Final Review

Chemistry 09

Lab Safety and Equipment

1. When diluting sulfuric acida. add the sulfuric acid to plenty of waterb. add plenty of water to the sulfuric acid

2. If you do not understand a direction or part of a lab procedure, you should

a. figure it out as you do the labb. try several methods until something worksc. ask the instructor before proceedingd. skip it and go on to the next part

3. After completing an experiment, all chemical wastes should be

a. left at your lab station for the next classb. disposed of according to your instructor’s directionsc. dumped in the sinkd. taken home

4. If an acid is splashed on your skin, wash at once witha. soapb. oilc. concentrated based. plenty of water

5. Sarah accidently broke a glass beaker while conducting a lab. The first safety procedure for Sarah to do is to –

a. sweep up the broken glass immediately and put it in the trash

b. inform her teacher immediately so that her teacher can sweep up the glass

c. leave it for the next class to clean upd. none of the above

6.________

7. ________

8. ________

9.________

a. The object may cause a burn.

b. There is a potential of punctures or cuts.

c. Use the chemical under a fume hood.

d. The chemical is corrosive.

b

c

a

d

10. ________

11. ________

12. ________

a. graduated cylinder- used to measure accurate liquid volumes

b. flask- glassware used to contain reaction solutions

c. beaker- multi-purpose glassware that is used to hold and heat substances

b

c

a

13. Define a meniscus and how you use it when reading a graduated cylinder.

14. What is the reading on the graduated cylinder below? _________ mL 43

Meniscus- the curve (dip) of a liquid substance in a graduated cylinder; read the graduated cylinder from the bottom of the meniscus

15. A triple beam balance is used to measure _______________. What is the reading on the triple beam balance below? _________ g

mass

545.2

16. The phrase used to remember metric conversion prefixes is “King Henry __________________________________________________________________.

17. A student has 0.45 L of a liquid. What is the volume in mL? 0.45 L = ________ mL450

“King Henry Died by Drinking Chocolate Milk”

Scientific Method & Graphs

1. The scientific method is a process that scientist use to _______________________________________.

2. Organize the 6 steps of the scientific method in the correct order 1-6.

________ Conclusion________ State the problem________ Experiment________ Gather information________ Analyze the data________ Formulate a testable hypothesis

1

6

2

5

3

4

Solve a problem

3. Tommy conducted an experiment and concluded that a species of mosquitoes (sp. S. ouch) will grow larger when exposed to microwaves for long periods of time. What could Tommy do to make his conclusion more valid?

A. Try a different species of mosquitoesB. Repeat the same experiment multiple times with the same

species of mosquitoesC. Use a large number of the mosquitoes (sp S. ouch)D. Both b and c

4. A hypothesis is _____________________________________. The format for writing a TESTABLE hypothesis is: If IV……… then DV (Ex. If I eat 20 pieces of chocolate then I will have a stomach ache)

an educated guess

5. In an activity, a ball is dropped from a height of 100 cm onto five different materials. The rebound height of each drop is shown in the graph. Which of the following describes the hypothesis most likely being tested?

A. The mass of the ball affects the rebound height.B. The material the ball is made of affects the rebound height.C. The height the ball is dropped from affects the rebound

height.D. The surface the ball is dropped onto affects the rebound

height.

6. A control is the standard to which test results can be compared

7. The independent variable is the variable that is manipulated or changed (MIX)

8. The dependent variable is the variable that responds to the changes in the independent variable (DRY)

9. An experiment was designed to investigate the effect of caffeine on the heartbeat of water fleas. Two populations of water fleas was cultured. Both populations had water with the same mineral content, were supplied with identical amounts of bacteria food, received the same amount of light, and had their temperature maintained at 20oC. Every two hours, water fleas from both populations were selected and their heartbeats were monitored. The fleas of population one had caffeine administered five minutes before their heartbeat was checked. The fleas of population two were given nothing.

I. What part of the experiment above is population two?

a. Independent variableb. Dependent variablec. Control

II. What part of the experiment above was the caffeine?

a. Independent variableb. Dependent variablec. Control

10. The ________________________ variable is graphed on the x- axis. The ___________________ variable is graphed on the y- axis.

11. You are measuring the how the temperature in your room changes over a period of time. What type of graph would you use to graph this data?

A. Line graph B. Bar graph C. Pie Chart

12. A researcher determined the percentage of electrical energy transformed into different forms of energy by a toaster. The best way to communicate these results is to display the data using a –

A. Line graph B. Bar graph C. Pie (Circle) graph

Independent

Dependent

13. The line graph below shows the month and the number of bathing suites sold each month. What variable does the number of bathing suits sold represent in the research?

A. independent variableB. dependent variableC. control

D. constant

Precision and Accuracy

Which of the following sets of measurements is most precise?A. 18.56, 20.56, 22.56B. 18, 20, 22C. 17.5, 20.5, 21.5D. 18, 19, 20

Which of the following will allow measurement of a liquid’s volume with the greatest precision.

A. 50 mL cylinder graduated in 1 mL incrementsB. 100 mL cylinder graduated in 0.5 mL incrementsC. 100 mL cylinder graduated in 1 mL incrementsD. 100 mL cylinder graduted in 5 mL increments

Density

1. Write the formula for density:

2. Complete the triangle below for the density formula.

3. Write the unit(s) of measure for density, volume, and mass.

Density units of measure: ____________ & ______________

Mass unit of measure: _______________

Volume units of measure: _____________ & ______________

x

m

vd

g/mL g/cm3

g

mL cm3

Density = mass/volume

4. Calculate the density of a metal cube that has a mass of 30 g and a volume of 16 cm3.

5. If you have a graduated cylinder that was filled to 25 ml and you dropped a rock into it and water in the cylinder raises to 29 ml. What is the volume of the rock? If this same rock has a mass of 44g what would the density of this rock be?

6. What is the density of water? ___________ g/mL

7. If an object has a density of 1.3 g/cm3, it will _________ in water.A. sink B. float

8. If an object has a density of 0.7 g/mL it will ________ in water.A. sink B. float

1

D= m/v D = 30g/16cm3 D=1.88 g/cm3

V= (29ml – 25mL= 4mL D= m/v D = 44g/4mL D= 11 g/mLVF

VI

Use the figure below to answer questions 9 and 10.

9. Which liquid in the beaker above is the most dense? _______________

10. Which liquid in the beaker above is the least dense? _______________

Volume 4

Volume 1

11. The volume of object “X” in the figure on the right is:

a. 20 mL b. 25 mL c. 30 mL d. 35 mL

Viscosity

1. Viscosity is a fluid’s ________________ to flow.

2. A fluid is any substance that flows. A fluid can be a liquid or a _______________.

3. Which substance below is the most viscous?

A. water B. honey

4. Which substance below is the least viscous?

A. water B. honey

resistance

gas

5. Students in a chemistry lab measure the time it takes four different 100 mL solutions to pass through a hole in the bottom of the cup. Which of the following properties of the solutions is most likely being measured?

A. buoyancy B. mass C. viscosity D. volume

6. When compared to a high viscosity liquid, a liquid with a low viscosity:A. must have a lower volumeB. is easier to pourC. takes longer to pour from one container to anotherD. must have a higher density

Buoyancy

1. Buoyancy is the __________ force exerted on an object by a fluid that it is immersed in.

A. downward B. upward

2. List two examples that illustrate buoyancy (example: ship on the sea) ________________________________

______________________________________________

_________________________________

Kinetic Theory and States of Matter

1. When a substance is heated, the molecules or atoms that make up the substance move _____.A. faster B. slower

2. List the 4 states of matter and 2 characteristics of each.

____________________- definite shape, definite volume

____________________- no definite shape, definite volume

____________________- no definite shape, no definite volume

____________________- no definite shape, no definite volume, charged particles, matter consisting of high-temperature gas

solid

gas

liquid

plasma

3. List the phase of water in order, from the phase with the slowest molecular movement to the phase with the fastest molecular movement.

A. gas liquid solid

B. liquid solid gas

C. solid liquid gas

D. gas solid liquid

4. Matter that has a definite volume and a definite shape is a _______.

A. gas B. liquid C. plasma D. solid

5. Fill in the heating curve for water using the following terms: freezing point, melting point, condense, and boiling point

Freezing point

Condense

Boiling point

Melting pointSOLID

LIQUID

GAS

Incr

easin

g Tem

perat

ureDecreasin

g Temperatu

re

6. Use the graph above to determine the freezing point of water ______ OC and the boiling point of water ______ OC.

0 100

SOLID

LIQUID

GAS

Classification of Matter

1. Pure substance – have a definite composition (Ex. Elements or compounds)

2. Element – simplest pure substance which CAN NOT be broken down through physical or chemical means

3. Compound- is a pure substance composed of 2 or more elements that are chemically combined in definite proportions (Ex. H2O, CO2)

4. Mixture – composed of 2 or more different substances that can be separated through physical means

5. Homogeneous mixture – a mixture that is the SAME throughout6. Heterogeneous mixture – a mixture that is NOT THE SAME

throughout7. Chemical reaction – when 2 or more substances react to form a new

substance8. Chemical change – A change of one substance to a new substance that

differ in appearance and chemical make-up (Ex. Rusting, digestion, burning)

9. Physical change – a change in the appearance or state of a substance but NOT its chemical make-up

10. Classify each of the following as a physical or chemical property:

___ hardness___ color___ reactivity___ melting point___ chalk breaks easily___ salt water conducts electricity___ flammability___ plastic does not rust___ density

PP

PP

PP

PP

PP

CP

CP

CP

CP

11. Classify each of the following as a physical or chemical change:

___ digestion___ two clear liquids are mixed and the mixture turns blue___ a tree is cut down___ water evaporates into steam___ burning a log

PC

CC

CC

CC

PC

12. Classify each as either a homogeneous mixture (HM), or heterogeneous mixture (HT):

____ marble____ air____ mixed vegetables____ hot chocolate with marshmallows

HM

HT

HT

HT

13. The figure below shows an experimental setup used to separate the components of a colored ink sample. Which of the following describes this laboratory technique?A. filtrationB. distillationC. chromatography

Periodic Table

1. Who attempted to classify the elements by organizing them into a seven column table by atomic mass?

A. Dalton B. Mendeleev C. Bohr

2. The metals are located on the __________ side of the zig-zag line.

3. The nonmetals are located on the __________ side of the zig-zag line.

4. Boron, silicon, germanium, arsenic, antimony, tellurium, polonium, and astatine are located along the zig-zag line and are called _________________.

left

right

metalloids

5. Label the periodic table box below with the following terms: atomic number, atomic mass, symbol, name, number of protons, number of electrons

15

Si

28.086

Silicon

symbol

Atomic mass

Atomic number, Number of protons,

number of electrons

Name

6. Periods on the periodic table are arranged in ________.A. horizontal rowsB. vertical columns

7. Groups on the periodic table are arranged in _________.A. horizontal rowsB. vertical columns

8. Periods are equal to ___________.A. valence electrons- electrons on outer energy levelB. energy levels- electron rings

9. Group numbers are equal to __________.A. valence electrons- electrons on outer energy levelB. energy levels- electron rings

10. Complete the table below. (halogens, noble gases, alkali metals, nitrogen group, carbon group, alkaline earth metals, oxygen group, boron group)

Group Group “Family” Name Valence Electrons

Oxidation Number

1A Alkali Metals 1 +12A Alkaline Earth Metals 2 +23A Boron Group 3 +34A Carbon Group 4 +4 or -45A Nitrogen Group 5 -36A Oxygen Group 6 -27A Halogens 7 -18A Noble Gases 8 0

11. The “group B” elements are called the ________.A. noble gasesB. halogensC. transition metals

12. Phosophorus (P) has ______ protons inside of the nucleus.

13. Aluminum (Al) has ______ electrons outside of the nucleus.

14. The symbol for lead is ________.

15. The most reactive metals are the _________.A. halogensB. noble gasesC. alkali metals

16. The most reactive nonmetals are the ______.A. alkaline earth metalsB. halogensC. alkali metals

15

13

Pb

17. The __________ are the most stable elements and undergo the fewest chemical reactions.

A. alkali metals B. halogens C. noble gases

18. Ca and Mg are located in the same _________ and they have the same number of ___________ electrons. Ca and Mg have similar ________________ and physical properties for this reason.

19. ________________ and ____________ are elements that have similar chemical properties to bromine (Br) and iodine (I)

20. What do lithium (Li), beryllium (Be) and carbon (C) all have in common?A. valance electrons B. atomic massC. atomic number D. energy levels

21. Name the element that has 2 valence electrons and 2 energy levels: ______________________

22. Name the element that has 7 valence electrons and 4 energy levels: _______________________

groupvalence

Chemical

Fluorine (F) Chlorine (Cl)

Beryllium- Be

Bromine- Br

Atomic Structure

1. Identify the parts of the atom by using the figure on the right. (proton, electron, neutron, nucleus, neutral, negative, positive)

A. ___________ - has a ___________ charge.

B. ___________ - the center of an atom; gives an atom its mass

C. ___________ - has a ____________ charge.

D. ___________ - has a ____________ charge

Neutron

Nucleus

Proton

Electron

neutral

positive

negative

2. How do you determine the number of neutrons? _________________________________

3. A certain atom has 26 protons, 26 electrons, and 30 neutrons. Its mass number is _____.

A. 26 B. 30 C. 56 D. 82

4. The diagram on the right represents _______ which is currently the accepted model of an atom.

A. a Bohr model B. an electron cloud model C. electron dot diagram

Neutrons = atomic mass – atomic number

5. What is the rule for the Bohr model of an atom? _____ : _____ : _____

Bohr Model

6. The atoms in Group A are different from the atoms in Group B because only the atoms in Group A have —

A their outer energy levels filled with electrons

B three energy levels of electrons

C electron arrangements typical of metals

D electron arrangements typical of nonmetals

82 8

7. The dots around an electron dot diagram represent the __________ electrons which is the same as the group number.

8. Complete the table below.

Element Bohr Model Electron Dot Diagram

Lithium Li

Sodium Na

Valence

9. The ___________ is the subatomic particle that is responsible for the chemical behavior of an element.

A. proton B. neutron C. electron

10. Observe the table above to determine the metal used during a fireworks display if a bright green spectrum was observed?

A. Copper B. Strontium chloride C. Lithium D. Copper chloride

Substance Element ColorCopper chloride Bright green

Lithium chloride Carmine red

Sodium chloride Yellow orange

Strontium chloride Scarlet red

11. An atom that has lost or gained electrons is called a(n) _______ and can have a positive or negative charge.A. particle B. isotope C. ion D. neutron

12. A _________ atom equals ZERO and has an equal number of protons and electrons.

A. negatively charged B. positively charged C. neutral

13. If an atom donates electrons it will have a _________ charge.A. positive B. neutral C. negative

14. If an atom accepts electrons it will have a _________ charge.A. positive B. neutral C. negative

15. All of these atoms donate electrons and form positive ions EXCEPT

Writing Chemical Formula

1. What type of bond is pictured on the right between two chlorine atoms?A. covalent B. metallic C. ionic

2. A __________ bond is formed between two _____________. The electrons are ____________.

3. What type of bond is pictured on the right between sodium and chlorine?A. covalent B. metallic C. ionic

covalent nonmetalsshared

4. A(n) _________ bond is formed between a ________ and a ___________ and the electrons are ______________.

5. What type of bond will be formed between the elements below? For a covalent bond write “CB” and for an ionic bond write “IB”

________ H and F ________ N and Cl

________ Ca and Br ________ K and I

________ H and S ________ Rb and Cl

ionic metal nonmetal

transferred

CB

IB IB

CB

CB IB

6. Write the chemical formula and name for the following binary ionic compounds.

Element Chemical Formula

Compound Name

Li and S Li2S Lithium Sulfide

Mg and P Mg3P2 Magnesium Phosphide

Na and Cl NaCl Sodium Chloride

Conservation of Mass and Reactions

1. Law of Conservation of Mass- ___________________________________________________________

2. Exothermic Reaction –____________________________________________________________

3. Endothermic Reaction –___________________________________________________________

4. Exergonic Reaction -_______________________________________________________________

5. Endergonic Reaction- _______________________________________________________

6. The reaction of CaO and water is exothermic. A student mixes the two chemicals in a test tube and touches the side of the test tube. Which statement describes the student’s observation?

A. The test tube becomes hot as heat is released. B. The test tube becomes hot as heat is absorbed

7. The reaction that takes place inside of a glow stick is best described as being a ________ reactionA. endergonic B. endothermic C. exergonic

8. The law of conservation of mass requires a chemical equation to have the ________ number of atoms on each __________. To balance a chemical equation, you must add _____________ in front of the chemical formulas in the equation. You can not ________ or ____________________ subscripts.

same sidecoefficients

add change/take away

Count up the number of atoms that are found for each element on each side of the equation. State whether the equation is balanced or not for questions 9 and 10.

9. Ca(OH)2 + 2HNO3 Ca(NO3)2 + 2H2O

Ca= Ca=O= O= Balanced or Not BalancedH= H=N= N=

10. Zn + 2HCl ZnCl2 + H2

Zn= Zn=H= H= Balanced or Not BalancedCl= Cl=

2

842

184

2

2

1

1 122

Determine the mass of the unknown substances below for questions 11 and 12.

11. What is the mass of reactant “X” in the equation below? _______ g

& + X &X 50g + __?__ g 80 g

12. What is the mass of product “*$” in the equation below? _______ g

@$ + *^ @^ + *$40g + 30g 60g + __?_ g

30

10

13. Use the figure below to determine the type of reaction taking place in each letter. (synthesis, decomposition, single replacement, double replacement)

F: Single-displacement

G: Decomposition

H: Synthesis

I: Double-displacement

14. Balance the chemical equations below.

_____P + _____O2 _____P2O5

_____Na2O + _____CO2 ______Na2CO3

15. Indications of a double displacement reaction are water, gas, and a(n) ____________.

A. acid B. base C. precipitate

16. Count the atoms

Ca(O2H4)2 Ca = O = H =

2NaCl2 Na = Cl =

4 25

1 11

1 4 8

2 4

17. 2Fe2O3 4Fe + 3O2

1. Coefficient2.”Yield”3. Subscript4. Reactants5. Products

18. What is the function of the coefficient in a chemical equation?

19. What is the purpose of the subscript in the chemical equation?

Coefficient- tells the number of units of a substance in a chemical equation

Subscript- tells the number of atoms in a chemical formula

Solubility

1. Solute: ____________________________________________________________

2. Solvent: ____________________________________________________________

3. Solubility: ___________________________________________________________

4. Electrolyte: ____________________________________________________________

5. Nonelectrolyte: ___________________________________________________________

6. Unsaturated: ___________________________________________________________

7. Saturated: ____________________________________________________________

8. Supersaturated: ____________________________________________________________

9. Polar Molecule: ____________________________________________________________

10. Nonpolar Molecule: _________________________________________________________________

11. To dissolve a polar solute, the solvent must be _________.A. polar B. nonpolar C. neutral

12. To dissolve a nonpolar solute, the solvent must be __________.A. polar B. nonpolar C. neutral

13. List 3 ways in which the rate of dissolving can be increased.

14. How do you increase the solubility of a gas into a liquid? (Ex. soda)

Stirring, increased temperature, increased surface area

Cold temperature, & high pressure

15. According to the graph below, if you had 80g of KBr dissolved in 100g water at 70 degrees C, what kind of saturation would it be?

A. saturated B. unsaturated C. supersaturated

16. According to the graph on the right, the solubility of ________ is least affected by an increase in temperature.

A. KNO3 B. KBr C. NaCl

17. Water is ____________ because it has a partially positive region and a partially negative region.

18. _________________ is the universal solvent because of the polar nature of its molecules.

19. A solution that has ions in it can produce electricity and be classified as a(n) __

A. nonelectrolyte B. electrolyte C. compound

polar

water

Acids and Bases

1. Acid: ____________________________________________________________

2. Base: ____________________________________________________________

3. Hydroxide ion: ____________________________________________________________

4. Hydronium ion: ____________________________________________________________

5. Neutralization: _________________________________________________

6. Ionization: __________________________________________________

7. The pH scale ranges from ________ to ________.

8. Classify the substances as acid (A), base (B) or neutral (N) based on the pH.

Substance pH Acid, Base, Neutral

A 2

B 7

C 9

0 14

Acid (0-6)

Neutral

Base (8-14)

9. What type of ions do acids form when dissolved in water?

_______________

10. What type of ions do bases form when dissolved in water?

_______________

11. List 3 properties of acids: ______________________________________________________ Corrosive, sour, electrolyte

Hydroxide Ions (OH-)

Hydrogen Ions (H+)

12. List 3 properties of bases:

______________________________________________________________

13. What are the products of a neutralization reaction (acid + base)? _

_______________________________

14. Which solution below is a base that is also an electrolyte? A. solution 1 B. solution 2 C. solution 3 D. solution

4

Corrosive, bitter, electrolyte

Water and a Salt

15. A solution that has more H+ ions than OH- ions is ________.A. acidic B. neutral C. basic