1.3 STANDARDIZED TEST PREPARATION

Multiple Choice

Choose the best answer.

Question 1.13

1. The density of zinc is 7.1 g/cm3 and the density of copper is 9.0 g/cm3. What statement correctly describes the density of a zinc block coated with copper?

  1. The block has a density of 7.1 g/cm3.

  2. The block has a density less than 7.1 g/cm3.

  3. The block has a density between 7.1 g/cm3 and 9.0 g/cm3.

  4. The block has a density of 9.0 g/cm3.

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Question 1.14

2. According to an ancient story, Archimedes had his “crowning moment” when he discovered the trickery of a goldsmith by using density. The goldsmith had received an order for a pure gold crown but crafted one from a mixture of metals. The volume of this crafted crown would have differed from the volume of a pure gold crown. If the mass of a pure gold crown was 1.2 kg, and the density of gold is 19.3 g/cm3, what would be the volume of a pure gold crown?

  1. 0.062 cm3

  2. 62.2 cm3

  3. 23.16 cm3

  4. 16.08 cm3

Question 1.15

3. The shell model below has 3 protons, 3 neutrons, and 3 electrons. What statement correctly describes this atom?

image

  1. The atomic number of this element is 6 because there are 3 protons and 3 neutrons; and the mass number is 3 because there are 3 protons.

  2. The atomic number of this element is 3 because there are 3 protons, 3 neutrons, and 3 electrons; and the mass number is 9 because there are 3 of each subatomic particle.

  3. The atomic number of this element is 3 because there are 3 protons; and the mass number is 6 because there are 3 protons and 3 neutrons.

  4. The atomic number is 6 because there are 3 protons and 3 electrons; and the mass number is 6 because there are 3 protons and 3 electrons.

Question 1.16

4. A shell model for a carbon atom is shown. Which statement correctly describes the electrons in carbon?

image

  1. Carbon has 6 core electrons and no valence electrons because there are a total of 6 electrons in the neutral atom.

  2. Carbon has 12 electrons because the mass number is 12.

  3. Carbon has a core similar to the helium atom, but carbon has 4 valence electrons.

  4. Carbon has a core similar to the neon atom, but carbon has 4 valence electrons.

Question 1.17

5. The element in the shell model below is a poor conductor of heat and electricity and is very reactive. Which element would have similar properties to this one?

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  1. Na, sodium

  2. Br, bromine

  3. Ar, argon

  4. S, sulfur

Use the periodic table shown to answer Exercises 6 and 7.

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Question 1.18

6. Two groups of the periodic table are highlighted in the figure. What are the names given to these groups?

  1. Alkali metals and noble gases

  2. Alkali metals and halogens

  3. Alkaline earth metals and noble gases

  4. Alkaline earth metals and halogens

Question 1.19

7. What type of bonding would you expect to find in substances made when an element from one highlighted group is combined with an element from the other highlighted group?

  1. Ionic only

  2. Molecular covalent only

  3. Network covalent only

  4. Ionic and network covalent

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Question 1.20

8. If an alkaline earth metal formed a compound with a polyatomic phosphate ion, PO43–, what would be the subscript given to the metal in the chemical formula for the compound?

  1. 3

  2. 2

  3. 1

  4. There would be no subscript written in the chemical formula.

Question 1.21

9. What is present in the nucleus of an atom of image ?

  1. 88 neutrons and 138 protons

  2. 88 electrons and 226 protons

  3. 88 protons and 226 neutrons

  4. 88 protons and 138 neutrons

Question 1.22

10. Thallium’s atomic number is 81 and the average atomic mass is 204.4 amu. Thallium has two isotopes, thallium-203 and thallium-205. Which statement correctly describes thallium?

  1. A naturally occurring sample of thallium contains both isotopes.

  2. Thallium-203 isotope has 122 protons, and thallium-205 has 124 protons.

  3. The most common atom of thallium has a mass of 204.48 amu.

  4. Thallium-203 and thallium-205 both have 81 neutrons.

Question 1.23

11. An element has three naturally occurring isotopes. One of the isotopes of the element has a mass number of 24 and is 79% abundant in nature. Another of the isotopes has a mass number of 25 and is 10% abundant in nature. The last isotope of the element has a mass number of 26 and is 11% abundant in nature. Based on this information, what is the most likely identity of this element?

  1. Beryllium, Be

  2. Sodium, Na

  3. Magnesium, Mg

  4. Aluminum, Al

Use the graph below of the radioactive decay of carbon-14 to answer Exercises 12 and 13.

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Question 1.24

12. What is the approximate half-life of carbon-14?

  1. 50 years

  2. 5,730 years

  3. 11,460 years

  4. 17,190 years

Question 1.25

13. If the original sample of carbon-14 were 10.0 g, how much would remain after two half-lives?

  1. 234.0 g

  2. 1.25 g

  3. 5.00 g

  4. 2.50 g

Question 1.26

14. A sheet of aluminum would protect a person from what type of radiation exposure?

  1. A sheet of aluminum would protect from alpha, beta, and gamma radiation.

  2. A sheet of aluminum would protect from alpha and beta, but not gamma radiation.

  3. A sheet of aluminum would protect from alpha and gamma, but not beta radiation.

  4. A sheet of aluminum would not protect a person from any form of radiation.

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Use the diagram of the copper cycle below to answer Exercises 15–19.

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Question 1.27

15. Which of these statements correctly describes the law of conservation of mass?

  1. The law of conservation of mass would be supported if the amount of copper at the beginning and end of a copper-cycle experiment were accurately measured.

  2. The law of conservation of mass states that good laboratory techniques will help prevent the accidental loss of lab materials.

  3. The law of conservation of mass states that small amounts of mass are lost in the course of an experiment because of spills, measurement errors, and other factors.

  4. The law of conservation of mass does not apply to gases or aqueous solutions.

Question 1.28

16. Which of the following are solids produced in the copper cycle? (Choose all that apply.)

  1. Nitrogen dioxide

  2. Copper hydroxide

  3. Sulfuric acid

  4. Copper oxide

Question 1.29

17. What is true about the copper ions present in the copper cycle?

  1. Only copper (I) is present in the ionic compounds.

  2. Only copper (II) is present in the ionic compounds.

  3. Both copper (I) and copper (II) are present in the ionic compounds.

  4. Only elemental copper is present in the copper cycle.

Question 1.30

18. What is the charge of the copper atoms in the copper solid, Cu(s)?

  1. +2

  2. +1

  3. 0

  4. –1

Question 1.31

19. Which substances, as written below, would most likely conduct electricity? (Choose all that apply.)

  1. NO2(g)

  2. Cu(NO3)2(aq)

  3. NaOH(aq)

  4. Cu(OH)2(s)

Question 1.32

20. The acetate ion C2H3O2– has a charge of –1. What is the correct formula for calcium acetate?

  1. CaC2H3O2

  2. Ca2C2H3O2

  3. Ca(C2H3O2)2

  4. C2H3O2Ca

Question 1.33

21. Which of the following compounds will generally not form?

  1. KBr

  2. NeBr2

  3. AlBr3

  4. All of these compounds will form.

Question 1.34

22. Four models of chemical bonding are illustrated in the diagram. The red spheres represent the nuclei and core electrons of atoms and blue areas represent where valence electrons are located.

image

Which statement below correctly identifies the type of bonding for the compound listed?

  1. MgCl2(s) bonds according to Model 1 because valence electrons are shared between the atoms.

  2. CO2(g) bonds according to Model 1 because valence electrons are shared between the atoms.

  3. Li(s) atoms are bonded according to Model 4 because valence electrons are free to move about the substance.

  4. N2(g) bonds according to Model 4 because valence electrons are shared throughout the entire substance.