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Periodic table test

TermDefinition
Who created the periodic table? Dmitri Mendeleev
What was Mendeleev able to do? He was able to predict elements that were not discovered at the time.
Periods Rows going across the the periodic table
Elements in the same period have the the same number of... Occupied principal energy levels (shells)
Valance electrons increase from 1-8 as you go down a... Period
Groups Also known as families, columns going down the periodic table
Elements in the same group have the same... number of valence electrons
What increases as you go down a group? Occupied principle energy levels
The periodic table is mainly arranged in order of increasing... atomic number
Elements with similar chemical properties are placed in the same... groups/families
Elements share similar chemical properties because they contain the same number of... valance electrons
Elements in the same group can form... ions with the same charge
What side of the table are metals located on Left
How do metals form ions They lose electrons to make an octet (losers on the left)
What side are nonmetals located on Right
How do nonmetals form ions They gain electrons to make an octet
What are metalloids Also known as semimetals, they are located on the staircase and have properties of both metals and nonmetals. Aluminum is located on the staircase but behaves like a metal.
Where are alkaline metals found Group 1
Where are alkaline earth metals found Group 2
Where are halogens found Group 17
Where are noble gases (inert gases) found Group 18
Atomic radius half the distance between two nuclei of two different atoms
How does atomic radius change across a period decreases because the charge of the nucleus increases (atomic number) creating a stronger pull on the electrons.
How does atomic radius change over a group Increases because there are more principal energy levels (shells)
Ionic radius the size of an ion
Positive ions are... smaller then their atom because they lost a shell
Negative ions are... larger than their atom they gain electrons
Ionization energy The amount of energy needed to remove the most loosely bound electron from an atom
How does ionization energy change across a period Increases because the pull of the nucleus (atomic number) gets larger and has a bigger pull
How does ionization energy change across a group Decreases because there are more shells, meaning that there is less of a pull from the nucleus
Electronegativity The ability of an atom to attract an electron
How does electronegativity change over a period It increases because the pull of the the nucleus increases,
How does electronegativity change over a group It decreases because the amount of shells increase
Characteristics of metals - Few valance electrons - lose electrons to form positive ions (losers on the left) - Low ionization and electronegativity - High melting and boiling point - Good conductors of heat and electricity - Malleable and ductile - luster
Characteristics of nonmetals - right side of staircase - more valance electrons - Gain electrons to form negative ions - High IE and EN - Soft and brittle - dull - insulators (do not conduct heat or electricity)
Created by: 29wernera
 

 



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