6.1 and 6.2 Review

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Chem: Chapter 6.1 and 6.2 Review

Last updated 11:16 PM on 12/1/22
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37 Terms

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atomic radii down a grp
increases
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Electronegativity down a grp
Decreases
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Ionization energy down a grp
Decreases
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Electron Affinity down a grp
Decreases
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Zeff down a grp
Constant
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Shielding down a grp
increases
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atomic radii across a period
decreases
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Electronegativity across a period
increases
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Ionization energy across a period
increases
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Electron affinity across a period
increases
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Zeff across a period
Increases
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Shielding across a period
constant
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What is Atomic Radius
The radius of an atom .... (how big)
The radius of an atom .... (how big)
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What is electronegativity
the tendency of an atom to attract an electron towards itself
the tendency of an atom to attract an electron towards itself
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What is ionization energy
the amount of energy required to remove an electron from an atom
the amount of energy required to remove an electron from an atom
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What is electron affinity
the change in energy (kj) when an electron is added (the atom's likeliness of gaining an electron)
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Zeff
effective nuclear charge ( Zeff = Z-S .... z= # of protons .... s= # of core electrons)
effective nuclear charge ( Zeff = Z-S .... z= # of protons .... s= # of core electrons)
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Sheilding
a reduction in effective nuclear charge (zeff), due to energy levels blocking the valence electrons from feeling the charge of the nucleus
a reduction in effective nuclear charge (zeff), due to energy levels blocking the valence electrons from feeling the charge of the nucleus
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Johann Doberereiner
Lived from : 1780 - 1849

1829; Classified elements into grps of 3 .... triads.

Each triad had similar chemical properties and orderly physical properties (Chlorine, Bromine and Iodine)
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John Newlands
Lived from 1838 -1898

1863; Suggested elements be arranged in "octaves"

He noticed that the properties repeat every 8 elements

(law of octaves)

Law of octaves failed past calcium

Ridiculed by chemical society XDDD (L Bozo)
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Mendeleev
Lived 1834-1907

Created the first periodic table

Arranged elements according to atomic mass, similarities and chemical properties

1871; he predicted the properties of elements that would fill up gaps in his table ..... in 1886 the three elements he predicted were found 馃く

remember ms tujauge screaming MENDELEEV!!!!
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Henry Moseley
Lived 1887 -1915

English Physicist who worked with Rutherford

Figured out the acc nuclear charge (atomic number) of elements
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Periodic Law
States that when elements are arranged in order of increasing atomic number.... THERE IS A PATTERN !!!!
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Glenn T. Seaborg (YEAAAAA)
1912-1999

Co-Discovered 10 new elements

1844; Moved 14 elements out of the main body of the periodic table and created the Actinide series (under the Lanthanides)

Had an element named after him while he was still alive
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WHere are the metals
Generally to the left of the periodic table
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Where are the metalloids
The diagonal line starting with Boron
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WHere are the nonmetals
Generally to the right of the periodic table (+ hydrogen)
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List the grp names left to right
- Alkali metals
- Alkaline earth metals
- Transition Metals
- Inner transition metals (Lanthanides top, and Actanides bottom)
- Main grp elements
- Halogens
- Noble gases
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What are the properties of metals
- Good heat and electricity conductors
- Usually solid at room temp
- Malleable
- Ductile
- SHiny Luster

Mercury is the only liquid metal
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What are the properties of nonmetals
- Poor heat and electricity conductors
- Can be solids, liquids or gases at room temp
- Solids are usually brittle and dull

bromine is the only nonmetallic element in liquid state
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What are the properties of metalloids
- Have properties of metals and nonmetals
- Mostly brittle solids
- Intermediate conductors of electricity - AKA emiconductors
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Properties of alkali metals
Extemely reactive (water, or air)
silvery appearance
soft
lower density
low melting points
not found freely in nature
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properties of alkaline earth metals
harder and stronger that alkali metals
high density, melting point than alkali metals
less reactive than alkali
not found freely in nature
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Properties of halogens
Most reacitve nonmetals
react with most metals to form salts
most electronegative
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properties of noble gases
least reactive because valence shell is compeltely filled
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properties of transition metals (d block)
high density
high melting point
good conductor of heat and electricity
high luster
less reactive than the alkali or alkaline metals
Birght colors
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Properties of p block metals
Harder and more dense than s block
softer and less dense than d block

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