Chemistry Midterm Flash Cards

Consider the following electron configurations to answer the questions that follow. (i) 1s22s22p63s1 (ii) 1s22s22p63s2 (iii) 1s22s22p63s23p1 (iv)1s22s22p63s23p4 (v) 1s22s22p63s23p5 The electron configuration belonging to the atom with the highest second ionization energy is (i) (ii) (iii) (iv) (v)

(i)

Consider the general valance electron configuration of ns2np5 and the following statements: (i) Elements with this electron configuration are expected to form -1 anions (ii) Elements with this electron configuration are expected to have large positive electron affinities (iii) Elements with this electron configuration are nonmetals (iv) Elements with this electron configuration form acidic oxides Which statements are true? (i),(ii), and (iii) (i),(iii), and (iv) (i) and (ii) (ii) and (iii) all are true

(i),(iii), and (iv)

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? (iii) and (iv) (ii) only (ii) and (iii) (i) and (ii) (iii) only

(ii) and (iii)

The charge on the copper ion in the salt CuO is ________ +3 +1 -2 +2 -1

+2

The oxidation number of iron in Fe2O3 is ___ -2 +1 -3 +3 +2

+3

The formal charge on carbon in the molecule below is ____ .. .. O=C=O .. .. +1 0 -1 +2 +3

0

What is the maximum number of double bonds that a hydrogen atom can form? 0 1 2 3 4

0

Which of the following liquids has the greatest density? 210 cm^3 with a mass of 12 g 0.022 cm^3 with a mass of 0.10 g 54 cm^3 with a mass of 45 g 13 cm^3 with a mass of 23 g 3.5 cm^3 with a mass of 10 g

0.022 cm^3 with a mass of 0.10 g

Osmium has a density of 22.6 g/cm3. What volume (in cm3) would be occupied by a 21.8 g sample of osmium? 2.03 × 10^3 0.965 2.03 × 10^-3 1.04 493

0.965

How many different types of resonance structures can be drawn for the ion SO32- where all atoms satisfy the octet rule? 4 3 1 5 2

1

Which of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranges was n, l, ml, and ms) 1,0,0,1/2 2,2,-1,-1/2 5,4,-5,1/2 3,3,3,1/2 3,3,3,-1/2

1,0,0,1/2

Hydrogen is unique among the elements because _____ 1. It is not really a member of any particular group 2.Its electron is not at all shielded from its nucleus 3.it is the lightest element 4.It is the only element to exist at room temperature as a diatomic has 5.It exhibits some chemical properties similar to those of groups 1A and 7A A)2,3,4,5 B)1,4,5 C)1,2,3,5 D)1,2,3,4,5 E)3,4

1,2,3,5

Gold has a density of 0.01932 kg/cm^3. What volume (in cm3) would be occupied by a 33.3 g sample of gold? 5.80 x 10^-4 0.663 5.80 1.72 0.581

1.72

Which species has 54 electrons? 128 52 Te2- 132 54 Xe2+ 118 50 Sn2+ 132 54 Xe+ 112 48 Cd

128 52 Te2-

Which pair of atoms constitutes a pair of isotopes of the same element? *20 21 10 X 11 X *14 12 6 X 6 X *17 17 9 X 8 X *14 14 6 X 7 X *19 19 10 X 9 X

14 12 6 X 6 X

At maximum, an f-subshell can hold _____ electrons , a d-subshell can hold _____ electrons, and a p-subshell can hold __ electrons. 14,10,6 2,8,18 2,12,21 2,6,10 14,8,2

14,10,6

The estimated costs for remodeling the interior of an apartment are: three 1 gallon cans of paint at $13.22 each, two paint brushes at $9.53 each, and $1.35 for a helper. The total estimated cost with the appropriate significant figure is $_________ 1.9 x 10^2 194 193.7 2 x 10^2 193.72

194

Which of the following has the same number of significant figures as the number 1.00310? 199.791 1 × 10^6 8.66 100 5.119

199.791

Which one of the following species has as many electrons as it has neutrons? 40Ca2+ 14C2+ 1H 14C 19F-

19F-

Which electron configuration represents a violation of Hund's rule for an atom in its ground state? 1s-up 2s-up 2p-upupup 1s-updown 2s-updown 2p-upup 1s-updown 2s-up 2p-empty 1s-updown 2s-updown 2p-up updown 1s-updown 2s-updown 2p-upup up up

1s-updown 2s-updown 2p-up updown

Which electron configuration represents a violation of Hund's rule for an atom at its ground state? 1s-updown 2s-updown 2p-up up up 1s-up 2s-updown 2p-empty 1s-updown 2s-updown 2p-updown 1s-updown 2s-updown 2p-up empty up 1s-upup 2s-updown 2p-empty

1s-updown 2s-updown 2p-updown

Which electron configuration represents a violation of the Pauli exclusion principle? 1s-updown 2s-up 2p-empty 1s-updown 2s-updown 2p-up updown 1s-updown 2s-updown 2p-up 1s-updown 2s-updown 2p-upup up up 1s-up 2s-up 2p-up up up

1s-updown 2s-updown 2p-upup up up

Which electron configuration represents a violation of the Pauli exclusion principle? 1s-upup 2s-updown 2p-empty 1s-up 2s-updown 2p-empty 1s-up 2s-up 2p-up up up 1s-updown 2s-updown 2p-up empty up 1s-updown 2s-updown 2p-updown

1s-upup 2s-updown 2p-empty

The ground state electron configuration of Ga is ____. [Ar]4s23d11 1s22s22p63s23p64s24d104p1 1s22s23s23p64s23d104p1 1s22s22p63s23p64s23d104p1 1s22s22p63s23p64s23d104d1

1s22s22p63s23p64s23d104p1

The ground state electron configuration of Fe is ______ 1s22s23s23p63d6 1s22s22p63s23p64s24d6 1s22s22p63s23p64s2 1s22s22p63s23p64s23d6 1s22s23s23p10

1s22s22p63s23p64s23d6

A double bond consists of ____ pairs of electrons shared between two atoms 1 3 2 4 6

2

The energy of a photon that has a wavelength of 9.0 m is ____ J. 4.5x10^-25 2.7x10^9 4.5x10^25 6.0x10^-23 2.2x10^-26

2.2x10^-26

What is the frequency of light (s-1) that has a wavelength of 1.23x10^-6 cm? 2.44x10^16 3.69 4.10x10^-17 1.04x10^-13 9.62x10^12

2.44x10^16

The wavelength of light that has a frequency of 1.20x10^13 s-1 is _____m 12.0 2.5 25.0 0.0400 2.50x10^-5

2.50x10^-5

Of the following, __________ is the smallest mass 2.5x10^-2 mg 25 kg 2.5x10^10 ng 2.5x10^15 g 2.5x10^-4 µg

2.5x10^-4 µg

A radio station broadcasts at 105.2 MHz. The wavelength of the signal is _____m. 2.85 3.10 3.02 3.84 2.90

2.85

An FM radio station broadcasts electromagnetic radiation at a frequency of 100.6 MHz. The wavelength of this radiation is ____ m. 3.018x10^16 2.982 3.018x10^10 0.3353 2.982x10^6

2.982

There are ____ valence electrons in the Lewis structure of CH3CH2Cl 14 10 18 12 20

20

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. Isotope Abundance(%) Mass 221X 74.22 220.9 220X 12.78 220.0 218X 13.00 218.1 A)221.0 B)218.5 C)220.42 D)219.7 E)220.4

220.4

The temperature of -25 °C is __________ in Kelvin. 266 103 298 138 248

248

There are ___ valence electrons in the Lewis structure of CH3OCH2CH3 18 36 20 26 32

26

How many significant figures should be retained in the result of the following calculation? 12.00000x0.9893+13.00335x0.0107 1 2 3 4 5 6

3

An electron cannot have the quantum numbers n=_____, l=_____, ml=____ 6, 1, 0 3, 2, 3 3, 2, -2 3, 2, 1 1, 0, 0

3, 2, 3

Which one of the following represents an impossible set of quantum numbers for an electron in an atom (arranged as n, l, ml, and ms) 2, 1, -1, -1/2 3, 3, 3, 1/2 5, 4, -3, -1/2 5, 4, -3, 1/2 1, 0, 0, 1/2

3, 3, 3, 1/2

The energy (J) required for an electron transition in a Bohr hydrogen atom from n=2 to n=3 is ____ J -7.90x10^-19 3.00x10^-19 4.00x10^-19 4.60x10^14 -3.00x10^-19

3.00x10^-19

The wavelength of a photon that has an energy of 6.33x10^-18 J is ____m. 3.10x10^-8 4.21x10^-24 3.79x10^-7 2.38x10^23 9.55x10^15

3.10x10^-8

Electromagnetic radiation with a wavelength of 531 nm appears as green light to the human eye. The energy of one photon of this light is 3.74x10^-19 J. Thus, a laser that emits 1.3x10^-2 J of energy in a pulse of light at this wavelength produces _______ 2.9x10^-17 1.8x10^19 6.5x10^13 9.2x10^-24 3.5x10^16

3.5x10^16

The recommended adult dose of Elixophyllin, a drug used to treat asthma, is 6.00 mg/kg of body mass. Calculate the dose in milligrams for a 115-lb person. 1 lb = 453.59 g 3.1 X 10^5 24 1.5 313 1521

313

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. Isotope Abundance Mass 31X 35.16 31.16 34X 64.84 34.30 A)30.20 B)32.73 C)35.22 D)34.02 E)33.20

33.20

Which species has 16 protons? 16O 34S^2- 36Cl 80Br- 31P

34S^2-

The ion ICl4- has ____ valence electrons 36 28 35 34 8

36

How many different principal quantum numbers can be found in the ground state electron configuration of nickel? 2 3 4 5 6

4

How many hydrogen atoms must bond to carbon to give it an octet of valence electrons? 1 2 3 4 5

4

In the Lewis symbol for a sulfur atom, there are ___ paired and ____ unpaired electrons 2,4 4,2 0,6 2,2 5,1

4,2

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. Isotope Abundance Mass 38X 5.07 37.919 39X 15.35 39.017 42X 79.85 42.111 A)38.64 B)39.07 C)33.33 D)39.68 E)41.54

41.54

When the electron in a hydrogen atom moves from n=5 to n=2 light with a wavelength of ____ nm is emitted 434 657 410 487 93.8

434

An object measuring 0.4500 kilograms will have a mass of ________ grams 45.00 4.500 2222 0.0004500 450.0

450.0

When the electron in a hydrogen atom moves from n=4 to n=2, light with a wavelength of ____ nm is emitted 93.8 410 434 657 486

486

The de Broglie wavelength of a 4.0 gram bullet traveling at the speed of sound is ____. The speed of sound is 331 m/sec. 3.35x10^-33m 2.7x10^-37m 2.7x10^-34m 6.6x10^-31m 5.0x10^-34m

5.0x10^-34m

What is the de Broglie wavelength (m) of a 25-g object moving at a speed of 5.0 m/s2 6.6x10^-36 3.32x10^-36 1.9x10^32 5.3x10^-33 3.02x10^45

5.3x10^-33

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The frequency of this light is ____. 1.58x10^11 1.75x10^-15 5.71x10^14 5.71x10^5 1.58x10^2

5.71x10^14

There are ___ protons, _____ neutrons, and ____ electrons in 131 I- 78, 53, and 72 53, 131, and 52 131, 53, and 54 53, 78, and 54 131, 53, and 52

53, 78, and 54

There are _____ electrons, _____ protons, and ____ neutrons in an atom of 132 54 Xe 54, 54, 132 78, 78, 132 54, 54, 78 78, 78, 54 132, 132, 54

54, 54, 78

Of the following, ________ is the smallest mass. 55 kg 55 ng 55 mg 55 dg 55 µg

55 ng

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. Isotope Abundance Mass 53X 19.61 52.62 56X 53.91 56.29 58X 26.48 58.31 A)55.74 B)33.33 C)57.23 D)56.11 E)56.29

56.11

A tin atom has 50 electrons. Electrons in the ____ subshell experience the lowest effective nuclear charge. A) 1s B) 3d C) 5s D) 5p E) 3p

5p

The _____ orbital is degenerate in energy with 5py in a many-electron atom 5dxy 5px 5d2 4py 5s

5px

The halogens, alkali metals, and alkaline earth metals have ___ valence electrons 7,4,6 2,7,4 7,1,2 1,5,7 8,2,3

7,1,2

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? 8 × 10^-1 g/mL 7.9 × 10^-1 g/mL 7.86 × 10^-1 g/mL 7.859 × 10^-1 g/mL 7.8586 × 10^-1 g/mL

7.859 × 10^-1 g/mL

The wavelength of light emitted from a traffic light having a frequency of 3.85x10^14 Hz is _____ 779 nm 702 nm 583 nm 674 nm 641 nm

779 nm

Which isotope has 45 neutrons? 34 17 Cl 78 34 Se 103 45 Rh 80 35 Br 80 36 Kr

80 35 Br

Elements in group ____ have a np6 electron configuration in the outer shell 5A 4A 7A 6A 8A

8A

There are _____ protons, _____ neutrons, and _____ electrons in 238U+5 146, 92, and 146 92, 92, and 87 92, 146, and 87 146, 92, and 92 92, 146, and 92

92, 146, 87

Which one of the following has the element name and symbol correctly matched? C, copper Sn, silicon Mg, manganese Ag, silver P, potassium

Ag, silver

Which of the following correctly represents the second ionization of aluminum? Al+(g)+e- to Al(g) Al-(g)+e- to Al2-(g) Al(g) to Al+(g)+e- Al+(g)+e- to Al2+(g) Al+(g) to Al2+(g)+e-

Al+(g) to Al2+(g)+e-

Which of the following correctly represents the third ionization of aluminum? Al(g) to Al+(g)+e- Al-2(g)+e- to Al3-(g) Al+2(g)+e- to Al3+(g) Al+2(g)+e- to Al+1(g) Al+2(g) to Al3+(g)+e-

Al2+ tp Al3+(g)+e-

Which statement below correctly describes the responses of alpha, beta, and gamma radiation to an electric field? *Both alpha and beta are deflected in the same direction, while gamma shows no response *Alpha and beta are deflected in opposite directions, while gamma shows no response *Only alpha is deflected, while beta and gamma shows no response *Both alpha and gamma are deflected in the same direction, while beta shows no response *Both betas and gamma are deflected in the same direction, while alpha shows no response

Alpha and beta are deflected in opposite directions, while gamma shows no response

Of the choices below, which gives the order for first ionization energies? S>Si>Cl>Al>Ar Cl>S>Al>Si>Ar Ar>Cl>S>Si>Al Cl>S>Al>Ar>Si Al>Si>S>Cl>Ar

Ar>Cl>S>Si>Al

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

Atoms are composed of protons, neutrons, and electrons

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet? H N B C O

B

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet? H C B O N

B

_____________-rays consist of fast-moving electrons Gamma Beta X Alpha none of the above

Beta

Which of the following correctly represents the electron affinity of bromine? Br2(g)+2e- to 2Br-(g) Br(g)+e- to Br-(g) Br+(g)+e- to Br-(g) Br2(g)+e- to Br-(g) Br(g) to Br+(g)+e-

Br(g)+e- to Br-(g)

In which set of elements would all members be expected to have very similar chemical properties? Cl, Br, Na Si, As, Te Br, I, At P, Se, I Ne, Na, Mg

Br, I, At

Which ion below has the largest radius? A) F⁻ B) Cl⁻ C) K⁺ D) Br⁻ E) Na⁺

Br-

In the symbol below X= 13 6 X C K Al N

C

What is the molecular formula for Ethane? C4H10 C4H8 C3H8 C3H6 C2H6

C2H6

Which one of the following molecular formulas is also an empirical formula? C6H6O2 H2O2 C2H6SO H2P4O6 C6H6

C2H6SO

The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is _____ C12H14O6 C6H7O3 CHO CH2O C2H4O

C6H7O3

The central atom in ___ does not violate the octet rule XeF4 ICl4- CF4 SF4 KrF2

CF4

The central atom in ____ does not violate the octet rule SF4 XeF4 CF4 ICl4- KrF2

CF4

Which compounds do not have the same empirical formulas? C2H4, C3H6 C2H4O2, C6H12O6 CO, CO2 C2H2, C6H6 C2H5COOCH3, CH3CHO

CO, CO2

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

CO, CO2

Of the following oxides, ____ is the most acidic Na2O Li2O CO2 Al2O3 CaO

CO2

Element M reacts with oxygen to form an oxide with the formula MO. Element MO is dissolved in water, the resulting solution is basic. Element M could be ___ N Na Ca S C

Ca

Which equation correctly represents the first ionization of calcium? Ca+(g)+e- to Ca(g) Ca(g) to Ca-(g)+e- Ca(g)+e- to Ca-(g) Ca-(g) to Ca(g)+e- Ca(g) to Ca+(g)+e-

Ca(g) to Ca+(g)+e-

Which equation correctly represents the electron affinity of calcium? Ca+(g)+e- to Ca(g) Ca(g)+e- to Ca-(g) Ca(g) to Ca-(g)+e- Ca-(g) to Ca(g)+e- Ca(g) to Ca+(g)+e-

Ca(g)+e- to Ca-(g)

Which of the following does not have eight valence electrons? Br- Rb+ Xe Ca+ All of the above

Ca+

Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? C, O Ca, Mg Cs, Ba H, Li Ga, Ge

Ca, Mg

Na reacts with element X to form an ionic compound with the formula Na3X. Ca will react with X to form __________. CaX2 CaX Ca2X3 Ca3X Ca3X2

Ca3X2

Which of the following compounds would you expect to be ionic? SF6 NH3 H2O2 CaS H2O

CaS

Of the following elements, ___ has the most negative electron affinity Be Cl N Na Li

Cl

Of the following elements, ___ has the most negative electron affinity P Al B Cl Si

Cl

Of the following elements, ____ has the most negative electron affinity Be Cl N Na Li

Cl

Of the following elements, _____ has the most negative electron affinity B P Si Cl Al

Cl

Of the ions below, only ___ has a noble gas electron configuration I+ O2+ K- Cl- S3-

Cl-

A valid Lewis structure of __________ cannot be drawn without violating the octet rule. SO3 PCl3 CO2 ClF3 CCl4

ClF3

Which one of the following compounds is chromium(III) oxide? Cr3O2 Cr2O3 Cr2O4 Cr3O CrO3

Cr2O3

In the molecule below, which atom has the largest partial negative charge? Cl l F- C-Br l I A)C B)Br C)F D)I E)Cl

F

The ion with the smallest diameter is ______ Cl- F- O2- Br- I-

F-

Which of the following has the element name and symbol correctly matched? B, bromine S, sodium Fe, iron N, neon Tn, tin

Fe, iron

The substance ____ is always produced when an active metal reacts with water H2 H2O O2 CO2 NaOH

H2

Of the molecules below, the bond in __________ is the most polar. HF HI HBr HCl H2

HF

The symbol for the element mercury is __________. Pb Sn Na Me Hg

Hg

A valid Lewis structure of ____ cannot be drawn without violating the octet rule NF3 IF3 PF3 SbF3 SO4^2-

IF3

Which one of the following is true about the liter? It is equivalent to a cubic decimeter It is slightly smaller than a gallon. It is slightly smaller than a quart. It contains 10^6 cubic centimeters.

It is equivalent to a cubic decimeter

The element that has a valance configuration of 4s1 is _____ K Cs Rb Na Li

K

Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge, and Kr? Kr>As>Ge>Ca>K Kr>Ge>As>K>Ca Ca>K>As>Ge>Kr Ge>As>Kr>K>Ca K>Ca>Ge>As>Kr

K>Ca>Ge>As>K

The list that correctly indicates the order of metallic character is Li>Na>K O>Se>S C>Ge>Si F>Cl>Br K>Na>Li

K>Na>Li

Which element would be expected to have chemical and physical properties closest to those of argon? Kr O Cl Fe S

Kr

Of the choices below, which gives the order for the first ionization energies? Kr>Br>Se>Ge>Ga Kr>Se>Br>Ga>Ge Ga>Ge>Se>Br>Kr Ga>Br>Ge>Kr>Se Br>Se>Ga>Kr>Ge

Kr>Br>Se>Ge>Ga

Based on the octet rule, magnesium most likely forms a ____ ion. A) Mg⁶⁺ B) Mg⁶⁻ C) Mg²⁻ D) Mg²⁺ E) Mg⁻

Mg2+

Which formula/name pair is incorrect? Mn(NO2)2 manganese(II) nitrite Mg3N2 magnesium nitrite Mn(NO3)2 manganese(II) nitrate Mg(NO3)2 magnesium nitrate Mg(MnO4)2 magnesium permanganate

Mg3N2 magnesium nitrite

The Lewis structure of HCN (H bonded to C) shows that ___ has ___ nonbonding electron pairs C,2 C,1 N,1 N,2 H,1

N,1

Which species below is the nitrite ion? NO3- N3- NO2- NH4+ N^3-

NO2-

Which species below is the nitride ion? NH4+ Na^+ N^3- NO3- NO2-

N^3-

Which ion below has a noble gas electron configuration? N2- C2+ B2+ Na+ Li2+

Na+

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si, and Ar? Na>Mg>Si>P>Ar Ar>P>Si>Mg>Na Ar>Si>P>Na>Mg Si>P>Ar>Na>Mg Mg>Na>P>Si>Ar

Na>Mg>Si>P>Ar

Of the elements below, ____ is the least metallic Ne Al Na Mg K

Ne

A cube of an unknown metal measures 1.61 mm on one side. The mass of the cube is 36 mg. Which of the following is most likely the unknown metal? Rhodium 12.4 Copper 8.96 Niobium 8.57 Vanadium 6.11 Zirconium 6.51

Niobium

Which atom has the smallest number of neutrons? Nitrogen-14 Neon-20 Oxygen-16 Carbon-14 Fluorine-19

Nitrogen-14

Of the following atoms, which has the largest first ionization energy? Sb O As Ge Se

O

Which one of the following elements has an allotrope that is produced in the upper atmosphere by lightning? O S N Cl He

O

Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br Sr Sr, O, Se O, Se Br Na

O, Se

Which of the following has the bonds correctly arranged in order of increasing polarity? O-F, Be-F, Mg-F, N-F Be-F, Mg-F, N-F, O-F Mg-F, Be-F, N-F, O-F N-F, Be-F, Mg-F, O-F O-F, N-F, Be-F, Mg-F

O-F, N-F, Be-F, Mg-F

Given the electronegativities below, which covalent single bond is most polar? Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5 O-C O-H N-H C-H O-N

O-H

Which of the following is an isoelectronic series? B5-, Si4-, As3-, Te2- S, Cl, Ar, K F-, Cl-, Br-, I- O2-, F-, Ne, Na+ Si2-, P2-, S2-, Cl2-

O2-, F-, Ne, Na+

Which of the following correctly represents the second ionization of phosphorus? P-(g)+ e- to P2-(g) P+(g) to P2+(g)+e- P+(g)+e- to P(g) P(g) to P+(g) +e- P+(g)+e- to P2+ (g)

P+ to P2+(g)+e-

Based on the octet rule, phosphorus most likely forms a _____ ion. A) P³⁻ B) P⁺ C) P⁵⁻ D) P³⁺ E) P⁵⁺

P3-

Of the choices below, which one is not an ionic compound? NaCl RbCl PCl5 MoCl6 PbCl2

PCl5

Which one of the following is a metal? Ge S C Pb Br

Pb

The formula of palladium(IV) sulfide is ____ PdS4 Pd2S4 Pd4S Pd2S2 PdS2

PdS2

Between which two elements is the difference in metallic character the greatest? O and I Rb and O Li and O Rb and I Li and Rb

Rb and O

Which one of the following is most likely to lose electrons when forming an ion? N P F S Rh

Rh

____ is isoelectronic with argon and ____ is isoelectronic with neon Ne-, Kr+ Ne-, Ar+ S-2, Na+ Cl-, Cl+ F+, F-

S-2, Na+

The most common and stable allotrope of sulfur is ____ S4 S2 S8 S

S8

Which species below is the sulfite ion? S^2- SO4^-2 HS- SO3^-2 SO2^-2

SO3^-2

In which set of elements would all members be expected to have very similar chemical properties? Li3N NaCl SiO2 K2O Na2SO4

SiO2

Of the following metals, _____ exhibits multiple oxidation states Sn Rb Mg Cs Al

Sn

Which metal forms cations of differing charges? Ba Cs Sn Al K

Sn

Which calculation clearly shows a conversion between temperatures in degrees Celsius, t(C), and temperature in Kelvins, T(K) T(K)=273.15-t(C) T(K)=t(C) T(K)=t(C)+273.15 T(K)=[t(C)-32]/1.8 T(K)=[t(C)+32]x1.8

T(K)=t(C)+273.15

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

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

Which one of the following is not true about the alkali metals? *They have the lowest first ionization energies of the elements *They are very reactive elements *They all have 2 electrons in their valence shells *They are low density solids at room temperature *They are all readily ions with a +1 charge

They all have 2 electrons in their valence shells

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

Water is 11% hydrogen and 89% oxygen by mass

The ground state configuration of fluorine is _____ [He]2s22p4 [He]2s22p2 [He]2s22p3 [He]2s22p6 [He]2s22p5

[He]2s22p5

The condensed electron configuration of silicon, element 14, is _____ [Ne]3s23p2 [He]2s42p6 [He]2s4 [He]2s62p2 [Ne]2p10

[Ne]3s23p2

The electron configuration of the phosphide ion (P3-) is ____ [Ne]3s23p3 [Ne]3s23p1 [Ne]3s2 [Ne]3s23p6 [Ne]3p2

[Ne]3s23p6

Which of the following is not a characteristic of metals? low ionization energies malleability ductility acidic oxides all of these

acidic oxides

The elements in groups 1, 16, and 17 are called, ____ respectively. alkali metals, chalcogens, and halogens alkaline earth metals, transition metals, and halogens alkali metals, halogens, and noble gases halogens, transition metals, and alkali metals alkaline earth metals, halogens, and chalcogens

alkali metals, chalcogens, and halogens

Which of the following has eight valence electrons? Cl- Na+ Ti4+ Kr all of the above

all of the above

Which one of the following orbitals can hold two electrons? 2px 3s 4dxy all of the above none of the above

all of the above

Which one of the following elements has a symbol that is not derived from its foreign name? aluminum lead mercury copper tin

aluminum

The _____ quantum number defines the shape of an orbital principal angular momentum psi spin magnetic

angular momentum

Which atom has the largest number of neutrons? chlorine-37 calcium-40 argon-40 potassium-39 phosphorus-30

argon-40

Elements in the modern version of the periodic table are arranged in order of increasing ______ atomic number average atomic mass number of isotopes atomic mass oxidation number

atomic number

In a px orbital, the subscript x denotes the _____ of the electron energy spin of the electrons size of the orbital probability of the shell axis along which the orbital is aligned

axis along which the orbital is aligned

Which pair of electrons is most apt to form an ionic compound with each other? oxygen, fluorine nitrogen, hydrogen sulfur, fluorine calcium, sodium barium, bromine

barium, bromine

An element cannot _______ be separated into other substances by chemical means be part of a heterogeneous mixture interact with other elements to form compounds be a pure substance be part of a homogeneous mixture

be separated into other substances by chemical means

For which of the following can the composition vary? element heterogeneous mixture both homogeneous and heterogeneous mixtures pure substance homogeneous mixture

both homogeneous and heterogeneous mixtures

The correct name for CCl4 is ________ carbon chloride carbon chlorate carbon tetrachlorate carbon perchlorate carbon tetrachloride

carbon tetrachloride

Of the elements below, ____ is the most metallic sodium calcium barium magnesium cesium

cesium

The correct name for HClO3 is _________ hydrochlorous acid chloric acid hydrochloric acid perchloric acid chlorous acid

chloric acid

Chlorine is much more apt to exist as an anion than is sodium. This is because *chlorine is a gas and sodium is a solid *chlorine is more metallic than sodium *chlorine has a greater ionization energy than sodium does *chlorine is bigger than sodium *chlorine has a greater electron affinity than sodium does

chlorine has a greater electron affinity than sodium does

The law of constant composition applies to __________ solids heterogeneous mixtures compounds solutions homogeneous mixtures

compounds

Transition metals within a period differ mainly in the number of ____ electrons p f s d all of the above

d

As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________. increases, increases decreases, decreases increases, decreases decreases, increases is unpredictable

decreases, increases

An element that appears in the lower left corner of the periodic table is ______ *either a metalloid or a non-metal *definitely a non-metal *definitely a metalloid *either a metal or a metalloid *definitely a metal

definitely a metal

Atomic radius generally increases as we move __________. *down a group and from right to left across a period *down a group; the period position has no effect *up a group and from left to right across a period *up a group and from right to left across a period *down a group and from left to right across a period

down a group and from right to left across a period

The Lewis structure of N2H2 shows ____ each nitrogen has one nonbonding electron pair a nitrogen-nitrogen single bond each hydrogen has one nonbonding electron pair a nitrogen-nitrogen triple bond each nitrogen has two nonbonding electron pairs

each nitrogen has one nonbonding electron pair

Cathode rays are _______ protons atoms electrons neutrons x-rays

electrons

Which one of the following is a pure substance salt water concrete milk wood elemental copper

elemental copper

The suffix -ide is used primarily ________ for monoatomic cations for polyatomic cation names for the name of the first element in a molecular compound for monoatomic anion names to indicate binary acids

for monoatomic anion names

Alkaline earth metals _____ exist as triatomic molecules form halides with the formula MX form monoanions form basic oxides have the smallest atomic radius in a given period

form basic oxides

The ____ have the most negative electron affinities. alkaline earth metals halogens chalcogens alkali metals transition metals

halogens

A combination of sand, salt, and water is an example of a ________. pure substance homogeneous mixture heterogeneous mixture solid compound

heterogeneous mixture

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

heterogeneous mixture

A small amount of salt dissolved in water is an example of a _________

homogeneous mixture

Precision refers to ________. how close a measured number is to other measured numbers how close a measured number is to zero how close a measured number is to infinity how close a measured number is to the calculated value how close a measured number is to the true value

how close a measured number is to other measured numbers

____ is a unique element and does not truly belong to any family nitrogen helium radium uranium hydrogen

hydrogen

Elements ________ exhibit similar similar physical and chemical properties *with similar chemical symbols *in the same period of the periodic table *in the same group of the periodic table *with similar atomic masses *on opposite sides of the periodic table

in the same group of the periodic table

The first ionization energies of the elements ____ as you go from left to right across a period of the periodic table, and ___ as you go from the bottom to the top of a group in the table. increase, increase increase, decrease decrease, increase decrease, decrease

increase, increase

Electronegativity _____ from left to right within a period and ___ from top to bottom within a group increases, stays the same increases, decreases increases, increases decreases, increases stays the same, increases

increases, decreases

In ionic bond formation, the lattice energy of ions ____ as the magnitude of the ion charges ____ and the radii ____ decreases, increase, increase increases, decrease, decrease increases, increase, increase increases, decrease, increase increases, increase, decrease

increases, increase, decrease

The effective nuclear charge of an atom is primarily affected by ____ orbital radical probability outer electrons inner electrons nuclear charge electron distribution

inner electrons

An element in the upper right corner of the periodic table ___. A) is definitely a metal B) is definitely a metalloid C) is either a metal or metalloid D) is either a metalloid of a non-metal E) is definitely a non-metal

is definitely a non-metal

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

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

The gold foil experiment performed in Rutherford's lab ______ *confirmed the plum-pudding model of the atom *led to the discovery of the atomic nucleus *utilized the deflection of beta particles by gold foil *proved the law of multiple proportions *was the basis for Thomson's model of the atom

led to the discovery of the atomic nucleus

In the following list, only __________ is not an example of matter. table salt light elemental phosphorus planets dust

light

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

liquid

The correct name for MgF2 is _____ manganese bifluoride magnesium fluoride magnesium difluoride manganese difluoride monomagnesium difluoride

magnesium fluoride

Which one of the following is not an intensive property? boiling point temperature density melting point mass

mass

According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the ____ of an electron mass color shape charge momentum

momentum

Which quantum number determines the energy of an electron in a hydrogen atom? l ml n E n and l

n

Which quantum number determines the energy of an electron in a hydrogen atom? ml l n E n and l

n

Of the following transitions in the Bohr hydrogen atom, the ____ transition results in the emission of the highest-energy photon n=1 to n=4 n=6 to n=4 n=2 to n=7 n=4 to n=6

n=6 to n=4

Of the following transitions in the Bohr hydrogen atom, the _____ transition results in the emission of the highest-energy photon. n=6 - n=3 n=3 - n=6 n=7 - n=1 n=1 - n=6 n=1 - n=4

n=7 - n=1

The correct name for HNO2 is ______ hypo nitrous acid nitric acid nitrous acid hydrogen nitrate pernitric acid

nitrous acid

_____ are found uncombined, as monoatomic species in nature noble gases alkaline earth metals halogens alkali metals chalcogens

noble gases

Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger __________ in Ar. diamagnetism Hund's rule azimuthal quantum number paramagnetism nuclear charge

nuclear charge

The type of compound that is most likely to contain a covalent bond is ____ *held together by the electrostatic forces between oppositely charged ions *one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table *one that is composed of only nonmetals *a solid metal *there is no general rule to predict covalence in bonds

one that is composed of only nonmetals

To convert from one resonance structure to another, _____ electrons and atoms can both be moved neither electrons nor atoms can be moved only atoms can be moved electrons must be added only electrons can be moved

only electrons can be moved

In the periodic table, the elements are arranged in _______ *order of increasing atomic number *order of increasing metallic properties *alphabetical order *order of increasing neutron content *reverse alphabetical order

order of increasing atomic number

Resonance structures differ by _____ number of electrons only placement of atoms only number of atoms only number and placement of electrons placement of electrons only

placement of electrons only

The de Broglie wavelength of a _____ will have the shortest wavelength when traveling at 30 cm/s marble hydrogen atom car planet uranium atom

planet

The acidity of carbonated water is due to the _____ nonmetal oxides presence of sulfur addition of acid reaction of CO2 and H2O none of the above

reaction of CO2 and H2O

The reaction of a metal with a non metal produces a(n) _____ acid hydroxide oxide base salt

salt

Which element forms an ion with the same charge as the ammonium ion? calcium chlorine sodium nitrogen oxygen

sodium

Nonmetals can be __________ at room temperature. liquid or gas solid or liquid liquid only solid, liquid, or gas solid only

solid, liquid, or gas

Formulas that show how atoms are attached in a molecule are called _________. structural formulas diatomic formulas ionic formulas molecular formulas empirical formulas

structural formulas

Which one of the following does not occur as diatomic molecules in elemental form? sulfur nitrogen oxygen bromine hydrogen

sulfur

Which pair of elements is the most apt to form a molecular compound with each other? barium, bromine magnesium, iodine aluminum, oxygen sulfur, fluorine potassium, lithium

sulfur, fluorine

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

tarnishing of silver

Which one of the following is an intensive property? heat content temperature mass volume amount

temperature

The law of constant composition says __________. that the composition of a compound is always the same that all substances have the same composition that the composition of a heterogeneous mixture is always the same that the composition of a homogeneous mixture is always the same that the composition of an element is always the same

that the composition of a compound is always the same

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

the condensation of water vapor

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

the condensation of water vapor

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

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

Lattice energy is ____ *the energy given off when gaseous ions combine to form one mole of an ionic solid *the energy required to convert a mole of ionic solid into its constituent ions in the gas phase *the energy required to produce one mole of an ionic compound from its constituent elements in their standard states *the sum of ionization energies of the components in an ionic solid *the sum of electron affinities of the components in an ionic solid

the energy required to convert a mole of ionic solid into its constituent ions in the gas phase

In the Rutherford nuclear-atom model ________ A)the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass B)mass is spread essentially uniformly throughout the atom C)the heavy subatomic particles, protons and neutrons, reside in the nucleus 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

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

Of the following _____ radiation has the longest wavelength and ____ radiation has the greatest energy gamma ultraviolet visible visible, ultraviolet ultraviolet, gamma visible, gamma gamma, visible gamma, gamma

visible, gamma

Oxides of the active metals combine with acid to form ____ water and a salt metal hydrides oxygen gas hydrogen gas metal hydroxides

water and a salt

Of the bonds C-C, C=C, and C(triple bond)C, the C-C bond is __ strongest/shortest weakest/longest weakest/shortest intermediate in both strength and length strongest/longest

weakest/longest

Of the following, _____ radiation has the shortest wavelength ultraviolet x-ray radio infrared microwave

x-ray

Of the three types of radioactivity characterized by Rutherford, which is/are not electrically charged? a-rays y-rays a-rays and y-rays a-rays and B-rays a-rays, B-rays, and y-rays

y-rays