Chemistry 11
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Transcript of Chemistry 11
Chemistry 11
“Wooot, yay, I love science”
“ Dmitri Ivanovich Mendeleev “
Certain characteristic properties of elements can be foretold from their atomic weights. – D.Mendeleev
The Periodic Table:Mendeleev - 1800’s
-63 elements known
-He recognized similarities in some of the elements
-Decided to group them according to mass and noticed a pattern in their bonding power or valence.
-When organized in this way the elements fell into columns which showed similar physical and chemical properties.
Your Turn To be a Scientist!!
• Your job is to arrange the fake elements you have been given according to the patterns you see and the trends you can create.
Modern Periodic Table
-When atomic numbers (number of protons in the nucleus) were discovered 50 years later the elements were arranged according to their atomic number.
-The periodic law states:
-other periods -calendars, music scales, periodicals.
Organization of the Periodic Table
Rows - called -elements in a period are not alike in properties.-1st element is an extremely active solid whereas
last element is a inactive gas ex. Columns - called
- elements in the same family have similar properties
ex. K, Na, Li are all soft, white, shiny metals.
Element key-
Metals - 88 elements to left of zigzag line are called metals.
Physical properties of metals:
• luster/shininess• good conductors of heat and electricity• • ductile-drawn into wires• malleable-hammered into thin sheets.
Chemical properties of metals:
• Tend to ex. rust/tarnish
Non-metals
- right of the zigzag line.
Physical properties:--
Chemical properties:-tend to
exception: Noble gases
Metalloids
- along both sides of the zigzag line are elements which have properties of both
ex. B, Si, Ge, As, Sb, Te, Po, At
Periodic Table
Chemical FamiliesMost Active MetalsAlkali Metals - elements in with one valence electron in their outermost energy level.- very reactive and readily bonded with other substances.
Ex.
Alkaline Earth Metals- elements in with two valence electrons in their outermost energy level. - still very reactive but not as reactive as Family 1 cause they have two electrons to get rid of.
Chemical Families
Transition Metals ( ) - have properties similar to one another and to other metals
-have one or two valence electrons in their outer shell.
-some have ability to an electron from their next to outermost energy level.
Chemical Families
From Metals to Non-Metals - five families to the right contain properties of metals as well as non-metals.
-named after the first element in the family.
Ex. c
Chemical Families
Halogens - have 7 valence electrons and are the most active of the non-metals.-react easily with alkali metals
Ex.
Noble Gases- , therefore normally unreactive.
Chemical Families
Rare-Earth Elements - two rows appearing at the bottom of the periodic table:
- lanthanoid series - soft malleable metals, high luster.
- actinoid series - radioactive, most made in lab.
Electron Configuration• The outer most electrons of an atom determines its
.
• These outer electrons are called .
• Elements in the same family/group have similar properties because they have similar valence electron configurations.
• Ex. Li=1s2 2s1Na=K=1s2s 2s2 2p6 3s2 3p6 4s1