CHM-113 PQ1 Ch1 Ch2 KEY - Practice test key PDF

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CHM-113 PRACTICE QUIZ 1 KEY CHAPTER 1 AND 2 1.

When nature behaves in a certain way over and over again, under all sorts of different conditions, we can summarize that behavior (typically a relationship), it is called a(n) _____. a) observation b) hypothesis c) theory d) law e) experiment

2.

A(n) _______ is formed after an observation and attempts to provide a testable explanation of an observed behavior of some natural phenomenon. a) observation b) hypothesis c) theory d) law e) scientific method

3.

A(n) _____ is a model that is based on a set of tested hypotheses and gives an overall explanation of some natural phenomenon. a) observation b) hypothesis c) theory d) law e) measurement

4.

Which of the following statements are incorrect? a) The state of matter for an object that has a definite volume but not a definite shape is a liquid state b) The state of matter for an object that has both definite volume and definite shape is solid state c) The state of matter for an object that has a definite shape and is highly compressible is gaseous state d) The state of matter for an object that has no definite volume and takes the shape of its container is gaseous state e) The state of matter for an object that is rigid is solid state

5.

An example of a pure substance is ____. a) an element b) a compound c) H 2O d) carbon dioxide e) all of these

6.

An example of an element is ____. a) chicken noodle soup b) powerade c) air inside a balloon d) lead pipe e) baking soda (NaHCO3)

7.

An example of a compound is _____. a) chicken noodle soup b) powerade c) air inside a balloon d) lead pipe e) baking soda (NaHCO3)

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8.

An example of a homogeneous mixture is _____. a) chicken noodle soup b) powerade c) the helium inside a balloon d) lead pipe e) baking soda (NaHCO3)

9.

An example of a heterogeneous mixture is _____. a) chicken noodle soup b) powerade c) air inside a balloon d) lead pipe e) baking soda (NaHCO3)

10.

Select the incorrectly matched pair for unit and dimension. a) Time – seconds b) Amount of substance – grams c) Mass – kilograms d) Length – meters e) Volume – cubic centimeters

11.

Which of the following metric relationships is incorrect? a) 1 microliter = 10 –6 liters b) 1 gram = 10 3 kilograms c) 103 milliliters = 1 liter d) 1 gram = 10 2 centigrams e) 10 decimeters = 1 meter

12.

2.0 ng is equal to a) 2.0 x 10-7 g b) 2 x 103 g c) 2.0 x 10 -9 g d) 2.0 x 10 9 g e) 2.0 x 107 g

13.

Select the correct answer below given the following numbers. 4250600 0.0560030 Significant Figures Scientific Notation Significant Figures Scientific Notation a) 5 4.2506 x 10 6 5 5.6003 x 10 -2 b) 4 4.251 x 10 6 8 5.60030 x 10-2 c) 5 4.2506 x 10 6 6 5.60030 x 10 -2 4 d) 5 4.2506 x 10 3 5.63 x 10 -2 e) 6 4.25060 x 10 6 7 5.6003 x 10-2

14.

Perform the indicated mathematical operation and round the answer to the correct number of significant figures. 4201.5 – 0.08 + 181/0.544 = a) b) c) d) e)

4530 4534.14 4534 4534.1 4500

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Questions 15-18 can be answered using one of the choices (a-e) below. a) measured number b) exact number c) accuracy 15. 16. 17. 18. 15 – D 16 – C 17 – B 18 – A 19.

d) precision

e) none of the above

How close a measured number is to other measured numbers is _____. How close a measured number is to the true value is _____. A dozen doughnuts is an example of _____. A BMI of 21 is an example of _____.

424 Kelvin equals a) b) c) d) e)

151 °F 273 °F 697 °F 151 °C 697 °C

20.

65.2°F is equal to _____ °C. a) 36.2 b) 4.20 c) 33.2 d) 18.4 e) 60.0

21.

Calculate the volume of silver metal that weighs exactly 2.50 kg. The density of silver is 10.5 g/cm 3. a) 0.238 mL b) 238 mL c) 26.3 mL d) 4.20 mL e) 0.00420 mL

22.

Calculate the density (in g/mL) of an object that has a mass of 12.2 g and occupies a volume of 0.50 m 3. a) 2.4 x 10 -5 g/mL b) 24 g/mL c) 0.24 g/mL d) 4.1 x 10 -2 g/mL e) 4.1 g/mL

23.

Calculate the mass of an object that has a volume of 100.0 L and a density of 1.00 g/mL. a) 100. g b) 1.00 x 10 5 g c) 1.00 x 10 3 g d) 1.00 x 10 -2 g e) 1.00 g

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24.

Which of the following statements about the atomic structure of an atom is false? I. An atom is mostly empty space. II. Almost all of the mass of the atom is concentrated in the nucleus. III. The protons and neutrons in the nucleus are very tightly packed. IV. The number of protons and neutrons is always the same for all neutral atoms of that element. V. Ions are formed by adding or removing either protons or electrons. a) b) c) d) e)

I, II, and III only IV and V only V only I and V only All statements are true, no statements are false.

25.

Which one of the following is not one of the postulates of Dalton's atomic theory? a) Atoms are composed of protons, neutrons, and electrons. b) All atoms of a given element are identical; the atoms of different elements are different and have different properties. c) Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions. d) Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. e) Each element is composed of extremely small particles called atoms.

26.

Which of the following pairs of compounds can be used to illustrate the law of multiple proportions? a) NH4 and NH4Cl b) ZnO2 and ZnCl2 c) H2O and HCl d) NO and NO2 e) CH4 and CO2

27.

The _____ states that the total mass of materials present after a chemical reaction is the same as the total mass present before the reaction. a) Dalton’s atomic theory b) law of conservation of mass c) law of multiple proportions d) law of constant composition e) none of the above

28.

The _____ states that the relative number of atoms of each element in the compound is the same in any sample. a) Dalton’s atomic theory b) law of conservation of mass c) law of multiple proportions d) law of constant composition e) none of the above

29.

The _____ states that if two elements A and B combine to form more than one compound, the masses of B that can combine with a given mass of A are in the ratio of small whole numbers. a) Dalton’s atomic theory b) law of conservation of mass c) law of multiple proportions d) law of constant composition e) none of the above

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30.

Select the incorrect statement below. a) Cations are positively charged ions. b) Anions are negatively charged ions. c) Atoms that gain an electron are called anions. d) Atoms that gain a neutron are called cations. e) All statements are correct.

31.

Select the correct statement below. a) Ionic compounds form between a metal cation and a anionic non-metal. b) Covalent compounds form between two metals. c) Isotopes of an element have different numbers of electrons. d) Ions of an element have different numbers of neutrons. e) Two different elements can have the same number of protons.

Question 32 and 33 refer to the figure below. 32.

The substance in BOX A could represent a sample of _____. a. b) c) d) e)

33.

34.

A

B

C

D

Select the incorrectly paired identification of each box above. a) Box A contains 12 atoms and 4 molecules of 1 compound. b) Box B contains 19 atoms from two different elements. c) Box C contains 7 molecules and only one type of compound. d) Box D contains a diatomic molecule and a total of 14 atoms of the same element. e) Box E contains 4 molecules of one compound and a total of 19 atoms. There are ________ electrons, ________ protons, and ________ neutrons in an isotope of sulfide ion-33. a) b) c) d) e)

35.

C and H atoms H 2O NH3 CH4 H2

17, 16, 17 18, 16, 16 16, 17, 18 18, 16, 17 16, 16, 16

What is the correct nuclear symbol for a neutral atom of sodium with a mass number of 20 and 10 electrons? 22 a) Na+ 11 b) Na+ 20 c) Na 22 d) Na 20 Na+ e)

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E

36.

Which of the following contain the same number of electrons? I. Cla) b) c) d) e)

II. Cl

III. S

IV. S2-

V. F-

I and II only I and V only II and III only I, IV, and V I and IV only

37.

Argon has three naturally occurring isotopes: argon-36, argon-38, and argon-40. Based on argon’s atomic weight on the periodic table, which isotope is the most abundant in nature? a) Ar-40 b) Ar-38 c) Ar-36 d) All isotopes are equally abundant in nature e) Not enough information is provided.

38.

The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. a) 219.7 Isotope Abundance Mass b) 220.4 221 X 74.22 220.9 c) 220.9 220 X 12.78 220.0 d) 218.5 218 X 13.00 218.1 e) 221.0

39.

Select the incorrectly paired items. a) Li and Na are alkali metals b) Ca and Ba are alkaline earth metals c) Cl and Br are halogens d) F and Ne are in the same period e) S and P are in the same group

40.

How many carbonite ions are in one formula unit of Al2(CO3)3? a) 0 b) 1 c) 2

41.

42.

d)

3

e)

The correct name of Al2(CO3)3 is _____. a) aluminum(III) carbonite b) aluminum(III) carbonate c) aluminum carbide d) aluminum carbonite e) aluminum carbonate The anion in Al2(CO3)3 has a charge of _____. a) +3 b) -3 c) -2 d) -1 e) it is neutral (no charge)

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9

43.

The correct name for LiCl is a) lithium monochloride b) lithium(I) chloride c) monolithium chloride d) lithium chloride e) monolithium monochloride

44.

The correct name for CuN is _____. a) copper(III) nitrate b) copper(I) nitrate c) copper(III) nitride d) copper(I) nitride e) copper mononitride

45.

The correct formula for tetraphosphorous hexasulfide is _____. a) P4S6 b) PS c) P3S6 d) P4S7 e) PS6

46.

The correct formula for carbonic acid is _____. a) H 4C b) HCO3 c) H2CO3 d) H2CO4 e) H3CO3

47.

The correct formula for hydroiodic acid is _____. a) HIO4 b) HIO3 c) HIO2 d) HIO e) HI

48.

All of the following are in aqueous solution. Which is incorrectly named? a) HC2H3O2, acetic acid b) HBr, bromic acid c) H2SO3, sulfurous acid d) HNO2, nitrous acid e) HClO3, chloric acid

49.

Which of the following pairs is incorrect? a) NH4Br, ammonium bromide b) K2CO3, potassium carbonate c) BaPO4, barium phosphate d) CuCl, copper(I) chloride e) MnO2, manganese(IV) oxide

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