Chemistry A- Periodic Table Packet

Name: ______Hour: ______

Periodic Table

Extra Practice

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!

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 (1B-12B) 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.

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

alkali metal metalloid

alkaline earth metal Moseley

atomic mass noble gas

atomic number nonmetal

family period

group periodic law

halogen periodic table

lanthanide series transition element

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 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 called a(n) __(7)__, or, because of the resemblance between elements in the same column, a(n) __(8)__.

In rows 4 through 7, there is a wide central section containing elements, 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 the __(11)__, respectively. Each of these elements, as well as those in the first two columns at the left end of the chart, is classified as a(n) __(12)__. Each of the 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 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…

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.

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?

2.  What is an element?

3.  What are the vertical (up and down) columns of the periodic table called? ______

4.  What are the horizontal (back and forth) rows of the periodic table called? ______

5.  Which elements have similar properties, those in the same period or in the same family? ______

6.  How did Mosley improve the organization of the periodic table?

MORE ON THE NEXT PAGE…

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.

7.  What is a sub-atomic particle?

8.  What is the difference between a proton, a neutron and an electron?

9.  Are the protons and neutrons found inside or outside the nucleus?

10.  Are the electrons found inside or outside the nucleus?

11.  How many electrons does carbon have?

12.  How many protons does carbon have?

13.  How many neutrons does carbon have?

14.  What is the total positive charge of carbon?

15.  What is the total negative charge of carbon?

Mass and Atomic Number Review

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?

1. Lead has an atomic number of 82. How many protons? Electrons?

1. How many protons does Silicon have? Electrons?

1. An atom has a mass number of 42 and an atomic number of 39. How many neutrons does it have?

1. What is the mass number of calcium?

1. How many neutrons does calcium have?

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? ______
Practice with Ions

Learning Target Addressed:

1.7 I can describe the relationship between neutral atoms and ions of the same element.

Remember: The charge on an ion will involve a number and a sign. The number will always be the number of electrons involved, e.g., loss of two electrons is +2. The sign will be positive if electrons (negatives) are lost and negative if electrons are gained.

I. Determine the following charges

1. An atom having lost two electrons ______

2. An atom having lost six electrons ______

3. An atom having gained one electron ______

4. An atom having gained three electrons ______

5. An atom having lost five electrons ______

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 ______Circle one: CATION or ANION

2. Magnesium______Circle one: CATION or ANION

3. Aluminum______Circle one: CATION or ANION

4. Hydrogen______Circle one: CATION or ANION

5. Barium______Circle one: CATION or ANION

6. Sulfur______ Circle one: CATION or ANION

7. Argon______Why don’t noble gases form cations or anions?

III. Fill in the table below:

Practice with Isotopes

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.

1. What is an isotope? ______

______

2. What does the number next to isotopes signify (ie: Carbon 12 vs. Carbon 13)? ______

______

3. How can you tell isotopes apart in lab? ______

______

4.  Here are three isotopes of an element: 612C 613C 614C

a.  The element is: ______

b.  The number 6 refers to the ______

c.  The numbers 12, 13, and 14 refer to the ______

d.  How many protons and neutrons are in the first isotope? ______

e.  How many protons and neutrons are in the second isotope? ______

f.  How many protons and neutrons are in the third isotope? ______

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

6.  Complete the following chart:

Practice Calculating Average Atomic Mass

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.

For example, consider element X:

60% mass 40 amu,

30% mass 42 amu

10% mass 44 amu,

then the periodic table mass would be calculated:

.60 x 40 amu = 24.0 amu

.30 x 42 amu = 12.6 amu

.10 x 44 amu = 4.4 amu

average mass based upon relative abundance = 41.0 amu

Calculate the average atomic mass for the following isotopes.

The Nucleus: Crash Course in Chemistry #1

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)

The video above should help you answer the following questions:

1.  What is “stuff” made of?

2.  What are atoms?

3.  What are the three sub-atomic particles?

4.  What is atomic number AND why is it important?

5.  True or False: If the number of neutrons in a silver atom changes, then the atomic number changes.

6.  Do all silver atoms have the same number of neutrons? Explain!

7.  How to do you calculate the relative atomic mass of silver?

8.  What are the masses of the two isotopes (forms) of silver?

9.  LABEL mass and atomic number on the chemical symbol of silver to the right:

Answers

1.  Atoms

2.  Tiny discrete particles with specific properties (depending on the arrangement of their subatomic particles)

3.  Protons, Electrons and Neutrons

4.  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)