Download Unit Expectations – Periodic Table

Student Expectations – Periodic Table
Big Idea / Question(s):
1. How is the periodic table organized and how does that organization maximize the periodic table’s
usefulness?
2. What similar properties do major groups (alkali metals, alkaline earth metals, transition metals, inner
transition metals, halogens, noble gases) in the periodic table share?
3. How do the size of an atom and the number of valence electrons within an atom effect the
properties of that atom / element?
Overview: This Periodic Table Unit will study how atomic structure (the number and position of
electrons, protons and neutrons) effects the properties (metallic character, state of matter, type of
compound most often formed by element…) and reactivity of elements. The periodic table is an
excellent tool for understanding atomic structure. The periodic table also contains properties of
elements both within the element boxes and from the position of the element within the table.
Hopefully by the end of the unit, we will understand how powerful tool the periodic table can be for
predicting properties and reactions of elements and relating those properties and reactions to atomic
structure.
Resources:
 Section 1.3
 Chapter 5 (All)
 There are a multitude of websites on the periodic table a few good resources are:
o http://www.webelements.com/, http://www.ptable.com/, http://www.periodicvideos.com/
Vocabulary Terms:
__ Columns
__ Periods
__ Nonmetal
__ Malleability
__ Electrons
__ State of matter
__ Covalent Bond
__ Groups
__ Chemical Properties
__ Metalloid / Semimetal
__ Ductility
__ Atomic radius
__ Radioactivity
__ Metallic Bond
__ Families
__ Physical Properties
__ Metallic character
__ Density
__ First ionization energy
__ Electronegativity
__ Alkali Metals
__ Rows
__ Metal
__ Conductivity
__ Valence
__ Reactivity
__ Ionic Bond
__ Alkaline Earth
__ Metals
__ Transition Metals
__ Halogens
__ Noble Gases
__ Inner Transition Metals
Assignments:
___ Outline and Section Review 1.3
___ Lab – Periodic Trends - Reactivity and Properties Metals
___ Outline and Section Review 5.1 (do not do question #4)
___ Quiz – Element Symbols and Names (Elements # 1-30, and Br, Kr, Ag, I, Pt, Au, Pb, Sn, Hg, Rn, U, Pu)
___ Lab – Densities of Elements in Column 15 (Optional Extra Credit)
___ WS – Periodic Table Trends - 1
___
___
___
___
___
WS – Periodic Table Trends – 2
Outline and Section Review 6.1
Ch 5 Review Questions Pg 166 #2, 3, 4, 8, 9, 12, 13, 22, 23, 24, 27, 28, 30, 31, 48, 49
Practice Test – Periodic Table
Test – Periodic Table
CONCEPTS TO KNOW (BOLDED ARE MORE IMPORTANT)
1. Introduced: _______ Basic: _________ Mastered: _________
Know the elements symbols
and names for elements up to an atomic number of 30 and Br, Kr, Ag, I, Pt, Au, Pb, Sn, Hg,
Rn, U, Pu
2. Introduced: _______ Basic: _________ Mastered: _________
I can define and give
examples of the following terms: Element, Mixture and Compound. Elements are a class of
substances composed of a single kind of atom. Compounds are composed of two or more
different elements chemically combined. Mixtures are composed of two or more different
elements and/or compounds physically combined. Each element and compound has physical
and chemical properties, such as boiling point, density, color, and conductivity, which are
independent of the amount of the sample.
3. C4.10 A Introduced: _______ Basic: _________ Mastered: _________
I can use
the periodic table to find the number of electrons, protons, neutrons, atomic mass,
state of matter and metallic character of any neutral element on the periodic table.
4. C4.10A Introduced: _______ Basic: _________ Mastered: _________
I can list
the number of protons, neutrons, and electrons for any given ion or isotope.
5. C4.10B Introduced: _______ Basic: _________ Mastered: _________
I recognize
that an element always contains the same number of protons which is also called atomic
number and I can state the atomic number as one of the periodic table's organizing
principles.
6. C4.8D Introduced: _______ Basic: _________ Mastered: _________
I can give the
number of valence electrons for any element within the "S" or "P" blocks of the periodic
table. Also, be able to determine whether the elements would gain or lose electrons
were they going to make an ion.
7. C4.9x Introduced: _______ Basic: _________ Mastered: _________
I can describe that
the rows (periods) in the periodic table represent the main electron energy levels of the
atom.
8. C4.9 Introduced: _______ Basic: _________ Mastered: _________
I can state the
Periodic Law and give it as the organizing principle for the periodic table. The Periodic
Law States: In the periodic table, elements are arranged in order of increasing number
of protons (called the atomic number). Vertical groups in the periodic table (families)
have similar physical and chemical properties due to the same outer electron structures,
9. C4.9A Introduced: _______ Basic: _________ Mastered: _________
I can identify
elements with similar chemical and physical properties using the periodic table. Know
and be able to state that the similarities present in element groups come from the
elements having the same number of valence electrons.
10. Introduced: _______ Basic: _________ Mastered: _________
number of valence electrons on an atom to its stability.
I can relate the
11. C4.9b Introduced: _______ Basic: _________ Mastered: _________
I can
define and identify metals, non-metals, and metalloids using the periodic table.
12. C4.9c Introduced: _______ Basic: _________ Mastered: _________
I can define the
terms and predict general trends in _____________ using the periodic table.
 atomic mass
 reactivity
 atomic number
 metallic character
 atomic radius
 state of matter
 valence electrons
 radioactivity
 first ionization energy
 electronegativity
13. Introduced: _______ Basic: _________ Mastered: _________
I can use the
combinations of metals and nonmetals (two metals  metallic bond, two nonmetals 
covalent bond, and metal with nonmetal  ionic bond) or electronegativity (two metals
 metallic bond, 0-1.7  covalent, >1.7 ionic bond) to determine the type of bond
made between two elements.
14. Introduced: _______ Basic: _________ Mastered: _________
I can describe
metallic, covalent and ionic bonds. Ionic bonds are bonds due to the attraction of
oppositely charged atoms. Covalent bonds are created between atoms with a strong,
mutual attraction for shared electrons. Metallic bonds are created between atoms with
a weak, mutual attraction for shared electrons.
HSCE – Periodic Table
C4.10 Neutral Atoms, Ions, and Isotopes - A neutral atom of any element will contain the same
number of protons and electrons. Ions are charged particles with an unequal number of protons
and electrons. Isotopes are atoms of the same element with different numbers of neutrons and
essentially the same chemical and physical properties.
C4.10A List the number of protons, neutrons, and electrons for any given ion or isotope.
C4.10B Recognize that an element always contains the same number of protons.
C4.8D Give the number of electrons and protons present if the fluoride ion has a -1 charge.
(IONS);
SWBAT - Identify the number of valence electrons, whether the elements would gain or lose
electrons and give the oxidation number / charge. Students will also be able to differentiate
between oxidation number and charge in words and through symbols using elements.;
C4.9x Electron Energy Levels The rows in the periodic table represent the main electron energy
levels of the atom. Within each main energy level are sublevels that represent an orbital shape
and orientation.
C4.9A Identify elements with similar chemical and physical properties using the periodic table.,
C4.9 Periodic Table - In the periodic table, elements are arranged in order of increasing number
of protons (called the atomic number). Vertical groups in the periodic table (families) have
similar physical and chemical properties due to the same outer electron structures.
C4.9b Identify metals, non-metals, and metalloids using the periodic table.
C4.9c Predict general trends in atomic radius, first ionization energy, and electronegativity of
the elements using the periodic table.
Plan - Periodic Table
Get Library Time (second half) for Day 5 and 6.
Day 1 and 2
C4.9, C4.10, C4.10A, C4.10b: Assign homework Section Review and Outline 1.3 due on Day 3 &
Outline and Section Review 5.1 (they do not need to do question #4) due on Day 5.
Announce quiz on Element Symbols and Names (Quiz on symbols for the elements up to A# 30
and Br, Kr, Ag, I, Pt, Au, Pb, Sn, Hg, Rn, U, Pu)
C4.9A, C4.9 c, C4.10D - (Reactivity Trends): Lab – Periodic Trends - Reactivity and Properties
Metals . Make sure to mention several times that all the elements in the first column have one
valence electron, the elements in the second column have two and third column have three, etc..
Start with Al, Mg, Ca in Water, then do Li, Na and K in water and end with Mg and Al in HCl.
Day 3
Discuss and Collect Lab – Reactivity of Metals; Check-In Out and SR 1.3
Videos of Na Dumping in Lake, Rb and Cs
Nottingham University, ptable, Webelements and …..
Mark Rosengarten Elemental Funkiness - http://www.youtube.com/watch?v=1PSzSTilu_s
OPTIONAL: Lab – Si, Sn, Pb Densities (Must have ample amount of chemical).
Day 4 –
They Might Be Giants Element Song
OPTIONAL: Lab – Quickly Review and Collect Lab – Si, Sn, Pb Densities.
Day 5 and 6 –
Grade and discuss Outline and Section Review 5.1.
Review use of information within the element box of the periodic table. Transition to trends
within the periodic table.
Hand-out the C4.9A, C4.9b, C4.9c, C4.10C, C4.10D WS – PT Trends 1 and 2 which will be
due on Day 7. Also mention that sections 5.2 and 5.3 are useful and may be some aid to the
worksheets and the quiz. Have them read the section on Materials Scientist (pg 145)
All Standards are covered - Power Point – Periodic Table. Lecture covers the organization of
the periodic table (periodic law), easy trends (atomic number, atomic mass…..), and trend of
atomic radius. Lecture will cover Ionization Energy, Valence Electrons and Bonding.
Demo – Na and Cl –
Add concentrated hydrochloric acid dropwise onto a small quantity of potassium permanganate
crystals (in a flask). Collect the chlorine gas by upward displacement of air in a hood. Use proper
safety precautions. Concentrated hydrochloric acid is extremely caustic. Chlorine gas is toxic.
Reaction
6HCl + 2KMnO4 + 2H+ --> 3Cl2 + 2MnO2 + 4H2O + 2K+ Add concentrated hydrochloric acid
dropwise onto a small quantity of potassium permanganate crystals (in a flask). Collect the
chlorine gas by upward displacement of air in a hood. Use proper safety precautions.
Concentrated hydrochloric acid is extremely caustic. Chlorine gas is toxic.
Reaction
6HCl + 2KMnO4 + 2H+ --> 3Cl2 + 2MnO2 + 4H2O + 2K+
Day 7 – Complete PPT – Periodic Table if necessary.
University of Nottingham Fluorine Video, Manson Murder Victim Introduce the Poster
Assignment.
Assign AT END OF HOUR Ch 5 Review Questions Pg 166 #2, 3, 4, 8, 9, 12, 13, 22, 23, 24, 27,
28, 30, 31, 48, 49 and Outline and Section Review 6.1 due on Day 7.
Day 8 – Grade and discuss WS - Periodic Trends; Complete Posters and Homework
Day 9 – Present Posters. Review for Test – Periodic Table
Day 10 – Quiz - Periodic Table.
DEMO – NI3 (let the NI3 steep long enough and let it dry long enough)
Name that element pg 35