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Chemistry Chapter 5

TermDefinition
triad groups of three related elements that are found in the same column on the periodic table
law of octaves every 8th element had similar repeating properties
periodic law the physical chemical properties of the elements are a periodic function of their atomic masses
modern periodic law the physical and chemical properties of the elements are a function of their atomic numbers
Johann Dobereiner discovered triads (groups of 3 related elements)
John Newlands organized elements in order of increasing atomic masses, law of octaves (found that every 8th element had similar repeating properties)
Lothar Meyer organized elements in order of increasing atomic masses, made an 8 column table of the elements
Dmitri Mendeleev organized elements in order of increasing atomic masses, his table was the basis of modern periodic table, grouped elements with similar characteristics in the same column, made an 8 column table of elements, left blanks for undiscovered elements, predicted properties for unknown elements (elements in the same column have similar characteristics), periodic law (physical and chemical properties of the elements are a periodic function of their atomic masses)
Henry Moseley arranged elements in order of increasing atomic number, modern periodic law (the physical and chemical properties of the elements are a periodic function of their atomic numbers)
atomic radius (periods) an estimate of the size of an atom trend: decreases ( in periods from left to right across the periodic table)
period the row of elements that lie in a horizontal row in the periodic table
atomic radius (groups) an estimate of the size of an atom trend: increases (in groups from top to bottom on the periodic table)
group elements that are in the same column of the periodic table, aka family
ionization energy (groups) the energy required to remove electrons from a gaseous atom or ion trend: decreases (in groups from top to bottom on the periodic table)
Shielding effect -the core electrons or inner shell electrons block/shield the positive charge of the nucleus -the proton pull is always less because of the shielding effect -the shielding effect is only a factor in groups
Ionization energy (periods) the energy required to remove electrons from a gaseous atom or ion trend: increases (in periods from left to right across the periodic table)
Effective Nuclear Charge aka Zeff -the net positive charge attracting the electrons -another way of saying proton pull * Remember electrons have a -1 charge and protons have a +1 charge = opposites attract
Electron affinity (periods) the energy change that occurs when an electron is added to a gaseous atom trend: increases (in periods from left to right on the periodic table)
Electronegativity (periods) the ability of an atom in a molecule to attract shared electrons to itself trend: increases (in periods from left to right across the periodic table)
Electron affinity (groups) the energy change that occurs when an electron is added to a gaseous atom trend: decreases (in groups from top to bottom on the periodic table)
Electronegativity (groups) the ability of an atom in a molecule to attract shared electrons to itself trend: decreases (in groups from top to bottom on the periodic table)
Why does ionization energy increase or decrease (periods) increase because more energy is needed to move the electrons
Why does electron affinity increase or decrease (periods) increase because there is more attraction for an electron
Why does electronegativity increase or decrease (periods) increase because there is more attraction for a shared pair of electrons
Why does ionization energy increase or decrease (groups) decrease because less energy is needed to remove an electron
Why does electron affinity increase or decrease (groups) decrease because there is less attraction for an electron
Why does electronegativity increase or decrease (groups) decrease because there is less attraction for a shared pair of electrons
Created by: user-1804934
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