Chem Review
Which compounds do not have the same empirical formula?
CO, CO2
The ground-state configuration of fluorine is ________.
[He]2s22p5
The condensed electron configuration of argon, element 18, is ________.
[Ne]3s23p6
All of the ________ have a valence shell electron configuration ns1.
alkali metals
The correct name for CCl4 is ________.
carbon tetrachloride
What is the correct formula for ammonium sulfide?
(NH4)2S
The charge on the silver ion in the salt AgCl is ________.
+1
What is the oxidation number of nitrogen in NO2-?
+3
Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) SubstanceΔH°f (kJ/mol)ΔG°f (kJ/mol)S (J/K-mol) Calcium Ca (s)0041.4 CaCl2 (s)-795.8-748.1104.6 Ca2+ (aq)226.7209.2200.8 Chlorine Cl2 (g)00222.96 Cl- (aq)-167.2-131.256.5 Oxygen O2 (g)00205.0 H2O (l)-285.83-237.1369.91 Phosphorus P2 (g)144.3103.7218.1 PCl3 (g)-288.1-269.6311.7 POCl3 (g)-542.2-502.5325 Sulfur S (s, rhombic)0031.88 SO2(g)-269.9-300.4248.5 SO3(g)-395.2-370.4256.2 The value of ΔH° for the decomposition of gaseous sulfur trioxide to its component elements,2SO3 (g) → 2S (s, rhombic) + 3O2 (g)is ________ kJ/mol.
+790.4
The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is ________ J.
-10,155
In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)△H = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.
-100.1kJ
Given the data in the table below, ΔH°rxn for the reaction4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l)is ________ kJ. H20(1) -286 NO(g) 90 NO2(g) 34 HNO3 (aq) -207 NH3 (g) -46
-1172
Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) SubstanceΔH°f (kJ/mol)ΔG°f (kJ/mol)S (J/K-mol) Carbon C (s, diamond)1.882.842.43 C (s, graphite)005.69 C2H2 (g)226.7209.2200.8 C2H4 (g)52.3068.11219.4 C2H6 (g)-84.68-32.89229.5 CO (g)-110.5-137.2197.9 CO2 (g)-393.5-394.4213.6 Hydrogen H2( g)00130.58 Oxygen O2 (g)00205.0 H2O (l)-285.83-237.1369.91 The value of ΔS° for the catalytic hydrogenation of ethene to ethane,C2H4 (g) + H2(g) → C2H6 (g)is ________ J/K ∙ mol.
-120.5
The value of ΔE for a system that performs 151 kJ of work on its surroundings and loses 79 kJ of heat is ________ kJ.
-230.
The value of ΔE for a system that performs 19 kJ of work on its surroundings and loses 9kJ of heat is 9kJ
-28
What is the oxidation state of nitrogen in ammonia?
-3
Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) SubstanceΔH°f (kJ/mol)ΔG°f (kJ/mol)S (J/K-mol) Carbon C (s, diamond)1.882.842.43 C (s, graphite)005.69 C2H2 (g)226.7209.2200.8 C2H4 (g)52.3068.11219.4 C2H6 (g)-84.68-32.89229.5 CO (g)-110.5-137.2197.9 CO2 (g)-393.5-394.4213.6 Hydrogen H2( g)00130.58 Oxygen O2 (g)00205.0 H2O (l)-285.83-237.1369.91 The combustion of acetylene in the presence of excess oxygen yields carbon dioxide and water:2C2H2 (g) + 5O2 (g) → 4CO2 (g) + 2H2O (l)The value of ΔS° for this reaction is ________ J/K ∙ mol.
-432.4
Given the data in the table below, ΔH°rxn for the reactionC2H5OH (l) + O2 (g) → CH3CO2H (l) + H2O (l)is ________ kJ.
-492.6
The value of ΔH° for the reaction below is -186 kJ.H2 (g) + Cl2 (g) → 2HCl (g)The value of ΔH°f for HCl (g) is ________ kJ/mol.
-93.0
In the Lewis structure of HCO3-, the formal charge on H is ________, and the formal charge on C is ________.
0,0
Which number of significant figures is incorrect?
0.00050 (five) This is incorrect since the first four zeros do not count. The correct number of significant figures is two.
Round the number 0.00637 to two significant figures.
0.0064
A 1.36-g sample of magnesium nitrate, Mg(NO3)2, contains ________ mol of this compound.
0.00917
How many moles of pyridine (C5H5N) are contained in 4.14 g of pyridine?
0.0523
An object measuring 77 milliliters will have a volume of ________ liters.
0.077
How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?
0.0800
Lithium and nitrogen react to produce lithium nitride:6Li (s) + N2 (g) → 2Li3N (s)How many moles of N2 are needed to react with 0.550 mol of lithium?
0.0917
Lithium and nitrogen react to produce lithium nitride:6Li (s) + N2 (g) → 2Li3N (s)How many moles of N2 are needed to react with 0.710 mol of lithium?
0.118
What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?
0.45
An object will sink in a liquid if the density of the object is greater than that of the liquid. The mass of a sphere is 9.83 g. If the volume of this sphere is less than ________ cm3, then the sphere will sink in liquid mercury (density = 13.6 g/cm3).
0.723
Osmium has a density of 22.6 g/cm3. What volume (in cm3) would be occupied by a 21.8 g sample of osmium?
0.965
For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?
1
When the following equation is balanced, the coefficient of H2 is __________.K (s) + H2O (l) → KOH (aq) + H2 (g)
1
Which of the following are combustion reactions?1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l)2) CaO (s) + CO2 (g) → CaCO3 (s)3) PbCO3 (s) → PbO (s) + CO2 (g)4) CH3OH (l) + O2 (g) → CO2 (g) + H2O (l)
1 and 4
An electron cannot have the quantum numbers n = ________, l = ________, ml = ________.
1, 1, 1
1 kilogram = ________ milligrams
1,000,000
An electron cannot have the quantum numbers n = ________, l = ________, ml = ________.
1,1,1
Which of the following are chemical processes?1. rusting of a nail2. freezing of water3. decomposition of water into hydrogen and oxygen gases4. compression of oxygen gas
1,3
The correct answer (reported to the proper number of significant figures) to the following is ________. (2.01)(6.936) / 12 = ________
1.2
45 m/s = ________ km/hr
1.6 × 10^2
A sample of aluminum metal absorbs 11.2 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is ________ g.
1.7
One million argon atoms is ________ mol (rounded to two significant figures) of argon atoms.
1.7 × 10^-18
How many total electrons are in the O2- ion?
10
In which one of the following numbers are all of the zeros significant?
100.090090
Perform the indicated operations and express the answer with the proper number of significant digits. 28.1 cm + 0.53 cm + 75.321 cm =
104.0 cm This number has one figure to the right of the decimal point and matches the quantity having the fewest digits to the right of the decimal point in the question.
The H-C-H bond angle in methane is approximately ________.
109.5
The wavelength of light emitted from a traffic light having a frequency of 2.74 × 1014 Hz is ________ nm.
1090
How many neutrons are there in one atom of 184W?
110
The F-B-F bond angle in the BF3 molecule is ________.
120°
Which of the following numbers is incorrectly rounded off to three significant figures?
1213 rounded to 1.213 × 103 This has four significant figures.
What is the mass % of aluminum in aluminum sulfate (Al2(SO4)3) rounded to three significant figures?
15.8
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. Mass 159.37 162.79 163.92
162.0
The element X has three naturally occurring isotopes. The isotopic 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 159/30.60/159.37 163/15.79/162.79 164/53.61/163.92
162.35
The value of ΔH° for the reaction below is -72 kJ. ________ kJ of heat are released when 5.5 mol of HBr is formed in this reaction.H2 (g) + Br2 (g) → 2HBr (g)
198
Which of the following has the same number of significant figures as the number 1.00310?
199.791
Which is the correct electron configuration for a nitrogen atom?
1s22s22p3
Which electron configuration represents a violation of the Pauli exclusion principle?
1s↑↑ 2s↑↓
Which electron configuration represents a violation of the Pauli exclusion principle?
1s↑↓ 2s↑↑ 2p ↑
Which one of the following is the correct electron configuration for a ground-state nitrogen atom?
1s↑↓ 2s↑↓ 2p↑↑↑
Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
1s↑↓ 2↑↓ 2p↑ ↑↓
How many total electrons are in the Li+ ion?
2
ΔS is positive for the reaction ________. A. HCl (g) + NH3 (g) → NH4Cl (s) B. Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s) C. CO2 (g) → CO2 (s) D. 2 KClO3 (s) → 2KCl (s) + 3 O2 (g) E. 2 Ca (s) + O2 (g) → 2 CaO (s)
2 KClO3 (s) → 2KCl (s) + 3 O2 (g)
If a iron atom loses 2 electrons to make an ion, what is the charge on that ion?
2+
Which of the following is a valid set of four quantum numbers? (n, l, ml, ms)
2, 1, 0, +1/2
When the following equation is balanced, the coefficients are ________.C8H18 + O2 → CO2 + H2O
2,25,16,18
When the following equation is balanced, the coefficients are ________.Al(NO3)3 + Na2S → Al2S3 + NaNO3
2,3,1,6
The central Xe atom in the XeF4 molecule has ________ unbonded electron pair(s) and ________ bonded electron pair(s) in its valence shell.
2,4
Oxygen forms an ion with a charge of ________.
2-
The combustion of propane (C3H8) produces CO2 and H2O:C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)The reaction of 2.5 mol of O2 will produce ________ mol of H2O.
2.0
Express the temperature, 275.18 K, in degrees Celsius.
2.03 °C
Round the following number to four significant figures and express the result in standard exponential notation: 0.00222755
2.228 × 10^-3
Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:CaO (s) + H2O (l) → Ca(OH)2 (s)A 3.50 g sample of CaO is reacted with 3.38 g of H2O. How many grams of water remain after completion of reaction?
2.25
Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:3 Mg + N2 → Mg3N2In a particular experiment, a 8.33-g sample of N2 reacts completely. The mass of Mg consumed is ________ g.
21.7
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 221/55.700/220.90 220/38.800/220.00 218/5.5000/218.10
220.40
The formula weight of PbCO3 is ________ amu.
267.2
What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide?
29.3
Of the reactions below, which one is not a combination reaction? A. 2N2 + 3H2 → 2NH3 B. CaO + H2O → Ca(OH)2 C. C + O2 → CO2 D. 2CH4 + 4O2 → 2CO2 + 4H2O E. 2Mg + O2 → 2MgO
2CH4 + 4O2 → 2CO2 + 4H2O
Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number?
2d
Aluminum forms an ion with a charge of ________.
3+
Which one of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranged as n, l, ml, and ms)
3, 0, 0, -1/2
Calculate the energy (J) found in one photon of visible light if the wavelength is 589 nm.
3.37 × 10^-19
Silver nitrate and aluminum chloride react with each other by exchanging anions:3AgNO3 + AlCl3 → Al(NO3)3 + 3AgClWhat mass in grams of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of AlCl3
3.56
The average distance from the Earth to the Moon, 383,000,000 m, can also be expressed as
3.83 × 1010 cm.
What is the mass % of carbon in dimethylsulfoxide (C2H6SO) rounded to three significant figures?
30.7
How many protons are there in one atom of 71Ga?
31
If 588 grams of FeS2 is allowed to react with 352 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced? DO NOT INCLUDE UNITS IN YOUR ANSWER. FeS2 + O2 → Fe2O3 + SO2
320
What volume (mL) of 7.48 × 10-2 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?
375
In which orbital will an electron add to the element chlorine to form a Cl-?
3p
How many different principal quantum numbers can be found in the ground-state electron configuration of nickel?
4
Which of the following are decomposition reactions?1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l)2) CaO (s) + CO2 (g) → CaCO3 (s)3) Mg (s) + O2(g) → MgO (s)4) PbCO3 (s) → PbO (s) + CO2 (g)
4 only
Which set of three quantum numbers (n, l, ml) corresponds to a 4s orbital?
4,0,0
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)
4,3,0,0
When the following equation is balanced, the coefficients are ________.NH3 (g) + O2 (g) → NO2 (g) + H2O (g)
4,7,4,6
Lithium and nitrogen react in a combination reaction to produce lithium nitride:6Li (s) + N2 (g) → 2Li3N (s)In a particular experiment, 2.50-g samples of each reagent are reacted. The theoretical yield of lithium nitride is ________ g.
4.18
How many atoms of carbon are in 23.1 g of glucose (C6H12O6)?
4.63 × 10^23
Electromagnetic radiation with a wavelength of 640 nm appears as orange light to the human eye. The frequency of this light is ________ s-1.
4.688 × 10^14
Which number is incorrectly labeled?
4.8 × 10−6 mL = 4.8 microliters 1 microliter is equal to 1 × 10−3 mL.
The density of silver is 10.5 g/cm3. A piece of silver that occupies a volume of 42.5 cm3 would have a mass of ________ g.
446
What is the volume (in cm3) of a 36.7 g piece of metal with a density of 6.95 g/cm3?
5.28
The density of silver is 10.5 g/cm3. A piece of silver with a mass of 61.3 g would occupy a volume of ________ cm3.
5.84
There are ________ electrons, ________ protons, and ________ neutrons in an atom of 132/54Xe.
54, 54, 78
The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 7.25 g of methane from 22.0 °C to 57.0 °C?
558J
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. Mass 52.62 56.29 58.31
56.14
There are ________ paired and ________ unpaired electrons in the Lewis symbol for a fluorine atom.
6,1
What is the mass in grams of 9.76 × 1012 atoms of naturally occurring potassium?
6.34 x 10^-10
The value of ΔH° for the reaction below is +128.1 kJ:CH3OH (l) → CO (g) + 2H2 (g)How many kJ of heat are consumed when 15.5 g of CH3OH (l) decomposes as shown in the equation?
62.0 kJ
What is the formula weight of magnesium fluoride?
62.3
Calculate the percentage by mass of lead in lead(II) nitrate.
62.6
An atom of 118Xe contains ________ neutrons.
64
How many grams of calcium cyanide (Ca(CN)2) are contained in 0.69 mol of calcium cyanide?
64
The value of ΔH° for the reaction below is -6535 kJ. ________ kJ of heat are released in the combustion of 16.0 g of C6H6 (l)?2C6H6 (l) + 15O2 (g) → 12CO2 (g) + 6H2O (l)
669
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?
7.859 × 10-1 g/mL
How much heat is released when 29.5 grams of Cl2 (g) reacts with excess hydrogen? H2 (g) + Cl2 (g) → 2HCl (g)ΔH° = -186 kJ.
77.4 kJ
An atom of the most common isotope of gold, 197Au, has ________ protons, ________ neutrons, and ________ electrons.
79, 118, 79
The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 10.0 g of Na2O2 with water is ________ kJ.2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)
8.08
The ΔE of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is ________ J.
8.2
Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:CaO (s) + H2O (l) → Ca(OH)2 (s)In a particular experiment, a 2.00-g sample of CaO is reacted with excess water and 2.14 g of Ca(OH)2 is recovered. What is the percent yield in this experiment?
81.1
Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:N2 (g) + 3H2 (g) → 2NH3 (g)Determine the mass of N2 (g) required to completely react with 18.5 g of H2.
85.7
Which group in the periodic table contains only nonmetals?
8A
Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:2Mg (s) + O2 (g) → 2MgO (s)When 5.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.
9.12
The number with the most significant zeros is ________.
90.300
Which of the following is an isoelectronic series? A. O2-, F-, Ne, Na+ B. B5-, Si4-, As3-, Te2- C. Si2-, P2-, S2-, Cl2- D. S, Cl, Ar, K E. F-, Cl-, Br-, I-
A. O2-, F-, Ne, Na+
Which one of the following is not an intensive property? A. mass B. boiling point C. density D. melting point E. temperature
A. mass
Which of the following species does the noble gas electron configuration [Kr]4d10 represent?
Ag+
When aqueous solutions of AgNO3 and KI are mixed, silver iodide precipitates. The balanced net ionic equation is ________.
Ag+ (aq) + I- (aq) → AgI (s)
The formula for aluminum hydroxide is ________.
Al(OH)3
Predict the empirical formula of the ionic compound that forms from aluminum and oxygen.
Al2O3
[Ar]4s23d104p3 is the electron configuration of a(n) ________ atom.
As
Which one of the following is not one of the postulates of Dalton's atomic theory?
Atoms are composed of protons, neutrons, and electrons.
Which species is oxidized in the reaction below?Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l) H+ N+5 O2- H2O Au
Au
Of the following, ________ is the largest mass. A. 2.5 × 1015 pg B. 25 kg C. 2.5 × 1010 ng D. 2.5 × 109 fg E. 2.5 × 10-2 mg
B. 25kg
Of the molecules below, the bond in ________ is the most polar. A. HBr B. HF C. HI D. HCl E. H2
B. HF
Which of the following statements is false? A. Any irreversible process results in an overall increase in entropy. B. The change in entropy in a system depends on the initial and final states of the system and the path taken from one state to the other. C. The total entropy of the universe increases in any spontaneous process. D. Entropy increases with the number of microstates of the system.
B. The change in entropy in a system depends on the initial and final states of the system and the path taken from one state to the other.
Of the following species, ________ will have bond angles of 120°.
BCl3
ΔS is positive for the reaction ________. A. 2NO2 (g) → N2O4 (g) B. 2Hg (l) + O2 (g) → 2HgO (s) C. 2H2 (g) + O2 (g) → 2H2O (g) D. BaF2 (s) → Ba2+ (aq) + 2F- (aq) E. CO2 (g) → CO2 (s)
BaF2 (s) → Ba2+ (aq) + 2F- (aq)
The element that has a valence configuration of 2s2 is ________.
Be
The reason Bromine is more likely to exist as an anion than is potassium is because ________.
Bromine has a greater electron affinity than potassium does
The ________ ion has a noble gas electron configuration. A. O- B. F C. Cl- D. F2- E. S2+
C. Cl-
Which of the following is insoluble in water ? A. Na2S B. (NH4)2CO3 C. Mg3(PO4)2 D. Ba(C2H3O2)2 E. Ca(OH)2
C. Mg3(PO4)2
Of the following molecules, only ________ is polar. A. CCl4 B. BeCl2 C. NCl3 D. Cl2 E. BCl3
C. NCl3
Which of the following Lewis structures would be an expansion to the octet rule? A. CF4 B. NF3 C. PO43- D. CCl4 E. SiF4
C. PO43-
A compound contains 40.0 grams of carbon, 6.71 grams of hydrogen, and 53.29 grams of oxygen. The molecular weight of the compound is 60.05 amu. The molecular formula of this compound is ________.
C2H4O2
Which one of the following molecular formulas is also an empirical formula?
C2H6SO
What is the empirical formula of a compound that is 66.6% C, 11.2% H, and 22.2% O by mass?
C4H8O
Which reaction produces an increase in the entropy of the system? A. CO2 (s) → CO2 (g) B. H2O (l) → H2O (s) C. N2 (g) + 3 H2 (g) → 2 NH3 (g) D. H2 (g) + Cl2 (g) → 2 HCl (g) E. Ag+ (aq) + Cl- (aq) → AgCl (s)
CO2 (s) → CO2 (g)
The formula of the carbonate ion is ________.
CO32-
The balanced net ionic equation for the precipitation of calcium carbonate when aqueous solutions of Na2CO3 and CaCl2 are mixed is ________.
Ca+(aq) + CO32- (aq) → CaCO3 (s)
Elements in Group 6A are known as the ________.
Chalcogens
The ________ ion is represented by the electron configuration [Ar]3d2.
Cr4+
The formula of the chromate ion is ________.
CrO42-
Which of the following elements has a ground-state electron configuration different from the predicted one?
Cu
Which of the following is an oxidation-reduction reaction?
Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq)
Which one of the following compounds is copper(I) chloride?
CuCL
Which one of the following is an incorrect subshell notation? A. 3s B. 3d C. 2p D. 2d E. 4f
D. 2d
The most electronegative atom of the ones listed below is ________. A. Ga B. In C. Al D. B E. Tl
D. B
Of the following species, ________ will have bond angles of 120°. A. NCl3 B. PH3 C. ClF3 D. BCl3 E. All of these will have bond angles of 120°.
D. BCl3
Which of the following does not have eight valence electrons? A. Rb+ B. Cl- C. Xe D. Sr+ E. Ti+4
D. Sr+
A typical triple bond ________.
D. consists of one σ bond and two π bonds
Which of the following is not a valid set of four quantum numbers? (n, l, ml, ms) A. 2, 0, 0, +1/2 B. 2, 1, 0, -1/2 C. 1, 0, 0, +1/2 D. 3, 1, -1, -1/2 E. 1, 1, 0, +1/2
E. 1, 1, 0, +1/2
With which of the following will the ammonium ion form an insoluble salt? A. carbonate B. sulfate C. chloride D. sulfate and carbonate E. none of the above
E. none of the above
In the molecule below, which atom has the largest partial negative charge? Cl ∣ F— C —Br ∣ I
F
Which one of the following compounds is soluble in water? A. CuS B. ZnS C. AgCl D. Mg(OH)2 E. Fe(NO3)3
Fe(NO3)3
The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is ________.
H+ (aq) + OH- (aq) → H2O (l)
In which of the molecules below is the carbon-carbon distance the shortest?
H-C≡C-H
The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is ________.
H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq)
What is the formula for perchloric acid?
HClO4
________ is credited with developing the concept of atomic numbers.
Henry Moseley
Which metal is a liquid at room temperature? Please type in the correct elemental symbol only.
Hg
The shape of an orbital is defined by the angular momentum quantum number which is represented as letter
I
Which element is solid at room temperature?
I2
Which of the following has the largest entropy at 25°C and atm?
I2
The SI unit of temperature is ________.
K
Which calculation clearly shows a conversion between temperatures in degrees Celsius, °C, and temperature in Kelvins, K?
K = °C + 273.15
Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr?
K > Ca > Ge > As > Kr
What are the spectator ions in the reaction between KCl (aq) and AgNO3 (aq)?
K+ and NO3-
In which species does sulfur have the highest oxidation number?
K2SO4
Which combination will produce a precipitate?
KOH (aq) and Mg(NO3)2 (aq)
The ion with the smallest diameter is ________.
Li+
Which of the following compounds would you expect to be ionic?
LiBr
Predict the empirical formula of the ionic compound that forms from magnesium and fluorine.
MgF2
Predict the empirical formula of the ionic compound that forms from magnesium and oxygen.
MgO
The charge on an electron was determined in the ________.
Millikan oil drop experiment
The ground-state electron configuration of the element ________ is [Kr]5s14d5.
Mo
The correct formula for molybdenum (IV) hypochlorite is ________.
Mo(CIO)4
Of the bonds below, ________ is the least polar. A. S-O B. C-O C. C-F D. K-Br E. N-O
N-O
In which species does nitrogen have an oxidation number of zero?
N2
What are the spectator ions in the reaction between sodium hydroxide and nitric acid?
Na+ and NO3-
Predict the empirical formula of the ionic compound that forms from sodium and fluorine.
NaF
Rank the following in terms of decreasing first ionization energies?
Ne > N > O > Be > B
When aqueous solutions of ________ are mixed, a precipitate forms.
NiBr2 and AgNO3
Which of the following correctly represents the first ionization of oxygen?
O (g) → O+ (g) + e-
Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?
O, S
In which set of elements would all members be expected to have very similar chemical properties?
O, S, Se
The central atom in ________ violates the octet rule. A. FCN B. SF2 C. PF5 D. Br2CO E. Cl2
PF5
No two electrons within the same orbtial can have the same set of quantum numbers. This statement describes ________.
Pauli's exclusion principle
________ and ________ reside in the atomic nucleus.
Protons, neutrons
The element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an electrical semiconductor is ________.
Si
Which of the following does not have eight valence electrons?
Si+
Of the molecules below, only ________ is polar. A. PF5 B. CO2 C. H2 D. CH4 E. SnF3
SnF3
Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2?
That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom.
Which one of the following compounds is insoluble in water?
ZnS
Elements in Group 1A are known as the ________.
alkali metals
The element lithium is in a group known as the ________.
alkali metals
The name of the ionic compound (NH4)3PO4 is ________.
ammonium phosphate
Elements in the modern version of the periodic table are arranged in order of increasing ________.
atomic number
The molecular geometry of the SF2 molecule is ________.
bent
What is the molecular shape of H2O?
bent
The element that corresponds to the electron configuration 1s22s22p2 is ________.
carbon
The correct name for H2CO3 is ________.
carbonic acid
Which one of the following will occur as diatomic molecules in elemental form?
chlorine
The law of constant composition applies to ________.
compounds
An element that appears in the lower left corner of the periodic table is ________.
definitely a metal
The correct name for N2O5 is ________.
dinitrogen pentoxide
The name of the binary compound N2O4 is ________.
dinitrogen tetroxide
Of the following, the smallest and lightest subatomic particle is the ________.
electron
In the Bohr model of the atom, ________.
electron energies are quantized
The point in a titration at which the indicator changes is called the ________. Select one:
end point
The reaction 4Al (s) + 3O2 (g) → 2 Al2O3 (s)ΔH° = -3351 kJ is ________, and therefore heat is ________ by the reaction.
exothermic, released
Which one of the following processes produces a decrease in the entropy of the system?
freezing of Fe(l) into Fe(s)
Elements in Group 7A are known as the ________.
halogens
A combination of sand, salt, and water is an example of a ________.
heterogeneous mixture
________ is a unique element and does not truly belong to any family.
hydrogen
The effective nuclear charge of an atom is primarily affected by ________.
inner electrons
Iron and chlorine form an ionic compound whose formula is FeCl3. The name of this compound is ________.
iron (III) chloride
An element in the upper right corner of the periodic table ________.
is definitely a nonmetal
The uncertainty principle states that ________.
it is impossible to know the exact position and momentum of an electron
The molecular geometry of the CS2 molecule is ________.
linear
The molecular geometry of the BeCl2 molecule is ________, and this molecule is ________.
linear, nonpolar
The correct name for MgF2 is ________.
magnesium fluoride
Which one of the following is not an intensive property? A. temperature B. mass C. density D. boiling point E. melting point
mass
According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the ________ of an electron.
momentum
Which of the quantum number(s) below represent the principal quantum number?
n only
Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a one-electron system (such as hydrogen)?
n only
The correct name for HNO3 is ________.
nitric acid
In the periodic table, the elements are arranged in ________.
order of increasing atomic number
The name of PCl3 is ________.
phosphorus trichloride
A ________ ΔH corresponds to an ________ process.
positive, endothermic
The correct name for K2S is ________.
potassium sulfide
All of the orbitals in a given electron shell have the same value as the ________ quantum number.
principal
Oxidation cannot occur without __________.
reduction
The correct name of the compound Na3N is ________.
sodium nitride
Homogeneous mixtures are also known as ________.
solutions
The hybrid orbital set used by the central atom in SO3 is ________.
sp2
The hybridizations of nitrogen in NF3 and NH3 are ________ and ________, respectively.
sp3, sp3
The molecular geometry of the IF5 molecule is ________, and this molecule is ________.
square pyramidal, polar
[Kr]5s2 is the electron configuration for
strontium
The correct name for SO is ________.
sulfur monoxide
The correct name for H2SO3 is ________.
sulfurous acid
Of the following, only ________ is a chemical reaction.
tarnishing of silver
Using the VSEPR model, the electron-domain geometry of the central atom in ClO3- is ________.
tetrahedral
The photoelectric effect is ________.
the ejection of electrons by a metal when struck with light of sufficient energy
An empirical formula always indicates ________.
the simplest whole-number ratio of different atoms in a compound
Cathode rays are deflected away from a negatively charged plate because ________.
they are negatively charged particles
The molecular geometry of the BrO3- ion is ________.
trigonal pyramidal
The molecular geometry of the H3O+ ion is ________.
trigonal pyramidal
The molecular geometry of the PF3 molecule is ________, and this molecule is ________.
trigonal pyramidal, polar
Of the following, only ________ is an extensive property.
volume
Of the bonds C-C, C═C, and C≡C, the C-C bond is ________.
weakest/longest
The first law of thermodynamics can be given as ________.
ΔE = q + w