CHE 140 Clicker Questions

The vapor pressure of a solution is an A.) extensive property B.) intensive property

A.) extensive property

Which electron transition in the hydrogen atom results in the emission of light of the longest wavelength? A.) n=4 to n=3 B.) n=1 to n=2 C.) n=1 to n=6 D.) n=3 to n=2

A.) n=4 to n=3

In CO2, chemical bonding is best described in terms of A.) one sigma, and three pi bonds B.) two sigma and two pi bonds C.) three sigma and one pi bond D.) four sigma bonds

A.) one sigma, and three pi bonds

Suppose you put helium-filled balloon in the trunk of your car on a hot day. What would happen to the balloon? A.) the balloon would expand B.) the balloon would shrink C.) nothing

A.) the balloon would expand

Which substance would have the highest vapor pressure A.) H3CCH2-O-CH2CH3 B.) H3CCH2CH2CH2-OH C.) H3CCH2CH2CH2-NH2 D.) HO-CH2CH2CH2-OH

A.)H3CCH2-O-CH2CH3

Which of the following hybridizations is incorrect? A.) SN 2= sp2 B.) SN 6= sp3d2 C.) SN 4= sp3 D.) SN 5= sp3d

A.) SN 2= sp2

Neon has a boiling point of 27K. Express this temperature in F

-411 F

If 30.34 ml of a .135 M solution of HCl were required to neutralize 25.00 ml of a NaOH solution, what is the molarity of the sodium hydroxide solution

.164

Calculate the moles of gas contained in a 4.0L container at STP

.18

How many moles are present in 58.4 of chalk (CaCO3)

.583 mol

Which of these regions of the electromagnetic spectrum has the shortest wavelength? A.) gamma rays B.) infrared C.) ultraviolet D.) visible

A.) Gamma Rays

Which of the following is not a strong acid: A.) HF B.) HCl C.) HBr D.) HI

A.) HF

Identify the most polar covalent bond? A.) N-H B.) O-H C.) H-F D.) C-F

A.) N-H

Round the answer for the mathematical operation below to the appropriate number of significant figures (1.23g-.567g)/.34442cm^3

1.92g/cm^3

Identify the atom with electron configuration: [Ar] 4s2, 3d2: A.) Ti B.) V C.) Y D.) Ca E.) S

A.) Ti

What is the frequency of yellow-orange light (589 nm)

5.09 x10^-14 s^-1

Calculate the energy of one photon of light with a wavelength fo 250 nm?

7.9 x10^-19 J

Calculate the pressure of 1.2 mol of methane gas in a 3.3 L container at 298 K

8.9 atm

How many grams are present in 3.40 moles in Nitrogen gas

95.3 g

Use molecular orbital theory to select the correct statement A.) O2- has a longer bond length than O2+ B.) O2- is an unstable species C.) O2 has a bond order of 2.5 D.) O2 is a diamagnetic molecule

A.) O2- has a longer bond length than O2+

What is the total concentration of ions in .10 M iron (III) solution? A.) .5 M B.) .1 M C.) .2 M D.) .4 M E.) .3 M

A.) .5 M

A 4.67 g Hershey's Kiss is combusted in a bomb calorimeter. If the combustion releases 20 Cal, how much will the temperature (in K) of the 10 L water bath rise A.) 2 B.) 4 C.) 14 D.) 2000 E.) 8368

A.) 2

What is the sum of the coefficients in the balances equation using the smallest integer coefficients for the reaction? B2O3 + NaOH --> Na3BO3 + H20 A.) 9 B.) 10 C.) 12 D.) 15

A.) 9

200 ml of .1 M NH4CL is being poured into 100 ml of .1 M AgNO3. What is the limiting reagent A.) AgNO3 B.) NH4Cl C.) AgCl D.) NH4NO3

A.) AgNO3

Predict the formula for the binary ionic compound formed by Al and O2 A.) Al2O3 B.) Al3O2 C.) Al2O D.) AlO2

A.) Al2O3

Which of the following represents melting on the heating curve?

B

How many double bonds are there in the hydrazine (N2H4) molecule A.) 0 B.) 1 C.) 2 D.) 3

B.) 1

The best Lewis structure of HCN (Carbon is the central atom) has A.) 1 nonbonding pair on carbon B.) 1 nonbonding pair on nitrogen C.) 2 nonbonding pair on carbon D.) 2 nonbonding pair on nitrogen

B.) 1 nonbonding pair of nitrogen

How much hydrogen gas (in grams) is produced from the decomposition of 1 mol of water? A.) 1.008 g B.) 2.016 g C.) 16.00 g D.) 32.00 g

B.) 2.016g

Which of these is a redox reaction A.) 2NaOH + H2SO4 --> Na2SO4 B.) 2AgNO3 + Cu--> Cu(NO3)2 +2Ag C.) Pb(NO3)2 + 2KI--> PbI2 + 2KNO3 D.) CaCO3 + 2HCl--> CaCl2 +CO2+ H20

B.) 2AgNO3 + Cu--> Cu(NO3)2 +2Ag

How much energy is required to heat 155 g of water (18.02 g/mol from 25.0 to 75.0 C; cp for H2O= 75.3 J/(molxC) A.)584 kJ B.) 32.4 kJ C) 434 J D.) 175 J

B.) 32.4 kJ

How many valence electrons does P have A.) 3 B.) 5 C.) 8 D.) 15

B.) 5

What is the percent of C in C10H16 A.) 78.48 B.) 88.16 C.) 66.84 D.) 92.41

B.) 88.16

Identify the weakest covalent bond A.) C-O B.) C-C

B.) C-C

Which salt exhibits the greatest ion-ion interactions A.) MgO B.) MgS C.) NaF D.) Nacl

B.) MgS

Which of the following has ∆H°ƒ=0 A.) N2 (l) B.) N2 (g) C.) H2O (l) D.) H2O (s) E.) H2O (g)

B.) N2 (g)

Select the correct statement pertaining to the properties of liquids A.) the meniscus is mercury in convex because the adhesive forces are stronger than the cohesive forces B.) Viscosity of a pure liquid decreases with increasing temperature C.) the surface tension of water is greater than that of mercury D.) water rises up a glass capillary tube because the cohesive forces are stronger than the adhesive forces

B.) Viscosity of a pure liquid decreases with increasing temperature

For which process is ∆H >0 A.) Propane gas combusting B.) Water boiling C.) Drops of candle wax harden D.) water freezing

B.) Water boiling

Which type of visible emission spectrum would you expect to get from a group of excited hydrogen atoms? A.) continuous B.) line

B.) line

Select the greater of each of the following pairs of IE A.) the 1st IE of Mg B) the 1st IE of Si

B.) the 1st IE of Si

what would happen to the gas if the temperature of the container were significantly decreased? A.) the average velocity would be faster and the distribution of velocities would be narrower B.) the average velocity would be slower and the distribution would be narrower C.)the average velocity would be faster and the distribution would be wider D.) the average velocity would be slower and the distribution would be wider

B.) the average velocity would be slower and the distribution would be narrower

The van't Hoff factor for an aqueous solution of an ionic compound is 2. Which of the following is not a possible explanation? A.) the solute is a 1:1 salt behaving ideally B.) the solute is a non-electrolyte C.) the solute is a 2:1 salt behaving non-ideally

B.) the solute is a non-electrolyte

Mercury is the liquid of choice in a barometer. At sea level, 1 atm=76 cm Hg; the density of Hg is 13.5 g/ml. How would the height of a water column at sea level compare with the height of a Hg column A.) both columns would have the same height B.) the water column would be higher C.) the water column would be shorter

B.) the water column would be higher

what happens to the number of moles of C12h22O11 (sucrose) when a .20 M soultion is diluted to a final concentration of .10 M A.) decreases B.) increases C.) nothing changes D.) not enough info

C.)

How many moles of ions are present in exactly 150 mL of a .260M ammonium phosphate solution, (NH4)3 PO4? A.) 1.04 mol B.) .156 mol C.) .0390 mol D.) .117 mol E.) .312 mol

C.) .156 mol

Which of the following is the correct form of a Standard Formation Reaction? A.) NH3 + Cl2 --> NH2Cl + HCl B.) HC2H3O2 + H2O --> H3O + C2H3O2 C.) .5N2 + 1.5 H2 --> NH3 D.) 2Na + Cl2 --> 2NaCl

C.) .5N2 + 1.5 H2 --> NH3

A 155.3 g sample of pond water is found to have .17 mg of nitrite. What is the concentration of nitrate in ppm? A.) 1.1 x10^-3 ppm B.) 914 ppm C.) 1.1 ppm D.) .91 ppm

C.) 1.1 ppm

For the n=4 level or shell: What is the total number of orbitals? A.) 4 B.) 9 C.) 16 D.) 32

C.) 16

Considering each atomic orbital can hold 2 electrons, what is the maximum number of electrons that can have a principle quantum number n=4 A.) 8 B.) 16 C.) 32 D.) 64

C.) 32

How many bonding electrons are in the C2 molecule? A.) 2 B.) 4 C.) 6 D.) 8

C.) 6

Which of the following does not represent an electrically neutral compound A.) NaCl B.) CaO C.) CH4 D.) TiO2 E.) AgBr

C.) CH4

Which element has the highest number of unpaired electrons? A.) Ca B.) Co C.) Cr D.) Cu

C.) Cr

Which of the following is an endothermic process? A.)Propane gas combusting B.) Water condensing on a bottle C.) ice cream melting D.) water freezing

C.) Ice cream melting

Predict the identity of the precipitate formed when solutions of Na2CO3 and MgCl2 are mixed? A.) Na2CO3 B.) MgCl2 C.) MgCO3 D.) NaCl

C.) MgCO3

Using VSEPR theory, predict the shape of IF4+ A.) Tetrahedral B.) Square planar C.) See Saw D.) Octahedral

C.) See Saw

If you have two nails. one clean and one rusty, which nail has more iron A.) Rusty Nail B.) Clean Nail C.) The nails have the same amount of iron

C.) They have the same amount of iron

Which molecule is polar and contains polar bonds A.) CO2 B.) Oxygen C.) Water D.) Ozone

C.) Water

Which of the following combinations of quantum numbers is not allowed? A.) n=1, l=0, ml= 0 B.) n=3, l=0, ml=0 C.) n=1, l=0, ml=-1 D.) n=2, l=1, ml=-1 E.) n=3, l=2, ml=1

C.) n=1, l=0, ml=-1

Which of these is correct set of quantum numbers to describe a 5d orbital A.) n=5, l=4, ml= +3 B.) n=5, l=3, ml= +2 C.) n=5, l= 2, ml=+1 D.) n=5, l=1 , ml=0

C.) n=5, l= 2, ml=+1

Which designation best describes the hybrid orbitals on the central atom in SF4? A.) sp2 B.) sp3 C.) sp3d D.) sp3d2

C.) sp3d

A balloon is inflated in a pressurized chamber and then tied off. What happens when the chamber pressure is increased A.) the pressure inside the balloon decreases B.) the balloon does not change C.) the balloon volume shrinks D.) the molecules in the balloon collide less often

C.) the balloon volume shrinks

Suppose you put a helium tank of your car on a hot day, what would happen to the tank A.) the tank would shrink B.) the pressure of the helium inside the tank would go down C.) the pressure inside the tank would increase D.) the tank would expand

C.) the pressure inside the tank would increase

Combustion analysis of an unknown compound indicated that is 92.23% C and 7.82% H. If the molar mass is 78 g/mol, what is the molecular formula?

C6H6

What is/are spectator ions in the reaction below: HBr + KOH --> H2O + KBr

K and Br

For thousands of years the mineral chalcocite has been highly prized source of copper. It's chemical composition is 79.85% Cu and 20.15% S. What is the empirical formula?

Cu2S

What is the oxidation number of phosphorous in the phosphate ion? A.) -5 B.) -3 C.) +3 D.) +5

D.) +5

Which of the following would have the lowest boiling point? A.) 10 m B.) 1 m C.) 5 m D.) .5 m

D.) .5 m

Select the correct relationship between the metric units of length or distance A.) 1km=100 m B.) 1mm=10cm C.) 1nm=10^9 m D.) 10^6 um= 1 m

D.) 10^6 um= 1m

What is the total number of atoms in 1 mole of aluminum iodide A.) 2 B.) 2x6.022 x10^23 C.) 3x 6.022x10^23 D.) 4x 6.022x10^23

D.) 4x 6.022x10^23

Predict the molecular geo and bond angle of the sulfur dichloride, SCl2, molecule A.) Linear B.) Trigonal planar C.) Trigonal pyramidal D.) Bent

D.) Bent

Using solubility rules select the compound that is least soluble in water? A.) Pb(NO3)2 B.) (NH4)2CO3 C.) K2SO4 D.)Ca3(PO4)2

D.) Ca3(PO4)2

Predict which liquid will have the strongest intermolecular forces of attraction A.) CH3COCH2CH2CH3 B.) CH3CH2CH2CH2CH2OH C.) CH3CH2CH2 H2 H3 D.) HOH2C-CH=CH-CH2OH

D.) HOH2C-CH=CH-CH2OH

Which of these is an exception to the octet rule? A.) NF3 B.) H3O + C.) PCl3 D.) IF4+

D.) IF4+

Which of the following is the strongest intermolecular force? A.) Dipole-dipole B.) dispersion forces C.) hydrogen bonding D.) Ion-Ion E.) Hydrogen bonding

D.) Ion-Ion

Which is of the given electronic configuration is incorrect? A.) As [Ar] 3d10,4s2,4p3 B.) Sc 1s2,2s2,2p6,3s2,3p6,4s2,3d1 C.) Os [Xe] 4f14, 5d6, 6s2 D.) K 1s2, 2s2, 2p6, 3s1

D.) K 1s2, 2s2, 2p6, 3s1

Which pair of ions has the largest Eel? A.) Na+ and O2- B.) Na+ and Cl- C.) Mg2+ and Cl- D.) Mg2+ and O2-

D.) Mg2+ and O2-

Which of the following is a weak electrolyte: A.) HCl B.) NaOH C.) NaCl D.) NH3

D.) NH3

If equal amounts of moles of oxygen and glucose are combusted, what will be the limiting reagent A.) H2O B.) C6H12O6 C.) CO2 D.) O2

D.) O2

Since only a small fraction of alpha particles were reflected back toward the source, what can we learn about the atom? A.) the atom is a homogenous mix of positive and negative charge B.) the atom only contains neutrons C.) The atom has electrons D.) Only a small region of the atom has a positive charge

D.) Only a small region of the atom has a positive charge

Which gas has the highest density A.) CO2 B.) SO2 C.) CH4 D.) SF6 E.) He

D.) SF6

Select the electron configuration of Cu+ A.) [Ar] 3d10, 4s1 B.) [Ar] 3d9, 4s2 C.) [Ar] 3d9, 4s1 D.) [Ar] 3d10

D.) [Ar] 3d10

n-Butane (C4H9) has a higher boiling point temperature than ethane (C2H6) mainly due to A.) stronger hydrogen bonding interactions B.) lower molecular mass C.) stronger covalent bonds D.) a greater degree of induced-dipole forces

D.) a greater degree of induced-dipole forces

For the n=4 level or shell: What are the letter designations of all the sub-shells A.) s B.) p C.) d D.) f

D.) f

A 19.5 g piece of titanium (cp= .523 J/(gxC) is heated and then submurged in 1.50 x10^2 grams of water (cp= 4.18 J/(gxC) initially at 22.7 C. The final temperature comes to 23.7 C. What is the initial temperature of the Ti metal? A.) 24.7 C B.) 32.2 C C.) 46.4 C D.) 61.5 C E.) 85.2 C

E.) 85.2 C

Which metal will undergo the smallest temperature change is an equal amount of heat is added to a 1.0 gram? A.) Fe, c= .473 J/gxK B.) Cu, c=.387 J/gxK C.) Au, c=.129 J/gxK D.) Zn, c=.389 J/gxK E.) Al, c= .904 J/gxK

E.) Al, c= .904 J/gxK

Which of the following compounds would you expect to have the smallest lattice energy A.) CaBr2 B.) MgBr2 C.) CaO D.) BaO E.) BaBr2

E.) BaBr2

Which would you expect to have the highest viscosity A.) C8H18 B.) C12H36 C.) C5H12 D.) C17H36 E.) C22H46

E.) C22H46

Which gas has the highest average speed at a given temperature A.) CO2 B.) SO2 C.) CH4 D.) SF6 E.) He

E.) He

Which of these are chemical properties of matter I. Corrosiveness II. Density III. Flammability IV. Melting Point

I and III

Which of the following pairs of molecules are miscible? I.) H2O and HOCH2 H2OH II.) CH3CH2CH2CH2CH2CH3 and CCl4 III.) CH3CN and CH2Cl2 IV.) H20 and CH3CH2OCH2CH3

I, II and III

Which pure substance will not form hydrogen bonds I.) CH3CH2OH II.) CH3OCH3 III.) H3C-NH-CH3 IV.) CH3F

II and IV

Identify a Bronsted-Lowry acid. NaHSO4 + NaOH --> Na2SO4 + H2O

NaHSO4

If work is done by surroundings on the system, the sign of the value for the work will be

Positive

Which compound would you expect to distill first from a mixture of acetone and dimethyl ether

dimethyl ether

When ozone molecules absorb UV light from the sun, the ozone breaks down into oxygen molecules and oxygen atoms. Does bond breaking occur when energy is absorbed or released?

absorbed

Is density and intensive or extensive property

intensive

The beaker contains a solution of sodium sulfate. Is sodium sulfate a covalent compound, an ionic, or a molecular compound

ionic compound

What are the units of molality?

moles of solute/kg of solvent