Download Periodic Table Extra Practice ANSWER KEY 2014

Name: _________________________________
Hour: ______
Periodic Table
Extra Practice
ANSWER KEY
Need more practice? Not sure how to study for a test or quiz?
Reviewing for the final exam?
The following worksheets are organized by learning targets, so
you can pick and choose which to complete or do them all!
Name: _________________________________
Hour: ______
Periodic Table Unit Learning Targets
Learning Targets 1.1, 1.5 and 1.12 will be assessed on quizzes, but not the unit test.
1.1 I can write the names and symbols of the elements in columns 1A – 4A on the periodic table.
1.5 I can write the names and symbols of the elements in columns 5A- 8A on the periodic table.
1.12 I can write the names and symbols of selected transition metals, lanthanides and actinides (1B12B) on the periodic table.
LT 1.2 I can describe how Mendeleev and Moseley organized the periodic table into groups with
similar properties.
LT 1.3 I can label and describe the major groups (families) of the periodic table: alkali metals,
alkaline metals, transition metals, halogens, noble gases, metals, non-metals and metalloids
LT 1.4 I can describe the charge and location of protons, neutrons, and electrons within the nucleus
and shells of an atom.
LT 1.6 I can calculate the number of protons, electrons and neutrons if given the mass and atomic
number of an element.
LT 1.7 I can describe the relationship between neutral atoms and ions of the same element.
LT 1.8 I can explain the relationship between isotopes of the same element.
LT 1.9 I can calculate the number of protons, electrons and neutrons in ions and isotopes of the
same element.
LT 1.10 I can explain the difference between mass number and average atomic mass.
LT 1.11 I can calculate average atomic mass.
Name: _________________________________
Hour: ______
Fill in the Blanks Review
Learning Targets Addressed
1.2 I can describe how Mendeleev and Moseley organized the periodic table into groups with similar properties.
1.3 I can label and describe the major groups (families) of the periodic table: alkali metals, alkaline metals, transition metals,
halogens, noble gases, metals, non-metals and metalloids
Directions: Fill in the blanks on the right with the information in the chart below.
Word List
actinide series
metal
1.
alkali metal
metalloid
alkaline earth metal
Moseley
2.
atomic mass
noble gas
atomic number
nonmetal
3.
family
period
4.
group
periodic law
halogen
periodic table
5.
lanthanide series
transition element
6.
Dmitri Mendeleev developed a chart-like arrangement of the elements
called the __(1)__. He stated that if the elements were listed in order of increasing
__(2)__, their properties repeated in a regular manner. He called this the __(3)__
of the elements. The arrangement used today, devised by __(4)__, differs from
Periodic Table
Atomic Mass
Periodic Law
Moseley
Atomic Number
Period
7. Group
8. Family
9. Transition Element
that of Mendeleev in that the elements are arranged in order of increasing __(5)__.
10. Lanthanide Series
Each horizontal row of elements is called a(n) __(6)__. Each vertical column is
11. Actinide Series
called a(n) __(7)__, or, because of the resemblance between elements in the same
12. Metal
column, a(n) __(8)__.
In rows 4 through 7, there is a wide central section containing elements,
13. Nonmetal
each of which is called a(n) __(9)__. Rows 6 and 7 also contain two other sets of
14. Metalloid
elements that are listed below the main chart. These are called the __(10)__ and
15. Alkali Metal
the __(11)__, respectively. Each of these elements, as well as those in the first two
16. Alkaline Earth Metal
columns at the left end of the chart, is classified as a(n) __(12)__. Each of the
17. Halogen
elements at the right side of the chart is classified as a(n) __(13)__. Each of the
elements between these two main types of elements, having some properties in
18. Noble Gas
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)__.
MORE ON THE NEXT PAGE…
Name: _________________________________
Hour: ______
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? The elements have similar
properties like members of a family have similar traits.
2. What is the definition of a metal? An element that loses one or more electron to create a
positively charged ion called a cation.
3. What is common table salt made of? sodium and chlorine
4. What is an unusual property of the alkaline earth metals? They dissolve better in cold water
than hot water.
5. Why don’t noble gases react with other elements? They already have the desired eight
electrons in their outermost shell.
6. What does the world “halogen” mean? Salt-former
7. What is the definition of a non-metal? An element that accepts electrons to form a desired
octet (a full outer shell)
8. What is the most reactive element? Fluorine
9. Label the periodic table below with: lanthanide series, actinide series, transition metals, alkali
metals, alkaline metals, halogens, noble gases.
Name: _________________________________
Hour: ______
Basic Atomic Structure Review
Learning Target Addressed:
1.4 I can describe the charge and location of protons, neutrons, and electrons within the nucleus and shells of an atom.
The periodic table is, in many ways, the world’s greatest cheat sheet. 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 table was created a long time ago by a guy named Dmitri Mendeleev who, probably like you,
did not want to memorize tons of information. He organized the elements by mass. That worked pretty well to group
elements with similar properties together. Soon after a guy named Henry Moseley realized that each element has a
specific number of protons. We call this the atomic number of the element. When he rearranged the periodic table by
atomic number the elements grouped into columns with similar properties.
Questions:
1.
Who created the first periodic table? Mendeleev
2.
What is an element? A simple substance that makes up more complex materials.
3.
What are the vertical (up and down) columns of the periodic table called? Groups (or families)
4.
What are the horizontal (back and forth) rows of the periodic table called? Periods
5.
Which elements have similar properties, those in the same period or in the same family? Family
6.
How did Mosley improve the organization of the periodic table? Organized by mass instead of atomic #
MORE ON THE NEXT PAGE…
Name: _________________________________
What makes up each element?
Hour: ______
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.
7.
What is a sub-atomic particle? The parts that make up an element.
8.
What is the difference between a proton, a neutron and an electron? Protons are positive, neutrons are neutral
and electrons are negative.
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
9.
Are the protons and neutrons found inside or outside the nucleus? INSIDE
10. Are the electrons found inside or outside the nucleus? OUTSIDE
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.
11. How many electrons does carbon have? 6 (same as the # of protons)
12. How many protons does carbon have? 6 (equal to the atomic number)
13. How many neutrons does carbon have? 12-6 = 6
14. What is the total positive charge of carbon? + 6 (from the protons)
15. What is the total negative charge of carbon? – 6 (from the electrons)
These + and – charges
“cancel out” making a
neutral carbon atom.
Name: _________________________________
Mass and Atomic Number Review
Hour: ______
Learning Target Addressed:
1.6 I can calculate the number of protons, electrons and neutrons if given the mass and atomic number of an element.
1. Carbon has 6 protons. How many electrons does it have? 6
2. Lead has an atomic number of 82. How many protons? Electrons? 82 protons and 82 electrons
3. How many protons does Silicon have? Electrons? 14 protons and 14 electrons
4. An atom has a mass number of 42 and an atomic number of 39. How many neutrons does it have?
42-39 = 3 neutrons
5. What is the mass number of calcium? 40 (round the number on the periodic table)
6. How many neutrons does calcium have? 40-20 = 20 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 “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? It is equal to the atomic number
How do you determine the number of electrons? It is equal to the number of protons
How to you determine the number of neutrons? Mass number – atomic number = # neutrons
Name: _________________________________
Practice with Ions
Hour: ______
Learning Target Addressed:
1.7 I can describe the relationship between neutral atoms and ions of the same element.
I. Determine the following charges
1. An atom having lost two electrons
2. An atom having lost six electrons
+2
When you get rid of
“negatives” it makes
you more positive.
Same for atoms!
+6
3. An atom having gained one electron - 1
4. An atom having gained three electrons - 3
5. An atom having lost five electrons
+5
II. Determine the charges on the following elements based on their locations on the
periodic table. Then circle if each ion is a cation or an anion.
1. Fluorine -1 Circle one: CATION or ANION
2. Magnesium + 2 Circle one: CATION or ANION
3. Aluminum +3 Circle one: CATION or ANION
4. Hydrogen +1 Circle one: CATION or ANION
5. Barium +2 Circle one: CATION or ANION
6. Sulfur -2 Circle one: CATION or ANION
7. Argon 0 Why don’t noble gases form cations or anions? They have a full octet (8 electrons in outer
shell)
III. Fill in the table below:
Ion
# of
protons
Atomic #
Mass #
# of neutrons
F-1
9 (on table)
19
(round #
on table)
9 (same as
atomic #)
10 (mass –
atomic #)
# of electrons
9 +1 =10 (#
protons plus
or minus the
charge)
Li+1
3
7
3
4
2
S-3
16
32
16
16
19
O-2
8
16
8
8
10
Na+1
11
23
11
12
10
B+3
5
11
5
6
2
Name: _________________________________
Practice with Isotopes
Hour: ______
Learning Target Addressed
1.8 I can describe the relationship between isotopes of the same element.
Isotopes are atoms of the same element with different masses (or weights) due to different numbers of neutrons
in their nuclei. All atoms of the same element must have the same number of protons (and thus the same number of electrons)
which is equal to the atomic number. However, atoms of the same element can have different numbers of neutrons and thus a
different mass number. The difference in mass does not influence the chemical behavior. Valence electrons are what determine
chemical behavior.
Hydrogen has three isotopes. The most abundant isotope is ordinary hydrogen-1. A second stable isotope is hydrogen-2 and the
third isotope is the radioactive hydrogen-3. The Bohr diagrams for the isotopes of hydrogen are shown below. Notice that
only the mass number and number of neutrons are different.
Hydrogen-1
Hydrogen-2
Hydrogen-3
K
K
K
1
2
3
1p
1p
1p
1H
1H
1H
1n
2n
1e
1e
1e
1. What is an isotope? Atoms of the same element with different masses due to different number of neutrons in the
nuclei
2. What does the number next to isotopes signify (ie: Carbon 12 vs. Carbon 13)? The mass (protons + neutrons)
3. How can you tell isotopes apart in lab? They have different masses (weights)
4. Here are three isotopes of an element:
12
6 C
13
6
C
14
6
C
a. The element is: Carbon
b. The number 6 refers to the _Atomic Number (or the number of protons)
c. The numbers 12, 13, and 14 refer to the _Mass Number (or the protons + neutrons)
d. How many protons and neutrons are in the first isotope? 6 protons, 6 neutrons
e. How many protons and neutrons are in the second isotope? _6 protons, 7 neutrons
f.
How many protons and neutrons are in the third isotope? 6 protons, 8 neutrons
5. Write the symbols for the isotopes of uranium with the following numbers of neutrons:
a. 142 neutrons
b. 143 neutrons
c. 146 neutrons
MORE ON THE NEXT PAGE
Name: _________________________________
Hour: ______
6. Complete the following chart:
Isotope name
Atomic #
# of
protons
Mass #
# of neutrons
# of electrons
Uranium-235
92
235
92
143
92
Uranium-238
92
238
92
146
92
Boron-10
5
10
5
5
5
Boron-11
5
11
5
6
5
Carbon – 12
6
12
6
6
6
Carbon – 14
6
14
6
8
6
Tin – 119
50
119
50
69
50
Tin – 120
50
120
50
70
50
Lithium – 7
3
7
3
4
3
Sodium – 23
11
23
11
12
11
Name: _________________________________
Practice Calculating Average Atomic Mass
Hour: ______
Learning Target Addressed: 1.11 I can calculate average atomic mass.
The atomic masses (or atomic weights) on the periodic table are the average of all the isotopes but it is not
a straight average. The atomic masses on the periodic table are the averages of all the isotopes based upon
abundance.
Calculate the average atomic mass for the following isotopes.
Name: _________________________________
The Nucleus: Crash Course in Chemistry #1
Hour: ______
Learning Targets Addressed:
LT 1.4 I can describe the charge and location of protons, neutrons, and electrons within the nucleus and shells
of an atom.
LT 1.6 I can calculate the number of protons, electrons and neutrons if given the mass and atomic number of
an element.
https://www.youtube.com/watch?v=FSyAehMdpyI (10:12) – You can google the title of this worksheet
The video above should help you answer the following questions:
1. What is “stuff” made of? Atoms
2. What are atoms? Tiny discrete particles with specific properties (depending on the
arrangement of their subatomic particles)
3. What are the three sub-atomic particles? Protons, Electrons and Neutrons
4. What is atomic number AND why is it important? The number of protons in an atom. It is
important because it determines what element it is (79 protons always means Gold and
47 means Silver)
5. True or False: If the number of neutrons in a silver atom changes, then the atomic
number changes. FALSE! As long as the number of protons stays the same so does the
atomic number.
6. Do all silver atoms have the same number of neutrons? Explain! No, some have 60
neutrons and others have 62 neutrons.
7. How to do you calculate the relative atomic mass of silver? Add the number of protons +
neutrons and average it across all the silver atoms on earth
8. What are the masses of the two isotopes (forms) of silver? Silver- 107 and Silver - 109
9. LABEL mass and atomic number on the chemical symbol of silver to the right:
Name: _________________________________
Hour: ______
What’s in the Box? Interactive
Learning Targets Addressed:
LT 1.3 I can label and describe the major groups (families) of the periodic table: alkali metals, alkaline metals, transition
metals, halogens, noble gases, metals, non-metals and metalloids
LT 1.8 I can describe the relationship between isotopes of the same element.
LT 1.11 I can calculate average atomic mass.
Part 1: What’s in the Box
1. Horizontal rows of the periodic table are called periods
2. How does the period of an element is in relate to its structure? The period equals the number of
energy levels or shells around the nucleus
3. How many periods are there on the periodic table? 7
4. Columns of the periodic table are called groups or families.
5. How many groups are there on the periodic table? 18
6. What does the atomic number of an element represent? The number of protons
7. What happens if you add a proton to carbon? It becomes nitrogen (the next element over)
8. Why do some elements have symbols that don’t look anything like their names? (Example Lead is
Pb and Sodium is Na)? They refer to older (latin) names for the elements
9. The mass of an element is the number of protons + neutrons found in the nucleus.
10. The average mass listed on the periodic table is the average mass of all the isotopes of an atom.
11. What was your score on the “Which one of these elements doesn’t belong” game? + ____/10
Hints for the game: Use a periodic table. “Belong” means to have similar properties.
12. Label the symbol for hydrogen with the terms “atomic number” and “average mass”
Name: _________________________________
Part 2: Isotopes, a Weighty Matter
Hour: ______
1. Which isotope of carbon is most common?
Carbon - 12
2. Considering the graph to the right, what would
the average mass of carbon be closest to?
a. 12
b. 13
c. 14
Part 3: Isotopes Quiz **Select “Skip Question” to see the first question** Weird, I know.
Show your work and box your final answer for each question. If you need more space, use another
sheet and attach it to this worksheet.
Name: ________________________Hr:___
Chemistry A- Periodic Table Packet
15
Revised 6/17/2017