icp: periodic table icp: periodic table infinite campus update: nuclear chemistry and electron...

ICP: Periodic TableICP: Periodic Table

Infinite Campus Update:•Nuclear Chemistry and Electron Arrangement Exam (33pts.)

Objectives: •I can classify elements as metals, non-metals, and metalloids.•I can classify elements based on the number of valence electrons.

Periodic Table: Locating Periodic Table: Locating ElementsElements•Classify elements as metals, non-metals, and metalloids.

Periodic Table: Locating Periodic Table: Locating ElementsElementsPeriods:

•Elements in the same row.

Groups: • Elements in the same column. • Have similar chemical properties.

Periodic Table : Bell Ringer1. a. What period and group is Aluminum on? b. What element is in period 4; group 2 ?

2. Circle the elements below that have similar chemical properties.

Carbon (C), Nitrogen, (N), Silicon (Si), Boron (B)

3.Classify the following as either a metal(M), non-metal (NM), or metalloid (MET)

a. H b. Si c. Al d. Sn e. Ar

ICP 12.2: Periodic TableICP 12.2: Periodic Table

Infinite Campus Update:•Nuclear Chemistry and Electron Arrangement Exam (33pts.)

Objectives: •I can classify elements as metals, non-metals, or metalloids.•I can classify elements based on the number of valence electrons.

Metallic vs. Non-metallic Metallic vs. Non-metallic PropertiesProperties

Periodic Table and Periodic Table and Groups Groups

Why do elements in the same group have similar chemical properties?

Periodic Table Lab: Group Periodic Table Lab: Group Patterns Patterns

Lab grps

grp 1ve-

grp 2 ve-

grp 13 ve-

grp 14ve-

grp 15 ve-

grp 16ve-

grp17ve-

grp18ve-

1. Li Be B C N O F Ne

2. Na Mg Al Si P S Cl Ar

• Count the number of electrons on the highest energy level and record in table above• Conclusion:


Valence Electrons: Electrons on the highest energy level.Elements in the same group have the same

number of valence electrons (why similar chemical properties).

ICP 12.9: Periodic TableICP 12.9: Periodic TableDue:Periodic Table Worksheet Infinite Campus Update:•Bohr’s model and valence electrons worksheet (10pts.)•Periodic Table: Bell Ringer (3pts.)•Periodic Table: Bell Ringer (7pts.)Objectives: •I can classify elements as metals, non-metals, or metalloids.•I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.

Homework:Check infinite campus of missing assignments/exams

Common Periodic Table Common Periodic Table GroupsGroupsPeriodic Groups Group # Valence

Electrons

Chemical Reactivity (Yes or No)

Alkali Metals

Alkaline-Earth Metals

TransitionalMetals

Halogens

Noble Gases(Inert Gases)


Transitional Groups: Short groups. Representative Groups: Tall groups

ICP 12.10: Periodic TableICP 12.10: Periodic Table

Objectives: •I can classify elements as metals, non-metals, or metalloids.•I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table. •I can predict the charge for an element when it is stable.

Homework:Check infinite campus of missing assignments/exams

Periodic Table Groups Check-up

1. Identify an element from each group below. a. Noble Gasesb. Alkali Metalsc. Alkaline Earth Metalsd. Transitional Metalse. Halogensf. Representative Element

2. a. Which group from above is most stable? b. Which metallic group above is most

reactive? c. Which non-metallic group above is most

reactive?

Chemical StabilityChemical StabilityOctet Rule: Atoms will gain or lose valence electrons to

reach maximum stability. Formation of ions.What is maximum stability for most

atoms? 8 valence electrons (ve-)Exceptions: H and He max. stability = 2 ve-

How do atoms achieve stability ? Atoms chemically bonding with other atoms.Formation of diverse compounds in nature.

Chemical Stability Chemical Stability PatternPattern

Metals tend to lose valence electrons to reach stability.

Non-metals tend to gain valence electrons to reach maximum stability?

Chemical Stability Chemical Stability PatternPatternMetals:Will lose ve- to reach stability.Form cations (+ charged atoms)

Non-metals: Will gain ve- to reach stability.Form anions (- charged atoms)

Chemical StabilityChemical StabilityDetermine what type of charge each

element below would form to reach maximum stability.

a. Sodium b. Oxygen c. Argon d. Phosphorus e.Chromium

Chemical Stability: Charged Chemical Stability: Charged AtomsAtomsa. What do we call charged atoms?

b. What do we call atoms with a positive charge?

c. What do we call atoms with a negative charge?

Chemical StabilityChemical StabilityDetermine what type of ion each element

below would form to reach maximum stability.

a. Sodium Na1+

b. Oxygen O2-

c. Argon Ard. Phosphorus P3-

e.Chromium Cr2+

Periodic Table: Periodic Table: Homework Homework 1. What element is on period 3 group 2 ?

2. Identify the elements below that are not representative elements:

Fe, S, Ca, Kr, Ag, U3. Identify an element on the periodic table that has

similar properties with oxygen.4. a. What is the name of the group that Chlorine is

in? b. How many valence electrons does Cl have? c. Will it gain or lose to reach maximum stability? d. Identify the charge for Cl when it reaches

maximum stability.

e. Is it classified as an anion or cation. Explain.

Periodic Table: Valence Periodic Table: Valence Electrons Electrons

Lab grps

grp 1ve-

grp 2 ve-

grp 3-12 ve-

grp 13 ve-

grp 14ve-

grp 15 ve-

grp 16ve-

grp17ve-

grp18ve-

A 1 2 2 3 4 5 6 7 8

B 1 2 2 3 4 5 6 7 2

C 1 2 2 3 4 5 6 7 8

D 1 2 2 3 4 5 6 7 8

What can be concluded from the data table?


Electrons


Alkali Metals 1

1ve-

Alkaline-Earth Metals 2

2ve-

TransitionalMetals 3-12 2 ve-

Halogens 17

7ve-


18

8ve-


Electrons


Alkali Metals

Alkaline-Earth Metals

TransitionalMetals

Halogens



Electrons


Alkali Metals 1

1ve- Yes, chemically reactive because they only has 1 ve-. Most reactive metallic group.

Alkaline-Earth Metals 2

2ve-

Yes , chemically reactive because they only have 2 ve-.

TransitionalMetals 3-12 2 ve-

Yes, chemically reactive because they only have 2 ve-.

Halogens 17

7ve- Yes, chemically reactive because they only have 7ve-. Most reactive non-metallic group.


18

8ve- No, not chemically reactive because they have the maximum number of ve-. Most noble elements = 8 ve.Exception: He = 2ve. Most stable elements.

Valence Electrons Post-Valence Electrons Post-Lab Qts.Lab Qts.Complete post-lab questions.

Metallic vs. Non-metallic Metallic vs. Non-metallic PropertiesProperties

Infinite Campus UpdateInfinite Campus UpdatePeriodic Table Quiz (8pts.)Periodic Table Worksheet (10pts.)Due Today: Valence Electron Lab (10pts)

Chemical Stability Chemical Stability PatternPattern

Predict what type of ion, if any, each neutral element below would form to reach maximum stability.

# of neutral/ion ve- max. stabilitya. Sodium b. Oxygen c. Argon d. Phosphorus e. Chromium

History of the Periodic TableHistory of the Periodic Table Dmitri Mendeleev: • Russian chemist and teacher

•When organized elements into groups by similar chemical properties, he observed the periods increasing in atomic mass. (1869)

• His organization system was successful at predicting undiscovered elements.

•Do you observe any inconsistencies with his organization system?

History of Periodic TableHistory of Periodic TableHenry Moseley:

•British Physicists

•Observed that when elements were placed in groups by chemical properties, the periods consistently increased by atomic number. (1913)

•Currently accepted organization system for elements.

Infinite Campus Update

Posted: Valence Electron Lab (15pts)Periodic Table Packet (10pts.)

*Reminder to complete ILPs by this Friday.

Bell Ringer: Atomic Bell Ringer: Atomic StabilityStability1. What is stability for an atom?2. Why do many atoms prefer to be ions?3. Identify each of the following atoms as

a neutral, anion, or cation.a. strontium has 36 electronsb. bromine has 36 electrons4. Predict, if any, what type of ion each

atom below would become to reach stability.

a. Fe b. Rn c. I

Bell Ringer: Atomic Bell Ringer: Atomic StabilityStability

1. What is stability for an atom? 2. Why do many atoms prefer to be ions?3. Identify each of the following atoms as

a neutral, anion, or cation.a. strontium has 36 electronsb. bromine has 36 electrons4. Predict, if any, what type of ion each

atom below would become to reach stability.

a. Fe b. Rn c. I

Periodic Table TrendsPeriodic Table Trends1. Define each term below related to an

atom. 2. Graph data to determine the trend for

each term below for an atom. Atomic Radius

Ionization Energy

Electronegativity

Periodic Trend Graph Periodic Trend Graph AnalysisAnalysisAnalysis Procedures:

1.Locate elements in the same period. Does the line graph increase or decrease

with these elements in the same period.

2. Repeat step one, but with elements in a different period.

3. Locate elements in the same group.Does the line graph increase or decrease

with these elements in the same group?

4.Repeat step three, but with elements in a different group.

5.Share your results with your partners.

Periodic Properties and Periodic Properties and TrendsTrendsAtomic Radius:

-Size of an atom.- Distance from nucleus to highest energy level

for that atom. (picometers, pm).Ionization Energy:- Energy required to remove an electron from an

atom. - Energy required to form a cation. Electronegativity: - The attraction one atom has toward another

atom’s valence electron.- Determines the type of chemical bond between

atoms.

Periodic Table TrendsPeriodic Table Trends1. Define each term below related to an

atom. 2. Graph data to determine the trend for

each term below for an atom. Atomic Radius

Ionization Energy

Electronegativity

Periodic Trends: Atomic Periodic Trends: Atomic RadiusRadius

Across a Period

Down a Group

Periodic Table : Atomic Periodic Table : Atomic RadiusRadius

Periodic Trends: Ionization Periodic Trends: Ionization EnergyEnergy


Across a Period:

Down a Group:

Periodic Trend ValuesPeriodic Trend Values

1. Use your atomic radius graph to rank the following elements in increasing atomic radius. Cl, Mg, Al, Na

2. Use your ionization energy graph to rank the following elements in decreasing ionization energy. Ba, Mg, Ca, Be

Periodic Trends: Atomic Periodic Trends: Atomic Radius Radius

Periodic Trend ValuesPeriodic Trend Values

1. Use your atomic radius graph to rank the following elements in increasing atomic radius. Cl, Mg, Al, Na

2. Use your ionization energy graph to rank the following elements in decreasing ionization energy. Ba, Mg, Ca, Be

Periodic Trend: Periodic Trend: ElectronegativityElectronegativity

mmsphyschem.com

Periodic Trend: Periodic Trend: ElectronegativityElectronegativity

mmsphyschem.com

Across a Period:

Down a Group:

Electronegativity and Chemical Electronegativity and Chemical BondingBonding•Do metals or non-metals have a greater electronegativity value?

Electronegativity and Chemical Electronegativity and Chemical BondingBonding•Which compound has a greater electronegativity value difference? NaCl or CO

Chemical BondingChemical BondingWhich compound has an ionic bond and which has a

covalent bond? NaCl and CO Ionic Bonding: NaClBetween a cation(metal) and an anion (non-metal)Electronegativity difference between atoms is large.Transfer of valence electron(s).Ionic Bond = Intramolecular ForcesCovalent Bonding: CO Between two non-metals.Electronegativity difference between atoms is smallShare valence electron(s)Covalent Bond = Intramolecular ForcesCovalent compounds are also called molecules.

Ionic Bonding Ionic Bonding

.

Chemical Bonds: Intramolecular Forces Physical Bonds: Intermolecular Forces

Octet Rule Revised:Octet Rule Revised:

Atoms will gain, lose, or share valence electrons to reach stability.

The need for stability produces compounds (ionic and covalent)

Ionic or Covalent Ionic or Covalent CompoundsCompounds

H2OBaCl2FeOC6H12O6

Size of an IonSize of an IonUse the diagram below to determine what happens to the size of a neutral atom(parent atom) when it becomes an ion.

Size of a CationSize of a CationWhy is the cation smaller than its parent atom (neutral)?

Size of a CationSize of a CationA cation is smaller than its parent atom.Why? Because metals will lose an energy level in the process of becoming a cation.

Size of an AnionSize of an AnionWhy is an anion larger than its parent atom?

Size of an AnionSize of an AnionA anion is larger than its parent isotope. Why? Repulsion force increases as more electrons are added to the outer most energy level. Swells the energy level.

Size of an AnionSize of an Anion

Size of IonsSize of Ions

1. Circle the atom that is larger in size.a. Ca or Ca2+

b. S or S2-

2. Circle the atom that is smaller in size.

a. Al or Al3+

b. N or N 3-

Ionic BondingIonic BondingTransfer of valence electrons from a

metal atom to a non-metal atom.

Creates a metal ion and non-metal ion that are held together by electrostatic attractive forces (chemical bond)

Chemical bonds are intramolecular forces.

Formation of Ionic Compounds

Ionic Bonding Ionic Bonding

IntraIntramolecular Forcesmolecular ForcesThe chemical bonds within a single

compound.

Ionic Bonding (Lewis Dot Ionic Bonding (Lewis Dot Transfer)Transfer)

Metal (Lewis Dot)

Non-metal(Lewis Dot)

Ionic Bonding(Lewis Dot Transfer)

Chemical Formula

Na Cl

Al N

Ca Cl

Chemical BondingChemical BondingLewis Dot Structures: Illustrates the

number of valence electrons a neutral atom has prior to chemical bonding.

Hydrogen Lab

icp: periodic table icp: periodic table infinite campus update: nuclear chemistry and electron...

Documents

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