Unit 4: The Periodic TableChapter 6 in your book

Name VOCABULARY: PERIODIC TABLE

1. family or group: a (vertical) column on the periodic table2. period: a (horizontal) row on the periodic table.3. periodic law: when the elements are arranged in order by increasing atomic number, there is a repeated

pattern of their physical and chemical properties.4. noble gas: one of the gases in the 18th column of the periodic table. All are non-reactive due to having 8

valence electrons.5. halogen: any element in column 17 of the periodic table.6. alkali metals: elements in the 1st column of the periodic table.7. alkaline earth metals: elements in the 2nd column of the periodic table.8. transition metals: elements in columns 3-12 of the periodic table. Their compounds are often intensely

colored.9. inner transition metals: elements in the f-block, the separate section below the main part of the periodic

table.10. metals: elements on the left side of the periodic table. Excellent conductors of heat and electricity.11. non-metals: elements on the right side of the periodic table. Poor conductors of heat and electricity.12. metalloids: elements that are along the “staircase” of the periodic table (but not aluminum). Have

properties of both metals and non-metals.13. atomic radius: a measure of the size of an atom. (Measured as ½ the distance between adjacent nuclei

in a crystal.)14. electronegativity: indicates the ability of an atom to attract electrons in a chemical bond. Measured on

an arbitrary scale of 0-4. Metals, as “losers” tend to have low electronegativities. 15. cation: a positively charged ion; formed by loss of electrons. Metals form cations, since they are

“losers”16. anion: a negatively charged ion; formed by gain of electrons.17. ionic radius: a measure of the size of an ion. Measured as the distance from the nucleus to the outer

energy level of the ion.18. ionization energy: the amount of energy needed to remove a valence electron from a neutral gaseous

atom.19. reactivity: the tendency of an atom to react; how active it is. The most reactive metals are the best

“losers” while the most reactive non-metals gain electrons most readily.

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20. shielding: the number of energy levels between the nucleus and the valence electrons; the more energy levels between the nucleus and the valence electrons, the less “pull” they feel from the nucleus, so the more easily they are lost. Shielding is responsible for all vertical trends on the periodic table.

21. nuclear charge: the charge on the nucleus, caused by the protons in it. Nuclear charge = number of protons. Increasing nuclear charge is responsible for all horizontal trends on the periodic table.

22. allotropes: two or more different molecular forms of the same element in the same physical state. Example: O2 and O3 are allotropes of oxygen. S7 and S8 are allotropes of sulfur. Allotropes have different appearances and chemical properties due to differing structures.

Periodic Table and Trends:Enduring Understandings:Models change with advances in technology.Essential Questions: How can we classify matter? Where do elements come from? How are elements used in Industry and Society? Students will be able to answer the questions: How are elements organized on the periodic table? What information can be gained by knowing an element’s placement on the periodic table? Learning Targets: I can shall know/ be able to/ demonstrate:

1. State that the placement or location of elements on the periodic table gives an indication of physical and chemical properties of that element. Elements on the periodic table are arranged in order of increasing atomic number.

2. Describe the states of the elements at STP (standard temperature and pressure)3. Given the number of protons in an element, identify the element. 4. Use the mass number of an atom to identify an isotope. Interpret elements presented in the form

146C, 14C, carbon-14, and C-14. Be able to write isotopic notation.

5. Identify an element on the periodic table as a metal, nonmetal, metalloid (B, Si, Ge, As, Sb, Te) and noble gas.

6. Explain that the physical properties of elements, such as density, conductivity, malleability, solubility and hardness differ. Elements can be distinguished by their physical properties.

7. Explain that elements differ in their chemical properties. Chemical properties determine how an element behaves during a chemical reaction.

8. Identify different forms of the same element in the same phase, such as O3, and S8, as differeing in their molecular structure, and hence their properties.

9. Explain the placement of an unknown element in the periodic table based on its properties.10. Determine the group of an element, given the chemical formula of a compound, eg. XCl or XCl2.11. State that in groups 1,2 and 13-18 elements in the same column have the same number of valence

electrons (with the exception of helium) and therefore have similar properties. 12. Recognize that trends in properties exist across periods and within groups; these include trends in

atomic radius, ionic radius, electronegativity, first ionization energy, reactivity, and metallic/ nonmetallic properties.

13. Identify the trend (as increasing or decreasing) in atomic radius, ionic radius, electronegativity, first ionization energy, reactivity, and metallic/ nonmetallic properties within a group or period.

14. Recognize that compounds of transition metals are often intensely colored.

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Calendar for unit 4 Regents Chemistry: Blue (1 & 2B) and Green (8 & 7B) Classes11/19 20 21 22 23

B C NO SCHOOLPeriodic table of

hardware (double period)

Topic 4.1 Introduction to the periodic table HW: Assign#1 due MON.

Happy Thanksgiving!

11/26 27 28 29 30D E S A B

Periodicity of Elements POGIL

Periodic trends labHW: part of lab

Connecting the periodic table to the

atomPeriodic trends lab

Topic 4.2Periodic trends lab

HW: Assign#4.2

Topic 4.4HW: Assign#4.4

Topic 4.5 (summary) Alien Periodic Table/

Finish trends labHW: Assign#5 only

evens due test day (odd answers online)

Chemistry work period

Topic 4.3 Periodic Trends lab

Chemistry work period

12/3 4 5 6 7C D E S A

Review/ Makeup day

Chemistry work period

Periodic Table testCalendar for unit 4 Regents Chemistry: Yellow (5 &6A) class

11/19 20 21 22 23B C NO SCHOOL

Topic 4.1 Introduction to the periodic table HW: Assign#1 due MON.

Periodic table of hardware (double

period)

Happy Thanksgiving!

11/26 27 28 29 30D E S A B

Periodicity of Elements POGIL

Periodic trends labHW: part of lab

Connecting the periodic table to the

atomPeriodic trends lab

Topic 4.2Periodic trends lab

HW: Assign#4.2

Topic 4.3 Topic 4.4

Work time onPeriodic Trends lab

HW: Assign#4.4

Topic 4.5 (summary) Alien Periodic Table/

Finish trends lab HW: Assign#5 only evens due test day (odd

answers online) Chemistry work

periodChemistry work

period12/3 4 5 6 7

C D E S A Review/ Makeup Periodic Table test

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day Chemistry work

period

Development/ Organization of the Periodic table: How are the elements organized on the periodic table?

In the beginning, scientists only knew of the existence of a few elements. Only 13 elements had been identified by 1700. As the rate of discovery increased, scientists had to use of elements to sort them into groups

John Newlands was the first scientist to notice a .

Dimitri Mendeleev was the first person to publish a periodic table in 1869. Lothar Meyer, later that year, published an almost identical table. Mendeleev is usually given more credit because his table was published first. Mendeleev was trying to show his students the relationship among more than 60 elements. He wrote the properties of all the elements on which allowed him to move them around. He ended by arranging the elements in his periodic table in order of increasing .

In 1913 Henry Moseley determined the atomic numbers (or number of ____ ) in each element. The modern periodic table is arranged so that elements are in order of .

The states that elements are arranged in order of increasing atomic number, there is a periodic of their and

properties. Let’s label Group and Period #s on the table

Checkpoint Question: How many periods are there in a periodic table?

Sublevel (room type) # of orbitals (bunk beds)

Maximum # of electrons (occupants)

spd 5f 7

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Topic 4.1

Have you ever wondered why the periodic table looks so oddly shaped? Check out the size of the “blocks” that make up the different sections of the periodic table.

Element Bohr Configuration Schrodinger Configuration

Be

F

K

Fe

Kr

What are the different types of elements present on the periodic table?

There are three types of elements on the periodic table: Metal Properties: 1. Metals are good of heat and electricity

2. Metals are , and have a high __ _ ____ .

3. Metals electrons readily (are “losers”) to become positive ions ( ____ ).

4. Metals are at room temperature, except mercury which is a ____ .

Metals are found on the side of the periodic table.

Non-metal Properties:

1. Non-metals are conductors of heat and electricity. 2. Non-metals are not , , and don’t have

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13 14 15 16 17

18

Topic 4.1

3 4 5 6 7 8 9 10 11 12

2

. They are .

3. Non-metals readily electrons to become negative ions ( ___ ).

4. Most non-metals are or network solids at room temperature, except ____ which is a liquid.

Non-metals are found on the side of the periodic table, except , which is found in group 1 but is not a metal.

Metalloid Properties:

1. Has properties similar to metals and non-metals. Depending on the situation behaves as one or the other.

Metalloid elements are found on the of the periodic table, but and are not metalloids.

POGIL!

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Assignment 4.1

Periodic Table Basics: ***CHALLENGE*** remembering past units: Complete the following blanks using notes and what you remember from previous units & from your POGIL.

The periodic table is set up in rows called _______________ which go _______________ and columns called _______________ or _______________ and go _______________. Elements in the same _______________ possess similar ____________ _____________.

Atoms of the same element all contain the same number of _______________, which is their _______________ _______________. Atoms of the same element may possess different numbers of neutrons. This makes them _______________ of one another, and they have different _______________ because of their different numbers of _______________.

The masses shown on the periodic table are the average mass for each element, taking into account the _______________ and the relative _______________ of each _______________.

When atoms of the same element have different number of they are called isotopes. 6

12

C

and 6

13

C are isotopes; their atomic number ( ___ ) is the same, but their (total protons + neutrons) are different, indicating different numbers of ____________.

Atoms may tend to gain or lose electrons; when they do this they are .

Seven elements are Diatomic: _____,_____,_____,_____,_____,_____,_____. When these elements are uncombined with other elements, they travel in pairs.

Several other elements occur as _______________, meaning that their atoms are sometimes combined to form molecules with 3 or more atoms, these include ozone (____), and carbon (_____, __________, and graphite).

Elements are arranged on the periodic table in order of increasing _____ , which is the number of . All atoms of the same element have the same number of .

A row on the periodic table is called a . A column is called a or .

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Elements in the same group have the same number of electrons or electrons. These valence electrons participate in chemical reactions with other atoms.

Elements in the same period ( ) have the same number of . Example: Sodium has an electron configuration of and occupied energy levels. Phosphorus which is in the same as sodium has an electron configuration of and occupied energy levels.

When placed in order (by atomic number), certain properties show repeated patterns by period and group. STOP

How does placement on the periodic table and number of electrons relate to one another?

_

Elements can be sorted into ______more categories based on their placement on the periodic table.

Transition elements are shown in columns ____ -____.

Inner transition metals (also known as the _ and series) are shown ______ .

There are four other groups that have special names. These groups are based on or .

Alkali metals are in group ____ and are very with water.

Alkaline earth metals are in group ____ and relatively with water, but less than alkali metals. They are harder and have a melting point than them as well.

Halogens are in group ___ and are the most _____ .

Noble gases are in group ____. These are special because

_____ .

Compounds that contain transition elements are frequently _____ .

An atom becomes a positive ion when it electrons; it is then known as a _____ . A will be than the atom it’s derived from because _____ .

Atom Dot diagram: Ion Dot diagram:

An atom becomes a negative ion when it electrons; it is then known as an _____ . An will be than the atom it’s derived from because _____ .

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Topic 4.2

Atom Dot diagram: Ion Dot diagram:

When an element has valence electrons, it is very and _____ .

Checkpoint Questions:

1. Into what four classes can elements be sorted based on their electron configurations?

2. Why do the elements potassium and sodium have similar chemical properties?

3. Which of the follow elements are transition metals: Cu, Sr, Cd, Au, Al, Ge, Co?

4. How many valence electrons do all halogens have?

5. If you find an element in nature in it’s pure elemental state, what can you infer about the element’s chemical reactivity?

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Assignment 4.2

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Assignment 4.2

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Why do periodic trends occur?

ALL trends that occur across a period occur because of

. Every time you go one element to the right in a period, there is

one more in the nucleus. These protons are what attract the to the

nucleus. As you go across a period, electrons are also being . As you go across the

2nd period, all the electrons are added are filling in the 2nd energy level. The

nuclear charge attracts these electrons for each

element you move to the right.

ALL trend that occur down a group occur because of increased . As you go

down a group, there are more and more electrons; so many more that an additional energy

level is needed. For example the Bohr configuration of Sodium is and the Bohr

configuration of Potassium is . has an additional energy level. So,

the electrons being added are farther and farther away from the nucleus. Each additional

energy level added “shields” the valence electrons from the pull of the nucleus, so they are held

and strongly.

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Topic 4.3

How can we summarize the trends that occur on the periodic table?

Trends in element activity/ reactivity: Video!

The most active/ reactive metals are found at the of their column. This is because their electrons are the most loosely held, and thus easily lost—by reacting.

The most active/ reactive non-metals are found at the of their column. This is because they are the elements that most desire to gain electrons—by reacting.

Elements in group 1, 2 and 17 are all so reactive that they are found alone in nature. Noble gases are so that they are never found combined in nature.

Trends in Atomic Size: is one half of the distance between the nuclei of two atoms of the same element when the atoms are joined. Atomic radius is a measure of the of an atom and is measured in __ meters or .

Trends in Ionization Energy: Ionization Energy is the amount of needed to remove a from a neutral atom (in the gas phase). Energy required to remove the first electron from an atom is called the . The cation that is produced has a 1+ charge.

Since metals are happy to be “losers” it is fairly easy to remove electrons from them, so their ionization energy is compared to . Non-metals want to electrons and so have higher ionization energies.

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Topic 4.4

The purpose of gaining and losing electrons is to end up with __ valence electrons and a stable compound.

Trends in Electronegativity: Electronegativity is the of an element to when the atom is bonded to another atom. It is measured on a scale of 0-4.

Atoms that want to gain electrons (non-metals) have electronegativities. Atoms that readily lose electrons (metals) have electronegativities.

*Note that because noble gases are inert (extremely stable) they do not want to form bonds and therefore are omitted from the electronegativities shown.

All trends can be determined by looking at table S (also reviewed in trends lab and summarized later in this notes packet). Topic 4.3 explains WHY all trends occur.

The electronegativity values among the transition metals are not as regular.

The most electronegative atom on the periodic table is . The least electronegative atom is .

Checkpoint question: Why are values for noble gases omitted from the diagram on the previous page?

Trends in Ionic size: An ion is an atom or group of atoms that has a or charge.

Ions aren't the same size as the atoms they come from. Compare the sizes of sodium and chloride ions with the sizes of sodium and chlorine atoms.

Positive ions: Positive ions (cations) are than the atoms they come from. When a sodium atoms loses and electron it goes from 2,8,1 to Na+ with 2,8 and the attraction between the remaining electrons and the nucleus is increased. The electrons are drawn closer to the nucleus.

Negative ions: Negative ions (anions) are bigger than the atoms they come from. Chlorine is 2,8,7; Cl- is 2,8,8. As the number of electrons increases, the attraction of the nucleus for any one electron _ .

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Topic 4.4

con’t

Using the information about ionic size, what can we determine about the trends in ionic radius down

and across the periodic table?

Ionic radius is similar to atomic radius and _____ as you go down a _____

because .

Cations tend to loose or electrons as you go across the table

and therefore have ions.

Anions tend to electrons left to right. To determine ionic radius trends

across a period, the number of protons versus electrons must be determined to see which ion

pulls electrons closer to the nucleus making the radius smaller.

Checkpoint Questions:

1. How does atomic size change within groups and across periods?

2. When do ions form?

3. What happens to first ionizations energy within groups and across periods?

4. Compare the size of ions to the size of the atoms from which they form? (positive and negative)

5. How does electronegativity vary within groups and across periods?

6. Arrange these elements in order of DECREASING atomic size: sulfur, chlorine, aluminum, and sodium. Does your arrangement demonstrate a periodic trend or a group trend and why?

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Assignment 4.4

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How can we summarize the trends that occur on the periodic table?

# of energy levels ______Electronegativity ______ Ionization Energy ______Atomic radius ______Ionic Radius ______Metallic character ______

Nuclear charge ______Electronegativity ______ Ionization Energy ______Atomic radius ______Ionic Radius ______Metallic character ______

Metals in reactivity as you go down a group.Non-metals in reactivity as you go up a group.

1. As you move to the right in a period, the metals become reactive.

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Topic 4.5

2. As you move to the left in a period, the non-metals become reactive.

3. Which would you expect to be larger, Cl- or P3- and why? Cl- or I-

4. Which would you expect to be larger, K+ or Ga3+and why? Na+ or Rb+

5. Which of the following would you expect to have the largest atomic radius: Na, Rb, F or Sc?

6. Which of the following has the smallest 1st ionization energy: F, Cs, or Mg?

7. For which of the following element would you expect the 2nd ionization energy to be much greater than the 1st ionization energy: F, Sr, K, or C?*****Challenge question*******

Choose the correct answer for each question- complete the Why box if there is one. ONLY evens due day of test. Odd answers will be posted on Mrs. Young’s website.

1. Of the following elements, which one would have the largest electronegativity energy?

A.       Fluorine (F, atomic #9)B.       Bromine (Br, atomic #35)C.       Iodine (I, atomic #53)D.       Chlorine (Cl, atomic #17)

2. The elements with the largest atomic radii are found in the:

A.      upper right-hand corner of the periodic tableB.       upper left-hand corner of the periodic tableC.      lower left-hand corner of the periodic tableD.      lower right-hand corner of the periodic table

3. The most active metals are located in the:

A.       lower left hand corner of the periodic tableB.       upper right hand corner of the periodic tableC.       lower right hand corner of the periodic table

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Assignment 4.5

WHY?

WHY?

D.       upper left hand corner of the periodic table

4. Anions have a ______________ charge and are ______________ than the atoms from which they formed.

A.       negative/largerB.       negative/smallerC.       positive/smallerD.       positive/larger

5. The least electronegative elements are the:

A.      Metalloids     B. Noble gasesC.      Alkali metalsD.      Halogens

6.Given the representation of a chlorine atom, which circle might represent an atom of bromine?

A.       Circle BB.       Circle DC.       Circle CD.       None of these

7. The energy required to remove an electron from an atom is known as:

A.       electron affinityB.       electronegativityC.       ionization energyD.       radioactivity

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WHY?

Assignment 4.5

8.Given the representation of a chlorine atom, which circle might a chloride ion, Cl-?

A.       Circle BB.       Circle DC.       Circle CD.       None of these

9. Of the following elements, which one would have the smallest radius?

A.       Bromine (Br, atomic #35)B.       Iodine (I, atomic #53)C.       Chlorine (Cl, atomic #17)D.       Fluorine (F, atomic #9)

10. As one moves from left to right ( → ) within a period across the periodic table, the atomic radius of the elements encountered tends to:

A.      stay the sameB.      decreaseC.      increase

11. A horizontal row ( → ) of elements on the periodic table may also be referred to as a:

family

group

a.

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WHY?

WHY?

Assignment 4.5

period

12. As one moves from left to right ( → ) within a period across the periodic table, the electronegativity of the elements encountered tends to:

A.      stay the sameB.     decreaseC.     Increase

13. Given the representation of a chlorine atom, which circle might represent an atom of sulfur?

B.      Circle DC.      Circle BD.      Circle C

14. As one moves from down ( ↓ ) a group on the periodic table, the electronegativity of the elements encountered tends to:

A.  Decrease   B. stay the sameC. Increase

15. Of the following elements, which one would have the smallest radius?

A.       Lithium (Li, atomic #3)B.       Boron (B, atomic #5)C.       Neon (Ne, atomic #10)D.       Nitrogen (N, atomic #7)

E. 16. Of the following elements, which one would have the largest radius?

F.       Nitrogen (N, atomic #7)G.       Boron (B, atomic #5)H.       Neon (Ne, atomic #10)I.       Lithium (Li, atomic #3)

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WHY?

WHY?

Assignment 4.5

16. As one moves from left to right ( → ) within a period across the periodic table, the ionization energy of the elements encountered tends to:

A.       decreaseB.       increaseC.       stay the same

17. Generally speaking, the group of elements with the highest first ionization energy is:

A.       Group 1B.       Group 17C.       Group 16

18.Given the representation of a chlorine atom, which circle might represent an atom of bromine?

A.       Circle DB.       None of theseC.       Circle BD.       Circle C

19. As one moves from down ( ↓ ) a group on the periodic table, the ionization energy of the elements encountered tends to:

A.       increaseB.       decreaseC.       stay the same

20. Of the following elements, which one would have the smallest ionization energy?

A.       Neon (Ne, atomic #10)B.       Boron (B, atomic #5)C.       Lithium (Li, atomic #3)D.       Nitrogen (N, atomic #7)

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WHY?

WHY?

Assignment 4.5

21. Cations have a ______________ charge and are ______________ than the atoms from which they formed.

A.       positive/smallerB.       negative/largerC.       positive/largerD.       negative/smaller

22. Of the following elements, which one would have the largest radius?

A.       Cesium (Cs, atomic #55)B.       Potassium (K, atomic #19)C.       Hydrogen (H, atomic #1)D.       Sodium (Na, atomic #11)

23.Which of these elements would have the lowest first ionization energy?

A.       Element CB.       Element AC.       Element BD.       Element D

24. The elements with the smallest atomic radii are found in the:

A.      lower left-hand corner of the periodic tableB.     lower right-hand corner of the periodic tableC.      upper right-hand corner of the periodic tableD.      upper left-hand corner of the periodic table

25. A vertical column ( ↓ ) of elements on the periodic table may also be referred to as a: (select 2)

group

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WHY?

WHY?

period

family

c.

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