MAIN GROUP
(GROUPS 1, 2, AND 13 - 18) ELEMENTS NOTES
GROUP
|
NAME
|
ENDING
OF CONFIG.
|
# OF VALENCE e-
|
ELECTRON DOT DIAGRAM
|
WANTS TO (lose or
gain) TO BE LIKE NOBLE GAS?
|
CHARGE OF ION &
OXID-ATION #
|
ION (smaller or
larger) THAN ATOM
|
|
1 |
|
|
|
|
|
|
|
|
2 |
|
|
|
|
|
|
|
|
13 |
|
|
|
|
|
|
|
|
14 |
|
|
|
|
|
|
|
|
15 |
|
|
|
|
|
|
|
|
16 |
|
|
|
|
|
|
|
|
17 |
|
|
|
|
|
|
|
|
18 |
|
|
|
|
|
|
|
LOCATING
MAIN GROUP ELEMENTS ON THE PERIODIC TABLE NOTES
Given
the electron configuration or noble gas configuration for an element, it is
possible to determine its location on the Periodic Table without actually
looking at a Periodic Table.
* To tell which period this element is in...
~ find the
highest occupied energy level for this element
You can do this by...
~ finding the
largest coefficient number
The largest coefficient number is the number of the period where
the element is located.
* To tell which "block" this element is in... (like "s" block, "p" block, "d"
block, etc)
~ find the
highest occupied sublevel for this element
You can do this by...
~ finding the
last lowercase letter written
The last lowercase letter written in the configuration is the
"block" where the element is located.
* To tell which group this element is in...
~ find the highest
occupied energy level for this element
You can do this by...
~ finding the
largest coefficient number
Then...
~ add up the
exponents of the largest coefficient number
This gives you the number of valence electrons in the element.
You will then know that 1 valence e- indicates that the element
is in Group 1, 2 valence e- indicates that the element is in Group 2, 3 valence
e- indicates that the element is in Group 13, 4 valence e- indicates that the
element is in Group 14, 5 valence e- indicates that the element is in Group 15,
6 valence e- indicates that the element is in Group 16, 7 valence e- indicates
that the element is in Group 17, and 8 valence e- indicates that the element is
in Group 18.
Look
at the following example:
EXAMPLE:
[Ar] 4s2 3d10 4p5
It
is possible to tell the period, group, and "block" where this element
is located.
* Period -- largest
coefficient number is 4, so element is in Period 4
* Block-- last lowercase
letter written is "p", so element is in "p" block
* Group-- largest coefficient
number is 4... 2 electrons in 4s, 5 electrons in 4p --> total of 7 valence electrons,
so this element is in Group 17.
LOCATION
OF ELEMENTS WORKSHEET
|
|
Noble
Gas Config. |
Period |
Block
(s, p, d, f) |
Group |
|
1 |
[Ne]
3s2 3p2 |
|
|
|
|
2 |
[Ar] 4s2 3d10 4p6 |
|
|
|
|
3 |
[Xe] 6s2 |
|
|
|
|
4 |
[Kr]
5s2 4d10 5p5 |
|
|
|
|
5 |
[Ar] 4s2 3d10 4p1 |
|
|
|
|
6 |
[He]
2s2 2p3 |
|
|
|
|
7 |
[Kr]
5s2 4d10 5p4 |
|
|
|
|
8 |
[He]
2s1 |
|
|
|
|
9 |
[Xe] 6s2 4f14 5d10 6p2 |
|
|
|
|
10 |
[Rn] 7s2 |
|
|
|
HISTORY
OF THE PERIODIC TABLE NOTES
I.
Mendeleev and Chemical Periodicity
A. Wanted to organize elements according to their ____________________
B. When elements were arranged in order of increasing atomic mass*,
similarities in chemical
properties appeared at regular intervals
(____________________)
C. *Several elements did not quite fit this
pattern - Mendeleev put elements with similar
____________________ in the same column or group
D. 1871 - Mendeleev predicted the existence and
properties of several (then undiscovered)
elements. These elements were:
E. Within 15 years, those elements with those properties had been
discovered
II. Moseley and the Periodic Law
A. When elements were arranged in order of increasing
___________________________________,
there was a distinct regular pattern.
B. ____________________: The physical and
chemical properties of the elements are periodic
functions of their atomic numbers.
C. In other words, when elements are arranged in order of increasing
atomic number, elements
with similar properties appear at regular intervals.
D. Bottom line = elements in the same group have similar properties
III. Modern Periodic Table: arrangement of the
elements in order of their atomic numbers so that elements with
similar properties fall in the same group
ELECTRON CONFIGURATION & THE PERIODIC
TABLE NOTES
I. Stability of
Noble Gases
A. Noble gases undergo very few chemical reactions - why?
B. Highest occupied energy level contains ________________________________________
C. Electrons in the highest occupied energy level are what determines an element's _____________
II. Periods and Blocks of the Periodic Table
A. Horizontal row = ____________________; 7
on modern Periodic Table
B. Length of period determined by the sublevels being filled in that
period
C. Period 1: only _____ sublevel being filled;
can hold a maximum of _____ electrons;
period contains _____ elements
D. Period 4: ____, ____, and ____ sublevels being filled; s can hold ___ electrons, d can hold ___
electrons, & p can hold ___ electrons; total of
_____ electrons;
Period 4 contains _____ elements
E. Period can be determined from the element's electron configuration
1. Bromine: [Ar] 4s2 3d10
4p5
2. Highest number in front of letter is the element's highest occupied
_____________________ -
tells which period the element is in
3. For bromine, _____ is highest number, so it is in Period _____
III. The "s" block elements:
Groups 1 and 2
A. Group 1 - Alkali Metals
1. generalized outermost energy level (valence) electron configuration:
2. silvery appearance
3. soft enough to cut with a knife
4. not found in nature as free elements -
they're always part of a compound
B. Group 2 - Alkaline Earth Metals
1. generalized valence electron configuration:
2. harder, stronger, more dense than Group 1
3. also have higher melting points than Group 1
4. less reactive than Group 1, but still not
found in nature as free elements
C. Exceptions: Hydrogen and Helium
1. Hydrogen (H)
a. electron configuration:
b. properties do not resemble those of any other
element on the periodic table
2. Helium (He)
a. electron configuration:
b. in Group 18 because
IV. The "d" block elements: Groups 3 -
12
A. called
B. have typical metallic properties: ductile,
malleable, shiny, solid, conduct electricity
C. less reactive than "s" block
elements
D. found in nature as free elements
E. usual ending of electron configuration:
V. The "p" block
elements: Groups 13 - 18
A. "s" and "p" block elements
together referred to as _____________________________ elements
B. ending electron configurations of
__________________ through ___________________
C. properties vary greatly b/c there are metals,
metalloids, and nonmetals
D. Group 17 - Halogens
1. most reactive nonmetals
2. seven electrons in outermost energy level
E. "p" block metals are harder and
more dense than "s" block , but not as hard or dense as the
"d"
block metals
PERIODIC TRENDS NOTES
Electronegativity/Electron
Affinity (EN/EA):
measure of how much an atom wants to gain an electron
EN/EA Left to Right across a Period:
INCREASES (not including Noble Gases)
Why?
*
Elements on the left side of the P.T. (metals) want to lose electrons. Elements on the right side of the P.T.
(nonmetals) want to
gain electrons. Trend does not include Noble Gases because
these elements do not want to
lose or gain electrons.
EN/EA
Top to Bottom in a Group:
DECREASES
Why?
*
This
interference (and resulting decreased hold) is referred to as the SHIELDING
EFFECT.
Ionization Energy (IE): amount of energy required to remove
an atoms most loosely held electron
IE
Left to Right across a Period:
INCREASES
Why?
*
Elements on the left side of the P.T. (metals) want to lose electrons.
Therefore, it will not require
much energy to remove an electron. Elements on the right side of the P.T.
(nonmetals) want to gain
electrons. Consequently, a lot of energy will be needed to remove (take
away) an electron.
IE Top to
Bottom in a Group:
DECREASES
Why?
*
Atomic Radius (AR): distance from the nucleus to the H.O.E.L.
AR Left to Right across a Period: DECREASES
Why?
*
AR Top to Bottom in a Group: INCREASES
Why?
*
There are more occupied energy levels as you move towards the bottom of the
P.T.
Metallic Character: how easily an atom will lose valence electrons
(easier to lose = more metallic = more reactive METAL)
Which metal loses its valence electron(s) most easily? Fr
Why?
*
Francium has one valence electron. It is more reactive than elements at
the top of Group 1 because there are many inner shell electrons that decrease
the attraction the nucleus has for the valence electrons.
Nonmetallic Character: how easily an atom will gain
electrons (easier to gain = more nonmetallic = more reactive NONMETAL)
Which nonmetal gains electron(s) most easily?
F
Why?
*
Fluorine has seven valence electrons. It is more reactive than elements
at the bottom of Group 17 because there are only a few inner shell
electrons. Consequently, the nucleus has a strong attraction for other
electrons.
PERIODIC
TRENDS (multiple choice w/o using Periodic Table)
WORKSHEET
1.)
Which element is most
metallic?
(A) Group 14, Period 2 (B)
Group 14, Period 3
(C) Group 14, Period 4 (D)
Group 14, Period 5
2.)
Which element is most
nonmetallic?
(A) Group 16, Period 2 (B)
Group 16, Period 3
(C) Group 16, Period 4 (D)
Group 16, Period 5
3.)
Which has the largest atomic
radius?
(A) Group 1, Period 2 (B)
Group 13, Period 2
(C) Group 15, Period 2 (D) Group 17, Period 2
4.)
Which has the highest ionization
energy?
(A) Group 2, Period 3 (B)
Group 2, Period 4
(C) Group 2, Period
5 (D) Group 2, Period 6
5.)
Which has the most metallic
properties?
(A) Group 13, Period 5 (B)
Group 14, Period 5
(C) Group 15, Period 5 (D)
Group 16, Period 5
6.)
Which has the greatest electron
affinity?
(A) Group 16, Period 4 (B)
Group 16, Period 5
(C) Group 17, Period 5 (D)
Group 17, Period 4
7.)
Which has the smallest atomic radius?
(A) Group 15, Period 2 (B)
Group 15, Period 3
(C) Group 15, Period 4 (D)
Group 15, Period 5
8.)
Which has the lowest electron
affinity?
(A) Group 13, Period 3 (B)
Group 15, Period 3
(C) Group 17, Period 3 (D)
Group 18, Period 3
9.)
Which has the lowest ionization
energy?
(A) Group 1, Period 2 (B)
Group 1, Period 3
(C) Group 1, Period 4 (D)
Group 1, Period 5
10.)
Which has the most metallic properties?
(A) Group 15, Period 5 (B)
Group 16, Period 5
(C) Group 15, Period 6 (D)
Group 16, Period 6
11.)
Which would most easily lose its valence
electrons?
(A) Group 1, Period 3 (B)
Group 14, Period 2
(C) Group 17, Period 3 (D)
Group 18, Period 2
12.)
Which would most easily gain
electrons?
(A) Group 13, Period 3 (B)
Group 14, Period 2
(C) Group 15, Period 2 (D)
Group 17, Period 3
13.)
Which has an octet of electrons in its outermost energy
level?
(A) Group 13, Period 3 (B)
Group 14, Period 2
(C) Group 18, Period 2 (D)
Group 17 , Period 5
14.)
Which has chemical properties most similar to [Ar] 4s1?
(A) Group 1, Period 3 (B)
Group 2, Period 3
(C) Group 13, Period 3 (D)
Group 14, Period 3
15.)
Which is most
reactive?
(A) Group 14, Period 2 (B)
Group 17, Period 2
(C) Group 15, Period 2 (D) Group 18, Period 2
16.)
Which is most
reactive?
(A) Group 13, Period 2 (B) Group 1, Period
5
(C) Group 2, Period 5 (D) Group 13, Period 5
17.)
Which has chemical properties most similar to [Ne] 3s2 3p5?
(A) Group 16, Period 3 (B) Group 18, Period
3
(C) Group 17, Period 4 (D) Group 18, Period
2
18.)
Which would never be found in the free state?
(A) Group 1, Period 4 (B) Group 13, Period
3
(C) Group 15, Period 3 (D) Group 14, Period 4
19.)
Which is the least reactive
gas?
(A) Group 16, Period
2 (B) Group 15, Period
2
(C) Group 17, Period 2 (D) Group 18, Period 2
20.)
Which is the most reactive
gas?
(A) Group 16, Period 2 (B) Group 15, Period
2
(C) Group 17, Period 2 (D)
Group 18, Period 2
21.)
Which would never be in a
compound?
(A) Group 1, Period 1 (B) Group 18, Period
1
(C) Group 13, Period 2 (D)
Group 1, Period 2
22.)
Which would be found in the d block of elements?
(A) Group 1, Period 3 (B)
Group 11, Period 4
(C) Group 17, Period
5 (D) Group 14, Period 2
1.)
Color the s block area pink.
2.)
Color the p block area yellow.
3.)
Color the d block area light green.
4.)
Color the f block area orange.
5.)
Draw an X in the boxes that represent the unreactive
elements
6.)
Draw a diagonal line (from upper left to lower right) in the area that
represents the very reactive nonmetals.
7.)
Draw a diagonal line (from upper right to lower left) in the area that
represents the very reactive metals.
8.)
Draw a purple capital letter R with a circle around it at the location that
represents the element with the largest
atomic radius.
9.)
Draw a blue capital letter I with a diamond around it at the location that
represents the element with the
highest ionization energy.
10.)
Draw a dark green capital letter E with a triangle around it at the location
that represents the element with
the highest electronegativity/electron
affinity.
11.)
Outline in black the boxes where metalloids with more nonmetallic properties
are located.
12.)
Outline in red the boxes where metalloids with more metallic properties are located.
13.)
Draw a star in the location that represents the most metallic element (or most
reactive metal).
14.)
Draw a heart in the location that represents the most nonmetallic element (or
most reactive nonmetal).
**Doing
this correctly will aid you in studying for your Unit 5 test. This
summarizes the bulk of the information covered. REMINDER: You will
not have a Periodic Table to use during your Unit 5 test.**