CHEMISTRY-1 CP, PERIOD 6
CHAPTERS 7 & 8—CHEMICAL BONDING
DAILY PLANNER
DAY
1
Mon, 3/19
2
3
4
5
6
7
8
9
10
Tent. Fri, 3/30
CLASSWORK
Intro to Ionic & Covalent Bonding WebTutorial (10 Points)
Review Sheet on Oxidation Numbers & Charges for
Homework
Notes: Illustrating Ionic Bonds/Metallic Bonding/
HOMEWORK
Finish today’s Review Sheet
Daily Quiz
Notes: Covalent Bonds/Lewis Structures
Lab: Properties of Ionic & Covalent Bonds
(40 Points)
Daily Quiz
VSEPR Activity (5 Points)
Notes: VSEPR
Daily Quiz
Notes: EN and Types of Bonds
Begin Molecular Models Activity
Daily Quiz
Notes: Polarity of Molecules/Intermolecular Forces
Finish Daily Quiz (25 Points)
Homework & Extra Credit Due (50 Points +)
Molecular Modeling Lab (40 Points)
Go Over Homework
Review for Test
Polarity Lab (50 Points)
Review for Test
Bonding Test (100 Points)
Finish Lab
HW3: Worksheet C
HW1: Worksheet A
HW2: Worksheet B
HW4: Worksheet D
Finish Lab
HW5: Worksheet E
HW6: Worksheet F
Finish Molecular Model Lab
Finish today’s lab
Congratulations to Alyssa Guthrie & Haley Warner—Top Pair for Chapter 6
Total Possible Points this Chapter: 320 + 19 Possible EC Points
Important Dates: 3rd Quarter ends April 2
HOMEWORK GRADES
A (30/30)
B (27/30)
C (24/30)
D (21/30)
F (18/30)
0 (0/30)
COMPLETED
6/6
5/6
4/6
3.5/6
3/6
Less than 3/6
EXTRA CREDIT:
5 Points: Worksheet G
4 Points: Worksheet H
5 Points: Text p. 251 Standardized
Test Prep #1-15
5 Points: Create a poster illustrating
5 different metals and their crystal
structures.
WORKSHEET A
A. Using Lewis Dot Diagrams or charges, illustrate how the following elements form ionic compounds
1. KBr
2. Sodium & Nitrogen
3. Ca & P
4. Magnesium and Oxygen
5. AlN
6 Lithium and Sulfur
7. Barium and Chlorine
8. CaS
9. Zn and Cl
B. Write the chemical formulas for each of the following binary ionic compounds. You may use the crisscross method or
you may draw the Lewis Structures to determine the formulas!
1. sodium nitride
______________________
6. Aluminum fluoride
______________________
2. lead (IV) iodide
______________________
7. Tin (IV) bromide
______________________
3. strontium oxide
______________________
8. Manganese (IV) oxide______________________
WORKSHEET B
True/False
_____ 1. Metals that are good conductors of electricity are said to be ductile.
_____ 2. Drifting valence electrons insulate cations from one another and contribute to the malleability of a metal
_____ 3. Metals are good conductors of electricity because electrons flow freely in them.
_____ 4. Most of the metals you encounter on a daily basis are in their pure elemental form.
_____ 5. Metals are crystalline.
MATCHING
_____ 6. Ductile
A. The attraction of valence electrons for positive metal ions
_____ 7. Metallic Bonds
B. A negatively charged ion
_____ 8. Ionic Bonds
C. Electrons in the outermost energy level
_____ 9. Malleable
D. A solid in which the atoms, ions or molecules are arranged in an orderly, repeating, 3-dimensional pattern
_____ 10. Anion
E. A mixture of 2 or more elements, at least one of which is a metal
_____ 11. Cation
F. A depiction of valence electrons around the symbol of an element
_____ 12. Alloy
G. Can be drawn into wires
_____ 13. Crystalline Solid
H. The electrostatic attraction that binds oppositely charged ions together
_____ 14. Lewis Structure
I. Atoms typically require 8 valence electrons to be stable
_____ 15. Valence Electron
J. Can be hammered or forced into shapes
_____ 16. Octet Rule
K. A positively charged ion
MULTIPLE CHOICE
_____ 17. Ionic bonds typically form between
a. members of the same family
b. a metal and a nonmetal
c. all nonmetals
d. all metals
_____ 18. Metals are good conductors of electricity because they
a. form crystal lattice
b. contain positive ions
c. contain mobile valence electrons
d. form ionic bonds
_____ 19. An ionic compound is
a. electrically neutral
b. composed of anions and cations
c. held together by ionic bonds
d. all of the above
_____ 20. A metallic bond is a bond between
a.
valence electrons and positively charged metal ions
b.
the ions of two different metals
c.
a metal and nonmetal
d.
none of the above
_____ 21. Which element when combined with chlorine would most likely form an ionic compound?
a. lithium
b. carbon
c. phosphorus
d. bromine
WORKSHEET C
A. Draw Lewis Structures for the following covalently bonded compounds.
a. HCl
b. CCl4
c. Cl2O
d. I2
e. N2O
f. PI3
g. C2H4
h. N2
i. CH4
j. HCN
k. H2S
l. O3
m. C2H2
n. CCl2Br2
o. NF3
B. Determine which of the following compounds contain covalent bonds. Circle the compounds that contain only covalent bonds.
KCl
C6H8O6
HNO3
Mg3N2
LiClO4
Br2
N2H4
WORKSHEET D
A. On the line at the left, write the term from the list that matches each description below.
trigonal planar
VSEPR theory
unshared pair
bond angle
ball-and-stick model
symmetry
hybrid orbital
_____________________ 1. a visual model of molecular geometry
_____________________ 2. the geometric angle between two adjacent bonds
_____________________ 3. a pair of valence electrons not involved in a bond
_____________________ 4. the theory that states that the pairs of valence electrons are arranged as far apart as possible in small
molecules
_____________________ 5. name for a triangular flat molecule
B. Complete the following table by filling in the molecular shape and bond angles for each of the molecules listed.
Molecule
Molecular Shape
Bond Angles
H2O
CHCl3
BF3
NH3
CO2
C. Draw a ball-and-stick model for each of the following molecules in the space provided. Label the bond angles in your drawings.
1. PCl3
2. H2S
3. CBr4
4. C2F2
5. C2H6
5. NH4+
WORKSHEET E
A. Find the electronegativity difference between each of the following pairs of elements and to predict the kind of bond that
will be formed.
Element Pairs
Electronegativity Difference
Type of Bond
calcium and fluorine
carbon and silicon
beryllium and sulfur
hydrogen and germanium
zinc and bromine
B. MULTIPLE CHOICE
Write the letter of the correct answer on the line. If you do not write the letter on the line, I will not count it as complete!
____1. An atom of which element has the greatest attraction for the electrons in a bond with a hydrogen atom?
a) chlorine
b) silicon
c) phosphorus
d) sulfur
____2. When the atoms within molecules have different electronegativities, the electrons are shared unequally and the bonds
are
a) nonpolar
b) ionic
c) polar
d) metallic
____ 3. What is the electronegativity difference between carbon and oxygen?
a) 1
b) 2
c) 3
d) 0
____ 4. Which of the following elements is the most electronegative?
a) aluminum
b) arsenic
c) nitrogen
d) fluorine
____ 5. Which element is more likely to give up an electron?
a) radium
b) bromine
c) gold
d) phosphorus
____ 6. What kind of bond forms between sulfur and fluorine?
a) nonpolar
b) ionic
c) polar
d) metallic
____ 7. Which element has the highest electronegativity?
a) bromine
b) oxygen
c) chlorine
d) fluorine
_____8. Classify the bonds in the following compounds as ionic, polar covalent, or non-polar covalent: NH3, LiF, H2,
respectively.
A. Polar covalent, ionic, non-polar covalent
B. Ionic, polar covalent, non-polar covalent
C. Polar covalent, non-polar covalent, ionic
D. Ionic, non-polar covalent, polar covalent
E. Non-polar covalent, ionic, polar covalent
_____9. Which of the following bonds is the most polar? Explain your response.
a) O–F
b) N–F
c) C–F
d) H–F
____ 10. The measure of an atom’s ability to attract electrons towards itself in a chemical bond is known as
a) electronegativity
b) bond strength
c) electron affinity
d) bond order
WORKSHEET F
A. The line below represents the range of differences in electronegativity that are possible between any two elements in
the periodic table. The smallest difference is represented by the left end of the line, and the greatest difference by the right
end of the line. In the space at the left below, write the letter of the labeled parts from this line that corresponds to the
descriptions. Some of the letters may be used more than once.
a
b
0.0
c d
0.5
1.0
1.5
e
f
2.0
2.5
g
3.0
1. ______ The lowest possible value of EN.
2. ______ The bond of greatest possible ionic character.
3. ______ A pure nonpolar covalent bond
4. ______ A polar covalent bond
5. ______ An ionic bond that would form between calcium and oxygen
6. ______ The bond in a diatomic molecule of an element
7. ______ A bond that is classified as nonpolar but that has a slight polarity
8. ______ The division between nonpolar covalent and polar covalent bonds
9. ______ A bond that would form between cesium and fluorine
10. ______ The division between ionic and polar covalent bonds
B. Illustrate the molecular shape of each of the following molecules. Identify each molecule as polar or nonpolar.
1) BFI2
2) NH2Cl
3) SCl2
4) CO2
5) BF3
6) NF3
C. Questions
1) Why is HCl a polar molecule while Cl2 is a nonpolar molecule?
WORKSHEET G—EXTRA CREDIT
A. Predict the type of chemical bond (metallic, covalent, or ionic) you would expect for each of the following
materials.
1. A material used in making electrical transmission wire. _____________________________________
2. A material used to make the insulation wrapped around transmission lines that lie on the ocean floor.
___________________________________________
3. A material used as a lubricating oil.
______________________________________________
4. A material that is dissolved in large quantities in sea water.
__________________________________
5. A material used to make high-temperature furnaces.
__________________________________
6. A material used in the manufacture of wires in suspension bridges.
7. A material used to make cans.
____________________________
__________________________________
8. A material used as a gaseous propellant in spray cans, such as deodorant or shaving cream dispensers.
_____________________________________________
9. A material that evaporates readily at room temperature.
_________________________________
10. A material that is a good conductor when melted but a poor conductor when solid.__________________
B. Complete each statement.
Electronegativity
Malleable
Metallic
Double Bond
Shielding Effect
Dipole
Ductile
Conductivity
Polar Molecule
1. The ___________________________________________ is caused when electrons in inner energy levels tend to block
the attraction of the nucleus for valence electrons.
2. When electrons are shared unequally between two atoms, a(n) ___________________ is formed.
3. A(n) __________________________________ metal is one that can be drawn into wires.
4. __________________________________ is a measure of the ability of an atom to attract electrons in a chemical bond.
5. A metal that can be hammered or rolled into thin sheets is said to be _______________________.
6. A bond formed by the sharing of two pairs of electrons is called a(n) __________________________.
7. _______________________________ is a measure of the ease with which electrons flow through a material to
produce an electric current.
8. A molecule in which there is an unequal distribution of electrical charges is called a(n)
_____________________________________.
9. In the type of bond called a(n) __________________________, valence electrons are shared among many atoms.
WORKSHEET H—EXTRA CREDIT
_____ 1. Which list of formulas represents compounds only?
A) CO2, H2O, NH3
B) H2, Ne, NaCl
C) H2, N2, O2
D) MgO, NaCl, O2
_____ 2. Which property could be used to identify a compound in the laboratory?
A) mass
B) temperature
C) melting point
D) volume
_____ 3. Given a formula for oxygen:
O=O
What is the total number of electrons shared between the atoms represented in this formula?
A) 1
B) 8
C) 2
D) 4
_____ 4. Which substance can not be decomposed by a chemical change?
A) AlCl3
B) HI
C) H2O
D) Cu
_____ 5. An atom in the ground state has seven valence electrons. This atom could be an atom of which
element?
A) calcium
B) oxygen
C) fluorine
D) sodium
_____ 6. As a bond between a hydrogen atom and a sulfur atom is formed, electrons are
A) shared to form an ionic bond
B) shared to form a covalent bond
C) transferred to form an ionic bond
D) transferred to form a covalent bond
_____ 7. A barium atom attains a stable electron configuration when it bonds with
A) one chlorine atom
B) two chlorine atoms
C) one sodium atom
D) two sodium atoms
_____ 8. Sodium atoms, potassium atoms, and cesium atoms have the same
A) atomic radius
B) first ionization energy
C) total number of protons
D) oxidation state
_____ 9. When sodium and fluorine combine to produce the compound NaF, the ions formed have the same electron configuration as
atoms of
A) argon, only
B) neon, only
C) both argon and neon
D) neither argon nor neon
_____ 10. Matter that is composed of two or more different elements chemically combined in a fixed
proportion is classified as
A) a compound
B) a mixture
C) an isotope
D) a solution
C) CH4
D) NH4Cl
_____ 11. Which formula represents an ionic compound?
A) H2
B) CH3OH
_____ 12. What is the total number of different elements present in NH4NO3?
A) 7
B) 3
C) 9
D) 4