6.1 and 6.2 Review

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atomic radii down a grp

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Chem: Chapter 6.1 and 6.2 Review

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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)

<p>The radius of an atom .... (how big)</p>
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What is electronegativity

the tendency of an atom to attract an electron towards itself

<p>the tendency of an atom to attract an electron towards itself</p>
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What is ionization energy

the amount of energy required to remove an electron from an atom

<p>the amount of energy required to remove an electron from an atom</p>
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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)

<p>effective nuclear charge ( Zeff = Z-S .... z= # of protons .... s= # of core electrons)</p>
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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

<p>a reduction in effective nuclear charge (zeff), due to energy levels blocking the valence electrons from feeling the charge of the nucleus</p>
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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 🤯

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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