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Chemistry-Unit-5

Periodic Trends

TermDefinition
Mendeleev Organized elements by increasing atomic mass and so that elements in the same row have similar properties
Moseley Rearranged the elements by increasing atomic number - what we use today
Periodic Law When elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties
Series The horizontal rows of the Periodic Table
Families The vertical columns on the Periodic Table
Do groups have similar properties? Yes
Do periods have similar properties? No
Representative Elements S and p blocks
Transition Metals D block
Inner Transition Metals F block
Alkali Metals Group 1
Alkaline Earth Metals Group 2
Halogens Group 17
Noble Gases Group 18
Properties of Metals Left of staircase, lustrous, malleable, ductile, good conductors
Properties of Nonmetals Right of staircase, non-lustrous, brittle, poor conductors
Metalloids Have properties of both nonmetals and metals, semiconductors
Atomic Radius 1/2 of the distance between the nuclei of two like atoms
Atomic Radius Group Trends Atomic size increases as you move down a group due to a greater number of occupied energy levels
Atomic Radius Period Trends Atomic size decreases from left to right
Shielding Effect The period trend is less significant for periods further down the Periodic Table
Cation Trends The more electrons lost, the smaller the ions become because there are more protons than electrons.
Anion Trends The more electrons grained, the bigger the ion becomes because there is less attractive force between electrons and nucleus.
Electronegativity Tendency for an element to attract electrons when chemically combined with another element
Highest Electronegativity Element Fluorine with 4.0 because it is the smallest element next to a noble gas
Group Electronegativity Trend Electronegativity decreases as you go down because electrons are less attracted to the nucleus since there are more energy levels.
Period Electronegativity Trend Electronegativity increases from left to right because electrons are more attracted to the nucleus due to an increased nuclear charge.
Ionization Energy Amount of energy required to remove an electron from a gaseous atom
Group Ionization Trend Decreases as you go down due to a greater number of energy levels.
Period Ionization Trend Increases as you move across due to an increased nuclear charge.
Removing More Electrons Ionization Trend It requires more energy to remove 2nd and 3rd electrons because they are more attracted to a positive ion than a neutral atom.
Noble Gas Ionization Trend A large increase in ionization energy occurs when an electron is removed from an atom/ion that is isoelectronic with a noble gas.
Created by: ClimbingBird
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