Starter: Breaking Down Misconceptions

Determine which of the following are true or false. Justify the statements you consider to be false.

1.The Modern Periodic Table organizes the elements based on atomic weight (mass).

2.Longitude is to GROUPS as Latitude is to PERIODS.

3.Although over 100 elements are found on the Periodic Table, several of them do not really exist.

Mendeleev Activity (The Hoya Table)

Organize yourselves into columns according to your similar physical properties and rows based on your age.

Mendeleev and Moseley will facilitate. All students should help!

The only rule is that Girls must be on the left side of the room and Boys on the left. The middle row can be mixed.

Possible properties that you could use: shirt color, hair color, glasses, shoe types, shirt type

You have 8 minutes to get as many of your classmates seated as possible. May the best Hoya Table win!

Pre-Periodic Table Chemistry ……was a mess!!!No organization of

elements.Imagine going to a

grocery store with no organization!!

Difficult to find information.

Chemistry didn’t make sense.

History of the Periodic Table: Mendeleev vs Moseley

MENDELEEV MOSELEYArranged the

elements by increasing ATOMIC WEIGHT

Put elements in columns by the way they reacted.

He left blank spaces for what he said were undiscovered elements. (Turned out he was right!)

Developed a new understanding of periodic law and REVISED Mendeleev’s organization of the PT

Realized that atomic mass (weight) was NOT as important in the organization of the elements as the ATOMIC NUMBER

Arranged the elements in order of increasing ATOMIC NUMBER

Background: The Periodic LawThe Periodic Law states that there is a recurring pattern in the PROPERTIES of elements when they are arranged in order of INCREASING ATOMIC NUMBER.

This pattern can be seen every 8 representative elements

The Periodic Road MapGROUPS PERIODS

Groups are the COLUMNS found on the PT

Elements in the same GROUP:

Apart of the same FAMILYHave the SAME number of

valence electronsForm the same kinds of IONSWhat would this say about

their properties?They demonstrate SIMILAR

properties

Periods are the ROWS on the PT

There are 7 periods on the PT that represent the 7 principal energy levels within the atom

Elements in the same PERIOD:

Valence Electrons exist within the SAME principal energy level

What BLOCK do you stay on?The PT can also be broken down into a

BLOCK SYSTEMElements on the PT reside in certain blocks

which are reflected at the end of their electron configuration

The block system is based on the SUBLEVELS that electrons can be found in within the atom. What are they?

S, P, D, F

What BLOCK do you stay on?

S block: blue D block: red

P block: yellow F block: green

To Be or Not To Be…Elements on the PT are either Metal, Non-metal

or MetalloidThese differences affect the properties of the

elements

METALS: solid at room temp, tend to LOSE electrons to become more stable (+ IONs), on the LEFT SIDE of the PT, good conductors of energy

NON-Metals: typically your gases, tend to GAIN electrons to become more stable (- IONs), on the RIGHT SIDE of the PT, poor conductors of energy

METALLOIDS: found in between metals and non-metals and so are their properties, on the STAIRCASE in the middle right of the table

To Be or Not To Be…

Metals = Blue Metalloids = Pink Non-metals = Yellow

Starter: PT Anatomy CFUExplain the difference between

Mendeleev’s and Moseley’s organization of the Periodic Table.

What are the columns and rows on the Periodic Table called and what information can you pull from them?

Which element would conduct electricity better, Phosphorus or Sodium? Why?

Families on the Periodic TableElements on the periodic table can be grouped into

families bases on their chemical properties.Each family has a specific name to differentiate it from

the other families in the periodic table.Elements in each family have a stronger reactions as

you move down the table. Why?Their valence electrons have more energy (on a higher

energy level)

ALKALI METALSGroup 1Hydrogen is not a member,

it is a non-metal1 electron in the outer shellSoft and silvery metalsVery reactive, esp. with

waterConduct electricity

Image: http://www.learner.org/interactives/periodic/groups2.html

ALKALINE EARTH METALSGroup 22 electrons in the

outer shellWhite and

malleableReactive, but less

than Alkali metalsConduct

electricity

TRANSITION METALSGroups in the

middle

Good conductors of heat and electricity.

Some are used for jewelry.

The transition metals are able to put up to 32 electrons in their second to last shell.

Can bond with many elements in a variety of shapes.

BORON FAMILY Group 33 electrons in

the outer shellMost are metalsBoron is a

metalloid

CARBON FAMILY Group 44 electrons in

the outer shellContains

metals, metalloids, and a non-metal Carbon (C)

NITROGEN FAMILY Group 55 electrons in

the outer shellCan share

electrons to form compounds

Contains metals, metalloids, and non-metals

OXYGEN FAMILY Group 66 electrons in

the outer shellContains

metals, metalloids, and non-metals

Reactive

HalogensGroup 77 electrons in

the outer shellAll are non-

metalsVery reactive

are often bonded with elements from Group 1

Noble GasesGroup 8Exist as gasesNon-metals8 electrons in

the outer shell = Full

Helium (He) has only 2 electrons in the outer shell = Full

Not reactive with other elements

Do NOT lose or gain electrons; They’re already stable

Rare Earth Metals: Lanthanides and Actinides

Some are Radioactive

The rare earths are silver, silvery-white, or gray metals.

Conduct electricity

Can also be called Inner Transition Metals

Periodicity Part II: TRENDSYou must know the following trends for on

the PT:1.Atomic Radius2.Ionic Radius3.Electronegativity4.Ionization Energy

Trend 1: Atomic RadiusAtomic Radius is A measure of the size of the atomhalf of the distance between the

centers of two atoms of that element that are just touching each other

Measured from the nucleus to the boundary of the farthest (highest) energy level for the valence electrons

Trend 2: Ionic RadiusIonic Radius is…A measure of the size of the ionhalf of the distance between the

centers of two atoms of that element that are just touching each other

Measured from the nucleus to the boundary of the farthest (highest) energy level for valence electrons

Trend 3: ElectronegativityElectronegativity is…a measure of the tendency of an atom to attract electrons

the desire an atom has for electrons in a bond

Similar to Electron Affinity

Trend 4: Ionization EnergyIonization energy is the amount of energy REQUIRED to remove an electron from an atom

The Trends…What you need to know

Know what each trend meansHow they change as you move to the…

1.Right and left of a period2.Up and down a groupBe able to compare the elements according to the trends

PT Trends ActivityPeriodic Table Trends Mendeleev’s Castle

Google: PT Trends lynchburg

Click on Cool PTUse the information

that you find when you click on each element to complete the WS

Important: You will have a quiz on this on Friday!

Complete the activity and correctly answer the questions

Important: This assignment is due at the end of class!

Starter: Analyzing TrendsExplain the difference between the

4 trends on the Periodic Table.Does Sodium or Chlorine have a

higher electronegativity?Does Copper or Gold have a higher

atomic radius?Does Potassium or Xenon have a

higher 1st Ionization energy?

Analyzing TrendsImportant: When analyzing a trend for elements in different groups and different periods…

1.consider the trend going down the group

2.consider the trend going across the period.

Analyzing the TrendsAtomic Radius Ionic RadiusIncreases as you move

DOWN the PTWhy? You’ve added more

energy levelsDecreases as you move

to the RIGHT of the PTWhy? The force of the

nucleus is stronger and it pulls the electrons closer

Increases as you move DOWN the PT

Why? You’ve added more energy levels.

As you move across the PT…- Decreases for Metals

because they tend to _______ electrons. (+ Ion = Cation)

- Increases for Non-metals because they tend to _______ electrons ( - Ion = Anion)

Analyzing the TrendsElectronegativity Ionization Energy

Decreases as you move DOWN the PT

Why? The attraction of the positive nucleus decreases as the shell gets farther.

Increases as you move to the RIGHT across the PT

Why? Elements want electrons more and more to become more stable.

Decreases as you move DOWN the PT

Why? Electrons are farther out from the nucleus which has less of a hold; more likely to get taken because it takes less energy

Increases as you move to the RIGHT across the PT

Why? As you move to the right the elements really want to keep their electrons so it requires more energy to take them.

Diatomic MoleculesWhy do atoms form ions?

To Become More STABLE!Well…a few elements can also do something

else to become stable.They come together and share electrons (or

BOND) with each other. They are called DIATOMIC MOLECULES.

Here are the Diatomic Molecules (Pay attention to which elements can form Diatomic Molecules!)

N2, O2, F2, Cl2, H2, Br2, & I2

Starter:Which is larger Ra or Ra+2 ? I or I-? Why?Identify at least 1 element in the

following families and what kind of ions they would form: Halogen, Alkali metals, Alkaline earth metals

Bromine has less Ionization energy and less Electronegativity than Fluorine. Explain why this is.

Which would have a more violent reaction to the same stimuli, Potassium or Francium? Why?

Introduction to Halide Lab:In this lab, you will explore ions of the

elements in Group 7A. Which family will you be observing?

Your objective is to mix the solutions containing these ions with Silver Nitrate and Lead Nitrate.

Record your observations in the data table provided. You may write on the lab handout.

While in the lab area, be sure to wear your goggles and apron at all times.

This assignment is graded and will be turned in today, so be sure to stay on task!

Halide Lab (Important Information):

Once you have completed the lab and cleaned your lab area, put your safety materials away and begin to answer the Analysis questions.

You are responsible the following questions: 2, 3 (excluding the equation portion), 4, and the question below

Based on your understanding of families on the Periodic Table, which halide ion would you expect to have the most reactivity in this experiment? Least reactivity? Why?

Focus of Study:Know the history of the PT (Mendeleev vs Moseley)Know the organization of the PT (sublevel blocks,

groups, periods, Metals vs Metalloids vs Nonmetals)

Know the difference between GROUPS (FAMILY) and PERIODS; How to determine them…

(Groups – same valence e- = similar activity/properties and types of IONS; Periods – principal (valence) energy level)

Know the 4 trends and their meaning- Be able to explain WHY the trends occur as they do

Starter: Do You Know the PTWhat is the valence energy level and

number of valence electrons in Silicon?Does Copper, Gold, or Cadmium have a

higher atomic radius?Does Cesium, Barium, or Francium have

a lower 1st ionization energy?Does Oxygen, Sulfur or Fluorine have a

higher electronegativity?