Transcript S block
Honors Chemistry
Chapter 5
J.W. Dӧbereiner
grouped elements
with similar
chemical
properties in
triads.
J.A.R. Newlands
arranged elements by
increasing atomic mass.
“Law of Octaves” from
similar properties repeating
every 8 elements.
Dmitri Mendeleev
produced the first
periodic table
predicted properties
and locations of
unknown elements
H.G.J. Moseley
able to determine
atomic numbers
arranged periodic table
by atomic number instead
of atomic mass
Periodic Law
When elements are
arranged in order of
increasing atomic
number, periodic patterns
exist in their properties.
Periodic Table
s1 s2 f1f2f3f4f5f6f7f8f9f10f11f12f13f14 d1d2d3d4d5d6d7d8d9d10 p1p2p3p4p5p6
Periods
the horizontal
rows on the
periodic table
Groups (Families)
the vertical
columns on the
periodic table
Group Names and #s
Alkali metals: #1 (1A)
Alkaline earth metals: #2
(2A)
Halogens: #17 (7A)
Noble Gas: #18 (8A)
Noble Gases
contain 8 electrons in
the valence shell
this is the most stable
type of atom due to its full
valence shell
Lanthanides
elements 57-71
“rare earth” elements
Actinides:
elements 89-103
all are radioactive
Do you know:
Mendeleev?
st
1 periodic table;
predicted properties &
locations of unknown
elements.
Moseley?
Atomic # instead of mass
Valence Shell
the outermost
principal energy level
(shell) that contains at
least one electron.
Valence Electrons
Electrons in the valence
shell
Valence electrons are
the most reactive
electrons in the atom.
S block
First two groups of the
periodic table. Last
electrons are in the s –
subshell.
P block
Last six groups of the
periodic table. Last
electrons are in the psubshell.
D-block Elements
F block
The Diagonal Rule
1s2
2
2s
3s2
2
4s
5s2
6s2
7s2
6
2p
3p6 3d10
6
10
4p 4d
5p6 5d10
6p6 6d10
7p6 7d10
14
4f
5f14
6f14
7f14
Write the electron
configuration of
Pb(#82)
[Xe]
2
6s
14
4f
10
5d
2
6p
Orbital Blocks
Representative
Elements: s + p
Transition Elements: d
Inner Transition
Elements: f
metals: left 2/3 of table
nonmetals: upper right side
of table
semimetals: “stairstep”
between metals & nonmetals
Metal Properties
have luster / shine
good conductors
usually exist as solids
malleable
ductile
H: Nonmetal Properties
no luster
poor conductors of
heat & electricity
not malleable
not ductile
Semimetals
(Metalloids)
properties are between
those of metals and
nonmetals
6 (to 8) semimetals
(Po & At classifications
vary)
S-block elements:
highly reactive
valence electrons easily
removed, forming ions
exist as compounds
Alkali metals
extremely reactive
soft
one valence
electron
Alkaline earth metals
reactive, but
not as highly
as alkali
metals
Brainiac Alkali metals
Strontium
P-block
representative elements
diverse properties
metals, semimetals and
nonmetals
reactive halogens
& unreactive noble gases
Carbon:
graphite
diamond
Allotropes
Forms of an element
differing in crystal
structure or bonding.
Review #1:
What group ends
with:
4
p
gp.16
1
gp.1
s
1
gp.3
d
1
gp.13
p
Review #2:
Where would an
element that is
unreactive be located
on the periodic table?
Noble gas: gp. 18
Write the electron
configuration of
Bi(#83)
[Xe]
2
6s
14
4f
10
5d
3
6p
Periodic Trends
Many properties of
elements change in a
predictable way as you
move through the
periodic table.
Atomic Radius
distance from center
to outermost electron
increases going down
a group.
decreases going right
across a period.
Atomic Radius
Which has the
largest radius?
C, Ne, Be, Li
Li
Which is the
largest atom?
Al, Si, C
Al
Ionic Size
atom gets larger
when it gains
electrons
atom gets smaller
when it loses
electrons
Atoms & Ions
Ionization Energy
energy needed to
remove the
outermost electron
Low ionization
energy means it is
easy to remove
Find the following
for Na, Mg, & Ca:
•Largest element Ca
•Highest ionization
energy Mg
Find the following
for P, S, & Se:
Largest element Se
Highest ionization
energy S
Octet Rule
atoms tend to gain
or lose electrons in
order to acquire a
full set of 8 valence
electrons.
Electron Affinity
attraction of an
atom for an
additional electron
Electronegativity
ability of a bonded
atom to attract
shared electrons to
itself.
D-block Elements
Alloy
A homogeneous
solid mixture of
metals
bronze
brass
pewter
d-block
transition elements
less reactive than s-block
many mix to form alloys
Uses: coins, wiring, living
organisms
d-block
high densities
high melting points
strong materials
f-block
inner transition elements
4f = lanthanide series
5f = actinide series
lanthanides: form +3 ions
actinides: radioactive
Review #1:
What group ends
with:
4
p
gp.16
1
gp.1
s
1
gp.3
d
1
gp.13
p
Review #2:
Where would an
element that is
unreactive be located
on the periodic table?
Noble gas: gp. 18
Review #3
Which is larger?
Mg, Sr Sr
Sr, Sn Sr
Ge, Sn Sn
Ge, Br Ge
Cr, W W
Which has
the larger atomic radius?
2+
Mg, Mg Mg
22S
S, S
2+
2+
2+
Ca , Ba Ba
I
Cl , I
+
+
3+
Na
Na , Al
Review #4
Review #5 Which has a
larger ionization energy?
Mg, Na Mg Cl, I Cl
S, O O Na, Al Al
Ca, Ba Ca Se, Br Br
Review #6
What element has
the greatest
electronegativity?
F: fluorine
Review #7
What element has
the largest atoms?
Fr: francium
Review #8
What group do alkali
metals tend to react
with?
Group 17: halogens
Review #9
What is the most
reactive metal on the
periodic table?
Francium
Review #10
What is the most
reactive nonmetal on
the periodic table?
Fluorine
Review #11
Identify the halogens,
alkaline earth metals,
representative elements,
& transition metals:
Sr Alk.earth & repres.
Cr transition
I
halogen & repres.
Review #12
How many valence
electrons are in:
Mg
two
Se
six
Sn
four