Transcript Periodic Law Review

Periodic Law Review
Chapter 5
• This man organized the periodic
table by increasing atomic mass.
Dmitri Mendeleev
• This man organized the periodic
table by increasing atomic
number.
Henry Moseley
• The definition of periodic law is…
Physical and chemical properties are periodic
functions of their atomic numbers.
• Periodic functions means….
A repeating trend because of..
• The name of the first family.
Alkali metals
• The name of the second family.
Alkaline Earth Metals
• The name of the 2nd to last family.
Halogens
• The name of the last family.
Noble Gases
• This family all ends in s2
Alkaline Earth Metals
• This family ends in p6
Noble Gases
• This family ends in s1
Alkali Metals
• This family ends in p5
Halogens
• These three families are highly
reactive.
Alkali metals, halogens, and
alkaline earth metals
• This family is relatively
unreactive.
Noble
gases
• This family gains 1e- when
bonding.
halogens
• This family loses 1 e- when
bonding.
Alkali
metals
• This family loses 2e- when
bonding.
Alkaline earth metals
• This family has a full s and p
orbital in the principal energy
level.
Noble gases
• The definition of
electronegativity…
The measure of the tendency of an atom to
gain an electron from another atom.
• The trend across a period….
Electronegativity increases.
• The trend down a family/group.
Electronegativity decrease or
remain the same.
• The definition of electron
affinity…
The energy change that occurs when an electron
is acquired by a neutral atom.
• The trend across a period….
Electron affinity become more negative in
the p block; becomes more positive going
from group 1 to group 2.
• The trend down a family/group.
The energies become less.
• The definition of ionization
energy…
The energy required to remove one electron
from a neutral atom of an element.
• The trend across a period….
Ionization energies of the main group
elements increase across a period.
• The trend down a family/group.
Ionization energies of the main group
generally decrease down a group.
• The definition of atomic radius…
The average distance between two
bonded atoms.
• The trend across a period….
Atomic radius decreases
across a group.
• The trend down a family/group.
Atomic radius increases down a
group.
• The definition of ionic radii…
The average distance between 2 bonded
atoms that are a cation or anion.
• The trend across a period….
Cationic radii decrease across a period.
Anionic radii decrease across each
period.
• The trend down a family/group.
Ionic radii (cationic and anionic)
increase down a group.
• The definition of valence
electrons…
The number of electrons found in the
outermost s and p orbitals. They are
available to gain, lose or share.
• The trend across a period….
Valence electrons increase by 1
in the main group.
• The trend down a family/group.
Valence electrons remain the same in
each family.
•H
Hydrogen
•V
Vanadium
•C
Carbon
•O
Oxygen
•S
Sulfur
•U
Uranium
•F
Fluorine
•I
Iodine
• Ne
Neon
• Br
Bromine
• Mg
Magnesium
• Ca
Calcium
• Pt
Platinum
• Ti
Titanium
• Sn
Tin
•W
Tungsten
• Au
Gold
• Hg
Mercury
• Rn
Radon
• Fr
Francium
• Ar
Argon
• Sc
Scandium
• Be
Beryllium
• Li
Lithium
• How many atoms are in 1 mol?
6.022 x 1023
• What is the above number
referred to as?
Avogadro’s number
• The number of protons is called?
Atomic
number
• The number of protons + neutrons is
called?
Mass
number
• Atoms of the same element which
differ in the number of neutrons are
called?
isotopes
• The average mass taking into account
the abundance of all of the isotopes of
that element is called?
Atomic mass (that’s why it is a
• How do you obtain the mass
number when all you are given on
the periodic table is atomic
number and atomic mass?
Rounding the atomic mass to the nearest
whole number will give you the mass
number of the most common isotope.
• The element [He] 2s2
Be
• The element [Kr] 5s1 Rb
• The electron configuration for K.
1s22s22p63s23p64s1
• The electron configuration for C.
1s22s22p2
• The electron configuration for Kr.
1s22s22p63s23p64s23d104p6
• The noble gas configuration for P.
[Ne]3s23p3
• The noble gas configuration for
As.
[Ar]4s23d104p3
• The noble gas configuration for
Ne.
[He]2s22p6
• Convert 4 .0mol O to atoms of O.
4.0 mol O x 6.022 x 1023 atoms =2.4 x 1024
1 mol O
• Convert 25.0 x 1023 atoms S to
mol S.
25.0 x 10 23 atoms S x 1 mol
=4.15 mol S
6.022 x 1023 atoms
• Convert 14.0 g Mg to mol Mg.
14.0 g Mg x 1 mol Mg = .576 mol Mg
24.30 g Mg
• Convert 14.0 g of O to mol O.
14.0 g O x 1 mol =.875 mol O
16.0 g O
• Convert 10.0 g of Au to atoms Au.
10.0 g Au x
6.022 x 1023 atoms Au =3.06 x 1022
196.97 g Au
• Convert 5.0 g S to atoms of S.
5.0 g S x 6.022 x 10 23 atoms S = 9.4 x 10 22 atoms S
32.065 g S