Download Honors Chemistry

Tustin HS AP Chemistry
SUMMER ASSIGNMENT
Instructor:
Email:
Textbook:
Ms. Abbey Zinsser
[email protected] or [email protected]
Chemistry: The Central Science, Brown, LeMay, Bursten, 11th edition (2006).
Publisher: Prentice Hall
ISBN # 978 013 600 6176
Due Date:
1st day of school (September 1st, 2015)
In order to complete the summer assignment you will need to have access to the textbook. A
copy of the textbook is available for use on Haiku or for checkout at the library.
Assignment: The assignment is divided into 7 modules. Each module (except for Module 01) will be collected
on the first day of school. I suggest you complete one to two modules a week and pace yourself throughout
the summer. Failure to complete this assignment may result in removal from the course.
Module
Topic
01
Polyatomic Ion Memorization
02
Rounding & Significant Figures
Module 02 Worksheet
15
03
Naming Ionic & Covalent
Compounds
Module 03 Worksheet
40
04
Naming Acids
Module 04 Worksheet
20
Chapter 1 Cover Sheet
with Notes
40
Textbook Problems
20
Chapter 2 Cover Sheet
with Notes
40
Textbook Problems
25
Chapter 3 Cover Sheet
with Notes
40
Textbook Problems
30
05
06
07
Submit…
Nothing…you will be
quizzed on the 2nd day
of school
Chapter 1
Chapter 2
Chapter 3
TOTAL
1
Point Value
40 quiz points
270
Modules:
 For Module 01: Nothing to turn in, but TEST on POLYATOMIC IONS on 2nd day of School. DON’T
PROCRASTINATE!!
 For Modules 02-04: Module Worksheets will be collected
 For Modules 05-07: You will need access the textbook through Haiku or checkout from the library
o You will be turning in Chapter 1-3 coversheets along with notes and bookwork.
o Title the assignment with Chapter # & problem numbers. Example: Chapter 1 #1, 7, 11, etc.
o SHOW ALL WORK, including units and dimensional analysis where appropriate
o Refer to the examples within in the textbook for help
o You may also email me for help; I will get back to you as soon as I can.
Scoring:
 Passing score: 190/270 (70%)
o Each question will be graded for accuracy and/or completion.
 To receive maximum score:
o Show all work. No work = no credit. If you aren’t sure what kind of work to show, view the
examples.
o All answers must be written in the boxes to the right with units (when given) and correct
significant figures.
o Submit on time on the first day of school.
Agenda for the First Week of School:
Day, Date
01
02
03
04
05
06
Agenda
Summer Assignment due
Review syllabus
Ion Memorization Test
Review Safety
Tuesday 09/01/15
Wednesday 09/02/15
Thursday 09/03/15
Review summer assignment
Friday 09/04/15
Review summer assignment
Monday 09/07/15
Review summer assignment
Tuesday 09/08/15
Unit 01 Test
2
MODULE 01: Common Ions to KNOW!!
This part of the summer assignment is quite simple. Just give yourself enough time to master the formulas,
charges and names of the common ions. On the 2nd day of school, you will be given a quiz on these ions. You
will be asked to:
 Write the names of these ions given the formula and charge
 Write the formula and charge when given the names
TABLE 1: Ionic Charges of Representative Elements
Cations: Full Name
1
+
Li
Na+
K+
Rb+
Cs+
2
3-11
12
13-14
2+
Be
Mg2+
Ca2+
Sr2+
Ba2+
3+
Al
2+
+
Ag
Zn
Cd2+
Anions: End in “-ide”
15
16
17
3-
2-
-
N
P3-
O
S2Se2-
18
F
ClBrI-
“From the Table” Ions: For the ions in Table 1, their placement in the Periodic Table suggest the charge on the
ion, since the neutral atom gains or loses a predictable number of electrons in order to obtain a noble gas
configuration. This was a focus in first year chemistry, so if you are unsure what this means, get HELP BEFORE
the start of the year. Three transition metals are also included (silver, cadmium and zinc). These three
elements will always have the charge given in the table and should be also be memorized. You will have a
periodic table to reference for this ion quiz, so the above ions should be quite easy.
3
Polyatomic Ions: The common ions in Table 2 need to be MEMORIZED. Below are a number of patterns that
can be used to greatly reduced the amount of memorizing one must do.
Hint 1: “-ate” ions have one more oxygen that the corresponding “-ite” ions, but the same charge. If
you memorize the “-ate” ions, then you should also be able to memorize the “-ite” ions quite easily,
and vice versa.
Example: Sulfate is SO42-, so sulfite is the same charge with one less oxygen (SO32-)
Example: Nitrate is NO3-, so nitrite is the same charge with one less oxygen (NO2-)
Hint 2: If you know that a sulfate ion is SO42-, then to get the formula for hydrogen sulfate, you add a
hydrogen ion to the front of the formula. Since hydrogen has a 1+ charge, the net charge on the new
ion is less negative by one.
Example:
PO43→
HPO42→
H2PO4phosphate
hydrogen phosphate
dihydrogen phosphate
Hint 3: Other prefixes: “Per-” indicates one more oxygen than the “–ate” form
“Hypo-” indicates one less oxygen than the “–ite” form
Example: ClO4→ ClO3- → ClO2- → ClOperchlorate
chlorate
chlorite hypochlorite

The Halogens are all the same: F, Cl, Br, I all behave the same, so if chlorate is ClO3- ,
Bromate is …… BrO3- !!!
Hint 4: Make FLASHCARDS to help with your memorization!!
TABLE 2: Common Polyatomic Ions
1- charge
Formula
-
Name
2- charge
Formula
2-
3- charge
Name
Formula Name
PO43PO33-
H2PO4
C2H3O2HSO3HSO4HCO3-
Dihydrogen Phosphate
Acetate
Hydrogen Sulfite
Hydrogen Sulfate
Hydrogen Carbonate
HPO4
C2O42SO32SO42CO32-
Hydrogen Phosphate
Oxalate
Sulfite
Sulfate
Carbonate
NO2-
Nitrite
CrO42-
Chromate
NO3CNOHMnO4ClOClO2ClO3ClO4BrO3SCNIO3-
Nitrate
Cyanide
Hydroxide
Permanganate
Hypochlorite
Chlorite
Chlorate
Perchlorate
Bromate
Thiocyanate
Iodate
Cr2O72SiO32O22S2O32-
Dichromate
Silicate
Peroxide
Thiosulfate
4
Phosphate
Phosphite
1+ charge
NH4+
H3O+
Ammonium
Hydronium
MODULE 02: Rounding & Significant Figures
NOTES: ROUNDING
Definition
Rounding involves reducing the number of digits in a number while still accurately
representing the original number
Example The number 4.9 is very close to 5. For simplicity or accuracy sake, we can round this
number to 5.
What are the
1. You may round to any “place” of a number.
rules?
2. The place you are rounding is followed by a 0, 1, 2, 3, or 4, then you “round down”
to the next number
3. The place you are rounding is followed by a 5, 6, 7, 8, or 9, then you “round up” to
the next number
Placements
Given
Round 24.45 to the nearest ones
place
EXAMPLES: ROUNDING
Work Shown
o Identify the ones place
24.45
Less than 5
24.00
573.67
Round 573.67 to the nearest
hundreds place
Greater than 5
600.00
1.483
Round 1.443 to the nearest tenths
place
Greater than 5
1.500
58.3382
Round 58.3382 to 3 decimal places
Less than 5
58.3380
o Identify the hundreds place
o If the number to the right of the hundreds
place is greater than or equal to 5, then
round up.
o To round up, raise the hundreds place to
the next number and use zeros for all other
numbers
o Identify the tenths place
o If the number to the right of the tenths
place is greater than 5, then round up.
o To round up, raise the tenths place to the
next number and use zeros for all other
numbers
rd
o Identify the 3 decimal place
o If the number to the right of this place is
less than 5, then round down.
o To round down, keep this place as it is and
use zeros for all other numbers
24
600
1.5
58.338
nd
4.8998
Greater than 5
Round 4.8998 to 2 decimal places
o If the number to the right of the ones place
is less than 5, then round down.
o To round down, keep the ones place as it is
and use zeros for all the places to the right
Final Answer
4.9000
5
o Identify the 2 decimal place
o If the number to the right of this place is
greater than 5, then round up.
o To round up, raise this place to the next
number and use zeros for all other
numbers
o If you have to round a 9 up, it becomes 0
and the # to the left increases by 1.
4.90
Definition
NOTES: SIGNIFICANT FIGURES
Significant figures are digits in a number that indicate the level of precision of a
measuring device
Example A ruler can only precisely measure based on each tick mark. In the following example,
each tick mark represents 1/10 of a centimeter, or 0.1cm. So, the ruler can only
precisely measure to the first decimal place but you can estimate the 2 nd decimal place
to some degree of “confidence.”
What are the rules?
1. All non-zero (1, 2, 3, 4, 5, 6, 7, 8, 9) digits are ALWAYS significant
2. All zeros are NOT significant, UNLESS
a. Zero is between two other non-zero numbers
b. Zero is at the end of the number AND has a decimal point (anywhere
within the number)
3. Exact values have infinite significant figures. This includes…
a. counting whole numbers (ie, counting the number of students in the
classroom).
b. some known relationships (ie, 12 in = 1 ft)
Adding/Subtracting When adding or subtracting, you must always take the lowest number of significant
figures AFTER the decimal place (or just the number of decimal places)
Multiplying/Dividing When multiplying or dividing, you must always take the lowest number of significant
figures before and after the decimal place
Multi-step Algebra When adding/subtracting AND multiplying/dividing, you must keep track of your
significant figures by rounding after each operation.
Don’t forget your order of operations!
PROBLEM
TYPE
Determining
the number
of significant
figures
Given
EXAMPLES: SIGNIFICANT FIGURES
Work Shown
Final Answer
o All non-zero digits are significant (Rule 1)
o Zero is not in between two other numbers (Rule
2a) and it is not at the end of the number (Rule
2b) not significant
2 significant
figures
0.56
0.56
4.560
4.560
o All non-zero digits are significant (Rule 1)
o Zero at the end of the number AND with a
decimal point is significant (Rule 2b)
4 significant
figures
2205.2
2205.2
o All non-zero digits are significant (Rule 1)
o Zero in between two other digits, 2 and 5 is
significant (Rule 2a)
5 significant
figures
o All non-zero digits are significant (Rule 1)
o Zero in between two other digits, 6 and 4 is
significant (Rule 2a)
o Zero in front of the number is not significant
(Rule 2)
0.60436
0.60436
6
5 significant
figures
Adding and
subtracting
with
significant
figures
4.322 + 2.57
5.080 – 1.400
2.13 x 5.0
Multiplying
and dividing
with
significant
figures
4.322
+2.57
6.892
3 decimals
2 decimals
6.89
5 . 0 8 0 3 decimals
+ 1 . 4 0 0 3 decimals
6.480
6.480
2.13
x 5.0
10.65
504 ÷ 40
2 sig figs
o Round answer to the smallest number of
significant figures (2 sig figs)
6.480
3.7 x108
o Divide the two numbers (divide = fraction)
o Count the number of significant figures for each
of the two numbers being divided
3 sig figs
1 sig fig
o Round answer to the smallest number of
significant figures (1 sig fig)
= 126
100
o Use the order of operations: simplify the
parentheses first
o When adding, significant figures are limited by
the number of decimal places. 8.6 has 1 decimal
place while 3.45 has 2 decimal places. Round to
1 decimal place
o Multiply the 6.6 and 12.1
o When multiplying, significant figures are limited
by the number with the lowest number of sig
figs. 6.6 has 2 significant figures and 12.1 has 3
significant figures. Round to 2 significant
figures.
6.6 (8.6+3.45)
6.6 (12.05)
Multi-step
algebra with
significant
figures
o Subtract the two numbers
o Count the number of decimal places for each of
the two numbers being added
o Answer should have the smallest number of
decimal places (3 decimal places)
6.89
o Multiple the two numbers
o Count the number of significant figures for each
of the two numbers being multiplied
3 sig figs
11
5040
40
o Add the two numbers
o Count the number of decimal places for each of
the two numbers being added
o Answer should have the smallest number of
decimal places
o Round to the lowest number of decimal places
(2 decimal places)
6.6 (12.1)
6.6(8.6+3.45)
79.86
80.
Decimal after the zero
makes the zero significant
(Rule 2b)
7
100
80.
MODULE 03: Naming & Writing Chemical Compounds
NOTES: Naming & Writing Ionic Compounds
An ionic compound is formed between a metal and a nonmetal, or a cation ion (positive
ion) and an anion (negative ion).
How do I know it
is an ionic
compound?
Naming Rule 1: Look at the cation first. If the cation has only one possible charge (Group 1, Group 2, Al,
Ag, Cd, Zn)
 Write cation first
 Write anion last ending in –ide
Examples: 1) CaCl2
 Look at Ca first! ← Ca is in group 2 (only can have a charge of 2+)
 Chlorine become Chloride
= Calcium Chloride
2) Al2O3 = Aluminum Oxide
Naming Rule 2: Look at the cation first. If the cation has more than one possible charge (most transition
metals, post-transition metals)
 Write cation first, write cation charge (as Roman Numeral) in parentheses
 Write anion last ending in –ide
 Charge of cation is based on charge balance
Examples:
1) FeCl3
o Look at Fe first! ← Fe is a transition metal (can have a charge of 2+ or 3+)
o To determine charge of Fe → look at Cl
o Cl has a charge of 1o There are 3 Cl1- → overall negative charge of -3
o To balance a negative three, you must have a positive three
o Fe must have a charge of 3+ →Iron(III)
= Iron (III) Chloride
2) Cr2S3
o Look at Cr first! ← Cr is a transition metal (can have a charge of 2+ or 3+)
o To determine charge of Cr → look at S
o S has a charge of 2o There are 3 S2- → overall negative charge of -6
o To balance a negative six, you must have a positive six
o The overall charge of Cr is +6, but there are 2 Cr’s , so each Cr will have
a charge of +3
o Cr has a charge of 3+ →Chromium(III)
= Chromium (III) Sulfide
Naming Rule 3: When polyatomic ions are involved, follow Rules 1 & 2. Write full polyatomic name in
place of cation or anion.
Examples:
1) K2SO4
o Look at K first! ← K is in group 1 (only can have a charge of 1+)
o Need to recognize SO4 as sulfate
= Potassium Sulfate
8
2) CuCO3
o Look at Cu first! ← Cu is a transition metal (can have a charge of 1+ or 2+)
o To determine charge of Cu → look at CO3
o You need to recognize CO3 as carbonate
o CO3 has a charge of 2o There is one CO32- → overall negative charge of -2
o To balance a negative two, you must have a positive two
o So, the overall charge of Cu is +2
o Cu has a charge of 2+ → Copper(II)
= Copper (II) Carbonate
Writing Rule 1:
1) Write the formulas for the cation and anion, including charges
2) Check to see if the charges are balanced
o If balanced, just remove charges
o If not balanced, continue with rule #3
3) Balance charges
o Use parentheses if more than one polyatomic in is needed
o Write subscripts if more than one ion is needed to balance
o Use crisscross method to balance subscripts
o Remove charges
Example:
1) Barium nitrate
 Write the formulas: Ba2+ NO31 Think: Do +2 and -1 balance each other? NO!….
 Ba2+ NO31- → Ba(NO3)2
NOTES: Naming Molecular Compounds
A molecular compound is formed between a two nonmetals. Also known as a covalent
compound.
How do I know it
is a molecular
compound?
Rule: For the 1st nonmetal:
o Name the element
o Use the prefix if there is more than one of
that element
For the 2nd nonmetal:
o Name the element
o Always include the prefix
o Use –ide ending
Example: NF3
o Two nonmetals! = covalent
o First element:
o Nitrogen → only one = no prefix
o Second element:
o Fluorine = fluoride
o 3 of them = prefix “tri-“
= nitrogen trifluoride
9
Prefixes Used in Naming Molecular
Compounds
Prefix
Number
mono1
di2
tri3
tetra4
penta5
hexa6
hepta7
octa8
nona9
deca10
MODULE 04: Naming & Writing Acids
What is an acid?


Types of Acids


NOTES: Naming & Writing Acids
A form of ionic compound
Hydrogen salt dissolved in water (aq)
Binary: contains two elements
o Hydrogen + nonmetal
Oxyacid: contains oxygen
o Hydrogen + polyatomic
Naming & Writing Use prefix “ hydro” – root of nonmetal -- ic acid
Binary Acids:
Example #1: HCl
 Hydro – Chlor- ic Acid → Hydrochloric Acid
Example #2: Hydrofluoric Acid
 HF
Naming & Use root of anion (polyatomic) then check ending
Writing Oxyacids
 Polyatomic ends in –ate
Root –ic acid
 Polyatomic ends in –ite
Root –ous acid
Example #1: HNO3
 HNO3 →Nitrate→ ends in -ate→ root-ic
→Nitric Acid
Example #2: HNO2
 HNO2 →Nitrite→ ends in -ite→ root-ous
→Nitrous Acid
Example #3: Sulfuric Acid
 Sulfuric → ends in –ic → polyatomic must end in –ate → sulfate
 Two H+ must balance -2 charge on sulfate ion, SO42→H2SO4
10
MODULE 02: Rounding & Significant Figures Worksheet
Question
1. Round 729.5005 to three decimal places.
Final Answer
2. Round 9.4514 to two decimal places.
3. Round 5.3798 to the thousandths place.
4. Round 0.00023350 to three significant figures.
5. Round 364080.22 to five significant figures.
6. How many significant figures are in the number 50200?
7. How many significant figures are in the number 0.00045080?
8. There are 59 students enrolled in AP Chemistry. How many significant figures
does this reflect?
9. Add 3.207 and 4.70 and report the answer with the appropriate significant
figures.
10. Subtract 0.0279 from 0.10 and report the answer with the appropriate significant
figures.
11. Find the product of 45.03 and 0.798 and report the answer with the appropriate
significant figures.
12. Divide 1080. and 40. and report the answer with the appropriate significant
figures.
13. Calculate the following and report the answer with the appropriate significant
figures:
(3.95 + 4.50)
10.
14. Calculate the following and report the answer with the appropriate significant
figures:
(13.9)(0.0058)
(978 − 863.7)
15. Calculate the following and report the answer with the appropriate significant
figures:
11.02 + 2.00(1.1)(13.5 − 1.6)
11
12
MODULE 03: Naming & Writing Compounds Worksheet
Name the following compounds:
Answer
1) NaBr
2) CaO
3) CO2
4) MgBr2
5) Be(OH)2
6) N2S
7) ZnSO4
8) AuBr3
9) CuC2H3O2
10) KMnO4
11) CaCO3
12) NH4NO3
13) CO
14) Li2S
15) MgCl2
16) SF6
17) Fe2O3
18) PbSO3
19) Zn3(PO4)2
20) NO2
13
MODULE 03: Naming & Writing Compounds Worksheet
Write the formula for the following compounds:
Answer
21) Potassium iodide
22) Magnesium oxide
23) Nitrogen monoxide
24) Ammonium chloride
25) Iron (III) oxide
26) Magnesium phosphate
27) Iron(II) sulfate
28) Calcium chromate
29) Silver bromide
30) Cooper (I) chloride
31) Silver carbonate
32) Nitrogen trichloride
33) Aluminum chloride
34) Sodium Cyanide
35) Nickel (II)Phosphate
36) Chromium (III) Hydroxide
37) Zinc nitrate
38) Barium Acetate
39) Calcium sulfide
40) Sodium phosphate
14
MODULE 04: Naming & Writing Acids Worksheet
Name the following compounds:
Answer
1) HF
2) HClO3
3) H2CO3
4) HCl
5) H2S
6) HClO
7) H2SO4
8) H2SO3
9) H3PO4
10) HI
11) Hydrobromic acid
12) Nitric acid
13) Acetic acid
14) Phosphorous acid
15) Hydrocyanic acid
16) Carbonic acid
17) Phosphoric acid
18) Sulfurous acid
19) Hydrochloric acid
20) Sulfuric acid
15
16
MODULE 05: Chapter 1 in Textbook
Title of Chapter #1:
Introduction: Matter & Measurement
______
List of Subheadings: (Fill-in)
1.1
__________
1.2
______
______
1.3
________
1.4
_______
1.5
______________
1.6
_______
Check
Grade
Filled-in by
teacher
I. Survey the Chapter
A. Read the chapter's opening page text & "What's Ahead" entry.
B. Examine all figures and all tables.
C. Read "Summary & Key Terms" at the end of each chapter.



II. Study the Textbook Content
A. Read text & take notes as you read. (You should have a minimum of 2 pages
front and back & may take several hours to complete)
B. Review all sample exercises and practice exercises


III. End of Chapter Visualizing Concepts & Exercises


A. Title of segment #1: Visualizing Concepts
Problems submitted by the student: 1, 2, 5, 6, 7
B. Title of segment #2: Classification and Properties of Matter



Problems submitted by the student: 11, 17, 20






C. Title of segment #3: Units and Measurement
Problems submitted by the student: 23, 27, 31




D. Title of segment #4: Uncertainty in Measurement
Problems submitted by the student: 34, 36, 37, 39
E. Title of segment #5: Dimensional Analysis
Problems submitted by the student: 41, 44, 47, 49, 53
17
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18
MODULE 06: Chapter 2 in Textbook
Title of Chapter #2:
__________________________________________ ______
List of Subheadings: (Fill-in)
2.1
__________________
2.2
_____________
______
2.3
________
______
2.4
_______
______
2.5
______________
__
2.6
_______
_______
______
2.7
______________
______
2.8
_______
______
2.9
_______
______
Check
Grade
Filled-in by
teacher
I. Survey the Chapter
A. Read the chapter's opening page text & "What's Ahead" entry.
B. Examine all figures and all tables.
C. Read "Summary & Key Terms" at the end of each chapter.



II. Study the Textbook Content
A. Read text & take notes as you read. (You should have a minimum of 2 pages
front and back & may take several hours to complete)
B. Review all sample exercises and practice exercises


III. End of Chapter Visualizing Concepts & Exercises


A. Title of segment #1: Visualizing Concepts
Problems submitted by the student: 1, 3, 4, 5
B. Title of segment #2: Atomic Theory and the Discovery of Atomic Structure



Problems submitted by the student: 12, 13, 15


C. Title of segment #3: Modern View of Atomic Structure: Atomic Weights
Problems submitted by the student: 17, 26, 27, 29, 30, 35
D. Title of segment #4: The Periodic Table; Molecules and Ions
Problems submitted by the student: 41, 42, 43, 47, 50, 51, 53, 56, 60
E. Title of segment #5: Naming Inorganic Compounds; Organic Molecules
Problems submitted by the student: 64, 68, 72
19
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
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
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20
MODULE 07: Chapter 3 in Textbook
Title of Chapter #3:
__________________________________________ ______
List of Subheadings: (Fill-in)
3.1
_____________
3.2
_____________
______
3.3
________
______
3.4
_______
______
3.5
______________
__
3.6
_______
_______
______
3.7
______________
______
Check
Grade
Filled-in by
teacher
I. Survey the Chapter
A. Read the chapter's opening page text & "What's Ahead" entry.
B. Examine all figures and all tables.
C. Read "Summary & Key Terms" at the end of each chapter.



II. Study the Textbook Content
A. Read text & take notes as you read. (You should have a minimum of 2 pages
front and back & may take several hours to complete)
B. Review all sample exercises and practice exercises


III. End of Chapter Visualizing Concepts & Exercises


A. Title of segment #1: Visualizing Concepts
Problems submitted by the student: 1, 5, 7
B. Title of segment #2: Balancing Chemical Equations



Problems submitted by the student: 10, 12, 14


C. Title of segment #3: Patterns of Chemical Reactivity
Problems submitted by the student: 17, 20








D. Title of segment #4: Formula Weights
Problems submitted by the student: 21a-d, 25
E. Title of segment #5: Avogadro’s Number and the Mole
Problems submitted by the student: 28, 34, 36, 39, 42
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F. Title of segment #6: Empirical Formulas
Problems submitted by the student: 44, 48, 50
G. Title of segment #7: Calculations Based on Chemical Equations
Problems submitted by the student: 57, 59, 61, 64
H. Title of segment #8: Limiting Reactants; Theoretical Yields
Problems submitted by the student: 67, 68, 69, 71, 73, 77, 79, 80
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