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nd
2 Quarter
Unit 1
Homework Packet
Ionic Basics
1. Which elements on the periodic table do not react with anything, they are inert?
2. What about an atom determines if it is chemically stable or not?
3. What are the “magic” or “perfect” number of electrons that make an atom stable?
4. If an atom does not have one of the numbers of electrons from question #3 above, what will it
do to try to get to one of those numbers?
5. What is an ion?
6. What is an ionic bond?
7. An atom gains an electron, what charge is it’s ion?
8. An atom loses an electron, what charge is it’s ion?
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Octet Rule and Charges
1. How many valence electrons does each of the following atoms have?
A. Potassium, K
B. Sulfur, S
C. Phosphorous, P
D. Neon, Ne
E. Aluminum, Al
F. Boron, B
G. Fluorine, F
H. Carbon, C
I. Magnesium, Mg
J. Sodium Na
2. What charge do each of these atoms go to when they become stable ions?
A. Potassium, K
B. Sulfur, S
C. Phosphorous, P
D. Neon, Ne
E. Aluminum, Al
F. Boron, B
G. Fluorine, F
H. Carbon, C
I. Magnesium, Mg
J. Sodium Na
Charge
s
+1
0
+2
+3
+/-4 -3
-2
-1
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3. What are the stable numbers of electrons?
4. What is the octet rule?
5. What charges do metals tend to go to, positive or negative?
6. What charges do non-metals tend to go to, positive or negative?
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Forming Ionic Compounds
1. What is a cation?
2. What is an anion?
3. Do metals tend to become cations or anions?
4. Do non-metals tend to become cations or anions?
5. What charge to all compounds have to be, positive, negative, or neutral?
6. Write the formula for the following ionic compounds:
A. Magnesium bromide
B. Aluminum fluoride
C. Potassium oxide
D. Lithium nitride
E. Sodium sulfide
F. Beryllium nitride
G. Aluminum sulfide
H. Calcium iodide
I. Cesium oxide
7. Write the name for the following ionic compounds:
A. NaBr
B. K2S
C. Ca3N2
D. BaO
E. BeCl2
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Polyatomic Ions and Transition Metals
1. Write the formula for the following ions:
A. Acetate
B. Bicarbonate
C. Thiocyanate
D. Peroxide
E. Ammonium
2. Write the name of the following ions:
A. CN-1
B. Cl-1
C. ClO3-1
D. SO4-2
E. PO3-3
3. Why are Roman numerals necessary for most transition metals?
4. Write the formula for the following ionic compounds:
A. Calcium iodide
B. Sodium oxide
C. Potassium oxalate
D. Ammonium hypochlorite
E. Aluminum hydroxide
F. Iron (III) phosphate
G. Copper (II) nitrite
H. Silver chloride
I. Zinc cyanate
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5. Write the name for each of the following ionic compounds:
A. KCN
B. (NH4)2O
C. AlPO4
D. CaSO3
E. Na2CrO4
F. LiH2PO4
G. Mg(OH)2
H. Cu2CO3
I. Fe2(S2O3)3
J. ZnCl2
6. Each of these formulas has something wrong with it. Fix it:
A. MgCl3
B. Na3SO4
C. CaOH2
D. Fe(III)Br3
E. Na+1I-1
F. OCa
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Crystal Lattices
1. Why do ionic compounds form crystal lattices when they are made?
2. What term is used to describe the strength of a crystal lattice?
3. How are lattice energy and ionic charge related?
4. How are lattice energy and ionic size related?
5. How is melting point related to lattice energy?
6. For each of the pairs below, circle the ionic compound that should have the stronger lattice
energy:
A. CaCl2
vs.
CaO
B. SrS
vs.
NaF
C. Al2O3
vs.
AlCl3
D. Na3PO4
vs.
K3PO4
E. LiF
vs.
NaF
F. K2O
vs.
Na2O
7. For each of the pairs below, decide which should have a higher melting point:
A. LiI
vs.
MgS
B. CaBr2
vs.
BeBr2
C. Al2O3
vs.
NaCl
D. CaSO4
vs.
K2SO4
E. MgF2
vs.
MgBr2
8. Arrange the following in order of increasing melting point (smallest to largest):
CaO
KCl
CaF2
BeO
9. Draw an example of a crystal lattice.
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Solubility
1. What does it mean that water is polar?
2. What is an aqueous ion?
3. Draw a cation surrounded by water molecules; be sure to point the waters the correct way.
4. Repeat #3 but this time use an anion.
5. When an ionic crystal dissolves in water, what has the water done to the crystal?
6. What is the general rule to decide if an ionic compound is soluble in water or not?
7. Decide whether each of the following compounds will be soluble or insoluble in water:
A. NaBr
soluble insoluble
B. K2SO4 soluble insoluble
C. AlPO4
soluble insoluble
D. CaCrO4 soluble insoluble
E. MgCl2
soluble insoluble
F. (NH4)2CO3 soluble insoluble
G. PbSO4
soluble insoluble
H. Ba(OH)2 soluble insoluble
I. LiCl
soluble insoluble
J. Pb(NO3)2 soluble insoluble
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Conductivity
1. Decide whether each of the following compounds will conduct electricity if their crystals are
put in de-ionized water and stirred:
A. NaBr
conduct
not conduct
B. K2SO4
conduct
not conduct
C. AlPO4
conduct
not conduct
D. CaCrO4
conduct
not conduct
E. MgCl2
conduct
not conduct
F. (NH4)2CO3
conduct
not conduct
G. PbSO4
conduct
not conduct
H. Ba(OH)2
conduct
not conduct
I. LiCl
conduct
not conduct
J. Pb(NO3)2
conduct
not conduct
2. What is the definition of electricity?
3. Why will a solid crystal of an ionic substance not conduct electricity?
4. If a solid dissolves into aqueous solution but does not conduct electricity, what must that
mean?
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Precipitation
1. What is a precipitate?
2. Do precipitates look cloudy or clear?
3. What is the rule to determine if a ppt will form?
4. For each combination below, determine if a ppt forms. If it does, write its formula:
A. Fe(NO3)3 + Na2CO3
B. AlCl3 + NaBr
C. Li3PO4 + K2SO4
D. MgBr2 + (NH4)2CrO4
5. For each combination below a ppt forms. Write its formula:
A. Na3PO4 + CaCl2
B. K2Cr2O7 + Al(ClO3)3
C. Mg(NO3)2 + Li2CO3
6. What is a spectator ion?
7. For each combination below a ppt forms. Write the ions that are the spectator ions:
A. (NH4)2CO3 + BaCl2
B. K3PO4 + Al(NO2)3
C. CaI2 + Li2CrO4
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8. For the chart below, if a ppt forms, write its formula. If no ppt forms, write NR. Also, write
the spectator ions for each mixture.
A
B
Ionic
Formulas
K2CO3
AlBr3
K2CO3
x
AlBr3
x
x
Ca(NO3)2
x
x
x
Mg(ClO2)2
x
x
x
x
(NH4)2CrO4
x
x
x
x
A
B
C
D
E
C
D
E
Ca(NO3)2 Mg(ClO2)2 (NH4)2CrO4
x
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Spectroscopic Notation
1. What are valence electrons?
2. How many valence electrons do each of the following atoms have:
A. Mg
B. O
C. Si
D. K
E. I
3. What charge do each of the following atoms go to:
A. Mg
B. O
C. Si
D. K
E. I
4. Write the full spectroscopic notation for:
A. Na
B. O
C. B
D. Cl
E. Ti
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5. Write the abbreviated, Noble Gas notation for:
A. Na
B. O
C. B
D. Cl
E. Ti
6. Write the abbreviated, Noble Gas notation for:
A. Ga
B. Cd
C. Y
D. Fe
E. Po
7. Why can we ignore many electrons in the Noble Gas configuration?
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