Name: ______KEY_________________________________________ Date: __________________ Block: __________ 1
Introduction to the Periodic Table
Label each characteristic as belonging to Metals, Nonmetals, or Metalloids.
1. ______M____ Found on the left side of the zig-zag line.
2. ________NM__ Found on the right side of the zig-zag line.
3. ________Met__ Located along the zig-zag line.
4. ____M______ Have luster
5. ____NM______ Not shiny (dull)
6. _____ M_____ With one exception, all are solids at room temperature.
7. ____NM______ Many are gases at room temperature.
8. ____NM______ Tend to gain electrons.
9. ____M______ Tend to lose electrons.
10. ____NM______ Valence electrons are held tightly.
11. ____M______ Valence electrons are held loosely.
12. ____Met______ Have properties of both metals and nonmetals.
13. ____Met______ Some are semiconductors.
14. ____M______ Malleable (definition: ____able to bend_____________________________)
15. ____M______ Ductile (definition: ___able to stretch into wire _____________)
16. ___NM_______ Brittle
17. ___M_______ Excellent conductors of heat and electricity.
18. ___Met_______ Good conductors of heat and electricity.
19. ____NM______ Poor conductors of heat and electricity.
How many energy levels are needed to hold the electrons for these elements?
Hint: Use the Period (row) Number.
1.
2.
3.
4.
Carbon: 2____
Barium: 6____
Aluminum: __3___
Helium: __1___
What are valence electrons? _____electrons in outermost ring/energy level ____
How many valence electrons do these elements have?
Hint: Use the “A” Group Number. You will never have more than 8 valence electrons.
1.
2.
3.
4.
Mg: _2___
C: _4___
O: _6___
Te: _6___
5.
6.
7.
8.
Cl: __7__
Ar: __8__
K: _1___
He: _2
9. H: _1___
10. Al: _3___
11. F: _7___
12. P: _5___
What is an oxidation number? ____charge of an element _______________
Oxidation Number Rules:
1. Elements with 1-4 valence electrons lose their electrons to form cations.
(except Helium which is stable with 2 electrons in the 1st energy level)
Name: ______KEY_________________________________________ Date: __________________ Block: __________ 2
2. Elements with 5-7 valence electrons gain enough electrons to meet the octet
rule, forming anions.
3. Elements with 8 valence electrons (and helium with 2) are stable and do not
lose or gain electrons.
If these elements follow the octet rule, what will their oxidation number be?
1. Li: _+1___
5. Si: __+/- 4__
9. He: __0__
2. Ca: _+2___
6. B: +3____
10. P: _-3___
3. O: _-2___
7. Ne: _0___
11. Cs: _+1___
4. Br: _-1___
8. H: _+1___
12. N: _-3___
Identify these elements as metals (M), nonmetals (NM), or metalloids:
1. Ca: __M_____
5. Al: __M_____
9. U: _M______
2. Fe: _M______
6. Sb: __Met_____
10. Si: __Met_____
3. Cl: _NM______
7. Po: __Met_____
11. C: __NM_____
4. S: ___NM____
8. K: __M_____
12. Ne: __NM_____
Element
# of Valence
Electrons
Oxidation
Number
Did it
lose or
gain e-?
# of
Energy
Levels
Family Name
Magnesium
2
+2
Lose
3
Alkaline Earth Metals
Sulfur
6
-2
Gain
3
Oxygen Family
Bromine
7
-1
Gain
4
Halogen
Cesium
1
+1
Lose
6
Alkali Metals
Boron
3
+3
Lose
2
Boron Family
Nitrogen
5
-3
Gain
2
Nitrogen Family
Argon
8
0
-
3
Noble Gases
Helium
2
0
-
1
Noble Gases
Calcium
2
+2
Lose
4
Alkaline Earth
3
Arsenic
5
-3
Gain
4
Nitrogen family
Periodic Trends Practice
Label the arrows with “increases” or “decreases” to show the trends on the periodic table and explain why.
Atomic Size
1.
2.
3.
4.
5.
6.
Which has a larger atomic radius: Francium or Rubidium?
Which has a larger atomic radius: Cesium or Lead?
Which has the largest atomic radius: Phosphorus, Sulfur, Potassium, or Sodium?
Which has a smaller atomic size: Sulfur or Polonium?
Which has a smaller atomic size: Gallium or Germanium?
Which has a smaller atomic size: Strontium, Calcium, Gallium, or Indium?
Ionic Size
7. Which is smaller: A fluorine atom or a fluorine ion?
8. Which is smaller: A barium atom or a barium ion?
9. Which is larger: A chromium atom or a chromium ion?
10. Which is the smaller ion: strontium ion(Sr+2) or rubidium ion (Rb+1)?
11. Which is the larger ion: nitrogen ion (N-3) or oxygen ion(O-2) ?
12. Which is the smallest ion: sodium ion (Na+1), magnesium ion (Mg+2), phosphorus ion (P-3),
sulfur ion (S-2)?
13. Which is the largest ion: selenium ion(Se-2), bromine ion (Br-1), potassium ion(K+1), or
gallium ion (Ga+3)b?
14. Which is the largest ion: cesium ion (Cs+1), nitrogen ion (N-3), magnesium ion (Mg+2), or
sulfur ion (S-2)?
Ionization Energy: Definition: amount of energy it takes to remove an electron
__________________________________________________________________________
15. Which has the lower ionization energy: cesium or sodium?
16. Which has the lower ionization energy: selenium or calcium?
17. Which has the highest ionization energy: magnesium, potassium, nitrogen, or oxygen?
18. Which has the lowest ionization energy: phosphorus, sulfur, arsenic, or selenium?
Electronegativity: Definition: amount of energy it takes to attract electrons
___________________________________________________________________________
19. Which has a higher electronegativity: oxygen or lithium?
20. Which has a higher electronegativity: bismuth or nitrogen?
21. Which has the lowest electronegativity: strontium, silicon, phosphorus, or fluorine?
22. Which has the highest electronegativity: argon, chlorine, selenium, or bromine?
4
Mixed
23. Which has the largest atomic radius: boron, carbon, aluminum, or silicon?
24. Which has the greatest ionization energy: sulfur, gallium, germanium, or tin?
25. Which has the largest ionic size: rubidium ion, strontium ion, tellurium ion, or iodine
ion?
26. Which has the smallest electronegativity: nitrogen, phosphorus, calcium, or chlorine?
Periodic Table Study Guide
1.
How did Mendeleev arrange the periodic table and what was unique about him?
By atomic mass
2.
Why was Moseley significant to the periodic table?
Arranged by atomic number
3.
What is the modern periodic law?
When elements are arranged by atomic number, similar properties exist when elements are
in the same group
4.
Where are metals located on the periodic table? What are their properties?
Left side of the stair case
-positive charge
-excellent conductors of electricity
-mostly solids
-has luster, ducticle, and malleable
5.
Where are nonmetals located on the periodic table? What are their properties?
Right side of stair case
-negative charges
-poor conductors of electricity
-mostly gases
-brittle
6.
Where are the metalloids? What are their properties?
Along the stair case
-semiconductors
-properties of both metals and nm
7.
Where are the alkali metals? What are their properties?
Group 1; most reactive metals
8.
Where are the alkaline metals? What are their properties?
Group 2; +2 charge
9.
Where are the halogens? What are their properties?
5
Group 17; most reactive nonmetals
10.
Where are the noble gases? What are their properties?
Group 18; most stable
11.
Where are the transition metals? What are their properties?
“B” group; mostly metals and radioactice
12.
Where are the lanthanide metals?
1st row on bottom
13.
Where are the actinide metals?
2nd row on bottom
14.
What are the properties of hydrogen?
Nonmetal, +1 charge
15.
What are the oxidation numbers for each group?
+1, +2, +3, +/- 4, -3, -2, -1
16.
What is the octet rule?
All elements want to meet 8 electrons in their outermost ring
17.
Do metals “like” to gain or lose electrons?
Lose
18.
Do nonmetals “like” to gain or lose electrons?
Gain
19.
What is atomic radius?
Half the diameter of the nucleus
20.
What is the trend for atomic radius as you go down a group? WHY?
Increases due to adding energy levels
21.
What is the trend for atomic radius as you go across (LR) a row? WHY?
Decreases due to the “Shielding effect” (attraction of protons and electrons increase)
22.
What is a cation? Does a cation have a bigger or smaller radius than a neutral atom?
Positive charged ion; smaller radius
23.
What is an anion? Does an anion have a bigger or smaller radius than a neutral atom?
Negative charged ion; bigger
24.
What is the most active metal? Why?
Francium-group 1, largest
25.
What is the trend for the reactivity of metals?
Decreases going across
26.
What is the most active nonmetal? Why?
6
Fluorine-needs one more electron to be stable
27.
What is the trend for the reactivity of nonmetals?
Decreases going down
28.
What is ionization energy? What is the trend for ionization energy?
Remove electron-Top right is the highest
29.
What is electronegativity? What is the trend for electronegativity?
Gain electron-top right is highest **NOT INCLUDING NOBLE GASES**