Periodic Table and Groups Periodic Table and Groups
Periodic Table and Groups
Periodic Table and Groups Transitional Groups: Representative Groups:
Periodic Table: Groups • • a. b. c. d. e. f. Identify the group number(s) for each group name below. Give an example of an element from each group below. Noble Gases Alkali Metals Alkaline Earth Metals Transitional Metals Rare Earth Metals Halogens
Periodic Table: Bell Ringer What element is on period 3 group 2 ? 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. 4. a. What is the name of the group that Chlorine is in? b. What is the short-hand electron configuration of Cl? c. How many valence electrons does Cl have? 1.
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) 3. What are valence electrons? 4. Why is it important to know the number of valence electrons an element can have?
Organization of Periodic Table Why do elements in the same group have similar chemical properties?
Periodic Table: Valence Electrons
Common Periodic Table Groups Periodic Groups Alkali Metals Alkaline-Earth Metals Transitional Metals Halogens Noble Gases (Inert Gases) Group # Valence Electrons Chemical Reactivity (Yes or No)
Common Periodic Table Groups Periodic Groups Alkali Metals Alkaline-Earth Metals Group # 1 2 Valence Electrons 1 ve- Chemical Reactivity (Yes or No) Yes, chemically reactive because they only has 1 ve-. Most reactive metallic group. 2 ve- Yes , chemically reactive because they only have 2 ve-. Yes, chemically reactive because they only have 2 ve-. Transitional Metals 3 -12 2 ve- Halogens 17 7 ve- Yes, chemically reactive because they only have 7 ve-. Most reactive nonmetallic group. Noble Gases (Inert Gases) 18 8 ve- No, not chemically reactive because they have the maximum number of ve. Most noble elements = 8 ve.
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.
Metallic vs. Non-metallic Properties
Bell Ringer: Chemical Stability 1. a. Most stable group on periodic table? Explain. b. Most reactive metallic group? Explain. c. Most reactive non-metallic group? Explain. 2. Predict what type of ion each element below would form to reach maximum stability. a. Cesium b. Selenium c. Helium 3. Identify which atom is larger in each example below.
Chemical Stability Pattern Will metals tend to gain or lose valence electrons to reach maximum stability? Will non-metals tend to gain or lose 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 Pattern Predict what type of ion, if any, each neutral element below would form to reach maximum stability. # of neutral/ion vemax. stability a. Sodium b. Oxygen c. Argon d. Phosphorus e. Chromium
Chemical Stability Determine what type of ion each element below would form to reach maximum stability. a. b. c. d. Sodium Na 1+ Oxygen O 2 Argon Ar Phosphorus P 3 e. Chromium Cr 2+
Valence Electrons Worksheet Key 1. 7 ve 2. 5 ve 3. 2 ve 4. 5 ve 5. 2 ve 6. 8 ve 7. 1 ve 8. 2 ve 9. 2 ve 10. 6 ve- 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 1 ve 2 ve 4 ve 7 ve 6 ve 2 ve 3 ve 1 ve 8 ve 2 ve-
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.
Bell Ringer: Atomic Stability 1. 2. 3. a. b. 4. a. 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. Fe b. Rn c. I
Bell Ringer: Atomic Stability 1. 2. 3. a. b. 4. a. 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. 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 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? 1.
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 Atomic Number vs. Atomic Radius 200 atomic raidus (pm) 180 160 140 120 100 80 60 40 20 0 1 2 3 4 5 6 7 8 9 10 11 12 atomic number 13 14 15 16 17 18
Periodic Trends: Atomic Radius Across a Period Atomic Number vs. Atomic Radius 200 atomic raidus (pm) 180 160 140 120 100 Down a Group 80 60 40 20 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 atomic number
Periodic Table : Atomic Radius
Periodic Trends: Ionization Energy Atomic Number vs. Ionization Energy (k. J/mol) 2500 2000 1500 1000 500 0 1 3 5 7 9 11 Atomic Number 13 15 17
Periodic Trends: Ionization Energy Atomic Number vs. Ionization Energy 2500 Ionization Energy (k. J/mol) Across a Period: 2000 1500 1000 Down a Group: 500 0 1 3 5 7 9 11 Atomic Number 13 15 17
Periodic Trend: Electronegativity mmsphyschem. com
Periodic Trend: Electronegativity Across a Period: Down a Group: mmsphyschem. com
Electronegativity and Chemical Bonding • In general what kind of elements have a greater electronegativity value? • Using the table, which compounds would have a greater electronegativity difference: Na. Cl or CO?
Electronegativity and Chemical Bonding What do you predict will happen when Na chemically bonds with Cl?
Chemical Bonding Ionic Bonding: Covalent Bonding:
Octet Rule Revised: Atoms will gain, lose, or share valence electrons to reach stability. The need for stability produces compounds (ionic and covalent)
Bell Ringer: Periodic Trends 1 Use your graph on atomic radius and ionization energy to answer the following questions: a. Rank the following elements from largest to smallest in size. Explain your results. Ar, Mg, S Al b. Rank the following elements from smallest to largest in ionization energy. Explain your results. Ne, Ar, He
Lewis Dot Structures • Illustrate Element Na Mg Si S valence electrons for an atom before bonding. # of valence electrons Lewis Dot Structure
Ions and Chemical Stability Lab In pairs, look at 16 different elements and answer the following questions: a. Metal or non-metal b. Neutral, anion, or cation. c. Symbol and specific charge if needed. *neutral if element is naturally stable (noble gas) *anion: non-metal not naturally stable *cation: metals
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 leve
Size of an Anion
Size of Ions Circle the atom that is larger in size. a. Ca or Ca 2+ 1. b. S or S 2 - Circle the atom that is smaller in size. a. Al or Al 3+ 2. 3 -
Ionic Bonding (Lewis Dot Transfer) Metal (Lewis Dot) Non-metal (Lewis Dot) Na Cl Al N Ca Cl Ionic Bonding (Lewis Dot Transfer) Chemical Formula
Chemical Bonding Lewis Dot Structures: Illustrates the number of valence electrons a neutral atom has prior to chemical bonding.
Bell Ringer: Chemical Stability 1. a. Most stable group on periodic table? Explain. b. Most reactive metallic group? Explain. c. Most reactive non-metallic group? Explain. 2. Predict what type of ion each element below would form to reach maximum stability. a. Cesium b. Selenium c. Helium 3. Identify which atom is larger in each example below.
Hydrogen Lab
- Slides: 51