CHMY121 Final Exam

How many centimeters are there in one kilometer?

10^5 cm

The reaction N2 + 3 H2 → 2 NH3 is used to produce ammonia. When 450. g of hydrogen was reacted with nitrogen, 1575 g of ammonia were produced. What is the percent yield of this reaction? A) 62.1% B) 41.5% C) 30.8% D) 20.7% E) More information is needed to solve this problem.

A) 62.1%

What is the pH of a solution in which [H3O+] = 3.8 × 10-8 M? A) 7.42 B) 6.58 C) 3.80 D) 1.0 × 10-8 E) 2.6 × 10-7

A) 7.42

Find the difference between two masses measured as 123.6 grams and 115.972 grams. Express the answer to the correct number of significant figures. A) 7.6 grams B) 7.63 grams C) 7.628 grams D) 8.0 grams E) 8 grams

A) 7.6 grams

The formula for carbon disulfide is A) CS2. B) C2S. C) CSi2. D) CaS2. E) (CS)2

A) CS2

Which compound produces an acidic solution when dissolved in water? A) NH4Cl B) NaF C) K2SO4 D) KCl E) Ca(NO3)2

A) NH4Cl

What is the conjugate base of HSO4-? A) SO42- B) H2SO4 C) H3O+ D) OHE) H2SO3

A) SO4^2-

Which of the following contains kinetic energy? A) bicycle at the top of a hill B) ball laying on the ground C) a moving car D) a battery E) a piece of chocolate

A) a moving car

In general, the solubility of ________ in water decreases as temperature increases. A) gases B) solids C) liquids D) none of these E) all of these

A) gases

The formula Ca(NO3)2 tells us that one formula unit of this compound is composed of ________ calcium atoms, ________ nitrogen atoms, and ________ oxygen atoms. A) one; two; six B) two; two; six C) one; two; five D) one; one; five E) one; one; six

A) one; two; six

In a neutral atom the number of ________ is equal to the number of ________. A) protons; electrons B) protons; neutrons C) neutrons; electrons D) protons + electrons; neutrons E) none of the above

A) protons; electrons

For the following reaction, increasing the pressure will cause the equilibrium to 2 SO2(g) + O2(g) ⇄ 2 SO3(g) + heat A) shift to the right, towards products. B) shift to the left, towards reactants. C) remain unchanged, but the reaction mixture will get warmer. D) remain unchanged, but the reaction mixture will get cooler. E) Pressure has no effect on equilibrium.

A) shift to the right, towards products.

Consider the following four liquids: water: highly polar; H-bonding hexanol: slightly polar; some H-bonding chloroform: slightly polar; no H-bonding octane: non-polar; no H-bonding Which pair of liquids is immiscible? A) water and octane B) water and hexanol C) hexanol and chloroform D) chloroform and octane E) none of the above

A) water and octane

Which of the statements regarding the symbol ΔG is false? A) It refers to the free energy of the reaction. B) Alone, allows us to predict the spontaneity of a reaction. C) Alone, allows us to identify an exothermic reaction. D) Alone, allows us to identify an endergonic reaction. E) It describes the effect of both enthalpy and entropy on a reaction.

Alone, allows us to identify an exothermic reaction

A balloon originally had a volume of 4.39 L at 44°C and a pressure of 729 torr. To what temperature must the balloon be cooled to reduce its volume to 3.78 L if the pressure is constant? A) 38°C B) 0.0°C C) 72.9 °C D) 273°C E) 237°C

B) 0.0°C

Which of the following pH's corresponds to a strongly acidic solution? A) 5.3 B) 1.4 C) 7.8 D) 9.2 E) 11.5

B) 1.4

What is the electron configuration of Mg? A) 1s2 2s2 2p8 B) 1s2 2s2 2p6 3s2 C) 1s2 2s2 2p6 3s1 3p3 D) 1s2 2s2 2p6 3s2 3p6 4s2 3d5 E) none of the above

B) 1s2 2s2 2p6 3s2

Which reaction is not an example of a redox reaction? A) 2 Hg(l) + O2(g) → 2 HgO(s) B) 2 (NH4)3PO4(aq) + 3 Ba(NO3)2(aq) → Ba3(PO4)2(s) + 6 NH4NO3(aq) C) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) D) 6 HCl(aq) + 2 Al(s) → 2 AlCl3(aq) + 3 H2(g) E) 2 Al2O3(s) → 4 Al(s) + 3 O(g)

B) 2 (NH4)3PO4(aq) + 3 Ba(NO3)2(aq) → Ba3(PO4)2(s) + 6 NH4NO3(aq)

How many molecules are present in 4.25 mol of CCl4? A) 9.26 × 1024 molecules B) 2.56 × 1024 molecules C) 653.69 molecules D) 153.81 molecules E) 3.69 × 10-23 molecules

B) 2.56 × 1024 molecules

The solubility of nitrogen in water exposed to the atmosphere, where the partial pressure of nitrogen is 593 mm, is 5.3×10-4 M. At the same temperature, what would be the solubility of pure nitrogen, at a pressure of 760 mm? Henry's Law: A) 4.1 × 10-4 M B) 6.8 × 10-4 M C) 1500 M D) 2400 M E) none of the above

B) 6.8 × 10-4 M

What is the pressure in a 1.00 liter container of methane, CH4, that contains 40.0 g of the gas at 25.0°C? A) 5.13 atm B) 61.0 atm C) 82.1 atm D) 979 atm E) 3920 atm

B) 61.0 atm

What is the pressure in mmHg if the weatherman says the current pressure today is 0.989 atm? A) 75.2 mmHg B) 752 mmHg C) 117 mmHg D) 945 mmHg E) 760 mmHg

B) 752 mmHg

Consider the reaction shown: N2 + O2 → 2 NO ΔH = 43.2 kcal When 50.0 g of N2 react, ________ kcal will be ________. A) 43.2; produced B) 77.1; consumed C) 77.1; produced D) 2160; consumed E) 2160; produced

B) 77.1; consumed

Which of the following is a weak acid? A) HNO3 B) H3PO4 C) NH3 D) HCl E) OH

B) H3PO4

Which of the following cannot have hydrogen bonds? A) H2O B) HCl C) HF D) CH3NH2 E) NH3

B) HCl

Which of the following contains potential energy? A) a person riding a bicycle B) a book on top of a table C) a bouncing ball D) a kid jumping rope E) a dog chasing a car

B) a book on top of a table

At a high altitude, water boils at 95°C instead of 100°C as at sea level because the A) atmospheric pressure is greater. B) atmospheric pressure is less. C) climate is cooler. D) vapor pressure of water is greater. E) vapor pressure of water is less

B) atmospheric pressure is less

Elements in the Periodic Table are arranged according to A) alphabetical order. B) atomic number. C) atomic weight. D) date of discovery. E) number of neutrons

B) atomic number

Identify the product(s) in the following reaction: calcium carbonate → calcium oxide + carbon dioxide A) calcium carbonate B) calcium oxide + carbon dioxide C) calcium carbonate + calcium oxide D) carbon dioxide + calcium carbonate E) calcium carbonate + calcium oxide + carbon dioxide

B) calcium oxide + carbon dioxide

A positively charged particle formed by loss of one or more electrons from an atom is called a(an) A) anion. B) cation. C) isotope. D) nucleus. E) proton.

B) cation

In a typical oxidation-reduction reaction, the electrons are transferred A) from the oxidizing agent to the reducing agent. B) from what is being oxidized to the substance being reduced. C) from what is being reduced to the substance being oxidized. D) from what is being oxidized to the reducing agent. E) none of these.

B) from what is being oxidized to the substance being reduced

When an atom donates an electron, that electron A) is lost for all time. B) is acquired by another atom which becomes an anion. C) is acquired by another atom which becomes a cation. D) neutralizes a proton to form a neutron. E) pairs with another electron to form a covalent bond.

B) is acquired by another atom which becomes an anion.

Which element is most likely to be "X" in the diatomic molecule shown? (two elements with a double bond with 8 outer electrons) A) nitrogen B) oxygen C) fluorine D) hydrogen E) helium

B) oxygen

) Which of the following is a physical change? A) the rusting of iron B) the condensation of water vapor C) the baking of a potato D) the explosion of nitroglycerin E) all of the above

B) the condensation of water vapor

All of the statements about molarity are correct except A) the abbreviation is M. B) the interpretation of the symbol is "moles of solute per mole of solvent." C) moles = molarity × volume. D) volume = moles/molarity. E) the molarity of a diluted solution is less than the molarity of the original solution

B) the interpretation of the symbol is "moles of solute per mole of solvent."

Acid rain forms in the upper atmosphere by the reaction of sulfur trioxide with water forming sulfuric acid. Calculate the mass in grams of 5.65 × 1021 molecules of SO3. A) 2.72 × 1047 g B) 1.17 × 10-4 g C) 0.751 g D) 0.0751 g E) 1.17 g

C) 0.751 g

At 25°C, the value of Kw is A) 1.00. B) 1.00 × 10-7. C) 1.00 × 10-14. D) 1.00 × 107. E) 1.00 × 1014.

C) 1.00 × 10-14

What is the molarity of a solution prepared by dissolving 0.750 mol CaCl2 in enough water to make 0.500 L of solution? A) 0.375 M B) 0.667 M C) 1.50 M D) 83.2 M E) 166.5 M

C) 1.50 M

How much Ca(NO3)2 should be weighed out to have 0.650 mol? A) 66.4 g B) 97.6 g C) 107 g D) 133 g E) 165 g

C) 107 g

The molecular weight of PCl3 is ________ amu. A) 66.42 B) 136.00 C) 137.33 D) 139.00 E) 199.26

C) 137.33

How many grams of NaOH are needed to make 750 mL of a 2.5% (m/v) solution? A) 3.9 g B) 7.5 g C) 19 g D) 20 g E) 50 g

C) 19 g

An atom with Z = 26 and A = 58 contains ________ protons and ________ neutrons. A) 26; 58 B) 58; 26 C) 26; 32 D) 32; 26 E) 26; 84

C) 26; 32

When the reaction shown is correctly balanced, the coefficients are: ________ KClO3 → ________ KCl + ________ O2 A) 1; 1; 1 B) 2; 2; 2 C) 2; 2; 3 D) 2; 2; 1 E) 4; 4; 6

C) 2; 2; 3

Which of the following numbers contains five significant figures? A) 0.04910 B) 0.4910 C) 4.9100 D) 49,100 E) 4,910,000

C) 4.9100

A mixture of the gases N2, O2, and He has a total pressure of 760 mm Hg. If the partial pressure of N2 is 90 mm Hg and of O2 is 270 mm Hg, what is the partial pressure of He? A) 1120 mm Hg B) 760 mm Hg C) 400 mm Hg D) 360 mm Hg E) 120 mm Hg

C) 400 mm Hg

. The combustion of propane gas (C3H8) is used to fuel barbeque grills. To produce 5.65 moles of water, how many moles of oxygen gas are needed? C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) A) 3.39 mol B) 4.52 mol C) 7.06 mol D) 1.13 mol E) 1.41 mol

C) 7.06 mol

How many electrons can occupy the shell having n = 2? A) 2 B) 6 C) 8 D) 18 E) 32

C) 8

Arrange the following molecules in order of increasing intermolecular forces: CH3OH, H2, CCl4, HBr A) CH3OH < H2 < HBr < CCl4 B) H2 < HBr < CCl4 < CH3OH C) H2 < CCl4 < HBr < CH3OH D) CH3OH < HBr < CCl4 < H2 E) H2 < CCl4 < CH3OH < HBr

C) H2 < CCl4 < HBr < CH3OH

Consider the 2 reaction profiles below. A B Reaction B is ________, and it occurs ________ reaction A. A) endergonic; faster than B) exergonic; faster than C) endergonic; slower than D) exergonic; slower than E) exergonic; at the same rate as

C) endergonic; slower than

A process or reaction which releases heat to the surroundings is said to be... A) conservative. B) endothermic. C) exothermic. D) isothermal. E) exergonic.

C) exothermic.

Vegetable oil is a(an) ________, and is found in the ________ phase. A) element; liquid B) compound; solid C) mixture; liquid D) compound; gas E) mixture; solid

C) mixture; liquid

Which group contains only elements which normally exist as diatomic molecules? A) nitrogen; sulfur, bromine B) helium; neon, argon C) nitrogen; oxygen, fluorine D) hydrogen; lithium, sodium E) oxygen; phosphorus, germanium

C) nitrogen; oxygen, fluorine

In the process of dissolving sugar in water, the entropy increases. This means that the sign of ΔS is ________, and that the randomness of the system ________. A) undetermined; increases B) positive; decreases C) positive; increases D) negative; decreases E) negative; increases

C) positive; increases

Making bonds ____________ and breaking bonds ________. A) absorbs energy; absorbs energy B) releases energy; releases energy C) releases energy; absorbs energy D) absorbs energy; releases energy E) requires no energy; requires energy

C) releases energy; absorbs energy

A chemical bond formed when two atoms share one pair of electrons is a ________ bond; it is best described as ________. A) double; covalent B) double; ionic C) single; covalent D) single; ionic E) triple; covalent

C) single; covalent

Although noble gases do not normally form covalent compounds, a sample of XeO3 has been prepared. The systematic name of this compound is A) trioxy xenon. B) trixenon trioxide. C) xenon trioxide. D) xenon(III) oxide. E) none of the above

C) xenon trioxide

Which has the highest boiling point? A) 0.1 M NH4NO3 B) 0.1 M CaF2 C) 0.1 M H2Se D) 0.1 M Na3PO4 E) pure water

D) 0.1 M Na3PO4

What is the osmolarity of a 0.20 M solution of Ba(OH)2? A) 0.10 Osmol B) 0.20 Osmol C) 0.40 Osmol D) 0.60 Osmol E) 0.80 Osmol

D) 0.60 Osmol

How many grams of fluorine are required to produce 20.0 grams of FeF3 from the reaction shown? 2 Fe + 3F2 → 2 FeF3 A) 4.49 g B) 5.05 g C) 6.74 g D) 10.1 g E) 20.2 g

D) 10.1 g

An imaginary element Xq consists of two isotopes having masses of 100.0 amu and 102.0 amu. A sample of Xq was found to contain 20.0% of the 100Xq isotope and 80.0% of the 102Xq. Calculate the atomic weight of Xq. A) 100.2 amu B) 100.4 amu C) 101.0 amu D) 101.6 amu E) 202.0 amu

D) 101.6 amu

How many mL of 0.100 M NaOH are needed to neutralize 24.0 mL of 0.150 M HCl? A) 12.0 mL B) 18.0 mL C) 24.0 mL D) 36.0 mL E) 48.0 mL

D) 36.0 mL

If the concentration of OH- in an aqueous solution is 1.4 × 10-7 M, the concentration of H3O+ is A) 7.1 × 10+6 M. B) 1.0 × 10-7 M. C) 1.4 × 10-7 M. D) 7.1 × 10-8 M. E) 1.3 × 10-8 M.

D) 7.1 × 10-8 M

Which of the following is an example of an ionic solid? A) Au(s) B) H2O(s) C) C(s) D) CaCl2(s) E) PCl5(s)

D) CaCl2(s)

Which symbol does not denote a compound?

D) Cr

. In the reaction shown, ________ is the oxidizing agent because it ________. Ni(s) + CuCl2(aq) → Cu(s) + NiCl2(aq) A) Ni; causes reduction B) Ni; gets reduced C) CuCl2; causes reduction D) CuCl2; gets reduced E) NiCl2; gets reduced

D) CuCl2; gets reduced

The combination of ions most likely to produce a precipitate is A) Li+ and PO43-. B) Pb2+ and NO3-. C) NH4+ and SO42-. D) Fe3+ and OH-. E) Mg2+ and C2H3O2-.

D) Fe3+ and OH-

Which reaction is an example of a precipitation reaction? A) H2CO3(aq) → H2O(l) + CO2(g) B) H2SO4(aq) + Ca(OH)2(aq) → CaSO4(aq) + 2 H2O(l) C) 6 HCl(aq) + 2 Al(s) → 2 AlCl3(aq) + 3 H2(g) D) FeCl3(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCl(aq) E) 2 Hg(l) + O2(g) → 2 HgO(s)

D) FeCl3(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCl(aq)

Which one of the following weak acids is the strongest? A) HCN (Ka = 4.9 × 10-10) B) HClO (Ka = 3.0 × 10-8) C) HNO2 (Ka = 4.5 × 10-4) D) HF (Ka = 6.8 × 10-4) E) Acid strength cannot be determined from the given information.

D) HF (Ka = 6.8 × 10-4)

The formula for ammonium hydroxide is A) OHNH4. B) NH4NO3. C) NH4O. D) NH4OH. E) Al(OH)3.

D) NH4OH

What is the formula of the nitrate ion? A) NO3 2- B) NO3- C) NO2 - D) NO3 - E) none of the above

D) NO3 -

Which of the following elements is a noble gas? A) Cl B) H C) N D) Ne E) O

D) Ne

Which statement about this system is not true? 2 SO2 (g) + O2 (g) ⇄ 2 SO3 (g) + heat K = 4.8 × 1027 A) At equilibrium, SO3 is the predominant substance. B) Heating the system will cause a decrease in the amount of SO3. C) Adding SO2 will cause an increase in the amount of SO3. D) Removing O2 will cause an increase in the amount of SO3. E) The large value of K means that the reaction essentially goes to completion.

D) Removing O2 will cause an increase in the amount of SO3.

Which of the following ions does not have the same electron configuration as the noble gas neon? A) O2- B) FC) Al3+ D) S2- E) Mg2+

D) S^2-

What is the correct Ka expression for the reaction below? CH3COOH(aq) + H2O(l) ⇄ CH3COO-(aq) + H3O+(aq) A) [CH3COOH][H2O] [CH3COO−][H3O+] B) [CH3COOH] [CH3COO−][H3O+] C) [CH3COO−][H3O+] [CH3COOH][H2O] D) [CH3COO−][H3O+] [CH3COOH] E) [CH3COO−] [CH3COOH]

D) [CH3COO−][H3O+] /[CH3COOH]

A Brønsted-Lowry base is a substance which A) produces hydrogen ions in aqueous solution. B) produces hydroxide ions in aqueous solution. C) donates protons to other substances. D) accepts protons from other substances. E) accepts hydronium ions from other substances

D) accepts protons from other substances

All of these statements regarding the symbol "ΔH" are correct except it A) represents the difference between the energy used in breaking bonds and the energy released in forming bonds in a chemical reaction. B) can be called heat of reaction. C) can be called enthalpy change. D) can be called entropy change. E) has a negative value for an exothermic reaction.

D) can be called entropy change

Consider the reaction shown: C3H8 + 5 O2 → 3 CO2 + 4 H2O + 488 kcal We can say that this reaction is ________ and that the sign of ΔH is ________. A) endothermic; positive B) exothermic; positive C) endothermic; negative D) exothermic; negative E) exothermic; neither positive nor negative

D) exothermic; negative

The amount of energy involved in melting a substance without changing its temperature is called the A) heat of vaporization. B) calorie. C) joule. D) heat of fusion. E) heat of combustion.

D) heat of fusion

The smallest possible unit of a covalent compound is a(an) A) atom. B) cation. C) formula unit. D) molecule. E) polyatomic ion

D) molecule

Consider a bent molecule, such as H2Se, in which the central atom has two lone pairs of electrons. The electronegativities of H and Se are 2.1 and 2.4, respectively. Based on these values and on consideration of molecular geometry, the H-Se bond can be considered almost ________ and the molecule is ________

D) nonpolar; polar

A reaction that is spontaneous can be described as A) proceeding in both the forward and reverse directions. B) having the same rate in both the forward and reverse directions. C) releasing heat to the surroundings. D) proceeding without external influence once it has begun. E) increasing in disorder

D) proceeding without external influence once it has begun

All of the following statements describing solutions are true except A) making a solution involves a physical change. B) solutions are homogeneous. C) the particles in a solution are atomic or molecular in size. D) solutions are colorless. E) solutions are transparent

D) solutions are colorless.

The name of S2- is A) sulfur. B) sulfate ion. C) sulfite ion. D) sulfide ion. E) sulfurous ion.

D) sulfide ion.

Which description best fits a gas? A) definite shape and volume; strong intermolecular attractions B) definite volume; shape of container; moderate intermolecular attractions C) definite volume; shape of container; weak intermolecular attractions D) volume and shape of container; no intermolecular attractions E) volume and shape of container; strong intermolecular attractions

D) volume and shape of container; no intermolecular attractions

Consider the balanced equation shown and identify the statement that is not true. Na2SO4(aq) + BaCl2(aq) → 2 NaCl(aq) + BaSO4(s) A) The coefficient of sodium sulfate is one. B) Barium sulfate is produced in solid form. C) Barium chloride is dissolved in water. D) The products are barium sulfate and sodium chloride. E) 2 NaCl (aq) could also be correctly written as Na2Cl2 (aq)

E) 2 NaCl (aq) could also be correctly written as Na2Cl2 (aq)

A 50.0 mL sample of a 12.0 M solution of HCl is diluted to 250. mL. What is the new concentration? A) 60.0 M B) 12.0 M C) 10.4 M D) 3.00 M E) 2.40 M

E) 2.40 M

A sample of gas has a volume of 135 mL at 0.600 atm. What would be the volume if the pressure is decreased to 0.200 atm while temperature is held constant? A) 45.0 mL B) 101 mL C) 135 mL D) 180 mL E) 405 mL

E) 405 mL

Which measurement represents the largest quantity? A) 4730 ng B) 4.73 × 10-4 g C) 4.73 × 103 μg D) 4.73 × 10-6 kg E) 47.3 mg

E) 47.3 mg

How many mL of 0.105 M AgNO3 are needed for an experiment that requires 0.00510 mol of AgNO3? A) 0.536 mL B) 17.8 mL C) 18.70 mL D) 20.6 mL E) 48.6 mL

E) 48.6 mL

What does the balanced equation given below mean? CH4 + 2 O2 → CO2 + 2H2O A) One mole of methane reacts with two moles of oxygen to produce one mole of carbon dioxide and two moles of water. B) One gram of methane reacts with two grams of oxygen to produce one gram of carbon dioxide and two grams of water. C) One molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide and two molecules of water. D) A, B, and C are correct. E) A and C are correct.

E) A and C are correct.

Which group of elements contains only non-metals? A) Mg, Ca, Sr B) V, Cr, Mn C) Cl, Ar, K D) P, As, Se E) C, S, I

E) C, S, I

What is the typical net ionic equation for an acid-base neutralization of KOH and HCl? A) HCl(aq) + KOH(aq) → H2O(l) + KCl(aq) B) KOH(aq) → K+(aq) + OH-(aq) C) H2O(l) → H+(aq) + OH-(aq) D) K+(aq) + OH-(aq) → KOH(aq) E) H+(aq) + OH-(aq) → H2O(l)

E) H+(aq) + OH-(aq) → H2O(l)

Based on the bond energies given for each of the following, which is the most stable bond? A) O=O 498 kJ/mol B) C=O 745 kJ/mol C) C=C 614 kJ/mol D) C≡C 839 kJ/mol E) N≡N 946 kJ/mol

E) N≡N 946 kJ/mol

. Consider the reaction: A + 2 B ⇄ 2 C + D The equilibrium expression for this reaction is: A) [A]^2[B] 2[C][D] B) 2[C][D] [A]2[B] C) [A][B] 2 [C]2[D] D) [A]2[B] 2 2[C]2[D] E) [C]2[D] [A][B]2

E) [C]^2[D] [A][B]^2

Water can be used to dissolve which type of compounds? A) nonpolar compounds B) polar compounds C) ionic compounds D) both A and B E) both B and C

E) both B and C

Activation energy can best be described as the A) energy level of the products. B) maximum energy level of the reaction. C) energy level of the reactants. D) difference in energy between reactants and products. E) difference in energy between reactants and the maximum energy

E) difference in energy between reactants and the maximum energy

When acids and bases react the product other than water is a A) hydrogen ion. B) hydroxide ion. C) hydronium ion. D) metal. E) salt.

E) salt

When a reaction system is at equilibrium A) there is no more chemistry happening. B) the amounts of reactants and products are exactly equal. C) the reaction rate in the forward direction is at a maximum. D) the reaction rate in the reverse direction is at a minimum. E) the rates of the reaction in the forward and reverse directions are exactly equal.

E) the rates of the reaction in the forward and reverse directions are exactly equal.

What is the molecular geometry of NH3? A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal

E) trigonal pyramidal

Which of the following is a correct dot structure for an element in Group 6A?

S with 6 electrons in its lewis structure