ICP: 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 Elements Classify elements as metals, non-metals, and metalloids.

Periodic Table: Locating Elements Periods: Elements in the same row. Groups: Elements in the same column. Have similar chemical properties.

Periodic Table : Bell Ringer 1. 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) 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 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 Properties

Periodic Table and Groups Why do elements in the same group have similar chemical properties?

Periodic Table Lab: Group Patterns grps grp 1 ve- grp 2 grp 13 ve- grp 14 grp 15 grp 16 grp17 grp18 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:

Periodic Table Lab: Group Patterns grps grp 1 ve- grp 2 grp 13 ve- grp 14 grp 15 grp 16 grp17 grp18 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:

Periodic Table and Groups 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 Table Due: 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 Groups Periodic Groups Group # Valence Electrons Chemical Reactivity (Yes or No) Alkali Metals Alkaline-Earth Metals Transitional Metals Halogens Noble Gases (Inert Gases)

Periodic Table and Groups Transitional Groups: Short groups. Representative Groups: Tall groups

ICP 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. Noble Gases Alkali Metals Alkaline Earth Metals Transitional Metals Halogens 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 Stability Octet 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 Pattern Metals tend to lose valence electrons to reach stability. Non-metals tend to gain valence electrons to reach maximum stability?

Chemical Stability Pattern Metals: Will lose ve- to reach stability. Form cations (+ charged atoms) Non-metals: Will gain ve- to reach stability. Form anions (- charged atoms)

Chemical Stability Determine what type of charge each element below would form to reach maximum stability. a. Sodium b. Oxygen c. Argon d. Phosphorus Chromium

Chemical Stability: Charged Atoms a. 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 Stability Determine what type of ion each element below would form to reach maximum stability. a. Sodium Na1+ b. Oxygen O2- c. Argon Ar d. Phosphorus P3- Chromium Cr2+

Periodic Table: Homework What element is on period 3 group 2 ? Identify the elements below that are not representative elements: Fe, S, Ca, Kr, Ag, U 3. Identify an element on the periodic table that has similar properties with oxygen. 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: Homework What element is on period 3 group 2 ? Identify the elements below that are not representative elements: Fe, S, Ca, Kr, Ag, U 3. Identify an element on the periodic table that has similar properties with oxygen. 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: Homework What element is on period 3 group 2 ? Identify the elements below that are not representative elements: Fe, S, Ca, Kr, Ag, U 3. Identify an element on the periodic table that has similar properties with oxygen. 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: Homework What element is on period 3 group 2 ? Identify the elements below that are not representative elements: Fe, S, Ca, Kr, Ag, U 3. Identify an element on the periodic table that has similar properties with oxygen. 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 Electrons Lab grps grp 1 ve- grp 2 grp 3-12 grp 13 ve- grp 14 grp 15 grp 16 grp17 grp18 A 1 2 3 4 5 6 7 8 B C D What can be concluded from the data table?

Common Periodic Table Groups Periodic Groups Group # Valence Electrons Chemical Reactivity (Yes or No) Alkali Metals 1 1ve- Alkaline-Earth Metals 2 2ve- Transitional Metals 3-12 2 ve- Halogens 17 7ve- Noble Gases (Inert Gases) 18 8ve-

Common Periodic Table Groups Periodic Groups Group # Valence Electrons Chemical Reactivity (Yes or No) Alkali Metals Alkaline-Earth Metals Transitional Metals Halogens Noble Gases (Inert Gases)

Common Periodic Table Groups Periodic Groups Group # Valence Electrons Chemical Reactivity (Yes or No) 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-. Transitional Metals 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. Noble Gases (Inert Gases) 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-Lab Qts. Complete post-lab questions.

Metallic vs. Non-metallic Properties

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

Chemical Stability Pattern Predict what type of ion, if any, each neutral element below would form to reach maximum stability. # of neutral/ion ve- max. stability a. Sodium b. Oxygen c. Argon d. Phosphorus e. Chromium

History 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 Table Henry 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 Stability What is stability for an atom? Why do many atoms prefer to be ions? Identify each of the following atoms as a neutral, anion, or cation. strontium has 36 electrons bromine has 36 electrons Predict, if any, what type of ion each atom below would become to reach stability. a. Fe b. Rn c. I

Bell Ringer: Atomic Stability What is stability for an atom? Why do many atoms prefer to be ions? Identify each of the following atoms as a neutral, anion, or cation. strontium has 36 electrons bromine has 36 electrons Predict, if any, what type of ion each atom below would become to reach stability. a. Fe b. Rn c. I

Periodic Table Trends 1. 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 Analysis Analysis Procedures: 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? Repeat step three, but with elements in a different group. Share your results with your partners.

Periodic Properties and Trends Atomic 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 Trends 1. 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 Radius Across a Period Down a Group

Periodic Table : Atomic Radius

Periodic Trends: Ionization Energy

Periodic Trends: Ionization Energy Across a Period: Down a Group:

Periodic 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 Radius

Periodic 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: Ionization Energy

Periodic Trend: Electronegativity mmsphyschem.com

Periodic Trend: Electronegativity Across a Period: Down a Group: mmsphyschem.com

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

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

Chemical Bonding Which compound has an ionic bond and which has a covalent bond? NaCl and CO Ionic Bonding: NaCl Between a cation(metal) and an anion (non-metal) Electronegativity difference between atoms is large. Transfer of valence electron(s). Ionic Bond = Intramolecular Forces Covalent Bonding: CO Between two non-metals. Electronegativity difference between atoms is small Share valence electron(s) Covalent Bond = Intramolecular Forces Covalent compounds are also called molecules.

Ionic Bonding

Chemical Bonds: Intramolecular Forces Physical Bonds: Intermolecular Forces .

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 Compounds H2O BaCl2 FeO C6H12O6

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

Size of a Cation Why is the cation smaller than its parent atom (neutral)?

Size of a Cation A 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 Anion Why is an anion larger than its parent atom?

Size of an Anion A 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 Anion

Size of Ions Circle the atom that is larger in size. Ca or Ca2+ S or S2- Circle the atom that is smaller in size. a. Al or Al3+ b. N or N 3-

Ionic Bonding Transfer 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

Intramolecular Forces The chemical bonds within a single compound.

Ionic Bonding (Lewis Dot Transfer) Metal (Lewis Dot) Non-metal Ionic Bonding (Lewis Dot Transfer) Chemical Formula Na Cl Al N Ca

Chemical Bonding Lewis Dot Structures: Illustrates the number of valence electrons a neutral atom has prior to chemical bonding.

Hydrogen Lab