CH 5 & 14 Notes.ppt

BELLWORK



Pick up graded papers and grade

report, if something is highlighted I

am missing it.



You have until Thursday to turn in

anything missing (end of the six weeks)



I have graded your test. I will pass

THE PERIODIC TABLE

MENDELEEV’S TABLE (~1872)



Arranged according to increasing

atomic mass



Elements with similar properties

placed in the same vertical column



Missing elements were yet to be

HENRY MOSELEY –

(1887-1915)



British Physicist

determined the

atomic numbers of

the elements



He arranged the

periodic table in

order of atomic

number



His periodic table is

PERIODS

–

PERIODIC LAW

–



When the elements are arranged in order

GROUPS

–

vertical

columns of

elements on

the Periodic

Table

REPRESENTATIVE ELEMENTS



Alkali Metals

– Group 1-A elements



Alkaline Earth Metals

– Group 2-A elements

Halogens

– Group 7-A elements

GROUP B ELEMENTS



Transition Metals

– In the middle of the

Periodic Table

Please label your periodic table with

the following:

 _{Color the families as follows:}

 _{Alkali metals – red}

 _{Alkaline earth metals – yellow}

 _{Halogens – green}

 _{Noble gases – blue}

 _{Please outline the representative elements in}

purple and the transition metals in orange.

 _{Make a key to your colors on the top of the}

CLASSIFICATION OF ELEMENTS

_{Metals – found on the left-side of the Periodic Table}

_{Nonmetals – found on the right-hand side of the Periodic Table} _{Metalloids (or semi-metals) – along the stair-step line}

 _{Metals are…}

 _{Malleable – can be}

hammered into sheets

 _{Ductile – can be drawn}

into wires

 _{Shiny or Lustrous}

 _{Good conductors/poor}

insulators of heat and electricity

 _{All solids at room}

temperature except Hg

 _{Non-metals are…}

 _{Brittle but often form}

crystals

 _Dull

 _{Good insulators/poor or}

non-conductors of heat and electricity

 _{Solids, liquids and gases}

at room temperature

 _Metalloids

 _{Have properties that are}

intermediate between metals and nonmetals.

Please label your periodic table with the metals,

nonmetals and metalloids. Add definitions of

14.1 – CLASSIFICATION OF THE

ELEMENTS

_{History of the Periodic Table (A Review)}

_{Mendeleev- arranged elements in order of increasing}

atomic mass

_{Moseley- arranged elements in order of increasing atomic}

number

_{Periodic Law- When the elements are arranged in}

Periodic Trends



The arrangement of the Periodic

Table also provides scientists with a

general idea of periodic trends. We

will now examine those trends. You

are responsible for the trends in

Effective Nuclear Charge (Z

)



The pull the nucleus exerts on the

electrons.



The larger the Z

, the tighter the

electrons are pulled and the smaller the

atom.



Trend: Z

is highest near the top right of

the periodic table



Write this trend on the appropriate

Question



Which elements in the

following pairs would have

the highest Z

?

14.2 –

PERIODIC

TRENDS

• _{Atomic radius – one-half the}

distance between the nuclei of two like atoms in a

diatomic molecule (ex: Cl₂)

• _{The more energy levels}

present, the larger the atom.

• _{When comparing atoms that}

all have similar energy

levels, the atoms with the largest nuclei (and thus

greatest number of protons) will have the smallest radii.

• _{Trend: atomic radius}

increases from right to left and from top to bottom.

• _{Write the trend in your}

Atomic Radius

Increasing Atomic Radius

Question



Place the following elements in

• Ionization energy - energy required to overcome

the attraction of the nuclear charge and remove on electron from a gaseous atom to form an ion.

• 1st ionization energy: the energy required to

remove the first electron

• 2nd ionization energy: the energy required to

remove the second electron

• 3rd ionization energy: the energy required

removing the second electron

• _{Trend: ionization energy increases from left to right}

and bottom to top.

• _{Please write this trend onto your flipbook.}

Question



What electron do you think

Ionization Energy

Increasing Ionization Energy

• _{Ion Size}

• _{Anions, or atoms that have gained electrons, are larger}

than the atoms from which they were formed.

• The negative charge means more electrons are

present causing the size of the ion to be larger.

• _{Cations, which are atoms that have lost electrons, are}

smaller than the atoms from which they were formed.

• _{The positive charge means fewer electrons are}

surrounding the nucleus, thus pulling the existing electrons closer and causing the ion to be smaller.

• _{Trend: ionic radius increases from right to left and from}

top to bottom.

• _{Please add this trend to your flipbook.}

Ionic Radius

Increasing Ionic Radius

Question



What is larger; an atom of

•

Electronegativity

– the tendency for the

atoms of the element to attract electrons

when they are chemically combined with

atoms of another element

•

Note: Nobel gases don’t have any

electronegativity because their orbitals are

filled so they don‘t bond with other elements.

•

Trend: electronegativity increases from left to

right and bottom to top.

•

Please add this trend to your flipbook.

Question



If hydrogen and fluorine made a