Lab 6 Molecular Geometry
1. Describe the difference between valence and core electrons.
Valence electrons are in the outermost shell and core electron are in the innermost shell.
2. What is the octet rule and which elements obe
Lab 3 Data Analysis & Graphing
1. In your own words, describe how to calculate density.
You divide the mass by the volume to get the density.
2. Explain why the metric system is used in science.
It is more widely used and becau
Lab 1 Introduction and Laboratory Safety
1. What would you do if you spilled a tiny amount of hydrochloric acid on your hand?
Rinse with water for 20 minutes.
2. Describe a possible danger than can occur if you put food, soda, coffee, pencil eras
Lab 2 The Scientific Method
1. Which of the following are testable using scientific experimentation.
a. Are there more seeds in a medium sized Red Delicious Apple or a medium size Green
Granny Smith Apple? Testable.
b. Why do p
Lab 4 Molar Mass
1. Imagine you are a guest speaker at a kindergarten class and you are asked to explain Avogadros
number. What would you say and why?
There a many, many tiny puzzle pieces that make up everything you see. Avoga
Lab 7 Precipitation Reactions
1. Under what conditions will a precipitate form?
When ionic compounds are placed in water, separate into negative and positive charges, and combine
into new ions(s) that are insoluble.
2. What inf
Lab 5 Electron Configuration
1. What is electron configuration?
Electron configuration is a way of describing where the electrons in an atom are located.
2. How is the light emitted by an atom related to its electron configurati
Answers Percent Composition and Empirical Formula
1.a)1moleKClO3 = (39.1 g K) + (35.4 g Cl) + (3 x 16.0 = 48.0 g O) = 122.5 g
% K = 39.1/122.5 = 31.9% K;
% Cl = 35.4/122.5 = 28.9 % Cl;
% O = 48.0/122.5 = 39.2% O
Molar Mass Problems
1. Calculate the mass of 1.000 mole of CaCl2
2. Calculate grams in 3.0000 moles of CO2
3. Calculate number of moles in 32.0 g of CH4
4. Determine mass in grams of 40.0 moles of Na2CO3
5. Calculate moles in 168.0 g of HgS
6. Calculate m
Answers to More Chapter 22 Study Questions
1. a) CH3CHCHCH2CH2CH3
lots of other isomers possible
2. 5-ethyl-3,5,7-trimethyl nonane
Answers to More Chapter 4 Study Questions
1. a) FeCl3(aq) + 3 NaOH(aq) Fe(OH)3(s) + 3 NaCl(aq).
b) 30.0 mL x
c) 30.0 mL x
0.500 moles NaOH
1000 mL solution
1 mol FeCl 3 1000 mL solution
3 mol NaOH
0.200 mol FeCl 3
Electrochemical Cells Worksheet
1. Calculate the standard cell potential produced by a galvanic cell consisting of a nickel electrode in contact with
a solution of Ni2+ ions and a silver electrode in contact with a solution of Ag + ions. Which is anode an
Activation Energy & Catalyst
1. Summarize 3 points of the collision reaction theory.
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V W5 /E6 sz/fl it, Cgr/T Oflzo/neiag/m ,
Use the following to answer the next questions
2. a) Is
T. J I "\N\
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\ , ELEQL 7A ICAL\EL5 , ,MJLLQA we H* 3
f R NOT" pres? _
' . / . _
, > 1. FOrmcfonowingq'estions design @ ectmchemicgl cell. 1: the diagram _
_ /<- properly. Write the/ f arm a V . -
Directions: Study the food label and answer the questions.
1. What is the serving size of this product?
2. How many calories per serving size are in this
3. What percent of daily value is the sodium?
4. In 2 servings, how much
1. A cylinder of argon gas contains 50.0 L of Ar at 18.4 atm and 127 C. How many
moles of argon are in the cylinder?
2. A 283.3-g sample of X2(g) has a volume of 30 L at 3.2 atm and 27 C. What is
3. An ideal gas sample is c
Alkane alkene al ne and C clic com ounds'
1. Alkanes, alkenes, and alkynes are the three main families of aliphatic hydrocarbons.
a) met is the gkgeral mwormula for each family?
b) . at type of carbkl-carbon bonds are iured in each fa
1. Write IUPAC names for the following compounds.
lg ' D c a a
2. Draw a condensed structural formula for each compound.
a) 3-methylbutan-l-ol b) methylpropan-Z-ol c) cyclopentanol
c? 0 H
. CH - ~ CH
C H73 a c (4 CHa ~CHa
Balancing Redox Reactions
Part A: Balance the following equations using Oxidation Numbers. Underline the oxidizing agent and circle the
24 H2S + 16 HNO3
3 S8 + 16 NO +
H2SO4 + 2 HBr SO2 + 2 Br2 + H2O
H2SO4 + 8 HI
Acid / Base Theories Worksheet
1. Dene an Arrhenius acid and a base.
lOrt'Ze/g 4'7 - [onus "6'0.
H+ /'/'cfw_30+W-)' I OH 2) ,
2. What is the Arrhenius Modied denition of an acid and a base? _
3 w95cfw_W9 2993044) what (aou, *4. x
Find each element in the puzzle, then write the leftover letters in order,
top to bottom and left to right, to complete the hidden message.
P A B
S C A N D
L H N
U M S M S
R O G E N U T H
A B O T
T A A S
U M Z
D C H R
CHEIMIS T R Y 30
HEA T LOSS = HEA T GAIN
1. Methanol IS one type of fuel that 13 used 1n fondue heaters. In an experiment using a simple
calorimeter, 2. 98 g of methanol was burned tthe temperature of 0.650 kg of water by 20. 9C.
Calculate the ar enthal
CHEMIS TR Y 30
1. What physical property of hydrocarbons is used for fractionation?
2. -Whv does. crude oil have to be chemically processed, in addition to being fractionated? - I
lo Mortgage #41 y 799 os cfw_4w 4raL(fmg *fKLa-G m (\YL
CHE TRY 30
REVIEW OF ACIDS AND BASES
1. Given the following reactions, write the balanced equation using Bronsted4Lowry
acid\base reactions: 9 cfw_I l ,
(a H ~09,
. C 02*
a) aqueous solutions of nitrOus acid reacts with cacfum carbonate
HHCxnai) * (O'S