Chemistry
CH 6 & 7 Reading Assignment (Ionic Bonds)
CH 6
Pg 175-176
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Define chemical bond:
Why do atoms bond?
What determines the type of bond formed between atoms?
What happens in an ionic bond and in a covalent bond?
Define electronegativity and why is it important in determining the type of bond between
atoms?
What is the factor involved in why bonds have both ionic and covalent characteristics?
In determining the type of bond created between atoms you subtract the electronegative values
of the atoms involved, if the difference is below 1.67 it will be a ____ bond, which can further be
classified into ___ if the difference is between 1.67 and 0.3 and if below 0.3 it will be ___.
Greater than 1.67 the bond will be classified as ___.
What type of atoms form molecules that are considered pure covalent (where their
electronegativity difference equals 0.0)?
What happens in a polar covalent bond and in a nonpolar covalent bond?
Pg 190-194
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What is an ionic compound?
What are ionic compounds referred as?
What is a formula unit and give an example?
Since ionic bonds, bond to be neutral, what would be the formula between Al+3 and O-2?
Write the ionic Lewis diagram for the following ionic bonds (show electron transfer with arrows,
the ions created, and finally the crystal created)
a. CaF2
b. AlCl3
c. Fe2O3 (Fe in Fe+3 state)
d. SnO2 (Sn in Sn+4 state)
Write the chemical formula between the following atoms: (find charges first)
a. Na and O
b. Aluminum Sulfide
c. Chromium (lll) Bromide
d. Cu (l) and N
What is the crisscross method in writing formulas for ionic compounds and what do you need to
do before expressing the answer?
Ionic crystals form into an ordered arrangement called ___.
How are crystal lattices arranged?
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In the crystal structure of salt, how many neighbors does each ion have?
Why in the crystal structure of CaF2 is the Ca ion surrounded by 8 F ions?
What is lattice energy and what does it mean if it has a negative sign?
What is a unit cell?
Why do ionic compounds have high melting and boiling points?
Why are ionic compounds hard?
Why are ionic compounds brittle?
What is needed for an ionic crystal to conduct electricity?
What form will ionic crystals conduct?
What makes some ionic compounds soluble in water and others not soluble?
What are polyatomic ions and how are they bonded internally and what type of bond does the
ion get involved in?
30. What does a negative and positive charge mean in a polyatomic ion?
31. Write the following ionic formulas for the following:
a. Ca and PO4
b. Lead IV Carbonate
c. Zinc Hypobromite
d. Ni and OH
CH 7
Pg 219-226
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What does a chemical formula tell us?
What is a molecular compound?
Define monoatomic ions:
The main group elements (which involve what PT blocks) gain or lose electrons to be like ___?
How do you name monoatomic cations?
How do you name monoatomic anions?
Name the following ionic compounds:
a. Ca3P2
b. PbO
c. AgO
d. Cr2S3
What is the stock system and why do we use it?
What are binary compounds
What is a subscript and what does it represent?
What is nomenclature?
What is an oxyanion?
The oxyanion that has one more oxygen atoms uses the ending ___ while the oxyanion with less
oxygen atoms uses the ending ___ when naming.
When a compound has one more oxygen than the ….ate we use ___ at the beginning (sometime
shorten as per), when compounds have one less oxygen than …ite we use ___ at the beginning.
46. Name the following a. ClO- b. ClO2- c. ClO3- d. ClO447. Name the following ionic compounds:
a. Fe(ClO4)3
b. (NH4)2SO4
c. Hg2(OH)2
d. Zn(C2H3O2)2
Pg 232-249
48. Know the general rules for assigning oxidation numbers (HC)
49. Assign oxidation numbers for each element below: (HC)
a. HCl
b. HClO3
c. P4O10
d. H2O2
e. PCl3
f. SO2
g. CF4
h. O2
i. OF2
j. SO4-2
50. Define molar mass and formula mass:
51. Calculate the formula mass of Calcium Phosphate.
52. What are the units of molar and formula mass?
53. What is % Composition?
54. To calculate % composition, find molar or formula mass and divide each atoms mass by the total
amount x 100, so calculate the % composition of (NH4)2CO3
55. What is an empirical formula?
56. What is the empirical formula of a. H2O2 b. CaCl3
57. To calculate an empirical formula 1. Find moles of each element (if given as % just change % to
grams) 2. Divide each elements mole by the smallest element mole to find mole ratio 3.
Express mole ratio to the smallest whole number ratio ( 1:1.5 is 2:3 ratio) 4. Insert mole ratio
into formula as subscripts, find empirical formula for the following:
a. 36.48% Na, 25.41% S and 38.11% O
b. 1.04g K, 0.70g Cr, and 0.86g O
58. An empirical formula is a reduced molecular, so when finding the molecular formula you must first start
with the empirical, 1. Find empirical formula given information 2. Find molecular mass of empirical
formula 3. Divide empirical molec. Mass into molecular formulas mass which will be given in the problem
4. Now take the number you got (which tells you how many times heavier the molecular formula is than
the empirical) and multiply the subscripts of the empirical formula by the number you got, ex. If you got 3
and empirical formula is X2Y3, then molecular is X6Y9. Find the molecular formula given; 26.7g of P, 18.1g
of N, and 107.2 g of Cl. The formula mass of the compound is 705.0 amu.