Honors Chemistry Midterm Review

Osmium has a density of 22.6 g/cm~3. What volume (in cm~3) would be occupied by a 21.8 g sample of osmium? a. 0.965 b. 2.03 * 10~-3 c. 493 d. 2.03 * 10~3 e. 1.04

a. 0.965

One million argon atoms is ____________ mol (rounded to two significant figures) of argon atoms. a. 1.7 * 10~-18 b. 1.0 * 10~-6 c. 6.0 * 10~23 d. 1.0 + 10~+6 e. 3.0

a. 1.7 * 10~-18

Which of the following has the same number of significant figures as the number 1.00310? a. 199.791 b. 100 c. 1 * 10~6 d. 5.119 e. 8.66

a. 199.791

Of the fallowing, _________ is the largest mass. a. 25 kg b. 2.5 * 10~9 fg c. 2.5 * 10~-2 mg d. 2.5 * 10~10 ng e. 2.5 * 10~15 pg

a. 25 kg

Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al2X3. Element X must be from Group ____________ of the Periodic Table of Elements. a. 6A b. 4A c. 7A d. 3A e. 5A

a. 6A

Which one of the following substances is the product of this combination reaction? Al (s) + I2(s) ----> _____________ a. AlI3 b. AlI2 c. Al2I3 d. AlI e. Al3I2

a. AlI3

______________ have the lowest first ionization energies of the groups listed. a. Alkali metals b. Noble gases c. Halogens d. Alkaline earth metals e. Transition elements

a. Alkali metals

Of the choices below, which fives the order for first ionization energies? a. Ar > Cl > S > Si > Al b. Cl > S > Al > Ar > Si c. Cl > S > Al > Si > Ar d. S > Si > Cl > Al > Ar e. Al > Si > S > Cl > Ar

a. Ar > Cl > S > Si > Al

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. Atoms of an element are not changed into different types of atoms by chemical reactions; atoms are neither created nor destroyed in chemical reactions. c. Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. d. Each element is composed of extremely small particles called atoms. e. All atoms of a given element are identical; the atoms of different elements are different and have different properties.

a. Atoms are composed of protons, neutrons, and electrons

Of the following species, __________ has the largest radius. a. Br- b. Sr2+ c. Kr d. Rb+ e. Ar

a. Br-

What is the molecular formula for 1-propanol? a. C3H8O b. C5H12O c. C4H10O d. CH4O e. C26O

a. C3H8O

Which one of the following has the element name and symbol correctly matched? a. Fe, iron b. N, neon c. B, bromine d. S, sodium e. Tn, tin

a. Fe, iron

You have to calculate the mass of a 30.0 mL liquid sample with density of 1.52 g/mL, but you have forgotten the formula. Which way of reasoning would help you in finding the correct mass? a. If 1 mL of a liquid has the mass of 1.52 g, then 30.0 mL has the mass of ____________ g. b. If 1.52 mL of a liquid has the mass of 1 g, then 30.0 mL has the mass of ____________ g.

a. If 1 mL of a liquid has the mass of 1.52 g, then 30.0 mL has the mass of ____________ g.

Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr? a. K > Ca > Ge > As > Kr b. Ca > K > As > Ge > Kr c. Ge > As > Kr > K > Ca d. Kr > Ge > As > K > Ca e. Kr > As > Ge > Ca > K

a. K > Ca > Ge > As > Kr

Of the compounds below, __________ has the smallest ionic separation a. KF b. RbCl c. RbF d. SrBr2 e. K2S

a. KF

Of the choices below, which gives the order for first ionization energies? a. Kr > Br > Se > Ge > Ga b. Ga > Br > Ge > Kr > Se c. Ga > Ge > Se > Br > Kr d. Br > Se > GA > Kr > Ge e. Kr Se > Br > Ga > Ge

a. Kr > Br > Se > Ge > Ga

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si, and Ar? a. Na > Mg > Si > P > Ar b. Ar > P > Si > Mg > Na c. Ar > Si > P > Na > Mg d. Mg > Na > P > Si > Ar e. Si > P > Ar > Na > Mg

a. Na > Mg > Si > P > Ar

Of the following, _____________ radiation has the shortest wavelength. a. X-ray b. infrared c. microwave d. radio e. ultraviolet

a. X-ray

Of the objects below, ___________ is the most dense. a. an object with a volume of 3.91 10~-24 nm~3 and a mass of 7.93 * 10~-1 ng b. an object with a volume of 13 dm~3 and a mass of 1.29 * 10~3 g c. an object with a volume of 2.5 L and a mass of 12.5 kg d. an object with a volume of 0.00212 m~3 and a mass of 4.22 * 10~4 mg e. an object with a volume of 139 mL and a mass of 93 g

a. an object with a volume of 3.91 10~-24 nm~3 and a mass of 7.93 * 10~-1 ng

An element cannot _________. a. be separated into other substances by chemical means b. interact with other elements to form compounds c. be part of a heterogeneous mixture d. be a pure substance e. be part of a homogeneous mixture

a. be separated into other substances by chemical means

Which one of the following basic forces is so small that it has no chemical significance? a. gravity b. Coulomb's law c. weak nuclear force d. electromagnetism e. strong nuclear force

a. gravity

Consider the following selected postulates of Dalton's atomic theory: i. Each element is composed of extremely small particles called atoms. ii. Atoms are indivisible iii. Atoms of a given element are identical. iv. Atoms of different elements are different and have different properties Which of the postulates is (are) no longer considered valid? a. ii and iii b. ii only c. iii and iv d. i and ii e. iii only

a. ii and iii

The effective nuclear charge of an atom is primarily affected by ______________. a. inner electrons b. outer electrons c. nuclear charge d. orbital radial probability e. electron distribution

a. inner electrons

What is the physical state in which matter has no specific shape but does have a specific volume? a. liquid b. gas c. salts d. solid e. ice

a. liquid

Which one of the following is not an intensive property? a. mass b. melting point c. boiling point d. density e. temperature

a. mass

Gravitational forces act between objects in proportion to their ____________. a. masses b. volumes c. charges d. polarizability e. densities

a. masses

Formulas that show how atoms are attached in a molecule are called a. structural formulas b. molecular formulas c. diatomic formulas d. ionic formlas e. empirical formulas

a. structural formulas

In the Rutherford nuclear-atom model, ____________. a. the heavy subatomic particles, protons and neutrons, reside in the nucleus b. the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass. c. mass is spread essentially uniformly throughout the atom d. the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass and mass is spread essentially uniformly throughout the atom e. the light subatomic particles, protons and neutrons, reside in the nucleus

a. the heavy subatomic particles, protons and neutrons, reside in the nucleus

A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of ____________. a. the law of constant composition b. the law of conservation of energy c. the law of multiple proportions d. the law of conservation of mass e. none of the above

a. the law of constant composition

The formula weight of a substance is __________. a. the sum of the atomic weights of each atom in its chemical formula b. the weight of a sample of the substance c. determined by combustion analysis d. identical to the molar mass e. the same as the percent by mass weight

a. the sum of the atomic weights of each atom in its chemical formula

When a hydrocarbon burns in air, a component produced is ___________. a. water b. argon c. oxygen d. carbon e. nitrogen

a. water

How many sulfur dioxide molecules are there in 0.180 mol of sulfur dioxide? a. 1.08 * 10~24 b. 1.08 * 10~23 c. 1.80 * 10~23 d. 6.02 * 10~23 e. 6.02 * 10~24

b. 1.08 * 10~23

How many atoms of nitrogen are in 10 g of NH4NO3? a. 2 b. 1.5 * 10~23 c. 3.0 * 10~23 d. 3.5 e. 1.8

b. 1.5 * 10~23

One angstrom, is 10~-10 m. 1 cm~3 = ____________ Angstrom~3 a. 10~-9 b. 10~24 c. 10~-30 d. 10~30 e. 10~-24

b. 10~24

If an object is accelerating at a rate of 25 m/s~2, how fast will it be moving (in m/s) after 1.50 min? (assume an initial velocity of zero). a. 3.6 b. 2.3 * 10~3 c. 17 d. 38 e. 0.060

b. 2.3 * 10~3

How many significant figures should be retained in the result of the following calculations? 12.000000 * 0.9893 + 13.00335 * 0.0107 a. 2 b. 3 c. 4 d. 5 e. 6

b. 3

How many oxygen atoms are contained in 2.74 g of Al2(SO4)3? a. 12 b. 5.79 * 10~22 c. 6.02 * 10~23 d. 7.22 * 10~24 e. 8.01 * 10~-3

b. 5.79 * 10~22

You have to calculate the volume of a gas sample with mas of 1.000 * 10~3 g and density of 1.027 g/L, but you have forgotten the formula. Which way of reasoning would help you in finding the correct mass? a. If 1.027 L of gas has a mass of 1 g, then __________ L has the mass of 1.000 * 10~3 g. b. If 1.027 g of a gas takes up a volume of 1L, then 1.000 * 10~3 g of te same gas takes up a volume of _____________.

b. If 1.027 g of a gas takes up a volume of 1L, then 1.000 * 10~3 g of te same gas takes up a volume of _____________.

One mole of __________ contains the smallest number of atoms. a. Al2(SO4)3 b. NaCl c. C10H8 d. S8 e. Na3PO4

b. NaCl

Which of the following correctly represents the electron affinity of phosphorus? a. P4 (g) + e- ----> P- (g) b. P (g) + e- ----> P- (g) c. P4 (g) + 4e- ----> 4P- (g) d. P (g) ----> P+ (g) + e- e. P+ (g) + e- ----> P (g)

b. P (g) + e- ----> P- (g)

Which one of the following is not true concerning cathode rays? a. They are made up of electrons b. The characteristics of cathode rays depend on the material from which they are emitted. c. They originate from the negative electrode. d. They impart a negative charge to metals exposed to them. e. They travel in straight lines in the absence of electric or magnetic fields.

b. The characteristics of cathode rays depend on the material from which they are emitted.

Which one of the following is considered to be ionizing radiation? a. infrared radiation b. X-rays c. visible light d. microwaves e. radio waves

b. X-rays

Which of the following elements has a symbol that is not derived from its foreign name? a. mercury b. aluminum c. copper d. tin e. lead

b. aluminum

The molecular formula of a compound is always ____________ the empirical formula. a. more complex than b. an integral multiple of c. the same as d. different form e. simpler than

b. an integral multiple of

___________-rays consist of fast-moving electrons. a. alpha b. beta c. X d. gamma e. none of the above

b. beta

Sodium is much more apt to exist as a cation than is chlorine. This is because _________. a. chlorine is bigger than sodium b. chlorine has a greater ionization energy than sodium does c. chlorine is more metallic than sodium d. chlorine has a greater electron affinity than sodium does e. chlorine is a gas and sodium is a solid

b. chlorine has a greater ionization energy than sodium does

If matter is uniform throughout and cannot be separated into other substances by physical means, it is ____________. a. a homogeneous mixture b. either an element or a compound c. a heterogeneous mixture d. a compound e. an element

b. either an element or a compound

A small amount of salt dissolved in water is an example of ____ . a. pure substance b. homogeneous mixture c. heterogeneous mixtuer d. solid e. compound

b. homogeneous mixture

Precision refers to ____________. a. how close a measured number is to the calculated value b. how close a measured number is to other measured numbers c. how close a measured number is to infinity d. how close a measured number is to the true value e. how close a measured number is to zero

b. how close a measured number is to other measured numbers

A molecular formula always indicates __________. a. the isotope of each element in a compound b. how many of each atom are in a molecule c. the geometry of a molecule d. the simplest whole-number ratio of different atoms in a compound e. which atoms are attached to which in a molecule

b. how many of each atom are in a molecule

Screening of the nuclear charge by core electrons in atoms is _________________. a. essentially identical to that by valence electrons b. more efficient than that by valence electrons c. less efficient than that by valence electrons d. responsible for a general decrease in atomic radius going down a group e. both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group

b. more efficient than that by valence electrons

Electrons in the 1s subshell are much closer to the nucleus in the Ar than in He due to the larger _______________ in Ar. a. diamagnetism b. nuclear charge c. paramagnetism d. azimuthal quantum number e. Hund's rule

b. nuclear charge

All atoms of a given element have the same ___________. a. number of electrons and neutrons b. number of protons c. number of neutrons d. mass e. density

b. number of protons

Expressing a number in scientific notation ___________. a. changes its value b. removes ambiguity as to the significant figures c. allows to increase the number's precision d. removes all significant zeros e. all of the above

b. removes ambiguity as to the significant figures

Homogeneous mixtures are also known as ________. a. substances b. solutions c. compounds d. solids e. elements

b. solutions

Which one of the following is an intensive property? a. amount b. temperature c. heat content d. mass e. volume

b. temperature

In the following list, only _________ is not an example of a chemical reaction. a. burning candle b. the condensation of water vapor c. the rusting of iron d. dissolution of a penny in nitric acid e. the formation of polyethylene from ethylene

b. the condensation of water vapor

Which one of the following is not true concerning automotive air bags? a. they are inflated as a result of a decomposition reaction b. the gas used for inflating them is oxygen c. a gas is produced when the air bag activates d. the two products of the decomposition reaction are sodium and nitrogen e. they are loaded with sodium azide initially

b. the gas used for inflating them is oxygen

The atomic radius of main-group elements generally increases down a group because _________________. a. effective nuclear charge increases down a group b. the principal quantum number of the valence orbitals increases c. effective nuclear charge decreases down a group e. both effective nuclear charge increase down a group and the principal quantum number of the valence orbitals increases

b. the principal quantum number of the valence orbitals increases

An empirical formula always indicates __________. a. how many of each atom are in a molecule b. the simplest whole-number ratio of different atoms in a compound c. the geometry of a molecule d. which atoms are attached to which in a molecule e. the isotope of each element in a compound

b. the simplest whole-number ratio of different atoms in a compound

Atomic radius generally decreases as we move ___________. a. down a group and from left to right across a period b. up a group and from left to right across a period c. down a group; the period position has no effect d. down a group and from right to left across a period e. up a group and from right to left across a period

b. up a group and from left to right across a period

Which one of the following is correct? a. v = cY b. vY = c c. Y = cv d. v + Y = c e. v / Y = c

b. vY = c

Of the three types of radioactivity characterized by Rutherford, which is/are not electrically charged? a. a-rays and y-rays b. y-rays c. a-rays and b-rays d. a-rays e. a-rays, b-rays, and y-rays

b. y-rays

A 30.5 gram sample of glucose (C6H12O6) contains ___________ mol of glucose a. 5.90 b. 0.424 c. 0.169 d. 2.36 e. 0.136

c. 0.169

Vanadium has two naturally occurring isotopes, 50V with an atomic mass of 49.9472 amu and 51V with an atomic mass of 50.9440. The atomic weight of vanadium is 50.9415. The percent abundances of the vanadium isotopes are __________% 50V and ____________ 51V. a. 1.0, 99 b. 49, 51 c. 0.25, 99.75 d. 99, 1.0 e. 99.75, 0.25

c. 0.25, 99.75

If an object is accelerating at a rate of 25 m/s~2, how long (in seconds) will it take to reach a speed of 550 m/s? (assume an initial velocity of zero). a. 0.045 b. 2.3 * 10~2 c. 22 d. 1.2 * 10~4 e. 1.4 * 10~4

c. 22

The number with the most significant zeros is ____________. a. 2.501 * 10~-7 b. 0.00002510 c. 250000001 d. 2.5100000 e. 0.02500001

c. 250000001

Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? a. 2s b. 2p c. 2d d. all of the above e. none of the above

c. 2d

Round the number 3456.5 to two significant figures a. 3400 b. 3400.0 c. 3500 d. 3000.0 e. 3000

c. 3500

Which one of the following is the highest temperature? a. 96 F b. 302 K c. 38 C d. none of the above e. the freezing point of water

c. 38 C

A sample of CH2F2 with a mass of 19 g contains __________ atoms of F. a. 3.3 * 10~24 b. 38 c. 4.4 * 10~23 d. 9.5 e. 2.2 * 10~23

c. 4.4 * 10~23

Acceleration due to gravity of a free-falling object is 9.8 m/s~2. Express this is millimeters/millisecond~2 a. 9.8 * 10~-6 b. 9.8 * 10~6 c. 9.8 * 10~-3 d. 9.8 * 10~-9 e. 9.8 * 10~3

c. 9.8 * 10~-3

Which of the following correctly represents the electron affinity of bromine? a. Br (g) ----> Br+ (g) + e- b. Br2 (g) + e- -----> Br- (g) c. Br (g) + e- -----> Br- (g) d. Br2 (g) + 2e- ----> 2Br- (g) e. Br+ (g) + e- ----> Br (g)

c. Br (g) + e- -----> Br- (g)

Which ion below has the largest radius? a. F- b. Cl- c. Br- d. Na+ e. K+

c. Br-

Which pair of substances could be used to illustrate the law of multiple proportions? a. H2O, O2 b. NaCl, KCl c. CO, CO2 d. SO2, H2SO4 e. CH4, C6H12O6

c. CO, CO2

Which of the following is true about the liter? a. It is the SI base unit for volume. b. It is slightly smaller than a gallon c. It is equivalent to a cubic decimeter. d. It contains 10~6 cubic centimeters e. It is slightly smaller than a quart

c. It is equivalent to a cubic decimeter

Which calculation clearly shows a conversion between temperatures in degrees Celsius, C, and temperature in Kelvins, K? a. K = [C + 32] * 1.8 b. K = C c. K = C + 273.15 d. K = 273.15 - C e. K = [C - 32] / 1.8

c. K = C + 273.15

The charge on an electron was determined in the ____________. a. Dalton atomic theory b. Rutherford gold foil experiment c. Millikan oil drop experiment d. cathode ray tube, by K.J. Thomson e. atomic theory of matter.

c. Millikan oil drop experiment

Which species below is the nitride ion? a. NO3- b. NO2- c. N3- d. NH4+ e. Na+

c. N3-

Which of the following is an illustration of the law of constant composition? a. Water and salt have different boiling points b. Water boil at 100 degrees C at 1 atm pressure c. Water is 11% hydrogen and 89% oxygen by mass d. Water is a compound. e. Water can be separated into other substances by a chemical process.

c. Water is 11% hydrogen and 89% oxygen by mass

Of the three types of radioactivity characterized by Rutherford, which are particles? a. a-rays, b-rays, and y-rays b. b-rays c. a-rays and b-rays d. y-rays e. a-rays and y-rays

c. a-rays and b-rays

For which of the following can the composition vary? a. homogeneous mixture b. pure substance c. both homogeneous and heterogeneous mixtures d. element e. heterogeneous mixture

c. both homogeneous and heterogeneous mixtures

In the following list, only ________ is not an example of a chemical reaction a. charging a cellular phone b. the tarnishing of a copper penny c. chopping a log into sawdust d. burning a plastic water bottle e. the production of hydrogen gas from water

c. chopping a log into sawdust

Of the following, the smallest and lightest subatomic particle is the ____________. a. neutron b. nucleus c. electron d. proton e. alpha particle

c. electron

In the Bohr model of the atom, ___________. a. electron paths are controlled by probability b. electrons travel in circular paths called orbitals c. electron energies are quantized d. electrons can have any energy e. both A and C

c. electron energies are quantized

Which states of matter are significantly compressible? a. solids and liquids b. solids only c. gases only d. liquids only e. liquids and gases

c. gases only

A combination of sand, salt, and water is an example of a ____ . a. compound b. solid c. heterogeneous mixture d. pure substance e. homogeneous mixture

c. heterogeneous mixture

Accuracy refers to ____________. a. how close a measured number is to other measured numbers b. how close a measured number is to zero c. how close a measured number is to the true value d. how close a measured number is to infinity e. how close a measured number is to the calculated value

c. how close a measured number is to the true value

The reaction used to inflate automobile airbags ____________. a. is a combustion reaction b. produces sodium gas c. is a decomposition reaction d. is a combination reaction e. violates he law of conservation of mass

c. is a decomposition reaction

In the periodic table, the elements are arranged in ____________. a. alphabetical order b. reverse alphabetical order c. order of increasing atomic number d. order of increasing metallic properties e. order of increasing neutron content

c. order of increasing atomic number

Of the following, only _________ is a chemical reaction. a. crushing of stone b. dissolving sugar in water c. tarnishing of silver d. dropping a penny into a glass of water e. melting of lead

c. tarnishing of silver

The law of constant composition says _______. a. that the composition of a homogeneous mixture is always the same b. that the composition of an element is always the same. c. that the composition of a compound is always the same d. that all substances have the same composition e. that the composition of a heterogeneous mixture is always the same

c. that the composition o a compound is always the same

In the absence of magnetic or electric fields, cathode rays ____________. a. become positively charged b. bend toward a light source c. travel in straight lines d. cannot be detected e. do not exist

c. travel in straight lines

Silver has two naturally occurring isotopes with the following isotopic masses: Ag 107 with mass of 106.90509 and Ag 107 with mass of 108.9047 The average atomic mass of silver is 107.8682 amu. The fractional abundance of the lighter of the two isotopes is ____________. a. 0.90474 b. 0.48168 c. 0.24221 d. 0.51835 e. 0.75783

d. 0.51835

How many sulfur dioxide molecules are there in 1.80 mol of sulfur dioxide? a. 6.02 * 10~24 b. 1.08 * 10~23 c. 6.02 * 10~23 d. 1.08 * 10~24 e. 1.80 * 10~24

d. 1.08 * 10~24

In which one of the following numbers are all of the zeros significant? a. 0.1000 b. 00.0030020 c. 0.143290 d. 100.090090 e. 0.05843

d. 100.090090

Which of the following is (are) the lowest temperature? a. The freezing point of water b. 5 C c. 280 K d. 30 F e. A and D

d. 30 F

A wooden object has a mass of 10.782 g and occupies a volume of 13.72 mL. What is the density of the object determined to an appropriate number of significant figures? a. 8 * 10~-1 g/mL b. 7.9 * 10~-1 g/mL c. 7.86 * 10~-1 g/mL d. 7.859 * 10~-1 g/mL e. 7.8586 * 10~-1 g/mL

d. 7.859 * 10~-1 g/mL

All of the orbitals in a given subshell have the same value as the _______________ quantum number. a. angular momentum b. principal c. magnetic d. A and B e. B and C

d. A and B

The formula for a salt is XBr. The X-ion in this salt has 46 electrons. The metal X is ____________. a. Cs b. Cd c. Pd d. Ag e. Cu

d. Ag

The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotope of ___________. a. oxygen b. hydrogen c. helium d. carbon e. sodium

d. carbon

The law of constant composition applies to ____ . a. homogeneous mixtures b. solutions c. heterogeneous mixtures d. compounds e. solids

d. compounds

Atomic radius generally increases as we move ______________. a. down a group and from left to right across a period b. up a group and from right to left across a period c. down a group; the period position has no effect d. down a group and from right to left across a period e. up a group and from left to right across a period

d. down a group and from right to left across a period

Elements ___________ exhibit similar physical and chemical properties. a. with similar atomic masses b. on opposite sides of the periodic table c. with similar chemical symbols d. in the same group of the periodic table e. in the same period of the periodic table

d. in the same group of the periodic table

Gases and liquids share the property of _________. a. incompressibility b. definite volume c. definite shape d. indefinite shape e. compressibility

d. indefinite shape

According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the _________ of an electron. a. shape b. color c. charge d. momentum e. mass

d. momentum

Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the lowest - energy photon. a. n = 6 -----> n = 1 b. n = 3 -----> n = 6 c. n = 1 -----> n = 6 d. n = 6 -----> n = 3 e. n = 1 -----> n = 4

d. n = 6 -----> n = 3

The de Broglie wavelength of a ____________ will have the shortest wavelength when traveling at 30 cm/s. a. hydrogen atom b. uranium atom c. car d. planet e. marble

d. planet

Which type of formula provides the most information about a compound? a. molecular b. simplest c. empirical d. structural e. chemical

d. structural

Cathode rays are deflected away from a negatively charged plate because ____________. a. they are neutral particles b. they are emitted by all matter c. they are positively charged particles d. they are negatively charged particles e. they are not particles

d. they are negatively charged particles

Of the three types of radioactivity characterized by Rutherford, which type does not become deflected by a magnetic field? a. a-rays and b-rays b. b-rays c. a-rays d. y-rays e. a-rays, b-rays, and y-rays

d. y-rays

Round the number 0.007222 to three significant figures. a. 0.007 b. 0.007225 c. 0.00723 d. 0.0072 e. 0.00722

e. 0.00722

Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gas 4. compression of oxygen gas a. 1, 3, 4 b. 1, 4 c. 2, 3, 4 d. 1, 2 e. 1, 3

e. 1, 3

The total number of atoms in 0.111 mol of Fe(CO)3(PH3)2 is ___________. a. 4.46 * 10~21 b. 1.67 c. 2.76 * 10~-24 d. 15.0 e. 1.00 * 10~24

e. 1.00 * 10~24

Iron has a density of 7.9 g/cm~3. What is the mass of a cube of iron with the length of one side equal to 55.0 mm? a. 4.3 * 10~2 g b. 2.1 * 10~4 g c. 1.4 g d. 2.3 * 10~-2 g e. 1.3 * 10~3 g

e. 1.3 * 10~3 g

How many molecules of CH4 re in 48.2 g of this compound? a. 5.00 * 10~24 b. 2.90 * 10~25 c. 3.00 d. 4.00 e. 1.81 * 10~24

e. 1.81 * 10~24

Gaseous argon has a density of 1.40 g/L at standard conditions. How many argon atoms are in 1.00 L of argon gas at standard conditions? a. 3.43 * 10~25 b. 1.59 * 10~25 c. 4.76 * 10~22 d. 6.02 * 10~23 e. 2.11 * 10~22

e. 2.11 * 10~22

Which one of the following is not a valid value for the magnetic quantum number of an electron in a 5d subshell? a. 1 b. -1 c. 2 d. 0 e. 3

e. 3

A sample f CH4) with a mass of 32.0 g contains ____________ molecules of CH40. a. 1.88 * 10~22 b. 5.32 * 10~-23 c. 32.0 d. 1.00 e. 6.02 * 10~23

e. 6.02 * 10~23

One mole of ___________ contains the largest number of atoms. a. Cl2 b. Na3PO4 c. Al2(SO4)3 d. S8 e. C10H8

e. C10H8

Which equation correctly represents the electron affinity of calcium? a. Ca (g) ----> Ca- (g) + e- b. Ca+ (g) + e- -----> Ca (g) c. Ca- (g) -----> Ca (g) + e- d. Ca (g) ----> Ca+ (g) + e- e. Ca (g) + e- ----> Ca- (g)

e. Ca (g) + e- ----> Ca- (g)

Barium reacts with a polyatomic ion to form a compound with the general formula Ba3(X)2. What would be the most likely formula for the compound formed between sodium and the polyatomic ion X? a. Na2X2 b. Na2X c. Na3X2 d. NaX e. Na3X

e. Na3X

Of the three types of radioactivity characterized by Rutherford, which is/are electrically charged? a. a-rays and y-rays b. a-rays, b-rays, and y-rays c. b-rays d. a-rays e. a-rays and b-rays

e. a-rays and b-rays

Which statement below correctly describes the responses of alpha, beta, and gamma radiation to an electric field? a. only alpha is deflected while beta and gamma show no response. b. both beta and gamma are deflected in the same direction, while alpha shows no response. c. both alpha and gamma are deflected in the same direction, while beta shows no response. d. both alpha and beta are deflected in the same direction, while gamma shows no response. e. alpha and beta are deflected in opposite directions, while gamma shows no response.

e. alpha and beta are deflected in opposite directions, while gamma shows no response.

Cathode rays are ___________. a. neutrons b. X-rays c. protons d. atoms e. electrons

e. electrons

Which one of the following is often easily separated into its components by simple techniques such as filtering or decanting? a. homogeneous mixture b. elements c. solutions d. compounds e. heterogeneous mixture

e. heterogeneous mixture

The uncertainty principle states that _______________. a. it is impossible to know how many electrons there are in an atom b. matter and energy are really the same thing c. there can only be one uncertain digit in a reported number d. it is impossible to know anything with certainty e. it is impossible to know the exact position and momentum of an electron

e. it is impossible to know the exact position and momentum of an electron

The gold foil experiment performed in Rutherford's lab ____________. a. was the basis for Thomson's model of the atom b. confirmed the plum-pudding model of the atom c. utilized the deflection of beta particles by god foil d. proved the law of multiple proportions e. led to the discovery of the atomic nucleus

e. led to the discovery of the atomic nucleus

Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? a. 4d b. 4s c. 4p d. 4f e. none of the above

e. none of the above

When a hydrocarbon burns in air, what component of air reacts? a. water b. carbon dioxide c. nitrogen d. argon e. oxygen

e. oxygen

All of the orbitals in a given electron shell have the same value as the ___________ quantum number. a. magnetic b. psi c. angular momentum d. spin e. principal

e. principal

The photoelectric effect is _________. a. a relativistic effect b. the total reflection of light by metals giving them their typical luster c. the darkening of photographic film when exposed to an electric field d. the production of current by silicon solar cells when exposed to sunlight e. the ejection of electrons by a metal when struck with light of sufficient energy

e. the ejection of electrons by a metal when struck with light of sufficient energy

Which of the following is not an exact number? a. the number of millimeters in a kilometer b. the number of seconds in a year c. the number of grams in a kilogram d. the number of centimeters in an inch e. the number of liters in a gallon

e. the number of liters in a gallon

Of the following, only _________ is an extensive property. a. density b. temperature c. boiling point d. freezing point e. volume

e. volume