TEKS End-of-Course Assessment Chemistry Practice Test...

TEKS

STAAR Chemistry Practice Test B

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End-of-Course AssessmentChemistry Practice Test B

1 A student performs the following tests to determine the identity of a mineral sample.

1. The mineral is heated in chlorine gas to see if it will produce a different substance.

2. The mineral is immersed in an ammonia solution to see if any new color is produced.

3. The mineral is rubbed on a streak plate to determine the color of its powdered form.

4. Dilute hydrochloric acid is placed on the mineral to see if bubbles will form.

Which of the above tests were for physical properties of the mineral?

A Test 1

B Test 2

C Test 3

D Test 4

2 A sample of sulfur obtained from the crater of a volcano is carefully measured. Which of the following is an intensive property of the sample?

A Density of 2.07 g/cm3

B Mass of 3.85 g

C Volume of 1.86 cm3

D Temperature of 20°C

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3 The diagram below shows the arrangement of atoms in liquid mercury. Which of the following properties of liquid mercury atoms explains why liquid mercury takes the shape of and fills only the bottom of a more voluminous container, but neither solid nor gaseous mercury does?

Liquid mercury atoms —

A are practically incompressible

B are close together but free to move

C have a random arrangement

D slightly increase their average separation when heated

4 Students in a laboratory are asked whether a given sample of liquid matter is a pure substance or a mixture. They brainstorm the following suggestions for a test to answer the question.

1. Add NaOH(aq) to see if a precipitate will form.

2. Evaporate it to see if a residue will remain.

3. Test the substance with a pH meter and record the value.

4. Examine it under a microscope to see if it is uniform throughout.

5. Run the liquid through a filter paper.

Which of the above tests could yield useful information to answer the question?

A 2 only

B 2, 4, and 5

C 1, 2, and 5

D 1, 3, and 4

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5 The graph below shows a periodic trend.

2500

2000

1500

1000

500

0 10 20 30Atomic number

40 50 60

He

H Be

N

Ne

Li Na

Mg

PZn As Cd

K Rb Cs

KrXe

Ar

Which of the variables below is plotted on the vertical axis of the graph?

A Ionic radius

B Atomic radius

C Electronegativity

D First ionization energy

6 During the discovery of many new elements in the 1800s, it was found that when the elements were arranged in order of increasing atomic mass —

A the gases all seemed to be grouped together

B reactivity decreased as the atomic mass increased

C density increased as the atomic mass increased

D the properties repeated in a regular pattern

7 Halogens and noble gases are alike in that most members of both families —

A have relatively low boiling points

B form ions with a +1 oxidation state

C form ions with a –1 oxidation state

D are relatively unreactive

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8 A student is asked to identify a substance on the basis of its chemical properties. The table below lists some of the properties of the element bromine (Br).

1. state liquid

2. color reddish-brown

3. elemental state diatomic

4. reactivity moderately high

5. melting point (°C) –7

6. boiling point (°C) 59

Which of the properties of bromine is/are chemical properties?

A 1 and 3 only

B 2 and 4 only

C 4 only

D 4, 5, and 6 only

9 A forensic technician is examining a fine white powder found at a crime scene. It appears to be of uniform texture and consistency. He finds that upon heating, the substance decomposes, releasing a colorless gas and leaving a black residue. Based on these observations the substance is —

A a homogeneous mixture

B a heterogeneous mixture

C either a heterogeneous mixture or a compound

D a compound

10 Group 1A elements differ from Group 2A elements in that Group 1A elements —

A form a lower oxidation state

B are less reactive

C are harder and have higher densities

D are found in nature only in compounds

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11 Some of the third period elements are listed alphabetically in the table below.

1. aluminum

2. argon

3. chlorine

4. magnesium

5. sodium

Arrange the elements in order of increasing atomic radius. List the numbers of the elements from the table above, with the smallest element on the left and the largest on the right.

Record your answer and fill in the bubbles on your answer document.

12 The modern Periodic Table has elements with similar properties arranged in —

A rows

B periods

C groups

D sequential atomic numbers

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13 Several students make the following statements about red light.

1. Red light has a longer wavelength than infrared.

2. Red light has a shorter wavelength than infrared.

3. Red light has a lower frequency than ultraviolet.

4. Red light has a higher frequency than ultraviolet.

Based on the diagram below, which statements are correct?

Frequency � (s−1)

Wavelength � (m)

Radio waves Radar Microwaves Infrared Ultraviolet X-rays Gamma rays

Visible light

102 10–2 10–4 10–6 10–8 10–10 10–12 10–141

3 × 106 3 × 108 3 × 1010 3 × 1012 3 × 1018 3 × 1020 3 × 1022

Red light, low energy (7.0 × 10–7 m =

700 nm)

Violet light, high energy (3.8 × 10–7 m =

380 nm)

3 × 1014 3 × 1016

A 1 and 3 are correct

B 2 and 4 are correct

C 1 and 4 are correct

D 2 and 3 are correct

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14 Medical x-rays have wavelengths between 0.1 nm and 0.01 nm. Which of the following could be the frequency of a medical x-ray?

A 8 × 1018 Hz

B 8 GHz

C 8 × 10–19 Hz

D 8 Hz

15 Niels Bohr conducted many experiments in 1913 as he developed a new atomic model.

Possible Observations that Led to Bohr’s Nuclear Atom Model

1. He observed that atoms will not emit electrons until light of a specific energy shines on them.

2. He observed that alpha particles would be deflected different amounts by the electrons in specific energy levels.

3. He observed that atoms always absorb or emit light with specific energies.

4. He observed different regions or electron clouds around the nucleus that had increased probability of containing electrons.

Which of the observations above led Bohr to conclude that each electron orbit has a different energy?

A 1

B 2

C 3

D 4

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16 Copper has two naturally occurring isotopes. Use the information in the table to calculate the average atomic mass of copper, to the nearest hundredth of an atomic mass unit.

Isotope Relative Abundance Mass (amu)

Cu-63 69.15% 62.93

Cu-65 30.85% 64.93


17 The electron configuration of fluorine is 1s22s22p5. Which of the following shows the correct electron dot structure of fluorine?

A F

B F

C F

D F

18 Many of the unique properties of tin (Sn) are due to the electron arrangement within the atom. What is the ground state electron configuration of tin?

A [Kr] 5s24d105p2

B [Kr] 5s25d105p2

C [Kr] 5s25p2

D [Kr] 5s24d104f145p2

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19 What element is produced by beta decay in the following nuclear reaction?

3415 P → X + 0

–1 e

A 3314 Si

B 3416 P

C 3414 Si

D 3416 S

20 Thorium-234 is produced in an alpha decay reaction as shown in the following reaction.

X → 42 He + 234

90 Th

What radioactive element decays to produce Th-234?

A Pu-236

B Ra-230

C U-238

D Ta-240

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21 Thorium-232 can undergo a nuclear reaction as shown in the equation below.

23290 Th + 1

0 n → 23390 Th + energy

Without knowing what nuclear decay steps come next, a student predicts whether the process is a fission or fusion reaction.

Neutron

23592 U

23692 U

Which of the following student’s reasoning is correct?

1. The process is fission, because energy is released.

2. The process is fission, because a neutron is absorbed to start the process, which can cause the nuclei to become unstable.

3. The process is fusion, because the final nuclei is larger than either of the initial nuclei.

4. The process is fusion, because there are no neutrons released which is what starts fission chain reactions.

A 1

B 2

C 3

D 4

22 H3PO4 is a clear, colorless, odorless and slightly viscous liquid. It is an ingredient in several kinds of soda beverages because of its sour taste. What is the name of the compound with the chemical formula H3PO4?

A Trihydrogen phosphate

B Trihydrogen phosphorus tetroxide

C Phosphoric acid

D Trihydrogen phosphite

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23 N2O, commonly known as laughing gas, is used in some medical procedures for its anesthetic and analgesic effects. It is also used as an oxidizer to increase the power output of engines in car racing. What is the name of the compound with the chemical formula N2O?

A Nitrogen oxide

B Dinitrogen oxide

C Dinitrogen monoxide

D Nitrogen monoxide

24 Ammonium carbonate is used as a smelling salt, which can revive someone who has fainted. What is the chemical formula for ammonium carbonate?

A NH4(CO3)2

B NH4CO3

C (NH)2(CO3)4

D (NH4)2CO3

25 Nitrous acid is a weak acid that is found in the lower atmosphere and is one of the components of acid rain. What is the chemical formula for nitrous acid?

A HN

B HNO3

C HNO2

D HNO4

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26 Ammonium fluoride (NH4F) crystals taste salty with a structure very similar to ice. Which of the following is the correct electron dot formula for this compound?

A N H H H H F

B F

H

H

NH H

C F −N+

H

H

H H

D F N

H

H

H H

27 Methanol (CH3OH), which is highly toxic to humans, can be used in antifreeze, as a fuel, and solvent. Which of the following electron dot formulas correctly represents the structure of the molecule?

A (CH3)+(OH)−

B C

H

H

H O H

C C

H

H H O H

D

C H H H O H

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28 A student made the following list about the nature of metallic bonding.

Metallic Bonding Theory

1. Loosely-held valence electrons can drift freely throughout the metal.

2. Metal cations are arranged in a crystalline lattice.

3. Metallic bonds form from the attraction of the positive metal ions to the negative valence electrons.

The property of thermal conductivity is explained by which of the above statements?

A 1

B 2

C 3

D 1 and 2

29 Using VSEPR theory, what is the molecular structure of acetylene (C2H2)?

A Trigonal planar

B Bent

C Tetrahedral

D Linear

30 How many atoms are in 28.0 grams of copper?

A 1.37 × 1024 atoms

B 1.07 × 1023 atoms

C 2.65 × 1023 atoms

D 3.38 × 1020 atoms

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31 How many ions are present in 37.0 grams of calcium chloride (CaCl2)?

A 1.81 × 1024 ions

B 6.02 × 1023 ions

C 4.01 × 1023 ions

D 2.01 × 1023 ions

32 What is the percent composition of nitrogen in ammonia (NH3)?

A 82.22%

B 93.33%

C 14.00%

D 25.00%

33 When this chemical equation is balanced, what is the coefficient of oxygen (O2)?

C3H8(g) + O2(g) → H2O(g) + CO2(g)

A 2

B 4

C 5

D 10

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34 When calcium carbonate reacts with vinegar, bubbles of carbon dioxide form. What is the missing product in the balanced reaction below?

CaCO3 + 2CH3COOH → Ca(CH3COO)2 + CO2 +

A C2HO

B CaO

C CO

D H2O

35 Natural gas, used for heating homes and in the production of electricity, is a gas mixture that is composed primarily of methane. The equation below describes the combustion of methane.

CH4(g) + 2O2(g) → 2H2O(g) + CO2(g)

What mass of oxygen, to the nearest gram, is needed to combine with 96.0 grams of methane?


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36 Some scuba divers use a gas mixture called Nitrox I, to lessen the chance of getting decompression sickness. It contains 32% oxygen and 68% nitrogen. What is the partial pressure of nitrogen, to the nearest tenth of an atmosphere, in a sample of Nitrox I at the pressure and depth in seawater indicated in the diagram?

Pressure = 4.97 atm at 40 m


37 Air is about 80% nitrogen and 20% oxygen. A balloon has a volume of 2.0 L. How many grams of oxygen are in the balloon at standard temperature and pressure?

A 0.57 g

B 0.29 g

C 2.9 g

D 13 g

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38 Some students are invited to a barbecue. The food is cooked with propane burning in excess oxygen to produce heat, as shown in this equation.

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) + heat

If 210 g of propane gas are consumed, what volume of gaseous products is produced at standard temperature and pressure?

A 320 L

B 747 L

C 427 L

D 1.28 × 103 L

39 When sodium bicarbonate is added to a beaker of vinegar, a bubbling reaction occurs that raises the temperature of the beaker’s contents. In this reaction, what is being transformed into thermal energy?

A Some of the mass of the reactants

B Some of the chemical energy of the reactants

C Some of the kinetic energy of the reactants

D Some of the kinetic energy of the products

40 Two students are trying to understand the direction of heat flow and the extent of the system when food is cooked on a grill. They each have an explanation for the heat flow direction and system.

Student 1 When the food is the system, there is an endothermic process occurring.

Student 2 When the grill and the food are the system, there is an exothermic process occurring.

A Only statement 1 is true.

B Only statement 2 is true.

C Both statements 1 and 2 are true.

D Neither statement is true.

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41 Elemental iron (Fe) can be reclaimed from iron(III) oxide (Fe2O3) according to the following reaction:

Fe2O3(s) + 3CO(g) → 2 Fe(s) + 3CO2(g) + 26.3 kJ

When 4.50 moles of iron(III) oxide react, which of the following statements is correct?

1. 26.3 kJ are absorbed in an exothermic reaction

2. 26.3 kJ are released in an endothermic reaction

3. 118 kJ are released in an exothermic reaction

4. 118 kJ are absorbed in an endothermic reaction

A 1

B 2

C 3

D 4

42 Glucose is produced by green plants during photosynthesis. Organisms use glucose as a source of energy. When 36.0 g of glucose is metabolized according to the equation below, which choice correctly identifies the amount of energy released or absorbed?

C6H12O6 + 6O2 → 6CO2 + 6H2O ΔH = –2880 kJ

A 2880 kJ released

B 2880 kJ absorbed

C 576 kJ absorbed

D 576 kJ released

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43 A student finds that 4.7 kJ of heat are required to raise the temperature of 250.0 g of metal X from 22°C to 63°C. Based on the data in the table, what is the identity of metal X?

Metal Specific Heat (J/(g∙°C)

Aluminum 0.90

Iron 0.46

Mercury 0.14

Silver 0.24

A Aluminum

B Iron

C Mercury

D Silver

44 Which of the following reactions is an oxidation-reduction reaction?

A 2Ca(s) + O2(g) → 2CaO(s)

B Ba(NO3)2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaNO3(aq)

C HBrO3(aq) + KOH(aq) → KBrO3(aq) + H2O(l )

D NaBr(aq) + AgNO3(aq) → NaNO3(aq) + AgBr(s)

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45 Based on the table below, which of the following solutions should be added to (NH4)3PO4(aq) to produce a precipitate?

Salts of alkali metals and ammonia

Nitrate salts and chlorate salts

Sulfate salts

Chloride salts

Carbonates, phosphates, chromates, sulfides, and hydroxides

Solubility Rules for Ionic Compounds in Aqueous Solutions

Compounds Solubility Exceptions

Soluble

Soluble

Soluble

Soluble

Most are insoluble

Some lithium compounds

Few exceptions

Compounds of Pb, Ag, Hg, Ba, Sr, and Ca

Compounds of Ag and some compounds of Hg and Pb

Compounds of the alkali metals and of ammonia

A LiCl(aq)

B K2CrO4(aq)

C Ca(ClO3)2(aq)

D Na2SO4(aq)

46 What would be the molar concentration of sugar in a can of soda, if it contained 40.0 g of sucrose (C12H22O11) in 355 mL of solution? Express your answer to three decimal places.


47 A student in a laboratory prepares a solution of NaCl(aq) using tap water instead of distilled water as directed. She notices a faint cloudiness of the solution due to a precipitate. This precipitate in the solution may indicate a presence in the tap water of —

A sulfate ions

B hydroxide ions

C calcium or magnesium ions

D silver or lead(II) ions

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48 A student is asked to determine whether a given solution is unsaturated, saturated, or supersaturated. The student drops a tiny crystal of the solute into the solution and observes carefully for any change in the size of the crystal. Which of the following statements is true?

A No observable change means the solution is supersaturated.

B A decrease in crystal size means the solution is unsaturated.

C A decrease in crystal size means the solution is saturated.

D An increase in crystal size means the solution is unsaturated.

49 A solution is classified as an electrolyte if the solution contains —

A a dissolved solute

B molecular compounds

C positive and negative ions

D substances with strong forces between their particles

50 Based on the graph to the right, an increase in temperature has the greatest effect on the solubility of compounds containing —

A nitrate ions

B chloride ions

C sodium ions

D potassium ions

140

160

120

100

80

60

40

0

20

10 20 30 40 50 60 70 80 90Temperature (ºC)

KNO3

NH4Cl

NaCl

NaNO3

Solu

bilit

y (g

/100

g H

2O)

KBr

Yb2(SO4)3

Solubility Varies With Temperature

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51 Which of the following procedures would increase the rate of dissolution of a gas in a liquid?

1. increase the temperature

2. increase the pressure

3. shake or stir the mixture

4. increase the surface area

A 2 and 3 only

B 1 and 2 only

C 1, 2, and 3

D 2, 3, and 4

52 In an acid-base reaction, which of the following are transferred?

A Protons and electrons

B Electrons and neutrons

C Protons only

D Electrons only

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STAAR Chemistry Practice Test B Answer Sheet

Answer Sheet

Name Date Class

24.25.26.27.28.29.30.31.32.33.34.35.

36.

37.38.39.40.41.42.43.44.45.

A B C D

A B C D

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1.2.3.4.5.6.7.8.9.

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17.18.19.20.21.22.23.

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STAAR Chemistry Practice Test B Answer Sheet

Answer Sheet

Name Date Class

47.48.49.50.51.52.

A B C D

A B C D

A B C D

A B C D

A B C D

A B C D

46. A B C D

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TEKS End-of-Course Assessment Chemistry Practice Test...

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