the periodic table of elements. early versions 1830: 55 elements had been discovered 1860’s:...
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Mendeleev Father of the periodic table Noticed patterns when the elements were arranged by increasing atomic massTRANSCRIPT
The Periodic Table of Elements
Early Versions 1830: 55 elements had been discovered
1860’s: Dimitri Mendeleev discovered a system that applied to all elements
Mendeleev
•Father of the periodic table•Noticed patterns when the elements were arranged by increasing atomic mass
Mendeleev Noted properties of elements
Melting point Density Color
Studied atomic mass and chemical bonds Compared mass to hydrogen
Mendeleev Noted that arranging elements
according to atomic mass did not always produce similar groups
Moved element cards into groups where they fit best
Predicted other elements and their properties
Mendeleev 1869: Published the 1st periodic table
The Modern Periodic Table
New elements were added as they were discovered
Early 1900’s: scientists learned about the atomic number
Reading the Periodic Table
Contains over 100
squares: one for each
element
Isotopes Atoms of a certain element ALWAYS have
the same # of protons….DO NOT always have the same mass May have different number of neutrons Isotope
Atoms of the same element that have a different number of neutrons
Isotopes Examples:
Chlorine-35 Chlorine-37 Carbon-14
Reading the Periodic Table
An element’s properties can be predicted from its location on the periodic table.
groups/familiesperiods
Groups/Families Elements in columns 18 columns Elements in each group have
similar characteristics. Example: Group 1 are metals that all react violently with water; Group 17 reacts violently with elements from Group 1; Group 18 rarely reacts at all
Groups/Families EXAMPLES OF FAMILIES
- Alkali Metals- Alkaline Earth Metals- Transition Metals- Halogen Gases- Inert Gases (Noble Gases)
Periods Horizontal rows Series of different elements from different groups
Have very different properties
Why it Works!It’s based on the structure of atoms, especially the valence electrons!
Metals Most elements are metals. Found to the left of the zig-zag line. Elements are classified as metals
based on physical properties. Hardness Shininess (luster) Malleability Ductility
Physical Properties Have luster (shiny) Good conductors of heat &
electricity (transmit easily) High density Very high melting point Ductile (drawn into thin wires) Malleable (hammered into thin
sheets) Most are solid at room temperature.
Chemical Properties
Wide range of chemical properties Some are very reactive and combine
quickly. (sodium) Some are unreactive. (gold) Other metals fall somewhere in
between Corrosion: the process of reaction and
wearing away of metals
Alloys A mixture of metals Combine the best properties of
2 or more metals into a single substance
Ex: copper + tin = bronze Ex: copper + zinc = brass
Group 1: Alkali Metals
From Lithium to Francium MOST reactive of ALL metals NEVER found uncombined in nature; exist as compounds
Very soft & shiny Have 1 valence electron (lose easily)
2 MOST IMPORTANT: sodium & potassium (essential for life)
Group 2: Alkaline Earth Metals
Not as reactive as group 1, but still more reactive than most metals
NEVER found uncombined in nature Have 2 valence electrons (lose easily) 2 MOST COMMON: magnesium &
calcium Magnesium: flash bulbs, alloys for
airplanes, ladders Calcium: teeth & bones, muscles
Groups 3-12: Transition Metals
Form a bridge between very reactive metals on the left and less reactive metals on the right
So similar to one another that differences between nearby columns are difficult to detect
Include the most familiar metals: iron, copper, nickel, silver & gold
Groups 3-12: Transition Metals
Most are hard and shiny All are good conductors of
electricity. Fairly stable, reacting slowly or
not at all with water and air
Groups 13-16: Metals in Mixed Groups
Metals to the right of the transition metals are not nearly as reactive as those on the left.
Most familiar: aluminum, tin, lead
Lanthanides and Actinides
Lanthanides: top row at the bottom of the periodic table
Actinides: bottom row at the bottom of the periodic table
Called rare earth elements Fall between alkaline earth metals and
transition metals Placed at the bottom for convenience
Lanthanides Soft, malleable, shiny metals High conductivity Used in industry to make various
alloys Different lanthanides are found
together in nature; difficult to separate because of the similar properties
Actinides Only thorium and uranium exist on
Earth in any significant amounts Uranium: used in nuclear power
All elements after uranium were created artificially in a laboratory.
NonmetalsLack most of the properties of metals
Located to the right of the zigzag line
Physical Properties In general: opposite of metals Gases at room temperature; means they
have low boiling points Dull Solid nonmetals are brittle. NOT malleable or ductile Lower densities than metals Poor conductors of heat and electricity
Chemical Properties
Readily form compounds; except Group 18
Group 18 elements do not react with other elements.
Many form molecules containing 2 atoms: diatomic molecules (O2)
Nonmetals can form compounds with metals (NaCl) or other nonmetals (CO2).
Families of Nonmetals
Carbon Family (Group 14) All have 4 valence electrons. Carbon is the only nonmetal in the group. 2 are metalloids; 2 are metals Carbon is special because it is important for life. ALL living things contain Carbon!
Families of Nonmetals
Nitrogen Family (Group 15) All have 5 valence electrons. Only 2 nonmetals in this group: nitrogen &
phosphorus N2 makes up about 80% of our air; most
living things can not use it in gas form Get nitrogen from food Phosphorus is not a stable element; always
found in compound in nature. Used to make matches and flares
Families of Nonmetals
Oxygen Family (Group 16) All have 6 valence electrons. Elements typically gain or share 2 electrons Oxygen we breathe = O2 Ozone = O3 Oxygen is very reactive and can combine easily
with other elements. Oxygen: most abundant element in Earth’s crust;
second most abundant in the atmosphere Sulfur is a common nonmetal in the Oxygen family
Families of Nonmetals
Halogen Family (Group 17) All have 7 valence electrons. All but Astatine are nonmetals; Astatine is a
metalloid Typically gain or share 1 electron ALL are very reactive; most are dangerous to
humans Compounds that they form are useful:
Flourine—toothpaste, nonstick cookware Chlorine—table salt Bromine—reacts with silver (photographic film)
Families of Nonmetals
Noble Gases (Group 18) Also known as inert gases ALL have 8 valence electrons Do Not ordinarily form compounds Do not gain, share, or lose electrons; very
stable and unreactive All exist in Earth’s atmosphere, but only in
small amounts
Families of Nonmetals
Hydrogen Simplest of all elements Generally contains only one proton and one electron Cannot be grouped in a family because its chemical
properties are so different from other elements Makes up 90% of the atoms in the universe; only 1%
of the mass of Earth’s crust, oceans, & atmosphere Rarely found on Earth as an element Mostly combined with oxygen (water)
Metalloids On zigzag line between metals & nonmetals 7 elements Some have characteristics of metals; some
have characteristics of nonmetals Most useful property is their varying ability
to conduct electricity Most common is silicon
Sand, glass, cement
Metalloids Whether they conduct electricity
depends on temperature, exposure to light, or presence of impurities
Semiconductors: substances that under certain conditions can carry electricity, while under others it cannot Silicon & germanium Used to make computer chips, transistors,
lasers