Name:
Date Due:
Chemical
Bonds
Physical Science
Chapter 11
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What are Chemical Bonds?
1. Define the following terms:
a. chemical bond=
a. electron dot diagram=
b. chemical formula=
c. subscript=
2. Describe when an atom is stable and not likely to react.
3. When is an atom unstable and likely to react?
4. What does each dot in an electron dot diagram represent?
5. When do elements tend to react?
6. What information is in a chemical formula?
7. What are subscripts used to show?
8. Why must magnesium react with two chlorine atoms to reach a stable electron configuration?
9. The compound sodium sulfide consists of a ratio of one sodium ion (Na+) to two sulfide ions
(S-2). Write the chemical formula for this compound.
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10. A molecule of sulfur dioxide consists of one sulfur atom (S) and two oxygen atoms (O). What is
the chemical formula for this compound?
11. Identify the ratio of atoms in the compound represented by the following chemical formula:
N2O5.
12. Complete the table. If you had the element hydrogen, you know that it belongs to the alkali
metals and has one valance electron, and the symbol H. Thus the electron dot configuration
would be H .
Element
# of
Valance
Electrons
Element
Symbol
Electron Dot Configuration
Hydrogen
1
H
H
Potassium
Carbon
Krypton
Selenium
Gallium
Beryllium
Fluorine
Calcium
4
Ionic Bonds
13. Define the following terms:
a. ion=
b. anion=
c. cation=
d. ionic bond=
e. ionization energy=
f. ionic compound=
g. crystals=
h. binary compound=
i.
polyatomic ions=
14. How can an atom end up with a more stable electron configuration?
15. What happens when sodium reacts with chlorine?
16. When is it easier to remove an electron from an atom?
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17. Across a period, how does the ionization energies change?
18. In a group, how does the ionization energies change?
19. Use ionization energy to explain why metals lose electrons more easily than nonmetals.
20. Once elements have become cations and anions, how do they create an ionic bond?
21. What does the shape of an ionic crystal depend on?
22. How would the properties of an ionic compound be explained?
23. Why do ionic crystals to shatter when struck?
24. What does the name for an ionic compound distinguish?
25. What does the formula for an ionic compound describe?
26. How are binary ionic compounds named?
27. How are transition metals distinguished from one another?
28. How do you write a formula for ionic compound?
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Covalent Bonds
29. Define the following terms:
a. covalent bond=
b. molecule=
c. polar covalent bond=
d. nonpolar=
30. How is a covalent bond different from an ionic bond?
31. What keeps the atoms together in a molecule?
32. What do you call it when an atom shared one pair of electrons?
33. Two pairs of electrons?
34. Three pairs of electrons?
35. Which elements have the greatest attraction for electrons?
36. What keeps the atoms together in a molecule?
37. Which atoms become more negative in a polar covalent bond? More positive?
38. How do you determine if a molecule is polar or non-polar?
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39. What are three ways that covalent bonds are different in their properties than ionic bonds?
a.
b.
c.
40. What does the name and formula for molecular compounds describe?
41. What is the general rule for which element appears first in a molecular compound?
42. How is the second element name changed?
43. What does the prefix hexa- mean?
44. How do you write a formula for molecular compounds?
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Metallic Bonds
45. Define the following terms:
a. Metallic bond=
b. Ductile=
c. Malleable=
d. Alloy=
46. How do metals achieve a stable electron configuration?
47. What holds metal ions together in a metal lattice?
48. How do metallic bonds produce some of the typical properties of metals?
49. What two important properties of metals can be explained by their structure?
50. How are metallic bonds similar and different to ionic and covalent bonds?
51. What are some useful ways alloys may differ from pure metals?
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Complete the concept map using the following words:
Anion
Ionic Bond
Non-polar
Cation
Metallic Bond
Polar
Covenant Bond
Have a Shared
Pool of
Electrons
Transfer
Electrons
Chemical
Bonds
Ions
Share
Electrons
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Ionic Compounds Lab
Pearson Education, Inc., publishing as Pearson Prentice Hall.
Background Information
Ionic compounds are composed of charged particles called ions. Positively charged ions are called cations,
and negatively charged ions are called anions. Although ionic compounds are composed of ions, they are
electrically neutral. The sum of the positive charges of the cations and the negative charges of the anions is
zero. The formula of an ionic compound can be determined from the ratio of cations and anions needed to
produce a total charge equal to zero. The symbol for the cation always appears first in the formula.
The names of ionic compounds are based on the names of their ions. For most cations, the name of the
cation is the same name as the element name. However, many transition metals form more than one ion.
For these ions, a Roman numeral is used to show the charge. For example, Fe2+ is iron(II) and Fe3+ is
iron(III). Anions are named by combining part of the name of the element and the ending –ide. For
example, the name for O2– is oxide. A covalently bonded group of atoms that has a positive or negative
charge is called a polyatomic ion. These ions have names that reflect their composition.
In this investigation, you will practice naming ionic compounds and writing their formulas by playing a card
game.
Problem
How are the names and formulas of ionic compounds determined?
Materials 40 unlined index cards
Procedure
Use the index cards to prepare four decks of playing cards.
a. Cation symbol cards. Prepare four cation symbol cards for each of the following cations. Write
the symbol for each cation on the front of an index card. On the back of each card, write
“Cation Symbol.”
Na+ K+ Mg2+ Ca2+ Al3+ Fe2+ Fe3+ Cu+ Cu2+ Zn2+
b. Cation name cards. Prepare one cation name card for each of the following cations. Write the
name of each cation on the front of an index card. On the back of each card, write “Cation
Name.”
sodium, potassium, magnesium, calcium, aluminum, iron(II), iron(III), copper(I),
copper(II), zinc
c. Anion symbol cards. Prepare four anion symbol cards for each of the following anions. Write
the symbol for each anion on the front of an index card. On the back of each card, write “Anion
Symbol.”
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F– Cl– O2– S2– PO 3– CO 2– NO – N3– Br– OH–
d. Anion name cards. Prepare one anion name card for each of the following anions. Write the
name for each anion on the front of an index card. On the back of each card, write “Anion
Name.”
fluoride, chloride, oxide, sulfide, phosphate, carbonate, nitrate, nitride, bromide, hydroxide
After you finish preparing the cards, shuffle each deck of cards separately and place the decks facedown on
the table.
To determine who goes first, have each player draw a cation symbol card. The player who draws the ion
with the highest charge goes first. If players draw the same charge, they should draw another card. Replace
the cards and shuffle the cation symbol
deck. Play continues clockwise.
To start the game, draws three cation symbol cards, three anion symbol cards, one cation name card, and
one anion name card. Then, turn over one card from each deck of symbol cards to start a discard pile.
The object of the game
is to gather the correct
number and type of
symbol cards to match
the formula
of the compound represented by the selected cation and anion name cards . Record the formula, the name,
and the number of points in the data table.
During a turn, the player may do one of the following:
Draw a card from either the cation symbol deck or discard pile, or from the anion symbol deck or
discard pile, and discard a cation or anion symbol card to the appropriate discard pile; or
Draw a new cation name card, anion name card, or both, and place the old name cards at the
bottom of the appropriate decks.
If either the cation symbol cards or the anion symbol cards are all used, mix the appropriate discard pile,
turn it over, and continue play. When either the cation name cards or the anion name cards are all used, the
game is over. The winner is the player with the most points.
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Observations
DATA TABLE
Match
Compound Name
Compound Formula
1
2
3
4
5
6
7
8
9
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Analysis and Conclusions
1. Describe how to determine the correct ratio of ions in a compound.
2. Explain why it is not possible to write a formula for a compound of sodium and calcium.
3. How many anions are required to balance one aluminum ion? Explain your answer.
5. How are the name and formula of an ionic compound determined?
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