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Name________________ Unit 4: Periodic Table Period____ 1. History and Language of the Periodic Table 2. Identifying PROPERTIES OF METALS,
METALLOIDS, & NONMETALS 3. Identifying GROUP PROPERTIES
4. Classifying elements 5. Identifying TRENDS IN THE PERIDIOC TABLE
Unit 4 Vocabulary……………………………………………………….Due Test Day
Word Definition
Mendeleev
Noble Gas
Malleable
Period
Group
Metalloid
Atomic Radius
Ionic Radius
Ionization Energy
Electronegativity
Allotrope
Element Refresh: Name the element in each square! If the name is given, give symbol.
B 14.01amu Bromine 16amu
55amu 4 protons Pb Chlorine
Gold 16.00amu 77protons Ne
259amu Zn I don’t have a neutron 40.08amu
Periodic à Periodic Law à Periodic Table
• Periodic occurs at _____________________ intervals
• Periodic law - physical and chemical properties of the elements are periodic
– By atomic number!
• Periodic Table of Elements – arranged by _________________ - shows patterns in properties
Skill1: History and Language of the Periodic Table
o Element: – A pure substance - one kind of _________ – Cannot be _____________ _____________ into simpler substances – 90 occur naturally on earth – 25 were synthesized (made) by scientists
o Dmitri Mendeleev: – Referred to as the ____________________ of the Period
_______________ – 1860’s – Grouped elements according to
_____________________________ ___
o Mendeleev’s Predictions - Mendeleev’s Table had missing elements or “gaps,” BUT he was able to predict
the characteristics of these missing elements because of ______________ _____________.
• Henry Mosely
- 1914
- Rearranged the elements by
__________________________
- He determined # protons = atomic # E
Important Features of the Periodic Table • Period (Row): Each __________________ row of elements on the periodic table
FROM LEFT TO RIGHT OR RIGHT TO LEFT
Periodic Properties:
• Seven periods (numbered from the top down) • _______________________________________ as you move from the left to the right in a
period • All elements in the same period have the ___________________________________________.
– Period 1 = 1 energy level – Period 2 = 2 energy levels – Period 3 = 3 energy levels – Etc…
Practice: 1) What period is potassium and bromine in? ____
2) Based on the period, how many principal energy levels do potassium and bromine
have? _______________
3) What period is sodium and lithium in? ______
4) Based on the period, how do the properties of sodium and lithium compare? _______________
How many periods (rows) are on the
Periodic Table Of
Elements?
118Uuo
117Uus
116Uuh(292)
115Uup(288)
114Uuq(289)
113Uut(284)
112Uub(285)
111
Rg(272)
110
Ds(269)
109
Mt(268)
108
Hs(269)
107
Bh(264)
106
Sg(266)
105
Db(262)
104
Rf(261)
103
Lr(262)
88
Ra(226)
87
Fr(223)
86
Rn(222)
85
At(210)
84
Po(209)
83
Bi208.980
82
Pb207.2
81
Tl204.383
80
Hg200.59
79
Au196.967
78
Pt195.078
77
Ir192.217
76
Os190.23
75
Re186.207
74
W183.84
73Ta180.95
72
Hf178.49
71Lu174.967
56
Ba137.327
55
Cs132.905
54
Xe131.29
53
I126.904
52
Te127.60
51
Sb121.760
50
Sn118.710
49
In114.818
48
Cd112.4
47
Ag107.868
46
Pd106.42
45
Rh102.906
44Ru101.07
43
Tc(98)
42Mo95.94
41Nb92.906
40
Zr91.224
39Y
88.906
38
Sr87.62
37
Rb85.468
36
Kr83.80
35
Br79.904
34
Se78.96
33
As74.922
32
Ge72.61
31
Ga69.723
30
Zn65.39
29
Cu63.546
28
Ni58.69
27
Co58.933
26
Fe55.845
25Mn54.938
24
Cr51.996
23
V50.942
22
Ti47.87
21Sc44.956
20
Ca40.078
19
K39.098
118Uuo
117Uus
116Uuh(292)
115Uup(288)
114Uuq(289)
113Uut(284)
112Uub(285)
111
Rg(272)
110
Ds(269)
109
Mt(268)
108
Hs(269)
107
Bh(264)
106
Sg(266)
105
Db(262)
104
Rf(261)
103
Lr(262)
88
Ra(226)
87
Fr(223)
86
Rn(222)
85
At(210)
84
Po(209)
83
Bi208.980
82
Pb207.2
81
Tl204.383
80
Hg200.59
79
Au196.967
78
Pt195.078
77
Ir192.217
76
Os190.23
75
Re186.207
74
W183.84
73Ta180.95
72
Hf178.49
71Lu174.967
56
Ba137.327
55
Cs132.905
54
Xe131.29
53
I126.904
52
Te127.60
51
Sb121.760
50
Sn118.710
49
In114.818
48
Cd112.4
47
Ag107.868
46
Pd106.42
45
Rh102.906
44Ru101.07
43
Tc(98)
42Mo95.94
41Nb92.906
40
Zr91.224
39Y
88.906
38
Sr87.62
37
Rb85.468
36
Kr83.80
35
Br79.904
34
Se78.96
33
As74.922
32
Ge72.61
31
Ga69.723
30
Zn65.39
29
Cu63.546
28
Ni58.69
27
Co58.933
26
Fe55.845
25Mn54.938
24
Cr51.996
23
V50.942
22
Ti47.87
21Sc44.956
20
Ca40.078
19
K39.098
102No(259)
101Md(258)
100Fm(257)
99
Es(252)
98
Cf(251)
97
Bk(247)
96Cm(247)
95Am(243)
94
Pu(244)
93Np(237)
92
U238.029
91
Pa231.036
90
Th232.038
89
Ac(227)
70
Yb173.04
69Tm168.934
68
Er167.26
67
Ho164.930
66
Dy162.50
65
Tb158.925
64
Gd157.25
63
Eu151.964
62Sm150.36
61
Pm(145)
60Nd144.24
59
Pr140.908
58
Ce140.116
57
La138.906
102No(259)
101Md(258)
100Fm(257)
99
Es(252)
98
Cf(251)
97
Bk(247)
96Cm(247)
95Am(243)
94
Pu(244)
93Np(237)
92
U238.029
91
Pa231.036
90
Th232.038
89
Ac(227)
70
Yb173.04
69Tm168.934
68
Er167.26
67
Ho164.930
66
Dy162.50
65
Tb158.925
64
Gd157.25
63
Eu151.964
62Sm150.36
61
Pm(145)
60Nd144.24
59
Pr140.908
58
Ce140.116
57
La138.906
12Mg24.305
11
Na22.990
4
Be9.012
3
Li6.941
12Mg24.305
11
Na22.990
4
Be9.012
3
Li6.941
1
H1.008
1
H1.008
2
He4.003
2
He4.003
18
Ar39.948
17
Cl35.453
16
S32.066
15
P30.974
14
Si28.086
13
Al26.982
18
Ar39.948
17
Cl35.453
16
S32.066
15
P30.974
14
Si28.086
13
Al26.982
10Ne20.180
9
F18.998
8
O15.999
7
N14.007
6
C12.001
5
B10.811
10Ne20.180
9
F18.998
8
O15.999
7
N14.007
6
C12.001
5
B10.811
1
2
3
4
5
6
7
1
2
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
18
Lanthanides
Actinides
Important Features of the Periodic Table • Group Family: Each column of the ______________________ on the periodic Table.
FROM TOP TO BOTTOM OR BOTTOM TO THE TOP
Group (Family) Properties:
• Eighteen groups (numbered from left to right)
• Atomic # and masses _____________________________________________________.
• Atoms in same group have ________________________________________________ - Exceptions: d block and f block
• Similar _______________________________________ properties
BECAUSE THEY HAVE THE SAME NUMBER OF _________________________________ Practice:
1. Which sequence of atomic numbers represents elements which have similar chemical properties?
A) 19, 23, 30, 36 C) 9, 16, 33, 50 B) 3, 12, 21, 40 D) 4, 12, 38, 88
2. Which two elements have the most similar chemical properties? A) Aluminum and Barium C) Nickel and Phosphorous B) Chlorine and Sulfur D) Sodium and Potassium
118Uuo
117Uus
116Uuh(292)
115Uup(288)
114Uuq(289)
113Uut(284)
112Uub(285)
111
Rg(272)
110
Ds(269)
109
Mt(268)
108
Hs(269)
107
Bh(264)
106
Sg(266)
105
Db(262)
104
Rf(261)
103
Lr(262)
88
Ra(226)
87
Fr(223)
86
Rn(222)
85
At(210)
84
Po(209)
83
Bi208.980
82
Pb207.2
81
Tl204.383
80
Hg200.59
79
Au196.967
78
Pt195.078
77
Ir192.217
76
Os190.23
75
Re186.207
74
W183.84
73Ta180.95
72
Hf178.49
71Lu174.967
56
Ba137.327
55
Cs132.905
54
Xe131.29
53
I126.904
52
Te127.60
51
Sb121.760
50
Sn118.710
49
In114.818
48
Cd112.4
47
Ag107.868
46
Pd106.42
45
Rh102.906
44Ru101.07
43
Tc(98)
42Mo95.94
41Nb92.906
40
Zr91.224
39Y
88.906
38
Sr87.62
37
Rb85.468
36
Kr83.80
35
Br79.904
34
Se78.96
33
As74.922
32
Ge72.61
31
Ga69.723
30
Zn65.39
29
Cu63.546
28
Ni58.69
27
Co58.933
26
Fe55.845
25Mn54.938
24
Cr51.996
23
V50.942
22
Ti47.87
21Sc44.956
20
Ca40.078
19
K39.098
118Uuo
117Uus
116Uuh(292)
115Uup(288)
114Uuq(289)
113Uut(284)
112Uub(285)
111
Rg(272)
110
Ds(269)
109
Mt(268)
108
Hs(269)
107
Bh(264)
106
Sg(266)
105
Db(262)
104
Rf(261)
103
Lr(262)
88
Ra(226)
87
Fr(223)
86
Rn(222)
85
At(210)
84
Po(209)
83
Bi208.980
82
Pb207.2
81
Tl204.383
80
Hg200.59
79
Au196.967
78
Pt195.078
77
Ir192.217
76
Os190.23
75
Re186.207
74
W183.84
73Ta180.95
72
Hf178.49
71Lu174.967
56
Ba137.327
55
Cs132.905
54
Xe131.29
53
I126.904
52
Te127.60
51
Sb121.760
50
Sn118.710
49
In114.818
48
Cd112.4
47
Ag107.868
46
Pd106.42
45
Rh102.906
44Ru101.07
43
Tc(98)
42Mo95.94
41Nb92.906
40
Zr91.224
39Y
88.906
38
Sr87.62
37
Rb85.468
36
Kr83.80
35
Br79.904
34
Se78.96
33
As74.922
32
Ge72.61
31
Ga69.723
30
Zn65.39
29
Cu63.546
28
Ni58.69
27
Co58.933
26
Fe55.845
25Mn54.938
24
Cr51.996
23
V50.942
22
Ti47.87
21Sc44.956
20
Ca40.078
19
K39.098
102No(259)
101Md(258)
100Fm(257)
99
Es(252)
98
Cf(251)
97
Bk(247)
96Cm(247)
95Am(243)
94
Pu(244)
93Np(237)
92
U238.029
91
Pa231.036
90
Th232.038
89
Ac(227)
70
Yb173.04
69Tm168.934
68
Er167.26
67
Ho164.930
66
Dy162.50
65
Tb158.925
64
Gd157.25
63
Eu151.964
62Sm150.36
61
Pm(145)
60Nd144.24
59
Pr140.908
58
Ce140.116
57
La138.906
102No(259)
101Md(258)
100Fm(257)
99
Es(252)
98
Cf(251)
97
Bk(247)
96Cm(247)
95Am(243)
94
Pu(244)
93Np(237)
92
U238.029
91
Pa231.036
90
Th232.038
89
Ac(227)
70
Yb173.04
69Tm168.934
68
Er167.26
67
Ho164.930
66
Dy162.50
65
Tb158.925
64
Gd157.25
63
Eu151.964
62Sm150.36
61
Pm(145)
60Nd144.24
59
Pr140.908
58
Ce140.116
57
La138.906
12Mg24.305
11
Na22.990
4
Be9.012
3
Li6.941
12Mg24.305
11
Na22.990
4
Be9.012
3
Li6.941
1
H1.008
1
H1.008
2
He4.003
2
He4.003
18
Ar39.948
17
Cl35.453
16
S32.066
15
P30.974
14
Si28.086
13
Al26.982
18
Ar39.948
17
Cl35.453
16
S32.066
15
P30.974
14
Si28.086
13
Al26.982
10Ne20.180
9
F18.998
8
O15.999
7
N14.007
6
C12.001
5
B10.811
10Ne20.180
9
F18.998
8
O15.999
7
N14.007
6
C12.001
5
B10.811
1
2
3
4
5
6
7
1
2
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
18
Lanthanides
Actinides
How many groups (families) are on the
Periodic Table Of Elements?
General Groups of Elements!
Using this as a guide, color code your periodic table to
show the three classes. Start by highlighting the “zig-zag.”
Skill 2: Identifying PROPERTIES OF METALS, METALLOIDS, & NONMETALS Metals, Groups 1-Zig Zag
Location Chemical Prop. Physical Prop.
Left of zig zag
Few electrons in VALENCE shell (outer shell)
Ductile Malleable
Except hydrogen Lose electrons easily Good __________________
POSITIVE charge Ca2+
Shiny
Make ___________________
Solid at room temp
o Define Alloy: _______________________________________________________________________
Non-Metals:
Location Chemical Prop. Physical Prop.
Right of zig zag Almost full, or totally full ____________________
NOT Ductile NOT malleable
Tend to ________ electrons BAD conductors
NEGATIVE charge N3-
Mostly solid
Make ________ Some are gas at room temp
o Allotrope: ___________________________________________________________________
Examples:
o Diatomic:__________________________________________________________________ Metalloids:
Location Chemical Prop. Physical Prop.
Border the zig zag
Most have half full valence shell Have properties of ____________AND non-____________
Make anions OR cations depending on their environment
No way to know which properties of each
o Synthetic:___________________________________________________________________
What metal is NOT solid at Room Temperature? ____________________
Name__________________________ Groups of Elements! Date___________
Color As Instructed At Each Station!
Skill 3: Identifying GROUP PROPERTIES
Group 1: Alkali Metals Please color the first column orange! Read and answer:
o What element is not in this group? _______________
o What elements are in this group? _______________________________________________ _______________________________________________
o They are very _______________. Why? They all have one ___________ in their outer shell. That's one electron away from being happy (____________)
o You will find that the alkali group is shiny and light in weight. They are also very soft and malleable.
Watch the 2nd link!
Group 2: Alkaline Earth Metals Watch link, read and answer the following:
o This is the second most reactive family of elements in the periodic table.
o Form “basic” or _______________ solutions.
o Each of them has _________ electrons in their outer shell.
Check for Understanding:
1. In General for Groups 1 and 2: As you move down
the groups, they become more ____________
2. What will be the charge of a Calcium atom when it forms an ion? ________________
3. List Group 1 metals in order from most to least reactive:
Color Orange
Color Green
MOST LEAST
Transition Metals: Groups 3-12 Watch and answer the following:
o Transition metals are located in the ________________ of the table.
o Compared to the alkali metals, transition metals have ____________________ densities, have
_________________ melting and boiling points, are strong and __________ and are less ___________________with oxygen and water.
o Transition metals often form ______________compounds and solutions.
o Transition metals can form more than one type of _____________ (have multiple oxidation
states).
Check for Understanding:
1. Identify the metal that has multiple oxidation states. A) K B) Ba
C) Be D) Pd
2. Which compound forms a green aqueous solution? A) RbCl B) CaCl2 C) NiCl2 D) BeCl2
3. Which set of properties is most characteristic of transition elements?
A) Colorless ions in solutions, multiple positive oxidation states B) Colorless ions in solutions, multiple negative oxidation states C) Colored ions in solutions, multiple negative oxidation states D) Colored ions in solutions, multiple positive oxidation states
Color Yellow
Misc. Group 13-16, (BCNO)
o Use Ptable link to determine which elements are LIQUID at STP.
o Use P table link to determine which elements are GAS at STP. Outline those elements in RED.
o Watch video link!
Group 17: Halogens Read and Answer:
o What elements are included in the halogens? ______________________________________
o Read and answer, then watch.
o Halogens all have __________________ electrons in their outer (valence) shell
o Fluorine is the most ____________ and
combines with most elements from around the periodic table.
o Reactivity ____________ as you move down the column.
o When halogens combine with other elements, the compound is called a _____________.
Check for Understanding:
1) Give an example of a metalloid: _______________________
2) How many valence electrons does Cl have?____________
3) What kind of ion will Br form? _______________
4) Which is the most reactive in the group? ________________
Highlight the Staircase
Outline those elements in BLUE.
Color Black/Gray
Noble Gases, Group 18 Watch and fill in the notes:
o Noble gases are the group _______ elements
o Each noble gas has a full _________ shells, which makes them very _________ elements
o They are also called the inert or
_______________ gases
o Light bulbs are filled with __________
CHECK FOR UNDERSTANDING:
1. What is the electron configuration of Argon? What does it have in common with Neon? ____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
2. Explain why noble gases don’t typically react with other elements? ____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
Color Purple
Name_______________________ Periodic Group Practice! Period________
name_________ HPS ____ # ____ date:________
Chapter 5 TEST: The Periodic Table
Multiple Choice Identify the choice that best completes the statement or answers the question.
____ 1. The order of elements in the periodic table is based on a. the number of protons in the nucleus. b. the electric charge of the nucleus. c. the number of neutrons in the nucleus. d. atomic mass.
____ 2. Atoms of elements that are in the same group have the same number of a. protons. c. valence electrons. b. neutrons. d. protons and neutrons.
____ 3. Which of the following elements is an alkali metal? a. calcium c. mercury b. magnesium d. sodium
____ 4. Semiconductors are elements that a. have large atomic masses but small atomic numbers. b. do not form compounds. c. can conduct heat and electricity under certain conditions. d. are extremely hard.
____ 5. Carbon and other nonmetals are found in which area of the periodic table? a. on the left-most side b. on the right side c. in the middle column of the periodic table d. in the bottom rows
____ 6. In Mendeleev’s periodic table, elements in each column had similar a. atomic masses. c. atomic numbers b. properties. d. symbols.
____ 7. Magnesium (Mg) is located to the right of sodium (Na) because Mg has a. fewer protons. c. no protons. b. no neutrons. d. more protons.
____ 8. As you move from left to right across the periodic table, elements a. become less metallic. c. have a lower atomic weight. b. have a lower atomic number. d. become more metallic.
____ 9. How was Mendeleev’s periodic table arranged? a. by increasing atomic mass c. by increasing atomic number b. by decreasing atomic mass d. by decreasing atomic number
____ 10. When did Mendeleev create a new row in his periodic table? a. when the first atomic mass was doubled b. when chemical properties were repeated c. when there were 10 elements in the row d. when the next element was a nonmetal
____ 11. Mendeleev left gaps in his periodic table because
a. the table was too small. c. the table was too full. b. protons belonged there. d. no known elements fit there.
____ 12. Each column of the periodic table is a. an element. c. an isotope. b. a group. d. a period.
____ 13. Atoms that gain or lose electrons are called a. metals. c. ions. b. nonmetals. d. isotopes.
____ 14. Group 17 elements form
a. +1 ion c. +7 ion b. -1 ion d. -7 ion
____ 15. The three main groups of elements are metals, nonmetals, and a. inert gases. c. radioactive isotopes. b. alkali metals. d. semiconductors.
____ 16. Most elements are a. metals. c. metalloids. b. nonmetals. d. semiconductors.
____ 17. Most nonmetals are a. brittle. c. metalloids. b. good conductors. d. shiny.
____ 18. Elements in an element family have similar a. atomic symbols. c. atomic weights. b. atomic sizes. d. chemical properties.
____ 19. How do you know that potassium, an alkali metal, is highly reactive? a. It conducts heat. c. It is a soft and shiny metal. b. It conducts electricity. d. It has one valence electron.
____ 20. The order of elements in the modern periodic table is based on an element’s a. atomic number. c. chemical symbol. b. name. d. atomic mass.
____ 21. Ionization refers to the process of a. changing from one period to another. c. turning lithium into fluorine. b. losing or gaining protons. d. losing or gaining electrons.
____ 22. Elements that share properties of both metals and nonmetals are called a. ions. c. semiconductors. b. periods. d. valences.
____ 23. Which statement about the alkali metals is correct? a. They are located in the left-most column of the periodic table. b. They are extremely nonreactive. c. They are usually gases. d. They form negative ions with a 1– charge.
____ 24. Which statement about noble gases is correct? a. They form compounds with very bright colors. b. They exist as single atoms rather than as molecules. c. They are highly reactive with both metals and nonmetals. d. They are extremely rare in nature.
____ 25. Which element is a semiconductor? a. carbon c. sodium b. silicon d. uranium
____ 26. Metals tend to be a. gases. c. dull. b. good conductors of heat. d. brittle.
____ 27. Different isotopes of the same element have different a. atomic numbers c. numbers if neutrons b. numbers of protons d. numbers of electrons
Matching Match each item with the correct statement below. a. halogens d. semiconductors b. alkaline-earth metals e. alkali metals c. transition metals f. noble (inert) gases
____ 28. Elements that have properties of both metals and nonmetals; located near the stair step line
____ 29. Reactive elements of Group 17 that are poor conductors
____ 30. Highly reactive elements that belong to Group 1 ____ 31. Very stable due to the fact that they have a full outermost energy level
____ 32. Elements that belong to Groups 3-12 and are somewhat reactive ____ 33. Group 2 elements that have two valence electrons
Essay
34. Why might a jewelry designer prefer to work with a metal rather than a nonmetal? Explain your answer.
35. Draw a Lewis Dot Diagram for oxygen.
Name _________________________ Period_____
POGIL Periodic Table TRENDS Activity The Periodic Table is a map of the elements. There are many patterns or trends on the periodic table. Let’s look and see what we can find. (Use your Regents Chemistry Reference Table and fill in the blanks with the appropriate answers.) Periods: (Horizontal)
1. Look at Na to Ar to answer the following questions. (Choose INCREASES, decreases, or remains the same.)
2. The atomic # (INCREASES, decreases, or remains the same.)
3. The # of protons _______________________
4. The # of valence electrons _________________
5. The # of principle energy levels _______________________
6. All elements in the same period have the same _______________________________
Groups: (Vertical) Look at H to Fr to answer the following questions. (Choose INCREASES, decreases, or remains the same.)
1. The atomic # (INCREASES, decreases, or remains the same.)
2. The # of protons _____________
3. The # of valence electrons _________________
4. The # of principle energy levels ____________________
5. All elements in the same group have the same ________________________________ and therefore react similarly.
Atomic Radii: The atomic radius (or radii) is the distance from the center of the nucleus to the outer
edge of the atom. This is used to tell how big the atom is. Look at your table S in your reference table and see if you can find these values. Let’s look at some trends for these. Write down the information below for each element.
The atomic radius is affected by 2 things: the number of principle energy levels and the attraction between protons and electrons. When comparing atomic radii, first, look at principle energy level….the more principle energy levels (p.e.l), the bigger the atom. Then, if the p.e.l. are the same, look at the number of protons to the number of electrons….more protons, means more attraction for electrons, and the electrons get sucked in closer to the nucleus, shrinking the atom. Periods: (Examine the elements in period 3)
Na: Radius _______________ # of principle energy levels ___________________ # of protons ____________________ # of electrons ____________________
Si: Radius _______________ # of principle energy levels ___________________ # of protons ____________________ # of electrons ____________________
Cl: Radius _______________
# of principle energy levels ___________________ # of protons ____________________ # of electrons ____________________
Groups: (Examine the elements in group 1)
Li: Radius _______________ # of principle energy levels ___________________
# of protons ____________________ # of electrons ____________________
K: Radius _______________
# of principle energy levels __________________ # of protons ____________________ # of electrons ____________________
Cs: Radius _______________
# of principle energy levels __________________ # of protons ____________________ # of electrons ____________________
The radius _________________________ (increases or DECREASES) as you go across a period due to an increase in the number of PROTONS in nucleus pulling electrons closer
The radius __________________________(INCREASES or decreases) as you go down a group due to more energy levels (shells of electrons)
Electronegativity Electronegativity is a measure of an atom’s ATTRACTION for electrons in a bond with another atom. Electronegativity is measured on a scale of 0 to 4, with 4 being the highest electronegativity value. Fluorine, F, is the most electronegative element with a value of 4. Fluorine is located in the upper right corner of the Periodic Table. In general, the closer an atom is to F, the higher its electronegativity value. So, as you go across a period or up a group (toward F), electronegativity values increase. These values can also be looked up in Table S. Ionization Energy Ionization energy is the amount of energy required to REMOVE an electron from an atom in the gaseous state. This property of atoms is directly related to their electronegativity values – the more attracted to electrons they are, the more energy it will take to pull an electron away. Ionization energies are also listed on Table S. Fill in the table below for the elements in Period 2 and Group 2 to note the general pattern of values.
Period 2 Elements Li Be B C N O F Electronegativity
Ionization Energy (kJ/mol)
*In general, as you go across a period, electronegativity and ionization energy ________________________ (INCREASE or decrease)
…This is because the number of ______________________________increases, so attraction to outermost electrons increases. (PROTONS or electron shells)
Group 2 Elements Electronegativity Ionization Energy
(kJ/mol) Be
Mg
Ca
Sr
Ba
*In general, as you go down a group, electronegativity and ionization energy ________________________ (increase or DECREASE)
…This is because the number of _____________________________ increases, so attraction to outermost electrons decreases. (protons or ELECTRON SHELLS)
Skill 5: Identify Trends in the Periodic Table
Trends Summary:
Atomic Radius:
- How far from valence to nucleus
- Period - atomic radius _______________as you go from left to right across a period.
Why?
- Stronger attractive forces in atoms (as you go from left to right) between the opposite charges in the nucleus, decreased shielding.
- Group - atomic radius ______________ as you go down a group.
Why?
- Added energy levels. Increased layers, meaning increased distance to the nucleus
Ionic Radius:
- How far from valence electron to _______________ in an ION.
- As one moves down a group
on the periodic table, the ionic radius________________ because additional electrons are being added to the atom.
- Within a period, the radius trend is dependent on whether the ion is ______________ or _________________. When moving across a period among positive ions, the number of protons increases. This decreases the ionic radius.
- Among negative ions, additional layers of electrons are being added, which increases the radius.
Ionization Energy
- Ionization energy is the amount of energy required to _____________ the outmost electron.
- Period - ionization energy _________________as you go from left to right across a period.
Why?
- Elements on the right of the chart want to take others atom's electron (not given them up) because they are close to achieving the _________________.
- The means it will ______________ more energy to remove the outer most electron.
- Elements on the left of the chart would prefer to give up their electrons so it is__________ to remove them, requiring______________ energy (low ionization energy).
- Group - ionization energy ________________ as you go down a group.
Why?
- The SHIELDING affect makes it easier to remove the outer most electrons from those atoms that have many electrons (those near the bottom of the chart).
Electronegativity
- Electronegativity is an atom's 'desire' to grab another atom's electrons
- Period- electronegativity ________________ as you go from left to right across a period.
Why?
- TRYING TO GET A NOBLE GAS CONFIGURATION.
- Group - electronegativity _____________________ as you go down a group.
Why?
- The lower you go, the more shielding due to the increase in number of electrons. It’s not such a big deal to lose a couple electrons.
