discovering a pattern in 1869, russian chemist dmitri mendeleev arranged the elements in order of...
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Discovering a Pattern
• In 1869, Russian chemist Dmitri Mendeleev arranged the elements in order of increasing atomic mass.
•His Periodic table showed that•Elements with similar properties occurred in a repeating pattern•There were gaps in its pattern •He could predict the properties of the missing elements
By 1886, all of the gaps had been filled and Mendeleev’s predictions were right.
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Changing the Arrangement
• A few elements’ properties did not fit in the pattern of Mendeleev’s table.
• 1914: British scientist Henry Moseley found the atomic number of atoms.
• Elements arranged by atomic number fit the pattern in Mendeleev’s table.
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Elements are arranged:
Vertically into Groups
Horizontally Into Periods
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Why?
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If you looked at one atom of every element in a group you would
see…
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Each atom has the same number of electrons in it’s outermost shell.
• An example…
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The group 2 atoms all have 2 electrons in their outer shells
Be (Beryllium)
Atom
Mg (Magnesium) Atom
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• The number of outer or “valence” electrons in an atom effects the way an atom bonds.
• The way an atom bonds determines many properties of the element.
• This is why elements within a group usually have similar properties.
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If you looked at an atom from each element in a period
you would see…
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Each atom has the same number of electron holding shells.
An example…
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The period 4 atoms each have 4 electron containing shells
K (Potassium)
AtomFe (Iron) Atom
Kr (Krypton)
Atom
4th Shell
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Each group has distinct properties
• The periodic Table is divided into several groups based on the properties of different atoms.
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The Periodic Table and Classes of Elements
• Elements are classified as metals, nonmetals, and metalloids based on number of electrons in outer shell
• an outer shell is considered complete when it contains 8 electrons
•The zigzag line on the periodic table can help you recognize which elements belong in which category.
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Group 1: Alkali Metals
Alkali metals properties:
• metals• 1 electron in the outer level• very reactive• softness, color of silver, shininess, low density
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Alkali Metals
Soft, silvery colored metals
Very reactive!!!
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• found to the left of the zigzag line
• have few electrons in their outer energy level.
• shiny, ductile, malleable, and are good conductors of electric current and thermal energy.
Metals
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Alkali Metals reacting with water:
• Li (Lithium)
• Na (Sodium)
• K (Potassium)
• Rb (Rubidium)
• Cs (Cesium)
What would you expect from Francium?!?!
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Group 2: Alkaline-Earth Metals
Alkaline-earth metals properties:
• metals• 2 electrons in the outer level• very reactive, but less reactive than alkali metals• color of silver, higher densities than alkali metals
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Alkaline Earth Metals
Silvery-White Metals
Fairly reactive
Many are found in rocks in the earth’s crust
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Group 3–12: Transition Metals
Properties of Transition Metals vary widely but include:
• metals• 1 or 2 electrons in the outer level• less reactive than alkaline-earth metals• shininess, good conductors of electric current and thermal energy
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Transition Metals
Malleable (easily bent/hammered into wires or sheets)
Most are good Conductors of electricity
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How many things can you think of that have Transition Metals in
them?
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Metalloids lie on either side of these “stairsteps”
They share properties with both metals and non-metals
Si (Silicon) and Ge (Germanium) are very important “semi-conductors”
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• border the zigzag line
• have about half of a complete set of electrons in their outer energy level.
• Metalloids have some properties of metals and some properties of nonmetals.
• Metalloids are also called semiconductors.
Metalloids
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What are semiconductors used in?
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Nonmetals
Brittle
Do not conduct electricity
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• to the right of the zigzag line
• have an almost complete set of electrons in their outer energy level.
•not shiny, ductile, or malleable, and poor conductors of electric current and thermal energy.
Nonmetals
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Group 13: Boron Group
Group 13 properties:
•one metalloid and five metals• 3 electrons in the outer level• reactive• solids at room temperature
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Group 14: Carbon Group
Group 14 properties:
•one nonmetal, two metalloids, and two metals• 4 electrons in the outer level• reactivity varies among the elements• solids at room temperature
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Group 15: Nitrogen Group
Group 15 properties:
•two nonmetals, two metalloids, and two metals• 5 electrons in the outer level• reactivity varies among the elements• solids at room temperature (except for nitrogen, which is a gas)
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Section 2 Grouping the Elements
Group 16: Oxygen Group
Group 16 properties:
• group contains three nonmetals, one metalloids, and one metal• 6 electrons in the outer level• reactive• solids at room temperature (except for oxygen, which is a gas)
Chapter 12
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Section 2 Grouping the Elements
Hydrogen
The properties of hydrogen do not match the properties of any single group, so hydrogen is set apart.
• a nonmetal• 1 electron in the outer level • reactive• colorless, odorless gas at room temperature, low density
Chapter 12
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Most are Poisonous
Fairly reactive
Halogens
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Section 2 Grouping the Elements
Group 17: Halogens
Halogens are the elements in Group 17. Group 17 properties:
• group contains nonmetals• 7 electrons in the outer level• very reactive• poor conductors of electric current, never in uncombined form in nature
Chapter 12
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Chlorine Gas was used as a chemical weapon during World War I.
It was used by the Nazis in World War II.
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Section 2 Grouping the Elements
Group 18: Noble Gases
Noble gases are the elements in Group 18. Group 18 properties:
• group contains nonmetals• 8 electrons in the outer level (except helium, which has 2)• unreactive• colorless, odorless gases at room temperature
Chapter 12
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Unreactive
Gases at room temperature
Noble Gases
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Jellyfish lamps made with noble gases artist- Eric Ehlenberger
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Colors Noble Gases produce in lamp tubes:
• Ne (Neon): orange-red
• Hg (Mercury): light blue
• Ar (Argon): pale lavender
• He (Helium): pale peach
• Kr (Krypton): pale silver
• Xe (Xenon): pale, deep blue
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Group 3–12: Transition Metals, continued
• Lanthanides and Actinides Some transition metals from Periods 6 and 7 appear in two rows at the bottom of the periodic table. Elements in the first row are called lanthanides and elements in the second row are called actinides.
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Lanthanide Series
Actinide Series
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The Periodic Tables
Use the terms below to complete the concept map on the next slide.
Chapter 12
Concept Map
elements
periods
metals
electrons
nonmetals
periodic table
groups (families)
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The Periodic TableChapter 12
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The Periodic TableChapter 12
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1. Which of the following statements is correct for the elements shown?
Chapter 12 Standardized Test Preparation
A Lithium has the greatest atomic number.
B Sodium has the least atomic mass.
C Atomic number decreases as you move down the column.
D Atomic mass increases as you move down the column.
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1. Which of the following statements is correct for the elements shown?
Chapter 12 Standardized Test Preparation
A Lithium has the greatest atomic number.
B Sodium has the least atomic mass.
C Atomic number decreases as you move down the column.
D Atomic mass increases as you move down the column.
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2. Which of the following statements best describes the outer electrons in atoms of the elements shown?
F The atoms of each element have 1 outer-level electron.
G Lithium atoms have 3 outer-level electrons, sodium atoms have 11, and potassium atoms have 19.
H Lithium atoms have 7 outer-level electrons, sodium atoms have 23, and potassium atoms have 39.
I The atoms of each element have 11 outer-level electrons.
Chapter 12 Standardized Test Preparation
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2. Which of the following statements best describes the outer electrons in atoms of the elements shown?
F The atoms of each element have 1 outer-level electron.
G Lithium atoms have 3 outer-level electrons, sodium atoms have 11, and potassium atoms have 19.
H Lithium atoms have 7 outer-level electrons, sodium atoms have 23, and potassium atoms have 39.
I The atoms of each element have 11 outer-level electrons.
Chapter 12 Standardized Test Preparation
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3. The elements featured in the image belong to which of the following groups?
A noble gases
B alkaline-earth metals
C halogens
D alkali metals
Chapter 12 Standardized Test Preparation
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3. The elements featured in the image belong to which of the following groups?
A noble gases
B alkaline-earth metals
C halogens
D alkali metals
Chapter 12 Standardized Test Preparation
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2. A chemical company is preparing a shipment of 10 g each of four elements. Each element must be shipped in its own container that is completely filled with the element. Which container will be the largest?
F the container of aluminum
G the container of arsenic
H the container of germanium
I the container of silicon
Chapter 12 Standardized Test Preparation
ElementDensity (g/cm3)
Mass (g)
Aluminum 2.702 10
Arsenic 5.727 10
Germanium 5.350 10
Silicon 2.420 10
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2. A chemical company is preparing a shipment of 10 g each of four elements. Each element must be shipped in its own container that is completely filled with the element. Which container will be the largest?
F the container of aluminum
G the container of arsenic
H the container of germanium
I the container of silicon
Chapter 12 Standardized Test Preparation
ElementDensity (g/cm3)
Mass (g)
Aluminum 2.702 10
Arsenic 5.727 10
Germanium 5.350 10
Silicon 2.420 10