Chemistry A- Periodic Table Packet s1

Chemistry A: Periodic Table Packet Name: ______Hour: ____ Page 1

Chemistry A Periodic Table Chemistry A: Periodic Table Packet Name: ______Hour: ____ Page 2 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 Here is a close-up of the element carbon symbol for carbon, an element that is very if we could see it under a very powerful common and we will study about this microscope: trimester: KEY Atomic Number p = proton n = neutron Mass Number = electron

Nucleus

6. Are the protons and neutrons foundThe inside electron or cloud outside is the nucleus? made of “shells” that hold the electrons. Carbon has 2 shells and 7. Are the electrons found inside or outside the nucleus? is in the 2nd row of the periodic table. 8. How many electrons does carbon have?

9. How many protons does carbon have?

10. How many neutrons does carbon have?

11. What is the total positive charge of carbon? These + and – charges “cancel out” making a 12. What is the total negative charge of carbon? 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) Chemistry A- Periodic Table Packet Name: ______Hr:___ 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) Electron – negative charge Neutron – no # of charge (neutral) shells= Proton – positive charge row of periodic table 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

bigge Atomic Number = # of r protons. smalle r 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.

Complete the following table: (+) charge + (-) charge = 0 Particle Name Charge Mass Location in Atom What tells you how many are in an atom? PROTON

ELECTRON NEUTRON

4 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___

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?

5 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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) What are the vertical (up and down) columns of the periodic table called? ______2) What are the horizontal (back and forth) rows of the periodic table called? ______3) Which elements have similar properties, those in the same period or in the same family? ______4) 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.

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 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 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)__. 11. ______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 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 15. ______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 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)__.

7 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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)

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 Group 1 18

Group Group Group Group Group Group H 2 13 14 15 16 17 He

Be B C N O F

Group Group Group Group Group Group Group Group Group Group 3 4 5 6 7 8 9 10 11 12

Sc Ti V Cr Mn Fe Co Ni Cu Zn

9 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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.

La Ac 95 96 97 98 99 100 101 102 103 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.

10 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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.

11 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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.

12 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ Periodic Table Review Sheet 1. On the periodic table below, label all of the following: a. Metals e. Noble gases h. Actinide series b. Transition metals f. Halogens i. Metalloids c. Alkali metals g. Lanthanide series j. nonmetals d. Alkaline metals

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

13 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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?

14 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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?

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:

16 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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. 17 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 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.

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-to- right 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.

18 Revised 4/23/2018 Chemistry A- Periodic Table Packet Name: ______Hr:___ 24. What are the general TRENDS of atomic radius on the periodic table? On the arrows write I for increasing or D for decreasing

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.

26. What are the general TRENDS of electronegativity on the periodic table? On the arrows write I for increasing or D for decreasing.

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

20 Revised 4/23/2018