Chemistry 110 - 02
Fall 2016
Fourth Homework
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Study Hill and McCreary Chapter 3 sections 4, and 5.
Study Hill and McCreary Chapter 4 sections 2, 6, and 7.
Prepare for the next lab. Check the Calendar in the syllabus to see which lab is next.
Finish the Iron and Sulfur Lab report.
Lab C Report due date is moved to October 20.
Complete the Study Group Assignment (see Homework 2).
The third quiz will include questions from the topics below and from homework 5. To be prepared
for the quiz, you should be able to answer these questions using only the periodic table you received
in class and the information given. Any quiz may include questions about lab safety and
procedures.
Using the periodic table, be able to give the number of valence electrons of each element in Groups
1, 2, 13, 14, 15, 16, 17, and 18.
Using the periodic table, be able to give the electronegativity values of these elements: H, Li, Be, B,
C, N, O, F, and Cl (See Hill and McCreary Figure 4.5 on page 110.)
Due 8:30 am Wednesday, October 12. 10 Points.
Late homework is not accepted after 8:30 am Thursday, October 13.
1. Your car has a dead battery. When you attempt to jump-start it, the battery explodes. Battery
acid splashes in your eyes, causing terrible pain. What should you do?
2. You are working in the lab when you accidentally spill some chemical inside the hood. What
should you do?
3. Properly record these measurements.
a.
b.
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4. What are the characteristic properties of
a. the metals
b. the halogens
5. Which of these elements are in the same period as magnesium on the periodic table?
potassium, sodium, calcium, chlorine
6. Which of these elements are in the same family as nitrogen?
carbon, phosphorus, arsenic, fluorine
7. List the seven common elements that are usually found as diatomic molecules. (A diatomic
molecule is a molecule made of two atoms.)
8. Where are the protons, electrons, and neutrons in a potassium atom?
9. What is the atomic number of each of these elements?
a. carbon
b. aluminum
c. iron
d. mercury
e. silver
10. How many protons does an atom of each of these elements contain?
a. carbon
b. aluminum
c. iron
d. mercury
e. silver
11. How many electrons does an atom of each of these elements contain?
a. carbon
b. aluminum
c. iron
d. mercury
e. silver
12. a. What experiment did Rutherford perform that led to the discovery that atoms
have a nucleus.
b. What experimental result led Rutherford to conclude that the atom has a nucleus
with a lot of mass in it?
c. What experimental result led Rutherford to conclude that the nucleus of the
atom is very small compared to the size of the atom?
d. Approximately when did Rutherford do these experiments?
13. For each pair of particles, tell whether they will attract, repel, or neither attract nor repel. Justify
your answer.
a. an electron and a proton
b. an electron and another electron
c. a proton and another proton
d. a neutron and an electron
14. Using the idea of electrical attractions and repulsions, explain why the electron in a hydrogen
atom does not fly away from the nucleus.
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15. Read the section on isotopes in Hill and McCreary on pages 74 – 75. Then answer
these questions.
137
In March 2011, iodine-131 ( 131
53 I ) and cesium-137 ( 55 Cs ) were detected coming
from the earthquake damaged Fukushima Daiichi nuclear plant in Japan.
a. How many electrons, neutrons, and protons are in one atom of iodine-131?
b. How many electrons, neutrons, and protons are in one atom of cesium-137?
16. How many valence electrons does each of these atoms have?
a. calcium
b. carbon
c. chlorine
17. Answer Hill and McCreary Chapter 4 Problem 10 (on page 131).
18. Answer Hill and McCreary Chapter 4 Problem 11 (on page 131).
19. On page 110 of Hill and McCreary is a table of electronegativities (Figure 4.5).
Atoms with higher electronegativity pull on valence electrons more strongly than
atoms with lower electronegativity. Use the values in Figure 4.5 to identify which
atom of each pair pulls on valence electrons more strongly.
a. O or C
b. H or C
c. Br or F
d. N or O
20. What are the patterns of the electronegativity of elements on the periodic table? (In other words,
where on the periodic table are the elements with low electronegativity, where are the elements
with high electronegativity, etc.)
21. According to Figure 4.5 on page 110 of Hill and McCreary, which five elements have the
highest electronegativity?
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22. Use this table, and the Lab Notebook section of the syllabus to grade your lab notebook up to
this point. Copy or reproduce this table in your homework.
Chemistry 110 Lab Notebook
14 Points
a. Thread-bound.
b. No pages added or removed.
c. Observations immediately recorded.
d. Black or blue permanent ink.
2 Points
e. Mistakes crossed out with single line.
3 Points
f. Measurements include units.
g. Table of Contents.
h. Pages numbered.
1 Point
i. Pages dated.
j. Blank pages crossed out with note & date.
k. Lab begins on a new page.
l. Table of Abbreviations (optional).
23. In the lab, you pour 50 mL of silver nitrate solution into a clean, dry graduated
cylinder. Then you discover that you were supposed to pour 5.0 mL, not 50 mL!
What should you do with the 45 mL you do not need?
And new Philosophy calls all in doubt,
The Element of fire is quite put out;
The Sun is lost, and th' earth, and no man's wit
Can well direct him where to looke for it.
And freely men confesse that his world's spent,
When in the Planets, and the Firmament
They seeke so many new; they see that this
Is crumbled out againe to his Atomies.
'Tis all in peeces, all cohaerence gone;
All just supply, and all Relation:
Prince, Subject, Father, Sonne, are things forgot,
For every man alone thinkes he hath got
To be a Phoenix, and that there can bee
None of that kinde, of which he is, but hee....
- from "The First Anniversary"
- John Donne
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