6.1 and 6.2 Review

Chem: Chapter 6.1 and 6.2 Review

atomic radii down a grp

increases

Electronegativity down a grp

Decreases

Ionization energy down a grp

Decreases

Electron Affinity down a grp

Decreases

Zeff down a grp

Constant

Shielding down a grp

increases

atomic radii across a period

decreases

Electronegativity across a period

increases

Ionization energy across a period

increases

Electron affinity across a period

increases

Zeff across a period

Increases

Shielding across a period

constant

What is Atomic Radius

The radius of an atom .... (how big)

What is electronegativity

the tendency of an atom to attract an electron towards itself

What is ionization energy

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

What is electron affinity

the change in energy (kj) when an electron is added (the atom's likeliness of gaining an electron)

Zeff

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

Sheilding

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

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)

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)

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!!!!

Henry Moseley

Lived 1887 -1915

English Physicist who worked with Rutherford

Figured out the acc nuclear charge (atomic number) of elements

Periodic Law

States that when elements are arranged in order of increasing atomic number.... THERE IS A PATTERN !!!!

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

WHere are the metals

Generally to the left of the periodic table

Where are the metalloids

The diagonal line starting with Boron

WHere are the nonmetals

Generally to the right of the periodic table (+ hydrogen)

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

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

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

What are the properties of metalloids

- Have properties of metals and nonmetals
- Mostly brittle solids
- Intermediate conductors of electricity - AKA emiconductors

Properties of alkali metals

Extemely reactive (water, or air)
silvery appearance
soft
lower density
low melting points
not found freely in nature

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

Properties of halogens

Most reacitve nonmetals
react with most metals to form salts
most electronegative

properties of noble gases

least reactive because valence shell is compeltely filled

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

Properties of p block metals

Harder and more dense than s block
softer and less dense than d block