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