Download Unit 4 Periodic Table Packet 2016-2017

Honors Chemistry
Unit 4
(2016-2017)
 Families (research and present)
 Metals/nonmetals
 Trends
o Atomic radius
o Electronegativity
o Ionization energy
o Metallic and nonmetallic character
 Review Ions
 Oxidation #’s
1
We are learning to:
1.
2.
3.
Describe the history/arrangement of the periodic table.
Describe periodicity as a result of electron configurations.
Give the name and formula with charge for the polyatomic ions.
We are looking for:
1a. Doberiener arranged the elements into triads.
1b. Newlands arranged the elements by the law of octaves.
1c. Mendeleev arranged the elements by atomic mass (periodic law).
1d. Moseley arranged the elements by atomic number (modern periodic law).
1e. Identify and describe the unique properties of the families on the periodic table (alkali metals, alkaline earth metals, transition metals,
inner transition metals, post transition/other metals, metalloids, halogens, noble gases, other nonmetals, hydrogen).
2a. Identify the number of valence electrons using the periodic table or given an electron configuration.
2b. Describe the periodic trends (metallic character, electronegativity, ionization energy, atomic radius, ionic radius).
3a. Given the name of a polyatomic ion, write the corresponding formula and charge.
3b. Given the formula and charge of a polyatomic ion, write the corresponding name.
Periodic Table History
~____________B.C.: _______________________

_______elements: ______________, ______________, __________,___________
By _________, ________ elements were known.
~_________: _________________________________

Wrote the first extensive list of _________ elements.
__________: ______________________________(German Chemist)


Noticed that _____, ______, and _______ had similar properties and that Br’s atomic
mass was between that of Cl & I.
He found three other groups with similarities and he called these
groups____________________________.
2
________: __________________________________ (English Chemist)



Arranged the now known 62 elements from ________________ to _____________.
He noticed that every _______ element had ___________________ chemical and
physical properties; their properties were repeating.
This became known as __________________________________________________
o Li
Be
B
C
N
O
F
o Na
Mg
Al
Si
P
S
Cl
________: _____________________________________ (Russian Chemist)






Organized the elements by atomic __________ also but also made it into ____________
form to help his students.
Elements with __________________ properties were put into the same
__________________.
Original Periodic Law : the properties of the elements are a function of their atomic
masses.
Considered the ______________________ of the modern periodic table.
He left _______________ where elements seemed to be _________________.
There were places where ________________ elements were put before
_______________ elements because of their _________________________:
o Te-I
Co-Ni
_______-_________
(He felt the mistake was in measuring the mass and this would be corrected with further research.)
________: ____________________________________ (English Chemist)


Arranged elements by atomic __________________.
Gave rise to the new Periodic Law, “Properties of the elements are a periodic function
of their ___________________________.”
1912-1999: Glenn ____________________________


Discovered ____ new elements.
Only living person for whom an element was named.
 _________ elements have been identified (naturally and artificially).
o _________elements occur naturally on Earth.
 Examples: gold, aluminum, lead, oxygen, carbon
o ________ elements have been created by scientists.
 Examples: technetium, americium, seaborgium
3
Periodic Table Terminology


___________________/Series =
__________________/Family =
Metals



Located to the ______________ of the staircase line.
Characteristics:
o _________________________ to form positive (+) ions (cations)
o
o
o
o
o React with ________________
Most metallic element (most reactive metal) = __________________________
Nonmetals



Located to the _________________ of the staircase line.
Characteristics:
o Tend to __________________________ to form negative (-) ions (anions)
o
o
o
Most nonmetallic element (most reactive nonmetal) = _________________________
Metalloids (Semimetals)


Located ______________and _____________ of the staircase line, except ______, _______,
and _________.
Characteristics:
o
o
o
o
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Element
Directions: (_____ is our assigned element) Due Date:_________
You need an unopened
following:
On one side:
. Decorate it with the
-assigned element symbol
-element name
- atomic # (above the symbol)
-average atomic mass (below the symbol)
Another side:
-who discovered & when
-where did the element name come from?
-picture of the element.
-at least 3 uses for the element & pictures of uses.
Another side:
-3 physical properties
-3 chemical properties
-orbital notation
-electron configuration
-Nuclear symbol for the most common isotope of the element
If you can’t fit all the information for a side on that side, it can be placed on the another
side.
You will be presenting your creation to the class on the due date.
5
Families on the Periodic Table
6
Family Name
List Elements
(Solid/Liquid/Gas)
(Metal/Metalloid/Nonmetal)
Characteristics
Hydrogen
Alkali Metals
Alkaline Earth
Metals
Transition Metals
Other Metals
(Post transition)
Metalloids
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Family Name
List Elements
(Solid/Liquid/Gas)
(Metal/Metalloid/Nonmetal)
Characteristics
Other Non metals
Halogens
Noble Gases
Lanthanoids
(Inner transition metals)
Actinoids
(Inner transition metals)
New Elements
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Oxidation Numbers:
The charge an atom acquires by gaining or losing electrons.
Label your periodic table with oxidation numbers as instructed by your teacher.
Isoelectronic Configurations
 Elements with similar electronic configurations tend to have similar chemical and physical
properties.
 It is possible for elemental ions to have exactly the same electronic configuration as other
elements or ions.
 When two elements and/or ions have the same electronic configuration it is said that
they are "isoelectronic" with one another.
 When two chemical species are isolectronic they again tend to have similar chemical
properties.
Examples of Isoelectronic Elements and/or Ions
Element or ion pair
Electronic configuration
Li+, He
1s2
Be2+, He
1s2
F-, Ne
1s2 2s2 2p6
S2-, Ar
1s2 2s2 2s6 3s2 3p6
Mg2+, Na+
1s2 2s2 2p6
Ca+, K
[Ne]4s1
P3-, S2-
1s2 2s2 2p6 3s2 3p6
Which of the atoms/ions are isoelectronic with each other?
C,
Cl- ,
Mn2+ ,
B- ,
Ar , Zn , Fe3+ , Ge2+
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10
Properties of Metals, Nonmetals, & Metalloids
Define the following terms/physical properties & determine how you can test a sample for this property.
1) Malleability
2) Luster
3) Conductivity
4) For reactivity with acid, how will you determine if a chemical reaction has occurred?
Purpose: To classify unknown samples as metal, nonmetal, or metalloid based on the observed
characteristics.
Use the procedures you described above to test each physical property of the samples. To test the
chemical property (reaction w/ acid) place a small piece of the sample into a test tube and then add 5-10
drops of acid. Record your observations in the table on the back.
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Properties of Metals, Nonmetals, & Metalloids Table
Sample #
Color
Luster
(lustrous)
Malleability Conductivity Reaction
(malleable)
w/ acid
Classification
See your notes for the basic properties of metals, nonmetals, and metalloids. Then classify each of your
samples as a metal, nonmetal, or metalloid.
Metals
Nonmetals
Metalloids
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Periodic Trends
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"Periodic Table Properties (Trends)”
Atomic Radius
Definition:
Left to right across a period radius gets ___________________
Why?
1.
2.
Electron – electron ________________________
Makes radius larger
Very weak interactions
Proton – electron _________________________
Makes radius smaller
Very strong interactions (proton to electron attraction
is a million times stronger than electron to electron
repulsion)
Down a group/family radius gets ________________________
Why?
Energy level, n, ______________________ from top to bottom
Radius gets larger by adding electrons to higher (farther away) energy levels.
Think Bohr model (adding rings)
Ionization Energy
The energy required to ___________________ one electron from a neutral atom.
Electronegativity
The ability of an atom to _______________ electrons.
Most electronegative element is F (fluorine).
It is assigned the number 4.
All other values are based on this value.
Electron Affinity
The energy change that occurs when a neutral atom ___________________ an electron.
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Ionic Radius:
# of protons
Na+
Mg2+
Al3+
P3-
S2-
Cl-
N3-
O2-
F-
11
12
13
15
16
17
7
8
9
electronic
structure of
ion
2,8
2,8
2,8
2,8,8
2,8,8
2,8,8
2, 8
2, 8
2, 8
ionic radius
(nm)
0.102
0.072
0.054
(0.212)
0.184
0.181
(0.171)
0.140
0.133
.
Cations
Anions
The Anion radius is ________________ compared to the atom; Why?
The Cation radius is ________________ compared to the atom; Why?
When comparing ions of different elements, determine how many electrons each ion has
and how many protons each ion has. If the electrons are the same, the one with more
protons will have the smaller radius. Why?
Which has a smaller atomic radius? K+ or Cl15
Summary of Periodic Table Trends
Top to Bottom
Left to Right
Atomic Radii
Ionization
Energy
Electron Affinity
Electronegativity
Metallic Character
1.
_______________ ionization energy (easy to remove electrons)
2.
_______________ electronegativities (don’t attract electrons)
3.
_______________ Luster – shiny
4.
_______________ conductor of electricity and heat
5.
_______________ and ductile
Most metallic element = _______________________
NonMetallic Character
1. ______________ ionization energy (hard to remove electrons)
2. ______________ electronegativities (attract electrons)
3. ______________ or no metallic luster
4. ______________ electrical and thermal conductors
5. ______________ solids
Most nonmetallic element = _____________________
Metalloid Character
1.
Characteristics of both metals and nonmetals.
2.
_______________________ between those of metals and nonmetals.
3.
_______________________ energies between those of metals and nonmetals.
4.
Boiling pts, Melting pts and _________________ vary widely.
Example: Silicon –
high luster, brittle, good conductor
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Periodicity Review Worksheet
1. Which atom in the following pairs would have the larger atomic radii?
P or Cl
K or Mg
As or Se
Si or O
P or Ge
Sn or Pb
Cl or Br
Ca or Al
Mg or Ca
Sn or As
Si or S
H or He
Na or Mg
Al or Cl
Sr or Ra
2. Which ion in the following pairs would have the larger radii?
Li+ or Be2+
Cr3+ or Cr6+
S2- or O2-
Mg2+ or Be2+
Na+ or Al3+
I- or Cl-
Cs+ or Be2+
Zn2+ or Fe2+
P3- or S2-
Cu+ or Cu2+
N3- or FBr- or S2-
3. Which member of the following pairs would have a larger radii?
Br or BrCa or Ca2+
S or S6+
Al or Al3+
O or O2Li or Li+
P or P3N3- or Al3+
4. Which atom in the following pairs would have the greater first ionization energy?
Sr or Ba
Cs or Ba
Cl or Ar
In or Sn
Xe or Kr
Mg or Sr
Ca or Cu
5. What is the difference between electron affinity and ionization energy?
6. Which member in the following pairs would have the greater electron affinity & electronegativity?
F or Cl
S or O
F or O
N or O
F or Any element
Nonmetal or Metal
S or Cl
C or S
Ca or K
Mg or Na
Ca or F
Na or K
Al or Si
7. What is the difference between a cation and an anion?
8. Identify three anions in Period 2 that can have the same number of electrons when they become
ions. Do they gain or lose electrons?
9. Identify three cations in Period 3 that can have the same number of electrons when they become
ions. Do they gain or lose electrons?
10. Identify the ions that are most likely to have an ion charge (oxidation state) of -2? (Hint: there
are five of them)
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11. Identify the ions that are most likely to have an ion charge (oxidation state) of +2? (Hint: there
are six of them)
12. Why do elements in the same family generally have similar properties?
13. Which element has the greatest electron affinity? Why?
14. Which element has the lowest ionization energy? Why?
15. Consider all elements in period 3 for the following (Na through Ar)
____ has the largest atomic radius
____ has the greatest electron affinity
____ has the highest first ionization energy
____ is the most reactive metal
____ is the most reactive non metal
____ is the least reactive
___________ are metalloids
___________ are most likely to be cations
___________ are most likely to be anions
_____ loses 3 electrons to have noble gas configuration
_____ gains 3 electrons to have noble gas configuration
16. Consider all elements in group 16 (O through Po)
____ is the least reactive
____ is the most reactive
____ has the greatest electron affinity
____ has the greatest first ionization energy
____ has the smallest atomic radius
17. In a given period, are cations larger or are anions bigger?
18. Is the radius of a cation larger or smaller than the neutral atom? Why?
19. Is the radius of an anion larger or smaller than the neutral atom? Why?
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Name ___________________________________
Honors Chemistry Practice Quiz
“The Periodic Law”: "Trends"
Answer the following problems by placing the correct letter next to the problem number.
For problems 1-5 indicate with answer "a" the element you would predict with the highest ionization energy. Continue
ranking the elements down to the lowest.
a. highest b. second highest c. third highest d. second lowest e. lowest
1. 37 - Rubidium
4. 39 - Yttrium
2. 55 - Cesium
5. 87 - Francium
3. 50 - Tin
For problems 6-10 indicate with answer "a" the element you would predict with the largest atomic radius. Continue
ranking the elements down to the smallest.
a. largest b. second largest c. third largest d. second smallest e. smallest
6. 73 - Tantalum
9. 84 - Polonium
7. 12 - Magnesium
10. 16 - Sulfur
8. 80 - Mercury
For problems 11-15 indicate with answer "a" the element you would predict with the highest electronegativity. Continue
ranking the elements down to the lowest.
a. highest b. second highest c. third highest d. second lowest e. lowest
11. 55 - Cesium
14. 87 - Francium
12. 9 - Fluorine
15. 7 - Nitrogen
13. 8 - Oxygen
For problems 16-20 indicate with answer "a" the element you would predict with the highest reactivity. Continue ranking
the elements down to the lowest.
a. highest b. second highest c. third highest d. second lowest e. lowest
16. 37 - Rubidium
19. 39 - Yttrium
17. 55 - Cesium
20. 87 - Francium
18. 50 - Tin
For problems 21-25 indicate with answer "a" the element you would predict with the metallic characteristics. Continue
ranking the elements down to the lowest.
a. highest b. second highest c. third highest d. second lowest e. lowest
21. 11 - Sodium
24. 20- Calcium
22. 18 - Argon
25. 30 - Zinc
23. 81 - Thallium
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Name ________________________________________
Class Period _______________
Ion Practice
1. An isotope has 106 proton, 157 neutrons, and 106 electrons:
a. Write the nuclear symbol for this isotope _________________
b. What is the name of this element? ___________________
c. Is this an atom or an ion? ______________________
d. What is the mass number of this isotope ________________
e. What is the atomic number? __________________
f. What is the net charge? _______________________
2. An isotope has 29 protons, 34 neutrons, and 28 electrons:
a. Write the hyphen notation for this isotope ______________________
b. What is the name of this element? ___________________
c. Is this an atom or an ion? ______________________
d. What is the mass number of this isotope ________________
e. What is the atomic number? __________________
f. What is the net charge? _______________________
3.
a. The species 104Rh3+ has _____protons, _____neutrons and _____electrons
b. The species 12C has _____protons, _____neutrons and _____electrons
c. The species 130Te-2 has _____protons, ____neutrons and ____electrons
4.
5.
Which element will produce an ion with 15 protons, 16 neutrons and 18 electrons?
_______________.
Which element will produce an ion with 20 protons, 20 neutrons and 18 electrons?
_______________.
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6.
a.
A Calcium atom will (lose or gain) _____ electrons. How many? _______
Is the calcium atom bigger or smaller than the calcium ion? ___________
b. A Francium atom will (lose or gain) ______electrons. How many? ______
Is the francium atom bigger or smaller than the francium ion? ___________
c. A Fluorine atom will (lose or gain) _______ electrons. How many?______
Is the fluorine atom bigger or smaller than the fluorine ion? ___________
d. A Oxygen atom will (lose or gain) ______ electrons. How many? _______
Is the oxygen atom bigger or smaller than the oxygen ion? ___________
e. A Carbon atom will (lose or gain) _______electrons. How many? ______
Is the carbon atom bigger or smaller than the carbon ion? ___________
7. Considering a 26Mg atom and and a 26Mg2+ ion, label the following true or false:
_____ They both have the same number of protons
_____ They both have the same number of electrons
_____ They both have the same number of neutrons
_____ The magnesium ion has 14 electrons and the magnesium atom as 10 electrons
_____ The net charge on the magnesium ion is 2+
_____ The Bohr model of the magnesium ion has 0 electrons in the outer most shell.
_____ The Mg2+ ion is larger than the Mg atom.
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Martian PT
Name ___________________________________
Honors Chemistry Worksheet
"Trends"
"Periodic Chart For Mars And Its 33 Known Elements"
Place the following elements in their proper place in the Martian periodic table. Remember, natural laws are the same for
the whole universe. Note that Mars has no transition metals.
a, b, c, d, e, f, g, h, i, j, k, l, m, n, o, p, q, r, s, t, u, v, w, x, y, z, !, #, $, %, +, =, ?
undiscovered
1. The most reactive metallic element is x.
2. The most reactive nonmetallic element is !.
3. Inert gases (like our noble gases) are $, %, a, and d. a has the highest ionization energy of this group and the least dense, $ has
the lowest ionization energy for this group, and d has a smaller atomic radius than %..
4. The lightest element of all is #.
5. All the following elements are in the 3rd energy level and have
n is the largest atomic radius
g is a metalloid
= is the most reactive nonmetal
? is a pretty reactive metal
+ is next to k but k has the higher ionization energy
e is in this period as well
6. Element g has 14 protons.
7. f has a total of 7electrons.
8. c has an atomic mass of 5 and its final electron is in the 2nd energy level.
9. r would correspond to our alkali metals and is in the 4th energy level.
10. The ! family is made up of the elements !, =, s and p in order of increasing atomic radii.
11. j is the most dense of all Martian atoms and is radioactive and its electron configuration would end with 5p 3..
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12. q is in period 5 and has an oxidation number of 2+.
13. m is in period 2 and will form a compound with ! that has the formula m! 2. In other words, m has two electrons that it would
like to give to !.
14. h is like our element carbon and is in same family as t, w and g.
15. t is bigger than w in atomic radius.
16. The Martian solvent is like our most important liquid and has the formula # 2y.
17. o is in the same family as e and has a lower electronegativity than e.
18. i is the only metalloid in the family of y.
19. l has a dot notation of 3 dots and an oxidation number of 3+.
20. z is in the same family as q and has a slightly higher ionization energy than q.
21. b is slightly smaller that q.
22. u has a final electron configuration of 4p 3.
23. v is next to s and has a larger atomic radius than s..
Extension Problems:
A. If you discovered the Martian element that is listed as undiscovered at this time on the
Martian periodic table, what would you name it?
______________________________
B. What chemical symbol would you give this element and why?
__________
C. Name at least three characteristics that this element would have because of its location on the Martian periodic table?
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Periodic Table Trends Review Worksheet
For each of the following, circle the correct element
1.
Li
Si
S
Metal
2.
N
P
As
Smallest Ionization Energy
3.
K
Ca
Sc
Largest Atomic Mass
4.
S
Cl
Ar
Member of the Halogen Family
5.
Al
Si
P
Greatest Metallic Characteristics
6.
Ga
Al
B
Largest Atomic Radius
7.
V
Nb
Ta
Largest Atomic Number
8.
Te
I
Xe
Member of Noble Gases
9.
Si
Ge
Sn
Has electrons in 4 energy levels
10.
Li
Be
B
Member of Alkali Metals
11.
As
Se
Br
Largest Electronegativity
12.
H
Li
Na
Nonmetal
13.
Hg
Tl
Pb
Member of Transition Metals
14.
Na
Mg
Al
Electron distribution ending in s2p1
15.
Sb
Bi
Pb
Metalloid
16.
B
C
N
Greatest Nonmetal characteristics
17.
Ca
Sc
Ti
Electron distribution ending in s2d2
18.
Be
K
Ga
Member of the Alkaline Earth Metals
19.
Si
Al
P
Semiconductor
20.
F-
Cl-
I-
Smallest Radius
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Honors Chemistry Review Unit 4
1. What contribution did the following people make to the creation of the periodic table:
a. Newlands:
b. Mendeleev:
c. Moseley:
d. Dobereiner:
2. What does the new periodic law state?
3. In the periodic table, the vertical columns are called ________________ and the
horizontal rows are called _________________.
4. Elements in the same group have the same number of _____________
_________________.
5. What family of the periodic table is the most stable because their valence shell is full
of electrons?
6. Give three properties of metals:
7. Give three properties of nonmetals:
8. What is ionization energy?
9. Why does the ionization energy decrease as you move down a group?
10. Why does the atomic radius increase as you move down a group?
11. As you move across a period, the _____________ decreases and the
_____________, ________________, and __________________ increases.
12. As you move down a group, the atomic radius ___________________ and the
ionization energy, electron affinity, and electronegativity ________________.
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For questions #13-36, use the following elements to answer the questions. Elements
may be used more than once and for some questions, there will be more than one
answer.
Na
Si
Br
Ag
Ne
Sb
H
Ga
S
Ca
Es
Pa
Cl
Ba
Li
He
Xe
Fr
F
Al
13. The most reactive metal: _______________________
14. The most reactive nonmetal: _____________________
15. A metal: _____________________________________________________
16. A nonmetal: __________________________________________________
17. A metalloid: __________________________________________________
18. A halogen: ___________________________________________________
19. An alkali metal: _______________________________________________
20. An alkaline earth metal: _________________________________________
21. A noble gas: __________________________________________________
22. A transition metal: _____________________________________________
23. A post transition metal: _________________________________________
24. An inner transition metal: ________________________________________
25. Other nonmetal: _______________________________________________
26. In a family all by itself: _____________
27. Radioactive: __________________________________________________
28. Made in a laboratory: ___________________________________________
29. A gas: _______________________________________________________
30. Found in a free-state (not part of a compound): ________________________
31. Has multiple oxidation states: _____________________________________
32. The only noble gas that does not contain eight valence electrons: ___________
33. Has the same number of valence electrons as Nitrogen: __________________
34. Has the same oxidation state as Potassium: ___________________________
35. Has an oxidation state of -1: ______________________________________
36. Has 4 valence electrons: _________________________________________
26
!
Trends in the Periodic Table
1. On the top graph, plot ionization energy (y-axis) vs, atomic number (x-axis). On the bottom graph,
plot a separate graph of atomic radius (y-axis) vs, atomic number (x-axis). For each graph, connect
successive dots with straight lines, label the axes, and include a title.
2. In order to make the graph easier to analyze, you should mark each group of elements with the same
color circle/dot.
a.
b.
c.
d.
e.
f.
Group 1 – Alkali Metals = Red (H, Li, Na, K)
Group 2 – Alkaline Earth Metals = Blue (Be, Mg, Ca)
Group 3 – Boron Family = Green (B, Al)
Group 5 – Nitrogen Family = Orange (N, P)
Group 7 – Halogens = Yellow (F, Cl)
Group 8 – Noble Gases = Purple (He, Ne, Ar)
3. Examine your graph of atomic radius vs. atomic number.
a. Which elements are found at the main peaks on
your graph?
i. What do these elements have in common?
b. Which elements are found at the main valleys on
your graph?
i. What do these elements have in common?
4. Generally, as you go from left to right across a period,
what happens to atomic radius? Explain why.
5. Generally, as you go down a group in the periodic table,
what happens to atomic radius? Explain why.
6. Examine your graph of ionization energy (IE) vs. atomic number.
a. Which elements are found at the main peaks on your graph?
i. What do these elements have in common?
b. Which elements are found at the main valleys on your graph?
i. What do these elements have in common?
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7. Generally, as you go from left to right across a period, what happens to IE? Explain why.
8. Generally, as you go down a group in the periodic table, what happens to IE? Explain why.
9. Why do you think there is an inverse relationship between atomic radius and ionization energy?
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