• Very reactive but not as reactive as Alkali Metals.
• Silver colored
• More dense than Group 1 metals
• Valence electrons = 2• Useful compounds include: Calcium
compounds such as cement, plaster, chalk, and YOU.
Group 3 to 12: Transition Metals
• Do not lose their valence electrons as easily as groups 1 & 2.
• Less reactive than Alkali and Alkaline Earth metals
• Shiny
• Good conductors of electricity
•Higher density and melting points (except mercury) than Group 1 and 2
Group 3 to 12: Transition Metals (cont’.)• Lanthanides: The first row underneath the periodic table: Shiny, reactive, many are used in the production of steel.
• Actinides: The second row underneath the periodic table: These elements are all radioactive and unstable..
Note: Elements found after 94 (Plutonium) are man made and not found in nature
5B
Boron10.811
13Al
Aluminum26.982
31Ga
Gallium69.723
49In
Indium114.818
81Tl
Thallium204.383
Group 13: Boron Group
• Reactive• Valence electrons = 3• Contains 1 Metalloid and 4 Metals
• Solid at room temperature
• Aluminum is the most abundant in this group and the most common in the Earth’s crust
6C
Carbon12.011
14Si
Silicon28.086
32Ge
Germanium72.64
50SnTin
118.71082Pb
Lead207.2
Group 14: Carbon Group
• Reactivity varies in this group depending on the element
• Valence electrons = 4• This group contains 2 metals, 1
nonmetal and 2 metalloids.
• Many forms found uncombined in nature such as diamonds
• Compounds are very useful: proteins, fats, carbohydrates, computer chips.
7N
Nitrogen14.007
15P
Phosphorous30.974
33As
Arsenic74.922
51Sb
Antimony121.760
83Bi
Bismuth208.980
Group 15: Nitrogen Group• Reactivity varies in this group depending
on the element
• Valence electrons = 5• Group contains 1 metal, 2 Nonmetals, and
2 metalloids
• Phosphorous is very reactive and only found in nature combined with other elements.
• All but nitrogen are solid at room temperature.
• Nitrogen makes up 78% of our atmosphere.
• Generally unreactive.
8O
Oxygen15.999
16S
Sulfur32.065
34Se
Selenium78.96
52Te
Tellurium127.60
84Po
Polonium209
Group 16: Oxygen Group• More reactive than group 15
• Valence electrons = 6• Group contains 1 Metals, 3 Nonmetals and 1
Metalloids
• Sulfur is found in nature and is used to make sulfuric acid, a very commonly used chemical in industry.
• All but oxygen are solid at room temperature.
• Oxygen makes up 21% of the Earth’s Atmosphere
• Oxygen is very reactive and combines with many other elements especially metals
• Rust is the result of the oxidation of metal.
9F
Fluorine18.998
17Cl
Chlorine35.453
35Br
Bromine79.904
53I
Iodine126.904
85At
Astatine210
Group 17: Halogen Group• Very reactive• Valence electrons = 7• Nonmetal group
• Poor Conductors of electricity and heat
• React violently with alkali metals to form salts
• Never found uncombined in nature
• Atoms of these elements only need to gain 1 electron to fill their outer shell
• Chlorine and Iodine are both in this group and can be combined to make disinfectants.
2He
Helium4.003
10
NeNeon
21.180
18Ar
Argon39.948
36Kr
Krypton83.80
54Xe
Xenon131.293
86Rn
Radon222
Group 18: Noble Gas Group• Non-reactant
• Valence electrons = 8• Outermost energy shell is full
• Colorless, odorless gases at room temp.
• Under normal conditions they do not react with other elements
• All found on Earth in very small amounts
• Argon is the most common in the group
• Their non-reactivity makes them very useful for light bulbs, helium for blimps and weather balloons.
1H
Hydrogen1.008
Hydrogen Stands Alone:
• Properties do not match the properties of any single group
• Valence Electrons = 1• Easily looses that one valence electron
• Physical properties are like the nonmetal group
• Most abundant element in the Universe
• Its reactive nature makes it useful as a fuel for rockets.
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