Transcript Periodic Table Flashcards

Periodic Table Flashcards
Group or Family
Column (up & down)
Period or Series
Row (across)
# of valence electrons
Elements in the same
column have the same …
# of principle energy levels
Elements in the same
row have the same …
the number of valence
electrons
Chemical properties are
determined by
one valence electron
Elements in column 1 (IA)
have
two valence electrons
Elements in column 2 (IIA)
have
Noble gases
The name of the family in
column 18 (VIIIA)
Halogens
The name of the family in
column 17 (VIIA)
H2, N2, O2, F2, Cl2, He, Ne,
Ar, Kr, Xe, & Rn
Elements that are gases at
room temperature
Hg (metal) & Br2 (nonmetal)
Elements that are liquids at
room temperature
Chemical properties
Elements in the same
column have similar
3 valence electrons
Elements in column 13
(IIIA) have
4 valence electrons
Elements in column 14 (IVA)
have
Half the diameter of an
atom, a measure of size
Atomic radius
Increases as you go down a
column (more principle energy
levels) & decreases across a row
(greater effective nuclear
charge)
Trends for atomic radius
Alkali Metals
Name of family for column 1
Alkaline Earth Metals
Name of family for column
2
Amount of energy required
to remove the most loosely
held valence electron from a
gas phase atom
Ionization Energy
X + energy  X+ + e-
Ionization
Decreases as you go down a
column, increases across a
row
Trends for Ionization
Energy
LOSERS
Metals are “_______”
Positive ions
Metals lose electrons to
form …
1) Malleable
2) Ductile
3) Good conductors of heat &
electricity
4) Lustrous
5) Low ionization energy
6) Low electronegativity
Properties of metals
1) Brittle
2) Dull
3) Poor conductors of heat &
electricity
4) High ionization energy
5) High electronegativity
Properties of nonmetals
winners
Nonmetals are “_______”
Negative ions
Nonmetals gain electrons to
form …
High ionization energies &
high electronegativies
Nonmetals have
low ionization energies & low
electronegativies
Metals have
Larger than the parent ion
Negative ions are
smaller than the parent ion
Positive ions are
On the staircase
Metalloids are located
To the left of the staircase
(except for H!)
Metals are located
To the right of the
staircase
Nonmetals are located
5 valence electrons
Elements in column 15 (VA)
have
6 valence electrons
Elements in column 16 (VIA)
have
Decreases across.
Increases down.
Trends for metallic
character
Cs & Fr
Most active metals?
Lose electrons
Metals are losers. Reactivity
of metals is judged by how
easily metals
In the lower left corner of
the periodic table.
Elements with strongest
metallic properties are
located
Atomic number
Periodic table is arranged by
Ability of an atom to
attract electrons in a bond.
Electronegativity
Fluorine
Most Electronegative
Element
Increases across &
decreases down.
Trends for electronegativity
Nonmetals are winners so we
judge the reactivity of
nonmetals by how easily they
gain electons.
How do we judge the
reactivity of Nonmetals?
Increases across and
decreases down.
Trends for nonmetallic
character
7 valence electrons
Elements in column 17 (VIIA)
have
8 valence electrons
Elements in column 18
(VIIIA) have
Transition metal ions
Form brightly colored salts
and solutions
(except Zn)
Hard solids
High MP
Multiple oxidation states
Ions have color
Properties of transition
metals (B Group elements)
Different forms of the
same element in the same
phase.
Allotropes
Have different structures so
they have different chemical
& physical properties.
Allotropes
O2 and O3
Allotropes of oxygen
Graphite, diamond, &
buckminsterfullerine (C60)
Allotropes of carbon
Use dots to represent
valence electrons.
Lewis Structures
•
Na
••
Al •
••
•
Br
•
• ••
••
• S•
••
••
Mg
Lewis Structures
The charge on an atom when
it has an octet in the
valence level.
Oxidation Number
Oxidation #’s
Group
1
2
13
14
15
16
17
18
Oxidation #
+1
+2
+1, +3
+2, +4
+3, +5, -3
Mostly -2
-1
0
M2O
General formula for a metal
from Group 1 + oxygen
MO
General formula for a metal
from Group 2 + oxygen
MX
General formula for a metal
from Group 1 + a halogen
MX2
General formula for a metal
from Group 2 + a halogen