chem final

Question 1 0 / 3 pts A small amount of sugar dissolved in water is an example of a ________. solid Correct Answer homogeneous mixture compound You Answered heterogeneous mixture pure substance Question 2 3 / 3 pts An element cannot ________. interact with other elements to form compounds Correct! be separated into other substances by chemical means be a pure substance be part of a heterogeneous mixture be part of a homogeneous mixture Question 3 3 / 3 pts The correct answer (reported to the proper number of significant figures) to the following is ________. Correct! 17.37 17.40 17.0 17.367 17.4 Question 4 3 / 3 pts Which one of the following has the element name and symbol correctly matched? None of the symbols are correctly matched to the element name. Ni, nitrogen Correct! Zn, Zinc Si, sulfur P, potassium Question 5 1 / 1 pts The number 0.0100 has ________ significant figures. 5 4 2 Correct! 3 6 Question 6 0 / 3 pts Round the number 0.00641 to two significant figures. 0.0063700 Correct Answer 0.0064 You Answered 0.0 0.006 0.00637 Question 7 3 / 3 pts All atoms of a given element have the same ________. Correct! number of protons number of electrons and neutrons number of neutrons density mass Question 8 3 / 3 pts There are ________ electrons, ________ protons, and ________ neutrons in an atom of Xe. 78, 78, 132 54, 54, 132 132, 132, 54 78, 78, 54 Correct! 54, 54, 78 Question 9 0 / 3 pts In the symbol below, X = ________. N not enough information to determine You Answered Al Correct Answer C K Question 10 0 / 3 pts Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? Ar, Br Correct Answer Mg, Ca You Answered Br, Kr C,O H, Li Question 11 3 / 3 pts The elements in groups 2A, 7A, and 8A are called ________, respectively. Correct! alkaline earth metals, halogens, and noble gases alkaline earth metals, transition metals, and halogens alkaline earth metals, halogens, and chalcogens alkali metals, halogens, and noble gases halogens, transition metals, and alkali metals Question 12 0 / 3 pts Of the choices below, which one is not an ionic compound? CuCl2 KCl You Answered CrCl3 Correct Answer P2O5 RbBr Question 13 3 / 3 pts An empirical formula always indicates ________. which atoms are attached to which in a molecule how many of each atom are in a molecule the isotope of each element in a compound the geometry of a molecule Correct! the simplest whole-number ratio of different atoms in a compound Question 14 0 / 3 pts Which pair of elements is most apt to form an ionic compound with each other? oxygen, sulfur sulfur, fluorine Correct Answer iron, bromine chromium, sodium You Answered nitrogen, oxygen Question 15 0 / 3 pts Which pair of elements is most apt to form a molecular compound with each other? barium, bromine aluminum, oxygen Correct Answer sulfur, fluorine You Answered magnesium, iodine potassium, lithium Question 16 3 / 3 pts Which of the following would be considered matter? sound music Correct! books thoughts light Question 17 3 / 3 pts The suffix -ide is used primarily ________. for the name of the first element in a molecular compound for polyatomic cation names for monoatomic cations to indicate binary acids Correct! for monatomic anion names Question 18 3 / 3 pts A correct name for Li2S is ________. Lithium sulfite Lithium surfur Lithium sulfate sulfide lithium Correct! Lithium sulfide Question 19 1 / 1 pts Which of the following is a metal? sulfate ammonia Correct! magnesium helium Bromine Question 20 3 / 3 pts The formula for the compound formed between aluminum ions (NH4+) and phosphate ions (PO43-) is ________. AlP Al3(PO4)3 Correct! AlPO4 Al(PO4)3 Al2(PO4)3 Question 21 3 / 3 pts Oxygen is a ________ and nitrogen is a ________. Correct! nonmetal, nonmetal nonmetal, metal metalloid, metalloid metal, metalloid nonmetal, metalloid Question 22 3 / 3 pts ________ typically form ions with a 2+ charge. Chalcogens Halogens Alkali metals Transition metals Correct! Alkaline earth metals Question 23 3 / 3 pts Predict the empirical formula of the ionic compound that forms from magnesium and oxygen. MgO2 Correct! MgO Mg2O2 Mg2O Mg3O2 Question 24 3 / 3 pts The correct name for CCl4 is ________. Correct! carbon tetrachloride carbon tetrachlorate carbon chloride carbon chlorate carbon perchlorate Question 25 1 / 1 pts The formula of the carbonate ion is ________. CO2- CO22- Correct! CO32- CO33- CO- Question 26 3 / 3 pts The name of the binary compound N2O4 is ________. nitrogen oxide Correct! dinitrogen tetroxide nitrous oxide oxygen nitride nitrogen (IV) oxide Question 27 3 / 3 pts Predict the product formed when Ca2+ combines with PO43- Ca2(PO4)3 Correct! Ca3(PO4)2 CaPO4 (PO4)3Ca2 (PO4)2Ca3 Question 28 3 / 3 pts Which formula could be that of an alkane? C4H8 Correct! C4H10 C3H6 C3H4 C2H8 Question 29 2 / 8 pts The mass of a flask is 38.1346 g empty and 63.1769 g when filled with water (dH2O= 1.000 g/mL). When the flask is filled with an unknown liquid, its mass is 75.5778 g. Determine the density of the unknown liquid, in g/mL. (d = m/v) (please show your work, otherwise NO credit!) Your Answer: 63.1769-38.1346=25.0423 75.5778-38.1346=37.4432 Step 1: mwater = m(flask+water) - mflask = 63.1769 g - 38.1346 g = 25.0423 g Step 2: Vwater = mwater/dwater=25.0423 g/(1.000 g/mL)=25.0423 mL Step 3: Vunknown liquid = Vwater = 25.0423 mL Step 4: dunknown liquid = munknown liquid /Vunknown liquid = 75.5778 g/ (25.0423 mL) = 3.018 g/mL Question 30 3 / 7 pts The density of Cu is 8.96 g/cm3. The density of Cu is ________ kg/m3. (1 kg= 1000 g; 1 m = 100 cm) (please show your work, otherwise NO credit!) Your Answer: 8.96/1000=0.00896 8.96/100=0.0896 LaTeX: \frac{8.96g}{cm^3}=\:\frac{8.96g}{cm\:\times cm\times cm}\times\frac{1\:kg}{1000\:g}\times\frac{100\:cm}{1\:m}\times\frac{100\:cm}{1\:m}\times\frac{100\:cm}{1m}=8.96\times10^3\frac{\:kg}{m^3} Question 31 0 / 7 pts The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. What is the average atomic mass of the element in amu? (please show your work, otherwise NO CREDIT!) Isotope Abundance (%) Mass (amu) 221X 55.700 220.90 220X 38.800 220.00 218X 5.500 218.10 Your Answer: 220.90+220.00+218.10=659 659/3=219.66 220.90 amu x 55.700% + 220.00amu x 38.800% + 218.10amu x 5.500% = 220.40 amu

exam 1

Question 1 0 / 3 pts When the following equation is balanced, the coefficients are ________. 2, 3, 4, 4 You Answered 2, 12, 8, 9 Correct Answer 2, 25, 16, 18 1, 4, 8, 9 4, 4, 32, 36 Question 2 3 / 3 pts The formula of nitrobenzene is C6H5NO2. The molar mass of this compound is ________ g/mol 43.03 107.11 3.06 Correct! 123.11 109.10 Question 3 3 / 3 pts The mass % of H in methane (CH4) is ________. 74.87 92.26 4.032 7.743 Correct! 25.13 Question 4 0 / 3 pts When the following equation is balanced, the coefficient of O2 is ________. C2H4O (g) + O2 (g) CO2 (g) + H2O (g) You Answered 3 1 Correct Answer 5 2 4 Question 5 3 / 3 pts There are ________ mol of carbon atoms in 4 mol of C4H8O2. 8 4 32 20 Correct! 16 Question 6 3 / 3 pts How many moles of carbon dioxide are there in 52.06 g of carbon dioxide? 6.022 × 1023 0.8452 8.648 × 1023 Correct! 1.183 3.134 × 1025 Question 7 0 / 3 pts Of the species below, only ________ is not an electrolyte. NaCl KOH You Answered HCl Correct Answer Ar Rb2SO4 Question 8 0 / 3 pts Which combination will produce a precipitate? NaC2H3O2 (aq) and HCl (aq) NaF (aq) and HCl (aq) You Answered NaOH (aq) and HCl (aq) AgNO3(aq) and Ca(NO3)2 (aq) Correct Answer KOH (aq) and Mg(NO3)2 (aq) Question 9 3 / 3 pts In which reaction does the oxidation number of hydrogen change? SO2 (g) + H2O (l) H2SO3 (aq) HCl (aq) + KOH (aq) KCl (aq) + H2O (l) Correct! 2K (s) + 2H2O (l) 2KOH (aq) + H2 (g) MgO (s) + H2O (l) Mg(OH)2 (s) 2HClO4 (aq) + CaCO3 (s) Ca(ClO4)2 (aq) + H2O (l) + CO2 (g) Question 10 3 / 3 pts Oxidation is the ________ and reduction is the ________. gain of electrons, loss of electrons Correct! loss of electrons, gain of electrons loss of oxygen, gain of electrons gain of oxygen, loss of electrons gain of oxygen, loss of mass Question 11 0 / 3 pts Which one of the following is a correct expression for molarity? You Answered mol solute/L solvent Correct Answer mol solute/L solution mol solute/L solution mol solute/kg solvent mol solute/mL solvent Question 12 3 / 3 pts The point in a titration at which the indicator changes is called the ________. volumetric point indicator point Correct! end point standard point setpoint Question 13 0 / 3 pts A strong electrolyte is one that ________ completely in solution. Correct Answer ionizes reacts associates You Answered disappears Question 14 3 / 3 pts Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ions are spectator ions in the reaction? Ba2+ only Ba2+ and SO42- Na+ only SO42- and I- Correct! Na+ and I- Question 15 3 / 3 pts How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2? (M=n/V) 0.160 Correct! 0.0800 0.0400 2.00 0.500 Question 16 8 / 8 pts What is the empirical formula of a compound that contains 27.3% C, and 72.7% O by mass? (Please show your work, otherwise no partial credit!) Your Answer: CO2 LaTeX: 27.3\:g\:C\times\frac{1\:mol\:C}{12.011\:g\:C}=2.27\:mol\:C LaTeX: 72.7\:g\:O\times\frac{1\:mol\:O}{15.9994\:g\:O}\:=4.54\:mol\:O LaTeX: C_{2.27}O_{4.54}=C_{\frac{2.27}{2.27}}O_{\frac{4.54}{2.27}}=CO_2 Question 17 0 / 5 pts What is the concentration (M) of 39.88 mL of an unknown NaOH solution if it required of to neutralize? \left(M_{NaOH}\times V_{NaOH}=M_{HCl}\times V_{HCl}\right) ( M N a O H × V N a O H = M H C l × V H C l ) (Please show your work, otherwise no partial credit!) Your Answer: M_{NaOH}V_{NaOH}=M_{HCl}V_{HCl} M_{NaOH}=\frac{M_{HCl}V_{HCl}}{V_{NaOH}}=\frac{0.6592\:M\times46.08\:mL}{39.88\:mL}=0.7617M Question 18 0 / 7 pts How many grams of NaOH (MW = 40.0) are there in 200.0 mL of a 0.175 M NaOH solution? (n=MV n = M V , 1L = 1000 mL) (Please show your work, otherwise no partial credit!) Your Answer: \frac{0.175mol}{L}\times200.0\:mL\times\frac{1L}{1000\:mL}\times\frac{40.0\:g}{1\:mol}=1.4\:g Question 19 2 / 2 pts To balance a chemical equation, one makes sure that the same types and numbers of atoms exist on each side of the arrow. Correct! True False Question 20 0 / 2 pts In oxidation-reduction reactions, one process gains electrons while the other accepts electrons. You Answered True Correct Answer False Question 21 0 / 3 pts The solvent in an aqueous solution is ________. H+ You Answered HCl Correct Answer water NaOH OH- Question 22 3 / 3 pts In which species does chlorine have an oxidation number of zero? NaClO3 Correct! Cl2 NaCl HClO4 HCl Question 23 2 / 2 pts one mole of O2 gas has the same mass as one mole of N2 gas. True Correct! False Question 24 0 / 5 pts Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3 (s) 2Na (s) + 3N2 (g) How many moles of N2 are produced by the decomposition of 1.60 mol of sodium azide? (Please show your work, otherwise no partial credit!) Your Answer: 10.0 g N2 X (1 mol N2/28.0 g N2) = 0.357 mol N2 X (2 mol NaN3 / 3 mol N2) = 0.238 mol NaN3 0.238 mol NaN3 X (65.0 g NaN3 / 1 mol NaN3) = 15.5 g NaN3 13.0 ft^3 X (28.3 L / 1 ft^3) = 368 L N2 X (1.25 g N2/L) = 460 g N2 / 28.0 g/mol = 16.4 moles N2 16.4 mol N2 X (2 mol NaN3 / 3 mol N2) = 10.9 mol NaN3 X 65.0 g/mol = 712 g NaN3 1.60mol\:NaN_3\times\frac{3\:mol\:N_2}{2\:mol\:NaN_3}=2.4mol\:N_2 Where did you get 10 g of nitrogen gas?? Question 25 3 / 3 pts What is the oxidation number of nitrogen in N2O? 2 Correct! +1 4 0 3 Question 26 0 / 3 pts Which one of the following substances is produced during the reaction of an acid with a metal hydroxide? H2 NaOH You Answered CO2 O2 Correct Answer H2O Question 27 0 / 3 pts The empirical formula of the reduced form of lactobionic acid, a sugar used in some medicial agents, is CH2O. the molecular mass of this compound is 180. What is the molecular formula? CH2O C4H8O4 C5H10O5 Correct Answer C6H12O6 You Answered C3H6O3 Question 28 3 / 3 pts The limiting reactant is the reactant present in smallest volume the reactant that limits the speed with which the reaction occurs the reactant present in fewest moles Correct! the reactant that is completely consumed in the reaction the reactant present in fewest grams Question 29 3 / 3 pts When it is balanced, what is the value of coefficient of Al in the equation shown below? 1 You Answered 2 6 3 Correct Answer 4 Question 30 3 / 3 pts Which one of the following could be an empirical formula? C2H4O2 C3H6 N2O4 Correct! C6H5Br C6H3F3

exam 2

One significant difference between gases and liquids is that ________. a gas may consist of both elements and compounds All of these answers are correct. gases are always mixtures Correct! a gas expands to fill its container a gas is made up of molecules Question 2 3 / 3 pts Of the following, ________ is a correct statement of Boyle's law. Correct! PV = constant Question 3 0 / 3 pts Of the following, only ________ is impossible for an ideal gas. Correct Answer V1T1 = V2T2 You Answered Question 4 3 / 3 pts The molar volume of a gas at STP is ________ L. 1.00 14.7 Correct! 22.4 0.08206 62.36 Question 5 3 / 3 pts Standard temperature and pressure (STP), in the context of gases, refers to ________. 298.15 K and 1 atm 298.15 K and 1 torr 273.15 K and 1 pascal 273.15 K and 1 torr Correct! 273.15 K and 1 atm Question 6 3 / 3 pts A pressure of 0.500 atm is the same as a pressure of ________ of mm Hg. (1 atm = 760 mmHg) 760. 33.0 193 Correct! 380. 29.9 Question 7 3 / 3 pts A system absorbs a given quantity of heat and does a given quantity of work on surroundings. Which of the following choices correctly indicates the signs for q and w? -q, -w -q, w none of above q, w Correct! q, -w Question 8 3 / 3 pts The density of nitric oxide (NO) gas at 0.970 atm and 308.05 K is ________ g/L. LaTeX: \left(d=\frac{pM}{RT};\:R=0.082058\:atm\cdot L\cdot K^{-1}\cdot mol^{-1}\right) ( d = p M R T ; R = 0.082058 a t m ⋅ L ⋅ K − 1 ⋅ m o l − 1 ) 10.2 0.869 0.339 Correct! 1.15 0.0384 Question 9 3 / 3 pts The density of F2 is __________ at STP. 0.85 Correct Answer 1.07 1.18 You Answered None of the above 0.59 Question 10 3 / 3 pts Which of the following best describes a closed can of soda? an isolated system none of above an open system system at thermal equilibrium Correct! a closed system Question 11 3 / 3 pts The enthalpy change for the following reaction is -483.6 kJ: 2H2 (g) + O2 (g) 2H2O (g) Therefore, the enthalpy change for the following reaction is ________ kJ. 4H2 (g) + 2O2 (g) 4H2O (g) Correct! -967.2 2.34 × 105 -483.6 483.6 967.2 Question 12 3 / 3 pts Which one of the following conditions would always result in a decrease in the internal energy of a system? None of the above is correct Correct! The system loses heat and does work on the surroundings. The system loses heat and has work done on it by the surroundings. The system gains heat and has work done on it by the surroundings. The system gains heat and does work on the surroundings. Question 13 0 / 3 pts The value of H° for the reaction below is -186 kJ. H2 (g) + Cl2 (g) 2HCl (g) The reaction is ____________, and therefore heat is ___________ by the reaction exothermic, absorbed endothermic, absorbed Correct Answer exothermic, released thermoneutral, neither released nor absorbed You Answered endothermic, released Question 14 1 / 3 pts The value of E for a system that performs 139 kJ of work on its surroundings and gains of heat is \left(\Delta E=q+w\right) ( Δ E = q + w ) 85 Correct Answer -85 7506 -193 You Answered 193 the work w has negative sign! Question 15 0 / 3 pts The value of H° 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) -72 0.44 Correct Answer 198 You Answered 72 144 Question 16 3 / 3 pts Equal moles of CO2, N2, O2 and He ideal gases are place into separate container with the same volume and at the same temperature. Which container has the highest pressure Correct! They would all exhibit the same pressure CO2 He N2 O2 Question 17 0 / 15 pts A gas mixture contains 1.5 mol CO2, 1.1 mol N2 and 1.8 mol Ar at 25.0 °C with total volume 1.6 L. (a) the molar fractions of the three gases. (b) the total gas pressure (c) their partial pressure Extra information: x_i=\frac{n_i}{n_{total}}; x i = n i n t o t a l ; PV=nRT; P V = n R T ; p_i=x_i\cdot p_{total} p i = x i ⋅ p t o t a l R=0.082058\:atm\cdot L\cdot K^{-1}mol^{-1} R = 0.082058 a t m ⋅ L ⋅ K − 1 m o l − 1 LaTeX: K=^\circ C+273.15 K = ∘ C + 273.15 Your Answer: LaTeX: \left(a\right)\:Since\:\:\:n_{CO_2}=1.5\:mol;\:n_{N_2}=1.1\:mol;\:n_{Ar}=1.8\:mol LaTeX: then\:n_{total}=n_{CO_2}+n_{N_2}+n_{Ar}=1.5\:mol\:+1.1\:mol\:+\:1.8\:mol\:=\:4.4\:mol LaTeX: \chi_{CO_2}=\frac{n_{CO_2}}{n_{total}}=\frac{1.5\:mol}{4.4\:mol}=0.35;\:\chi_{N_2}=\frac{n_{N_2}}{n_{total}}=\frac{1.1\:mol}{4.4\:mol}=0.25;\:\chi_{Ar}=\frac{n_{Ar}}{n_{total}}=\frac{1.8\:mol}{4.4\:mol}=0.41 LaTeX: \left(b\right)\:p_{total}=\frac{n_{total}RT}{V}=\frac{4.4\:mol\:\times0.082058\:atm\cdot L\cdot K^{-1}\cdot mol^{-1}.\left(273.15+25\right)K}{1.6\:L}=67.3\:atm LaTeX: \left(c\right)\:P_{CO_2}=\chi_{CO_2}\cdot P_{total}=0.35\:\times67.3\:atm=23.6\:atm;\:P_{N_2}=\chi_{N_2}\cdot P_{total}=0.25\:\times67.3\:atm=16.8\:atm;\:P_{Ar}=\chi_{Ar}\cdot p_{total}=0.41\times67.3\:atm\:=\:27.6\:atm Why did not answer this question! There is a similar question in the sample exam III Question 18 0 / 5 pts Consider the following two reactions: A → 2B ΔH°rxn = 456.7 kJ/mol A → C ΔH°rxn = -22.1 kJ/mol Determine the enthalpy change for the process: 2B → C Your Answer: (a) A → 2B ΔH°a = 456.7 kJ/mol (b) A → C ΔH°b = -22.1 kJ/mol Label the two reactions with known ΔH as (a) and (b), respectively. Since, the target reaction = (a) x(-1) + (b) then ΔHtarget reaction= ΔHa x (-1) + ΔHb =(-456.7 kJ/mol) +(22.1 kJ/mol) =-434.6 kJ Question 19 0 / 3 pts A closed system differs from an isolated system in that Correct Answer the closed system exchanges energy with its surroundings and the isolated system does not. the isolated system exchanges energy with its surroundings and the closed system does not. the closed system exchanges matter with its surroundings and the isolated system does not. the closed system exchanges both matter and energy with its surroundings and the isolated system does not. You Answered the closed system exchanges neither matter nor energy with the surroundings. Question 20 0 / 5 pts An 6.11 g sample of calcium carbonate [CaCO3 (s)] absorbs 84 J of heat, upon which the temperature of the sample increases from 19.2 °C to 35.9 °C. What is the specific heat of calcium carbonate? q = mass·specific heat·(Tf - Ti) Your Answer: LaTeX: specific\:heat=\frac{q}{mass\times\left(T_f-T_i\right)}=\frac{84\:J}{6.11\:g\:\times\left(35.9\:-19.2\right)^\circ C}=0.82J\cdot g^{-1}\cdot^{^\circ C} Question 21 3 / 3 pts A ________ ΔH corresponds to an ________ process positive, exothermic negative, endothermic Correct! positive, endothermic zero, exothermic zero, endothermic Question 22 3 / 3 pts When a system ________, ΔE is always negative. gives off heat and has work done on it None of the above is always negative. absorbs heat and has work done on it absorbs heat and does work Correct! gives off heat and does work Question 23 0 / 3 pts Which of the following pairs involve variables that are inversely proportional? Correct Answer p, V p, n You Answered p, T V, n V, T Question 24 3 / 3 pts How many grams of oxygen gas occupy 22.4 L at STP 16.0 22.4 8 Correct! 32.0 44.8 Question 25 3 / 3 pts Five 10.0 L containers each hold a different gas at STP. The container holding which gas would have the greatest mass, in gram? O2 Correct! Ar CO H2 H2 Question 26 3 / 3 pts Which of the following is an example of an object possessing kinetic energy? water at the top of a dam a boulder resting on a cliff Correct! a ball rolling downhill a stick of dynamite a bird perched in a tree Question 27 3 / 3 pts Which one of the following is an endothermic process? A. boiling soup Correct! Both A and C D. Hydrochloric acid and barium hydroxide are mixed at 25 °C: the temperature increases. C. ice melting B. water freezing Question 28 3 / 3 pts The internal energy of a system ________. is the sum of the kinetic energy of all of its components refers only to the energies of the nuclei of the atoms of the component molecules none of the above is the sum of the rotational, vibrational, and translational energies of all of its components Correct! is the sum of the potential and kinetic energies of the components

exam 3

Question 1 3 / 3 pts How many p orbitals are occupied in a nitrogen atom? 5 4 2 1 Correct! 3 Question 2 0 / 3 pts In which atom are the 2s and 2p orbitals equal in energy? You Answered C Correct Answer H He O none of these Question 3 3 / 3 pts Unpaired electrons in the same orbital have __________ spins. perpendicular Correct! parallel unordered elemental opposite Question 4 3 / 3 pts How many electrons are there in a half-filled p subshell? 6 8 2 Correct! 3 18 Question 5 0 / 3 pts How many electrons are there in a filled n = 2 principal shell? 32 6 Correct Answer 8 2 You Answered 18 Question 6 3 / 3 pts How many electrons are there in a filled 4f subshell? Correct! 14 18 10 2 6 Question 7 3 / 3 pts Which of the following orbital diagrams is not allowed? Correct! Question 8 3 / 3 pts How many electrons are there in the 3d orbitals of Ti? 0 5 10 Correct! 2 1 Question 9 0 / 3 pts What is the number of unpaired electrons in a silicon atom? Correct Answer 2 5 0 You Answered 4 6 Question 10 3 / 3 pts Which element would have the following electron configuration in the ground state? B Ga N Correct! Al P Question 11 3 / 3 pts Which of the following is the electron configuration of Ne? Correct! Question 12 3 / 3 pts The horizontal rows in the Periodic Table are called Correct! periods. groups. families. subshells. energy levels. Question 13 3 / 3 pts How many valence electrons are there in a N atom? 2 Correct! 5 4 3 6 Question 14 3 / 3 pts How many core electrons does an atom of Na have? 1 6 8 Correct! 10 2 Question 15 0 / 3 pts Which one of the following atoms has the largest radius? You Answered Cs Sn O Ca Correct Answer As Question 16 3 / 3 pts In which list are all of the elements in the same group? Ce, Pr, Nd N, O, F K, Ca, Sr Correct! F, Cl, Br Ba, La, Hf Question 17 3 / 3 pts Which set of elements is in an incorrect order of increasing first ionization energy (lowest value first, etc.)? Al, B, C Te, S, O Mg, Si, Cl Correct! Li, Na, K Question 18 3 / 3 pts Which of the following is a metalloid? C Correct! Si Ga Al Se Question 19 3 / 3 pts Which element belongs to the group called the alkali metals? Mg Cl Sc H Correct! Rb Question 20 3 / 3 pts Which of the following atoms is a metal? N Correct! Fe O Te Ne Question 21 3 / 3 pts Which of the following atoms is a non-metal? Cr Correct! N Hg Ge Al Question 22 3 / 3 pts Which of the following atoms is a noble gas? B Mg Fr Correct! Ne As Question 23 0 / 3 pts Which of the following is a p-block element? Correct Answer N Ca Ce You Answered Na Ni Question 24 3 / 3 pts Which of the following orbitals fills first? 4s More information is needed. 4d 3s Correct! 2s Question 25 3 / 3 pts The gound-state electron configuration of ________ is [Ar]4s13d5 Correct! Cr V Mn K Fe Question 26 3 / 3 pts Of the following elements, ________ has the most negative electron affinity. Correct! Cl I S Br Se Question 27 0 / 3 pts Which set of three quantum number (n, l, ml) corresponds to a 2s orbital? 2,0,1 Correct Answer 2, 0, 0 2,0,2 You Answered 2,1,1 2,1,0 Question 28 3 / 3 pts The only noble gas that does not have the ns2np6 valence electron configuration is _____ Correct! He Ne All noble gases have the ns2np6 valence electron configuration. Kr Ar Question 29 3 / 3 pts Nonmetals can be ________ at room temperature. solid only liquid or gas liquid only solid or liquid Correct! solid, liquid, or gas Question 30 0 / 3 pts Alkali metals tend to be more reactive than alkaline earth metals because ________. You Answered alkali metals have greater electron affinities alkali metals have lower densities alkali metals have lower melting points Correct Answer alkali metals have lower ionization energies Alkali metals are not more reactive than alkaline earth metals. Question 31 0 / 3 pts In a ground-state copper atom, the _________ subshell is partially filled. 2p 3s Correct Answer 4s You Answered 3d 3p Question 32 0 / 3 pts Which of the following atoms has 1 unpaired electron? C Correct Answer F You Answered Be O Fe Question 33 3 / 3 pts In which set of elements would all members be expected to have very similar chemical properties? Ne, Na, Mg Correct! O, S, Se S, Se, Si N, O, F Na, Mg, K Question 34 0 / 3 pts Which electron configuration represents a violation of the Pauli exclusion principle? You Answered Correct Answer Question 35 3 / 3 pts Which electron configuration represents a violation of Hund's rule for an atom in its ground state? Correct!

final