Download Chemistry A- Periodic Table Packet

Chemistry A: Periodic Table Packet
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Chemistry A
Periodic Table
Chemistry A: Periodic Table Packet
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Worksheet #1: Periodic Table Inquiry Activity
Directions: I know that we have not talked about these ideas yet, but I want to see how much you can figure out on your
own. Sometimes you might feel like you are “guessing” at the answers, but if you read carefully and look at the pictures
and diagrams all the information you need to answer the questions is on this sheet.
A little background…
The periodic table is, in many ways, the world’s greatest cheat sheet. It was created a long time ago by a guy named Dmitri
Mendeleev who, probably like you, did not want to memorize tons of information. The periodic table lists all of the
elements (simple substances that make up more complex materials) like gold, silver, tin, lead and mercury. It also provides
lots of information about these elements. The good news is that you will be able to use the periodic table on all of your
chemistry exams. The bad news is that first you have to learn all the symbols Mendeleev used for this information.
Questions:
1.
Who created the first periodic table?
2.
What is an element?
3.
Each box represents a different element. How many elements are on this periodic table?
What makes up each element?
The parts that make up an element are called sub-atomic particles. There are three basic sub-atomic particles that we will
talk about in chemistry, they are called protons, neutrons and electrons. Each proton has one positive charge of
electricity (+1). Each electron has one negative charge of electricity (-1). Neutrons are neutral, which means they do not
have a charge.
4.
What is a sub-atomic particle?
5.
What is the difference between a proton, a neutron and an electron?
Chemistry A: Periodic Table Packet
Name: ____________________________ Hour: ____ Page 3
Here is a close-up of the periodic table symbol
Here is a close-up of the element carbon if we
for carbon, an element that is very common and
could see it under a very powerful microscope:
we will study about this trimester:
KEY
Atomic
Number
p = proton
n = neutron
Mass
Number
= electron
Nucleus
6.
Are the protons and neutrons found inside or outside the nucleus?
7.
Are the electrons found inside or outside the nucleus?
8.
How many electrons does carbon have?
9.
How many protons does carbon have?
The electron cloud is
made of “shells” that hold
the electrons. Carbon has
2 shells and is in the 2nd
row of the periodic table.
10. How many neutrons does carbon have?
11. What is the total positive charge of carbon?
12. What is the total negative charge of carbon?
These + and – charges
“cancel out” making a
neutral carbon atom.
13. Match the following
a.
Atomic Number
i. the number of protons in the nucleus of an atom
b.
Atomic Mass
ii. the number of protons + number of neutrons (approximately)
Name: ________________________Hr:___
Chemistry A- Periodic Table Packet
Worksheet #2: Atoms
All matter (air, water, soil, people) is made the elements on the Periodic Table. The smallest unit of one
element that can exist on its own is called an atom. Atoms are made of a central nucleus, which contains
protons and neutrons. Protons are positively charged and neutrons have no charge. Surrounding these nuclei
are little negatively charged particles called electrons. The space around the nucleus that contains the electrons
is called the electron cloud or shell.
Electron Cloud
(Shell)
# of shells=
row of
periodic
table
Electron – negative
charge
Neutron – no
charge
(neutral)
Proton – positive
charge
Each atom is different from every other atom by the number of protons it has in its nucleus. Hydrogen has one
proton; helium has two. Calcium has 20 and gold has 79. The number of protons in an atom is equal to the
atomic number of the element.
Mass Number = # protons
+ number of neutrons
bigger
Atomic Number = #
of protons.
smaller
The proton has a positive charge and a mass of approximately one amu (atomic mass unit). A neutron is a
neutral particle with a mass of approximately one amu. To determine the number of neutrons in an atom
you subtract the atomic number from the mass number of the atom. The electrons are negatively charged
particles located in energy levels outside the nucleus. The mass of an electron is extremely small—we describe
it as negligible since it would take nearly two thousand electrons to have the mass of a single proton. The
number of electrons in an atom is equal to the atomic number and, since the charge on an electron is equal
in size but opposite in sign to that of the proton, an atom is neutral.
(+) charge + (-) charge = 0
Complete the following table:
Particle Name
Charge
Mass
Location in Atom
What tells you how many are in an
atom?
PROTON
ELECTRON
NEUTRON
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Chemistry A- Periodic Table Packet
Worksheet #3: Atomic and Mass Number Practice
Draw a picture of the symbol of carbon from the periodic table. Label its atomic number and mass number:
1. Carbon has 6 protons. How many electrons does it have?
2. Lead has an atomic number of 82. How many protons? Electrons?
3. How many protons does Silicon have? Electrons?
4. An atom has a mass number of 42 and an atomic number of 39. How many neutrons does it have?
5. What is the mass number of calcium?
6. How many neutrons does calcium have?
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Chemistry A- Periodic Table Packet
Worksheet #4: Organization of the Periodic Table
In addition to being different from each other because of the number of protons they have, atoms also
differ in their behavior. Potassium and sodium are extremely explosive in the presence of water, while a chunk
of copper or silver would just sink effortlessly to the bottom of a swimming pool.
Dmitry Mendeleev (1834-1907) was a Russian chemist who proposed a method of arranging atoms
according to their mass as well as their behavior. He noticed that certain elements behaved similarly to others,
and he arranged these on his table so that they were in the same vertical row.
For example, if you look at a periodic table of elements, you will notice that H, Li, Na, K, Rb, Cs,
and Fr are all in the same vertical column. These elements all share common behaviors and also share a
similar electron arrangement.
Mendeleev's work is important to us today because he was able to successfully classify the chemical
elements in order to give scientists a better understanding of how atoms interact with each other and of the
properties they hold. The periodic table organizes the elements into a grid of horizontal rows called
periods and vertical columns called groups or families. By setting up this periodic table, he was even
successful in predicting the existence of at least three more elements that had yet to be discovered (gallium,
scandium, and germanium).
Arranging elements by mass resulted in several elements being placed in groups of elements with
different properties. Henry Mosely (1913) discovered that atoms of each element contain a unique number of
protons in their nuclei (plural of nucleus), the number of protons being equal to the atomic number. Arranging
the periodic table by atomic number, instead of mass, eliminated the problems with the Mendeleev’s periodic
table.
1)
2)
3)
4)
What are the vertical (up and down) columns of the periodic table called? ___________________
What are the horizontal (back and forth) rows of the periodic table called? __________________
Which elements have similar properties, those in the same period or in the same family? _________
How did Mosley improve the organization of the periodic table?
Have your table
out so we can
label it together.
The Modern Periodic Table:
There are three main classifications for the elements- metals, nonmetals, and metalloids. Metals are
elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors
of heat and electricity. Most metals are ductile and malleable, meaning that they can be pounded into thin
sheets and drawn into wires.
Most group A elements and all group B elements are metals. If you look at boron (B), you see a heavy
stair-step line that zigzags down to astatine (At) at the bottom of group 7A. This stair step line serves as a visual
divider between the metals and the nonmetals on the table. Except for hydrogen, all of the elements on the
left side of the table are metals. The group 1A elements (except for hydrogen) are known as the alkali metals.
The group 2A elements are known as the alkaline earth metals. Both the alkali metals and the alkaline
earth metals are chemically reactive, with the alkali metals being more reactive of the two groups.
The elements in the center of the periodic table are called transition metals. As with all metals, the
transition elements are both ductile and malleable, and conduct electricity and heat. We will learn later in the
trimester what makes transition metals unique in their behavior. The 2 sets of inner transition metals, known as
the lanthanide and actinide series, are located along the bottom of the periodic table.
Nonmetals are elements that are generally gases or brittle dull-looking solids found in the upper
right side of the periodic table. They are poor conductors of heat and electricity. The highly reactive
group 7A elements are known as halogens, and the extremely unreactive group 8A elements are
commonly called the noble gases.
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Chemistry A- Periodic Table Packet
Worksheet #4 Continued: Organization of the Periodic Table
The elements bordering the stair-step line are called metalloids. Metalloids are elements with
physical and chemical properties of both metals and nonmetals. Silicon and germanium are 2 of the most
important metalloids, as they are extensively used in computer chips and solar cells.
Directions: Fill in the blanks on the right with the information in the chart below.
Word List
actinide series
alkali metal
alkaline earth metal
atomic mass
atomic number
family
group
halogen
lanthanide series
metal
metalloid
Moseley
noble gas
nonmetal
period
periodic law
periodic table
transition element
1. ____________________
2. ____________________
3. ____________________
4. ____________________
5. ____________________
6. ____________________
Dmitri Mendeleev developed a chart-like arrangement of the elements
7. ____________________
called the __(1)__. He stated that if the elements were listed in order of increasing
8. ____________________
__(2)__, their properties repeated in a regular manner. He called this the __(3)__
9. ____________________
of the elements. The arrangement used today, devised by __(4)__, differs from
10. ____________________
that of Mendeleev in that the elements are arranged in order of increasing __(5)__.
Each horizontal row of elements is called a(n) __(6)__. Each vertical column is
11. ____________________
called a(n) __(7)__, or, because of the resemblance between elements in the same
12. ____________________
column, a(n) __(8)__.
13. ____________________
In rows 4 through 7, there is a wide central section containing elements,
14. ____________________
each of which is called a(n) __(9)__. Rows 6 and 7 also contain two other sets of
elements that are listed below the main chart. These are called the __(10)__ and
15. ____________________
the __(11)__, respectively. Each of these elements, as well as those in the first two
16. ____________________
columns at the left end of the chart, is classified as a(n) __(12)__. Each of the
17. ____________________
elements at the right side of the chart is classified as a(n) __(13)__. Each of the
18. ____________________
elements between these two main types of elements, having some properties in
common with each, is called a(n) __(14)__.
Each of the elements in Group 1A is called a(n) __(15)__. Each of the elements in
the Group 2A is called a(n) __(16)__. Each of the elements in Group 7A is called a(n)
__(17)__. Each of the elements in Group 8A is called a(n) __(18)__.
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Chemistry A- Periodic Table Packet
Worksheet #5: Color Coding the Periodic Table
REVIEW: The Periodic Table is a list of all the known elements. It is organized by increasing atomic number. There
are two main groups on the periodic table: metals and nonmetals. The left side of the table contains elements with
the greatest metallic properties. As you move from the left to the right, the elements become less metallic with the far
right side of the table consisting of nonmetals. The elements in the middle of the table are called “transition”
elements because they are changed from metallic properties to nonmetallic properties. A small group whose
members touch the zigzag line are called metalloids because they have both metallic and nonmetallic properties.
NEW: The table is also arranged in vertical columns called “groups” or “families” and horizontal rows called
“periods.” Each arrangement is significant.
Groups (vertical, “up and down”) – same number of valence electrons (electrons in outermost shell of
atom) which gives elements of the same group similar properties.
Example: All group 1 elements have one electron in the outer shells and all group 2 elements have
two electrons in their outer shells.
Periods (horizontal, “back and forth”) – same number of electron shells around nucleus
Example: The elements in the first period all have one shell, the elements in the second period all
have two shells etc.
There are a number of major groups with similar properties. They are as follows:
Hydrogen: This element does not match the properties of any other group so it stands alone. It is placed
above group 1 but it is not part of that group. It is a very reactive, colorless, odorless gas at room
temperature. (1 valence electron)
Group 1: Alkali Metals – These metals are extremely reactive and are never found in nature in their pure
form. They are silver colored and shiny. They are soft enough to be cut with a knife. (1 valence electron)
Group 2: Alkaline-earth Metals – Slightly less reactive than alkali metals. They are silver colored and more
dense than alkali metals. (2 valence electrons)
Groups 3 – 12: Transition Metals – These metals have a wide range of properties. In general, they are shiny
and good conductors of heat and electricity. They also have higher densities and melting points than groups 1
& 2. (1 or 2 valence electrons)
Lanthanides and Actinides: These are also transition metals that were taken out and placed at the bottom of
the table so the table wouldn’t be so wide. The elements in each of these two periods share many properties.
The lanthanides are shiny and reactive. Elements 95 through 103 do not exist in nature but have been
manufactured in the lab-thus are man-made.
Group 13: Boron Group – Contains one metalloid (B) and 4 metals. Reactive. Aluminum is in this group. It
is also the most common metal in the earth’s crust. (3 valence electrons)
Group 14: Carbon Group – Contains one nonmetal, two metalloids (Si & Ge), and two metals. (4 valence
electrons)
Group 15: Nitrogen Group – Contains two nonmetals, two metalloids (As & Sb), and one metal.(5 valence
electrons)
Group 16: Oxygen Group – Contains three nonmetals and two metalloids (Te & Po).(6 valence electrons)
Groups 17: Halogens – All nonmetals. Very reactive. (7 valence electrons)
Groups 18: Noble Gases – Unreactive nonmetals. All are colorless, odorless gases at room temperature. All
found in earth’s atmosphere in small amounts. (8 valence electrons)
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Chemistry A- Periodic Table Packet
Worksheet #5 Continued: Color Coding the Periodic Table
This worksheet will help you understand how the periodic table is arranged. Using the periodic table below, color each group on the table as follows:
1. Color the square for Hydrogen pink.
7. Color the nonmetals orange.
2. Lightly color the metalloids purple (if the square touches the staircase,
8. Draw small brown circles in each box of the halogens.
the element is a metalloid).
9. Draw checkerboard lines through all the boxes of the noble gases.
3. Lightly color all metals yellow.
10. Using a black color, trace the zigzag line that separates the metals from
4. Place black dots in the squares of all alkali metals.
the nonmetals.
5. Draw a horizontal line across each box in the group of alkaline earth
11. Color all the lanthanides red.
metals.
12. Color all the actinides light green and the MAN MADE dark green.
6. Draw a diagonal line across each box of all transition metals.
Group
1
H
Group
18
Group
2
Group
13
Group
14
Group
15
Group
16
Group
17
Be
B
C
N
O
F
Group
3
Group
4
Group
5
Group
6
Group
7
Group
8
Group
9
Group
10
Group
11
Group
12
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
95
96
He
La
Ac
La
Ac
9
97
98
99
100
101
102
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Chemistry A- Periodic Table Packet
BrainPOP: The Periodic Table of Elements
Watch the video “The Periodic Table of the Elements” on brainpop.com
Username- greenwichps Password- gps2009
1. The periodic table categorizes elements according to the _________________________of their
atoms.
2. Atoms are the _____________________ ____________________ of an element.
3. The numbers of ______________________, ____________________ and ___________________ determine an
element’s properties.
4. The modern table organizes elements so we can see how they ___________________ to each other.
5. Elements are listed by their __________________ __________________; or number of protons in their
nuclei.
6. Reading across the table, the sets are called ____________________.
7. Periods describe the number of _____________________ that elements have. Hydrogen and helium
have one electron shell. Period two elements have ________________ electron shells.
8. The first shell contains _____________ electrons and the second one can hold up to________________
electrons.
9. As you read across a period the outer shell fills up with ______________________. Lithium has one
electron in its outer shell, beryllium has ____________, boron has ___________. By the time you get
to the far right side the outer shell is completely _______________.
10. Elements with similar ___________________ _______________________ are organized into the same
groups.
11. Elements in _________________ ____________ have one electron in their outermost shells. This
means they are likely to form positive ions.
12. ___________________ metals react with water.
13. _________________________ metals like iron are strong and shiny.
14. Nonmetals include carbon, nitrogen and oxygen.
15. ___________________ _____________________ have outer electron shells that are ___________ and don’t
often react with other elements.
16. Any element above element 92 is too ______________________ to occur in nature.
17. Scientists used the periodic table to ______________________ the existence of elements like neon
and germanium before they were discovered.
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Chemistry A- Periodic Table Packet
Directions:
1. Go to mrscrane.wiki.farmington.k12.mi.us
2. Following the links to “Chemistry A” and “Periodic Table Unit”
3. Follow the link to “Element Math Game”
4. When you get to the website, uncheck the “Nucleons” box
5. Click on “I’m Ready, Let’s Start!”
What was your score? + __________/10
How do you determine the number of protons? ______________________________________________
How do you determine the number of electrons? ____________________________________________
How to you determine the number of neutrons? ______________________________________________
Directions:
1. Go to mrscrane.wiki.farmington.k12.mi.us
2. Following the links to “Chemistry A” and “Periodic Table Unit”
3. Follow the link to “Groups of the Periodic Table”
4. When you get to the website, read and answer the following questions.
1. How are the families of the periodic table like real life families?
2. What is the definition of a metal? __________________________________________________________________
3. What is common table salt made of? ____________________________ and _____________________________
4. What is an unusual property of the alkaline earth metals? ________________________________________
5. Why don’t noble gases react with other elements? _________________________________________________
6. What does the world “halogen” mean? ______________________________________________________________
7. What is the definition of a non-metal? ______________________________________________________________
8. What is the most reactive element? __________________________
9. Label the periodic table below with: lanthanide series, actinide series, transition metals, alkali
metals, alkaline metals, halogens, noble gases.
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Chemistry A- Periodic Table Packet
Periodic Table Review Sheet
1. On the periodic table below, label all of the following:
a. Metals
e. Noble gases
b. Transition metals
f. Halogens
c. Alkali metals
g. Lanthanide series
d. Alkaline metals
h. Actinide series
i. Metalloids
j. nonmetals
The Periodic Table of the Elements
Questions:
1. What is an atom?
2. Name the three subatomic particle that make up an atom:
3. Complete the following table:
Particle Name
Charge
Mass
Location in Atom
What tells you how many are in an
atom?
PROTON
ELECTRON
NEUTRON
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Chemistry A- Periodic Table Packet
4. What does the atomic number of an atom tell us?
5. What does the mass number of an atom tell us?
6. Why aren’t the metalloids categorized as metals or nonmetals?
7. How did Mendeleev arrange the periodic table?
8. How did Mosely improve on Mendeleev’s periodic table? Why was it better this way?
9. What does a group/family of elements have in common?
10. What do the elements in a period have in common?
11. Nitrogen has 7 protons. How many electrons does it have?
12. Uranium has an atomic number of 92. How many protons? Electrons?
13. How many protons does bromine have? Electrons?
14. An atom has a mass number of 35 and an atomic number of 17. How many neutrons does it have?
15. What is the mass number of magnesium?
16. How many neutrons does magnesium have?
17. What is matter?
18. What is the main difference between a compound and an element?
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Chemistry A- Periodic Table Packet
A Quick Review of Atoms
Part 1: Match the terms in the first column with the definitions in the second column.
1. molecule
______A. Substance made of only one kind of atom.
2. nucleus
______B. The total of protons and neutrons in an atom.
3. atomic number
______C. The center of an atom.
4. mass number
______D. A group of atoms bonded to each other.
5. electron
______E. The total protons in a nucleus.
6. neutron
______F. Particle with a positive charge.
7. proton
______G. Particle with no charge.
8. atom
______H. Particle with a negative charge.
9. element
______I. Smallest particle of an element
Part 2: Write a brief answer for each question below.
1. Name the three particles found in an atom. Give the charge and location with the atom of
each.
2. A certain oxygen atom has an atomic number of 8 and a mass number of 16. How many
protons, neutrons and electrons does this oxygen atom have?
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Chemistry A- Periodic Table Packet
3. Use your periodic table to list the period and group of each of the following elements:
a. Oxygen
b. Carbon
c. Fluorine
d. Sodium
e. Helium
4. What are some properties that metals have that non-metals do not have?
5. What did Dmitri Mendeleev contribute to chemistry?
6. What did Henry Mosely contribute to chemistry?
7. Use your periodic table to determine which of these is a metal and which is a non-metal:
a. Oxygen
b. Carbon
c. Fluorine
d. Sodium
e. Helium
8. Name the 7 metalloids:
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Chemistry A- Periodic Table Packet
EXTRA INFORMATON: Periodic Trends
Atomic Radius:
Unlike a ball, an atom does NOT have a fixed size. The electron cloud surrounding the nucleus is based
on probability and doesn’t have a clearly defined edge, so it is not possible to accurately measure its size.
Instead we measure how far away one atom is from another in a bond.
The radius of an atom can only be found by measuring the distance between the nuclei of two touching
atoms, and then halving that distance (dividing by 2). Atomic Radius is defined as half the distance between
nuclei of identical atoms that are chemically bonded together.
Trends within Periods and Groups:
A pattern in atomic size emerges as you look across a period (row). In general, there is a decrease in
atomic radii as you move left-to-right across a period. This trend is caused by the increasing positive charge in
the nucleus and the fact that the principle energy level within a period (row) remains the same. The increasing
number of protons in the nucleus as you go across the period pulls the electrons closer together. See image on p.
163.
Atomic radii generally increase as you move down a group. Electrons are added to larger energy levels
that are found farther away from the nucleus. Each energy level added is larger than the last resulting in a larger
atomic radius. See image on p. 163.
ON ANOTHER PIECE OF PAPER ANSWER these questions in COMPLETE sentences:
1. What trend in atomic radius do you see as you go down a group/family on the periodic table?
2. What causes the trend?
3. What trend in atomic radius do you see as you go across a period/row on the periodic table?
4. What causes the trend?
5. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.
6. Rank the following elements by decreasing atomic radius: krypton, polonium, cesium, indium
7. In each of the following pairs, circle the species with the larger atomic radius:
a. Li or Cs
b. Cl or Ar
c. Ca or Br
d. Na or Ne
e. B or Be
8. On the periodic table record in the space provided
whether the atomic radius INCREASES or
DECREASES as you go from left to right.
9. AND whether the atomic radius INCREASES or
DECREASES as you go down a column.
Ionization Energy:
To form a positive ion, an electron must be removed from a neutral atom. This requires energy. The
energy is needed to overcome the attraction between the positive charge in the nucleus and the negative charge
of the electron. Ionization energy- is defined as the energy required to remove an electron from a gaseous
atom. Think of ionization energy as an indication of how strongly an atom’s nucleus holds onto its valence
electrons. A high ionization energy value indicates that the atom has a strong hold on its electrons. Atoms with
large ionization values are less likely to form positive ions. A low ionization energy value indicates an atom
loses its outer electron easily forming a positive ion.
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The energy required to remove the first electron from an atom is called the first ionization energy. After
removing the first electron from an atom, it is possible to remove additional electrons. The amount of energy
needed to remove a second electron is called the second ionization energy, and so on.
Chemistry A- Periodic Table Packet
Trends within Periods and Groups:
Ionization energies generally increase as you move left to right across a period due to the increase in
nuclear charge. Ionization energies generally decrease as you move down a group. This occurs because atomic
size increases as you move down the group, thus the electron is further from the positive nucleus.
CONTINUE ON OTHER PAGE!
10. Define ionization energy.
11. Is it easier to form a positive ion with an element that has a high ionization energy or an element that has
a low ionization energy? Explain:
12. Why does fluorine have a higher ionization energy than iodine?
13. What trend in ionization energy do you see as you go down a group/family on the periodic table?
14. What causes this trend?
15. What trend in ionization energy do you see as you go across a period on the periodic table?
16. What causes this trend?
17. Circle the atom in each pair that has the greater ionization energy.
a. Li
Be
c. Cl
Si
e. P Ar
b. Na
K
d. Ca
Ba
f. Li
K
18. On the periodic table record in the space provided
whether the ionization energy INCREASES or
DECREASES as you go from left to right.
19. AND whether the ionization energy INCREASES or
DECREASES as you go down a column.
Electronegativity:
Electronegativity- is defined as the ability of an atom
to attract and hold electrons. Elements that commonly form negative ions have high electronegativities, while
low electronegativity correlates with the tendency to lose electrons and for positive ions.
Trends within Periods and Groups:
Electronegativity generally decreases as you move down a group, and increases as you move left-toright across a period. See image on p. 169.
CONTINUE ON OTHER PAGE:
20. Define electronegativity:
21. Circle the atom in each pair that has the greater electronegativity.
a. Ca
Ga
c. Cl S
e. Ba Sr
b. Li
O
d. Br As
f. O S
22. On the periodic table record in the space provided
whether the electronegativity NCREASES or
DECREASES as you go from left to right.
23. AND whether the electronegativity INCREASES or
DECREASES as you go down a column.
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24. What are the general TRENDS of atomic radius on the periodic table? On the arrows write I for
increasing or D for decreasing
Chemistry A- Periodic Table Packet
Explain why these trends occur:
25. What are the general TRENDS of ionization energy on the periodic table? On the arrows write I for
increasing or D for decreasing.
Explain why these trends occur:
26. What are the general TRENDS of electronegativity on the periodic table? On the arrows write I for
increasing or D for decreasing.
Explain why these trends occur:
27. For the following series of atoms: Cs, K, Mg, Al, P, S, Cl, rank the following properties from
LARGEST to SMALLEST:
a. Atomic Radius: ____________________________________
b. Ionization Energy: __________________________________
c. Electronegativity: ___________________________________
28. For the following pairs of atoms, fill in the blank with either < (less than) or > (greater than) to
correctly order the periodic trend:
i.
Atomic Radius:
Si ___ Cl
Br___I
Au___Hf
Co ___ S
ii.
Ionization Energy:
K___Cs
F___Ne
Mn ___ K
Pb ___ Po
iii.
Electronegativity:
Cl___I
O___F
Na___Mg
Rb
18
Revised 6/23/2017
Name: ________________________Hr:___
Chemistry A- Periodic Table Packet
19
Revised 6/23/2017