Chem Non Math Questions

Electrons in energy level number _____ have the least amount of energy.

1

Which of the following is not allowed in the quantum model of the atom? A) 4f B) 5p C) 2d D) 7s

2d

Round the number 3456.5 to two significant figures. A) 3400.0 B) 3400 C) 3500 D) 3000.0

3500

The number of electrons in the ion As-3 is _____. As = 33

36 electron

18. In the resonance form of ozone shown below, the formal charge on the central oxygen atom is _____. .. .. .. O = O - O: .. .. .. A) +1 B) 0 C) - 1 D) + 2

A

19. Nitrogen triiodide, NI3, is an unstable molecule that is used as a contact explosive. Its molecular structure is: A) Trigonal Pyramidal B) Tetrahedral C) Bent D) Trigonal Planar E) None of these

A

20. How many of the following molecules can have their structures drawn within a plane? i. CH4 ii. H2O iii. CO2 iv. BF3 A) Two molecules B) One molecule C) Three molecules D) All molecules E) No molecules

A

3. A molecule is defined as a Bronsted acid if it A) donates a proton to water B) increases the concentration of H+1 C) accepts a proton from water D) increases the concentration of OH-1

A

3. The reaction is an example of a(n) _____ reaction. 2 PCl3 + O2 → 2 POCl3 A) synthesis B) decomposition C) single replacement. D) double replacement

A

7. An ideal gas most closely approaches the behavior of a real gas under conditions of A) high P and low T B) low P and high T C) STP D) gases behave ideally under all conditions

A

A) ionic B) covalent C) polar covalent D) metallic E) hydrogen bonding 2. When the electronegativity difference between two atoms is 2 or greater, what type of bond can be predicted?

A

H2S + H2O ⇄ H3O+1 + HS-1 5. The conjugate acid of hydrogen sulfide ion, HS-1 is A) H2S B) S^-2 C) H3O^+1 D) H2O

A

What are the products of the following neutralization reaction? C6H5NH3+1 + OH-1 --> A. C6H5NH2 + H2O B. C6H6 + NH3 + H2O C. C6H5NH2-1 + H3O+1 D. C6H5OH + NH3

A

The correct result (indicating the proper number of significant figures) of the following addition is _. 12 1.2 0.12 + 0.012 ________ A) 13 B) 13.3 C) 13.33 D) 13.332

A) 13

The statement that electrons occupy empty equal-energy orbitals first is: A) Hund's Rule. B) the Aufbau Principle. C) Bohr's Law D) the Pauli Exclusion Principle.

A) Hund's Rule

The SI unit of temperature is __________. A) K B) °C C) °F D) t

A) K

10. Substance A has a higher specific heat than substance B. With all other factors equal, which requires more energy to heat equal masses of A and B to the same temperature? A) Substance A B) Substance B C) Both require the same amount of heat D) The answer depends on the density of each substance

A) Substance A

Solids have a __________ shape and are not appreciably __________. A) definite, compressible B) definite, incompressible C) indefinite, compressible D) indefinite, incompressible

A) definite, compressible

E = hv are... A) directly proportional B) inversely proportional C) inverses D) have no correlation

A) directly proportional

The quantum number that indicates the energy of an electron's orbital is called the _____ quantum number. A) principal B) angular momentum C) magnetic D) spin

A) principal

A photon of energy is released when an electron moves from one energy level: A) to a lower energy level. B) to a higher energy level. C) into the nucleus. D) to another position in the same level.

A) to a lower energy level.

1. Enthalpy is an expression for the A) total heat content of a system B) energy state of a system C) reaction rate D) activation energy

A) total heat content of a system

The maximum number of electrons that can occupy the s orbital at any energy level is: A) two, if they have opposite spins. B) two, if they have the same spin. C) one only. D) no more than eight.

A) two, if they have opposite spins

5. The condensation of water vapor actually A) warms the surroundings B) cools the surroundings C) sometimes warms and sometimes colds the surroundings, depending on the relative humidity at the time D) neither warms nor cools the surroundings

A) warms the surroundings

1. In a chemical bond, the link between atoms results from the attraction between electrons and A) Lewis electron dot structures B) nuclei C) dispersion forces D) isotopes

B

13. Arrhenius bases A) produce H3O+1 ions B) produce hydroxide ions C) are electron pair donors D) are proton acceptors

B

16. Bases cause red litmus to turn A) green B) blue C) yellow D) black

B

17. In which of the compounds below is there more than one kind of hybridization (sp, sp2, and/or sp3) for carbon? i. CH3CH2CH2CH3 ii. CH3CH=CHCH3 iii. CH2=CH−CH=CH2 iv. H−C≡C−H A) i and iii B) ii only C) iii and iv D) I and iv

B

22. A weak electrolyte exists predominantly as _____ in solution. A) ions B) molecules C) electrons D) an isotope

B

2KClO3 → 2KCl + 3O2 6. Theodore is performing a _____ reaction. A) synthesis B) decomposition C) single replacement. D) double replacement

B

4. Which of these equations is correctly balanced? A) CaO + H2O → 2 Ca(OH)2 B) NH3 + 2 O2 → HNO3 + H2O C) Ca(OH)2 + 2 H3PO4 → Ca3(PO4)2 + 3 H2O D) Cu + H2SO4 → CuSO4 + H2O + SO2

B

5. Which of the following statements is NOT consistent with the kinetic molecular theory of gases? A) Individual gas molecules are relatively far apart. B) Different gases have different average kinetic energies at the same temperature. C) The actual volume of the gas molecules themselves is very small compared to the total volume of the container occupied by the gas at ordinary temperatures and pressures. D) There is no net gain or loss of the total kinetic energy in collisions between gas molecules.

B

8. Which is NOT an acid-base conjugate pair? A) HS-1 and S-2 B) H3O+1 and OH-1 C) C6H5COOH and C6H5COO-1 D) HNO2 and NO2-1

B

Acids taste A) sweet B) sour C) bitter D) salty

B

Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gases 4. compression of oxygen gas A) 1, 3, 4 B) 1, 3 C) 1, 2 D) 1, 4

B) 1, 3

6. For which one of the following reactions is ΔH°rxn equal to the heat of formation of the product? A) N2(g) + 3 H2(g) → 2 NH3(g) B) 1/2 N2(g) + O2(g) → NO2(g) C) 6 C(s) + 6 H(g) → C6H6(l) D) P4(s) + 12 Br(l) → 4 PBr3(l)

B) 1/2 N2(g) + O2(g) → NO2(g)

A d sublevel can hold a maximum of _____ electrons: A) 14 B) 10 C) 6 D) 5

B) 10

How many electrons in an atom can have the same first three quantum numbers? A) 1 B) 2 C) 3 D) 4

B) 2

The number of significant figures that should be retained in the result of the following calculation is [(11.13-2.6) x 10^4] / (103.05+16.9) x 10^-6 A) 1 B) 2 C) 3 D) 4

B) 2

10. A certain solid substance is hard, has a high melting point, and is non-conducting unless melted. It is most likely A) I2 B) NaCl C) CO2 D) Cu

B) NaCl

Electron dot or Lewis dot notation only needs to account for: A) s, p, and d sublevel electrons. B) at most 8 electrons. C) the lowest energy electrons. D) 2 electrons per energy level.

B) at most 8 electrons.

Of the following, only __________ is an extensive property. A) density B) mass C) boiling point D) temperature

B) mass

The product of the frequency of a wave and its wavelength is equal to the: A) number of waves passing a point in a second. B) speed of light. C) distance between successive wave crests. D) time for one full wave to pass a given point.

B) speed of light.

Which of the following is a correct mathematical statement about the relationship between wavelength and frequency? A) ν = λ / c B) ν ∝ 1 / λ C) ν ∝ λ D) ν ∝ −λ

B) ν ∝ 1 / λ

1. A compound contains 1.10 mol of K, 0.55 mol of Te, and 1.65 mol of O. What is the empirical formula of this compound? A) KTeO B) KeTe2O C) K2TeO3 D) K2TeO6

C

10. Which gives a basic solution when dissolved in water? I. CH3COO-1 II. NO3-1 III. NH4+1 A) I only B) II only C) I and II only D) I, II, and III

C

12. Arrange the following according to increasing bond polarity (least polar bond first): HF Br2 SO2 SrO A) SO2 < Br2 < SrO < HF B) Br2 < HF < SrO < SO2 C) Br2 < SO2 < HF < SrO D) SO2 < Br2 < HF < SrO

C

13. Which species exhibits molecular geometry usually described as v-shaped or bent? A) NH3 B) CH4 C) NO2-1 D) NO3-1

C

15. A typical triple bond consists of A) three sigma bonds B) three pi bonds C) one sigma bond and two pi bonds D) two sigma bonds and one pi bond

C

15. Which of the following is a strong base? A) NH3 B) C6H5NH2 C) NaOH D) C2H3O2-1

C

19. Which of the following is a correct expression for molarity? A) mol solute/liter solvent B) mol solute/mL solvent C) mol solute/L solution D) mol solute/kg solvent

C

2. Which of the following is NOT true at equilibrium? A) The forward reaction runs at the same rate as the reverse reaction. B) The reaction is a reversible reaction. C) All the substances in the reaction have equal concentrations at equilibrium. D) At equilibrium, the ratio of the concentrations of products to reactants equals an equilibrium constant, K.

C

4. The general reaction is a(n) _____ reaction. MX + N → NX + M A) synthesis B) decomposition C) single replacement. D) double replacement MX + N → NX + M

C

7. The relationship between [H+1] and [OH-1] in a solution determines whether a solution is acidic, basic or neutral. Choose the correct relationship. A) if [H+1] < [OH-1], then the solution is acidic B) if [H+1] = [OH-1], then the solution is acidic C) if [H+1] > [OH-1], then the solution is acidic D) none of the above are correct

C

H2S + H2O ⇄ H3O+1 + HS-1 6. In the equilibrium represented above, the species that act as bases include which of the following? I. HS-1 II. H2O III. H2S-1 A) II only B) III only C) I and II D) I and III

C

Express the temperature, 422.35 K, in degrees Celsius. A) 792.23 °C B) 695.50 °C C) 149.20 °C D) 50.89 °C

C) 149.20 °C

The number of possible orbital shapes that can exist in the third energy level is: A) 1 B) 2 C) 3 D) 4

C) 3

There are _____ unpaired electrons in a ground state nitrogen atom. A) 1 B) 2 C) 3 D) 4

C) 3

How many quantum numbers are needed to specify a particular electron in an atom? A) 2 B) 3 C) 4 D) 5

C) 4

How many significant figures are in the number 0.0034050? A) 7 B) 6 C) 5 D) 4

C) 5

How many valence electrons are shown by the notation 1s22s22p63s23p64s23d104p4? A) 2 B) 4 C) 6 D) 10

C) 6

2. Which of the following is a statement of the first law of thermodynamics? A) kinetic energy = Ek = 1/2 mv² B) ΔE = Efinal - Einitial C) Energy lost by the system must be gained by the surroundings D) 1 calorie = 4.184 joules (exactly)

C) Energy lost by the system must be gained by the surroundings

4. The addition of heat causes particles to _____ their average kinetic energy. A) lessen the effect of B) decrease C) increase D) stay the same

C) increase

The quantum model of the atom locates the electrons: A) at a specific distance from the nucleus. B) in a definite path around the nucleus. C) within a region of high probability. D) both inside and outside the nucleus.

C) within a region of high probability

B) chromium(III) oxide

Cr2O3

1. Which of the following compounds is NOT an electrolyte in water? A) HNO3 B) Na2SO4 C) KOH D) Ar

D

12. A substance that ionizes completely in aqueous solutions, producing H3O+1, is a A) weak base B) strong base C) weak acid D) strong acid

D

14. Which of the following should have the lowest boiling point? A) Na2S B) HF C) NH3 D) N2

D

16. The molecules in a sample of SO2 are attracted to each other by a combination of A) Dispersion forces and hydrogen bonding B) Dispersion forces and ionic bonding C) Covalent bonding and dipole-dipole interactions D) Dispersion forces and dipole-dipole interactions

D

17. Bases are said to be neutralized when they A) melt B) dissolve in water C) react with salts D) react with acids

D

2. How many moles of Fe(OH)3 can be formed by reacting 2 moles of O2 according to the reaction 4 Fe(OH)2 + O2 + 2 H2O → 4 Fe(OH)3 represented below? A) 2 moles B) 4 moles C) 6 moles D) 8 moles

D

21. The point in a titration at which the indicator changes is called the A) setpoint B) indicator point C) standard point D) end point

D

1 kilogram = __________ milligrams A) 1 × 10-6 B) 1,000 C) 10,000 D) 1,000,000

D) 1,000,000

Which one of the following is an endothermic process? A) ice melting B) water freezing C) boiling soup D) Both A and C

D) Both A and C

4. Which of the following are strong acids? HI HNO3 HF HBr A) HF and HBr B) HI, HNO3, HF, and HBr C) HI, HF, and HBr D) HI, HNO3, and HBr

D) HI, HNO3, and HBr

9. Which of the following statements is false? A) Enthalpy is a state function B) The enthalpy change for a reaction is equal in magnitude, but opposite in sign, to the enthalpy change for the reverse reaction. C) The enthalpy change for a reaction depends on the state of the reactants and products D) The enthalpy of a reaction is equal to the heat of a reaction at constant volume.

D) The enthalpy of a reaction is equal to the heat of a reaction at constant volume.

8. Which one of the following conditions would always result in an increase in the internal energy of a system? A) The system loses heat and does work on the surroundings. B) The system gains heat and does work on the surroundings. C) The system loses heat and has work done on it by the surroundings. D) The system gains heat and has work done on it by the surroundings.

D) The system gains heat and has work done on it by the surroundings.

If matter is uniform throughout and cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical processes, it is called a (an) __________. A) heterogeneous mixture B) element C) homogeneous mixture D) compound

D) compound

The size and shape of the electron cloud is most closely related to the electron's: A) charge. B) spin. C) mass. D) energy.

D) energy

3. For a given process at constant pressure, ΔHreaction of -100 kJ/mole. This indicates the reaction is A) endothermic B) unstable C) in need of a catalyst D) exothermic

D) exothermic

A common English set of units for expressing velocity is miles/hour. The SI unit for velocity is __. A) km/hr B) km/s C) m/hr D) m/s

D) m/s

According to Heisenberg the better an electron's momentum is known: A) the better its energy is known. B) the better its speed is known. C) the more poorly its charge is known. D) the more poorly its position is known.

D) the more poorly its position is known.

His atomic theory was the first to explain several laws of chemical combination.

Dalton

C) magnesium sulfide

MgS

D) dinitrogen tetroxide

N2O4

Write formulas of the following compounds. (1 point each) A) sodium carbonate ______________________

Na2CO3

E) phosphorus pentabromide

PBr5

In the equation E=hν the h stands for a value called _____ constant.

Planck's

According to Bohr's theory of electron structure an electron must _____ energy to move from a lower energy orbit to a higher one.

absorb

11. Name each of the following compounds. (1 point each) A) BF3

boron trifluoride

For which of the following can the composition vary? A) pure substance B) both homogeneous and heterogeneous mixtures C) homogeneous mixture D) heterogeneous mixture

both homogeneous and heterogeneous mixtures

B) Ca3P2

calcium phosphide

D) Cr(OH)3

chromium (III) hydroxide

A spectrum containing radiation of all wavelengths is called a _____ spectrum.

continuous

3. All of the following elements exist as diatomic molecules in nature except _____. A) fluorine B) oxygen C) nitrogen D) helium

d) HELIUM

If matter is uniform throughout and cannot be separated into other substances by physical means, it is A) a compound B) either an element or a compound C) a homogeneous mixture D) a heterogeneous mixture

either an element or a compound

Millikan measured the charge on one _____ from his oil drop experiment.

electron

Thomson discovered the _____ from observations made from his cathode ray experiments.

electron

The lowest energy condition of an atom is called the _____ _____.

ground state

A combination of salt, sand, and water is an example of..... a) pure substance b) homogeneous mixture c) heterogeneous mixture d) compound

heterogeneous mixture

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

heterogeneous mixture

Gases and liquids share the property of __________. A) compressibility B) definite volume C) incompressibility D) indefinite shape

indefinite shape

Which is NOT an example of matter? planets, light, dust, elemental phosphorus

light

Bohr devised his theory to explain _____ spectra that were then being used to identify elements.

line

The "12" written in the isotope symbol, carbon-12, is its _____ _____.

mass number

E) Hg2S

mercury (I) sulfide

C) CH4

methane

The principal quantum number is represented with the letter _____.

n

Most of the mass of an atom is in its _____.

nucleus

Rutherford discovered the _____ from his alpha scattering experiment.

nucleus

A highly probable location where a maximum of two electrons may be located is called a(n) _____.

orbital

Atoms emit energy in "packets" called _____.

photons

The popular name given to Thomson's model of the atom. (2 words)

plum pudding

According to the Pauli Exclusion Principle, no two electrons in an atom can have the same set of _____ _____.

quantum numbers

Most of the volume of an atom is taken up by _____ ______ _____.

the electron cloud

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

water is 11% hydrogen and 89% oxygen by mass